Chem final (all quizzes)
Which of the following statements is true for neutral solutions in which the water is the solutions in which water is the solvent? a. Neutral solutions contain no H₃O⁺ ions b. Neutral solutions contain no OH⁻ ions c. Neutral solutions contain H₃O⁺ and OH⁻ ions in equal concentrations d. More than one response is correct
C
Which of the following violates the Pauli exclusion principle? a. b. c. Circle with two down arrows d.
C
Which of the following will not have electrons in the 3rd orbital? a. K b. Mg c. Na+ d. Ag+
C
Which one of these elements is a gas at room temperature? a. antimony b. phosphorus c. nitrogen d. arsenic
C
You discover a new element which consists of two isotopes. The first isotope, 243X (mass=242.45 u) comprises 40.000% of the total. The second isotope, 248X (mass= 247.11 u) accounts for the rest. What would be the average atomic mass for your new element? a. 242.45 u b. 244.32 u c. 245.25 u d. 247.11 u
C
You want to remove as much CO2 gas as possible from a water solution. Which of the following treatments would be most effective? a. cool the solution c. boil the solution b. filter the solution d. aerate the solution
C
if 13% of a class cheats on an exam and there are 93 students in the class, how many students should you recommend be expelled (to the nearest whole student)? a. 9 b. 10 c. 12 d. 15
C
which of the following particles is the smallest a. proton b. electron c. neutron d. They are all the same size
C
A 5.00 liter gas sample is collected at a temperature and pressure of 27.0˚C and 1.20 atm. It is desired to transfer the gas to a 3.00 liter container at a pressure of 1.00 atm. What must be the temperature of the gas in the 3.00 liter container? a. 216 K b. 417 K c. 13.5 ˚C d. 150 K
D
A mixture of helium, argon and krypton is made and stored in a cylinder at a total pressure of 2.80 atm. The partial pressure of helium is 900 torr, and that of argon is 250 torr. What is the partial pressure of krypton in the mixture? a. 1.18 atm b. 1.51 atm c. 1150 torr d. 978 torr
D
A polar molecule must have a. polar bonds b. an unsymmetrical arrangement c. neither polar bonds nor an unsymmetrical arranement d. both polar bonds and an unsymmetrical arrangement
D
A solution has a pH of 11.60. What is the value of [H⁺]? a. 2.4 x 10⁻⁴ b. b. 4.0 x 10⁻³ c. 4.0 x 10⁻¹¹ d. 2.5 x 10⁻¹²
D
A solution is made by combining 4.00 g of sugar and 100 mL of water (density = 1.00 g/mL). What is the concentration in % (w/w)? a. 26.0 b. 4.00 c. 0.0400 d. 3.85
D
A student completes 5 problems out of a total of 8 on a pop quiz, what percentage of the quiz was completed? a. 0.625 b. 6.25 c. 16.0 d. 62.5
D
Antacids contain a substance that neutralizes hydrochloric acid. Which of the following is a candidate for use as an antacid? a. Al(NO₃)₃ b. MgCl₂ c. Al₂(SO₄)₃ d. MgCO₃
D
Calculate the kinetic energy of a .500 g particles traveling at 5.50 cm/s a.2.75 g cm2/s2 b. 7.56 g cm2/s2 b. 51.1 g cm2/s2 d. 6.88 g cm2/s2
D
Calculate the weight percentage of hydrogen in water. a. 33.3 b. 66.7 c. 2.00 d. 11.1
D
Consider the reactants in the partial equation given. Which choice is a product? H₃PO₄ + Sr(OH)₂ a. no reaction b. SrH₃PO₅ c. SrH₅PO₆ d. Sr₃(PO₄)₂
D
Convert a temperature of 45˚C into Kelvins. a. -45 K b. -228 K c. 228 K d. 318 K
D
Drinking water can be purified by which of the following methods? a. reverse osmosis b. distillation c. ion exchange d. all of the choices
D
Given the following: heat of fusion of ice = 80.0 cal/g, specific heat of ice = .480 cal/g, and specific heat of water = 1 cal/g. Calculate the amount of heat required to melt 30.0 g of ice a. 14.4 cal b. 2.41 cal c. 80.0 cal d. 2.40 kcal
D
How many grams of solid KCl are needed to prepare 250 mL of 0.235 M solution? a. 9.32 b. 31.3 c. 15.6 d. 4.38
D
How many moles of Na2CO3 would be needed to react with 750 mL of 0.250 M H2SO4 solution? Na2CO3 + H2SO4→Na2SO4 + CO2 + H2O a. 3.00 × 103 b. 0.333 c. 1.33 d. 0.188
D
How many significant figures are used in expressing a measurement as .2503 L? a. one b. two c. three d. four
D
In a buffer solution made up of equal concentration of acetic acid and sodium acetate, NaC₂H₃O₂, which component is used to buffer against OH⁻? a. C₂H₃O₂ b. Na⁺ c. OH⁻ d. HC₂H₃O₂
D
Knowing that 1 g = .035 oz and 16 ounces = 1 lb, calculate the number of grams in 10 pounds. a. 35 b. .56 c. 1.8 d. 4.6 x 10^3
D
The basic unit of length in the metric system is the ______ a. mil b. millimeter c. foot d. meter
D
The buffer capacity is the amount of _______ that can be absorbed without causing significant changes in pH. a. acid c. base b. neither acid nor base d. both acid and base
D
The cleaning action of soaps and detergents is attributable to a. their ionic character b. the long hydrocarbon tail in their structure c. their ability to dissociate into ions d. all of the above
D
The density of zinc is 7.13 g/cm3. What is the mass in kilograms of a 125 cm3 cylinder of zinc? a. 891 kg b. 17.5 kg c. .0175 kg d. .891 kg
D
The force resulting from particle motion is referred to as: a. cohesive b. chemical c. nuclear d. disruptive
D
The number .00816 expressed correctly using scientific notation is a. 8.16 x 10^2 b. 8.16 x 10^3 c. 8.16 x 10^-2 d. 8.16 x 10^-3
D
The rigid three‐dimensional arrangement assumed by the ions of ionic compounds is called a: a. molecule. b. binary compound. c. lattice site. d. crystal lattice.
