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Chapter 8: Problem 85

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?

Short Answer

Expert verified
(a) The most polar single bond would form between B (Boron) and O (Oxygen) as they have the highest difference in electronegativity (1.4). (b) The longest single bond would form between As (Arsenic) and I (Iodine), with a total atomic size of 254 pm. (c) Boron (B) would be likely to form a compound of the formula XY3, as it has 3 valence electrons. (d) Oxygen (O) is the element most likely to participate in two covalent bonds, as it has 6 valence electrons, and hence has two lone pairs of electrons available for sharing in covalent bonds.

Step by step solution

01

Determine electronegativity values

First, we need to find the electronegativity values for B, As, O, and I. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. We can use a periodic table or electronegativity chart to find these values. Here they are: - B (Boron): 2.04 - As (Arsenic): 2.18 - O (Oxygen): 3.44 - I (Iodine): 2.66
02

Determine atomic sizes

Next, we'll determine the atomic sizes of the given elements by looking at their atomic radius. The atomic size generally decreases as we move across a period and increases as we go down a group in the periodic table: - B (Boron): 87 pm (picometers) - As (Arsenic): 114 pm - O (Oxygen): 66 pm - I (Iodine): 140 pm
03

(a) Most polar single bond

In order to determine which two elements would form the most polar single bond, we need to find the pair with the highest difference in electronegativity. The higher the difference, the more polar the bond will be: 1. B-O: \(|2.04 - 3.44| = 1.4\) 2. B-I: \(|2.04 - 2.66| = 0.62\) 3. As-O: \(|2.18 - 3.44| = 1.26\) 4. As-I: \(|2.18 - 2.66| = 0.48\) The highest difference is between Boron (B) and Oxygen (O), with a difference of 1.4. Answer: (a) The most polar single bond would form between B and O.
04

(b) Longest single bond

To find which two elements would form the longest single bond, we should look for the pair with the largest atomic sizes: 1. B-As: \(87 + 114 = 201\) pm 2. B-I: \(87 + 140 = 227\) pm 3. As-O: \(114 + 66 = 180\) pm 4. As-I: \(114 + 140 = 254\) pm The largest sum of atomic radii is between As (Arsenic) and I (Iodine), with a total of 254 pm. Answer: (b) The longest single bond would form between As and I.
05

(c) Compound of formula XY3

In order to determine which element is most likely to form a compound with the formula XY\(_3\), it's essential to consider their valence electrons and group in the periodic table: - B (Boron): Group 13, 3 valence electrons - As (Arsenic): Group 15, 5 valence electrons - O (Oxygen): Group 16, 6 valence electrons - I (Iodine): Group 17, 7 valence electrons Boron (B) has 3 valence electrons, which means it can form three bonds with other elements to achieve a stable electron configuration. Answer: (c) Boron (B) would be likely to form a compound of the formula XY3.
06

(d) Element likely to participate in two covalent bonds

To find the element most likely to participate in two covalent bonds, we need to identify which element can share two of its valence electrons: - B (Boron): 3 valence electrons - As (Arsenic): 5 valence electrons - O (Oxygen): 6 valence electrons - I (Iodine): 7 valence electrons Oxygen (O) has 6 valence electrons, which means it has two lone pairs of electrons available for sharing in covalent bonds. Answer: (d) Oxygen (O) is the element most likely to participate in two covalent bonds.

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Most popular questions from this chapter

A classmate of yours is convinced that he knows everything about electronegativity. (a) In the case of atoms X and Y having different electronegativities, he says, the diatomic molecule \(X-Y\) must be polar. Is your classmate correct? (b) Your classmate says that the farther the two atoms are apart in a bond, the larger the dipole moment will be. Is your classmate correct?

There are many Lewis structures you could draw for sulfuric acid, \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (each \(\mathrm{H}\) is bonded to an \(\mathrm{O}\) ). (a) What Lewis structure(s) would you draw to satisfy the octet rule? (b) What Lewis structure(s) would you draw to minimize formal charge?

(a) Which of these compounds is an exception to the octet rule: carbon dioxide, water, ammonia, phosphorus trifluoride, or arsenic pentafluoride? (b) Which of these compounds or ions is an exception to the octet rule: borohydride \(\left(\mathrm{BH}_{4}^{-}\right),\) borazine $\left(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6},\right.$ which is analogous to benzene with alternating \(\mathrm{B}\) and \(\mathrm{N}\) in the ring \(),\) or boron trichloride?

(a) Is lattice energy usually endothermic or exothermic? (b) Write the chemical equation that represents the process of lattice energy for the case of NaCl. (c) Would you expect salts like \(\mathrm{NaCl}\), which have singly charged ions, to have larger or smaller lattice energies compared to salts like CaO which are composed of doubly-charged ions?

Consider the lattice energies of the following Group \(2 \mathrm{~A}\) compounds: $\mathrm{BeH}_{2}, 3205 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{MgH}_{2}, 2791 \mathrm{~kJ} / \mathrm{mol} ;\( \)\mathrm{CaH}_{2}, 2410 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{SrH}_{2}, 2250 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{BaH}_{2}, 2121 \mathrm{~kJ} / \mathrm{mol}$ (a) What is the oxidation number of H in these compounds? (b) Assuming that all of these compounds have the same three-dimensional arrangement of ions in the solid, which of these compounds has the shortest cation-anion distance? (c) Consider BeH \(_{2}\). Does it require \(3205 \mathrm{~kJ}\) of energy to break one mole of the solid into its ions, or does breaking up one mole of solid into its ions release \(3205 \mathrm{~kJ}\) of energy? (d) The lattice energy of \(\mathrm{ZnH}_{2}\) is \(2870 \mathrm{~kJ} / \mathrm{mol}\). Considering the trend in lattice enthalpies in the Group 2 compounds, predict which Group 2 element is most similar in ionic radius to the \(\mathrm{Zn}^{2+}\) ion.
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