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SCH4U1 - Chemistry > Exam Review > Flashcards

Exam Review Flashcards

1
Q

Three regions of space

A

trigonal planar, 120

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2
Q

Three regions of space, 1 LP

A

bent, <120

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3
Q

Four regions of space

A

tetrahedral, 109.5

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4
Q

Four regions of space, 1 LP

A

trigonal pyramidal, < 109.5

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5
Q

Four regions of space, 2 LP

A

bent, «109.5

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6
Q

Five regions of space

A

trigonal bipyramidal, 90 & 120

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7
Q

Five regions of space, 1 LP

A

seesaw, 90 & 120

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8
Q

Five regions of space, 2 LP

A

t shape, 90

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9
Q

Five regions of space, 3 LP

A

linear

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10
Q

Six regions of space

A

octahedral, 90

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11
Q

Six regions of space, 1 LP

A

square pyramidal, 90

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12
Q

Six regions of space, 2 LP

A

square planar, 90

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13
Q

Intermolecular forces & Types

A
  • Btwn atoms
  • Dipole-dipole
  • H bonding
  • LD forces
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14
Q

Intramolecular force

A

Btwn subatomic particles

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15
Q

Ionic Solids

A
  • More e- given = stronger
  • High pnts
  • Brittle
  • Unconductive as solid, conductive as liquid
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16
Q

Molecular/atomic Solids

A
  • Neutral molecules w/weak intermolecular forces
  • Noble gases
  • Low pnts
  • Poor conductors
  • Variety
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17
Q

Network/covalent Solids

A
  • Atoms w/covalent bonds
  • Hard
  • High pnts
  • Nonconductors
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18
Q

Metallic Solids

A
  • Malleable
  • High pnts
  • Conductors
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19
Q

Thermal Energy

A

KE + PE

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20
Q

Types of KE

A
  • Translation
  • Rotational
  • Vibrational
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21
Q

Enthalpy (H)

A

Total internal nrg of a substance (even w/o change in T)

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22
Q

Exo and Endothermic Enthalpy

A
  • Exo = -ive
  • Endo = +ive
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23
Q

BDE

A

Nrg needed to break bonds (H = react - prod)

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24
Q

Strong bonds have

A

Low PE, high BDE

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25
Q

Weak bonds have

A

High PE, low BDE

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26
Q

As bond strength increases

A
  • Needs more nrg (like 2/3 bonds)
  • d btwn atoms decreases
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27
Q

Standard Enthalpy of Formation

A
  • Uses standard form of element as 0KJ
  • Hf = change in H for 1 mol (H = prod - react)
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28
Q

Ways of Measuring Rates

A
  • Gas
  • Colour
  • Mass
  • pH
  • Conductivity
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29
Q

Collision Theory

A

Rxns only happens when entities collide at right orientation & KE

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30
Q

Factors that affect Rate of Reaction

A
  • Ea
  • Temp
  • Bond type/strength (covalent needs more)
  • C
  • SA
  • Catalysts
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31
Q

Rate law

A

= K [A]^m [B]^n

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32
Q

Reaction Mechanisms Requirements

A
  1. Steps must added to eqn
  2. Rate determ step = rate eqn
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33
Q

Characteristics of EQ

A
  • Only macroscopi properties change
  • System is closed, temp constant
  • Rate F/B =
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34
Q

K Properties

A
  • K always same regardless of C, except temp
  • If EQ eqn reversed, K = 1/k
  • When rxns +, xK
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35
Q

Changes in Pressure

A

EQ shifts to side that has less molecules

36
Q

Endothermic Reactions

A
  • Cooled = shift L
  • Heated = shift R
37
Q

Exothermic Reactions

A
  • Cooled = shift R
  • Heated = shift R
38
Q

Changing EQ Sys without Changing Position

A
  • Catalysts
  • Inert gases
  • Diff states
39
Q

Solubility

A

Amount of solute that dissolves in a solvent at a temp

40
Q

Molar Solubility is used to calculate

41
Q

Salt Ratios

A
  • 1:1 = s^2
  • 1:2 = 4s^3
  • 1:3 = 27s^4
42
Q

Trial Ion Product

A

Uses Q to find if precip will form

43
Q

Common Ion Effect

A

Decrease in solubility when same ion present

44
Q

Bronsted-Lowry Theory

A

Acid are donors, bases are acceptors

45
Q

Strong acid/base

A

Very weak conjugate

46
Q

Weak acid/base

A

Weak conjugate

47
Q

Very weak acid/base

A

Strong conjugate

48
Q

Weak A/B Ksp Value

49
Q

Salt is neutral if

A
  • Cation from grp 1 or 2
  • Anion is from a SA
50
Q

Salt is basic if

A

Anion is a Cb to WA

51
Q

Salt is acidic if

A

Cation is Ca to WB

52
Q

Metallic Oxides

53
Q

Non-metallic

54
Q

Orbitals

A

Cloud of probability for e

55
Q

Principal Quantum Number

A

Size & nrg for atomic orbital

56
Q

Secondary Quantum Number

A

Nrg sublvls (l = n-1)

57
Q

Magnetic Quantum Number

A

Orientation of orbital (-l to +l)

58
Q

Spin Quantum Number

A

Spin up or down (+/- 0.5)

59
Q

Pauli Exclusion Principle

A

No same quantum #s

60
Q

Aufbau Principle

A

lowest orbitals first

61
Q

Hund’s Rule

A

No pairing first

62
Q

Hybrid Orbital

A

Orbital formed from combination of diff orbitals

63
Q

Sigma Bonds

A

Orbitals overlap head to head

64
Q

Pi Bonds

A

Orbitals overlap side to side

65
Q

Covalent Bonds with Sigma and Pi Bonds

A
  • Single = sigma
  • Double = pi
  • Triple = sigma, pi, pi
66
Q

Oxidation Number Rules

A
  • F always -1
  • O2 usually -2, except peroxides = -1
67
Q

Oxidizing Agent

A

Gains e-, is reduced

68
Q

Reducing Agent

A

Loses e-, is oxidized

69
Q

Reactions happens if

A

OA is above RA

70
Q

Anode and Cathode Redox Reactions

A
  • Anode = oxidized
  • Cathode = reduced
71
Q

Ethers

A
  • Has O in the middle
  • +oxy
72
Q

Aldehyde

A
  • Has O2 at the end
  • +al
73
Q

Ketones

A
  • Has O2 in the middle
  • +one
74
Q

Carboxylic Acid

A
  • COOH
  • +oic acid
75
Q

Ester

A
  • COOH + OH
  • +oate for COOH chain
76
Q

Amine

77
Q

Amides

A
  • COOH + NH
  • +amide for O2 + N chain
78
Q

Types of Addition Reactions

A
  • Hydrogenation
  • Halogenation
  • Hydrohalogenation
  • Hydration
79
Q

Alcohols Reactions

A
  • Dehydrate into akenes
  • Oxidize into aldehyde/ketone
80
Q

Aldehydes and Ketones Reactions

A

Hydrogenation into 1 or 2nd alcohol

81
Q

Estertification

A

COOH + OH = ester

82
Q

Amine Condensation

A

Alkyl Halide + amine

83
Q

Amides Condensation

A

COOH + amine

84
Q

Organic Compound Hierarchy

A
  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
Q

Electron Configuration Exceptions

A
  • Cr: [Ar] 4s13d5
  • Cu: [Ar] 4s13d10
  • Ag: [Kr] 5s14d10
  • Au: [Xe] 6s14f145d10

SCH4U1 - Chemistry (6 decks)

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