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Chemical Formula

3.3 Chemical Formula - Pandai Notes
CHEMISTRY • Form 4 • Chapter 3: The Mole Concept, Chemical Formula and Equation

3.3Chemical Formula

Chemical formulas are the universal language of chemistry. They show the exact elements present in a substance and the proportions in which their atoms combine.

Learning Objectives

  • State the meaning of chemical formula, empirical formula, and molecular formula.
  • Determine the empirical formula of magnesium oxide, MgO, through an activity.
  • Determine the empirical formula of copper(II) oxide, CuO, through an activity.
  • Solve numerical problems involving empirical formula and molecular formula.
  • Construct and write the chemical formulae of ionic compounds and name chemical compounds systematically according to IUPAC nomenclature.

Two Methods for Determining Empirical Formulae

Magnesium oxide vs. copper(II) oxide — contrasting setups, precautions and rationale based on metal reactivity.

Method 1: Direct Heating in Air

For reactive metals such as magnesium.

  • Clean the magnesium ribbon with sandpaper to remove the oxide layer.
  • Heat the crucible without the lid initially.
  • Cover with the lid when burning begins to prevent white fumes of MgO from escaping.
  • Lift the lid slightly from time to time to allow oxygen to enter for complete combustion.
  • Heat strongly for 1–2 minutes after burning stops.
  • Repeat heating, cooling and weighing until a constant mass is obtained.

Method 2: Reduction by Hydrogen Gas

For less reactive metals such as copper.

  • Copper(II) oxide is reduced by dry hydrogen gas.
  • Reaction: CuO + H2 → Cu + H2O
  • Hydrogen is produced from zinc granules and dilute hydrochloric acid.
  • Let hydrogen flow for about 10 seconds before heating to expel all air and prevent an explosion.
  • Heat black copper(II) oxide until it turns completely brown.
  • Keep hydrogen flowing while cooling to prevent hot copper from reoxidising.
  • Repeat heating, cooling and weighing until a constant mass is obtained.

Brief Explanation

Chemical formula, empirical formula, molecular formula and naming rules.

A chemical formula conveys the chemical identity and composition of a substance. It uses chemical symbols for elements and subscript numbers to represent the proportions of atoms.

Empirical Formula

Shows the simplest whole-number ratio of atoms of each element in a compound. It is calculated experimentally from mass data by converting grams to moles and simplifying the ratio.

Molecular Formula

Shows the actual number of atoms of each element found in a molecule of a compound. It is an integer multiple of the empirical formula:

\[ \text{Molecular formula} = (\text{Empirical formula})_n \]

Compound Molecular formula Empirical formula Value of n
WaterH2OH2O1
AmmoniaNH3NH31
HydrazineN2H4NH22
PropeneC3H6CH23
BenzeneC6H6CH6
GlucoseC6H12O6CH2O6
HexaneC6H14C3H72

Steps to Determine Empirical Formula

  1. Determine the mass of each element.
  2. Calculate the number of moles of atoms of each element: \(\text{mole} = \dfrac{\text{mass}}{\text{RAM}}\).
  3. Divide each mole value by the smallest mole value to find the mole ratio.
  4. Convert the ratio to the simplest whole number ratio.

Worked Example

1.35 g of Al combines with 1.2 g of O.

Moles of Al \(= \dfrac{1.35}{27} = 0.05\)

Moles of O \(= \dfrac{1.2}{16} = 0.075\)

Ratio Al : O \(= \dfrac{0.05}{0.05} : \dfrac{0.075}{0.05} = 1 : 1.5\)

Multiply by 2 → Al : O \(= 2 : 3\) → Al2O3

Ionic Compounds

Composed of cations (positively charged) and anions (negatively charged). Use the cross-change method to balance charges.

Example: Aluminium sulphate — Al3+ and SO42− → Al2(SO4)3

Naming Compounds

Ionic: cation first, then anion. Metals with multiple oxidation states use Roman numerals, e.g. FeO = iron(II) oxide, Fe2O3 = iron(III) oxide.

Covalent: more electropositive element first, more electronegative element second with suffix -ide. Greek prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-.

Examples: CO = carbon monoxide, NO2 = nitrogen dioxide, SO3 = sulphur trioxide.

Try to Answer First

Answer mentally, then check the explanation.

1

A sample contains 6.24 g of potassium and 12.8 g of bromine. Determine the empirical formula of this compound. [Relative atomic mass: K = 39, Br = 80]

Answer: Number of moles of K \(= \dfrac{6.24}{39} = 0.16\) mol. Number of moles of Br \(= \dfrac{12.8}{80} = 0.16\) mol. Mole ratio K : Br \(= 1 : 1\). Empirical formula = KBr.
2

Why must the hydrogen gas be allowed to flow continuously while the glass tube cools down to room temperature in the determination of the empirical formula of copper(II) oxide?

