The ionic compounds NaCl and MgS are represented by the diagrams above. Which statement correctly identifies diagram 1 and identifies the compound with the lower melting point, explaining why?

Diagram 1 represents NaCl ; it has a lower melting point than MgS because the coulombic attractions between its singly charged Na+ ions and the Cl- ions are weaker than those between the ions in MgS.

Diagram 1 represents NaCl ; it has a lower melting point than MgS has because the coulombic attractions between the singly charged Na+ ions and the Cl- ions in NaCl are stronger than those between the ions in MgS

Diagram 1 represents MgS ; it has a lower melting point than NaCl because the coulombic attractions between its doubly charged Mg2+ ions and the S2- ions are stronger than those between the ions in NaCl.

Diagram 1 represents MgS ; it has a lower melting point than NaCl because the coulombic attractions between the doubly charged Mg2+ ions and the S2_ ions are weaker than those between the ions in NaCl.

A student is given a sample of a pure, white crystalline substance. Which of the following would be most useful in providing data to determine if the substance is an ionic compound?

Testing the electrical conductivity of an aqueous solution of the substance

Examining the crystals of the substance under a microscope

Determining the density of the substance

Testing the electrical conductivity of the crystals

Based on the diagram above, which of the following best helps to explain why MgO(s) is not able to conduct electricity, but MgO(l) is a good conductor of electricity?

MgO(s) consists of separate Mg2+ ions and O2− ions held in a fixed lattice, but in MgO(l) the ions are free to move and conduct electricity.

MgO(s) does not contain free electrons, but MgO(l) contains free electrons that can flow.

MgO(s) contains no water, but MgO(l) contains water that can conduct electricity.

MgO(s) consists of separate Mg2+ ions and O2− ions, but MgO(l) contains MgO molecules that can conduct electricity.

The table above provides some information about two types of steel, both of which are alloys of iron and carbon. Which of the following best helps to explain why high-carbon steel is more rigid than low-carbon steel?

The additional carbon atoms within the alloy make it more difficult for the iron atoms to slide past one another.

Elemental carbon is harder than elemental iron.

The additional carbon atoms within the alloy make the high-carbon steel less dense.

The additional carbon atoms within the alloy increase the thermal conductivity of the high-carbon steel.

Which statement best helps to explain the observation that NH3 (l) boils at -28°C , whereas PH3 (l) boils at -126 °C ?

NH3 has hydrogen bonding that is stronger than the dipole-dipole forces in PH3.

The dispersion forces in NH3 are weaker than the dispersion forces in PH3.

The dispersion forces in NH3 are stronger than the dipole-dipole forces in PH3.

NH3 has hydrogen bonding that is weaker than the dipole-dipole forces in PH3.

At room temperature I2(s) is a molecular solid. Which of the following provides a characteristic of I2(s) with a correct explanation?

It is not a good conductor of electricity because its valence electrons are localized in bonding and nonbonding pairs.

It has a high melting point because it has weak intermolecular forces.

It is hard because it forms a three dimensional covalent network.

It is very soluble in water because its molecules are polar.

The structure of one form of boron nitride is represented above. This form of boron nitride is one of the hardest substances known. Which of the following best helps explain why boron nitride is so hard?

Boron nitride is a network solid of atoms connected by covalent bonds with fixed bond angles.

Boron ions and nitrogen ions are held together by ionic bonds.

Boron nitride is an alloy, and alloys are typically harder than the elements used to make them.

Boron nitride is a polymer made of long chains of boron atoms and nitrogen atoms held together by london dispersion forces.

The best explanation for the fact that diamond is extremely hard is that diamond crystals

are giant molecules in which each atom forms strong covalent bonds with all of its neighboring atoms

are made up of atoms that are intrinsically hard because of their electronic structures

consist of positive and negative ions that are strongly attracted to each other

are formed under extreme conditions of temperature and pressure

contain orbitals or bands of delocalized electrons that belong not to single atoms but to each crystal as a whole

Of the following, the best explanation for the fact that most gases are easily compressed is that the molecules in a gas

move slower as temperature decreases

The reaction between NO(g) and O2(g) to produce NO2(g) in a rigid reaction vessel is represented in the diagram above. The pressure inside the container is recorded using a pressure gauge. Which of the following statements correctly predicts the change in pressure as the reaction goes to completion at constant temperature, and provides the correct explanation?

The pressure will decrease because there are fewer molecules of product than of reactants.

The pressure will increase because the product molecules have a greater mass than either of the reactant molecules.

The pressure will decrease because the product molecules have a lower average speed than the reactant molecules.

The pressure will not change because the total mass of the product molecules is the same as the total mass of the reactant molecules.

When a sample of oxygen gas in a closed container of constant volume is heated until its absolute temperature is doubled, which of the following is also doubled?

