Chemistry Final Exam Study Guide

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

____	1.	An element that is a poor conducter of electricity and heat is classified as a
a.	Nonmetal	c.	Alkali metal	
b.	Transition Metal	d.	Alkaline Earth Metal	

____	2.	Which of the following shows correctly an ion pair and the ionic compound the two ions form?
a.	Fe3+, O2-;Fe2O3	c.	Cu2+, O2-; Cu2O2	
b.	Cr3+, I-; CrI	d.	Sn4+, N3-; Sn4N3	

____	3.	As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true?
a.	The nucleus is made of electrons and protons.	
b.	Electrons are distributed around the nucleus and occupy almost all the volume of the atom.	
c.	The nucleus is made of protons, electrons, and neutrons.	
d.	Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.	

____	4.	As you move from left to right across the second period of the periodic table ____.
a.	electronegativity decreases	c.	atomic radii increase	
b.	atomic mass decreases	d.	ionization energy increases	

____	5.	To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI solution. What is the molarity of the new solution?
a.	2.8M	c.	180M	
b.	0.18M	d.	0.35M	

____	6.	If energy is added to a boiling liquid, what happens to the temperature of the liquid?
a.	It decreases.	c.	It increases.	
b.	It does not change.	d.	The change cannot be determined.	

____	7.	What is ammonia classified as?
a.	Arrhenius acid	c.	Bronsted-Lawry base	
b.	Arrhenius base	d.	Bronsted-Lawry acid	

____	8.	The temperature at which the motion of particles theoretically ceases is ____.
a.	0°C	c.	–273 K	
b.	0 K	d.	273°C	

____	9.	Which of the following occurs in an ionic bond?
a.	Oppositely charged ions attract.	
b.	Two atoms share more than two electrons.	
c.	Like-charged ions attract.	
d.	Two atoms share two electrons.	

____	10.	Why does the pressure inside a container of gas increase if more gas is added to the container?
a.	There is an increase in the temperature of the gas.	
b.	There is an increase in the force of the collisions between the particles and the walls of the container.	
c.	There is a decrease in the volume of the gas.	
d.	There is an increase in the number of collisions between particles and the walls of the container.

____	11.	Of the elements Fe, Hg, U, and Te, which is a representative element?
a.	U	c.	Fe	
b.	Hg	d.	Te	

____	12.	Density is found by dividing ____.
a.	volume by mass	c.	mass by area	
b.	area by mass	d.	mass by volume	

____	13.	What would likely happen if you were to touch the flask in which an endothermic reaction were occurring?
a.	The flask would probably feel cooler than before the reaction started.	
b.	The flask would feel the same as before the reaction started.	
c.	The flask would probably feel warmer than before the reaction started.	
d.	none of the above	

____	14.	A gas occupies a volume of 2.4 L at 14.1 kPa. What volume will the gas occupy at 84.6 kPa?
a.	14 L	c.	2.5 L	
b.	497 L	d.	0.40 L	

____	15.	A catalyst works by ____.
a.	changing the particle size of the reactants	
b.	lowering the activation energy barrier	
c.	shifting the equilibrium position toward the products	
d.	changing the temperature of the reactants	

____	16.	You can classify water that is stored behind a dam as compared to water flowing through a dam as an example of _______________.
a.	potential energy transformed into kinetic energy	c.	chemical energy transformed into potential energy	
b.	kinetic energy transformed into potential energy	d.	thermal energy transformed into kinetic energy	

____	17.	What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?
a.	0.23 mL	c.	4.34 mL	
b.	479 mL	d.	none of the above	

____	18.	The experimental variable that is graphed on the x-axis is the __________.
a.	responding variable	c.	dependent variable	
b.	controlled variable	d.	manipulated variable	

____	19.	Which of the following is a property of an acid?
a.	unreactive	c.	nonelectrolyte	
b.	strong color	d.	sour taste	

____	20.	Which of the following usually makes a substance dissolve faster in a solvent?
a.	agitating the solution	
b.	decreasing the number of particles	
c.	increasing the particle size of the solute	
d.	lowering the temperature	

