13 e-groups, 2 bonding groups, 0 lone pairs
EG: linear
MG: linear
180deg
23 e groups, 3 bonding groups, 0 lone pairs
EG trigonal planar
MG Trigonal planar
120deg
33 e groups, 2 bonding groups, 1 lone pairs
EG: Trigonal planar
MG Bent
<120deg
44 e groups, 4 bonding groups, 0 lone pairs
EG tetrahedral
MG tetrahedral
109.5deg
54 e groups, 3 bonding groups, 1 lone pairs
EG Tetrahedral
MG trigonal pyramidal
<109.5deg
64 e groups, 2 bonding groups, 2 lone pairs
EG tetrahedral
MG bent
<109.5deg
75 e groups, 5 bonding groups, 0 lone pairs
EG trigonal bipyramidal
MG trigonal bipyramidal
120deg equatorial
90deg axial
85 e groups, 4 bonding groups, 1 lone pairs
EG trigonal bipyramidal
MG seesaw
<120deg equatorial
<90deg axial
95 e groups, 3 bonding groups, 2 lone pairs
EG trigonal bipyramidal
MG t shaped
<90deg
105 e groups, 2 bonding groups, 3 lone pairs
EG trigonal bipyramidal
MG linear
180deg
116 e groups, 6 bonding groups, 0 lone pairs
EG octahedral
MG octahedral
90deg
126 e groups, 5 bonding groups, 1 lone pairs
EG octahedral
MG square pyramidal
<90deg
136 e groups, 4 bonding groups, 2 lone pairs
EG octahedral
MG square planar
90deg
16HCO3 [-]
Hydrogen carbonate (or bicarbonate)
17Hydrogen carbonate (or bicarbonate)
HCO3 [-]
34Hydrate
Ionic compound with water component
35How name hydrates?
prefix then hydrate
ex.
mono-1
di-2
tri-3
tetra-4
penta-5
hexa-6
hepta-7
octa-8
nona-9
deca-10
36diamagnetic
CHEMICAL SPECIES w no unpaired electrons, all electrons are paired
37paramagnetic
chemical species w unpaired electron
38Are ionic compounds balanced
yes
39which elements MUST exist as diatomic molecules
H, N, O, F Cl, Br, I
40exceptions to the octet rule
incomplete octets, compounds w odd number of electrons, expanded octets
41what is a free radical
a highly unstable atom w an unpaired valence electron
42Formal charge equation
valence electrons - # covalent bonds - unpaired electrons
43steps to drawing a lewis structure
1. add up valence electrons
2. frame the structure
3. fill the octets on outer atoms
4. fill octet on central atom (may have to use double/triple bonds
5. add formal charges
44constitutional isomeres
compound shaving the same molecular formula but different bonding sequences
45how fill dots on lewis structures
by conventionm, one on each side, then fill in pairs
46which element goes in the center of a lewis structure
the most electronegative one
47resonance structures
multiple valid structures for same compound
in nature, the true structure is an average of the two resonance structures
48best resonance structure is
the one with a formal charge closest to zero
49if formal charges are equal across multiple resonant strcutures which is the bst
the one which places the formal charge on the atom w lowest electronegativity
50which elements can make an expanded octet
3rd row and below of pd. tbl
51is it better to have no expanded octets or a formal charge of 0
formal charge of 0
52what is the VSEPR method used for
determining shape
53Most electronegative element
Flourine (F)
54Tendancy of atoms to draw electrons to themselves in chemical bonds
electronegativity
55Bond energy
strength required to break bond
56how do we know bonds are between single and double in nature
bond energy is between that of a single and a double bond
57Are longer or shorter bonds stronger
Shorter bonds are stronger, Longer bonds are weaker
58covalent molecules with a polar end
poilar covalent molecules
59bond where electrons are shared equally
non-polar covalent bond
60electronegativety differnence of non-p[olar covalent bond
less that 0.4 (varies, not exact)
61electronegativity difference of a polar covalent bond
0.4 to 2.0 (varies, not exact)
62electronegativity difference of an ionic bond
2.0 to 3.3 (varies, not exact)
63formal charge equation
valence electrons - nonbonding valance - covalent bonds