by Class 10 Science notes are so useful for upcoming CBSE exams for better preparation and concept learning. Chapter 3 of chemistry is about the basic knowledge of metals and non metals. You will learn the concept of the physical and chemical properties of metals and non metals.
These notes will give you the full chapter learning of Class 10 Science chapter 3.
Class 10 Science notes
CHAPTER 3 METALS AND NON-METALS.
METALS –
Metals are the substances which are electropositive in nature is, they have a tendency to lose electrons.
All metals except mercury exist as solids room temperature.
About 118 elements are known today. There than 90 metals, 22 non-metals and a few metalloids. For example – Sodium (Na), Potassium (K), magnesium (Mg), aluminum (Al), calcium (Ca), Iron (Fe) Barium (Ba) are some metals.
PHYSICAL PROPERTIES OF METALS –
1. Metals in their pure state, have a shining surface. This property called metallic lustre. Like – Gold, Silver etc..
2. Metals are generally hard. The hardness waves from metal to metal.
3.Some Metals are malleable – Metals which can be beaten into thin sheets, this property is called malleability.
Gold and silver are the most malleable metals.
4. Some metals are ductile. – The ability of metals to be drawn into thin wires is called ductility.
Gold (most-ductile about 2km length can be drawn from one gram of gold).
5. Metals are good conductor of heat. (Best – sliver and copper) like aluminum in corking vessels.
6. Metals have high melting and boiling point.
– Tungsten has the highest melting point where as silver has low boiling point.
– Sodium and potassium have low melting point.
7. Metals are good conductor of electricity, like copper, aluminum etc.
Some metals are used to coat the electrical wires are polyvinylchloride (PVC) of a rubber like material.
8.Some metals are sonorous –
The metals that produce a sound on striking a hard surface are called sonorous.
9.Metals have high density and are very heavy, iridium and osmium have highest densities where lithium has the lowest density.
#WHAT IS NON METAL?
There are the substances which are electronegative in nature ,
i.e tendency to gain electrons.
There are example have 22 non- metals.
Examples – carbon, Sulphur, iodine, oxygen, hydrogen etc.
The non- metals are either solids or gases except bromine which are is a liquid
* PHYSICAL PROPERTIES OF NON-METALS.
1. Non-Metals are non-lustrous (no shine)
2. They are not sonorous .
3.Non-Metals are not malleable.
4. Non-Metals are not ductile
5.They are poor – conductor of electricity
6.Non-Metals are soft.
7.They have too low density.
#EXCEPTION TO METAL & NON-METAL PHYSICAL PROPERTIES –
1.All metals except mercury at room temperature. exist as solid at room temperature
2.Gallium and cesium (metals) have very low melting points.
3 Iodine is a non- metal but it is lustrous.
4.Carbon is a non-metal that can exist in different forms.
Each form is called an allotrope. like diamond-hardest natural substance, very high
melting point and polling point. Graphite , allotrope of carbon is a conductor of electricity.
5. Alkali metals (lithium, sodium, potassium) are so soft, have low densities, and low
melting points.
#QUESTIONS
Give an example of a metal
(i)which liquid at room temperature. – Mercury
(ii) can be easily cut with a – Sodium
(iii) is the best conductor of heat. – Silver
(iv) is a poor conductor of heat Mercury & lead.
# Chemical Properties of Metals
Metal’s reaction with almost all metals combine with to form metal oxide.
Metal +Oxygen →Metal Oxide
(for example – When copper is heated in air, it combines with oxygen to form Copper Oxide,
a black oxide.)
2Cu+O₂—2CuO
Aluminum forms aluminum oxide
4AL + 3O₂ → 2Al₂O₃
→ When copper oxide reacts with hydrochloric acid it produced salt and water.
Means here copper oxide or metal oxides are both in nature..