Answer: To prevent hot copper from reacting with oxygen in the surrounding air to reform copper(II) oxide.
3

Construct the chemical formula for aluminium sulphate and iron(III) oxide using the cross-change method.

Answer: Aluminium sulphate: Al3+ and SO42− → Al2(SO4)3. Iron(III) oxide: Fe3+ and O2− → Fe2O3.

Common Mistakes

Avoid these errors when working with chemical formulae.

!
Rounding non-integers prematurely: rounding a mole ratio like \(1 : 1.5\) directly to \(1 : 2\) instead of multiplying by 2 to obtain the correct whole number ratio \(2 : 3\).
!
Forgetting brackets around polyatomic ions: writing AlOH3 instead of Al(OH)3, or CaNO32 instead of Ca(NO3)2.
!
Writing charges inside the final neutral chemical formula: writing Mg2+O2− or Na+Cl− instead of neutral formula MgO and NaCl.
!
Omitting Roman numerals for transition metals: naming Fe2O3 as "iron oxide" instead of iron(III) oxide.
!
Using Greek prefixes for ionic compounds: incorrectly calling MgCl2 "magnesium dichloride" instead of magnesium chloride.

Concept Misunderstandings

Compare each misconception with the correct fact.

Misconception

All compounds have different empirical and molecular formulas.

Correct Fact

Compounds whose molecular formula is already in the simplest whole number ratio (such as H2O, NH3, CO2) have identical empirical and molecular formulas (n = 1).

Misconception

The empirical formula of copper(II) oxide can be determined by heating copper ribbon in a crucible like magnesium.

Correct Fact

Copper is much less reactive towards oxygen than magnesium and will not burn readily or react completely to form copper(II) oxide in a crucible. It must be determined by reducing copper(II) oxide using dry hydrogen gas.

Misconception

The subscript 1 must always be written in a chemical formula.

Correct Fact

By IUPAC convention, the subscript number 1 is omitted (e.g. NaCl, not Na1Cl1).

Summary

Key facts to remember.

  • A chemical formula represents a substance using element symbols and subscript numbers. Subscript 1 is omitted.
  • Empirical formula is the simplest whole-number ratio of atoms of each element in a compound.
  • Molecular formula represents the actual number of atoms of each element in a molecule: \(\text{Molecular formula} = (\text{Empirical formula})_n\).
  • Magnesium oxide determination involves heating Mg in a crucible with a lid, lifting the lid intermittently to supply O2, closing to retain white fumes (MgO), and heating to constant mass.
  • Copper(II) oxide determination involves reducing CuO with dry H2 gas; requires expelling air before heating to avoid explosion and cooling under H2 gas to prevent reoxidation.
  • Ionic formulas balance cation and anion charges using the cross-change method.
  • Naming: ionic compounds use cation + anion (with Roman numerals for variable oxidation states). Simple covalent compounds use Greek numerical prefixes and end with '-ide'.

Short Activity

Complete all parts before checking your score.

A. Objective Quiz

1

In an experiment to determine the empirical formula of magnesium oxide, why must the crucible lid be lifted slightly from time to time during heating?

2

A compound has the empirical formula CH2 and a relative molecular mass (RMM) of 56. What is the molecular formula of the compound? [Relative atomic mass: H = 1, C = 12]

B. Fill in the Blanks

3

Before heating copper(II) oxide in Activity 3.13, hydrogen gas must flow through the apparatus for about 10 seconds to expel all ______ from the glass tube to prevent an explosion.

4

The chemical formula that shows the simplest whole number ratio of atoms of each element in a compound is known as the ______ formula.

C. Match the Item with Its Description

Drag each item on desktop. On mobile, tap an item and then tap the matching box.

Item / Chemical Term

Heating to a constant mass Sandpapering magnesium ribbon Carbon monoxide Iron(III) oxide

Correct Description / Rationale

1Ensuring that the chemical reaction has taken place completely
2Removing the oxide layer on the metal surface before burning
3Simple molecular compound represented by the formula CO
4Ionic compound formed by combining Fe3+ and O2− ions
Complete every answer before checking.
 

Keywords

Tap or hover over a term to read its meaning.

Chemical formula Empirical formula Molecular formula Cation Anion Constant mass Cross-change method
The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.

