Chem - Bond/structure - Metals

Question 1

Type of structure

Answer 1

metallic Metal-Metal

Question 2

Electrical conductivity

Answer 2

Delocalised electrons
Free to move in solid and liquid

Question 3

particles and type of bond

Answer 3

Atoms Ions and delocalised electrons
Metallic bond

Question 4

Melting and boiling point

Answer 4

High
Strong metallic bonds

Question 5

Other properties may need to account for

Answer 5

Hard
Malleable and ductile
- metallic bond meaning that the attractions between ions and delocalised electrons is non directional and will still operate even if the metal is deformed as atoms can move past each other

Question 6

Why are metals have high melting and boiling points

Answer 6

As there strong attraction to overcome between valence electrons and the nuclei of neighbouring atoms.

Question 7

Why are metals not soluble in water

Answer 7

Because the metallic bonds are too strong to be broken by the attraction to the water molecules

Question 8

How can metals conduct electricity

Answer 8

Metal atoms are held together in a 3D lattice by metallic bonding, in which loosely held valence electrons are attracted to the neighbouring ions. The valence electrons are free to move throughout the structure in both solid and liquid state