Ionic and metallic bonding

Question 1

What is ionic bonding?

Answer 1

The electrostatic force of attraction between positive ions and negative ions

Question 2

Where does ionic bonding usually occur?

Answer 2

Between a metal and a non-metal.

Question 3

What is it known as when there is an imbalance in the number of protons and electrons?

Answer 3

ions

Question 4

What happens when ionic compounds are soluble in water?

Answer 4

As they dissolve the lattice structure breaks up allowing water molecules to surround the separated ions

Question 5

Do ionic compounds have high or low melting and boiling points and why?

Answer 5

High melting/boiling points because strong ionic bonds must be broken in order to break up the lattice.

Question 6

When do ionic compounds conduct electricity?

Answer 6

Only when molten or in solution as the lattice structure breaks up allowing the ions to be free to move.

Question 7

What type of bonding have high melting points and conduct electricity when liquid but not when solid?

Answer 7

Ionic lattice

Question 8

What structure conducts electricity when solid and have a wide range of melting points.

Answer 8

metallic lattice

Question 9

How can you identify the metal ions in a substance.

Answer 9

Flame tests, the colour observed will identify the metal ions present.

Question 10

What are ions?

Answer 10

Ion are particles that have an imbalance in the number of positive protons and negative electrons.

Question 11

What is the attraction between positive and negative charges known as?

Answer 11

Electrostatic attraction

Question 12

What are properties of metals?

Answer 12

Good conductors of heat and electricity due to the delocalised electrons, they have a range of melting/boiling points

Question 13

What is the type of bonding that can conduct electricity when solid and have a wide range of melting and boiling points?

Answer 13

Metallic lattice

Question 14

Explain why ionic compounds have high melting points

Answer 14

a large number of strong ionic onds must be broken

Question 15

Explain what happens to compunds such as magnesium chloride when they dissolve in water

Answer 15

The lattice structure breaks up to form free ions

Question 16

Explain why ionic compounds such as magnesium chloride conduct electricity when molten but not oslid

Answer 16

Ions are only free to move when molten

Question 17

What is an ion

Answer 17

a charged atom

Question 18

What is an ionic compunf

Answer 18

A compound made up of a metal and non metal

Question 19

Explain why ionic compounds have high melting points

Answer 19

They have an ionic lattice structure which is strong so it takes alot of energy to break up

Question 20

Explain why covalent networks have high melting and boiling points

Answer 20

All the atoms are held togetehr by strong covalent bonds in a large network of atoms and it takes alot of energy to break these bonds

Question 21

Explain how an ionic bond holds the atoms together

Answer 21

Electrostatic force of attraction between a positive metal ion and a negative non metal ion

Question 22

Explain fully in terms of electron arrangement why the nobles gases are unreactive

Answer 22

They have a full outer shell of electrons so they are unreactive as they don’t gain or lose electrons

Question 23

explain what holds the negatively charged electrons in place around the nucleus

Answer 23

the force of attraction between the positive protons and the negative electrons