1. List and use the units of the modernized metric system(SI) in measurements of length, volume, mass and density.

1. Define the terms evaporation, condensation, bacterial action, filtration, hard water, water softening, ion exchange, turbidity, water softener, regenerated, water treatment, sewage treatment, pre-chlorination, flocculation, post-chlorination, chlorination, aeration, fluoridation, osmosis and reverse osmosis and apply them in an example.

2. Compare and contrast natural and artificial water purification systems.

3. Identify the chemicals used to adjust pH and to flocculate the water in a treatment plant.

4. Identify the problems of chlorination including the problems with trihalomethanes.

5. Identify ions associated with hard water and discuss how they might be removed

6. Compare methods of water softening and the chemistry of the systems including the methods of regeneration.

7. Assess the risks and benefits of water softening and chlorination.

Sample Quiz Questions:

.ID6) Type the word that means the process of removing certain anions or cations from a solution and replacing them with other anions or cations. Usually accomplished on a resin such as zeolite.

.ID6) The halogen most frequently used in water and sewage plants to kill microorganisms is _____________.

.ID6) Much of the raw water that comes from reservoirs and wells is acidic and the pH must be adjusted by adding a base. The base most commonly used in a water or sewage plant for pH adjustment is: •lye •lime •vinegar •milk of magnesia •ammonia

.ID6) Some water softening units use ion exchange resins. What occurs in such a unit? A. Magnesium ions are exchanged for chloride ions. B. Calcium ions are exchanged for iron ions. C. Calcium ions are exchanged for magnesium ions. D. Calcium ions are exchanged for sodium ions.

.ID6) There are three ions which bear the primary responsibility for the hardness of water. One of them is the __________ ion.

.ID6) THM's(trihalomethanes) are formed when chlorine reacts with ____________ in water A. hard water ions B. suspended matter C. bacteria D. organic chemicals from decayed matter

.ID6) Some municipalities add a soluble fluoride compound to their drinking water supply. The reason is to A. improve the taste of the water. B. eliminate the bacteria found in the water, making it safer to drink. . precipitate the organic solids found in surface water reservoirs. D. reduce tooth decay by strengthening tooth enamel.

 

Unit II

You will be tested on the following objectives at the end of section II. A.5

1. Define the terms physical properties, physical change, chemical properties, chemical change, metals, nonmetals, metalloids, conductor, nonconductor, periodic table, Mendeleev, and atomic mass, malleable and brittle and apply them in an example.

2. Distinguish between chemical and physical properties and/or changes when given specific examples of each.

3. Classify selected elements as metals, nonmetals, or metalloids based on observations of their chemical and physical properties.

4. Construct a workable periodic table and explain its organization, given chemical and physical properties of a set of elements.

Sample Quiz Questions:

II.A.5) The high melting point of tungsten makes it useful for light bulb

filaments. A. Chemical Property B. Physical Property

II.A.5) Classify the element Sn. A. Metal B. Nonmetal C. Metalloid

II.A.5) Give the word or words that mean the arrangement of the elements into periods and groups or families according to their properties.

II.A.5) Which choice is a chemical change? A. Wood burns in a fireplace.

B. A glass of milk becomes sour. C. Mold "grows" on cheese. D. All of these.

II.A.5) Name a diatomic element that is not in column 1 of the periodic table.

You will be tested on the following objectives at the end of section II. A.8

1. Define the terms atomic number, nucleus, mass number, isotope, periods, groups or families, alkali metal, noble gas, alkaline earth metal, halogens and apply them in an example.

2. Use the periodic table to (a) predict physical and chemical properties of an element; (b) write formulas for various compounds; (c) identify elements by their atomic masses and atomic numbers; and (d) locate periods and groups(families) of elements.

3. Construct a workable periodic table and explain its organization, given chemical and physical properties of a set of elements.

4. Compare the reactivities of selected elements, and explain the results in terms of the structure of their atoms.

5. Determine properties of elements by the number and arrangement of the electrons in the atom.

Sample Quiz Questions:

II.A.8) Give the word or words used to name the elements of the first column of the periodic table.

