These notes were the ones I had compiled over the course of my A Levels, which took my grade from a B to consistently above 90%, including in my actual A Level in which I achieved 289/300 (96.3%), so I know these contain all the information you could possibly need to achieve a high score in the act...
A* PHYSICAL CHEMISTRY
A LEVEL NOTES
Marlowe Taylor
,Contents
Atomic Structure (1.1) ......................................................................................................... 3
Fundamental particles (1.1.1) ...................................................................................................................................... 3
Mass number and isotopes (1.1.2) ............................................................................................................................... 4
Electron configuration (1.1.3) ....................................................................................................................................... 6
Amount of Substance (1.2) .................................................................................................. 9
Relative atomic mass and relative molecular mass (1.2.1) ............................................................................................ 9
The mole and the Avogadro constant (1.2.2) ................................................................................................................. 9
The ideal gas equation (1.2.3) ...................................................................................................................................... 9
Empirical and molecular formula (1.2.4) .................................................................................................................... 10
Balanced equations and associated calculations (1.2.5) ........................................................................................... 10
Bonding (1.3) .................................................................................................................... 12
Ionic bonding (1.3.1) .................................................................................................................................................. 12
Nature of covalent and dative covalent bonds (1.3.2) ................................................................................................. 12
Metallic bonding (1.3.3) ............................................................................................................................................. 13
Bonding and physical properties (1.3.4) ..................................................................................................................... 13
Shapes of simple molecules and ions (1.3.5).............................................................................................................. 15
Bond polarity (1.3.6) .................................................................................................................................................. 16
Forces between molecules (1.3.7) ............................................................................................................................. 17
Energetics (1.4)................................................................................................................. 19
Enthalpy change (1.4.1) ............................................................................................................................................. 19
Calorimetry (1.4.2) .................................................................................................................................................... 19
Applications of Hess’ Law (1.4.3) ............................................................................................................................... 21
Bond enthalpies (1.4.4) .............................................................................................................................................. 21
Kinetics (1.5) .................................................................................................................... 22
Collision theory (1.5.1)............................................................................................................................................... 22
Maxwell-Boltzmann distribution (1.5.2) ...................................................................................................................... 22
Effect of temperature on reaction rate (1.5.3) ............................................................................................................. 22
Effect of concentration and pressure (1.5.4) ............................................................................................................... 23
Catalysts (1.5.5) ........................................................................................................................................................ 23
Chemical equilibria, Le Chatelier’s principle, and Kc (1.6) .................................................... 24
Chemical equilibria and Le Chatelier's principle (1.6.1) .............................................................................................. 24
Equilibrium constant, Kc for homogeneous systems (1.6.2) ........................................................................................ 24
Oxidation, reduction, and redox reactions (1.7) ................................................................... 25
Equilibrium constant Kp for homogenous systems (1.10)...................................................... 32
Electrode potentials and electrochemical cells (1.11) ......................................................... 33
Electrode potentials and cells (1.11.1) ....................................................................................................................... 33
Commercial applications of electrochemical cells (1.11.2) ........................................................................................ 35
Acids and Bases (1.12) ...................................................................................................... 38
Bronsted-Lowry acid-base equilibria in aqueous solutions (1.12.1)............................................................................. 38
Definition and determination of pH (1.12.2) ................................................................................................................ 38
The ionic product of water, Kw (1.12.3) ........................................................................................................................ 38
Weak acids and bases, Ka for weak acids (1.12.4) ....................................................................................................... 38
pH curves, titrations, and indicators (1.12.5) .............................................................................................................. 39
Buffer action (1.12.6) ................................................................................................................................................. 40
Page 2 of 40
, Atomic Structure (1.1)
Fundamental particles (1.1.1)
Particle Position Relative Mass Actual Mass (kg) Relative Charge Actual Charge (C)
Proton Nucleus 1 1.673x10-27 +1 +1.6x10-19
Neutron Nucleus 1 1.675x10-27 0 0
Electron Orbitals 1/1800 9.11x10-31 -1 -1.6x10-19
When neutrons were discovered, model was improved – knowledge and understanding of atomic
structure has evolved over time.
Models of the atom:
Dalton Thomson Rutherford Bohr
The first model Plum Pudding Model Nuclear Model Most recent model
- Every form of - Discovered the - Fired alpha - Found that
matter was made electron, theorised particles at a thin electrons orbited
up of small that the atom was film of gold foil the nucleus in fixed
individual particles a plum pudding energy levels – this
model – a ball of - Discovered that came from
- All matter is made positive charge most of the atom excitation energies
of atoms – with negative was empty space,
individual spheres electrons and positive - Better than
embedded in it charge is Rutherford’s model
- All atoms of a given concentrated in a as it does not
element are small, central, collapse inwards
identical in mass massive nucleus
and properties
- Electrons orbit this
- Compounds are nucleus
combinations of
different atoms - This disproved
Thomson’s work
which gave rise to
the nuclear model
Page 3 of 40
The benefits of buying summaries with Stuvia:
Guaranteed quality through customer reviews
Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.
Quick and easy check-out
You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.
Focus on what matters
Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!
Frequently asked questions
What do I get when I buy this document?
You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.
Satisfaction guarantee: how does it work?
Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.
Who am I buying these notes from?
Stuvia is a marketplace, so you are not buying this document from us, but from seller marlowetaylor. Stuvia facilitates payment to the seller.
Will I be stuck with a subscription?
No, you only buy these notes for $13.69. You're not tied to anything after your purchase.
