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INTRODUCTION TO CHEMISTRY
Practice Problems In your notebook, solve the following problems.
SECTION 1.1 CHEMISTRY 1. Match the project to the appropriate field of chemistry (inorganic chemistry, organic chemistry, biochemistry, analytical chemistry, or physical chemistry). a. Determine the composition of a moon rock sample. b. Do research on making a new medicine to treat high blood pressure. c. Investigate ways to regulate the rate of gasoline burning in an automobile engine. d. Develop a plastic that can be decomposed by bacteria. e. Improve the method for extracting iron from iron ore. 2. Classify the following examples as examples of pure chemistry or applied chemistry. a. developing a shampoo to be used with dry or damaged hair b. determining the conditions required for materials to burn c. figuring out the general structure of materials such as cotton and silk d. designing a large-scale method for producing nylon
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e. explaining why water expands when it freezes
SECTION 1.2 CHEMISTRY FAR AND WIDE 1. Identify three areas of energy research that scientists are working on today. 2. The following statements are all concerned with the work chemists do. Write T for each true statement and F for each false statement. a. Chemists design materials to meet specific needs. b. Oil from the soybean plant is used to make biodiesel. c. As the world’s population increases, the amount of land available to grow food increases. d. Many drugs are effective because they interact in a specific way with chemicals in cells. e. The trend in crop protection is toward chemicals that are less specific. f. The use of lead paint in houses was banned in 1978. g. Chemists are doing research to improve batteries. h. To study the universe, chemists gather data from afar and analyze matter that is brought back to Earth. i. Chemists have developed a plastic “skin” that can heal itself when it cracks to help patients with burns.
Chapter 1 Introduction to Chemistry
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SECTION 1.3 THINKING LIKE A SCIENTIST 1. One cold morning your car does not start. Make two hypotheses about why the car will not start. 2. Suppose you try several experiments with your car. You try a battery jump, which does not work. There seems to be enough gas in the car. You wiggle a wire in the engine, and the car starts on the next try. Explain how these tests help you decide what was wrong with the car. 3. The following is a list of observations from everyday experiences: Hummingbirds have long beaks. Moisture forms on the outside of a cold glass. Ice cubes float. Oil and water don't mix. There are fewer fish in a particular creek this year. a. Propose one hypothesis for each observation. b. Select one of the hypotheses and describe an experiment that you could do to test it. 4. Discuss the statement “No theory is written in stone.”
SECTION 1.4 PROBLEM SOLVING IN CHEMISTRY 1. Apples are selling for $1.50 a pound. Each apple weighs, on average, 0.50 pounds. You have $6.00. How many apples can you purchase? a. ANALYZE (List the knowns and unknown.) Knowns: Unknown: cost of apples !
number of apples purchased ! ?
dollars available ! b. CALCULATE (Solve for the unknown.) Use an expression that converts cost per pound to cost per apple. $1.50 cost per apple ! 0.50 pound " ## 1 pound cost per apple ! Use an expression that relates cost per apple to dollars available. $6.00 number of apples purchased ! # $0.75 number of apples purchased ! 2. Describe an alternate way to solve Problem 1.
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Core Teaching Resources
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weight of an apple !
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MATTER AND CHANGE
2
Practice Problems In your notebook, solve the following problems.
SECTION 2.1 PROPERTIES OF MATTER 1. Which of the following is not a physical change? a. dissolving sugar in water
c. evaporating sea water to obtain salt
b. burning gasoline in an engine
d. slicing a piece of bread
2. Which of the following is not a property of a gas? a. has a definite shape
c. assumes the shape of its container
b. has an indefinite volume
d. is easily compressed
3. Which of the following is not a physical property of sucrose? a. solid at room temperature
c. dissolves in water
b. decomposes when heated
d. tastes sweet
4. Which of the following is in a different physical state at room temperature than the other three? a. salt
b. sugar
c. flour
d. water
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5. Complete the following table. Physical state
Definite Shape?
Definite Volume?
