chapter 9: states of matter name: chapter notes & …jimchatt.com/ch9.xmas.ex.pdfchapter 9:...

7

Click here to load reader

Upload: truongliem

Post on 13-Jul-2018

212 views

Category:

Documents


0 download

TRANSCRIPT

Page 1: Chapter 9: States of Matter Name: Chapter Notes & …jimchatt.com/ch9.xmas.ex.pdfChapter 9: States of Matter Name:_____ Chapter Notes & Exercise: A) Kinetic Theory & the Nature of

Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry

=================================================== page 1

Chapter 9: States of Matter Name:_______________________ Chapter Notes & Exercise:

A) Kinetic Theory & the Nature of Gases:

- molecules spread through space because of the kinetic theory; what does this theory basically say: …………………………………………………………………………………………………..

- The first basic assumption of the kinetic theory is that a gas is composed of molecular or atomic particles.

- T/F: ___ There is a force of attraction/repulsion between the particles. - T/F: ___ The particles are hard, with little volume and very far apart. - The second assumption states: ………………………………………………………………… - Finally, all particle collisions are elastic meaning that………………………………………… - If a bottle of perfume is opened in Vancouver, B.C., in 3 hours the gas particles will be in

Washington, D.C. (T/F) …. Why not, if false? ……………………………………………….. - What 2 things affect the volume of a gas? …………………………………………………….

B) Kinetic Energy & Temperature: - The energy an object has because of its motion is termed ……………………………….. - In a collection of molecules, some have very high and very low speeds. As a result, scientists

use the ………………………………….. This energy is proportional to the ………………….. of the substances. Particles of substances at the same temperature have the same …………………………..

- What can be said of the average energies in a block of ice at 0°C and the energy in a gas filled dirigible at 0°C? ………………………………………………………………………………………

- What is different between molecules at high temperature compared to molecules at low temperatures when compared in an energy distribution curve? ……………………………………………………

- What is the temperature called when the motion of molecules ceases? …………………………….

- What is superconductivity? ………………………………………………………………………….

- Diamagnetism results in what phenomena? ………………….. Which means what? ………………………………………………………………………………………………….

- Why is the Kelvin scale so useful? …………………………………………………………………

Page 2: Chapter 9: States of Matter Name: Chapter Notes & …jimchatt.com/ch9.xmas.ex.pdfChapter 9: States of Matter Name:_____ Chapter Notes & Exercise: A) Kinetic Theory & the Nature of

Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry

=================================================== page 2

C) Pressure: - The result of simultaneous collisions of billions upon billions of gas particles upon an object

is termed ………………………………… - If no gas particles are present, this is termed a ……………………………… . Commonly

used to measure atmospheric pressure is the ……………………………………… - STP stands for ……………………………………………. Numerically, this is equivalent

to……………… and a pressure of ……………. - The inventor of the barometer was _______________________________ - Equivalences: 1 atm = ______ kPa = ______ mm = ______ cm = ______ torr - 190 mm = _______ kPa - Why, on the top of Mt. Everest, does air pressure support a column of mercury that is only

253 mm high? _______________________________________________________________________

- Today’s barometers do not contain mercury but are based on a metal diaphragm controlling a pointer. They are called ________________ barometers.

D) Avogadro’s Hypothesis: - Avogadro’s hypothesis states

that:___________________________________________________ ___________________________________________________________________________

- One mole of any gas at STP occupies what volume? _____________ - Find the volume of a container that holds 10.0 g of CO2 at STP?

- What is the volume occupied by 0.50 mol of a gas at STP?

- A gas has a volume of 2.24 L at STP. How many moles of gas is this?

E) The Nature of Liquids: - Unlike gases, the particles of liquids are held together by ___________________ forces.

These forces also reduce the _________ between the particles. Both liquids and gases ______.

- Liquids are much ___________ than gases. - Increasing the ______________ on liquids has hardly any affect on their volumes. Hence,

liquids and solids are known as _____________________________ of matter. - Particles in a liquid do no usually escape from the liquid by themselves because of the

__________________ forces between them. - Properties of liquids are based on the _____________ motion of the particles and the

____________ forces between the particles.

Page 3: Chapter 9: States of Matter Name: Chapter Notes & …jimchatt.com/ch9.xmas.ex.pdfChapter 9: States of Matter Name:_____ Chapter Notes & Exercise: A) Kinetic Theory & the Nature of

Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry

=================================================== page 3

F) Vaporization: - The conversion of a liquid to a gas or a vapor below its boiling point is termed

_______________. When this process occurs with an uncontained liquid, it is termed _______________.

- T/F: ___ Equilibrium cannot be established in an open container when a liquid’s molecules evaporate from its surface.

