Honors Chemistry - Study Guide for Fall Final - Everett
Aqueous solutions of barium chloride and silver nitrate are mixed to form silver chloride and aqueous barium nitrate. a. AgCl(s) b. 3AgCl(aq) c. 2Ba(NO3)2(aq) d. 2AgCl(s) e. BaNO3(aq)
d. 2AgCl(s)
All of the following are in aqueous solution. Which is incorrectly named? a. HC2H3O2, acetic acid b. H2So3, sulfurous acid c. HBr, bromic acid d.HClO3, chloric acid e. HNO2, nitrous
HBr, brommic acid
You mix 275.0 mL of 1.20 M lead(II) nitrate with 300.0 mL of 1.85 M potassium iodide. The lead(II) iodide is insoluble. Which of the following is false? a. The final concentration of NO3- is 0.965 M. b. The final concentration of Pb2+ ions is 0.0913 M. c. You form 128 g of lead(II) iodide. d. The final concentration of K+ is 0.965 M. e. All are true
The final concentration of NO3- is 0.965 M.
WHich of the following has 61 neutrons, 47 protons, and 46 electrons? a. 108/47 Ag+ b. 108/46 Pd- c. 108/47 Cd+ d. 80/61 Pm e. 108/47 Ag
a. 108/47 Ag+
How should the number 1.230 x 10^3 be properly expressed as a decimal? a. 1230. b. 1230.0 c. 0.001230 d. 1230
a. 1230.
WHich of the following unit factors is incorrect? a. 1cg/100 g b. 1000 m/1 km c. 1 microliter/ 100 nL d. 1 L/1000mL
a. 1cg/100 g
40/20 Ca2+ has: a. 20 protons, 20 neutrons, and 18 electrons b. 22 protons, 18 neutrons , and 18 electrons c. 20 protons, 22 neutrons, and 18 electrons d. 20 protons, 20 neutrons, and 22 electrons e. 22 protons, 20 neutrons, and 20 electrons
a. 20 protons, 20 neutrons, and 18 electrons
WHen sodium chloride and lead(II) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation? a. 2NaNO3(aq) b. Pb2Cl(s) c. PbCl(s) d. 2PbCl2(s) e. NaNO3(aq)
a. 2NaNO3(aq)
WHen solutions of phosphoric acid and iron(III) nitrate react, which of the following terms will be present in the balanced molecular equation? a. 3HNO3(aq) b. 3FePO4(s) c. 2HNO3(aq) d. 2FePO4(s) e. HNO3(aq)
a. 3HNO3(aq)
Which of the following statements from Dalton's atomic theory is no longer true, according to modern atomic theory? a. All atoms of a given element are identical b. Atoms are not created or destroyed in chemical reactions c. Atoms are indivisible in chemical reactions d. Elements are made up of tiny particles called atoms e. All of these statements are true according to modern atomic theory.
a. All atoms of a given element are identical
Which of the following pairs is incorrect? a. BaPO4, barium phosphate b. NH4Br, ammonium bromide c. K2CO3, potassium carbonate d. CuCl, copper(I) chloride e. MnO2, manganese(IV) oxide
a. BaPO4, barium phosphate
When solutions of carbonic acid and aluminum react, which of the following are NOT present in the net ionic equation? I. hydrogen ion II. carbonate ion III. aluminum ion IV. hydroxide ion a. I and IV b. I and II c. I, II, and III d. II and III e. I and III
a. I and IV
Which of the following statements is always true concerning a reaction represented by the following balanced chemical equation? 2C2H6(g) + 7O2(g) -->6H20(l) + 4CO2(g) a. If we have more mass of C2H6, then O2 must be limiting. b. None of these statements are true. c. If we have equal masses of C2H6 and O2, there is no limiting reactant. d. If we have more mass of O2, then C2H6 must be limiting. e. If we have an equal number of moles of C2H6 and O2, there is no limiting reactant
a. If we have more mass of C2H6, then O2 must be limiting.
