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Test: Bond Parameters


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20 Questions MCQ Test Chemistry Class 11 | Test: Bond Parameters

Test: Bond Parameters for NEET 2022 is part of Chemistry Class 11 preparation. The Test: Bond Parameters questions and answers have been prepared according to the NEET exam syllabus.The Test: Bond Parameters MCQs are made for NEET 2022 Exam. Find important definitions, questions, notes, meanings, examples, exercises, MCQs and online tests for Test: Bond Parameters below.
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Test: Bond Parameters - Question 1

Two atoms are said to be bonded when:

Detailed Solution for Test: Bond Parameters - Question 1

Attractive forces tend to bring two atoms close to each other whereas repulsive forces tend to move them away. In hydrogen, the magnitude of the new attractive forces is greater than that of new repulsive forces. As a result, two atoms come close to each other and potential energy decreases. The atoms approach each other until the equilibrium stage is reached where the net force of attraction balances the force of repulsion and system acquires minimum energy. 

Test: Bond Parameters - Question 2

The decreasing order of the repulsive interactions between various electron pairs is:

Detailed Solution for Test: Bond Parameters - Question 2

The bond pair of electrons is shared by two atoms whereas the lone pair of electrons is only under the influence of central atom.

So the electron cloud of lone pair occupies more space as compared to the bond pair.

This causes greater repulsion between the lone pairs as compared to lone pair-bond pair and bond pair-bond pair interactions.

Test: Bond Parameters - Question 3

Valence bond theory was introduced by:

Detailed Solution for Test: Bond Parameters - Question 3

Valence bond theory was introduced by Heitler and London (1927) and further work was done by Pauling and others.

In the valence bond (VB) theory, proposed in large part by the American scientists Linus Pauling and John C. Slater, bonding is accounted for in terms of hybridized orbitals of the metal ion, which is assumed to possess a particular number of vacant orbitals available for coordinate bonding that equals its coordination number. 

Test: Bond Parameters - Question 4

Which molecule has a bent shape?

Detailed Solution for Test: Bond Parameters - Question 4

CO2 and BeH2 possess linear geometry as well as linear shape , while H2O possess traversal geometry and bent shape.NF3 possess traversal geometry and trigonal pyramidal shape . Thus correct option is (c)

Test: Bond Parameters - Question 5

The s-orbital does not show preference to any direction because

Detailed Solution for Test: Bond Parameters - Question 5

The s-orbital is spherically symmetric in shape so it does not show preference to any direction. It is the same from all the directions.

Test: Bond Parameters - Question 6

The number of lone pairs of electrons on SF4, CF4 and XeF4 are:

Detailed Solution for Test: Bond Parameters - Question 6

SF4 molecule has 1 lone pair of electrons, CF4 has no lone pair of electrons and XeF4 has 2 lone pair of electrons respectively.

Test: Bond Parameters - Question 7

 Pick out the pair of species having identical shapes for both the molecules.

Detailed Solution for Test: Bond Parameters - Question 7

Both XeF& CO2 have linear structures. Both are actually linear Tri-atomic molecules. 

Test: Bond Parameters - Question 8

 Among the following species octahedral shape is found in:

Detailed Solution for Test: Bond Parameters - Question 8

SF6 has an octahedral geometry.

Test: Bond Parameters - Question 9

 Which molecule has a trigonal pyramidal shape?

Detailed Solution for Test: Bond Parameters - Question 9

AB3E: trigonal pyramidal (central atom + 3 outer atoms make a pyramid)
→ start with AB4 molecule (tetrahedral) and replace a B atom w/ lone pair
→ lone pair electrons push bonding electrons away
→ bond angles are now less than 109.5°

Test: Bond Parameters - Question 10

Which of the following orbitals give a zero overlap?

