2 Science Chemistry Unit 01: Laboratory Management Students are using heat, chemicals andglassware in a laboratory experiment. Which of these is the best method of eye protection?A. safety gogglesB. contact lensesC. prescription eye glassesD. eye protection is not needed
3 Where should a student discard solid chemical waste?A. sinkB. trash canC. disposable boxD. container identified by the chemistry teacher
4 What should be used to put out a fire in person’s hair or clothing?A. your handsB. a fire blanketC. a fire extinguisherD. water from the sink faucet
5 Eating in the laboratory A. is not permitted.B. is permitted if it was purchased in thecafeteria.C. is permitted if the lab experiment doesnot involve chemicals.D. is permitted as soon as the labexperiment is finished.
6 Safety goggles and a lab apron must be worn when handling chemicals labeled corrosive because they A. may stain clothesB. react with the skinC. are difficult to pourD. are highly flammable
7 This hazardous materials symbol indicates that the chemicals stored in that container are highly reactive.Which of the following procedures should be taken when dealing with the chemical?A. Always use safety goggles whenworking with this chemical.B. Always leave the container sealed,never open it.C. Always keep water nearby in case of spills.D. Always keep this chemical away from openflame.
8 This hazardous materials symbol indicates that the chemical in the container with this symbol A. is flammable and combustible.B. is poisonous and infectious.C. is biohazardous and can produce bodyinfections.D. is highly corrosive and able to burn organic material.
9 Science Chemistry Unit 02: Matter Which of the following is NOT considered a type of matter?A. rockB. lightC. airD. steam
10 Which of the following is NOT considered a chemical property of matter?A. reactivityB. pHC. solubilityD. heat of combustion
11 Which two features are used to describe matter? A. mass and speed of particlesB. weight and color of particlesC. weight and volumeD. mass and volume
12 Which of the following is NOT a physical property of matter? A. viscosityB. reactivityC. textureD. density
13 Which state of matter is most resistant to compression? A. solid stateB. gaseous stateC. liquid stateD. plasma state
14 Definite shape and definite volume describe which state of matter? A. liquid stateB. solid stateC. plasma stateD. gaseous state
15 Material that has neither a definite shape nor a definite volume is in which state of matter? A. gaseous stateB. liquid stateC. plasma stateD. solid state
16 Which of the following is NOT a method of separating a mixture? A. filtrationB. evaporationC. meltingD. chromatography
17 Which of the following methods involves heating or boiling a mixture to recover the solid elements? A. evaporationB. distillationC. chromatographyD. filtration
18 An increase in which of the following would increase the boiling point of a liquid? A. volumeB. the mass of the liquidC. pressureD. temperature
19 Which of the following is correct statement regarding mixtures? A. mixtures are composed of a single substanceB. mixtures are composed of more than one substanceC. mixtures have a fixed compositionD. all substances in a mixture are visible at all times
20 Solid sodium chloride has a crystal structure. Which of the following best explains why some solids can form crystals?A. Particles experience strong intermolecular forces, causing them to be held in very orderly positions.B. Particles spread out and mix with each other, even if they are not stirred, making crystal formation more likely.C. Particles experience strong intermolecular forces, but can still move about freely and are not bound to fixed positions.D. Particles are very closed together and, therefore, barely compress at all, making them predisposed to form crystals
21 Breakfast Cereal A costs $4. 99 for 793 g, Cereal B costs $3 Breakfast Cereal A costs $4.99 for 793 g, Cereal B costs $3.79 for 400 g, Cereal C costs $4.19 for 1.19 kg, and Cereal D costs $3.99 for 567 g. Which cereal has the lowest price per gram?A. Cereal AB. Cereal BC. Cereal CD. Cereal D
22 A student measures the mass of an object as 32. 4g A student measures the mass of an object as 32.4g. The actual mass of the object is g. What is the percent error of the student's measurement?A %B. 1.01%C %D. 60.0%
23 If you wanted to separate a mixture of isopropyl alcohol and water, what example below would help you select the technique you should use?A. The boiling point is 82ºC.B. The mixture is clear.C. The water was tap water.D. 8 oz of alcohol was added to 8 oz of water.