Chemical Formula

3.3 Chemical Formula - Pandai Notes
CHEMISTRY • Form 4 • Chapter 3: The Mole Concept, Chemical Formula and Equation

3.3Chemical Formula

Chemical formulas are the universal language of chemistry. They show the exact elements present in a substance and the proportions in which their atoms combine.

Learning Objectives

  • State the meaning of chemical formula, empirical formula, and molecular formula.
  • Determine the empirical formula of magnesium oxide, MgO, through an activity.
  • Determine the empirical formula of copper(II) oxide, CuO, through an activity.
  • Solve numerical problems involving empirical formula and molecular formula.
  • Construct and write the chemical formulae of ionic compounds and name chemical compounds systematically according to IUPAC nomenclature.

Two Methods for Determining Empirical Formulae

Magnesium oxide vs. copper(II) oxide — contrasting setups, precautions and rationale based on metal reactivity.

Method 1: Direct Heating in Air

For reactive metals such as magnesium.

  • Clean the magnesium ribbon with sandpaper to remove the oxide layer.
  • Heat the crucible without the lid initially.
  • Cover with the lid when burning begins to prevent white fumes of MgO from escaping.
  • Lift the lid slightly from time to time to allow oxygen to enter for complete combustion.
  • Heat strongly for 1–2 minutes after burning stops.
  • Repeat heating, cooling and weighing until a constant mass is obtained.

Method 2: Reduction by Hydrogen Gas

For less reactive metals such as copper.

  • Copper(II) oxide is reduced by dry hydrogen gas.
  • Reaction: CuO + H2 → Cu + H2O
  • Hydrogen is produced from zinc granules and dilute hydrochloric acid.
  • Let hydrogen flow for about 10 seconds before heating to expel all air and prevent an explosion.
  • Heat black copper(II) oxide until it turns completely brown.
  • Keep hydrogen flowing while cooling to prevent hot copper from reoxidising.
  • Repeat heating, cooling and weighing until a constant mass is obtained.

Brief Explanation

Chemical formula, empirical formula, molecular formula and naming rules.

A chemical formula conveys the chemical identity and composition of a substance. It uses chemical symbols for elements and subscript numbers to represent the proportions of atoms.

Empirical Formula

Shows the simplest whole-number ratio of atoms of each element in a compound. It is calculated experimentally from mass data by converting grams to moles and simplifying the ratio.

Molecular Formula

Shows the actual number of atoms of each element found in a molecule of a compound. It is an integer multiple of the empirical formula:

\[ \text{Molecular formula} = (\text{Empirical formula})_n \]

Compound Molecular formula Empirical formula Value of n
WaterH2OH2O1
AmmoniaNH3NH31
HydrazineN2H4NH22
PropeneC3H6CH23
BenzeneC6H6CH6
GlucoseC6H12O6CH2O6
HexaneC6H14C3H72

Steps to Determine Empirical Formula

  1. Determine the mass of each element.
  2. Calculate the number of moles of atoms of each element: \(\text{mole} = \dfrac{\text{mass}}{\text{RAM}}\).
  3. Divide each mole value by the smallest mole value to find the mole ratio.
  4. Convert the ratio to the simplest whole number ratio.

Worked Example

1.35 g of Al combines with 1.2 g of O.

Moles of Al \(= \dfrac{1.35}{27} = 0.05\)

Moles of O \(= \dfrac{1.2}{16} = 0.075\)

Ratio Al : O \(= \dfrac{0.05}{0.05} : \dfrac{0.075}{0.05} = 1 : 1.5\)

Multiply by 2 → Al : O \(= 2 : 3\) → Al2O3

Ionic Compounds

Composed of cations (positively charged) and anions (negatively charged). Use the cross-change method to balance charges.

Example: Aluminium sulphate — Al3+ and SO42− → Al2(SO4)3

Naming Compounds

Ionic: cation first, then anion. Metals with multiple oxidation states use Roman numerals, e.g. FeO = iron(II) oxide, Fe2O3 = iron(III) oxide.

Covalent: more electropositive element first, more electronegative element second with suffix -ide. Greek prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-.

Examples: CO = carbon monoxide, NO2 = nitrogen dioxide, SO3 = sulphur trioxide.

Try to Answer First

Answer mentally, then check the explanation.

1

A sample contains 6.24 g of potassium and 12.8 g of bromine. Determine the empirical formula of this compound. [Relative atomic mass: K = 39, Br = 80]

Answer: Number of moles of K \(= \dfrac{6.24}{39} = 0.16\) mol. Number of moles of Br \(= \dfrac{12.8}{80} = 0.16\) mol. Mole ratio K : Br \(= 1 : 1\). Empirical formula = KBr.
2

Why must the hydrogen gas be allowed to flow continuously while the glass tube cools down to room temperature in the determination of the empirical formula of copper(II) oxide?

