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Chapter 7: Q18E (page 392)

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity: (a)\({\rm{As, H, N, P, Sb}}\)(b)\({\rm{Cl, H, P, S, Si}}\)(c)\({\rm{Br, Cl, Ge, H, Sr}}\)(d)\({\rm{Ca, H, K, N, Si}}\)(e)\({\rm{Cl, Cs, Ge, H, Sr}}\).

Short Answer

Expert verified

The atoms are arranged in their increasing electronegativity order as:

  1. \({\rm{H < Sb < As < P < N}}\)
  2. \({\rm{H < Si < P < S < Cl}}\)
  3. \({\rm{Sr < H < Ge < Br < Cl}}\)
  4. \({\rm{K < Ca < H < Si < N}}\)
  5. \({\rm{Cs < Sr < H < Ge < Cl}}\)

Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Explanation

As, the addition of a proton has a greater effect than the addition of an electron, the size of the atom decreases as you travel from left to right in the periodic table. Because of the strong force of the nucleus, it will be able to receive electrons more easily as its size decreases.

According to the foregoing argument, electronegativity rises as one moves from left to right in the periodic table.

As you progress from top to bottom in a group, the size of the group grows due to the addition of fresh energy shells. Because the force of attraction of the nucleus is no longer able to attract additional electrons as the size of the nucleus rises, electronegativity will drop as the group size decreases.

03

Arranging the atom in increasing order of electronegativity

a. The atoms in order of increasing electronegativity is:

\({\rm{H < Sb < As < P < N}}\)

Therefore, the order is: \({\rm{H < Sb < As < P < N}}\).

04

Arranging the atom in increasing order of electronegativity

b. The atoms in order of increasing electronegativity is:

\({\rm{H < Si < P < S < Cl}}\)

Therefore, the order is: \({\rm{H < Si < P < S < Cl}}\).

05

Arranging the atom in increasing order of electronegativity

c. The atoms in order of increasing electronegativity is:

\({\rm{Sr < H < Ge < Br < Cl}}\)

Therefore, the order is: \({\rm{Sr < H < Ge < Br < Cl}}\).

06

Arranging the atom in increasing order of electronegativity

d. The atoms in order of increasing electronegativity is:

\({\rm{K < Ca < H < Si < N}}\)

Therefore, the order is: \({\rm{K < Ca < H < Si < N}}\).

07

Arranging the atom in increasing order of electronegativity

e. The atoms in order of increasing electronegativity is:

\({\rm{Cs < Sr < H < Ge < Cl}}\)

Therefore, the order is: \({\rm{Cs < Sr < H < Ge < Cl}}\).

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Most popular questions from this chapter

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.

Identify the electron pair geometry and the molecular structure of each of the following molecules:

  1. \({\rm{CNIO}}\) (N is the central atom)
  2. \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\)(C is the central atom)
  4. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SO}}\)(S is the central atom)
  5. \({\rm{S}}{{\rm{O}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)(S is the central atom)
  6. \({\rm{Xe}}{{\rm{O}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)(Xe is the central atom)
  7. \({\rm{ClOF}}_{\rm{2}}^{\rm{ + }}\)(Cl is the central atom)

Draw the Lewis electron dot structures for these molecules, including resonance structures where appropriate:

(a) \({\rm{CS}}_{\rm{3}}^{{\rm{2 - }}}\)

(b) \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)

(c) \({\rm{CS}}\)

(d) predict the molecular shapes for \({\rm{C}}{{\rm{S}}_{\rm{3}}}^{{\rm{2 - }}}\) and \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)and explain how you arrived at your predictions

Which is the most polar bond? (a) \({\rm{C - C}}\) (b) \({\rm{C - H}}\) (c) \({\rm{N - H}}\) (d) \({\rm{O - H}}\) (e) \({\rm{Se - H}}\) .

How are single, double, and triple bonds similar? How do they differ?
See all solutions

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