Metal

Those substance which can lose electrons are called metals. They are generally found on the side of the periodic table.

Non- Metal

Those Substance which gain electron to form negative ions are called non-metals. They are found on the side of the periodic table.

Metalloid

Elements which show properties of both metals and non-metals are called metalloids.

Example- Silicon (Si)

Difference Between Metals And non-metals

Metals	Non-Metals
Metals are generally Solid in Nature. Like Na, Mg, Ca etc.	Non-Metals generally soft.
Metals generally solid in nature.	Non-Metals May be Solid, Liquid or Gas.
Metals are shiny in appearance.	Non-Metals are dull in appearance.
Metals are good conductors of heat and Electricity.	Non-Metals are poor conductors of heat and Electricity.
Metal have high melting point.	Non-Metal have low melting point.
Metals have 1,2 or 3 Electron in their outermost shell.	Non-Metals have 4,5,6 or 7 Electron in their outermost shell.
Metals easily lose electrons.	Non- Metals gain electrons easily.
Metals react with water to form metal hydroxide and hydrogen gas.	Non- Metals generally do not react with water.

Reactivity Series

Arrangement of metals in decreasing order of their reactivity is called the reactivity series.

Reactivity Series (High to Low)- K>Na>Ca>Mg>Al>Zn>Pb>H>Cu>Hg>Ag>Au

Potassium is the most reactive metal, while Gold is the least reactive metal.

Metal Name	Symbol	Reactivity
Potassium	K	Very High
Sodium	Na	Very High
Calcium	Ca	High
Magnesium	Mg	Medium
Aluminium	Al	Medium
Zinc	Zn	Medium
Lead	Pb	Medium
Hydrogen	H	Reference
Copper	Cu	Low
Mercury	Hg	Low
Silver	Ag	Very Low
Gold	Au	Least

Chemical Properties Of Metals

1 Reaction of metals with air

• Metals react with oxygen present in air to form metal oxides.

Metal + O (Oxygen)——-> Metal Oxide

• Sodium (Na) and Potassium (K) react very fast with air and catch fire easily. Therefore, to prevent them from reacting , they are stored in kerosene oil.

4Na + O₂ —–> 2NaO

• Some Metals like ( Mg, Al, Zn & Pb) react slowly with air. Due to this reaction, a thin layer of oxide is formed on their surface. This oxide layer is useful for these metals because it is hard and prevents further contact of the metal with air.

4Al + 3O₂ ——> 2Al₂O₃

2Mg + O₂ ——> 2MgO

• Iron (Fe) does not react with air even on heating, but when iron powder is heated strongly, it reacts rapidly with air.

• Silver(Ag) and Gold(Au) do not react with oxygen.

Amphoteric Oxides Definition

Those metal oxides which react with both acids and bases to form salt and water are called amphoteric oxides.

Al₂O₃ + 6HCl —> 2AlCl₃ + H₂O

Al₂O₃ + 2NaOH —-> 2NaAlO₂ + H₂O

2 Reactions Of Metals With Water

When metals react with water, they form metal hydroxide ( Metal oxide) and hydrogen gas. Highly reactive metals such as sodium, potassium and calcium react with cold water.

Sodium (Na) Reacts with water to form Sodium Hydroxide (NaOH) and Hydrogen (H) gas.

2Na + H₂O —-> 2NaOH + H₂

Calcium (Ca) Reacts with Water to form Calcium Hydroxide (CaOH) And Hydrogen gas.

Ca + H₂O —–> Ca(OH)₂ + H₂

Magnesium(Mg) React With Hot Water.

Mg + 2H₂O ——> Mg(OH)₂ + H₂

Calcium and Magnesium React with Water, they start floating on the surface of water. This happens because during the reaction, bubbles of hydrogen gas are produced, which stick to the surface of the metal and make it float.

Al, Fe And Zn are less reactive metals. They react only with steam.

2Al + 3H₂O (Steam) ——-> Al₂O₃ + 3H₂

2Fe + 4H₂O (Steam) ——> Fe₃O₄ + 4H₂

Cu, Al, Ag, Au And Si do not react with water.

Reaction of Metals With Dilute Acids Complete Explanation

Highly reactive metals react with dilute acids. During this reaction, Salt and Hydrogen gas are formed.

Metal + Dilute —-> Salt + Hydrogen gas

2Na + 2HCl —-> 2NaCl + H₂ (gas)

Mg + 2HCl —-> MgCl2 + H₂ (gas)

Zn + 2HCl —-> ZnCl2 + H₂ (gas)

2Al + 6HCl —-> 2AlCl3 + 3H₂ (gas)

Note- Metals that are below hydrogen in the reactivity series do not react with dilute Acids.

Reaction of Metals with Other Metals ( Displacement Reaction)

A more reactive metal displaces a less reactive metal form its compound solution. This type of reaction is called a Displacement Reaction.

