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Definition
| A bond that results from the sharing of electrons between atoms |
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| THe unit of matter held together by covalent bonds |
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-optimum distance between nuclei forming a bond.
-where net attractive forces are maximized and molecule is most stable
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-shows specific bonds between atoms
-gives much more info than a chemical formula
-uses lines between atoms to represent covalent bonds
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| lists the symbols of the compound's constituent elements and uses subscripts to indicate the number of atoms of each element |
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| bond dissociation energy (D) |
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Definition
| the amount of energy that must be supplied to break a chemical bond in an isolated molecule in the gaseous state, and thus the amount of energy released when the bond forms |
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range of strength of bonds commonly encountered in naturally occuring molecules
Ex. (C-H , C-C , C-O) |
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| The amount of energy that must be supplied to break an ionic solid into its individual gaseous ions and is thus a measurement of the strength of the crystal's ionic bonds |
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the large majority of bonds in which bonding electrons are shared unequally between two atoms but are not completely transferred
Represented by delta (δ)
- (δ+) for atom w/ smaller share
- (δ-) for atom w/ larger share |
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| electrostatic potential map |
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Definition
-uses cols to portray the calculated electron distribution in an isolated, gas-phase molecule
-blue represents electron shortage (partial positive) and red represents electron surplus (partial negative) |
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-the bond between the two atoms is equal
-occurs with diatomic molecules that contain a covalent bond between two identical atoms |
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-The ability of an atom in a molecule to attract shared electrons in a covalent bond
-fluorine has the highest
-metallic elements have weakest
-highest top right decreases to lowest bottom left |
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| what is bond polarity caused by |
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Definition
| differences in electronegativity |
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Definition
| the energy change that occurs when an electron is added to an isolated gaseous atom |
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| the amount of energy needed to remove the highest-energy electron from an isolated neutral atom in the gaseous state |
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Lewis Structes
(Electron-Dot Structures) |
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Definition
| represents an atom's valence electrons by dots and indicates by the placement of the dots how the valence electrons are distributed in a molecule |
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| states that main-group elements tend to undergo reactions that give them a noble-gas electron configuration with filled s and p sublevels in their valence electron shells |
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Definition
| pairs of nonbonding electrons on each atom in a covalent bond |
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Definition
| the shared electrons between two atoms in a covalent bond |
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Definition
number of pairs of electrons shared in a covalent bond
Delineated by lines
- is 1
= is 2
i dont have a button with three lines but you get the idea |
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| Coordinate Covalent Bonds |
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Definition
Bond formed whenone atom donates both electrons (a lone pair) to another atom that has a vacant valence orbital.
Ex.
ammonium ion (NH4+) forms when two lone pair electrons from the nitrgen atom of ammonia (NH3) bond to (H+)
N,O,P, and S form these regularly |
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