Download 2017 Yr10 Ext Chem program Rev2

Year 10 Science
Extension
Term 1: CHEMISTRY
Text: Pearson Science 10 SB 2e
Year 10 Chemical Sciences Content Descriptions
The atomic structure and properties of elements are used to organise them in the Periodic Table (ACSSU186)
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recognising that elements in the same group of the periodic table have similar properties
describing the structure of atoms in terms of electron shells
explaining how the electronic structure of an atom determines its position in the periodic table and its properties
investigating the chemical activity of metals
Different types of chemical reactions are used to produce a range of products and can occur at different rates (ACSSU187)
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investigating how chemistry can be used to produce a range of useful substances such as fuels, metals and pharmaceuticals
predicting the products of different types of simple chemical reactions
using word or symbol equations to represent chemical reactions
investigating the effect of a range of factors, such as temperature and catalysts, on the rate of chemical reactions
Wk
Topic
Content
Activities
Resources and Experiments
Assessment &
Homework
1
Atomic
Structure

AB: 5.1 – Knowledge preview
SB: p193 prac 1 –
Investigating a metallic
element
Unit Review
Questions SB:
5.1 p192
SB 5.1

2
Ionic
Compounds
Revise the structure of an atom. Explain that the
existence of atoms has been shown using a
scanning tunnelling microscope (STM). The
existence of sub-atomic particles has been
postulated using indirect evidence.
All elements are basically structurally the same.
They have protons and neutrons in the nucleus
and the nucleus is orbited by electrons. The
number of protons determines the type of
element. The number of protons is known as the
atomic number. The atomic mass is the number
of protons plus the number of neutrons.

Discuss how analogies and models can be used
to help with the visualisation of abstract
concepts.

Explain that all atoms of the same element have
the same number of protons in the nucleus but
that the number of neutrons can vary.
Understand that ionic bonding occurs between
metals and non-metals. In ionic bonding atoms
gain a full outer shell of electrons through metals
give electrons to non-metals causing the
formation of ions
Know the properties of ionic compounds and
describe them
o Can conduct electricity when molten or
aqueous but not solid
o High melting and boiling points
o Hard
o Brittle
Understand that in ionic solids the ions are
organised in a lattice, but when ionic solids are
placed in solution the ions separate.
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
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SB: p194 prac 2 –
Investigating a nonmetallic element
Chemical formula writing
worksheet- polyatomic and
simple plus Lewis structures
Chemical bondingintroduction and properties of
metallic and ionic worksheet
Experiments- A rough
diamond from page 124
using soft lollies to make
diamond
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Topic
Content
Metallic
compound


Covalent
compound
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

Understand that in metallic bonding metals lose
their valence electrons to form positive ions. The
lost valence electrons become delocalised and
are shared amongst all the metal ions forming a
sea of electrons
Use the atomic structure of metallic compounds
to explain the properties of metals
o Good conductors of heat and electricity
o Hard
o High melting and boiling points
o Malleable and ductile
Understand that covalent bonding occurs
between non-metals. The atoms share electron
pairs to gain a full outer shell of electrons.
Covalent substances can either be found as
molecules or networks
Use the structure of covalent compounds to
explain their properties
o Molecules
 Poor conductors of heat and
electricity
 Brittle and soft when solid
 low melting and boiling points
o Networks
 high melting and boiling points
 strong and hard
 Can sometimes conduct
electricity
Activities
Resources and Experiments
Assessment &
Homework
Wk
Topic
Content
Activities
3
Arranging the
elements

AB: 5.2 – Periodic nature of the
elements
SB 5.2
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
Family
groupings
SB 5.3
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



How the periodic table is arranged. Use Figure
5.2.1 to assist.
Define the terms period and group as related to
the periodic table. Outline the two numbering
systems for the groups. Explain why elements in
the same group have similar properties.
The concept of grouping in the periodic table
means that certain elements within the same
group will have similarities. However, there are
also a lot of differences within the family
groupings. Outline the importance of the
groupings, but also remind students of their
differences.
The properties of the alkali metals. Explain
where they can be found in the periodic table.
The properties of the Group 14 elements. Where
they can be found in the periodic table and
compare their diversity to the other groups
The properties of the halogens. Explain where
they can be found in the periodic table.
The noble gases and their unreactive nature.
Explain where they can be found in the periodic
table.
The properties of the transition metals. Explain
where they can be found in the periodic table.
AB: 5.5 – Organic chemistry
(Extension activity)
AB: 5.6 – Hydrocarbons
(Extension activity)
SB: p208 SkillBuilder –
Predicting chemical equations
AB: 5.4 – Families of the periodic
table
Resources and Experiments
SB: p204 prac 2 – Cardgame analogy
Alkali metals and alkaline
earths, the halogens, noble
gases, transition gases.
SB: p213 Prac 1 – The
alkaline earths
SB: p204 Prac 2 – Halogen
precipitates
Assessment &
Homework
Unit Review
Questions
SB:5.2 p202
Unit Review
Questions SB:
5.3 p212
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Topic
Content
Activities
4
Electrons and
the periodic
table
 Discuss how the development of human
SB: p216 SkillBuilder – Electron
configuration
SB: 5.4
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




