This document discusses a science presentation about the properties and reactions of metals and non-metals. It lists the group members giving the presentation and describes several properties of metals like malleability and conductivity. It then discusses how metals react with oxygen, water, acids, salt solutions, chlorine, hydrogen and how alloys are formed and used. For non-metals, it summarizes their reactions with oxygen, water, acids, salt solutions, chlorine, hydrogen and describes ionic compounds.

1. Welcome to the science presentation
of Formative Assessment-3
The topic we are going to
discuss now is

3. Group Members
Chirag jain
Sanyam jain
Risahbh
Deepanshu
Akshay
Tushant
Uttkarsh
Swarndeep
Gaurav

5. 1. Metals are malleable , that is , metals
can be beaten into thin sheets with a
hammer .
2. Metals are ductile , that is , metals can
be drawn into thin wires.
3. Metals are good conductors of heat .
4. Metals are lustrous and can be polished .
5. Metals are good conductors of electricity .
6. Metals are sonorous .
7. Metals have high densities .

6. Almost all metal combing with oxygen to
from metal.
For example:-
Metal + Oxygen Metal oxide
 Copper (Cu) reacts with oxygen to from
copper (ll) oxide , a black oxide.
2Cu + O₂ 2CuO

7. Aluminium (Al) reacts with oxygen to from
aluminium Oxide.
4Al + 3O₂ 2Al₂O₃
Sodium reacts with oxygen at room temprature
to from sodium oxide .
4Na + O₂ 2Na₂O
Magnesium does not react with oxygen at room
temprature. On heating in oxygen , magnesium
burns with dazzling white light to give
magnesium oxide
2Mg + O₂ 2MgO

8.  Reaction of metal with water
 Metal + Water Metal oxide + Hydrogen
 Metal oxide + Water Metal Hydroxide
For Example:-
 Sodium and Potassium react violently with cold
water. The reaction is so violent and exothermic
that the evolved hydrogen immediately catches
fire.
2K + 2H₂O 2KOH + H₂ + Heat energy
2Na + 2H₂O 2NaOH + H₂ + Heat energy

9.  Calcium also reacts with water at room
temprature forming calcium hydroxide .
Ca + 2H₂O Ca(OH)₂ + H₂
 Reaction of metal with Acid
When metal reacts with a dilute acid , then a
metal salt and hydrogen gas are formed.
Metal + Dilute acid Metal salt + Hydrogen
Example will shown in table on next slide

10. Metal Acid Nature of Reaction Reaction
Sodium Dil. HCl
Dil. H₂SO₄
Sodium reacts vigorously
with dil. HCl and dil. H₂SO₄
2Na + 2HCl 2NaCl + H₂
2Na + 2H₂SO₄ Na₂SO₄ + H₂
Magnesium Dil. HCl
Dil. H₂SO₄
Magnesium reacts rapidly
with dil. HCl and dil. H₂SO₄
Mg + 2HCl MgCl₂ + H₂
Mg + H₂SO₄ MgSO₄ + H₂
Zinc Dil. HCl
Dil. H₂SO₄
Zinc reacts with dil.HCl
and dil. H₂SO₄ at
moderate rate .
Zn + 2HCl ZnCl₂ + H₂
Zn + H₂SO₄ ZnSO₄ + H₂
Iron Dil. HCl
Dil. H₂SO₄
Iron reacts with dil.HCl as
well as Dil. H₂SO₄ slowly
at room temprature.
Fe + 2HCl FeCl₂ + H₂
Fe + H₂SO₄ FeSO₄ + H₂
Copper Dil. HCl
Dil. H₂SO₄
Copper does not react
with dil. HCl and dil. H₂SO₄
slowly at room
temprature
But slowly dissolve in dil.
H₂SO₄ in the presence of
air.
No reaction
2Cu + 2H₂SO₄ + O₂ 2CuSO₄ +
H₂O

11.  Reaction of metal with salt solution
A less reactive metal is displaced from its salt
solution by a more reactive metal.
Reaction of zinc with copper sulphate solution
When a strip of zinc metal is put in copper sulphate
solution, then the blue colour of copper sulphate
solution fades gradually due to the formation of
colourless zinc sulphate, and red-brown copper
metal is deposited on the zinc strip:
CuSO₄ + Zn ZnSO₄ + Cu

12.  Reaction of metals with Chlorine
Metals react with chlorine to from ionic
chlorides. For example:-
Sodium is a metal. So, sodium reacts with
chlorine to from an ionic chloride called
sodium chloride:
2Na + Cl₂ 2NaCl
Calcium is a metal which reacts vigorously with
chloride called calcium chloride:
Ca + Cl₂ CaCl₂

13. Reaction of metal with hydrogen
Only few reactive metal like sodium, potassium,
calcium, and magnesium reacts with hydrogen to
from metal hydrides. For example:
 When hydrogen gas is passed over heated
sodium then sodium hydride is formed :
2Na + H₂ 2NaH
 When hydrogen gas is passed over heated
calcium then calcium hydride is formed:
Ca + H₂ CaH₂

14. Chemical properties of non metal
Reaction of non-metals with oxygen
Non-metals react with oxygen to form acidic
oxides or neutral oxides . The acidic oxides of
non-metals dissolves in water to form acids .
C (s) + o₂ - co₂
Carbon oxygon carbon dioxide
CO2 (g) + H2O (l) – H2CO3 (aq)
carbon dioxide water carbonic acid

15. Reaction of non-metals with water
• Non-metals do not react with water to
evolve hydrogen gas . This is because
non-metals cannot give electrons to
reduce the hydrogen ions of water into
hydrogen gas

16. Reaction of non-metals with dilute acids
Non-metals do not react with dilute acids .
Non-metals do not displaces hydrogen from
acids . Non-metals like carbon , sulphur or
phosphorus are put into a test tube
containing dilute sulphuric acid or dilute
hydrochloric acid , then no hydrogen gas is
evolved .