- What method should be used in the laboratory to evaporate flammable liquids? - _________________________________________________________________________ - Why does heating a liquid allow it to evaporate faster? _____________________________

_________________________________________________________________________ - If the liquid in a closed container begins to evaporate and condense at the same rate, we say

that the system is in _______________________.It is actually termed to be ____________. - As vaporized particles collide with the walls of a sealed container, they produce what is

called a _____________________ above the liquid. - T/F: ____ A terrarium exhibits equilibrium. - It is general knowledge that liquids, upon evaporating, create a vapor pressure. (T/F) ____

The same can be said about solids. The general rule is that increases in temperature will _____________ the vapor pressure.

- Similar to a barometer is a _____________ which can also be used to measure the pressure of a gas sample.

- Draw a small graph to illustrate this fact based on the temperatures (°C) and vapor pressures (kPa) for ethanol:

-

Temperature (°C)

Page 4: Chapter 9: States of Matter Name: Chapter Notes & …jimchatt.com/ch9.xmas.ex.pdfChapter 9: States of Matter Name:_____ Chapter Notes & Exercise: A) Kinetic Theory & the Nature of

Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry

=================================================== page 4

G) The Boiling Point of a Liquid: (read continuously going across) - The temperature at which the vapor pressure of the liquid is just equal to the external

pressure is termed the ___________________. (bp) The vapor begins to escape to the atmosphere and this stage marks the onset of ______________.

- Evaporation is the process that occurs only at the _____________ of a liquid whereas boiling occurs _______________ the liquid.

- The boiling point of a liquid at a pressure of 101 kPa is called the ____________________________

- The boiling point of a liquid changes with __________________ changes. - The boiling point will decrease with lower ___________________ since the particles will

need less kinetic energy to escape from the liquid. - What is the boiling point of ethanol and its formula?

_________________________________ - At about what temperature would ethanol boil in Banff where the atmospheric pressure is

89.3 kPa? _______________ (use graph on page 208) - T/F: ____ The temperature of a boiling liquid never rises above its boiling point. - Why do pressure cookers reduce cooking time?

__________________________________________ - A pressure cooker is similar to an _________________ which is used to sterilize medical

instruments. - Usually, when solids melt, they change from an orderly pattern to a more disorderly pattern.

What are substances called that flow like liquids yet are still orderly? ______________________

- The molecules in these substances are shaped like rods with the rods organized in 3 different ways. The _________ substances contain rod like molecules that are parallel to each other. In _____________ substances, the rods are parallel and in layers, moving back and forth with certain molecules stationary in the layer. In ___________________ crystal liquids, the moving molecules are in layers, parallel to each other in the layers but each layer is not parallel to the other layers.

- What 2 things determine the color & color changes in the crystals? ____________________ - In a calculator, what types of liquid crystals are used? ______________ . The crystals,

sandwiched between 2 layers of glass, are oriented to prevent light from passing through which we see as the numbers. This is due to the top layer of glass being ______________ied causing segmentation for the numbers.

H) The Nature of Solids:

- What is the motion of molecules in a solid? _______________________________________ - How are vibrations, increased temperature and kinetic energy related to the (mp) of a solid?

___________________________________________________________________________

Page 5: Chapter 9: States of Matter Name: Chapter Notes & …jimchatt.com/ch9.xmas.ex.pdfChapter 9: States of Matter Name:_____ Chapter Notes & Exercise: A) Kinetic Theory & the Nature of

Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry

=================================================== page 5

- Why do ionic solids have high (mp)? _______________________________________

whereas ______________ have relatively low melting points. (T/F) ____ Wood melts when heated.

- Most solids are _________________ in nature. The atoms, ions or molecules are arranged in an orderly, repeating, 3-D pattern in _________________.

- This arrangement/array is called a _______________________. - Crystal solids occur in ___ crystal systems depending upon the ______ between the faces and

how many of the edges are _________. - The smallest group of particles within a crystal that retains the geometric shape of the crystal

is called a ____________________. The lattice is one of fourteen types of these. The seven types of crystal systems are : 1)___________________ 2) ___________________ 3) __________________ 4) _____________________ 5) _______________________ 6) _____________________ and 7) ________________________.

- __________ is an example of an element that can exist in more than one type of solid state. - The three types are _________________, _________________ and _____________. - Solids that lack an ordered internal structure are called _______________ such as soot,

rubber, plastic and asphalt. - Glasses are amorphous solids called _______________________. They are transparent,

fusion products, of inorganic materials, cooled to a solid, but not having crystallized. Glasses do not have a definite __________.

