Representative Metals, Metalloids, and Nonmetals

The equivalence point for the titration of a \(25.00 - mL\)sample of \(CSOH\) solution with \(0.1062MHN{O_3}\) is at\(35.27mL\). What is the concentration of the \(CsOH\)solution?

Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.

(a) \(P{H_3}\).

(b) \(P{H_4} + \).

(c) \({P_2}{H_4}\).

(d) \(P{O_4}^3 - \)

(e) \(P{F_5}\)

Describe the molecular structure of each of the following molecules or ions listed. You may wish to review the chapter on chemical bonding and molecular geometry.

(a) \({\rm{P}}{{\rm{H}}_3}\) 

(b) \({\rm{P}}{{\rm{H}}_4} + \)

(c) \({{\rm{P}}_2}{{\rm{H}}_4}\) 

(d) \({\rm{P}}{{\rm{O}}_4}^{3 - }\)

Question: Complete and balance each of the following chemical equations. (In some cases, there may be more than one correct answer.)

(a) \({{\rm{P}}_4} + {\rm{Al}}\) 

(b) \({{\rm{P}}_4} + {\rm{Na}}\)

(c) \({{\rm{P}}_4} + {{\rm{F}}_2}\) 

(d) \({{\rm{P}}_4} + {\rm{C}}{{\rm{l}}_2}\)

(e) \({{\rm{P}}_4} + {{\rm{O}}_2}\)

(f) \({{\rm{P}}_4}{{\rm{O}}_6} + {{\rm{O}}_2}\)

Describe the hybridization of phosphorus in each of the following compounds: \({{\rm{P}}_4}{{\rm{O}}_{10}},{{\rm{P}}_4}{{\rm{O}}_6},{\rm{P}}{{\rm{H}}_4}{\rm{I}}\) (an ionic compound), \({\rm{PB}}{{\rm{r}}_3},{{\rm{H}}_3}{\rm{P}}{{\rm{O}}_4},{{\rm{H}}_3}{\rm{P}}{{\rm{O}}_3},{\rm{P}}{{\rm{H}}_3}\) and\({{\rm{P}}_2}{{\rm{H}}_4}\). You may wish to review the chapter on advanced theories of covalent bonding. 

What volume of \(0.200MNaOH\)is necessary to neutralize the solution produced by dissolving \(2.00\;{g^{g }}PC{l_3}\) is an excess of water? Note that when \({H_3}P{O_3}\)is titrated under these conditions, only one proton of the acid molecule reacts.

How much \(POC{l_3}\) can form from \(25.0\;g\) of \(PC{l_5}\) and the appropriate amount of \({H_2}O\) ?

Write equations showing the stepwise ionization of phosphorous acid.

Draw the Lewis structures and describe the geometry for the following:

(a) \({\rm{P}}{{\rm{F}}_4} + \) 

(b) \({\rm{P}}{{\rm{F}}_5}\)

(c) \({\rm{P}}{{\rm{F}}_6}^ - \)

(d) \({\rm{PO}}{{\rm{F}}_3}\)

Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?

Assign an oxidation state to phosphorus in each of the following:

(a) \({\rm{Na}}{{\rm{H}}_2}{\rm{P}}{{\rm{O}}_3}\)

(b) \({\rm{P}}{{\rm{F}}_5}\)

(c) \({{\rm{P}}_4}{{\rm{O}}_6}\)

(d) \({{\rm{K}}_3}{\rm{P}}{{\rm{O}}_4}\)

(e) \({\rm{N}}{{\rm{a}}_3}{\rm{P}}\)

(f) \({\rm{N}}{{\rm{a}}_4}{{\rm{P}}_2}{{\rm{O}}_7}\)

 Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of phosphorus (V) oxide, an acidic oxide, with water. Phosphorus (V) oxide is prepared by the combustion of phosphorus.

(a)  Write the empirical formula of phosphorus (V) oxide.

(b)  What is the molecular formula of phosphorus (V) oxide if the molar mass is about 280.

(c)  Write balanced equations for the production of phosphorus (V) oxide and phosphoric acid.

