8.Elements of Group 1 and Group 2

Qno.1. Explain the following  

A. Hydrogen shows similarity with alkali metals as well as halogens.[2 Marks]

Ans:-

i. Electronic configuration of hydrogen is 1s¹ which is similar to the outer electronic configuration of alkali metals of group 1 i.e., ns¹.

ii. However, 1s¹ also resembles the outer electronic configuration of group 17 elements i.e., ns²np⁵.

iii. By adding one electron to H, it will attain electronic configuration of the inert gas He which is 1s² and by adding one electron to ns²np⁵ we get ns²np⁶ which is the outer electronic configuration of the remaining inert gases.

iv. Therefore, some chemical properties of hydrogen are similar to those of alkali metals while some resemble halogens.

Hence, hydrogen shows similarity with alkali metals as well as halogens.

B. Standard reduction potential of alkali metals have high negative values. 

[2 Marks ]

Ans:-

i. The general outer electronic configuration of alkali metals is ns¹.

ii. They readily lose one valence shell electron to achieve stable noble gas configuration and hence, they are highly electropositive and are good reducing agents.

Hence, standard reduction potentials of alkali metals have high negative values.

C. Alkaline earth metals have low values of electronegativity; which decrease down the group. [2 Marks]

Ans:-

i. Electronegativity represents attractive force exerted by the nucleus on shared electrons.

ii. The general outer electronic configuration of alkaline earth metals is ns². They readily lose their two valence shell electrons to achieve stable noble gas configuration.

iii. They are electropositive and hence, they have low values of electronegativity.

As we move down the group atomic size increases, shielding effect increases and effective nuclear charge decreases. Thus, tendency to attract shared electrons decreases down the group.

Hence, the values of electronegativity decrease down the group.

D. Sodium dissolves in liquid ammonia to form a solution which shows electrical conductivity.  [1 Marks]

Ans:-

i. Sodium dissolves in liquid ammonia giving deep blue coloured solutions which is electrically conducting in nature.

Na + (x + y) NH₃ → [Na(NH₃)x]⁺ + [e(NH₃)y]⁻

ii. Due to formation of ions, the solution shows electrical conductivity.

E. BeCl₂ is covalent while MgCl₂ is ionic.

[2 Marks]

Ans:- 

i. Be²⁺ ion has very small ionic size and therefore, it has very high charge density.

ii. Due to this, it has high tendency to distort the electron cloud around the negatively charged chloride ion (Cl⁻) which is larger in size.

iii. This results in partial covalent character of the bond in BeCl₂.

iv. Mg²⁺ ion has very less tendency to distort the electron cloud of Cl⁻ due to the bigger size of Mg²⁺ as compared to Be²⁺.

Hence, BeCl₂ is covalent while MgCl₂ is ionic.

F. Lithium floats on water while sodium floats and catches fire when put in water.  

[2 Marks]

Ans:-

i. When lithium and sodium react with water, hydrogen gas is released. Due to these hydrogen gas bubbles, lithium and sodium float on water.

eg. 2Na + 2H₂O ⟶ 2NaOH + H₂↑

ii. The reactivity of group 1 metals increases with increasing atomic radius and lowering of ionization enthalpy down the group.

iii. Thus, sodium having lower ionization enthalpy, is more reactive than lithium.

iv. Hence, lithium reacts slowly while sodium reacts vigorously with water.

v. Since the reaction of sodium with water is highly exothermic, it catches fire when put in water.

Qno.2. Write balanced chemical equations for the following.  

A. CO₂ is passed into concentrated solution of NaCl, which is saturated with NH₃.  [2 Marks]

Ans:-

2NH₃(aq) + H₂O(l) +  

(Ammonia)

 CO₂(g)→(NH₄)₂CO₃(aq)

                 Ammonium carbonate 

(NH₄)₂CO₃(aq) + H₂O(l) + CO₂(g)→2NH₄HCO₃(s)

              Ammonium bicarbonate 

(NH₄)₂CO₃(aq) + NaCl(aq) →NaHCO₃(s) + 

Ammonium     From brine      sodium 

bicarbonate     solution         bicarbonate 

                                                 ( Precipitate)

NH₄Cl(aq)

B. A 50% solution of sulphuric acid is subjected to electrolytic oxidation and the product is hydrolysed.  [2 Marks]

Ans:-

i. Electrolytic oxidation:

At anode:

2HSO₄⁻→{Electrolysis} H₂S₂(O₂)₄ + 2e

                         (Peroxydisulphuric acid)

ii. Hydrolysis:

 HO - SO₂ - O - O - SO₂ - OH + 2H₂O 

(Peroxydisulphuric acid)

→ 2H₂SO₄ + H₂O₂

                   (Hydrogen peroxide)

C. Magnesium is heated in air.    [1 Marks]

Ans:-

i. 2Mg        +   O₂(Δ) →2MgO

 Magnesium  oxygen  Magnesium oxide 

ii. 3Mg       +  N₂(Δ)    → Mg₃N₂

Magnesium Nitrogen     Magnesium 

                                            nitride

D. Beryllium oxide is treated separately with aqueous HCl and aqueous NaOH solutions.  [2 Marks]

Ans:-

Beryllium oxide (BeO) is an amphoteric oxide and thus, it reacts with both acid (HCl) as well as base (NaOH) to give the corresponding products.

i.BeO + 2HCl→ BeCl₂ + H₂O 

            (Acid)

ii.BeO + 2NaOH→Na₂BeO₂ + H₂O 

              (Base)

Qno.3. Answer the following questions  

A. Describe the diagonal relationship between Li and Mg with the help of two illustrative properties.  [4 Marks]

Ans:-

i.

a. The relative placement of these elements with similar properties in the periodic table is across a diagonal and is called diagonal relationship.

b. Lithium is placed in the group 1 and period 2 of the modern periodic table. It resembles with magnesium which is placed in the group 2 and period 3.

ii. Li and Mg show similarities in many of their properties.

e.g.  

a. Reaction with oxygen:  

1. Group 1 elements except lithium, react with oxygen present in the air to form oxides (M₂O) as well as peroxides (M₂O₂) and superoxides (MO₂) on further reaction with excess of oxygen.  

