Physical Science Worksheet: Chapters 4 and 5
Physical Science Worksheet: Chapters 4 and 5
Multiple Choice
1. Polymers are large organic molecules that are made of
A) cations. B) anions. C) carbon and oxygen only. D) repeating units.
2. Each molecule of hydrochloric acid, HCl, contains one atom of hydrogen and
A) one atom of chlorine. B) one atom of oxygen. C) two atoms of chlorine. D) two atoms of oxygen.
3. The average atomic mass of the element cesium is approximately 133 amu. What is the mass of 3.00 mol of cesium?
A) 0.133 g B) 133 g C) 266 g D) 399 g
4. It is possible for different covalent compounds to have the same empirical formula because empirical formulas represent
A) a total of all ionic bonds. B) only the cations in the compound. C) a model of the compound. D) a ratio of atoms in the compound.
5. An atom’s mass number equals the number of
A) protons plus the number of electrons. B) protons plus the number of neutrons. C) protons. D) neutrons.
6. A mixture is different from a compound because each substance in a mixture
A) retains its own properties. B) changes its electric charge. C) forms an ion. D) changes from a solid to a liquid.
7. In which substance do the molecules have the strongest attractions to one another?
A) sugar, a solid B) hydrogen, a gas C) sulfuric acid, a liquid D) water, a liquid
8. Ionization refers to the process of
A) changing from one period to another. B) losing or gaining protons. C) turning lithium into fluorine. D) losing or gaining electrons.
9. When two hydrogen atoms bond, the positive nucleus of one atom attracts the
A) negative nucleus of the other atom. B) positive electron of the other atom. C) negative electron of the other atom. D) positive nucleus of the other atom.
10. Valence electrons determine an atom’s
A) mass. B) chemical properties. C) electric charge. D) period.
11. Molar mass is defined as
A) the number of particles in 1 mole of a substance. B) the SI base unit that describes the amount of a substance. C) the amount of a substance necessary to have a positive charge. D) the mass in grams of 1 mole of a substance.
12. The charge of an electron is
A) −2. B) −1. C) 0. D) +1.
13. The “rings” of the DNA “ladder” are made up of
A) paired monomers. B) sugar molecules. C) phosphates. D) amino acids.
14. Oxygen’s atomic number is 8. This means that an oxygen atom has
A) eight neutrons in its nucleus. B) a total of eight protons and neutrons. C) eight protons in its nucleus. D) a total of eight neutrons and electrons.
15. Covalent bonds are formed between
A) ions. B) metal atoms. C) nonmetal atoms. D) compounds.
16. When nickel combines with fluorine to form nickel (III) fluoride, the charge of the nickel ion is
A) Ni1+. B) Ni2+. C) Ni3+. D) Ni4+.
17. When copper combines with oxygen to form copper (II) oxide, the charge of the copper ion is
A) Cu1+. B) Cu2+. C) Cu3+. D) Cu4+.
18. Dalton’s atomic theory was accepted because
A) there was evidence to support it. B) Democritus said that it was correct. C) Dalton invented the electron microscope. D) Dalton showed how molecules are formed.
19. The order of elements in the periodic table is based on
A) the number of protons in the nucleus. B) the electric charge of the nucleus. C) the number of neutrons in the nucleus. D) atomic mass.
20. Semiconductors are elements that
A) have large atomic masses but small atomic numbers. B) do not form compounds. C) can conduct heat and electricity under certain conditions. D) are extremely hard.
21. Copper is a good conductor of electricity because its electrons
A) are positively charged. B) are free to move from atom to atom. C) can take on either positive or negative charges. D) are shared between neighboring compounds.
22. You have 85.5 g of fluorine, which has a molar mass of approximately 19 g/mol. How many moles of fluorine do you have?
A) 4.5 mol B) 19 mol C) 45 mol D) 85 mol
23. If the atomic mass of carbon is 12 amu, 1 mole of pure carbon will have a mass of
A) 6 g. B) 6 mol. C) 12 g. D) 12 mol.
