ChemistrySemester I Review

Students are using heat, chemicals and

glassware in a laboratory experiment. Which of these is the best method of eye protection?

A. safety goggles B. contact lenses C. prescription eye glasses D. eye protection is not needed

Science Chemistry Unit 01: Laboratory Management

Where should a student discard solid chemical

waste? A. sink B. trash can C. disposable box D. container identified by the chemistry teacher

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

Eating in the laboratory A. is not permitted. B. is permitted if it was purchased in the

cafeteria. C. is permitted if the lab experiment does

not involve chemicals. D. is permitted as soon as the lab experiment is finished.

Safety goggles and a lab apron must be worn when handling chemicals labeled corrosive because they

A. may stain clothes B. react with the skin C. are difficult to pour D. are highly flammable

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 when working 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 open flame.

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

body infections. D. is highly corrosive and able to burn

organic material.

Which of the following is NOT considered a type of matter?

A. rockB. lightC. airD. steam

Science Chemistry Unit 02: Matter

Which of the following is NOT considered achemical property of matter? A. reactivity B. pH C. solubility D. heat of combustion

Which two features are used to describe matter?

A. mass and speed of particles B. weight and color of particles C. weight and volume D. mass and volume

Which of the following is NOT a physical property of matter?

A. viscosity B. reactivity C. texture D. density

Which state of matter is most resistant to compression?

A. solid state B. gaseous state C. liquid state D. plasma state

Definite shape and definite volume describe which state of matter?

A. liquid state B. solid state C. plasma state D. gaseous state

Material that has neither a definite shape nor a definite volume is in which state of matter?

A. gaseous state B. liquid state C. plasma state D. solid state

Which of the following is NOT a method of separating a mixture?

A. filtration B. evaporation C. melting D. chromatography

Which of the following methods involves heating or boiling a mixture to recover the solid elements?

A. evaporation B. distillation C. chromatography D. filtration

An increase in which of the following would increase the boiling point of a liquid?

A. volume B. the mass of the liquid C. pressure D. temperature

Which of the following is correct statement regarding mixtures?

A. mixtures are composed of a single substance

B. mixtures are composed of more than one substance

C. mixtures have a fixed composition

D. all substances in a mixture are visible at all times

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

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 A B. Cereal B C. Cereal C D. Cereal D

A student measures the mass of an object as 32.4g. The actual mass of the object is 31.8 g. What is the percent error of the student's measurement?

A. 0.060% B. 1.01% C. 1.85 % D. 60.0%

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.

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 crystal

B. See if the crystals will dissolve in water

C. Find the crystal's melting point D. Use a ruler and balance to

measure the crystals

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.

The cathode ray experiments lead to whichparticle being discovered? A. nucleus B. proton C. neutron D. electron

The proton, in Rutherford’s experiments, were used to —

A. identify chemical properties B. identify the melting point C. determine molecular mass D. bombard sheets of gold

Which nuclear particle has the same relativemass as the proton, but has no electrical

charge? A. electron B. neutron C. isotope D. quark

Why is an atom considered electrically neutral?

A. neutrons equal the number of protons

B. proton forces pull on the neutrons C. electrons equal the number of

protons D. electrons equal the number of

neutrons

Which of the following statements describesisotopes of an atom? A. different chemical properties B. different numbers of protons C. different masses D. different numbers of electrons

What happens to the number of electrons in an

atom as the atomic number on the periodictable increases? A. increases B. decreases C. remains the same D. depends on the atom

Which of the following is used to calculate theaverage atomic mass of an element? A. the naturally occurring isotopes B. the five most abundant isotopes C. the isotopes that are man made D. the least most common isotopes

What is the mass number of a carbon isotopethat consists of 6 protons, 6 electrons, and 8neutrons? A. 13 B. 14 C. 20 D. 28

Which of the following showed electrons inspecific, fixed orbits? A. Rutherford Model B. Planck Model C. Bohr Model D. Quantum Model

Which orbitals are dumbbell-shaped and arearranged along the x, y, and z axes? A. s orbitals B. d orbitals C. p orbitals D. f orbitals

Which of the following orbitals containsquantum number combinations that are NOTpossible? A. 4d B. 3s C. 4p D. 3f

How many electrons are required to completely fill the 3rd energy level?

