Term
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Definition
- The properties of the elements are determined by their electron configurations.
- Electron configurations (and orbital properties) determine periodic trends: electron affinity, ionization energy, atomic size, metal vs nonmetal characteristics, bonding abilities.
- Each group shares common properties and distinct differences based on electron configurations. |
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Term
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Definition
H, alkali metals (Li, Na, K, Rb, Cs, Fr)
- All but H are very active metals.
- ns1 electron configuration (n=1 to 7)
- Metals readily oxidized to X+ state. |
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Term
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Definition
| Binary compounds containing H. |
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Term
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Definition
| - Hydrogen combines with G1A or G2A metal; contains hydride ion and metal cation; H+ is strong reducing agent. |
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Term
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Definition
| Hydrogen combines with other nonmetals..HCl, CH4, etc. |
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Term
| Metallic (Interstitial) Hydrides |
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Definition
| - Transition metal catalysts treated with H2 (g); H2 molecules dissociate at the metal surface and H atoms occupy holes in the crystal structure (potential use as a portable fuel). |
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Term
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Definition
- Alkaline earth metals: Be, Mg, Ca, Sr, Ba, Ra.
- All are reactive metals (Be and Mg less reactive with water at 25 degrees Celsius).
- ns2 electron configuration (n=2 to 7).
- Readily oxidized to X2+ state. |
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Term
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Definition
- Nonmetallic (B), Metals (Al, Ga, In, Tl)
- ns2p electron configuration (n=2 to 6).
- Cannot achieve valence electron octets in neutral molecules.
- B and Al form strong bonds to F and O. |
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Term
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Definition
- Nonmetallic (C), Metalloids (Si, Ge), Metals (Sn, Pb)
- ns2p2 electron configuration (n=2 to 6)
- Can achieve valence electron octets in neutral molecules.
- All form covalent bonds with other nonmetals). |
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Term
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Definition
- Nonmetallic (N, P), Metalloid (As), Metals (Sb, Bi).
- ns2p3 electron configuration (n=2 to 6).
- Electronegativity decreases down the group.
- Metallic character increases down the group.
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Term
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Definition
- Nonmetallic (O, S, Se), Metalloids (Te, Po).
- ns2p4 electron configuration (n=2 to 6).
- Metallic properties increase down the column, but not G6A element behaves like a true metal.
- Common behaviour: reaction with metal to become 2- ion in ionic compound; for most metals, most common minerals are oxides or sulfides.
- Covalent bonds with other NMs; series of covalent hydrides (H2X).
- All but O have d orbitals available, so more than an octet is common.
- Te and Po can be 4+ cations, but with limited chemistry. |
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Term
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Definition
- Nonmetallic: F, Cl, Br, I, At.
- ns2p5 electron configuration (n=2 to 6).
- All are nonmetals.
- Properties vary smoothly down the group, except for unexpectedly low E.A. of fluorine and small bond energy of F2.
- Highly reactive, not found as free elements in nature, but rather as halide ions (X-) in minerals and seawater.
- Highly electronegative..form polar covalent bonds with other NMs and ionic bonds with lower O.S. metals.
- Compounds with metals in higher O.S. are polar covalent. |
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Term
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Definition
- Nonmetallic (He, Ne, Ar, Kr, Xe, Rn)
- ns2p6 electron configuration (n=2 to 6)..full octet!
- All are nonmetals.
- All are very non-reactive, but some compounds can be formed. |
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