24 A student is trying to identify an unknown white crystalline solid made of small grains. The student believes these are sugar crystals. How should the student test this hypothesis?A. Identify the particle pattern in the crystalB. See if the crystals will dissolve in waterC. Find the crystal's melting pointD. Use a ruler and balance to measure the crystals
25 Science Chemistry Unit 03: Atomic Structure and the Periodic Table Which of the following statements is most accurate regarding atoms?A. Most atoms cannot combine with other atoms.B. Chemical reactions divide atoms into smaller units.C. Atoms of the same element may have different mass numbers.D. Atoms only contain protons.
26 The cathode ray experiments lead to which particle being discovered?A. nucleusB. protonC. neutronD. electron
27 The proton, in Rutherford’s experiments, were used to — A. identify chemical propertiesB. identify the melting pointC. determine molecular massD. bombard sheets of gold
28 Which nuclear particle has the same relative mass as the proton, but has no electrical charge?A. electronB. neutronC. isotopeD. quark
29 Why is an atom considered electrically neutral? A. neutrons equal the number of protonsB. proton forces pull on the neutronsC. electrons equal the number of protonsD. electrons equal the number of neutrons
30 Which of the following statements describes isotopes of an atom?A. different chemical propertiesB. different numbers of protonsC. different massesD. different numbers of electrons
31 What happens to the number of electrons in an atom as the atomic number on the periodictable increases?A. increasesB. decreasesC. remains the sameD. depends on the atom
32 Which of the following is used to calculate the average atomic mass of an element?A. the naturally occurring isotopesB. the five most abundant isotopesC. the isotopes that are man madeD. the least most common isotopes
33 What is the mass number of a carbon isotope that consists of 6 protons, 6 electrons, and 8neutrons?A. 13B. 14C. 20D. 28
34 Which of the following showed electrons in specific, fixed orbits?A. Rutherford ModelB. Planck ModelC. Bohr ModelD. Quantum Model
35 Which orbitals are dumbbell-shaped and are arranged along the x, y, and z axes?A. s orbitalsB. d orbitalsC. p orbitalsD. f orbitals
36 Which of the following orbitals contains quantum number combinations that are NOTpossible?A. 4dB. 3sC. 4pD. 3f
37 How many electrons are required to completely fill the 3rd energy level? B. 8C. 18D. 32
38 An electron must occupy the lowest available energy orbital is stated by —A. the Aufbrau PrincipleB. Hund's RuleC. the Pauli Exclusion PrincipleD. Bohr's Law
39 What is the electron configuration for manganese, atomic number 25? A. 1s2 2s2 2p6 3s2 3p6 4s2 3d5B. 1s2 2s2 2p6 3s2 3p6 4s2 3d10C. 1s2 2s2 2p6 3s2 3p6 4s2D. 1s2 2s2 2p6 3s2 3p6
40 The properties of elements, according to periodic law, can be predicted by —A. the number of isotopesB. the solubility of the elementC. the position on the periodic tableD. the color of the element
41 Which family correctly labels the elements in Group 1 on the periodic table?A. transition metalsB. alkali seriesC. lanthanide elementsD. actinide series
42 As the atomic number increases, within a group of elements, the atomic radius usually —A. decreasesB. remains the same as the one above itC. increasesD. decreases, then increases
43 What happens to the ionization energy of an element as electrons are removed?A. increasesB. decreasesC. remains constantD. decreases, then increases
44 Which of the following best explains why Mendeleev's periodic table was organized according to atomic mass rather than atomic number?A. Atomic number had not yet beendiscovered.B. Atomic mass is unaffected bychemical reactions.C. Atomic number is more closely relatedto reactivity.D. Atomic mass varies among theisotopes of an element.
45 Science Chemistry Unit 04: Chemical Bonding Which of the following groups, with a fewexceptions, has the d-orbitals unfilled?A. transition metalsB. nonmetalsC. gasesD. metalloids
46 Which of the following describes the properties of noble gases? A. They have high boiling points.B. They are highly reactive.C. They are generally unreactive.D. They are solid at room temperature.
