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Chapter 3: Problem 98

Use formal charge arguments to explain why CO has a less polar bond than expected on the basis of electronegativity.

Short Answer

Expert verified
The carbon-oxygen bond in CO is less polar than expected based on electronegativity values due to the formal charges of -1 on carbon and +1 on oxygen, which are opposite to what we would expect. These formal charges result in electrons being shared more equally across both atoms, making the bond less polar. Additionally, the presence of a coordinate covalent bond contributes to the equal sharing of electrons between carbon and oxygen atoms.

Step by step solution

01

Definition of Electronegativity and Polar Bonds

Electronegativity is the ability of an atom to attract electrons towards itself in a chemical bond. The greater the difference in electronegativity between two elements, the more polar the bond is. A polar bond occurs when an atom with a higher electronegativity attracts electrons more than the other atom in the bond, creating a partial negative charge (δ-) on the more electronegative atom and a partial positive charge (δ+) on the less electronegative atom.
02

Electronegativity Values for Carbon and Oxygen

Carbon (C) has an electronegativity value of 2.55, while oxygen (O) has an electronegativity value of 3.44. They have an electronegativity difference of 3.44 - 2.55 = 0.89.
03

Coordinate Covalent Bond in Carbon Monoxide (CO)

In carbon monoxide, there is a triple bond between the carbon and oxygen atoms, with one sigma bond and two pi bonds (C≡O). A coordinate covalent bond forms when the bonding electrons are provided by one atom, also known as a dative bond. In CO, the carbon atom shares a pair of its electrons with the oxygen atom, forming a coordinate covalent bond.
04

Formal Charges on Carbon and Oxygen

To understand the less polar bond in CO, we need to consider the formal charges on carbon and oxygen atoms: 1. Formal Charge of Carbon \( (FC_C) = \) (Number of Valence Electrons in a Free Carbon Atom) - (Number of Non-bonding Electrons on Carbon) - (1/2)(Number of Bonding Electrons with Carbon) \( FC_C = 4 - 0 - (1/2)(10) = -1\) 2. Formal Charge of Oxygen \( (FC_O) = \) (Number of Valence Electrons in a Free Oxygen Atom) - (Number of Non-bonding Electrons on Oxygen) - (1/2)(Number of Bonding Electrons with Oxygen) \( FC_O = 6 - 4 - (1/2)(10) = +1\) The formal charge of carbon is -1, and the formal charge of oxygen is +1.
05

Formal Charges and Polarity in CO

Due to the formal charges of -1 on carbon and +1 on oxygen, the charges are opposite from what we expected based on the electronegativity values. It results in the electrons in the bond being shared more equally across both atoms, making the bond less polar than expected. The presence of the coordinate covalent bond also contributes to the equal sharing of electrons between carbon and oxygen atoms.

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Most popular questions from this chapter

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form in ionic compounds. a. 13 b. 34 c. 56 d. 7 e. 87 f. 35

Borazine \(\left(B_{3} N_{3} H_{6}\right)\) has often been called "inorganic" benzene. Write Lewis structures for borazine. Borazine contains a sixmembered ring of alternating boron and nitrogen atoms with one hydrogen bonded to each boron and nitrogen.

By analogy with phosphorus compounds, name the following: \(\mathrm{Na}_{3} \mathrm{AsO}_{4}, \mathrm{H}_{3} \mathrm{AsO}_{4}, \mathrm{Mg}_{3}\left(\mathrm{SbO}_{4}\right)_{2}\)

Which of the following ions have noble gas electron configurations? a. \(\mathrm{Fe}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Sc}^{3+}, \mathrm{Co}^{3+}\) b. \(\mathrm{Tl}^{+}, \mathrm{Te}^{2-}, \mathrm{Cr}^{3+}\) c. \(\mathrm{Pu}^{4+}, \mathrm{Ce}^{4+}, \mathrm{Ti}^{4+}\) d. \(\mathrm{Ba}^{2+}, \mathrm{Pt}^{2+}, \mathrm{Mn}^{2+}\)

Hydrogen has an electronegativity value between boron and carbon and identical to phosphorus. With this in mind, rank the following bonds in order of decreasing polarity: \(\mathrm{P}-\mathrm{H}\) \(\mathbf{O}-\mathbf{H}, \mathbf{N}-\mathbf{H}, \mathbf{F}-\mathbf{H}, \mathbf{C}-\mathbf{H}\)
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