D
The term "strong acid" refers to: a. the number of hydrogens attached to the acid molecule. b. the speed at which it will dissolve metal. c. if it will cause burns to the skin. d. the ability of the acid to dissociate completely in solution.
D
Using d = m/V, what is the volume of a solid that has a density is 3.14g/cm3 and has a mass of 7.04 grams? a. 22.1 cm3 b. 22.11 cm3 c. 2.24 cm3 d. 2.242 cm3
D
What is the basis for placing groups of elements into a family on the periodic table a. similar atomic mass numbers b. identical chemical and physical properties c. similar colors, shapes, and uses d. similar valence electron configurations
D
What is the formula mass of the compound formed between Al³⁺ and Cl⁻ a. 187.5 u b. 62.5 u c. 116.5 u d. 133.5 u
D
What is the molar mass of Ba3(PO4)2? a. 232.30 g/mol b. 327.27 g/mol c. 369.63 g/mol d. 601.92 g/mol
D
What is the oxidation number of Br in BrO⁻₂? a. -1 b. +1 c. +2 d. +3
D
What is the oxidation number of Cl in HClO₃? a. +2 b. +3 c. +4 d. +5
D
When a strong acid is added to ammonia and mixed, which of the following would not be produced? a. conjugate acid b. conjugate base c. salt d. water
D
When making some iced tea, you find that you can dissolve 100 grams of table sugar in a liter of tea at 20°C. Based on this, what did you learn? a. Based on the solubility, tea must be a nonpolar solvent b. the solubility of table sugar in tea at 20°C is 100g/L c. Table sugar must be a strong electrolyte d. you can dissolve 100 grams of sugar in tea at 20°C
D
Which interparticle forces would you expect to find in a sample of the element lithium? a. covalent. b. dispersion forces. c. ionic. d. metallic.
D
Which ions will appear in the total ionic equation for the following reaction? Ba²⁺+CO₃²⁻+2H⁺+SO₄²⁻→CO₂+H₂O+BaSO₄ a. Ba²⁺ and CO₃²⁻ b. H⁺and SO₄²⁻ c. Ba²⁺, CO₃²⁻, and H⁺ D. Ba²⁺, CO₃²⁻, H⁺, and SO₄²⁻
D
Which of the following covalent molecules contains polar bonds? a. O≡C b. H—H c. H—Cl d. more than one response is correct
D
Which of the following elements is nonmetal? a. Ni b. Cu c. Ba d. I
D
Which of the following has the largest mass? a. 5.0 mol H2O b. 3.5 mol NH3 c. 8.0 mol C d. 6.0 mol C2H2
D
Which of the following is a chemical property of matter? a. color b. density c. freezing point d. flammability
D
Which of the following is a correct electron dot formula for a group IIIA (13) element M? a. (M w/ 4 dots evenly spaced) b. (M w/ 5 dots, one on bottom none on top) c. (M w/ 3 dots all on right) d.(M w/ 3 dots 1 on left, 1 on top, 1 on right)
D
Which of the following is present in pure water? a.H₃O⁺ b.OH⁻ c.H₂O d. more than one response is correct
D
Which of the following pairs of gases would diffuse at essentially the same rate? a.NO2 and NO b.O2 and Ar c.PH3 and C2H2 d.N2O and CO2
D
Which of the following pressure units is largest? a. one torr b. one mm Hg c. one psi d. one atm
D
Which of the following statements IS true about the reaction? 2 CH₄ + 3 O₂→2 CO₂ + 4 H₂O a. Water is a reactant b. Methane and carbon dioxide are products c. Methane is a product d. Water and Carbon dioxide are products
D
Which of the following subshells has the higher energy? a. 4s b. 4p c. 4d d. 4f
D
Which of the following substances are composed of heteroatomic molecules? a. an iron nail b. oxygen c. copper wire d. water
D
Which of the following substances would behave as an Arrhenius base? a. Na₂CO₃ b. Na₃PO₄ c. K₂S D. KOH
D
Which of the following uses the unit of "u" or "amu"? a. atomic weights of atoms b. relative masses of atoms c. molecular weights of molecules d. more than one response is correct
D
Which species would be considered a spectator ion based on the following equation? Ba²⁺+2NO₃⁻+2Na⁺+SO₄²⁺→BaSO₄+2NO₃⁻+2Na⁺ a. Ba²⁺ b. SO₄²⁺ c. BaSO₄ D. 2NO³⁻
D
Write the formula for a compound consisting of 3 sodium atoms, 1 phosphorus atom, and 4 oxygen atoms a. S3PO4 b. 3NaP4O c. Na3P2(O2) d. Na3PO4
D
a REDOX reaction can also be a(n) a. combination reaction b. single replacement reaction c. decomposition reaction d. more than one response is correct
D
2500 liters of oxygen gas is produced at 1.00 atm of pressure. It is to be compressed and stored in a 20.0 liter cylinder. If temperature is constant, calculate the pressure of the oxygen in the cylinder a.125 atm b.4.0 atm c.80.0 atm d.8.00 atm
