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Y12 Organic Chemistry > Bonding > Flashcards

Bonding Flashcards

(78 cards)

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1
Q

Ionic Bond

A

Electrostatic attraction between oppositely charged ions.

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2
Q

Melting point for ionic compounds

A

High - strong electrostatic attraction between oppositely charged ions

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3
Q

Ionic bonding is stronger when…

A

Ions are smaller and/or have higher charges. (A higher charge density)

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4
Q

Covalent Bond

A

Shared pair of electrons

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5
Q

Dative covalent bond

A

When the shared pair of electrons both come from one of the bonding atoms. Also called co-ordinate bonding.

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6
Q

Metallic bonding

A

electrostatic force of attraction between cations and a sea of delocalised electrons

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7
Q

Factors that affect strength of metallic bond

A

Number of protons (more = stronger), number of delocalised electrons (more = stronger), size of ion (smaller = stronger)

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8
Q

4 crystal structures are…

A

ionic, simple molecular, macromolecular and metallic

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9
Q

conductivity of ionic compounds

A

poor when solid - ions can’t move. Higher when molten or dissolved - ions free to move

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10
Q

boiling points of molecular compounds

A

low - weak intermolecular forces between molecules (Van der Waals)

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11
Q

melting point of macromolecular compounds

A

high - many strong covalent bonds to break

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12
Q

melting point of metallic substances

A

high - strong electrostatic forces of attraction between cations and delocalised electrons

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13
Q

Conductivity of molecular substances

A

Poor - no charged particles

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14
Q

Conductivity of macromolecular

A

Diamond and silica - poor. Not electrons or ions.

Graphite - good as delocalised electrons able to move between layers

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15
Q

Conductivity of metals

A

Good - delocalised electrons able to move

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16
Q

Shape of molecule with 2 bp, 0 lp

A

linear 180 angles

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17
Q

Shape of molecule with 3 bp, 0 lp

A

trigonal planar, 120 angles

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18
Q

Shape of molecule with 4 bp, 0 lp

A

tetrahedral, 109.5 angles

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19
Q

Shape of molecule with 3 bp, 1 lp

A

trigonal pyramidal, 107 angles

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20
Q

Shape of molecule with 2 bp, 2 lp

A

V shape or bent. 104.5 angles

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21
Q

Shape of molecule with 5 bp, 0 lp

A

trigonal bypyramidal, 120 and 90 angles

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22
Q

Shape of molecule with 5 bp, 1 lp

A

See-saw

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23
Q

Shape of molecule with 6 bp, 0 lp

A

Octahedral 90 angles

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24
Q

How to explain shape

A
  1. State number of bonding pairs and lone pairs.
  2. State that electron pairs repel to get as far apart as possible
    3a. If no lone pairs state that electron pairs repel equally
    3b. If there are lone pairs state that lone pairs repel more than bonding pairs
  3. State shape and bond angle
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25
Shape of molecule with 4 bp, 2 lp
Square planar 90 angles
26
Shape of molecule with 5 bp, 1 lp
Square based pyramid
27
How to calculate number of electron pairs
Group of central atom + number of electrons from bonding atoms +/- electrons from charge = total number of electrons. Divide by 2 = number of pairs. Work out whether they are bonding or lone pairs
28
Shape CO2
linear 180 angles
29
Shape CS2
linear 180 angles
30
Shape HCN
linear 180 angles
31
Shape BeF2
linear 180 angles
32
Shape BF3
Trigonal planar, 120 angles
33
AlCl3
Trigonal planar, 120 angles
34
SO3
Trigonal planar, 120 angles
35
NO3 -
Trigonal planar, 120 angles
36
CO3 2-
Trigonal planar, 120 angles
37
SiCl4
Tetrahedral, 109.5 angles
38
CH4
Tetrahedral, 109.5 angles
39
NH4+
Tetrahedral, 109.5 angles
40
PF3
Trigonal planar, 107 angles
41
NH3
Trigonal planar, 107 angles
42
H30 +
Trigonal planar, 107 angles
43
H2O
Bent/ V-shape 104.5
44
OCl2
Bent/ V-shape 104.5
45
H2S
Bent/ V-shape 104.5
46
OF2
Bent/ V-shape 104.5
47
SCl2
Bent/ V-shape 104.5
48
PF5
Trigonal bypyramidal, 120 & 90
49
PCl5
Trigonal bypyramidal, 120 & 90
50
SF6
octahedral, 90
51
XeF4
Square planar, 90
52
BrF5
Square pyramid, 89
53
I3 -
Linear, 180
54
ClF3
T shape, 89
55
SF4
see saw, 119 & 89
56
IF4 +
see saw, 119 & 89
57
Electronegativity
Ability of an atom to attract a pair of electrons in a covalent bond
58
How electronegativity changes across a period
increases - more protons, same number of shells and shielding so easier to attract incoming pair of electrons
59
How electronegativity changes down a group
decreases - more protons but greater distance to outer shell so less easy to attract an incoming pair of electrons
60
Effect of large electronegativity difference between elements
perfect ionic compound
61
Effect of small difference in electronegativity between elements
purely covalent compound
62
Effect of some difference in electronegativity between elements
Polar bond or ionic bond with covalent character
63
Polar bond
covalent bond with an unequal distribution of electrons in the bond. This causes a dipole with partially charged atoms
64
Non-polar molecule
A symmetric molecule with all identical bonds and no lone pairs. Individual dipoles cancel out.
65
Polar molecules
Asymmetric molecules with at least one polar bond
66
3 types of intermolecular force in order of strength
weakest: van der Waals' forces, permanent dipole-dipole, strongest: hydrogen bond
67
How Van der Waals' forces form
Electrons move constantly and randomly in any molecule. A temporary, instantaneous dipole can occur. This induces a dipole in a neighbouring molecule forming an attraction
68
Main factors affecting the size of Van der Waals.
More electrons and larger surface area of a molecule increases the VdWs so boiling points are higher
69
Trend in bp down group 7
Larger molecules with more electrons so greater temporary and induced dipoles therefore stronger attraction between molecules so higher bp
70
Trend in bp in alkanes
Longer alkanes have more electrons so have greater VdWs between molecules. Less branched alkanes have a greater surface area of contact between molecules so also have stronger VdWs between molecules and so have higher bps
71
Cause of permanent dipole-dipole forces
Occur between polar molecules with a dipole. Stronger than VdWs so compounds have a higher bp
72
Explanation of hydrogen bonding
Occurs in compounds with a H atom attached to very electronegative F, O or N. The large difference of electronegativity creates a partial charge difference with d+ H and d- FON. An attraction is formed between the H and a lone pair on the FON
73
3 marks for drawing a hydrogen bond
Partial charges shown, All lone pairs shown Attraction shown between lone pair on FON and H attached to a FON
74
Requirements for hydrogen bonding
Hydrogen atom attached to a F,O or N. and a FON on another molecule
75
Trend in bp of group 4 hydrides - CH4, SiH4, GeH4, SnH4
Increases down group as molecules become larger so have more electrons and stronger VdWs between molecules
76
Trend in bp of group 5,6 and 7 hydrides
Generally increases down the group as molecules become larger and have stronger VdWs. HF, H2O and NH3 have unexpectedly high bp because they can form H bonds as well as VdWs
77
What is unusual about ice?
It is less dense than liquid water. The H bonding between molecules holds them further apart from each other in a regular arrangement
78
Diagram of iodine
herringbone structure of I2 molecules

Y12 Organic Chemistry (3 decks)

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