Term
1. Non Metals
2. Metals and Non Metals |
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Definition
Covalent bonds happen between ______
Ionic bonds happen between ______ |
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| When nonmetals bond together, energy is lowest when the electrons are between the ___________ |
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| molecular stability, shape, size, and polarity |
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| Lewis structures allow us to predict many properties of covalent molecules such as. |
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| Beryllium (Be) only requires ___ VEs. |
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| Boron (B) only requires __ VEs. |
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| ______ and higher period elements can exhibit bonding where an octet on the central atom is exceeded--can expand up to __ e-. |
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| The _______ electronegative atom goes in the center. |
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| One end of the bond has a larger electron density than the other "Electronegativity" results in a ____________ bond. |
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| The larger the diff. in electronegativity, the more _____ the bond. (greater unsharing of electrons) |
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If the diff. in electronegativity b/w bonded atoms is 0 to 0.4, the bond is _________.
-equal sharing of e- |
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If the diff. in electronegativity b/w bonded atoms is 0.5 to 1.9 the bond is _________.
-unequal sharing of e- |
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Definition
| If the diff. in electronegativity b/w bonded atoms is > or = 2.0, the bond is _________ |
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| Formal Charge - any ______ formal charges on the _____ electronegative atoms are considered to best describe the bonding in the molecule or ion. |
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| Polar covalent bonds have ______ moments. Based on bond polarity and EN |
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| is a measure of bond polarity. Has a + and - end. End with larger EN gets -. End with electron dificient gets a +. Drawn from less EN atom toward more EN atom |
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| The more electrons two atoms share and the larger the atoms are, the ______ the dipole moment |
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| = Valence e- - lone pair e- - bonds |
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| Why molecular shape matters |
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Definition
Determines overal polarity of a molecule
- Solubility
-MP and BP
how molecules "fit" together
Material properties
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| Steric Number (SN) = number of ___________ to the central atom + number of ________ on central atom |
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| SN of the central atom determines _________. |
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| _________ that make up SN (bonds vs lonepairs) determines "shape". |
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| The relative sizes of repulsive force interactions are: |
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| When all electron groups in SN are bonding groups the arrangement = shape... when there are lone pairs on the central atom you will have a ________ shape |
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| SN = 5 (4 bonds and 1 LP) |
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| SN = 5 (3 bonds and 2 LP) |
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| SN = 5 (2 bonds and 3 LP) |
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| SN = 6 (5 bonds and 1 LP) |
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| SN = 6 (4 bonds and 2 LP) |
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| For Trigonal Bipyramidal (SN=5) The bond angle b/w axial and equatorial positions is ___ |
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| For Trigonal Bipyramidal (SN=5) The bond angle b/w equatorial positions is ___ |
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| axial. (only equatorial lone pair) |
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Definition
| Replacing atoms w/ LPs in the Trigonal Bipyramidal _____ lone pair does not occur. |
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