Metal (A) + Salt Solution (B) ——-> Salt Solution Of Metal (A) + Metal (B)

Reaction of Metals with Non-Metals

When a metal reacts with a non-metal, the atoms of the metal lose their electrons and form positive ions (cations). On the other hand, the atoms of the non-metal gain these electrons and form negative ions (anions). The positively charged ion of the metal and the negatively charged ion of the non-metal combine together to form an ionic compound. The bond formed between two atoms due to the transfer of electrons is called an ionic bond.

Example – Sodium chloride (NaCl), Potassium chloride (KCl)

Properties of Ionic Compounds

Physical Nature

Ionic compounds are generally solids.

This is because the force of attraction between their ions is very strong.

High Melting Point and Boiling Point

Due to very strong force of attraction between ions, ionic compounds have high melting point and high boiling point.

Solubility

Ionic compounds are soluble in water because water and ionic compounds are similar in nature. However, ionic compounds are not soluble in organic solvents like kerosene and petrol.

Electrical Conductivity

The aqueous solution of ionic compounds and molten (fused) ionic compounds conduct electricity because the positive and negative ions are free to move. In the solid state, ionic compounds do not conduct electricity.

Reaction of Sodium and Chlorine

Sodium is a metal. It has a total of 11 electrons.

Its electronic configuration is 2, 8, 1. Because it has one electron in its outermost shell, sodium easily loses this electron. Sodium wants to achieve the electronic configuration of a noble gas by losing one electron.

Chlorine is a non-metal. It has a total of 17 electrons.

Its electronic configuration is 2, 8, 7. Chlorine can gain one electron to complete 8 electrons in its outermost shell.

Reaction of Sodium and Chlorine In the reaction between sodium and chlorine, the sodium atom transfers one electron to the chlorine atom and forms sodium chloride.

Electron transfer process:

Na (2, 8, 1) → Na⁺ (2, 8) + e⁻

Cl (2, 8, 7) + e⁻ → Cl⁻ (2, 8, 8)

After this transfer, Na⁺ and Cl⁻ ions attract each other and form an ionic bond.

Extraction of Metals

The substance from which metals are extracted is called an ore. Those ores from which a metal can be extracted profitably and conveniently are called ores.

The ores which do not allow profitable extraction of metal are called gangue.

All ores are minerals, but all minerals are not ores.

Ores of Metals (Examples and Chemical Formula)

Metal	Ore	Chemical Formula
Iron	Hematite	Fe2O3
Iron	Magnetite	Fe3O4
Aluminium	Bauxite	Al2O3
Copper	Copper Sulphide	CuS
Zinc	Zinc Sulphide	ZnS
Mercury	Cinnabar	HgS

Various Steps of Extraction of Metals

Concentration of Ore

The ore is crushed and converted into fine powder.

The unwanted impurities present with the ore are separated. This process is called concentration of ore.

The impurities present with the ore are called gangue.

Roasting

Heating the ore in the presence of oxygen is called roasting. This process is used to convert metal sulphides into metal oxides.

Example  ZnS + O₂ (heat) → ZnO + SO₂

Calcination

Heating the ore in the absence of oxygen is called calcination. This process is used to convert metal carbonates into metal oxides.

Example ZnCO₃ (heat) → ZnO + CO₂

Corrosion of Metals

The weakening of metals due to environmental factors is called corrosion. The corrosion of iron is called rusting. The rusting of iron is affected by the following factors:

Presence of air

Presence of water

Presence of acidic gases in air

Corrosion of Silver

Silver articles react with sulphur dioxide present in air and form a layer of silver sulphide, which is black in colour.

Corrosion of Copper

Copper reacts with moisture and carbon dioxide to form copper carbonate, which is green in colour.

That is why copper articles turn green after some time.

Reduction

After converting the metal present in the ore into its oxide, it is reduced using carbon. Carbon is used because it is a cheap and easily available reducing agent. Carbon reacts with metal oxide and converts it into pure metal.

Example 2ZnO + C → 2Zn + CO₂ ↑

Extraction of Highly Reactive Metals

Metals like copper, zinc, sodium and potassium are extracted by the electrolytic refining method.

Electrolytic Refining

Anode-Impure metal

Cathode-Pure metal

Electrolyte-Copper sulphate solution with a small amount of sulphuric acid.

Electrolytic Refining (Working Method)

When electric current is passed, the impure metal from the anode dissolves into the solution along with impurities. The pure metal gets deposited on the cathode in the same amount. After some time, all the metal from the anode dissolves and gets deposited on the cathode. The impurities settle down below the anode, which is called anode mud.

Alloy

A homogeneous mixture of two or more metals is called an Alloy

Two important alloys of Copper

Brass– Cu 60-80% + Zinc 40-20%

German Silver – Copper(50)% + Zinc (30)% + Nickel (20)%

Use of Alloys

• Used in making household utensils and wires.
• Used in making statues and idols.