The hybridization of the central atom in NO3- is

A) p3 B) sp2 C) sp3 D) sp E) dsp2 A) p3 B) sp2 C) sp3 D) sp E) dsp2

Explain the concept of delocalization of electrons in SO3.Indicate how this idea relates to resonance.

When we draw the Lewis dot structure for

Draw a molecular orbital diagram for O2 and N2.Using molecular orbital theory,explain why the removal of one electron in O2 strengthens bonding,while the removal of one electron in N2 weakens bonding.

@#IMG-DLM& The bond order for N 2 is 3,b

The hybridization of the central atom in I3- is:

A) sp B) sp2 C) sp3 D) dsp3 E) d2sp3 A) sp B) sp2 C) sp3 D) dsp3 E) d2sp3

When a carbon atom has sp3 hybridization,it has

A) four $\pi$ bonds B) three $\pi$ bonds and one $\sigma$ bond C) two $\pi$ bonds and two $\sigma$ bonds D) one $\pi$ bond and three $\sigma$ bonds E) four $\sigma$ bonds A) four $\pi$ bonds B) three $\pi$ bonds and one $\sigma$ bond C) two $\pi$ bonds and two $\sigma$ bonds D) one $\pi$ bond and three $\sigma$ bonds E) four $\sigma$ bonds

A species has the following MO configuration: ( $\sigma$1s)2( $\sigma$1s*)2( $\sigma$2s)2( $\sigma$2s*)2( $\sigma$2p)2($\pi$2p)2 This substance is

A) paramagnetic with one unpaired electron B) paramagnetic with two unpaired electrons C) paramagnetic with three unpaired electrons D) paramagnetic with four unpaired electrons E) diamagnetic A) paramagnetic with one unpaired electron B) paramagnetic with two unpaired electrons C) paramagnetic with three unpaired electrons D) paramagnetic with four unpaired electrons E) diamagnetic

Exam 9: Covalent Bonding: Orbitals

If a molecule demonstrates paramagnetism,then : I.The substance can have both paired and unpaired electrons. II.The bond order is not a whole number. III.It can be determined by drawing a Lewis structure. IV.It must be an ion.

(Multiple Choice)

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Question 41

The hybridization of the central atom in NO₃^- is

(Multiple Choice)

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Question 42

Which of the nitrogen-containing molecules below is paramagnetic in its lowest energy state?

(Multiple Choice)

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Question 43

Which of the following has the largest bond order?

(Multiple Choice)

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Question 44

Tetracyanoethylene has the skeleton shown below: From its Lewis structure determine the following: -How many of the atoms are sp hybridized?

(Multiple Choice)

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Question 45

Explain the concept of delocalization of electrons in SO₃.Indicate how this idea relates to resonance.

(Essay)

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Question 46

Which of the following statements about the species CN^- is false?

(Multiple Choice)

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Question 47

According to MO theory,F₂ should be diamagnetic.

(True/False)

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Question 48

For how many of the following does the bond order decrease if you add one electron to the neutral molecule? B₂,C₂,P₂,F₂

(Multiple Choice)

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Question 49

Draw a molecular orbital diagram for O₂ and N₂.Using molecular orbital theory,explain why the removal of one electron in O₂ strengthens bonding,while the removal of one electron in N₂ weakens bonding.

(Essay)

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Question 50

As the bond order of a bond increases,the bond energy and the bond length .

(Multiple Choice)

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Question 51

When an electron pair is shared in the area centered on a line joining the atoms,a $\sigma$ (sigma)bond is formed.

(True/False)

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Question 52

Consider the skeletal structure shown below: N-C-C-N Draw the Lewis structure and answer the following: -How many pi bonds does the molecule contain?

(Multiple Choice)

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Question 53

The hybridization of a molecule is measured to determine the shape of the molecule.

