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Physical Science Final

True/False
Place a check by each element that forms diatomic molecules and is not found in nature as single atoms.
 

1. 
Bromine
 

2. 
Cesium
 

3. 
Chlorine
 

4. 
Helium
 

5. 
Iodine
 

6. 
Hydrogen
 

7. 
Nitrogen
 

8. 
Oxygen
 

9. 
Carbon
 

10. 
Xenon
 

11. 
Neon
 

12. 
Fluorine
 

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

13. 
Matter is defined as anything that
a.
can be seen and touched.
c.
can be weighed.
b.
has mass and takes up space.
d.
contains kinetic or potential energy.
 

14. 
A substance that cannot be broken down into simpler substances is
a.
a compound.
c.
an element.
b.
a mixture.
d.
an atom.
 

15. 
The chemical formula for water, H2O, means that each water molecule contains
a.
two hydrogen atoms and two oxygen atoms.
b.
two hydrogen atoms and one oxygen atom.
c.
two hydrogen atoms and zero oxygen atoms.
d.
one hydrogen atom and two oxygen atoms.
 

16. 
The science of what matter is made of and how it changes is called
a.
chemistry.
c.
kinetics.
b.
physics.
d.
engineering.
 

17. 
The chemical symbol for sulfuric acid is H2SO4. How many atoms are contained in each molecule of sulfuric acid?
a.
3
c.
6
b.
5
d.
7
 

18. 
The chemical formula for table sugar is C12H22O11. How many oxygen atoms are in each sugar molecule?
a.
2
c.
12
b.
11
d.
22
 

19. 
Which state of matter will hold its shape without a container?
a.
solid
c.
gas
b.
liquid
d.
plasma
 

20. 
The change of a substance from a solid directly to a gas is called
a.
condensation.
c.
melting.
b.
evaporation.
d.
sublimation.
 

21. 
All changes of the state of matter require
a.
water.
c.
energy.
b.
vibration.
d.
sublimation.
 

22. 
Evaporation refers to the change of state from a
a.
liquid to a gas.
c.
solid to a liquid.
b.
gas to a liquid.
d.
liquid to a solid.
 

23. 
The law of conservation of mass states that mass cannot be
a.
burned.
c.
created or destroyed.
b.
changed in form.
d.
heated or cooled.
 

24. 
A liquid changes rapidly into a gas at the liquid's
a.
boiling point.
c.
melting point.
b.
freezing point.
d.
condensation point.
 

25. 
Which statement about the atomic nucleus is correct?
a.
The nucleus is made of protons and neutrons and has a negative charge.
b.
The nucleus is made of protons and neutrons and has a positive charge.
c.
The nucleus is made of electrons and has a positive charge.
d.
The nucleus is made of electrons and has a negative charge.
 

26. 
The charge of an electron is
a.
–2
c.
0
b.
–1
d.
+1
 

27. 
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.
 

28. 
According to Bohr's model of the atom, electrons behave like
a.
planets orbiting the sun.
c.
light energy in a vacuum.
b.
waves on a vibrating string.
d.
planets rotating on their axes.
 

29. 
According to modern atomic theory, it is nearly impossible to determine an electron's exact
a.
color.
c.
charge
b.
position.
d.
mass.
 

30. 
The order of elements in the periodic table is based on
a.
the number of protons in the nucleus.
c.
the number of neutrons in the nucleus.
b.
the electric charge of the nucleus.
d.
atomic mass.
 

31. 
Atoms of elements that are in the same group have the same number of
a.
protons.
c.
valence electrons.
b.
neutrons.
d.
protons and neutrons.
 

32. 
Valence electrons determine an atom's
a.
mass.
c.
electric charge.
b.
chemical properties.
d.
period.
 

33. 
Oxygen has atomic number 8. This means that an oxygen atom has
a.
eight neutrons in its nucleus.
c.
eight protons in its nucleus.
b.
a total of eight protons and neutrons.
d.
a total of eight neutrons and electrons.
 

34. 
An atom's mass number equals the number of
a.
protons plus the number of electrons.
c.
protons.
b.
protons plus the number of neutrons.
d.
neutrons.
 

35. 
Which of the following elements is an alkali metal?
a.
calcium
c.
mercury
b.
magnesium
d.
sodium
 

36. 
Alkali metals are extremely reactive because they
a.
have very small atomic masses.
b.
are not solids at room temperature.
c.
have one valence electron that is easily removed to form a positive ion.
d.
have two valence electrons that form compounds with calcium and magnesium.
 

37. 
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.
 

38. 
Group 18 noble gases are inert because
a.
they readily form positive ions.
b.
they can have either a positive or a negative charge.
c.
their outermost energy level is missing one electron.
d.
their outermost energy level is full.
 

39. 
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.
 

40. 
A mole is an SI base unit that describes the
a.
mass of a substance.
c.
volume of a substance.
b.
amount of a substance.
d.
electric charge of a substance.
 

