Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Textbook Question
Chapter 9, Problem 41E

In each of the following groups of substances, pick the one that has the given property. Justify your answer.

a. highest boiling point: HBr, Kr, or Cl2

b. highest freezing point: H2O, NaCl, or HF

c. lowest vapor pressure at 25°C: Cl2, Br2, or I2

d. lowest freezing point: N2, CO, or CO2

e. lowest boiling point: CH4, CH3CH3, or CH3CH2CH3

f. highest boiling point: HF, HCl, or HBr

g. Chapter 9, Problem 41E, In each of the following groups of substances, pick the one that has the given property. Justify

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

From the given set of compounds, the compounds with highest boiling point, highest freezing point, lowest vapor pressure, lowest freezing point and lowest boiling point have to be identified and the same has to be justified.

Concept Introduction:

Matter is generally classified into three distinct categories - solid state, liquid state, gaseous state. In all of these three states of matter, the constituents (molecules or ions) of the matter do possess forces between them which are not the same in each state. These forces are called intermolecular forces.

The intermolecular forces are relatively strong in the solids than liquids and weaker in the gaseous substances. This variation influences many of the properties of all the three distinct states of the matter.

If the strength of intermolecular force is high in a substance then its melting point, freezing point, boiling point will be high and the vapor pressure will be low.

The strength of intermolecular forces is,

Londondispersionforces<Dipole-dipoleforces<Hydrogenbonding

Answer to Problem 41E

The compound with highest boiling point is HBr .  Because this is the only compound in the set that has strong intermolecular force – dipole force.

Explanation of Solution

Kr,HBr,Cl2

Identify the compound which has highest boiling point and justify it.

HBr has the highest boiling point. Compare to the other compounds, the   intermolecular force in HBr is high in strength.

HBr is the only polar covalent compound among the given compounds. Being a polar covalent compound HBr has dipole forces. Hence among the given compounds only in HBr the intermolecular force is strong. At normal temperature, the intermolecular forces are not broken. So at high temperature the intermolecular forces are broken allowing the substance to boil. So HBr has the highest boiling point.

Analyze why the other compounds don’t have the highest boiling point and justify the same.

The compounds other than HBr have intermolecular force of low strength.

Kr and Cl2 are non-polar covalent compounds unlike HBr . The intermolecular force in them is London dispersion force which is not as strong as dipole forces. London dispersion forces can be collapsed easily. So a higher temperature is not required to boil them. Due to this their boiling point is lower than that of HBr .

Conclusion

      The compound with the highest boiling point is identified and the same is justified.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

From the given set of compounds, the compounds with highest boiling point, highest freezing point, lowest vapor pressure, lowest freezing point and lowest boiling point have to be identified and the same has to be justified.

Concept Introduction:

Matter is generally classified into three distinct categories - solid state, liquid state, gaseous state. In all of these three states of matter, the constituents (molecules or ions) of the matter do possess forces between them which are not the same in each state. These forces are called intermolecular forces.

The intermolecular forces are relatively strong in the solids than liquids and weaker in the gaseous substances. This variation influences many of the properties of all the three distinct states of the matter.

If the strength of intermolecular force is high in a substance then its melting point, freezing point, boiling point will be high and the vapor pressure will be low.

The strength of intermolecular forces is,

Londondispersionforces<Dipole-dipoleforces<Hydrogenbonding

Answer to Problem 41E

The compound with highest freezing point or melting point is NaCl due to the strongest electrostatic forces present in the molecule.

Explanation of Solution

H2O,NaCl,HF

Identify the compound which has highest melting point and justify it.

NaCl has the highest melting point. The intermolecular force in NaCl is highest in strength.

NaCl is the only ionic compound among the given compounds. Ionic compounds have the electrostatic forces which are known to be strong. Hence among the given compounds only NaCl has strong intermolecular force. At normal temperature, the intermolecular forces are not broken. So high temperature is required to break the strong intermolecular forces and allow the substance to melt. So NaCl has the highest melting point.

Analyze why the other compounds don’t have the highest melting point and justify the same.

The compounds other than NaCl have intermolecular force of low strength.

H2O and HF are polar covalent compounds. The intermolecular forces in them are dipole forces and hydrogen bonding which are not as strong as electrostatic forces.

Hence H2O and HF have low freezing/melting point than NaCl .

Conclusion

      The compound with the highest melting point is identified and the same is justified.

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

From the given set of compounds, the compounds with highest boiling point, highest freezing point, lowest vapor pressure, lowest freezing point and lowest boiling point have to be identified and the same has to be justified.