____	21.	What is the formula for sodium sulfate?
a.	Na(SO4)2	c.	Na2(SO4)2	
b.	NaSO4	d.	Na2SO4	

____	22.	In a chemical reaction, the mass of the products ____.
a.	is less than the mass of the reactants	
b.	is equal to the mass of the reactants	
c.	has no relationship to the mass of the reactants	
d.	is greater than the mass of the reactants

____	23.	At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water? 
2H2(g) + O2(g) ® 2H2O(g)
a.	3.6 L	c.	2.0 L	
b.	1.8 L	d.	2.4 L	

____	24.	According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?
a.	pairs of valence electrons	c.	mobile electrons	
b.	the electrons closest to the nuclei	d.	inner shell electrons	

____	25.	The average speed of oxygen molecules in air is about ____.
a.	170 km/h	c.	1700 km/h	
b.	0 km/h	d.	17,000 km/h	

____	26.	The combined gas law relates which of the following?
a.	temperature and pressure only	c.	volume and temperature only	
b.	pressure and volume only	d.	temperature, pressure, and volume	

____	27.	What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
a.	4.0M	c.	0.081M	
b.	81M	d.	12M	

____	28.	Which is a typical characteristic of an ionic compound?
a.	The ionic compound has a high melting point.	
b.	The ionic compound is described as a molecule.	
c.	Electron pairs are shared among atoms.	
d.	The ionic compound has a low solubility in water.	

____	29.	In which of these systems is the entropy decreasing?
a.	snow melting	c.	a liquid cooling	
b.	air escaping from a tire	d.	salt dissolving in water	

____	30.	What happens to the pressure of a gas inside a container if the temperature of the gas decreases?
a.	The pressure increases.	c.	The pressure does not change.	
b.	The pressure decreases.	d.	The pressure cannot be predicted.	

____	31.	Why does a higher temperature cause a reaction to go faster?
a.	Collisions occur with greater energy only.	
b.	There are more collisions per second or the collisions are of greater energy.	
c.	There are more collisions per second and the collisions are of greater energy.	
d.	There are more collisions per second only.	

____	32.	The variable that is observed during an experiment is called what type of variable?
a.	independent	c.	controlling	
b.	responding	d.	manipulated	

____	33.	Standard conditions when working with gases are defined as ____.
a.	0°C and 101.3 kPa	c.	0 K and 101.3 kPa	
b.	0 K and 1 kPa	d.	0°C and 1 kPa	

____	34.	Compared to the melting points of ionic compounds, the melting points of molecular solids tend to be ____.
a.	unpredictable	c.	lower	
b.	higher	d.	similar	

____	35.	Which expression represents a reaction rate?
a.	number/time	c.	time/mass	
b.	energy/time	d.	time/energy

____	36.	If a balloon is squeezed, what happens to the pressure of the gas inside the balloon?
a.	It stays the same.	
b.	It increases.	
c.	The pressure depends on the type of gas in the balloon.	
d.	It decreases.	

____	37.	Consider the reaction N2(g) + 3H2(g)  2NH3(g). What is the effect of decreasing the volume on the contained gases?
a.	The system reacts by increasing the number of gas molecules.	
b.	The pressure on the gases decreases momentarily.	
c.	Ammonia is consumed in the reaction.	
d.	The reaction shifts toward the product gas.	

____	38.	If the volume of a container of gas is reduced, what will happen to the pressure inside the container?
a.	The pressure will increase.	
b.	The pressure depends on the type of gas.	
c.	The pressure will not change.	
d.	The pressure will decrease.	

