query: in the third period as the atomic number increases from group 1 to group 18 the atomic radius

pos: Period 3 element two, sodium and magnesium, are members of the s-block of the periodic table, while the others are members of the p-block. Note that there is a 3d subshell, but it is not filled until period 4, such giving the period table its characteristic shape of "two rows at a time". All of the period 3 elements occur in nature and have at least one stable isotope. As the atomic number of elements in Period 3 increases, the atomic radius decreases. As the atomic mass of elements in Period 3 increases, the electronegativity increases. As the atomic number of elements in

pos: Atomic radius they provided important evidence for the development and confirmation of quantum theory. The atomic radii decrease across the Periodic Table because as the atomic number increases, the number of protons increases across the period, but the extra electrons are only added to the same quantum shell. Therefore, the effective nuclear charge towards the outermost electrons increases, drawing the outermost electrons closer. As a result, the electron cloud contracts and the atomic radius decreases. In 1920, shortly after it had become possible to determine the sizes of atoms using X-ray crystallography, it was suggested that all atoms of the same element

pos: Period 3 element two, sodium and magnesium, are members of the s-block of the periodic table, while the others are members of the p-block. Note that there is a 3d subshell, but it is not filled until period 4, such giving the period table its characteristic shape of "two rows at a time". All of the period 3 elements occur in nature and have at least one stable isotope. As the atomic number of elements in Period 3 increases, the atomic radius decreases. As the atomic mass of elements in Period 3 increases, the electronegativity increases. As the atomic number of elements in

pos: Periodic table 11, electronegativity increases farther down the group. A "period" is a horizontal row in the periodic table. Although groups generally have more significant periodic trends, there are regions where horizontal trends are more significant than vertical group trends, such as the f-block, where the lanthanides and actinides form two substantial horizontal series of elements. Elements in the same period show trends in atomic radius, ionization energy, electron affinity, and electronegativity. Moving left to right across a period, atomic radius usually decreases. This occurs because each successive element has an added proton and electron, which causes the electron to be drawn

pos: Period 2 element because the two elements behave nothing like other s-block elements. Period 2 has much more conclusive trends. For all elements in period 2, as the atomic number increases, the atomic radius of the elements decreases, the electronegativity increases, and the ionization energy increases. Period 2 only has two metals (lithium and beryllium), making it the least metallic period (period 1 has no metals, but as mentioned above, only has two elements, so it would be impossible to have more metals) and the most nonmetals, with four. The elements in period 2 often have the most extreme properties in their respective

pos: Ionization energy configuration of Mg. That electron is much closer to the nucleus than the previous 3s electron. Ionization energy is also a periodic trend within the periodic table organization. Moving left to right within a period, or upward within a group, the first ionization energy generally increases, with some exceptions such as aluminum and sulfur in the table above. As the nuclear charge of the nucleus increases across the period, the atomic radius decreases and the electron cloud becomes closer towards the nucleus. Atomic ionization energy can be predicted by an analysis using electrostatic potential and the Bohr model of the

pos: Ionic radius ionic radius values are sufficiently transferable to allow periodic trends to be recognized. As with other types of atomic radius, ionic radii increase on descending a group. Ionic size (for the same ion) also increases with increasing coordination number, and an ion in a high-spin state will be larger than the same ion in a low-spin state. In general, ionic radius decreases with increasing positive charge and increases with increasing negative charge. An "anomalous" ionic radius in a crystal is often a sign of significant covalent character in the bonding. No bond is "completely" ionic, and some supposedly "ionic" compounds,

pos: Atomic radius and electrons because opposite charges attract, and more protons creates a stronger charge. The greater attraction draws the electrons closer to the protons, decreasing the size of the particle. Therefore, atomic radius decreases. Down the groups, atomic radius increases. This is because there are more energy levels and therefore a greater distance between protons and electrons. In addition, electron shielding causes attraction to decrease, so remaining electrons can go farther away from the positively charged nucleus. Therefore, size (atomic radius) increases. The following table summarizes the main phenomena that influence the atomic radius of an element: The electrons in the

pos: Atomic radius the next outer shell, accounting for the sudden increase in the atomic radius. The increasing nuclear charge is partly counterbalanced by the increasing number of electrons, a phenomenon that is known as shielding; which explains why the size of atoms usually increases down each column. However, there is one notable exception, known as the lanthanide contraction: the 5d block of elements are much smaller than one would expect, due to the shielding caused by the 4f electrons. Essentially, atomic radius decreases across the periods due to an increasing number of protons. Therefore, there is a greater attraction between the protons

pos: Periodic trends the same. Valency in the periodic table across a period first increases and then decreases. There is no change going down a group. However, this periodic trend is sparsely followed for heavier elements (elements with atomic number greater than 20), especially for lanthanide and actinide series. The greater the number of core electrons, the greater the shielding of electrons from the core charge of the nucleus. For this reason ionization energy is lower for elements lower down in a group, and polarizability of species is higher for elements lower down in a group. The valency does not change going down

pos: Alkali metal metals decreases down the group. This is because metal atoms are held together by the electromagnetic attraction from the positive ions to the delocalised electrons. As the atoms increase in size going down the group (because their atomic radius increases), the nuclei of the ions move further away from the delocalised electrons and hence the metallic bond becomes weaker so that the metal can more easily melt and boil, thus lowering the melting and boiling points. (The increased nuclear charge is not a relevant factor due to the shielding effect.) The alkali metals all have the same crystal structure (body-centred

pos: Diagonal relationship effects on atomic radii of isolated atoms. Moving rightward across the period decreases the atomic radii of atoms, while moving down the group will increase the atomic radii . Similarly, on moving rightward a period, the elements become progressively more covalent, less basic and more electronegative, whereas on moving down a group the elements become more ionic, more basic and less electronegative. Thus, on both descending a period "and" crossing a group by one element, the changes "cancel" each other out, and elements with similar properties which have similar chemistry are often found – the atomic size, electronegativity, properties of

pos: Core charge the net charge of a nucleus, considering the completed shells of electrons to act as a 'shield.' As a core charge increases, the valence electrons are more strongly attracted to the nucleus, and the atomic radius decreases across the period. Core charge Core charge is the effective nuclear charge experienced by an outer shell electron. In other words, core charge is an expression of the attractive force experienced by the valence electrons to the core of an atom which takes into account the shielding effect of core electrons. Core charge can be calculated by taking the number of protons in

