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Chemistry Edexcel A Level > Topic 2 Bonding & Structure > Flashcards

Topic 2 Bonding & Structure Flashcards

1
Q

What angle is linear?

A

180
No lone pair, furthest repel

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2
Q

What angle is V shape?

A

104.5
2 lone pairs

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3
Q

What angle is trigonal planar?

A

120
No lone pairs

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4
Q

What angle is trigonal pyramidal?

A

107
1 lone pair

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5
Q

What angle is tetrahedral?

A

109.5
No lone pairs

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6
Q

What angle is trigonal bypyrimidal?

A

5 bonds formed
90 in 2
120 in 3

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7
Q

What angle is hexagonal?

A

90 between every 2 bonds
180 between bottom ones
6 bonds in total

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8
Q

What is an ionic bond?

A

Strong electrostatic attraction between opposite charged ions

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9
Q

What is the ionic attraction affected by?

A

Ionic radius (smaller=stronger)
Ionic charge (higher=stronger)

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10
Q

Qualities of ionic bonds

A

High mp
Soluble in water
Poor electron conductivity when solid but good when molten
Brittle (bcs can slide over each other, same charge repel)

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11
Q

How are ionic bond qualities proven?

A

Electrolysis

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12
Q

What are covalent bonds? (2 marks)

A

Strong electrostatic attraction (1)
Between 2 nuclei and the share of pair of electrons (1)

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13
Q

What do σ bonds look like?

A

Overlap of s orbitals
2 O O overlapping
Or 1 s 1 p (O ∞ overlap)
Or ∞ ∞ overlap

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14
Q

What do π bonds look like?

A

8 8 overlap
2 p orbital overlapping sideways so 2 areas where electrons are shared

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15
Q

What is the definition of electronegativity?

A

Ability for an atom to attract bonded pair of electrons from covalent bonds

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16
Q

What is a dative covalent bond?

A

Empty orbital of one atom overlap with an orbital with lone pair
(Donating a lone pair to an empty orbital)

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17
Q

What are examples of dative covalent bonds? Give 2

A

NH4+ (N donates to H)
Al2Cl6 (Cl donates to Al)

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18
Q

When u see mp/bp what do u think of?

A

London forces
PDPD
H bonds

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19
Q

Why can’t S form H bonds?

A

Not electronegative enough, much less electronegative than O
, doesn’t form very polar bonds like F O N

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20
Q

The structural feature that graphene and graphite have in common is that the carbon atoms are arranged in…

A

Hexagonal rings within a layer

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21
Q

What is the bond angle in BF3?

A

120

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22
Q

What are the strongest interactions between molecules in solid boric acid? (H3BO3)

A

Hydrogen bonds

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23
Q

How to find out the succession ionisation energies and their groups?

A

Biggest jump
Eg from 2 to 3 then it must be a G2 element

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24
Q

How to determine isoelectronic ion size?

A

For atoms or ions that are isoelectronic, the number of protons determines the size. The greater the nuclear charge, the smaller the radius in a series of isoelectronic ions and atoms

