Term
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Definition
| A way in which atoms interact with each other |
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Term
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Definition
Occurs when there is a complete transfer of electrons from one atom to another
Cation + Anion
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Term
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Definition
Occurs when two atoms share electrons due to a partial transfer of electrons from one atom to another
Nonmetal + Nonmetal |
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Term
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Definition
| Bonds shared between two metals |
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Term
| Lewis Symbols (Lewis Dot) |
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Definition
| The chemical symbol for an element with a dot for each valence electron |
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Term
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Definition
| Atoms gain or lose electrons until they reach 8 valence electrons |
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Definition
| Energy required to completely separate a mole of a solid ionic compound into its gaseous ions |
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Term
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Definition
| A thermodynamic cycle based on Hess's law that relates the lattice energy of an ionic substance to its enthalpy of formation and to other measurable quantities. |
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Term
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Definition
| A representation of covalent bonding in a molecule that is drawn using Lewis symbols |
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Term
| Single, Double, and Triple Bonds |
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Definition
Single: 1 pair e-
Double: 2 pair e-
Triple: 3 pair e- |
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Term
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Definition
| A measure of the degree to which the electrons are shared unequally between atoms in a chemical bond |
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Term
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Definition
| A covalent bond in which the electrons are shared equally |
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Term
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Definition
| A covalent bond in which the electrons are not shared equally |
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Term
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Definition
| The ability of an atom to attract shared electrons |
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Term
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Definition
| A molecule that posses a nonzero dipole moment |
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Term
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Definition
| A molecule with one end having a partial negative charge and other end having a partial positive change |
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Term
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Definition
| A measure of a separation and magnitude of the positive and negative charges in polar molecules |
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Term
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Definition
| The number if valence electrons in an isolated atom minus the nuber of electrons assigned to the atom in the Lewis structure |
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Term
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Definition
| Individual Lewis structures in cases where two or more Lewis structures are equally good description of a single molecule |
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Term
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Definition
| The enthalpy change, ΔH, required to break a particular bond when the substance is in the gas phase |
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Term
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Definition
| FOR MAIN GROUP ATOMS: Number of val e- = group number |
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Term
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Definition
Closer to F = more EN
Closer to Fr = less EN |
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Term
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Definition
1.) Calculate total number of valence electrons
2.) Determine arrangement
3.) Place one pair of electrons between each pair of bonded atoms to form a single bond
4.) Distributed the remaining electrons as lone pairs on terminal atoms
5.) Check to see if the octets are satisfied
6.) Calculate formula charges |
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Term
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Definition
| Helps to determine which Lewis structure is the best |
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Term
| # of val e- - (# lone pair e- + ½ * # bonding e-) |
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Definition
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