Unit 1 Section 3: Bonding

Question 1

What is the ionic formula of sulfate?

Answer 1

SO4^2-

Question 2

Ionic formula for hydroxide?

Answer 2

OH^-

Question 3

Ionic formula for Nitrate?

Answer 3

NO3^-

Question 4

Ionic formula for carbonate?

Answer 4

CO3^2-

Question 5

Ionic formula for ammonium?

Answer 5

NH4^+

Question 6

Sodium forms ionic bonds with chlorine.

a) Give the formula of the compound formed.
b) Describe the formation of an ionic bond between sodium and chlorine atoms.

Answer 6

a) NaCl
b) Sodium loses and electron to form a sodium ion (Na^+). Chlorine loses an electron to form a chloride ion (Cl^-). Electrostatic attraction holds the positive and negative ions together - this is an ionic bond.

Question 7

What is the structure of sodium chloride? Draw it out.

Answer 7

Giant ionic lattice

Question 8

Describe 3 physical properties you would expect an ionic compound to have.

Answer 8

1. Electrical conductivity when molten or dissolved
2. High melting points
3. Will dissolve in water

Question 9

Why do ionic compounds conduct electricity when molten and dissolved, but not solid?

Answer 9

Ions in liquid are free to move and carry charge throughout the structure.
In a solid they are fixed in position by strong ionic bonds

Question 10

Why do ionic compounds have high melting points?

Answer 10

Giant ionic lattices held together by strong electrostatic forces
Takes a lot of energy to overcome these forces.

Question 11

Why do ionic compounds dissolve in water?

Answer 11

Water molecules are polar
Pull ions away from the lattice and cause it to dissolve