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Midterm Review 2013-2014

A. Matching

Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line.


Column A
1. error
2. precision
3. 1 liter
4. temperature
5. density
6. conversion factor
7. dimensional analysis
8. weight
9. 1 kilogram
10. accuracy

Column B
a. a measure of the pull of gravity on a given mass
b. concerned with the reproducibility of measurements
c. a ratio of equivalent measurements
d. originally defined as the mass of 1 L of water at 4C
e. a way to analyze and solve problems, using the units of a measurement
f. the ratio of the mass of an object to its volume
g. the degree of hotness or coldness of an object
h. closeness of a measurement to the true value
i. difference between the experimental value and the accepted value
j. the volume of a cube 10 cm on each edge



B. Multiple Choice

Choose the best answer and write its letter on the line.
11. How many significant figures are in the measurement 2103.2 g?

a. 2 c. 4

b. 3 d. 5
12. Which of these equalities is not correct?

a. 100cg = 1 g c. 1 cm3 = 1 mL

b. 1000 mm = 1 m. d. 10 kg = 1 g
13. How many of the zeros in the measurement 0.000 040 200 m are significant?

a. 2 c. 7

b. 3 d. 8

70 Core Teaching Resources

Name Date Class
14. How many milligrams are in 2.5 kg?

a. 2.5 × 106 mg c. 2.5 × 10–4 mg

b. 25 mg. d. 2.5 × 102 mg.
15. The closeness of a measurement to its true value is a measure of its:

a. usefulness. c. accuracy.

b. precision. d. reproducibility.
16. Which of these measurements is expressed to three significant figures?

a. 0.070 mm c. 7007 mg

b. 7.30 ×10–7 km d. 0.007 m
17. A metric unit of volume is the:

a. L. c. km.

b. mg. d. K.
18. The number of seconds in a 40-hour work week can be calculated as follows:

a. c.

b. d.
19. The metric prefix kilo- means:

a. 100 times smaller. c. 1000 times smaller.

b. 1000 times larger. d. 100 times larger.
20. What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?

a. 86 mL c. 2.4 × 10–2 mL

b. 1.2 × 10–2 mL d. 42 mL.
21. The temperature reading of –14C corresponds to a Kelvin reading of:

a. 297.6 K c. 287 K.

b. –287 K. d. 259 K.
22. Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams, of 2.00 liters of this acid?

a. 2.38 × 103 g c. 4.20 × 10–4 g

b. 2.38 g d. 4.20 × 10–4 g
23. A conversion factor:

a. is equal to 1.

b. is a ratio of equivalent measurements.

c. does not change the value of a measurement.

d. all of the above
24. Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius?

a. 93°C c. –61°C

b. 34°C d. –34°C
25. A student measures a volume as 25 mL, whereas the correct volume is 23 mL. What is the percent error?

a. 0.087% c. 0.92%

b. 8.7% d. 8.0%
Chapter 3 Scientific Measurement 71

Name Date Class


C. True-False

Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
26. Precise measurements are also accurate measurements.
27. Zeros in a measurement are significant.
28. In converting between units, it is necessary to use more than one conversion factor.
29. When converting complex units, you should check that the units cancel, the conversion factors are correct, and the answer has the correct units.
30. The weight of an object changes with its location.
31. A kilogram is the mass of 1 mL of water at 4°C.
32. The density of a substance decreases at its temperature increases.
33. Heat transfers from objects at high temperatures to objects at low temperatures.
34. To convert density from g/cm3 to kg/m3, one of the conversion factors you could use is mg3/kg.
D. Problems

Solve the problems in the space provided. Show your work.
35. A cube of gold-colored metal with a volume of 64 cm3 has a mass of 980 g. The density of pure gold is 19.3 g/cm3. Is the metal pure gold?

36. Perform the following operations. Make sure that your answers have the correct number of significant digits.

a. 4.15 cm × 1.8 cm

b. 13.00 m – 0.54 m

c. (1.7 × 105 m) × (3.72  104 m)


72 Core Teaching Resources

Name Date Class


37. Calculate the density of a liquid that has a mass of 14.0 g and a volume of 18.0 cm3.

E. Essay

Write a short essay for the following.
38. Explain how density differs from volume.




















