(a)
Interpretation:
The hybrid-orbital picture for the water molecule using oxygen
Concept introduction:
A new set of orbitals formed from the combination of the atomic orbitals is known as hybrid orbitals. The hybrid orbitals are obtained due to the mixing of atomic orbitals with different azimuthal quantum numbers. The hybrid orbitals have the property of directionality that is the electron density in the hybrid orbitals is directional.
(b)
Interpretation:
The departures from tetrahedral geometry that might be expected from the presence of two unshared electron pairs are to be explained.
Concept introduction:
A new set of orbitals formed from the combination of the atomic orbitals is known as hybrid orbitals. The hybrid orbitals are obtained due to the mixing of atomic orbitals with different azimuthal quantum numbers. The hybrid orbitals have the property of directionality that is the electron density in the hybrid orbitals is directional.
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Organic Chemistry
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- . Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?arrow_forwardFor each of the following molecule: (i) draw the correct Lewis structure; (ii) determine the molecular geometry and the type of hybridization on the central atom, and (iii) predict whether the molecule is polar or nonpolar. (a) BrCl5arrow_forward7. Nitrogen is the central atom in each of the species given. (a) Draw the Lewis electron-dot structure for each of the species. + NO₂ NO₂ NO₂ (b) List the species in order of increasing bond angle. Justify your answer. (c) For NO₂ and NO₂, give the hybridization of the nitrogen atom in it. (d) Identify the only one of the species that dimerizes and explain what causes it to do so.arrow_forward
- Nitrogen trifluoride (NF3) is used in the electronics industry to clean surfaces. NF3 is also a potent greenhouse gas. (A) Draw the Lewis structure of NF3 and determine its molecular geometry. (B) BF3 and NF3 both have three covalently bonded fluorine atoms around a central atom. Do they have the same dipole moment? (C) Could BF3 also behave as a greenhouse gas? Explain why or why not.arrow_forwardFor each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. [b] The greater the orbital overlap in a bond, the shorter the bond. [c] To create a hybrid orbital, you could use the s orbital on one atom with a p orbital on another atom. [d] Nonbonding electron pairs cannot occupy a hybrid orbital.arrow_forwardThe lactic acid molecule, CH3CH(OH)COOH, gives sourmilk its unpleasant, sour taste. (a) Draw the Lewis structurefor the molecule, assuming that carbon always forms fourbonds in its stable compounds. (b) How many π and howmany σ bonds are in the molecule? (c) Which CO bond isshortest in the molecule? (d) What is the hybridization ofatomic orbitals around the carbon atom associated withthat short bond? (e) What are the approximate bond anglesaround each carbon atom in the molecule?arrow_forward
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