A. 0 B. 8 C. 18 D. 32

An electron must occupy the lowest availableenergy orbital is stated by — A. the Aufbrau Principle B. Hund's Rule C. the Pauli Exclusion Principle D. Bohr's Law

What is the electron configuration for manganese, atomic number 25?

A. 1s2 2s2 2p6 3s2 3p6 4s2 3d5

B. 1s2 2s2 2p6 3s2 3p6 4s2 3d10

C. 1s2 2s2 2p6 3s2 3p6 4s2

D. 1s2 2s2 2p6 3s2 3p6

The properties of elements, according toperiodic law, can be predicted by — A. the number of isotopes B. the solubility of the element C. the position on the periodic table D. the color of the element

Which family correctly labels the elements inGroup 1 on the periodic table? A. transition metals B. alkali series C. lanthanide elements D. actinide series

As the atomic number increases, within agroup of elements, the atomic radius usually

— A. decreases B. remains the same as the one above it C. increases D. decreases, then increases

What happens to the ionization energy of anelement as electrons are removed? A. increases B. decreases C. remains constant D. decreases, then increases

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 been discovered. B. Atomic mass is unaffected by chemical reactions. C. Atomic number is more closely related to reactivity. D. Atomic mass varies among the isotopes of an element.

Which of the following groups, with a fewexceptions, has the d-orbitals unfilled? A. transition metals B. nonmetals C. gases D. metalloids

Science Chemistry Unit 04: Chemical Bonding

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.

The number of valence electrons in Group 2elements is — A. 0 B. 1 C. 2 D. 3

Which of the following are involved in forming a chemical bond?

A. electrons and protons B. protons and neutrons C. neutrons and electrons D. dipoles and electrons

What happens to the potential energy of atoms

when they form a chemical bond? A. increase their potential energy B. decrease their potential energy C. their potential energy remains the

same D. their potential energy fluctuates

over time

When 2 atoms share a pair of electrons, which

type of bond is formed? A. ionic B. sublevel C. static D. covalent

The unequal attraction for the electrons in achemical bond is called — A. nonpolar B. polar C. triplanar D. ionic

Which of the following increases as theelectronegativity difference between 2 atomsincreases? A. ionic nature of the bond B. covalent nature of the bond C. metallic nature of the bond D. electron sharing between the 2

atoms

Which of the the 2 outermost orbitals must be filled to satisfy the octet rule?

A. d and f orbitals B. d and p orbitals C. s and d orbitals D. s and p orbitals

Which of the following is used to draw a Lewis structure of either a molecule or atom?

A. bond length between 2 atoms B. electronegativity of an atom C. number of valence electrons D. atomic mass or masses

How many double bonds are in the Lewisstructure for carbon dioxide, CO2? A. none B. one C. two D. three

O C O for carbon to have 8 valence electrons it will have to have two pairs on each side sharing with oxygen

Which of the following is a property of amolecular compound? A. low boiling point B. tend to be brittle C. conducts electricity well when dissolved D. hardness

The attraction between positive ions andsurrounding mobile electrons forms which

type of bond? A. polar covalent bond B. nonpolar covalent bond C. ionic bond D. metallic bond

What happens to electron pairs, according toVSEPR, 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.

According to the VSEPR theory, which shaperepresents a carbon tetrafluoride molecule,

CF4? A. tetrahedral B. trigonal planar C. bent D. linear

Which of the following has the greatest affecton the strength of London dispersion forcesbetween molecules? A. the number of electrons B. the number of protons and neutrons in the molecule C. the number of electrons and the

number of neutrons in the molecule D. the number of electrons in the

molecule and the mass of the molecule

Which statement is true regarding the strengthof 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.

Oxygen forms covalent bonds with carbon andsulfur, 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.

Assuming an element has 8 electrons in thevalence shell, what conclusions can be drawnregarding 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.

