Periodic table and chemical change

Pretest states of matter

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general yr 9 chem pretest
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Key Concept
Suggested activity

  1. Atomic structure include Protons,Neutrons, Electrons
  2. Atomic number and mass - calculate
  3. Difference between elements, compounds, molecules and atoms and mixtures.
  4. Features of the periodic table – Groups, Periods, areas of metals, non-metals
  5. Valency and ionic compounds (first 20 elements)
  6. Predict valency based on electron configuration.
  7. Metals vs non metals – basic properties Conductors of heat and electricity, lustrous when cut, malleable, ductile etc
  8. Groups and common properties
Energy levels
Noble gas
Inert gas
Melting point
Practical work
Homework Book pages
1 x Assignment/Project
1 x End of topic test
Done at school
Done at Home
Priority 1


1. What’s the matter
  • Label a model of the atom
  • Compare and identify the differences between an atom of an element, an atom of a compound,(can’t be done) molecule of an element, molecule of a compound.
  • Draw chemical models of some compounds p 4 fig 1.1.3 to 1.1.6
    • Prac 1.1 page 8 Making the compound CO2
    • Revision questions p5~6
1, 3, 4, 5, 9, 11, 12, 13, 14,
  • Homework Book 1.1
Revision Questions
16, 17, 18, 19, 20, 24, 25, 26

make a 3D model of the atom

2. The periodic table
  • History of the periodic table – video available (BBC A Volatile History part 2 of 3
  • Features of the periodic table – alkali metals, alkaline-earth metals, transition metals, halogens, non-metals, noble gases, lanthanides, actinides - Daniel Radcliffe singing 'the Elements' on the Graham Norton Show

p 12 of text book
Ques -6,7,9,10,11,12, 13
go here to check your answers
try this one about their position in the periodic table

Or this one about the patterns in the periodic table
Here is the task - add a verse!!! to this song about patterns.
Revision Questions 18, 20, 21

the periodic table song by Tom Leherer with words

and here's avery good one that builds the table

or learn the elements in order with a story

3. Role of electrons**
  • Memorise the first 20 elements
  • Electon shells & configurations
  • Use periodic table (the groups) to determine the charge on an ion and then show how compounds are ‘created’. [Combining ions to form compounds]

Useful websites to assist learning of the 20 elements
  • Prac 1.3 page 19 Firework Colours
  • Write symbol and name for first 20 elements and complete the electron shells
  • Activity – page 20 Ions Get Together
  • Compound creating worksheet
  • Revision Questions 1~16,

  • Assignment / Project Choices
Revision Questions
17, 18, 20, 21, 23, 24

What's gone wrong here
Ricky's atoms activity (Courtesy of Ms Selir)

4. Metals, non metals and metalloids
  • Properties of metals and non-metals
    • Prac 1.4 page 24 Observing Elements
    • Prac 1.4 page 25 Metal Crystals
    • Prac 1.4 page 27 Using metals to make non-metals

5. Families of Importance
  • Noble gases, and halogens
  • Alkali Metals
  • Alkaline Earth metals
  • Transition metals
  • Prac 1.5 page 34 Halogen precipitates
  • Prac 1.5 page 35 The Alkaline Earths
  • Homework Book 1.5, 1.6, 1.7

6. Test

Class notes
an over view of the periodic table.
the columns in the periodictable are called groups
rows are called periods
as you count across from the left of the periodic table the groups are numbered
some interesting facts
elements in group 1 have only one electron in the outer shell
elements in group two have two electrons in the outer shell.
elements in group IIIA or group 13 have 3 electrons in the outer shell etc
until you get to the inett gases that have a full fomplement of electrons in the outer shell.
this full complement is 2 in the first period
8 in the second period
8 in the third period
18 in the fourth period

have a look at this periodic table that shows the electronic configuration or the electrons patterns in their orbits

Equation writing exercise
The point of this exercise is to use the language of chemistry to describe the combination of ions to form a compound
  1. Na+ + Cl -à

  1. H+ + O2- à

  1. Mg 2+ + F- à

  1. Mg2+ + O 2-à

  1. Na+ + Fl -à

  1. H+ + Cl- à

  1. o2- + Mg2+ à

  1. Mg2+ + Cl-à

  1. C4+ + o2-à

10.n3- + H+ à


Prac 5 : Making metals into non metals (making metal compounds from elements)

Possible product (s)
Magnesium Mg
Hydrochloric HCl
Bubbles, solid Mg seemed to disappear. Gas exploded with a pop when it was lit.
Hydrogen gas H2 (g) and
Magnesium ions (Mg 2+)and Chlorine ions (Cl1-)
If we evaporated the water we would be left with salt crystals of Magnesium Chloride (MgCl2)
Copper Cu
Hydrochloric HCl
Hardly any bubbles of gas, slight blue tinge in the solution
Hydrogen gas H2 (g) and
Copper ions (Cu 2+)and Chlorine ions (Cl1-)
If we evaporated the water we would be left with salt crystals of Copper Chloride (CuCl2)
Iron Fe
Hydrochloric HCl

Hydrogen gas H2 (g) and
Iron ions (Fe 2+)and Chlorine ions (Cl1-)
If we evaporated the water we would be left with salt crystals of Iron Chloride (FeCl2)

The hydrogen pop test is to place a lit match nest to the gas and if it pops it is Hydrogen.

A general rule is an acid added to a metal will give off Hydrogen gas.

Halogen Precipitate Exercise

We combined KI (potassium iodide) with Pb(NO3)2 (lead nitrate) andcreated 2 new products.

One was the yellow compoundPbI2 (Lead Iodide) the remaining clear liquid was KNO3

Potassium Nitrate.

What elements combined to make PbI2

What are the ion forms of these elements? Pb2+ and I-

The second reaction combined with . This time the white

precipitate was and the remaining clear liquid was KNO3

What elements combined to make the white precipitate

What are the ion forms of these elements?

The halogens referred to in this exercise are the non metal component of each compound.

That is the and the _.

The thing about the halogens is that they all have a valency of 1- and form ions with a 1- charge.

When these are in a gas form they are coloured and poisonous. They are all in group VII (or 17)

The noble or inert gases are in group VIII (or 18). These don’t react and don’t form ions.

Group I (or 1) are called the alkali metals. They are very reactive and form ions with a 1+ charge.

Group II (or 2) are called the alkali earth metals. They are very reactive also and form ions with a 2+


Group IV (or 14) begins with elements that are non metals ( carbon and Silicon) Germanium

has metalloid properties and the others like Pb are metallic. C and Si are important to

organic molecules but can also be in other forms (allotropes) like diamond and graphite

The big block in the middle of the periodic table is the transition metals and stretch from group 3

to group 12. They all have metallic properties (good conductors of heat and electricity, ductile,

malleable, high melting and boiling points. Some of the metals have similar properties across

a period. Eg Co, Ni, Fe are all magnetic.

Questions -1 to 10 of this chapter
start the chapter review