Using the periodic table only, arrange the members of each of the following sets

Question

Using the periodic table only, arrange the members of each of the following sets in order of increasing bond strength.

(b) H-Cl, H-Br, H-F

Using the periodic table only, arrange the members of each of the following sets in order of increasing bond lengths.

(a) H-F, H-I, H-Cl

(b) C-S, C=O, C-O

(c) N-H, N-S, N-O

Using the periodic table only, arrange the elements in each set in order of increasing electronegativity.

(a) Mg, P, As

(b) S, O, Si

In each pair, determine which compound has bonds with greater ionic character.

a. HI or HCl

b. NH3 or PH3

c.CS2 or CO2

Please answer all Please and thank you!

Explanation / Answer

(a)

Carbon-nitrogen single bond is formed by overlap of sp3 orbital of C with sp3 orbital of N. It is a sigma bond. Carbon-nitrogen double bond has one sigma bond and one additional pi bond making it stronger than carbon-nitrogen single bond. Carbon –nitrogen triple bond has one sigma bond and additional two pi bonds. Hence, carbon-nitrogen triplebond is strongest. Therefore, bonds can be arranged in increasing order of bond strength as follows:

(b)

Bond strength of H-Cl, H-Br and H-F changes with size of halogen atom. As the size of halogen atom increases, bond strength decreases. The atomic size of Br is greater than Cl, which is greater than F. Therefore, H-F bond is stronger than H-Cl, which in turn is stornger than H-Br. The increasing order of bond strength is given below:

H-Br < H-Cl < H-F

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(a)

Bond length in H-F, H-I and H-Cl increases with increase in size of halogen atom. The atomic size of I is larger than that of Cl, which in turn is larger than that of F. Therefore, bond length of H-F is smallest and that of H-I is largerst. The increasing order of bond length is given below:

H-F < H-Cl < H-I

(b)

Bond length in C-S, C=O and C-O increases with increase in size of atoms and decrease in number of bonds. Atomic size of O is smaller than S. Thus, bond length of C-O is less than C-S and bond length of C=O is less than C-O. The increasing order of bond length is given below:

C=O < C-Ol < C-S

(c)

Bond length in N-H, N-S and N-O increases with increase in size of halogen atom. The atomic size of S is larger than that of O, which in turn is larger than that of H. Therefore, bond length of N-H is smallest and that of N-S is largerst. The increasing order of bond length is given below:

N-H < N-O < N-S

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(a)

As we move across the period from left to right, electronegativity increases and as we move down the group electronegativity decreases. Therefore, electronegativity of P is more than that of Mg and electronegativity of As is less than that of P but more than that of P. The increasing order of electronegativity is given below:

Mg < As < P

(b)

As we move across the period from left to right, electronegativity increases and as we move down the group electronegativity decreases. Therefore, electronegativity of S is more than that of Si and electronegativity of S is less than that of O. The increasing order of electronegativity is given below:

Si < S < O

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(a)

Greater the differenec in electronegativity, greater is the ionic character. Difference in electronegativity is more in H and Cl than H and I. Therefore, HCl has greater ionic character than HI.

(b)

Greater the differenec in electronegativity, greater is the ionic character. Difference in electronegativity is more in H and N than H and P. Therefore, NH3 has greater ionic character than PH3.

(c)

Greater the differenec in electronegativity, greater is the ionic character. Difference in electronegativity is more in C and O than C and S. Therefore, CO2 has greater ionic character than CS2

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