The average velocity of the gas molecules

The number of molecules per cm3

The potential energy of the molecules

A sample of an unknown gas from a cylinder is collected over water in the apparatus shown opposite. After all the gas sample has been collected, the water levels inside and outside the gas collection tube are made the same. Measurements that must be made to calculate the molar mass of the gas include all of the following except

mass of the water in the apparatus

volume of gas in the gas-collection tube

initial and final mass of the gas cylinder

A gas mixture at 0°C and 1.0 atm contains 0.010 mol of H2, 0.015 mol of O2, and 0.025 mol of N2. Assuming ideal behavior, what is the partial pressure of hydrogen gas (H2) in the mixture?

About 0.20 atm, because H2 comprises 20% of the total number of moles of gas.

About 0.010 atm, because there is 0.010mol of H2 in the sample.

About 0.050 atm, because there is 0.050mol of gases at 0°C and 1.0 atm.

About 0.40 atm, because the mole ratio of H2 : O2 : N2 is 0.4 : 0.6 : 1.

Diagram 1 above shows equimolar samples of two gases inside a container fitted with a removable barrier placed so that each gas occupies the same volume. The barrier is carefully removed as the temperature is held constant. Diagram 2 above shows the gases soon after the barrier is removed. Which statement describes the changes to the initial pressure of each gas and the final partial pressure of each gas in the mixture and also indicates the final total pressure?

The partial pressure of each gas in the mixture is half its initial pressure; the final total pressure is half the sum of the initial pressures of the two gases.

The partial pressure of each gas in the mixture is double its initial pressure; the final total pressure is half the sum of the initial pressures of the two gases.

The partial pressure of each gas in the mixture is double its initial pressure; the final total pressure is twice the sum of the initial pressures of the two gases.

The partial pressure of each gas in the mixture is half its initial pressure; the final total pressure is the same as the sum of the initial pressures of the two gases.

An equimolar mixture of N2(g) and Ar(g) is kept inside a rigid container at a constant temperature of 300 K. The initial partial pressure of Ar in the mixture is 0.75atm. An additional amount of Ar was added to the container, enough to double the number of moles of Ar gas in the mixture. Assuming ideal behavior, what is the final pressure of the gas mixture after the addition of the Ar gas?

2.25 atm, because doubling the number of moles of Ar doubles its partial pressure.

0.75 atm, because increasing the partial pressure of Ar decreases the partial pressure of N2.

1.13 atm, because 33% of the moles of gas are N2.

1.50 atm, because the number of moles of N2 did not change.

Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct?

It depends on the relative molecular masses of X, Y, and Z.

It is equal to ⅓ the total pressure

It depends on the intermolecular forces of attraction between molecules of X, Y, and Z.

It depends on the average distance traveled between molecular collisions.

It can be calculated with knowledge only of the volume of the container.

A 0.5 mol sample of He(g) and a 0.5 mol sample of Ne(g) are placed separately in two 10.0 L rigid containers at 25°C. Each container has a pinhole opening. Which of the gases, He(g) or Ne(g), will escape faster through the pinhole and why?

He(g) will escape faster because the He(g) atoms are moving at a higher average speed than the Ne(g) atoms.

Ne(g) will escape faster because its initial pressure in the container is higher.

Ne(g) will escape faster because the Ne(g) atoms have a higher average kinetic energy than the He(g) atoms.

Both gases will escape at the same rate because the atoms of both gases have the same average kinetic energy.

A rigid metal tank contains oxygen gas. Which of the following applies to the gas in the tank when additional oxygen is added at constant temperature?

The average speed of the gas molecules remains the same.

The volume of the gas increases.

The pressure of the gas decreases.

The total number of gas molecules remains the same.

The average distance between the gas molecules increases.

At standard temperature and pressure, a 0.50 mol sample of H2 gas and a separate 1.0 mol sample of O2 gas have the same

average molecular kinetic energy

A 1L sample of helium gas at 25°C and 1atm is combined with a 1L sample of neon gas at 25°C and 1atm. The temperature is kept constant. Which of the following statements about combining the gases is correct?

The average kinetic energy of the helium atoms and neon atoms do not change when the gases are combined.

The average speed of the helium atoms increases when the gases are combined.

The average speed of the neon atoms increases when the gases are combined.

The average kinetic energy of the helium atoms increases when the gases are combined.

The graph above shows the distribution of molecular speeds for four different gases at the same temperature. What property of the different gases can be correctly ranked using information from the graph, and why?

The molecular masses of the gases, because the gas molecules have the same average kinetic energy and mass can be calculated using the equation KEavg=½mv2 .

The densities of the gases, because as the density of a gas increases, the average speed of its molecules decreases.

The pressures of the gases, because the pressure exerted by a gas depends on the average speed with which its molecules are moving

The volumes of the gases, because at a fixed temperature the volume of a gas can be calculated using the equation PV=nRT .

The average kinetic energy of the gas molecules is?

D the same in all three containers

Ap Chem Unit 3 Review

Quiz

•

Chemistry

•

12th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS3-2, HS-PS4-3, HS-PS1-3

+10

Standards-aligned

Amanda Oldson

Used 7+ times

FREE Resource

123 questions

Show all answers

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The diagram opposite is a molecular model of a gaseous
diatomic element that is just above its boiling point.
Intermolecular forces between the gas molecules will cause
them to condense into the liquid phase if the temperature is lowered.
Which of the following best describes how the model is limited in its depiction of the phenomenon?

