Name _______________

Class _______________

Aylsham High School Science

Year 7
C1: Atoms and the
periodic table

Contents:
Core Knowledge
Concept 1: Models of Atoms
Concept 2: Atoms, elements, compounds and mixtures
Concept 3: Chemical symbols
Concept 4: Chemical and physical change
Concept 5: Physical and chemical properties of elements
Concept 6 :The periodic table
5 quick questions templates
Core Knowledge

What is an atom? The smallest part of an element that can exist

Describe Dalton’s model of the atom. Atoms as solid spheres that cannot be
divided into smaller parts
What is an element? A substance made of one type of atom
e.g oxygen=O2, Iron= Fe
What is a molecule? A particle made of two or more atoms
joined together e.g. Oxygen =O2,
Water =H2O
What is a diatomic molecule? A molecule that consists of two
atoms, often the same. E.g. O2 , Cl2
What is a chemical symbol? A one or two universal letter code of each element
Where are chemical symbols of elements found? In the periodic table
What is a compound? A substance made of more than one type
of atom chemically joined together. E.g.
Water = H2O, Carbon dioxide = CO2
What is a chemical formula? A formula that shows the number and type of
atoms present in a molecule.
What do the compound endings: 1) ide – a compound of only the named
1) ide substances
2) ate 2) ate – a compound of the named substances
mean? and oxygen
What is a physical change? Changes of state as no new substances are made.
What is a chemical change (Chemical reaction)? When atoms rearrange to make new substances
Where do we find metals in the period table? On the left
Where do we find non-metals on the periodic On the right
table?
Who designed the modern periodic table? Mendeleev
What are the groups in the periodic table? Columns
What are the rows called in the periodic table? Periods
What are the physical properties of most metals? Good conductors of electricity, good conductors of
heat, shiny, high density (heavy for its size),
malleable (can be hammered), sonorous (makes a
ringing sound when hit ), ductile (can be pulled
into wires), high melting points (except mercury),
hard
What are the physical properties of non-metals? Poor conductors of electricity, poor conductors of
heat, dull, low density (light for its size), brittle (
breaks easily), non-sonorous ( no ringing sound
when hit), low melting points
Concept 1: Models of Atoms
We are going to look at what atoms are and how we use a simple model to describe them

John Dalton published his ideas about atoms in 1803. He thought that all
matter was made of tiny particles called atoms, which he imagined as tiny
solid balls.

In 1803, an English scientist, , carried out experiments

with different elements. From his experiments he found that:

 different elements seemed to consist of particles (atoms). He described atoms as tiny, hard balls.

 He thought that each chemical element had its own kind of atom.

 Although he did not know what their structure was, he knew he had found out something
important.

Element, atom , John Dalton, elements, atoms

What is an atom?
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Draw a picture of Dalton’s model of the atom.

Can we see atoms?

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Where do we find atoms?
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Concept 2: Atoms, elements, compounds and mixtures
We are going to explore the differences between elements, compounds and mixtures and use our model of
an atom to help us explain these

A substance made from only one type of atom is called an element.

Elements are listed on the periodic table.

Atoms can be drawn as circles. But all the atoms of an element need to look exactly the same e.g.

Atoms can form strong bonds with each other, making molecules.

A molecule is a particle made of two or more atoms joined together

More than one type of element joined together makes a compound.

When drawing a diagram of molecules made from the atoms of more than one
element, different sizes and colours can show the different elements. E.g.

A mixture consists of two or more different substances, not chemically joined together e.g Air

What is an element? Definition and particle diagram.

How many different types of element are there?

Give some examples of elements?

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What do scientists make if different elements are joined together?
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Draw a particle diagram to represent two different elements joined together? E.g. Salt NaCl

What do scientists make if different elements are not joined together?

 Investigating compounds and mixtures:

1. Would you describe iron as an element, mixture or compound?

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2. Draw a diagram showing what the particles might look like in pure iron.
Explain your diagram.

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3. Would you describe sulfur as an element, mixture or compound?

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4. Draw a diagram showing what the particles might look like in pure sulfur. Explain your diagram

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Now watch the teacher:
5. When the teacher mixed the 2 together how would you describe them?

