tuesday may 25, 2010 (review for semester final) (day 1)

TuesdayMay 25, 2010

(Review for Semester Final)(Day 1)

Bell RingerTuesday, 5/25/10

No Bell Ringer Today.

Semester Exam Information• If your score is higher on the EOC than on the

semester exam, your may take your EOC grade as your semester exam grade.

• Semester Exam Exemptions– If you passed the Science TAKS test, you may choose

to be exempt from the semester final exam. You may take your second semester average as your exam grade, but only if by doing so you pass the course. If you choose to go ahead and take the exam, you will receive the higher of the two grades. You must report to class during the exam period. This option applies to sophomores and juniors only.

– If you have a spring semester average of 85 or higher at the end of the fifth week of the final six-weeks and have been absent 2 or fewer days this semester, you may take your second semester average as your exam grade. This option applies to juniors and seniors only.

Assignment Currently Open Page

Date of Notes on Website

Date Issued Date Into GradeSpeed

Date Due

WS: Organic Chemistry 161 5/10 5/11 5/18 5/25

Review for Final Exam

(Day 1)

1The Kinetic-

Molecular Theory of Matter is based upon what idea?Particles of

matter are always in motion.

•

2The average kinetic

energy of gas particles depends upon the

_________________ of the gas.

temperature

3Which of the

common phases of matter has the lowest density?gases

4Which of the

common phases of matter is the most

compressible?gases

5Give an example of the

diffusion of a gas.smelling breakfast

cooking in the next room

6The force of the collisions of gas

particles against the inside walls of their container is called

_______.pressure

786.34 kilopascals of pressure is how

many atmospheres?1 atm = 101.325

kPa0.8521 atm

8The pressure exerted on a 650. mL sample of oxygen gas at

constant temperature is increased from 0.285 atm to

0.785 atm. What will the final volume of the sample be?

Law? Formula?Boyle’s Law

P1V1 = P2V2

236 mL P1V1 / P2 = V20.285 x 650. / 0.785 =

V2

9A sample of fluorine gas at 22oC and 3.03 atm occupies a volume of 5.12 L. What

volume would this gas occupy at 66oC and 0.650

atm?Law? Formula?

Combined Law

P1V1/T1 = P2V2/T2

27.4 L

P1V1T2 = P2V2T1P1V1T2/P2T1 = V2

3.03x5.12x339/0.650x295 = V2

10How many moles of oxygen gas

are there if the gas has a volume of 4.50 L, a pressure of 2.50 atm,

and a temperature of 40oC?Law? Formula?Ideal Gas

LawPV = nRT

0.440 mol

PV / RT = n2.50x4.50 /

0.0821x313 = n

11The insect in this picture is able to

stand on the surface of the water because

the force of the surface tension on the water’s

surface is stronger than the pull of gravity

on the insect.

12 If the attractive forces

between water molecules in the liquid phase become much stronger, the liquid

water will freeze into ice.

13According to the density column in

the picture, which of the materials is

the most dense?

glycerinthe least

dense?

cork

14A student discovers that the

sample of matter she is working with is incompressible, has an

extremely low rate of diffusion, and has a high density. What is most likely the identity of her

material?a solid

15Water normally boils at 100°C at sea level and at 97°C on a

North American mountaintop. This difference in boiling points

can be explained by the difference between the

locations’ air pressure.

16The picture shows the results of

pouring a blue liquid into a clear

liquid and allowing the mixture to settle for 25

minutes. Compared to the clear liquid, the

blue liquid is more

dense.

17Clouds are formed when

water vapor in the atmosphere changes into

tiny droplets of liquid water. This is the process

of Condensation.

18According to the diagram, if water boils at 1000C,

the pressure will be

1.00 atm

19Water is a very effective

solvent because it is a polar

molecule.

+ +

-

20Name a common instance

that proves that solid water is less dense than liquid

water.

Ice floats in liquid water.

21 If a student is trying to

determine the saturation point of a solid solute in a liquid

solvent, what factors would he most be concerned with?the nature (identity) of the solute and

solvent and the temperature of the solvent.

22 According to the chart, how many grams of sodium nitrate

(NaNO3) will dissolve in

100 grams of water when the water is

at a temperature

of 57oC?

about 120 grams

23What factor will most

directly affect the solubility of a solid in a

liquid? the temperature of

the solvent

24A fish is living in a small pond. One

night in November the air temperature falls from 74oF to 43oF. The water

temperature decreases as a result. What is a major change that will most

likely occur in the fish’s life? The colder water will now hold more oxygen gas and the fish will not have

to work as hard to get enough.