Concept Introduction:

Matter is generally classified into three distinct categories - solid state, liquid state, gaseous state. In all of these three states of matter, the constituents (molecules or ions) of the matter do possess forces between them which are not the same in each state. These forces are called intermolecular forces.

The intermolecular forces are relatively strong in the solids than liquids and weaker in the gaseous substances. This variation influences many of the properties of all the three distinct states of the matter.

If the strength of intermolecular force is high in a substance then its melting point, freezing point, boiling point will be high and the vapor pressure will be low.

The strength of intermolecular forces is,

Londondispersionforces<Dipole-dipoleforces<Hydrogenbonding

Answer to Problem 41E

The compound with lowest vapor pressure is I2 due to the presence of strong hydrogen London dispersion force in it.

Explanation of Solution

Cl2,Br2,I2

Identify the compound that has the lowest vapor pressure and justify it.

I2 has the lowest vapor pressure. Compare to the other compounds, the intermolecular force in I2 is strong.

A boiling liquid partly vaporizes and the vaporized molecules do exist in equilibrium with the liquid molecules. The pressure exerted by the vaporized molecules is termed as vapor pressure. If the intermolecular forces are weak the molecules are not held together strongly that they are able to move freely. The pressure exerted by the molecules is directly proportional to the free movement of molecules. If the intermolecular forces are strong, the movement of the molecules is restricted to some extent that the pressure exerted by them will be low. Thus increase in the strength of intermolecular forces in a substance decreases its vapor pressure.

I2 is a large non-polar covalent compound. The London dispersion forces in them are strong due to its large molecular size. Hence, I2 has the lowest vapor pressure.

Analyze why the other compounds don’t have the lowest vapor pressure and justify the same.

The intermolecular forces exist in them are not of high strength.

Both Cl2andBr2 are non-polar covalent compounds like I2. The intermolecular force exist in them is London dispersion force. Their molecular size is not as large as I2 that the London dispersion force in them is not strong. Thus they readily exhibit free movement and exert vapor pressure.

Conclusion

The compound with the lowest vapor pressure is identified and the same is justified.

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

From the given set of compounds, the compounds with highest boiling point, highest freezing point, lowest vapor pressure, lowest freezing point and lowest boiling point have to be identified and the same has to be justified.

Concept Introduction:

Matter is generally classified into three distinct categories - solid state, liquid state, gaseous state. In all of these three states of matter, the constituents (molecules or ions) of the matter do possess forces between them which are not the same in each state. These forces are called intermolecular forces.

The intermolecular forces are relatively strong in the solids than liquids and weaker in the gaseous substances. This variation influences many of the properties of all the three distinct states of the matter.

If the strength of intermolecular force is high in a substance then its melting point, freezing point, boiling point will be high and the vapor pressure will be low.

The strength of intermolecular forces is,

Londondispersionforces<Dipole-dipoleforces<Hydrogenbonding

Answer to Problem 41E

The compound with lowest freezing point is N2 due to the presence of weakest London dispersion force in it.

Explanation of Solution

(d)N2,CO,CO2

Identify the compound that has the lowest freezing point and justify it.

N2 has the lowest freezing point. Among the given compounds the intermolecular force in N2 is the weakest.

N2 is a non-polar covalent molecule. It has only London dispersion forces. N2 is a small molecule that the strength of the intermolecular force that is London dispersion force is not high. So that the N2 molecules readily freeze and it has the lowest freezing point.

Analyze why the other compounds don’t have the lowest freezing point and justify the same.

The compounds other than N2 have intermolecular force of high strength.

The other compounds CO and CO2 are polar covalent compound and non-polar covalent compounds respectively. Both CO and CO2 have London dispersion forces and they are larger molecular size than N2 . Thus they have strong London dispersion forces than that of N2 . Further, CO has dipole-dipole force. So overall, the strength of intermolecular force in CO and CO2 is higher than that of N2 . So their freezing point is not lower than that of N2 .

Conclusion

The compound with the lowest freezing point is identified and the same is justified.

(e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

From the given set of compounds, the compounds with highest boiling point, highest freezing point, lowest vapor pressure, lowest freezing point and lowest boiling point have to be identified and the same has to be justified.

Concept Introduction:

Matter is generally classified into three distinct categories - solid state, liquid state, gaseous state. In all of these three states of matter, the constituents (molecules or ions) of the matter do possess forces between them which are not the same in each state. These forces are called intermolecular forces.

The intermolecular forces are relatively strong in the solids than liquids and weaker in the gaseous substances. This variation influences many of the properties of all the three distinct states of the matter.

