mid term review 2010

8/3/2019 Mid Term Review 2010

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HONORS CHEMISTRY MID-TERM REVIEWAllen; January

This is the material from our first test:Chapter 1: Section 1.1 and 1.3

Definition of Chemistry Five types of Chemistry Scientific Method

Chapter 2: Section 2.1, 2.2, and 2.3 What is matter? States of matter Mixtures Elements and Compounds

Chapter 3: All Sections Accuracy, precision, uncertainty, and significant figures SI system of units Dimensional Analysis Density

You should be able to:

LJNrr 2: Scientific Method and Problem SolvingI. Differentiate between quantitative and qualitativeobservations and interpretations.2. Differentiate between the accuracy and precision of ameasurement.3. Identif the number of significant figures in ameasurement1. Appropriately use measurement tools in thelaboratoay.2. Record measurements to the correct number ofsignificant figures, with the correct uncertaintyvalue, and with the correct label.3. Us e the rules for significant figures in calculationsto correctly round off numbers and performaddition, subtraction, multiplication and division.4. Use the uncertainty in recorded measurements tocorrectly report uncertainty in a calculation usingthose measurements.5. Calculate % error in a determined value.


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4. Identify the metric units of length, mass, time andvolume.5. Differentiate between basic and derived units.6. Identify the common metric prefixes and convertmeasurements with in the metric system. .6. Use a decimeter cube to explam why the milli literand cubic centimeter have the same volume.

7. Differentiate between mass and the weight of an object8. Differentiate between density and specific gravity. 7. Calculate the density of an object fromexperimental data.8. Convert between the Celsius and Kelvin

temperature scales.9. Find the mass, volume or density of a substancewhen any two of these values are known.10. Construct conversion factors from equivalentmeasurementS.11. Apply the techniques of dimensional analysis to avariety of conversion problems.12. Use dimensional analysis to solve multi-stepproblems.

UNIT 3: Introduction to Matter, Change, and Energy1. Define chemistry and discuss the various

branches of chemistry. 1. Show how the terms experiment, hypothesis,theory, and law fit into the scientific method.2. Differentiate between matter and pure

substance.3. Identify the four states ofmatter.4. Characterize the solid, liquid, and gas phases of

matter. 2. Classify matter as a pure substance or a mixture.3. Further classify matter as homogeneous or

heterogeneous.5. State the difference between an element an

d acompound

6. Write the symbols and names of commonelements, given one or the other. 4. Distinguish between potential and kinetic

energy, and provide an example of energyconversion.

7. State the law of conservation of energy. 5. Classify changes in matter as physical orchemical changes.

8. Define a chemical reaction.9. State the law of conservation ofmass. 6. Interpret experimental results, based on the law

of conservation ofmass.


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This is the material from our second test:Chapter 4: Sec tion 4.1-4.3

Five atomic theories Subatomic particles of the atom Atomic Number, Mass Number, Isotopes Atomic Mass (what it is; how to calculate)

Chapter 25 : Section 25.1 -25.4 Radioactivity Seven types of Radioactive Decay

-Alpha-Beta-Gamma-Positron Emission-Electron Capture-Fission-Fusion

Nuclear Stability and Decay Half-Life Understand fission and fusion

You should be able to:

UNiT 4: Atomic Structure and Nuclear Ch emistry1. Summ arize past atom ic theories (Greeks,Dalton, Thomson, Rutherford, and Bohr).

1. Expla in how Bohrs model of the atom differedfrom its predecessors.2. Distinguish be tween protons, electron s, andneutrons in tenns of the ir relative masses andcharges.3. Defm e an atom ic ma ss unit.4. State how isotopes of an atom differ. 2. Determine the num ber of subatomic par ticlesgiv en the isotopic symbol or atomic n umber andmass num ber.

3 Use th e c oncepts of iso topes to expla in why theatom ic mass es of elements are no t wholenumbers.4. Calcu late the average atom ic mass of an elementfrom isotope dat a.


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5. Write balanced nuclear equations for alpha andbeta decay.6. Use the ha lf-life to calculate the amount ofradioisotope remaining at a given tim e.7. Differentiate among classifications of nuclearreactions including fission, fusion, naturalradioactivity and ar tif icial radioactivity.

5. Define radioisotope, radioactive decay, andtransmutation.6. Characterize alpha, beta, and gamma radiationby composition and penetrating power.