41. 
Avogadro's constant is defined as the number of particles in
a.
one mole of a pure substance.
c.
one gram of a pure substance.
b.
one liter of a pure substance.
d.
one kilogram of a pure substance.
 

42. 
The average atomic mass of potassium is approximately 39 amu. What is the mass of 2.0 mol of potassium?
a.
0.39 g
c.
39 g
b.
0.78 g
d.
78 g
 

43. 
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
c.
266 g
b.
133 g
d.
399 g
 

44. 
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
c.
338 g
b.
33.8 g
d.
3.38 kg
 

45. 
What is the mass in grams of 0.75 mol of sulfur, which has a molar mass of approximately 32 g/mol?
a.
16 g
c.
32 g
b.
24 g
d.
240 g
 

46. 
Each molecule of hydrochloric acid, HCl, contains one atom of hydrogen and
a.
one atom of chlorine.
c.
two atoms of chlorine.
b.
one atom of oxygen.
d.
two atoms of oxygen.
 

47. 
In which substance do the molecules have the strongest attractions to one another?
a.
sugar, a solid
c.
sulfuric acid, a liquid
b.
hydrogen, a gas
d.
water, a liquid
 

48. 
Gases take up a lot of space because
a.
they have weak chemical bonds.
b.
their molecules have very little attraction for one another.
c.
they contain very few atoms.
d.
they have a small molar mass.
 

49. 
The bonds that hold atoms together behave most like
a.
snap-together blocks.
c.
rubber cement.
b.
glue.
d.
flexible springs.
 

50. 
An ionic bond is a bond that forms between
a.
ions with opposite charges.
b.
atoms with neutral charges.
c.
one atom's nucleus and another atom's electrons.
d.
the electrons of two different atoms.
 

51. 
Covalent bonds are formed between
a.
ions.
c.
nonmetal atoms.
b.
metal atoms.
d.
compounds.
 

52. 
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.
 

53. 
In which type of bond do atoms share electrons?
a.
covalent bonds
c.
ionic bonds
b.
metallic bonds
d.
polyatomic bonds
 

54. 
The name dinitrogen tetroxide tells you that this compound contains
a.
two nitrogen atoms and two oxygen atoms.
b.
four nitrogen atoms and two oxygen atoms.
c.
two nitrogen atoms and four oxygen atoms.
d.
four nitrogen atoms and four oxygen atoms.
 

55. 
Fe2O3 is named iron(III) oxide because it contains
a.
three oxygen atoms.
c.
three iron atoms.
b.
Fe3+ ions.
d.
O3+ ions.
 

56. 
When copper combines with oxygen to form copper(II) oxide, the charge of the copper ion is
a.
Cu1+.
c.
Cu3+.
b.
Cu2+.
d.
Cu4+.
 

57. 
When nickel combines with fluorine to form nickel(III) fluoride, the charge of the nickel ion is
a.
Ni1+.
c.
Ni3+.
b.
Ni2+.
d.
Ni4+.
 

58. 
Polymers are large organic molecules that are made of
a.
cations.
c.
carbon and oxygen only.
b.
anions.
d.
repeating units.
 

59. 
A change in color, such as rusting of metal, is a sign that
a.
a chemical change is taking place.
c.
oxygen is present.
b.
a physical change has just occurred.
d.
organic chemicals are present.
 

60. 
What happens in a chemical reaction?
a.
Atoms are destroyed.
c.
Atoms are heated and cooled.
b.
Atoms are created.
d.
Atoms are rearranged.
 

61. 
In an exothermic reaction, energy is transferred from
a.
the reactants to the surroundings.
c.
one reactant to another.
b.
the surroundings to the reactants.
d.
the container to the chemicals.
 

62. 
A synthesis reaction is a reaction between at least two compounds in which
a.
one breaks down into at least two products.
b.
a compound is decomposed by an electric current.
c.
a compound burns in the presence of oxygen.
d.
a new, more complex compound is formed.
 

63. 
Which of the following is an example of a decomposition reaction?
a.
photosynthesis
b.
digestion
c.
respiration
d.
exchange of ions between two compounds
 

64. 
A chemical equation is balanced by changing or adding
a.
chemical symbols.
c.
coefficients.
b.
subscripts.
d.
reactants.
 

65. 
In the reaction 2H2O ® 2H2 + O2, if you start with 2 mol of water, how many moles of hydrogen gas are produced?
a.
1 mol
c.
3 mol
b.
2 mol
d.
4 mol
 

66. 
If you start with 5 mol of O2 in the reaction 2Mg + O2 ® 2MgO, how many moles of Mg will you need?
a.
4 mol
c.
8 mol
b.
5 mol
d.
10 mol
 

67. 
In the reaction 2Mg + O2 ® 2MgO, the law of definite proportions states that for every 2 moles of Mg you will need how many moles of O2?
a.
1 mol
c.
3 mol
b.
2 mol
d.
4 mol
 

68. 
In a balanced chemical reaction, the total mass of the products always equals the