(d)  Determine the mass of phosphorus required to make \(1.00 \times {10^4}\;{\rm{kg}}\) of phosphoric acid, assuming a yield of 98.85%.

Predict the product of burning francium in air.

Using equations, describe the reaction of water with potassium and with potassium oxide.

Write balanced chemical equations for the following reactions:

a.  zinc metal heated in a stream of oxygen gas

b.  zinc carbonate heated until loss of mass stops

c.  zinc carbonate added to a solution of acetic acid, \({\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}{\rm{H}}\)

d.  zinc added to a solution of hydrobromic acid

Write balanced chemical equations for the following reactions:

(a) cadmium burned in air

(b) elemental cadmium added to a solution of hydrochloric acid

(c) cadmium hydroxide added to a solution of acetic acid, \({\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}{\rm{H}}\)

Illustrate the amphoteric nature of aluminum hydroxide by citing suitable equations.

Write balanced chemical equations for the following reactions:

(a)  metallic aluminum burned in air

(b)  elemental aluminum heated in an atmosphere of chlorine

(c)  aluminum heated in hydrogen bromide gas

(d)  aluminum hydroxide added to a solution of nitric acid

Write balanced chemical equations for the following reactions:

1. (a )sodium oxide added to water
2. (b) cesium carbonate added to an excess of an aqueous solution of HF
3. (c) Aluminum oxide added to an aqueous solution of \({\bf{HCl}}{{\bf{O}}_{\bf{4}}}\)
4. (d) A solution of sodium carbonate added to solution of barium nitrate
5. (e) Titanium metal produced from the reaction of titanium tetrachloride with elemental sodium

What volume of  \(0.250{\rm{M }}{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\) solution is required to neutralize a solution that contains \(5.00\;{\rm{g}}\) of \({\rm{CaC}}{{\rm{O}}_3}\)?

Which is the stronger acid, \({\rm{HCl}}{{\rm{O}}_4}\)or \({\rm{HBr}}{{\rm{O}}_4}\)? Why?

Oxygen forms double bonds in\({{\rm{O}}_2}\), but sulfur forms single bonds in \({{\rm{S}}_8}\). Why?

99. How many grams of Epsom salts \(\left( {{\rm{MgS}}{{\rm{O}}_4} \cdot 7{{\rm{H}}_2}{\rm{O}}} \right)\) will form from\(5.0\;{\rm{kg}}\)of magnesium?

Write a balanced chemical equation for the reaction of an excess of oxygen with each of the following.

Remember that oxygen is a strong oxidizing agent and tends to oxidize an element to its maximum oxidation state.

1. Mg.
2. Rb.
3. Ga.
4. \({{\rm{C}}_2}{{\rm{H}}_2}\)
5. CO

Which is the stronger acid, \({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\) or  \({{\rm{H}}_2}{\rm{Se}}{{\rm{O}}_4}\)? Why? You may wish to review the chapter on acid-base equilibrium.

Give the hybridization and oxidation state for sulfur in \({\rm{S}}{{\rm{O}}_2}\), in \({\rm{S}}{{\rm{O}}_3}\), and  in \({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\).

Which is the stronger acid, \({\rm{NaHS}}{{\rm{O}}_3}\)or \({\rm{NaHS}}{{\rm{O}}_4}\) ?

Determine the oxidation state of sulfur in \({\rm{S}}{{\rm{F}}_6},{\rm{S}}{{\rm{O}}_2}\;{{\rm{F}}_2}\), and KHS.

Which is a stronger acid, sulfurous acid or sulfuric acid? Why?

Give the Lewis structure of each of the following:

\(\begin{array}{l}(a){\rm{S}}{{\rm{F}}_4}.\\(b){{\rm{K}}_2}{\rm{S}}{{\rm{O}}_4}.\\(c){\rm{S}}{{\rm{O}}_2}{\rm{C}}{{\rm{l}}_2}.\\(d){{\rm{H}}_2}{\rm{S}}{{\rm{O}}_3}.\\(e){\rm{S}}{{\rm{O}}_3}.\end{array}\)

Write two balanced chemical equations in which sulfuric acid acts as an oxidizing agent.

