Question 1

The amount of energy released when a covalent bond is formed is called its ________.

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Question 2

The Lewis symbol for the selenium atom shows ________ valence shell electrons. The number of covalent bonds that selenium normally forms to complete its valence shell and obey the octet rule is ________.

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Question 3

The Lewis symbol for the nitrogen atom shows ________ valence shell electrons. The number of covalent bonds that nitrogen normally forms to complete its valence shell and obey the octet rule is ________.

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Question 4

The Lewis symbol for the oxygen atom shows ________ valence shell electrons. The number of covalent bonds that oxygen normally forms to complete its valence shell and obey the octet rule is ________.

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Question 5

The Lewis symbol for the carbon atom shows ________ valence shell electrons. The number of covalent bonds that carbon normally forms to complete its valence shell and obey the octet rule is ________.

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Question 6

The Lewis representation of the PH₃ molecule shows ________ covalent bonds, and ________ lone pair on the ________atom.

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Question 7

In a covalent bond between S and Cl, which atom carries the partial negative charge?

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Question 8

For the HCl molecule, the dipole moment is calculated from q × r. Calculations show that q equals 0.17 electronic charge units. This means the hydrogen carries a charge of ________ and the chlorine a charge of ________.

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Question 9

In the C-S molecule, the dipole moment is 1.96 D and the bond length is 153 pm. Determine the sign and magnitude of the charge on the carbon atom. Hint: Carefully watch your units and signs when completing this problem.

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Question 10

In the S-Si molecule, the silicon atom has a charge of 0.187 e⁻ and the bond length is 193 pm. Determine the dipole moment of this molecule. Hint: Carefully watch your units and signs when completing this problem.

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Question 11

A covalent bond has about 50 % ionic character when the electronegativity difference between the atoms is approximately ________.

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Question 12

The total number of bonds in the thiocyanate ion, SCN⁻.

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Question 13

The total number of non-bonding electrons in the NF₃ molecule is ________.

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Question 14

The total number of non-bonding electrons in molecular nitrogen is ________.

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Question 15

The total number of non-bonding electrons in molecular oxygen is ________.

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Question 16

The formal charge on the most stable Lewis structure for the central oxygen in ozone, O₃, is ________.

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Question 17

Draw the most favorable Lewis structure for the NCO molecule. Hint: Remember to minimize formal charge for your most favorable Lewis structure.

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Question 18

Draw the most favorable Lewis structure for the NCO molecule. The formal charge on the oxygen molecule is ________. Hint: Consider double and triple bonds for your structure.

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Question 19

In PCl₅, the P atom violates the octet rule by sharing ________electrons. This is because the valence shell for elements in which n = 3 can hold a maximum of _______electrons.

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Question 20

For bonds formed between the same elements, as the bond order increases, the bond length ________ and the bond energy ________.

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Quiz 9: The Basics of Chemical Bonding

The amount of energy released when a covalent bond is formed is called its ________.

The Lewis symbol for the selenium atom shows valence shell electrons. The number of covalent bonds that selenium normally forms to complete its valence shell and obey the octet rule is .

The Lewis symbol for the nitrogen atom shows valence shell electrons. The number of covalent bonds that nitrogen normally forms to complete its valence shell and obey the octet rule is .

The Lewis symbol for the oxygen atom shows valence shell electrons. The number of covalent bonds that oxygen normally forms to complete its valence shell and obey the octet rule is .

The Lewis symbol for the carbon atom shows valence shell electrons. The number of covalent bonds that carbon normally forms to complete its valence shell and obey the octet rule is .

The Lewis representation of the PH₃ molecule shows covalent bonds, and lone pair on the atom.

In a covalent bond between S and Cl, which atom carries the partial negative charge?

For the HCl molecule, the dipole moment is calculated from q × r. Calculations show that q equals 0.17 electronic charge units. This means the hydrogen carries a charge of and the chlorine a charge of .

In the C-S molecule, the dipole moment is 1.96 D and the bond length is 153 pm. Determine the sign and magnitude of the charge on the carbon atom. Hint: Carefully watch your units and signs when completing this problem.

In the S-Si molecule, the silicon atom has a charge of 0.187 e⁻ and the bond length is 193 pm. Determine the dipole moment of this molecule. Hint: Carefully watch your units and signs when completing this problem.

A covalent bond has about 50 % ionic character when the electronegativity difference between the atoms is approximately ________.

The total number of bonds in the thiocyanate ion, SCN⁻.

The total number of non-bonding electrons in the NF₃ molecule is ________.

The total number of non-bonding electrons in molecular nitrogen is ________.

The total number of non-bonding electrons in molecular oxygen is ________.