A
A balloon has a volume of 5.00 liters of 22˚C and 1.00 atmosphere of pressure. What will be the balloon's volume in liters if the pressure is increased to 3.00 atmospheres at 22˚C? a. 1.67 b. 0.600 c. 1.30 d. 0.800
A
A correct lewis dot structure for BrCl is______ a. Br-Cl (both have 4 dots each) ONE LINE b. c. d.
A
A gas sample is collected in a balloon. What happens to the density of the gas sample as the sample is heated? a. decreases b. increases c. does not change d. could increase or decrease, depending on how much it was heated
A
A salt sample is placed into some water and nearly all of it dissolves without heating. The resulting solution is: a. saturated. c. unsaturated. b. supersaturated. d. canʹt tell from the data given
A
A sample of gas collected at 21.0˚C and a pressure of 660 torr has a volume of 1.83 liters. What volume in liters will the gas occupy at 38.0˚C under a pressure of 500 torr? a. 2.56 b. 4.37 c. 2.28 d. 1.33
A
A solution for which [OH⁻]=3.0 x 10⁻¹⁰ is classified as a. acidic b. basic c. neutral d. more than one response is correct
A
A solution is made by dissolving 15.0 mL of oil in enough gasoline to give 50.0 mL of solution. What is the % (v/v) of oil in the solution? a. 30.0 b. 23.1 c. 42.9 d. 3.33
A
A solution is made by dissolving 5.85 grams of NaCl in enough distilled water to give a final volume of 1.00 L. What is the molarity of the solution? a. 0.100 b. 1.00 c. 0.0250 d. 0.400
A
According to the Arrhenius theory, what is produced when acid dissolves in water? a. H+ b. OH- c. H₃O+ c. NH₄⁺
A
Choose the correct electronic configuration for the element As a. [Ar]4s2-3d10-4p3 b. 4s2-3d10-4p3 c. [Ar]-4s2-4d10-4p3 d. 4s2-4d10-4p3
A
Definite shape is a characteristic of which state of matter? a. solid b. liquid c. gaseous d. more than one response is correct
A
How many electrons are in the outer shell of element 15? a. 5 b. 3 c. 15 d. 2
A
How many silicon atoms (Si) are contained in a 12.5 g sample of silicon? a. 2.68 x 10^23 b. 5.83 x 10^-22 c. 1.35 x 10^24 d. 1.71 x 10^21
A
If a solution of acetic acid (a weak acid) is titrated with the NaOH solution, what will be the pH at the equivalence point? a. higher than 7 b. lower than 7 c. equal to 7 d. can't be predicted
A
If the electronegativity difference between A and B is 0.8, what type of bond is formed between the two elements? a. polar covalent b. nonpolar covalent c. ionic d. metallic
A
If the formula for sulfuric acid is H2SO4, what would be the expected formula for the compound between hydrogen and tellurium, Te? a. H2TeO4 b. HTe c. Hte2 d. H2Te
A
If urine has a density of 1.08 g/mL, what would be the mass of a 125 mL urine sample? a. 135 g b. .00864 g c. 116 g d. 125 g
A
Many cleaning agents contain bases because bases react with a. fats or oils b. glass c. salts d. more than one response is correct
A
On a cold winter day the weather report gives the temperature as -5.0 degrees F. What would this temperature be if reported on the Kelvin scale? a. 252 k b. 258 k c. 268 k d. -20.6 k
A
One Avogadro's number of iron (Fe) atoms would weigh ______. a. 55.9 g b. 6.02 x 10^23 g c. 55.9 u d. 6.02 x 10^-23 g
A
Single replacement reactions are always a. redox reactions b. nonredox reactions c. combination reactions d. decomposition reactions
A
Some salts isolated by evaporation retain water which is called a. water of hydration b. hydroxide c. hydronium d. crystallized water
A
Suppose an electron moved from the second shell to the third shell. a. The move required an input of energy b. The move gave off energy c. Electrons can move spontaneously from shell to shell d. electrons can't move from shell to shell, but can move into the nucleus
A
Table salt, NaCl is best classified as a(n)_____ a. compound b. element c. homogeneous mixture d. heterogeneous mixture
A
The boiling point of a solution of sugar water is a. Higher than that of pure solvent b. The same as that of a pure solvent c. Lower than that of pure solvent d. Impossible to determine
A
The correct name for the covalent compound N2O4 is: a. dinitrogen tetroxide. b. nitrogen oxide. c. nitrogen quartoxide. d. dinitrogen quartoxide.