What is the hybridization of iodine in \({\rm{I}}{{\rm{F}}_3}\) and  \({\rm{I}}{{\rm{F}}_5}\)?

Which halogen has the highest ionization energy? Is this what you would predict based on what you have learned about periodic properties?

Name each of the following compounds:

\(\begin{array}{l}(a){\rm{Br}}{{\rm{F}}_3}\\(b){\rm{NaBr}}{{\rm{O}}_3}\\(c){\rm{PB}}{{\rm{r}}_5}\\(d){\rm{NaCl}}{{\rm{O}}_4}\\(e){\rm{KClO}}\end{array}\)

Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.

What is the oxidation state of the halogen in each of the following?

\(\begin{array}{l}(a){{\rm{H}}_5}{\rm{I}}{{\rm{O}}_6}\\(b){\rm{IO}}_4^ - \\(c){\rm{Cl}}{{\rm{O}}_2}\\(d){\rm{IC}}{{\rm{l}}_3}\\(e){F_2}\end{array}\)

Give the hybridization of xenon in each of the following. You may wish to review the chapter on the advanced theories of covalent bonding.

\(\begin{array}{l}(a){\rm{Xe}}{{\rm{F}}_2}\\(b){\rm{Xe}}{{\rm{F}}_4}\\(c){\rm{Xe}}{{\rm{O}}_3}\\(d){\rm{Xe}}{{\rm{O}}_4}\\(e){\rm{XeO}}{{\rm{F}}_4}\end{array}\)

What is the molecular structure of each of the following molecules?

        (a) \(Xe{F_2}\)        (b) \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)      (c) \({\rm{Xe}}{{\rm{O}}_{\rm{3}}}\)        (d) \({\rm{Xe}}{{\rm{O}}_{\rm{4}}}\)        (e) \({\rm{XeO}}{{\rm{F}}_{\rm{4}}}\)

Indicate whether each of the following molecules is polar and non-polar.

         (a) \(Xe{F_2}\)               (b) \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)               (c) \({\rm{Xe}}{{\rm{O}}_{\rm{3}}}\)                (d)  \({\rm{XeO}}{{\rm{F}}_{\rm{4}}}\)    

What  is the oxidation state of the nobel gas in each of the following ? 

    (a)   \({\rm{Xe}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_2}\)           (b)  \({\rm{Kr}}{{\rm{F}}_{\rm{2}}}\)        (c) \({\rm{XeF}}_{\rm{3}}^{\rm{ + }}\)               (d) \(\)\({\rm{XeO}}_{\rm{6}}^{{\rm{4 - }}}\)

A mixture of Xenon and Flourine was heated. A sample of white solid that formed reacted with hydrogen to yield 81 mL of Xenon (at STP) and hydrogen fluoride , which was collected in water, giving a solution of hydrofluoric acid . The hydrofluoric acid solution was titrated , and 68.43 mL of 0.3172 M of Sodium Hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced chemical equations for the reactions involving xenon .

Basic solutions of  \({\rm{N}}{{\rm{a}}_{\rm{4}}}{\rm{Xe}}{{\rm{0}}_{\rm{6}}}\) are powerful oxidants . What mass of \({\rm{Mn(N}}{{\rm{0}}_{\rm{3}}}{{\rm{)}}_{\rm{2}}}{\rm{.6}}{{\rm{H}}_{\rm{2}}}{\rm{0}}\) reacts with 125.0 ml  of 0.1717 M basic solution of \({\rm{N}}{{\rm{a}}_{\rm{4}}}{\rm{Xe}}{{\rm{0}}_{\rm{6}}}\)  that contains an excess of Sodium Hydroxide if the products include Xe and the solution of Sodium Permanganate ?

The electrolysis of molten sodium chloride or of aqueous sodium chloride produces chlorine. Calculate the mass of chlorine produced from 3.00 kg sodium chloride in each case. You may wish to review the chapter on electrochemistry for relevant examples.