Chemical Bonding and Molecular Structure Test

Result

Chemical Bonding and Molecular Structure Test - 10

Score
-
out of -
Rank
-
out of -

TIME Taken - -

SHARING IS CARING

If our Website helped you a little, then kindly spread our voice using Social Networks. Spread our word to your readers, friends, teachers, students & all those close ones who deserve to know what you know now.

Weekly Quiz Competition

Question 1
1 / -0

The following question has four choices, out of which ONLY ONE is correct.

Arrangement of the molecules CH3Cl, CH2Cl2, CHCl3 and CCl4 in the order of increasing dipole moment is:

A
CH₃Cl < CH₂Cl₂< CHCl₃< CCl₄

B
CH₂Cl₂< CH₃Cl < CCl₄< CHCl₃

C
CCl₄< CHCl₃< CH₂Cl₂< CH₃Cl

D
CH₃Cl < CHCl₃< CH₂Cl₂< CCl₄

Solution

Let the C-Cl bond moment be denoted by μ. Since the C-Cl bond moments are inclined to each other at an angle of 109⁰27, the dipole moments of the molecules are as follow:
CCl₄ = 0; CH₃Cl = μ_^; CH₂Cl_{2 =}μ -_1/3μ= 2/3 μ_^;CHCl₃= μ - 2/3μ = 1/3μ
So, the correct order is CCl₄< CHCl₃< CH₂Cl₂< CH₃Cl.
Question 2
1 / -0

The following question has four choices, out of which ONLY ONE is correct.

Which of the following statements is true?

A
Bond angle in I₃^- is 90^o as the central I atom is sp³d hybridised with 3 of the orbitals occupied by the lone pairs.

B
Bond angle in BF₃ is 110^o; while that in [BF₄]^-,bond angle is nearly 109^o due to change in hybridisation of the central boron atom.

C
Bond angle in NH₃ is more than that in NF₃, as the greater electronegativity of fluorine causes the bonded electrons to move much towards fluorine atoms.

D
CIF₃ molecule is planar triangular as the lone pairs occupy axial positions.

Solution

This statement is true as bond pair-lone pair repulsion is weaker than lone pair-lone pair repulsion, and this leads to greater distortion of the bond angles from the tetrahedral value and gives F-N-F bond angle of 102^o30' as compared to 107^o48' in ammonia.
Question 3
1 / -0

On the basis of molecular orbital theory, bond order of NO is 2.5 and that of NO⁺ is 3. Which of the following statements is correct about bond lengths of NO and NO⁺?

A
Bond length of NO⁺ is greater than that of NO.

B
Bond length of NO⁺ is less than that of NO.

C
Bond length of NO⁺ is equal to that of NO.

D
Bond lengths cannot be predicted.

Solution

As we know that bond length is inversely proportional to bond order, bond length of NO⁺ is less than that of NO.
Question 4
1 / -0

Four elements A, B, C and D have atomic numbers Z - 4, Z, Z + 4 and Z + 5, respectively. If Z = 7, then which pair of the elements forms ionic bond?

A
B and C

B
A and D

C
A and C

D
C and D

Solution

If Z = 7, then atomic numbers of A, B, C and D are 3, 7, 11 and 12, respectively. Therefore, elements A, C and D are metallic elements and form metallic bonds with each other, while B is non-metallic in nature, it will form ionic bonds with A, C and D.

User

Question Analysis

Correct -
Wrong -
Skipped -

My Perfomance

Score
-
out of -
Rank
-
out of -

Re-Attempt Weekly Quiz Competition

Chemical Bonding and Molecular Structure Test - 10

Result

Chemical Bonding and Molecular Structure Test - 10

Score

-

Rank

-

SHARING IS CARING

Question 1

CH3Cl < CH2Cl2 < CHCl3 < CCl4

CH2Cl2 < CH3Cl < CCl4 < CHCl3

CCl4 < CHCl3 < CH2Cl2 < CH3Cl

CH3Cl < CHCl3 < CH2Cl2 < CCl4

Solution

Question 2

Bond angle in I3- is 90o as the central I atom is sp3d hybridised with 3 of the orbitals occupied by the lone pairs.

Bond angle in BF3 is 110o; while that in [BF4]-, bond angle is nearly 109o due to change in hybridisation of the central boron atom.

Bond angle in NH3 is more than that in NF3, as the greater electronegativity of fluorine causes the bonded electrons to move much towards fluorine atoms.

CIF3 molecule is planar triangular as the lone pairs occupy axial positions.

Solution

Question 3

Bond length of NO+ is greater than that of NO.

Bond length of NO+ is less than that of NO.

Bond length of NO+ is equal to that of NO.

Bond lengths cannot be predicted.

Solution

Question 4

B and C

A and D

A and C

C and D

Solution

User

Question Analysis

My Perfomance

Score

-

Rank

-

Results Announcement on: coming Monday

Stay Tuned: We’ll update you on your result via email or SMS.

CH₃Cl < CH₂Cl₂< CHCl₃< CCl₄

CH₂Cl₂< CH₃Cl < CCl₄< CHCl₃

CCl₄< CHCl₃< CH₂Cl₂< CH₃Cl

CH₃Cl < CHCl₃< CH₂Cl₂< CCl₄

Bond angle in I₃^- is 90^o as the central I atom is sp³d hybridised with 3 of the orbitals occupied by the lone pairs.

Bond angle in BF₃ is 110^o; while that in [BF₄]^-,bond angle is nearly 109^o due to change in hybridisation of the central boron atom.

Bond angle in NH₃ is more than that in NF₃, as the greater electronegativity of fluorine causes the bonded electrons to move much towards fluorine atoms.

CIF₃ molecule is planar triangular as the lone pairs occupy axial positions.

Bond length of NO⁺ is greater than that of NO.

Bond length of NO⁺ is less than that of NO.

Bond length of NO⁺ is equal to that of NO.