All of the following are true except: a. IOns are formed by changing the number of protons in an atom's nucleus b. Ions are formed by adding electrons to a neutral atom c. An ion has a positive or negative d. Ions are formed by removing electrons from a neutral atom e. Metals tend to form positive ions
a. Ions are formed by changing the number of protons in an atom's nucleus
IN writing the complete ionic equation for the reaction ( if any) that occurs when aqueous solution of KOH and Mg(NO3)2 are mixed, which of the following would not be written as ionic species? a. Mg(OH)2 b. KNO3 c. All of the above would be written as ionic species d. Mg(NO3)2 e. KOH
a. Mg(OH)2
Which of the following pairs can be used to illustrate the law of multiple proportions? a. SO and SO2 b. CO and CaCo3 c. H2o and C12H22O11 d. H2SO4 and H2S e. KCl and KClO2
a. SO and SO2
Which of the following statements is true? a. Scientists believe that solids are mostly open space b. Heating water with a Bunsen burner results in a 2:1 mixture of hydrogen and oxygen gases c. At least two of the above statements (A-C) are true d. Ions are formed by adding or removing protons or electrons e. All of the statements(A-C) are false
a. Scientists believe that solids are mostly open space
Many classic experiments have given us indirect evidence of the nature of the atom. Which of the experiments listed below did not give the results described? a. The Rutherford experiment proved the Thomson "plum-pudding" model of the atom to be essentially correct b. All of the above experiments gave the results described c. Millikan's oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the electron d. The electric discharge tube proved that electrons have a negative charge e. The Rutherford experiment was useful in determining the nuclear charge on the atom
a. The Rutherford experiment proved the Thomson "plum-pudding" model of the atom to be essentially correct
Which one of the following statements about atomic structure is false? a. The number of protons and neutrons is always the same in the neutral atom b. The protons and neutrons in the nucleus are very tightly packed c. An atom is mostly empty space d. Almost all of the mass of the atom is concentrated in the nucleus e. All of the above statements (A-D) are true
a. The number of protons and neutrons is always the same in the neutral atom
A reducing agent is an electron donor. a. True b. False
a. True
Oxides of copper include CuO and Cu2O. You heat 1.51 g of one of these copper oxides in the absence of air and obtain 1.21 g of Cu. True or False: You must have had CuO. a. True b. False
a. True
Polar molecules have an unequal distribution of charge within the molecule. a. True b. False
a. True
The molecular formula always represents the total number of atoms of each element present in a compound. a. True b. False
a. True
The reactant which, when used up completely, can produce the least amount of product, is the limiting reactant. a. True b. False
a. True
Which metals form cations with varying positive charges? a. Group 3 metals b. metalloids c. transition metals d. Group 2 metals e. Group 1 metals
c. transition metals
The amount of uncertainty in a measure quantity is determined by: a. both the skill of the observer and the limitation of the measuring instrument b. the skill of the observer only c. none of these d. neither the skill of the observer nor the limitations of the measuring instrument e. the limitation of the measuring instrument only
a. both the skill of the observer and the limitation of the measuring instrument
Which separation technique is based on differences in the volatility of the substances to be separated? a. distillation b. solvent extraction c. paper chromatography d. filtration
a. distillation
When solutions of carbonic acid and potassium hydroxide react, which of the following are NOT present in the complete ionic equation? a. hydrogen ion b. carbonate ion c. potassium ion d. hydroxide ion e. water
a. hydrogen ion
