🟠 Ionic Compounds

Question 1

Metals and Non-Metals that combine with ionic bonding form what?

Answer 1

Ionic compounds.

Question 2

What structure do ionic compounds have?

Answer 2

Giant ionic lattice – a 3D arrangement where ions are held together by strong electrostatic forces in all directions.

Question 3

What holds the ions together in an ionic lattice?

Answer 3

Strong electrostatic forces of attraction between oppositely charged ions (ionic bonding).

Question 4

What is an ionic lattice?

Answer 4

The regular arrangement of ions in an ionic substance.

Question 5

Extra - How many ions can a single grain of salt contain?

Answer 5

Around 1.2 × 10¹⁸ ions.

Question 6

Why do ionic compounds have high melting and boiling points?

Answer 6

Strong electrostatic forces of attraction between oppositely charged ions require a lot of energy to overcome.

Question 7

Why do ionic compounds conduct electricity when molten or aqueous?

Answer 7

The ions are free to move, allowing them to carry charge.

Question 8

Why do ionic compounds not conduct electricity when solid?

Answer 8

Ions are fixed in position and cannot move, so they cannot carry charge.

Question 9

What does “molten” mean in chemistry?

Answer 9

Melted to liquid.

Question 10

What does “aqueous” mean in chemistry?

Answer 10

Dissolved in water to make a solution.

Question 11

Can many ionic compounds dissolve in water?

Answer 11

Yes, many dissolve, allowing the ions to separate and move freely.

Question 12

Name four ways to represent ionic compounds.

Answer 12

Dot and cross diagrams, ball and stick models, two-dimensional diagrams, three-dimensional diagrams.

Question 13

What are the advantages of dot and cross diagrams?

Answer 13

Simple, easy to draw, show electrons.

Question 14

What are the disadvantages of dot and cross diagrams?

Answer 14

Do not show 3D arrangement, do not show relative sizes of ions.

Question 15

What are the advantages of ball and stick models?

Answer 15

Show 3D arrangement, easy to see how ions are arranged.

Question 16

What are the disadvantages of ball and stick models?

Answer 16

Difficult to draw for complex structures, show gaps between ions that do not exist, do not show electrons.

Question 17

What are the advantages of two-dimensional diagrams?

Answer 17

Simple, easy to draw.

Question 18

What are the disadvantages of two-dimensional diagrams?

Answer 18

Do not show 3D arrangement, difficult to interpret for complex structures.

Question 19

What are the advantages of three-dimensional diagrams?

Answer 19

Show 3D arrangement of ions.

Question 20

What are the disadvantages of three-dimensional diagrams?

Answer 20

Difficult and time-consuming to draw, may not show all ions in a large structure, do not show electrons.

Question 21

How can you determine the formula of an ionic compound?

Answer 21

By using diagrams or looking at the charges of the elements.

Question 22

How do dot and cross diagrams help determine the formula?

Answer 22

They show the ratio of ions in a compound.

Question 23

How do you balance charges to determine the formula?

Answer 23

Swap the numbers of charges so the overall charge of the compound is zero.

Question 24

Example: How do you write the formula for calcium chloride?

Answer 24

Calcium +2, Chlorine -1 → formula is CaCl₂.

Question 25

What is the key property of a giant ionic lattice?

Answer 25

A regular, repeating arrangement of oppositely charged ions.

Question 26

How are sodium and chloride ions arranged in sodium chloride?

Answer 26

A giant ionic lattice consisting of alternating, adjacent positively charged sodium ions and negatively charged chloride ions in a tightly packed, regular arrangement of rows and columns

Question 27

What does the strength of ionic bonds depend on?

Answer 27

The charge on the ions; higher charges → stronger forces → higher melting points.

Question 28

Why do solid ionic compounds not conduct electricity?

Answer 28

Ions are held in fixed positions in the lattice, so aren't free to move around to carry a charge, and therefore cannot conduct electricity.

Question 29

Why do molten or aqueous ionic compounds conduct electricity?

Answer 29

Ions aren't held together by strong electrostatic forces of attraction anymore, so can therefore move around freely, carry a charge, and conduct electricity.

Question 30

What does “giant” mean in giant ionic lattice?

Answer 30

The lattice contains a very large number of ions.

Question 31

Why do ionic compounds form crystals with regular shapes?

Answer 31

The lattice arrangement continues in three dimensions, producing a regular external structure.

Question 32

What happens to electrostatic forces during melting and boiling?

Answer 32

Large amounts of energy break the bonds and overcome the strong electrostatic forces of attraction.

Question 33

Why is energy needed to melt or boil ionic compounds?

Answer 33

To overcome the strong electrostatic forces of attraction between the bonds of the oppositely charged ions.

Question 34

What is an empirical formula, and

Answer 34

Count the number of atoms of each element and write the ratio.

Question 35

How can you find the empirical formula from a 3D diagram?

Answer 35

Identify the ions in the lattice and balance their charges to ensure overall neutrality.

Question 36

What is electrostatic force?

Answer 36

A force of attraction between particles with opposite charges.

Question 37

What are the three main properties of ionic compounds?

Answer 37

1) High melting/boiling points, 2) Conduct electricity when molten/aqueous, 3) Some are soluble in water.

Question 38

Why are ionic compounds insulators when solid?

Answer 38

Ions cannot move in the fixed lattice structure, so cannot flow and therefore not carry a charge.

Question 39

What is the main reason all ionic compounds have similar properties?

Answer 39

They all have giant ionic lattices held together by strong electrostatic forces acting in all directions.