1 Which statement correctly describes the charge of the nucleus and the charge of the electron

cloud of an atom?
(1) The nucleus is positive and the electron cloud is positive.
(2) The nucleus is positive and the electron cloud is negative.
(3) The nucleus is negative and the electron cloud is positive.
(4) The nucleus is negative and the electron cloud is negative. 2 structure of the atom + nucleus,
cloud of electrons is negative 2 Which Period 4 element has the most metallic properties?
(1) As (3) Ge
(2) Br (4) Sc 4 one on the left side 3 Which property makes it possible to separate the oxygen
and the nitrogen from a sample of iquefied air?
(1) boiling point (3) hardness
(2) conductivity (4) electronegativity 1 boiling points are different 4 Which statement explains
why ozone gas, O3, and oxygen gas, O2, have different properties?
(1) They are formed from different elements.
(2) They have different molecular structures.
(3) They have different oxidation numbers.
(4) They have different electronegativities. 2 their molecules are different 5 Which statement is
true about oxidation and reduction in an electrochemical cell?
(1) Both occur at the anode.
(2) Both occur at the cathode.
(3) Oxidation occurs at the anode and reduction occurs at the cathode.
(4) Oxidation occurs at the cathode and reduction occurs at the anode. 3 An OX Red CAT 6 A
compound is made up of iron and oxygen, only. The ratio of iron ions to oxide ions is 2:3 in this
compound. The IUPAC name for this compound is
(1) triiron dioxide (3) iron(III) oxide
(2) iron(II) oxide (4) iron trioxide 3 Fe2O3 now name it 7 Which process is a chemical change?
(1) melting of ice
(2) boiling of water
(3) subliming of ice
(4) decomposing of water 4 look for a reaction 8 Which substance contains bonds that involved
the transfer of electrons from one atom to another?
(1) CO2 (3) KBr
(2) NH3 (4) Cl2 3 transfer=IONIC=metal and nonmetal 9 What is the total number of pairs of
electrons shared in a molecule of N2?
(1) one pair (3) three pairs
(2) two pairs (4) four pairs 3 N2= has a triple bond (3 pairs or 6 electrons) 10 Which formula
represents a nonpolar molecule containing polar covalent bonds?
(1) H2O (3) NH3
(2) CCl4 (4) H2 2 H2 non polar bonds (OUT)

NH3, H2O are polar

CCl4 symmetrical and the bonds are between 2 different

11 The degree of polarity of a chemical bond in a molecule of a compound can be predicted by
determining the difference in the
(1) melting points of the elements in the compound
(2) densities of the elements in the compound
(3) electronegativities of the bonded atoms in a molecule of the compound
(4) atomic masses of the bonded atoms in a molecule of the compound 3 Bond=bend= Bonds
(think) Electronegativity Differences 12 Which statement best describes the shape and volume of
an aluminum cylinder at STP?
(1) It has a definite shape and a definite volume.
(2) It has a definite shape and no definite volume.
(3) It has no definite shape and a definite volume.
(4) It has no definite shape and no definite volume. 1 Al is a solid at STP 13 Which two
substances can not be broken down by chemical change?
(1) C and CuO (3) CO2 and CuO
(2) C and Cu (4) CO2 and Cu 2 Definition of Elements 14 Which compound is insoluble in
water?
(1) BaSO4 (3) KClO3
(2) CaCrO4 (4) Na2S 1 Use table F 15 A sample of a gas is contained in a closed rigid cylinder.
According to kinetic molecular theory, what occurs when the gas inside the cylinder is
heated?
(1) The number of gas molecules increases.
(2) The number of collisions between gas molecules per unit time decreases.
(3) The average velocity of the gas molecules increases.
(4) The volume of the gas decreases. 3 Closed Container. Temperature is avg. KE= motion 16
Which statement best describes how a catalyst increases the rate of a reaction?
(1) The catalyst provides an alternate reaction pathway with a higher activation energy.
(2) The catalyst provides an alternate reaction pathway with a lower activation energy.
(3) The catalyst provides the same reaction pathway with a higher activation energy.
(4) The catalyst provides the same reaction pathway with a lower activation energy. 2 Definition
of a catalyst (always on test) 17 The compounds 2-butanol and 2-butene both contain
(1) double bonds, only (3) carbon atoms
(2) single bonds, only (4) oxygen atoms 3 but-= 4 carbon atoms
 2 Avogadro's hypothesis, same
conditions, same volume, same # molecules 19 A chemical reaction is at equilibrium. Compared
to the rate of the forward reaction, the rate of the reverse reaction is
(1) faster and more reactant is produced
(2) faster and more product is produced
(3) the same and the reaction has stopped
(4) the same and the reaction continues in both directions 4 Con Con Requal (Equilibrium)