47 The number of valence electrons in Group 2 elements is —A. 0B. 1C. 2D. 3
48 Which of the following are involved in forming a chemical bond? A. electrons and protonsB. protons and neutronsC. neutrons and electronsD. dipoles and electrons
49 What happens to the potential energy of atoms when they form a chemical bond?A. increase their potential energyB. decrease their potential energyC. their potential energy remains the sameD. their potential energy fluctuates over time
50 When 2 atoms share a pair of electrons, which type of bond is formed?A. ionicB. sublevelC. staticD. covalent
51 The unequal attraction for the electrons in a chemical bond is called —A. nonpolarB. polarC. triplanarD. ionic
52 Which of the following increases as the electronegativity difference between 2 atomsincreases?A. ionic nature of the bondB. covalent nature of the bondC. metallic nature of the bondD. electron sharing between the 2 atoms
53 Which of the the 2 outermost orbitals must be filled to satisfy the octet rule? A. d and f orbitalsB. d and p orbitalsC. s and d orbitalsD. s and p orbitals
54 Which of the following is used to draw a Lewis structure of either a molecule or atom? A. bond length between 2 atomsB. electronegativity of an atomC. number of valence electronsD. atomic mass or masses
55 How many double bonds are in the Lewis structure for carbon dioxide, CO2?A. noneB. oneC. twoD. threeO C O for carbon to have 8 valence electrons it will have to have two pairs on each side sharing with oxygen
56 Which of the following is a property of a molecular compound?A. low boiling pointB. tend to be brittleC. conducts electricity well whendissolvedD. hardness
57 The attraction between positive ions and surrounding mobile electrons forms which type of bond?A. polar covalent bondB. nonpolar covalent bondC. ionic bondD. metallic bond
58 What happens to electron pairs, according to VSEPR, when a molecule is formed?A. Electron pairs form negative ions.B. Electron pairs form positive ions.C. Electron pairs cause molecules to attract each other to form electrostatic positions.D. Electrons pairs move away from each other to electrostatic balanced positions.
59 According to the VSEPR theory, which shape represents a carbon tetrafluoride molecule, CF4?A. tetrahedralB. trigonal planarC. bentD. linear
60 Which of the following has the greatest affect on the strength of London dispersion forcesbetween molecules?A. the number of electronsB. the number of protons and neutrons inthe moleculeC. the number of electrons and the number of neutrons in the moleculeD. the number of electrons in the molecule and the mass of the molecule
61 Which statement is true regarding the strength of molecular bonds compared to the strengthof intermolecular forces?A. Molecular bonds tend to be weaker.B. Molecular bonds tend to be stronger.C. Intermolecular bonds tend to be stronger.D. The bond strengths are about the same.
62 Oxygen forms covalent bonds with carbon and sulfur, but forms ionic bonds with sodium andmagnesium. What is the best inference for this difference in how oxygen behaves?A. Oxygen bonds randomly with elements in unpredictable ways.B. The difference in atomic radii between the groups accounts for the difference in behavior.C. Oxygen only bonds with elements that have a smaller atomic mass.D. Electronegativity differences between the bonding elements allow electrons to be either shared or donated.
63 Assuming an element has 8 electrons in the valence shell, what conclusions can be drawn regarding the type of bonding behavior? A. The element will form polar covalent bonds. B. The element will form non-polar covalent bonds. C. The element will form ionic bonds. D. The element will form no bonds.
64 Which statement is true comparing the research of Bohr, Rutherford, and Dalton? A. Dalton and Bohr modeled their experiments and their theories after Rutherford.B. Rutherford and Bohr modeled their experiments and their theories after Dalton.C. Dalton and Rutherford modeled their experiments and their theories after Bohr.D. All three scientists developed their theories at the same time.
