Metals and Non metals Class 10 Notes: Metals and non-metals are basic elements that show different physical and chemical properties.
Their study helps us understand the materials used in daily life, industrial processes, the extraction of metals, corrosion, and chemical reactions
What is Metals and Non-Metals?
Elements are broadly categorised as metals and non-metals. This classification relies on their distinct properties.
These notes explore the characteristics that define each group. We examine their reactivity and how they form compounds. Understanding metals and non-metals class 10 notes is crucial for basic chemistry.
Physical Properties: Difference between Metal and Non-Metal
Metals and Non-Metals Class 10 Notes explain the physical and chemical properties of metals and non-metals with clear examples and reactions.
These notes cover the reactivity series, extraction of metals, corrosion, and prevention methods. They are NCERT-based and exam-focused, helping students revise concepts quickly and score better.
| Physical Properties: Difference between Metal and Non-Metal |
| Property |
Metals |
Non-Metals |
| Lustre |
Shiny (metallic lustre) |
Generally dull |
| Hardness |
Usually hard |
Usually soft |
| Malleability |
Can be beaten into sheets |
Brittle |
| Ductility |
Can be drawn into wires |
Non-ductile |
| Conductivity |
Good conductors of heat and electricity |
Poor conductors |
| Melting Point |
Generally high |
Generally low |
| Sonority |
Produce sound when struck |
Non-sonorous |
Exceptions in Physical Properties
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Alkali metals such as sodium (Na), potassium (K), and lithium (Li) are very soft and can be easily cut with a knife.
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Mercury is the only metal that exists in a liquid state at room temperature, while lead and mercury are poor conductors of heat compared to other metals.
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Gallium and caesium have extremely low melting points and can even melt when held in the palm.
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Iodine, though a non-metal, shows a shiny appearance, making it a lustrous non-metal.
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Graphite, a form of carbon, is a non-metal that conducts electricity.
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Diamond, another form of carbon, is an excellent conductor of heat and has a very high melting point, making it the hardest natural substance.
Examples of Non-metals
- Hydrogen – Gas
- Nitrogen – Gas
- Oxygen – Gas
- Fluorine – Gas
- Chlorine – Gas
- Bromine – Liquid
- Iodine – Solid
- Carbon – Solid
- Sulphur – Solid
- Phosphorous – Solid
- Silicon – Solid
2. Chemical Properties of Metals
The chemical reactions of metals depend on their position in the reactivity series. More reactive metals react faster and more vigorously than less reactive ones.
Reaction with Oxygen
Metals react with oxygen to form metal oxides, which are generally basic in nature.
General Equation:
Metal + O2 -> Metal Oxide
Example:
2Cu + O2 -> 2CuO
Observation:
Copper reacts with oxygen to form black copper oxide (CuO).
Amphoteric Oxides
Some metal oxides show both acidic and basic behaviour. Such oxides are called amphoteric oxides.
Example: Aluminium Oxide (Al2O3)
Reaction with Acid:
Al2O3 + 6HCl -> 2AlCl3 + 3H2O
Reaction with Base:
Al2O3 + 2NaOH -> 2NaAlO2 + H2O
Reaction with Water
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Sodium and Potassium react violently with cold water
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Calcium reacts slowly and floats
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Magnesium reacts with hot water
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Iron and Aluminium react with steam
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Gold and Silver do not react
2Na + 2H2O -> 2NaOH + H2
Ca + 2H2O -> Ca(OH)2 + H2
Reactivity Series
The reactivity series arranges metals from most reactive to least reactive.
K > Na > Ca > Mg > Al > Zn > Fe > Pb > Cu > Hg > Ag > Au
It helps predict displacement reactions.
Key Mechanisms of Metals and Non-Metals
This section explains the important chemical processes related to metals and non-metals that help students understand bond formation, metal extraction, corrosion prevention, and industrial reactions.
1. Ionic Bond Formation
Metals have a tendency to lose electrons and form positively charged ions (cations), while non-metals gain electrons to form negatively charged ions (anions).
The strong electrostatic attraction between oppositely charged ions results in the formation of an ionic bond. This transfer of electrons allows both atoms to achieve a stable electronic configuration.
Example:
Na + Cl -> NaCl
2. Metal Extraction Overview
Most metals occur in nature as ores mixed with impurities called gangue. The extraction of metals involves several systematic steps:
a) Concentration of Ore:
Impurities are removed using physical or chemical methods.
b) Conversion to Oxide:
c) Reduction:
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Moderately reactive metals are reduced using carbon or carbon monoxide.
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Highly reactive metals (Na, K, Al) are extracted by electrolytic reduction of molten salts.
d) Refining:
The impure metal is purified, commonly by electrolytic refining, to obtain pure metal.
3. Corrosion Protection
Corrosion weakens metals by reacting with air and moisture. Several methods are used to prevent it:
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Galvanisation: Coating iron or steel with zinc to prevent rusting.
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Anodising: Forming a thick, protective aluminium oxide layer on aluminium to resist corrosion.
4. Thermit Welding Reaction
The thermit reaction is a highly exothermic reaction in which aluminium reduces metal oxides to produce molten metal.
It is commonly used for welding railway tracks and heavy machinery parts.
Reaction:
Fe2O3 + 2Al -> Al2O3 + 2Fe + Heat
How Do Metals and Non-Metals React?
Metals generally lose one or more valence electrons to form positively charged ions (cations), while non-metals gain these electrons in their valence shell to form negatively charged ions (anions).
The strong electrostatic attraction between oppositely charged ions leads to the formation of an ionic bond.
Example: Calcium Chloride (CaCl₂)
A calcium atom loses two electrons and attains the stable electronic configuration of the nearest noble gas (argon), thereby forming a Ca²⁺ ion.
Each chlorine atom gains one electron, forming Cl⁻ ions, and also achieves the noble gas configuration.
The attraction between Ca²⁺ and Cl⁻ ions results in the formation of ionic calcium chloride (CaCl₂).
Metal and Non-Metals Class 10 Notes PDF
Metals and Non-Metals Class 10 Notes PDF provide a clear and structured explanation of physical and chemical properties, reactivity series, extraction of metals, and corrosion.