Detailed Solution for Test: Bond Parameters - Question 10

Test: Bond Parameters - Question 11

 Among the following molecules, the molecule with trigonal planar geometry is:

Detailed Solution for Test: Bond Parameters - Question 11

(a) BF₃ ⇒ 3bp + 0/p ⇒ sp³ -hybridisation and triagonal planar geometry.
(b) IF₃ ⇒ 3bp + 2/p ⇒ sp³d -hybridisation and T shape.
(c) NH₃ ⇒ 3bp + 1/p ⇒ sp³ -hybridisation and pyraminal geometry.
(d) PH₃ ⇒ 3bp + 1/p ⇒ sp³ -hybridisation and pyraminal geometry.

Test: Bond Parameters - Question 12

A pi-bond is formed by the overlap of:

Detailed Solution for Test: Bond Parameters - Question 12

pi-bond is always formed by sidewise overlapping of p – p orbitals in sidewise manner.

Test: Bond Parameters - Question 13

Which of the following has a square pyramidal shape?

Detailed Solution for Test: Bond Parameters - Question 13

Br-atom has configuration

To get pentavalency, two of the p-orbitals are unpaired and electrons are shifted to 4d-orbitals. 

In this excited state, sp3d2-hybridisation occurs giving octahedral structure. Five positions are occupied by F atoms forming sigma bonds with hybrid bonds and one position occupied by lone pair, i.e., the molecule as a square pyramidal shape. 

 

Test: Bond Parameters - Question 14

 According to the VSEPR theory, the geometry and shape of the molecule depends upon:

Detailed Solution for Test: Bond Parameters - Question 14

For geometry and shape of a molecule, both bond pair and lone pair of electron in valence shell of central atom.

Test: Bond Parameters - Question 15

The statement that is true about H2O molecule is:

Detailed Solution for Test: Bond Parameters - Question 15

Central atom: O

At. no. = 8,

No. of valence electrons in oxygen is 6

Lewis dot structure of O atom

No. of electrons required for completing the octet = 8 - 6 =2

Atoms attached to the central atom: two H atoms

At. no. of H = 1

H atoms need one electron each for getting fully-filled K shells.

Representation of Lewis dot structures of H2O, which satisfies these conditions:

 

No. of valence shell electron pairs on the central atom O, after forming two covalent bonds with two H atoms = 4.

Geometry of 4 pairs, as predicted by VSEPR theory = Tetrahedral.

No. of lone pairs = Two.

Type, according to VSEPR theory:

So, geometry of pairs and geometry of atoms are different.

The geometry of atoms is derived from the geometry of pairs. At two of the four corners of the tetrahedron, there are no atoms.

Diagrams showing the geometry of 2 H atoms and two lone pairs:

 

Geometry of atoms in H2O is V-shaped. i.e. H2O molecule has a bent geometry

Test: Bond Parameters - Question 16

Valence Bond Theory was developed in the year

Detailed Solution for Test: Bond Parameters - Question 16

The valence bond (VB) theory of bonding was mainly developed by Walter Heitler and Fritz London in 1927, and later modified by Linus Pauling to take bond direction into account. The VB approach concentrates on forming bonds in localized orbitals between pairs of atoms, and hence retains the simple idea of Lewis structures and electron pairs. 

Test: Bond Parameters - Question 17

Among the following species linear shape is found in:

Detailed Solution for Test: Bond Parameters - Question 17

 

Test: Bond Parameters - Question 18

Which of the following molecule doesn’t have a lone pair?

Detailed Solution for Test: Bond Parameters - Question 18

BeCl2 has no lone pairs on the beryllium. Thus, the electrons on the chlorides willtry to stay far apart from each other, since their corresponding electrons repel each other (while experiencing no deflection from electrons on a central atom). Thus themolecule is linear in shape.

Test: Bond Parameters - Question 19

Among the following species the pair that have V-shaped geometry is:

Detailed Solution for Test: Bond Parameters - Question 19

Both are bent shape molecule.

Test: Bond Parameters - Question 20

Among the following compounds the maximum number of lone pair is present on the central atom of:

Detailed Solution for Test: Bond Parameters - Question 20

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