chapter 11 solids, liquids and gases - mr. morrow's …€¦ · · 2015-11-22solids, liquids...

© 2012 Pearson Education, Inc.

Chapter 11

SOLIDS, LIQUIDS

AND GASES


States of Matter

Because in the solid

and liquid states

particles are closer

together, we refer to

them as

________________

________________.


The States of Matter • The state of matter

a substance is (or are) depends on three “things” – ________________

– ________________

– ________________ ________________ ________________.


Bonding in Solids

• Which of the two

substance is an

amorphous

solid, pyrite or

obsidian?


Bonding in Solids

• There are four general

types of solids.

• ________solids share

a network of highly

delocalized electrons.

• ________solids are

sets of cations and

anions mutually

attracted to one

another.


Bonding in Solids

• ________________

solids are joined by an

extensive network of

covalent bonds.

• __________ solids

are discrete molecules

that are linked to one

another only by van

der Waals forces.


Metallic Bonding

• Why can metals be hit

with a hammer and not

break?

• Why are metals good

conductors of heat and

electricity?


Metallic Structure

Why do some metals when hit with a hammer

enough times start to tear?


Alloys

• Which of the above alloys is a

substitutional alloy and which

is an interstitial alloy?

• Which is more malleable?


Ionic Solids

The different-sized

ions in an ionic

compound _______

the distance

between oppositely

charged ions while

keeping ________-

charged ions away

from each other.


What determines the crystal structure in an ionic

solid? A. The size (radius) of the cation and the anion

B. Minimize repulsion between the cations (and also the anions)

C. Maximize attraction between the cations and anions

D. All of the above

Do the anions touch each other in any of these three

structures? If not, which ions do touch each other? A. Yes, if the anions are sufficiently large.

B. Yes, if the anions are sufficiently small.

C. No, because anions repel one another.

D. No, because each anion adopts different lattice points in the

unit cell.


Covalent-Network and

Molecular Solids

• __________are an

example of a

covalent-network

solid, in which

atoms are covalently

bonded to each

other.

– They tend to be hard

and have high

melting points.


Covalent-Network and

Molecular Solids

• __________ is an

example of a

molecular solid, in

which atoms are

held together with

van der Waals

forces.

– They tend to be

softer and have

lower melting points.


How many bonds does each carbon

atom in C60 make? Based on this

observation would you expect the

bonding in C60 to be more like that in

diamond or that in graphite?

A. Four bonds and bonding is like that in diamond.

B. Four bonds and bonding is like that in graphite.

C. Three bonds and bonding is like that in diamond.

D. Three bonds and bonding is like that in graphite.


Summarizing Intermolecular Forces


In which substance, benzene or toluene, are the

intermolecular forces stronger? In which substance do

the molecules pack more efficiently? A. Benzene possesses stronger intermolecular forces and has

molecules packed more efficiently.

B. Benzene possesses stronger intermolecular forces and toluene has


C. Toluene possesses stronger intermolecular forces and has


D. Toluene possesses stronger intermolecular forces and benzene

has molecules packed more efficiently.


Intermolecular Forces

The attractions between molecules ______

_______ nearly as strong as the

intramolecular attractions that hold

compounds together.


Intermolecular Forces vs

Intramolecular Forces

15.2 KJ/mol 427 KJ/mol


Intermolecular Forces

These intermolecular attractions are,

however, strong enough to control ________

properties, such as boiling and melting points,

vapor pressures, and viscosities.


London Dispersion Forces

Another helium

atom nearby, then,

would have a dipole

induced in it, as the

electrons on the left

side of helium atom

2 repel the electrons

in the cloud on

helium atom 1.


Factors Affecting London Forces

• The shape of the molecule

affects the strength of dispersion

forces: long, skinny molecules

(like n-pentane) tend to have

stronger dispersion forces than

short, fat ones (like neopentane).

• This is due to the increased

__________ ________ in n-

pentane.


Factors Affecting London

Forces

• The strength of

dispersion forces

tends to increase

with increased

molecular weight.

