Arnoldi / LazaarChem ComFinal Review

UNIT 1Water: Exploring Solutions

Section A – Sources and Uses of Water

1. Definitions Word Bank: Distillation Filtration Electrolytes

a. The process of solid particles being separated from a liquid by passing them through a material that retains the solid parts

while the liquid continues through, is called ______________________.

b. A separation technique based upon the boiling point of a liquid is called _____________________.

c. Substances that can conduct electricity when dissolved in water are called _____________________.

2. Fill in the Blanks BelowWord Bank: Charcoal Distillation Gravel Sand

Chlorine Filter Larger Smaller

In our Foul Water laboratory, we used several techniques to “purify” our water. The sand was held in place by the ______________ layer below it. The gravel acted as a __________________ for very large particles. The sand trapped the _______________ solid particles. The odor was removed by the ___________________, which also clarified the water. If this was a real sample of water, we would have added _______________ at this point in order to eliminate any remaining contaminates so that we could drink the water. If we truly needed PURE water, we would continue with __________________, which would remove the very smallest, dissolved particles. 3. What instrument is most precise in measuring a volume of water: a beaker, a pipette, or a graduated cylinder? Explain how to take this reading. Include the term “meniscus”.

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4. List 3 examples in your home where water is wasted. How might you better conserve this water?

5. Using the hydrologic cycle shown below to answer the following questions.

Word Bank: Compounds Condensation Suspended Matter

Water is purified naturally during the hydrologic cycle. Dissolved substances are removed through evaporation and _________________. Bacterial action converts dissolved organic contaminants into a few simple __________________. Filtration through sand and gravel removes ______________________________.

Precipitation

Evaporation

Evaporation

Precipitation

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Section B – Looking at Water and its Contaminants

6. What compound has a density of 1 g/mL and is a polar liquid? _________

7. A compound has a density less than 1 g/mL and doesn’t mix with water.

Is this compound polar or nonpolar? __________________ Will it sink or float when placed in water? __________________

8. DefinitionsWord Bank: Anion Colloid Ions Neutrons

Atom Compound Isotope SolutionCation Electrons Mass Number Suspension

a. A homogeneous mixture, such as air or brass, is a(n) __________.

b. A heterogeneous mixture, with large particles that will separate upon standing, like river water, is a(n) _________________. This may or may not reflect light (Tyndall Effect).

c. A heterogeneous mixture that will reflect light and whose particles will remain suspended over time, such as whipped cream, is a(n) ________________.

d. The smallest piece of an element that retains the characteristics of that element is a(n) ___________________.

e. Any charged particle is called a(n) _____________. Positively charged particles are _______________, while negatively charged particles are ________________. The particles become charged because they have gained(-) or lost(+) ___________________.

f. A(n) ___________________ is an atom of a particular element whose protons will always be the same, but whose __________________ may differ. Because they have different numbers of neutrons, they have a(n) different ___________ as well.

g. A chemical combination of two or more elements is called a(n) ______________.

EXAMPLES: Classify each of the following as colloid, suspension or solution:

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a. salt water c. Tyndalls, but doesn’t filter

b. river water d. may Tyndall, does filter

EXAMPLES: Classify each of the following as solution, compound, element or heterogeneous mixture:

a. CO c. CoCl2 (aq)

b. Co d. Cu & Ni thrown in a box and shaken

9. Give an atom inventory for the following:

a. C6H12O6 b. Al2(SO4)3

(continued on next page)10. Fill in the Blanks

Word Bank: “Ide” NegativeMemorized / Come from the List Oxidation NumbersPeriodic Table Roman NumeralsPositive

When given a name and writing the formula for ionic compounds, remember to place the _______________ion first and the _______________ ion second. Then, put in the _____________________. These numbers can come from the ___________________________ if it is in group one, two,

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three, five, six, or seven, they can come from the ______________________________ if it is a transition metal or lead or tin, or they can be ________________________ if it is a polyatomic ion. Once the oxidation numbers are put in, crisscross them to become the subscripts on the other ion. Remember to use ( ) if you are putting a number on a polyatomic ion. Lastly, reduce if it is possible.

