1) The heat absorbed when ice melts can be measured in a unit called a

1. torr
2. degree
3. mole
4. calorie

2) Which substance is a binary compound?

1. ammonia
2. argon
3. glucose
4. glycerol

3) Which sample of matter is a mixture?

1. H₂O (s)
2. H₂O (g)
3. NaCl (l)
4. NaCl (aq)

4) Which graph below represents the variation in the vapor pressure of water as temperature changes?

1	3
2	4

5) Which atom in the ground state has five electrons in its outer level and ten electrons in its kernel?

1. C
2. CL
3. Si
4. P

6) Which type of radiation continues in a straight line when passed through an electric field?

1. alpha
2. beta
3. gamma
4. proton

7) The Atomic mass unit is defined as exactly

1. 12
   	C
   6

2. 14
   	C
   6

3. 24
   	Mg
   12

4. 26
   	Mg
   12

8) When an atom loses an electron, the atom becomes an that is

1. positively charged and gains a small amount of mass.
2. Positively charged and loses a small amount of mass.
3. Negatively charged and gains a small amount of mass.
4. Negatively charged and loses a small amount of mass.

9) The Nucleus of which atom contains 48 neutrons?

1. 32
   	S
   16

2. 48
   	Ti
   22

3. 85
   	Rb
   37

4. 112
   	CD
   48

10) Experiments performed to reveal the structure of atoms led scientists to conclude that an atom's

1. positive charge is evenly distributed throughout its volume.
2. Negative charge is mainly concentrated in its nucleus.
3. Mass is evenly distributed throughout its volume.
4. Volume is m,mainly unoccupied.

11) Given the unbalanced equation:

__Al(s) + __O₂(g)---> __Al₂O₃(s)

When this equation is correctly balanced using smallest whole numbers, what is the coefficient of O₂(g)?

1. 6
2. 2
3. 3
4. 4

12) Which pair of atoms is held together by a covalent bond?

1. HCl
2. LiCl
3. NaCl
4. KCl

13) The formula H₂O₂ is an example of

1. a molecular formula
2. an empirical formula
3. an ionic formula
4. an organic formula

14) What happens when NaCl(s) is dissolved in water?

1. CL ions are attracted to the oxygen atoms of water molecules
2. Na⁺ ions are attracted to the oxygen atoms of water molecules
3. CL ions are repelled by the hydrogen atoms of water molecules
4. NA⁺ ions are repelled by the hydrogen atoms of water molecules

15) Which molecule has an asymmetrical shape?

1. N₂
2. NH₂
3. Cl₂
4. CCl₄

16) The forces between atoms that create chemical bonds are the result of interactions between

1. nuclei
2. electron
3. protons and electrons
4. protons and nuclei

17) Which Group 16 element undergoes natural radioactive disintegration?

1. Po
2. S
3. Se
4. Te

18) Pure silicon is chemically classified as a metalloid because silicon

1. is malleable and ductile
2. is an excellent conductor of heat and electricity
3. exhibits hydrogen bonding
4. exhibits metallic and nonmetallic properties

19) In which group of elements do most atoms have completely filled s and p valence sublevels?

1. halogens
2. noble gases
3. alkali metals
4. alkaline earth metals

20) Which ion has the largest radius?

1. NA⁺
2. Mg²⁺
3. K⁺
4. Ca²⁺

21) An aqueous solution of XCl₂ contains colored ions. Element X could be

1. Ba
2. Ca
3. Ni
4. Bi

22) Which properties are most common in nonmetals?

1. low ionization energy and low electronegativity
2. low ionization energy and high electronegativity
3. high ionization energy and low electronegativity
4. high ionization energy and high electronegativity

23) One mole of O₂ has approximately the same mass as one mole of

1. CH₄
2. S
3. LiH
4. Cl₂

24) Based on Reference Table E, which compound could form a concentrated solution?

1. AgBr
2. AgCl
3. Ag₂CO₃
4. AgNO₃

25) A 2.00 liter sample of a gas has a mass of 1.80 grams at STP. What is the density, in grams per liter, of this gas at STP?

1. 0.900
2. 1.80
3. 11.2
4. 22.4

26) What is the total number of neon atoms contained in 20.2 grams of neon gas?

1. 1.01 x 10²⁴
2. 2.02 x 10²⁴
3. 3.01 x 10²³
4. 6.02 x 10²³

27) What is the total number of moles of oxygen atoms in one mole of N₂O₃?

1. 1
2. 2
3. 3
4. 5

28) Which 1.0 mole sample at 1 atm has particles with the greatest entropy?