- When crystalline substances break the pieces have surface ________ the same as the original but glasses, being ________________, do not.

I) Phase Changes: - These occur when the physical state of a substance changes. What does not change when the

physical change is occurring is the __________________. - An element that sublimates is _______________, going from a solid to gas without going

through the liquid state.

J) Energy and Phase Changes: - What does the number 4.19 really tell you? _______________________________________ - What does the slope on a heating curve tell one? ___________________________________ - The heat required to melt 1 g of a solid at its melting point is its _______________________. - The amount of heat given up as 1 g of liquid changes to a solid at the melting point is called

the heat of _______________________. We likewise have the heat of vaporization and the heat of condensation.

- When a gas is heated to a very high temperature, the molecules will separate into _____. Next, upon continued heating, the __________ will separate from the atoms. This forms a mixture of ____________ and positive _______ formed from the _________ of the atom. We now have the 4th state of matter termed __________________.

- The creation of highly ionized plasmas requires a lot of _________ and high __________________.

Page 6: Chapter 9: States of Matter Name: Chapter Notes & …jimchatt.com/ch9.xmas.ex.pdfChapter 9: States of Matter Name:_____ Chapter Notes & Exercise: A) Kinetic Theory & the Nature of

Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry

=================================================== page 6

- Since no known material can contain plasma at these high temperatures, scientists use strong____________________________ in a device called a ________________ to confine the plasma.

- Metal surfaces could be coated with protective coverings because of plasma’s _______________ property. Because plasma conducts___________ and creates a _____________ field, plasma could be used to make __________ and ____________________.

- An alternative form of electricity generation could come about from MHD or___________________________. This is an expanding field of plasma _____________.

Review Questions: circle the best answer

1. How far can a molecule travel in the air before it collides with another molecule? a. much less than a metre b. about a metre c. much more than a metre

2. What is the SI unit of pressure? a. candela b. mole c. Pascal d. Newton e. Joule

3. What happens to the range of energies of the molecules in matter when the temperature is increased? a. it becomes narrower b. it becomes broader c. it does not change 4. Which temperature scale provides a direct measure of the average kinetic energy of a substance? a. Celsius b. Fahrenheit c. Kelvin 5. How does the atmospheric pressure at altitude below sea level compare with atmospheric pressure at sea

level? a. the atmospheric pressure below sea level is higher b. the atmospheric pressure below sea level is lower c. the pressures are the same 6. What is the volume occupied by 1.8 X 10 23 molecules of fluorine at STP? a. 22.4 L b. 44.8 L c. 56.0 L d. 67.2 L e. 78.4 L 7. What types of forces exist between particles of a liquid? a. weak attractive forces b. strong attractive forces c. weak repulsive forces d. strong repulsive forces 8. Which of the following will evaporate fastest? a. water at 0 degrees C b. 20 c. 40 d. all of the following evaporate at the same rate 9. What is the pressure when a liquid is boiling at its normal boiling point? a. 0 atm b. 1 atm c. 2 atm d. 5 atm 10. If heat is added to a boiling liquid, what happens to the temperature of the liquid? a. it increases b. it decreases c. it does not change 11. Liquid crystals are characterized by….. a. sharp melting points b. a disorganized structure c. the ability to flow d. covalent bonding 12. What happens to the evaporation rate of a liquid as the liquid is cooled? a. it increases b. it decreases c. it is unchanged 13. When the external pressure is 5 atm, what is the vapor pressure of water at its boiling point? a. 0 atm b. 1 atm c. 5 atm d. 10 atm 14. The boiling points of ionic solids tend to be…. a. low b. high c. average 15. Which of the following forms of carbon is an amorphous solid? a. diamond b. graphite c. soot 16. Crystals are characterized by particular patterns that repeat…. a. in 1-D b. in 2-D c. in 3-D 17. What is plasma? a. an ionized gas b. a charged solid c. a supercooled gas d. a superheated liquid crystal 18. Molecules in liquid crystals are usually in the shape of… a. spheres b. rods c. corkscrews d. cubes 19. In dynamic equilibrium between the liquid state and the gas state, the rate of evaporation is… a. greater than the rate of condensation b. less than the rate of condensation c. equal to the rate of condensation

Page 7: Chapter 9: States of Matter Name: Chapter Notes & …jimchatt.com/ch9.xmas.ex.pdfChapter 9: States of Matter Name:_____ Chapter Notes & Exercise: A) Kinetic Theory & the Nature of

Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry 534 Chemistry

=================================================== page 7