Concentrations are constant because the rates are equal

20 Which organic compound is a saturated hydrocarbon?

(1) ethyne (3) ethanol
(2) ethene (4) ethane 4 Saturated all single bonds, ALKANE

21 A substance is classified as an electrolyte because

(1) it has a high melting point
(2) it contains covalent bonds
(3) its aqueous solution conducts an electric current
(4) its aqueous solution has a pH value of 7 3 definition of electrolyte 22 Half-reactions can be
written to represent all
(1) double-replacement reactions
(2) neutralization reactions
(3) fission and fusion reactions
(4) oxidation and reduction reactions 4 half reactions are oxidation reduction reactions
 1 isomers
same formula different structure

count atoms

24 Given the balanced equation representing a redox reaction:

2Al + 3Cu2+ --> 2Al3+ + 3Cu
Which statement is true about this reaction?
(1) Each Al loses 2e- and each Cu2+ gains 3e-
(2) Each Al loses 3e- and each Cu2+ gains 2e-
(3) Each Al3+ gains 2e- and each Cu loses 3e-
(4) Each Al3+ gains 3e- and each Cu loses 2e- 2 Al charge goes up oxidation, lose electrons 0--
>+3 is 3 electrons

Cu2+ charge goes down reduction, gain electrons, +2 to 0 is 2 electrons

25 Which conversion of energy always occurs in a voltaic cell?

(1) light energy to chemical energy
(2) electrical energy to chemical energy
(3) chemical energy to light energy
(4) chemical energy to electrical energy 4 voltaic is a battery, chemical to electrical 26 The
compound NaOH(s) dissolves in water to yield
(1) hydroxide ions as the only negative ions
(2) hydroxide ions as the only positive ions
(3) hydronium ions as the only negative ions
(4) hydronium ions as the only positive ions 1 Arrhenius base definition
 3 acid and base makes salt and water

4 Use table N (for decay) and table O

(for notation) 29 Atoms of one element are converted to atoms of another element through
(1) fermentation (3) polymerization
(2) oxidation (4) transmutation 4 Definition of transmutation 30 An atom of potassium-37
and an atom of potassium-42 differ in their total number of
(1) electrons (3) protons
(2) neutrons (4) positrons 2 They are isotopes, so the # of neutrons

31 What is the mass number of an atom that has six protons, six electrons, and eight neutrons?
(1) 6 (3) 14

(2) 12 (4) 20 3 6 protons =atomic # 6 2 mass# of

27= 13p+ and 14no 4 an electron mass is
approximately 1/1836 of a proton, so the proton is about 2000x more massive 34 Based on
electronegativity values, which type of elements tends to have the greatest attraction for electrons
in a bond?
(1) metals (3) nonmetals
(2) metalloids (4) noble gases 3 fluorine is the greatest, it is a nonmetal 35 Which list of
elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius?
(1) Be, Mg, Ca (3) Ba, Ra, Sr
(2) Ca, Mg, Be (4) Sr, Ra, Ba 1 Table S has the values, put them in order 36 Which half-
reaction shows conservation of charge?
(1) Cu + e- --> Cu+ (3) Cu+ --> Cu + e-
(2) Cu + 2e --> Cu (4) Cu2+ -->Cu + 2e- 2 The total charge on the left must equal the total
2+ -

charge on the right 1 plug in mass of

MG and divide by total x100% 38 Given the balanced equation:
CaCO3(s) + 2HCl(aq) -->CaCl2(aq) + H2O(l) + CO2(g)
What is the total number of moles of CO2 formed when 20. moles of HCl is completely
consumed?
(1) 5.0 mol (3) 20. mol
(2) 10. mol (4) 40. mol 2 set up a proportion