24. A mole is an SI base unit that describes the
A) mass of a substance. B) amount of a substance. C) volume of a substance. D) electric charge of a substance.
25. In which type of bond do atoms share electrons?
A) covalent bonds B) metallic bonds C) ionic bonds D) polyatomic bonds
26. The name for the compound with the formula CuBr2 would be written as
A) copper(II) bromide. B) copper(I) bromide. C) copper bromine. D) copper(III) bromide.
27. Most halogens form compounds by
A) gaining an electron to form a negative ion. B) losing an electron to form a positive ion. C) losing protons. D) joining with both calcium and carbon.
28. Atoms of elements that are in the same group have the same number of
A) protons. B) neutrons. C) valence electrons. D) protons and neutrons.
29. You have 6.50 mol of chromium, which has a molar mass of approximately 52 g/mol. What is the mass in grams of this amount of chromium?
A) 3.38 g B) 33.8 g C) 338 g D) 3.38 kg
30. Atoms have no electric charge because they
A) have an equal number of charged and noncharged particles. B) have neutrons in their nuclei. C) have an equal number of electrons and protons. D) have an equal number of neutrons and protons.
31. Each molecule of table sugar, C12H22O11, contains
A) 0 atoms of carbon. B) 1 atom of carbon. C) 6 atoms of carbon. D) 12 atoms of carbon.
32. Which statement about the alkali metals is correct?
A) They are located in the left-most column of the periodic table. B) They are extremely nonreactive. C) They are usually gases. D) They form negative ions with a 1- charge.
33. A lithium ion is much less reactive than a lithium atom because it
A) is much more massive. B) has a full outermost energy level. C) has a negative electric charge. D) is in a different group in the periodic table.
34. Which compounds have carbon-carbon double bonds?
A) alkanes B) alkenes C) alcohols D) ionic compounds
35. According to Bohr’s model of the atom, electrons behave like
A) planets orbiting the sun. B) waves on a vibrating string. C) light energy in a vacuum. D) planets rotating on their axes.
36. Often atoms join so that each atom will have
A) an even number of electrons. B) an outermost energy level that is full of electrons. C) an equal number of protons and electrons. D) more electrons than either protons or neutrons.
37. Alcohols are organic compounds that contain
A) carbon and oxygen only. B) carbon and hydrogen only. C) carbon, oxygen, and hydrogen. D) carbon, nitrogen, and hydrogen.
38. The name for the compound with the formula Cr2O3 would be written as
A) chromium(I) oxide. B) chromium(II) oxide. C) chromium oxygen. D) chromium(III) oxide.
39. The simplest organic compound is
A) aspirin. B) table sugar. C) salt. D) methane.
40. Carbon and other nonmetals are found in which area of the periodic table?
A) on the left-most side B) on the right side C) in the middle column of the periodic table D) in the bottom rows
41. Dalton’s atomic theory stated that every element was made of atoms that could not be subdivided, atoms of the same element are alike, and
A) atoms are made of protons, neutrons, and electrons. B) the nucleus is the center of the atom. C) atoms can join to form molecules. D) atoms are constantly in motion.
42. Solid ionic compounds have very high melting points because they
A) are positively charged. B) contain metallic elements. C) are made of elements that are solid at room temperature. D) contain charged ions that are locked tightly together.
Physical Science Worksheet: Chapters 4 and 5
Answer Section
MULTIPLE CHOICE
1. D
2. A
3. D
4. D
5. B
6. A
7. A
8. D
9. C
10. B
11. D
12. B
13. A
14. C
15. C
16. C
17. B
18. A
19. A
20. C
21. B
22. A
23. C
24. B
25. A
26. A
27. A
28. C
29. C
30. C
31. D
32. A
33. B
34. B
35. A
36. B
37. C
38. D
39. D
40. B
41. C
42. D
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