• Larger atoms have

larger electron

clouds that are

easier to ________.


How do the halogens indicate ldf strength?


Dipole–Dipole Interactions

The more _______ the molecule, the

higher its boiling point.


Which Have a Greater Effect? Dipole–Dipole Interactions or Dispersion Forces

• If two molecules are of comparable size

and shape, dipole–dipole interactions

will likely be the ____________ force.

• If one molecule is much larger than

another, ____________forces will likely

determine its physical properties.


Using the terms H-bonding, dipole-dipole interaction and

electronegativity explain the following trends in boiling point.


Which compound below is not

capable of forming hydrogen

bonds?

a. CH4

b. NH3

c. H2O

d. HF


To form a hydrogen bond what must the non-

hydrogen atom (N, O, or F) involved in the bond

possess?

A. The non-hydrogen atom must have a nonbonding electron pair.

B. The non-hydrogen atom must have low electronegativity.

C. The non-hydrogen atom must have a large atomic size.

D. The non-hydrogen atom must have a small electron affinity.


Which force below is the

strongest intermolecular

attractive force?

a. Hydrogen bonding

b. Ion-dipole forces

c. Dipole-dipole forces

d. London dispersion forces


A. CH3OH in water, because CH3OH is a strong

electrolyte and forms ions.

B. Ca(NO3)2 in water, because Ca(NO3)2 is a

strong electrolyte and forms ions.

C. CH3OH in water, because CH3OH is a weak

electrolyte and forms ions.

D. Ca(NO3)2 in water, because Ca(NO3)2 is a

weak electrolyte and forms ions.


Intermolecular Forces Affect

Many Physical Properties

The strength of the

attractions between

particles can greatly

affect the properties of

a substance or

______________.


Which element below has the

highest boiling point?

a. Kr

b. F2

c. Cl2

d. Br2


A. CH4 < CBr4 < CCl4

B. CCl4 < CH4 < CBr4

C. CH4 < CCl4 < CBr4

D. CBr4 < CCl4 < CH4


A. CBr4 because dispersion forces between its

molecules are greater than in CCl4 .

B. CBr4 because polar forces between its

molecules are smaller than in CCl4 .

C. CCl4 because polar forces between its

molecules are greater than in CBr4 .

D. CCl4 because dispersion forces between its

molecules are smaller than in CBr4 .


Surface Tension

Surface tension

results from the net

_________ force

experienced by the

molecules on the

surface of a liquid.


Viscosity

• Resistance of a liquid

to flow is called

_____________.

• It is related to the ease

with which molecules

can move past each

other.

• Viscosity _________

with stronger

intermolecular forces

and decreases with

higher temperature.


Which liquid below is the least

viscous?

a. water

b. hydrogen peroxide

c. glycerol (1,2,3-propanetriol)

d. all the above have equal

viscosity


A. Viscosity increases as intermolecular forces increase while

surface tension decreases. Both viscosity and surface tension

increase with increasing temperature.

B. Viscosity decreases as intermolecular forces increase while

surface tension increases. Both viscosity and surface tension

increase with decreasing temperature

C. Both viscosity and surface tension increase as intermolecular

forces increase and temperature decreases.

D. Both viscosity and surface tension decrease as intermolecular

forces increase and temperature increases.


Phase Changes


A. Melting (or fusion) and endothermic

B. Melting (or fusion) and exothermic

C. Freezing and endothermic

D. Freezing and exothermic


Energy Changes Associated

with Changes of State • The heat added to the

system at the melting

and boiling points goes

into pulling the

molecules farther apart

from each other.

• The temperature of the

substance does not rise

during a phase change.

http://www.kentchemistry.com/links/Matter/HeatingCurve.htm

http://www.kentchemistry.com/links/Matter/HeatingCurve.htm


Heating Curves

• Draw a heating curve for benzene (bp of 80 oC

and fp of 6 oC) if the heat added is equal.

http://s-owl.cengage.com/ebooks/vining_owlbook_prototype/ebook/ch5/Sect5-3-c.html


When heat is added to ice at

zero degrees Celsius, what

will happen?

a. The temperature will increase.

b. The temperature will decrease.

c. The temperature will not change.

d. A supercritical fluid will form.


