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Chapter 7: Problem 58

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?

Short Answer

Expert verified
I disagree with the statement, "Since elements that form cations are metals and elements that form anions are nonmetals, elements that do not form ions are metalloids." This is because metalloids have intermediate properties between metals and nonmetals and can sometimes lose electrons to form cations or gain electrons to form anions, depending on the specific element and the conditions. Their ion-forming abilities depend on their specific properties and electron structures.

Step by step solution

01

Understand the properties of metals, nonmetals, and metalloids

Metals are elements that are generally shiny, conductive, and malleable. They tend to lose electrons and form positive ions (cations). Nonmetals are elements that do not share the characteristics of metals. They are generally poor conductors of heat and electricity and tend to gain electrons, forming negative ions (anions). Metalloids, also called semi-metals, have properties that are intermediate between metals and nonmetals. They can sometimes behave like metals and other times like nonmetals, depending on the conditions.
02

Analyze the ion-forming abilities of metals and nonmetals

Metals lose electrons to form cations, and nonmetals gain electrons to form anions. This ion-forming ability is mainly due to their respective properties and electron structures. Metals, having low ionization energy, tend to lose electrons easily, while nonmetals, with high electron affinities, have a tendency to gain electrons.
03

Assess the ion-forming abilities of metalloids

Metalloids have intermediate properties between metals and nonmetals, which means they can sometimes lose electrons to form cations or gain electrons to form anions, depending on the specific element and the conditions in which they are present. Therefore, saying that metalloids do not form ions is not entirely accurate.
04

Conclusion

Based on the above analysis, we can disagree with the statement, "Since elements that form cations are metals and elements that form anions are nonmetals, elements that do not form ions are metalloids." Metalloids can form ions under certain conditions, and their ion-forming abilities depend on their specific properties and electron structures.

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Most popular questions from this chapter

Elemental cesium reacts more violently with water than does elemental sodium. Which of the following best explains this difference in reactivity? (i) Sodium has greater metallic character than does cesium. (ii) The first ionization energy of cesium is less than that of sodium. (iii) The electron affinity of sodium is smaller than that of cesium. (iv) The effective nuclear charge for cesium is less than that of sodium. (v) The atomic radius of cesium is smaller than that of sodium.

The electron affinities, in \(\mathrm{kJ} / \mathrm{mol},\) for the group 1 \(\mathrm{B}\) and group 2 \(\mathrm{B}\) metals are as follows: (a) Why are the electron affinities of the group 2 \(\mathrm{B}\) elements greater than zero? (b) Why do the electron affinities of the group 1 \(\mathrm{B}\) elements become more negative as we move down the group? [Hint: Examine the trends in the electron affinities of other groups as we proceed down the periodic table.]

Potassium superoxide, \(\mathrm{KO}_{2},\) is often used in oxygen masks (such as those used by firefighters) because \(\mathrm{KO}_{2}\) reacts with \(\mathrm{CO}_{2}\) to release molecular oxygen. Experiments indicate that 2 \(\mathrm{mol}\) of \(\mathrm{KO}_{2}(s)\) react with each mole of= \(\mathrm{CO}_{2}(g) .\) (a) The products of the reaction are \(\mathrm{K}_{2} \mathrm{CO}_{3}(s)\) and \(\mathrm{O}_{2}(g) .\) Write a balanced equation for the reaction between \(\mathrm{KO}_{2}(s)\) and \(\mathrm{CO}_{2}(g) .(\mathbf{b})\) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced? (c) What mass of \(\mathrm{KO}_{2}(s)\) is needed to consume 18.0 \(\mathrm{g} \mathrm{CO}_{2}(g) ?\) What mass of \(\mathrm{O}_{2}(g)\) is produced during this reaction?

The first ionization energy of the oxygen molecule is the energy required for the following process: $$\mathrm{O}_{2}(g) \longrightarrow \mathrm{O}_{2}^{+}(g)+\mathrm{e}^{-}$$ The energy needed for this process is 1175 \(\mathrm{kJ} / \mathrm{mol}\) , very similar to the first ionization energy of \(\mathrm{Xe} .\) Would you expect \(\mathrm{O}_{2}\) to react with \(\mathrm{F}_{2} ?\) If so, suggest a product or products of this reaction.

(a) Does metallic character increase, decrease, or remain unchanged as one goes from left to right across a row of the periodic table? (b) Does metallic character increase, decrease, or remain unchanged as one goes down a column of the periodic table? (c) Are the periodic trends in (a) and (b) the same as or different from those for first ionization energy?
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