3: Metals

Question 1

Features of the Metallic bonding model

Answer 1

Fixed and closely packed cations

Cations are surrounded by a ‘sea of delocalized electrons’

Held together by an electrostatic force of attraction, non-directionally (In all directions)

Question 2

Limitations of the Metallic bonding model

Answer 2

Doesn’t show metal’s magnetism/lack of magnetism

Doesn’t show each metals individual H.P and B.P

Doesn’t show variation in electrical conductivity

Question 3

Why do metals have high melting/boiling points?

Answer 3

‘Strong metallic bonding between cations and delocalised e- allow metals to keep their shape under high energy, hence the high melting/boiling point.’

Question 4

Why are metals ductile?

Answer 4

‘When a force is applied, the cations and the delocalised e- shift to prevent similarly charged particles from getting too close, repelling away, and breaking the metal

Question 5

How do metals conduct heat?

Answer 5

When metals absorb heat, kinetic energy of delocalised e- and cations increase (greater vibrations). This kinetic energy is transferred to nearby cations and e-.

Question 6

How can metals conduct electricity

Answer 6

Electrical conduct requires free moving charged particles (can’t just refer to electrons). Metals have a sea of delocalised electrons, allowing them to conduct electricity

Question 7

Metals are lustrous

Answer 7

Delocalized electrons on the surface of metals reflect light

Question 8

Trends in Metal reactivity

Answer 8

Reactivity of Transition metals
^
Reactivity of Group 2 metals
^
Reactivity of Group 1 metals

Question 9

Explain the Chemistry behind why reactivity of metals increases going down a group in the periodic table

Answer 9

First ionization energy is the energy required to lose a valence e- from an atom. Ionization energy decreases down a group because the amount of shells increases, increasing the atomic radius. Because of this, the electrostatic force of attraction becomes weaker, making valence electrons easier to remove.

Question 10

Metal reaction with Water

Answer 10

Metal + Water -> Metal Hydroxide + Hydrogen

Question 11

Metal reaction with Acids

Answer 11

Metal + Acid -> Ionic salt + Hydrogen gas

Question 12

Metal reaction with Oxygen

Answer 12

Metal + Oxygen -> Metal Oxide

Question 13

Linear economy

Answer 13

The product is used, then disposed

Question 14

Circular economy

Answer 14

Product is used, then recycled to be used again

Question 15

Metal recycling advantages

Answer 15

• Conserving natural resources
• Endless recycling
• Reduces landfill
• Reduces energy consumption
• Reduces greenhouse gas emissions
• Metallic properties aren’t degraded