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Chapter 7: Q26 E (page 394)

In the Lewis structures listed here, M and X represent various elements in the third period of the periodic table. Write the formula of each compound using the chemical symbols of each element:

Short Answer

Expert verified

The Lewis structure having the formula as:

  1. \({\rm{MgS}}\)
  2. \({\rm{AlC}}{{\rm{l}}_{\rm{3}}}\)
  3. \({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}\)
  4. \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{S}}_{\rm{3}}}\)

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

Due to third-period elements may create single positive charge cations\({\rm{Na(N}}{{\rm{a}}^{\rm{ + }}}{\rm{)}}\).

The double positive charge cations can be formed by\({\rm{Mg(M}}{{\rm{g}}^{{\rm{2 + }}}}{\rm{)}}\).

Thetriple positive charge cations can be formed by\({\rm{Al(A}}{{\rm{l}}^{{\rm{3 + }}}}{\rm{)}}\).

\({\rm{Cl(C}}{{\rm{l}}^{\rm{ - }}}{\rm{)}}\)can also produce a single negative charge anion.

The double negative charge anion is \({\rm{S(}}{{\rm{S}}^{{\rm{2 - }}}}{\rm{)}}\).

03

Writing the formula

(a)

The chemical formula is:

\({\rm{MgS}}\)

Therefore, the formula is: \({\rm{MgS}}\).

04

Writing the formula

(b)

The chemical formula is:

\({\rm{AlC}}{{\rm{l}}_{\rm{3}}}\)

Therefore, the formula is: \({\rm{AlC}}{{\rm{l}}_{\rm{3}}}\).

05

Writing the formula

(c)

The chemical formula is:

\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}\)

Therefore, the formula is: \({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}\).

06

Writing the formula

(d)

The chemical formula is:

\({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{S}}_{\rm{3}}}\)

Therefore, the formula is: \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{S}}_{\rm{3}}}\).

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Most popular questions from this chapter

Write resonance forms describing the distribution of electrons in each molecule or ion.

a) selenium dioxide, \({\rm{OSeO}}\)

(b) nitrate ion, \({\rm{NO}}_{\rm{3}}^{\rm{ - }}\)

(c) nitric acid, \({\rm{HN}}{{\rm{O}}_{\rm{3}}}\) (\({\rm{N}}\) is bonded to an \({\rm{OH}}\) group and two \({\rm{O}}\) atoms)

(d) benzene, \({{\rm{C}}_{\rm{6}}}{{\rm{H}}_{\rm{6}}}\):

(e) the formate ion:

Describe the molecular structure around the indicated atom or atoms:

  1. The sulfur atom in sulfuric acid, H2SO4 [ (HO)2 SO2]

  2. The chlorine atom in chloric acid, HClO3 [HOClO2]

  3. The oxygen atom in Hydrogen peroxide, HOOH

  4. The nitrogen atom in nitric acid, HNO3 [HONO2]

  5. The oxygen atom in OH group in nitric acid, HNO3 [HONO2]

  6. The central oxygen atom in the ozone molecule, O3

  7. Each of the carbon atoms in the propyne, CH3 CCH

  8. The carbon atom in Freon, CCl2 F2

  9. each of the carbon atoms in allene H2CCCH2

Which atoms can bond to sulfur so as to produce a positive partial charge on the sulfur atom?

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.

Question: Using the bond energies in Table \({\rm{7}}{\rm{.2}}\), determine the approximate enthalpy change for each of the following reactions:

(a) \({{\rm{H}}_{\rm{2}}}{\rm{(g) + B}}{{\rm{r}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2HBr(g)}}\)

(b) \({\rm{C}}{{\rm{H}}_{\rm{4}}}{\rm{(g) + }}{{\rm{I}}_{\rm{2}}}{\rm{(g)}} \to {\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{I(g) + HI(g)}}\)

(c) \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_4}{\rm{(g) + 3}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2C}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + 2}}{{\rm{H}}_{\rm{2}}}{\rm{O(g)}}\)
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