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Chapter 8: Problem 95

Consider the hypothetical molecule \(\mathrm{A}-\mathrm{A}=\mathrm{A}\) with a bent shape. Are the following statements true or false? (a) This molecule cannot exist. (b) If this molecule exists, it must possess an odd electron.

Short Answer

Expert verified
In conclusion, for the hypothetical molecule A-A=A with a bent shape, the two statements are: (a) This molecule cannot exist: False. (b) If this molecule exists, it must possess an odd electron: True.

Step by step solution

01

The hypothetical molecule has a bent structure and is written as A-A=A. To better understand the molecule, we need to determine the type of bonds and the number of valence electrons involved for each atom in the molecule. #Step 2: Examine bonding and valence electrons#

For the A-A single bond, each A atom would contribute 1 valence electron resulting in a shared pair of electrons. Similarly, for the A=A double bond, each A atom would contribute 2 valence electrons, resulting in two shared pairs of electrons. In total, each A atom would need to share X, Y, and Z valence electrons: - X: Valence electrons for the A-A single bond - Y: Valence electrons for the A=A double bond - Z: Valence electrons for the bent shape #Step 3: Analyze the valence electron count#
02

According to the octet rule, an atom should have 8 valence electrons to achieve stability. In this hypothetical molecule, we can write the following equation for an A atom participating in both bonding and bent shape electron pairs: X+Y+Z = 8 Since X is the valence electron for the A-A single bond, it is equal to 1. Y is the valence electron for A=A double bond, which is equal to 2. The equation now becomes: 1+2+Z = 8 Solve for Z: Z = 5 #Step 4: Determine the validity of both statements#

Now that we have the valence electron count for this hypothetical molecule, let's examine both statements: (a) This molecule cannot exist: - There is no specific rule that states molecules with a valence electron arrangement like this cannot exist. Therefore, we cannot definitively say that this molecule cannot exist. So, this statement is False. (b) If this molecule exists, it must possess an odd electron: - The valence electron count Z for an 'A' atom in this hypothetical molecule is 5, which is an odd number. Therefore, if this molecule exists, it must possess an odd electron. So, this statement is True. In conclusion, the first statement is False, and the second statement is True.

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Most popular questions from this chapter

Write Lewis structures for the following: (a) \(\mathrm{H}_{2} \mathrm{CO}\) (both \(\mathrm{H}\) atoms are bonded to $\mathrm{C} \mathrm{)},(\mathbf{b}) \mathrm{H}_{2} \mathrm{O}_{2},(\mathbf{c}) \mathrm{C}_{2} \mathrm{~F}_{6}($ contains a \(\mathrm{C}-\mathrm{C}\) bond $),(\mathbf{d}) \mathrm{AsO}_{3}^{3-},(\mathbf{e}) \mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{H}$ is bonded to \(\mathrm{O})\) (f) \(\mathrm{NH}_{2} \mathrm{Cl}\).

(a) What is the trend in electronegativity going from left to right in a row of the periodic table? (b) How do electronegativity values generally vary going down a column in the periodic table? (c) True or false: The most easily ionizable elements are the most electronegative.

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

A new compound is made that has a \(\mathrm{C}-\mathrm{N}\) bond length of $118 \mathrm{pm}$. Is this bond likely to be a single, double, or triple C-N bond?

Which of these elements are unlikely to form ionic bonds? $\mathrm{Mg}, \mathrm{Al}, \mathrm{Si}, \mathrm{Br}, \mathrm{I}$.
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