Year 10 The Periodic Table - For additional resources visit: http://www.iheartscience.net

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
www.wpclipart.com

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.
www.askamathematician.com

19. • Electrons are negative and attracted to the
positive nucleus.
• The number of electrons and protons is the
same.
Galleryhip.Com

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.
Galleryhip.Com

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.
commons.wikimedia.org

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

29. ignatius10science.weebly.com

30. Bonding
• Atoms that are joined = molecules or large
lattices.
• These atoms are held together by chemical
bonds.
catalog.flatworldknowledge.com

31. Group 18 of the periodic table are the noble
gases – they are extremely stable and rarely
bond with other atoms.
commons.wikimedia.org

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.
www.allaboutcircuits.com

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.
www.gcsescience.com

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.
commons.wikimedia.org

36. Opposite charges attract and the electrostatic
force provides bonding between the positive
ions and the loose electrons surrounding them.
www.bbc.co.uk

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.
chemistry.tutorvista.com

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.
en.wikibooks.org

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.
chemwiki.ucdavis.edu

40. Non-metals only share enough electrons to fill
their outer-shell or have eight electrons in their
outer-shell.
www.ducksters.com

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.
http://periodictable.com/index.html

42. Alkaline Earth metals all react in a similar way –
just slightly less reactive.
http://periodictable.com/index.html

43. Group 14
These elements display a wide range of
properties.
– non-metal carbon
– metalloids silicon and germanium
– metallic tin and lead
http://periodictable.com/index.html

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.
http://periodictable.com/index.html

45. Group 18 – the Noble Gases
• Colourless
• Occur naturally in the atmosphere.
• Incredibly stable and only react under extreme
circumstances.
http://periodictable.com/index.html

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.
http://periodictable.com/index.html