pos: Period 6 element used in general discussions of lanthanide chemistry. All but one of the lanthanides are f-block elements, corresponding to the filling of the 4f electron shell; lanthanum, a d-block element, is also generally considered to be a lanthanide due to its chemical similarities with the other fourteen. All lanthanide elements form trivalent cations, Ln, whose chemistry is largely determined by the ionic radius, which decreases steadily from lanthanum to lutetium. The lanthanide elements are the group of elements with atomic number increasing from 57 (lanthanum) to 71 (lutetium). They are termed lanthanide because the lighter elements in the series are chemically

pos: Atomic mass (nucleon count). The amount that the ratio of atomic masses to mass number deviates from 1 is as follows: the deviation starts positive at hydrogen-1, then decreases until it reaches a local minimum at helium-4. Isotopes of lithium, beryllium, and boron are less strongly bound than helium, as shown by their increasing mass-to-mass number ratios. At carbon, the ratio of mass (in daltons) to mass number is defined as 1, and after carbon it becomes less than one until a minimum is reached at iron-56 (with only slightly higher values for iron-58 and nickel-62), then increases to positive values in

pos: Core charge across a row of the periodic table, the outer-shell electrons are pulled more and more strongly towards the nucleus and the atomic radius decreases. This can be used to explain a number of periodic trends such as atomic radius, first ionization energy (IE), electronegativity, and oxidizing. Core charge can also be calculated as 'atomic number' minus 'all electrons except those in the outer shell'. For example, chlorine (element 17), with electron configuration 1s 2s 2p 3s 3p, has 17 protons and 10 inner shell electrons (2 in the first shell, and 8 in the second) so: A core charge is

pos: Plumbane energies of hydrides of the formula MH or MH. Plumbane is an unstable colorless gas and is the heaviest group IV hydride. Furthermore, plumbane has a tetrahedral (T) structure with an equilibrium distance between lead and hydrogen of 1.73 Å. By weight percent, the composition of plumbane is 1.91% hydrogen and 98.09% lead. In plumbane, the formal oxidation states of hydrogen and lead are -1 and +4, respectively, because the electronegativity of hydrogen is higher than that of lead. The stability of metal hydrides with the formula MH (M = C–Pb) decreases as the atomic number of M increases. Early

pos: Metal ions in aqueous solution by the magenta line which passes through Ca, Mn and Zn, for which there is no stabilization in an octahedral crystal field. Hydration energy increases as size decreases. Crystal field splitting confers extra stability on the aqua ion. The maximum crystal field stabilization energy occurs at Ni. The agreement of the hydration enthalpies with predictions provided one basis for the general acceptance of crystal field theory. The hydration enthalpies of the trivalent lanthanide ions show an increasingly negative values at atomic number increases, in line with the decrease in ionic radius known as the lanthanide contraction. Single ion hydration entropy

neg: Alkali metal the nuclear charge (which is equal to the atomic number) is cancelled by the inner electrons; the number of inner electrons of an alkali metal is always one less than the nuclear charge. Therefore, the only factor which affects the atomic radius of the alkali metals is the number of electron shells. Since this number increases down the group, the atomic radius must also increase down the group. The ionic radii of the alkali metals are much smaller than their atomic radii. This is because the outermost electron of the alkali metals is in a different electron shell than the

neg: Periodic trends Periodic Law. Periodic Law also led to the development of the periodic table, which is widely used nowadays. The atomic radius is the distance from the atomic nucleus to the outermost stable electron orbital in an atom that is at equilibrium. The atomic radius tends to decrease across a period from left to right due to the shrinking of the atom because of increasing nuclear force on the electrons. The atomic radius usually increases while going down a group due to the addition of a new energy level (shell which causes shrinkage in the size of the atoms across the

neg: Alkali metal cubic) and thus the only relevant factors are the number of atoms that can fit into a certain volume and the mass of one of the atoms, since density is defined as mass per unit volume. The first factor depends on the volume of the atom and thus the atomic radius, which increases going down the group; thus, the volume of an alkali metal atom increases going down the group. The mass of an alkali metal atom also increases going down the group. Thus, the trend for the densities of the alkali metals depends on their atomic weights and atomic

neg: Atomic radius and the size and shape of molecules. Atomic radii vary in a predictable and explicable manner across the periodic table. For instance, the radii generally decrease along each period (row) of the table, from the alkali metals to the noble gases; and increase down each group (column). The radius increases sharply between the noble gas at the end of each period and the alkali metal at the beginning of the next period. These trends of the atomic radii (and of various other chemical and physical properties of the elements) can be explained by the electron shell theory of the atom;

neg: Atomic radii of the elements (data page) on the atom's state and context. Atomic radii vary in a predictable and explicable manner across the periodic table. For instance, the radii generally decrease rightward along each period (row) of the table, from the alkali metals to the noble gases; and increase down each group (column). The radius increases sharply between the noble gas at the end of each period and the alkali metal at the beginning of the next period. These trends of the atomic radii (and of various other chemical and physical properties of the elements) can be explained by the electron shell theory of the atom;

neg: Periodic table intervals) and the formulation of the first periodic tables. Atomic radii vary in a predictable and explainable manner across the periodic table. For instance, the radii generally decrease along each period of the table, from the alkali metals to the noble gases; and increase down each group. The radius increases sharply between the noble gas at the end of each period and the alkali metal at the beginning of the next period. These trends of the atomic radii (and of various other chemical and physical properties of the elements) can be explained by the electron shell theory of the atom;

neg: Atomic radius The way the atomic radius varies with increasing atomic number can be explained by the arrangement of electrons in shells of fixed capacity. The shells are generally filled in order of increasing radius, since the negatively charged electrons are attracted by the positively charged protons in the nucleus. As the atomic number increases along each row of the periodic table, the additional electrons go into the same outermost shell; whose radius gradually contracts, due to the increasing nuclear charge. In a noble gas, the outermost shell is completely filled; therefore, the additional electron of next alkali metal will go into

neg: Noble gas molecule that led Bartlett to attempt oxidizing xenon using platinum hexafluoride, an oxidizing agent known to be strong enough to react with oxygen. Noble gases cannot accept an electron to form stable anions; that is, they have a negative electron affinity. The macroscopic physical properties of the noble gases are dominated by the weak van der Waals forces between the atoms. The attractive force increases with the size of the atom as a result of the increase in polarizability and the decrease in ionization potential. This results in systematic group trends: as one goes down group 18, the atomic radius,

