chemistry-the-periodic-table.ppt

© Boardworks Ltd 2004
KS4 Chemistry
The Periodic Table

The Periodic Table
Contents
Elements and atomic number
Arranging elements
Electronic structure
Patterns of behaviour
Teacher resources

What are all substances made of?
…to gold, an unreactive metal.
From chlorine, a poisonous gas…
From sodium, a reactive metal…
There are millions of different substances in the world
but what are they all made of?
Elements the building blocks of all substances.
There are about 100 different elements in a variety of forms.
…to oxygen, a life-giving gas.

Properties of elements
What is a property of an element?
A property is any characteristic of an element.
For example, here are some properties of sodium:
It would be really useful to be able to predict properties
of elements instead of having to remember them!
metallic
highly reactive
solid but melts easily
feels light (low density)
Are there any patterns in the properties of elements?

Properties and atomic number
particle charge relative mass
proton +1 1
neutron 0 1
electron -1 0.0005
Scientists discovered that the properties of elements
seemed to depend on atomic number.
What is the atomic number of an element?
Atoms contain three types of particles:
Where are these particles found in an atom?

What is atomic number?
Atomic number = the number of protons in an atom
proton
electron neutron
helium
nucleus
What are the particles in this helium atom?
What is the atomic number of helium?

Atomic number and electrons
Atoms of elements contain equal numbers of protons
and electrons.
Atoms of elements have no charge, they are neutral.
What is the charge on a fluorine atom?
19
F
9
How are the number of electrons and atomic number
related in a neutral atom?
9 protons
9 electrons
10 neutrons
charge = +9
charge = - 9
charge = 0
total charge = 0
They are the same.
How does this affect the charge of such atoms?

Atomic number and patterns
K
H Li Na
Be Mg Al P
N O S Cl
F Ne Ar
Si
He B C
reactive metals
unreactive gases
reactive gases
When scientists arranged elements in order of increasing
atomic number they found patterns in their properties.

Positions of similar elements
How many elements are there from one reactive metal
to the next?
How many elements are there from one reactive gas
to the next?
K
H Li Na
Be Mg Al P
N O S Cl
F Ne Ar
Si
He B C
19
1 3 11
4 12 13 15
7 8 16 17
9 10 18
14
2 5 6
8
8
Compare the positions of similar elements.
reactive gases reactive metals

Arranging elements
Arranging these strips in rows…
Divide the elements at set intervals, arrange them according
to their properties and what patterns do you see?
cut here
K
H Li Na
Be Mg Al P
N O S Cl
F Ne Ar
Si
He B C
19
1 3 11
4 12 13 15
7 8 16 17
9 10 18
14
2 5 6
cut here
cut here
NaMg Al P S Cl Ar
Si
H He
Li Be N O F Ne
B C
K

Arranging elements
K
He
Al P S
Si
Mg
Na Ar
Cl
Be N O
B C
Li Ne
F
When elements are arranged according to their properties
what patterns do you see and what element is missing?
reactive
metals
unreactive
gases
reactive
gases
Similar elements go into the same columns.
Hydrogen is an exception. This reactive gas is best
positioned above the reactive metals.
H
hydrogen is a
special case

The periodic table
Arranging all the elements by atomic number and properties
led to the creation of…
the periodic table
H He
Fr Ra Rf Db Sg Bh Hs Mt ? ?
Ac ?
K Ca Ga Ge As Se Kr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Br
Cs Ba Tl Pb Bi Po Rn
Hf Ta W Re Os Ir Au Hg
La Pt At
Na Mg Al Si P S Ar
Cl
Li Be B C N O Ne
F
Rb Sr In Sn Sb Te Xe
Y Zr Nb Mo Tc Ru Pd Ag Cd
Rh I

Columns of elements
H
Li
Na
K
Rb
Cs
Fr
Be
Mg
Ca
Sr
Ba
Ra
Ga
In
Tl
Al
B
Ge
Sn
Pb
Si
C
Sb
Bi
P
N
As Se
Te
Po
O
S
He
Kr
Ne
Ar
Rn
Xe
Sc Ti V Cr Mn Fe Co Ni Cu Zn
Rh
La Pt
Rf Db Sg Bh Hs Mt ? ?
Ac ?
Br
At
Cl
F
I
What are columns of elements called?
7
6
5
4
3
2
Groups
1 0
Group number
transition elements

Rows of elements
H He
Li Be N O F Ne
B C
Na Mg Al P S Cl Ar
Si
K Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br
Ca Kr
As
Rb Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb
Sr Te
Rh I Xe
Cs Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po
La At
Pt Rn
Ac ?
Periods
What are rows of elements called?
1
2
3
4
5
6
7
Period number

H He
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br
Ca Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb
Sr Te
Rh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po
La At
Pt
Ra Rf Db Sg Bh Hs Mt ? ?
Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
B C
As
What is the Group and Period of this element?
Mg
C
Group 2
Group 4
Group 7
Cl
K
Group 1
Mg
C
Cl
K
Name the position
7
6
5
4
3
2
1 0
2
3
4
5
6
7
Period 3
Period 2
Period 3
Period 4
1

H
1 He
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
Ca Kr
Sr Te
Rh
La At
Pt
Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
B C
As
3
11
19
37
55
87
4
21 22
12
23 24 25 26 27 28 29 30 31 32 34 35
20 36
39 40 41 42 43 44 46 47 48 49 50 51
38 52
45
56 72 73 74 75 76 77 79 80 81 82 83 84
57 85
78
88 104105106107108109 111 112
89 110
13 15
7 8
16 17
9 10
18
86
53
14
54
2
5 6
33
Missing elements!
In this periodic table the symbols are replaced by atomic
numbers. Some of the numbers are missing – where?
Two more periods of elements fit here but are
only shown on some periodic tables.
These are called the lanthanides and actinides.