CuO + 2HC1→ CuCl₂+ H₂O
(salt) ( water)
*Some metal oxide such as aluminum oxide, zine oxide etc. show both acidic and basic behavior. when there metal oxides react with base, then they act like acid, and when these metal oxide reacts with acid, then they like base
Al₂O₃+6HCL→ 2AlCL₃+3H2O
(base) (acid) salt water
Al₂O₃+2NaOH→2NaAlO2+H2O
Acid base salt water
(sodium aluminate)
→Most metal oxides are insoluble in water but some these dissolve in water to form
alkalis. Sodium oxide and potassium oxide. dissolve in water to produce alkalis
Na₂0(s) + H2O(l) →2NaOH
K₂0 (S) + H₂0(l) →2KOH(aq)
#REACTIVITY OF METALS TOWARD OXYGEN-
- Potassium and Sodium. Highly reactive in air, they kept in the open, they catch fire.
Hence, to protect them and to prevent accidental fire, they are kept in Kerosene oil.
2.Magnesium, aluminum, zine, lead – are covered with thin layer of oxide, the protective
layer prevents the metal from further oxidation.
3.Iron – It does not burn on heating but iron filings burn vigorously heating.
4. Copper – Copper does not burn, but the hot Metal layers is coated with a black colored
copper oxide.
5.Silver and Gold – They do not react with oxygen even at high temperature.
So. Sodium is the most reactive metal
(2) Metals react with Water
When Metal react with water and produce a metal oxide and hydrogen gas.
Metal oxide that are soluble in water dissolve in It are to further form metal hydro.
Metal + Water → Metal oxide + Hydrogen
Metal oxide + Water →Metal hydroxide
Metals like potassium and sodium react violently with cold water.
In case of sodium and potassium, the reaction is so violent and exothermic that the
evolved hydrogen immediately catches fire.
2K (S)+ 2H₂0 (1) → 2KOH (ag) + H₂(g) + Heat
2 Na (s) + 2H₂O (1)→ 2NaOH (aq) + H₂ (g)+ Heat
The reaction of calcium with water is less violent . the heat evolved is not sufficient for
the hydrogen to catch fire.
Ca(s) + 2H₂0 (1)→ Co(OH)₂ (aq) + H₂(g)
Calcium starts floating because the bubbles of hydrogen gas formed sticks to the surface of
the metals.
→ Magnesium does not react with cold water. It react with hot water to form magnesium hydroxide.
And hydrogen and starts floating due to the bubbles of hydrogen gas
Mg+2H2O—Mg(OH)2+H2
Aluminum, iron and zine do not react either with cold or hot water.
But they react with steam to form the metal oxide and hydrogen.
2AL (S) + 3H₂0 (g) → Al₂O3 (s) + 3H₂(g)
3fe (s) + 4H20 (2) → Fe₂O4 (s) + 4H₂ (g)
Metals such as lead, copper, silver and gold do not react with water at all.
[3] Metals react with acids-
Metal react with acid to give salt and hydrogen gas.
Metal+ Dilute acid→ Salt+ Hydrogen gas
when magnesium, aluminum, zine and iron react with HCl they produce salt and
hydrogen.
Metal + HNO3→H2-X
Hydrogen gas is not evolved when a metal reacts with nitric acid.
It is because HNO3 Is a strong oxidizing agent.
But Magnesium (mg) and manganese (mn) reacts with very dilute
HNO3 to evolve H2 gas.
→ The rate of formation of bubbles is the fastest in case of magnesium.
The reaction is so the most exothermic in this case.
Reactivity decreases in order
Mg > Ad > Zn > Fe.
Copper- does not reacts with dilute HCL, so no bubbled were formed.
[4] Metals react with Solutions of other metal Salts
-In this case Reactive metals can displace less reactive metals from their compounds in
solution or molten form.
→ Displacement reaction occured in the case. If metal A displaces metal B from its
solution, It more reactive than B.
Metal A +Salt Solution of B → Salt solution of A+ Metal B.
CuSO4+FeSO4 → FeSO4+CuSO4
Fe+CuSO4→FeSO4+Cu
Cu+FeSO4→CuSO4+Fe
[5] Reactivity series-
K Potassium Most reactive
Na Sodium
Ca Calcium
Mg Magnesium
Al aluminum
Zn zinc reactivity decreases
Fe iron
Pb lead
H hydrogen
Cu copper
Hg mercury
Ag sliver
Au gold least reactive
SOME IMPORTANT TERMS-
- Anodising
Anodising is process of forming a thick oxide layer of aluminum.
