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KS4 Chemistry
The Periodic Table
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The Periodic Table
Contents
Elements and atomic number
Arranging elements
Electronic structure
Patterns of behaviour
Teacher resources
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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.
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Properties of elements
What is a property of an element?
A property is any characteristic of an element.
For example, here are some properties ofsodium:
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?
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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 ofparticles:
Where are these particles found in an atom?
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What is atomic number?
Atomic number = the number of protons in an atom
proton
electron neutron
heliumnucleus
What are the particles in this helium atom?
What is the atomic number of helium?
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Atomic number andelectrons
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
F9
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?
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The Periodic Table
Contents
Elements and atomic number
Arranging elements
Electronic structure
Patterns of behaviour
Teacher resources
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Atomic number and patterns
KH Li NaBe Mg Al PN O S ClF Ne ArSiHe B C
reactive metalsunreactive gases
reactive gases
When scientists arranged elements in order of increasing
atomic number they found patterns in their properties.
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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?
KH Li NaBe Mg Al PN O S ClF Ne ArSiHe B C
191 3 114 12 13 157 8 16 179 10 18142 5 6
8
8
Compare the positions of similar elements.
reactive gases reactive metals
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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
KH Li NaBe Mg Al PN O S ClF Ne ArSiHe B C
191 3 114 12 13 157 8 16 179 10 18142 5 6
cut herecut here
Na Mg Al P S Cl ArSi
H He
Li Be N O F NeB C
K
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Arranging elements
K
He
Al P SSiMgNa ArCl
Be N OB CLi NeF
When elements are arranged according to their properties
what patterns do you see and what element is missing?
reactive
metals
unreactive
gases
reactive
gasesSimilar elements go into the same columns.
Hydrogen is an exception. This reactive gas is best
positioned above the reactive metals.
Hhydrogen is a
special case
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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 KrSc Ti V Cr Mn Fe Co Ni Cu Zn Br
Cs Ba Tl Pb Bi Po RnHf Ta W Re Os Ir Au HgLa Pt At
Na Mg Al Si P S ArClLi Be B C N O NeF
Rb Sr In Sn Sb Te XeY Zr Nb Mo Tc Ru Pd Ag CdRh I
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Columns of elements
H
LiNa
K
Rb
Cs
Fr
BeMg
Ca
Sr
Ba
Ra
Ga
In
Tl
AlB
Ge
Sn
Pb
SiC
Sb
Bi
PN
As Se
Te
Po
OS
He
Kr
NeAr
Rn
Xe
Sc Ti V Cr Mn Fe Co Ni Cu Zn
Y Zr Nb Mo Tc Ru Pd Ag CdRh
Hf Ta W Re Os Ir Au HgLa Pt
Rf Db Sg Bh Hs Mt ? ?Ac ?
Br
At
ClF
I
What are columns of elements called?
765432
Groups
1 0Group number
transition elements
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Rows of elements
H He
Li Be N O F NeB CNa Mg Al P S Cl ArSi
K Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa KrAs
Rb Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh I Xe
Cs Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt Rn
Fr Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
PeriodsWhat are rows of elements called?
1
23
4
5
6
7
Period number
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H He
LiNa
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt
Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
Al PN O
S ClF Ne
Ar
Rn
I
Si
Xe
B C
As
What is the Group and Period of this element?
MgC
Group 2Group 4Group 7
Cl
K
Group 1MgCClK
Name the position
7654321 0
23
4
5
6
7
Period 3Period 2Period 3Period 4
1
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H1 He
LiNa
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt
Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
Al PN O
S ClF Ne
Ar
Rn
I
Si
Xe
B C
As
311
19
37
55
87
4
21 22
12
23 24 25 26 27 28 29 30 31 32 34 3520 36
39 40 41 42 43 44 46 47 48 49 50 5138 5245
56 72 73 74 75 76 77 79 80 81 82 83 8457 8578
88 104 105 106 107 108 109 111 11289 110
13 157 8
16 179 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.
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The Periodic Table
Contents
Elements and atomic number
Arranging elements
Electronic structure
Patterns of behaviour
Teacher resources
P 1 M l d l
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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-metalsmetalloids
Metalloids arent type of rock music fan!
Metalloids actually have some properties similar to metalsand other properties similar to no-metals.
Can you name a metalloid element?
M l l d ll id
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Metals, non-metals and metalloids
M t l t l t ll id?
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H
LiNa
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt
Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
Al PN O
S ClF Ne
Ar
Rn
I
Si
Xe
He
B C
As
silicon (Si) metalloidfrancium (Fr) metalscandium (Sc) metalkrypton (Kr) non-metalcobalt (Co) metal
Is this element a metal, non-metal or metalloid?
KrSc
Fr
Si
Co
Metal, non-metal or metalloid?
P tt 2 Ph i l t t
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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 rightgases
mercury bromine
Can you name these two elements?
Patterns 2: Physical state
Ph i l t t
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Physical state
S lid li id ?
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H
LiNa
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt
Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
Al PN O
S ClF Ne
Ar
Rn
I
Si
Xe
He
B C
As
krypton (Kr) gas
Kr
niobium (Nb) solid
Nb
barium (Ba)
Ba
solidnitrogen (N)
N
gasbromine (Br)
Br
liquid
Is this element a solid, liquid or gas at room temperature?
Solid, liquid or gas?
P tt 3 R ti it f t l
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Patterns 3: Reactivity of metals
more reactive
m
orereactiv
e
What happens the reactivity of metals along a period?