Which of the following ions forms the fewest insoluble salts? a. Mg2+ b. (NO3)- c. OH- d. Al3+ e. Cl-
b. (NO3)-
Which of the following metric relationships is incorrect? a. 1 gram =10^2 centigrams b. 1 gram = 10^3 kilograms c. 1 microliter= 10^-6 liters d. 10 decimeter= 1 meter e. 10^3 milliliters= 1 liter
b. 1 gram = 10^3 kilograms
Which of the following aqueous solutions contains the greatest number of ions? a. 800.0 mL of 0.10 M sucrose b. 300.0 mL of 0.10 M CaCl2 c. 200.0 mL of 0.10 M KBr d. 200.0 mL of 0.10 M FeCl3 e. 400.0 mL of 0.10 M NaCl
b. 300.0 mL of 0.10 M CaCl2
How many protons, neutron and electrons, in that order are present in the anion formed by one atom of 79 Se? a. 34, 45,34 b. 34, 45, 36 c. 36, 45, 36 d. 34, 34 45 e. 32, 45, 34
b. 34, 45, 36
Which of the following ions is NOT likely to form from the appropriate atom? a. Na+ b. C4+ c. As3- d. Ti4+ e. Mg2+
b. C4+
For what compound does 0.256 mole weigh 12.8 g? a. C2H4O b. CH3Cl c. none of these d. CO2 e. C2H6
b. CH3Cl
Which of the following are incorrectly paired? a. Cobalt, Co b. Cesium, Ce c. Carbon, C d. Copper, Cu e. Calcium, Ca
b. Cesium, Ce
A chemical that changes color at the endpoint of a reaction is called a colorimeter. a. True b. False
b. False
A chemical theory that has been known for a long time becomes a law. a. True b. False
b. False
All physical changes are accompanied by chemical changes. a. True b. False
b. False
An acid is a substance that produces OH- ions in water. a. True b. False
b. False
Color changes always indicate a chemical change. a. True b. False
b. False
Given the equation 3A + B --> C + D, you react 1 mole of A with 3 mole of B. True or False: A is the limiting reactant because you have fewer moles of A than B. a. True b. False
b. False
The concentration of a salt water solution that sits in an open beaker decreases over time. a. True b. False
b. False
The filtrate is the solid formed when two solution are mixed. a. True b. False
b. False
The number of neutrons in an atom is the same for all the neutral atoms of that element. a. True b. False
b. False
The reactant with the highest molar mass is always the limiting reactant. a. True b. False
b. False
When balancing a chemical equation, it is generally best to start with least complicated molecules. a. True b. False
b. False
Identify the precipitate(s) formed (if any) in the following reaction in aqueous solution, Fe(NO3)2 + (NH4)2CO3-->: a. (NH4)2C03(s) b. FeCO3(s) c. Fe2(CO3)3 d. NO precipitate will be observed e. NH4NO3(s)
b. FeCO3(s)
WHich among the following represent a set of isotopes? Atomic nuclei containing: I. 20 protons and 20 neutrons II. 21 protons and 19 neutrons III. 22 neutrons and 18 protons IV. 20 protons and 22 neutrons V. 21 protons and 20 neutrons a. I, V b. I, IV, and II, V c. No isotopes are indicated d. I, II, III e. III, IV
b. I, IV and II, V
Select the spectator ions for the following reaction, Pb(NO3)2 + 2KCl --> PbCl2 + 2NaNO3: a. Pb2+(aq), NO3-(aq) b. K+(aq), NO3-(aq) c. K+(aq), Cl-(aq) d. Pb2+(aq), Cl-(aq) e. Pb2+(aq), Cl-(aq), K+(aq), NO3-(aq)
b. K+(aq), NO3-(aq)
Balanced chemical equation imply which of the following? a. Numbers of molecules are conserved in a a chemical change b. Numbers of atoms are conserved in a chemical change c. B and C d. A and B e. Volume is conserved in chemical change
b. Numbers of atoms are conserved in chemical change
An example of a pure substance is: a. pure water b. all of these c. carbon dioxide d. compounds e. elements
b. all of these
Which of the following compounds has the same percent composition by mass as styrene, C8H8? a. a-ethyl naphthalene, C12H12 b. all of these c. acetylene, C2H2 d. benzene, C6H6 e. cyclobutadiene, C4H4
b. all of these
The limiting reactant in a reaction: a. none of these b. has the lowest ratio of moles available/coefficient in the balanced equation c. is the reactant for which you have the fewest number of moles d. has the lowest coefficient in a balanced equation e. has the lowest ratio of coefficient in the balanced equation/ moles available
