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AY is not teaching this course in 2022-
AY is not teaching this course in 2022-
NOT UPDATED FOR 2022
NOT UPDATED FOR 2022
LOCKDOWN UPDATE:
LOCKDOWN UPDATE:
21/08/2021. Work on weeks 5 and 6 of Acids and Bases. There are page selections for each idea on the slides, if you don't have your book you can use scipad online. I have also recorded mini talks for each idea that are linked to in the slide show (only week 5 so far).
SciPAD online: use your school google account (make an account if you haven't already. Then it will ask you for a classroom join code. For Acids and Bases topic the code is: B6K1T
Week 1: Atomic Structure
Week 1: Atomic Structure
1. Atoms
Protons: Positive charge, mass of 1, in the nucleus.Electrons: Negative charge, mass of 1/2000, in shells. Neutrons: Neutral (no charge), mass of 1, in the nucleus.Atomic Number= the number of protons. The number of protons= number of electrons. Mass Number= number of protons + number of neutrons.
2. Elements
The periodic table shows all the elements- simplest form of particles (atoms).Columns are called groups= they all share similar characteristics. = All elements in a group have the same number of valence electrons in their outer shell.Rows are called periods= all elements in a period have the same numbers of electron shells.
3. Electron Configuration
Each element has a different number of electrons, these electrons are arranged in a configuration around the nucleus of the atom.Each shell has a set total number of electrons it can hold. 2 in the first shell, and a maximum of 8 in the rest.
The electron configuration is written as 2, 8, 8, 8 e.g. Mg has 12 electrons= 2, 8, 2
4. Ions
Ions form when an atom loses or gains electrons to get a full outer shell, and become stable.It will have a positive or negative charge depending on whether it gained or lost electrons. Losing electrons (-ve) means the ion has a positive charge, as it is now less negative. Positively charged ions are called Cations.Gaining electrons (-ve) means the ion has a negative charge, as it has now got more negatively charged particles. Negatively charged ions are called Anions.Ionic Compounds are a +ve and -ve ion held together by strong electrostatic forces of attraction.Week 2: Atomic Structure
Week 2: Atomic Structure
5. Counting Atoms and Chemical formulas
A large number (coefficient) at the front of the molecule tells you how many of the whole molecule there are. e.g. 5 Al₂(SO₄)₃ means there are 5 molecules of Al₂(SO₄)₃.A subscript after an atom applies just to the element in front of the number. e.g. Al₂(SO₄)₃ means there are 2 Aluminium's (Al) and 4 Oxygen's (O). A subscript after a bracket applies to the ion or compound inside the brackets. e.g. Al₂(SO₄)₃ means that there are 3 sulfate's (SO₄) in the molecule.6. Polyatomic Ions
Monoatomic Ions are ions with only one atom.Polyatomic Ions have more than one atom present (even if they are the same element).
7. Chemical Equations and Balancing Equations
Swap and Drop method for writing ionic formula. Swap the charges of the two ions, then change it to subscript. e.g. Al3+ and S2- , forms Al₂S₃ Balancing equations- you must have the same number of each element present in the products and reactants. You can only add more, rather than take atoms away. This is done by adding coefficients at the front of molecules.8. Test
Week 3: Rates of Reaction
Week 3: Rates of Reaction
1. Chemical Reactions
For a reaction to occur two or more reactant particles must collide with sufficient force and at the correct orientation. The minimum energy needed for a reaction to occur is called the activation energy.2. Rates of Reactions
The rate of reaction depends on how many particles can collide at each moment in time.3. Measuring reaction rates
How quickly a reaction occurs depends on a range of factors:-Temperature -Concentration -Surface Area -Catalysts4. Rate- Temperature
Higher temperatures mean particles have more kinetic energy, they move faster, there are more collisions, therefore a faster reaction rate compared to cold temperatures where particle move less.Week 4: Rates of Reaction
Week 4: Rates of Reaction
5. Rate- Concentration
Increasing the concentration (amount) of reactants means there will be more frequent collisions, therefore a faster reaction rate than when there is less particles present in the solution to collide.6. Rate- Surface Area
Increasing the surface area by making the size/shape of the solute smaller (solid -> powder) means more particles are exposed to the solvent, able to collide, causing more successful reactions and a faster rate of reaction.7. Catalysts
A catalysts role is to speed up a reaction. If a catalyst is present the rate of reaction is faster. Catalysts are not used up in the reaction process. (The rate decreases over time, as the reactants are converted to products, meaning less reactants to collide with)8. Test
Week 5: Acids and Bases
Week 5: Acids and Bases
1. Acids and Bases
Acids contain Hydrogen Ions (H+). Common acids in chemistry are: Sulfuric Acid (H2SO4 ), Nitric Acid (HNO3 ), and Hydrochloric Acid (HCl). Strong Acids will fully dissociate (separate atoms), weak acids will partly dissociate.Bases contain Hydroxide ions (OH-). Alkalis are bases which dissolve in water.
2. Concentration
Concentration is about how many acid or base moleculees are present in a set volume of solution. If it is a concentrated acid or base (strong) there is a high number of molecules. If it is a dilute acid or base (weak) there is a low number of molecules.3. pH and Indicators
pH scale is from 1-14. 1 is strong acid to 6 a weak acid, 7= neutral, 8 is a weak base to 14 a strong base. 1=Red, 2-4= orange, 5-6= yellow, 7= green, 8-10= blue, 11-12= indigo, 13-14= Violet.Litmus Paper: Red or Blue. If blue turns red= acid, stays blue= base. If red turns blue= base, stays red= acid.
4. Neutralisation
Neutralisation reactions change the pH to 7 (neutral), by producing water from the acid and base (as they dissociate). An acid and base reaction also forms a salt. Link the colour changes of a neutralisation to the amount of Hydrogen and Hydroxide present.The more OH- ions present, the more basic it will be (blue, indigo and violet). The more H+ ions present the more acidic it will be (Red, orange, yellow). If there are equal numbers of each it will be neutral (green).Nitric Acid forms Nitrate salts. Sulfuric Acid forms Sulfate salts. Hydrochloric acid forms Chloride salts.
Week 6: Acids and Bases
Week 6: Acids and Bases
5. Salts and Equations-
Salts and Metal Salts
Acid + Base --> Salt + WaterAcid + Metal oxide --> Metal Salt + Water
6. Salts and Equations- Carbonates
Acid + Carbonate --> Salt + Water + Carbon dioxide7. Summary
8. Test
ACIDS AND BASES SUMMARY
ACIDS AND BASES SUMMARY
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