I made this for my national 5 chemistry test in lockdown , I hope you enjoy

1. National 5 Chemistry
Chemical Changes and Structure
Atomic Structure

2. • Atoms
• Protons/neutrons/electrons
• Atomic number and mass number
• Metals/non-metals zigzag line
• Chemicals with similar chemical
properties/valency arranged in the
same group.
• Elements outer electron number
indicates group number
For more practice, read and complete all
questions from the Nat 5 ‘Chemistry’ purple
textbook. pages 11-16.
You should know..

3. 1. Convert info about atomic number and mass number into
the numbers of protons, neutrons and electrons
2. Use nuclide notation to represent numbers of
protons/neutrons in ions and atoms
3. Distinguish between atoms/ions by comparing the
number of positive protons to the number of negative
electrons
4. Identify isotopes of elements (atoms of the same
element with different mass numbers)
5. Explain that the relative atomic mass of an element is an
average mass of all the isotopes present taking into
account their relative proportions
Mandatory Key Areas

4. To learn how convert info about atomic number and
mass number into the numbers of protons,
neutrons and electrons
Learning Intention
Success Criteria
• I can define atomic number and mass number
• I can represent the atomic number in terms of
the numbers of protons or electrons in an atom
• I can represent the mass number in terms of
the numbers of protons and neutrons in an atom
• I can calculate the number of sub atomic
particles if given the mass number and atomic
number.

5. The Periodic Table

6. Structure of the Atom
Copy diagram
Video

7. Sub Atomic Particles
Sub-atomic
particle
Charge Mass
Location in the
atom
Proton 1 + 1 amu In the Nucleus
Electron 1 - 0 amu
Electron shells
outside the
nucleus
Neutron 0 1 amu In the Nucleus

8. Atomic number = number of protons
Number of protons = number of electrons
Atomic Number
Element
Atomic
Number
No of
protons
No of
electrons
Oxygen
3
19

9. Mass number = protons + neutrons
Number of neutrons = mass – atomic
Mass Number
Element Mass Number
Atomic
Number
No of
neutrons
12 6
11 12
Potassium 39

10. Electrons are arranged in shells, each only
holding a maximum number of electrons
Electron Arrangements

11. Lithium:
Atomic number = 3
No of electrons = 3
Electron arrangement = 2,1
Now you write the electron arrangement and
draw how the electrons are arranged for
a) carbon b) oxygen c) sodium
Electron Arrangements

12. To learn how convert info about atomic number and
mass number into the numbers of protons,
neutrons and electrons
Learning Intention
Success Criteria
• I can define atomic number and mass number
• I can represent the atomic number in terms of
the numbers of protons or electrons in an atom
• I can represent the mass number in terms of
the numbers of protons and neutrons in an atom
• I can calculate the number of sub atomic
particles if given the mass number and atomic
number.

13. Calculating Sub-Atomic Particles
Complete the first 5 rows in the what you need to know booklet.
Element
Atomic
Number
Mass
Number
Number
of
Protons
Number
of
neutrons
Number
of
Electrons
12
C
6
22
Ne
10
18
O
8
24 12
7 3

14. • Atom
• Proton
• Electron
• Nucleus
• Neutron
• Electron shells
• Electron
arrangements
• Atomic number
• Mass number
Key Words to Know
Ensure that you know the definitions of the
following words:

15. To distinguish between atoms/ions by comparing
the number of positive protons to the number of
negative electrons
To learn use nuclide notation to represent numbers
of protons/neutrons in ions and atoms
Learning Intention
Success Criteria
• I can define an ion and explain how they are made
• I can distinguish between an ion and an atom
• I can convert information about the number of
sub-atomic particles into nuclide notation.

16. Nuclide Notation - Atoms
This is a shorthand way of writing the atomic
number, mass number and symbol of an atom.

17. Nuclide Notation - Atoms
1. K 2. Cl
39
19
37
17
3. Na 4. C
23
11
12
6

18. Nuclide Notation - Atoms
1. K 2. Cl
39
19
37
17
3. Na 4. C
23
11
12
6
p = 17
e = 17
n = 20
p = 11
e = 11
n = 12
p = 6
e = 6
n = 6
p = 19
e = 19
n = 20

19. • Nuclide Notation
• Ions
• Stable electron arrangement
Key Words to Know
Ensure that you know the definitions of the
following words:

20. To distinguish between atoms/ions by comparing
the number of positive protons to the number of
negative electrons
To learn use nuclide notation to represent numbers
of protons/neutrons in ions and atoms
Learning Intention
Success Criteria
• I can define an ion and explain how they are made
• I can distinguish between an ion and an atom
• I can convert information about the number of
sub-atomic particles into nuclide notation.

