Exam Review Flashcards
1
Q
Three regions of space
A
trigonal planar, 120
2
Q
Three regions of space, 1 LP
A
bent, <120
3
Q
Four regions of space
A
tetrahedral, 109.5
4
Q
Four regions of space, 1 LP
A
trigonal pyramidal, < 109.5
5
Q
Four regions of space, 2 LP
A
bent, «109.5
6
Q
Five regions of space
A
trigonal bipyramidal, 90 & 120
7
Q
Five regions of space, 1 LP
A
seesaw, 90 & 120
8
Q
Five regions of space, 2 LP
A
t shape, 90
9
Q
Five regions of space, 3 LP
A
linear
10
Q
Six regions of space
A
octahedral, 90
11
Q
Six regions of space, 1 LP
A
square pyramidal, 90
12
Q
Six regions of space, 2 LP
A
square planar, 90
13
Q
Intermolecular forces & Types
A
- Btwn atoms
- Dipole-dipole
- H bonding
- LD forces
14
Q
Intramolecular force
A
Btwn subatomic particles
15
Q
Ionic Solids
A
- More e- given = stronger
- High pnts
- Brittle
- Unconductive as solid, conductive as liquid
16
Q
Molecular/atomic Solids
A
- Neutral molecules w/weak intermolecular forces
- Noble gases
- Low pnts
- Poor conductors
- Variety
17
Q
Network/covalent Solids
A
- Atoms w/covalent bonds
- Hard
- High pnts
- Nonconductors
18
Q
Metallic Solids
A
- Malleable
- High pnts
- Conductors
19
Q
Thermal Energy
A
KE + PE
20
Q
Types of KE
A
- Translation
- Rotational
- Vibrational
21
Q
Enthalpy (H)
A
Total internal nrg of a substance (even w/o change in T)
22
Q
Exo and Endothermic Enthalpy
A
- Exo = -ive
- Endo = +ive
23
Q
BDE
A
Nrg needed to break bonds (H = react - prod)
24
Q
Strong bonds have
A
Low PE, high BDE
25
Weak bonds have
High PE, low BDE
26
As bond strength increases
- Needs more nrg (like 2/3 bonds)
- d btwn atoms decreases
27
Standard Enthalpy of Formation
- Uses standard form of element as 0KJ
- Hf = change in H for 1 mol (H = prod - react)
28
Ways of Measuring Rates
- Gas
- Colour
- Mass
- pH
- Conductivity
29
Collision Theory
Rxns only happens when entities collide at right orientation & KE
30
Factors that affect Rate of Reaction
- Ea
- Temp
- Bond type/strength (covalent needs more)
- C
- SA
- Catalysts
31
Rate law
= K [A]^m [B]^n
32
Reaction Mechanisms Requirements
1. Steps must added to eqn
2. Rate determ step = rate eqn
33
Characteristics of EQ
- Only macroscopi properties change
- System is closed, temp constant
- Rate F/B =
34
K Properties
- K always same regardless of C, except temp
- If EQ eqn reversed, K = 1/k
- When rxns +, xK
35
Changes in Pressure
EQ shifts to side that has less molecules
36
Endothermic Reactions
- Cooled = shift L
- Heated = shift R
37
Exothermic Reactions
- Cooled = shift R
- Heated = shift R
38
Changing EQ Sys without Changing Position
- Catalysts
- Inert gases
- Diff states
39
Solubility
Amount of solute that dissolves in a solvent at a temp
40
Molar Solubility is used to calculate
Ksp
41
Salt Ratios
- 1:1 = s^2
- 1:2 = 4s^3
- 1:3 = 27s^4
42
Trial Ion Product
Uses Q to find if precip will form
43
Common Ion Effect
Decrease in solubility when same ion present
44
Bronsted-Lowry Theory
Acid are donors, bases are acceptors
45
Strong acid/base
Very weak conjugate
46
Weak acid/base
Weak conjugate
47
Very weak acid/base
Strong conjugate
48
Weak A/B Ksp Value
-4 to -10
49
Salt is neutral if
- Cation from grp 1 or 2
- Anion is from a SA
50
Salt is basic if
Anion is a Cb to WA
51
Salt is acidic if
Cation is Ca to WB
52
Metallic Oxides
Basic
53
Non-metallic
Acidic
54
Orbitals
Cloud of probability for e
55
Principal Quantum Number
Size & nrg for atomic orbital
56
Secondary Quantum Number
Nrg sublvls (l = n-1)
57
Magnetic Quantum Number
Orientation of orbital (-l to +l)
58
Spin Quantum Number
Spin up or down (+/- 0.5)
59
Pauli Exclusion Principle
No same quantum #s
60
Aufbau Principle
lowest orbitals first
61
Hund's Rule
No pairing first
62
Hybrid Orbital
Orbital formed from combination of diff orbitals
63
Sigma Bonds
Orbitals overlap head to head
64
Pi Bonds
Orbitals overlap side to side
65
Covalent Bonds with Sigma and Pi Bonds
- Single = sigma
- Double = pi
- Triple = sigma, pi, pi
66
Oxidation Number Rules
- F always -1
- O2 usually -2, except peroxides = -1
67
Oxidizing Agent
Gains e-, is reduced
68
Reducing Agent
Loses e-, is oxidized
69
Reactions happens if
OA is above RA
70
Anode and Cathode Redox Reactions
- Anode = oxidized
- Cathode = reduced
71
Ethers
- Has O in the middle
- +oxy
72
Aldehyde
- Has O2 at the end
- +al
73
Ketones
- Has O2 in the middle
- +one
74
Carboxylic Acid
- COOH
- +oic acid
75
Ester
- COOH + OH
- +oate for COOH chain
76
Amine
- N
- +amine
77
Amides
- COOH + NH
- +amide for O2 + N chain
78
Types of Addition Reactions
- Hydrogenation
- Halogenation
- Hydrohalogenation
- Hydration
79
Alcohols Reactions
- Dehydrate into akenes
- Oxidize into aldehyde/ketone
80
Aldehydes and Ketones Reactions
Hydrogenation into 1 or 2nd alcohol
81
Estertification
COOH + OH = ester
82
Amine Condensation
Alkyl Halide + amine
83
Amides Condensation
COOH + amine
84
Organic Compound Hierarchy
1. COOH
2. Amides
3. Alcohol
4. Amines
5. Ketones
6. Aldehyde
7. Ester
8. Ether
9. Benzene
10. Alkynes
11. Alkenes
12. Alkanes
85
Electron Configuration Exceptions
- Cr: [Ar] 4s13d5
- Cu: [Ar] 4s13d10
- Ag: [Kr] 5s14d10
- Au: [Xe] 6s14f145d10