II.A.8) The properties of the elements are closely related to the

arrangement of •protons •electrons •neutrons

II.A.8) Lithium melts at 181°C, sodium melts at 98°C,

rubidium melts at 40°C, and cesium melts at 29°C. Refer to the periodic table and predict the melting point of potassium in °C. •22 •34 •58 •126 •254

II.A.8) Which of the following does NOT belong in this family? •Cl •F

•I •Ar •Br

II.A.8) From the "Metal Reactivities" lab results, the metal elements can

be ranked in order of their chemical reactivity. This ranking is

called the :A. Periodic table B. Activity series C. Data table D. Bar graph

You will be tested on the following objectives at the end of section II. B

1. List the major layers of our planet and state what each is composed of.

2. List the three primary layers of our planet and some resources that are "mined" from each region.

3. Relate the abundance of various elements to the layers of the earth.

4. Define the terms reduction, oxidation, oxidation-reduction reactions, redox reactions, reducing agent, electrometallurgy, pyrometallurgy, hydrometallurgy, dot structure and oxdizing agent and apply them in an example.

5. Outline the production of a metal from its ore (using copper as an example) and list four factors which determine the profitability of mining.

6. Define oxidation and reduction, and compare the three most common redox-reaction methods for separating metals from their ores.

7. Use metal reactivities to predict if a given reaction will occur.

8. Identify which substances in a reaction are oxidized and which are reduced.

Sample Quiz Questions:

II.B) The process of combining a metal into a compound. Any process in which electrons are lost by a species.

II.B) Will zinc metal react with a solution of gold(III) nitrate? •Yes •No

II.B) Which row 3 metal is most reactive? •sodium •magnesium

•aluminum

II.B) Consider this reaction: Zn(s) + Cu¤+(aq) -----> Cu(s) + Zn¤+(aq)

Which species undergoes oxidation? a) Zn(s) b) Cu¤+(aq) c) Cu(s)

d) Zn¤+(aq)

II.B) For the reaction:

Cu(s) + 2 Ag±Ú(aq) -----> Cu¤±(aq) + 2 Ag(s) Type the element name of the most active metal.

You will be tested on the following objectives at the end of section II. C.2.

1. State the law of conservation of matter and apply the law by balancing chemical equations.

2. Write balanced chemical equations and relate them to the law of conservation of matter.

3. Given a chemical equation be able to complete an atom inventory.

Sample Quiz Questions:

II.C.2) Referring to a molecule consisting of two atoms.

II.C.2) Name one of the products of the reaction between beryllium and hydrochloric acid.

II.C.2) Fill in the blank to balance this equation

4 NH3 + 5 O2 -----> ____ NO + 6 H2O

II.C.2) Is the following equation balanced

2 CuO + C --> 2 Cu + CO2

II.C.2) When the equation --- H3PO4 + KOH ---> K3PO4 + H2O ---

is balanced, what is the coefficient for H3PO4?

You will be tested on the following objectives at the end of section II. C.5.

1. Define the terms mole, molar mass, percent composition, renewable resources and nonrenewable resources and apply them in an example.

2. Calculate the molar mass of a compound when provided its formula and the atomic masses of its elements from a periodic table.

3. Calculate the number of moles and/or grams of products produce in a reaction when given the number of moles/grams of reactants.

4. Calculate the percent composition by mass of a specified element in a given compound.

5. Distinguish between renewable and nonrenewable resources, and identify the methods of conserving our resources.

Sample Quiz Questions:

II.C.5) Consider the "four R's" of resource conservation: To ____________ a resource means to refurbish or repair manufactured items or redistribute unwanted items, such as clothing, for use by others.

II.C.5) What is the mass of one mole of strontium atoms? Answer to the nearest 0.1 g and be sure to include units! (XX.X g)

II.C.5) What is the molar mass of aluminum sulfate, Al2(SO4)3? Answer to the nearest 0.1 g and be sure to include units! (XXX.X g)

II.C.5) Nitrogen reacts with hydrogen to form ammonia according to this equation: N2 + 3 H2 -----> 2 NH3. If 32.0 grams of nitrogen reacts completely with 9.0 grams of hydrogen, how many grams of ammonia will form? Answer to one decimal place and don't forget units! (XX.X U)

II.C.5) A mole of sulfur atoms has a mass of approximately 32 g. How many moles of sulfur atoms are in 80 g of sulfur?