(True/False)

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Question 54

The hybridization of the central atom in I₃^- is:

(Multiple Choice)

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Question 55

When a carbon atom has sp³ hybridization,it has

(Multiple Choice)

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Question 56

A species has the following MO configuration: ( $\sigma$ _1s)²( $\sigma$ _1s)²( $\sigma$ _2s)²( $\sigma$ _2s)²( $\sigma$ _2p)²( $\pi$ _2p)² This substance is

(Multiple Choice)

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Question 57

Consider the molecule and the following hybridization choices: -What is the hybridization of the nitrogen atom?

(Multiple Choice)

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Question 58

For which of the following diatomic molecules would the bond order become greater if an electron is removed (i.e. ,if the molecule is converted to the positive ion in its ground state)?

(Multiple Choice)

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Question 59

__________ is the difference between the number of bonding electrons and the number of antibonding electrons divided by two.

(Short Answer)

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Question 60

Showing 41 - 60 of 101

Exam 9: Covalent Bonding: Orbitals

If a molecule demonstrates paramagnetism,then : I.The substance can have both paired and unpaired electrons. II.The bond order is not a whole number. III.It can be determined by drawing a Lewis structure. IV.It must be an ion.

The hybridization of the central atom in NO3- is

Which of the nitrogen-containing molecules below is paramagnetic in its lowest energy state?

Which of the following has the largest bond order?

Tetracyanoethylene has the skeleton shown below: From its Lewis structure determine the following: -How many of the atoms are sp hybridized?

Explain the concept of delocalization of electrons in SO3.Indicate how this idea relates to resonance.

Which of the following statements about the species CN- is false?

According to MO theory,F2 should be diamagnetic.

For how many of the following does the bond order decrease if you add one electron to the neutral molecule? B2,C2,P2,F2

Draw a molecular orbital diagram for O2 and N2.Using molecular orbital theory,explain why the removal of one electron in O2 strengthens bonding,while the removal of one electron in N2 weakens bonding.

As the bond order of a bond increases,the bond energy ______ and the bond length ______.

When an electron pair is shared in the area centered on a line joining the atoms,a σ\sigmaσ (sigma)bond is formed.

Consider the skeletal structure shown below: N-C-C-N Draw the Lewis structure and answer the following: -How many pi bonds does the molecule contain?

The hybridization of a molecule is measured to determine the shape of the molecule.

The hybridization of the central atom in I3- is:

When a carbon atom has sp3 hybridization,it has

A species has the following MO configuration: ( σ\sigmaσ 1s)2( σ\sigmaσ 1s*)2( σ\sigmaσ 2s)2( σ\sigmaσ 2s*)2( σ\sigmaσ 2p)2( π\piπ 2p)2 This substance is

Consider the molecule and the following hybridization choices: -What is the hybridization of the nitrogen atom?

For which of the following diatomic molecules would the bond order become greater if an electron is removed (i.e. ,if the molecule is converted to the positive ion in its ground state)?

__________ is the difference between the number of bonding electrons and the number of antibonding electrons divided by two.

Chemical Foundations

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The hybridization of the central atom in NO₃^- is

Explain the concept of delocalization of electrons in SO₃.Indicate how this idea relates to resonance.

Which of the following statements about the species CN^- is false?

According to MO theory,F₂ should be diamagnetic.

For how many of the following does the bond order decrease if you add one electron to the neutral molecule? B₂,C₂,P₂,F₂

Draw a molecular orbital diagram for O₂ and N₂.Using molecular orbital theory,explain why the removal of one electron in O₂ strengthens bonding,while the removal of one electron in N₂ weakens bonding.

As the bond order of a bond increases,the bond energy and the bond length .

When an electron pair is shared in the area centered on a line joining the atoms,a $\sigma$ (sigma)bond is formed.

The hybridization of the central atom in I₃^- is:

When a carbon atom has sp³ hybridization,it has

A species has the following MO configuration: ( $\sigma$ _1s)²( $\sigma$ _1s)²( $\sigma$ _2s)²( $\sigma$ _2s)²( $\sigma$ _2p)²( $\pi$ _2p)² This substance is