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Chapter 7: Q22 E (page 392)

Which of the following molecules or ions contain polar bonds? (a) \({{\rm{S}}_{\rm{8}}}\) (b) \({{\rm{S}}_{\rm{8}}}\) (c) \({{\rm{O}}_{\rm{2}}}^{{\rm{2 - }}}\) (d) \({\rm{N}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) (e) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\) (f) \({{\rm{H}}_{\rm{2}}}{\rm{S}}\) (g) \({\rm{B}}{{\rm{H}}_{\rm{4}}}^{\rm{ - }}\) .

Short Answer

Expert verified

The values which have non-polar bonds are:\({{\rm{O}}_{\rm{3}}}{\rm{ , }}{{\rm{S}}_{\rm{8}}}\)and\({{\rm{O}}_{\rm{2}}}^{{\rm{2 - }}}\).

The values which have polar bonds are: \({\rm{N}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}{\rm{ , C}}{{\rm{O}}_{\rm{2}}}{\rm{ , }}{{\rm{H}}_{\rm{2}}}{\rm{S}}\) and \({\rm{B}}{{\rm{H}}_{\rm{4}}}^{\rm{ - }}\) .

Step by step solution

01

Define Chemical Bonding

A chemical bond is an attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Finding which molecules or ions contain polar bonds?

The concept applied in this topic is that compounds having a single kind of element will have non-polar bonds since the electronegativity difference will be zero.

As a result of the foregoing reasoning,\({{\rm{O}}_{\rm{3}}}{\rm{ , }}{{\rm{S}}_{\rm{8}}}\), and\({{\rm{O}}_{\rm{2}}}^{{\rm{2 - }}}\)have nonpolar bonds, whereas\({\rm{N}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}{\rm{ , C}}{{\rm{O}}_{\rm{2}}}{\rm{ , }}{{\rm{H}}_{\rm{2}}}{\rm{S}}\), and\({\rm{B}}{{\rm{H}}_{\rm{4}}}^{\rm{ - }}\)have polar bonds.

Therefore, the values having non-polar bonds are:\({{\rm{O}}_{\rm{3}}}{\rm{ , }}{{\rm{S}}_{\rm{8}}}\)and\({{\rm{O}}_{\rm{2}}}^{{\rm{2 - }}}\).

The values having polar bonds are: \({\rm{N}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}{\rm{ , C}}{{\rm{O}}_{\rm{2}}}{\rm{ , }}{{\rm{H}}_{\rm{2}}}{\rm{S}}\) and \({\rm{B}}{{\rm{H}}_{\rm{4}}}^{\rm{ - }}\) .

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Most popular questions from this chapter

Predict the electron pair geometry and the molecular structure of each of the following ions:

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\,\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}{\rm{ - }}\)
  3. \({\rm{SnC}}{{\rm{l}}_{\rm{3}}}^{\rm{ - }}\)
  4. \({\rm{BrC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)

Write Lewis structures for the following: (a)\({\rm{Se}}{{\rm{F}}_{\rm{6}}}\)(b)\({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)(c)\({\rm{SeC}}{{\rm{l}}_{\rm{3}}}^{\rm{ + }}\)(d)\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\)(contains a\({\rm{B - B}}\)bond).

Does a cation gain protons to form a positive charge or does it lose electrons?

The lattice energy of \({\rm{LiF}}\) is \({\rm{1023 kJ/mol}}\), and the \({\rm{Li - F}}\) distance is \({\rm{201 pm}}\). \({\rm{MgO}}\) crystallizes in the same structure as \({\rm{LiF}}\) but with a \({\rm{Mg - O}}\) distance of \({\rm{205 pm}}\). Which of the following values most closely approximates the lattice energy of \({\rm{MgO}}\): \({\rm{256 kJ/mol, 512 kJ/mol, 1023 kJ/mol, 2046 kJ/mol,}}\) or \({\rm{4008 kJ/mol}}\)? Explain your choice.

Write Lewis structures for the following: (a)\({{\rm{O}}_{\rm{2}}}\)(b)\({{\rm{H}}_{\rm{2}}}{\rm{CO}}\)(c)\({\rm{As}}{{\rm{F}}_{\rm{3}}}\)(d)\({\rm{ClNO}}\)(e)\({\rm{SiC}}{{\rm{l}}_{\rm{4}}}\)(f)\({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\)(g)\({\rm{N}}{{\rm{H}}_{\rm{4}}}^{\rm{ + }}\)(h)\({\rm{B}}{{\rm{F}}_{\rm{4}}}^{\rm{ - }}\)(i)\({\rm{HCCH}}\)(j)\({\rm{CICN}}\)(k)\({{\rm{C}}_{\rm{2}}}^{{\rm{2 + }}}\).
See all solutions

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