neg: Compounds of zinc electron shells. That two elements so different in atomic number have the same radius is a consequence of the d-block contraction. Whilst calcium is somewhat larger than magnesium, there is a steady decrease in size as atomic number increases from calcium to zinc. Zn(II) complexes are kinetically labile, i.e. the Zn-ligand bonds exchange with other ligands rapidly. For this reason, zinc ions are at the catalytic centers in many enzymes. Compounds with zinc in the oxidation state +1 are extremely rare. The compounds have the formula RZnR and they contain a Zn — Zn bond analogous to the metal-metal bond

neg: Atomic radius have the same radii. However, in 1923, when more crystal data had become available, it was found that the approximation of an atom as a sphere does not necessarily hold when comparing the same atom in different crystal structures. Widely used definitions of atomic radius include: The following table shows empirically measured covalent radii for the elements, as published by J. C. Slater in 1964. The values are in picometers (pm or 1×10 m), with an accuracy of about 5 pm. The shade of the box ranges from red to yellow as the radius increases; gray indicates lack of data.

neg: Metalloid nuclear charge increases with atomic number as do the number of electrons. The additional pull on outer electrons as nuclear charge increases generally outweighs the screening effect of having more electrons. With some irregularities, atoms therefore become smaller, ionization energy increases, and there is a gradual change in character, across a period, from strongly metallic, to weakly metallic, to weakly nonmetallic, to strongly nonmetallic elements. Going down a main group, the effect of increasing nuclear charge is generally outweighed by the effect of additional electrons being further away from the nucleus. Atoms generally become larger, ionization energy falls, and metallic

neg: Carbon group has a density of 5.32 grams per cubic centimeter. Tin has a density of 7.26 grams per cubic centimeter, and lead has a density of 11.3 grams per cubic centimeter. The atomic radii of the carbon group elements tend to increase with increasing atomic number. Carbon's atomic radius is 77 picometers, silicon's is 118 picometers, germanium's is 123 picometers, tin's is 141 picometers, and lead's is 175 picometers. Carbon has multiple allotropes. The most common is graphite, which is carbon in the form of stacked sheets. Another form of carbon is diamond, but this is relatively rare. Amorphous carbon is

neg: Periodic trends period). However, atomic radii tend to increase diagonally, since the number of electrons has a larger effect than the sizeable nucleus. For example, lithium (145 picometer) has a smaller atomic radius than magnesium (150 picometer). The atomic radius can be further specified as: The ionization potential is the minimum amount of energy required to remove one electron from each atom in a mole of atoms in the gaseous state. The "first ionization energy" is the energy required to remove the first electron, and generally the "nth ionization energy" is the energy required to remove the atom's "n"th electron, after the

neg: In Hearing of Atomic Rooster In Hearing of Atomic Rooster In Hearing of is the third album by British rock band Atomic Rooster. Although not included on the album, "The Devil's Answer" single was released just prior to it, becoming the band's highest chart success at number 4 in the UK. This helped push the album to a number 18 UK chart placing, despite the fact that the four musicians pictured on the inside cover never played together. The backing tracks (and some vocals) were recorded by Vincent Crane, John Cann and Paul Hammond, but Cann and Hammond were let go from the group soon

neg: Atomic number atomic numbers 1 to 118 have been observed. Synthesis of new elements is accomplished by bombarding target atoms of heavy elements with ions, such that the sum of the atomic numbers of the target and ion elements equals the atomic number of the element being created. In general, the half-life becomes shorter as atomic number increases, though an "island of stability" may exist for undiscovered isotopes with certain numbers of protons and neutrons. Atomic number The atomic number or proton number (symbol "Z") of a chemical element is the number of protons found in the nucleus of an atom. It

neg: Nonmetal among these elements are consequently higher than would otherwise be expected, having regard to periodic trends. The small atomic radii of carbon, nitrogen, and oxygen facilitates the formation of triple or double bonds. The larger atomic radii, which enable higher coordination numbers, and lower electronegativities, which better tolerate higher positive charges, of the heavier group 15–18 nonmetals means they are able to exhibit valences other than the lowest for their group (that is, 3, 2, 1, or 0) for example in PCl, SF, IF, and XeF. Period four elements immediately after the first row of the transition metals, such as

neg: Chemistry: A Volatile History – there cannot be any fractional values. Moseley realised it was the atomic number, not the atomic weight that determines the order of the elements. What's more, because the atomic number increases in whole numbers from one element to the next there can be no extra elements between Hydrogen (atomic number 1) and Uranium (atomic number 92) – there can only be 92 elements, there is no room for any more. Moseley was just 26 when he completed this research. Aged 27 he was killed in action during the First World War – shot through the head by a sniper.

neg: Alkali metal atomic radius, decreasing electronegativity, increasing reactivity, and decreasing melting and boiling points as well as heats of fusion and vaporisation. In general, their densities increase when moving down the table, with the exception that potassium is less dense than sodium. The atomic radii of the alkali metals increase going down the group. Because of the shielding effect, when an atom has more than one electron shell, each electron feels electric repulsion from the other electrons as well as electric attraction from the nucleus. In the alkali metals, the outermost electron only feels a net charge of +1, as some of

neg: Yttrium atomic number, it would have an apparent number of 64.5 to 67.5, placing it between the lanthanides gadolinium and erbium. It often also falls in the same range for reaction order, resembling terbium and dysprosium in its chemical reactivity. Yttrium is so close in size to the so-called 'yttrium group' of heavy lanthanide ions that in solution, it behaves as if it were one of them. Even though the lanthanides are one row farther down the periodic table than yttrium, the similarity in atomic radius may be attributed to the lanthanide contraction. One of the few notable differences between the

neg: Block (periodic table) side of the periodic table and includes elements from the first two columns, the alkali metals (group 1) and alkaline earth metals (group 2), plus hydrogen and helium. Helium can be placed in the second group of s block as well as the 18th group of p-block, but most scientists consider it to rest at the top of group 18 i.e. above neon (atomic number 10) as it has many properties similar to the group 18 elements.General valance configration is ns1-2 Most s-block elements are highly reactive metals due to the ease with which their outer s-orbital electrons interact to

