NAME: ~ ~

PERIOD:

REVIEW

CHEMISTRY MID-TERM

2013 - 2014

Mr. Chuba

I. Express the following numbers in scientific notation to three significant figures:

a. 0.000000027 s. 70 1-(08

61b. 356 ~. S(p XlO

-.1c. 0.096 9. ~o 'I. 10

;;.

d. 802.6 g. 0:3 -y I 0

2. Convert the following numbers to regular form:

d. 6.03 X 106

Isaoo

O. 00 00000 17fc . ooo03JS~

~O -s OOOQ

a. l.52 x 104

b. 7.78 X 10-8

c. 3.256 X 10-5

3. Determine the number of significant figures in each of the following numbers:

a. 4867 miles ~

b. 56 mL d

c. 60104 tons S

d. 2900.0 g 5

e. 0.0000003 cm

f. 4.6 x 1019 atoms ~

4. Express each answer in the correct number of significant figures:

a. 7.310 -7 5.70

-3b. 3.26 x 10-3 -7.88 X 10-5 3. I 8 'f. 10

d. 4.51 x 3.6666 J~, S

e. 3.70 - 2.9133

OVER

5. A lead sphere has a mass of 1.20 x 104g and its volume is 1.05 x 103 cm3. Calculate the density oflead.1./

1,;J4X/OJ

6. Mercury is the only metal that is a liquid at room temperature. Its density is 13.6 g/cm'. How manygrams of mercury will occupy a volume of95.8 crrr'?

dV =

7. The price of gold on a certain day in 2004 was $315 per ounce. Determine the price of 1.00g of gold onthat day.

loz=31.03g

::_',_0_0_..5_11-_)_0_1,. __ /' 11 31S

I I 3/. 0 3j IOl::

8. The speed of sound in air at room temperature is 343 m/s. Determine the speed in mi/hr.

1 mi = 1.609 km

3l/3vr( fk:»t 11%~ ~OS to 011("" ,Jnl

/I'll' - 7" 7 Tr-- I. ~oq jc.V)'l !lI1./n / hr -- Ie 00 111Ih,.. - /s

9. The human stomach can expand to hold up to 4.20 quarts offood. A pistachio nut has a volume of0.900 mL. Determine the number of pistachio nuts that the stomach can hold.

1 gallon = 3.79 L 1 gallon = 4 quarts 1 L = 1000 mL

IJ ".f 3.71L /000"", L I nu -t-AI • .io ;.t

() • Clo(jk'>" L.: v

I.{ 6t lJol Il.-I

.:: t/JjC)/; ~ct" 7

= r"/. 'f.J 'A 103

I'ISTII~/O AiVT.j ]L --

10. Determine whether these statements describe either a physical (P) or chemical (C) property:

a: C oxygen gas supports combustion.

b.CUlP fertilizers help increase agricultural production.

c. pp

water boils below ioo-c on top of a mountain.

d. lead is denser than aluminum.

e. P uranium is a radioactive element.

f. ~ iron has a tendency to rust.

g. L rainwater in industrialized regions tends to be acidic.

11. Determine whether each of the following is either a physical change (P) or a chemical change (C):

a. P when a glass of water is left out in the sun, the water gradually disappears.

b. ~ carbon dioxide in air is converted to more to more complex molecules by plants duringphotosynthesis.

c. f the helium gas in a balloon tends to leak out after a few hours.

d. ~ rocks are ground into sand.

e. ~ frozen orange juice is liquefied by adding water to it.

f. ~ digesting a pizza.

g. L a spoonful of table salt dissolves in a bowl of soup.

