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A-Level Chemistry is DIFFICULT, there’s no denying it! They don’t make it easy to study all the theory, memorise all the practicals, and apply it all to exam methodology.
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100+ Video Tutorials
We have over 100 video tutorials covering each Chemistry topic from every exam board specification
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Pre-written Chemistry flashcards for every topic so you can utilise and perfect your studying techniques
We cover every A-Level Chemistry specification
1. Atomic Structures
2. Amount of Substance
3. Bonding
4. Energetics
5. Kinetics
6. Organic Chemistry
7. Alkanes
8. Thermodynamics
And More!
1. Atomic Structures
11 Lessons
Atomic structure refers to the structure of an atom comprising a nucleus (centre) in which the protons (positively charged) and neutrons (neutral) are present. The negatively charged particles called electrons revolve around the centre of the nucleus.
Tutorials
Lesson 1 Fundamental Particles
Lesson 2 Subatomic Particles
Lesson 3 Electron Arangement
Lesson 4 Electrons in Atoms
Lesson 5 Mass Numbers
Lesson 6 Element Isotopes
Lesson 7 Mass Spectrometry
Lesson 8 Electron Configuration
Lesson 9 Trends along Period
Lesson 10 Ionisation Energies
Lesson 11 Measuring Relative Masses
Lesson 1
Fundamental Particles
Quarks are fundamental particles of matter that make up protons and neutrons. Leptons are a type of fundamental particle that includes electrons.
The arrangement of electrons within an atom is called the electronic configuration and the electrons are filled up according to the energy of the levels as: 1s, 2s, 2p and more.
Isotopes are different forms of the same atom that differ solely in the number of neutrons they have. The mass number of an element is determined by the number of protons and neutrons added together: mass number = protons + neutrons.
Isotopes are different forms of the same atom that differ solely in the number of neutrons they have. The mass number of an element is determined by the number of protons and neutrons added together: mass number = protons + neutrons.
A mole is the SI unit for the amount of substance. The amount of elementary entities in a mole is equal to the number of atoms in 12g of the carbon-12 isotope. The number of entities per mole is the Avogadro constant or 6.022 x 10^(23).
Tutorials
Lesson 1 RAM
Lesson 2 RMM
Lesson 3 The Mole and the Avogadro Constant
Lesson 4 Calculating Percentage Yield
Lesson 5 The Ideal Gas Equation
Lesson 6 Empirical and Molecular Formula
Lesson 7 Stoichiometric Calculations
Lesson 8 Balanced Equations and Calculations
Lesson 9 Balancing Chemical Equation
Lesson 10 Further Mole Calculations
Lesson 1
RAM
RAM is a mass of an atom, relative to the mass of C-12. Since it is a ratio, it is unitless. 2. RMM is a mass of a molecule, relative to the mass of C-12.
RAM is a mass of an atom, relative to the mass of C-12. Since it is a ratio, it is unitless. 2. RMM is a mass of a molecule, relative to the mass of C-12.
One mole of a substance is equal to 6.022 × 10²³ units of that substance (such as atoms, molecules, or ions). The number 6.022 × 10²³ is known as Avogadro's number or Avogadro's constant.
The ideal gas law can be written in terms of the number of molecules of gas: PV = NkT, where P is pressure, V is volume, T is temperature, N is number of molecules, and k is the Boltzmann constant k = 1.38 × 10–23 J/K.
Chemists employ balanced equations to calculate how much product will be produced from their reactants. In balanced equations, the co-efficients denote the amount of moles reacting and being created; however, this exact ratio is rarely employed in a reaction.
Chemical bonding is the creation of a chemical compound by forming a chemical link between two or more atoms, molecules, or ions. The atoms in the resultant molecule are held together by chemical bonds.
Tutorials
Lesson 1 Ionic Bonding
Lesson 2 Covalent and Dative Covalent Bonding
Lesson 3 Metallic Bonding
Lesson 4 Bonding and Properties
Lesson 5 Shapes of Molecules and Ions
Lesson 6 Bond Polarity
Lesson 7 Forces Between Molecules
Lesson 8 Predicting Bonding
Lesson 9 Bond Polarity
Lesson 10 Molecular Shapes
Lesson 11 Forces Between Molecules
Lesson 1
Ionic Bonding
The electrostatic attraction between oppositely charged ions in a chemical molecule forms an ionic bond, also known as an electrovalent bond.
When two atoms share an electron pair, they form a covalent connection, which is a type of chemical bond. A dative bond occurs when one atom donates its electron pair to another atom. They differ from one another in terms of how they form.
Chemical bonds can hold atoms together. Atoms can develop a stable electron configuration when they form bonds. Atoms can lose, gain, or share electrons to establish a stable electron configuration.
Bond polarity is the separation of electric charge along a bond in chemistry, resulting in an electric dipole or dipole moment in a molecule or its chemical groups. Between two bonding atoms, electrons are not always shared equally.