65 Science Chemistry Unit 05: Chemical Formulas How many atoms of carbon are present in amolecule of carbon tetrachloride, CCl4?A. 1B. 2C. 4D. 5
66 Changing the subscript on an element within a correctly written chemical formula —A. changes the charges of all the other ions in the compoundB. changes the number of ions represented by the formulaC. changes the oxidation number of eachelement in the formulaD. changes the formula so that it no longer represents that compound
67 What is the formula for potassium fluoride? A. KFB. KF2C. K2FD. K2F2
68 What is the formula for the compound formed by iron (II) ions and chromate ions?A. FeCrO4B. Fe2CrO4C. Fe2(CrO4)3D. Fe(CrO4)2
69 What is the formula for aluminum hydroxide? A. AlOHB. Al(OH)3C. Al2(OH)3D. Al3OH
70 What is the formula for tin (IV) oxide? A. Tn4O2B. SnOC. TnO2D. SnO2
71 What is the formula for barium nitrate? A. Ba(NO3)2B. BaNO2C. Ba2NO3D. Ba(NO4)2
72 What is the name of the compound NiSO4 ? A. nickel (II) sulfiteB. nickel (II) sulfideC. nickel (II) sulfateD. nickel (II) sulfuroxide
73 What is the name of the compound AlPO4? A. aluminum phosphideB. aluminum phosphateC. aluminum phosphiteD. aluminum phosphoroxide
74 Which of the following is the metallic ion in scandium (II) chloride?A. Sd 2+B. Cl 2-C. Sc 2+D. Cl 1-
75 What is the name of the compound N2O3? A. sodium dioxideB. dinitrogen oxideC. nitrous oxideD. dinitrogen trioxide
76 What is the formula for sulfur trioxide? A. SOB. SO2C. SO3D. SrO3
77 What is the oxidation number of nitrogen in most compounds?A. -3B. -2C. -1D. +1
78 What is the oxidation number of hydrogen in HCl?A. 0B. +1C. +2D. +3
79 Which law states that "when two or more compounds are composed of the same two elements, the ratio of the masses of one element that combine with a fixed mass of the other element is a simple whole number"?A. Conservation of MassB. Atomic LawC. Multiple ProportionsD. Definite Composition
80 Which of the following is a possible compound formed from Calcium (2+) and the polyatomic ion Nitrate, NO3 (1-)?A. Ca2NO3B. Ca3NO2C. CaNOD. Ca(NO3)2
81 Science Chemistry Unit 06: Mole Theory How many grams of NaCl are present in 11.00moles?A gB gC gD g11.0 moles x 58.5g/mole =
82 How many Mg 2+ ions are present in 3.00 moles of MgCl2? A x 1024B x 1024C x 1025D x 10233.00 moles x 6.02 x 1023 molecules/mole x 1Mg/molecule
83 Which of the following is the scientific name for NH3 ?A. WaterB. AmmoniaC. Nitric acidD. Methane
84 What is the formula mass of MgSO4? A amuB amuC amuD amuMg = 1 x 24.31= 24.31S = 1 x = 32.06O = 4 x =
85 The mass of one _________ is the molar mass of the element. A. mole of the elementB. picogram of the elementC. milliliter of the elementD. representative particle of the element
86 The sum of the atomic masses of all the atoms in a formula for a compound is the—A. real massB. formula massC. Avogadro massD. molecule mass
87 What is the formula mass of sodium chloride, NaCl?A amuB amuC amuD amuNa = 1 x amuCl = 1 x amu
88 What is the formula mass of glucose, C6H12O6?A amuB amuC amuD amu
89 Describe the process of calculating the molar mass of Li2S.A. Add the masses of 1 mole of lithium and 2 moles of sulfur.B. Add the masses of 1 mole of lithium and 1 mole of sulfur.C. Add the masses of 2 moles of lithium and 1 mole of sulfur.D. Add the masses of 2 moles of lithium and 2 moles of sulfur.