12. Which of these properties are intensive (I) and which are extensive (E)?

a. E area

b. :r color

c. .r density

d. ~ length

e.,;

volume

f. ..l- temperature

[ massg.

h. ~ ductility

OVER

._-- _._-----------_._._- ..._.- _. -'---- .-.-

13. Classify each ofthese substances as an element (E), compound (C), homogeneous mixture (horn), orheterogeneous mixture (het):

C watera.

b. E gold

c. he.J raisin bran cereal

d. ~ orange soda

e. C rubbing alcohol (C3H70H)

f. _C_sugar

g. ~ cellulose

h. E uranium

i. he,t sand on the beach

j. ~ brass

13. List the major contributions of each of the following scientists:

Tl4c 47VMfC -n-l~Otl.ta. Dalton - "DEVELOPED c;.

b. Thomson - bll S CO'\}t'fLED e -

c. Milliken

of

d. Rutherford - GOL.i) FOIL ExPEJi!.\ W\tt-JT)eMPT'f SPA.C£

ATOYl1. IS. hfOSn Y)

e. Chadwick - t-JEU"'fv<'O,.J

14. Define the following:

a. atomic number - ,.w W\B~ oF" Pt2.oTt)"-..U

b. mass number - fte.oTO "-' S + NeU rtl..O,JS

c. average atomic mass - WE"IGI-ITh-n 411fTlAGt: mASS of=: ALl... 11-/(; ISoToPe,s()F- AN '=.L/;"...1t:N T

15. Why does a knowledge of atomic number enable us to deduce the number of electrons present in anatom?

:/I Pteo TON.s s:

16. Why do all atorris of an element have the same atomic number, although they may have different massnumbers? DII=FI3Z.I?NT ISOTOPE,:) of AN FLEIYIl!l\lT I-!F/V/£ blt="Fi::"""R..f:7JT

NtJYY\tSEtl.. of tJElJT(l.oI'JS IN mE tJVC.LEVS#

17. What do we call atoms of the same element with different mass numbers?

.I..$0 TOP ES

18. Explain the meaning of each term in the symbol ~X.

4 z; Y\'\ A So S IJ V (tV~ <:-7ta -n v = /::.~'I"V\aJ" SYM60Ll .s: A TO YV\ , C. ""' U f\t'\ ·..;d:' i~ r-;

19. Write the isotopic symbol for each of the following:

lqS pia. platinum-195 7g t

b. copper-63

c. tungsten-186

20. Write the name for each ofthe following isotopes:

a. 33S16

b. 20lHg80

M82CU..e. 'I - ;)0 I

c. 23NaII

SODIIJM - ~3

d. 64Ni28

21. Complete the following table:

SYMBOL PROTONS NEUTRONS ELECTRONS MASS NUMBERSI.P

~ S 1'1" 25 3/ dS 56262Bh

155 /07 ;;) (, ;)107 10 7288UUp

/15 ;J2~115 115 173204Hg

&>-0 ?O ;;0 V80 124$1 ,::'e s I2/., 0)(,

, 26 57

OVER

22. What are allotropes? How are allotropes different from isotopes?AL-LOT12.0P£S A~t: nl FFl2e8\lT PIiYSlcAL fJICI!4A1GEII19JTS 0-'::: /-iN cLE"rYlf:A.lT.

AN LsoTVI't= of AIJ /:;LE~ENT VAtel E.) fjY THE NUWlt5~ of NE(jmON.S .IA..!

THt: NUC.LI::.IJ~,

23. Determine the average atomic mass of titanium given the following information:

Titanium-46Titanium-47Titanium-48Titanium-49Titanium-50

mass = 45.95 amumass = 46.95 amumass = 48.00 amumass = 48.95 amumass = 49.94 amu

relative abundance = 8.000%relative abundance = 7.500%relative abundance = 73.70%relative abundance = 5.500%relative abundance = 5.300%

(48.00)(73.7) + (1/!.q$)(S.S)+(~9. Qlf) (5.3)

I o 0

24. Name the concept, theory, model, etc. that each of the following scientists is known for in thedevelopment of the modem atomic model:

a. Max Planck QuA.·..IT)I.\ OF /::::NI::."YlG Y

b. BohrPLArJETAr2 'I fYlOO6L - THE € - EX IS T AT C.E!2TfJIAi ALLOWeD

6JE'i<G" LEvElS

c. de Broglie WA"~ PM..TICLE bU A L I i Y

d. Heisenberg UN C8HA IN 1"( p~ IAi C I P LE

e. Schrodinger WAvE EQ VAnON

25. Write the abbreviation for and describe each of the following quantum numbers:

a. principal quantum number n

b. azimuthal quantum number J

c. magnetic quantum number YY) ~ at<1 /:;7Jm 170 Ai .J:JJ sPACE

d. spin quantum number rY1 S SPIN OF mE l:'"l.fC~o,,-1

26. Define each of the following:

a. Pauli Exclusion principleA r'YlA')( 11'1 UrY) of TWO ELE<:.i£o,...).j

(3vT ol\..ll'i IF THE EU~CnlO".J.s

M/)8 OCCVP'I ft s/AfGLE

I-IAVE OPPOSITE SPIN$"