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This is the material from our third test:Chapter 5: Section 5.1 5.3

Bohr ModelQuantum Mechanical ModelEnergy levels, subshells, and atomic orbitalsQuantum numbersElectron Configurations (using only periodic table)o Configurationso Dot Diagramso Orbital box diagrams

* *Remember ExceptionsChapter 6: Sections 6.1 6.3

Periodic Table Periodic Law Classifying elements (alkali, alkaline earth metals, etc) Periodic Trendso Atomic Radiuso Ionizations Energyo Electronegativity

You should be able to:UNIT 5: Electronic Structure and PeriodicityExplain the significance of quantizied energies ofelec trons.2. Compare the quantum mechanical model of the atomwith previous models.3. Distinguish among principle energy level, energysublevel, and atomic orbital.4. Describe the general shape of s, p, and d orbitals.5. Explain why the electron configuration for chrom iumand copper differ from those assigned using theAufbau diagram.

6. Use quantum theory to explain the photoelectriceffect.7. Explain the origin of the atomic emission spectrum ofan element.8. Explain the origin of the periodic table.9. Distinguish between a period and a group on theperiod ic tab le.10. State the periodic law.

1. Use the Aufbau principle , the Pauli exclusion princ iple,and Hunds rule to write the electron configurations ofthe elements.

2. Given the wavelength of light, calculate the frequency,and vice versa.3. Calculate the energy of a photon associated with a givenwavelength or frequency of light.


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11. Identify the s, p, d and f blocks on the periodic table. 4. Write the ele ctron configurat ion of elements using theperiodic table as a guide .

5. Explain how atomic radii , ioniza tion energies, electronaff in ities, ionic size, and electronegativities vary withina group and within a period on the periodic table.

6. Classify an element as a representative element, noblegas, transition meta l or inn er transition metal.12. Identify an element as an alk ali meta l, alkaline earth

metal, halogen , noble gas , actinide or lanthanide. 7. Compare and contrast phy sic al a nd chemical propertiesin any group of representative elem ents .8. Draw elect ron dot diagrams of the representative

elem ents.13. State the octet rule. 9. Predict t he charge on an ion giv en its electron

configuration.


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This is the material from our fourth test:Chapter 7: Ionic BondsSome topics include...

EN values associated with ionic compounds Properties of Ionic compounds (melting points, solubility, etc.) Formula writing including assigning charges to ions.

Chapter 8: Covalent BondsSome topics include...

Octet rule and electron dot diagrams (make sure you understand and know how tothem!); also, coordinate covalent bonds.

Polar and Non-polar covalent: EN Values (remember a lot of this material youwere quizzed on already so dont expect to see too much of the same thing)

Intermolecular forces: what are they? Be able to explain the three types. Resonance structures VSEPR and hybridization theories: You will be responsible for the naming and

drawing of the structures (i.e. - bent, square pyramidal, etc.) Know how to predict the hybridization of the central atom along with the number

of sigma and pi bonds associated with the compound.You should be able to:

1. State the octet rule and the importance of thenoble-gas configuration in the formation of ions.1. Draw electron do t structures of the representative elements.2. Define anion and cation. 2. Use electron dot structures to show cation formation from metals andanion formation from nonmetals.

3. Define an ionic bond. 3. Use location of elements on the periodic table to identify a compoundas having ionic bonds.4. Identify characteristics of ionic compounds. 4. Explain the electrical conductivity of molten and aqueous solutions ofionic compounds.5. Define metallic bonds. 5. Use the theory ofmetallic bonding to explain the physical properties of

metals.6. Define covalent bonds. 6. Differentiate between polar covalent, nonpolar covalent, and ionicbonds using electronegativity differences as well as location ofelements on the periodic table.7. Use electron dot structures to show formation of covalent bondsbetween nonmetallic elements.7. Define double and triple covalent bonds. 8. Use electron dot structures to show coordinate covalent bondformation.

9. Draw electron dot structures for simple covalent molecules containingsingle, double and triple bonds.8. Define hybridization. 10. Use the theory of hybridization to show how carbon is able to form upto four bonds.9. Describe the shapes of simple covalently bondedmolecules. 11. Show the relationship between polar covalent bonds and polarmolecules.


