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Chapter 7: Question 42 E (page 397)

Two arrangements of atoms are possible for a compound with a molar mass of about\({\rm{45 g/mol}}\)that contains\({\rm{52}}{\rm{.2 \% C, 13}}{\rm{.1 \% H}}\), and\({\rm{34}}{\rm{.7 \% O}}\)by mass. Write the Lewis structures for the two molecules.

Short Answer

Expert verified

The formula is:\({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{6}}}{\rm{O}}\).

The Lewis structure is:

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

Writing the Lewis symbol

In a \({\rm{100}}{\rm{.0 g}}\) sample, there are \({\rm{52}}{\rm{.2 g C}}\), \({\rm{34}}{\rm{.7 g O}}\) and\({\rm{13}}{\rm{.1 g H}}\).

Now we must compute the mole of\({\rm{C}}\) and\({\rm{H}}\), which we shall accomplish by dividing their mass by their molecular weight, as follows:-

The moles of carbon are:

\(\frac{{{\rm{52}}{\rm{.2 g}}}}{{{\rm{12}}{\rm{.001 g mo}}{{\rm{l}}^{{\rm{ - 1}}}}}}{\rm{ = 4}}{\rm{.346 mol C}}\)

The moles of hydrogen are:

\(\frac{{{\rm{13}}{\rm{.1 g}}}}{{{\rm{1}}{\rm{.0079 g mo}}{{\rm{l}}^{{\rm{ - 1}}}}}}{\rm{ = 12}}{\rm{.997 mol H}}\)

The moles of oxygen are:

\(\frac{{{\rm{34}}{\rm{.7 g}}}}{{{\rm{15}}{\rm{.9994 g mo}}{{\rm{l}}^{{\rm{ - 1}}}}}}{\rm{ = 2}}{\rm{.1668 mol O}}\)

To compute the formula, divide the mole by the smallest mole:-

\(\frac{{{\rm{4}}{\rm{.346 mol}}}}{{{\rm{2}}{\rm{.1688 mol}}}}{\rm{ = 2 C}}\)

\(\frac{{{\rm{12}}{\rm{.997 mol}}}}{{{\rm{2}}{\rm{.1688 mol}}}}{\rm{ = 6 H}}\)

\(\frac{{{\rm{2}}{\rm{.1688 mol}}}}{{{\rm{2}}{\rm{.1688 mol}}}}{\rm{ = 1 O}}\)

The formula is \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{6}}}{\rm{O}}\).

The Lewis structure is as follows:-

Therefore, the formula is\({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{6}}}{\rm{O}}\) and the Lewis structure are:

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Most popular questions from this chapter

Question: Use principles of atomic structure to answer each of the following:

(a) The radius of the \({\rm{Ca}}\) atom is \({\rm{197 pm}}\); the radius of the \({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}\) ion is \({\rm{99 pm}}\). Account for the difference.

(b) The lattice energy of \({\rm{CaO(s)}}\) is \({\rm{ - 3460 kJ/mol}}\); the lattice energy of \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) is \({\rm{ - 2240 kJ/mol}}\). Account for the difference.

(c) Given these ionization values, explain the difference between \({\rm{Ca}}\) and \({\rm{K}}\) with regard to their first and second ionization energies.

(d) The first ionization energy of \({\rm{Mg}}\) is \({\rm{738 kJ/mol}}\) and that of \({\rm{Al}}\) is \({\rm{578 kJ/mol}}\). Account for this difference.

Identify the more polar bond in each of the following pairs of bonds: (a) \({\rm{HF or HCl}}\) (b) \({\rm{NO or CO}}\) (c) \({\rm{SH or OH}}\) (d) \({\rm{PCl or HCl}}\) (e) \({\rm{CH or NH}}\) (f) \({\rm{SO or PO}}\) (g) \({\rm{CN or NN}}\) .

Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.

(a) \(C{O_2}\)

(b) \(CO\)

For which of the following substances is the least energy required to convert one mole of the solid into separate ions?

(a) \({\rm{MgO}}\)

(b) \({\rm{SrO}}\)

(c) \({\rm{KF}}\)

(d) \({\rm{CsF}}\)

(e) \({\rm{Mg}}{{\rm{F}}_{\rm{2}}}\)

Write Lewis structures for the following: (a) \({\rm{CI}}{{\rm{F}}_{\rm{3}}}\) (b) \({\rm{PC}}{{\rm{I}}_{\rm{5}}}\) (c) \({\rm{B}}{{\rm{F}}_{\rm{3}}}\) (d) \({\rm{P}}{{\rm{F}}_{\rm{6}}}^{\rm{ - }}\) .
See all solutions

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