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Chapter 7: Problem 81

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Ozone decomposes to dioxygen. (b) Xenon reacts with fluorine. (Write three different equations.) (c) Sulfur reacts with hydrogen gas. (d) Fluorine reacts with water.

Short Answer

Expert verified
a) 2O3 → 3O2 b) 1) Xe + 3F2 → XeF6 2) Xe + 2F2 → XeF4 3) Xe + F2 → XeF2 c) S + H2 → H2S d) F2 + 2H2O → 4HF + O2

Step by step solution

01

Write unbalanced equation

Ozone (O3) decomposes to dioxygen (O2), which can be written as: O3 → O2
02

Balance the equation

In order to balance the equation, we need two molecules of ozone decomposing to three molecules of dioxygen, so the balanced equation is: 2O3 → 3O2 b) Xenon reacts with fluorine (Three different equations).
03

Write unbalanced equations

Xenon can react with fluorine to form three different xenon fluorides: Xenon hexafluoride (XeF6), xenon tetrafluoride (XeF4), and xenon difluoride (XeF2). The three unbalanced reactions are: 1) Xe + F2 → XeF6 2) Xe + F2 → XeF4 3) Xe + F2 → XeF2
04

Balance the equations

To balance these three reactions, we must adjust the stoichiometric coefficients like this: 1) Xe + 3F2 → XeF6 2) Xe + 2F2 → XeF4 3) Xe + F2 → XeF2 c) Sulfur reacts with hydrogen gas.
05

Write unbalanced equation

Sulfur (S) reacts with hydrogen gas (H2) to form hydrogen sulfide (H2S), which can be written as: S + H2 → H2S
06

Balance the equation

In order to balance the equation, we need two hydrogen atoms for every one sulfur atom. The balanced equation is: S + H2 → H2S d) Fluorine reacts with water.
07

Write unbalanced equation

Fluorine (F2) reacts with water (H2O) to form hydrogen fluoride (HF) and oxygen gas (O2), which can be written as: F2 + H2O → HF + O2
08

Balance the equation

In order to balance the equation, we must have four atoms of hydrogen, two atoms of oxygen and two atoms of fluorine on both sides. So, the balanced equation is: F2 + 2H2O → 4HF + O2

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Most popular questions from this chapter

Identify at least two ions that have the following ground-state electron configurations: (a) \([\mathrm{Ar}] ;\) (b) \([\mathrm{Ar}] 3 d^{5}\); (c) \([\mathrm{Kr}] 5 s^{2} 4 d^{10}\)

Arrange the following oxides in order of increasing acidity: \(\mathrm{CO}_{2}, \mathrm{CaO}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{SO}_{3}, \mathrm{SiO}_{2},\) and \(\mathrm{P}_{2} \mathrm{O}_{5}\)

Consider the isoelectronic ions \(\mathrm{F}^{-}\) and \(\mathrm{Na}^{+}\). (a) Which ion is smaller? (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, \(S,\) calculate \(Z_{\text {eff }}\) for the \(2 p\) electrons in both ions. (c) Repeat this calculation using Slater's rules to estimate the screening constant, \(S\). (d) For isoelectronic ions, how are effective nuclear charge and ionic radius related?

Consider the first ionization energy of neon and the electron affinity of fluorine. (a) Write equations, including electron configurations, for each process. (b) These two quantities will have opposite signs. Which will be positive, and which will be negative? (c) Would you expect the magnitudes of these two quantities to be equal? If not, which one would you expect to be larger? Explain your answer.

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) \(\mathrm{Ti}, \mathrm{Ba} ;(\mathrm{b}) \mathrm{Ag}, \mathrm{Cu} ;(\mathrm{c}) \mathrm{Ge}\) \(\mathrm{Cl} ;\) (d) \(\mathrm{Pb},\) Sb. (In each case use electron configuration and effective nuclear charge to explain your answer.)
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