Chemistry 105 Practice Final Exam

Front 1

1. All of the following are examples of matter except
a) water
b) salt
c) soil
d) air
e) heat

Back 1

e) heat

Front 2

3. Which of the following is NOT a chemical change?
a) butter becomes rancid
b) decay of leaves in winter
c) melting of ice in spring
d) tarnishing of silverware e) rusting of nails

Back 2

c) melting of ice in spring

Front 3

4. The metric unit used to measure mass is the ________.
a) gram, g
b) grams per cubic centimeter, g/cm3 c) Kelvin, K
d) liter, L
e) meter, m

Back 3

a) gram, g

Front 4

7. Which of the following regions of the electromagnetic spectrum has the highest energy?
a) ultraviolet light b) infrared light
c) radio waves
d) red light
e) gamma rays

Back 4

e) gamma rays

high to low
Gamma rays, X-ray, ultraviolet light, visible light, infrared light, microwaves, radio waves

Front 5

12. Where is most of the mass of an atom concentrated?
a) electrons
b) neutrons
c) nucleus
d) orbitals
e) protons

Back 5

c) nucleus

Front 6

14. Which elements all belong in the same group?
a) N, O, F
b) Fe, Co, Ni
c) B, Si, As
d) Na, K, Cs
e) Al, Ge, Sb

Back 6

d) Na, K, Cs

group is vertical roll

Front 7

15. Elements in the Periodic Table are arranged according to ____________.
a) alphabetical order
b) atomic number
c) atomic weight
d) date of discovery
e) number of neutrons

Back 7

b) atomic number

Front 8

16. Which of the following sets of three elements contains only metals?
a) Na, Ca, Zn
b) K, C, Mg
c) U, Cl, Hg,
d) P, W, S
e) C, S, I

Back 8

a) Na, Ca, Zn

Front 9

17. Which element is most likely to have chemical properties similar to those of chlorine?
a) carbon
b) sodium
c) argon
d) bromine
e) selenium

Back 9

d) bromine

Front 10

22. Based on its position in the Periodic Table, which of the following is the most probable charge of a
magnesium ion?
a) -2
b) -6
c) +1
d) +2
e) +3

Back 10

d) +2

Front 11

24. Which of the following is a pure substance?
a) tap water
b) blood
c) carbon dioxide
d) perfume
e) air

Back 11

c) carbon dioxide

Front 12

Which has the greater atomic size? (magnesium or sulfur)

Back 12

Magnesium

-Decrease in size from Left to right.
-Increase in size from top to bottom.
-Some exceptions exist.

Front 13

Which has the greater ionization energy? (barium or magnesium)

Back 13

Magnesium

The energy required to remove an electron from an isolated atom.
-Reading down a group, the ionization energy decreases, because of the atom's size increases. The outermost electron is progressively farther from the nuclear charge, hence easier to remove.
-Reading across a period, the ionization energy increase, note that atomic size decreases, because the outer most electrons are close to the nucleus, thus harder to remove.

Front 14

Which has the larger size? (a neutral aluminum atom or an aluminum ion with a +3 charge)

Back 14

a neutral aluminum atom

Front 15

Structure of the Atom
Name, Location, Relative Charge, Relative Mass (amu)
1.
2.
3.

Back 15

1. Electron, Charge: -1, Mass: 5.4 x 10^-4 amu
2. Proton, Charge: +1, Mass: 1 amu
3. Neutron, Charge: 0, Mass: 1 amu

Front 16

A) 6.85 m = ____ cm

Back 16

0.0685 cm

100cm=1m

Front 17

B) 932 mg = ____ g

Back 17

0.932g

1,000mg=1g

Front 18

List four properties of metals.

Back 18

-metals are shinny, are malleable; are ductile, are good conductors of heat and electricity; and most are solids at room temp.

Front 19

1. Which pair of elements is most likely to form an ionic compound if allowed to react together?
a) Al & I
b) Cu & Ca
c) C & Cl
d) P & Br
e) K & Ni

Back 19

a) Al & I

Front 20

2. Which of the following is a property typical of ionic compounds?
a) exist as crystalline solids at room temperature
b) conduct electrical current if dissolved in water or melted
c) have very high melting points and boiling points
d) are hard and brittle and shatter when crystals are struck
e) all of these

Back 20

e) all of these

Front 21

5. A chemical bond formed when two atoms share one pair of electrons is a __________ bond.
a) double covalent b) double ionic c) single covalent
d) single ionic e) triple covalent

Back 21

c) single covalent

Front 22

6. In forming covalent bonds where the octet rule is obeyed, chlorine usually forms _____ single covalent bond(s) and carbon usually forms _____ single covalent bond(s).
a) one; one b) two; two c) one; four d) four; one e) seven; four

Back 22

c) one; four

Front 23

9. Which property could describe a binary molecular compound?
a) It has a high boiling point.
b) It conducts electricity when dissolved in water.
c) It has a high melting point.
d) It is composed of a metal and a nonmetal
e) None of these.

Back 23

e) None of these.