21. To learn how to about isotopes of elements and
how to identify them
To be able to explain and calculate the relative
atomic mass (RAM) of an element
Learning Intention
Success Criteria
• I can define what is meant by an isotope
• I can determine the number of sub-atomic
particles in each isotope
• I can explain what is meant by RAM and carry out
calculations to determine the RAM of an atom

22. Isotopes
Look at the nuclide notation for the atoms of
chlorine below:
Cl Cl
37 38
17 17
How are they different from each other?
How are they the same?

23. Isotopes
Atoms of the same element
but with different masses
are called isotopes.
This is due to the fact that
they have:
• the same number of
protons
• different numbers of
neutrons.

24. Isotopes
Isotope
Atomic
number
Mass
number
No of
protons
No of
electrons
No of
neutrons
video

25. Relative Atomic Mass (RAM)
Relative atomic mass is the average mass of all
the isotopes for a particular element.
An isotope of 35Cl is present in 75% and there is
25% of 37Cl. Calculate the RAM.
RAM = (% abundance x mass) + (% abundance x mass)
100
RAM = (75 x 35) + (25 x 37)
100
RAM = 35.5 a.m.u.

26. Relative Atomic Mass (RAM)
Relative atomic mass is the average mass of all
the isotopes for a particular element
Copper has 2 isotopes:
1. What is the RAM of Copper?
2. What does this tell us about the abundance
of each of the copper isotopes?

27. Relative Atomic Mass (RAM)
Relative atomic mass is the average mass of all
the isotopes for a particular element
Bromine has 2 isotopes : 79 Br 81 Br
1. What is the RAM of bromine?
2. What does this tell you about the
abundance of each isotope in the element?

28. Relative Atomic Mass (RAM)
1. Copper : 2 isotopes
63 Cu = 69.1%
65 Cu = 30.9%
2. Silicon : 3 isotopes
28Si = 93.17%
29Si = 4.71%
30Si = 2.12%
3. Boron : 2 isotopes
10B = 20%
11B = 80%

29. To learn how to about isotopes of elements and
how to identify them
To be able to explain and calculate the relative
atomic mass (RAM) of an element
Learning Intention
Success Criteria
• I can define what is meant by an isotope
• I can determine the number of sub-atomic
particles in each isotope
• I can explain what is meant by RAM and carry out
calculations to determine the RAM of an atom

30. To distinguish between atoms/ions by comparing
the number of positive protons to the number of
negative electrons
To learn use nuclide notation to represent numbers
of protons/neutrons in ions
Learning Intention
Success Criteria
• I can define an ion and explain how they are made
• I can distinguish between an ion and an atom
• I can convert information about the number of
sub-atomic particles into nuclide notation.

31. When there is a different number of protons and
electrons in a particle it is no longer an atom. The
particle will now have a charge and is known as an
ION.
Ions form when an atom loses or gains electrons to
achieve a stable electron arrangement similar to the
noble gases in group 8. This will mean that the
number of electrons will be different to those in the
corresponding atom, therefore there will be an upset
in the overall charge of the particle.
Ions

32. Consider the two particles of potassium below:
Ions
39
19
K
39
19
K+Electron arrangement
2,8,8,1
Electron
arrangement
2,8,8
p = 19
e = 19
n = 20
p = 19
e = 18
n = 20

33. Nuclide Notation - Ions

34. Nuclide Notation- Ions
Ion Atomic
number
Mass
number
No of
protons
No of
neutrons
No of
electrons
35
Cl-
17
17 35 17 18 18
40 20 18
16 16 18
Now fill in the last 2 rows in the table in the “What You need to Know”
booklet.
Finished?? Do Q7 on pg 28 of the small, purple N5 question book.

35. To distinguish between atoms/ions by comparing
the number of positive protons to the number of
negative electrons
To learn use nuclide notation to represent numbers
of protons/neutrons in ions
Learning Intention
Success Criteria
• I can define an ion and explain how they are made
• I can distinguish between an ion and an atom
• I can convert information about the number of
sub-atomic particles into nuclide notation.