FiltersDone

Question type

Essay

Multiple Choice

Short Answer

True False

Matching

Exam 9: The Basics of Chemical Bonding

Show Answer

Share

---

All types

Filters

Study FlashcardsPractice ExamLearn

Question 1

Multiple Choice

Review LaterAdd Note

Review Later

The chlorite ion has a Lewis structure that is based on the skeletal structure shown below: O=Cl -O Draw the Lewis structure minimizing the formal charges present in the structure. Based on this structure, the chlorite ion has ,Hint: Consider all possible resonance structures when working with formal charge.

A) two single bonds, the sum of absolute values of formal charges = 3, and no resonance hybrids.
B) one single and one double bond, sum of absolute values of formal charges = 5, and two contributing resonance hybrids.
C) one single and one double bond, sum of absolute values of formal charges = 3, and two contributing resonance hybrids.
D) two double bonds, sum of absolute values of formal charges = 1, and no resonance hybrids.
E) one single and one double bond, sum of absolute values of formal charges = 1, and two contributing resonance hybrids.

F) None of the above
G) B) and E)

Correct Answer

verified

Show Answer

Question 2

Short Answer

Review LaterAdd Note

Review Later

When the Sn²⁺ ion is formed, the electrons are removed from which set of orbital(s)?

Correct Answer

verified

5p

Question 3

Short Answer

Review LaterAdd Note

Which of these species, Fe³⁺, P³⁻, B⁻, Ca²⁺, has the most valence electrons?

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

Sodium forms a monatomic ion that has the electron configuration of a noble gas. What is the electron configuration of that noble gas?

In the family of compounds called aldehydes, the carbon in C=O group is directly attached to another ________ atom and a ________ atom.

Which of these ions shown, Fe³⁺, P³⁻ , B⁻, Ca²⁺, has the same number of valence electrons as a germanium atom?

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 ________.

Which bond is the most polar?Hint: Consider the electronegativity values of each element.

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

There are three resonance structures for the hydrogen carbonate ion. Hint: Draw the Lewis structure and look at the double bonds. How could they be re-arranged?

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

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.

Given that the first ionization energy of cesium is +376 kJ/mol and the electron affinity of bromine is -325 kJ/mol, calculate $\Delta$ E for the reaction, Cs(g) + Br(g) s Cs⁺(g) + Br^?(g) .

Which of the following solids would have the highest melting point?

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

Draw the Lewis structure for SOCl₂. Considering formal charges, there will be ________ bonds and ________ resonance structures in the molecule.

Which of the following solids is likely to have the largest exothermic lattice energy?

A student drew four possible Lewis structures for HBrO₄ Complete these Lewis structures presented above by filling in the remaining valence electrons that are not in the bonds. Based on these structures, the preferred structure would be the structure shown as ________ in which the sum of the absolute values of the formal charges on all the atoms is ________. Hint: When determining remaining valence electrons remember to account for the electrons already present in the bonds.

Which ionic solid is likely to have the least exothermic lattice energy?