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Ch.9 - Molecular Geometry and Bonding Theories
All textbooksBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 113
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Chapter 9, Problem 113

A compound composed of 6.7% H, 40.0% C, and 53.3% O has a molar mass of approximately 60 g>mol. (c) What is the geometry and hybridization of the C atom that is bonded to 2 O atoms?

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1
Step 1: Determine the empirical formula of the compound. Start by assuming you have 100 g of the compound, which means you have 6.7 g of H, 40.0 g of C, and 53.3 g of O. Convert these masses to moles by dividing by their respective atomic masses: H (1.01 g/mol), C (12.01 g/mol), and O (16.00 g/mol).
Step 2: Calculate the mole ratio of the elements by dividing each element's mole value by the smallest number of moles calculated in Step 1. This will give you the simplest whole number ratio of the elements, which is the empirical formula.
Step 3: Determine the molecular formula. Use the empirical formula mass and compare it to the given molar mass of the compound (60 g/mol). Divide the molar mass by the empirical formula mass to find the multiplier needed to convert the empirical formula to the molecular formula.
Step 4: Identify the structure of the compound. Based on the molecular formula, consider possible structures that include a carbon atom bonded to two oxygen atoms. A common structure is the carboxyl group (-COOH), where the carbon is double-bonded to one oxygen and single-bonded to another oxygen (which is also bonded to hydrogen).
Step 5: Determine the geometry and hybridization of the carbon atom in the carboxyl group. The carbon atom in a carboxyl group is typically sp² hybridized, resulting in a trigonal planar geometry. This is due to the presence of three regions of electron density around the carbon atom (one double bond and two single bonds).
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Textbook Question

The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding π orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the p2p to the p*2p molecular orbital. (a) Assuming this electronic transition corresponds to the HOMO-LUMO transition, what is the HOMO in ethylene?

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Textbook Question

The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding π orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the p2p to the p*2p molecular orbital. (b) Assuming this electronic transition corresponds to the HOMO-LUMO transition, what is the LUMO in ethylene?

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Textbook Question

The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding π orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the p2p to the p*2p molecular orbital. (c) Is the C¬C bond in ethylene stronger or weaker in the excited state than in the ground state? Why?

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Textbook Question

Sulfur tetrafluoride 1SF42 reacts slowly with O2 to form sulfur tetrafluoride monoxide 1OSF42 according to the following unbalanced reaction: SF41g2 + O21g2¡OSF41g2 The O atom and the four F atoms in OSF4 are bonded to a central S atom. (a) Balance the equation.

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Textbook Question

Sulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfur tetrafluoride monoxide (OSF4) according to the following unbalanced reaction: SF4(g) + O2(g) → OSF4(g) The O atom and the four F atoms in OSF4 are bonded to a central S atom. (b) Write a Lewis structure of OSF4 in which the formal charges of all atoms are zero.

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Textbook Question

Sulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfur tetrafluoride monoxide (OSF4) according to the following unbalanced reaction: SF4(g) + O2(g) → OSF4(g) The O atom and the four F atoms in OSF4 are bonded to a central S atom. (c) Use average bond enthalpies (Table 8.3) to estimate the enthalpy of the reaction. Is it endothermic or exothermic?

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