S- And p-Block Elements Test

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S- And p-Block Elements Test - 4

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following statements are FALSE?

P. All the bonds that are present in PCl₅ are similar.
Q. ICl is more reactive than I₂.
R. Chlorine is a stronger oxidising agent than fluorine.
S. Pentahalides are more covalent than trihalides.

A
Both P and Q

B
Both P and R

C
Both P and S

D
Both Q and R

E
Both Q and S

Solution

PCl₅ has a trigonal bipyramidal structure. All the bonds that are present in PCl₅ are not similar. The bond length of the P-Cl bonds in the equatorial plane is different from the bond length of the P-Cl bonds in the axial plane. Hence, the statement 'P' is false.
F₂ is a stronger oxidising agent than Cl₂. Hence, the statement 'R' is false.
The I-I bond is stronger than the I-Cl bond, consequently ICl is more reactive than I₂. Hence, the statement 'Q' is true.
Pentahalides are more covalent than trihalides as the polarizing power of the central ion is greater in the higher oxidation state. This imparts a greater covalent character to the molecule. Hence, the statement 'S' is true.
Question 2
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What is the correct order of thermal stability of hydrides of group 16 elements?

A
H₂Po > H₂Te > H₂Se > H₂S > H₂O

B
H₂Po > H₂Se > H₂S > H₂Te > H₂O

C
H₂S > H₂O > H₂Te > H₂Se > H₂Po

D
H₂O > H₂S > H₂Se > H₂Te > H₂Po

E
H₂O > H₂Se > H₂S > H₂Po > H₂Te

Solution

The bond dissociation enthalpy (H−E) of hydrides decreases on moving down the group and consequently the thermal stability decreases.
The decreasing order of thermal stability of the group 16 hydrides is:
H₂O > H₂S > H₂Se > H₂Te > H₂Po
Question 3
1 / -0

Which of the following represents the correct order of reducing character of hydrides of group 15 elements?

A
NH₃< PH₃< AsH₃< SbH₃< BiH₃

B
PH₃< NH₃< AsH₃< SbH₃< BiH₃

C
NH₃< PH₃< BiH₃< AsH₃< SbH₃

D
BiH₃< PH₃< AsH₃< SbH₃< NH₃

E
BiH₃< SbH₃< AsH₃< PH₃< NH₃

Solution

As we move down a group, the atomic size increases and the stability of the hydrides of group 15 elements decreases. Since the stability of hydrides decreases on moving from NH₃ to BiH₃, the reducing character of the hydrides increases on moving from NH₃ to BiH₃. Hence, the correct order of reducing character is NH₃< PH₃< AsH₃< SbH₃< BiH₃.
Question 4
1 / -0

Which of the following statements are FALSE?

P. The boiling point of PH₃ is lower than that of NH₃.
Q. Red phosphorus is more reactive than white phosphorus.
R. Phosphorus is sp³ hybridised in PCl₃.
S. In the solid state, PCl₅ exists as a covalent solid.

A
Both P and Q

B
Both P and R

C
Both P and S

D
Both Q and S

E
Both Q and R

Solution

White phosphorus has a tetrahedral basic unit where four phosphorus atoms arranged at the four corners of a tetrahedron are joined together by a total of six single bonds.
The molecule is under tremendous strain, hence white phosphorous is highly reactive.
However, the strain is much less in case of red phosphorous on account of its polymeric structure.
Therefore, chemically, red phosphorus is much less reactive than white phosphorus and statement Q is incorrect.
In the solid state, PCl₅exists as an ionic solid [PCl₄]⁺[PCl₆]^–, in which the cation [PCl₄]⁺ is tetrahedral and the anion [PCl₆]^– is octahedral.
Hence, statement S is incorrect.
Option (4) is the correct answer.
Question 5
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Directions: In the following question, there are two statements, Assertion A and Reason R. Consider both the statements independently and mark your answer.

Assertion A: Elements of Group 16 generally show lower value of first ionization enthalpy as compared to the corresponding periods of Group 15.
Reason R: Due to extra stable half-filled p orbital electronic configurations of Group 15 elements, larger amount of energy is required to remove electrons as compared to Group 16 elements.

A
A and R both are correct and R is the correct explanation of A.

B
A and R both are correct and R is not the correct explanation of A.

C
A is correct and R is incorrect.

D
A is incorrect and R is correct.

E
A and R both are incorrect.

Solution

A and R both are correct and R is the correct explanation of A.
Elements of Group 16 generally show lower value of first ionization enthalpy as compared to the corresponding periods of group 15. Due to extra stable half-filled p orbitals electronic configurations of Group 15 elements, larger amount of energy is required to remove electrons as compared to Group 16 elements.
Question 6
1 / -0

Which of the following statements are TRUE?

