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Chapter 8: Problem 72

State whether each of these statements is true or false. (a) An oxygen-oxygen double bond is shorter than an oxygenoxygen single bond. (b) There are three lone pair electrons in the \(\mathrm{NH}_{3}\) molecule. (c) The \(\mathrm{C}-\mathrm{C}\) bond in ethene is longer than the \(\mathrm{C}-\mathrm{C}\) bond in polyethene. (d) The \(\mathrm{C}-\mathrm{Cl}\) bond is shorter than the \(\mathrm{C}-\mathrm{Br}\) bond. \((\mathbf{e})\) The greater the difference in the electronegativity of atoms in a bond, the stronger the bond.

Short Answer

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

Step by step solution

01

Statement (a) - Oxygen-oxygen double bond and single bond

To determine whether an oxygen-oxygen double bond is shorter than an oxygen-oxygen single bond, we consider the fact that double bonds involve the sharing of more electrons between the bonded atoms. This leads to a higher electron density and stronger electrostatic attraction between the nuclei and the bonding electrons. As a result, double bonds are generally shorter and stronger than single bonds. Hence, the statement (a) is true.
02

Statement (b) - Lone pair electrons in NH3 molecule

The NH3 molecule has one nitrogen atom and three hydrogen atoms. Nitrogen has 5 valence electrons and each hydrogen atom contributes 1 electron. The nitrogen atom forms three single bonds with the three hydrogen atoms, using 3 of its 5 valence electrons. The remaining 2 electrons form a lone pair on the nitrogen atom. This means there is only one lone pair of electrons in the NH3 molecule. Thus, statement (b) is false.
03

Statement (c) - C-C bond in ethene and polyethene

Ethene has a carbon-carbon double bond, while polyethene has carbon-carbon single bonds. As previously discussed, double bonds are generally shorter and stronger than single bonds due to a higher electron density and stronger electrostatic attraction. Therefore, the C-C bond in ethene is shorter than the C-C bond in polyethene. Statement (c) is true.
04

Statement (d) - C-Cl and C-Br bond lengths

The bond length between two atoms is influenced by their atomic size. Generally, as you move down a group in the periodic table, the atomic size increases. Chlorine is above bromine in the periodic table, so it is smaller in size than bromine. As a result, the C-Cl bond is shorter than the C-Br bond. Statement (d) is true.
05

Statement (e) - Bond strength and electronegativity difference

The electronegativity of an atom is its ability to attract electrons in a bond. A bond formed between two atoms with a large electronegativity difference is polar and has a significant amount of ionic character. Such bonds are generally stronger than non-polar bonds. However, this statement is not universally true, as bond strength will also depend on other factors such as the size of the atoms and electron configuration. Therefore, statement (e) is false. In conclusion: - Statement (a) is true - Statement (b) is false - Statement (c) is true - Statement (d) is true - Statement (e) is false

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Most popular questions from this chapter

Consider the collection of nonmetallic elements: \(\mathrm{B}\), As, O, and I. (a) Which two would form the most polar single bond? (b) Which two would form the longest single bond? (c) Which one would be likely to form a compound of formula XY \(_{3} ?(\mathbf{d})\) Which element would likely to participate in two covalent bonds?

In the vapor phase, \(\mathrm{BeCl}_{2}\) exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule? (b) What other resonance structures are possible that satisfy the octet rule? (c) On the basis of the formal charges, which Lewis structure is expected to be dominant for \(\mathrm{BeCl}_{2}\) ?

Which ionic compound is expected to form from combining the following pairs of elements? (a) calcium and nitrogen, (b) cesium and bromine, (c) strontium and sulfur, (d) aluminum and selenium.

Some chemists believe that satisfaction of the octet rule should be the top criterion for choosing the dominant Lewis structure of a molecule or ion. Other chemists believe that achieving the best formal charges should be the top criterion. Consider the dihydrogen phosphate ion, $\mathrm{H}_{2} \mathrm{PO}_{4}^{-},\( in which the \)\mathrm{H}$ atoms are bonded to \(\mathrm{O}\) atoms. (a) What is the predicted dominant Lewis structure if satisfying the octet rule is the top criterion? (b) What is the predicted dominant Lewis structure if achieving the best formal charges is the top criterion?

Using Lewis symbols and Lewis structures, make a sketch of the formation of \(\mathrm{NCl}_{3}\) from \(\mathrm{N}\) and \(\mathrm{Cl}\) atoms, showing valence- shell electrons. (a) How many valence electrons does N have initially? (b) How many bonds Cl has to make in order to achieve an octet? (c) How many valence electrons surround the \(\mathrm{N}\) in the \(\mathrm{NCl}_{3}\) molecule? (d) How many valence electrons surround each Cl in the \(\mathrm{NCl}_{3}\) molecule? (e) How many lone pairs of electrons are in the \(\mathrm{NCl}_{3}\) molecule?
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