Subject: Chemistry Year: 7 and 8 Term: Topic: C1 The Particulate Nature of Matter Topic: Lesson Sequence 1. Matter and its Properties 2. The Particle Model 3. Particle Behaviour 4. Changing State 5. Gases 6. Water 7. Mixtures 8. Filtering 9. Evaporation 10. Chromatography 11. Distillation

Key Assessments Assessment: Melting Ice Cube EA Exam 2

Core Texts Smart Science Text Book

Key Words

Chromatogram The picture or pattern of coloured results produced by a chromatography experiment.

Element Substances made of only one type of atom.

Chromatography Process in which different coloured chemicals are separated from a mixture based on their solubility.

Evaporating basin

Scientific equipment made of ceramic, used to encourage evaporation of a liquid.

Contract When a substance reduces in volume. Expand To increase in volume.

Density How much mass or matter there is in a given volume.

Filter paper Used to separate a mixture based on the size of the molecules/substance. Large molecules/substances are held back by the paper smaller molecules/substances may pass through.

Diffusion Particles (in a liquid or gas) moving from an area of high concentration to a lower concentration.

Funnel Scientific equipment used to hold filter paper.

Dissolve Combining a solute with a solvent to make a solution.

Gas One of the three states of matter - particles have low density.

Distillation Used to separate mixtures based on the boiling points of the chemicals. Chemicals are evaporated and condensed.

Insoluble When a solute will not dissolve in a given solvent.

Changing State: When a substance moves from one state to another. Caused by the heating or cooling of a substance or a change in pressure. Heating/Decrease Pressure Melting: Solid Liquid Boiling: Liquid Gas Sublimation: Solid Gas Cooling/Increase Pressure Freezing: Liquid Solid Condensation: Gas Liquid Deposition: Gas Solid

Particle Behaviour

Structure of an Atom

State Changes

Key Words

Liquid One of the three states of matter. Rf Factor A measure of how easily a substance dissolves in a solvent. Calculated by 'Distance moved by spot'/ 'Distance moved from start'.

Matter A general name for the 'stuff' all substances are made up of. Solid Substances in a state with a fixed shape and volume.

Melt When a solid is heated to become a liquid (reaches its melting point). Solubility Ability to dissolve in a liquid/solvent.

Mixture Different substances combined physically but not chemically, can be separated. Soluble Will dissolve.

Particles Small pieces (such as atoms or molecules) that make up a substance. Solute A solid that dissolves in a liquid to form a solution.

Particle Theory Description of how particles behave in solids, liquids and gases. Solvent The liquid in which a solid is dissolved to form a solution.

Pressure Measure of the ‘concentration of a force’ in an area (Pressure = Force/Area). State The particular state that a substance is in at that time, solid, liquid or gaseous.

Pure A substance containing the atoms or molecules of only one substance. Vibrate A regular back and forth movement.

Random No pattern, unpredictable.

Chromatography Method 1. Draw a straight line in pencil 1 cm from the bottom of the

chromatography paper. 2. Place a dot of ink on the pencil line. 3. Dip the paper in a solvent (usually water). 4. Hold paper in place until solvent has absorbed to the top of

paper. 5. Remove paper from solvent and leave to dry. 6. Substances move at different speeds based on how well they

dissolve in a given solvent. 7. Measure the distance the solvent travelled and the distance

each spot moved in cm. Use this to calculate each spots Rf

value.

Chromatogram and Calculating Rf Value

Filtration Method 1. Fold round filter paper into quarters, and

open to form a triangular shape. 2. Place filter paper into a filter funnel. 3. Pour suspension or solution into filter paper. 4. Tiny pores in the filter paper will allow

liquids and small particles through, but undissolved solids or large particles will be too large to pass through the holes in the paper.

5. Solids left behind are called the residue. 6. Liquid that passes through the filter is called

the filtrate.

