IB SL Structure 2.1: Ionic bonding

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34 Terms

1

Name 3 types of bonding

  • Ionic (metal + non-metal)

  • Covalent (non-metal + non-metal)

  • Metallic (metal)

2

Electronegativity

is a measure of the tendency of an atom to attract a bonding pair of electrons

3

Describe what happens to electrons in ionic bonding

In ionic bonding, electrons are transferred from one atom (metal) to another atom (non-metal) to form a positive and a negative ions.

4

Ionic bonding (definition)

is the electrostatic attraction between oppositely charged ions

5

Ammonium ion

NH4ithium

6

Lithium ion

Li+

7

Potassium ion

K+

8

Silver ion

Ag+

9

Sodium ion

Na+

10

Calcium ion

Ca2+

11

Copper (II) ion

Cu2+

12

Iron (II)

Fe2+

13

Lead (II)

Pb2+

14

Magnesium ion

Mg2+

15

Zinc ion

Zn2+

16

Aluminium ion

Al3+

17

Iron (III) ion

Feromide

18

Bromide

Br-

19

Chloride

Cl-

20

Fluoride

F-

21

Hydroxide

OH-

22

Iodide

I-

23

Nitrate

NO3-

24

Hydrogencarbonate

HCO3-

25

Carbonate

CO32-

26

Oxide

O2-

27

Sulfate

SO42-

28

Sulfide

S2-

29

Phosphate

PO43-

30

What is the structure of ionic compounds?

Giant ionic lattice

31

Explain why ionic substances have high melting and boiling points, and low volatility

  • Ionic substances have a giant ionic lattice

  • There is strong electrostatic attraction between oppositely charged ion

  • It takes a lot of energy to overcome this attraction

32

What factors affect the strength of ionic bonding?

  • ionic charge: the higher the charge, the stronger the ionic bond

  • ionic radius: the smaller the radius, the stronger the ionic bond

33

Explain why ionic substances conduct electricity when molten and aqueous, but do not conduct in solid

  • Ionic substances do not conduct electricity when solid because ions are held in the lattice, so are not mobile.

Ionic substances conduct electricity when molten or in the solution because ions are free to move and carry the charge.

34

Lattice enthalpy

is the enthalpy (energy) change when 1 mole of a solid ionic crystal is broken into its scattered gaseous ions. Lattice enthalpy can be used to measure the strength of ionic bonds in different compounds.