You will be tested on the following objectives at the end of section II. D & E

1. Define the terms allotropes, ceramics, alloys, semiconductors, doping, coating, and electroplating and apply them in an example.

2. Describe the difference in the properties of an element due to the arrangement of the element's atoms.

3. Describe the difference between the proterties of an element and the properties of its alloy.

4. Describe how the conductivity of a material can be changed.

5. Describe how the properties of a material may be changed by applying a coating.

6. Given a burner be able to safely and properly adjust and use the burner.

Sample Quiz Questions:

II.D) Brass is an alloy of: A. tin and zinc B. sodium hydroxide and

copper C. copper and zinc D. copper and tin

II.D) In an experiment, the ____________ is a setup that duplicates all of the conditions of the experiment except the one being tested.

II.D) Two or more forms of an element in the same state that have distinctly different physical and/or chemical properties. Type the word.

II.D) Ceramics can be used to make all of the following except: A.

Engines B. dishes C. pool balls D. electrical insulators

II.D) What do you do at once if your hand is splashed with hot, liquid

NaOH? A. Put on your goggles. B. Wash with plenty of water.

C. Apply Vaseline over the splased area of skin. D. Remove the penny

from the liquid.

UNIT III

You will be tested on the following objectives at the end of section III. A.1-A.5.

1. Identify objects made from petroleum.

2. Compare the usage of petroleum for "building" and "burning".

3. Identify regions of high petroleum usage and regions of petroleum reserves.

4. Describe the chemical makeup of petroleum, how it differs from other natural resources, and how it is refined.

5. Describe the process of fractional distillation and name the typical products manufactured from each fraction.

6. Define crude oil, hydrocarbons, distillation, distillate, fractional distillation, fractions, intermolecular forces, organic chemistry, carbon chain, energy levels, covalent bonds, electron-dot formulas, and structural formula.

Sample Quiz Questions:

III.A.5) Which of the following objects is NOT made from petroleum or petroleum products?

• plastic switchplate cover •kerosene •synthetic vitamins •PVC irrigation pipe •facial tissue

III.A.5) Which region of the earth has the majority of the earths oil reserves? •Africa •Asia and the Pacific •Middle East

•North America •Western Europe

III.A.5) Is North America primarily an importer or an exporter of petroleum?

III.A.5) In 1990 Iraq attacked a small oil rich country of Kuwait that supplied the United States with petroleum. This act led to "The Gulf War." Was America's response motivated in any part by fear of loss of petroleum supplies?

III.A.5) If new environmental regulations were enforced so that the oil companies would have to invest 10% of their earnings in new pollution control devices, we would expect the price of gasoline to •increase •decrease

You will be tested on the following objectives at the end of section III. A.6-7

1. Define alkanes, saturated hydrocarbons, tetrahedron, extrapolation, straight-chain alkanes, branched-chain alkanes, and isomers.

2. Name the first ten alkanes.

3. Draw structural and electron-dot formulas for each of the first ten alkanes.

4. Describe the process involved in ionic and covalent bonding.

5. State and explain the effect of carbon length and side groups on the boiling point of a hydrocarbon.

6. Predict the relative boiling point of a hydrocarbon based on the carbon length and side groups

7. Draw structural formulas for the isomers of a given hydrocarbon.

8. Define the term isomer and draw the structural formulas for the first trhree isomers of a given compound.

8. Build models of the first 10 alkanes and their isomers.

9. Extrapolate data from a graph.

Sample Quiz Questions:

IIIA7) Give the name of the term that refers to a chemical bond in which two atoms hold tightly to one another by sharing electrons.

IIIA7) A straight-chain alkane has the formula C₇H₁₄. What is the name of this compound?

IIIA7) Which of the following is the correct structural formula for butane?(You will be given 5 structures to chose from.)

IIIA7) Which of the following isomers of hexane has the highest boiling point? (Type letter only!) (You will be given 5 structures to chose from.)

When carbon bonds to hydrogen, neither atom is able to remove electrons from the other, yet they form a bond by sharing electrons. What type of bond is this? •metallic •ionic •van der Waals •hydrogen •covalent

IIIA7) Give the word that means: the mass per unit volume of a substance, usually expressed in g/mL in this class.

Hydrocarbons with 12 to 16 carbon atoms. Useful as a fuel and for lamps, stoves, tractors. A starting material for the cracking process. Fraction of petroleum collected between 200 degrees Celsius and 300 degrees Celsius.. •gas •gasoline •kerosene •gas oil •lubricating stocks •bottoms

IIIA7) Type the chemical name of the alkane whose molar mass is 58 g/mole.

You will be tested on the following objectives at the end of section III. B.

1. Explain endothermic and exothermic reactions in terms of bond breaking and forming.

2. Identify energy conversions and explain energy conversion efficiency.

3. Define the terms heat of combustion and specific heat and calculate energies of various combustion reactions.

4. Write balanced equations for the combustion of hydrocarbon fuels, including energy changes.

5. Explain the term octane number, state its relationship to grades of gasoline, and identify two ways of increasing octane numbers.

6. Give examples of endothermic and exothermic reactions.

7. Identify the joule(J) as the SI unit of energy.

8. Measure temperature to the nearest 0.1 degree using an alcohol thermometer.

8. Measure volume to the nearest milliliter using a 100 mL graduated cylinder.

10. Use an electronic balance to determine mass to the nearest 0.01 grams.

11. Calculate the amount of heat in Joules required to raise a given amount of water a given number of degrees C.

12. Define the terms fossil fuels, potential energy, kinetic energy, endothermic, exothermic, law of conservation of energy, specific heat, heat of combustion, molar heat of combustion, cracking, octane number, oxygenated fuel and gasohol and apply them in an example.

13. Calculate the savings resulting from increased automobile efficiency.

Sample Quiz Questions:

IIIB) Refer to the table at right. How many Joules are required to raise the temperature of the water in the experiment? Answer to the nearest hundred and include units. (XXX00 J)

IIIB) Which of the following examples is an example of a chemical-potential to kinetic conversion? A. riding a bike B. light bulb burning C. wind powered electricl generator D. gasoline powered lawn mower

IIIB) Rating that indicates the combustion quality if gasoline relative to an isomer of C•H¡•.

IIIB) Assume that you drive your car 200 miles per week and your car can travel 18.0 miles on a gallon of gasoline that costs $1.10. How many gallons of gas would you use in a week? Answer to one decimal place without units. (XX.X)

IIIB) Here is the unbalanced equation for the burning of propane.

What coefficient should go where letter B is?

_A._ C£H• + _B._ O™ ---> _C._ CO™ + _D._ H™O

You will be tested on the following objectives at the end of section III. C.

1. Compare saturated and unsaturated hydorcarbons in terms of molecular models, formulas, and structures.

2. Compare the physical and chemical properties of saturated and unsaturated hydorcarbons.

3. Build a model of an alkene.

4. Given its formula, list the isomers of an alkene.

5. Identify the functional groups for common alcohols, ethers, carboxylic acids, and esters.

6. Synthesize a simple ester.

7. Describe polymerization and give one example of addition and condensation reactions.

8. Define the terms petrochemicals, addition reaction, polymer, monomer, addition polymers, branched polymers, alkenes, double covalent bonds, unsaturated, alkynes, cycloalkanes, aromatic compounds, alcohols, functional group, carboxylic acids, esters, condensation reaction and condensation polymer.

Sample Quiz Questions:

IIIC) Attractive force between two atoms in a molecule resulting from the sharing of one pair of electrons.

IIIC) Which of these carbon skeletons represents a compound which contains exactly 6 hydrogen atoms? Answer name only. (You will be given several drawings to choose from.)

IIIC) Organic (carboxylic) acid plus alcohol yields ester plus

____________ . A. ether B. alkene C. alkane D. alkyne E. water

IIIC) C°H¡™ (straight chain) is A. saturated B. unsaturated

IIIC) Which plastic contains an aromatic (benzene) ring? A. polyvinyl

Chloride B. polyacrylonitrile C. polystyrene D. polyethene

You will be tested on the following objectives at the end of section III. D.

