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IB Chemistry > Chapter 4 - Bonding > Flashcards

Chapter 4 - Bonding Flashcards

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0
Q

Charges of Ions

A

Most transition metals are 2+ (except Ag 1+)

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1
Q

Ionic Bond

A

The electrostatic attraction between oppositely charged ions.

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2
Q

Exceptions to Charges

A

Fe (+2, +3)
Cu (+1, +2)
Pb (+4, +2)

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3
Q

Nitrate

A

NO3 -1

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4
Q

Sulfate

A

SO4 -2

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5
Q

Hydroxide

A

OH -

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6
Q

Carbonate

A

CO3 -2

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7
Q

Phosphate

A

PO4 -3

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8
Q

Ammonium

A

NH4 +1

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9
Q

Lewis Dot Diagram

A

A representation of the valence electrons and their behaviour.

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10
Q

Covalent Bonds

A

Occur by the mutual attraction of nuclei for the shared electrons.

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11
Q

Naming Covalent Bonds

A 
1 - Mono
2 - Di
3 - Tri
4 - Tetra
5 - Penta
6 - Hexa
7 - Septa
8 - Octa
9 - Nona
10 - Deca
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12
Q

Structural Diagram

A

Lewis diagram but only show bonded pairs.

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13
Q

Length and Strength

A

Decreasing length = Increasing strength

Single bond —> Double bond —> Triple bond

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14
Q

Rulebreakers

A

Be only needs 4 valence electrons.

B only needs 6 valence electrons.

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15
Q

Dative Bonding

A

Anytime the central atom has more bonds than normal, the central atom is doing all the sharing.

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16
Q

Macromolecules

A

Large/giant covalent molecules (network solids)

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17
Q

VSEPR

A

Valence Shell Electron Pair Repulsion

  1. Valence electrons act in pairs
  2. Pairs repel
  3. Unbonded pairs repel more
  4. Electrons in multiple bonds act as a single “charge centre”
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18
Q

4 Bonded Pairs

A

Electrons: Tetrahedral

Atoms: Tetrahedral

19
Q

4 Pairs (3 bonded)

A

Electrons: Tetrahedral

Atoms: Trigonal Pyramid

20
Q

4 Pairs (2 bonded)

A

Electrons: Tetrahedral

Atoms: Bent

21
Q

4 Pairs (1 bonded)

A

Electrons: Tetrahedral

Atoms: Linear

22
Q

2 Charge Centres

A

Electrons: Linear

Atoms: Linear

23
Q

3 Pairs

A

Electrons: Flat Triangle

Atoms: Planear Triangle

24
Q

3 Charge Centres

A

Electrons: Flat Triangle
Atoms: Bent

25
Q

Polarity

A

HIGH: 1.7-3.3 (ionic bonds)
MODERATE: 0.5-1.7 (polar bonds)
LOW: 0-0.5 (diatomic bonds)

26
Q

Bond Dipole vs Molecular Dipole

A

Bond dipoles add to give you the overall molecular dipole.

27
Q

Bonding Capacity

A 
H - 1
Cl (halogens) 1
O, S - 2
N, P - 3
C - 4
28
Q

Intermolecular Bonds

A

Bonds between molecules are weaker than bonds in the molecule.

The bond is broken when a substance melts, boils, evaporates or dissolves.

The weaker the bond, the lower the bp, mp, and more volatile.

29
Q

Van der Waals’

A

Fluctuating dipole bond.
The bigger the molecule, the more likely to happen.
Present in non-polar substances.
(weakest)

30
Q

Dipole-Dipole

A

Dipole bond between 2 polar substances (stronger)

31
Q

H-Bonding

A

Occurs when H is bonded to O, N, F (strongest)

32
Q

SiO2

A

Silicon dioxide

  • Very high melting
33
Q

Graphite

A

Sheets of carbon atoms (size of sheets determines hardness)

Conducts electricity because double bond can move.

34
Q

Diamond

A

Very hard, high melting, doesn’t conduct.

35
Q

Bucky Ball (C-60)

A

Closed cage of 60 carbons (12 pentagons, 20 hexagons)

Good conductor

Forms crystals

36
Q

Metallic Bonding

A

The electrostatic attraction between a lattice of positive ions and delicacies electrons.

37
Q

Metallic Ions

A 
Good conductors (delocalized electrons are mobile)
Very malleable (delocalized electrons move non-directionally)
38
Q

Trends in Melting Point

A

Na - Al are metallic bonds (strong)
Si is a giant covalent bond (very strong)
P4 - Ar are Van der Waals’ (weak)

39
Q

Bond Strength

A

VDW < Dipole-Dipole < H-bonding < Metallic < Ionic/Covalent

40
Q

Conductivity

A

Depends on ability to have free moving charges (either electrons or ions)

41
Q

Solubility

A

Depends on ability to bind with solvent (“like dissolves like”)

42
Q

Physical Properties: Ionic

A

Very high melting point
Can conduct in liquid/aqueous, but not solid
Very soluble in water because ions are attracted to different ends of water molecules

43
Q

Physical Properties: Covalent (VDW, DD, H-bond)

A

Very low melting point
Poor conductors
Can bond with water if polar or H-bond

44
Q

Physical Properties: Covalent

A 
Very high melting point
Not good conductor (diamond) unless bonds can move (graphite) 
Not soluble (non-polar)
45
Q

Physical Properties: Metallic

A 
Greater the charge, higher the melting point
Good conductor (liquid, solid)
Not soluble

IB Chemistry (2 decks)

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