The electromagnetic forces of attraction and repulsion that act between atoms and other types of nearby particles, such as atoms or ions, are examples of intermolecular interactions (or secondary forces).
Understand the energy changes that occur throughout a reaction and apply what you've learned to predict how chemical reactions will behave.
Tutorials
Lesson 1 Enthalpy Change
Lesson 2 Calorimetry
Lesson 3 Application of Hess's Law
Lesson 4 Bond Enthalpies
Lesson 5 Lattice Enthalpies
Lesson 6 Enthalpy of Hydration
Lesson 7 Enthalpy of Solution
Lesson 8 Total Entropy Changes
Lesson 9 Calculations Involving Free Energy
Lesson 10 Entropy Changes Prediction
Lesson 1
Enthalpy Change
The heat energy shift caused by a chemical reaction or process at a constant pressure is known as enthalpy change. The enthalpy change for a reaction is denoted by the symbol rH and is measured in kJ mol-1.
Calorimetry is a technique for determining how much heat is generated or absorbed during a chemical reaction. It is possible to identify whether a process is exothermic (releases heat) or endothermic (stores heat) by measuring the change in heat (absorbs heat).
The Maxwell-Boltzmann equation, which is the foundation of gas kinetic theory, determines the speed distribution for a gas at a given temperature. The most likely speed, the average speed, and the root-mean-square speed can all be calculated using this distribution function.
A reaction mechanism is the step-by-step sequence of elementary reactions that results in total chemical change in chemistry. A chemical mechanism is a theoretical hypothesis that attempts to describe in detail what happens at each stage of a chemical reaction as a whole.
The phenomenon of isomerism occurs when two or more compounds have the same chemical formula but distinct chemical structures. Isomers are chemical compounds with identical chemical formulae but differ in characteristics and atom arrangement in the molecule.
An alkane, often known as paraffin is an acyclic saturated hydrocarbon in organic chemistry. To put it another way, an alkane is made up of hydrogen and carbon atoms arranged in a tree structure with single carbon–carbon bonds.
Tutorials
Lesson 1 Fractional Distillation of Crude Oil
Lesson 2 Modification of Alkanes by Cracking
Lesson 3 Combustion of Alkanes
Lesson 4 Chlorination of Alkanes
Lesson 5 Reactivity of Halogenoalkanes
Lesson 6 Environmental impact of Halogenoalkanes
Lesson 7 Alkene reactivity
Lesson 8 Alcohol oxidation
Lesson 9 Alcohol production
Lesson 10 Practical Purification Techniques
Lesson 1
Fractional Distillation of Crude Oil
The method by which oil refineries split crude oil into different, more valuable hydrocarbon compounds depending on their relative molecular weights in a distillation tower is known as fractional distillation.
Alkanes are cracked by breaking C–C bonds. Thermal cracking yields a large percentage of alkenes when it occurs at high pressure and high temperature (mechanism not required).
Chlorination of alkane gives a mixture of different products. When consider mechanism of alkanes chlorination, free radicals are formed during the reaction to keep the continuous reaction. Learn the products and the mechanisms.
The study of the relationships between heat, work, temperature, and energy is known as thermodynamics. The rules of thermodynamics define how energy evolves in a system and whether it can do beneficial work on its surroundings.
Tutorials
Lesson 1 Lattice Enthalpies
Lesson 2 Enthalpy Key Terms
Lesson 3 Construction of Born-Haber Cycles
Lesson 4 Calculations involving Born-Haber Cycles
Lesson 5 Enthalpy of Hydration
Lesson 6 Enthalpy of Solution
Lesson 7 Calculating Enthalpy of Solution
Lesson 8 Introduction to Entropy
Lesson 9 Total Entropy Changes
Lesson 10 Entropy Change Predictions
Lesson 11 Gibbs Free Energy
Lesson 12 Calculations Free Energy
Lesson 1
Lattice Enthalpies
The strength of the forces between the ions in an ionic solid is measured by lattice enthalpy. The stronger the forces, the higher the lattice enthalpy.
The Born Haber cycle is a series of enthalpy changes in a process that results in the synthesis of a solid crystalline ionic compound from elemental atoms in their standard state and a net enthalpy of formation of the solid compound of zero.
The enthalpy change associated with the dissolving of a substance in a solvent at constant pressure, resulting in infinite dilution, is known as the enthalpy of solution, enthalpy of dissolution, or heat of solution.
Entropy is the amount of thermal energy in a system per unit temperature that isn't available for meaningful work. Because work is generated by ordered molecular motion, entropy is also a measure of a system's molecular disorder, or unpredictability.
We can calculate total entropy change if we have the entropy changes of the system and its surrounds. The sum of the system and its surrounds is the total entropy change.
The Gibbs free energy is a thermodynamic potential in thermodynamics that can be used to calculate the maximum work that a thermodynamically closed system can accomplish at constant temperature and pressure.
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