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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) 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) \( Sr + 2H_2O \rightarrow Sr(OH)_2 + 2H_2\) (c) \( 4Na + O_2 \rightarrow 2Na_2O \) (d) \( Ca + I_2 \rightarrow CaI_2 \)

Step by step solution

01

Write the unbalanced equation

Cesium (Cs) reacts with water (H2O) to form cesium hydroxide (CsOH) and hydrogen gas (H2). Cs + H2O -> CsOH + H2
02

Balance the equation

Checking the number of atoms on each side of the equation, we need to put a coefficient of 2 in front of CsOH to balance cesium and a coefficient of 2 in front of H2O to balance hydrogen and oxygen atoms. 2Cs + 2H2O -> 2CsOH + H2 So, our final balanced equation is: \[ 2Cs + 2H_2O \rightarrow 2CsOH + H_2 \] (b) Strontium is added to water.
03

Write the unbalanced equation

Strontium (Sr) reacts with water (H2O) to form strontium hydroxide (Sr(OH)2) and hydrogen gas (H2). Sr + H2O -> Sr(OH)2 + H2
04

Balance the equation

Looking at the atoms in the equation, the strontium and oxygen atoms are already balanced. To balance the hydrogen atoms, we need to put a coefficient of 2 in front of H2O and H2. Sr + 2H2O -> Sr(OH)2 + 2H2 The final balanced equation is: \[ Sr + 2H_2O \rightarrow Sr(OH)_2 + 2H_2\] (c) Sodium reacts with oxygen.
05

Write the unbalanced equation

Sodium (Na) reacts with oxygen (O2) to form sodium oxide (Na2O). Na + O2 -> Na2O
06

Balance the equation

To balance this equation, place a coefficient of 4 in front of Na and a coefficient of 2 in front of Na2O. 4Na + O2 -> 2Na2O Our final balanced equation is: \[ 4Na + O_2 \rightarrow 2Na_2O \] (d) Calcium reacts with iodine.
07

Write the unbalanced equation

Calcium (Ca) reacts with iodine (I2) to form calcium iodide (CaI2). Ca + I2 -> CaI2
08

Balance the equation

This equation is already balanced, as there is an equal number of each type of atom on both sides. Our final balanced equation is: \[ Ca + I_2 \rightarrow CaI_2 \]

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Key Concepts

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

Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships of the substances used and produced by chemical reactions.
Chemical Reactions
Chemical reactions involve the breaking and forming of bonds between atoms to produce new substances. During a chemical reaction, the identities of substances change as atoms are rearranged. Knowledge of how to write balanced chemical equations is crucial because it reflects the law of conservation of mass, where the total mass of reactants equals the total mass of products.
Compounds and Elements
Elements are pure substances consisting of only one type of atom, while compounds are substances composed of two or more different elements that are chemically bonded. The process of a chemical reaction often involves elements reacting to form compounds, or compounds breaking down into elements or smaller compounds.

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Most popular questions from this chapter

Consider the \(\mathrm{A}_{2} \mathrm{X}_{4}\) molecule depicted here, where \(\mathrm{A}\) and \(\mathrm{X}\) are elements. The \(\mathrm{A}-\mathrm{A}\) bond length in this molecule is \(d_{1},\) and the four \(\mathrm{A}-\mathrm{X}\) bond lengths are each \(d_{2}\). (a) In terms of \(d_{1}\) and \(d_{2}\), how could you define the bonding atomic radii of atoms \(A\) and \(X ?(b)\) In terms of \(d_{1}\) and \(d_{2}\), what would you predict for the \(\mathrm{X}-\mathrm{X}\) bond length of an \(\mathrm{X}_{2}\) molecule? \([\) Section 7.3\(]\)

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) \(\mathrm{Au}^{+}\).

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.

(a) Write the electron configuration for \(\mathrm{Li}\), and estimate the effective nuclear charge experienced by the valence electron. (b) The energy of an electron in a one-electron atom or ion equals \(\left(-2.18 \times 10^{-18} \mathrm{~J}\right)\left(\frac{Z^{2}}{n^{2}}\right)\) where \(Z\) is the nuclear charge and \(n\) is the principal quantum number of the electron. Estimate the first ionization energy of Li. (c) Compare the result of your calculation with the value reported in Table 7.4 and explain the difference. (d) What value of the effective nuclear charge gives the proper value for the ionization energy? Does this agree with your explanation in \((\mathrm{c}) ?\)

(a) As described in Section \(7.7,\) the alkali metals react with hydrogen to form hydrides and react with halogens- for example, fluorine to form halides, Compare the roles of hydrogen and the halogen in these reactions. How are the forms of hydrogen and halogen in the products alike? (b) Write balanced equations for the reaction of fluorine with calcium and for the reaction of hydrogen with calcium. What are the similarities among the products of these reactions?
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