1. H₂S is more acidic than H₂Te.
2. Ozone is thermodynamically more stable than oxygen.
3. The two oxygen-oxygen bond lengths in the ozone molecule are identical.
4. Rhombic sulphur is the stable form of sulphur at room temperature.

A
Both 1 and 2

B
Both 1 and 4

C
Both 2 and 3

D
Both 3 and 4

E
Both 2 and 4

Solution

The two oxygen-oxygen bond lengths in the ozone molecule are identical (128 pm) and the molecule is angular as expected with a bond angle of about 117^o.
Sulphur forms numerous allotropes, of which the yellow rhombic and monoclinic forms are the most important. The stable form at room temperature is rhombic sulphur, which transforms to monoclinic sulphur when heated above 369 K.
Question 7
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Directions: In the following question, there are two statements, Assertion (A) and Reason (R). Consider both the statements independently and mark your answer.

Assertion (A): Halogens have the maximum negative electron gain enthalpy in their respective periods in the periodic table.
Reason (R): Halogens have the largest size in their respective periods and therefore, the highest effective nuclear charge.

A
A and R both are correct and R is the correct explanation of A.

B
A and R both are correct and R is not the correct explanation of A.

C
A is correct and R is incorrect.

D
A is incorrect and R is correct.

E
A and R both are incorrect.

Solution

Halogens have the maximum negative electron gain enthalpy in their respective periods in the periodic table. They have the smallest size in their respective periods and therefore, the highest effective nuclear charge. As a consequence, they readily accept one electron to acquire noble gas electronic configuration.

Question 8

1 / -0

Match the following:

Column – I (Compound)	Column – II (Use)
A. O₂F₂	1. Estimation of carbon monoxide
B. ClO₂	2. Bleaching agent for paper pulp and textiles
C. I₂O₅	3. Removal of plutonium from spent nuclear fuel

A - 1, B - 2, C - 3

A - 2, B - 1, C - 3

A - 3, B - 2, C - 1

A - 2, B - 3, C - 1

A - 3, B - 1, C - 2

Solution

O₂F₂ oxidises plutonium to PuF₆ and the reaction is used in removing plutonium as PuF₆ from spent nuclear fuel.
ClO₂ is used as a bleaching agent for paper pulp and textiles and in water treatment.
I₂O₅ is a very good oxidising agent and is used in the estimation of carbon monoxide.

Question 9
1 / -0

The correct order of hydration enthalpies of alkali metal ions is

A
Na⁺> Li⁺ > K⁺> Rb⁺ > Cs⁺

B
Li⁺> K⁺ > Na⁺ > Rb⁺> Cs⁺

C
Li⁺> Na⁺> K⁺ > Rb⁺ > Cs⁺

D
Cs⁺> Rb⁺ > Na⁺ > K⁺ > Li⁺

E
Cs⁺> Rb⁺ > K⁺ > Na⁺ > Li⁺

Solution

Correct order of hydration enthalpies is Li⁺ > Na⁺ > K⁺ > Rb⁺ > Cs⁺, because as we move from Li to Cs, the size increases and charge to radius ratio decreases, and it is difficult for the metal to be surrounded by water molecules. Hence, less energy is released when the size increases. Therefore, Li is the most heavily hydrated ion among alkali metal cations and Cs⁺ is the least hydrated ion.
Question 10
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The alkali metals and their salts impart characteristic colour to an oxidising flame. Which of the following matchings of alkali metals and characteristic colour imparted to an oxidising flame by them is correct?

A
Li : Red violet

B
Na : Blue

C
K : Violet

D
Rb : Crimson red

E
Cs : Yellow

Solution

Potassium imparts violet colour to an oxidising flame.

Question 11

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Match the column – I (element) with column – II (use) and select the correct option.

Column – I	Column – II
A. Sodium	1. Making windows of X-ray tubes
B. Beryllium	2. Coolant in fast breeder nuclear reactors
C. Cesium	3. Radiation therapy
D. Radium	4. Photoelectric cells

A - 1, B - 2, C - 3, D - 4

A - 2, B - 1, C - 4, D - 3

A - 4, B - 2, C - 3, D - 1

A - 2, B - 3, C - 1, D - 4

A - 4, B - 3, C - 2, D - 1

Solution

Liquid sodium metal is used as a coolant in fast breeder nuclear reactors.
Metallic beryllium is used for making windows of X-ray tubes.
Cesium is used in devising photoelectric cells.
Radium salts are used in radiotherapy, for e.g., in the treatment of cancer.

Question 12
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In which of the following does the solubility in water increase down the group?

I. Alkaline earth metal hydroxides
II. Alkaline earth metal carbonates
III. Alkaline earth metal sulphates

A
Only I

B
Only II

C
Only III

D
Both I and II

E
Both II and III

Solution

In alkaline earth metal hydroxides, the anion being common, the cationic radius will influence the lattice enthalpy.
Question 13
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Which of the following statements are FALSE?

