2.2.2

Question 1

What is ionic bonding

Answer 1

The electrostatic forces of attraction between cations and anions

Question 2

What is the structure of ionic bonding

Answer 2

Giant ionic lattice

Question 3

What are the properties of giant ionic lattices

Answer 3

High mp/ bp
Soluble
Conducts electricity (when molten)

Question 4

Why does a giant ionic lattice conduct electricity when molten but not when solid

Answer 4

When solid, the ions are in fixed positions so they can’t move but when molten, the ions are free to move so they can carry the charge

Question 5

Why does a giant ionic lattice have a high melting point

Answer 5

The strong electrostatic forces of attraction require a lot of energy to overcome

Question 6

Why are giant ionic lattices soluble in water

Answer 6

Water is polar which means that the H+ and O- attract the charged cations and anions. The solubility depends on the charge of the ions as the higher charges mean there is a greater force of attraction

Question 7

What is covalent bonding

Answer 7

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

Question 8

What are the properties of simple molecular structures

Answer 8

Low mp/ bp
Doesn’t conduct electricity

Question 9

Which elements always follow the octet rule for covalent bonding

Answer 9

Carbon
Nitrogen
Oxygen
Fluorine

Question 10

Why can graphite conduct electricity

Answer 10

It only forms 3 covalent bonds from each carbon so there are demoralised electrons between the layers, which can carry the charge

Question 11

Why do giant covalent networks have high mp/ bp

Answer 11

Strong covalent bonds require a lot of energy to break

Question 12

Why doesn’t diamond conduct electricity

Answer 12

It forms 4 covalent bonds so there are no delocalised electrons to carry the charge

Question 13

What are 4 examples of giant covalent structures

Answer 13

Diamond
Graphite
Graphene
Silicon dioxide

Question 14

What is the shape and bond angle in a shape with 2 bonded and 0 lone pairs

Answer 14

Linear
180°

Question 15

What is the shape and bond angle in a shape with 3 bonded and 0 lone pairs

Answer 15

Trigonal planar
120°

Question 16

What is the shape and bond angle in a shape with 2 bonded and 1 lone pair

Answer 16

Non-linear
117.5°

Question 17

What is the shape and bond angle in a shape with 4 bonded and 0 lone pairs

Answer 17

Tetrahedral
109.5°

Question 18

What is the shape and bond angle in a shape with 5 bonded and 0 lone pairs

Answer 18

Trigonal bipyramidal
90° and 120°

Question 19

What is the shape and bond angle in a shape with 6 bonded and 0 lone pairs

Answer 19

Octahedral
90° and 180°

Question 20

What is the shape and bond angle in a shape with 3 bonded and 1 lone pair

Answer 20

Trigonal pyramidal
107°

Question 21

What is the shape and bond angle in a shape with 2 bonded and 2 lone pairs

Answer 21

Non-linear
104.5

Question 22

How does each lone pair change the bond angle

Answer 22

It decreases it by 2.5°

Question 23

How would you show single, double, triple, and dative covalent bonds in displayed formula

Answer 23

C–C
C=C
C≡C
C<–C

Question 24

What is metallic bonding

Answer 24

Electrostatic FOA between positive metal ions and at delocalised electrons

Question 25

What is average bond enthalpy

Answer 25

Measure of average energy needed to break a bond

Question 26

What is electronegativity

Answer 26

The ability of an atom to attract a pair of electrons in a covalent bond

Question 27

What is the most electronegative element

Answer 27

Fluorine

Question 28

What are the types of intermolecular forces

Answer 28

London dispersion forces Permanent dipole– Permanent dipole interactions Hydrogen bonding

Question 29

Which is the strongest type of IMF

Answer 29

Hydrogen bonding

Question 30

What are London dispersion forces

Answer 30

Caused by random movement of electrons Leads to instantaneous dipole which induces a dipole in a nearby molecule Induced dipole attract each other

Question 31

Why are LDFs greater in larger molecules

Answer 31

There are more electrons

Question 32

Which molecules have to be involved with hydrogen bonding

Answer 32

O–H N–H F–H

Question 33

Why is ice less dense than water

Answer 33

In ice it forms more hydrogen bonds (up to 4) so it has an open lattice structure In water there are fewer hydrogen bonds (2-3) so the bonds break more frequently

Question 34

Why does water have a high surface tension

Answer 34

The strong hydrogen bonds between molecules

Question 35

Why does water have a high mp/ bp

Answer 35

The hydrogen bonds are stronger than other IMF so more energy is required to break bonds