A
Two objects are moving with the same velocity, but one has twice the kinetic energy of the other. How does the mass of the object with higher kinetic energy compare to the other object's mass? a. It is larger by a factor of 2. b. It is smaller by a factor of 2. c. It is larger by a factor of 4. d. It is smaller by a factor of 4.
A
What are the missing products in the following reaction when it is written as a molecular equation? 3HBr+SrCO₃→____ + ______ +H₂O a. SrBr₂+CO₂ b. SrBr₂+HCO₃⁻ c. Sr₂+H₂CO₃ d. HBr+CO₂
A
What is the mass number of a carbon-13 (13C) atom? a. 13 b. 12 c. 6 d. 7
A
What is the pKa of an acid with a Ka of 1.82 x 10‐5? a. 4.74 b. ‐4.74 c. 9.26 d. ‐9.26
A
What is the shell number for the outer shell electrons in bromine, Br? a. 4 b. 3 c. 5 d. 6
A
What substance is oxidized in the following reaction? 4HCl+MnO₂→Cl₂+2H₂O+MnCl₂ a. Cl in HCl b. Mn in MnO₂ c. H in HCl d. O in MnO₂
A
What the reducing agent in the following reaction? 4HCl+MnO₂→Cl₂+2H₂O+MnCl₂ a. Cl in HCl b. Mn in MnO₂ c. H in HCl d. O in MnO₂
A
When a liquid sample is taken from sea level to a higher elevation, what happens to the external (atmospheric) pressure on the liquid and the boiling point of the liquid a. both decrease b. both increase c. pressure goes down, but boiling point goes up d. pressure goes up, but boiling point goes down
A
When solid NaOH is dissolved in water, the solution becomes hot. The solution process is: a. exothermic. b. endothermic c. neither exothermic nor endothermic d.Can't be classified
A
Where an acid is analyzed by adding a measured quantity of base, the point at which all the acid has reacted correctly is called? a. the equivialence point b. the neutral point c. the endpoint d. the analysis point
A
Which of the following Lewis structures depicts a reasonable representation of SO₂? a. Can't paste it in. Just remember A b. c. d.
A
Which of the following correctly illustrates hydrogen bonding in water? a. I can't paste these in! Just remember the letter b. c. d.
A
Which of the following distinguishing electrons represents an element with properties similar to an element with a 3p3 distinguishing electron? a. 4p3 b. 3p2 c. 3d3 d. 2p2
A
Which of the following has the highest electronegativity? a. O b. N c. Si d. P
A
Which of the following is a combination reaction? a. SO₂+O₂→2SO₃ b.2C₂H₂+5O₂→4CO₂+2H₂O c. 2H₂O₂→2H₂O₂+O₂ d.AgNO₃+NaCl→AgCl+NaNO₃
A
Which of the following is a property of acid solutions? a. sour taste b. slippery feel c. change red litmus to blue d. more than one response is correct
A
Which of the following is a reasonable explanation as to why atomic radii become smaller as one moves to the right for the representative elements in a period a. The charge of the nucleus increases, pulling the shells closer b. More densely packed shells are always smaller c. elements become less metallic d. atomic radii actually increase as you move to the right
A
Which of the following is a single replacement reaction? a. CuO+H₂→Cu+H₂O b. HBr+KOH→H₂O+KBr c. SO₂+O₂→2SO₃ d. 2Hl→I₂+H₂
A
Which of the following is an oxidizing agent? a. O₂ b. H₂ C. H₂O d. HCl
A
Which of the following is the correct lewis structure for C2H4? a. To carbons in middle connected by 2 lines, each C bonded to 2 H's via one line each. No dots
A
Which of the following would you expect to be a weak electrolyte? a. acetic acid b. sodium acetate c. tap water d. more than one answer is correct
A
Which pair of the following represents the same electron configuration? a. [Ne]3s2 and 1s2-2s2-2p6-3s2 b. [He]3s2 and 1s2-2s2-2p6-3s2 c. [Ar]3s2 and 1s2-2s2-2p6-3s2 d. All represent the same configuration
A
____ states that, electrons will not join other electrons in an orbital if an empty orbital same energy is available a. Hund's rule b. Pauli exclusion rule c. Periodic law d. None of these
A
a 25.00 mL sample of hydrochloric acid solution, HCl, is titrated with .0512 M NaOH solution. the volume of naOH solution required is 21.68 mL. What is the molarity of the HCl solution? a. .0444 b. .0590 c. .0295 d. .0148
A
identify the substance with the lowest pH a. orange juice b. household ammonia c. baking soda, NaHCO₃ d. milk
A
As NH4NO3 dissolves in water, the resulting solution becomes colder. Which of the following expressions is most correct? a. NH4NO3→NH + NO + heat b. heat + NH4NO3→NH + NO3 c.NH4NO3→NH + NO3 d.NH4NO3 + heat→NH + NO + heat