1. Interpret complex graphs with multiple lines that represent the sums of the information below each line.

2. Trace the history of energy sources and consumption patterns in the United States, and account for major changes.

3. Describe major sources of energy for the United States today.

4. Describe major sources of energy for the United States in the future.

5. Define biomolecules.

6. Describe major sources of energy and alternative sources of fuels and builder molecules for the future.

7. Describe alternative fuels that may be used to extend, supplement, or replace petroleum as Earth's primary fuel.

Sample Quiz Questions:

IIID) Which of the following is NOT a fossil fuel?•coal •hydrogen

•petroleum •natural gas

IIID) Probably the MAJOR problem with our present energy use pattern is

That A. our resources don't give us enough energy per gram

consumed. B. the nuclear wastes have no place to be discarded. C. the

major resources are nonrenewable. D. it is too expensive.

IIID) What are the advantages and disadvantages of a electric alternative

fuel vehicle? A. non-renewable, hard to store, burns easily, polluting B.

renewable, hard to store, nonpolluting C. renewable, hard to store,

nonpolluting, efficient D. complex hardware, hard to store, gasoline

pollutes-renewable

IIID) Press the "Graph" button below to see the graph! Then answer this

question! What per cent of our energy came from fossil fuels in 1970?

•12 •17 •45 •58 •94 (Graph is the same as the one in your book.)

IIID) An advantage of petroleum over wood could be that it is A. easier to

get. B. renewable. C. easier to transport. D. not polluting. E. cheaper.

UNIT IV

You will be tested on the following objectives at the end of section IV.A.5.

1. Be able to state the percent of oxygen, nitrogen and carbon dioxide in air.

2. Identify the major components of the troposphere and indicate their relative concentrations.

3. Sketch or graph the relationship between altitude and air pressure.

4. Discuss air pressure and explain how to measure it.

5. Define troposphere, derived units, barometer, kinetic energy, kinetic molecular theory, Boyle's Law, pressure, newton, pascal, and mmHg.

6. With force, area and pressure be able to determine the missing value if one is missing.

7. Describe with words and mathematical equations the interrelationships among volume and pressure of a gas(Boyle's law), and list one practical application.

8. Given volume and pressure information on a system be able to solve for the new volume or pressure.

Sample Quiz Questions:

IV.A.5) Standard atmospheric pressure is A. 100 atmosphere

B. 1 mm Hg C. 760 mm Hg D. 760 atmospheres

IV.A.5) Clean, unpolluted air is a pure substance. (True/False)

IV.A.5) Which can be used to explain both Boyle's Law and Charles'

Law? A. atomic theory B. law of conservation of atoms C. kinetic

molecular theory D. law of conservation of charges

IV.A.5) A given mass of oxygen occupies 400 mL when the pressure is

800 mm Hg. If the temperature is kept constant, what is the volume that

the gas will occupy when the pressure is decreased to 400 mm Hg? A.

200 mL C. 1600 mL B. 800 mL D. 2400 mL

IV.A.5) You have 1.42 L of a gas exerting a pressure of 125 kPa.

Assuming constant temperature, what pressure will the gas exert if its

volume is reduced to .853 L? A. 75.1 kPa C. 151 kPa B. 208 kPa

D. more information needed

You will be tested on the following objectives at the end of section IV.A.End.

1. Show how Avogadro's law and the concept of molar volume clarify the interpretation of chemical equations involving gases.

2. Be able to determine the number of liters of a gas in a chemical equation if given the volumes of the other gases.

3. Describe with words and mathematical equations the interrelationships among amount, temperature, volume, and pressure of a gas(Avogadro's, Charles' and Boyle's laws), and list one practical application of each law.

4. Account for the gas laws in terms of the kinetic molecular theory of gases.

5. Be able to solve problems involving pressure, temperature and volume in gases.

6. Define and apply in appropriate situations Charles' law, kelvins, ideal gase, Avogadro's Law, molar volume, absolute zero and STP.

Sample Quiz Questions:

IV.A.9) At constant pressure, the kelvin temperature divided by the

volume of a given gas sample is a constant value.

IV.A.9) What would the kelvin temperature be if the Celsius temperature

were 110 degrees?