Front 24

11. The molar mass of octane, C8H18, is _____ grams.
a) 22.0
b) 97.0
c) 30.0
d) 114.0
e) none of these

Back 24

d) 114.0

Front 25

13. Consider the reaction shown and identify the statement that is true.
CaCO3(s) (heat)/-> CaO(s) + CO2(g)
a) This reaction is balanced as written. b) Heat is required for this reaction to occur.
c) The products are a solid and a gas. d) This is a decomposition reaction.
e) All of these.

Back 25

e) All of these.

Front 26

14. What is the mass of 0.255 mol of K?
a) 0.255 g
b) 39.1 g
c) 9.97 g
d) 7.91 g
e) 153 g

Back 26

c) 9.97

use the conversion triangle

Front 27

15. How many moles of NaCl are in 4.86 g of NaCl?
a) 0.0831
b) 2.93 x 1024
c) 4.86
d) 284
e) 12.0

Back 27

a) 0.0831

Use conversion traingle

Front 28

16. In the reaction given, how many moles of I2 are needed to react with 1.2 mol of Al?
2 Al + 3 I2 -> 2 AlI3
a) 0.60
b) 1.2
c) 1.8
d) 2.4
e) 3.6

Back 28

c) 1.8

Front 29

17. What term describes a compound that conducts an electric current when dissolved in water
(or melted)?
a) amorphous
b) nonelectrolyte
c) electrolyte
d) superconductor
e) none of these

Back 29

c) electrolyte

Front 30

1. The solubility of gases in liquids is highest at _____________________.
a) low temperature and high pressure
b) low temperature and low pressure
c) high temperature and high pressure
d) high temperature and low pressure

Back 30

a) low temperature and high pressure

Front 31

3. Which of the following is a nonelectrolyte?
a) NaCl
b) C12H22O11
c) CaCl2
d ) NaOH(aq)
e) KCl

Back 31

b) C12H22O11

Front 32

5. The temperature at which the motion of particles theoretically ceases is _____.
a) -273 K
b) 0 K
c) 0 C
d) 273 C

Back 32

b) 0 K

Front 33

6. Which of the following is a part of the kinetic theory of gases?
a) Gas particles are in constant, rapid motion.
b) There are no attractive forces between gas particles.
c) The distance between gas particles is very large.
d) The collisions between gas particles are perfectly elastic.
e) All of these

Back 33

e) All of these

Front 34

7. If the temperature of a fixed volume of a gas is increased, what effect will this have on the
pressure of the gas?
a) The pressure will increase. b) The pressure will decrease.
c) The pressure will be unchanged.
d) The pressure will increase and then decrease.

Back 34

a) The pressure will increase.

Front 35

8. Which of these changes would NOT cause an increase in the pressure of a gaseous system?
a) The container is made larger.
b) More gas is added to the container.
c) The temperature is increased.

Back 35

a) The container is made larger.

Front 36

10. Increasing the volume of a given amount of gas at constant temperature causes the pressure to decrease because:
a) the molecules are striking a larger area with the same force.
b) there are fewer molecules. c) the molecules are moving more slowly.

Back 36

a) the molecules are striking a larger area with the same force.

Front 37

11. What is the term that describes a liquid changing to a vapor at a temperature less than its
boiling point?
a) evaporation
b) sublimation
c) dissociation
d) condensation

Back 37

a) evaporation

Front 38

17. A certain solid substance that is very hard, has a high melting point, and conducts electricity when melted or dissolved in water is most likely to be
a) S
b) NaCl
c) Cu
d) ice
e) diamond

Back 38

An electrolyte
b) NaCl

Front 39

18. What happens to the temperature of a liquid as it evaporates? It ______.
a) increases
b) decreases
c) remains the same
d) increases and then decreases

Back 39

b) decreases

Front 40

22. When the vapor pressure of a liquid is equal to the atmospheric pressure, the liquid _____.
a) condenses
b) freezes
c) boils
d) no change is observed

Back 40

c) boils

Front 41

24. Why does air leave a tire when the tire valve is opened?
a) because the pressure outside the tire is lower than the pressure inside the tire
b) because the pressure outside the tire is greater than the pressure inside the tire
c) because the temperature is higher outside the tire than inside the tire
d) because there are more gas particles outside the tire than inside the tire

Back 41

a) because the pressure outside the tire is lower than the pressure inside the tire

Front 42

25. What happens to the pressure of a gas inside a container if the temperature of the
gas is lowered? The pressure _____.
a) increases b) does not change c) decreases

Back 42

c) decreases

Front 43

26. A balloon is filled with helium. If the balloon is taken outside on a cold winter night, the volume of the balloon ______.
a) increases
b) does not change c) decreases

Back 43

c) decreases

Front 44

3. Consider the reaction: 22 kcal + 2 NH3(g) -> N2(g) + 3 H2(g) We can say
that this reaction is _____ and that the sign of H is _____.
a) endothermic; negative
b) exothermic; negative
c) endothermic; positive
d) exothermic; positive
e) exothermic; neither positive nor negative

Back 44

c) endothermic; positive

Front 45

7. Which factor(s) would increase the rate of a reaction?
I) increasing the temperature II) increasing the concentration of reactants III) adding a catalyst
a) I & II only b) II & III only
c) III only
d) I & III only
e) I, II, & III