17. Reaction of non-metals with salt solutions
A more reactive non-metal displaces a less
reactive non-metal from its salt solution.
2NaBr (aq) + Cl2 (g) - Br2 (aq) + 2NaCl (aq)
Sodium chlorine bromine Sodium
Bromide chloride

18. Reaction of non-metals with chlorine
Non-metals react with chlorine to form
covalent chlorides which are non-electrolytes
(do not conduct electricity )
H2 (g) + Cl2 (g) - 2HCl (g)
Hydrogen chlorine hydrogen chloride
(non-metal) (covalent hydride)
P4 (s) + 6Cl2 (g) - 4PCl3 (l)
(non-metal) (covalent hydride)

19. Reaction of non-metals with hydrogen
Non-metals react with hydrogen to form
covalont hydrides
 H2 (g) + S (l) - H2S (g)
Hydrogen sulphur hydrogen sulphide
(non-metal) (covalent hydride)
N2 (g) + 3H2 (g) - 2NH3 (g)
Nitrogen hydrogen ammonia
(non-metal) (covalent hydride)

20. Ionic compounds
The compounds containing ionic bonds
are called ionic compounds.Theyare
formed by transfer of electrons from one
atom to another . Ionic compounds are
made up of positively charged
ions[cataions]+ and negatively charged
ions [anions].Ionic compounds are
also known as Electrovalent
compounds.

21. Some common ions

22. Structure of ionic copounds
The forces between the particles are
strong.
There are no free-moving electrons
present, unlike in metals.
There are charged particles present,
but in solid state they are not free to
move.
When an ionic compound melts,
however, the particles are free to
move and the compound will conduct
electricity.

23. A notation showing the valence electrons
surrounding the atomic symbol.

27. 1 THESE COMPOUNDS ARE USUALL
CRYSTALLINE SOLIDS . BECAUSE THEIR
OPPOSITELY RGED IONS ATTRACT
EACH OTHER.THESE IONIC
COMPOUNDS ARE HARD AND BRITTLE
. IONIC COMPOUNDS HAVE HIGH
MELTING AND HIGH BOILING POINT.
EX – SODIUM CHLORIDE HAS HIGH
MELTING POINT.

28. IONIC COMPOUNDS CONDUCT ELECTRICITY
WHEN DISSOLVED IN WATER.
THERE ARE PLENTY OF
FREE IONS IN SOLUTION WHICH ARE ABLE
TO CONDUCT ELECTRICITY. EX-ACETONE,
KEROSENE etc.

29. TAKE A SMALL AMOUNT
OF SODIUM CHLORIDE ON
METAL SPATULA . HESTED
OVER A FLAME OF BURNER
SODIUM CHLORIDE MELTS
ONLY ON STRONG HEATING
THIS SHOWS THAT SODIUM
CHLORIDE HAS A HIGH
MELTING POINT

30. FILL A BEAKER HALF WITH
WATER AND DISSOLVE SOME
SODIUM CHLORIDE IN IT. TWO
CARBON AND ELECTRODES ARE
PLACED IN IT. AN ELECTRIC
SWITCH IS SET UP BY
INCLUDING BATTERY BULB AND
SWITCH. ON PRESSING THE
SWITCH BULB LIGHTS UP . THIS
MEANS THAT THE SOLUTION
TAKEN IN THE BEAKER IS
ALLOWS TO CONDUCT
ELECTRICITY. SINCE SODIUM
CHLORIDE IS AN IONIC
COMPOUND CONDUCT
ELECTRICITY WHEN DISSOLVE
IN WATER.

31. Corrosion :-
The surface of some metals gets corroded when exposed to
moist air for a long time. This is called corrosion.
Prevention of corrosion of metals :-
The corrosion of metals can be prevented by:
i) Applying oil or grease.
ii) Applying paint
iii) Galvanisation ( coating of metals with non corrosive
metals like zinc)
iv) Electroplating ( coating of metals with non corrosive
metals like chromium tin by passing
electricity)
v) Alloying ( Eg. When iron is alloyed with chromium
and nickel, it forms stainless steel which
is resistant to corrosion)

32. Alloys :
An alloy is a homogeneous mixture of a metal with other
metals or non metal.
Alloy Constituents Uses
Steel iron, carbon construction of tools, machines,
tanks, vehicles, ships, rails, building,
bridges, dams etc.
Stainless steel iron, chromium utensils, cutlery, surgical
instruments etc.
Brass copper, zinc utensils, handicrafts musical
instruments etc.
Bronze copper, tin statues, medals, bells ornament

33. Why alloys are made?
 Alloys are stronger than the metals from
which they are made.
Alloy are harder than the constituent metals.
Alloy are more resistant to corrosion.
Alloy have lower melting points than the
constituent metals.
Alloys have lower electrical conductivity than
pure metals.

34. A. The most abundant metal in the earth’s crust
is: aluminium
B. The constituent of stainless steels are:
Iron,nickel,chromium
C. For iron to rust : both air and water are
necessary
D. Amalgam is an alloy of one or more metal:
mercury