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25
Ionic bonding is the strong electrostatic attraction between….
Cations and anions (There are NO delocalised e-s in ionic bonds!)
26
What does HCl exist at room temperature as?
Giant lattice of oppositely charged ions (Gas)
27
What are the bond angles within a layer of graphene and a layer of graphite?
All 120
28
How is a dative covalent bond formed in NH3BF3?
Lone pair donated from N BF3 accepts the lone pair and forms a full outer shell
29
What’s the bond angle and name when there is a lone pair and 3 bonds?
107 Trigonal pyramidal
30
What’s the bond angle and name when there are 4 bonds?
Tetrahedral 109.5
31
Why is the mp of silicon(IV) dioxide way higher than iodine when both of them are covalent bonded?
Silicon oxide is a giant structure so contains many strong covalent bonds (1) Iodine only has weak London forces (1) More **energy** is needed to break silicon dioxide
32
Why do both water and carbon dioxide have polar bonds but only water is a polar molecule? 4 marks
Oxygen is more electronegative than both H and C, so arrow points towards O So polar bonds are formed, O is delta negative, C and H are delta positive Water has V-shape, so vectors don’t cancel out CO2 has linear shape, vectors cancel
33
In terms of bonding and structure, why is the melting point of silicon way higher than chlorine when both are Period 3 elements?
Silicon: giant molecular, strong covalent bonds, lots of energy needed to break Chlorine: simple molecular, diatomic and has weak London Forces
34
Graphite vs graphene
Both hexagonal layer with C joined with 3 other C London forces hold graphene layers together and make graphite Unbonded Cs have delocalised electrons that are free to move
35
Describe structure of diamond
Each C joined with 4 other C by covalent bonds Regular Tetrahedral structure No free electrons Giant covalent lattice structure
36
Why is lots of energy needed to break CaCO3?
Because of strong bonds **within** the carbonate ion
37
Why is more energy required to break AlF than AlCl? (In terms of electronegativity) (6 marks)
- larger electronegativity difference between Al and F than Al and Cl - AlCl mostly simple covalent - AlF more polar - AlCl more weaker London forces/intermolecular - AlF is giant structure, strong electrostatic attraction between ions - more energy needed to break stronger bonds
38
What’s the only covalently bonded compound with a metal in it?
AlCl
39
What’s the order of strength of intermolecular forces?
H bonds > PDPD > London
40
Why is methanol and water ‘soluble in all proportions’?
Methanol forms H bonds with water At least 1 lone pair on oxygen atom at 180 degrees
41
What are 2 elements with special electronic configurations?
Copper and chromium
42
What is it mean by hydrogen bonds? 2 marks
Hydrogen atom forming evident bond in the same or different molecule With another atom (F,O or N) that is more electronegative than H
43
What is a metallic bond? 2 marks
Electrostatic attraction between metal cation and delocalised electrons (outer shell electrons)
44
Why is magnesium a better electric conductor than sodium?
Mg is a smaller ion and has 1 extra delocalised electron than Na (group 2 vs group 1)
45
Why is nitrogen much less reactive than carbon monoxide and hydrogen cyanide? (Given they are isoelectronic) (1 mark)
N has triple bonds with diatomic N, much stronger than C=O, C (triple) N, C-H N2 also non polar, while the other two are polar
46
Why is sodium chloride soluble in water? 3 marks
- energy to overcome electrostatic attraction between sodium cation and chloride anion - lattice breaks down and ions are separated - energy supplied by hydration of ions by water molecules
47
What structure is sodium chloride?
Lattice ionic structure
48
What is it meant by a polar bond? How does polarity arise?
- there is a charge separation between molecules of a bond , one is δ+ and one is δ- - when bond formation and one molecule is more electronegative than the other - electron cloud produce higher electron density towards electronegative element
49
What is a Hydrogen bond like?
Very polarised high charge density
50
Why does melting point in G2 decrease down?
Ionic radius increases so metallic bond becomes weaker, making it easier for them to slide past each other Weaker efoa with e-s so easier to break
51
Why does electronegativity decrease down G7?
the number of electron shells increases down, so larger atomic radius. Hence weaker attraction for electrons, making it harder to attract them, hence lower electronegativity.
52
Predict state of astatine in standard conditions and why.
Solid Because of increasing London forces down G7 (NOT mp/bp!)
53
Why is ice less dense than water in terms of hydrogen bonds? (2 marks)
- more space between molecules - due to 3D lattice structure in ice - H bonds are stronger than covalent bonds
54
Which element has the highest bp in Period 3? (1 mark)
Si
55
What does white phosphorus consist of?
small molecules
56
What cation would be most polarising?
High charge small radius
57
Why is the electrical conductivity of pure silicon very low?
Because there are no free delocalised electrons all of Si's free electrons are used to form covalent bonds
58
Explain the high melting temperature of Silicon in terms of bonding. (2 marks)
Lot of strong covalent bonds (1) needed to be broken by lots of energy to overcome (1)
59
How to work out if an ion has the largest ionic radius in a MCQ?
least num of proton : electron ratio so least attraction
60
How to work out if an ion has the smallest ionic radius in a MCQ?
most num of proton : electron ratio so most attraction
61
In terms of orbital overlap, a double bond is
a σ and π bond
62
What is the C-C-C bond angle in a cycloalkane?
109.5°
63
Which Intermolecular Force is the strongest?
Hydrogen bonds!!!
64
Deduce 2 possible reasons why there are 2 widely different values for the compressive strength of graphite. (2.3 and 15.3 GPa) (2 marks)
- due to weaker London forces (between layers) - strong C-C bonds within layers (in the one with higher GPa)
65
How do you explain sodium sulfide dissolving in water?
**Energy released** when sodium ions and sulfide ions are **hydrated** > energy required to **break** the attraction between sodium ions and sulfide ions
66
Why does HCl (g) not conduct but HCl (aq) conduct electricity?
Covalent bond in HCl (g) changes to ionic bond in aqueous solution
67
What is **observed** when HCl is added to Na2CO3? (2 marks)
Solid dissolves Effervescence
68
Explain why Iron(III) ions form pale green solution but zinc ions form colourless solution. (2 marks)
Zinc ions have full orbitals So no e-s promoted / move between 3D orbitals
69
State what it is meant by homologous series. (1)
Series of compounds with same functional group AND same general formula
70
Why does sulfur not follow the increasing ionisation energy trend across Period 3 fro Al? (2 marks)
- it has 2 electrons in the 3p orbital - they repel each other and lowers IE
71
What is the bond angle when there is one lone pair and two bonded pairs? What is the name?
bent 117.5°
72
73
Explain why a nitrogen atom is larger than an oxygen atom. (2 marks)
- they have the same shielding - nitrogen has one less proton - so nuclear attraction is weaker
74
Explain why P can form PCl5 but N cannot form NCl5. (1 mark)
P can accommodate more than 8 electrons in its orbital (3d) N cannot has it does not have a d orbital
75
What is the bonding of NO3^- ?
One double bond One single One dative
76
What is the bonding of SO4^2- or CrO4^2-?
2 double bonds 2 single bonds 2 O have an external e- each to make 2- charge
77
How is CO bonded?
C and O each has 1 lone pair Double covalent, 1 dative from O

Chemistry Edexcel A Level (24 decks)

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