The document explains the organization of the periodic table, highlighting group numbers that indicate valence electrons and the periodicity of elements. It discusses the atomic radius, ionization energy, electron affinity, and electronegativity, emphasizing trends as one moves across periods and down groups. Various factors influencing these properties, such as nuclear charge and electron shielding, are also mentioned.

2. The structure of the
Periodic Table

4. GROUPS
Group numbers
indicate
the amount of
valence
electrons in the
relevant
element’s
atom.

5. Valence electrons
Electrons that occur in
the highest (outer)
energy level of the
atom.

6. PERIODSThere are seven periods on the
Periodic Table.
The period number will indicate the amount of energy
levels that an atom consist of.

7. O
is in group 6, so has
6 valence electrons.
ydghkjgjl
3s24p4
Group
6
Period
3
Ca
is in group 2, so has
2 valence electrons.
4s2
Group
2
Period
4

8. Recurring pattern of
physical and chemical
properties as you move
across the Periodic Table.
Periodicity

9. The elements of the same
group have similar
properties. These
properties differ from left
to right.
Periodic Law

10. Atomic Radius

11. Distance from the
nucleus and the
outermost stable
electron orbital.
Atomic Radius

12. Decreases
• Atomic number increases from left to right.
• This means the nuclear charge increases.
• The electrostatic forces between the nucleus
and electrons increase, pulling electrons closer.
• Thereby decreasing the atomic radius.

13. I
n
c
r
e
a
s
e
s
• The main energy levels increase by one
as you move down one period, thus
taking up more space.
• The valence electrons are further away
from the core.
• The electrons from the inner orbitals
shield the outer electrons,
• Which weakens the attractive forces of
the core on the outer electrons.

14. Meltingpointandboilingpoint
Metals
Non-metals

15. Density
Metals
Non-metals

16. Ionisation
energy

17. Energy required to
remove the electron
from an atom in the
gaseous state.
Ionisation energy

19. Factors that influence ionisation energy:
Nuclear charge
Atomic radius
Electron repulsion

20. Successive
ionisation
energies

21. • When the first electron is removed, the
nuclear charge increases, holding the
remaining electrons tighter.
• To remove the next electron requires
more energy.

22. The change in energy
when an electron is added
to a neutral atom or ion in
the gaseous phase.
Electron affinity

24. Electron affinity increases from left
to right.
Decreases from top to bottom.

25. The amount of energy
released when an electron
is added to atoms in the
ground state.
Electronegativity

26. Pauling Scale

28. OLIVIER, A. : Physical Sciences Theory and Workbook Book 2 Chemistry, Grade 10; AmaniYah .
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