Back 45

e) I, II, & III

Front 46

8. The function of a catalyst in a reaction is to _____.
a) increase the yield of product
b) decrease the amount of heat produced
c) increase the rate of the reaction
d) decrease the amount of reactants consumed
e) decrease the amount of energy consumed in the reaction

Back 46

c) increase the rate of the reaction

Front 47

9. Consider the reaction: N2(g) + 3 H2(g)  2 NH3(g) + 22 kcal Which change to
this reaction system would cause the equilibrium to shift to the left?
a) addition of catalyst b) addition of N2(g) c) addition of H2(g)
d) increasing the temperature e) increasing the pressure by decreasing the volume

Back 47

d) increasing the temperature

Front 48

12. When a reaction system is at equilibrium, _____.
a) there is no more chemistry happening
b) the amounts of reactants and products are exactly equal
c) the reaction rate in the forward direction is at a maximum
d) the reaction rate in the reverse direction is at a minimum
e) the rates of the forward and reverse directions are exactly equal

Back 48

e) the rates of the forward and reverse directions are exactly equal.

Front 49

14. Which statement concerning Arrhenius acid-base theory is correct?
a) An Arrhenius acid produces hydrogen ions in water solution.
b) An Arrhenius base produces hydroxide ions in water solution.
c) A neutralization reaction produces water and a salt.
d) Acid-base reactions must take place in aqueous solution.
e) All of the above are correct.

Back 49

e) All of the above are correct.

Front 50

18. Hydrochloric acid is a strong acid in water because it _____.
a) ionizes only slightly into hydronium ions and chloride ions
b) ionizes completely into hydronium ions and chloride ions
c) is concentrated d) is completely soluble e) none of these

Back 50

b) ionizes completely into hydronium ions and chloride ions

Front 51

21. If the [H3O+] of a solution is 1 x 10^-10 M, the pH is _____ and the solution is _______ .
a) 4; basic
b) 4; acidic
c) 10; acidic
d) 10; basic
e) 10; neutral

Back 51

d) 10; basic

Front 52

22. Which of the following is a property of acids?
a) sour taste b) neutralizes bases c) turns blue litmus paper red
d) reacts with many metals to produce H2 gas e) all of these

Back 52

e) all of these

Front 53

26. In the reaction, CO32- + H2O <-> HCO31- + OH1-, the CO32- ion is acting as a(n) _____.
a) Arrhenius acid
b) Arrhenius acid
c) Bronsted-Lowry acid
d) Bronsted-Lowry base e) none of these

Back 53

d) Bronsted-Lowry base

Front 54

27. What is the purpose of a titration?
a) to determine the color of an indicator in an acid and a base
b) to determine the concentration of an acid only
c) to determine the concentration of a base only
d) to determine the concentration of an acid or a base
e) none of these

Back 54

d) to determine the concentration of an acid or a base

Front 55

28. A buffer solution __________.
a) maintains a pH at 7.0
b) is a strong base c) is a weak acid
d) acts to prevent a drastic change in pH e) neutralizes only acids

Back 55

d) acts to prevent a drastic change in pH

Front 56

30. Which of the following is a characteristic of bases?
a) turn litmus blue b) feel slippery c) taste bitter
d) neutralize acids e) all of these

Back 56

e) all of these

Front 57

1. The emission of a particle from an unstable nucleus is called _______.
a) fission
b) transmutation
c)fusion
d) nuclear decay
e) none of these

Back 57

d) nuclear decay

Front 58

3. Ionizing radiation is dangerous to living things because
a) its penetrating power varies with its source.
b) it alters the chemical structure of molecules within the cells.
c) it causes electrons to be captured by the nucleus.
d) it causes nuclear reactions.
e) it causes thermal burns.

Back 58

b) it alters the chemical structure of molecules within the cells.

Front 59

5. When two small nuclei join together to form a larger nucleus, the process is called
a) fission
b) fusion
c) spontaneous decay d) mutation
e) none of these

Back 59

b) fusion

Front 60

7. An atom of uranium-238 has how many neutrons? (atomic number = 92)
a) 92 b) 146 c) 238 d) 330 e) none of these

Back 60

b) 146

Front 61

8. What is the change in mass when a nucleus emits gamma radiation?
a) decreases by 4 b) decreases by 1 c) remains the same
d) increases by 1 e) increases by 4

Back 61

c) remains the same

Front 62

9. What is the change in atomic number when a nucleus emits an alpha particle?
a) decreases by 2 b) decreases by 1 c) remains the same
d) increases by 1 e) increases by 2

Back 62

a) decreases by 2

Front 63

10. The most penetrating form of radiation is ____________.
a) alpha radiation b) beta radiation c) gamma radiation
d) a, b, & c are all the same e) a & b

Back 63

c) gamma radiation

Front 64

10. The most penetrating form of radiation is ____________.
a) alpha radiation b) beta radiation c) gamma radiation
d) a, b, & c are all the same e) a & b

Back 64

c) gamma radiation