H
LiNa
K
Rb
CsFr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga GeCa
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr Rh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa PtRa Rf Db Sg Bh Hs Mt ? ?Ac ?
Al
What happens the reactivity of metals down a group?
Which is the most reactive metal?
Whi h t l i ti ?
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potassium (K) or lithium (Li)
H
LiNa
K
Rb
CsFr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga GeCa
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr Rh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa PtRa Rf Db Sg 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
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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 increasesto the right of a period
Se BrKr
Te
At
PN O
S ClF Ne
Ar
Rn
I
Si
Xe
He
B C
As
mo
rereactive
Which is the most reactive non-metal?
un
reactive
and up a group.
Which non metal is more reactive?
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neon (Ne) or iodine (I)
Which non-metal is more reactive?
Se BrKr
Te
At
PN O
S ClF 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?
Contents
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The Periodic Table
Contents
Elements and atomic number
Arranging elements
Electronic structure
Patterns of behaviour
Teacherresources
Patterns and atomic number
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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.
electronsH He
Fr Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
K Ca Ga Ge As Se KrSc Ti V Cr Mn Fe Co Ni Cu Zn Br
Cs Ba Tl Pb Bi Po RnHf Ta W Re Os Ir Au HgLa Pt At
Na Mg Al Si P S ArClLi Be B C N O NeF
Rb Sr In Sn Sb Te XeY Zr Nb Mo Tc Ru Pd Ag CdRh I
Patterns and electrons
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Patterns and electrons
atomic number = number of protons
atomic number = number of electrons in elements 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
H1
4
He2
7
Li3
10
B5
9
Be4
As atomic number increases by one, the number of electronsalso increases by one.
So the elements in the periodic table are also arranged in
order of the number of electrons.
Patterns and electrons
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Patterns and electrons
How is layout of the periodic table related to the numberand arrangement of electrons in these shells?
Electrons are arranged in shellsaround an atoms nucleus.
cut herecut herecut here
The point at which a new period starts is the point at whichelectrons begin to fill a new shell.
How many electrons can the first three electron shells hold?
KH Li NaBe Mg Al PN O S ClF Ne ArSiHe B C
191 3 114 12 13 157 8 16 179 10 18142 5 6
Rules for electron arrangements
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Rules for electron arrangements
2,8,8
The rules for the maximum number of electrons shells inthe first three shells are:
Electrons are arranged in shellsaround an atoms nucleus.
first shell maximum = 2 electrons
second shell maximum = 8 electrons
third shell maximum = 8 electrons
This electron arrangement is written as:
Electrons in Period 1
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Elements in Period 1 only have electrons in the first shell.
1 2
7654321 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 ofHe?
Electrons in Period 1
Electrons in Period 2
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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
7654321 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 ofNe?
What happens to electrons in the second shell in Period 2?
Electrons in Period 2
Electrons in Period 3
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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.
7654321 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 ofAr?
Na Mg Al Si P S Cl Ar
What happens to electrons in the third shell in Period 3?
Electrons in Period 3
Patterns of electron arrangements
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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.
7654321 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
23
4
What is the pattern for the number of outer shell electronsin each group?
Why do elements in the same group have similar
chemical reactivity?
Electrons in Group 1
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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
Electrons in Group 2
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Group 2 elements have
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 twoouter electrons and form ions
with a 2+ charge.
Electrons in Group 2
Electrons in Group 3
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Group 3 elements have
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 formions with a 3+ charge.
Electrons in Group 3
Electrons in Group 4
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Group 4 elements have
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 dont like tolose their electrons and prefer
to share them with other atoms.
What type of bonding is this?
The elements at the top ofGroup 4 bond covalently.
Electrons in Group 4
Electrons in Group 5
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Group 5 elements have
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.
Electrons in Group 5
Electrons in Group 6
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Atoms form negative ions by
gaining extra electrons.
What type of ions will theseGroup 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
Group 6 elements have
six electrons in the
outermost shell.
Electrons in Group 6
Electrons in Group 7
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Group 7 elements have
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 arepulled more strongly into shells
that are closer to the nucleus.
Electrons in Group 7
Electrons in Group 0
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Group 0 (or 8) elements all have
a complete set of electrons in
the outermost shell.1
2
3
0
2He
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.
Electrons in Group 0
What is the electron arrangement?
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H He
LiNa
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt
Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
Al PN O
S ClF Ne
Ar
Rn
I
Si
Xe
B C
As
MgC
2, 8, 22, 42, 8, 7
Cl
K
2, 8, 8, 1MgCClK
What is the electron arrangement?
What is the electron arrangement in this elements atoms?
7654321 0
23
4
5
6
7
1
Different types of elements
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Different types of elements
Periodic table quiz
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Periodic table quiz
Contents
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The Periodic Table
Elements and atomic number
Arranging elements
Electronic structure
Patterns of behaviour
Teacher resources
Periodic table
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H
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt
Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
He
B C
As
Periodic table
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H
Li
Na
K
Rb
Cs
Fr
Be
Sc Ti
Mg
V Cr Mn Fe Co Ni Cu Zn Ga Ge Se BrCa Kr
Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn SbSr TeRh
Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi PoLa AtPt
Ra Rf Db Sg Bh Hs Mt ? ?Ac ?
Al P
N O
S Cl
F Ne
Ar
Rn
I
Si
Xe
He
B C
As