When given the formula and writing the name for ionic compounds, remember to place the names in the same order as they appear in the formula. Remember, that if a transition metal, tin or lead appears, you will need a ______________________. The Roman Numeral indicates the charge of the ______________ ion and is determined by sauce-apple-cross-criss. Also, remember that unless it ends in a polyatomic ion, the ending is always “_________”.

(examples on next page)

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EXAMPLES:

a. SnCl4 e. Calcium Sulfate

b. KI f. Magnesium Phosphate

c. MgBr2 g. Aluminum Oxide

d. LiNO3 h. Copper (II) Chloride

EXAMPLE: What is the formula of the compound that combines Al+3

with ClO2-1?

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Section C – Investigating the Cause of the Fishkill

14. Definitions

Word Bank Insoluble Polar SoluteLikes Dissolve Likes Polar Bond Solvent

Nonpolar Saturated SupersaturatedNonpolar Bond Soluble

Unsaturated

a. When a solution contains the maximum amount of solute for that amount of solvent at a particular temperature, it is considered to be ______________.

b. When a solution contains less than the maximum amount of solute for that amount of solvent at a particular temperature, it is considered to be _________________.

c. When a solution contains more solute than it should be able to hold at a particular set of conditions, (this is a very rare circumstance), we call the solution ___________________________.

d. The substance in a solution that is dissolved is called the _________.

e. The substance in a solution that does the dissolving is called the _________.

f. An uneven distribution of charge results in a ____________ bond.

g. An even distribution of charge results in a ______________ bond.

h. When something is able to be dissolved, we call it ____________.

i. When something is not able to be dissolved, we call it __________.

j. The concept that substances that are alike will dissolve in each other is called _______________________. This means that polar solutes dissolve in ______________ solvents, nonpolar solutes dissolve in _______________ solvents, and ionic solutes dissolve in _________________ solvents.

EXAMPLE: Which of the following will oil dissolve in? Explain your answer.

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CCl4 CH3OH

15. Circle the Correct AnswerWhen an ionic solute dissolves in water, several steps are

involved. First, the positive and negative ions in the solute break apart from each other. Then, the ( positive / negative ) ion goes near the partially negative part of the water molecule, which is the ( H / O ) atom, and the ( positive / negative ) ion goes near the partially positive part of the water, which is the ( H / O ) atom.

16. If temperature rises, solubility of most solid solutes ( increases / decreases ).

17. In a mixture composed of 100 grams of water and 25 grams of KCl,

a. What is the solute?

b. What is the solvent?

c. List two ways to make more salt dissolve

PROBLEMS:

(X)Mass 80 ___Solute (g) ___

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per 60 ___100 g (Y)water ___

40 ___ (Z)

| | | |20 40 60 80Temperature ‘C

18. What is the solubility of “X” in 100 mL of water at 40’C?

19. What is the solubility of “Y” in 75 g of water at 50’C?

20. At what temperature will 45 grams of “Z” dissolve in 100 g water?

21. What is the percent by mass of a solution containing 20.0 g of MgCl2 in 85.0g of water?

22. What is the PPM of a solution consisting of .325g of gold ions in 750g of water?

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23. What mass of solute is needed to make a 35% MgCl2 solution containing 3.95 L of water?

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Section D – Water Purification and Treatment

26. A solid formed when two aqueous substances combine is called a(n) _______________.

27. How did early soaps / detergents contribute to problems in the water cycle?

28. Fill in the Blanks BelowWord Bank: Aeration Flocculation Prechlorination

Alum Fluorine Pre-use PurificationFish, Sticks, etc. Odor Taste pH

The Water Treatment ProcessThe first step in the water treatment process is the ________-

________ _________________. In this step, the water is filtrated through metal screens which remove large items like _________________. The next step is _________________. This is where chlorine is added before other treatments are begun. It is added to kill disease carrying organisms. Then, we need to remove the suspended particles. In order to do this, _____________ is added, which makes Aluminum Hydroxide, Al(OH)3, which is a gooey substance. This gooey substance traps the particles, and then they settle or are filtered out. The special name for this process is __________________. We then might __________ the water. This is when the water is sprayed into the air. Aeration is done to remove __________ and improve __________. Also, we might add lime. Lime (which is stone – basic) is added if we need to adjust __________ making an acidic water sample more neutral. Finally, we might add _____________ for health reasons. In particular, it helps reduce tooth decay.

