Chapter 10 Practice Test Flashcards
Use the Lewis Dot structure for POCl3 to calculate the SN value for the central phosphorous atom.
4
The Lewis Dot structure for water can be drawn in the following manner.
What is the steric number value and predicted geometric shape of water based on the SN value?
4; tetrahedral
Which of the following best defines the term steric number (SN)?
The steric number is equal to the number of atoms in a molecule that are bonded to the central atom plus the number of lone pairs of electrons.
What are the steric numbers for the central nitrogen atoms in these two molecules?
2, 2
Which of the following molecules has only one lone pair on the central atom?
SO2
Which of the following has a steric number of three and a bent molecular geometry?
O3
What is the geometry of the molecule chlorine trifluoride, which has steric number 5?
T-shaped
Which of the following has a square planar molecular geometry?
IF4−
Which pair of molecules has the same steric number, but different shapes?
NO3− and O3
Which statement best explains why the molecule in the diagram is polar?
The molecule is linear but is polar because the electronegativity of oxygen is greater than the electronegativity of sulfur
The Lewis dot structure for oxalic acid is shown in the drawing. Which statement about the bond angles for oxalic acid is not true?
The H–O–C bond angle is 120°
Which of the following best describes why phosphorous trichloride has a net dipole moment downward?
There is nothing on the “top” of the molecule to effectively cancel the downward dipole effect of the three Cl–P bonds
What is the difference between a σ bond and a π bond?
A σ bond’s overlap occurs along the internuclear axis.
Suppose that a theoretical gas atom has an electron configuration of 1s22s22p6. Which statement best describes this atom’s electron arrangement and theoretical reactivity with an atom that has an unpaired electron?
This atom has five orbitals, 1s, 2s, and three 2p orbitals. They each contain paired electrons. This atom will not display highly reactive tendencies, because its orbitals are already filled
Which statement best describes the bonding in an O2 molecule?
O2 has one σ bond and one π bond