understanding of atomic structure influenced the
periodic table. Explain how scientists came to
understand that the electrons were largely
responsible for the chemical activity of elements.
Explain how electrons do not orbit the nucleus in
a completely random way. They are arranged in
energy levels or shells. Define the term electron
configuration.
Explain that electrons can gain or lose energy. As
electrons gain energy they gain kinetic energy
and move into high orbits around the nucleus as
they lose energy the kinetic energy is converted
to light and heat. (Remind students that energy is
never created or destroyed; it is changed from
one form to another.) The amount of energy being
lost as light determines the colour of the flame.
Emphasise that all elements in the same group
have the same number of outer shell electrons.
Explain that each period has one more shell than
the previous period. This means that although
elements are in the same group their properties
are a little different.
Emphasise that all elements in the same group
have the same number of outer shell electrons.
Explain that each period has one more shell than
the previous period. This means that although
elements are in the same group their properties
are a little different.
Explain why elements in the same group have
similar properties.
Discuss why the properties of elements change
down a group.
AB: 5.7 – Electron configuration
and shells
SB: p222 Prac 1 – Firework
colours
SkillBuilder – Periods and
groups
SB: p218 Worked example –
Periods and groups
Resources and Experiments
Assessment &
Homework
Unit Review
Question SB:
5.4 p221
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Topic
Content
Activities
Resources and Experiments
5
Chemical
equations

AB: 6.1 – Knowledge preview
SB: p236 Prac 2 –
Conservation of mass
SB: 6.1

Explain that chemical equations are a simple
method for giving a detailed description of the
changes which take place during a chemical
reaction. Chemical equations can be written in
words but convey much more information if
symbols are used. An even more informative
equation uses symbols for the chemicals and
also indicates the state of those chemicals.
States can be solid, liquid or gas or aqueous.
Explain aqueous is not a state of matter but
means the substance is dissolved in water.
Revise the terms product and reactant.
Emphasize that matter is not gained or lost
during chemical reactions so every atom must be
accounted for on both sides of a chemical
equation. When the number of atoms of each
atom is the same in the products and reactants
then the equation is balanced.
SB: p235 Prac 1 – Reactions with
modelling clay
SB: p232 STEM4fun –
Conserving mass in chemical
reactions
SB: p236 SkillBuilder –
Balancing equations
SB: p233 Worked example –
Balancing equations
AB: 6.8 – Balancing chemical
equations
Assessment &
Homework
Atomic
Structure,
Periodic table,
Bonding, topic
test
Unit Review
Questions SB:
6.1 p234
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Topic
Content
Activities
Resources and Experiments
Assessment &
Homework
6
Energy in
Chemical
Reactions

Revise the concept that the bonds between
atoms in compounds store energy.
SB: p237 science4fun –
Acrobatic flame

Unit Review
Questions SB:
6.2 p242
Define the terms exothermic and endothermic.
Explain that in endothermic reactions the
products possess more energy than the
reactants and that the reverse is true for
exothermic reactions.
SB: p243 Prac 1 –
Exothermic and
endothermic reactions
AB: 6.2 – Combustion of
magnesium
SB: 6.2
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7
8
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Combustion

Corrosion
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Respiration
The atomic structure and properties of elements are
used to organise them in the Periodic Table
(ACSSU186)
SB: 6.3
 investigating the chemical activity of metals
Different types of chemical reactions are used to
produce a range of products and can occur at
different rates (ACSSU187);
 investigating how chemistry can be used to

SB: p245 Prac 3 – Rust
prevention
These reactions are all exothermic but
combustion reactions are more vigorous and
produce large amounts of heat and light quickly.
Investigation
Classifying
Chemical
Reactions

SB: p241 SHE – Biofuels
Reactions with oxygen include:
SB: p244Prac 2 –
Corrosion as an
exothermic reaction
produce a range of useful substances such as
fuels, metals and pharmaceuticals
using word or symbol equations to represent
chemical reactions
predicting the products of different types of simple
chemical reactions
SB: p246 science4fun – Raisin
lava lamp
SB: p251 SkillBuilder –
predicting precipitation reactions
SB: p251 Worked example –
Predicting precipitation
reactions.
AB: 6.3 – Classifying chemical
reactions
AB: 6.4 – Classifying chemical
reactions in context
SB: p255 Prac 1 – Heating
metal carbonates
Investigation
validation
SB: p256 Prac 2 –
Precipitation reactions
Unit Review
Questions SB:
6.3 p254
SB: p257 Prac 3 –
Identifying unknown
solutions Student design
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Topic
Content
Activities
Resources and Experiments
Assessment &
Homework
9
Rates of
Chemical
Reaction
 Explain that reactions can occur at different rates.
 Explain that the rates of chemicals reactions can
SB: p258 science4fun – Jellied
fruit
SB: p266 Prac 1 –
Temperature and reaction
rate
Unit Review
Questions SB:
6.4 p265
be influenced by external factors. Discuss each of
these factors and how they change the rate of
SB: 6.4
reaction. These factors include:

Temperature

Concentration of the reactants

Surface area of the reactants

Agitation (stirring of the reactants)
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Use of catalysts (either chemical or
enzymes)
AB: 6.5 – Reaction rate and
surface area of reactants
AB: 6.6 – Fast and slow reactions
AB: 6.7 – Rate of chemical
reactions–particle diagrams
SB: p263 Working with science –
Molecular gastronomy chef
SB: p267 Prac 2 –
Concentration and reaction
rate
SB: p268 Prac 3 – Agitation
and reaction rate
SB: p269 Prac 4 – Surface
area and reaction rate
Student design
SB: p264 SHE – Enzymes in
medicine
10
Topic Test
Equations, Reactions
Topic Test
Assessment Outline
Assessment Type
Title
Weighting
Test
Topic test.
10%
Practical Investigation and Validation
Electrolysis
10%