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Chapter 2: Problem 36

Write the names of the following molecules. (a) \(\mathrm{CO}\) (b) \(\mathrm{SiC}\) (c) \(\mathrm{XeF}_{6}\) (d) \(\mathrm{P}_{4} \mathrm{O}_{10}\) (e) \(\mathrm{C}_{2} \mathrm{H}_{2}\)

Short Answer

Expert verified
Answer: The names of the given chemical molecules are as follows: (a) Carbon monoxide, (b) Silicon carbide, (c) Xenon hexafluoride, (d) Tetraphosphorus decoxide, and (e) Diacetylene (also called ethyne).

Step by step solution

01

Identify the Elements in Each Molecule

Determine the elements represented by the symbols in each molecule: (a) C: Carbon, O: Oxygen (b) Si: Silicon, C: Carbon (c) Xe: Xenon, F: Fluorine (d) P: Phosphorus, O: Oxygen (e) C: Carbon, H: Hydrogen
02

Determine the Type of Compound

Determine if the compound is a binary molecular compound (composed of nonmetals) or an ionic compound (composed of a metal and nonmetal): (a) CO: Binary molecular compound (b) SiC: Ionic compound (c) XeF6: Binary molecular compound (d) P4O10: Binary molecular compound (e) C2H2: Binary molecular compound
03

Naming Binary Molecular Compounds

Name the binary molecular compounds using the appropriate Greek prefixes for the number of atoms of each element: (a) CO: Carbon monoxide (c) XeF6: Xenon hexafluoride (d) P4O10: Tetraphosphorus decoxide (e) C2H2: Diacetylene (also called ethyne)
04

Naming Ionic Compounds

Name the ionic compound by combining the cation (metal) name and the anion (nonmetal) name, ending in -ide: (b) SiC: Silicon carbide

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Most popular questions from this chapter

Consider the elements oxygen, fluorine, argon, sulfur, potassium, and strontium. From this group of elements, which ones fit the descriptions below? (a) Two elements that are metals. (b) Four elements that are nonmetals. (c) Three elements that are solid at room temperature. (d) An element that is found in nature as \(\mathrm{X}_{8}\). (e) One pair of elements that may form a molecular compound. (f) One pair of elements that may form an ionic compound with formula \(\mathrm{AX}\) (g) One pair of elements that may form an ionic compound with formula \(\mathrm{AX}_{2}\) (h) One pair of elements that may form an ionic compound with formula \(\mathrm{A}_{2} \mathrm{X} .\) (i) An element that can form no compounds. (j) Three elements that are gases at room temperature.

A molecule of ethylamine is made up of two carbon atoms, seven hydrogen atoms, and one nitrogen atom. (a) Write its molecular formula. (b) The reactive group in ethylamine is \(\mathrm{NH}_{2}\). Write its condensed structural formula.

Which period of the periodic table (a) has no metals? (b) has no nonmetals? (c) has one post-transition metal and two metalloids?

Calculate the average density of a single Al-27 atom by assuming that it is a sphere with a radius of \(0.143 \mathrm{~nm}\). The masses of a proton, electron, and neutron are \(1.6726 \times 10^{-24} \mathrm{~g}, 9.1094 \times 10^{-28} \mathrm{~g}\), and \(1.6749 \times 10^{-24} \mathrm{~g}\), respectively. The volume of a sphere is \(4 \pi r^{3} / 3\), where \(r\) is its radius. Express the answer in grams per cubic centimeter. The density of aluminum is found experimentally to be \(2.70 \mathrm{~g} / \mathrm{cm}^{3} .\) What does that suggest about the packing of aluminum atoms in the metal?

Mercury(II) oxide, a red powder, can be decomposed by heating to produce liquid mercury and oxygen gas. When a sample of this compound is decomposed, \(3.87 \mathrm{~g}\) of oxygen and \(48.43 \mathrm{~g}\) of mercury are produced. \(\operatorname{In}\) a second experiment, \(15.68 \mathrm{~g}\) of mercury is allowed to react with an excess of oxygen and \(16.93 \mathrm{~g}\) of red mercury(II) oxide is produced. Show that these results are consistent with the law of constant composition.
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