All substances are made of atoms, which are the building blocks of matter. Atoms contain a nucleus with protons and neutrons surrounded by electrons. Elements are substances made of only one type of atom, with 118 known elements. The periodic table arranges elements based on their chemical and physical properties, grouping them according to their atomic structure and how they bond with other atoms through ionic, metallic, or covalent bonds to form molecules or crystalline structures.

1. vimeo.com
The Periodic Table
Sarah Jones

2. Atoms and Elements
• All substances are made of ATOMS.
• Substances that are made of only ONE type of
atom are called ELEMENTS.

3. Elements
• Elements are the building blocks of matter.
• 118 known elements.
He Helium
H Hydrogen
Au Gold
N Nitrogen
Pb Lead
K Potassium

4. Image Source: http://www.periodictable.com/theelements/pages.html

16. The Structure of Atoms
• Neutrons = neutral
• Protons = positive charge
• Electrons = negative charge
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17. The Nucleus
• At the centre of an atom.
• Made up of protons and neutrons.
• Neutrons are heavier than protons – both are
much heavier than electrons.
• Atomic Number = Number of Protons

18. Electron Shells
• Electrons spin around the nucleus. They don't
stay in defined areas around the nucleus. They
are found in clouds that can have different
shapes.
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19. • Electrons are negative and attracted to the
positive nucleus.
• The number of electrons and protons is the
same.
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20. • The electrons spin around the nucleus in
electron shells.
• The closer the shell is to the nucleus the
greater the attraction.
• Closer shells have lower energy levels and the
outermost shells the highest energy level.
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21. Maximum number of electrons = 2n2
Shell Max. Number of Electrons
n = 1 2
n = 2 8
n = 3 18
n = 4 32

22. commons.wikimedia.org

23. The Periodic Table
Elements arranged based on the similarities of
their chemical and physical properties - colour,
size, density, freezing and boiling points.
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24. www.ducksters.com

25. chemistry.about.com

26. Groups

27. • Groups are numbered 1-18 or an older way is
I-VIII in Roman Numerals.
• Using the group numbers 1-18 – the last digit
is usually the number of electrons in the outer
shell.

28. Periods

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30. Bonding
• Atoms that are joined = molecules or large
lattices.
• These atoms are held together by chemical
bonds.
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31. Group 18 of the periodic table are the noble
gases – they are extremely stable and rarely
bond with other atoms.
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32. • All other atoms react, gain, lose or share
electrons – result is a bond.
• The result is particles with full outer shells
that hold eight electrons.
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33. Ions
• Ions are atoms that have become charged
because they have had electrons removed –
or because they have removed electrons
from other atoms.
• No longer neutral.
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34. • Positively charged ions (+) have more protons
– lose electrons.
• Negatively charged ions (-) have more
electrons – gain electrons.

35. Metallic Bonding
• Metal atoms only have a weak hold on their
outer-shell electrons.
• The outer-shell electrons can move
throughout the metal without being bound to
any one atom.
• Each metal atom becomes a positively
charged ion.
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36. Opposite charges attract and the electrostatic
force provides bonding between the positive
ions and the loose electrons surrounding them.
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37. Ionic Bonding
• When metallic elements bond with non-metallic
elements.
• Metal atoms – weak hold on outer-shell
electrons.
• Non-metallic atoms – strong hold on outer-shell
electrons.
• Non-metallic tend to remove outer-shell
electrons from any metal atoms they are near.
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38. • Electrostatic forces pull the +ve and –ve ions
together to form a strong ionic bond.
• Result in a three-dimensional structure called
a lattice.
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39. Covalent Bonding
• When non-metallic atoms bond with each
other.
• Non-metals can’t remove electrons from other
non-metals.
• They share some of their outer-shell electrons
and form covalent bonds.
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40. Non-metals only share enough electrons to fill
their outer-shell or have eight electrons in their
outer-shell.
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41. Group 1 and 2 – Alkali Metals and
Alkaline Earths
Alkali metals form +1 ions, are too reactive to be
found naturally in pure form, have typical metal
properties, display similar chemical behaviour,
react violently with water producing an alkaline
solution and hydrogen gas.
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42. Alkaline Earth metals all react in a similar way –
just slightly less reactive.
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43. Group 14
These elements display a wide range of
properties.
– non-metal carbon
– metalloids silicon and germanium
– metallic tin and lead
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44. Group 17 – the Halogens
• Atoms form ions with a charge of -1.
• Are not found in nature in pure form – found
in salts.
• Get bigger and less reactive as you move
down the group.
• All form molecules of two atoms.
• Have coloured and poisonous vapours.
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45. Group 18 – the Noble Gases
• Colourless
• Occur naturally in the atmosphere.
• Incredibly stable and only react under extreme
circumstances.
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46. Transition Metals
• Groups 3-12
• Many of the most useful, colourful and
valuable metals.
• All tend to be relatively hard with high melting
points.
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