b. has the lowest ratio of moles available/coefficient in the balanced equation
A solution is also called a: a. pure mixture b. homogenous mixture c. heterogenous mixture d. distilled mixture e. compound
b. homogenous mixture
Which of the following is not a fundamental metric unit? a. kilogram b. liter c. meter d. second
b. liter
The boiling of water is a: a. chemical change because a gas (steam is given off b. physical change because the gaseous water is chemically the same as the liquid c. physical change because the water merely disappears d. chemical and physical damage e. chemical change because heat is needed for the process to occur
b. physical change because the gaseous water is chemically the same as the liquid
Which of the following equations is not balanced? a. 4Al + 3O2 --> 2Al2O3 b. C2H6 + 7/2O2 -->2CO2 + 3H2O c. 2KClO3 --> 2KCl + 3/2O2 d. P4 + 5O2 --> P4O10 e. 4P4 + 5S8 --> 4P4S10
c. 2KClO3 --> 2KCl + 3/2O2
You have two solution of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M solution. You have much more of the 4.00 M solution and you add the solutions together. Which of the following could be the concentration of the final solution? a. 6.00 M b. 8.10 M c. 3.50 M d. 3.00 M e. 2.70 M
c. 3.50 M
Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The net ionic equation contains which of the following terms? a. Ba2+(aq) b. AgCl(aq) c. Ag+(aq) d. NO3-(aq) e. H+(aq)
c. Ag+(aq)
If the Thomson model of the atom had been correct, Rutherford would have observed: a. Positive particles formed in the foil b. Alpha particles greatly deflected by the metal foil c. Alpha particles going through the foil with little or no deflection d. None of the above observations is consistent with the Thomson model of the atom e. Alpha particles bouncing off the foil
c. Alpha particles going through the foil with little or no deflection
Avogadro's hypothesis states that: a. A given compound always contains exactly the same proportion of elements by mass. b. Each atom of oxygen is 16 times more massive than an atom of hydrogen. c. At the same temperature and pressure, equal volumes of different gases contain an equal number of particles. d. Mass is neither created nor destroyed in a chemical reaction. e. When two elements form a series of compounds, the ratios masses that combine with 1 gram of the first element can always be reduced to small whole number
c. At the same temperature and pressure, equal volumes of different gases contain an equal number of particles.
Which of the following ions is most likely to form an insoluble sulfate? a. Li_ b. CL- c. Ca2+ d. S2- e. K+
c. Ca2+
When solutions of cobalt(II) chloride acid react, which of the following terms will be present in the net ionic equation? a. 2CoCO3(s) b. two of these c. CoCO3(s) d. 2Cl-(aq) e.H+(aq)
c. CoCO3(s)
Select the spectator ions for the following reaction in aqueous solution, AgNO3 + LiI -->Agl + LiNO3 a. Ag+(aq), I-(aq) b. Ag+(aq), NO3-(aq) c. Li+(aq), NO3-(aq) d. Ag+(aq), I-(aq), LI+(aq), NO3-(aq) e. Li+(aq), I-(aq)
c. Li+(aq), NO3-(aq)
Complete the following reaction in aqueous solution and select the spectator ions, Fe(NO3)2 + (NH4)2CO3 -->: a. Fe2+(aq), CO32-(aq) b. NH4+(aq), CO32-(aq) c. NH4+(aq), NO3-(aq) d. Fe2+(aq), NO3-(aq) e. Fe2+(aq), NH4+(aq), NO3-(aq), CO32-(aq)
c. NH4+(aq), NO3-(aq)
Equal masses (in grams) of hydrogen gas and oxygen gas are reacted to form water. Which substance is limiting? a. Water is limiting. b. Nothing is limiting. c. Oxygen gas is limiting. d. More information is needed to answer this question. e. Hydrogen gas is limiting
c. Oxygen gas is limiting
As part of the calibration of a new laboratory balance, a 1.000-g mass is weighed with the following results: Trial Mass 1 1.201+-0.001 2 1.202+-0.001 3 1.200+-0.001 The Balance is: a. Accurate but imprecise b. Both inaccurate and imprecise c. Precise but inaccurate d. Accuracy and precision are impossible to determine with available information e. Both accurate and precise