It does not show how hydrogen bonds are constantly forming, breaking, and reforming, which results in a net force of attraction between the molecules.

It does not show how the interactions between ions and the induced molecular dipoles result in a net force of attraction between the molecules.

It does not show how the interacting permanent dipoles of the molecules result in a net force of attraction between the molecules.

It does not show how the temporary fluctuating dipoles of the molecular electron clouds result in a net force of attraction between the molecules.

The electron cloud of HF is smaller than that of F2 , however, HF has a much higher boiling point than has F2 . Which of the following explains how the dispersion-force model of intermolecular attraction does not account for the unusually high boiling point of HF ?

F2 is soluble in water, whereas HF is insoluble in water.

The F2 molecule has a greater mass than the HF molecule has.

Liquid F2 has weak dispersion force attractions between its molecules, whereas l iquid HF has strong ionic interactions between H+ and F- ions.

Liquid F2 has weak dispersion force attractions between its molecules, whereas liquid HF has both weak dispersion force attractions and hydrogen bonding interactions between its molecules.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Four different liquid compounds in flasks at are represented above. The table below identifies the compounds. Flask C shows the most particles in the vapor phase.

Which of the following is not shown in the model but best helps to explain why flask C must contain pentane?

The random motion of the particles within the liquids.

The relative speeds of the vapor particles in each flask.

The strength of the intermolecular forces between the particles in the liquids.

The structural formula of the molecules of the liquid and vapor in each flask.

The structural formula of the molecules of the liquid and vapor in each flask.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

In which of the following liquids do the intermolecular forces include dipole-dipole forces?

F2 (l)

CH4 (l)

CF4 (l)

CH2F2 (l)

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The London (dispersion) forces are weakest for which of the following gases under the same conditions of temperature and pressure?

A H2

B O2

C Xe

D F2

E N2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Thymine and adenine form a base pair in the DNA molecule. These two bases can form a connection between two strands of DNA via two hydrogen bonds.
Which of the following diagrams shows the correct representation of the hydrogen bonding (denoted by dashed lines) between thymine and adenine base pairs?
(In each diagram, thymine is shown at the left and adenine is shown at the right. The bases are attached to the backbone portion of the DNA strands.)

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Ap Chem Unit 3 Review

123 questions

The electron cloud of HF is smaller than that of F2 , however, HF has a much higher boiling point than has F2 . Which of the following explains how the dispersion-force model of intermolecular attraction does not account for the unusually high boiling point of HF ?

Four different liquid compounds in flasks at are represented above. The table below identifies the compounds. Flask C shows the most particles in the vapor phase.

Which of the following is not shown in the model but best helps to explain why flask C must contain pentane?

The structural formula of the molecules of the liquid and vapor in each flask.

In which of the following liquids do the intermolecular forces include dipole-dipole forces?

The London (dispersion) forces are weakest for which of the following gases under the same conditions of temperature and pressure?

Which of the following is the strongest type of interaction that occurs between the atoms within the circled areas of the two molecules represented below?

The ionic compounds NaCl and MgS are represented by the diagrams above. Which statement correctly identifies diagram 1 and identifies the compound with the lower melting point, explaining why?

A sample of a hard, solid binary compound at room temperature did not conduct electricity as a pure solid but became highly conductive when dissolved in water.
Which of the following types of interactions is most likely found between the particles in the substance?

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

Ap Chem Unit 3 Review

123 questions

The electron cloud of HF is smaller than that of F2 , however, HF has a much higher boiling point than has F2 . Which of the following explains how the dispersion-force model of intermolecular attraction does not account for the unusually high boiling point of HF ?

Four different liquid compounds in flasks at are represented above. The table below identifies the compounds. Flask C shows the most particles in the vapor phase.Which of the following is not shown in the model but best helps to explain why flask C must contain pentane?

The structural formula of the molecules of the liquid and vapor in each flask.

In which of the following liquids do the intermolecular forces include dipole-dipole forces?

The London (dispersion) forces are weakest for which of the following gases under the same conditions of temperature and pressure?

Which of the following is the strongest type of interaction that occurs between the atoms within the circled areas of the two molecules represented below?

The ionic compounds NaCl and MgS are represented by the diagrams above. Which statement correctly identifies diagram 1 and identifies the compound with the lower melting point, explaining why?

A sample of a hard, solid binary compound at room temperature did not conduct electricity as a pure solid but became highly conductive when dissolved in water.Which of the following types of interactions is most likely found between the particles in the substance?

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

Four different liquid compounds in flasks at are represented above. The table below identifies the compounds. Flask C shows the most particles in the vapor phase.

Which of the following is not shown in the model but best helps to explain why flask C must contain pentane?

A sample of a hard, solid binary compound at room temperature did not conduct electricity as a pure solid but became highly conductive when dissolved in water.
Which of the following types of interactions is most likely found between the particles in the substance?