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Chapter 7: Problem 82

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Chlorine reacts with water. (b) Barium metal is heated in an atmosphere of hydrogen gas. (c) Lithium reacts with sulfur. (d) Fluorine reacts with magnesium metal.

Short Answer

Expert verified
The balanced chemical equations for the given reactions are: a) Cl2 + H2O 鈫� HCl + HClO b) Ba + H2 鈫� BaH2 c) 2 Li + S 鈫� Li2S d) F2 + Mg 鈫� MgF2

Step by step solution

01

Identify the reactants and products

a) Chlorine reacts with water: Reactants: Chlorine (Cl2) and water (H2O). Products: Hydrochloric acid (HCl) and hypochlorous acid (HClO). b) Barium metal is heated in an atmosphere of hydrogen gas: Reactants: Barium metal (Ba) and hydrogen gas (H2). Product: Barium hydride (BaH2). c) Lithium reacts with sulfur: Reactants: Lithium (Li) and sulfur (S). Product: Lithium sulfide (Li2S). d) Fluorine reacts with magnesium metal: Reactants: Fluorine (F2) and magnesium (Mg). Product: Magnesium fluoride (MgF2).
02

Write the unbalanced chemical equation

a) Cl2 + H2O 鈫� HCl + HClO b) Ba + H2 鈫� BaH2 c) Li + S 鈫� Li2S d) F2 + Mg 鈫� MgF2
03

Balance the chemical equation

a) The balanced equation for chlorine reacting with water is: Cl2 + H2O 鈫� HCl + HClO b) The balanced equation for barium metal being heated in an atmosphere of hydrogen gas is: Ba + H2 鈫� BaH2 c) The balanced equation for lithium reacting with sulfur is: 2 Li + S 鈫� Li2S d) The balanced equation for fluorine reacting with magnesium metal: F2 + Mg 鈫� MgF2

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Most popular questions from this chapter

Consider the gas-phase transfer of an electron from a sodium atom to a chlorine atom: $$ \mathrm{Na}(\mathrm{g})+\mathrm{Cl}(\mathrm{g}) \longrightarrow \mathrm{Na}^{+}(\mathrm{g})+\mathrm{Cl}^{-}(g) $$ (a) Write this reaction as the sum of two reactions, one that relates to an ionization energy and one that relates to an electron affinity. (b) Use the result from part (a), data in this chapter, and Hess's law to calculate the enthalpy of the above reaction. Is the reaction exothermic or endothermic? (c) The reaction between sodium metal and chlorine gas is highly exothermic and produces \(\mathrm{NaCl}(\mathrm{s})\), whose structure was discussed in Section 2.7. Comment on this observation relative to the calculated enthalpy for the aforementioned gas-phase reaction.

(a) Which will have the lower energy, a 4 s or a \(4 p\) electron in an As atom? (b) How can we use the concept of effective nuclear charge to explain your answer to part (a)?

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.

Consider the stable elements through lead \((Z=82)\). In how many instances are the atomic weights of the elements in the reverse order relative to the atomic numbers of the elements? What is the explanation for these cases?

Compare the elements sodium and magnesium with respect to the following properties: (a) electron configuration, (b) most common ionic charge, (c) first ionization energy, (d) reactivity toward water, (e) atomic radius. Account for the differences between the two elements.
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