Term
| FOR NEARLY ALL THEIR COMPOUNDS: |
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Definition
Hydrogen atoms form one bond.
Carbon atoms form four bonds.
Nitrogen atoms form three bonds.
Oxygen atoms form two bonds
Halogens form one bond when they are surrounding atoms; fluorine is always a surround atom. |
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Term
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Definition
| Same relative placement of ATOMS but different locations of BONDING and LONE electron pairs. |
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Term
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Definition
| gaseous molecules containing either BERYLLIUM or BORON as the central atom; they have FEWER than 8 e- |
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Term
| OXIDATION NUMBERS (FORMULA) |
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Definition
| [valence electron/group#] - [lone pair e- + bonding e-] |
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Term
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Definition
| molecules that contain a central atom with an ODD # of valence e-...so they cannot have all their electrons in pairs. thus they are PARAMAGNETIC and are extremely REACTIVE |
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Definition
| central nonmetal atom from PERIOD 3 or higher, expands shell to form more bonds |
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Definition
| m and n are integers; A is central atom; X is a surrounding atom; E is a nonbonding v.e- group(lone pair) |
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Definition
| the double bond, with its greater electron density, repels the two single bonds more strongly than they repel each other |
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Term
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Definition
| a lone pair repels bonding pairs more strongly than bonding pairs repel each other. |
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Term
| do LEWIS STRUCTURES DEPICT SHAPE? |
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Definition
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Term
| for similar molecules within a given electron-grp arrangement, electron-pair repulsions cause deviations from ideal bond angles in the following order: |
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Definition
| lone pair-lone pair> lone pair-bonding pair> bonding pair-bonding pair |
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Term
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Definition
| the product of the partial charges and the distance between them |
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Term
when the compound CANCELS OUT it is:
when the compound DOES NOT CANCEL OUT: |
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Definition
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