c. Precise but inaccurate
The formula of water, H2O, suggests: a. There is twice as much mass of hydrogen as oxygen in each molecule b. There are two oxygen atoms and one hydrogen atom per water molecule c. There are two hydrogen atoms and one oxygen atom per water molecule d. None of these e. There is twice as much of oxygen as hydrogen in each molecule
c. There are two hydrogen atoms and one oxygen atom per water molecule
In march 2008, gold reached a milestone value of $100 pper troy ounce. At that price, what was the cost of a gram of gold?(1 troy ounce= 31.10g) a. less than $1 b. over $100 c. between $10 and $50 d. between $50 and $100 e. between $1 and $10
c. between $10 and $50
Which of the following is not a unit in the SI system? a. meter b. candela c. calorie d. ampere e. Kelvin
c. calorie
Which of the following is not a fundamental metric unit? a. meter b. second c. gram d. mole
c. gram
Order the four metric prefixes from smallest to largest. a. kilo<centi<nano<milli b. milli<nano<centi<kilo c. nano<milli<centi<kilo d. centi<nano<kilo<milli e. kilo<centi<milli<nano
c. nano<milli<centi<kilo
The limiting reactant in a reaction: a. is the reactant for which there is the fewest number of moles b. is the reactant which has the lowest coefficient in a balanced equation c. none of the above d. is the reactant for which there is the least amount in grams e. is the reactant for which there is the most amount in grams
c. none of the above
When 87.7 is added to 73.841, the result should be reported with ___ significant figures. And when 87.7 is divided by 73.841 the result should be reported with ___significant figures. a. 3,5 b. 4,4 c. 4,3 d. 3,3
d. 4,3
Calculate 5.1234 + 0.033/ 1.650 and report to the correct number of significant figures. a. 5.1 b. 3.1 c. 3.125 d. 5.143
d. 5.143
A wavelength of red light is measured at 655 nm. What is this measurement in cm? a. 6.55 x 10-7 cm b. 0.00655 c. 6.55 cm d. 6.55 x 10-5 cm
d. 6.55 x 10-5
Which of the following statements are true of uranium-238 I. Its chemical properties will be exactly like those of uranium-235 II. Its mass will be slightly different from that of an atom of uranium-235 III. It will contain a different number of protons than an atom of uranium-235 IV. It is more plentiful in nature than uranium-235 a. II, II, IV b. all of these c. I, II,III d. I, II, IV e. III, IV
d. I, II, IV
Which of the following is incorrectly name? a. PO43-, phosphate ion b. NH4ClO4, ammonium perchlorate c. Mg(OH)2, magnesium hydroxide d. NO3-, nitrite ion e. Pb(NO3)2, lead(II) nitrate
d. NO3-, nitrite ion
Which of these statements is a consequence(follows from) the Law of Multiple Proportions? a. The atomic masses of all the elements in the periodic table have fixed values b. All samples of chlorine contain 35Cl and 37Cl in the same (definite) ratio c. The %lead by mass in the compound galena is the same for all pure samples obtained from any source d. The mass of oxygen that is combined with a fixed mass of nitrogen in each of the binary nitrogen oxides can be expresses as a ratio of small whole numbers e. None of these is correct
d. The mass of oxygen that is combined with a fixed mass of nitrogen in each of the binary nitrogen oxides can be expresses as a ratio of small whole numbers
The density of a liquid is determined by successively weighing 35, 50, 75, 100, and 125 mL of the liquid in a 250-mL beaker> Considering the plot of total mass (y-axis) versus volume (x-axis), which of the following is true? a. The plot should be curved upward because the mass of the liquid is higher in successive trials b. None of the above c. The plot should be linear because the mass of the beaker stays constant d. The plot should be rather linear because the slope measures the density of a liquid. e. The plot should be curved upward because the slope measures the density of a liquid
d. The plot should be rather linear because the slope measures the density of a liquid.