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UNIT 2Materials: Structure and Uses

Section A – Why We Use What We Do

1. DefinitionsWord Bank (may be used more than once)

Atomic number Isotopes NonmetalsChemical Mass Number Periods

Combustion Metaloids Physical

Families Metals Semimetals

Groups Noble Gases

a. A property that can be observed without changing the substance is called a(n) _________________ property.

b. A change in shape, size, color, etc., which maintains the identity of the substance is called a(n) ________________ change.

c. A property that can only be observed by actually changing the substance is called a(n) ________________ property.

d. A change that results in a new substance, with new properties, being formed is a(n) ________________ change.

e. The fancy chemical word for burning is ____________________.

f. ________________ are located on the left of the staircase on the periodic table. Aluminum is also considered a metal,

even though it is touching the staircase because its characteristics are much more metallic than nonmetallic.

g. ________________ are located on the right of the staircase on the periodic table. h. _______________ or _________________ are located touching the staircase on the periodic table. An exception is Aluminum,

which is considered to be a metal.

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i. The number of protons in an element is called its____________________.

j. The mass of a particular isotope, which is equal to the sum of the protons and neutrons, is called the _____________________.

k. Atoms of the same element with different numbers of neutrons, which results in different masses, are called _________________.

l. The average mass of the isotopes of an element is called the ____________________.

m. On the periodic table, _______________ or _______________ run up and down (they are the columns).

n. On the periodic table, _________________ run side to side, they are the rows.

o. Also known as the Inert Gases, the ____________________ are the family on the periodic table that does not react. They are the last column.

2. In the periodic table, elements with similar properties are arranged in the same ____________, which is called a _____________ or _______________.

3. The Modern Periodic Table classifies elements according to _______________________________________.

4. Identify the following as a Metal (M), nonmetal (NM) or Metalloid (ML) / Semimetal.

_____ a. Found along the “staircase” on the Periodic Table

_____ b. Found on the left of the Periodic Table

_____ c. Dull and non-conductive

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_____ d. Si

_____ e. Calcium

5. List three properties of metals and three properties of non-metals.

6. Circle the word that best completes the sentence.

a. The size of elements (increases or decreases) across a period from left to right.

b. The most metallic elements are located to the (left or right) of the periodic table.

c. The most reactive nonmetals are located to the (left or right) of the periodic table.

d. The electronegativity of elements (increases or decreases) across a period.

7. Identify each of the following as a Physical Property (PP), Chemical (CP) property, Physical Change (PC) or Chemical Change (CC):

_____ a. The hardness of diamonds enables them to be used in drill bits.

_____ b. Silver utensils are tarnishing.

_____ c. Iron can corrode and rust when exposed to moist air.

_____ d. The high melting point of tungsten makes it useful in light bulb filaments.

_____ e. Metals are ductile.

_____ f. Salt is dissolved in water.

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_____ g. Water is boiling off in a pot on the stove.

8. Give the location of the following elements by period and group number.

a. Calcium: period ________ group ________

b. Nitrogen: period ________ group ________

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9. Complete the following table:

Name Symbol At. # Mass # Protons

Neutrons

Electrons

Gold 197

K +1

53 54

14 6

Remember:

Atomic Number = number of protons and is the whole number on the periodic table.

The number of electrons = the number of protons if the element is neutral, if the ion is negative, add that number to the number of protons to get the number of electrons, if the ion is positive, subtract that number from the number of protons to get the number of electrons.

The number of neutrons = Mass Number - number of protons.

Atomic Mass is on the periodic table. It is the average mass of the isotopes, and a decimal number. Mass number is NOT on the periodic Table. It is the sum of the protons and neutrons and is for a single isotope only.