A. Multiple Choice

Choose the best answer and write its letter on the line.
1. Identify the activity that belongs in the field of chemistry.

a. developing medicines c. production of a new plastic

b. analysis of a compound d. all of the above
2. Which of these chemicals is definitely inorganic?

a. one that is made of carbon and hydrogen

b. one that is made of nitrogen and carbon

c. one that is made of nitrogen and hydrogen

d. one that is made of carbon and oxygen
3. Which of the following is not a step for solving a numeric word problem?

a. calculate c. analyze

b. conclude d. evaluate
4. Identify the false statement.

a. Chemistry plays an important role in efforts to increase the world's food supply and to protect crops.

b. Biodiesel is a fossil fuel.

c. Potato plants with a jellyfish gene will glow when they need to be watered.

d. Chemists are working to develop more pest-resistant and disease-resistant plants.
5. A hypothesis is

a. an observation recorded from an experiment.

b. a proposed explanation for what is observed.

c. a summary of the results of many experiments.

d. a well-tested explanation for many observations.
6. Which of the following is not a part of the scientific method?

a. experimenting c. proving

b. observing d. hypothesizing
7. Identify the false statement.

a. A scientific law fully explains a set of observations.

b. The scientific method is a logical, systematic approach to the solution of a problem.

c. For the results of an experiment to be accepted, the experiment must produce the same results no matter how many times it is repeated.

d. The scientific method is repeated until a hypothesis either fits all the observed experimental results or the hypothesis is discarded.

Chapter 1 Introduction to Chemistry 21

Name Date Class


8. Which of these steps of the scientific method involves stating a relationship but not proposing an explanation for the relationship?

a. observation c. theory

b. scientific law d. hypothesis
B. Questions

Write your answer in the space provided.
9. Define chemistry.





10. List the major steps in the scientific method and describe each briefly.










A. Matching

Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line.


Column A
1. a physical blend of two or more components
2. the change of one or more substances into new substances
3. amount of matter that an object contains
4. a homogeneous mixture
5. a substance that can be separated into simpler substances only by chemical means
6. the simplest form of matter that has a unique set of properties
7. depends on the type of matter in a sample
8. matter that takes both the shape and the volume of its container
9. matter that has a uniform and definite composition
10. a quality or condition of a substance that can be observed or measured without changing the substance’s composition

Column B
a. solution
b. element

c. substance
d. chemical reaction
e. gas

f. intensive property
g. physical property
h. mass

i. mixture
j. compound



B. Multiple Choice

Choose the best answer for each question and write its letter on the line.
11. Another name for homogenous mixture is

a. solution. c. element.

b. matter. d. mass.
12. The chemical symbol for iron is:

a. Ir. c. Fe.

b. FE. d. I.
13. Which of the following is a physical property?

a. color c. freezing point

b. hardness d. all of the above

48 Core Teaching Resources

Name Date Class
14. Which of the following statements describes a solid?

a. It takes the shape of its container.

b. It takes the volume of its container.

c. Its particles are packed together tightly.

d. It is easily compressed.
15. At room temperature, which of the following is typically in a physical state different from that of the other three?

a. water c. grape juice

b. milk d. oxygen
16. Which term does not fit with the others listed?

a. ice c. salt

b. steam d. water
17. Which of the following is an example of a physical change?

a. toasting bread c. digesting a banana

b. cooking a hamburger d. melting butter
18. An example of a heterogeneous mixture would be

a. sugar. c. tap water.

b. salt water. d. vegetable soup.
19. Which of the following is a compound?

a. carbon c. oxygen

b. hydrogen d. water
20. Iron is an example of a(n)

a. element. c. heterogeneous mixture.

b. compound. d. homogeneous mixture.
21. The element whose chemical symbol is C is

a. calcium. c. copper.

b. carbon. d. chlorine.
22. Which of the following events can best distinguish a physical change from a chemical change?

a. Energy is absorbed or released. c. A gas is produced.

b. a different chemical composition d. Mass is conserved.
23. Which of the following is an example of a chemical change?

a. cooking meat c. dissolving sugar in iced tea

b. slicing cheese d. freezing water
C. True-False

Classify each of these statements as always true (AT), sometimes true (ST), or never true (NT).
24. In a chemical reaction, mass is neither created nor destroyed; it is conserved.
25. Dissolving salt in water is a chemical change.

