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the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

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the amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated gaseous atom to form a cation.

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the change in energy of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion.

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a measure of an atom's ability to attract the shared electrons of a covalent bond to itself.

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an electron shell, or a principal energy level, may be thought of as an orbit followed by electrons around an atom's nucleus.

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explains the nature and behavior of matter and energy on the atomic and subatomic level.

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each of the actual or potential patterns of electron density that may be formed in an atom or molecule by one or more electrons, and that can be represented as a wave function.

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an element (e.g., germanium or silicon) whose properties are intermediate between those of metals and solid nonmetals. They are electrical semiconductors.

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are (usually) poor conductors of heat and electricity, and are not malleable or ductile; many of the elemental nonmetals are gases at room temperature, while others are liquids and others are solids.

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are good conductors of heat and electricity, and are malleable (they can be hammered into sheets) and ductile (they can be drawn into wire).  Most of the metals are solids at room temperature, with a characteristic silvery shine (except for mercury, which is a liquid).

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any of the gaseous elements helium, neon, argon, krypton, xenon, and radon, occupying Group 0 (18) of the periodic table. They were long believed to be totally unreactive but compounds of xenon, krypton, and radon are now known.

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any of the six nonmetallic elements that constitute Group 17 (Group VIIa) of the periodic table. They were given the name halogen, from the Greek roots hal- (“salt”) and -gen (“to produce”), because they all produce sodium salts of similar properties, of which sodium chloride—table salt, or halite—is best known.

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any of the set of metallic elements occupying a central block (Groups IVB–VIII, IB, and IIB, or 4–12) in the periodic table, e.g., iron, manganese, chromium, and copper. Chemically they show variable valence and a strong tendency to form coordination compounds, and many of their compounds are colored.

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are all of the elements in the second column (column 2A) of the periodic table. This group includes beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). Alkaline earth metals have only two electrons in their outermost electron layer.

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include all of the elements in column 1A of the periodic table: hydrogen, lithium, sodium, potassium, rubidium, cesium, and francium.
These metals are united by the fact that they all have one electron in their outermost layer of electrons.

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a set of elements occupying a column in the periodic table and having broadly similar properties arising from their similar electronic structure.

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a set of elements occupying an entire horizontal row in the periodic table.

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a table of the chemical elements arranged in order of atomic number, usually in rows, so that elements with similar atomic structure (and hence similar chemical properties) appear in vertical columns.