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Formulae (CIE IGCSE Chemistry: Co-ordinated Sciences (Double Award))

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Caroline

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Caroline

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Molecular formulae

  • Elements are often represented using their chemical symbol from the Periodic Table

Chemical symbols of elements table

Element Symbol Element Symbol
Lithium Li Calcium Ca
Chromium Cr Gold Au
Aluminium Al Sulfur S

 

  • Seven elements exist as diatomic molecules, which means that they are molecules made of two atoms:
    1. Hydrogen, H2 
    2. Nitrogen, N2 
    3. Oxygen, O2 
    4. Fluorine, F2 
    5. Chlorine, Cl2 
    6. Bromine, Br2 
    7. Iodine, I2 

Periodic Table identifying the 7 diatomic elements

Periodic Table highlighting the seven elements that for diatomic molecules with the formula X2

The highlighted elements all exist as diatomic molecules with the formula X2

  • These 7 elements are also classed as simple molecules
  • Atoms combine together in fixed ratios that will give them full outer shells of electrons
    • When this happens, a molecule is formed
  • The molecular formula of a molecule shows:
    • The type of atoms involved, given by the chemical symbol
      AND
    • The number of atoms, given by the subscript (little) number after a chemical symbol

Examples of molecular formulae

Substance Molecular formula Made from
Hydrogen H2 2 hydrogen atoms
Chlorine Cl2 2 chlorine atoms
Water H2O  2 hydrogen atoms
1 oxygen atom
Methane CH4 1 carbon atom
4 hydrogen atoms
Ammonia NH3 1 nitrogen atom
3 hydrogen atoms
Sulfuric acid H2SO4 2 hydrogen atoms
1 sulfur atom
4 oxygen atoms

  • The table also shows that the molecular formula can be deduced from the relative number of atoms present
    • E.g. Ammonia contains 3 atoms of hydrogen and 1 atom of nitrogen, which means its molecular formula is NH3

Diagrammatic representation of chemicals

  • Diagrams or models can be used to represent and/or deduce the molecular formula of elemetns and simple compounds:

Diagrams showing how chemicals can be represented visually

When simple molecules are represented using coloured atoms, a key is used to show the colours for each type of atom

  • Using the water examples it is important to know that these representations also show the arrangement of the atoms in the molecule
    • Water, H2O
      • The hydrogen atoms are on either side of the oxygen atom
      • It does not have two hydrogen atoms and an oxygen atom all joined together in a  row

Worked example

What is the molecular formula of the following compound? 

butane

Answer:

  • The molecule contains:
    • 4 carbon atoms
    • 10 hydrogen atoms
  • Therefore, the molecular formula is C4H10 

Deducing formulae of ionic compounds

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Deducing formulae of ionic compounds

Extended tier only

  • Metals and non-metals react together to form ionic compounds
    • Ionic compounds are not simple molecules 
    • Remember: Simple molecules are formed when non-metals react together to form compounds
  • Ionic compounds involve the metal losing electrons and the non-metal gaining electrons to form ions
  • Some ions that you will be expected to be able to use, because they are stated in the exam specification, include:
    • Hydrogen ions, H+ - sometimes referred to as protons
    • Group 1 ions, e.g. Li+, Na+, K+ 
    • Group 7 ions, F–, Cl–, Br– 
    • Copper(II) ions, Cu2+ 
    • Iron(II) ions, Fe2+ 
    • Iron(III) ions, Fe3+ 
  • There are some polyatomic (containing more than one atom) ions stated in the exam specification: 
    • Carbonate ions, CO32– 
    • Sulfate ions, SO42– 
    • Hydroxide ions, OH– 
    • Nitrate ions, NO3–
    • Ammonium ions, NH4+ 

How to determine the formulae of ionic compounds

  • Ionic compounds typically have no overall charge
    • This means that the size of any positively charged ion is cancelled by the size of any negatively charged ion
    • Careful: This should not be confused with an atom having no overall charge

Direct comparison

  • The formula of an ionic compound can be determined by directly comparing the charges of the ions:
    • For example, iron(II) sulfate
      • The iron(II) ion is Fe2+, which means that it has a 2+ or +2 charge
      • The sulfate ion is SO42–, which means that it has a 2– or –2 charge
      • The charges cancel each other out
        • Mathematically, (+2) + (–2) = 0
      • This means that one SO42– ion is needed to cancel the +2 charge on Fe2+ 
      • Therefore, the formula of iron(II) sulfate is FeSO4 

The swap-and-drop method

  • When the ions in the ionic compound have different charges, it can be easier to use the swap-and-drop method
    • Careful: If you use this method with ions that have the same charge, then you must give the simplest whole number ratio to get the correct answer
  • For example, copper(II) chloride:
    • The copper(II) ion is Cu2+, which means that it has a 2+ or +2 charge
    • The chloride ion is Cl–, which means that it has a 1– or –1 charge
    • The size of the charge on the copper(II) ion indicates the number of chloride ions needed, and the size of the charge on the chloride ion indicates the number of copper(II) ions needed

Determining the formula of copper(II) chloride

~5RmSBVa_copperii-chloride-swap-and-drop

The charges swap from element to element and drop down. The positive and negative signs are removed and there is no need for the number 1.

      • This gives the overall formula of copper(II) chloride as CuCl2 

Worked example

The compound produced in the reaction between iron wool and chlorine contains the ions Fe3+ and Cl–.

a)
Give the formula of this compound.
 
b)
State the name of this compound.
 

Answers:

Part a)

  • Direct comparison method:
    • The iron ion is Fe3+, which means that it has a 3+ or +3 charge
    • The chloride ion is Cl–, which means that it has a 1– or –1 charge
    • The charges do not cancel each other out
      • Mathematically, (+3) + (–1) ≠ 0
    • Three Cl– ions are needed to cancel the +3 charge on Fe3+ 
    • Therefore, the formula is FeCl3 
  • Swap-and-drop method

d5o2dGJS_ironiii-chloride-swap-and-drop

  • The formula is FeCl3 

Part b)

  • The metal is iron and the chlorine will change to chloride 
  • Therefore the name is iron chloride

Examiner Tip

Take your time determining the chemical formula of ionic compounds with

  • Different charges on the ions
  • Polyatomic ions

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    Caroline

    Author: Caroline

    Expertise: Physics Lead

    Caroline graduated from the University of Nottingham with a degree in Chemistry and Molecular Physics. She spent several years working as an Industrial Chemist in the automotive industry before retraining to teach. Caroline has over 12 years of experience teaching GCSE and A-level chemistry and physics. She is passionate about creating high-quality resources to help students achieve their full potential.