B
Atoms are neutral. How can they have no charge? a. equal numbers of protons and neutrons b. equal numbers of protons and electrons c. equal numbers of neutrons and electrons d. any charge has been drained out of the atom
B
Cohesive forces in matter are related to: a. potential energy from particle repulsions. b. potential energy from particle attractions. c. kinetic energy. d. more than one response is correct
B
Convert 30.0 degrees C to Fahrenheit a. 112 b. 86 c. 48.7 d. 34.4
B
Convert a temperature 76 degrees F to a celcius value a. 10 b. 24 c. 44 d. 169
B
Do the following calculation and express the answer using correct scientific notation a. 5.53 x 10^3 b. 1.81 x 10^-4 c. 4.88 x 10^8 d. 2.05 x 10^-9
B
Do the following calculation and express the answer using the correct number of significant figures. ______=(342)x(0.0012) / 100 a. .00410 b. .0041 c. 4.10 x 10^-3 d. .004104
B
Early measurements of length were based on a. dimensions of astronomical bodies b. dimensions of the human body c. dimensions of bodies of water d. distances between two cities
B
How many moles of oxygen atoms are in one mole of C02? a. 1 b. 2 c. 6.02 x 10^23 d. 12.04 x 10^23
B
How many neutrons are found in the nucleus of a boron-11 (11B) atom? a.11 b. 6 c. 5 d. 4
B
Hydrogen bonds form between the molecules of the hypothetical compound ABCH and do not form between DEFH molecules. Which of the following is true? a. ABCH has a higher molecular weight than DEFH. b. The chemical bonds in ABCH tend to be more polar than in DEFH. c. ABCH tends to be a compound with color, and DEFH does not have color. d. There is no significant difference between ABCH and DEFH.
B
Identify the Bronsted acids in the following reaction: HIO₃+H₂O↔H₃O⁺+IO₃⁻ a. HIO₃ b. HIO₃ and H₃O⁺ c. H₂O d. H₂O and HIO₃
B
If a sample of blood was found to have a density of 1.05 g/mL, what would be the mass of 1.000 liters of this material? Express your answer with the proper number of significant figures a. 1.05 x 10^-3 g b. 1.05 x 10^3 g c. 1050 g d. 1.050 kg
B
If you have 3.011 x 10^23 atoms of carbon, what would you expect its mass to be? a. 12.01 g b. 6.005 g c. 3.003 g d. 1.000 g
B
In the following reaction, all substances are soluble, and all dissociate except for H₂O. Identify the spectator ions a. H⁺ and OH⁻ b. K⁺ and Cl⁻ c. H⁺ and K⁺ d. Cl⁻ and OH⁻
B
Isotopes differ from each other in what way a. They have different numbers of protons in the nucleus b. they have different numbers of neutrons in the nucleus c. they have different numbers of electrons in the nucleus d. More than one response is correct
B
Naturally occurring lithium (Li) consists of only two isotopes, Li-6 (6.02 u) and Li-7 (7.02 u), where the isotopic masses are given in parentheses. Use the periodic table and determine which isotope is present in the larger percentage in the natural element. a. Li-6 b. Li-7 c. each is present at 50% d. cannot be determined from the information available
B
Nh₃ (ammonia) exhibits what type of structure? a. triangle b. pyramid with square base c. pyramid with triangular base d. none of these
B
Oxalic acid is found in many plans, like spinach and black tea. What is the mass of the carbon found in one mole of oxalic acid, H2C2O4 a. 12.01 g of C b. 24.02 g of C c. 45.01 g of C d. 90.02 g of C
B
Suppose a solution contains 200 grams of water and 15 grams of sugar. Which of the following statements is true? a. Sugar would be classified as the solvent. b. Water would be classified as the solvent. c. Either component could be classified as the solvent. d. More than one response is correct.
B
The classification of an acid or base as weak or strong is based upon a. the solubility of the acid or base b. the extent of dissociationof the acid or base c. the concentration of acid or base solution d. more than one response is correct
B
The correct formula for ammonium sulfate is_____ a.NH₄SO₄ b.(NH₄)₂SO₄ c.NH₄(SO₄)₂ d.(NH₄)₂(SO₄)₃
B
The correct formula of an ionic compound containing Al3+ and PO4 3- would be ______ a. Al₃(PO₄)₃ b. AlPO₄ c.Al₃(PO₄)₂ d.Al₂(PO₄)₃
B
The direct change from the solid state to the vapor state is called: a. evaporation b. sublimination c. boiling d. fusion
B
The ionic compound that forms between magnesium (Mg) and oxygen (O) has the formula: a. Mg2O. b. MgO. c. MgO2. d. Mg2O3.
