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Chapter 7: Problem 74

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water. (b) Stontium is added to water. (c) Sodium reacts with oxygen. (d) Calcium reacts with iodine.

Short Answer

Expert verified
(a) \( 2 Cs + 2 H鈧侽 \rightarrow 2 CsOH + H鈧� \) (b) \( Sr + 2 H鈧侽 \rightarrow Sr(OH)鈧� + H鈧� \) (c) \( 4 Na + O鈧� \rightarrow 2 Na鈧侽 \) (d) \( Ca + I鈧� \rightarrow CaI鈧� \)

Step by step solution

01

(a) Cesium reacts with water.

First, we need to identify the reactants and products of the reaction as follows: - Reactants: Cesium (Cs) and water (H鈧侽) - Products: Cesium hydroxide (CsOH) and hydrogen gas (H鈧�) Now, we can write the unbalanced equation: \( Cs + H鈧侽 \rightarrow CsOH + H鈧� \) To balance this equation, we need to adjust the coefficients: \( 2 Cs + 2 H鈧侽 \rightarrow 2 CsOH + H鈧� \) So, the balanced equation for this reaction is: \( 2 Cs + 2 H鈧侽 \rightarrow 2 CsOH + H鈧� \)
02

(b) Strontium reacts with water.

First, we need to identify the reactants and products of the reaction: - Reactants: Strontium (Sr) and water (H鈧侽) - Products: Strontium hydroxide (Sr(OH)鈧�) and hydrogen gas (H鈧�) Now, we can write the unbalanced equation: \( Sr + H鈧侽 \rightarrow Sr(OH)鈧� + H鈧� \) To balance this equation, we need to adjust the coefficients: \( Sr + 2 H鈧侽 \rightarrow Sr(OH)鈧� + H鈧� \) So, the balanced equation for this reaction is: \( Sr + 2 H鈧侽 \rightarrow Sr(OH)鈧� + H鈧� \)
03

(c) Sodium reacts with oxygen.

First, we need to identify the reactants and products of the reaction: - Reactants: Sodium (Na) and oxygen (O鈧�) - Products: Sodium oxide (Na鈧侽) Now, we can write the unbalanced equation: \( Na + O鈧� \rightarrow Na鈧侽 \) To balance this equation, we need to adjust the coefficients: \( 4 Na + O鈧� \rightarrow 2 Na鈧侽 \) So, the balanced equation for this reaction is: \( 4 Na + O鈧� \rightarrow 2 Na鈧侽 \)
04

(d) Calcium reacts with iodine.

First, we need to identify the reactants and products of the reaction: - Reactants: Calcium (Ca) and iodine (I鈧�) - Products: Calcium iodide (CaI鈧�) Now, we can write the unbalanced equation: \( Ca + I鈧� \rightarrow CaI鈧� \) To balance this equation, there is no need to adjust the coefficients, since it is already balanced. So, the balanced equation for this reaction is: \( Ca + I鈧� \rightarrow CaI鈧� \)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Reaction with Water
When metals react with water, an interesting transformation takes place. This is typically characterized by the formation of hydroxides and the release of hydrogen gas. Let's look at cesium and strontium as examples.
  • Cesium and Water: When cesium is added to water, cesium hydroxide (CaOH) is produced, and hydrogen gas is released. The balanced reaction is: \[2Cs + 2H_2O \rightarrow 2CsOH + H_2\]
  • Strontium and Water: Strontium undergoes a similar reaction. It forms strontium hydroxide (Sr(OH)鈧�) and hydrogen gas: \[ Sr + 2H_2O \rightarrow Sr(OH)_2 + H_2\]
These reactions highlight how active metals typically displace the hydrogen in water, forming hydroxides and releasing hydrogen gas.
Reaction with Oxygen
When metals react with oxygen, they form metal oxides. Sodium, for instance, contributes to forming this type of compound.
  • Sodium and Oxygen: Sodium reacts vigorously with oxygen to produce sodium oxide. The reaction can be represented and balanced as: \[4Na + O_2 \rightarrow 2Na_2O\]

This process illustrates how various metals create different kinds of oxides depending on their reactivity with oxygen. Understanding the ability of a metal to react with oxygen can offer insights into its basic chemical behavior.
Chemical Reactions
Chemical reactions occur when substances (reactants) interact to form new substances (products). These interactions involve the breaking and forming of bonds, which can significantly change the properties of the materials involved. For example:
  • Cesium and Water: A violent reaction yielding cesium hydroxide and hydrogen gas.
  • Sodium and Oxygen: Formation of sodium oxide through powerful oxidation.
In these reactions, new compounds with distinct properties from the initial elements are formed, demonstrating the transformative power of chemical reactions.
Chemical Equations
Chemical equations are symbolic representations of a chemical reaction. They display the reactants and products with their respective amounts, represented by coefficients, for balance. Let's analyze:
  • Balancing Equations: This essential part involves adjusting coefficients to ensure the same number of each type of atom on both sides of the equation. For instance, with sodium and oxygen:\[4Na + O_2 \rightarrow 2Na_2O\]
  • Significance: Balanced equations reflect the law of conservation of mass, meaning matter cannot be created or destroyed. Thus, both sides of the equation must have equal atom counts.
Balanced chemical equations are important tools for understanding the quantitative aspects of a chemical reaction. They help predict the quantities of reactants required or products formed during a reaction.

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Most popular questions from this chapter

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

Make a simple sketch of the shape of the main part of the periodic table, as shown (a) Ignoring \(\mathrm{H}\) and \(\mathrm{He}\), write a single straight arrow from the element with the smallest bonding atomic radius to the element with the largest. (b) Ignoring \(\mathrm{H}\) and \(\mathrm{He}\), write a single straight arrow from the element with the smallest first ionization energy to the element with the largest. (c) What significant observation can you make from the arrows you drew in parts (a) and (b)? [Sections \(7.3\) and 7.4]

Little is known about the properties of astatine, At, because of its rarity and high radioactivity. Nevertheless, it is possible for us to make many predictions about its properties. (a) Do you expect the element to be a gas, liquid, or solid at room temperature? Explain. (b) What is the chemical formula of the compound it forms with Na?

When magnesium metal is burned in air (Figure 3.5), two products are produced. One is magnesium oxide, \(\mathrm{MgO}\). The other is the product of the reaction of \(\mathrm{Mg}\) with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas. (a) Based on the charge of the nitride ion (Table 2.5), predict the formula of magnesium nitride. (b) Write a balanced equation for the reaction of magnesium nitride with water. What is the driving force for this reaction? (c) In an experiment a piece of magnesium ribbon is burned in air in a crucible. The mass of the mixture of \(\mathrm{MgO}\) and magnesium nitride after burning is \(0.470 \mathrm{~g}\). Water is added to the crucible, further reaction occurs, and the crucible is heated to dryness until the final product is \(0.486 \mathrm{~g}\) of \(\mathrm{MgO}\). What was the mass percentage of magnesium nitride in the mixture obtained after the initial burning? (d) Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a \(6.3-\mathrm{g} \mathrm{Mg}\) ribbon reacts with \(2.57 \mathrm{~g} \mathrm{NH}_{3}(\mathrm{~g})\) and the reaction goes to \(\mathrm{com}\) pletion, which component is the limiting reactant? What mass of \(\mathrm{H}_{2}(\mathrm{~g})\) is formed in the reaction? (e) The standard enthalpy of formation of solid magnesium nitride is \(-461.08 \mathrm{~kJ} / \mathrm{mol}\). Calculate the standard enthalpy change for the reaction between magnesium metal and ammonia gas.

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