1.31 deduce the charge of an ion from the electronic configuration of the atom from which the ion is formed

An atom with less then four electrons on its outer shell will want to lose electrons because that is the quickest way for it to have a full outer shell. So we know the atom will lose electrons (this makes positive ions).

Atoms with more than four electrons will gain electrons to fill their outer shell (as it is easier than losing electrons). This will result in negative ions.

Here are some examples...

Na has the electronic configuration of  2.8.1 (it has 1 electron on it's outer shell, so it is easiest to lose 1 electron to make a full outer shell). This results in the positive ion (a cation), Na+, which has the electronic configuration of 2.8

Cl has the electronic configuration of 2.8.7 (it has 7 electrons on it's outer shell, so it is easiest to gain 1 electron to make a full outer shell). This results in the negative ion (an anion), Cl-, which has the electronic configuration of 2.8.8

1.37 draw a diagram to represent the positions of the ions in a crystal of sodium chloride

Sodium chloride has a typical ionic structure, it has alternating positive  (Na+) and negative (Cl-) ions, this is how it should be drawn...

1.36 describe an ionic crystal as a giant three-dimensional lattice structure held together by the attraction between oppositely charged ions

Compounds with ionic bonding always have giant ionic structures, the ions are held closely together by the attraction between oppositely charged ions in a 3-D lattice arrangement.

1.35 understand the relationship between ionic charge and the melting point and boiling point of an ionic compound

Basically, the bigger the charge (e.g 3-), the stronger the electrostatic forces. This means that the bigger the ionic charge, the higher the melting/boiling point of the ion(s)

1.34 understand that ionic compounds have high melting and boiling points because of strong electrostatic forces between oppositely charged ions

Ionic compounds are held together by strong electrostatic forces that hold them together due to the attraction of the opposing charges (+ and -). To melt or boil anything, heat is used to break the electrostatic forces. The force will get stronger the higher the charge of the ion is, therefore, the stronger the bonds, the more heat needed. Ionic compounds have strong bonds, so they don't melt or boil unless there is a considerable amount of heat, this means they have high melting and boiling points.

1.33 understand ionic bonding as strong electrostatic attraction between oppositely charged ions

In ionic bonding, atoms gain or lose electrons to form charged particles (ions) which are then strongly attracted to each other (because of the attraction of opposite charges, + and -). This strong attraction is known as electrostatic attraction. This electrostatic attraction gives ionic compounds high melting and boiling points.

1.32 explain, using dot and cross diagrams, the formation of ionic compounds by electron transfer, limited to combinations of elements rom groups 1, 2, 3 and 5, 6, 7

Dot and cross diagrams show what's happening regarding the electrons when ionic bonding happens, the best way to explain is just to show you

Sodium Chloride (NaCl)
Sodium ions have the formula Na⁺ and chloride ions have the formula Cl^-. To have an outer shell, sodium wants to lose an electron and chloride wants to gain an electron. To make this happen, sodium gives chloride an electron. In the exam, make sure the dots and crosses are clear.

Magnesium oxide (MgO)

Magnesium ions have the formula Mg²⁺, while oxide ions have the formula O^2-. Magnesium gives oxygen two electrons

Calcium chloride, CaCl₂ (a little trickier)

Calcium ions have the formula Ca²⁺. Chloride ions have the formula Cl^-. Calcium wants to lose 2 electrons but chloride only wants 1. Therefore, two chloride ions bond with one calcium ion, this means that each chloride ion gets 1 electron and calcium loses two, so everyone happy :)


Image source: bitesize

1.30 recall the charges of common ions in this specification

All this means is that we've got to learn a few charges...

CATIONS

Group 1
Na+
Li+
K+

Group 2
Ca2+
Be2+
Mg2+


ANIONS

Group 6
O2-
S2-

Group 7 (halogens)
F-
Cl-
Br-

1.29 understand oxidation as the loss of electrons and reduction as the gain of electrons

In ionic bonding, atoms either lose or gain electrons (to form ions). When an atom loses electrons, it is called oxidation, when an atom gains electrons, it is called reduction.

NOTE: a useful was of remembering which is which is with the anagram 'O.I.L.R.I.G' (Oxidation.Is.Loss.Reduction.Is.Gain)

1.28 describe the formation of ions by the gain or loss of electrons

An ion is any atom (or group of atoms) that has charge / is electrically charged. Ions are formed due to the loss or gain of electrons.

If an atom gains an electron it becomes a negatively charged ion. Non-metals tend to do this, and they form anions. So elements from group 5-7 will form anions.

If an atom loses an electron it becomes a positively charged ion.the ion has a positive charge. Metals tend to do this, and they form cations (positive ions), so normally elements from group 1-3 will form cations. 

Group 0/8 are the noble gases and are inert + unreactive, so they do not form ions.

NOTE: an easy way to remember anion is A-Negative-ION - ANIONAn easy way to remember a cation is that if its not an anion, its a cation :)