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Chapter 7: Problem 102

Which of the following is the expected product of the reaction of \(\mathrm{K}(s)\) and \(\mathrm{H}_{2}(g)\) ? (i) \(\mathrm{KH}(s)\), (ii) \(\mathrm{K}_{2} \mathrm{H}(s)\), (iii) \(\mathrm{KH}_{2}(s)\), (iv) \(\mathrm{K}_{2} \mathrm{H}_{2}(s)\), or (v) \(\mathrm{K}(s)\) and \(\mathrm{H}_{2}(g)\) will not react with one another.

Short Answer

Expert verified
The expected product for the reaction between K(s) and H鈧�(g) is (i) KH (s).

Step by step solution

01

Potassium (K) is an alkali metal in Group 1 of the periodic table, so it has a valency of +1. Hydrogen (H) generally has a valency of +1 as well but can act as a reducing agent and accept an electron, making its valency -1 in certain situations. #Step 2: Analyze the possible products and their stoichiometry#

We have five options for the reaction's product: (i) KH(s): One K (+1) reacts with one H (-1), forming a 1:1 stoichiometry compound. (ii) K鈧侶(s): Two K (+1 each) react with one H (-1), forming a 2:1 stoichiometry compound. (iii) KH鈧�(s): One K (+1) reacts with two H (-1 each), forming a 1:2 stoichiometry compound. (iv) K鈧侶鈧�(s): Two K (+1 each) react with two H (-1 each), forming a 2:2 stoichiometry compound. (v) K(s) and H鈧�(g) will not react with one another: No reaction occurs between potassium and hydrogen. #Step 3: Determine the most likely product based on the valencies of the elements#
02

We know K has a valency of +1 and wants to lose one electron, while H will generally have a valency of +1 but can also have a valency of -1 and accept an electron. So it is likely that a compound will form in which K loses one electron and H gains one electron. This situation is achieved in product (i) KH(s), having a 1:1 stoichiometry and satisfying both elements' valency. Therefore, the expected product for the reaction between K(s) and H鈧�(g) is: #Final Answer#

(i) KH (s)

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Key Concepts

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

Stoichiometry
Stoichiometry is the process of determining the relative quantities of reactants and products in chemical reactions. It is essential for predicting the amounts of substances consumed and produced. In the given exercise, stoichiometry helps us understand that potassium (\(K\)) and hydrogen (\(H_2\)) can form a compound with a 1:1 ratio.

Here's why stoichiometry is important:
  • It ensures the correct balance of atoms, satisfying the Law of Conservation of Mass.
  • It helps predict the outcome of reactions, like forming \(KH\) from \(K\) and \(H_2\).
  • It guides chemical synthesis and industrial production by determining how much reactant is needed.
In \(KH\), one potassium atom combines with one hydrogen atom, explaining the 1:1 stoichiometry observed in this reaction. Understanding these ratios allows chemists to predict products accurately.
Alkali Metals
Alkali metals belong to Group 1 of the periodic table and are known for their high reactivity. Potassium (\(K\)) is an alkali metal that reacts readily with other elements. These metals have unique properties:
  • They have a single electron in their outer shell, which they tend to lose easily, forming cations with a +1 charge.
  • They are soft and have low melting points compared to other metals.
  • They react vigorously with water and other substances, which is why handling them requires care.
In the exercise, potassium's reactivity explains why it can readily react with hydrogen. Its tendency to lose an electron allows it to form stable ionic compounds like \(KH\), demonstrating typical alkali metal behavior.
Compound Formation
Compound formation involves the combination of two or more elements to create a new substance with different properties. It's essential to understand valency and electron transfer during this process.

In the reaction between potassium (\(K\)) and hydrogen (\(H_2\)), potassium donates an electron to hydrogen, transforming their individual properties into a stable compound, \(KH\).
  • The electron transfer promotes stability, resulting in ionic bonding.
  • Such reactions often release energy, indicating the formation of a strong bond.
  • Ionic compounds generally have high melting and boiling points due to these strong interactions.
Understanding compound formation helps in predicting the feasibility and outcome of reactions, crucial for both academic studies and practical applications in industry.

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Most popular questions from this chapter

(a) The measured \(\mathrm{Bi}-\mathrm{Br}\) bond length in bismuth tribromide, \(\mathrm{BiBr}_{3}\), is \(2.63 \AA\). Based on this value and the data in Figure 7.8, predict the atomic radius of Bi. (b) Bismuth tribromide is soluble in acidic solution. It is formed by treating solid bismuth(III) oxide with aqueous hydrobromic acid. Write a balanced chemical equation for this reaction. (c) While bismuth(III) oxide is soluble in acidic solutions, it is insoluble in basic solutions such as \(\mathrm{NaOH}(a q)\). Based on these properties, is bismuth characterized as a metallic, metalloid, or nonmetallic element? (d) Treating bismuth with fluorine gas forms \(\mathrm{BiF}_{5}\). Use the electron configuration of \(\mathrm{Bi}\) to explain the formation of a compound with this formulation. (e) While it is possible to form \(\mathrm{BiF}_{5}\) in the manner just described, pentahalides of bismuth are not known for the other halogens. Explain why the pentahalide might form with fluorine but not with the other halogens. How does the behavior of bismuth relate to the fact that xenon reacts with fluorine to form compounds but not with the other halogens?

Consider the stable elements through lead \((Z=82)\). In how many instances are the atomic weights of the elements out of order relative to the atomic numbers of the elements?

Arrange the following oxides in order of increasing acidity: $$ \mathrm{CO}_{2}, \mathrm{CaO}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{SO}_{3}, \mathrm{SiO}_{2}, \mathrm{P}_{2} \mathrm{O}_{5} \text {. } $$

Which of the following statements about effective nuclear charge for the outermost valence electron of an atom is incorrect? (i) The effective nuclear charge can be thought of as the true nuclear charge minus a screening constant due to the other electrons in the atom. (ii) Effective nuclear charge increases going left to right across a row of the periodic table. (iii) Valence electrons screen the nuclear charge more effectively than do core electrons. (iv) The effective nuclear charge shows a sudden decrease when we go from the end of one row to the beginning of the next row of the periodic table. (v) The change in effective nuclear charge going down a column of the periodic table is generally less than that going across a row of the periodic table.

Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like nonmetals. Its properties can be explained in part by its electron configuration and by the values for its ionization energy and electron affinity. (a) Explain why the electron affinity of hydrogen is much closer to the values for the alkali elements than for the halogens. (b) Is the following statement true? "Hydrogen has the smallest bonding atomic radius of any element that forms chemical compounds. If not, correct it. If it is, explain in terms of electron configurations. (c) Explain why the ionization energy of hydrogen is closer to the values for the halogens than for the alkali metals. (d) The hydride ion is \(\mathrm{H}\). Write out the process corresponding to the first ionization energy of the hydride ion. (e) How does the process in part (d) compare to the process for the electron affinity of a neutral hydrogen atom?
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