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I have put together a collection ofmultiple choice questions for you to use as a study tool.No organic chemistry will be on thismid-term!! Study and good luck!!Mid-Term Review

Multiple Choice CAt. 3Identfy the letter of the choice that best completes the statement or answers the question.1. Which of the following measurements is expressed to three si?ificant figures?a. 0.007 m C. 7.30 x 10 kmb. 7077 mg d. 0.070 mm2. In the measurement 0.503 L, which digit is the estimated digit?a. 5

b. the 0 immedia tely to the left of the 3c. 3d. the 0 to the left of the decimal point3. How many significant figures are in the measurement 811.40 grams?a. two c. fourb. three d. five

2 3 3. What is the luipe of a salt crystal measuring 2.44 x 10 ny .4 x 10 m by 8.4 x 10 m?a. 2.9 x 10 m C. 2.9 x 10 mb. 2.9x10 m d. 2.9x10 m5. What quantity is represented by the metric system prefix deci-?a. 1000 c. 0.1b. 100 d. 0.016. Which tempera ture scale has no negative temperatures?a. Celsius c. Jouleb. Fahrenheit d. KelvinCommonly Used_Metnc PrefixesPrefix Meaning Factormega (M) 1 million times larger than the unit it precedes iokilo (k) 1000 times larger than the unit it precedes

1odeci (d) 10 times smaller than the unit it precedes 10centi (c) 100 times smaller than the unit it precedes 10_2milli (m ) 1000 times smaller than the unit it precedes 1micro (J) 1 million times smaller than the unit it precedes ionano (n) 1000 million times smaller than the unit it precedes 1opico (p) 1 trillion times smaller than the unit it precedes 1 0_127. What is the quantity 0.0075 meters expressed in centimeters? Use the table above to help you.a. 0.075 cm

c. 7.5 cmb. 0.75 cm d. 70.5 cm8. Which of the following equalities is NOT correct? Use the table above to help you.


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(tciyy) 3a. lOOcg=lg 1cm lmLb. 1000 mm = 1 m d. 10 kg = I g

9. Density is found by dividinga. mass by volume c. mass by areab. volume by mass d. area by mass

10. If a liter ofwater is heated from 20C to 50C, what happens to its volume?a. The volume decreases.b. The volume increases.c. The volume first increases, then decreases.d. The volume first decreases , then increases.

Multiple ChoiceIdentify the letter of the choice that best completes the statement or answers the question.1. A golf ball has more mass than a tennis ball because ita. takes up more space c. contains different kinds ofmatte r

b. contains more mat ter d. has a definite composition2. All of the following are ph ysical properties ofmatte r EXCEPTa. mass c. melting pointb. co lor d. ability to rust3. Which of the following is NOT a phys ica l property ofwater?a. It has a boiling point of 100C.

b. It is a colorless liquid.c. It is composed of hydrog en and oxygen.d. Sugar dissolves in it.4. Which of the following are con sidered physical properties of a sub stance?a. color and odor c. malleability and hardnes sb. melting and boiling points d. all of the above5. Which of the following materia ls is a substance?a. air c. stainless steelb. gasoline d. silver6. Which of the following is used for chemical symbols today?a. drawings c. lettersb. icons d. numbers7. The chemical formula of a compound does NOT indicate thea. identity of the elements in the compoundb. how elements are joined in the compoundc. the composition of the compoundd. relative proportions of the elements in the compound8. In the chemical reaction in which sucrose is heated and decomposes to form carbon dioxid

e andwater, which of the following is a reac tan t?a. sucrose c. waterb. carbon dioxide

d. heat


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9. Which of the fo llowing indicates that a ch em ica l change has happened dur ing cooking?a. The food darkens .b. Bubbles form in boiling water.c. Butter melts.d. Energy is transferred from the stove to a pan.

10. Which action ch anges the identit y of the substan ce ref erenc ed ?a. melting goldb. running an elec tri c curren t th rough copperc. corro ding irond. breaking an ice cube

Multiple Choice C4. )fIdentjfy the letter of the choice tha t best completes the statement or answers the question.1. Why did J. J. Thomson reason that elect ron s must be a par t of the atom s of all elements?

a. Cathode rays are negat ively -charged par tic les.b. Cathode rays can be defle cted by magne ts.c. An elect ron is 2000 times ligh te r than a hydrogen atom.d. Charge -to -mass ratio of elec trons was the same, reg ardles s of the gas used.

2. Which of the fol low ing is true abou t subatomic particles?a. Electrons are negat ive ly charged and are the heav iest suba tomic particle.b. Protons are po sitively charged and the lig htes t sub atom ic par tic le .c. Neutrons have no charge and are the lightest suba tomic partic le.d. The mass of a neu tron nea rly equals the mass of a proton .

