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Chapter 8: Problem 72

State whether each of these statements is true or false. (a) A carbon-carbon triple bond is shorter than a carbon-carbon single bond. (b) There are exactly six bonding electrons in the \(\mathrm{O}_{2}\) molecule. (c) The \(\mathrm{C}-\mathrm{O}\) bond in carbon monoxide is longer than the \(\mathrm{C}-\mathrm{O}\) bond in carbon dioxide. (d) The O \(-\mathrm{O}\) bond in ozone is shorter than the \(\mathrm{O}-\) O bond in \(\mathrm{O}_{2}\) . (e) The more electronegative the atom, the more bonds it makes to other atoms.

Short Answer

Expert verified
(a) True. (b) True. (c) False. (d) True. (e) False.

Step by step solution

01

Statement a: A carbon-carbon triple bond is shorter than a carbon-carbon single bond.

This statement is true. In general, as the number of bonds between two atoms increases, the bond length decreases because the atoms are held more closely together by the increasing attractive forces between the positively charged nuclei and the negatively charged electrons.
02

Statement b: There are exactly six bonding electrons in the O2 molecule.

This statement is true. In O2, oxygen has a double bond which involves four electrons in two σ (sigma) bonds, and two electrons in one π (pi) bond. Therefore, there are a total of six bonding electrons in the O2 molecule.
03

Statement c: The C-O bond in carbon monoxide is longer than the C-O bond in carbon dioxide.

This statement is false. In carbon monoxide (CO), there is a triple bond between the C and O atoms, while in carbon dioxide (CO2), the C atom forms two double bonds with two O atoms. Because a triple bond is stronger and shorter than a double bond, the C-O bond in carbon monoxide is shorter than the C-O bond in carbon dioxide.
04

Statement d: The O-O bond in ozone is shorter than the O-O bond in O2.

This statement is true. In ozone (O3), there are three oxygen atoms forming a resonance structure, which results in a bond order of 1.5 (halfway between a single and double bond). In O2, there is a double bond between the two oxygen atoms. Since bond length decreases as bond order increases, the O-O bond in ozone is shorter than the O-O bond in O2.
05

Statement e: The more electronegative the atom, the more bonds it makes to other atoms.

This statement is generally false. Electronegativity is the ability of an atom to attract electrons towards itself, and highly electronegative atoms tend to form strong bonds with fewer atoms. For example, fluorine is the most electronegative element, but it forms only one bond with other atoms. However, one must also consider that molecular structure and other factors can also influence the number of bonds formed by atoms.

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Most popular questions from this chapter

Which of the following statements about electronegativity is false? (a) Electronegativity is the ability of an atom in a molecule to attract electron density toward itself. (b) Electronegativity is the same thing as electron affinity. (c) The numerical values for electronegativity have no units. (d) Fluorine is the most electronegative element. (e) Cesium is the least electronegative element.

Write Lewis structures that obey the octet rule for each of the following, and assign oxidation numbers and formal charges to each atom: (a) OCS, (b) SOCl_ \(_{2}(S\) is the central atom), \((\mathbf{c}) \mathrm{BrO}_{3}^{-},(\mathbf{d}) \mathrm{HClO}_{2}(\mathrm{H}\) is bonded to O)

Write the electron configuration for each of the following ions, and determine which ones possess noble-gas configurations: (a) \(\mathrm{Sr}^{2+},(\mathbf{b}) \mathrm{Ti}^{2+},(\mathbf{c}) \mathrm{Se}^{2-},(\mathbf{d}) \mathrm{Ni}^{2+},(\mathbf{e}) \mathrm{Br}^{-}\) \((\mathbf{f}) \mathrm{Mn}^{3+}\)

Consider the formate ion, \(\mathrm{HCO}_{2}^{-},\) which is the anion formed when formic acid loses an \(\mathrm{H}^{+}\) ton. The \(\mathrm{H}\) and the two O atoms are bonded to the central \(\mathrm{C}\) atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? (c) Would you predict that the \(\mathrm{C}-\mathrm{O}\) bond lengths in the formate ion would be longer or shorter relative to those in \(\mathrm{CO}_{2} ?\)

(a) True or false: An element's number of valence electrons is the same as its atomic number. (b) How many valence electrons does a nitrogen atom possess? (c) An atom has the electron configuration 1\(s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}\) . How many valence electrons does the atom have?
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