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6. Draw a diagram showing what the particles might look like when iron and sulfur are mixed. Explain
your diagram
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Watch what happens when you bring a magnet near:

7. How and why could you separate the mixture of iron and sulfur?
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Watch what happens when you heat the substances:
8. What did you observe when the mixture of iron and sulfur was heated.
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9. What has been made? How could you describe it?
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10. Draw a diagram showing what the particles might look like when iron and sulfur have reacted with one
another. Explain your diagram ________________________________________________
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Let’s compare and contrast elements, compounds
and mixtures:
Compound Mixture
Does the
substance have
a fixed
composition?
Give some
examples

Joined
together?

Draw a diagram
to show how
the particles
could be
arranged
Properties
compared to
the particles it
made from

Can it be
separate?
Concept 3: Chemical symbols
Each element is represented by its own chemical symbol. A chemical symbol:
 consists of one or two letters
 always starts with a capital letter, with any other letter in lower case
For example, the element mercury is shown as Hg. Do not show it as HG, hg or hG.

Symbols and formulae

1. Which is the correct symbol for Hydrogen?

H h Hy hy

2. Which is the correct symbol for Potassium?

P Po K k

3. What is the correct symbol for Magnesium?

mg M mG Mg

4. What is the correct symbol for Chlorine?

C cl CL Cl

5. Which is the correct symbol for Carbon?

C Ca c CA

6. Which is the correct symbol for Iron?

I Ir Fe FE

7. What is the correct symbol for Copper?

CU Cu cU cu

8. What is the correct symbol for Oxygen?

O OX ox Ox
 The chemical formula of a compound shows how many of each type of atom join together to
make the units which make up the compound.

The first Three rules for working out formula

1. Every time there is a new capital letter there is a new element to count. For example:
 CO = 1 x Carbon and 1 x Oxygen.
 Whereas, Co = 1 x Cobalt

2. If there is no number present (big or small) there is actually an invisible number 1. For example:
 CuSO4 would probably be more clear if it were written like this 1Cu1S1O4 and contains 1 x
Copper, 1 x Sulphur and 4 x Oxygen

3. If a big number is before a substance everything needs to be multiplied by that number. For
example:
 4H2O = 4 x 2 = 8 Hydrogen and 4 x 1 = 4 Oxygen

Look carefully at the list of chemicals below,

Br2, He, H2, H2O, O2, Cl2, I2, NH3, N2, CO2, HF, F2, CH4, HBr, C2H4, Ne,
From the list write down the formula of any elements
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From the list write down the formula of any substances that contain 2 atoms
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From the list write down the formula of any compounds that contain 3 atoms
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From the list write down the formula of any compounds that contain 4 atoms
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From the list write down the formula of any compounds that contain 5 atoms
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From the list write down the formula of any compounds that contain 6 atoms
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Are all the substances with 2 atoms compounds?
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 Some non-metal elements exist as simple molecules with two atoms joined together.
We say that these elements are diatomic. To show this, their formulae contain a
subscript number 2. For example:
hydrogen, H2, nitrogen, N2, oxygen, O2, fluorine, F2, bromine, Br2, chlorine, Cl2, iodine, I

What is a diatomic molecule?

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Why are He, Ne, Xe called monoatomic substances?
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What do Br2, H2, O2, HF, F2, HBr all have in common?
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Which ones are elements?
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Which ones are compounds?

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Why are Br2, H2, O2, HF, F2, HBr called diatomic molecules?
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Draw a diagram of each of the chemicals:

Br2 H2 O2 HF F2 HBR
 1. What elements have we got?
Let’s practice the rules:
2. What little numbers do they have?
3. Are there any big numbers?

CO H2O
Element Number of atoms Element Number of atoms

Total Total

CO2 2MgO
Element Number of atoms Element Number of atoms

Total Total

CuSO4 N2
Element Number of atoms Element Number of atoms

Total Total

C6H12O6 4Li2OH
Element Number of atoms Element Number of atoms

Total Total
 Ones to learn! This year you will be tested on the elements in year 8 and 9
elements and compounds.