If the strength of intermolecular force is high in a substance then its melting point, freezing point, boiling point will be high and the vapor pressure will be low.

The strength of intermolecular forces is,

Londondispersionforces<Dipole-dipoleforces<Hydrogenbonding

Answer to Problem 41E

The compound with lowest boiling point is CH4 due to the presence of weakest London dispersion force in it.

Explanation of Solution

CH4, CH3CH3,CH3CH2CH3

Identify the compound which has lowest boiling point and justify it.

CH4 has the lowest boiling point. The intermolecular force in CH4 is of low strength.

CH4 is a non-polar covalent compound. Among the given compounds CH4 has the smallest size. Being a non-polar covalent compound CH4 has London dispersion forces. When the molecule is smaller in size London dispersion forces is not well pronounced. Hence in CH4 the intermolecular force is very weak. The weak intermolecular force leads to its lowest boiling point.

Analyze why the other compounds don’t have the lowest boiling point and justify the same.

The compounds other than CH4 have intermolecular force of high strength.

CH3CH3 and CH3CH2CH3 are also non-polar covalent compounds like CH4. But they have larger sizes that the intermolecular force in them are strong and cannot be collapsed easily. So a higher temperature is required to boil them.  Due to this their boiling point is higher than that of CH4.

Conclusion

The compound with the lower boiling point is identified and the same is justified.

(f)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

From the given set of compounds, the compounds with highest boiling point, highest freezing point, lowest vapor pressure, lowest freezing point and lowest boiling point have to be identified and the same has to be justified.

Concept Introduction:

Matter is generally classified into three distinct categories - solid state, liquid state, gaseous state. In all of these three states of matter, the constituents (molecules or ions) of the matter do possess forces between them which are not the same in each state. These forces are called intermolecular forces.

The intermolecular forces are relatively strong in the solids than liquids and weaker in the gaseous substances. This variation influences many of the properties of all the three distinct states of the matter.

If the strength of intermolecular force is high in a substance then its melting point, freezing point, boiling point will be high and the vapor pressure will be low.

The strength of intermolecular forces is,

Londondispersionforces<Dipole-dipoleforces<Hydrogenbonding

Answer to Problem 41E

The compound with highest boiling point is HF because it forms the strongest hydrogen bonding unlike other compounds in the given set.

Explanation of Solution

HF,HCl,HBr

Identify the compound which has highest boiling point and justify it.

HF has the highest boiling point. Compare to the other compounds, the   intermolecular force in HF is high in strength.

HF is the only compound among the given set of compounds that exhibits hydrogen bonding. Hydrogen bonded liquids have high boiling point.

Analyze why the other compounds don’t have the highest boiling point and justify the same.

The compounds other than HF have intermolecular force of low strength.

All the compounds in the given set are polar covalent compounds. Among the given compounds HF has high polarity due to the high electronegativity of Fluorine. All these compounds have London dispersion forces and dipole forces. But only HF has hydrogen bonding as additional intermolecular force. As a result, among the given compounds HF has the strongest intermolecular force and higher boiling point.

Conclusion

      The compound with the highest boiling point is identified and the same is justified.

(g)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

From the given set of compounds, the compounds with highest boiling point, highest freezing point, lowest vapor pressure, lowest freezing point and lowest boiling point have to be identified and the same has to be justified.

Concept Introduction:

Matter is generally classified into three distinct categories - solid state, liquid state, gaseous state. In all of these three states of matter, the constituents (molecules or ions) of the matter do possess forces between them which are not the same in each state. These forces are called intermolecular forces.

The intermolecular forces are relatively strong in the solids than liquids and weaker in the gaseous substances. This variation influences many of the properties of all the three distinct states of the matter.

If the strength of intermolecular force is high in a substance then its melting point, freezing point, boiling point will be high and the vapor pressure will be low.

The strength of intermolecular forces is,

Londondispersionforces<Dipole-dipoleforces<Hydrogenbonding

Answer to Problem 41E

The compound with the lowest vapor pressure is CH3CH2CH2OH because it forms the strongest hydrogen bonding unlike other compounds in the given set.

Explanation of Solution

CH3CH2CH3, CH3COCH3,CH3CH2CH2OH

Identify the compound which has lowest vapor pressure and justify it.

The compound CH3CH2CH2OH has the lowest vapor pressure because the molecules of CH3CH2CH2OH exhibit hydrogen bonding, the strongest intermolecular force.