Easily Compressed?
gas no
no
yes Use the Table 2.1 to answer the following questions. 6. Which substance is a colored gas? 7. Which liquids boil at a lower temperature than water? 8. Classify the following properties as extensive or intensive. a. color
b. volume
c. mass
d. boiling point
Chapter 2 Matter and Change
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SECTION 2.2 MIXTURES 1. How might you separate a mixture of water and salt? 2. What is a homogeneous mixture? 3. Which of the following mixtures are homogeneous? Which are heterogeneous? a. gasoline
b. chunky peanut butter
c. oil and vinegar salad dressing
4. Which of the following are substances? Which are mixtures? a. ethanol
b. motor oil
c. vinegar
d. neon
SECTION 2.3 ELEMENTS AND COMPOUNDS 1. What elements make up ammonia, chemical formula NH3? 2. Name the elements represented by the following chemical symbols. a. Pb
b. K
c. Au
d. Fe
3. Classify the following as elements, compounds, or mixtures. a. table salt
b. water
c. iron
d. stainless steel
4. Write the chemical symbol for each of the following elements. a. tin
b. sodium
c. silver
d. carbon
5. A liquid is allowed to evaporate and leaves no residue. Can you determine whether it was an element, a compound, or a mixture? 6. Which of the following is not an element? a. copper
b. sulfur
c. sucrose
d. helium
1. Which one of the following is a chemical change? a. Gasoline boils.
c. Gasoline burns.
b. Oxygen is added to gasoline.
d. Gasoline is poured into a tank.
2. Classify each of the following changes as physical or chemical. a. A puddle is dried by the sun.
c. Bread is toasted.
b. A dark cloth is faded by sunlight.
d. Soap is mixed with water.
3. Carbon dioxide plus water yields carbonic acid. a. Name the product(s) of this reaction. b. Name the reactant(s) of this reaction. 4. If 44 grams of carbon dioxide react completely with 18 grams of water, what is the mass of carbonic acid formed? 5. In an engine, octane combines with oxygen to form carbon dioxide and water. If 22.8 grams of octane combine completely with 80 grams of oxygen to form 70.4 grams of carbon dioxide, what mass of water is formed? 6. What is the name of the chemical law on which problems 4 and 5 are based?
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SECTION 2.4 CHEMICAL REACTIONS
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SCIENTIFIC MEASUREMENT
Practice Problems In your notebook, solve the following problems.
SECTION 3.1 MEASUREMENTS AND THEIR UNCERTAINTY Using different rulers, Bruce and Pete each measure the length of the same object three times. 1. Bruce’s three measurements are 19 cm, 20 cm, and 22 cm. Calculate the average value of his measurements and express the answer with the correct number of significant figures. 2. Pete’s three measurements are 20.9 cm, 21.0 cm, and 21.0 cm. Calculate the average value of his measurements and express the answer with the correct number of significant figures. 3. Multiply the answer to problem 1 by the answer to problem 2. Express the answer in scientific notation with the correct number of significant figures. 4. Whose measurements are more precise? 5. The actual length of the object is 20 cm. Whose measurements are more accurate? 6. What is the error of Pete’s average measurement? 7. What is the percent error of Pete’s average measurement?
SECTION 3.2 THE INTERNATIONAL SYSTEM OF UNITS (SI) A fish tank measures 0.40 meter long by 0.20 meter wide by 0.30 meter high. 1. What is the width of the tank in centimeters? 2. What is the length of the tank in millimeters? 3. What is the volume of the tank in liters? 4. What is the mass of water, in grams, that would fill the tank halfway? 5. An astronaut in her spacesuit weighs 300 lb on Earth. What would her weight be on the moon? 6. How many nanoseconds are there in one minute? 7. A chemical reaction takes place at 20!C. What is this temperature in kelvins? 8. A typical refrigerator keeps food at 277 K. What is this temperature in degrees Celsius?
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Core Teaching Resources
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8. Four boards each measuring 1.5 m are laid end to end. Multiply to determine the combined length of the boards, expressed with the correct number of significant figures.
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SECTION 3.3 CONVERSION PROBLEMS 1. The population of San Francisco is 750,000 in an area of 49 square miles. What is the population density in San Francisco? Express your answer in people per acre. (1 mi2 " 640 acres) 2. A sugar-free powdered drink mix sells for $2.99 per can. Each can of the mix contains 50.2 g of powder, which, when added to water, will make 8 quarts of drink. What is the cost of the powdered drink mix in dollars/lb? (454 g " 1 lb) 3. A car is travelling at 60 miles per hour. Express this speed in kilometers per hour (km/h). (1 mi " 1.609 km) 4. A whole chicken sells for $7.06 and has a mass of 1.5 kg. A beef shank sells for $10.00 with a mass of 2.5 kg. Compare the per pound cost for each item. (1 kg " 2.2 lb) 5. How many seconds are there in a day? (1 day " 24 h) 6. The speed limit on a certain highway is 72 km/h. What is this speed in cm/s? 7. Gold has a density of 19.3 g/cm3. What is the mass, in kilograms, of one cubic meter of gold? 8. An automobile can travel 40.0 miles on one gallon of gasoline. How many kilometers per liter is this? (1.61 km " 1 mi; 1 L " 0.264 gal) 9. Suppose that gold is selling at $375/ounce. How many milligrams of gold could you buy for one cent? (16 oz " 1 lb; 1 lb " 454 g)
SECTION 3.4 DENSITY © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
Use the data in Table 3.7 to solve problems 1–4. 1. What is the mass at 20!C of 5 liters of air? 2. A balloon filled with air is released in a room filled with carbon dioxide. Will the balloon float to the ceiling or sink to the floor? 3. What is the volume in liters of a kilogram of ice at 0!C? 4. What is the mass of a bar of aluminum measuring 1.0 cm by 1.0 cm by 10.0 cm?