•Write an expression that represents each molecule diagram.

Use the following key:

Settling
task
Molecule diagram Expression
 Compelte the table:

Name Picture Atom, element or Formula

compound,
Mono/diatomic?
Oxygen
( Two oxygen atoms
joined togther)

Carbon
( A single carbon atom)

Water
( 2 hydrogen atoms
joined to oxygen)

Carbon dioxde
( 2 oxygen atoms joined
to 1 carbon atom)

Bromine
( Two bromine atoms
joined togther )

Hydrogen
( Two hydrogen atoms
joined together)

Sodium
( A single sodium atom)

Sodium chloride
( A sodium atom joined
to a chlorine atom)

Sulfur
( A single sulfur atom)

Carbon monoxide
( A carbon atom joined
to a oxygen atom)
 Naming compounds

Naming compounds is easy if you follow these 3 simple rules.

Rule one
The element that is furthest left in the periodic table comes first, eg Sodium Chloride/Carbon dioxide
Rule two
If there are only two elements in the compound then the compounds name ends in –ide, eg A compound
of copper and sulfur is called copper sulfide.
Rule three
If the compound contains three elements one of which is oxygen then the compound name will end in –ate
or –ite, eg Calcium carbonate contains calcium, carbon and oxygen.
Additional point: Sometimes more than one compound is made from the same elements. For example,
there are several different types of nitrogen oxide.
When this happens, the number of a particular type of atom is shown by using ‘mono-’ (one), ‘di-’ (two) or
‘tri-’ (three).

Carbon Monoxide Nitrogen dioxide Sulfur Trioxide

Naming compounds

Use the naming rules you have learnt to answer the following questions.

1. Compounds that contain oxygen and one other element are called oxides.
Name these oxides: (3)
a. MgO _______________________________
b. CaO _______________________________
c. Na2O _______________________________
2. Some oxides contain more than one oxygen atom. Name these oxides: (3)
a. CO2 _______________________________
b. SO2 _______________________________
c. SO3 _______________________________
3. Compounds that contain sulfur and one other element are called sulfides.
Name these sulfides: (3)
a. FeS _______________________________
b. ZnS _______________________________
 c. H2S _______________________________

4. Compounds that contain chlorine and one other element are called chlorides.
Name these chlorides: (3)
a. KCl _______________________________
b. NaCl _______________________________
c. HCl _______________________________
5. Compounds that contain oxygen, sulfur and one other element are called sulfates.
Name these sulfates: (3)
a. CuSO4 _______________________________
b. ZnSO4_______________________________
c. Na2SO4 _______________________________
6. Compounds that contain oxygen, carbon and one other element are called carbonates.
Name these carbonates: (3)
a. CuCO3 _______________________________
b. Na2CO3 _______________________________
c. MgCO3 _______________________________
7. Compounds that contain oxygen, nitrogen and one other element are called nitrates.
Name these nitrates: (3)
a. NaNO3 _______________________________
b. KNO3 _______________________________
c. AgNO3 _______________________________

8. Now you've got the hang of it, try naming these compounds: (12)
a. LiCl ____________________ g. CaCO3 ____________________
b. MgSO4 ____________________ h. K2SO4 ____________________
c. Li2O ____________________ i. RbNO3 ____________________
d. CaS ____________________ j. CaCl2 ____________________
e. ZnO ____________________ k. NiS ____________________
f. LiNO3 ____________________ l. K2CO3 ____________________

Extension:
9. These may look a bit different, but you can use the same rules. Try naming them: (4)
a. Al2O3 ____________________ c. Al2(SO2)3 ___________________
b. Zn(NO3)2 ____________________ d. Al2(CO3)3 ___________________
10. Suggest names for these compounds: (4)
a. KBr ____________________ c. AlPO4 ___________________
b. BN ____________________ d. NaHCO3 ___________________
All:
When does a compound end in-ide?
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When a compound end in does –ate?
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Now lets put it all together

Elements found in the Name of compound Number of each element

compound

MgO Magnesium and Oxygen 1 Mg and 1 O

K2O

CuBr2

NaNO3

FeS

FeSO4

CaCO3
Concept 4: Chemical and physical change
We are going to explore the differences between a chemical and physical change

A physical change: Changes of state as no new substances are made.

