Molecular Geometry and Intermolecular Forces

How many electrons are shared in a single covalent bond?

What is the VSEPR number (number of electron domains) of PF3, where P is the central atom?

Based on VSEPR theory, what is the molecular geometry of PF3 (phosphorus trifluoride)?

What is the molecular geometry and polarity of water (H₂O)?

Which intermolecular forces (IMFs) are present in a 20% MgCl₂ aqueous solution?

Which of the following molecules does NOT exhibit dipole-dipole forces?

What type of crystalline solid is graphite?

Which three elements, when bonded to hydrogen, can participate in hydrogen bonding?

Which of the following substances is expected to have the highest boiling point?

According to the phase diagram, what phase exists at 10 atm and 300 K?

What phase change occurs when mothballs gradually disappear from a cabinet without leaving a liquid residue?

On a phase diagram, what point represents the triple point?

How many liters of 16 M stock solution are needed to prepare 8.00 L of a 0.50 M nitric acid solution?

If a 1.00 L solution of NaCl is diluted to 1.80 L, what changes?

What is the molarity of a solution containing 0.444 mol of CoCl₂ in 654 mL of solution?

Convert 199 parts per million (ppm) to parts per billion (ppb).

What is the mass percent of a solution containing 9 g of solute dissolved in 100 g of solvent?

To which group in the periodic table does the octet rule generally apply most directly?

In a thin-layer chromatography experiment with a polar solvent, three dyes separate on the TLC plate. If the solvent front is at 10 cm, the blue dye is at 8 cm, the purple dye is at 6 cm, and the red dye is at 2 cm from the origin, which dye is likely the least polar?

What is considered to be the value of standard atmospheric pressure?

What type of crystalline solid is table salt (NaCl)?

Which of the following compounds would you expect to exhibit hydrogen bonding?

Consider a closed system containing a mixture of ice, water, and water vapor at equilibrium. If the temperature is increased slightly, what will initially happen to the partial pressure of the water vapor?

A solution is prepared by dissolving 25.0 g of glucose (C6H12O6) in 250.0 mL of water. Given the molar mass of glucose is 180.16 g/mol, what is the molality of the solution?

When KNO3 is dissolved in water, the solution becomes noticeably colder. What can be concluded about the dissolution of KNO3?

Which of the following phase transitions releases the most energy per mole of substance?

Which factor primarily determines the strength of London Dispersion Forces in a molecule?

Which statement best describes the vapor pressure of a liquid?

A solution is prepared by dissolving a nonvolatile solute in a volatile solvent. Which of the following statements is TRUE regarding the vapor pressure of the solution?

What is the primary reason that representative elements follow the octet rule?

Which of the following statements accurately describes the relationship between interparticle forces and viscosity?

Which type of intermolecular force is primarily responsible for the high boiling point of water compared to other molecules of similar size?

Which of the following contributes most to the surface tension of a liquid?

What happens to the solubility of most solid solutes in water as the temperature of the water increases?

Which of the following statements is true regarding the effect of pressure on the solubility of gases in liquids?

Which type of solid generally has the lowest melting point?

Which of the following properties is colligative?

Which of the following is an example of a covalent network solid?

Under what conditions does a real gas behave most ideally?