Chapter 3 Scientific Measurement
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ATOMIC STRUCTURE
Practice Problems In your notebook, solve the following problems.
SECTION 4.1 DEFINING THE ATOM 1. According to Figure 5.2, 100,000,000 copper atoms would form a line 1 cm long. How long would a line formed by 1 ! 107 copper atoms be? Express your answer in millimeters.
SECTION 4.2 STRUCTURE OF THE NUCLEAR ATOM 1. A sulfur-32 atom contains 16 protons, 16 neutrons, and 16 electrons. What is the mass (in grams) of a sulfur-32 atom? 2. The mass of a neutron is 1.67 ! 10"24 g. Approximately what number of neutrons would equal a mass of one gram? 3. Which statement is consistent with the results of Rutherford’s gold foil experiment? a. All atoms have a positive charge. b. Atoms are mostly empty space.
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c. The nucleus of an atom contains protons and electrons. d. Mass is spread uniformly throughout an atom.
SECTION 4.3 DISTINGUISHING BETWEEN ATOMS 1. How many protons are found in an atom of each of the following? a. boron c. neon b. sulfur
d. lithium
2. Complete the table for the following elements. Element
Number of Protons
Manganese
25
Sodium Bromine
Number of Electrons
Actinium
Atomic Number
Mass Number
39
89
30 11
35
12 45
Yttrium Arsenic
Number of Neutrons
33
75 227 Chapter 4 Atomic Structure
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3. How many neutrons are in each atom? a. 23 c. 81 11Na 35Br b.
238 92 U
d.
19 9F
4. The two most abundant isotopes of carbon are carbon-12 (mass # 12.00 amu) and carbon-13 (mass # 13.00 amu). Their relative abundances are 98.9% and 1.10%, respectively. Calculate the atomic mass of carbon. 5. Element X has two isotopes: X-100 and X-104. If the atomic mass of X is 101 amu, what is the relative abundance of each isotope in nature?
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ELECTRONS IN ATOMS
Practice Problems In your notebook, solve the following problems.
SECTION 5.1 MODELS OF THE ATOM 1. How many sublevels are in the following principal energy levels? a. n ! 1
c. n ! 3
e. n ! 5
b. n ! 2
d. n ! 4
f. n ! 6
2. How many orbitals are in the following sublevels? a. 1s sublevel
d. 4f sublevel
g. fifth principal energy level
b. 5s sublevel
e. 7s sublevel
h. 6d sublevel
c. 4d sublevel
f. 3p sublevel
3. What are the types of sublevels and number of orbitals in the following energy levels? a. n ! 1
c. n ! 3
b. n ! 2
d. n ! 4
e. n ! 5
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SECTION 5.2 ELECTRON ARRANGEMENT IN ATOMS 1. Write a complete electron configuration of each atom. a. hydrogen
d. barium
g. krypton
b. vanadium
e. bromine
h. arsenic
c. magnesium
f. sulfur
i. radon
SECTION 5.3 PHYSICS AND THE QUANTUM MECHANICAL MODEL 1. What is the wavelength of the radiation whose frequency is 5.00 " 1015 s#1? In what region of the electromagnetic spectrum is this radiation? 2. An inexpensive laser that is available to the public emits light that has a wavelength of 670 nm. What are the color and frequency of the radiation? 3. What is the energy of a photon whose frequency is 2.22 " 1014 s#1? 4. What is the frequency of a photon whose energy is 6.00 " 10#15 J? 5. Arrange the following types of electromagnetic radiation in order of increasing frequency. a. infrared
c. visible light
e. microwaves
b. cosmic rays
d. radio waves
f. ultraviolet
6. Suppose that your favorite AM radio station broadcasts at a frequency of 1600 kHz. What is the wavelength in meters of the radiation from the station? Chapter 5 Electrons in Atoms
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THE PERIODIC TABLE
Practice Problems In your notebook, solve the following problems.
SECTION 6.1 ORGANIZING THE ELEMENTS 1. Which element listed below should have chemical properties similar to fluorine (F)? a. Li b. Si c. Br d. Ne 2. Identify each element as a metal, metalloid, or nonmetal. a. fluorine b. germanium c. zinc d. phosphorus e. lithium © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
3. Which of the following is not a transition metal? a. magnesium b. titanium c. chromium d. mercury 4. Name two elements that have properties similar to those of the element potassium. 5. Elements in the periodic table can be divided into three broad classes based on their general characteristics. What are these classes and how do they differ?
Chapter 6 The Periodic Table
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SECTION 6.2 CLASSIFYING THE ELEMENTS 1. Use the periodic table to write the electron configuration for silicon. Explain your thinking. 2. Use the periodic table to write the electron configuration for iodine. Explain your thinking. 3. Which group of elements is characterized by an s2p3 configuration? 4. Name the element that matches the following description. a. one that has 5 electrons in the third energy level b. one with an electron configuration that ends in 4s24p5 c. the Group 6A element in period 4 5. Identify the elements that have electron configurations that end as follows. a. 2s22p4 b. 4s2 c. 3d104s2 6. What is the common characteristic of the electron configurations of the elements Ne and Ar? In which group would you find them? 7. Why would you expect lithium (Li) and sulfur (S) to have different chemical and physical properties? 8. What characterizes the electron configurations of transition metals such as silver (Ag) and iron (Fe)?
SECTION 6.3 PERIODIC TRENDS 2. Predict the size of the astatine (At) atom compared to that of tellurium (Te). Explain your prediction. 3. Would you expect a Cl! ion to be larger or smaller than an Mg2" ion? Explain. 4. Which effect on atomic size is more significant, an increase in nuclear charge across a period or an increase in occupied energy levels within a group? Explain. 5. Explain why the sulfide ion (S2!) is larger than the chloride ion (Cl!). 6. Compare the first ionization energy of sodium to that of potassium. 7. Compare the first ionization energy lithium to that of beryllium. 8. Is the electronegativity of barium larger or smaller than that of strontium? Explain. 9. What is the most likely ion for magnesium to form? Explain. 10. Arrange oxygen, fluorine, and sulfur in order of increasing electronegativity.
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1. Explain why a magnesium atom is smaller than atoms of both sodium and calcium.
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IONIC AND METALLIC BONDING
Practice Problems In your notebook, answer the following.
SECTION 7.1 IONS 1. For each element below, state (i) the number of valence electrons in the atom, (ii) the electron dot structure, and (iii) the chemical symbol(s) for the most stable ion. a. Ba
b. I
c. K
2. How many valence electrons does each of the following atoms have? a. gallium
b. fluorine
c. selenium
3. Write the electron configuration for each of the following atoms and ions. e. O2"
a. Ca
c. Na!
b. chlorine atom
d. phosphide ion
4. What is the relationship between the group number of the representative elements and the number of valence electrons? 5. How many electrons will each element gain or lose in forming an ion? State whether the resulting ion is a cation or an anion. c. tellurium
e. bromine
b. aluminum
d. rubidium
f. phosphorus
6. Give the name and symbol of the ion formed when a. a chlorine atom gains one electron. b. a potassium atom loses one electron. c. an oxygen atom gains two electrons. d. a barium atom loses two electrons. 7. How many electrons are lost or gained in forming each of the following ions? a. Mg2!
b. Br"
c. Ag!
8. Classify each of the following as a cation or an anion.
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a. Na!
c. I"
e. Ca2!
b. Cu2!
d. O2"
f. Cs!
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d. Fe3!
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a. strontium
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SECTION 7.2 IONIC BONDS AND IONIC COMPOUNDS 1. Use electron dot structures to predict the formula of the ionic compounds formed when the following elements combine. a. sodium and bromine
d. aluminum and oxygen
b. sodium and sulfur
e. barium and chlorine
c. calcium and iodine 2. Which of these combinations of elements are most likely to react to form ionic compounds? a. sodium and magnesium
c. potassium and iodine
b. barium and sulfur
d. oxygen and argon
3. What is the meaning of coordination number? 4. How is the coordination number determined?
SECTION 7.3 BONDING IN METALS 1. What is a metallic bond? 2. How is the electrical conductivity of a metal explained by metallic bonds? 3. Are metals crystalline? Explain. 4. Give three possible crystalline arrangements of metals. Describe each. 5. What is an alloy?
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6. Name the principal elements present in each of the following alloys. a. brass
d. sterling silver
b. bronze
e. cast iron
c. stainless steel
f. spring steel
Chapter 7 Ionic and Metallic Bonding
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