B
The mass of an object is a. the force between the object and the earth b. a measure of the amount of matter in the object c. the amount of space the object occupies d. depends on the location of the object on earth
B
The melting of ice to liquid water is correctly classified as a. a chemical change b. a physical change c. both a chemical and a physical change d. neither a chemical nor a physical change
B
The molar concentration of OH in a water solution is 1.0 x 10⁻⁹. what is the pH of the solution? a. 5.00 b. 3.00 c. >9.00 d. <5.00
B
The prefix centi- denotes what fraction of a basic unit? a. 1/10 b. 1/100 c. 1/1000 d. 1000
B
The procedure commonly used to determine the amount of base in a solution by adding a measured quality of acid is called: a. dissociation b. titration c. ionization d. normalization
B
The radius of a K atom is ______ a Ca atom a. smaller than b. larger than c. equal to d. inverted from
B
The temperature of a liquid is decreased. What happens to the vapor pressure of the liquid as a result a. it increases b. it decreases c. it is not changed d. varies over time
B
The weight % of S in K2SO4 is _______. a. 14.2% b. 18.4% c. 54.4% d. 22.4%
B
Two pure substances A and B react to form a new pure substance C. From this, we may conclude that a. A and B are both elements b. C is a compound, A and B may or may not be elements c. C is an element, A and B are compounds d. A, B, and C are all compounds
B
What is the meaning of the two (2) in ethyl alcohol, C2H5OH? a. all the alcohol molecules contain two carbon atoms b. there are two carbon atoms per molecule of ethyl alcohol c. carbon is diatomic d. all of these are correct statements
B
What is the molarity of a solution containing 0.325 moles of solute in 250 mL of solution? a. 1.30 × 10⁻³ b. 1.30 c. 0.769 d. 8.13 × 10⁻²
B
What is the pH of a solution for which [H⁺]=1.0x10⁻³ a. 5.00 b. 3.00 c. -5.00 d. -9.00
B
What is the total pressure of a gaseous mixture that contains three gases with partial pressures of 0.845 atm, 120 torr and 210 mm Hg? a. 1175 torr b. 972 torr c. 0.411 atm d. 331 torr
B
What pressure will 3.20 mol of N2 gas exert if confined in a 15.0 L container at 100 ˚C? a. 1.75 atm b. 6.53 atm c. 3.27 atm d. 13.0 atm
B
What substance is reduced in the following reaction? 4HCl+MnO₂→Cl₂+2H₂O+MnCl₂ a. Cl in HCl b. Mn in MnO₂ c. H in HCl d. O in MnO₂
B
What type of electron is the distinguishing electron in S? a. s b. p c. d d. f
B
What would be the pH of a solution of NH₄Cl in pure water? a. higher than 7 b. lower than 7 c. equal to 7 d. can't be predicted
B
When sodium acetate dissolves in water, the following reaction occurs NaC₂H₂O₂(s)+Heat→Na⁺(aq)+C₂H₃O₂⁻(aq) The solution could be used a. in a hot pack b. in a cold pack c. either a hot pack or cold pack d. neither a hot pack or cold pack
B
When the equation below is properly balanced, what coefficient is in front of KCl? KClO₃→KCl + O₂ a. 1 b. 2 c. 3 d. 4
B
Which number has the greatest number of significant digits? a. 1.0035 b. 17.5000 c. .0000625 d. 6.022 x 10^23
B
Which of the following carries a negative charge? a. Proton b. electron c. neutron d. both proton and neutron
B
Which of the following elements has the electronic configuration 1s2-2s2-2p6-3s2-3p1 a. F b. Al c. Mg d. Ga
B
Which of the following is a double replacement reaction? a. CuO+H₂→Cu+H₂O b. HBr+KOH→H₂O+KBr c. SO₂+O₂→2SO₃ d. 2Hl→I₂+H₂
B
Which of the following is the correct valence electron configuration of phosphorus? a. b. 3s full, 3 electrons in 3p c. d.