____	39.	A neutral atom contans
a.	varying numbers of protons and an equal number of neutrons and electrons	c.	more electrons than protons	
b.	an equal number of protons and electrons	d.	more protons than electrons	

____	40.	What is the molar mass of (NH4)2CO3?
a.	96 g	c.	78 g	
b.	138 g	d.	144 g	

____	41.	Which statement is true about electronegativity?
a.	Electronegativity is the ability of an anion to attract another anion.	
b.	Electronegativity generally increases from left to right across a period.	
c.	Electronegativity generally is higher for metals than for nonmetals.	
d.	Electronegativity generally increases as you move from top to bottom within a group.	

____	42.	An ionic bond is a bond between ____.
a.	valence electrons and cations	c.	a cation and an anion	
b.	the ions of two different nonmetals	d.	the ions of two different metals	

____	43.	Express the sum of 7.68 m and 5.0 m using the correct number of significant digits.
a.	12.68 m	c.	10 m	
b.	13 m	d.	12.7 m	

____	44.	Which of the following covalent bonds is the most polar?
a.	H—F	c.	H—C	
b.	H—H	d.	H—N	

____	45.	What happens to the temperature of a gas when it is compressed?
a.	The temperature does not change.	
b.	The temperature becomes unpredictable.	
c.	The temperature decreases.	
d.	The temperature increases.	

____	46.	How many moles of glucose, C6H12O6, can be "burned" biologically when 10.0 mol of oxygen is available? 

C6H12O6(s) + 6O2(g) ® 6CO2(g) + 6H2O(l)

a.	60.0 mol	c.	53.3 mol	
b.	1.67 mol	d.	0.938 mol

____	47.	What is the molar mass of AuCl3?
a.	96 g	c.	130 g	
b.	232.5 g	d.	303.6 g	

____	48.	Atomic size generally ____.
a.	decreases as you move from left to right across a period	
b.	decreases as you move from top to bottom within a group	
c.	increases as you move from left to right across a period	
d.	remains constant within a period	

____	49.	How many moles of aluminum are needed to react completely with 1.2 mol of FeO? 
2Al(s) + 3FeO(s) ® 3Fe(s) + Al2O3(s)
a.	2.4 mol	c.	1.6 mol	
b.	1.2 mol	d.	0.8 mol	

____	50.	Which of the following is a heterogeneous mixture?
a.	air	c.	vinegar in water	
b.	oil and vinegar	d.	milk	

____	51.	How many liters of NH3, at STP, will react with 5.3 g O2 to form NO2 and water?
4NH3(g) + 7O2(g)  4NO2 + 6H2O(g)
a.	2.12 L	c.	6.49 L	
b.	0.004 23 L	d.	3.03 L	

____	52.	What is the density of an object having a mass of 8.0 g and a volume of 25 cm3?
a.	2.0 g/cm3	c.	0.32 g/cm3	
b.	200 g/cm3	d.	3.1 g/cm3	

____	53.	Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many grams of aluminum sulfate would be formed if 250 g H2SO4 completely reacted with aluminum?

		2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g)

a.	0.85 g	c.	870 g	
b.	450 g	d.	290 g	
____	54.	Atomic radius of atoms will generally
a.	increase from left to right within a period	c.	decrease from top to bottom within a group	
b.	decrease from left to right within a period	d.	remain constant within a period	

____	55.	The experimental variable that is graphed on the y-axis is the __________?
a.	independent variable	c.	dependent variable	
b.	controlled variable	d.	secondary variable	

____	56.	What SI unit is used to measure the number of representative particles in a substance?
a.	ampere	c.	kilogram	
b.	mole	d.	kelvin	

____	57.	What is the electron configuration of potassium?
a.	1s2s2p3s3p4s	c.	1s2s2p3s3p4s	
b.	1s2s2p3s3p	d.	1s2s3s3p3d	

____	58.	What is the result of adding 2.5 x 103 and 3.5 x 102?
a.	2.9 x 103	c.	6.0 x 103	
b.	2.9 x 102	d.	6.0 x 105	

____	59.	What is the SI unit of pressure?
a.	candela	c.	mole	
b.	pascal	d.	newton	

____	60.	Which of the following occurs as temperature increases?
a.	Solubility decreases.	c.	Solubility remains the same.	
b.	Solubility increases.	d.	Molarity doubles.	