Answer: To prevent hot copper from reacting with oxygen in the surrounding air to reform copper(II) oxide.
3

Construct the chemical formula for aluminium sulphate and iron(III) oxide using the cross-change method.

Answer: Aluminium sulphate: Al3+ and SO42− → Al2(SO4)3. Iron(III) oxide: Fe3+ and O2− → Fe2O3.

Common Mistakes

Avoid these errors when working with chemical formulae.

!
Rounding non-integers prematurely: rounding a mole ratio like \(1 : 1.5\) directly to \(1 : 2\) instead of multiplying by 2 to obtain the correct whole number ratio \(2 : 3\).
!
Forgetting brackets around polyatomic ions: writing AlOH3 instead of Al(OH)3, or CaNO32 instead of Ca(NO3)2.
!
Writing charges inside the final neutral chemical formula: writing Mg2+O2− or Na+Cl− instead of neutral formula MgO and NaCl.
!
Omitting Roman numerals for transition metals: naming Fe2O3 as "iron oxide" instead of iron(III) oxide.
!
Using Greek prefixes for ionic compounds: incorrectly calling MgCl2 "magnesium dichloride" instead of magnesium chloride.

Concept Misunderstandings

Compare each misconception with the correct fact.

Misconception

All compounds have different empirical and molecular formulas.

Correct Fact

Compounds whose molecular formula is already in the simplest whole number ratio (such as H2O, NH3, CO2) have identical empirical and molecular formulas (n = 1).

Misconception

The empirical formula of copper(II) oxide can be determined by heating copper ribbon in a crucible like magnesium.

Correct Fact

Copper is much less reactive towards oxygen than magnesium and will not burn readily or react completely to form copper(II) oxide in a crucible. It must be determined by reducing copper(II) oxide using dry hydrogen gas.

Misconception

The subscript 1 must always be written in a chemical formula.

Correct Fact

By IUPAC convention, the subscript number 1 is omitted (e.g. NaCl, not Na1Cl1).

Summary

Key facts to remember.

  • A chemical formula represents a substance using element symbols and subscript numbers. Subscript 1 is omitted.
  • Empirical formula is the simplest whole-number ratio of atoms of each element in a compound.
  • Molecular formula represents the actual number of atoms of each element in a molecule: \(\text{Molecular formula} = (\text{Empirical formula})_n\).
  • Magnesium oxide determination involves heating Mg in a crucible with a lid, lifting the lid intermittently to supply O2, closing to retain white fumes (MgO), and heating to constant mass.
  • Copper(II) oxide determination involves reducing CuO with dry H2 gas; requires expelling air before heating to avoid explosion and cooling under H2 gas to prevent reoxidation.
  • Ionic formulas balance cation and anion charges using the cross-change method.
  • Naming: ionic compounds use cation + anion (with Roman numerals for variable oxidation states). Simple covalent compounds use Greek numerical prefixes and end with '-ide'.

Short Activity

Complete all parts before checking your score.

A. Objective Quiz

1

In an experiment to determine the empirical formula of magnesium oxide, why must the crucible lid be lifted slightly from time to time during heating?

2

A compound has the empirical formula CH2 and a relative molecular mass (RMM) of 56. What is the molecular formula of the compound? [Relative atomic mass: H = 1, C = 12]

B. Fill in the Blanks

3

Before heating copper(II) oxide in Activity 3.13, hydrogen gas must flow through the apparatus for about 10 seconds to expel all ______ from the glass tube to prevent an explosion.

4

The chemical formula that shows the simplest whole number ratio of atoms of each element in a compound is known as the ______ formula.

C. Match the Item with Its Description

Drag each item on desktop. On mobile, tap an item and then tap the matching box.

Item / Chemical Term

Heating to a constant mass Sandpapering magnesium ribbon Carbon monoxide Iron(III) oxide

Correct Description / Rationale

1Ensuring that the chemical reaction has taken place completely
2Removing the oxide layer on the metal surface before burning
3Simple molecular compound represented by the formula CO
4Ionic compound formed by combining Fe3+ and O2− ions
Complete every answer before checking.
 

Keywords

Tap or hover over a term to read its meaning.

Chemical formula Empirical formula Molecular formula Cation Anion Constant mass Cross-change method
The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.
Chapter : Mole Concept, Chemical Formulae and Equations
Topic : Chemical Formula
Form 4 Chemistry
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