Patterns 1: Metals and non-metals
on the left and centre
mostly on the right
Where are different types of elements grouped together
on the periodic table?
metals
non-metals
in between metals and non-metals
metalloids
Metalloids aren’t type of rock music fan!
Metalloids actually have some properties similar to metals
and other properties similar to no-metals.
Can you name a metalloid element?

Metals, non-metals and metalloids

H
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
Ca Kr
Sr Te
Rh
La At
Pt
Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
He
B C
As
silicon (Si) metalloid
francium (Fr) metal
scandium (Sc) metal
krypton (Kr) non-metal
cobalt (Co) metal
Is this element a metal, non-metal or metalloid?
Kr
Sc
Fr
Si
Co
Metal, non-metal or metalloid?

Only two elements are liquids at room temperature.
Where are elements of different states grouped
together on the periodic table?
on the left, in the centre and to the right
only two elements are liquid
solids
liquids
mostly on the far right
gases
mercury bromine
Can you name these two elements?
Patterns 2: Physical state

Physical state

H
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
Ca Kr
Sr Te
Rh
La At
Pt
Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
He
B C
As
krypton (Kr) gas
Kr
niobium (Nb) solid
Nb
barium (Ba)
Ba
solid
nitrogen (N)
N
gas
bromine (Br)
Br
liquid
Is this element a solid, liquid or gas at room temperature?
Solid, liquid or gas?

Patterns 3: Reactivity of metals
more reactive
more
reactive
What happens the reactivity of metals along a period?
H
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr MnFe Co Ni Cu ZnGaGe
Ca
Y Zr NbMo Tc Ru Pd AgCd In Sn Sb
Sr Rh
Ba Hf Ta W ReOs Ir AuHg Tl Pb Bi Po
La Pt
Ra Rf DbSg Bh Hs Mt ? ?
Ac ?
Al
What happens the reactivity of metals down a group?
Which is the most reactive metal?

potassium (K) or lithium (Li)
H
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr MnFe Co Ni Cu ZnGaGe
Ca
Y Zr NbMo Tc Ru Pd AgCd In Sn Sb
Sr Rh
Ba Hf Ta W ReOs Ir AuHg Tl Pb Bi Po
La Pt
Ra Rf DbSg Bh Hs Mt ? ?
Ac ?
Al
calcium (Ca) or magnesium (Mg)
calcium (Ca) or iron (Fe)
copper (Cu) or barium (Ba)
From the positions of these metals in the periodic table,
which metal in each pair is the more reactive?
Which metal is more reactive?

Patterns 4: Reactivity of non-metals
more reactive
What are the rules for the reactivity of the non-metals?
1. Group 0 is the most unreactive group of elements.
2. For the remaining non-metals, reactivity increases
to the right of a period
Se Br Kr
Te
At
P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
He
B C
As
more
reactive
Which is the most reactive non-metal?
u
n
r
e
a
c
t
i
v
e
and up a group.

neon (Ne) or iodine (I)
Which non-metal is more reactive?
Se Br Kr
Te
At
P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
He
B C
As
oxygen (O) or silicon (Si)
fluorine (F) or chlorine (Cl)
carbon (C) or oxygen (O)
From the positions of these non-metals in the periodic table,
which non-metal in the pair is the more reactive?

Patterns and atomic number
What links atomic number and the properties of elements?
The periodic table shows that patterns in the properties
of elements are linked to atomic number.
electrons
H He
Ac ?
K Ca Ga Ge As Se Kr
Sc Ti V Cr Mn Fe Co Ni Cu Zn Br
Cs Ba Tl Pb Bi Po Rn
La Pt At
Na Mg Al Si P S Ar
Cl
Li Be B C N O Ne
F
Rb Sr In Sn Sb Te Xe
Rh I

Patterns and electrons
atomic number = number of protons
atomic number = number of electrons in element’s atoms
The properties of elements are hugely influenced by the
number and arrangement of electrons in the atom.
What links atomic number and the number of electrons?
1
H
1
4
He
2
7
Li
3
10
B
5
9
Be
4
As atomic number increases by one, the number of electrons
also increases by one.
So the elements in the periodic table are also arranged in
order of the number of electrons.

