First Year Chemistry Chapter 6 Online Short Questions for 1st Year Chemistry Chapter 6 Chemical Bonding Preparation

Why positively charged ions are mostly smaller in sizes than their neutral atoms?

• Ans 1: By the removal of electrons the cloud of outermost orbitals becomes thin. In this way, the remaining electrons are accommodated in smaller space. The nuclei have better attractive forces for them, and so the size are decreased as compared to the neutral atoms.

Why the electron affinities of II-A are less then those of I-A?

• Ans 1: The elements of II-A have fulfilled outermost s-orbitals, so electron has to be accommodated in the higher orbitals. Their electron affinities are positive. The elements of I-A can accommodate incoming electron in partially filled s-orbital.

Most of He elements of the periodic table attain the electronic configuration of inert gases during bond formation. Justify it.

• Ans 1: Inert gases are not reactive due to complete octet except He. Most of He s-and p-block elements may attain eight electrons in the outermost orbitals. They do so either by losing, gaining or sharing the electrons.

The melting points, boiling points, heat of vaporization and heat of sublimation of electrovalent compounds are higher as compared to those of covalent compounds. Why?

• Ans 1: Electrovalent or ionic compounds have high melting and boiling points due to the close packing of oppositely charged ions. The positively charged ions are surrounded by negatively charged ions and vice versa. That is why, they have very high melting points, boiling points, heat of vaporizations and heats of sublimation.

• Ans 1:

Why the bond angles of H₂O and NH₃ are not 109.5° like that of CH₄, although O and N-atoms are sp³ —hybridized?

• Ans 1:

  Like CH₄, the molecules of H₂O and NH₃ are also AB₄ type molecules. Carbon, oxygen and nitrogen atoms undergo sp³ -hybridization. CH₄ is perfectly tetrahedral with the angle of 109.5°. In case of ammonia, there are three bond pairs and one lone pair. Lone pair-bond pair repulsion is greater than bond pair-bond pair repulsion. Due to this reason, angle reduces to 107.5° In case of H₂O, there are two lone pairs on oxygen. Due to this increased repulsion of two lone pairs, the angle further reduces to 104.5°

How does the electronegativity difference decide the nature of ionic bond?

• Ans 1: When the electronegativity difference between two bonded atoms is 1.7 or more than that, then the bond is said to be ionic, otherwise covalent. The % age of ionic character is more than 51% when the electronegativity difference is 1.7.

Why the atomic radii increase down the group?

• Ans 1: The number of shells increase along with the increasing shielding effect down the group. These two factors are dominant in increasing the sizes. no doubt, the nuclear charges are increased, but this is not a dominant factor.

How do you justify that all the bonds between I-A and II-A with VI-A and VII-A are not equally ionic?

• Ans 1: The I.E. values of the I-A are less than II-A and the E.A. of VII-A are greater than VI-A. So, the bond between I­A and VII-A should be ionic to a good extent. The bonds between II-A and VI-A should be poorly ionic. It means that all the above mentioned compounds are not equally ionic.

How shielding effect is thought to be one of the parameters for the variation of ionization potential in group and periods?

• Ans 1:

  Greater the number of the inner electons, greater the shielding effect and lesser the I.E. values. In a period, the shielding effect remains the same from left to the right. So the I.E. value are not affected by this parameter. No doubt, other parameters affect it.

Why the ionization energies decrease down the group although the nuclear charges increase?

• Ans 1: When we go down the group, the number of shells increase and shielding effects also increase. These two factors decrease the force of attraction between the nucleus and the outermost electrons and is a cause of decreasing ionization energy.

Dipole moment of CO₂ is zero but that of CO is 0.12 Debye. Why?

• Ans 1: CO₂ is linear molecule and the two dipoles cancel the effect of each other. In CO there is a single dipole directed from carbon to oxygen and it not cancelled.

How the %age of ionic character of the polar bond can be determined?

• Ans 1:

Most of He elements of the periodic table attain the electronic configuration of inert gases during bond formation. Justify it.

• Ans 1: Inert gases are not reactive due to complete octet except He. Most of He s-and p-block elements may attain eight electrons in the outermost orbitals. They do so either by losing, gaining or sharing the electrons.

• Ans 1:

Why the lone pairs of electrons on an atom occupy greater space?

• Ans 1: The lone of electrons of the central atom is only attracted by the nucleus of the central atom. It creates more forces of repulsion due to nearness of nucleus and occupies greater space as compared to the bond pair.

How do you justify that all the bonds between I-A and II-A with VI-A and VII-A are not equally ionic?

• Ans 1: The I.E. values of the I-A are less than II-A and the E.A. of VII-A are greater than VI-A. So, the bond between I­A and VII-A should be ionic to a good extent. The bonds between II-A and VI-A should be poorly ionic. It means that all the above mentioned compounds are not equally ionic.

Why the atomic radii increase down the group?

• Ans 1: The number of shells increase along with the increasing shielding effect down the group. These two factors are dominant in increasing the sizes. no doubt, the nuclear charges are increased, but this is not a dominant factor.

How does the electronegativity difference decide the nature of ionic bond?

• Ans 1: When the electronegativity difference between two bonded atoms is 1.7 or more than that, then the bond is said to be ionic, otherwise covalent. The % age of ionic character is more than 51% when the electronegativity difference is 1.7.

The melting points, boiling points, heat of vaporization and heat of sublimation of electrovalent compounds are higher as compared to those of covalent compounds. Why?

• Ans 1: Electrovalent or ionic compounds have high melting and boiling points due to the close packing of oppositely charged ions. The positively charged ions are surrounded by negatively charged ions and vice versa. That is why, they have very high melting points, boiling points, heat of vaporizations and heats of sublimation.