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1. A Review of General Chemistry

Hybridization

1. A Review of General Chemistry

Hybridization

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How carbon creates 4 partially-filled orbitals.

How carbon creates 4 partially-filled orbitals.

Johnny Betancourt

How carbon makes 4 sp3 orbitals.

How carbon makes 4 sp3 orbitals.

Johnny Betancourt

Using bond sites to predict hybridization

Using bond sites to predict hybridization

Johnny Betancourt

Introduction to the reactive intermediates.

Introduction to the reactive intermediates.

Johnny Betancourt

Bond sites, hybridization, and intermediate orbitals

Bond sites, hybridization, and intermediate orbitals

Johnny Betancourt

Showing 5 of 5 videos

Practice this topic

Multiple Choice

What kind of atom is sp hybridized?

Multiple Choice

What is the hybridization of the nitrogen atom in acetamide:

Multiple Choice

What is the hybridization of the indicated oxygen atom?

Multiple Choice

What is the hybridization of the indicated nitrogen atom?

Multiple Choice

What is the hybridization of the nitrogen atom in the following molecule?

Textbook Question

What is the hybridization of the indicated atom in each of the following? d.

Textbook Question

What is the hybridization of the indicated atom in each of the following? a.

Textbook Question

b. What is the hybridization of each of the C, N, and O atoms in the following compounds:

Textbook Question

Put a number in each of the blanks: a. ___ s orbital and ___ p orbitals form ____ sp3 orbitals. b. ___ s orbital and ___ p orbitals form ____ sp2 orbitals. c. ___ s orbital and ___ p orbitals form ____ sp orbitals.

Textbook Question

For each of the following molecules, indicate the hybridization of each carbon and give the approximate values of all the bond angles: d. CH2═CH—CH═CH2

Textbook Question

In which orbitals are the lone pairs in nicotine?

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Textbook Question

Assessments 2.69–2.73 and 2.76 refer to the following Lewis structures. (e)

(••) Predict the hybridization of all non-hydrogen atoms.

Textbook Question

Assessments 2.69–2.73 and 2.76 refer to the following Lewis structures. (c)

(••) Predict the hybridization of all non-hydrogen atoms.

Textbook Question

Assign the hybridization of the nitrogen in each resonance structure of acetamide.

Textbook Question

(••) Connect the atoms using the indicated hybrid orbitals. (b) C (sp²) with C (sp²)

Textbook Question

Assessments 2.69–2.73 and 2.76 refer to the following Lewis structures. (a) (b) (••) Predict the hybridization of all non-hydrogen atoms.

Textbook Question

Assessments 2.69–2.73 and 2.76 refer to the following Lewis structures. (a) (b) (••) If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?

Textbook Question

Assessments 2.69–2.73 and 2.76 refer to the following Lewis structures. (c) (d) (••) If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?

Textbook Question

Hydrogen forms bonds without hybridizing. Why?

Textbook Question

(••••) The C―H σ bond length in ethane is 1.09 Å. The C―H σ bond in ethene is 1.07 Å. Explain. [See Assessment 2.70.]

<IMAGE> <IMAGE>

ethane ethene

Textbook Question

(••••) In propene, the indicated C―C bond length is 1.51 Å. In the allyl cation, the indicated C―C bond length is 1.41 Å. Explain. [See Assessment 2.68.]

<IMAGE> <IMAGE>

propene allyl cation

Textbook Question

What is the hybridization of carbon in each of the following molecules? (a)

Textbook Question

What is the hybridization of carbon in each of the following molecules? (d)

Textbook Question

Draw the molecular orbital picture for propane. Your picture should clearly show the shape and hybridization of the carbons. Label all σ bonds.

Textbook Question

Predict the shape and hybridization of the indicated atoms.

Textbook Question

What orbitals are used to form the carbon–carbon s bond between the highlighted carbons? g.

Textbook Question

What orbitals contain the electrons represented as lone pairs in the structures of quinoline, indole, imidazole?

Textbook Question

What orbital do the lone-pair electrons occupy in each of the following compounds? a.

Textbook Question

(••••) In addition to radicals, anions, and cations, a fourth class of reactive intermediates is carbenes. A neutral species, the simplest carbene has a molecular formula of CH₂ . (b) What are the hybridization and shape of the central carbon of CH₂ ?

Textbook Question

Predict the hybridization of the indicated atoms. (b)

Textbook Question

(••) For the following partial structures, the bond is shown. Add the indicated number of bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.

(a) <IMAGE> ( 2 π bond)

Textbook Question

Rank C―H σ the following bonds in terms of their bond length. Explain your ranking ( 1= longest ; 3 = shortest).

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Textbook Question

What orbitals are used to form the carbon–carbon s bond between the highlighted carbons?

a. <IMAGE>

b. <IMAGE>

c. <IMAGE>

Textbook Question

Predict the hybridization and geometry of the carbon and nitrogen atoms in the following molecules and ions. (Hint: Resonance.)

d. <IMAGE>

Textbook Question

Predict the hybridization and geometry of the carbon and nitrogen atoms in the following molecules and ions. (Hint: Resonance.)

f. <IMAGE>

Textbook Question

Predict the hybridization and geometry of the carbon and nitrogen atoms in the following molecules and ions. (Hint: Resonance.)

e. <IMAGE>

Textbook Question

What orbitals contain the electrons represented as lone pairs in the structures of purine, and pyrimidine?

Textbook Question

Use hybrid orbitals to draw the following molecules. (a)

Textbook Question

Use hybrid orbitals to draw the following molecules. (b)

Textbook Question

Use hybrid orbitals to draw the following molecules. (c)

Textbook Question

Use hybrid orbitals to draw the following molecules. (d)

Textbook Question

Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (b) BH₃

Textbook Question

Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (c) AlCl₃

Textbook Question

Explain why a σ bond formed by overlap of an s orbital with an sp3 orbital of carbon is stronger than a σ bond formed by overlap of an s orbital with a p orbital of carbon.

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?

i. H3O+

j. H2C═O

Showing 45 of 45 practice