2. This anomalous behaviour of lithium is due to its resemblance with magnesium as a result of diagonal relationship.  

3. As group 2 elements form monoxides i.e., oxides, lithium also form monoxides.

4Li + O₂ (Δ) → 2Li₂O  

Lithium metal + Oxygen → Lithium monoxide

Mg + O₂(Δ) → 2MgO  

Magnesium metal + Oxygen → Magnesium monoxide (oxide)

b. Reaction with nitrogen:

1. All the group 1 elements react only with oxygen present in the air to form oxides while group 2 elements react with both nitrogen and oxygen present in the air forming corresponding oxides and nitrides.

2. However, lithium reacts with oxygen as well as nitrogen present in the air due to its resemblance with magnesium.

6Li + N₂ (Δ)→2Li₃N  

Lithium  Lithium nitride                

3Mg + N₂ (Δ)→ Mg₃N₂  

Magnesium  Magnesium nitride                    

B. Describe the industrial production of dihydrogen from steam. Also write the chemical reaction involved.  [3 Marks]

Ans:-

Three stages are involved in the industrial production of dihydrogen from steam.

i. Stage 1:

a. Reaction of steam on hydrocarbon or coke (C) at 1270 K temperature in presence of nickel catalyst gives water-gas which is a mixture of carbon monoxide and hydrogen.

1. Reaction of steam with hydrocarbon:

CH₄(g) + H₂O(g) →(1270K, Ni)   

Methane Steam      

(Hydrocarbon)

CO(g) + 3H₂(g)

Water-gas(syngas)            

2. Reaction of steam with coke or carbon (C):

C(s) + H₂O(g) →(1270K, Ni) CO(g) + H₂(g)

b.Sawdust, scrapwood, etc. can also be used in place of carbon.

ii. Stage 2: Water-gas shift reaction:

When carbon monoxide in the water-gas reacts with steam in the presence of iron chromate (FeCrO₄) as catalyst, it gets transformed into carbon dioxide. This is called water-gas shift reaction.

CO(g) + H₂O(g) →(673K, Iron chromate Carbon  Steam                          catalyst)

monoxide 

(from syngas mixture) 

 CO₂(g) + H₂(g)   

 Carbon    Hydrogen

 dioxide  

iii. Stage 3: In the last stage, carbon dioxide is removed by scrubbing with sodium arsenite solution.

C. A water sample, which did not give lather with soap, was found to contain Ca(HCO₃)₂ and Mg(HCO₃)₂. Which chemical will make this water give lather with soap? Explain with the help of chemical reactions.  [2 Marks]

Ans:-

i. Soap does not lather in hard water due to presence of the soluble salts of calcium and magnesium in it. So, the given water sample is hard water.

ii. Hardness of hard water can be removed by removal of these calcium and magnesium salts.

iii. Sodium carbonate is used to make hard water soft as it precipitates out the soluble calcium and magnesium salts in hard water as carbonates. Thus, it will make water give lather with soap.

e.g. Ca(HCO₃)₂(aq) + Na₂CO₃(aq) → CaCO₃(s) + 2NaHCO₃(aq)

D. Name the isotopes of hydrogen. Write their atomic composition schematically and explain which of these is radioactive?

[3 Marks]

Ans:-

i. Hydrogen has three isotopes i.e., hydrogen (¹H ), deuterium (²H) and tritium (³H) with mass numbers 1, 2 and 3 respectively.

ii. They all contain one proton and one electron but different number of neutrons in the nucleus.

iii. Atomic composition of isotopes of hydrogen:

iv. Tritium is a radioactive nuclide with half-life period 12.4 years and emits low energy ẞ particles.

v. Schematic representation of isotopes of hydrogen is as follows:

Qno.4. Name the following

A. Alkali metal with smallest atom.

Ans:- Lithium (Li)

B. The most abundant element in the universe.

Ans:- Hydrogen (H)

C. Radioactive alkali metal.

Ans:- Francium (Fr)

D. Ions having high concentration in cell sap.

Ans:- Potassium ions (K⁺)

E. A compound having hydrogen, aluminium and lithium as its constituent elements.

Ans:- Lithium aluminium hydride(LiAlH₄)

Qno.5. Choose the correct option.

A. The unstable isotope of hydrogen is .....

 a. H-1

 b. H-2

 c. H-3 

 d. H-4

B. Identify the odd one.

 a. Rb

 b. Ra

 c. Sr 

 d. Be

C. Which of the following is Lewis acid?

 a. BaCl₂ 

 b. KCl

 c. BeCl₂

 d. LiCl

D. What happens when crystalline Na₂CO₃ is heated?

   a. releases CO₂

   b. loses H₂O

   c. decomposes into NaHCO₃

   d. colour changes.