3. Which of the following is correct conce rn ing suba tomic part icles?a. The electron was discovered by Goldstein in 1886.b. The neutron was discovered by Chadwick in 1932.c. The proton was discove red by Thomson in 1880.d. Cathode rays were found to b e made of pro tons .

4. As a consequence of the discovery of the nu cleu s by Rutherford, which mode l of the atom isthought to be true?a. Protons, electrons, and neu tron s are evenly dis tributed throughout the volume of the atom .b. The nucleus is made of protons , elec trons, and neutrons.c. Electrons are distr ibuted around the nucleus and occupy almost all the volume of the atom.d. The nucleus is made of electron s and protons.

5. What does the num ber 84 in the name krypton -84 represent?a. the atomic number c. the sum of the proton s and elect ronsb. the mass number d. tw ice the nu

mber of pro tons6. Isotopes of the same elem ent have diff er ent

a. numbers of neutrons c. num bers of electronsb. numbers of protons d. atomic numbers7. In which of the following is the number of neutro ns correct ly represented?a.

F has 0 neutrons. c. Mg has 24 neut ron s.238

33s has 108 neutrons. . 93 has 146 neu tro ns.8. Which of the following isotopes has the same numbe r of neu trons as phosphorus-3 1?

a. c.15 14b. 3 d. 2816 149. The atomic mass of an elemen t de pend s upon the .a. mass of each electron in tha t elem entb. mass of each isotope of that elem entC. relative abundance of protons in that elemen t. mass and relative abundance of each isotope of that element


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Multiple Choice: C h. 15Identy5 the letter of the choice that best completes the statement or answers the question.

1. A beta particle is a(n)a. photon c. helium nucle

usb. electron d. hydrogen nucl

eus2. What is the change in the atomic number when an atom emits a

n alpha particle?a. decreases by 2 c. increases by 1b. decreases by 1 d. increases by 2

3. What is the change in atomic number caused by the emissionof gamma radiation?

a. decreases by 2 c. remains the same

b. decreases by 1 d. increases by 14. Which symbol is used for an alpha particle?a. He C. He

b. He d. 44e5. What particle decomposes to produce the electron of beta radiation?a. proton c. electron

b. rwtwon a. pC5i+ron6. What symbol is used for beta radiation?

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a. 0eb. 0

d. 1e.1

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7. If an isotope decays by the process of beta emission,a. the mass number changesb. the atomic number changesc. protons are given offd. the number of neutrons remains the same

8. What type of radiation is best detected by a scintillation counter?

a. alpha radiation only c. alphaand beta radiation only

b. gamma radiation only d. all types of radiation

Multiple Choice CA. 5/ LoIdentify the letter of

the choice that best completes the statement or answers the question.

1. How many energy sublevels are in the second principal energy level?

a. 1c. 3

b. 2d. 4

2. When an electron moves from a lower to a higher energy level, the electron

a. always doubles its energyb. absorbs a continuously variable amount of energy

c. absorbs a quantum of energyd. moves closer to the nucleus

3. What is the number of electrons in the outermost energy level of an oxygen atom?

a. 2c. 6

b. 4 d.8

4. Which electron configuration of the 4fenergysublevel is the most stable?

a. 4/c. 4/3

b. 4fd. 4f

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5. Which of the following electron configurations of outer sublevels is the most stable?a. 4d5s C. 4dsb. 4ds d. 4ds

6. Which variable is directly proportional to frequency?a. wavelength

c. positionb. velocity d. energy

7. How do the energy differences between the higher energy levels of an atom compare with the

energy differences between the lower energy levels of the atom?a. They are greater in magnitude than those between lower energy levels.b. They are smaller in magnitude than those between lower energy levels.c. There is no significant difference in the magnitudes of these differences.d. No answer can be determined from the in formation given.8. Bohrs model could only explain the spectra ofwhich type of atoms?a. single atoms with one electronb. bonded atoms with one electron

c. single atoms with more than one electrond. bonded atoms with more than one electron9. The wavelike properties of electrons are useful in.a. defming photonsb. writing electron configurationsc. magnifying objectsd. determining the velocity and position of a particle10. Which of the following categories includes the majority of the elements?a. metalloids c. metalsb. liquids d. nonmetals11. Which of the following groupings contains only representative elements?a. Cu, Co, Cd c. Al, Mg, Lib. Ni, Fe, Zn d. Hg, Cr, Ag12. Which of the following is true about the electron configurations of the repr

esentative elements?a. The highest occupied s andp sublevels are completely filled.b. The highest occupied s andp sublevels are partially filled.c. The electrons with the highest energy are in a d sublevel.d. The electrons with the highest energy are in anf sublevel.