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Section B – Earth’s Mineral Resources

10. Definitions:

Word Bank:Activity Series Mineral ReductionHigher Ore Reducing AgentLithosphere OxidationLower Oxidizing Agent

a. A naturally occurring rock/mineral that can be mined to get a metal or other material is called a(n) _________________.

b. The solid part of the Earth, which contains the greatest variety of chemical resources, is the ___________________.

c. A naturally occurring solid compound containing the element or group of elements of interest is called a(n) _________________.

d. The _____________________ tells us if one metal can replace another. Remember, the _____________ the metal appears on the series, the more active it is.

e. A chemical change in which an electron is lost is called ___________________.

f. A chemical change in which an electron is gained is called _________________.

g. The ______________________ causes another element to gain an electron, it is giving away that electron, so it is oxidized.

h. The ______________________ causes another element to lose an electron, it is gaining that electron, so it is reduced.

11. Most atoms are found in ____________________ or __________________ in nature. Metals and most other raw materials are found in the ________________ layer of the Earth.

12. The three methods of metal purification are ________________, ________________________ and _______________________.

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13. Which is more active?

a. Calcium or Chromium

b. Manganese or Sodium

14. In each of the following reactions identify what was reduced, oxidized, the reducing agent, and the oxidizing agent:

Cu(s) + Ag+1(aq) Cu+2(aq) + 2Ag(s)

Cu+2(aq) + Mg(s) Mg+2(aq) + Cu(s)

15. Write the correct equation for the oxidation of copper to copper+2.

16. Write the correct equation for the reduction of Chlorine to Chlorine -1.

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Section C – Conserving Matter

17. Define:Word Bank

Coefficient Reactants SubscriptMole RecyclingProducts Reusing

a. In a reaction, the “big number in front” of an element or compound, which represents the number of moles reacting, is called the _____________________.

b. In a formula, the “little number after the element symbol”, which represents the number of atoms of that element in the compound, is called the _______________.

c. The substances that you begin the reaction with are called the _____________.

d. The substances that you form in the reaction are called the _______________.

e. A(n) _________________ is a number – 6.02 X 1023. It was Avogadro’s Number. It is represented by the coefficient in the

reaction.

f. Taking used materials, and reprocessing them into new, usable materials is called ______________________,

g. Taking used materials, and using them in the same form for the same or a new purpose, is called _____________________.

18. The easiest way to obtain Aluminum is from _______________________________.

19. In a chemical equation, the total number of atoms for each element on the reactant side must be _________ to the total number of atoms for each element on the product side.

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20. The Law of __________________________________ states that the total number of atoms on the reactants must equal the total number of atoms on the products

21. Since 1982, pennies are mostly (97.5%) made with ____________________________.

22. Name two renewable resources. Name two resources considered non-renewable.

23. Fill in the BlanksWord Bank

Energy Increase WasteFly Ash Other Solid Residue

In a __________-to-____________ plant, we burn waste (trash) to create __________________. There is some polulution created, for example ______________ and _______________________, but it does use otherwise unusable materials. Also, it tends to ____________________ recycling.24. Balance the following equations:

___ Zn + ___ CuSO4 ___ Cu + ___ ZnSO4

___ Al + ___ ZnC12 ___ A1C13 + ___ Zn

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25. In the second equation above:

a. What are the reactants?

b. What are the products?

c. What is the subscript on the chlorine atom in the reactants?

d. What is its coefficient?

e. What is the total number of aluminum chloride units formed?

26. What is the molar mass of HClO3?

27. Convert 1.2 moles NH3 to mass.

28. Convert 32.8 g H2S to moles.

29. Given the following reaction for burning gasoline:

2 C8H18 (g) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g)

How many liters of O2 are necessary to react with 5 liters of C8H18?

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30. Calculate the percent by mass of copper in the compound, Cu(OH)2.

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Section D – Materials: Designing for Desired Properties

31. Definitions: Word Bank NonconductorAllotrope SemiconductorElectroplating Superconductor

a. A substance that cannot conduct heat/electricity is called a(n) _____________.

b. A substance that can conduct heat/electricity a little, but needs a boost to do so, is called a(n) ________________.

c. A substance that conducts very well, with little or no resistance is a(n) ___________________.

d. Putting a thin layer of metal on a surface by an electrical process involving oxidation and reduction is called ____________________.

e. Various forms of the same element, for example oxygen, O2, and ozone, O3, or carbon as graphite, diamond, and the “bucky” ball –

buckminsterfullerene, are called ________________.

