U2.1: Ionic model

Question 1

Define Ionic bond

Answer 1

Electrostatic attraction between oppositely charged ions.

Question 2

What ions have a stronger electrostatic attraction and a stronger ionic bond?

Answer 2

Ions with a greater charge have stronger electrostatic attractions and stronger ionic bonds

Question 3

What is the relation between the radius, the charge and the ionic bond of an element?

Answer 3

• Smaller the radius and greater the charge of ions, the stronger of ionic bonds and vice versa

Question 4

Define melting point

Answer 4

The temperature at which a solid will undergo a change of state to a liquid

Question 5

Define Volatility

Answer 5

The ease at which a substance vaporises or becomes a gas.

Question 6

Define lattice enthalpy

Answer 6

A measure of the strength of the electrostatic attraction between ions in an ionic compound

Question 7

Relation between the lattice enthalpy and ionic bond?

Answer 7

• The larger the enthalpy, the stronger the ionic bond and vice versa

Question 8

Define electrical conductivity

Answer 8

The ability of charged particles to move through a region of space

Question 9

What is conductivity exclusively NOT for

Answer 9

Conductivity is not exclusively for electrons, it’s the mobility of ions too (in molten or aqueous state)

Question 10

What does the strength of ionic bonds depend on

Answer 10

Atomic Radius
Nuclear Charge

Question 11

What are the polyatomic ions

Answer 11

• Sulfate
• Sulfite
• Nitrate
• Nitrite
• Carbonate
• Hydrogen Carbonate
• Hydroxide
• Ammonium
• Phosphate

Question 12

Charge of sulfate

Answer 12

SO4 2-

Question 13

Charge of Sulfite

Answer 13

SO3 2-

Question 14

Charge of nitrate

Answer 14

NO3 -

Question 15

Charge of Nitrite

Answer 15

NO2 -

Question 16

Charge of Carbonate

Answer 16

CO3 2-

Question 17

Charge of Hydrogen Carbonate

Answer 17

HCO3 -

Question 18

Charge of Hydroxide

Answer 18

OH -

Question 19

Charge of Ammonium

Answer 19

NH4 +

Question 20

Charge of Phosphate

Answer 20

PO4 3-

Question 21

Order of energy required to breakl the bonds in all tyopes of bonds?

Answer 21

Covalent < metallic < ionic

Question 22

Explain why the bonding of HCl is less than that of LiCl

Answer 22

• LiCl has ionic bonding whereas HCl has polar, covalent bonding
• The electrostatic forces of attraction in Ionic bonds are much stronger than the Intermolecular forces of attraction in polar covalent bonds.

Question 23

Which, out of CaO and CaF2, will have a higher melting point

Answer 23

• CaO
• O has a greater charge than Fluorine meaning there’s a stronger ionic bond in CaO than CaF2 hence a greater magnitude of enthalpy charge

Question 24

When ions lose electrons what do they gain

Answer 24

A positive charge (or forming cations)

And vice versa