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Unit 14: States of Matter

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Name: __________________________________ Date:__________________ Class period:_____

Unit 14: States of Matter

14.1 The Kinetic Theory of Gases

The word __________________ means __________________. The Kinetic Molecular Theory (KMT) of Matter says:

________________________________________________________________________________ ________________________________________________________________________________

• Even in _______________, but it’s so slight that it is hard for us to see.

KINETIC MOLECULAR THEORY OF GASES

The word “gas” comes from the Greek word meaning “chaos.”

Numerous experiments have led to evidence that suggests the following behaviors of gas particles at the atomic level…

Major Postulates of KMT of Gases

1. Gases are made up of __________________________________________________________ _____________________________________________________________________________ 2. These particles are considered to have __________________________________________.

• Gas particles are ___________________ than the distance between particles. • Gases are mostly ____________________________.

• Gases __________________________________________________________________. 3. Gas particles have zero ________________________________________________________.

• Gases ______________________________________________ and/or the walls of a container.

*** There _______________________________________________________________________ ________________________________________________________________________________ 4. Gas particle move with ________________________________________________________. • Gas particles move ________________________________________________________. • Particles continue moving in ________________________________________________

until they __________________ with another particle or the wall of a container. this is why ________________________________________________________________ • We call this the “________________________.” Gas particles will move in a ________

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• Particles move ______________________________________________, this is why _______________________________________________________________________.

- The word “_______________” means _________________________________ • Example:__________________________________________________________________

__________________________________________________________________________ __________________________________________________________________________ __________________________________________________________________________ __________________________________________________________________________ 5. All collisions between gas particles are __________________, meaning ________________ _____________________________________________________________________________ • Kinetic energy (KE) _________________________________________________________ __________________________________________________________________________

6.

The _______________________________________________ of a collection of

gas particles depends on the ______________________________________

and nothing else.

Gas Pressure

Gas Pressure is caused by the ______________________________________________________ ________________________________________________________________________________

• As the number of collisions ___________________, pressure will ___________________ More collisions will result if…

• There are _________________________________________________________________ • As temperature _____________________, pressure will __________________, because particles are colliding with each other and the walls of the container more frequently. A region of space where no gas pressure is exerted is called a __________________________

• Gas pressure is equal to zero, so there are _____________________________________ • Example: Peeps! J

Atmospheric pressure (atm) ______________________________________________________ ________________________________________________________________________________

• There are changes based on altitude and other weather conditions.

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Standard Pressure is the __________________ pressure as measured at sea level. • Standard pressure equals __________ quantities. These

equalities all represent the same thing just with different units. Standard Pressure = ______ atm (atmosphere)

= ______ mm Hg (millimeters of Hg) = ______ torr (old school chemistry) = ______ kPa (kilopascal)

A barometer is _______________________________________________ _____________________________________________________________

14.2 Temperature and Pressure Basics

Recall, gas pressure is caused by ___________________________________________________ ________________________________________________________________________________ Pressure can be measured in three different units: ___________________________

Conversions with Pressure Units

All pressure conversions ___________________________________________________________ Example: The pressure inside a balloon is 4.17atm, how many kPa is this?

What conversion factor are you using? _____atm = _____mm Hg = _____ torr = _____ kPa

Kinetic Energy and Temperature

Temperature is really ____________________________________________________________ ________________________________________________________________________________ • But not all particles in the sample have the _________________ amount of KE.

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• Some particles move _________________ than average

• Some particles move _________________ than average.

Average KE

is____________________________________________________________________ • The formula to calculate temperatures in Kelvin is:

• Kelvin is never ________________________________________________________________ Example: Room temperature is 25°C. What is this in Kelvin?

As temperature __________________________________________________________________ • The particles would theoretically ________________________________________________ _____________________________________________________________________________ • _____________________________________________________________________________

Standard Temperature

• Recall, STP ___________________________________________________________________ • Equals ________________ or ________________.

Calculating the factor by which KE changes

Since KE is directly proportional to the Kelvin temperature, the factor by which KE increases or decreases can be easily calculated.

Examples: Calculate the factor by which the average KE will change.

If temperature goes from 200K à 400K, then the average KE will __________________. 400/200 = _____

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If temperature goes from 100K à 300K, then the average KE will __________________. 300/100 = _____ If temperature goes from 300K à 100K, then the average KE will __________________.

100/300 = _____ If temperature goes from -73°C à 127°C, then the average KE will _________________.

_____/_____ = _____ 14.3 The Kinetic Theory of Liquids

Holding molecules together

_______________________________ are forces of attraction that hold separate molecules together.

• As opposed to _______________________________ which hold atoms together in an individual molecule (i.e. bonding)

• IM forces have a huge effect on the physical properties of matter. Specifically, __________________________________________________________________. There are _______ types of IM forces but we are going to focus on ______. (Listed in order, weakest to strongest):

1. 2. 3. 4.

London (Dispersion) Forces

• ___________ are always moving, at any given time electrons in a molecule could be on any side of the molecule and can cause ______________ and _____________ partial ________________ and partial _________________ charges on the molecule.

- These temporary tiny charges can weakly attract one another. - London Forces are ___________________.