32. Give an example of a:

a. Conductor

b. Nonconductor

c. Semiconductor

d. An element that can be used to electroplate.

e. Two Allotropes of Oxygen

f. Three Allotropes of Carbon

33. Plastics are made of …

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UNIT 3 Petroleum: Breaking and Making Bonds

Section A – Petroleum: What is it?

1. Definitions WORD BANK: Covalent Bond Fractional Distillation

Crude Oil HydrocarbonEnergy Levels Intermolecular

ForcesForces Organic ChemistryFraction Valence Electrons

Valence Shell

a. Petroleum that is pumped from underground is called __________.

b. A C-H chain is called a(n) ___________________.

c. A portion (smaller mixture) distilled out of a larger mixture using fractional distillation is called a(n) _____________________.

d. A separation process of a large mixture into several smaller mixtures via their boiling points is called

____________________.

e. The forces of attractions between two molecules is called_________________.

f. In an atom, electrons are found in _________________________.

g. The branch of chemistry dealing with hydrocarbons and their derivatives is called ______________________.

h. The electrons in the outermost energy level, ( the ones most directly involved in bonding), are called __________________.

i. The outermost energy level containing electrons is called the _______________.

j. A bond (force of attraction) in which two or more electrons are shared is called a(n) _________________________________.

2. Complete the following table: HINTS:

) up to 2 e- ) up to 8 e- ) up to 8 e-

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#p

# of electrons = number of protons = atomic #

# valence electrons = outer e- = PT column

Element nameEnergy Levels

(Bohr Diagram)# of

Valence Electrons

Fluorine

Carbon

Silicon

Magnesium Ion

3. Draw the electron dot diagram for the following:HINTS:

Element Symbol in Center

For Electrons: number = column number on PT

first two together, next three apart, then pair up

a. Argon c. Phosphorus

b. Magnesium ion d. Fluorine ion4. How many bonds would each of the following form:

HINTS:Draw Lewis Dot Structure

CANNOT bond on a side with no dots

CANNOT bond on a side with two dots

CAN bond on a side with 1 dot

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DON’T FORGET THE EXCEPTION(S)!

a. Carbon b. Hydrogen c. Nitrogen

5. Draw the Lewis Dot Structure for each of the following

a. methane (CH4) b. water

c. NH3 d. propene (C3H6)

6. Fractional distillation is based on the fact that substances found in crude oil have different _________________________.

7. Hydrocarbon boiling points _______________________ as the number of C atoms per molecule increases

8. Based on the length of the carbon chain, which of the following would have the HIGHEST boiling point: C7H14, C3H8 or C6H14? Why?

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Section B – Petroleum: An Energy Source

9. Define:WORD BANK: Chemical Kinetic Potential Specific Heat

a. The energy of position is called _______________ energy.

b. The energy of motion is called _______________ energy.

c. The energy held within a bond, which is a specific kind of potential energy, is called ________________ energy.

d. The energy needed to raise one gram of a sample 1’C is called ___________________.

10. Classify each of the following as an example of kinetic or potential energy:

a. _____ A boulder perched at the top of a hill.

b. _____ A train traveling down the tracks.

c. _____ A tank of gasoline.

d. _____ Water flowing down a river.

11. When a chemical reaction occurs, energy is __________________ when bonds break, and ____________________ when new chemical bonds form.

12. Is the following reaction endothermic or exothermic? Explain your answer.

2 C2H2 + 5 O2 4 CO2 + 2 H2O + 2512 kJ

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13. Write the chemical reaction for the combustion of heptane. (C7H16)

14. How much energy is needed to raise the temp of 125 g sample of liquid water from 50 degrees Celsius to 135 degrees Celsius? (Cp = 4.2 J/g’C) q = m Cp ^T

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Section C – Petroleum: A Building Material Source

15. Draw the structure of the following compounds. Label each as an alkane, alkene or alkyne.

Remember, alkane = all single bonds, alkene – one double bond, alkyne = one triple bond.

a) Pentane (C5H12)

b) Pentene (C5H10)

c) Pentyne (C5H8)

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Section D – Energy Alternatives to Petroleum

16. Definitions: WORD BANK: Biodiesel Biomolecules

a. Large organic molecules that are found in living systems are called __________________________.

b. _____________________ is an alternative fuel or fuel additive for diesel engines that is made from various materials such as

new or recycled vegetable oils and animal fats.