B
Which of the following molecules would be classified as polar covalent? a. NaCl b. CH₃Cl c. KCl d. CaCl₂
B
Which of the following numbers is correctly expressed using scientific notation a. 3489 b. 5.248 x 10^4 c. 45.78 x 10^6 d. .0987 x 10^3
B
Which of the following salts would produce a basic solution (pH higher than 7) upon being dissolved in pure, distilled water? a. NaCl b. Na₂SO₃ c. Mg(NO₃)₂ d. NH₄Cl
B
Which of the following would be a polar molecule a.O₂ b. HCl c. CH₄ d. F₂
B
Which of the following would cause a calcium atom (Ca) to achieve a noble gas configuration? a. lose one electron b. lose two electrons c. gain one electron d. gain two electrons
B
Which pair of elements will be further apart in electronegativity? a. Cl and F b. Li and Cl c. Mn and Se d. U and Cs
B
_____ explains why orbitals contain a maximum of two electrons a. Hund's rule b. Pauli exclusion rule c. Periodic law d. None of these
B
a higher pH responds to: a. a higher [H+] b. a lower [H+} c. no change in [H+] d. a lower [OH-]
B
the cation (positive ion) in a salt can come from a. an acid b. a base c. either an acid or a base d. water
B
Which of the following is a weak acid a. HNO₃ b. HCl c. H₂CO₃ d. H₂SO₄
C
Which of the following mixtures would represent a buffer? a. sodium chloride/hydrochloric acid b. sodium sulfate/sulferic acid c. sodium formate/formic acid d. none of these
C
Which of the following pairs are about equal in mass? a. proton and electron b. electron and neutron c. proton and neutron d. nucleus and surrounding electrons
C
A 100 mL sample of a saturated CaSO4 solution is evaporated to dryness. The water solvent all evaporates and leaves a solid residue of CaSO4 that weighs 0.23 g. The CaSO4 would be classified as: a. insoluble in water. b. slightly soluble in water c. soluble in water d. very soluble in water.
B
A 3.2 liter sample of gas is at 40˚C and 1.0 atmosphere of pressure. If the temperature decreases to 20˚C and the pressure decreases to 0.60 atmospheres, what is the new volume in liters? a. 5.7 b. 5.0 c. 1.8 d. 0.20
B
A patient comes to you suffering from a battery acid burn (sulfuric acid). What is the best thing to use to neutralize the acid, while you continue to run cool water over the affected area? a. a 1 M sodium hydroxide solution (NaOH) b. a 1 M sodium bicarbonate solution (NaHCO3) c. a 1 M acetic acid solution (CH3COOH) d. a 1 M carbonic acid solution (H2CO3)
B
A pressure is recorded as 622 torr. What is this pressure in atm? a. 1.22 b. 0.818 c. 5.17 d. 0.0393
B
A reaction in which an acid and a base react completely, leaving only a salt and water, is referred to as a: a. hydrolysis reaction. c. oxidation reaction. b. neutralization reaction. d. none of the above
B
A solution has a pH of 8.72. What is the value of [H+]? a. 5.2 x 10⁻⁶ b. 1.0 x 10⁻⁹ c. 5.2 x 105.2 x 10⁻⁸ d. 1.9 x 10⁻⁵
B
After heating, a pure substance, A, is found to produce both B and C. What can be said about the substance A? a. it is an element b. it is a compound c. it is either an element or a compound d. impossible to predict
B
An aqueous solution is found to have a molar OH- concentration of 3.2 x 10⁻⁵. The solution would be classified as a. acidic b. basic c. neutral d. can't be classified
B
The vapor pressure of a liquid: a. decreases with increasing temperature b. is independent of temperature c. is equal to one atmosphere at the normal boiling point d. cannot be measured
C
What is the function of H₂C₆H₅O₇⁻ in the first ionization of citric acid? H₃C₆H₅O₇⁻→H⁺+H₂C₆H₅O₇⁻ a. the ion serves as an Arrhenius acid in this reaction b. the ion serves as an Arrhenius base in this reaction c. The ion serves as the conjugate base of the acid, H₃C₆H₅O₇ d. the ion serves as the conjugate acid of the base, H₃C₆H₅O₇
C
What is the maximum number of electrons that can occupy the third shell? a. 2 b. 10 c. 18 d. 32
C
What is the oxidation number of Mn in KMnO₄? a. +9 b. +5 c. +7 d. +4
C
What is the oxidizing agent in the following reaction? 4HCl+MnO₂→Cl₂+2H₂O+MnCl₂ a. Cl in HCl b. Mn in MnO₂ c. H in HCl d. O in MnO₂
C
What is the reason that U-238 is different from U-235? a. three more electrons b. three more protons c. three more neutrons d. there is no difference
C
What salt would be produced by the reaction H₂SO₄ with LiHCO₃? a. Li₂S b. LiSO₄ c. Li₂SO₄ d. Li₂CO₃
C
What volume in liters is occupied by 8.22 g of SO2 gas confined at a pressure of 1200 torr at 75.0 ˚C? a. 0.499 b. 4.22 x 101 c. 2.32 d. 32.1
C
What volume of 6.0 M HNO₃ would be needed to make 500 mL of .50 M solution? a. 6 mL b. 417 mL c. 42 mL d. 6 liters
C
