Metallic Bonding Flashcards Preview

Chemistry - Miss Dales > Metallic Bonding > Flashcards

Flashcards in Metallic Bonding Deck (10):
1

Define: Delocalised

Free to move.

2

Define: Malleable

Bendy, can shape it.

3

Define: Ductile

Can draw it out into a line.

4

Electron charge.

Where are they found?

Negative

In the outer shell of atoms.

5

Metallic ion charge.

How're they formed?

Positive

A metal loses an electron.

6

Can you describe the structure?

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

 

A image thumb
7

How are they held together?

Strong electrostatic forces of attraction as the opposite charges attract.

8

What increases the bond strength?

Having more delocalised electrons.

9

What does the bond strength depend on?

(2 things)

  • 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.

10

Name some properties of metals.

(8 in total)

  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.