1. Compounds of alkaline earth metals are less hydrated than those of alkali metals.
2. Quicklime exhibits thermoluminescence.
3. Aqueous solution of calcium hydroxide is known as milk of lime.
4. Oxide and hydroxide of beryllium are amphoteric in nature.

A
Only 1 and 2

B
Only 1 and 3

C
Only 1 and 4

D
Only 2 and 3

E
Only 3 and 4

Solution

Compounds of alkaline earth metals are more extensively hydrated than those of alkali metals.
Aqueous solution of calcium hydroxide is known as slaked lime and when excess water is added, a suspension is formed which is known as the milk of lime or whitewash. On filtration, the filtrate (saturated solution) obtained is known as limewater.
Question 14
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Which of the following alkaline earth metals crystallize in face centered cubic structure?
1. Beryllium
2. Magnesium
3. Calcium
4. Strontium
5. Barium

A
Both 1 and 2

B
1, 2 and 5

C
Both 2 and 3

D
Both 3 and 4

E
3, 4 and 5

Solution

Calcium and strontium crystallize in face centered cubic structure.
Question 15
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Which of the following metals do not impart characteristic colour to oxidizing flame?

A
Li and Na

B
Cs and Ba

C
Be and Mg

D
K and Ca

E
Li and Be

Solution

Yes, Beryllium and magnesium do not impart characteristic colour to oxidizing flame.
Question 16
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Which of the following terms statements are TRUE?
P. All alkali metal elements form solid hydrogen carbonates.
Q. Calcium is fifth most abundant element in the earth's crust.
R. Francium is highly radioactive.
S. Hydration enthalpies of alkaline earth metal ions are larger than those of alkali metal ions.

A
P and Q

B
P and S

C
Q and R

D
Q and S

E
R and S

Solution

Francium is highly radioactive; its longest-lived isotope 223-Fr has a half-life of only 21 minutes.
The hydration enthalpies of alkaline earth metal ions are larger than those of alkali metal ions. Thus, compounds of alkaline earth metals are more extensively hydrated than those of alkali metals, e.g., MgCl₂ and CaCl₂ exist as MgCl₂.6H₂O and CaCl₂.6H₂O while NaCl and KCl do not form such hydrates.
Question 17
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Which of the following statements regarding alkaline earth metals is/are incorrect?

1. All alkaline earth metal oxides are basic.
2. All alkaline earth metal hydrides are ionic.
3. Stability of peroxides of alkaline earth metals increases down the group.
4. The thermal stability of alkaline earth metal hydroxides increases down the group.

A
1 and 2

B
1 and 4

C
2 and 3

D
2 and 4

E
3 and 4

Solution

Except BeO, which is amphoteric, all alkali metal and alkaline earth metal oxides are basic.
Question 18
1 / -0

Li resembles Mg mainly due to similarity in sizes of their atoms and ions. The main points of similarity are:

i. Both LiOH and Mg(OH)₂ are strong bases.
ii. Carbonates of both, on heating, decompose to produce oxides and carbon dioxide.
iii. Both react with nitrogen to give covalent nitrides.
iv. Both Li and Mg form solid bicarbonates.
v. LiCl and MgCl₂ are soluble in ethanol.
vi. The hydroxides, bicarbonates and fluorides of both Li and Mg are sparingly soluble in water.

A
i, iii and iv

B
i, iv and vi

C
ii, iii and v

D
ii, v and vi

E
iv, v and vi

Solution

Li resembles Mg mainly due to similarity in sizes of their atoms and ions. The main points of similarity are:
1. Both Li and Mg are quite hard.
2. Both LiOH and Mg(OH)₂ are weak bases.
3. Carbonates of both Li and Mg, on heating, decompose to produce oxides and carbon dioxide.
4. Both Li and Mg react with nitrogen to give ionic nitrides.
5. Nitrates of both Li and Mg decompose on heating to give oxides.
6. Both Li and Mg do not form solid bicarbonates.
7. Because of covalent character, LiCl and MgCl₂ are soluble in ethanol.
8. The hydroxides, bicarbonates and fluorides of both Li and Mg are sparingly soluble in water.
Hence, option (4) is correct.
Question 19
1 / -0

Which of the following statement are true?

1. Melting points of alkaline earth metals are greater than those of alkali metals.
2. All alkali metal carbonates are stable at a temperature around 800^oC.
3. Carbonates of alkali metals are more stable to heat than carbonates of alkaline earth metals.

