5. Bonding

Question 1

DELETE

Answer 1

Question 2

Draw and name the shape.
Find the bond angle

Answer 2

Question 3

Draw and name the shape.
Find the bond angle

Answer 3

Question 4

Draw and name the shape.
Find the bond angle

Answer 4

Question 5

Draw and name the shape.
Find the bond angle

Answer 5

Question 6

Draw and name the shape.
Find the bond angle

Answer 6

Question 7

Draw and name the shape.
Find the bond angle

Answer 7

Question 8

Draw and name the shape.
Find the bond angle

Answer 8

89⁰, 119⁰

Question 9

Draw and name the shape.
Find the bond angle

Answer 9

Question 10

Draw and name the shape.
Find the bond angle

Answer 10

Question 11

Draw and name the shape.
Find the bond angle

Answer 11

Question 12

Draw and name the shape.
Find the bond angle

Answer 12

Question 13

Draw and name the shape.
Find the bond angle

Answer 13

Question 14

Formula for Nitrate

Answer 14

NO3⁻

Question 15

Formula for Nitrite

Answer 15

NO2⁻

Question 16

Formula for Hydrogencarbonate

Answer 16

HCO3⁻

Question 17

Formula for Chlorate(I)

Answer 17

ClO⁻

Question 18

Formula for Chlorate(V)

Answer 18

ClO3⁻

Question 19

Describe Metallic Bonding

Answer 19

• between 2 or more metals
• giant metallic lattice
• metallic → strong electrostatic attraction between positive metal ions and delocalised e-

Question 20

Describe Ionic Bonding

Answer 20

• between metal and non metal
• giant ionic lattice
• ionic → strong electrostatic attraction between oppositely charged ions

Question 21

Describe Covalent (Macromolecular) Bonding

Answer 21

• uses either Carbon or Silicon
• macromolecular structure
• covalent bonds between atoms

Question 22

Examples of Macromolecular

Answer 22

Diamond
- each C atom has 4 covalent bonds
- tetrahedral shape
- very high mpt, very strong
- non-conductor = no free (delocalised) e-

Graphite
- layered
- each 3 atom has 3 covalent bonds
- each C atoms has delocalised e-
- layers held together by weak intermolecular forces
- soft layers can slide over each other
- conductor = has delocalised e-
- high mpt

Question 23

Describe covalent (simple molecular) bonding

Answer 23

• Hydrogen bonding: H,F, H-N, H-O
• P.D.D: polar molecule
• I.D.D: non-polar molecular
• structure: simple molecular
• bodning: intermolecular (Hydrogen, P.D.D, I.D.D) forces between molecules

Question 24

Coordinate Bond Definition:

Answer 24

a shared pair of e- which have both come from the same atom

represented by an arrow coming from the atom that is sharing it e-.

is exactly like a normal covalent bond

Question 25

Rank the strength of repulsions between e- pairs:

Answer 25

- LP to LP > LP to BP > BP to BP - to minimise repulsion, e- pairs repel each other as much as possible - LP repel more than BP

Question 26

Electronegativity Definition:

Answer 26

the power of an atom to attract a pair of e- in a covalent bond

Question 27

Factors affecting electronegativity

Answer 27

- shielding - nuclear charge (proton number) - (atomic radius)

Question 28

How do you work out if a molecule is polar?

Answer 28

1. assymetrical 2. 1. - all atoms around the central atom are the same - lone pair 2. - 1 atom around the central atom is different - no lone pairs OR - >1 lone pair

Question 29

How do you work out if the molecule is non-polar?

Answer 29

- symmetrical - all atoms around central atom are the same - no lone pairs

Question 30

Name and decribe the type of bonding

Answer 30

Question 31

Name and decribe the type of bonding

Answer 31

Question 32

Name and decribe the type of bonding

Answer 32

Question 33

Name and decribe the type of bonding

Answer 33

Question 34

Name and decribe the type of bonding

Answer 34

Question 35

Name and decribe the type of bonding

Answer 35

Question 36

When does H bonding occur?

Answer 36

- strongest IMF - between a H atom (boded to an O/F/N) and a lone pair on a N/O/F atom

Question 37

How does H bonding arise?

Answer 37

- large difference in electronegativity between N/O/F and H atom - creates a dipole on the H-F/H-N/H-O bond - lone pair on N/O/F atom on 1 molecules strongly attracts a 𝝳+ H atom on a different molecule

Question 38

Draw H bonding between 2 NH3 atoms

Answer 38

Question 39

When does P.D.D occur?

Answer 39

- generally weaker than H bonding - occurs between polar (assymetrical molecules)

Question 40

How does P.D.D arise?

Answer 40

- difference in electronegativity leads to bond polarity - dipoles don't cancel and therfore molecule has an overall permanent dipole - attraction between 𝜹+ on one molecules and 𝜹- on another molecule

Question 41

Draw P.D.D forces between 2 SbCl3 molecules

Answer 41

Question 42

When does I.D.D occur?

Answer 42

- generally the weakest force, but can be stronger than both P.D.D and hydrogen bonding if the molecule is large - occurs between all molecules (as well as atoms of nobles gases) - most important for non-polar molecules (as they don't have any other IMFs)

Question 43

How does it arise?

Answer 43

RUTID - R: random Movement of e- in 1 molecules leads to ... - U: uneven distribution of e-, creating a ... - T: temporary dipole in 1 molecules (atom). This ... - I: induces a dipole in the neighbouring molecule (atom). - D: dipole attract

Question 44

How to draw it?

Answer 44

Question 45

Importance of H bonding:

Answer 45

1) ice: ice less dense than water bc the H bonds in ice hold the molecules further apart 2) proteins: proteins are held in their specific complex 3D shape by H bonds (secondary/tertiary structure) 3) DNA: 2 strands are held together by H bonds. strong enought to hold strands together but weak enough to allow strands to separate for DNA replication