 “In a physical change the arrangement of the particles

changes, but the composition of the particles (what is
actually inside them) does not change.

 Another way of saying this is that the physical state of the

substance changes, but the substance itself stays the same.

 The substance is the same at the beginning and at the end.

No new substance has been formed.”

A chemical change: When atoms rearrange to make new substance

 “A chemical reaction involves

atoms rearranging to form a new
substance that wasn’t there
before. The composition of the
particles always changes, the arrangement of particles may also change.

 You can think of atoms a bit like lego pieces. Imagine taking one or more objects made of lego, then
rearranging the pieces to build something new. That’s basically what a chemical reaction is”

 “The process is often difficult to reverse: Once atoms have rearranged into a new substance, it can
be difficult (but not impossible) for them to rearrange back to how they were at the start.

Substances I saw… (all your Was something Can it be reversed? Chemical or

mixed observations) new made? If so, how? physical
change?
Task 1

Physical change
 Task 2: Chemical Physical
Change Change
1) A new substance is formed

2) Boiling

3) Baking a cake

4) Rotting fruit

5) Lighting a candle

6) Melting candle wax

7) Atoms rearrange and bond with different ones

8) Particles rearrange into a regular order, all touching

9) CO2 (g) → CO2 (s)

10) C (s) + O2 (g) → CO2 (g)

Task 3
Concept 5: Physical and chemical properties of elements
We are going look at the varying physical properties of different elements

The position of an element on the periodic table provides information about its properties.

The majority of elements are metals and they are found on the left and in the middle of the
periodic table.
Metals and non-metals have different properties and different reactions.
Complete the table as you are shown different elements

Name Metal/ Appearance Melting Conducts Density Malleable

non metal point electricity Ductile
and heat? Brittle?

Oxygen

Magnesium

Copper

Chlorine

Carbon

Sodium

Most metals share a lot of properties, such as being good conductors of heat and electricity.
Non-metals often have the opposite properties. For example, they are usually poor conductors of
heat and electricity.
 Task:
Complete the table:

How did you tell apart the metals form the non-metals?
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Concept 6 :The periodic table
We are going to look at how the periodic table is ordered to show a list of elements

What do you think?

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______________________________ ______________________________
______________________________ ______________________________
______________________________ ______________________________
______________________________ ______________________________
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 Like many scientists working at the end of the 19th-century the Russian chemist Dmitri
Mendeleev (1834-1907) was looking for ways to organise the known elements. Mendeleev
published his first periodic table of the elements in 1869. Mendeleev arranged the elements in
order of increasing mass. When he did this he noted that the chemical properties of the elements and their
compounds showed various trends. He then arranged the elements by putting those with similar
properties below each other into groups. To make his classification work Mendeleev made a few changes
to his order.

Task 1 : Highlighted the following on your periodic table –Metals, Non-metals, Group 1, Group 2,
Transition Metals, Group 7 and Group 0/8.
Task 2: Complete the table

Symbol Name Period Group

H Hydrogen Period 1 Not really in a group

Period 2 Group 1

Period 2 Group 3

Period 2 Group 5

Oxygen

Fluorine

Na Sodium Period 3 Group 1

Mg

Period 3 Group 3

Si Silicon

Period 3 Group 5

Period 3 Group 6

Period 3 Group 7

Ar Argon

K Potassium

Ca
5 quick questions templates
Test 1: Test 2:

Question 1 Question 1

Question 2 Question 2

Question 3 Question 3

Question 4 Question 4

Questions 5 Question 5
Test 3: Test 4:
Question 1 Question 1

Question 2 Question 2

Question 3 Question 3

Question 4 Question 4

Questions 5 Question 5
Test 5: Test 6:
Question 1 Question 1

Question 2 Question 2

Question 3 Question 3

Question 4 Question 4

Questions 5 Question 5
Formula Literacy check Elements: