© boardworks ltd 2004 ks4 chemistry the periodic table

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Page 1: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

KS4 Chemistry

The Periodic Table

Page 2: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

The Periodic Table

Contents

Elements and atomic number

Arranging elements

Electronic structure

Patterns of behaviour

Teacher resources

Page 3: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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.

Page 4: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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!

metallichighly reactivesolid but melts easilyfeels light (low density)

Are there any patterns in the properties of elements?

Page 5: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Properties and atomic number

particleparticle chargecharge relative massrelative 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?

Page 6: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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?

Page 7: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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?

1919

FF99

How are the number of electrons and atomic number related in a neutral atom?

9 protons 9 electrons10 neutrons

charge = +9 charge = - 9 charge = 0

total charge = 0

They are the same.

How does this affect the charge of such atoms?

Page 8: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

The Periodic Table

Contents

Elements and atomic number

Arranging elements

Electronic structure

Patterns of behaviour

Teacher resources

Page 9: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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.

Page 10: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

Page 11: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

NaMg Al P S Cl ArSi

H He

Li Be N O F NeB C

K

Page 12: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 gases

Similar 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

Page 13: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 ArCl

Li Be B C N O NeF

Rb Sr In Sn Sb Te XeY Zr Nb Mo Tc Ru Pd Ag CdRh I

Page 14: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

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

Cl

F

I

What are columns of elements called?

765432

GroupsGroups

1 0Group number

transition elements

Page 15: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Rows of elements

H He

Li Be N O F NeB C

Na 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 ?

PeriodsPeriodsWhat are rows of elements called?

1

2

3

4

5

6

7

Period number

Page 16: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

H He

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

B C

As

What is the Group and Period of this element?

Mg

C

Group 2 Group 4Group 7

Cl

K

Group 1MgCClK

Name the position

7654321 0

2

3

4

5

6

7

Period 3Period 2Period 3Period 4

1

Page 17: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

H1 He

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

B C

As

3

11

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 104105106107108109 11111289 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.

Page 18: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

The Periodic Table

Contents

Elements and atomic number

Arranging elements

Electronic structure

Patterns of behaviour

Teacher resources

Page 19: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 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?

Page 20: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Metals, non-metals and metalloids

Page 21: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

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?

Page 22: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

Page 23: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Physical state

Page 24: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

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?

Page 25: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Patterns 3: Reactivity of metals

more reactive

mo

re reactive

What happens the reactivity of metals along a period?

H

Li

Na

KRbCs

Fr

Be

Sc Ti

Mg

V Cr MnFe Co Ni Cu ZnGaGeCaY Zr NbMoTc Ru Pd AgCd In Sn SbSr Rh

Ba Hf Ta W ReOs Ir AuHg Tl Pb Bi PoLa Pt

Ra Rf DbSg Bh Hs Mt ? ?Ac ?

Al

What happens the reactivity of metals down a group?

Which is the most reactive metal?

Page 26: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

potassium (K) or lithium (Li)

H

Li

Na

KRbCs

Fr

Be

Sc Ti

Mg

V Cr MnFe Co Ni Cu ZnGaGeCaY Zr NbMoTc Ru Pd AgCd In Sn SbSr Rh

Ba Hf Ta W ReOs Ir AuHg Tl Pb Bi PoLa 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?

Page 27: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 KrTe

At

PN O

S ClF Ne

Ar

Rn I

Si

Xe

HeB C

As

mo

re r

eact

ive

Which is the most reactive non-metal?

unreactive

and up a group.

Page 28: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

neon (Ne) or iodine (I)

Which non-metal is more reactive?

Se Br KrTe

At

P

N O

S Cl

F Ne

Ar

Rn I

Si

Xe

HeB 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?

Page 29: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

The Periodic Table

Contents

Elements and atomic number

Arranging elements

Electronic structure

Patterns of behaviour

Teacher resources

Page 30: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

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 ArCl

Li Be B C N O NeF

Rb Sr In Sn Sb Te XeY Zr Nb Mo Tc Ru Pd Ag CdRh I

Page 31: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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?

11

HH11

44

HeHe22

77

LiLi33

1010

BB55

99

BeBe44

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.

Page 32: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 herecut herecut 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?

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

Page 33: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Rules for electron arrangements

22,88,88

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:

Page 34: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 of He?

Electrons in Period 1

Page 35: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 of Ne?

What happens to electrons in the second shell in Period 2?

Electrons in Period 2

Page 36: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 of Ar?

Na Mg Al Si P S Cl Ar

What happens to electrons in the third shell in Period 3?

Electrons in Period 3

Page 37: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

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?

Page 38: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

Page 39: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 two outer electrons and form ions with a 2+ charge.

Electrons in Group 2

Page 40: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 form ions with a 3+ charge.

Electrons in Group 3

Page 41: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 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.

Electrons in Group 4

Page 42: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

Page 43: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

Group 6 elements have six electrons in the outermost shell.

Electrons in Group 6

Page 44: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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 are pulled more strongly into shells that are closer to the nucleus.

Electrons in Group 7

Page 45: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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.

Electrons in Group 0

Page 46: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

H He

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

B C

As

Mg

C

2, 8, 22, 42, 8, 7

Cl

K

2, 8, 8, 1MgCClK

What is the electron arrangement?

What is the electron arrangement in this element’s atoms?

7654321 0

2

3

4

5

6

7

1

Page 47: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Different types of elements

Page 48: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

Periodic table quiz

Page 49: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

The Periodic Table

Contents

Elements and atomic number

Arranging elements

Electronic structure

Patterns of behaviour

Teacher resources

Page 50: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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

Page 51: © Boardworks Ltd 2004 KS4 Chemistry The Periodic Table

© Boardworks Ltd 2004

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