neg: Periodic table in the same group tend to show patterns in atomic radius, ionization energy, and electronegativity. From top to bottom in a group, the atomic radii of the elements increase. Since there are more filled energy levels, valence electrons are found farther from the nucleus. From the top, each successive element has a lower ionization energy because it is easier to remove an electron since the atoms are less tightly bound. Similarly, a group has a top-to-bottom decrease in electronegativity due to an increasing distance between valence electrons and the nucleus. There are exceptions to these trends: for example, in group

neg: Sodium valence shell, resulting in weak metallic bonding and free electrons, which carry energy. Due to having low atomic mass and large atomic radius, sodium is third-least dense of all elemental metals and is one of only three metals that can float on water, the other two being lithium and potassium. The melting (98 °C) and boiling (883 °C) points of sodium are lower than those of lithium but higher than those of the heavier alkali metals potassium, rubidium, and caesium, following periodic trends down the group. These properties change dramatically at elevated pressures: at 1.5 Mbar, the color changes from

neg: Group 2 organometallic chemistry the atomic radius increases resulting in increasingly ionic character, higher coordination numbers, and increased ligand reactivity. Many dialkyl group 2 metals are polymeric in the crystalline phase and resemble trimethylaluminium in three-center two-electron bond. In the gas-phase they are once again monomeric. The metallocenes in this group are unusual. Bis(cyclopentadienyl)beryllium or beryllocene (CpBe) with a molecular dipole moment of 2.2 D rules out a classical metallocene with two hapticity 5 ligands. Instead the compound is a so-called slip η/η sandwich and on top of that also fluxional up to −125 °C. While magnesocene (CpMg) is a regular metallocene, bis(pentamethylcyclopentadienyl)calcium (Cp)Ca

neg: Dendral and its mass spectrum has a peak at 18 units. Heuristic Dendral would use this input mass and the knowledge of atomic mass numbers and valence rules, to determine the possible combinations of atomic constituents whose mass would add up to 18. As the weight increases and the molecules become more complex, the number of possible compounds increases drastically. Thus, a program that is able to reduce this number of candidate solutions through the process of hypothesis formation is essential. New graph-theoretic algorithms were invented by Lederberg, Harold Brown, and others that generate all graphs with a specified set of

neg: Wigner–Seitz radius volume formula_5, the Wigner–Seitz radius is defined by Solving for formula_1 we obtain where formula_9 is the particle density of free electrons. The radius can also be calculated as where formula_11 is molar mass, formula_12 is amount of free electrons per atom, formula_13 is mass density, and formula_14 is the Avogadro number. This parameter is normally reported in atomic units, i.e., in units of the Bohr radius. Values of formula_1 for the first group metals are listed below : Wigner–Seitz radius The Wigner–Seitz radius formula_1, named after Eugene Wigner and Frederick Seitz, is the radius of a sphere whose volume

neg: Right Now (Atomic Kitten album) Right Now (Atomic Kitten album) Right Now is the debut studio album by English girl group Atomic Kitten released originally on 23 October 2000 featuring original member Kerry Katona, following the departure of Katona the album was re-released on 6 August 2001 featuring vocals from Jenny Frost and the singles "You Are" and "Eternal Flame" with additional new tracks featured on the album. The first release of the album originally peaked at number 39, putting the group at risk of being dropped by the record label; the second release peaked at number 1. Orchestral Manoeuvres in the Dark members and

neg: Mercury(I) hydride to develop a mercury(I) hydride molecular laser. Mercury(I) hydride is an unstable gas and is the heaviest group 12 monohydride. The composition of mercury(I) hydride is 0.50% hydrogen and 99.50% mercury. In mercury(I) hydride, the formal oxidation states of hydrogen and mercury are −1 and +1, respectively, because of the electronegativity of mercury is lower than that of hydrogen. The stability of metal hydrides with the formula MH (M = Zn-Hg) increases as the atomic number of M increases. The Hg-H bond is very weak and therefore the compound has only been matrix isolated at temperatures up to 6 K.

neg: Nihonium nihonium to have an atomic radius larger than that of thallium due to it being one period further down the periodic table, but calculations suggest nihonium has an atomic radius of about 170 pm, the same as that of thallium, due to the relativistic stabilisation and contraction of its 7s and 7p orbitals. Thus nihonium is expected to be much denser than thallium, with a predicted density of about 16 to 18 g/cm compared to thallium's 11.85 g/cm, since nihonium atoms are heavier than thallium atoms but have the same volume. Bulk nihonium is expected to have a hexagonal close-packed

neg: Atomic radius Atomic radius The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding cloud of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius. Three widely used definitions of atomic radius are: Van der Waals radius, ionic radius, and covalent radius. Depending on the definition, the term may apply only to isolated atoms, or also to atoms in condensed matter, covalently bound in molecules, or in ionized and

neg: Atomic radius 1967. The values are in picometres (pm). Atomic radius The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding cloud of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius. Three widely used definitions of atomic radius are: Van der Waals radius, ionic radius, and covalent radius. Depending on the definition, the term may apply only to isolated atoms, or also to atoms in condensed matter, covalently

neg: Period 1 element lithium and fluorine (appearing twice), or left floating above the other elements and not assigned to any group in the periodic table. Helium is almost always placed above neon (which is in the p-block) in the periodic table as a noble gas, although it is occasionally placed above beryllium due to their similar electron configuration. Hydrogen (H) is the chemical element with atomic number 1. At standard temperature and pressure, hydrogen is a colorless, odorless, nonmetallic, tasteless, highly flammable diatomic gas with the molecular formula H. With an atomic mass of 1.00794 amu, hydrogen is the lightest element. Hydrogen is

neg: Nuclear binding energy to the whole. The region of increasing binding energy is followed by a region of relative stability (saturation) in the sequence from magnesium through xenon. In this region, the nucleus has become large enough that nuclear forces no longer completely extend efficiently across its width. Attractive nuclear forces in this region, as atomic mass increases, are nearly balanced by repellent electromagnetic forces between protons, as the atomic number increases. Finally, in elements heavier than xenon, there is a decrease in binding energy per nucleon as atomic number increases. In this region of nuclear size, electromagnetic repulsive forces are beginning to