Chapter 2 Matter and Change 49

Name Date Class


26. Physical changes are not easily reversed.
27. Elements can be separated into simpler substances by chemical reactions.
28. Energy is transferred during chemical reactions.
D. Completion

Fill in the word(s) that will make each statement true.
29. A ________________________ is a form of matter that flows, has a fixed volume, and takes the shape of its container.
30. A ________________________ is a gaseous substance that is generally a liquid or solid at room temperature.
31. A tossed green salad is an example of a ________________________ mixture.
32. The chemical symbol for the element nitrogen is ________________________.
33. In a chemical reaction, the starting substances are called ________________________.
34. The burning of wood is an example of a ________________________ change.
35. The evaporation of water is an example of a ________________________ change.
36. Any matter that has a uniform and definite composition is a(n) ________________________.
E. Essay

Write a short essay for the following.
37. Name at least one physical property of each of the following four materials that could be used to separate it from a mixture of all four. Describe how you would separate a mixture of salt, water, iron filings, and sawdust.













A. Matching

Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line.


Column A
1. proton
2. atom

3. mass number
4. atomic mass unit
5. electron
6. isotopes
7. atomic number
8. atomic mass
9. period
10. neutron

Column B
a. the total number of protons and neutrons in the nucleus of an atom
b. the weighted average mass of the atoms in a naturally occurring sample of an element
c. the mass of a carbon-12 atom
d. the number of protons in the nucleus of an element
e. atoms with the same number of protons but different numbers of neutrons
f. negatively charged subatomic particle
g. the smallest particle of an element that retains its identity in a chemical reaction
h. a horizontal row of the periodic table
i. subatomic particle with no charge
j. positively charged subatomic particle


B. Multiple Choice

Choose the best answer and write its letter on the line.
11. Which of the following is not a part of Dalton’s atomic theory?

a. All elements are composed of atoms.

b. Atoms of the same element are alike.

c. Atoms are always in motion.

d. Atoms that combine do so in simple whole-number ratios.
12. The nucleus of an atom is

a. negatively charged and has a low density.

b. negatively charged and has a high density.

c. positively charged and has a low density.

d. positively charged and has a high density.

Chapter 4 Atomic Structure 93

Name Date Class
13. Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now know that

a. Dalton’s theories are completely correct.

b. atoms of an element can have different numbers of protons.

c. atoms are all divisible.

d. all atoms of an element are not identical but they all have the same mass.
14. The number of neutrons in the nucleus of an atom can be calculated by

a. adding together the numbers of electrons and protons.

b. subtracting the number of protons from the number of electrons.

c. subtracting the number of protons from the mass number.

d. adding the mass number to the number of protons.
15. The sum of the protons and neutrons in an atom equals the

a. atomic number. c. atomic mass.

b. number of electrons. d. mass number.
16. All atoms of the same element have the same:

a. number of protons. c. mass number.

b. number of neutrons. d. mass.
17. Which of these statements is false?

a. Electrons have a negative charge.

b. Electrons have a mass of 1 amu.

c. The nucleus of an atom is positively charged.

d. The neutron is found in the nucleus of an atom.
18. An atom of an element with atomic number 48 and mass number 120 contains

a. 48 protons, 48 electrons, and 72 neutrons.

b. 72 protons, 48 electrons, and 48 neutrons.

c. 120 protons, 48 electrons, and 72 neutrons.

d. 72 protons, 72 electrons, and 48 neutrons.
19. How do the isotopes hydrogen-2 and hydrogen-3 differ?

a. Hydrogen-3 has one more electron than hydrogen-2.

b. Hydrogen-3 has two neutrons.

c. Hydrogen-2 has three protons.

d. Hydrogen-2 has no protons.
20. The number 80 in the name bromine-80 represents

a. the atomic number.

b. the mass number.


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