IV.A.9) Standard pressure is the pressure exerted by the column of

mercury with a height of exactly A. 273 mm B. 760 mm C. 760 cm‹

D. 1.00 mL E. 1 ATM

IV.A.9) A sample of nitrogen occupies a volume of 250.0 mL at 298 K.

What volume will it occupy at 368 K? (Assume pressure is constant.)

2. 20.2 mL B. 31 mL C. 202 mL D. 309 mL E. 950 mL

IV.A.9) You have 23.5 mL of a gas collected at 755 mm Hg and 285 K.

What volume will it occupy at 742 mm Hg and 295 K. A. 22.3 mL

B. 23.1 mL C. 29.9 mL D. 24.8 mL

You will be tested on the following objectives at the end of section IV.B.

1. Define and apply in appropriate situations electromagnetic radiation, electromagnetic spectrum, photons, frequency, wavelength, greenhouse effect, greenhouse gases, reflectivity and carbon cycle.

2. Compare the various components of solar radiation. Electromagnetic radiation includes x-rays, gamma rays, ultraviolet(UV), visible and infrared(IR) radiation, radio waves and microwaves. The energy transmitted by radiation varies according to its wavelength---the shorter the wavelength, the higher the energy.

3. Earth's atmosphere protects living organisms by absorbing and distributing solar energy.

4. Electromagnetic radiation can interact with matter to transfer energy.

5. Describe the greenhouse effect, its natural incidence and causes, and the significance of industrial contributions.

6. Discribe the function of the ozone layer and how human acitivities may be affecting it.

Sample Quiz Questions:

IV.B) 90.0 ml of water in an insulated container is at a temperature of 25º C. A 24.3 g mass at 103º C. is lowered into the container and the water temperature changes to 29º C. What is the specific heat of the mass? Type your answer to the nearest hundredth without units.

IV.B) This part of sunlight has the most energy A. infrared B. visible light

3. ultraviolet

IV.B) What fraction of the energy absorbed from the Sun powers the

Earth's hydrologic cycle? A. one-eighth B. one-fifth C. one-fourth

4. one-third E. one-half

IV.B) Which has the highest energy and therefore may be most harmful?

A. cosmic rays B. ultraviolet rays C. infrared rays D. radio waves

IV.B) If a substance has a high specific heat capacity, which of the

following is true? A. It requires only a small amount of energy to

increase its temperture. B. Its temperture has been increased to the

maximum point. C. It will heat up quickly. D. It will glow in the dark.

E. It requires a large amount of energy to increase its temperature.

You will be tested on the following objectives at the end of section IV. C.

1. Define acid rain, hydronium ion, pH, alkaline, neutralization, molarity, dynamic equilibrium, and buffer.

2. Describe the sources and consequences of acid rain.

3. Define the terms acid and base, give examples of each, describe their formation with balanced ionic equations, and relate hydrogen ion concentration to the pH scale.

4. Rain water is naturally acidic, but contaminants in the atmosphere can produce precipitation that is even more acidic than normal.

5. Sulfur oxides and nitrogen oxides generated from natural and human sources contribute to acid rain.

6. Acids produce hydrogen(hydronium) ions in water, while bases produce hydroxide ions. Strong acids and bases ionize completely: weak acids and bases ionize only partially.

7. Acidic solutions contain a higher concentration of hydrogen ions than hydroxide ions; basic solutions contain a higher concentration of hydroxide ions than hydrogen ions. Neutral solutions contanin equal concentrations of hydrogen and hydroxide ions.

8. pH is a measure of the molar concentration of hydrogen ions in a solution. Solutions with pH 7.0 at room temperature are neutral, while those with a lower pH are acidic and those with a higher pH are basic.

9. Acidic precipitation can lower the pH of lakes and streams, which can adversely affect aquatic life.

Sample Quiz Questions:

IV.C) Normal rainwater has a pH of A. 14 B. 9.6 C. 7

5. 5.6

V.C) What color is Cu¤± in solution? A. colorless D. green

B. orange E. scarlet C. blue

VI.C&D) E = mc¤ is the equation that describes the amount of

given credit for this equation? A. Lise Meitner B. Neils Bohr