neg: Atomic Robo in the "Best Coloring" category subsequently won by Dave Stewart. The first six issues of the series have been collected as "Atomic Robo Volume 1: Atomic Robo and the Fightin' Scientists of Tesladyne". "Atomic Robo Volume 2: Atomic Robo and the Dogs of War" was released as a trade paperback on February 18, 2009. The third series, "Atomic Robo Volume 3: Atomic Robo and the Shadow From Beyond Time", was released in trade on December 23, 2009, and a fourth, "Atomic Robo Volume 4: Atomic Robo and Other Strangeness", has been released in issue format and will be published in

neg: Periodic table closer to the nucleus. This decrease in atomic radius also causes the ionization energy to increase when moving from left to right across a period. The more tightly bound an element is, the more energy is required to remove an electron. Electronegativity increases in the same manner as ionization energy because of the pull exerted on the electrons by the nucleus. Electron affinity also shows a slight trend across a period. Metals (left side of a period) generally have a lower electron affinity than nonmetals (right side of a period), with the exception of the noble gases. Specific regions of

neg: Noble gas applied at a temperature of to convert it to a solid. The noble gases up to xenon have multiple stable isotopes. Radon has no stable isotopes; its longest-lived isotope, Rn, has a half-life of 3.8 days and decays to form helium and polonium, which ultimately decays to lead. Melting and boiling points generally increase going down the group. The noble gas atoms, like atoms in most groups, increase steadily in atomic radius from one period to the next due to the increasing number of electrons. The size of the atom is related to several properties. For example, the ionization potential

neg: Copernicium towards selenide formation being lower for copernicium than for mercury. This was unexpected as the stability of the group 12 selenides tends to decrease down the group from ZnSe to HgSe, while it increases down the group for the group 14 selenides from GeSe to PbSe. Copernicium Copernicium is a synthetic chemical element with symbol Cn and atomic number 112. It is an extremely radioactive element, and can only be created in a laboratory. The most stable known isotope, copernicium-285, has a half-life of approximately 29 seconds. Copernicium was first created in 1996 by the GSI Helmholtz Centre for Heavy

neg: Charge radius Charge radius The rms charge radius is a measure of the size of an atomic nucleus, particularly of a proton or a deuteron. It can be measured by the scattering of electrons by the nucleus and also inferred from the effects of finite nuclear size on electron energy levels as measured in atomic spectra. The problem of defining a radius for the atomic nucleus is similar to the problem of atomic radius, in that neither atoms nor their nuclei have definite boundaries. However, the nucleus can be modeled as a sphere of positive charge for the interpretation of electron scattering

neg: Transition metal groups (4 to 11), with some authors including some elements in groups 3 or 12. The elements in group 3 have an "ns"("n" − 1)"d" configuration. The first transition series is present in the 4th period, and starts after Ca ("Z" = 20) of group-2 with the configuration [Ar]4"s", or scandium (Sc), the first element of group 3 with atomic number "Z" = 21 and configuration [Ar]4"s"3"d", depending on the definition used. As we move from left to right, electrons are added to the same "d"-sub-shell till it is complete. The element of group 11 in the first transition series

neg: Atomic radius 4f-subshell, which is progressively filled from cerium ("Z" = 58) to lutetium ("Z" = 71), are not particularly effective at shielding the increasing nuclear charge from the sub-shells further out. The elements immediately following the lanthanides have atomic radii which are smaller than would be expected and which are almost identical to the atomic radii of the elements immediately above them. Hence hafnium has virtually the same atomic radius (and chemistry) as zirconium, and tantalum has an atomic radius similar to niobium, and so forth. The effect of the lanthanide contraction is noticeable up to platinum ("Z" = 78), after

neg: Period 6 element living organism. Tungsten interferes with molybdenum and copper metabolism, and is somewhat toxic to animal life. Rhenium is a chemical element with the symbol Re and atomic number 75. It is a silvery-white, heavy, third-row transition metal in group 7 of the periodic table. With an "estimated" average concentration of 1 part per billion (ppb), rhenium is one of the rarest elements in the Earth's crust. The free element has the third-highest melting point and highest boiling point of any element. Rhenium resembles manganese chemically and is obtained as a by-product of molybdenum and copper ore's extraction and refinement. Rhenium

neg: Period 3 element Period 3 element A period 3 element is one of the chemical elements in the third row (or period) of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when the periodic table skips a row and a chemical behaviour begins to repeat, meaning that elements with similar behavior fall into the same vertical columns. The third period contains eight elements: sodium, magnesium, aluminium, silicon, phosphorus, sulfur, chlorine, and argon. The first

neg: Periodic table structure explain group trends by proposing that elements within the same group generally have the same electron configurations in their valence shell. Consequently, elements in the same group tend to have a shared chemistry and exhibit a clear trend in properties with increasing atomic number. In some parts of the periodic table, such as the d-block and the f-block, horizontal similarities can be as important as, or more pronounced than, vertical similarities. Under an international naming convention, the groups are numbered numerically from 1 to 18 from the leftmost column (the alkali metals) to the rightmost column (the noble gases).

neg: Transactinide element mix characteristics of the elements of group 10, 12, and 18. Transactinide element In chemistry, transactinide elements (also, transactinides, or super-heavy elements) are the chemical elements with atomic numbers from 104 to 120. Their atomic numbers are immediately greater than those of the actinides, the heaviest of which is lawrencium (atomic number 103). Glenn T. Seaborg first proposed the actinide concept, which led to the acceptance of the actinide series. He also proposed the transactinide series ranging from element 104 to 121 and the superactinide series approximately spanning elements 122 to 153. The transactinide seaborgium was named in his honor.

