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Chemistry Revision Sheets - Topic 1 – The Atom

Questions Answers

What are the three subatomic particles? Proton, Neutron, Electron

State the masses of the three subatomic particles Proton (1), Neutron (1), Electron (0)

State the charges of the three subatomic particles Proton (+1), Neutron (0), Electron (-1)

What information does the ‘atomic number’ give you?

Number of protons in an atom

What information does the ‘mass number’ give you?

Number of protons and neutrons

How can you calculate the number of neutrons in an atom?

Mass number – atomic number

What is the approximate radius of an atom? 0.1 nm (1 x 10-10 m)

What is the approximate size of a nucleus? 1/10000th of the atom (or 1 x 10-14 m)

What is an isotope? Atom of the same element with the same number of protons but a different number of neutrons

In what order were the subatomic particles discovered?

Electron Proton Neutron

Describe the plum pudding model Ball of positive charge containing negative electrons

What did the alpha particle scattering experiment prove?

Atoms have a dense nucleus with a positive charge

Which scientist adapted the nuclear model of the atom by discovering electrons orbit in shells?

Niels Bohr

Which scientist’s experimental work proved that neutrons exist within the nucleus?

James Chadwick

History of the Atom

Gold foil experiment showed atoms have a dense, positively charged nucleus

1913Niels Bohr

400 BC First IdeaSpheres

Early Greece

1897Plum PuddingJJ Thompson

1905Nuclear Model

Ernest Rutherford

Electrons in shells

1932James ChadwickNeutrons exist

Chemistry Revision Sheets - Topic 2 – Elements, Compound and Mixtures

Questions Answers

Define the term ‘Atom’ The smallest part of an element that can still be recognised as that element

Define the term ‘Element’ Substance made of one type of atom only

Approximately how many elements are organised into the periodic table?

100

Define the term ‘Compound’ A substance made of two or moredifferent atoms chemically bonded together

Define the term ‘Mixture’ Two or moredifferent elements or compounds, not chemically bonded together.

What type of bonding would you find in a molecule?

Simple covalent bonding

How can you separate an insoluble solid and a liquid?

Filtration

How can you separate a soluble solid and a liquid?

Crystallisation

How can you separate the colours in an ink?

Chromatography

How does distillation work? Evaporation then condensing

Element X Element Y Mixture of Element X and Element Y

Compound of Element X and

Element Y

Chromatography Distillation

Filtration Crystallisation

Separating Mixtures

Terminology

Separate mixtures of soluble substances (ink, food colourings) Separate mixtures of two or

more substances with different boiling points. The mixture is heated until one substance evaporated and removed, then cooled to condense back to a liquid.

Separates a mixture of a liquid and an insoluble solid Separating a mixture of a soluble

solid and a liquid

Chemistry Revision Sheets - Topic 3 – Periodic Table, Groups and Trends

Questions Answers

What are the columns in the periodic table called?

Groups

What can the group tell you about the electrons in an atom?

Number of electrons in outershell

What are the rows in the periodic table called?

Periods

What can the period tell you about the electrons in an atom?

How many shells an atom has

How did scientists originally organise the periodic table?

Atomic weight

Why did Mendeleev group some elements together?

Similar chemical properties

Why did Mendeleev leave gaps in his periodic table?

For elements that hadn’t been discovered yet

How was Mendeleev proved correct? Elements matching his predictions were found.

Which alkali metal (Group 1) is more reactive, sodium or lithium?

Sodium

Which halogen (Group 7) is more reactive, chlorine or bromine?

Chlorine

Why are noble gases (Group 0) unreactive?

Full outer shells so do not need to gain/lose electrons

What is a displacement reaction? A more reactive element can take the place of a less reactive element in a compound

Group 1 – Alkali Metals• One electron in outer

shell. • As you go down the

group, the reactivity of the elements increases. This is because… more shells = more shielding = easier to lose electrons

Group 7 – Halogens• Seven electron in outer

shell. • Non-metals.• As you go down the

group, the reactivity of the elements decreases. This is because… more shells = more shielding = harder to gain electrons

• As you go down the group melting/boiling points increase. At room temp. F/Cl = Gas. Br = Liquid. I = Solid.

Group 0 – Noble Gases• Unreactive. Full outer

shells of electrons.• As you go down the

group, the boiling points of the noble gases increases.