____	61.	What are the missing coefficients for the skeleton equation below?
Cr(s) + Fe(NO3)2(aq)  Fe(s) + Cr(NO3)3(aq)
a.	2, 3, 3, 2	c.	1, 3, 3, 1	
b.	4, 6, 6, 2	d.	2, 3, 2, 3	

____	62.	Why is a gas easier to compress than a liquid or a solid?
a.	Its volume increases more under pressure than an equal volume of solid does.	
b.	The volume of a gas’s particles is small compared to the overall volume of the gas.	
c.	The space between gas particles is much less than the space between liquid or solid particles.	
d.	Its volume increases more under pressure than an equal volume of liquid does.	

____	63.	The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change?
a.	It is doubled.	
b.	It does not change.	
c.	It varies depending on the type of gas.	
d.	It is reduced by one half.	

____	64.	What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)
a.	2.1M	c.	2.2M	
b.	0.0022M	d.	1.5M	

____	65.	What determines that an element is a metal?
a.	its position in the periodic table	c.	the molecules that it forms	
b.	when it is a Group A element	d.	the magnitude of its charge	

____	66.	What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
a.	K2+	c.	K1-	
b.	K+	d.	K2-	

____	67.	What is a property of a base?
a.	watery feel	c.	bitter taste	
b.	unreactive	d.	strong color	

____	68.	Which of these is an Arrhenius base?
a.	CH3COOH	c.	H2PO2	
b.	LiOH	d.	NH3	

____	69.	According to the kinetic theory, collisions between molecules in a gas ____.
a.	never occur	c.	are inelastic	
b.	cause a loss of total kinetic energy	d.	are perfectly elastic	

____	70.	What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?
a.	4.0M	c.	10M	
b.	0.40M	d.	2.0M	

____	71.	How many significant figures are in the measurement 811.40 grams?
a.	two	c.	five	
b.	four	d.	three	

____	72.	What products will form when sodium hydroxide reacts with hydrochloric acid?
a.	Sodium hydride and chlorine hydroxide	c.	Sodium hydroxide and hydrochloric acid	
b.	Sodium chloride and water	d.	Sodium chloride, hydrogen gas, and oxygen gas	

____	73.	Which compound can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base?
a.	sodium hydroxide	c.	ammonia	
b.	water	d.	hydrochloric acid	

____	74.	What element has the electron configuration 1s22s22p63s23p2?
a.	silver	c.	nitrogen	
b.	silicon	d.	selenium	

____	75.	Symbols used in equations, together with the explanations of the symbols, are shown below. Which set is correct?
a.	(g), grams	c.	(l), liters	
b.	(aq), dissolved in water	d.	(s), solid product	

____	76.	When an acid reacts with a base, what compounds are formed?
a.	a salt and water	c.	metal oxides only	
b.	water only	d.	a salt only	

____	77.	Which step in the scientific method requires you to use your senses to obtain information?
a.	making an observation	c.	designing an experiment	
b.	revising a hypothesis	d.	stating a theory	

____	78.	What is the number of moles of solute in 250 mL of a 0.4M solution?
a.	0.16 mol	c.	0.62 mol	
b.	0.1 mol	d.	1.6 mol	

____	79.	What happens to a catalyst in a reaction?
a.	It is unchanged.	c.	It is incorporated into the reactants.	
b.	It evaporates away.	d.	It is incorporated into the products.	

