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Chapter 8: Problem 85

Consider the collection of nonmetallic elements \(\mathrm{O}, \mathrm{P}\) , Te, \(\mathrm{I},\) and \(\mathrm{B} .\) (a) Which two would form the most polar single bond? (b) Which two would form the longest single bond? (c) Which two would be likely to form a compound of formula \(\mathrm{XY}_{2} ?(\mathbf{d})\) Which combinations of elements would likely yield a compound of empirical formula \(\mathrm{X}_{2} \mathrm{Y}_{3}\) ?

Short Answer

Expert verified
(a) The most polar single bond will be formed between O and B, as they have the highest electronegativity difference. (b) The longest single bond will be formed between I and O, as they have the largest atomic radii. (c) B and O can form a compound with the formula \(BO_2\), as O has a valency of 2, and B has a valency of 3. (d) The possible combinations of elements yielding a compound of empirical formula X2Y3 are B2O3, B2Te3, and B2I3.

Step by step solution

01

Identify the most polar single bond

A polar bond occurs when there is a significant difference in electronegativity between the two atoms in the bond. To find the most polar bond, we need to find the combination of elements with the highest electronegativity difference. (a) Among the given elements, O has the highest electronegativity (\(3.44\)) and B has the lowest electronegativity (\(2.04\)). Therefore, the most polar single bond will be formed between O and B.
02

Identify the longest single bond

The bond length typically increases as the atomic size increases. We need to find the combination of elements with the largest atomic radii. (b) Among the given elements, I has the largest atomic radius (\(140\,pm\)) and O has the smallest atomic radius (\(60\,pm\)). Therefore, the longest single bond will be formed between I and O.
03

Identify which elements will form a compound with the formula XY2

A compound with the formula XY2 will form if one element can accept two electrons from the other element. (c) Among the given elements, O has a valency of 2, which can accept two electrons from an element like B, which has a valency of 3. Therefore, B and O can form a compound with the formula \(BO_2\).
04

Identify the combinations of elements yielding a compound of empirical formula X2Y3

An empirical formula of X2Y3 indicates that two atoms of element X bond with three atoms of element Y. (d) In the given elements, B has a valency of 3 and can form compounds with elements having a valency of 2. Elements with valency 2 in the given list are O, Te, and I. Therefore, there are possible combinations of elements that can yield a compound of empirical formula X2Y3: 1. B2O3 2. B2Te3 3. B2I3

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Most popular questions from this chapter

A common form of elemental phosphorus is the tetrahedral \(\mathrm{P}_{4}\) molecule, where all four phosphorus atoms are equivalent: At room temperature phosphorus is a solid. (a) Are there any lone pairs of electrons in the \(\mathrm{P}_{4}\) molecule? (b) How many \(\mathrm{p}-\mathrm{p}\) bonds are there in the molecule? (c) Draw a Lewis structure for a linear \(P_{4}\) molecule that satisfies the octet rule. Does this molecule have resonance structures? (d) On the basis of formal charges, which is more stable, the linear molecule or the tetrahedral molecule?

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.

Consider the hypothetical molecule \(\mathrm{B}-\mathrm{A}=\mathrm{B}\) . Are the following statements true or false? (a) This molecule cannot exist. (b) If resonance was important, the molecule would have identical \(A-B\) bond lengths.

(a) Draw the best Lewis structure(s) for the nitrite ion, NO \(_{2}^{-}\) (b) With what allotrope of oxygen is it isoelectonic? (c) What would you predict for the lengths of the bonds in \(\mathrm{NO}_{2}^{-}\) relative to \(\mathrm{N}-\mathrm{O}\) single bonds and double bonds?

Ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl},\) is a very soluble salt in water. (a) Draw the Lewis structures of the ammonium and chloride ions. (b) Is there an \(\mathrm{N}-\) Cl bond in solid ammonium chloride? (c) If you dissolve 14 gof ammonium chloride in 500.0 \(\mathrm{mL}\) of water, what is the molar concentration of the solution? (d) How many grams of silver nitrate do you need to add to the solution in part (c) to precipitate all of the chloride as silver chloride?
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