HYBRIDIZATIONREVIEWWORKSH

HYBRIDIZATION REVIEW WORKSHEET

1. What is the number of sigma (s) and pi (p) bonds and the hybridization of the carbon atom in

-

Sigma Pi Hybridization

A. 4 1 sp²

B. 4 1 sp³

C. 3 2 sp³

D. 3 1 sp²

2. What is the best description of the carbon-oxygen bond lengths in ?

A. One short and two long bonds

B. One long and two short bonds

C. Three bonds of the same length

D. Three bonds of different lengths

3. Which allotropes contain carbon atoms with sp² hybridization?

I. Diamond

II. Graphite

III. C₆₀ fullerene

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

4. Which of the following species is (are) planar (has (have) all the atoms in one plane)?

I.

II.

III.

A. I only C. I and II only

B. II only D. II and III only

5. What is the molecular shape and the hybridization of the nitrogen atom in NH₃?

Molecular shape Hybridization

A. tetrahedral sp³

B. trigonal planar sp²

C. trigonal pyramidal sp²

D. trigonal pyramidal sp³

6. Which statement about sigma and pi bonds is correct?

A. Sigma bonds are formed only by s orbitals and pi bonds are formed only by p orbitals.

B. Sigma bonds are formed only by p orbitals and pi bonds are formed only by s orbitals.

C. Sigma bonds are formed by either s or p orbitals, pi bonds are formed only by p orbitals.

D. Sigma and pi bonds are formed by either s or p orbitals.

7. NO is trigonal planar and NH₃ is trigonal pyramidal. What is the type of hybridization of N in each of these species?

N in NO N in NH₃

A. sp² sp³

B. sp² sp²

C. Sp³ sp²

D. sp³ sp³

8. In ethanol, C₂H₅OH (l), there are covalent bonds, hydrogen bonds and van der Waals?? forces. Which bonds or forces are broken when ethanol is vaporized?

A. only hydrogen bonds

B. covalent bonds and hydrogen bonds

C. covalent bonds and van der Waals?? forces

D. hydrogen bonds and van der Waals?? forces

9. Which statement best describes the attraction present in metallic bonding?

A. the attraction between nuclei and electrons

B. the attraction between positive ions and electrons

C. the attraction between positive ions and negative ions

D. the attraction between protons and electrons

10. Which statement is correct about multiple bonding between carbon atoms?

A. Double bonds are formed by two ?? bonds.

B. Double bonds are weaker than single bonds.

C. ?? bonds are formed by overlap between s orbitals.

D. ?? bonds are weaker than sigma bonds.

Short Answers:

1. (i) List the following substances in order of increasing boiling point (lowest first).

CH₃CHO C₂H₆ CH₃COOH C₂H₅OH

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(2)

(ii) State whether each compound is polar or non-polar, and explain the order of boiling points in (c)(i).

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(8)

2. Atomic orbitals can mix by hybridization to form new orbitals for bonding.

Identify the type of hybridization present in each of the three following molecules.
Deduce and explain their shapes.

(i) OF₂

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(3)

(ii) H₂CO

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(3)

(iii) C₂H₂

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(3)

3. (i) Use the VSEPR theory to predict and explain the shape and the bond angle of each of the molecules SCl₂ and C₂Cl₂

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(ii) Deduce whether or not each molecule is polar, giving a reason for your answer.

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(3)

4. (i) Explain the meaning of the term hybridization.

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..................................................................................................................................... (1)

(ii) Discuss the bonding in the molecule CH₃CHCH₂with reference to

· the formation of ?? and ?? bonds

· the length and strength of the carbon-carbon bonds

· the types of hybridization shown by the carbon atoms

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(6)

5. The boiling points of the hydrides of group 6 elements increase in the order

H₂S < H₂Se < H₂Te < H₂O.

Explain the trend in the boiling points in terms of bonding.

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................................................................................................................................................  (6)

Answers:

1) A 2) C 3) C 4) C 5) D 6) C 7) A 8) D

9) B 10) D

      Short Answers:

1) Lowest    Highest

     Ethane             Ethanone           Ethanol            Ethanoic acid

Van der Waals     dipole-dipole     H-bonding H-bonding

                                                                                 with larger mass - therefore, greater Van der Waal??s

2) i) bent  ii) trigonal planar  iii) planar

SCl₂; bent (107⁰) - polar

      C₂Cl₂: planar (180⁰) - non-polar

5) As size increases down Family 16, the electronegativity decreases. As a result, the H-bonding progressively weakens, making for easier breaking of the intermolecular forces.

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	Sigma	Pi	Hybridization
A.	4	1	sp²
B.	4	1	sp³
C.	3	2	sp³
D.	3	1	sp²

	Molecular shape	Hybridization
A.	tetrahedral	sp³
B.	trigonal planar	sp²
C.	trigonal pyramidal	sp²
D.	trigonal pyramidal	sp³

	N in NO	N in NH₃
A.	sp²	sp³
B.	sp²	sp²
C.	Sp³	sp²
D.	sp³	sp³