Group Group Group1 7 0

Chemistry Revision Sheets - Topic 4a – Ionic Bonding

Questions Answers

What form of bonding is between a metal and non-metal?

Ionic

In ionic bonding, are electrons transferred or shared?

Transferred

What is an ion? Atom which has lost/gained electron(s)

Do metals form positive or negative ions? Positive

Do non-metals form positive or negative ions? Negative

If an atom gains electrons, what will the charge on the ion be?

Negative

If an atom loses electrons, what will the charge on the ion be?

Positive

What term describes the attraction between oppositely charged ions?

Electrostatic Attraction

What term describes a large structure of charged ions joined together?

Giant Ionic Lattice

What is the melting point of ionic substances? High/Low?

High

Why do ionic substances have high melting points?

Strong bonds between oppositely charged ionsare in a giant lattice structure. This requires a lot of energy to break.

Can ionic substances conduct electricity as a solid? Why/why not?

No, ions are not free to move.

Can ionic substances conduct electricity as a liquid? Why/why not?

Yes, ions are free to move and carry charge through the whole structure

Which two forms can an ionic substance be in to conduct electricity?

Molten and dissolved in water (aqueous)

Ionic Bonding – Dot Cross Diagram Example

Oxygen will gain two electrons from calcium atom to become a negative oxide ion (O2-).Oxygen has been reduced.

Calcium will transfer two electrons to an oxygen atom to become a positive calcium ion (Ca2+). Calcium has been oxidised.

Giant Ionic Lattice

Chemistry Revision Sheets - Topic 4b – Covalent Bonding

Questions Answers

What form of bonding is between non-metals only?

Covalent

In covalent bonding, are electrons transferred or shared?

Shared

What is a molecule? A small group of atoms, covalently bonded together

What are intermolecular forces? Weak forces between covalent molecules

Why do simple covalent molecules have low boiling points?

They have weak forces between molecules which take little energy to overcome.

Why can’t simple covalent molecules conduct electricity?

No charged particles (ions/delocalised electrons)

How would you describe the bonding in diamond, graphite and silicon dioxide?

Giant Covalent

How many bonds can each carbon atom form? 4

Why can graphite conduct electricity? Each carbon only forms 3 covalent bonds. One electron from each carbon atom is delocalised and can carry charge through the whole structure

Why is graphite soft? Weak forces between layers. Layers can slide

What is graphene? One layer of graphite

Give a use of fullerenes/nanotubes? Drug delivery. Conductors. Catalysts. Lubricants.

Why is diamond hard/why does it have a high melting point?

Each carbon forms 4 covalent bonds. It has a giant structure and these bonds require a lot of energy to break.

Simple Covalent Bonding – Dot Cross Diagram Examples

Giant Covalent Structures

Shared pair of electrons, single bond

Two shared pairs of electrons, double bond

Diamond Graphite

Chemistry Revision Sheets - Topic 5 – Metallic Bonding, Alloys and Polymers

Questions Answers

Describe the structure/bonding of a metal. It has positive metal ions, arranged in layers, with delocalised electrons.

Why do metals have high melting points? Strong electrostatic attraction between negative delocalised electrons and positive metal ions.

Why can metals conduct electricity? Delocalised electrons carry charge through the whole structure.

Why are metals soft? Metal ions are in layers which can slide.

What is an alloy? A mixture of two or more elements ((at least one must be a metal).

Why are alloys harder than metals? Different sizer atoms disrupt the layers. This stops sliding.

Why would you use an alloy instead of a metal? Alloys are harder, look better and are less reactive.

What is each unit of a polymer called? Monomer

What type of bonding is between the atoms in one polymer molecule?

Covalent

What type of bonding is between polymer molecules?

Intermolecular forces

Why do polymers have high melting points? Although intermolecular forces are weak, because polymers are long, they have a lot of these forces to break.

Metallic Bonding

Alloy

Positive metal ions

Monomer Polymer

Negative delocalised electrons

Different sized atoms.No layers.No Sliding.Harder.

Chemistry Revision Sheets – Topic 6 – Quantitative Chemistry

Questions Answers

What is the law of conservation of mass? No atoms are lost or made in a chemical reaction

In a reaction, the mass of reactants is less than / equal to / more than / the mass of the products.

Equal to

Why might a reaction appear to have a decrease in mass?

One product is a gas which escapes

How do you calculate relative formula mass (Mr)? Add up all mass numbers of each atom in the formula

What unit is used to measure the amount of substance?

Moles

How many particles are in one mole of a substance? 6.02 x 1023

6.02 x 1023, the number of particles in one mole, is known as…

Avogadro's Constant

What is the formula that links mass, moles and relative formula mass (Mr)?

Moles = Mass / Mr

What is the formula that links concentration, mass and volume?

Concentration = Mass / Volume

What unit is used for volume in calculations involving solutions?

Decimetre cubed (dm3 )

How do you convert from cm3 to dm3? Divide by 1000

What is the unit for concentration? g/dm3

What is a limiting reactant? The reactant that is used up first in a reaction.

Relative Formula Mass (Mr)

Mr of CaCO3?

40 + 12 + (16x3) = 100

Moles

Reacting Masses

Concentration

If you have 20g of CaCO3, how many moles is this?

Moles = Mass / Mr 20 / 100 = 0.2 moles

0.5g of lithium reacts with oxygen. How much lithium oxide is made?

2Li + O2 Li2O

Step 1) moles of lithium = mass / Mr

= 0.5 / 7 = 0.071 moles

Step 2) mole ratio Li : Li2O2 : 1

0.071 : 0.0355 moles of lithium oxide

Step 3) mass of lithium oxide = moles X Mr

= 0.0355 x (7+7+16)= 1.065g Li2O

From equation

What is the concentration if 1.5g of potassium iodide dissolves in 150cm3 of solution?

Step 1) Convert units. 150cm3 = 0.150dm3

Step 2) Concentration = Mass / Volume = 1.5 / 0.150 = 10g/dm3

Chemistry Revision Sheets - Topic 7 – Reactivity Series and Metal Extraction

Reactivity Series

Reaction with cold water

Reaction with acid

How to extract

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Questions Answers

What experiment can you do to order metals by reactivity?

Add metals to water/acid to see which reacts the most (amount of fizzing)

Which type of reaction is oxygen removed? Reduction

Define oxidation in terms of electrons Loss of electrons

Define reduction in terms of electrons Gain of electrons

What is a displacement reaction? A more reactive element takes the place of a less reactive element in a compound

Why can carbon displace zinc from zinc oxide?

Carbon is more reactive than zinc

Why can’t carbon displace magnesium from magnesium oxide?

Magnesium is more reactive than carbon

What is an ore? Material containing enough metal for it to be economically worth extracting

Why is gold found naturally in the Earth’s crust, and not need extracting?

It is unreactive

How do you extract metals which are less reactive than carbon?

Reduction with carbon

How do you extract metals which are more reactive than carbon?

Electrolysis

Describe bioleaching Bacteria can break down low-grade copper ores to produce an acidic solution containing copper ions (a leachate).

Describe phytomining Plants are grown in soil that contains low grade copper ore. Plants absorb metal ions,they’re burnt and ash contains metal compounds.

Unreactive

Copper oxide + carbon → copper + carbon dioxide

2CuO(s) + C(s) → 2Cu(l) + CO2(g)

• This is displacement; the carbon has displaced the copper.

• This is a redox reaction; the carbon has been oxidised and the copper has been reduced.

Reduction with Carbon

Chemistry Revision Sheets - Topic 8 – Electrolysis

Questions Answers

What is electrolysis? Using electricity to break down a substance

What happens to an ionic substance when it is melted or dissolved in water?

The ions become free to move around

What is the name for the positive electrode?

The anode

What is the name for the negative anode? The cathode

Do positive ions move to the anode or the cathode?

Cathode

Do negative ions move to the anode or the cathode?

Anode

Metals that are ____ reactive than carbon need to be extracted using electrolysis

More

What is the main disadvantage of using electrolysis to extract metals?

Requires a large amount of energy to melt the compounds.

Why is aluminium oxide mixed with cryolite when extracting aluminium?

To lower the melting point

What is produced at the anode and cathode in the electrolysis of aluminium oxide?

Aluminium at the cathode and oxygen at the anode

Why does the anode need to be replaced in the electrolysis of aluminium oxide?

The oxygen reacts with the carbon electrode to produce carbon dioxide.

In electrolysis of an aqueous substance, what is the rule for what is formed at the positive anode?

Oxygen is formed, unless a halogen is present.

In electrolysis of an aqueous subtance, what is the rule for what is formed at the negative cathode?

It the metal is more reactive than hydrogen, hydrogen is produced instead.

Half Equations

Aqueous – Anode Rule

Electrolyte must be molten or dissolved in water (aqueous) so that ions are free to move.

At negative cathode, hydrogen is made, unless the metal present is less reactive than hydrogen.

As a solid (giant ionic lattice) ions are not free to move so this substance cannot conduct electricity.

At positive anode, oxygen is made, unless there is a halogen present (Cl-, Br-

or I-)

Aqueous – Cathode Rule

Oxygen production at cathode: Oxygen is produced in electrolysis of aqueous substances which don’t contain a halide ion:

4OH- O2 + 2H2O + 4e-

Reduction at anode. e.g.) Cu2+ + 2e- Cu

Copper ions have gained electrons to become copper element.Oxidation at cathode. e.g.) 2Cl- Cl2 + 2e-

Chloride ions have lost electrons to become chlorine element.

In aqueous substances, hydrogen and hydroxide ions are formed by some water molecules breaking down. H2O OH- + H+

Chemistry Revision Sheets - Topic 9 – Acids, Salts and Neutralisation

Questions Answers

Define acid in terms of pH A substance with a pH of less than 7

Define acids in terms of ions A substance which releases H⁺ ions in solution

State the three common acids and give their formulaeHydrochloric acid, HCl(aq), Sulphuric acid, H₂SO₄(aq), Nitric acid, HNO₃

What is a neutral solution? A solution with a pH of 7. Water is an example.

How do you measure pH? With an indicator or pH probe.

What is a base?A metal oxide, hydroxide or carbonate that will react with an acid. E.g. copper oxide

What is an alkali? A soluble base. E.g. sodium hydroxide

Which ions are always present in a solution of an alkali? OH⁻

What type of salts are formed by the three main acids?Hydrochloric acid produces chlorides, sulphuric acid = sulphates, nitric acid = nitrates

What is a neutralisation reaction?A reaction involving an acid that results in a neutral solution

Which ions always react together in a neutralization reactions between acids and alkalis? H⁺ and OH⁻

Write the equation showing the reaction between H⁺ and OH⁻ ions H⁺ + OH⁻ → H₂O

metal + acid → → salt + hydrogen gas

metal hydroxide + acid → → salt + water

metal oxide + acid → → salt + water

metal carbonate + acid → → salt + water + carbon dioxide

What is a strong acid? An acid which completely ionises in water.

What is a weak acid? An acid which partially ionises in water.

What is a concentrated acid?An acid where there are lots of acid particles in the water.

What is a dilute acid?An acid where there are fewer acid particles in the water.

Strong Acids

Weak Acids

Fully dissociate in solution:

Partially dissociate in water:

Chemistry Revision Sheets - Topic 10 – Endothermic and Exothermic

Questions Answers

State the law of conservation of energy. Energy cannot be created or destroyed, it can only transferred from one place to another.

How does the law of conservation of energy apply to chemistry?

In all chemical reactions, energy is either transferred to the surroundings or from the surroundings.

What is an exothermic reaction? A reaction where energy is transferred to the surroundings.

Give two examples of exothermic reactions. Combustion, respiration

What happens to the temperature of the surroundings during an exothermic reaction?

It increases.

What is an endothermic reaction? A reaction where energy is transferred from the surroundings.

Give two examples of endothermic reactions. Thermal decomposition reactions, citric acid and sodium hydrogencarbonate.

What happens to the temperature of the surroundings during an endothermic reaction?

It decreases.

State two uses of exothermic reactions Self-heating cans, hand warmers

State two uses of endothermic reactions Some cooling sports injury packs

What are reactants? The substances involved in a chemical reaction

What are products? The substances formed when reactants have a chemical reaction

If the reactants have more energy than the products, what kind of a reaction must have taken place?

An exothermic one. The missing energy has been transferred to the surroundings as heat.

If the reactants have less energy than the products, what kind of a reaction must have taken place?

An endothermic one. The extra energy has been taken in by the surroundings.

Is breaking bonds endothermic or exothermic? Endothermic. (Chemical bonds are strong so require energy to break).

Is making bonds endothermic or exothermic? Exothermic. (Energy is released when chemical bonds are formed)

Reaction Profiles

How do we work out the overall energy change of a reaction? Work out the difference between the energy needed to break all the bonds in the reactants and the energy released to form all the bonds in the products.

Endothermic

Exothermic