When solutions of strontium chloride and sodium sulfate react, which of the following is a spectator ion? a. sodium ion b. chloride ion c. strontium ion d. two of these e. sulfate ion
d. two of these
Which of the following has a different value on the moon compared to earth? a. moles b. mass c. time d. weight
d. weight
SO2 reacts with H2S as follows: 2H2s + SO2 -->3S + 2H2O When 7.50 g of H2S reacts with 12.75 g of SO2, which statement applies? a. SO2 is the limiting reagent b. 6.38 g of sulfur are formed c. 0.0216 moles of H2S remain d. 1.13 g of H2S remain e. 10.6 g of sulfur are formed
e. 10.6 g of sulfur are formed
Which of the following atomic symbols is incorrect? a. 14/6 C b. 37/17 Cl c. 32/15 P d. 39/19 K e. 14/8 N
e. 14/8 N
The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species? a. 2Ca3(PO4)2(s) b. 6NaBr(aq) c. 2Br-(aq) d. (PO4)3-(aq) e. 3Ca2+(aq)
e. 3Ca2+(aq)
Which of the following atoms, isotopes or ions contains 23 protons, 18 electrons and 27 neutrons? a. 45Co5+ b. 41Kr5- c. 50Kr d. 50V5- e. 50V5+
e. 50V5+
An isotope, X, of a particular element has an atomic number of 15 and a mass number of 31. Therefore: a. A, B, and C b. X has an atomic mass of 30.973 c. X has 16 neutrons per atom d. X is an isotope of phosphorous e. A and B
e. A and B
Which of the following statements is false? a. Elements can exist as atoms or molecules b. The terms "atom" and "element"can have different meanings c. Solutions are always homogenous mixtures d. At least two of the above statements (A-D) are false e. Compounds can exist as atoms or molecules
e. Compounds can exist as atoms or molecules
WHen solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the net ionic equation? I. hydrogen ion II. acetate ion III. sodium ion IV. hydroxide ion a. I and IV b. I, II, and III c. II and III d. I and II e. I and III
e. I and III
Which of the following compounds is soluble in water? a. CoCO3 b. Ni(OH)2 c. PbCL2 d. BaSO4 e. K3PO4
e. K3PO4
You have equal masses of different solutes dissolved in equal volumes of solution. Which of the solutes would make the solution having the highest molar concentration? a. KOH b. NaOH c. all the same d. KCl e. LiOH
e. LiOH
Which pair of ions would not be expected to form a precipitate when dilute solution of each are mixed? a. Pb2-, Cl- b. Ba2+, (PO4)3- c. Pb2+, OH- d. Al3+, S2- e. Mg2+, (SO4)2-
e. Mg2+, (SO4)2-
You have a sample of zinc (Zn) and a sample of aluminium (Al). You have an equal number of atoms in each sample. WHich of the following statements concerning the masses of the samples is true? a. The mass of the aluminium sample is more than twice as great as the mass of the zinc sample b. The masses of each sample are equal c. The mass of the zinc sample is more than the mass of the aluminium sample, but it is not twice as great d. The mass of the aluminium sample is more than the mass of the zinc sample, but it is not twice as great e. The mass of the zinc sample is more than twice as great as the mass of the aluminium sample
e. The mass of the zinc sample is more than twice as great as the mass of the aluminium sample
As warm water sits in a cool room, you measure the temperature change(ΔT = T(initial) - T(final)).Which of the following is true? a. The temperature change (ΔT)will be the same regardless of the scale you use b. None of the above c. The temperature change (ΔT) is bigger if you are measuring in Celsius d. Answer A or B is correct, depending on the difference in temperature between the water and the room e. The temperature change (ΔT) is bigger if you are measuring in Fahrenheit
e. The temperature change (ΔT) is bigger if you are measuring in Fahrenheit
Which statement is not correct? a. A gamma ray is high-energy light b. An alpha particle has a 2+ charge c. Three types of radioactive emission are gamma rays, beta rays, and alpha rays d. The mass of an alpha particle is 7300 times that of the electron e. There are only three types of radioactivity known to scientists today
e. There are only three types of radioactivity known to scientists today
WHich of the following names is incorrect? a. magnesium oxide b. All of the above names are correct c. cobalt(II) chloride d. diphosphorus pentoxide e. aluminium(III) oxide
e. aluminium(III) oxide
An ion is formed: a. by either adding or subtracting neutrons from the atom b. two of the above are true c. by either adding or subtracting protons from the atom d. All of the above are true e. by either adding or subtracting electrons from the atom
e. by either adding or subtracting electrons from the atom
A quantitative observation: a. must be obtained through experimentation b. does not contain a number c. is none of these d. always makes a comparison e. contains a number and a unit
e. contains a number and a unit
All of the following are characteristics of metals except: a. ductile b. malleable c. often lustrous d. good conductors of heat e. tend to gain electrons in chemical reactions
e. tend to gain electrons in chemical reactions
By knowing the number of protons a neutral atom has, you should be able to determine: a. the number of electrons in the neutral atom b. the name of the atom c. none of the above d. the number of neutrons in the neutral atom e. two of the above
e. two of the above