Substance X has a boiling

point of 150 degrees F and a

freezing point of 15 degrees F.

The condensation point of X

a. is 150 degrees F.

b. is 15 degrees F.

c. is 165 degrees F.

d. is 135 degrees F.


As the temperature increases, does the rate of

molecules escaping into the gas phase increase

or decrease? A. Increases

B. Decreases


Energy Changes Associated

with Changes of State

What types of IMF can explain the heat of

phase change for each of the above

substances?


Isopropyl alcohol feels cool to

the touch because it has an

(X) heat of (Y).

a. X = exothermic, Y = vaporization

b. X = endothermic, Y = vaporization

c. X = exothermic, Y = fusion

d. X = endothermic, Y = fusion


The energy required to cause

a liquid to boil is called the

_______ of the liquid.

a. boiling point

b. freezing point

c. heat of vaporization

d. heat of fusion


Is it possible to calculate the heat of sublimation

for a substance given its heats of vaporization and

fusion? If so, what is the relationship?

A. No, because we are not dealing with state functions.

B. No, because we need heat of melting.

C. Yes, ΔHsub = ΔHfus + ΔHvap

D. Yes, ΔHsub = ΔHfus – ΔHvap


Use line angle formulas and the types of IMF to explain

the boiling point of the three organic liquids.

How can a small molecule like water, have a higher

boiling point than ether or ethanol?


What is the boiling point of water at the top of Mt.

Everest where atmospheric pressure is 400 mmHg ? A. 20 oC

B. 60 oC

C. 80 oC

D. 100oC

What is the vapor pressure of ethylene glycol at its

normal boiling point? A. 260 torr

B. 460 torr

C. 660 torr

D. 760 torr


Vapor Pressure

The natural log of the

vapor pressure of a liquid

is inversely proportional

to its temperature. The

slope of the line is called

the

___________________

equation:

ln P = −Hvap/RT + C,

where C is a constant


Vapor Pressure

The liquid and vapor

reach a state of

________________:

liquid molecules

evaporate and vapor

molecules condense

at the same rate.


What does a phase diagram

show about a substance?


Phase Diagram of Water


The temperature and pressure

at which all three phases exist

simultaneously is called the

_______ point of a substance.

a. boiling

b. freezing

c. triple

d. critical


If the pressure exerted on a water is increased,

while the temperature is held constant at 0 oC,

what type of phase transition will eventually

occur? A. Freezing

B. Melting

C. Vaporization

D. Condensation

If the temperature of water is increased from -20 oC to 120 oC, while the pressure is held constant,

what type of phase transition will occur? A. Melting

B. Vaporization

C. Both of the above

D. Neither of the above


Which substance below has a

greater density in its liquid

state than in its solid state?

a. Iron

b. Glass

c. Water

d. Carbon dioxide


For a given substance, do you expect the density

of the substance in its liquid state to be closer to

the density in the gaseous state or in the solid

state?

A. Closer to the density of a gas

B. Closer to the density of a solid

C. Both are somewhat close to one another in density.

D. They are significantly different in density.


Why is the boiling point of SnH4 higher than that

of CH4?

A. SnH4 is more polar than CH4.

B. SnH4 is smaller in size than CH4.

C. SnH4 has greater internal dispersion forces than in CH4.

D. SnH4 is ionic in structure and CH4 is molecular.


Which compound below has

the highest boiling point?

a. H2O

b. H2S

c. H2Se

d. H2Te


If the inside surface of each tube were coated with

wax, would the general shape of the water

meniscus change? Would the general shape of

the mercury meniscus change?

Shape of Water Meniscus Shape of Hg Meniscus

A. Yes, Inverted U Yes, downward U

B. No change Yes, downward U

C. No change No change

D. Yes, Inverted U No change

chapter 11 solids, liquids and gases - mr. morrow's …€¦ · · 2015-11-22solids, liquids...

Documents