17. Complete the following paragraphs about alternative fuels.

WORD BANK:CO Fire PetroleumCompressed Natural Gas High Pressure Tanks TrunkExpensive NOx Wide

_____________________________, or CNG, is a natural gas that is compressed and stored in ___________________________. The gas is obtained from gas wells or during ________________________ processing. The tank is installed in the ______________________ of the car. There are several advantages of CNG, including its __________ availability and its 80% decrease in _________ and ______________ emissions. However, it is ________________ and does present a higher _____________ risk.

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WORD BANK: Air Pollution Expensive WaterEnergy Fuel Cells

The most common form of ________________ result in the combination of oxygen and hydrogen gases to form _________________. In this process, which is exothermic, _______________ is also made. Fuel Cells eliminate the _______________ released from vehicles, but they are very _________________.

WORD BANK: Battery Emissions IdlingBraking Hybrid Miles Per

Gallon

The goal of a gasoline-electric __________________ is to make the car more efficient. Instead of wasting energy (during ______________ or ______________, for example), it is converted into stored energy in the ______________. Then, the battery is used whenever possible. This results in lower __________________ and higher ____________________.

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UNIT 4 Air: Chemistry and the Atmosphere

Secation A – Gases in the Atmosphere

1. Fill in the blanks about the earth’s atmosphere. WORD BANK: Decreases Oxygen NitrogenTroposphere

The atmosphere is composed of 78% _____________ and 21% _____________. The _____________ is a thin layer within 10-15 km of the earth's surface. As altitude increases, air pressure ________________.

2. Fill in the blanks about gas characteristics.WORD BANK: 0 1.00 273 760

collide with walls

Standard temperature is _______________K or ____________ºC. Standard pressure is _____________mm Hg or _____________atm. A gas in a closed container exerts pressure because the gas particles ___________ the ___________ of the container.

3. Fill in the blanks about gas behavior.WORD BANK: Increase Decrease

If pressure is lowered and the temperature and number of moles are constant, the volume will ______________. If temperature is raised and the volume and number of moles are constant the pressure will _________________.

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4. Fill in the blanks about Ideal Gas Behavior.WORD BANK: Attractions Kelvin Pressure

Directly Large RepulsionsElastic Motion Temperature

The gas laws do NOT predict gas behavior well when the ____________________ is very high or the _____________________ is very low. The assumptions of the Kinetic Molecular Theory of Gases include: (1). Gases are composed of ___________ numbers of particles, (2). Gas molecules are in constant, random _________________, (3) There are no molecular __________________ or ______________________, (4) The collisions between particles are ___________________, (5) Kinetic Energy and Temperature (in ________) are ______________ proportional.

5. Complete the following problems.

a. Convert −45ºC to Kelvin.

b. Determine the volume exerted by 0.25 mole neon gas at STP.

c. A gas in a balloon at 1000 mm Hg occupies 1500 mL. At what pressure will the gas occupy 3000 mL if the temperature

remains unchanged?

d. A 4 L sample of hydrogen is collected at 800.0 mm Hg and 30.0ºC. What volume will the gas occupy at STP?

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Section B – Radiation and Climate Definitions:

6. DefinitionsWORD BANK: Electromagnetic Radiation Infrared

Electromagnetic Spectrum VisibleFrequency Wavelength

a. All radiation, ranging from low-energy radio waves to high energy xrays and gamma rays, including visible light, is called

____________________

b. The ________________________ is comprised of the full range of electromagnetic radiation frequencies.

c. _________________ is the number of waves that passes a certain spot in a certain amount of time.

d. The ________________ is the distance from a point on a wave to that same point on the next wave.

e. Electromagnetic radiation, which is known as heat radiation, and has lower energy and wavelength, but higher frequency, is called

_______________ radiation.

f. ___________________ radiation has medium energy, frequency and wavelength, and causes the colors that we see.

