Question 1

Draw the Lewis structure for ClSO3−, optimized for formal charge considerations, showing all resonance structures.

Accepted Answer

Question 2

The F-O bond is more polar than the H-O bond.

Accepted Answer

A) True 
 B)False

Question 3

Draw a Lewis structure for NH4+. Based on this Lewis structure, the calculated value for the formal charge on the nitrogen atom is

Accepted Answer

A)  0.
B)  4+.
C)  1+.
D)  1-.
E)  4- .F) A) and B)
G) A) and C)

Question 4

The formal charge on the nitrogen atom in the nitrate ion (NO3-) is

Accepted Answer

A)  3-
B)  0
C)  1+
D)  3+
E)  5+F) All of the above
G) B) and E)

Question 5

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

Accepted Answer

A)  5, 1
B)  5, 2
C)  3, 4
D)  5, 3
E)  5, 4F) None of the above
G) A) and D)

Question 6

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 ________.

Accepted Answer

The answer of For the HCl molecule, the dipole moment...

Question 7

Draw the Lewis structure for the sulfur dioxide molecule. When formal charge considerations are fully considered and adjustments made, if necessary, how many resonance structures, if any, can be drawn?

Accepted Answer

The answer of Draw the Lewis structure for the sulfur...

Question 8

Based on the "best"Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the nitrogen atom in the nitrate ion?

Accepted Answer

A)  0
B)  2
C)  4
D)  6
E)  8F) A) and E)
G) C) and D)

Question 9

Draw the Lewis structure for H2SeO4. If the valence shells are filled to the usual limit (a maximum of 8) , what is the formal charge on the Se? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Accepted Answer

A)  2-
B)  1-
C)  0
D)  1+
E)  2+F) A) and D)
G) A) and E)

Question 10

Based on electronegativity considerations, which species should be the strongest oxidizing agent?

Accepted Answer

A)  Xe
B)  As
C)  Br2
D)  I2
E)  SbF) A) and E)
G) A) and D)

Question 11

How many lone pairs of electrons are on the group of atoms that characterize organic acids?

Accepted Answer

A)  6
B)  4
C)  3
D)  2
E)  1F) A) and E)
G) A) and C)

Question 12

When electrons are removed from a given shell to form a cation, they come from the highest energy occupied subshell first before any are removed from a lower-energy subshell.

Accepted Answer

A) True 
 B)False

Question 13

The fluorophosphonate ion, FPO32−, has a structure similar to that of the orthophosphate ion, the difference being that one of the oxygen atoms has been replaced by a fluorine atom. Draw the Lewis structure for this ion, optimized for formal charge considerations, showing all resonance structures.

Accepted Answer

Question 14

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 ________.

Accepted Answer

The answer of The Lewis symbol for the selenium atom...

Question 15

Draw the Lewis structure for the F2CO molecule. Based on this structure, how many polar bonds and non-polar bonds are present? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Accepted Answer

A)  3 polar bonds and no non-polar bonds
B)  2 polar bonds and 1 non-polar bond
C)  1 polar bond and 2 non-polar bonds
D)  no polar bonds and 3 non-polar bonds
E)  2 polar bonds and 2 non-polar bondsF) A) and B)
G) A) and C)

Question 16

The Born-Haber cycle, which is an enthalpy diagram that can be used to calculate the lattice energy of an ionic compound, has how many endothermic steps?

Accepted Answer

The answer of The Born-Haber cycle, which is an enthalpy...

Question 17

The octet rule is generally followed for cations of elements located where on the periodic table?

Accepted Answer

A)  post transition metals and transition metals
B)  Group IA and Group IIA metals
C)  Group IVA elements
D)  lanthanide elements
E)  actinide elementsF) A) and B)
G) B) and C)

Question 18

Based on the "best"Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the carbon atom in the CO molecule?

Accepted Answer

A)  0
B)  2
C)  4
D)  6
E)  8F) B) and C)
G) All of the above

Question 19

Draw a Lewis structure for CH3NO2. Based on the Lewis structure, what is the formal charge on the nitrogen atom for the most favorable structure? Hint: Minimize formal charge to ensure you have the most stable or "best"Lewis structure.

Accepted Answer

A)  -2
B)  -1
C)  0
D)  +1
E)  +2F) A) and E)
G) B) and E)

Question 20

Based on the  Δ\DeltaΔ  H°f data given, which compound is the most stable?

Accepted Answer

A)  N2O4(g) , +9.7 kJ/mol
B)  H2S(g) , -20.6 kJ/mol
C)  N2H4(g) , +94.5 kJ/mol
D)  PH3(g) , +5.4 kJ/mol
E)  NH3(g) , -46.4 kJ/mol F) A) and B)
G) A) and E)

Exam 9: The Basics of Chemical Bonding

How many lone pairs of electrons are on the group of atoms that characterize organic acids?

Correct Answer
verified

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 .

Correct Answer
verified

Draw the Lewis structure for ClSO₃⁻, optimized for formal charge considerations, showing all resonance structures.

Correct Answer
verified

Based on the "best"Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the nitrogen atom in the nitrate ion?

Correct Answer
verified

Draw a Lewis structure for NH₄⁺. Based on this Lewis structure, the calculated value for the formal charge on the nitrogen atom is

Correct Answer
verified

The octet rule is generally followed for cations of elements located where on the periodic table?

