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Chapter 7: Problem 70

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

Short Answer

Expert verified
(a) \(2Cs + 2H_2O \rightarrow 2CsOH + H_2\) (b) \(Sr + 2H_2O \rightarrow Sr(OH)_2 + H_2\) (c) \(4Na + O_2 \rightarrow 2Na_2O\) (d) \(Ca + I_2 \rightarrow CaI_2\)

Step by step solution

01

(a) Cesium is added to water.

Cesium (Cs) is an alkali metal that reacts with water (H鈧侽) to form cesium hydroxide (CsOH) and hydrogen gas (H鈧�). The unbalanced equation for this reaction is: Cs + H鈧侽 -> CsOH + H鈧� To balance the equation, we simply need to adjust the coefficients: 2Cs + 2H鈧侽 -> 2CsOH + H鈧�
02

(b) Strontium is added to water.

Strontium (Sr) is an alkaline earth metal that reacts with water (H鈧侽) to form strontium hydroxide (Sr(OH)鈧�) and hydrogen gas (H鈧�). The unbalanced equation for this reaction is: Sr + H鈧侽 -> Sr(OH)鈧� + H鈧� To balance the equation, we simply need to adjust the coefficients: Sr + 2H鈧侽 -> Sr(OH)鈧� + H鈧�
03

(c) Sodium reacts with oxygen.

Sodium (Na) is an alkali metal that reacts with oxygen (O鈧�) to form sodium oxide (Na鈧侽). The unbalanced equation for this reaction is: Na + O鈧� -> Na鈧侽 To balance the equation, we need to adjust the coefficients: 4Na + O鈧� -> 2Na鈧侽
04

(d) Calcium reacts with iodine.

Calcium (Ca) is an alkaline earth metal that reacts with iodine (I鈧�) to form calcium iodide (CaI鈧�). The unbalanced equation for this reaction is: Ca + I鈧� -> CaI鈧� To balance the equation, we simply need to adjust the coefficients: Ca + I鈧� -> CaI鈧� The balanced chemical equations for each reaction are as follows: (a) 2Cs + 2H鈧侽 -> 2CsOH + H鈧� (b) Sr + 2H鈧侽 -> Sr(OH)鈧� + H鈧� (c) 4Na + O鈧� -> 2Na鈧侽 (d) Ca + I鈧� -> CaI鈧�

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Key Concepts

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

Balancing Chemical Equations
Balancing chemical equations is a fundamental skill in chemistry. It ensures that the mass and the number of atoms are equal on both sides of a chemical reaction. The principle behind balancing equations is the conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.
  • To balance an equation, start by writing the unbalanced equation with all reactants on the left and products on the right.
  • Use coefficients to multiply the number of molecules of each substance until the number of each type of atom is the same on both sides.
  • Balanced equations allow chemists to accurately predict the amounts of products that will form from given reactants.
As an example, when balancing the equation for the reaction of cesium with water, the initial unbalanced equation is Cs + H鈧侽 -> CsOH + H鈧�. By adjusting the coefficients to 2 Cs + 2 H鈧侽 on the left, we ensure that they balance with 2 CsOH + H鈧� on the right, conserving mass and atoms.
Alkali Metals
Alkali metals are located in Group 1 of the periodic table. This group includes elements like sodium (Na), potassium (K), and cesium (Cs). These metals are highly reactive, especially with water and oxygen.
  • Their reactivity increases as you move down the group in the periodic table.
  • They have a single electron in their outermost shell, making them eager to lose that electron in reactions.
  • Often these reactions are vigorous and even explosive. For instance, when cesium is added to water, it reacts to form cesium hydroxide and hydrogen gas, as shown in the balanced equation: 2 Cs + 2 H鈧侽 -> 2 CsOH + H鈧�.
Understanding the behavior of alkaline metals helps in predicting their reactions with other elements, which is a crucial part of chemistry.
Alkaline Earth Metals
Alkaline earth metals are found in Group 2 of the periodic table. This category includes elements like magnesium (Mg), calcium (Ca), and strontium (Sr). These metals are also reactive, but less so than alkali metals.
  • They typically form +2 ions because they have two electrons in their outer shell that they tend to lose in reactions.
  • These metals react with water, albeit less violently than alkali metals, forming hydroxides and releasing hydrogen gas.
  • An example of this is strontium reacting with water, forming strontium hydroxide: Sr + 2 H鈧侽 -> Sr(OH)鈧� + H鈧�.
Alkaline earth metals are essential in various industries and have important applications due to their unique properties and reactivity.

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Most popular questions from this chapter

Write equations that show the process for (a) the first two ionization energies of lead and (b) the fourth ionization energy of zirconium.

Discussing this chapter, a classmate says, "Since elements that form cations are metals and elements that form anions are nonmetals, elements that do not form ions are metalloids." Do you agree or disagree? Explain your answer.

Detailed calculations show that the value of \(Z_{\text {eff }}\) for the outermost electrons in \(\mathrm{Na}\) and \(\mathrm{K}\) atoms is \(2.51+\) and \(3.49+\), respectively. (a) What value do you estimate for \(Z_{\text {eff }}\) experienced by the outermost electron in both \(\mathrm{Na}\) and \(\mathrm{K}\) by assuming core electrons contribute \(1.00\) and valence electrons contribute \(0.00\) to the screening constant? (b) What values do you estimate for \(Z_{\text {eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text {eff ? }}\) ? (d) Does either method of approximation account for the gradual increase in \(Z_{\text {eff }}\) that occurs upon moving down a group? (e) Predict \(Z_{\text {eff }}\) for the outermost electrons in the \(\mathrm{Rb}\) atom based on the calculations for \(\mathrm{Na}\) and \(\mathrm{K}\).

(a) One of the alkali metals reacts with oxygen to form a solid white substance. When this substance is dissolved in water, the solution gives a positive test for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\). When the solution is tested in a burner flame, a lilac-purple flame is produced. What is the likely identity of the metal? (b) Write a balanced chemical equation for the reaction of the white substance with water.

Which neutral atom is isoelectronic with each of the following ions? \(\mathrm{Ga}^{3+}, \mathrm{Zr}^{4+}, \mathrm{Mn}^{7+}, \Gamma, \mathrm{Pb}^{2+}\).
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