Test: The Valence Shell Electron Pair Repulsion Theory (NCERT)


15 Questions MCQ Test NCERTs for NEET: Textbooks, Tests & Solutions | Test: The Valence Shell Electron Pair Repulsion Theory (NCERT)


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Attempt Test: The Valence Shell Electron Pair Repulsion Theory (NCERT) | 15 questions in 15 minutes | Mock test for NEET preparation | Free important questions MCQ to study NCERTs for NEET: Textbooks, Tests & Solutions for NEET Exam | Download free PDF with solutions
QUESTION: 1

According to VSEPR theory

Solution:

The pairs of electrons tend to occupy such positions that place them farthest from each other and minimise repulsions.

QUESTION: 2

In a bonded molecule, the order of repulsion between the bonded and non-bonded electrons is

Solution:

Lone pair-lone pair lp - lp repulsions are considered stronger than lone pair-bonding pair lp - bp repulsions, which in turn are considered stronger than bonding pairbonding pair bp - bp repulsions, This is because the lone pair of electrons are attracted towards single nuclei only whereas bond pair electrons are attracted towards two nuclei. Thus the strength of the lone pair-lone pair repulsion is supposed to be more than bond pair-bond pair or bond pair-lone pair repulsion.

QUESTION: 3

The shape of water molecule which should be tetrahedral has a bent or distorted tetrahedral shape with a bond angle 104.5°. What could be the reason for this?

Solution:

Due to presence of lone pairs, the repulsion is more which changes the bond angle to 104.5°.

QUESTION: 4

Which of the following shapes of SF4 is more stable and why?

Solution:

In structure (ii), Ip-bp repulsions are minimum.

QUESTION: 5

The most stable shape of ClF3 is shown by

Solution:

In (i), the Ip are atequatorial position so there are less Ip - bp repulsions as compared to other positions.

Hence, T-shape is moststable.

QUESTION: 6

In which of the following molecules the central atomdoes not retain any lone pair of electrons?

Solution:

In all other molecules, N and O retain lone pair
of electrons.

QUESTION: 7

Few examples of the compounds formed by chemical bonding are given below. Mark the incorrect example.

Solution:

The correct example is H2O. NH3 is pyramidal and bond angle is 104.50.

QUESTION: 8

Which of the following statements is correct regarding the structure of PCI5?

Solution:

In PCI5, three axial and two equatorial bonds are present.

QUESTION: 9

Match the molecules given in column I with their shapes given in column II and mark the appropriate choice

Solution:

(A) SF−  Octahedral

(B) SiCl− Tetrahedral

(C) AsF− Trigonal bipyramidal

(D) BCl3− Trigonal planar

QUESTION: 10

What is common between the following molecules

SO3, CO2-3, No-3

Solution:


All the moleculeshave trigonal planar structure.

QUESTION: 11

Which molecule is depicted by the given ball and stick models?

Solution:

BF3 - Trigonal planar with bond angle 120º.
PCI5 - Trigonal bipyramidal with bond angles 120º and 90º.

QUESTION: 12

Which of the following does not show octahedral geometry?

Solution:

SF4 has trigonal bipyramidal geometry. SF6, IF5, and SiF62- have octahedral geometry.

QUESTION: 13

Given below is the table showing shapes of some molecules having lone pairs of electrons. Fill up the blanks left in it.

Solution:
QUESTION: 14

The BCI3 is a planar molecule whereas NCI3 is pyramidal, because

Solution:

No lone pair ofelectrons is available in BCI3

One lone pair of electrons is available on N atom, occupies a corner in the tetrahedral arrangement. Therefore, NCI3 appears pyramidal in shape.

QUESTION: 15

CF4, SF4 and XeF4 contain the following electronicstructure on their central atoms. Which one iscorrect option?

Solution:

CF4−sp3 , tetrahedral but no unpaired electron.

SF4−sp3d, trigonal bipyramidal with one unpaired electron.


XeF4−sp3d2, square planar, two lone pairs of electrons.

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