Patterns and electrons
How is layout of the periodic table related to the number
and arrangement of electrons in these shells?
Electrons are arranged in shells around an atom’s nucleus.
cut here
cut here
cut here
The point at which a new period starts is the point at which
electrons begin to fill a new shell.
How many electrons can the first three electron shells hold?
K
H Li Na
Be Mg Al P
N O S Cl
F Ne Ar
Si
He B C
19
1 3 11
4 12 13 15
7 8 16 17
9 10 18
14
2 5 6

Rules for electron arrangements
2,8,8
The rules for the maximum number of electrons shells in
the first three shells are:
Electrons are arranged in shells around an atom’s nucleus.
first shell maximum = 2 electrons
second shell maximum = 8 electrons
third shell maximum = 8 electrons
This electron arrangement is written as:

Elements in Period 1 only have electrons in the first shell.
1 2
7
6
5
4
3
2
1 0
1
H He
The first shell can only hold a maximum of two electrons,
so Period 1 only includes the elements hydrogen and helium.
Why are there only two elements in Period 1?
What is special about the outer shell of He?
Electrons in Period 1

Elements in Period 2 all have a complete first shell.
2,1 2,2 2,3 2,4 2,5 2,6 2,7 2,8
7
6
5
4
3
2
1 0
2
Li Be B C N O F Ne
The second shell is completed one electron at a time
going across Period 2 from left to right.
What is special about the outer shell of Ne?
What happens to electrons in the second shell in Period 2?

2,8,1 2,8,2 2,8,3 2,8,4 2,8,5 2,8,6 2,8,7 2,8,8
Elements in Period 3 have complete first and second shells.
7
6
5
4
3
2
1 0
3
The third shell is completed one electron at a time
going across Period 3 from left to right.
What is special about the outer shell of Ar?
Na Mg Al Si P S Cl Ar
What happens to electrons in the third shell in Period 3?

Patterns of electron arrangements
2,8,8,1 2,8,8,2
2,8,1 2,8,2
1
2,1 2,2
Consider the electron arrangements of the first 20 elements
in the periodic table.
7
6
5
4
3
2
1 0
1
2,3 2,4 2,5 2,6 2,7 2,8
2,8,3 2,8,4 2,8,5 2,8,6 2,8,7 2,8,8
2
2
3
4
What is the pattern for the number of outer shell electrons
in each group?
Why do elements in the same group have similar
chemical reactivity?

Why does reactivity increase
going down the group?
Going down Group 1 the
outer electron becomes
further from the nucleus
and so is more easily lost
in chemical reactions.
The Group 1 metals are
called the alkali metals.
1
2
3
2,1
Li
2,8,1
Na
Group 1 elements have
one electron in the
outermost shell.
Electrons in Group 1

two electrons in the
outermost shell.
2,2
Be
2,8,2
Mg
2
2
3
In chemical reactions metals
tend to lose their outer
electrons to form positive ions.
What is the charge on the ions
of Group 2 elements?
These elements lose the two
outer electrons and form ions
with a 2+ charge.

three electrons in the
outermost shell.
3
2
3
2,3
B
2,8,3
Al
Metals lose their outer
electrons to form positive ions.
What is the charge on the ions
of Group 3 elements?
These elements lose the
three outer electrons and form
ions with a 3+ charge.

four electrons in the
outermost shell.
4
2
3
2,4
C
2,8,4
Si
The elements at the top of
Group 4 are non-metals.
These elements don’t like to
lose their electrons and prefer
to share them with other atoms.
What type of bonding is this?
The elements at the top of
Group 4 bond covalently.

five electrons in the
outermost shell.
5
2
3
2,5
N
2,8,5
P
How many electrons do the
elements shown need for
a full outer shell?
The Group 5 elements shown
need three more electrons
to achieve a full outer shell.

Atoms form negative ions by
gaining extra electrons.
What type of ions will these
Group 6 elements form?
These Group 6 atoms can gain
two extra electrons to complete
their outer shell and form
negative ions with a 2- charge.
6
2
3
2,6
O
2,8,6
S
six electrons in the
outermost shell.

seven electrons in the
outermost shell.
7
2
3
2,7
F
2,8,7
Cl
These atoms need one extra
electrons for a complete outer
shell and form 1- ions.
Why does reactivity increase
going up Group 7?
The incoming electrons are
pulled more strongly into shells
that are closer to the nucleus.

Group 0 (or 8) elements all have
a complete set of electrons in
the outermost shell.
1
2
3
0
2
He
2,8
Ne
2,8,8
Ar
Why are these elements so
unreactive?
The Group 0 atoms do not need
to lose or gain any electrons to
complete their outer shells which
means they are unreactive.
The Group 0 elements are called
the noble (or inert) gases.

H He
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
Ca Kr
Sr Te
Rh
La At
Pt
Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
B C
As
Mg
C
2, 8, 2
2, 4
2, 8, 7
Cl
K
2, 8, 8, 1
Mg
C
Cl
K
What is the electron arrangement?
What is the electron arrangement in this element’s atoms?
7
6
5
4
3
2
1 0
2
3
4
5
6
7
1

Different types of elements

Periodic table quiz

H
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
Ca Kr
Sr Te
Rh
La At
Pt
Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
He
B C
As
Periodic table

chemistry-the-periodic-table.ppt

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