Distillation Method

1. Water and ethanol mixture is heated. 2. Ethanol has a lower boiling point (70°C) than water (100 °C), so begins to boil and evaporate (turn into a gas) first. Different substances boil at different temperatures. 3. Ethanol evaporates first. 4. The thermometer shows the boiling point of pure ethanol. 5. & 6. Cool tap water enters the condenser (7) at point 6, warm water leaves at point 5. 7. As gas vapour passes through the tube surrounded by the condenser (7), heat is lost to the cool water and the gas condenses to a liquid. 8. Pure liquid ethanol is collected in a beaker at the end of the condenser tube.

Subject: Science Year: 7 and 8 Term: Topic: C4 Acids and Alkalis Topic: Lesson Sequence 1. Everyday Acids and Alkalis 2. Universal Indicator 3. Red Cabbage Indicator 4. Acid Concentration 5. Neutralisation 6. Naming Salts 7. Indigestion 8. Indigestion Assessment 9. Acids Rain 10. Acids and Metals Key Assessments

Indigestion Assessment EA Exam 1

Core Texts SMART Science Textbook

Common Acids and Bases (Alkalis)

Acid Base (alkali)

Hydrochloric Acid Sodium hydroxide Lemon Juice Milk

Vinegar Soap/Shampoo

Nitric Acid Bleach

Sulfuric Acid Calcium carbonate

Making Red Cabbage Indicator – Method

Collect red cabbage.

Add boiling water and leave for 5 minutes.

Crush cabbage and water mixture using a mortar and pestle.

Filter mixture, discard unfiltered cabbage, use the filtrate.

Indicator turns red in acidic conditions, blue/purple in neutral conditions and yellow/green in basic conditions.

Naming Salts The first part of the salts name comes from the metal. The second part of the salts name comes from the acid.

Acid Salt Formed

Hydrochloric Acid …………… chloride

Sulfuric Acid …………… sulfate

Nitric Acid …………… nitrate E.g. magnesium + hydrochloric acid magnesium chloride + hydrogen

Key Words

Acid Substances with a pH less than 7, they neutralise alkalis. Limewater A solution of calcium hydroxide that goes white when carbon dioxide passes through it.

Acid Rain Rain in which sulfur dioxide (or nitrogen dioxide) has been dissolved making it acidic.

Litmus Paper Coloured paper that changes colour in acids (red) or alkalis (blue).

Alkali Substances with a pH greater than 7, they will neutralise acids and are bases that will dissolve in water.

Neutral A solution of pH 7.

Antacid A tablet (containing the base, calcium carbonate) given to treat indigestion and neutralise stomach acid.

Neutralisation Reacting an acid and alkali to form a neutral solution containing a salt.

Base Solid or powdered substances that neutralise acids, some may dissolve in water to form alkalis.

pH Scale used to measure the strength of acids and alkalis.

Concentration

How many particles of a certain type are present in a liquid or gas.

Reactivity Series

A list of substances, often metals, in order of their reactivity.

Corrodes Process in which a compound is worn away by chemical reactions e.g. Rusting.

Salt A chemical containing a metal and a non-metal element formed by the reaction of an acid and an alkali.

Corrosive A chemical that causes corrosion. Sodium chloride

A salt formed by mixing hydrochloric acid and sodium hydroxide, the scientific name for common table salt.

Hazard Symbol

Labels on chemical containers that warn about the ways in which a chemical can be dangerous.

Squeaky pop test

Test for hydrogen, a glowing split makes hydrogen gas burn with a squeaky pop sound.

Indicator Chemicals that change colour depending on the pH. Sulfur dioxide The common cause of acid rain, along with nitrogen dioxide.

Indigestion Pain or discomfort in the stomach caused by the production of too much stomach acid.

Tarnish A layer of oxide forms on a metal making it look dull and not shiny.

Irritant A substance causing slight inflammation or discomfort to the body.

Universal Indicator

A mixture of dyes that change colour depending upon pH.

pH Scale

Reactions of Acids

Acid + alkali Salt + WaterAcid + Metal Salt + HydrogenAcid + Metal hydroxide Salt + WaterAcid + Metal oxide Salt + WaterAcid + Carbonate Salt +Carbon dioxide + Water