Metallic Bonding

Question 1

Define: Delocalised

Answer 1

Free to move.

Question 2

Define: Malleable

Answer 2

Bendy, can shape it.

Question 3

Define: Ductile

Answer 3

Can draw it out into a line.

Question 4

Electron charge.

Where are they found?

Answer 4

Negative

In the outer shell of atoms.

Question 5

Metallic ion charge.

How’re they formed?

Answer 5

Positive

A metal loses an electron.

Question 6

Can you describe the structure?

Answer 6

Positive metal ions in a sea of negative, delocalised electrons.

Question 7

How are they held together?

Answer 7

Strong electrostatic forces of attraction as the opposite charges attract.

Question 8

What increases the bond strength?

Answer 8

Having more delocalised electrons.

Question 9

What does the bond strength depend on?

(2 things)

Answer 9

• The charge of the ion and so the free electron number.

Example: Na+ Mg2+ Al3+

Stronger——–>

• Size of the ion (shielding)

Smaller = delocalsied electrons are closer to the nucleus, so feel the pull of the nucleus (nuclear charge) more. So have a stronger bond.

Question 10

Name some properties of metals.

(8 in total)

Answer 10

1. Malleable - layers can slide
2. Sonourous
3. Solid at room temperature (not mercury)
4. Conduct heat and electricity - delocalised electrons.
5. Ductile (copper) - layers can slide.
6. High boiling and melting point - strong electrostatic forces.
7. Hard - regular arrangement.
8. Strong - strong electrostatic forces.