Bonding

Question 1

Describe the properties of metals

Answer 1

• High MP: Charge density, atomic radius
• Conducts electricity: sea of delocalised electrons carry charge through structure
• Malleable/ductile: layers of positive ions that can slide over each other

Question 2

What are the strongest to weakest intermolecular forces?

Answer 2

1. Hydrogen Bonds
2. Permanent dipole-dipole forces
3. VDW’s forces

Question 3

Define electronegativity

Answer 3

Electronegativity is the power of an atom to attract the pair of electrons in a covalent bond

Question 4

Difference between polar and non-polar molecules

Answer 4

polar: non-symmetric, partial charges
non-polar: opposite

Question 5

Factors that affect electronegativity + explain why

Answer 5

1. nuclear charge- increase = EN increase
2. atomic radius- increase = EN decrease
3. electron shielding- increase = EN decrease

(EX ANSWER: As nuclear charge increases, electronegativity increases/ there is a greater attraction between the nucleus and the pair of electrons in the bond)

Question 6

Simple molecular properties

Answer 6

• weak intermolecular forces + simple molecular structure
• low mp as little energy required to break weak intermolecular forces
• do not conduct electricity

Question 7

EXAM Q.
Explain why nickel is ductile (can be stretched into wires) 1 mark

Answer 7

it has layers (of positive ions) which can slide over each other

Question 9

What is the strongest intermolecular force in HF a Dow does it arise?

Answer 9

HF has hydrogen bonds this is because it is between hydrogen and fluorine which is one of the three elements that can create hydrogen bounds when bonded with hydrogen