Ionic Bonding

Question 1

Compare the electrical conductivity of sodium chloride in solid, molten liquid and solution

Answer 1

Solid - not conduct electricity
Molten liquid - conduct electricity
Solution - conduct electricity

Question 2

Compare the melting points of sodium chloride and magnesium oxide

Answer 2

Sodium chloride - high melting point

Magnesium oxide - even higher melting point

Question 3

What does it mean if an atom has an outer shell of 8 electrons

Answer 3

They have a stable electronic structure

Question 4

Explain how and why metal form from positive ions

Answer 4

Metal atoms lose the electron, or electrons, in their highest energy level and become positively charged ions

Question 5

Explain and why non-metal atoms form negative ions

Answer 5

Non-metal atoms gain an electron, or electrons, from another atom to become negatively charged ions

Question 6

What happens in ionic bonding?

Answer 6

A metal and non-metal combine by transferring electrons to form positive ins and negative ions which then attract one another

Question 7

Describe the structure of sodium chloride or magnesium oxide

Answer 7

A giant ionic lattice in which positive ions are strongly attracted to negative ions

Question 8

Explain, in terms of structure and bonding, some of the physical properties of sodium chloride

Answer 8

• high melting points

- electrical conductivity of solid, molten liquid and solution

Question 9

Explain, in terms of structure and bonding, why the melting point of sodium chloride is lower than that of magnesium oxide

Answer 9

Because it has weaker ionic bonds, which need less heat energy to overcome

Question 10

What is an ion?

Answer 10

A charged atom or group of atoms