A boiling liquid partly vaporizes and the vaporized molecules do exist in equilibrium with the liquid molecules. The pressure exerted by the vaporized molecules is termed as vapor pressure. If the intermolecular forces are weak the molecules are held together loosely. Then they exhibit faster movement. The more the free movement of molecules the more will be the pressure exerted by them. If the intermolecular forces are strong, the movement of the molecules is restricted to some extent that the pressure exerted by them will be low. Thus increase in the strength of intermolecular forces in a substance decreases its vapor pressure.

CH3CH2CH2OH is a hydroxyl compound. It exhibits hydrogen bonding to a very large extent that the molecules of CH3CH2CH2OH are held together tightly and does not move freely. So the molecules of CH3CH2CH2OH exhibits low vapor pressure

Analyze why the other compounds don’t have the lowest vapor pressure and justify the same.

The intermolecular forces exist in them are not of high strength.

In CH3COCH3 due to the absence of direct O-H bonding, the hydrogen bonding does not exist and has dipole force and London dispersion forces. CH3CH2CH3 is a non-polar covalent compound and has only London dispersion forces. Both the dipole forces and London dispersion forces are weaker than hydrogen bonding. Thus these compounds can have vapor pressure higher than that of CH3CH2CH2OH.

Conclusion

The compound with the lowest vapor pressure is identified and the same is justified.