A
Only 1

B
Only 2

C
3 only

D
Both 1 and 2

E
Both 2 and 3

Solution

Melting points of alkaline earth metals are greater than those of alkali metals.
Reason:
1. The atoms of alkaline earth metals have two delocalized electrons and their sizes are smaller than those of alkali metals.
2. Alkaline earth metals have closed-packed structure while alkali metals have open structure (body-centered cubic).
Hence, the statement (1) is correct.

All alkali metal carbonates (except lithium carbonate) are stable at a temperature around 800°C. Lithium carbonate decomposes around 700°C forming lithium oxide and carbon dioxide. The relative instability of lithium carbonate is due to the small size Li⁺, and hence a very large charge/radius ratio of Li⁺ ion.
Hence, the statement (2) is incorrect.

Alkaline earth metal ions are much smaller than alkaline metal ions and carry a higher charge. Therefore, their polarizing power is greater. Electron cloud of carbonate anions are more easily distorted by alkaline earth metal ions than by alkali metal ions. Carbonates of alkali metals are therefore less stable to heat and decompose to metal oxide and carbon dioxide. Hence, the statement (3) is incorrect.
Question 20
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Which of the following elements are radioactive?

1. Cesium
2. Barium
3. Radium
4. Francium
5. Rubidium

A
Cesium, Barium, Radium

B
Only Barium and Francium

C
Radium and Francium

D
Radium, Francium and Rubidium

E
Only Francium and Rubidium

Solution

Radium (Alkaline earth metal) and Francium ( alkali metal) are radioactive elements.

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S- And p-Block Elements Test - 4

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S- And p-Block Elements Test - 4

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Question 1

Both P and Q

Both P and R

Both P and S

Both Q and R

Both Q and S

Solution

Question 2

H2Po > H2Te > H2Se > H2S > H2O

H2Po > H2Se > H2S > H2Te > H2O

H2S > H2O > H2Te > H2Se > H2Po

H2O > H2S > H2Se > H2Te > H2Po

H2O > H2Se > H2S > H2Po > H2Te

Solution

Question 3

NH3 < PH3 < AsH3 < SbH3 < BiH3

PH3 < NH3 < AsH3 < SbH3 < BiH3

NH3 < PH3 < BiH3 < AsH3 < SbH3

BiH3 < PH3 < AsH3 < SbH3 < NH3

BiH3 < SbH3 < AsH3 < PH3 < NH3

Solution

Question 4

Both P and Q

Both P and R

Both P and S

Both Q and S

Both Q and R

Solution

Question 5

A and R both are correct and R is the correct explanation of A.

A and R both are correct and R is not the correct explanation of A.

A is correct and R is incorrect.

A is incorrect and R is correct.

A and R both are incorrect.

Solution

Question 6

Both 1 and 2

Both 1 and 4

Both 2 and 3

Both 3 and 4

Both 2 and 4

Solution

Question 7

A and R both are correct and R is the correct explanation of A.

A and R both are correct and R is not the correct explanation of A.

A is correct and R is incorrect.

A is incorrect and R is correct.

A and R both are incorrect.

Solution

Question 8

A - 1, B - 2, C - 3

A - 2, B - 1, C - 3

A - 3, B - 2, C - 1

A - 2, B - 3, C - 1

A - 3, B - 1, C - 2

Solution

Question 9

Na+ > Li+ > K+ > Rb+ > Cs+

Li+ > K+ > Na+ > Rb+ > Cs+

Li+ > Na+ > K+ > Rb+ > Cs+

Cs+ > Rb+ > Na+ > K+ > Li+

Cs+ > Rb+ > K+ > Na+ > Li+

Solution

Question 10

Li : Red violet

Na : Blue

K : Violet

Rb : Crimson red

Cs : Yellow

Solution

Question 11

A - 1, B - 2, C - 3, D - 4

H₂Po > H₂Te > H₂Se > H₂S > H₂O

H₂Po > H₂Se > H₂S > H₂Te > H₂O

H₂S > H₂O > H₂Te > H₂Se > H₂Po

H₂O > H₂S > H₂Se > H₂Te > H₂Po

H₂O > H₂Se > H₂S > H₂Po > H₂Te

NH₃< PH₃< AsH₃< SbH₃< BiH₃

PH₃< NH₃< AsH₃< SbH₃< BiH₃

NH₃< PH₃< BiH₃< AsH₃< SbH₃

BiH₃< PH₃< AsH₃< SbH₃< NH₃

BiH₃< SbH₃< AsH₃< PH₃< NH₃

Na⁺> Li⁺ > K⁺> Rb⁺ > Cs⁺

Li⁺> K⁺ > Na⁺ > Rb⁺> Cs⁺

Li⁺> Na⁺> K⁺ > Rb⁺ > Cs⁺

Cs⁺> Rb⁺ > Na⁺ > K⁺ > Li⁺

Cs⁺> Rb⁺ > K⁺ > Na⁺ > Li⁺