Chemistry Unit 1

Omar Amura
Mind Map by , created over 6 years ago

Exam is on the 23rd of May

Omar Amura
Created by Omar Amura over 6 years ago
AS-Level Chemistry: Unit 1:The Atom
Daena Targaryen
AS Chemistry - Enthalpy Changes
Sarah H-V
AQA Biology B1 Questions
Bella Statham
GCSE - AQA: C1.1 The Fundamental Ideas in Chemistry
Olly Okeniyi
GCSE AQA Chemistry 1 Fuels & The Environment
Lilac Potato
Atoms and Reactions
Flame tests
Joshua Rees
Testing for ions
Joshua Rees
Chemistry Unit 1
1 Formulae, Equations and Amount of Substance ALWAYS LOOK AT THE SYMBOL GIVEN (g OR dm³, etc.)
1.1 Empirical Formula: %/ram = x for each element, x/smallest value, then ajust
1.2 Ionic Equations: Write out full molecular formula, balance, separate into ions, look if soluble or not, then cancel spectator ions and re-write
1.3 Moles = mass/molar mass OR n=m/Mr
1.3.1 For Gases: moles= volume(dm³)/Molar volume(24) OR n= v/Mv (24dm³mol­ˉ¹)
1.3.2 4 Solutions: moles=concentration(moldmˉ³)Xvolume(dm³) OR n=cv REARRAGE: c(moldm³)=n/v WATCH OUT 4 CONVERTIONS cm³->dm³ 1cm³->0.001dm³ 1dm³->1000g
1.4 Calculations based on reactions
1.4.1 To get Mass B from Mass A: mass A -> moles A -> moles B -> mass B Moles A -> Moles B: moles A x ratio B/A
1.5 Calculation of No. of Particles: No. molecules = Moles x Avogadro =>no. MOLECULES=nx6.02x10²³ =>no. IONS=no.molecules x No. of ions in the formula
1.6 Concentration of Solutions:
1.6.1 amount of solute(moles)/volume(dm³) = moldmˉ³
1.6.2 amount of solute (grams)/volume(dm³) = gdmˉ³
1.6.3 [amount of solute (grams) / amount of solution {solute + solvent} (grams)x10^6] x 10^6/10^6=ppm TRY N WORK IT OUT SYSTEMATICALLY! USE X IF NEED BE!


  • video with explaining ppm in greater depth:
1.7 Gas Volume Calculations
1.7.1 To get Volume B from Mass A: mass A -> moles A -> moles of gas B -> volume of GAS B Moles A -> Moles B: moles A x ratio B/A Moles of gas B -> Volume of GAS B: moles B x molar volume
1.7.2 Calculations for GASES ONLY: ratio B/A x mass A = volume of GAS B


  • For Calculations involving gases only, you can skip using the molar mass or volume because you divide and then multiply the same number. So: ratio B/A x Mass A = volume of gas Bis all the working that is needed!
1.8 Percentage yield (%) = (actual yield/theoretical yield) x 100
1.9 Atom economy = (Mr of product [that you want!!] x No. of formulae of it in the equation x 100) / sum of Mr of all reactants
2 Introduction to Organic Chemistry
3 Atomic Structure and The Periodic Table
4 Energetics
4.1 Exothermic reaction = bond breaking ∴ loses heat energy to surroundings ∴ change in enthalpy is negative (-ΔH)
4.2 Endothermic reaction = bond making ∴ gains heat energy from surroundings ∴ change in enthalpy is positive (+ΔH)
4.3 The activation energy is the energy required by certain chemicals to undergo a reaction
4.4 E=mcΔT


  • E=mcΔT E- Energy transfered m- mass c- specific heat capacity ΔT- change in temperature (Specific Heat Capacity- The energy in joules (j) needed to raise the temperature of 1Kg of a substance by 1 Kelvin)
4.5 ENTHALPY OF REACTION: is when the molar quantities as written in the equation react under standard conditions (1atm pressure + a stated temp of 298K)
4.6 ENTHALPY OF FORMATION: is the enthalpy change when 1 mole of a compound is formed from its elements under standard conditions
4.7 ENTHALPY OF COMBUSTION: is the enthalpy change when 1 mol of a substance if burnt completely in oxygen under standard conditions
4.8 ENTHALPY OF NEUTRALISATION: is the enthalpy change when an acid and base react to form 1 mol of water under standard conditions
4.9 HESS'S LAW: Law which states that the energy change in an overall chemical reaction is equal to the sum of the energy changes in the individual reacti
5 Bonding
6 Weak Points

Media attachments