Bonding & Properties of Metallic & Ionic Lattices - Structure & Properties (2.1)

Question 1

What interactions do the properties of metallic, ionic & giant covalent structures depend on?

Answer 1

The strength & type of bonding between the atoms or ions

Question 2

What interactions do the properties of simple covalent molecules & (single) atoms depend on?

Answer 2

The strength & type of intermolecular force between molecules

Question 3

What happens when giant lattice structures melt?

Answer 3

When giant lattice structures melt, the bonds between the atoms/ions are broken

Question 4

Give two factors that affect the strength of electrostatic forces

Answer 4

Charge & radius

Question 5

How does the strength of a force relate to the amount of energy required to break the bond?

Answer 5

Stronger the force = More energy required to break the bond

Question 6

Compare group 1 & 2 elements in terms of bond strength & charge. How does this affect their melting points?

Answer 6

• G 1 elements form ions of +1 charge
• G 2 elements form ions of +2 charge
• The forces of attraction between 2+ ions & their electrons is stronger than 1+ ions & their electrons
• Therefore, G 2 elements have stronger metallic bonding & higher melting point

Question 7

Explain how atomic radius affects bond strength

Answer 7

• Strength of bond decreases as atomic radius becomes larger
• The positive nucleus is further from the negatively charged species (electron or ion) the electrostatic attraction is weaker

Question 8

Give the two factors that affect atomic radius

Answer 8

Nuclear charge

Shielding

Question 9

How does nuclear charge affect the atomic radius?

Answer 9

The nuclear charge pulls electrons towards the nucleus - so it decreases the radius

Question 10

How does shielding affect the atomic radius?

Answer 10

• Shielding is the repulsive charge between electrons
  (especially from electrons in lower energy levels - energy levels get closer in higher energy levels)
• Increasing shielding increases the radius

Question 11

State & explain the trends in nuclear charge across a period

Answer 11

Nuclear charge increases - more protons are added to the nucleus

Question 12

State & explain the trends in shielding across a period

Answer 12

Shielding is similar - you are filling he same outer energy level

Question 13

Explain how the atomic radius change across a period

Answer 13

• The outer electrons are pulled closer to the nucleus by the increased electrostatic attraction (nuclear charge increases)
• Shielding is constant so atomic radius decreases

Question 14

State the change in atomic radii down a group

Answer 14

Atomic radius increases down a group

Question 15

Explain the difference between atomic radii and their cations

Answer 15

• Nuclear charge stays the same & shielding decreases

- Therefore, cations are always smaller than their respective atoms

Question 16

Explain the difference between atomic radii and their anions

Answer 16

• Nuclear charge stays the same & shielding decreases

- Therefore, anions are always larger than their respective atoms