7. What is the source of Earth's energy? What is the source of the Sun's energy?

8. What is the relationship between frequency and wavelength?

9. What is the relationship between frequency and energy?10. What is the relationship between wavelength and energy?

11. What happens to the 30% of the Sun's solar energy that does not reach the Earth's surface?

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12. What is the relationship between amount of heat reflected, absorbed and color?

13. What is the relationship between specific heat and how much heat is needed to change the temperature of an object?

14. What is the function of the ozone layer?

15. List three examples of greenhouse gases.

16. Fill in the Blanks

___________ (higher or lower) ___________frequency wavelengthEnergy

___________ (higher or lower) ___________wavelength frequency

Energy

UV___ V I B G Y O R InfraredUV___ (aka __________)UV___ (ultraviolet)

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a. How much ___ radiation reaches the Earth?

UVC

UVA

UVB

infrared

b. What is the effect of __ radiation on the Earth?

UVC

UVA

UVB

infrared

VisibleSection C – Acids in the Atmosphere

17. __________ __________ is fog, sleet or snow with pH lower than 5.6

18. THREE natural sources of acidity in rain are CO2 in the atmosphere, ________________, _________________, and _______________.

19. The major components of acid rain are _________________, _________________, and __________________.

20. ________________, a natural gas, makes rainwater slightly acidic.

21. Coal burning power plants are major contributors of _______________ from the burning of high sulfur coal.

22. Identify the following as acidic, basic, or neutral a. _____H3PO4 c._____Ca(OH)2

b. _____CaCl2 d. _____ C2H6

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23. Which of the following is a neutralization reaction? Which is ionization? Which is dissociation?

a. Ca(OH)2 + H2O Ca+2 (aq) + 2 OH-1 (aq)

b. HCl + NaOH NaCl + H2O

c. HCl + H2O H3O+ + Cl−

c. MgO + H2O Mg(OH)2

24. Identify the following as a strong acid, a weak acid, a strong base, a weak base or neutral.

a. _____ 1 M HCl, pH = 0.1 c. _____ pure water, pH = 7.0

b. _____ saliva, pH = 6.7 d. _____ 0.1 N NaOH, pH = 14.0

25. Complete the following table:

Substance pH [H3O+] Acid, Base, or Neutral?

Vinegar 3 N/A

Milk 1.00 x 10-6 M

Pure water

Rainwater 2.51 x 10-6 M

Ammonia 1.21 x 10-11M

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Section D – Air Pollution: Sources, Effects and Solutions

26. Fill in the blanks. Some answers may be used more than once.Air conditioners Filter Sulfur dioxide RefrigeratorsCarbon monoxide Nitrogen dioxide Transportation OzoneCatalytic converter Wet scrubber Chlorine Electrostatic precipitator Photochemical smog

The main source of air pollution in the United States is ____________________The major pollutant from cars is ____________________. This is a deadly

gas that is given off due to incomplete combustion. It is important not to idle a car in a closed garage due to this gas. It can also be given off in a home by a faulty furnace. The Air Quality Index (AQI) measures these four pollutants: _______________, _______________, ______________ and _______________. Two harmful components of ______________ are NO2 and O3

(ozone). ___________ can inhibit plant growth. ___________ is a powerful oxidizing agent that can crack rubber, corrode metals and damage plant and animal tissues. A very thin layer of ____________ in the stratosphere protects the earth by absorbing UV radiation. Chlorofluorocarbons deplete the ozone layer because they supply ___________ radicals to the atmosphere. Because of their destruction of the ozone layer, CFC's are no longer produced in over 170 countries in the world. CFC's were once widely used for _______________________ and _____________________. Three ways to reduce particulate pollution is with _____________________,__________________, and __________________. A ______________ _____________ reduces the amount of NOx and CO emissions from a car. Ozone can be both harmful and helpful to humans. Tropospheric or "ground-level" ozone is harmful while stratospheric ozone is helpful. Explain.

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