Chemistry Paper 1Content Booklet

Topics C1 – C7

Name ________________Class ______________

Exam date: ______________________

pg. 2

Contents Page

C1 – Atomic structure

Topic Booklet Pages

Revision Guide Pages

Exam Questio

nsStructure of the atom 96 - 99

History of the atom 104

Separating mixtures 100-103

C2 – The periodic table

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Exam Questio

nsDevelopment of the periodic table 106 - 108

Group 1 109

Group 7 110

C3 – Structure and Bonding

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Exam Questio

nsStates of matter 121-122

Ionic Bonding 113 - 115

Covalent Bonding 116 -118

Fullerenes 119

Metallic bonding 120

C4 – Chemical calculations

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Exam Questio

nsRelative mass and moles 123

Equations and calculations 124-125

pg. 3

Concentrations 126

C5 – Chemical changes

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Exam Questio

nsReactivity series 130

Displacement & extracting metals 131

Required Practical: Making salts 129

pH scale 128-129

C6 – Electrolysis

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Exam Questio

nsElectrolysis 132

Extraction of aluminium 132

Electrolysis of aqueous solutions 133

C7 – Energy changes

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Exam Questio

nsExothermic and endothermic 134 - 135

Reaction profiles 136

Bond energy calculations

pg. 4

C1 – structure of the atom

Label the diagram with as much information as you can:

Fill in the table:

Proton Neutron Electron

Location

Mass

Charge

The Atom:

pg. 5

An atom contains equal numbers of protons and electrons. Atoms have no overall electrical charge because the number of positive protons equals the number of negative electrons.

Number of protons = atomic number.

All atoms of an element have the same number of protons. Atoms of different elements have different numbers of protons.

Most of the mass of an atom can be found in the nucleus. Number of protons + neutrons in the nucleus = Mass number

Element

Chemical

SymbolRelative Atomic

MassAtomic Number

Number of

Protons

Number of

Neutrons

Number of Electrons

Gold 197 79

Copper 64 29

Potassium 19

Caesium 133

Fluorine 19

Iodine 53

Chromium 24

Argon 40

Hydrogen 1

Phosphorus 31

Tin 50

Find all of the information you need for the last 2 from your Periodic Table

Silver

Aluminium

Isotopes:Atoms of the same element can have different numbers of neutrons – an isotope.The relative atomic mass of an element is an average value that takes account of the abundance of the isotopes of the element.

pg. 6

Samples of different isotopes of an element have different physical properties (e.g. different density), however, they always have the same chemical properties. It is calculated by working out the relative abundance of each isotope. The relative atomic mass is therefore calculated using the equation:

(% of isotope 1 × mass of isotope 1) + (% of isotope 2 × mass of isotope 2) ÷ 100

Electronic structure:

pg. 7

C1 – History of the atom:

Fill in the summary tables:pg. 8

DateDiagram of atomic

model

Name of the scientist

credited with model

Description of atomic model Ideas/experiments

Pre 1900

Tiny solid spheres that could not be divided

Idea that the solid sphere made up the different elements.

1897 ‘plum pudding’

A ball of positive charge with negative electrons embedded in it

Experiments showed that an atom must contain small negative charges (discovery of electrons).

1909 nuclear model

Positively charge nucleus at the centre surrounded negative electrons

Alpha particle scattering experiment showed that the mass was concentrated at the centre of the atom.

1913Bohr model

Electronsorbit the nucleus at specific distances

Electrons orbited in fixed shells; this was supported by experimental observations.

What are the sub atomic particles in an atom?

P___________________

N__________________

E__________________

What idea did John Dalton put?IDEA

Who discovered the electron? What experiments did Thomson do?

Describe Rutherford’s gold foil experiment. In 1914 Niels Bohr revised the atomic model, what did he discover?

pg. 9

Who discovered the existence of neutrons?

C1 – separating mixtures

1. A student carried out an experiment in which they measured the temperature of two substances whilst they were heated. During the experiment both substances melted.

Time in seconds 0 5 10 15 20 25 30 35 40 45 50Temperature of substance A OC 30 35 39 40 40 40 40 44 49 54 59

Temperature of substance B OC 30 35 37 39 40 42 44 46 49 54 59

What can be concluded about each chemical from the results the student obtained? Explain your answer. (4)

………………………………………..………………………………………..………………………………………..……………………………………….………………………………………..………………………………………..………………………………………..……………………………………….………………………………………..………………………………………..………………………………………..……………………………………….………………………………………..………………………………………..………………………………………..……………………………………….

pg. 10

Pure substances have specific melting and boiling temperatures.

These can be used to distinguish pure substances from mixtures.

FILTRATION: This technique separates substances that are insoluble in a solvent from those that are soluble

Explain, in terms of particles and soluble & insoluble substances, how filtration works. Use this diagram to help you.

CRYSTALLISATION: This technique separates a soluble substance from a solvent by evaporation

Explain, in terms of the kinetic energy in particles and soluble & insoluble substances, how crystallisation works. Use this diagram to help you.

SIMPLE DISTILLATION: This technique separates a liquid from a mixture by evaporation follow by condensation

Explain, in terms of the kinetic energy in particles, condensation and evaporation how simple distillation separates a mixture . Use this diagram to help you.

pg. 11

Mixtures can be separated by physical processes including:1. Filtration2. Crystallisation3. Simple distillation4. Fractional distillation5. Chromatography

These physical processes do not involve chemical reactions and no new substances are made.

FRACTIONAL DISTILLATION: This technique separates a mixture into a number of different parts, called fractions. Substances with high boiling points condense at the bottom and substances with low boiling points condense at the top.

Fractional distillation works because the different substances in the mixture have different boiling points.

Fizzy drinks are a mixture of several compounds including water, sugar, carbon dioxide. Describe how fractional distillation could be used to separate these compounds from the mixture.

CHROMATOGRAPHY: This technique separates small amounts of dissolved substances by running a solvent along absorbent paper. Chromatography involves a stationary phase and a

mobile phase.

Describe how to identify the different pigments found in a leaf using chromatography. Identify the mobile and stationary phases.

pg. 12

C2 – The periodic table

Development of the periodic table

pg. 13