25List the factors that would

increase the amount of solid solute that will dissolve in a

liquid solvent.increase the temperature of the solvent

add more solvent

26What is the main

difference between the three types of mixtures: solutions, colloids and

suspensions?the size the solute particles are broken

down to in the dissolving process

27The table shows properties of four

liquids that are insoluble in water. If the four liquids are poured into a

beaker containing water, which liquid will form a layer below the water?Liquid

Q

28Why will

gasoline not dissolve in

water? Gasoline is a non-polar solute and water is a polar

solvent.

29Why does saltwater conduct

electrical current? water breaks the salt into charged

ions, which conduct current.

30If a student dissolves 1.5 moles of NaCl in water and makes 4.0 liters of a saltwater solution, what is the

molarity of the solution?

M = 0.38

M = mol solute / L solution

31What is occurring in the equation below?

HCl æ H+ + Cl- HCl is being ionized by

water.

H2O

32In the equation below, Compound X is

Compound X æ H+ + an anion-an

acid.

H2O

33What is true of an acid in

regards to ion concentration?

[H+] > [OH-]

34List three common household items that can

be classified as acids.Battery acidLemon

juiceVinega

r

35 Name the following

acid: H2SO4 sulfuric acid

36 When the indicator

bromthymol blue is added to HCl, it changes color from blue to yellow. When it is added to NaOH it remains blue. What

does this indicate?Bromthymol blue is an acid-

only indicator.

37A student has a solution that tastes bitter, feels slippery, and is a weak electrolyte.

What is most likely the identity of her solution?a base

38Which ion, H+ or OH-, is present in greater number in vinegar at a pH of 5, and how many more ions of this

type are there than the other type? H+ is present in greater number.

There are 100x more H + ions than OH- ions at a pH of 5.

39Which of the following statements

is the most accurate? Soap and shampoo are acidic, while oranges and lemons are basic.

The foods we eat can contain many different types of acids, whereas household cleaning supplies can contain bases.

Acids are always safe to taste as long as you don’t taste too much.

All bases are harmful and should never be touched.

40List three

environmental problems caused by

acid rain.the deterioration of buildings and

statues.

the killing of plants and animals in a forest.

the killing of plants and animals in rivers and streams.

41Can you make an element

(like gold) from other elements? Explain.

Yes, you can make gold atoms from other atoms, but only in vary small

amounts.

42Name a pair of elements that could undergo nuclear

fusion to produce gold.Any elements

that have atomic

numbers that total 79, like iridium and

helium

43List two examples each of nuclear

fission and nuclear fusion.Fission

a submarine using a nuclear reactor

for powerthe explosion of an atomic-bomb

Fusionthe Sun

generating heat and light

the explosion of a hydrogen-bomb

44What parts of the atom participate

directly in a nuclear reaction?protons and

neutrons

45Which one of the

following is not a result of a nuclear reaction? the generation of x-rays for

cancer treatment the Sun generating radiationhydrogen gas and oxygen gas combining to make water

radioactivity produced from the detonation of an atom bomb

46 What force holds an atom

together and makes matter as we know it possible?

the Strong Nuclear Force

47The following reaction

is an example of

nuclear fission.

48What is

happening in the picture to

the right?A radioactive atom is

undergoing beta decay.

49What is

happening in the

picture to the right?A radioactive atom is

undergoing alpha decay.

50Radium-226 has a half-life of 1599 years. If someone gave you a box

containing 100 000 atoms of radium-226 today, how many of

those atoms would have decayed 1599 years from today?

50 000 atoms would have decayed.

51 From a scientific perspective, what is the best definition of

the term “organic chemistry”?Organic chemistry is the study

of the element carbon.

52 List three allotropes of

pure carbon.diamond

graphite

fullerenes

53 How do you identify a

hydrocarbon as an alkane?

An alkane contains only single bonds.

An alkane has a general formula of

CnH2n+2

54 Write the chemical formula

for the hydrocarbon pentane.

C5H12

55 Name the following

hydrocarbon:

propene

56heptane

Name the following hydrocarbon:

57

2-methylbutan

e

Name the following hydrocarbon:

58

2,2,4-trimethylhexane

Name the following hydrocarbon:

59

3-methyl-1-pentyne

Name the following hydrocarbon:

60

3-ethyl-3-methyl-1-pentene

Name the following hydrocarbon: