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Chapter 22: Problem 64

Give the chemical formula for (a) fullerene, (b) potassium cyanide, (c) zinc carbide, (d) zinc acetylide, (e) carbon disulfide.

Short Answer

Expert verified
(a) C60, (b) KCN, (c) ZnC2, (d) Zn(C2H)2, (e) CS2

Step by step solution

01

(a) Fullerene

Fullerene is a form of carbon where the atoms are arranged in the shape of hollow spheres or tubes. The most common form of fullerene is C60, also known as Buckminsterfullerene or "buckyballs," which has 60 carbon atoms arranged in a spherical structure resembling a soccer ball. Chemical formula: C60
02

(b) Potassium cyanide

Potassium cyanide is a salt made up of potassium (K) and cyanide (CN) ions. Potassium (K) is a metal from group 1 of the periodic table, and it has an oxidation state of +1. Cyanide (CN) is a polyatomic ion with a charge of -1. To determine the chemical formula, we balance the positive and negative charges. In this case, one potassium ion (K+) is required to balance one cyanide ion (CN−). Chemical formula: KCN
03

(c) Zinc carbide

Zinc carbide is a compound made up of zinc (Zn) and carbon (C). Zinc is a metal from group 12 of the periodic table, and it usually has an oxidation state of +2. Carbon, in the form of carbide (C2), has an oxidation state of -4. To balance the charges, one zinc ion (Zn2+) and one carbide ion (C2-4) are required. Chemical formula: ZnC2
04

(d) Zinc acetylide

Zinc acetylide is a compound made up of zinc (Zn) and acetylide ion (C2H). Zinc is a metal from group 12 of the periodic table, and it usually has an oxidation state of +2. Acetylide ion (C2H) has an oxidation state of -1. To balance the charges, one zinc ion (Zn2+) requires two acetylide ions (C2H-) for charge balance. Chemical formula: Zn(C2H)2
05

(e) Carbon disulfide

Carbon disulfide is a molecular compound made up of carbon (C) and sulfur (S). The prefix "di" in disulfide indicates that there are two sulfur atoms. Carbon can form four covalent bonds in molecules like this, and sulfur can form two covalent bonds. In carbon disulfide, one carbon atom forms two double bonds with two sulfur atoms. Chemical formula: CS2

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Most popular questions from this chapter

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q),(\mathbf{b})\) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+}\) (c) aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) to mercury metal. Write balanced equations for these reactions.

Consider the elements \(\mathrm{N}, \mathrm{F}, \mathrm{Si}, \mathrm{Rb},\) Te, and Ir. From this list, select the element that \((\mathbf{a})\) is most electronegative, \((\mathbf{b})\) exhibits a maximum oxidation state of \(+6,(\mathbf{c})\) loses an electron most readily, (d) forms \(\pi\) bonds most readily, (e) is a transition metal, \((\mathbf{f})\) forms four covalent bonds to achieve octet.

Identify each of the following elements as a metal, nonmetal, or metalloid: (a) germanium, (b) bismuth, (c) sul- (d) calcium, phur, (e) rhenium, (f) tin.

Both dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\), and methylhydrazine, \(\mathrm{CH}_{3} \mathrm{NHNH}_{2}\), have been used as rocket fuels. When dinitrogen tetroxide $\left(\mathrm{N}_{2} \mathrm{O}_{4}\right)$ is used as the oxidizer, the products are \(\mathrm{H}_{2} \mathrm{O}, \mathrm{CO}_{2}\), and \(\mathrm{N}_{2}\). If the thrust of the rocket depends on the volume of the products produced, which of the substituted hydrazines produces a greater thrust per gram total mass of oxidizer plus fuel? (Assume that both fuels generate the same temperature and that \(\mathrm{H}_{2} \mathrm{O}(g)\) is formed.)

The maximum allowable concentration of \(\mathrm{H}_{2} \mathrm{~S}(g)\) in air is \(20 \mathrm{mg}\) per kilogram of air ( 20 ppm by mass). How many grams of FeS would be required to react with hydrochloric acid to produce this concentration at \(101.3 \mathrm{kPa}\) and \(25^{\circ} \mathrm{C}\) in an average room measuring $3.5 \mathrm{~m} \times 6.0 \mathrm{~m} \times 2.5 \mathrm{~m} ?\( (Under these conditions, the average molar mass of air is \)29.0 \mathrm{~g} / \mathrm{mol} .)$
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