neg: Lanthanide contraction The radii are very similar even though the number of electrons increases from 40 to 72 and the atomic mass increases from 91.22 to 178.49 g/mol. The increase in mass and the unchanged radii lead to a steep increase in density from 6.51 to 13.35 g/cm. Zirconium and hafnium therefore have very similar chemical behaviour, having closely similar radii and electron configurations. Radius-dependent properties such as lattice energies, solvation energies, and stability constants of complexes are also similar. Because of this similarity hafnium is found only in association with zirconium, which is much more abundant, and was discovered as a

neg: Carbon group electron configuration, especially in the outermost shells, resulting in trends in chemical behavior: Each of the elements in this group has 4 electrons in its outer orbital (the atom's top energy level). The last orbital of all these elements is the p orbital. In most cases, the elements share their electrons. The tendency to lose electrons increases as the size of the atom increases, as it does with increasing atomic number. Carbon alone forms negative ions, in the form of carbide (C) ions. Silicon and germanium, both metalloids, each can form +4 ions. Tin and lead both are metals while

neg: The Last Goodbye (Atomic Kitten song) The Last Goodbye (Atomic Kitten song) "The Last Goodbye" is a song by British girl group Atomic Kitten. It was composed by Daniel Poku, Espen Lind, Mikkel Storleer Eriksen, Tor Erik Hermansen, Hallgeir Rustan, and Peter Björkl and produced by Stargate for the band's second album "Feels So Good" (2002). The pop ballad was released as the third single from the album in 2002; in Ireland and the United Kingdom it was released as a double A-side with "Be with You". The song peaked at number two on the UK Singles Chart in December of that year. Two versions of

neg: Period 2 element Period 2 element A period 2 element is one of the chemical elements in the second row (or period) of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behavior of the elements as their atomic number increases; a new row is started when chemical behavior begins to repeat, creating columns of elements with similar properties. The second period contains the elements lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon. This situation can be explained by modern theories of atomic structure. In a quantum mechanical

neg: Period 1 element Period 1 element A period 1 element is one of the chemical elements in the first row (or period) of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate periodic (recurring) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when chemical behaviour begins to repeat, meaning that elements with similar behaviour fall into the same vertical columns. The first period contains fewer elements than any other row in the table, with only two: hydrogen and helium. This situation can be explained by

neg: Period 4 element Period 4 element A period 4 element is one of the chemical elements in the fourth row (or "period") of the periodic table of the elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when chemical behaviour begins to repeat, meaning that elements with similar behaviour fall into the same vertical columns. The fourth period contains 18 elements, beginning with potassium and ending with krypton. As a rule, period 4 elements fill their 4s shells first, then their

neg: Period 5 element Period 5 element A period 5 element is one of the chemical elements in the fifth row (or "period") of the periodic table of the elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when chemical behaviour begins to repeat, meaning that elements with similar behaviour fall into the same vertical columns. The fifth period contains 18 elements, beginning with rubidium and ending with xenon. As a rule, period 5 elements fill their 5s shells first, then their

neg: Atomic Kitten Atomic Kitten Atomic Kitten are a British pop girl group formed in Liverpool in 1998 whose current members are Natasha Hamilton and Liz McClarnon. The group was founded by Orchestral Manoeuvres in the Dark (OMD) members Andy McCluskey and Stuart Kershaw, who served as principal songwriters during Atomic Kitten's early years. The group's debut album "Right Now" was released in October 2000 and charted at number 39 in the United Kingdom. After five top ten singles, original member Kerry Katona quit – four weeks before "Whole Again" reached number one in the UK Singles Chart – and was replaced by

neg: Symbol (chemistry) (see Chemical elements in East Asian languages). However, Latin symbols are also used, especially in formulas. A list of current, dated, as well as proposed and historical signs and symbols is included here with its signification. Also given is each element's atomic number, atomic weight or the atomic mass of the most stable isotope, group and period numbers on the periodic table, and etymology of the symbol. Hazard pictographs are another type of symbols used in chemistry. Antimatter atoms are denoted by a bar above the symbol for their matter counterpart, so e.g. H is the symbol for antihydrogen. The

neg: Heavy metals of heavy metals are generally given as greater than 20 (calcium); sometimes this is capped at 92 (uranium). Definitions based on atomic number have been criticised for including metals with low densities. For example, rubidium in group (column) 1 of the periodic table has an atomic number of 37 but a density of only 1.532 g/cm, which is below the threshold figure used by other authors. The same problem may occur with atomic weight based definitions. The United States Pharmacopeia includes a test for heavy metals that involves precipitating metallic impurities as their coloured sulfides." In 1997, Stephen Hawkes, a

neg: Molecular orbital orbitals, which are allowed if the symmetries (determined from group theory) of the atomic orbitals are compatible with each other. Efficiency of atomic orbital interactions is determined from the overlap (a measure of how well two orbitals constructively interact with one another) between two atomic orbitals, which is significant if the atomic orbitals are close in energy. Finally, the number of molecular orbitals formed must be equal to the number of atomic orbitals in the atoms being combined to form the molecule. For an imprecise, but qualitatively useful, discussion of the molecular structure, the molecular orbitals can be obtained from

neg: Period 1 element by a low-temperature separation process called fractional distillation. Period 1 element A period 1 element is one of the chemical elements in the first row (or period) of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate periodic (recurring) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when chemical behaviour begins to repeat, meaning that elements with similar behaviour fall into the same vertical columns. The first period contains fewer elements than any other row in the table, with only two: hydrogen

neg: Atomic radii of the elements (data page) they provided important evidence for the development and confirmation of quantum theory. Note: All measurements given are in picometers (pm). For more recent data on covalent radii see Covalent radius. Data is as quoted at http://www.webelements.com/ from these sources: More recent data can be found in Covalent radius. The above values are based on Atomic radii of the elements (data page) The atomic radius of a chemical element is the distance from the centre of the nucleus to the outermost shell of the electron. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic

neg: Relativistic quantum chemistry the electron velocity. Notice how the relativistic model shows the radius decreasing with increasing velocity. When the Bohr treatment is extended to hydrogenic atoms, the Bohr radius becomes where formula_9 is the principal quantum number and Z is an integer for the atomic number. From quantum mechanics the angular momentum is given as formula_10. Substituting into the equation above and solving for formula_11 gives From this point atomic units can be used to simplify the expression into Substituting this into the expression for the Bohr ratio mentioned above gives At this point one can see that for a low value

neg: Periodic table Periodic table The periodic table, or periodic table of elements, is a tabular arrangement of the chemical elements, ordered by their atomic number, electron configuration, and recurring chemical properties, whose structure shows "periodic trends". Generally, within one row (period) the elements are metals to the left, and non-metals to the right, with the elements having similar chemical behaviours placed in the same column. Table rows are commonly called periods and columns are called groups. Six groups have accepted names as well as assigned numbers: for example, group 17 elements are the halogens; and group 18 are the noble gases. Also