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.

How many atoms of carbon are present in amolecule of carbon tetrachloride, CCl4? A. 1 B. 2 C. 4 D. 5

Science Chemistry Unit 05: Chemical Formulas

Changing the subscript on an element within a

correctly written chemical formula — A. changes the charges of all the other

ions in the compound B. changes the number of ions

represented by the formula C. changes the oxidation number of

each element in the formula D. changes the formula so that it no

longer represents that compound

What is the formula for potassium fluoride? A. KF B. KF2

C. K2F D. K2F2

What is the formula for the compound formedby iron (II) ions and chromate ions? A. FeCrO4

B. Fe2CrO4

C. Fe2(CrO4)3

D. Fe(CrO4)2

What is the formula for aluminum hydroxide? A. AlOH B. Al(OH)3

C. Al2(OH)3

D. Al3OH

What is the formula for tin (IV) oxide? A. Tn4O2

B. SnO C. TnO2

D. SnO2

What is the formula for barium nitrate? A. Ba(NO3)2

B. BaNO2

C. Ba2NO3

D. Ba(NO4)2

What is the name of the compound NiSO4 ? A. nickel (II) sulfite B. nickel (II) sulfide C. nickel (II) sulfate D. nickel (II) sulfuroxide

What is the name of the compound AlPO4? A. aluminum phosphide B. aluminum phosphate C. aluminum phosphite D. aluminum phosphoroxide

Which of the following is the metallic ion inscandium (II) chloride? A. Sd 2+

B. Cl 2-

C. Sc 2+

D. Cl 1-

What is the name of the compound N2O3? A. sodium dioxide B. dinitrogen oxide C. nitrous oxide D. dinitrogen trioxide

What is the formula for sulfur trioxide? A. SO B. SO2

C. SO3

D. SrO3

What is the oxidation number of nitrogen inmost compounds? A. -3 B. -2 C. -1 D. +1

What is the oxidation number of hydrogen inHCl? A. 0 B. +1 C. +2 D. +3

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 Mass B. Atomic Law C. Multiple Proportions D. Definite Composition

Which of the following is a possible compound formed from Calcium (2+) and the polyatomic ion Nitrate, NO3 (1-)?

A. Ca2NO3

B. Ca3NO2

C. CaNO D. Ca(NO3)2

Science Chemistry Unit 06: Mole Theory

How many grams of NaCl are present in 11.00

moles? A. 0.45 g B. 156.60 g C. 331.00 g D. 642.93 g

11.0 moles x 58.5g/mole =

How many Mg 2+ ions are present in3.00 moles of MgCl2? A. 1.806 x 1024

B. 3.02 x 1024

C. 12.00 x 1025

D. 16.00 x 1023

3.00 moles x 6.02 x 1023 molecules/mole x 1Mg/molecule

Which of the following is the scientific namefor NH3 ? A. Water B. Ammonia C. Nitric acid D. Methane

What is the formula mass of MgSO4? A. 116.13 amu B. 272.83 amu C. 111.21 amu D. 120.36 amu

Mg = 1 x 24.31= 24.31 S = 1 x 32.06 = 32.06 O = 4 x 15.999= 63.99

The mass of one _________ is the molar mass of the element.

A. mole of the element B. picogram of the element C. milliliter of the element D. representative particle of the

element

The sum of the atomic masses of all the atoms

in a formula for a compound is the— A. real mass B. formula mass C. Avogadro mass D. molecule mass

What is the formula mass of sodium chloride,NaCl? A. 53.023 amu B. 58.439 amu C. 102.771 amu D. 112.539 amu

Na = 1 x 22.99 amuCl = 1 x 35.45 amu

What is the formula mass of glucose,C6H12O6? A. 58.347 amu B. 137.490 amu C. 180.017 amu D. 231.369 amu

Describe the process of calculating the molarmass 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.

How many moles of CO2 are present in 200.00 g?

A. .22 mol B. 4.54 mol C. 9.08 mol D. 88.02 mol

200g CO2 x 1 mole CO2/44g CO2

Calculate the number of representative particles that are present in .20 moles of H2O without regards to significant figures.

