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Chapter 7: Problem 70

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Lithium is added to water. (b) Calcium is added to water. (c) Potassium reacts with chlorine gas. (d) Rubidium reacts with oxygen.

Short Answer

Expert verified
(a) 2 Li (s) + 2 H₂O (l) -> 2 LiOH (aq) + H₂ (g) (b) Ca (s) + 2 H₂O (l) -> Ca(OH)₂ (aq) + H₂ (g) (c) 2 K (s) + Cl₂ (g) -> 2 KCl (s) (d) 4 Rb (s) + O₂ (g) -> 2 Rb₂O (s)

Step by step solution

01

(a) Lithium is added to water.

Lithium (Li) is an alkali metal, and it reacts with water (H₂O) to form lithium hydroxide (LiOH) and hydrogen gas (H₂). The balanced equation for this reaction can be obtained by ensuring that the number of H and O atoms is equal on both sides. Thus, the balanced equation is: \( \) 2 Li (s) + 2 H₂O (l) -> 2 LiOH (aq) + H₂ (g) \( \)
02

(b) Calcium is added to water.

Calcium (Ca) is an alkaline earth metal, and it reacts with water (H₂O) to form calcium hydroxide (Ca(OH)₂) and hydrogen gas (H₂). To balance this equation, ensure that the number of H and O atoms is equal on both sides. The balanced equation is: \( \) Ca (s) + 2 H₂O (l) -> Ca(OH)₂ (aq) + H₂ (g) \( \)
03

(c) Potassium reacts with chlorine gas.

Potassium (K) is an alkali metal, and it reacts with chlorine gas (Cl₂) to form potassium chloride (KCl). To balance this equation, ensure that the number of K and Cl atoms is equal on both sides. The balanced equation is: \( \) 2 K (s) + Cl₂ (g) -> 2 KCl (s) \( \)
04

(d) Rubidium reacts with oxygen.

Rubidium (Rb) is an alkali metal, and it reacts with oxygen (O₂) to form rubidium oxide (Rb₂O). To balance this equation, ensure that the number of Rb and O atoms is equal on both sides. The balanced equation is: \( \) 4 Rb (s) + O₂ (g) -> 2 Rb₂O (s) \( \)

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Most popular questions from this chapter

Give three examples of +2 ions that have an electron configuration of $n d^{10}(n=3,4,5 \ldots)$

Which of the following chemical equations is connected to the definitions of (a) the first ionization energy of oxygen, (b) the second ionization energy of ox ygen, and (c) the electron affinity of oxygen? (i) \(\mathrm{O}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{O}^{-}(g)\) (ii) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{+}(g)+\mathrm{e}^{-}\) (iii) \(\mathrm{O}(g)+2 \mathrm{e}^{-} \longrightarrow \mathrm{O}^{2-}(g)\) (iv) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{2+}(g)+2 \mathrm{e}^{-}\) $(\mathbf{v}) \mathrm{O}^{+}(g) \longrightarrow \mathrm{O}^{2+}(g)+\mathrm{e}^{-}$

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal is exposed to an atmosphere of chlorine gas. (b) Strontium oxide is added to water. (c) A fresh surface of lithium metal is exposed to oxygen gas. (d) Sodium metal reacts with molten sulfur.

Write a balanced equation for the reaction that occurs in each of the following cases: (a) White phorphrous, \(\mathrm{P}_{4}(\mathrm{~s})\), reacts with chlorine gas. (b) Sodium metal reacts with water. (c) Hydrogen bromide gas reacts with chlorine gas. (d) Aluminum trichloride reacts with aqueous sodium hydroxide.

Arrange the following atoms in order of increasing effective nuclear charge experienced by the electrons in the \(n=2\) shell: Be, Br, Na, P, Se.
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