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Chapter 9 Solutions

Chemistry: An Atoms First Approach

Ch. 9 - It is possible to balance a paper clip on the...Ch. 9 - Prob. 2ALQCh. 9 - Prob. 3ALQCh. 9 - Prob. 4ALQCh. 9 - Prob. 5ALQCh. 9 - Prob. 6ALQCh. 9 - Prob. 7ALQCh. 9 - Prob. 8ALQCh. 9 - Prob. 9ALQCh. 9 - Prob. 10ALQCh. 9 - Prob. 11ALQCh. 9 - Prob. 12QCh. 9 - In the diagram below, which lines represent the...Ch. 9 - Prob. 14QCh. 9 - Atoms are assumed to touch in closest packed...Ch. 9 - Define critical temperature and critical pressure....Ch. 9 - Prob. 17QCh. 9 - Prob. 18QCh. 9 - Prob. 19QCh. 9 - Prob. 20QCh. 9 - Prob. 21QCh. 9 - A common response to hearing that the temperature...Ch. 9 - Prob. 23QCh. 9 - Prob. 24QCh. 9 - When wet laundry is hung on a clothesline on a...Ch. 9 - Cake mixes and other packaged foods that require...Ch. 9 - You have three covalent compounds with three very...Ch. 9 - Prob. 28QCh. 9 - Compare and contrast the structures of the...Ch. 9 - Prob. 30QCh. 9 - How could you tell experimentally if TiO2 is an...Ch. 9 - A common prank on college campuses is to switch...Ch. 9 - A plot of In (Pvap) versus 1/T (K) is linear with...Ch. 9 - Prob. 34QCh. 9 - Identify the most important types of interparticle...Ch. 9 - Prob. 36ECh. 9 - Predict which substance in each of the following...Ch. 9 - Consider the compounds CI2, HCI. F2, NaF, and HF....Ch. 9 - Prob. 39ECh. 9 - Consider the following electrostatic potential...Ch. 9 - In each of the following groups of substances,...Ch. 9 - Prob. 42ECh. 9 - The shape of the meniscus of water in a glass tube...Ch. 9 - Prob. 44ECh. 9 - Prob. 45ECh. 9 - Prob. 46ECh. 9 - X rays from a copper X-ray tube ( = 154 pm) were...Ch. 9 - The second-order diffraction (n = 2) for a gold...Ch. 9 - A topaz crystal has an interplanar spacing (d) of...Ch. 9 - X rays of wavelength 2.63 were used to analyze a...Ch. 9 - Prob. 51ECh. 9 - Prob. 52ECh. 9 - Prob. 53ECh. 9 - Iridium (Ir) has a face-centered cubic unit cell...Ch. 9 - You are given a small bar of an unknown metal X....Ch. 9 - A metallic solid with atoms in a face-centered...Ch. 9 - Titanium metal has a body-centered cubic unit...Ch. 9 - Barium has a body-centered cubic structure. If the...Ch. 9 - The radius of gold is 144 pm, and the density is...Ch. 9 - The radius of tungsten is 137 pm and the density...Ch. 9 - What fraction of the total volume of a cubic...Ch. 9 - Iron has a density of 7.86 g/cm3 and crystallizes...Ch. 9 - Prob. 63ECh. 9 - Prob. 64ECh. 9 - Selenium is a semiconductor used in photocopying...Ch. 9 - Prob. 66ECh. 9 - Prob. 67ECh. 9 - Prob. 68ECh. 9 - The structures of some common crystalline...Ch. 9 - The unit cell for nickel arsenide is shown below....Ch. 9 - Cobalt fluoride crystallizes in a closest packed...Ch. 9 - The compounds Na2O, CdS, and ZrI4. all can be...Ch. 9 - What is the formula for the compound that...Ch. 9 - Prob. 74ECh. 9 - A certain metal fluoride crystallizes in such a...Ch. 9 - The structure of manganese fluoride can be...Ch. 9 - The unit cell of MgO is shown below l Does MgO...Ch. 9 - In solid KCl the smallest distance between the...Ch. 9 - The CsCl structure is a simple cubic array of...Ch. 9 - MnO has either the NaCI type structure or the CsCI...Ch. 9 - Prob. 81ECh. 9 - What type of solid will each of the following...Ch. 9 - The memory metal, nitinol, is an alloy of nickel...Ch. 9 - Superalloys have been made of nickel and aluminum....Ch. 9 - Perovskite is a mineral containing calcium,...Ch. 9 - A mineral crystallizes in a cubic closest packed...Ch. 9 - Materials containing the elements Y, Ba, Cu, and O...Ch. 9 - The structures of another class of ceramic,...Ch. 9 - Plot the following data and determine Hvap for...Ch. 9 - From the following data for liquid nitric acid,...Ch. 9 - Prob. 91ECh. 9 - Prob. 92ECh. 9 - Prob. 93ECh. 9 - Diethyl ether (CH3CH2OCH2CH3) was one of the first...Ch. 9 - A substance, X, has the following properties:...Ch. 9 - Use the heating-cooling curve below to answer the...Ch. 9 - The molar heat of fusion of sodium metal is 2.60...Ch. 9 - Prob. 98ECh. 9 - What quantity of energy does it take to convert...Ch. 9 - Consider a 75.0-g sample of H2O(g) at 125C. What...Ch. 9 - An ice cube tray contains enough water at 22.0C to...Ch. 9 - A 0.250-g chunk of sodium metal is cautiously...Ch. 9 - Prob. 103ECh. 9 - Prob. 104ECh. 9 - Prob. 105ECh. 9 - Prob. 106ECh. 9 - Prob. 107ECh. 9 - Consider the following data for xenon: Triple...Ch. 9 - Some of the physical properties of H2O and D2O are...Ch. 9 - Rationalize the following boiling points:Ch. 9 - Prob. 111AECh. 9 - Consider the following enthalpy changes:...Ch. 9 - Prob. 113AECh. 9 - Boron nitride (BN) exists in two forms. The first...Ch. 9 - Prob. 115AECh. 9 - Argon has a cubic closest packed structure as a...Ch. 9 - Prob. 117AECh. 9 - A 20.0-g sample of ice at 10.0C is mixed with...Ch. 9 - In regions with dry climates, evaporative coolers...Ch. 9 - The critical point of NH3 is 132C and 111 atm, and...Ch. 9 - Which of the following compound(s) exhibit only...Ch. 9 - Which of the following statements about...Ch. 9 - Prob. 123CWPCh. 9 - Aluminum has an atomic radius of 143 pm and forms...Ch. 9 - Pyrolusite is a mineral containing manganese ions...Ch. 9 - The structure of the compound K2O is best...Ch. 9 - Prob. 127CWPCh. 9 - Some ice cubes at 0c with a total mass of 403 g...Ch. 9 - The enthalpy of vaporization for acetone is 32.0...Ch. 9 - Prob. 130CWPCh. 9 - When I mole of benzene is vaporized at a constant...Ch. 9 - Prob. 132CPCh. 9 - Using the heats of fusion and vaporization for...Ch. 9 - Prob. 134CPCh. 9 - Consider two different organic compounds, each...Ch. 9 - Prob. 136CPCh. 9 - Prob. 137CPCh. 9 - Prob. 138CPCh. 9 - Prob. 139CPCh. 9 - Prob. 140CPCh. 9 - Mn crystallizes in the same type of cubic unit...Ch. 9 - Prob. 142CPCh. 9 - Some water is placed in a sealed glass container...Ch. 9 - The molar enthalpy of vaporization of water at 373...Ch. 9 - Prob. 145CPCh. 9 - Rubidium chloride has the sodium chloride...Ch. 9 - Prob. 147IPCh. 9 - A metal burns in air at 600c under high pressure...Ch. 9 - Prob. 149IPCh. 9 - General Zod has sold Lex Luthor what Zod claims to...
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