1. CH₄(g) at 25^oC
2. H₂S(g) at 40^oC
3. CH₄(g) at 300 K
4. H₂S(g) at 310 K

29) A 1.0 gram sample of powdered Zn reacts faster with HCl than a single 1.0 gram piece of Zn because the surface atoms in powdered Zn have

1. higher average kinetic energy
2. lower average kinetic energy
3. more contact with the H⁺ ions in the acid
4. less contact with the H⁺ ions in the acid

30) In a reversible reaction, chemical equilibrium is attained when the

1. rate of the forward reaction is greater than the rate of the reverse reaction
2. rate of the reverse reaction is greater than the rate of the forward reaction
3. concentration of the reactants reaches zero
4. concentration of the products remains constant

31) Which statement correctly describes the reaction?

1. It is endothermic and energy is absorbed.
2. It is endothermic and energy is released.
3. It is exothermic and energy is absorbed.
4. It is exothermic and energy is released.

32) Which numbered interval will change with the addition of a catalyst to the system?

1. 1
2. 2
3. 3
4. 4

33) Carbon dioxide gas is most soluble in water under conditions of

1. high pressure and low temperature
2. high pressure and high temperature
3. low pressure and low temperature
4. low pressure and low temperature

34) A solution contains 130 grams of KNO₃ dissolved in 100 grams of water. When 3 more grams of KNO₃ is added, none of it dissolves, nor do any additional crystals appear. Based on Reference table D, the temperature of the solution is closest to

1. 65^oC
2. 68^oC
3. 70^oC
4. 72^oC

35) If equal volumes of 0.1 M NaOH and 0.1 M HCl are mixed, the resulting solution will contain a salt and

1. HCl
2. NaOH
3. H₂O
4. NaCl

36) According to Reference Table L. which of the following 1.0 M acid solutions has the greatest [H3O⁺] at 1 atmosphere and 298 K?

1. HNO₃
2. HF
3. H₃PO₄
4. HNO₂

37) The [H3O⁺] of a solution is 1 x 10^-8. This solution has a pH of

1. 6, which is acidic
2. 8, which is basic
3. 6, which is basic
4. 8, which is acidic

38) Which of the following is the strongest Bronsted-Lowry base?

1. l^-
2. Br^-
3. Cl^-
4. F^-

39) In the reaction NH₃ + HCl --> NH₄⁺ + CL, the NH₃ acts as

1. a Bronsted acid only
2. a bronsted base only
3. both a Bronsted acid and a Bronsted base
4. neither a Bronsted acid nor a Bronsted base

40) Which species is amphoteric (amphiprotic)?

1. H₂
2. H₂SO₄
3. HSO₄^-
4. SO₄^2-

41) When a redox reaction occurs, there must be a transfer of

1. electrons
2. neutrons
3. protons
4. ions

42) What is the oxidation number of carbon in NaHCO₃

1. -2
2. +2
3. -4
4. +4

43) A redox reaction is set up so that both half reactions take place in separate beakers that are connected by a salt bridge and an external conductor. The path for the transfer of ions is provided by the

1. anode
2. cathode
3. salt bridge
4. external conductor

44) an oxidation half reaction always involves the

1. gain of electrons and a decrease in the oxidation number
2. gain of electrons and an increase in the oxidation number
3. loss of electrons and a decrease in the oxidation number
4. loss of electrons and an increase in the oxidation number

45) Given the electrochemical cell reaction

Zn(s) + Ni²⁺(aq) --> Zn²⁺(aq) + Ni(s)

Which species is the reducing agent?

1. Zn
2. Ni²⁺
3. Zn²⁺
4. Ni

46) Which equation represents an oxidation reduction reaction?

1. HCl + KOH --> KCl + H₂O
2. 4HCl + MnO₂ --> MnCl₂ + 2H₂O + Cl₂
3. 2HCl + CaCO₃ --> CaCl₂ + H₂O +CO₂
4. 2HCl + FeS --> FeCl₂ +H₂S

47) An example of a synthetic polymer is

1. starch
2. cellulose
3. protein
4. nylon

48) What are the two main products of a fermentation reaction?

1. ethanol and carbon dioxide
2. ethanol and water
3. sugar and carbon dioxide
4. sugar and water

49) Which structural formula represents a saturated hydrocarbon?

1	3
2	4

50) A compound with the formula CH₃CH₂OH is classified as an

1. alkane
2. alkene
3. alcohol
4. acid

51) In general, which property do organic compounds share?

1. high melting point
2. high electrical conductivity
3. readily soluble in water
4. slow reaction rate

52) As an acid solution is added to neutralize a base solution, the OH^- concentration of the base solution

1. decreases
2. increases
3. remains the same

53) A cylinder with a tightly fitted piston is shown in the diagram below

As the piston moves downward, the number of molecules of air in the cylinder

1. decreases
2. increases
3. remains the same

54) As noble gases are considered in order of increasing atomic number, the van der Waals forces between the atoms in a given sample of each of these gases

1. decreases
2. increases
3. remains the same

55) Within Period 2 of the Periodic Table, as the atomic number increases, the atomic radius generally

1. decreases
2. increases
3. remains the same

56) As an electron moves from 3s orbital to a 2s orbital, the energy of the atom

1. decreases
2. increases
3. remains the same