Acids and bases AS90944 revision part 2

We are working through a practise paper from the Ministry website

You should have completed question 1 last night. Do question 2 tonight. See last night’s post for instructions on how to hand this work in.

Also revise writing chemical formulae, word equations, fully balanced chemical equations and the reactions of acids and bases by watching the embeded videos below. They are based on lessons and lesson notes I did with you earlier in the year. There is video of practical work you carried out when you were making salts by neutralising acids with bases.

Ions, ionic compounds, word equations and fully balanced chemical equations.

Neutralisation reactions and practical work you carried out. Acids bases and salts.

Acids and bases AS90944 year 11 revision.


End of term exams are looming. We revised the atomic structure aspects of this topic in class today and you may choose how you do your exam revision homework.

1) Print the practise test paper out at home and answer the questions on the printout

2) Download the practise paper onto your computer and answer the questions separately on your own paper.

3) Flick through the practise paper questions on the blog and answer them on your own paper.


Practise paper

Atoms and atomic structure

A look at the periodic table


Writing chemical formulae

Writing chemical formulae

Compounds made up of ions are called ionic compounds. When they are named the metal ion goes first and the non metal ion comes last.

To write the chemical formula from the name go through these steps.

(1)Write down the ions from the table (you are always given this)

(2)successively add postive and negative ions till the total charges balance

(3)Write the chemical formula. Aluminium oxide has been done for you. 

(4)in the case of copper nitrate where two nitrate ions are needed to balance charge we need to put the nitrate ions in brackets e.g.  Cu(NO3)2.


Enter the date in your book and write the chemical formula for these these compounds.


(1) sodium oxide

(2) calcium hydroxide

(3) potassium carbonate

(4) zinc chloride

(5) magnesium nitrate

(6) aluminium carbonate 


Sodium and chlorine reacting to form an ionic compound sodium chloride

What happens when sodium and chlorine atoms react?

Sodium has one electron in its outer shell. Chlorine has seven electrons in its outer shell. When they react sodium loses an electron to become a sodium ion with a charge of +1. Chlorine atoms accept an electron to become chloride ions with a charge of -1. After reacting the sodium and chloride ions have a full outer shell of electrons. A full outer shell of electrons is a stable arrangement. The inert gasses in group 18 of the periodic table all have a full outer shell and characteristically are very unreactive (they don’t easily combine with other elements). The new substance sodium chloride is made up of ions. Compounds that have ions bonded together are called ionic. The ions are held together by powerful electrostatic forces. Ionic compounds typically have high melting and boiling points as a consequence.

Homework… how much of this do you understand?

Watch the video especially the bit that deals with the changes to sodium and chlorine atoms when they react with each other. Magnesium has two electrons in its outer shell and it burns in chlorine gas like sodium.
Draw sodium and chlorine atoms and show how ions are produced when they react.
What are the charges of the ions?
what is the formula of magnesium chloride?

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