neg: Ladies Night (Atomic Kitten album) UK Albums Chart, selling 48,000 copies in its first week of release. It was a considerable decline from the band's previous two studio albums "Right Now" (2000) and "Feels So Good" (2002), both of which had been certified double platinum by the British Phonographic Industry (BPI) and became number-one hits. A steady seller, "Ladies Night" was however certified platinum by the BPI for the shipment of over 550,000 copies in the United Kingdom. Ladies Night (Atomic Kitten album) Ladies Night is the third studio album by English girl group Atomic Kitten released on 10 November 2003. "If You Come to

neg: Lead shielding Lead shielding Lead shielding refers to the use of lead as a form of radiation protection to shield people or objects from radiation so as to reduce the effective dose. Lead can effectively attenuate certain kinds of radiation because of its high density and high atomic number; principally, it is effective at stopping gamma rays and x-rays. Lead's high density is caused by the combination of its high atomic mass and the relatively small size of its bond lengths and atomic radius. The high atomic mass means that more electrons are needed to maintain a neutral charge and the small

neg: Neptunium are less stable than the actinides before it on the periodic table such as thorium and uranium and more stable than those after it such as plutonium and americium. This phenomenon is because the stability of an ion increases as the ratio of atomic number to the radius of the ion increases. Thus actinides higher on the periodic table will more readily undergo hydrolysis. Neptunium(III) hydroxide is quite stable in acidic solutions and in environments that lack oxygen, but it will rapidly oxidize to the IV state in the presence of air. It is not soluble in water. Np(IV) hydroxides

neg: Atomic Kitten (album) group teamed up with Disney to include "The Tide Is High" in "The Lizzie McGuire Movie" starring Hilary Duff. However the album failed to chart on the "Billboard" 200. This resulted in Atomic Kitten focusing their attention on Europe, Oceania and Asia where they already were an established act. It was also released in New Zealand, where both "Right Now" and "Feels So Good" were successful and peaked at number 7. The album solely contained radio edits of the group's singles. Atomic Kitten (album) Atomic Kitten is the American debut album by Atomic Kitten. The girl group had previously been

neg: Period 3 element pulmonary agent in chemical warfare; however, chlorine is necessary to most forms of life, including humans, in form of chloride ions. Argon has no biological role. Like any gas besides oxygen, argon is an asphyxiant. Period 3 element A period 3 element is one of the chemical elements in the third row (or period) of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when the periodic table skips a row and

neg: Atomic radii of the elements (data page) Atomic radii of the elements (data page) The atomic radius of a chemical element is the distance from the centre of the nucleus to the outermost shell of the electron. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius. Depending on the definition, the term may apply only to isolated atoms, or also to atoms in condensed matter, covalently bound in molecules, or in ionized and excited states; and its value may be obtained through experimental measurements, or computed from theoretical models. Under some definitions, the value of the radius may depend

neg: Hubbard model spacing, which reduces the "hopping integral" to the point where the on-site potential is dominant. Similarly, this can explain the transition from conductor to insulator in systems such as rare-earth pyrochlores as the atomic number of the rare-earth metal increases, because the lattice parameter increases (or the angle between atoms can also change — see Crystal structure) as the rare-earth element atomic number increases, thus changing the relative importance of the hopping integral compared to the on-site repulsion. The hydrogen atom has only one electron, in the so-called "s" orbital, which can either be spin up (formula_1) or spin down

neg: Argon Argon Argon is a chemical element with symbol Ar and atomic number 18. It is in group 18 of the periodic table and is a noble gas. Argon is the third-most abundant gas in the Earth's atmosphere, at 0.934% (9340 ppmv). It is more than twice as abundant as water vapor (which averages about 4000 ppmv, but varies greatly), 23 times as abundant as carbon dioxide (400 ppmv), and more than 500 times as abundant as neon (18 ppmv). Argon is the most abundant noble gas in Earth's crust, comprising 0.00015% of the crust. Nearly all of the argon in

neg: Argon in Alaska, highlights the dangers of argon tank leakage in confined spaces and emphasizes the need for proper use, storage and handling. Argon Argon is a chemical element with symbol Ar and atomic number 18. It is in group 18 of the periodic table and is a noble gas. Argon is the third-most abundant gas in the Earth's atmosphere, at 0.934% (9340 ppmv). It is more than twice as abundant as water vapor (which averages about 4000 ppmv, but varies greatly), 23 times as abundant as carbon dioxide (400 ppmv), and more than 500 times as abundant as neon (18

neg: Atomic Kitten markets. Before recording their third album, Kool & the Gang approached the group about a collaboration for their album of duets, "Odyssey". Kool & the Gang wanted to record an updated version of their hit "Ladies Night" and were looking for a girl group to sing the lyrics. Atomic Kitten liked the idea and inquired whether they could use it for their next album which was subsequently named "Ladies Night" in honour of this collaboration. Atomic Kitten spent late 2002 and early 2003 in the studio recording their third and final studio album. Up until the recording of "Ladies Night",

neg: Atomic Knight alternate universe is not the original setting of the 1960s stories. In "Countdown: Arena #2" (2007) an alternate version of Captain Atom appears who is the leader of that world's Atomic Knights. Atomic Knight Atomic Knight is a DC Comics superhero and was briefly a member of the Outsiders team. He is sometimes depicted as one of a group of Atomic Knights, which first appeared in "Strange Adventures" #117 (June 1960) and ran quarterly in that monthly comic up through #160 (January 1964). The Atomic Knights appeared in every third issue of "Strange Adventures" in the early 1960s, beginning with

neg: Atomic Knight Atomic Knight Atomic Knight is a DC Comics superhero and was briefly a member of the Outsiders team. He is sometimes depicted as one of a group of Atomic Knights, which first appeared in "Strange Adventures" #117 (June 1960) and ran quarterly in that monthly comic up through #160 (January 1964). The Atomic Knights appeared in every third issue of "Strange Adventures" in the early 1960s, beginning with #117 (June 1960) and running through #160 (January 1964). In all there were 15 early-1960s Atomic Knights stories created by writer John Broome and artist Murphy Anderson; they were a band of

neg: Rydberg atom the atom is useful in explaining these properties. Classically, an electron in a circular orbit of radius "r", about a hydrogen nucleus of charge +"e", obeys Newton's second law: where "k" = 1/(4πε). Orbital momentum is quantized in units of "ħ": Combining these two equations leads to Bohr's expression for the orbital radius in terms of the principal quantum number, "n": It is now apparent why Rydberg atoms have such peculiar properties: the radius of the orbit scales as "n" (the "n" = 137 state of hydrogen has an atomic radius ~1 µm) and the geometric cross-section as "n". Thus