What volume of a 10.00% (w/v) solution of sugar is needed to provide 2.00 g of sugar? a. 0.200 liter b. 1.00 mL c. 20.0 mL d. 5.00 mL
C
What volume of ethyl alcohol is contained in 35 mL (1 oz.) of 86 proof liquor, which is 43% (v/v) alcohol? a. 30mL b. 43mL c. 15mL d. 37mL
C
Which element has the distinguishing electron, 5p4? a. Br b. Mn c. Te d. Kr
C
Which ions in the following reaction would be classified as spectator ions? Zn+2H⁺+2Cl→Zn²⁺+2Cl⁻+H₂ a. Zn²⁺ b. H⁺ c. Cl⁻ d. more than one response is correct
C
Which of the following contains the metal with the highest oxidation number? a. CaCl₂ b. NaCl c. FeCl₃ d. CuCl₂
C
Which of the following elements is classified as a representative metal? a. element 30 b. element 26 c. element 38 d. element 63
C
Which of the following has a noble gas electronic configuration? a. Cl b. O‐ c. Br‐ d. Cl⁺
C
Which of the following is a decomposition reaction? a. SO₂+O₂→2SO₃ b. 2C₂H₂+5O₂→4CO₂+2H₂O c. 2H₂O₂→2H₂O₂+O₂ d. AgNO₃+NaCl→AgCl+NaNO₃
C
235/92U is the form of urainum used to make atomic bombs. One atom of this isotope consists of a. 92 protons, 92 electrons, 92 neutrons b. 92 protons, 143 electrons, 92 neutrons c. 92 protons, 92 electrons, 143 neutrons d. 143 protons, 143 electrons, 92 neutrons
C
A 25.00 mL sample of H₂SO₄ acid solution requires 17.35 mL of .118 M naOH for titration. What is the molarity of the acid solution? a. .0819 M b. .164 M c. .0409 M d. .236 M
C
A covalent bond results when: a. one atom gives up an electron to another atom. b. one atom gives up two electrons to another atom. c. two atoms share a pair of electrons. d. two atoms share a single electron.
C
A solution is made by dissolving a small amount of salt in a beaker of water. The water is referred to as the: a. precipitate. b. filtrate. c. solvent. d. solute.
C
Consider the reactants and propose the right side of the equation Mg + H₂SO₄ + H₂ → _____ a. no raction. b. MgHSO₄ C. MgSO₄ + H₂ D. MgH₂ + SO₄
C
Determine the molecular weight of hydrogen peroxide, H2O2 in u (or amu) a. 17.01 b. 18.02 c. 34.02 d. 33.01
C
How many equivalents are contained in .25 moles of H₂SO₄? a. .25 b. .13 c. .50 d. impossible to say
C
Identify the bronsted base(s) in the following reaction N₃⁻+H₂O↔H₃O⁺OH⁻ a. H₂O and HN₃ b. N₃⁻ c. N₃⁻ and OH⁻ d. H₂O
C
In the Bronsted theory, both acids and bases are defined in terms of how substances lose or gain: a. OH⁻ B. H₃O⁺ c. H⁺ d. Cl⁻
C
In which of the following processes does the energy of the water increase? a. water freezes b. steam condenses to liquid c. water evaporates d. more than one response is correct
C
Metalloids can express the characteristics of both metals and nonmetals. Which of the elements below is more likely to have the characteristics of a metal than a nonmetal? a. As b. Se c. Si d. Sb
C
Phosphoric acid, H₃PO₄, undergoes three acid reactions. Which of the three acids is the weakest? a. H₃PO₄ b. H₂PO₄⁻ c. HPO₄²⁻ d. more than one response is correct
C
The average relative mass of an ozone molecule is 48.0 u. An ozone molecule contains only oxygen atoms. What does this molecular weight indicate about the formula of the ozone molecule? a. it is monoatomic b. it is diatomic c. it is triatomic d. impossible to determine
C
The correct formula of an ionic compound containing Fe²⁺ and ClO₄⁻ is _______ a. FeClO₄ b. Fe₂(ClO₄)₃ c. Fe(ClO₄)₂ d. Fe₃(ClO₄)₂
C
The correct name for BaCO₃ is _____ a. barium trioxide. b. barium monocarbon trioxide. c. barium carbonate. d. barium monocarbonate.
C
The correct name for KHPO₄ is _____ a. potassium phosphate b. monopotassium phosphate c. potassium hydrogen phosphate d. KHPO₄ is not a compound
C
The highest-energy shell of an element that contains electrons is known as the ______. a. subshell b. atomic orbital c. valence shell d. none of these
C
The molar concentration of H⁺ ions in a solution is 5.9 x 10⁻⁹. What is the pH of the solution? a. 9.00 b. 5.80 c. between 8.00 and 9.00 d. between 9.00 and 10.00
C
The molecular structure of water should be: a. linear because of the electron configuration of the oxygen atom. b. trigonal planer because water contains 3 atoms. c. bent because of the non‐bonded electrons on the molecule. d. undetermined as there is no way to predict the shape of the water molecule.
C
The total number of f orbitals in an f subshell is____ a. 2 b. 5 c. 7 d. 10
C
The total number of unpaired electrons in silicon, Si, is _____ a. 0 b.1 c. 2 d. 3
C
Increasing the pressure on a gas at constant temperature does what to the volume of the gas? a.increases b.decreases c.has no effect d.increases up to a certain point
b
