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A - Level Chemistry > C6 Shapes Of Molecules And Intermolecular Forces > Flashcards

C6 Shapes Of Molecules And Intermolecular Forces Flashcards

1
Q

What are the 3 main types of chemical bonds

A

Ionic

Covalent

Metallic

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2
Q

Define ionic bonding

A

Electrostatic attraction between pos and neg ions

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3
Q

Give an example of a ironically bonded substance

A

NaCl

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4
Q

Define covalent bonding

A

Electrostatic attraction between a shared pair of electrons and the nuclei

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5
Q

Define metallic bonding

A

Electrostatic attraction between the pos metal ions and sea of delocalised electrons

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6
Q

Electrons in which shell are represented in dot and cross diagrams

A

The outer shell

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7
Q

Why does giant ionic lattices conduct electricity when liquid but not when solid

A

In solid state, ions are in fixed positions and thus cannot move.

When they’re in liquid state, ions are mobile and this can freely carry the charge

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8
Q

Giant ionic lattices have high or low MP and BP?

A

High MP & BP

Large amount of energy is required to overcome the electrostatic bonds

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9
Q

In what type of solvents do ionic lattices dissolve

A

Polar solvents

E.g. water

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10
Q

What are ionic compounds soluble in water

A

Water has polar bond

H atoms have delta pos charge and O atoms have delta neg charge

These charges are able to attract charged ions

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11
Q

What is it called when atoms are bonded by a single pair of shared electrons

A

Single bond

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12
Q

How many covalent bonds does C form

A

4

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13
Q

How many CBs does Oxygen form

A

2

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14
Q

What is a lone pair

A

Electrons in the outer shell that are not involved in the bonding

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15
Q

What is formed when atoms share 2 pairs of electrons

A

Double bond

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16
Q

What is formed when atoms share 3 pairs of electrons

A

Triple bond

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17
Q

What is average bond enthalpy

A

Measure of average energy needed to break the bond

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18
Q

What is a dative CB

A

A bond where both of the shared electrons are supplied by one atom

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19
Q

How are oxonium ions formed

A

Formed when acid is added to water, H3O+

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20
Q

What does expansion of the octet mean

A

When a bonded atom has more than 8 electrons in the outer shell

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21
Q

What are the types of covalent structure

A

Simple molecular lattice

Giant covalent lattice

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22
Q

Describe the bonding in simple molecular structures

A

Atoms within the same molecule are held by strong CBs and different molecules are held by weak IMFs

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23
Q

Why do simple molecular structures have low MP and BP

A

Small amount of energy is enough to overcome the IMFs

24
Q

Can simple molecular structures conduct electricity

A

No

They are non conductors

25
Why do simple molecular structures not conduct electricity
Have no free charged particles to move around
26
Simple molecular structures dissolve in what type of solvent
Non polar solvents
27
Give examples of giant covalent structures
Diamond Graphite Silicon dioxide, SiO2
28
List some properties of giant covalent structures
High MP and BP Non conductors of electricity, except graphite Insoluble in polar and non polar solvents
29
How does graphite conduct electricity
Delocalised electrons present between the layers are able to move freely carrying the charge
30
Why do giant covalent structures have high MPs and BPs
Strong CBs within the molecules need to be broken which requires a lot of energy
31
What does the shape of a molecule depend on
Number of electron pairs in the outer shell Number of these electrons which are bonded and lone pairs
32
What is the shape and bond angle in a shape with 2 BPs and 0 LPs
Linear 180*
33
What is the shape and bond angle in a shape with 3 BPs and 0 LPs
Trigonal planar 120*
34
What is the shape and bond angle in a shape with 4 BPs and 0 LPs
Tetrahedral 109.5*
35
What is the shape and bond angle in a shape with 5 BPs and 0 LPs
Trigonal bipyramid 90* and 120*
36
What is the shape and bond angle in a shape with 6 BPs and 0 LPs
Octahedral 90*
37
What is the shape and bond angle in a shape with 3 BPs and 1 LPs
Pyramidal 107*
38
What is the shape and bond angle in a shape with 2 BPs and 2 LPs
Non-linear 104.5*
39
By how many degrees does each lone pair reduce the bond angle
2.5*
40
Define electronegativity
The ability of an atom to attract the pair of electrons (the electron density) in a covalent bond
41
In which direction of the periodic table does electronegativity increase
Top right, towards fluorine
42
What does it mean when the bond is non-polar
The electrons in the bond are evenly distributed
43
What’s the most electronegative element
Fluorine
44
How is a polar bond formed
Bonding atoms have different electronegativities
45
Why is water polar, but CO2 is non-polar
CO2 is symmetrical molecule, so there’s no overall dipole
46
What’s meant by IMF
Attractive force between neighbouring molecules
47
What are the 2 types of IMFs
Hydrogen bonding Van der Waals’ forces
48
What is the strongest type of IMF
Hydrogen bonding
49
What are the 2 interactions that can be referred as Van der Waals’ forces
Permanent dipole - induced dipole interaction Permanent dipole - permanent dipole interaction
50
Describe permanent dipole -induced dipole interactions
When a molecule with a permanent dipole is close to other non-polar molecules it causes the non-polar molecule to become slightly polar leading to attraction
51
Describe permanence dipole- permanent dipole interactions
Some molecules with polar bonds have permanent dipoles —> forces of attraction between those dipoles and those of neighbouring molecules
52
Describe London forces
London forces are caused by random movements of electrons This leads to instantaneous dipoles Instantaneous dipole induces a dipole in nearby molecules Induced dipoles attract one another
53
Are LFs greater in smaller or larger molecules
Larger due to more electrons
54
Does BP increase or decrease down the noble gas group? Why?
BP increases As number of electrons increases and hence strength of LFs also increases
55
What conditions are needed for hydrogen bonding to occur
O-H, N-H or F-H bond Lone pair of electrons on O, F, N because O, N and F are highly electronegative, H nucleus is left exposed Strong force of attraction between H nucleus and lone pair of electrons on O, N, F
56
Why is ice less dense than liquid water
In ice, water molecules are arranged in an orderly pattern. It has an open lattice with hydrogen bonds In water, the lattice is collapsed and the molecules are closer together
57
Why does water have a MP and BP higher than expected
Hydrogen bonds are stronger than other IMFs so extra strength is required to overcome the forces

A - Level Chemistry (40 decks)

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