- London Forces exist in ________________________________________ as well. • Molecules with only London Forces have low ___________________________

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Dipole-Dipole Interactions

• In _____________________ the molecules tend to orient themselves in a way that __________________________ of a molecule are close to the

________________________ of another molecule. - __________ than London Forces.

- ____________ partial charges while London Dispersion Forces are ____________ • Molecules with Dipole-Dipole Interactions also have _____________________________

and have ____________________________________ higher than molecules with only London Forces

• Examples: HCl, CO, NH3

Hydrogen Bonding (___________________________________________________)

• Unusually strong __________________________________ which occurs in substances where ___________________________________________________________________. • Hydrogen has almost a full _________________________ and the more electronegative

elements have a very ______________________________________.

• The __________________ hydrogen is attracted to the ________________________> • Example: H2O, Ethanol (CH3CH2OH)

Summary of IM Forces:

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• The forces of attraction in a liquid are ___________________________________________ _____________________________________________________________________________ • The intermolecular (IM) forces of attraction _______________________________________ _____________________________________________________________________________ Particles in a liquid _______________________________________________________ and have the ability to __________________________.

• Liquids and gases can flow, but _________________________________________________ _____________________________________________________________________________ • The particles of gases have the ____________________ amount of KE and solids have the

____________________. A liquid’s KE is in between that of solids and gases.

• Liquids tend to _______________________________________________________________ They change from ________________ to ________________.

Evaporation of Liquids

________________________________________________________________________________ ________________________________________________________________________________ In order to evaporate, ____________________________________________________________ ________________________________________________________________________________ ________________________________________________________________________________ • As particles with the highest KE evaporate away from liquids, _____________________

_____________________________________________________________________________

Kinetic Energy vs. # of Particles

Heat: Flows from warmer to cooler objects.

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_____________________________________________________________________________ • Evaporation is a “_________________________________.” The particles that move the

fastest ________________ and __________________ the average kinetic energy. Example: When you sweat! J

Evaporation in a Closed Container

In a closed container particles will still _____________________________________________ ________________________________________________________________________________ • As gas particles build in concentration, they are more likely to ______________ with each other. Then they _____________________________________________________________ _____________________________________________________________________________

14.4 The Kinetic Theory of Liquids: V.P. and B.P.

Vapor Pressure (V.P.)

________________________________________________________________________________ ________________________________________________________________________________ • With a lid, the vapor will be ____________________________________________________ • Without the lid, the particles will ___________________.

Vapor Pressure and Temperature

As temperature ___________________, vapor pressure will ___________________.

• This occurs ___________________________________________________________________ ____________________________________________________________________________ • There is a __________________ relationship.

As IM forces in a liquid _____________________, the __________________________________ • As forces of attraction _________________________________________________________ _____________________________________________________________________________

There is an _____________________ relationship.

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Boiling Point (B.P.)

________________________________________________________________________________ • Boiling is _____________________________________________________________________ _____________________________________________________________________________ • Recall, evaporation is a conversion from liquid to gas at the ________________________. In order to boil:

Normal Boiling Point (n.B.P.)

________________________________________________________________________________ • _____________________________________________________________________________

_____________________________________________________________________________

Boiling point is __________________________________________________________________ • When there is _____________ atmospheric pressure, B.P. __________________

• Where there is ____________ atmospheric pressure, B.P. __________________ Recall, when a substance is boiling, temperature remains __________________. (In any phase change, temperature is constant.)

• At the boiling point, ___________________________________________________________ _____________________________________________________________________________ • Boiling can also occur by _______________________________________________________

_____________________________________________________________________________ =

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14.5 The Kinetic Theory of Solids

In the solid state, ________________________________________________________________ The IM forces ____________________________________________________________________ ________________________________________________________________________________ The particles in the solid state are _________________________________________________ • The particles ___________________________________ and do not ___________________.

Two Types of Solids:

1. Crystalline: __________________________________________________________________ _____________________________________________________________________________ • Example: ______________________________________

2. Amorphous: _________________________________________________________________ • Example: ______________________________________

Types of Crystalline and Amorphous Solids

Ionic: (________________ and _________________) ___________________________________ ________________________________________________________________________________ • Are always ___________________________________________________________________ • _____________________________________________________________________________ Molecular: (_____________________) _______________________________________________ ________________________________________________________________________________ • The IM forces for ______________________________________________________________ _____________________________________________________________________________ • _____________________________________________________________________________

Phase Changes for Solids

A solid will ____________ when the particles in the solid state __________________________ ________________________________________________________________________________ • The temperature at which this occurs is called the _________________________________ • Since IM forces are ________________ in ionic solids, they will have __________________

than molecular solids.

Sublimation

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________________________________________________________________________________ • The reverse process is called ____________________________________________________ • Sublimation occurs when _______________________________________________________

_____________________________________________________________________________

• The vapor pressure of solids is usually _____________________ than the VP of liquids. • VP will increase if the solid is _________________. However, most substances will melt

______________ the vapor pressure = atmospheric pressure. (This is why sublimation is difficult.)

• It is easier to get a solid to sublime by ___________________________________________ • Dry ice sublimates at room temperature and pressure because _______________________

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Two Types of Phase Diagrams

1. Liquid state is more dense than the solid state (Example: ________________________) 2. Solid state is more dense than the liquid state (Example: ________________________) • If the solid/liquid line slants to the ______________________________________________ _____________________________________________________________________________

References

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