A. 3.612x 1023 atoms B. 1.204 x 1024 atoms C. 2.408 x 1024 atoms D. 2.944 x 1025 atoms

.20 moles x 6.02 x 1023 H20/1mole x 3rp/1H20

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 data B. Throw out this data C. Redo the experiment D. Change your hypothesis

If the average mass of a one pound bag ofSkittles is 453.6 g and there are 927 Skittles

ina bag, determine which best represents the

mass of one Skittle. A. 489.3 mg B. 4893 mg C. 2.044 g D. 204.4 mg

Which of the following is the mass in grams of 4.25 × 10³ mol of N2

A. 2.35 × 10-4 g B. 1.52 × 102 g C. 5.95 × 104 g D. 1.19 × 105 g (4.25 × 10³ mol of N2) x (28.012g/ 1 mol N2)

After the correct formula for a reactant in anequation has been written, the — A. chemical formula cannot be altered B. subscripts of the formula are changed

to balance the equation C. chemical symbols in the formula must

appear only on the reactant side D. same chemical formula must be written

on the product side of the equation

Science Chemistry Unit 07: Chemical Equations andReactions

Which of the following reactions involves twoor more substances combining to form a newcompound? A. single-replacement reaction B. synthesis reaction C. combustion reaction D. double-replacement reaction

Which of the following reactions involves oneelement replacing an element in a compoundthat is from the same activity series? A. combustion reaction B. decomposition reaction C. single-replacement reaction D. double-replacement reaction

Which of the following reactions involves asingle compound producing two or more

simpler substances? A. synthesis reaction B. decomposition reaction C. combustion reaction D. double-replacement reaction

Which of the following reactions involves theions of two compounds exchanging places toform two new compounds? A. synthesis reaction B. single-replacement reaction C. double-replacement reaction D. combustion reaction

By predicting the outcome of the followingreactants mixing together in an aqueoussolution, what type of reaction will take

place? Pb(NO3)2 (aq) + 2 KI (aq) --> A. double-replacement reaction B. synthesis reaction C. decomposition reaction D. single-replacement reaction

When an acid, such as carbonic acid, decomposes, the products are —

A. non-metal oxides and a salt B. non-metal oxides and water C. metal oxides and oxygen D. metal oxides and peroxide

Predict the products of the following reaction:Na2O + CO2 --> A. Na2CO3

B. Na + CO3

C. NaCO2 + O2

D. NaC + O3

Typically a synthesis reaction will occur that is balanced

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.

Predict the outcome of the reaction where zincmetal 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

Predict the outcome of the reaction where asolution of silver nitrate is added to a solutionof sodium chloride. A. No reaction occurs B. Silver chloride forms C. Nitric acid is produced D. Calcium chloride is formed

In the solubility chart silver is insoluble in chlorine so a precipitate will form. Nitrate is soluble with sodium

According to the Law of Conservation ofMatter, the total mass of all the reactingSubstance is — A. more than the mass of all the

products B. more than the total mass of all the

products and the reactants C. less than the total mass of all the

products D. equal to the mass of all the products

What are the coefficients that would correctlybalance this reaction?____Ni + ____C4H8N2O2 --> ____Ni(C4H8N2O2)2

A. 1, 2, 1 B. 2, 2, 1 C. 2, 1, 1 D. 2, 2, 2

What are the coefficients that would correctlybalance this equation?____Zn + ____K2CrO4 -->____K + ____ZnCrO4

A. 2, 1, 2, 1 B. 1, 2, 3, 1 C. 1, 2, 1, 2 D. 1, 1, 2, 1

What is the balanced equation for thecombustion 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) --> MgO4

First the product must be balanced = MgO

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.

The safest way to dilute concentratedhydrochloric acid is to add - A. a series of small volumes of water to

the acid while stirring slowly B. the acid to water slowly while

stirring constantly C. the acid to a small volume of water

and then add more water D. dilute hydrochloric acid to a small

volume of the concentrated acid