Correct Answer
verified

Based on the "best"Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the carbon atom in the CO molecule?

Correct Answer
verified

Draw the Lewis structure for H₂SeO₄. If the valence shells are filled to the usual limit (a maximum of 8) , what is the formal charge on the Se? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Draw the Lewis structure for the F₂CO molecule. Based on this structure, how many polar bonds and non-polar bonds are present? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Correct Answer
verified

The F-O bond is more polar than the H-O bond.

Correct Answer
verified

Draw the Lewis structure for the sulfur dioxide molecule. When formal charge considerations are fully considered and adjustments made, if necessary, how many resonance structures, if any, can be drawn?

Correct Answer
verified

The Born-Haber cycle, which is an enthalpy diagram that can be used to calculate the lattice energy of an ionic compound, has how many endothermic steps?

Correct Answer
verified

The formal charge on the nitrogen atom in the nitrate ion (NO₃^-) is

Correct Answer
verified

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 .

Correct Answer
verified

Draw a Lewis structure for CH₃NO₂. Based on the Lewis structure, what is the formal charge on the nitrogen atom for the most favorable structure? Hint: Minimize formal charge to ensure you have the most stable or "best"Lewis structure.

Correct Answer
verified

When electrons are removed from a given shell to form a cation, they come from the highest energy occupied subshell first before any are removed from a lower-energy subshell.

Correct Answer
verified

Based on the $\Delta$ H°_f data given, which compound is the most stable?

Correct Answer
verified

Based on electronegativity considerations, which species should be the strongest oxidizing agent?

Correct Answer
verified

Exam 9: The Basics of Chemical Bonding

How many lone pairs of electrons are on the group of atoms that characterize organic acids?

Correct AnswerverifiedShow Answer

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 ________.

Correct AnswerverifiedShow Answer

Draw the Lewis structure for ClSO3−, optimized for formal charge considerations, showing all resonance structures.

Correct AnswerverifiedShow Answer

Based on the "best"Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the nitrogen atom in the nitrate ion?

Correct AnswerverifiedShow Answer

Draw a Lewis structure for NH4+. Based on this Lewis structure, the calculated value for the formal charge on the nitrogen atom is

Correct AnswerverifiedShow Answer

The octet rule is generally followed for cations of elements located where on the periodic table?

Correct AnswerverifiedShow Answer

Based on the "best"Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the carbon atom in the CO molecule?

Correct AnswerverifiedShow Answer

Draw the Lewis structure for H2SeO4. If the valence shells are filled to the usual limit (a maximum of 8) , what is the formal charge on the Se? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Draw the Lewis structure for the F2CO molecule. Based on this structure, how many polar bonds and non-polar bonds are present? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Correct AnswerverifiedShow Answer

The F-O bond is more polar than the H-O bond.

Correct AnswerverifiedShow Answer

Draw the Lewis structure for the sulfur dioxide molecule. When formal charge considerations are fully considered and adjustments made, if necessary, how many resonance structures, if any, can be drawn?

Correct AnswerverifiedShow Answer

The Born-Haber cycle, which is an enthalpy diagram that can be used to calculate the lattice energy of an ionic compound, has how many endothermic steps?

Correct AnswerverifiedShow Answer

The formal charge on the nitrogen atom in the nitrate ion (NO3-) is

Correct AnswerverifiedShow Answer

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 ________.

Correct AnswerverifiedShow Answer

Draw a Lewis structure for CH3NO2. Based on the Lewis structure, what is the formal charge on the nitrogen atom for the most favorable structure? Hint: Minimize formal charge to ensure you have the most stable or "best"Lewis structure.

Correct AnswerverifiedShow Answer

When electrons are removed from a given shell to form a cation, they come from the highest energy occupied subshell first before any are removed from a lower-energy subshell.

Correct AnswerverifiedShow Answer

Based on the Δ\DeltaΔ H°f data given, which compound is the most stable?

Correct AnswerverifiedShow Answer

Based on electronegativity considerations, which species should be the strongest oxidizing agent?

Correct AnswerverifiedShow Answer

Correct Answer
verified

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 .

Correct Answer
verified

Draw the Lewis structure for ClSO₃⁻, optimized for formal charge considerations, showing all resonance structures.

Correct Answer
verified

Correct Answer
verified

Draw a Lewis structure for NH₄⁺. Based on this Lewis structure, the calculated value for the formal charge on the nitrogen atom is

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Draw the Lewis structure for H₂SeO₄. If the valence shells are filled to the usual limit (a maximum of 8) , what is the formal charge on the Se? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Draw the Lewis structure for the F₂CO molecule. Based on this structure, how many polar bonds and non-polar bonds are present? Hint: Do not forget about double or triple bonds potentially being in the Lewis structure.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The formal charge on the nitrogen atom in the nitrate ion (NO₃^-) is

Correct Answer
verified

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 .

Correct Answer
verified

Draw a Lewis structure for CH₃NO₂. Based on the Lewis structure, what is the formal charge on the nitrogen atom for the most favorable structure? Hint: Minimize formal charge to ensure you have the most stable or "best"Lewis structure.

Correct Answer
verified

Correct Answer
verified

Based on the $\Delta$ H°_f data given, which compound is the most stable?

Correct Answer
verified

Correct Answer
verified