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Chapter 7: Problem 73

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal burns in 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 is reacted with molten sulfur.

Short Answer

Expert verified
(a) \(2K + Cl_2 \rightarrow 2KCl\) (b) \(SrO + H_2O \rightarrow Sr(OH)_2\) (c) \(4Li + O_2 \rightarrow 2Li_2O\) (d) \(2Na + S \rightarrow Na_2S\)

Step by step solution

01

(a) Potassium metal and chlorine gas reaction

: 1. Identify reactants and products: The reactants are potassium metal (K) and chlorine gas (\(Cl_2\)). When a metal reacts with a halogen, it forms a metal halide. In this case, the product is potassium chloride (KCl). 2. Write the unbalanced equation: \(K + Cl_2 \rightarrow KCl\) 3. Balance the equation: To balance the equation, we must ensure that there are equal numbers of each atom on both sides of the equation. Adjusting the coefficients, we get the balanced equation: \(2K + Cl_2 \rightarrow 2KCl\).
02

(b) Strontium oxide and water reaction

: 1. Identify reactants and products: The reactants are strontium oxide (SrO) and water (H_2O). When a metal oxide reacts with water, it forms a corresponding metal hydroxide. In this case, the product is strontium hydroxide (Sr(OH)_2). 2. Write the unbalanced equation: \(SrO + H_2O \rightarrow Sr(OH)_2\) 3. Balance the equation: The equation is already balanced, so we have \(SrO + H_2O \rightarrow Sr(OH)_2\).
03

(c) Lithium metal and oxygen gas reaction

: 1. Identify reactants and products: The reactants are lithium metal (Li) and oxygen gas (\(O_2\)). When a metal reacts with oxygen, it forms a metal oxide. In this case, the product is lithium oxide (Li_2O). 2. Write the unbalanced equation: \(Li + O_2 \rightarrow Li_2O\) 3. Balance the equation: To balance the equation, we must ensure that there are equal numbers of each atom on both sides of the equation. Adjusting the coefficients, we get the balanced equation: \(4Li + O_2 \rightarrow 2Li_2O\).
04

(d) Sodium metal and molten sulfur reaction

: 1. Identify reactants and products: The reactants are sodium metal (Na) and molten sulfur (S). When a metal reacts with a non-metal, it forms a metal sulfide. In this case, the product is sodium sulfide (Na_2S). 2. Write the unbalanced equation: \(Na + S \rightarrow Na_2S\) 3. Balance the equation: To balance the equation, we must ensure that there are equal numbers of each atom on both sides of the equation. Adjusting the coefficients, we get the balanced equation: \(2Na + S \rightarrow Na_2S\).

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Most popular questions from this chapter

An element \(X\) reacts with oxygen to form \(\mathrm{XO}_{2}\) and with chlorine to form \(\mathrm{XCl}_{4} . \mathrm{XO}_{2}\) is a white solid that melts at high temperatures (above \(\left.1000^{\circ} \mathrm{C}\right)\). Under usual conditions, \(\mathrm{XCl}_{4}\) is a colorless liquid with a boiling point of \(58^{\circ} \mathrm{C}\). (a) \(\mathrm{XCl}_{4}\) reacts with water to form \(\mathrm{XO}_{2}\) and another product. What is the likely identity of the other product? (b) Do you think that element \(\mathrm{X}\) is a metal, nonmetal, or metalloid? Explain. (c) \(\mathrm{By}\) using a sourcebook such as the CRC Handbook of Chemistry and Physics, try to determine the identity of element \(\mathrm{X}\).

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?

Write electron configurations for the following ions, and determine which have noble-gas configurations: (a) \(\mathrm{Cr}^{3+}\), (b) \(\mathrm{N}^{3-},(\mathrm{c}) \mathrm{Sc}^{3+},(\mathrm{d}) \mathrm{Cu}^{2+}\) (e) \(\mathrm{Tl}^{+}\), (f) \(\mathrm{Au}^{+}\).

(a) Why is calcium generally more reactive than magnesium? (b) Why is calcium generally less reactive than potassium?

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 \(\mathrm{P}_{2} \mathrm{O}_{5}\)
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