The formal charge on the most stable Lewis structure for the central oxygen in ozone, O₃, is ________.

Draw the most favorable Lewis structure for the NCO molecule. Hint: Remember to minimize formal charge for your most favorable Lewis structure.

Draw the most favorable Lewis structure for the NCO molecule. The formal charge on the oxygen molecule is ________. Hint: Consider double and triple bonds for your structure.

In PCl₅, the P atom violates the octet rule by sharing __electrons. This is because the valence shell for elements in which n = 3 can hold a maximum of _electrons.

For bonds formed between the same elements, as the bond order increases, the bond length and the bond energy .

Quiz 9: The Basics of Chemical Bonding

The amount of energy released when a covalent bond is formed is called its ________.

The Lewis symbol for the selenium atom shows ________ valence shell electrons. The number of covalent bonds that selenium normally forms to complete its valence shell and obey the octet rule is ________.

The Lewis symbol for the nitrogen atom shows ________ valence shell electrons. The number of covalent bonds that nitrogen normally forms to complete its valence shell and obey the octet rule is ________.

The Lewis symbol for the oxygen atom shows ________ valence shell electrons. The number of covalent bonds that oxygen normally forms to complete its valence shell and obey the octet rule is ________.

The Lewis symbol for the carbon atom shows ________ valence shell electrons. The number of covalent bonds that carbon normally forms to complete its valence shell and obey the octet rule is ________.

The Lewis representation of the PH3 molecule shows ________ covalent bonds, and ________ lone pair on the ________atom.

In a covalent bond between S and Cl, which atom carries the partial negative charge?

For the HCl molecule, the dipole moment is calculated from q × r. Calculations show that q equals 0.17 electronic charge units. This means the hydrogen carries a charge of ________ and the chlorine a charge of ________.

In the C-S molecule, the dipole moment is 1.96 D and the bond length is 153 pm. Determine the sign and magnitude of the charge on the carbon atom. Hint: Carefully watch your units and signs when completing this problem.

In the S-Si molecule, the silicon atom has a charge of 0.187 e− and the bond length is 193 pm. Determine the dipole moment of this molecule. Hint: Carefully watch your units and signs when completing this problem.

A covalent bond has about 50 % ionic character when the electronegativity difference between the atoms is approximately ________.

The total number of bonds in the thiocyanate ion, SCN−.

The total number of non-bonding electrons in the NF3 molecule is ________.

The total number of non-bonding electrons in molecular nitrogen is ________.

The total number of non-bonding electrons in molecular oxygen is ________.

The formal charge on the most stable Lewis structure for the central oxygen in ozone, O3, is ________.

Draw the most favorable Lewis structure for the NCO molecule. Hint: Remember to minimize formal charge for your most favorable Lewis structure.

Draw the most favorable Lewis structure for the NCO molecule. The formal charge on the oxygen molecule is ________. Hint: Consider double and triple bonds for your structure.

In PCl5, the P atom violates the octet rule by sharing ________electrons. This is because the valence shell for elements in which n = 3 can hold a maximum of _______electrons.

For bonds formed between the same elements, as the bond order increases, the bond length ________ and the bond energy ________.

The Lewis symbol for the selenium atom shows valence shell electrons. The number of covalent bonds that selenium normally forms to complete its valence shell and obey the octet rule is .

The Lewis symbol for the nitrogen atom shows valence shell electrons. The number of covalent bonds that nitrogen normally forms to complete its valence shell and obey the octet rule is .

The Lewis symbol for the oxygen atom shows valence shell electrons. The number of covalent bonds that oxygen normally forms to complete its valence shell and obey the octet rule is .

The Lewis symbol for the carbon atom shows valence shell electrons. The number of covalent bonds that carbon normally forms to complete its valence shell and obey the octet rule is .

The Lewis representation of the PH₃ molecule shows covalent bonds, and lone pair on the atom.

For the HCl molecule, the dipole moment is calculated from q × r. Calculations show that q equals 0.17 electronic charge units. This means the hydrogen carries a charge of and the chlorine a charge of .

In the S-Si molecule, the silicon atom has a charge of 0.187 e⁻ and the bond length is 193 pm. Determine the dipole moment of this molecule. Hint: Carefully watch your units and signs when completing this problem.

The total number of bonds in the thiocyanate ion, SCN⁻.

The total number of non-bonding electrons in the NF₃ molecule is ________.

The formal charge on the most stable Lewis structure for the central oxygen in ozone, O₃, is ________.

In PCl₅, the P atom violates the octet rule by sharing __electrons. This is because the valence shell for elements in which n = 3 can hold a maximum of _electrons.

For bonds formed between the same elements, as the bond order increases, the bond length and the bond energy .