QnA - Metals and Non Metals

1. Silver is a better conductor of heat and causes the wax to melt faster

2. Aluminium wire will not melt due to high melting point , the spirit lamp undergoes incomplete combustion

1. Copper does not react even with steam

2. Calcium and magnesium float on water as they form hydroxides.

1. 2Al + 3H₂SO₄ → Al₂(SO₄)₃ +3H₂

2. Mg + 2HNO₃ → Mg(NO₃)₂ + H₂

1. Iron is more reactive than copper

2. Displacement reaction occurs displacing the copper in the iron to form FeSO4 

3. Fe + CuSO₄ → FeSO₄ + Cu

YX₂

1. Sodium and pottasium

2. FeO an Fe₂O₃

3. Iron , nickel , chormiuium , manganese

1. Due to the oxidation of copper and the formation CuCO₃ and Cu(OH)₂

2. No we should not , rusting of iron is far more dangerous and causes damage to the structure of the building , oxidation of copper only forms a protective layer around it. 

3. Copper is malleable making it easier to shape into domes. It is more resistant to corrosion.

1. No we cannot stroe X in water , it will undergo a highly explosive exothermic reaction.

2. Sodium 

3. NaCl ⇌ Na⁺ + Cl⁻

4. Obtained by electrolytic refining of their molten chlord

5. At chathode - Na+ + e- → Na

6. At anode - 2Cl⁻ → Cl₂ + e⁻

1. Sodium - cold water and hot water

2. Calcium - cold water and hot water

3. Magnesium - hot water 

1. Nitric acid is. strong oxidising agent. When a metal reacts with nitric acid the hydrogen produced is immediately oxidised to water. Nitric acid gets reduced into nitrogenous oxides.

2. Zinc oxide can react with both acid and bases to produce salt and water , which makes it an amphoteric.

3. Due to the presence of free electrons it allows for eletricity to flow through the metal

1. B is the most reactive

2. B can displace copper from copper sulphate solution

3. B - A - C -  D

1. Bubbles  is observed showing the formation of hydrogen gas

2. The solid dissolved into water as both water and salt are formed

3. No reaction occurs

4. Brisk Effervescence due to evolution of CO2

1. Aluminum

2. 2Al + 6HCl → 2AlCl₃ + 3H₂

3. 2Al + 2NaOH + 2H₂O → 2NaAlO₂ + 3H₂

4. Thermite reaction occurs , which is highly exothermic

   1. 2Al + Fe₂O₃ → Al₂O₃ + 2Fe + Heat

1. Aluminium has 3 electrons in its outermost shell giving it a valency of 3 , Oxygen has 6 electrons in its outermost shell , hence it would like to receive 2 electrons or in other words has a valency of 2. They combine to form Al₂O₃ (show electron structure)

2. It is an ionic compound so it will

3. Ionic compounds are soluble in water and insoluble in organic solvents like alcohol and kerosene.

4. Stronger inter-ionic  force of attraction the postive and negative ions and it takes a large amount of energy to break said bonds.

1. 2Cu + O₂ → 2CuO

2. As they react with both acids and bases. ZnO or Al₂O₃

3. Na₂O + H₂O → 2NaOH

4. 2Al + 2NaOH → 2NaAlO₂ + 3H₂

1. It is placed in the middle of reactivity below Zinc and above lead

2. found as oxides (Fe₂O₃) , sulphides (FeS) or carbonates (FeCO₃)

Feature	Roasting	Calcination
Process	Heating the ore strongly in thepresence of excess air.	Heating the ore strongly inlimited air(or absence of air).
Ore Type	Generally used forSulphide ores.	Generally used forCarbonate ores.
Example	$2ZnS + 3O_2 \xrightarrow{\text{Heat}} 2ZnO + 2SO_2$	$ZnCO_3 \xrightarrow{\text{Heat}} ZnO + CO_2$