90 How many moles of CO2 are present in 200.00 g? A. .22 molB molC molD mol200g CO2 x 1 mole CO2/44g CO2
91 Calculate the number of representative particles that are present in Calculate the number of representative particles that are present in .20 moles of H2O without regards to significant figures.A x 1023 atomsB x 1024 atomsC x 1024 atomsD x 1025 atoms.20 moles x 6.02 x 1023 H20/1mole x 3rp/1H20
92 You are performing an experiment to determine whether the "S" on Skittles dissolves faster in cold water, warm water or hot water. In 9 out 10 trials the data indicates that the "S" dissolves faster in hot water. "S“ dissolves in warm water faster than hot water. What should you do?A. Report this dataB. Throw out this dataC. Redo the experimentD. Change your hypothesis
93 If the average mass of a one pound bag of Skittles is g and there are 927 Skittles ina bag, determine which best represents the mass of one Skittle.A mgB mgC gD mg
94 Which of the following is the mass in grams of 4.25 × 10³ mol of N2 A × 10-4 gB × 102 gC × 104 gD × 105 g(4.25 × 10³ mol of N2) x (28.012g/ 1 mol N2)
95 Science Chemistry Unit 07: Chemical Equations and Reactions After the correct formula for a reactant in anequation has been written, the —A. chemical formula cannot be alteredB. subscripts of the formula are changed to balance the equationC. chemical symbols in the formula must appear only on the reactant sideD. same chemical formula must be written on the product side of the equation
96 Which of the following reactions involves two or more substances combining to form a newcompound?A. single-replacement reactionB. synthesis reactionC. combustion reactionD. double-replacement reaction
97 Which of the following reactions involves one element replacing an element in a compoundthat is from the same activity series?A. combustion reactionB. decomposition reactionC. single-replacement reactionD. double-replacement reaction
98 Which of the following reactions involves a single compound producing two or more simpler substances?A. synthesis reactionB. decomposition reactionC. combustion reactionD. double-replacement reaction
99 Which of the following reactions involves the ions of two compounds exchanging places toform two new compounds?A. synthesis reactionB. single-replacement reactionC. double-replacement reactionD. combustion reaction
100 By predicting the outcome of the following reactants mixing together in an aqueoussolution, what type of reaction will take place?Pb(NO3)2 (aq) + 2 KI (aq) -->A. double-replacement reactionB. synthesis reactionC. decomposition reactionD. single-replacement reaction
101 When an acid, such as carbonic acid, decomposes, the products are — A. non-metal oxides and a saltB. non-metal oxides and waterC. metal oxides and oxygenD. metal oxides and peroxide
102 Predict the products of the following reaction: Na2O + CO2 -->A. Na2CO3B. Na + CO3C. NaCO2 + O2D. NaC + O3Typically a synthesis reaction will occur that is balanced
103 What are the advantages of using an activity series in predicting the outcome of chemical reactions? A. The freezing point of the elements can be determined.B. Reactions can be categorized as either exothermic or endothermic.C. The ionization energy can be calculated for each element in the reaction.D. The reaction can be categorized as possible or not possible.
104 Predict the outcome of the reaction where zinc metal is added to a solution of potassiumchloride.A. No reaction occurs.B. Gaseous zinc is formed.C. Potassium calcide forms.D. Zinc chloride forms.Zinc is below Potassium on the reactivity series chart
105 Predict the outcome of the reaction where a solution of silver nitrate is added to a solutionof sodium chloride.A. No reaction occursB. Silver chloride formsC. Nitric acid is producedD. Calcium chloride is formedIn the solubility chart silver is insoluble in chlorine so a precipitate will form. Nitrate is soluble with sodium
106 According to the Law of Conservation of Matter, the total mass of all the reactingSubstance is —A. more than the mass of all the productsB. more than the total mass of all the products and the reactantsC. less than the total mass of all the productsD. equal to the mass of all the products
107 What are the coefficients that would correctly balance this reaction?____Ni + ____C4H8N2O2 --> ____Ni(C4H8N2O2)2A. 1, 2, 1B. 2, 2, 1C. 2, 1, 1D. 2, 2, 2
108 What are the coefficients that would correctly balance this equation?____Zn + ____K2CrO4 -->____K + ____ZnCrO4A. 2, 1, 2, 1B. 1, 2, 3, 1C. 1, 2, 1, 2D. 1, 1, 2, 1
109 What is the balanced equation for the combustion of magnesium?A. Mg (s) + O2 (g) --> MgO (g)B. Mg (s) + O2 (g) --> MgO2 (g)C. 2 Mg (s) + O2 (g) --> 2 MgO (s)D. Mg (s) + 2 O2 (g) --> MgO4First the product must be balanced = MgO
110 Lavoisier used a variety of experiments to draw conclusions regarding the chemical reactivity of a number of elements. Critique the following statements and select the statement that was determined later to be false.A. Water is formed from a reaction of hydrogen (what he called phlogiston) and oxygen.B. Sulfur, when burned, combines with air to form new substances.C. Oxygen makes some substances acidic.D. The weight gained by the products of a burning reaction came from the air.
111 The safest way to dilute concentrated hydrochloric acid is to add -A. a series of small volumes of water to the acid while stirring slowlyB. the acid to water slowly while stirring constantlyC. the acid to a small volume of water and then add more waterD. dilute hydrochloric acid to a small volume of the concentrated acid