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1. A Review of General Chemistry

Molecular Geometry

1. A Review of General Chemistry

Molecular Geometry

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Molecular Geometry Explained.

Molecular Geometry Explained.

Johnny Betancourt

Predict the hybridization and molecular geometry

Predict the hybridization and molecular geometry

Johnny Betancourt

Practice this topic

Multiple Choice

Determine the hybridization of the following selected atoms:

Multiple Choice

PRACTICE:Determine the hybridization and molecular geometry of the following selected atoms:

Multiple Choice

Which atom in the following structure has trigonal planar geometry?

Textbook Question

In pent-2-yne (CH3CCCH2CH3), there are four atoms in a straight line. Use dashed lines and wedges to draw a three-dimensional representation of this molecule, and circle the four atoms that are in a straight line.

Textbook Question

For each of the following compounds, 1. Give the hybridization and approximate bond angles around each atom except hydrogen. 2. Draw a three-dimensional diagram, including any lone pairs of electrons. d. (CH3)3N e. [CH3NH3]+ f. CH3COOH

Textbook Question

Predict the hybridization, geometry, and bond angles for the central atoms in CH3CH=NH

Textbook Question

Predict the hybridization, geometry, and bond angles for the central atoms in but-2-ene, CH3CH=CHCH

Textbook Question

a. Which of the species have bond angles of 109.5°? b. Which of the species have bond angles of 120°? H2O H3O+ +CH3 BF3

Textbook Question

Do the sp2 carbons and the indicated sp3 carbons lie in the same plane?

Textbook Question

For each of the following molecules, indicate the hybridization of each carbon and give the approximate values of all the bond angles: a. CH3C≡CH

Textbook Question

Predict the hybridization and geometry of the carbon and nitrogen atoms in the following molecules and ions. (Hint: Resonance.) a. [CH3C(=O)CH2]-

b. [H2NCH=CHCH2]+

Textbook Question

In most amines, the nitrogen atom is sp3 hybridized, with a pyramidal structure and bond angles close to 109°. In urea, both nitrogen atoms are found to be planar, with bond angles close to 120°. Explain this surprising finding. (Hint: Consider resonance forms and the overlap needed in them.) [

Textbook Question

Predict the hybridization, geometry, and bond angles for the carbon and nitrogen atoms in acetonitrile ([CH3C=N]^2-)

Textbook Question

Describe the orbitals used in bonding and the bond angles in the following compounds: e. BF3

Textbook Question

Predict the approximate bond angles in a. the methyl cation. b. the methyl radical. c. the methyl anion.

Textbook Question

Predict the approximate bond angles for the following: c. the C—C—N bond angle in CH3C≡N d. the C—C—N bond angle in CH3CH2NH2

Textbook Question

Circle the coplanar atoms in the following structure:

Textbook Question

For each of the following compounds and ions, 1. Draw a Lewis structure. 2. Show the kinds of orbitals that overlap to form each bond. 3. Give approximate bond angles around each atom except hydrogen. c. CH2=NCH3

Textbook Question

For each of the following compounds and ions, 1. Draw a Lewis structure. 2. Show the kinds of orbitals that overlap to form each bond. 3. Give approximate bond angles around each atom except hydrogen. b. [CH2OH]+

Textbook Question

You drew the Lewis structures of the following compounds and ion in Assessment 2.32. Predict their shapes around the central atom based on the Lewis structure. (d) CO²⁻/₃

Textbook Question

Predict the approximate size of the following bond angles. (Hint: See Sections 1.11 and 1.12.) (b) the C—N—C bond angle in a secondary amine

Textbook Question

You drew the Lewis structures of the following compounds and ion in Assessment 2.32. Predict their shapes around the central atom based on the Lewis structure.

(c) HCO₂H

Textbook Question

Describe the orbitals used in bonding and the bond angles in the following compounds:

a. CH₃O^-

Textbook Question

What is the hybridization of all the atoms (other than hydrogen) in each of the following?

What are the bond angles around each atom?

c. ^-CH₃

d. ⋅CH₃

Textbook Question

For each of the following molecules, indicate the hybridization of each carbon and give the approximate values of all the bond angles:

b. CH3CH═CH2

Textbook Question

a. Which of the species have bond angles of 109.5°?

b. Which of the species have bond angles of 120°?

NH₃ ⁺NH₄ ^-CH₃

Textbook Question

Predict the approximate size of the following bond angles. (Hint: See Sections 1.11 and 1.12.)

(a) the C—O—C bond angle in an ether

Textbook Question

Predict the approximate size of the following bond angles. (Hint: See Sections 1.11 and 1.12.)

(d) the C—N—C bond angle in a quaternary ammonium salt

Textbook Question

Describe the orbitals used in bonding and the bond angles in the following compounds:

c. H2CO

Textbook Question

Describe the orbitals used in bonding and the bond angles in the following compounds:

d. N2

Textbook Question

Predict the approximate bond angles for

c. the H—C—N bond angle in (CH3)2NH.

d. the H—C—O bond angle in CH3OCH3

Textbook Question

Predict the approximate bond angles:

c. the C—N—H bond angle in (CH3)2NH

d. the C—N—C bond angle in (CH3)2NH

Textbook Question

Use your molecular models to make ethane, and compare the model with the preceding structures.

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Textbook Question

For each of the following compounds and ions, 1. Draw a Lewis structure. 2. Show the kinds of orbitals that overlap to form each bond. 3. Give approximate bond angles around each atom except hydrogen. a. [NH2]-

Textbook Question

For each of the given species: a. Draw its Lewis structure. b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles. 3. CCl4

Textbook Question

Predict the hybridization of the oxygen atom in water, H2O. Draw a picture of its three-dimensional structure, and explain why its bond angle is 104.5°

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