13. What causes the shielding effect to remain constant across a period?a. Electrons are added to the same principal energy level.b. Electrons are added to different principal energy levels.c. The charge on the nucleus i

s constant.d. The atomic radius increases.

14. Atomic size generallya. increases as you move from left to right across a periodb. decreases as you move from top to bottom within a groupc. remains constant within a periodd. decreases as you move from left to right across a period

15. Which of the following factors contributes to the increase in atomic size within a group in the

periodic table as the atomic number increases?a. more shielding of the electrons by the highest occupied energy levelb. an increase in size of the nucleusc. an increase in number of protonsd. fewer electrons in the highest occupied energy level

C ____


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16. In which of the following sets are the charges given correctly for all the ions?

a. Na, Mg, Al C. Rb,Ba,Pb. K, Sr,O d. N, 02_, F3

17. In which of the following groups of ions are the charges all shown correctly?a. Li, 02_, S C. K2 F , Mgb. Ca,Al, Br d. Na, F, Rb

18. For Group 2A metals, which electron is the most difficult to remove?a. the firstb. the secondc. the thirdd. All the electrons are equally difficult to remove.

19. Of the following elements, which one has the smallest first ionization energy?

a. boron c. aluminumb. carbon d. silicon

Multiple Choice C..h.Identfy the letter of the choice that best completes the statement or answers the question.

1. How does calcium obey the octet rule when reacting to form compounds?a. It gains electrons.b. It gives up electrons.c. It does not change its number of electrons.d. Calcium does not obey the octet rule.2. What . tl ectron configuration of the oxide ion (0 2 )

a. 1s2s2p C. 1ss 2b. ls2s2p d.3. What t1j ect?n ongu;itin cth iode ion?a.1sspspd0spd0s 5pb.1sspspd0spd0 2C.1sspspd0spd 5sd. ls2s2p3s3p3d 4s4p4. What is the net charge of the ionic compound calcium fluoride?a. 2 c. 0b. 1 d. 1+5. What is the formula unit of aluminum oxide?a. AlO c. A10

b. Al d. Al 036. What is the name of the ionic compound formed from lithium and bromine?a. lithium bromine c. lithium bromiumb. lithium bromide d. lithium bromate7. What is the formula for sodium sulfate?a. NaSO c. Na(S02

b. NaO d. NaSO428. What does the term coordination number in ionic cryst

als refer to?a. the total number of valence electrons in an atomb. the number of oppositely charged ions surrounding a particular ionc. the number of atoms in a particular formula unitd. the number of like-charged ions surrounding a particular ion

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9. Under what conditions can potassium bromide conduct electricity?

a. only when meltedb. only when dissolvedc. only when it is in crystal forma. onJ whQI rrtId or dissolved i,- yvoAcr

10. Which of the following elements can form diatomic molecules held together by triple covalent

bonds?a. carbon c. fluorineb. oxygen d. nitrogen11. Which elements can form diatomic molecules joined by a single covalent b

ond?a. hydrogen onlyb. halogens onlyc. halogens and members of the oxygen group onlyd. hydrogen and the halogens only

12. Which of the following electron configurations gives the correct arrangement of the four valence

electrons of the carbon atom in the molecule methane (CH.)?2 2 1 2 1a. 2sp 1

C. 2spsb. 2s2p3s d. 2s2p

13. Which of the following diatomic molecules is joined by a double covalentbond?

a. 2 c.N2

b. Cl d. He14. According to VSEPR theory, molecules adjust their shapes to keep which o

f the following as farapart as possible?a. pairs of valence electrons c. mobile electronsb. inner shell electrons d. the electrons closest to the n

uclei15. What causes water molecules to have a bent shape, according to VSEPR the

ory?

a. repulsive forces between unshared pairs of electrons

b. interaction between the fixed orbitals of the unshared pairs of oxygenc. ionic attraction and repulsiond. the unusual location of the free electrons16. What type of hybrid orbital exists in the methane moleule?

a. sp SJ 21. 2 d. spd

17. How many pi bonds are formed when sp hybridization occurs in ethene,CHa. 0 c. 2b.1 d.3

18. Which of the following atoms acquires the most negative charge in a covalent bond with

hydrogen?a.C c.Ob. Na d. S


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mid term review 2010

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