The document describes the atomic structure of elements including protons, neutrons, electrons and isotopes. It explains how elements are arranged in the periodic table according to their atomic number and properties, with elements in the same group having similar properties. The periodic table is then used to describe the characteristics and properties of different groups of elements including metals, non-metals, transition metals, and synthetic heavy elements.

2. Atomic Structure

3. The structure of the atom
The Ancient Greeks used to believe that
everything was made up of very small particles.
I did some experiments in 1808 that proved
this and called these particles ATOMS:
Dalton
ELECTRON –
negative, mass
nearly nothing
NEUTRON – PROTON –
neutral, same positive, same
mass as proton mass as
(“1”) neutron (“1”)

4. The Atom
Nucleus Electron
Shell or Orbit

5. The Atom Hydrogen
Proton Electron
Hydrogen has one proton, one electron and NO neutrons

6. The Atom Helium
Proton Electron
Neutron
Helium has two electrons, two protons and two neutrons

8. Mass and atomic number Charge
Particle Relative Mass Relative
Proton 1 1
Neutron 1 0
Electron 0 -1
MASS NUMBER = number of
protons + number of neutrons
SYMBOL
PROTON NUMBER = number of
protons (obviously)

9. The Atom Helium
Proton Electron
Neutron
Helium has two electrons, two protons and two neutrons

10. The Atom Lithium
Protons Electrons
Neutrons

11. The Atom Beryllium
Protons Electrons
Neutrons
Beryllium has four electrons, four protons and five neutrons.

12. The Atom Boron
Protons Electrons
Neutrons
Boron has five electrons, five protons and six neutrons.

13. The Atom Carbon
Protons Electrons
Neutrons
Carbon has six electrons, six protons and six neutrons.

14. The Atom Nitrogen
Protons Electrons
Neutrons
Nitrogen has seven electrons, seven protons and seven neutrons.

15. The Atom Oxygen
Protons Electrons
Neutrons
Oxygen has eight electrons, eight protons and eight neutrons.

16. The Atom Fluorine
Protons Electrons
Neutrons
Fluorine has nine electrons, nine protons and ten neutrons.

17. The Atom Neon
Protons Electrons
Neutrons
Neon has ten electrons, ten protons and ten neutrons.

18. The Atom Sodium
Protons Electrons
Neutrons
Sodium has eleven electrons, eleven protons and twelve neutrons.

19. How many protons, neutrons and electrons?

20. Isotopes
Atoms of the same number of protons and
a different number of neutrons
Isotopes of Lithium Isotopes of Carbon

22. Sec 2; Organizing The
Elements
• Patterns in the Elements Mendeleev
• 1869: Dmitri Mendeleev made first periodic table
– arranged elements by increasing atomic mass
– switched problem elements
– made predictions for gaps
– he was right
– nominated for Nobel prize
• Henry Moseley (English chemist) found that
pattern of table was due to atomic number, not
atomic mass

24. Sec 2; Organizing The Elements
The periodic table arranges all the elements
in groups according to their properties.
Vertical
columns are Mendeleev
called GROUPS
Horizontal rows are called PERIODS

25. The Periodic Table
Fact 1: Elements in the same group have the
same number of electrons in the outer shell
Mendeleev’s
(this correspond to their group number) work
H He
Li Be B C N O F Ne
M
Na Al Si P S Cl Ar
g
C
K Ca Fe Ni Zn Br Kr
u
Ag I Xe
A H
Pt
u g
E.g. all group 1 metals These elements have These elements
have __ electron in __ electrons in their have __ electrons
their outer shell outer shells in their outer shell

26. The Periodic Table
Fact 2: As you move down through the periods
an extra electron shell is added:
E.g. Lithium has 3
electron H the
in He
configuration 2,1
Li Be B C N O F Ne
M
Na Al Si P S Cl Ar
g
Sodium has 11 C
K Ca electrons in the Ni
Fe Zn Br Kr
u
configuration 2,8,1
Ag I Xe
A H
Pt
u g
Potassium has 19
electrons in the
configuration __,__,__

27. Fact 3: Most of the elements are metals:
The Periodic Table
These elements
are metals
H He
Li Be B C N O F Ne
M
Na Al Si P S Cl Ar
g
C
K Ca Fe Ni Zn Br Kr
u
Ag I Xe
A H
Pt
u g
This line divides
These elements
metals from non-
are non-metals
metals

28. The Periodic Table
Fact 4: (Most important) All of the elements
in the same group have similar PROPERTIES.
This is how I thought of the periodic table in
the first place. This is called PERIODICITY.
H He
Li Be B C N O F Ne
M
Na Al Si P S Cl Ar
g
C
K Ca Fe Ni Zn Br Kr
u
E.g. consider the group 1 metals. They all:
Ag I Xe
A H
2) Are soft Pt
u g
3) Can be easily cut with a knife
4) React with water

30. Group 1 – The alkali metals
Li
Na
K
Rb
Cs
Fr

31. Properties of Metals
Physical Properties Chemical Properties
• Includes shininess, • Elements can combine
malleability, ductility, or react by losing
and conductivity. electrons to other atoms
• Malleable means can to produce a new
be hammered. product.
• Ductile means can be • Ex. Sodium reacts
pulled out into long strongly when exposed
wires. to air or water to produce
• Conductivity is ability of
sodium hydroxide.
element to conduct heat • Corrosion destruction of
or electricity. metals through chemical
process

32. Group 1 – The alkali metals
Some facts…
1) These metals all have ___
electron in their outer shell
2) Reactivity increases as you go _______ the group. This is
because the electrons are further away from the _______
every time a _____ is added, so they are given up more easily.
3) They all react with water to form an alkali (hence their
name) and __________, e.g:
Potassium + water potassium hydroxide + hydrogen
2K(s) + 2H2O(l) 2KOH(aq) + H2(g)
Words – down, one, shell, hydrogen, nucleus

33. Group 2- Alkaline Earth Metals
• Fairly hard.
• gray-white in colour.
• Good conductor of
electricity.
• React by losing two
electrons.
• Less reactivity than
group 1 but still more
reactive than the other
groups.

34. TRANSITION METALS
• Elements in group 3 through 12 are
called Transition Element
• Most of them are hard and shiny.
• All of them form colourful
compounds.
• All of them are good conductors of
heat and electricity.
• They less reactive than group 1 and
2 elements.
• Some of them are very important to
our health such as iron that forms
haemoglobin which carries oxygen in
our blood.

35. Metals in Mixed Groups
• they are metals in groups 13 through 15
of the periodic table.
• Aluminium is the lightweight metal that
used in beverage cans and airplanes
bodies.
• Lead is used in paints and water pipes,
but it is very poisonous and does not used
any more, now is using for batteries of car
and weights for balancing tires.
• Tin is used for coating other elements to
prevent their rust.

36. Heavy elements
• Lanthanides • Actinides
• Soft, malleable, shiny • Nuclei of those elements
metals with high are heavy.
conductivity. • Uranium is used to
• They are mixed with produce energy in nuclear
more common elements power plants.
to form alloys. • All elements heavier than
• They are found together uranium were created
and hard to separate artificially in laboratories.
them due to their similar • They are unstable that
properties. they are last for only a
fraction of second after
they are made.

37. Synthetic Elements
They are elements with atomic number
higher than 92 and follow uranium in the
periodic table.
Ex. Plutonium is made by bombarding
nuclei of uranium-238 with neutrons in a
nuclear reactor.
Scientists synthesized element 112 in
1996 by accelerating zinc nuclei and
crashing it into lead in the nuclear
accelerator.