This aluminum oxide coat makes it resistant to further corrosion(makes Al₂O3)
The resistance can be improved further by making the oxide layer thicker.
During anoding, a clean aluminum article is made the anode and Is electrolyzed
with dilute sulphuric acid.
The oxygen gas evolved at the anode reacts with aluminum to make a thicker proactive oxide layer.
2.Aqua regia –(Royal water)
-It is a freshly prepared mixture of concentrated hydrochloric aic and concentered nitic
acid in the ratio of 3:1.
-the solution is used for dissolving gold
-it is one of the few reagents that is able to dissolve gold and platinum.
#QUESTIONS
Que-1 Why is sodium kept in kerosene oil?
Ans-because sodium is the most reactive metal.
And Metal +HCL→ Salt H2 gas
Que -2 Write the chemical reaction when iron reacts with dilute H2SO4.
Ans Fe + H2SO4 → FeSO +H2
When a metal and non-metal reacts with each other transfer of electrons take place f
rom metal to non-metals
→Compounds the formed known as ionic compounds.
→they have strong electrostatic force of attraction.
Electronic configuration of elements
*NOBLE GAS-
Compounds which have a completely filled valence shell, and show little chemical activity like
Helium(He)— k-2
Neon (Ne)— k-2 L-8 Etc.
*METALS –
sodium (Na) k-2 l-8 m-1
Magnesium(mg) k-3 l-8 m-3
*NON METALS –
Oxygen (O) k-2 l-6
Chlorine(Cl) k-2 l-8 m-7
FORMATION OF SODIUM CHLORIDE –
Sodium (metal) is electro-positive and reducing agent.
So it will lose one electron from its outer shell.
Chloride (non metals) is electro -negative and oxidizing agent.
so it will gain one electron by sodium .
(2,8,1) (2,8)
(sodium cation)
Cl + e-→ Cl-
(chloride anion)
- Formation of magnesium chloride-
Mg → Mg2+ + 2e-
(2,8,2) (2,8)
(magnesium cation)
Cl+ e-→Cl-(chloride anion )
*PROPERTIES OF IONIC COMPOUNDS-
I) PHYSICAL NATURE-
ionic compounds are solid and are somewhat hard because of the strong force of attraction between the positive and negative ions. compounds are brittle, and break into pieces when pressure is applied.
II) MELTING AND BOILING POINT-
ionic compounds have high melting and boiling point.
III) SOLUBILITY-
Electrovalent compounds are . generally soluble in water and insoluble solvents such
as kerosene, petrol etc.
(IV)CONDUCTION OF ELECTRICITY-
The conduction of electricity through a solution involves the movement of charged
particles .A solution of an ionic compound in water contains ions, which move to the
opposite electrodes when electricity is passed through the solution.
→ Ionic compounds the solid state do not conduct electricity because movement of ions in
solid is not possible.
→Ionic compounds conduct electricity in the molten state.
Because electrostatic. forces of attraction between the oppositely charged ions are overcome
due to the heat. Thus, the ions moves freely and conduct electricity.
Cathode→ Reduction→ Gain of electron Oxidation
Anode→ Oxidation→ Loss of electron
Que 1) (a)electron -dot structure of oxygen
O2(2,6) → 
(b)Formation of Na2Oand MgO by the transfer of electrons
Que 2) why do ionic compounds have high melting point?
Ans: Because ionic compounds have strong force of attraction so they need a considerable
amount of energy is required to break the strong inter- ionic attraction.
* OCCURRENCE OF METALS –
Earth’s crust is the major source of metals, the elements or compounds ,
which naturally in the earth’s crust occur known as minerals.
– When Minerals contain a very high percentage of a particular metal and the metal can
be profitably extracted from it. These minerals are called ores.
EXTRACTION OF METALS –
Some metals. Are found in the earths crust in the free state. Some are found in the form of
their compounds.
The metals at the bottom of the activity series are the least reactive.
Notes for the class 10 science.
We hope you got the best knowledge of chapter 3 metals and non metals. Class 10 Science more notes are available for the other chapter.