____	80.	Which of the following measurements (of different masses) is the most accurate?
a.	3.1000 g	c.	3.100 00 g	
b.	3.000 000 g	d.	3.122 22 g	

____	81.	In the reaction 2CO(g) + O2(g) ® 2CO2(g), what is the ratio of moles of oxygen used to moles of CO2 produced?
a.	1:1	c.	1:2	
b.	2:1	d.	2:2	

____	82.	What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration?
a.	P3-	c.	P3+	
b.	P2-	d.	P2+	

____	83.	Which of the following compounds contains the Mn3+ ion?
a.	Mn2O3	c.	MnBr2	
b.	MnO	d.	MnS	

____	84.	When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is ____.
a.	KOH + BaCl2  KCl2 + BaOH	c.	2KOH + BaCl2  2KCl + Ba(OH)2	
b.	KH + BaCl  KCl + BaH	d.	KOH + BaCl  KCl + BaOH	

____	85.	Which of the following correctly represents an ion pair and the ionic compound the ions form?
a.	Pb4+, O2-; Pb2O4	c.	Ca2-, F-; CaF2	
b.	Na+, Cl-; NaCl2	d.	Ba2+, O2-; Ba2O2

	

____	86.	What information is needed to calculate the percent composition of a compound?
a.	the formula of the compound and the atomic mass of its elements	
b.	the weight of the sample to be analyzed and its density	
c.	the formula of the compound and its density	
d.	the weight of the sample to be analyzed and its molar volume	

____	87.	The average kinetic energy of water molecules is greatest in ____.
a.	liquid water at 373 K	c.	steam at 100°C	
b.	ice at 0°C	d.	liquid water at 90°C	

____	88.	Entropy measures ____.
a.	force	c.	energy	
b.	disorder	d.	heat transferred	

____	89.	Which of the following is a heterogeneous mixture?
a.	air	c.	soil	
b.	salt water	d.	steel	

____	90.	How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O?
a.	35 x (6.02 x 1023)	c.	35	
b.	5	d.	5 x (6.02 x 1023)	

____	91.	What is the formula for potassium sulfide?
a.	K2S	c.	K2S2	
b.	KS2	d.	KS	

____	92.	The average kinetic energy of the particles of a substance ____.
a.	is equal to the total energy absorbed by the substance	
b.	is directly proportional to the temperature of the substance	
c.	increases as the temperature of the substance is lowered	
d.	is not affected by the temperature of the substance	

____	93.	What mass of sucrose, C12H22O11, is needed to make 500.0 mL of a 0.200M solution?
a.	17.1 g	c.	68.4 g	
b.	34.2 g	d.	100 g	

____	94.	Express the product of 2.2 mm and 5.00 mm using the correct number of significant digits.
a.	11.00 mm2	c.	10 mm2	
b.	11.0 mm2	d.	11 mm2	

____	95.	A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 101.4 kPa if PHe = 82.5 kPa and PCO2 = 0.4 kPa?
a.	18.5 kPa	c.	82.9 kPa	
b.	19.3 kPa	d.	101.0 kPa	

____	96.	What is pH?
a.	the negative logarithm of the hydroxide ion concentration	
b.	the negative logarithm of the hydrogen ion concentration	
c.	the positive logarithm of the hydrogen ion concentration	
d.	the positive logarithm of the hydroxide ion concentration	

____	97.	What are the missing coefficients for the skeleton equation below? 
Al2(SO4)3(aq) + KOH(aq) ® Al(OH)3(aq) + K2SO4(aq)
a.	4, 6, 2, 3	c.	1, 3, 2, 3	
b.	2, 12, 4, 6	d.	1, 6, 2, 3

____	98.	In which of the following groups of ions are the charges all shown correctly?
a.	Na, I, Rb	c.	Li, O, S	
b.	Ca, Al, Br	d.	K, F, Mg	

____	99.	The formula of the hydrogen ion is often written as ____.
a.	H	c.	OH	
b.	HO	d.	HN	

____	100.	How many moles of tungsten atoms are in 4.8 x 1025 atoms of tungsten?
a.	1.3 x 10-2 moles	c.	1.3 x 10-1 moles	
b.	8.0 x 101 moles	d.	8.0 x 102 moles