Question 1

Refer to Image 1. Which element is most likely represented by this Bohr model, and what is its atomic number?

Accepted Answer

Nitrogen, atomic number 7

Question 2

Image 2 shows an atomic orbital. Which type of orbital is depicted, and what is its characteristic shape?

Accepted Answer

s-orbital; spherical

Question 3

Image 3 shows three atomic orbitals. What is the significance of these orbitals in the context of electron configuration?

Accepted Answer

They are three degenerate 2p orbitals, each oriented along a different axis (x, y, z)

Question 4

Image 4 shows an energy level diagram for atomic orbitals. According to the Aufbau principle, which orbital is filled immediately after the 3p orbital?

Accepted Answer

$$4s$$

Question 5

Image 5 shows the crystal structure of lithium fluoride. What type of bonding is present in this compound, and what is a key property of such solids?

Accepted Answer

Ionic bonding; high melting point

Question 6

Image 6 shows the structure of methane. What is the hybridization of the central carbon atom, and what is the ideal bond angle?

Accepted Answer

sp3; 109.5°

Question 7

Image 7 shows an electron configuration diagram. Which element is represented, and what rule is illustrated by the way electrons are filled in the 2p orbitals?

Accepted Answer

Carbon; Hund's Rule

Question 8

Image 8 compares the ground state and sp3 hybridized state of carbon. What is the main consequence of this hybridization for carbon's bonding in organic molecules?

Accepted Answer

It allows carbon to form four equivalent bonds in a tetrahedral geometry

Question 9

Image 9 shows the bonding in acetylene. What is the hybridization of the carbon atoms in acetylene, and how many sigma and pi bonds are present between the two carbons?

Accepted Answer

sp; 1 sigma, 2 pi

Question 10

Image 10 compares the geometry and hybridization of methane, methyl anion, methyl cation, and methyl radical. Which of these species is planar, and what is its hybridization?

Accepted Answer

Methyl cation; sp2

Question 11

Image 11 shows the geometry of ammonia and water. What is the main reason for the difference in bond angles between these two molecules?

Accepted Answer

Water has two lone pairs, causing greater repulsion and a smaller bond angle

Question 12

Image 12 shows the bonding in an aldehyde. What is the hybridization of the carbonyl carbon, and what types of bonds are present between the carbon and oxygen?

Accepted Answer

sp2; one sigma and one pi bond

Question 13

Image 13 shows the structure of propane. What is the molecular formula of propane, and what is the hybridization of each carbon atom?

Accepted Answer

$$C_3H_8$$; $$sp^3$

Question 14

Image 14 shows the general structure of an ether. Which functional group is present, and what is a key property of ethers in organic chemistry?

Accepted Answer

Ether; generally unreactive and good solvents

Question 15

Image 15 shows the structure of a steroid. Which hybridization is present at the carbonyl carbon, and what is the geometry around this atom?

Accepted Answer

sp2; trigonal planar

Question 16

Image 16 shows the open chain and bond line forms of gamma-hydroxybutyric acid. What is the molecular formula of this compound, and which functional groups are present?

Accepted Answer

$$C_4H_8O_3$$; alcohol and carboxylic acid

Question 17

Image 17 shows the formation of a hydrogen molecule. What type of bond is formed between the two hydrogen atoms, and what is the bond length?

Accepted Answer

Covalent sigma bond; 1 Å

Question 18

Image 18 shows hydrogen bonding between water molecules. What is required for hydrogen bonding to occur?

Accepted Answer

A hydrogen atom bonded to a highly electronegative atom (N, O, or F) and a lone pair on another electronegative atom

Question 19

Image 19 shows the dipole moment in chloromethane. What causes the dipole moment in this molecule?

Accepted Answer

The difference in electronegativity between carbon and chlorine

Foundations of Organic Chemistry: Atomic Structure, Bonding, and Molecular Geometry

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