Midterm #1 Flashcards
(99 cards)
1
Q
What 2 characteristics of carbon are why carbon is important to life?
A
(1) versatility - to make single, double, triple bonds
(lots of molecules with different shapes)
(2) bond strength - not too strong and not too weak
2
Q
What 2 things happen to a molecule during a reaction?
A
collision
covalent bonds break/form
3
Q
Period
A
across periodic table
4
Q
Group
A
down periodic table (columns)
5
Q
constitutional isomers
A
same formula but different structure/arrangement (differ in the way they are connected)
6
Q
O # of valence electrons
A
6
7
Q
He # of valence electrons
A
2
8
Q
Li # of valence electrons
A
1
9
Q
Be # of valence electrons
A
2
10
Q
B # of valence electrons
A
3
11
Q
C # of valence electrons
A
4
12
Q
N # of valence electrons
A
5
13
Q
F # of valence electrons
A
7
14
Q
Na # of valence electrons
A
1
15
Q
Mg # of valence electrons
A
2
16
Q
K # of valence electrons
A
1
17
Q
Al # of valence electrons
A
3
18
Q
Si # of valence electrons
A
4
19
Q
P # of valence electrons
A
5
20
Q
S # of valence electrons
A
6
21
Q
Cl # of valence electrons
A
7
22
Q
Br # of valence electrons
A
7
23
Q
I # of valence electrons
A
7
24
Q
At # of valence electrons
A
7
25
Electronegativity increases...
left to right across period (row)
| bottom to top of group (column)
26
Electronegativity of Li
1.0
27
Electronegativity of Be
1.5
28
Electronegativity of C
2.5
29
Electronegativity of N
3.0
30
Electronegativity of O
3.5
31
Electronegativity of F
4.0
32
Electronegativity of Na
0.9
33
Electronegativity of Mg
1.2
34
Electronegativity of Al
1.5
35
Electronegativity of Si
1.8
36
Electronegativity of P
2.1
37
Electronegativity of S
2.5
38
Electronegativity of Cl
3.0
39
Electronegativity of K
0.8
40
Electronegativity of Br
2.8
41
Covalent bonds
| difference in EN?
<0.5
42
Polar covalent bonds
| difference in EN?
0.5< EN<1.7
43
Ionic bonds
| difference in EN?
>1.7
44
C-Br
| what kind of bond?
polar covalent
45
Induction
withdrawal of e toward EN atom
46
4 sigma bonds - has what kind and how many hybridized orbitals?
4 sp3
47
3 sigma bonds, 1 pi bond - has what kind and how many hybridized orbitals?
3 sp2 `
48
2 sigma bonds, 2 pi bonds - what kind and how many hybridized orbitals?
2 sp
49
steric number
total number of s bonds and lone pairs
50
For any sp3 hybridized atom, the 4 valence e's will form a ____ electorn group geometry
tetrahedral
51
Steric number = 4
| no lone pairs
sp3
| tetrahedral
52
Steric number = 4
| 1 lone pair
sp3
| trigonal pyramidal
53
Steric number = 4
| 2 lone pairs
sp3
| bent
54
Steric number = 3
| one lone pair
sp2
| bent
55
Steric number = 3
| no lone pairs
sp2
| trigonal pyramidal
56
Steric number = 2
sp
| linear
57
dipole moment
center of negative and positive charge are separated from each other by a certain distance
58
molecular dipole moment
vector sum of individual dipole moments
| -sum of magnitude and direction of each dipole moment
59
carbocation
ion containing + charged carbon atom
60
carbanion
ion containing - charged carbon atom
61
delocalization of either a + or - charge __ a molecule
stabilizes
62
curved arrows generally show?
electron movement for PAIRS
63
curved arrows start where?
| end where?
start where electrons are currently located
| end where electrons will end up
64
Bronsted-Lowry Acid
proton donor
65
Bronsted-Lowry Base
proton acceptor
66
conjugate acid is the product that results when ?
base is protonated
67
conjugate base is the product that results when?
acid is deprotonated
68
curved arrows are used to illustrate a ?
reaction mechanism - how a reaction occurs in terms of the motion of electrons
69
value of Ka measures?
measures strength of acid
70
strong acid has __ Ka and a ___ pKa
high Ka, low pKa
71
weak acid has __ Ka and a ___ pKa
low Ka, high pKa
72
4 factors affecting stability of (-) charge
1) type of atom that carries charge
2) resonance
3) induction
4) type of orbital where charge resides
73
When two atoms are in the same row, which atom is better at stabilizing (-) charge?
ELECTRONEGATIVITY is dominant effect
| more EN atom is better at stabilizing charge
74
When two atoms are in the same group (column), which atom is better at stabilizing (-) charge?
SIZE is dominant effect
| Larger atom can better stabilize the (-) charge
75
How does RESONANCE affect stability of negative charge?
delocalized charge is more stable
| resonance structures show electron delocalization
76
How does INDUCTION affect stability of negative charge?
if atoms withdraw e density away from negatively charged region of compound, it stabilizes (-) charge
77
How does TYPE OF ORBITAL affect stability of negative charge?
sp orbitals hold e's closer to nucleus than sp2 or sp3
| therefore sp is more stable
78
Order of priority for stabilizing negative charge?
```
ARIO
atom (EN)
resonance
induction
orbitals
```
79
Steric hindrance occurs when...
the large size of groups within a molecule prevents chemical reactions that are observed in related molecules with smaller groups
80
lewis acid
e pair acceptor
81
lewis base
e pair donor
82
Not all __ acid/bases can't be classified as __ acid/bases
Lewis
| BL
83
Hydrocarbon
compounds comprised of JUST C and H
84
Saturated Hydrocarbons or ALKANES
hydrocarbons that lack pi boinds
85
Isopropyl
(1-methylethyl)
86
sec-Butyl
(1-methylpropyl)
87
Isobutyl
(2-methylpropyl)
88
tert-Butyl
(1,1-dimethylethyl)
89
Isopentyl or isoamyl
(3-methylbutyl)
90
Neopentyl
(2,2-dimethylpropyl)
91
dihedral angle or torsional angle
angle between two atoms on different carbons
92
torsional strain
difference in energy b/w staggered and eclipsed conformations
93
gauche interaction
steric interaction that results when two groups are seperated by 60
94
anti conformation
staggered conformation with dihedral angle of 180
95
angle strain
increase in energy associated with bond angle that has deviated from preferred angle of 109.5
96
most stable conformation of the cyclohexane ring is?
chair conformation
97
In chair conformation, all H's are?
staggered
98
axial
parallel to vertical axis passing through center of ring
99
equatorial
positioned at angles parallel to the sets of parallel lines