20/2 =x/1

39 What amount of heat is required to completely melt a 29.95-gram sample of H2O(s) at 0°C?
(1) 334 J (3) 1.00 × 103 J
(2) 2260 J (4) 1.00 × 104 J 4 melt (fusion)

q=mHf= 29.95 x 334

 4 elements are not attached

41 An unsaturated aqueous solution of NH3 is at 90.°C in 100. grams of water. According to

Reference Table G, how many grams of NH3 could this unsaturated solution contain?
(1) 5 g (3) 15 g
(2) 10. g (4) 20. g 1 NH3 would be saturated with 10 grams. Unsaturated is less than 10g. 42
How many total moles of KNO3 must be dissolved in water to make 1.5 liters of a 2.0 M
solution?
(1) 0.50 mol (3) 3.0 mol
(2) 2.0 mol (4) 1.3 mol 3 M=mol/L; mol= M/L=2.0/1.5 43 Which statement explains why low
temperature and high pressure are required to liquefy chlorine gas?
(1) Chlorine molecules have weak covalent bonds.
(2) Chlorine molecules have strong covalent bonds.
(3) Chlorine molecules have weak intermolecular forces of attraction.
(4) Chlorine molecules have strong intermolecular forces of attraction. 3 Cl2 is nonpolar and
have weak intermolecular forces

van der waals

44 Given the balanced equation representing a reaction:

CH4(g) + 2O2(g) --> 2H2O(g) + CO2(g) + heat
Which statement is true about energy in this reaction?
(1) The reaction is exothermic because it releases heat.
(2) The reaction is exothermic because it absorbs heat.
(3) The reaction is endothermic because it releases heat.
(4) The reaction is endothermic because it absorbs heat. 1 heat is on the right of the arrow, it is
exothermic and releases heat 45 Given the reaction at equilibrium:
N2(g) + 3H2(g) -->2NH3(g) + 91.8 kJ
What occurs when the concentration of H2(g) is increased?
(1) The rate of the forward reaction increases and the concentration of N2(g) decreases.
(2) The rate of the forward reaction decreases and the concentration of N2(g) increases.
(3) The rate of the forward reaction and the concentration of N2(g) both increase.
(4) The rate of the forward reaction and the concentration of N2(g) both decrease. 1 LeChaterliers
Principle, add a reactant it shifts right, reactants decrease [H2] and products increase.

4 Potential Energy Diagrams

Difference in products and reactants is Delta H

Arrow 4

47 Based on bond type, which compound has the

highest melting point?
(1) CH3OH (3) CaCl2
(2) C6H14 (4) CCl4 3 The Ionic One (Metal and Nonmetals)

the other 3 are covalent (made of all nonmetals)

 1 (Mass x %) x (mass x %) / 100%

they distributed the divide by 100

49 Which list of the phases of H2O is arranged in order of increasing entropy?

(1) ice, steam, and liquid water
(2) ice, liquid water, and steam
(3) steam, liquid water, and ice
(4) steam, ice, and liquid water 2 Entropy is Randomness, increase from

Solid to liquid to gas

50 Solution A has a pH of 3 and solution Z has

a pH of 6. How many times greater is the
hydronium ion concentration in solution A than
the hydronium ion concentration in solution Z?
(1) 100 (3) 3
(2) 2 (4) 1000 4 for each pH value it is 10x's more concentrated

3 pH units 1000 xs