Ionic bonding

Question 1

What are the properties of salts (ionic compounds)?

Answer 1

High melting and boiling points, brittle, soluble in water, only conduct electricity when melted or dissolved in water

Question 2

What is the perfect ionic model?

Answer 2

All salts are made of positive and negative ions arranged in a 3D lattice, and that these ions are all perfect spheres. Overall charge of the salt is zero

Question 3

What keeps the lattice together?

Answer 3

Ionic bonding - the electrostatic attraction between all positive and negative ions in a lattice

Question 4

Charge of group 1 cations?

Answer 4

1+ (just write plus)

Question 5

Charge of group 2 cations?

Answer 5

2+

Question 6

Charge of Aluminium (Al) cations?

Answer 6

3+

Question 7

Charge of Silver (Ag) cations?

Answer 7

1+ (just write plus)

Question 8

Charge of Zinc (Zn) cations?

Answer 8

2+

Question 9

Charge of Iron (Fe) cations?

Answer 9

2+ / 3+

Question 10

Charge of Copper (Cu) cations?

Answer 10

1+ / 2+

Question 11

Charge of Lead (Pb) cations?

Answer 11

2+ / 4+

Question 12

How do you name anions?

Answer 12

Change ending to -ide e.g. sulfide

Question 13

What is a polyatomic ion?

Answer 13

Ions made of more than one atom

Question 14

How are sulfate ions represented?

Answer 14

SO4^2-

Question 15

How are hydroxide ions represented?

Answer 15

OH-

Question 16

How are nitrate ions represented?

Answer 16

NO3^-

Question 17

How are carbonate ions represented?

Answer 17

CO3^2-

Question 18

How are ammonium ions represented?

Answer 18

NH4^+

Question 19

How do you represent ionic compounds?

Answer 19

In the ratio that they combine in to get to a neutral charge (as subscripts)

Question 20

How are ionic compounds (bonding) formed?

Answer 20

____ electron/s is transferred from one (metal atom) to one (non-metal atom)

Question 21

Why do ionic compounds conduct electricity when molten or dissolved?

Answer 21

Ions in a liquid are free to move around and they can carry a charge. In a solid the ions are strongly bonded in place, so cannot carry charge and conduct electricity

Question 22

What happens when you boil ionic compounds?

Answer 22

Ions separate into pairs, cannot carry charge and can’t conduct electricity

Question 23

Why do ionic compounds have high melting and boiling points?

Answer 23

There is a strong electrostatic attraction between cations and anions. Lots of energy is needed to overcome this attraction

Question 24

How does charge affect the strength of ionic bonding?

Answer 24

The larger the charge of ions in the lattice, the stronger the electrostatic attraction so the stronger the ionic bond

Question 25

How does distance affect ionic bonding?

Answer 25

The larger the distance between ions in the lattice, the weaker the electrostatic attraction so the weaker the ionic bonding

Question 26

How do you compare the size of ions?

Answer 26

The larger the distance between the nucleus and outer shell of electrons, the larger the ion

Question 27

What happens to the size of ions down a group?

Answer 27

Increases

Question 28

How do you compare melting/boiling points of ionic compounds?

Answer 28

Compare size and charge of ions

Question 29

Why are ionic compounds brittle?

Answer 29

When the ions are forced out of position, like charges line up and cause repulsion, cracking the ionic compound