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9 Cards in this Set
- Front
- Back
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Alkali metals |
Although hydrogen has 1 valence electron and is found on the periodic table in Group 1A, it does not truly belong to any particular group. |
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Alkaline earth metals |
The alkaline earth metals have 2 valence electrons.They have characteristic metal properties but are harder, more dense, and melt at higher temperatures than the alkali metals. |
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Transition metals |
The Co2+ and Co3+ ions have the following electron configurations. In general, electrons are removed from the valence-shell s orbitals before they are removed from valence d orbitals when transition metals are ionized. |
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Halogens |
Electrons orbit the nucleus -- made of protons and neutrons -- in concentric levels. The outermost level that contains electrons is called the valence level, and the electrons in this level are called valence electrons. Each group, or column, in the periodic table has a particular number of valence electrons. |
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Period |
The periodic table has seven periods. Period 1 contains only two elements: hydrogen and helium. Period 6 (including the lanthanides running from lanthanum tolutetium) contains 32 elements and so is home to more elements than any other period. |
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Group |
a group (also known as a family) is a column of elements in the periodic table of the chemical elements. There are 18 numbered groups in the periodic table, but the f-block columns (between groups 2 and 3) are not numbered. |
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Valence electrons |
The valence electrons (VE) are theelectrons in the outer shell of an atom. Thevalence electrons are the ones involved in forming bonds to adjacent atoms. Therefore, the number of VE is important for determining the number of bonds an atom will form, the number of unpaired electrons, and an atom's formal charge. |
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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. |
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Ionization energy |
the quantity of energy that an isolated, gaseous atom in the ground electronic state must absorb to discharge an electron, resulting in a cation |
