Ionic bonding, metallic bonding, and structure (C3)

Question 1

What is ionic bonding?

Answer 1

When metal atoms react with non-metal atoms they transfer electrons to the non-metal atom (instead of sharing them).

Question 2

What charges do the atoms have after Ionic bonding?

Answer 2

Metal atoms lose electrons to become positive ions. non-metal atoms gain electrons to become negative ions

Question 3

What is the structure of metals?

Answer 3

The atoms that make up metals form layers. The Electrons in the outer shells of atoms are delocalized this means they are three to move throughout the whole structure. The positive metal ions are then attracted to these delocalized electrons by the electrostatic force of attraction

Question 4

What is the hardness of pure metals?

Answer 4

Pure metals are malleable because the layers can slide over each other.

Question 5

What is the conductivity of pure metals?

Answer 5

Metals are good conductors of electricity and thermal energy because delocalized electrons are free to move through the whole structure

Question 6

What are the melting and boiling points of pure metals?

Answer 6

Metals have high melting and boiling points because the electrostatic force of attraction between metal ions and delocalized electrons is strong so lots of energy is needed to break it

Question 7

What is an alloy?

Answer 7

The combination of different metal atoms

Question 8

What are some properties of alloys?

Answer 8

Adding atoms of different elements can make the resulting mixture harder because the new atoms will be a different size to the pure metal’s atoms. This will disturb the regular arrangement of the layers, preventing them from sliding over each other