Download Chapter 10 – States of Matter

Hemet High  Honors Chemistry
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Chapter 10 Homework Packet
Date
Assigned
Date
Due
Assignment
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All Notes Completed and Attached
___/10
Ch 10.1 pg 332 #2-6
Ch 10.2 pg 336 #4-6
Ch 10.3 pg 341 #2
Ch 10.4 pg 348 #5, 6
Ch 10.5 pg 351 #4, 6
and practice problems #1-2
Chapter 10 Review Worksheet
Due End of Class Today!
Final Packet
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Hemet High  Chemistry
10  States of Matter
Notes
Section 1: The Kinetic Molecular Theory of Matter

Based on the idea that particles of matter are always in _______________.
How it relates to gases:

____________________ = a hypothetical gas that perfectly fits all the assumptions of the KMT.
o No ideal gases actually exist; some come close though, which is why we learn this.

5 Assumptions
o Gases consist of large numbers of tiny particles that are far apart relative to their size.
o Collisions between gas particles and between particles and container walls are elastic collisions.
There is no net loss of total _____________________.
o Gas particles are in continuous, rapid, random _________. Thus, they possess kinetic energy.
o There are no forces of _________________ between gas particles.
o The ______________ of the gas depends on the average kinetic energy of the particles of the gas.
Properties of Gases:

No Definite ______________

Ability to be compressed _______________

No Definite ______________

_______________

Ability to _________ (fluid)

Effusion

_________ Density
Real Gases

A gas that does not behave completely according to the assumptions of the __________________.

___________ gases and _____________ diatomic gases behave most like an ideal gas, as well as gases at
high ___________________ and low _____________________.
Section 2 and 3: Liquids and Solids
Properties of Liquids:

No Definite _____________

____________ Tension

___________ density

Evaporation

Mostly incompressible, so definite _______

____________

Diffusion

Can Form ____________
Properties of Solids:

Definite _________

________ Density

Definite ___________

Incompressible

Defined _____________ Point

______ Rate of Diffusion
Type of Solids:


Crystalline Solids
o __________ Crystals
o __________ Crystals
o Covalent ____________ Crystals
o Covalent ___________ Crystals
Amorphous Solids
o Glass and ___________
Section 4: Changes of State
Matter on earth can exist in any state—gas, ______, or solid—and can change from one state to another.
The Possible changes of state are:
Change of State
Solid  Liquid
Solid  Gas
Liquid  Solid
Liquid  Gas
Gas  Solid
Gas  Liquid
Process
Example
Ice  Water
Dry Ice  CO2 Gas
Water  Ice
Water  Steam
Water Vapor  Ice
Water Vapor  Water
Endo or Exo?
Phase Diagram

A graph of _____________ versus ______________ that shows the conditions under which the phases of a
substance exist.

Tells you what __________ a substance will be in at a certain temperature and pressure.

______________________: the temperature and pressure conditions at which the solid, liquid, and vapor
phases of the substance can coexist at equilibrium.

______________________: the critical temperature and critical pressure of a substance.

______________________: the temperature above which the substance cannot exist as a liquid.

______________________: the lowest pressure at which the substance can exist as a liquid.
Phase Diagram of H2O
In which state is water at the following Temperatures and
Pressures?
Temperature Pressure
70°C
2.0 atm
100°C
0.5 atm
0°C
1.0 atm
State
Section 5: Changes of State
Structure of Water

Recall: Water has ____ Hydrogen and ____ Oxygen and has a ________ structure.

Ice forms a hexagonal pattern: Look at Fig 19 on pg 350

The empty spaces result in ice’s low density and are why it ___________.
Properties of Water

Pure water is transparent, _____________, tasteless and almost ___________________.

Water freezes and ice melts at 0°C and 1 atm.

Water boils at 100°C and 1 atm.

Molar enthalpy of fusion is 6.009 kJ/mol

Molar enthalpy of vaporization is 40.79 kJ/mol

Going from ice to water ___________ energy.

Going from water to steam __________ energy.

Going from water to ice ___________ energy.

Going from steam to water __________ energy.
The amount of energy is the ___________, it is just either required or released.
Calculating Amount of Energy
What quantity of energy is released when 804 g of water vapor condenses?
Calculating Mass from Energy
What mass of ice is required to release 2000 kJ of energy when melting?