neg: Pair production results in a complicated function. To simplify, the cross section can be written as: formula_19 Where formula_20 is the fine structure constant, formula_21 is the classical electron radius, formula_22 is the atomic number of the material and formula_23 is some complex function that depends on the energy and atomic number. Cross sections are tabulated for different materials and energies. In 2008 the Titan laser aimed at a 1-millimeter-thick gold target was used to generate positron–electron pairs in large numbers. The symmetry of the phenomena complies to what would be the definition of a fractal. Therefore if formula_14 produces quantities of

neg: Ladies Night (Atomic Kitten album) sing the lyrics. Atomic Kitten liked the idea and inquired whether they could use it for their next album which was subsequently named "Ladies Night" in honour of this collaboration. Atomic Kitten spent late 2002 and early 2003 in the studio recording their third and final studio album. Up until the recording of "Ladies Night", the group mainly relied on songwriters, though they had occasionally co-written songs featured on their albums. While recording "Ladies Night", they decided to be directly involved in the creation of eight of the fifteen songs. "Ladies Night" debuted and peaked at number five on the

neg: Boron group characteristics. Boron differs from the other group members in its hardness, refractivity and reluctance to participate in metallic bonding. An example of a trend in reactivity is boron's tendency to form reactive compounds with hydrogen. Most of the elements in the boron group show increasing reactivity as the elements get heavier in atomic mass and higher in atomic number. Boron, the first element in the group, is generally unreactive with many elements except at high temperatures, although it is capable of forming many compounds with hydrogen, sometimes called "boranes". The simplest borane is diborane, or BH. Another example is BH.

neg: Period 5 element blood cells in the body. Tin is a chemical element with the symbol Sn (for ) and atomic number 50. It is a main group metal in group 14 of the periodic table. Tin shows chemical similarity to both neighboring group 14 elements, germanium and lead and has two possible oxidation states, +2 and the slightly more stable +4. Tin is the 49th most abundant element and has, with 10 stable isotopes, the largest number of stable isotopes in the periodic table. Tin is obtained chiefly from the mineral cassiterite, where it occurs as tin dioxide, SnO. This silvery, malleable

neg: Boron group which is generally only stable in the oxidation state of +1, although the +3 state is seen in some compounds. Stable and monomeric gallium, indium and thallium radicals with a formal oxidation state of +2 have since been reported. There are several trends that one could notice as they look at the properties of Boron group members. The Boiling Points of these elements drop from period to period, while densities tend to rise. With the exception of the synthetic nihonium, all of the elements of the boron group have stable isotopes. Because all their atomic numbers are odd, boron, gallium

neg: Periodic table they provided important evidence for the development and confirmation of quantum theory. The electrons in the 4f-subshell, which is progressively filled across the lanthanide series, are not particularly effective at shielding the increasing nuclear charge from the sub-shells further out. The elements immediately following the lanthanides have atomic radii that are smaller than would be expected and that are almost identical to the atomic radii of the elements immediately above them. Hence hafnium has virtually the same atomic radius (and chemistry) as zirconium, and tantalum has an atomic radius similar to niobium, and so forth. This is known as the

neg: Boron porphyrins Boron porphyrins Boron porphyrins are a variety of porphyrin, a common macrocycle used for photosensitization and metal trapping applications, that incorporate boron. The central four nitrogen atoms in a porphyrin macrocycle form a unique molecular pocket which is known to accommodate transition metals of various sizes and oxidation states. Due to the diversity of binding modes available to porphyrin, there is a growing interest in introducing other elements (i.e. main group elements) into this pocket. Boron in particular has been shown to prefer binding to porphyrin in a 2:1 stoichiometry, primarily due to its small atomic radius, but the Group

neg: Group 12 element have some similarities to oganesson as well as to the other group 12 elements. Unhexquadium should be at most moderately reactive, having a first ionization energy that should be around 685 kJ/mol, comparable to that of molybdenum. Due to the lanthanide, actinide, and superactinide contractions, unhexquadium should have a metallic radius of only 158 pm, very close to that of the much lighter magnesium, despite its being expected to have an atomic weight of around 474 u, about 19.5 times as much as that of magnesium. This small radius and high weight cause it to be expected to have an

neg: Jenny Frost 4 March 2012 it was confirmed that Atomic Kitten would reform but was later confirmed that Frost would not be returning to the group and would be replaced by Kerry Katona. Hamilton has since confirmed that Frost would be welcomed back if she wanted to rejoin the group in the future. After the split of Atomic Kitten, Frost embarked on a solo career and released her first single "Crash Landing" on 10 October 2005, which peaked at number 47 and thus failed to reach the Top 40. Frost originally recorded the song for the band Route 1, but decided to

neg: Atomic Kitten (album) Atomic Kitten (album) Atomic Kitten is the American debut album by Atomic Kitten. The girl group had previously been successful in Europe, Oceania and Asia and already released "Right Now" and "Feels So Good", which both went to number one on the UK Albums Chart, however there had not been any release in the United States. It was therefore decided to make an album consisting of tracks from both previous albums. Unlike Europe, Oceania and Asia, the success of Atomic Kitten in the United States was non-existent. The American music market is difficult for European acts and therefore the girl

neg: Atomic Kitten Hamilton. In January 2004, Hamilton announced she wanted to take a hiatus from the group and devote more time to her young son. Atomic Kitten released the double A-side single Someone like Me/"Right Now 2004" as a "goodbye" to their fans, but still performed on Valentine's Day 2005 and release the charity single "Cradle", a new version of the original song from their album "Right Now" which was a number-one hit in Asia back in 2000. "Cradle 2005" peaked at number ten, selling 35,000 copies worldwide, with proceeds going to World Vision. In 2005, Atomic Kitten were featured on the

neg: Cradle (Atomic Kitten song) Cradle (Atomic Kitten song) "Cradle 2005" is a song recorded by English girl group Atomic Kitten. It was released on 14 February 2005, in aid of World Vision. It is a remixed version of a song that was previously included on their debut album, "Right Now" (2000). "Cradle" was released a year after the group's announcement of their split in 2004; it was the last official single release by the group, although they released two charity singles in 2006 and 2008. "Cradle 2005" is Atomic Kitten's lowest-selling single, with sales of 35,000 copies worldwide. It reached number 10 on the