/-}7VrvtIC

b. Aufbau PrincipleEAC-I-l ELtCnto,J OCCuPIES THE LOw6'ST '="7Vf!26-Y ot<l3rrJC/L f-/vf-/ILAtSLF

c. Hund's Ruleat=C~oN.s W In\ "TI4t:- SAmE" SPIN f'VIvsr occupy I="Y-/CH E<4>VAL l=7V1:1€.6 YLEVeL (0 a.e,TA 1..) SIf.J6L Y (j~"j(E" f-/DO' nOA/AL cLECmO/l.lS W In-i o,oPOS I IE'

SPINS CArJ occuPy Tl-/E SAmE ORJ3ITALSd. Heisenberg's Uncertainty principle

.:tT I.$ FVNDA""E"NTf-\Ll'( .rn'l.aoS51I.3Lt= TO I<AlOLV fl'(Ee/~f:L y /Jom THEVaO(.IT'f AND f'05mOI'J oF' A (lAR:nCi..E AT THE S(.Jm€' TIME.

27. Complete the following table:

Value of! Letter Range of nu Number of Maximum # of electronsorientations

0 S 0 I ;;

1 f -I) 0, I 3 ~

2 of -~\-I,OI'IJ. S 10

3 t -3-~-IOld3 1 1'1I \ ) I I I

28. Write the complete electron configuration for each of the following:

a. As I~/ ~s2. d,a Go 3.s Z 3(' ~~Is' 3d If) '-If3

29. Draw the orbital diagram for each of the following:

1~ 1~ 1~1 .1--df~1

a.O

b. V 1v 1t-. 11r 1/' 1 ~ .1l 1~ 1~1~ jj,- .11-~----- ---Is 2- Jsz. Jf fc 3£ 2- 3fiD us z. 3d 3

c. AI 11r 1// 1~ 1j,. 1b 1~ ~-~--Is z: ,;}sz. dflD 3s 2- 3f'

OVER

30. Determine the frequency of electromagnetic radiation with a wavelength of 3.33 x 10-8 m.e

,3,00 -X 10

3,33 ~ 10-8c-). z: =

,sr;,OI X/O -IS

31. Determine the minimum frequency of light needed to eject an electron from an atom of platinum if theenergy required is 9.08 x 10-19 J. -'9~ Q,08)<. 10-J::- h = t. ,(,,:3 )( 10-3'1

=,s

/,37><10 -/S

32. The argon-fluoride laser used in some refractive eye surgeries emits a wavelength of1.933 x 1O-7m. Determine the energy of this laser.

h( U(),~3~IO'34)(3.00 x/0g

)f z: ::A /,((33)</0-7

:::-18

I. 0;) 9 X 10 .r

33. State the periodic law./HE PI-I'ISICA LAND C'.HEYl'\ Itl-l L

"..(c: A f'81' 0Die FutJ c.TJ(),J

P~OPt~TI£,5 OF THE ae )v) (;l\JiS

OF THE/~ ATOmiC A/uml3c~.

34. Identify each of the following as a metal, nonmetal or metalloid

a. phosphorus N (Y) b. niobium M,

c. arsenic mEn1 LLbl D d. holmium M

e. krypton rJ fY) f. strontium M

35. Name each of the following groups by their family name.

a. Group 17 1-1ALO G ENS b. Groupl AL!<::I-)LI METALS

c. Group 18 /'Jo(!>LE GA:>€,s d. Group 2 ALKALINE c-f-l,.ell-l h"IETf.\W

36. Classify each of the following elements as a (an) alkali metal, alkaline earth metal, halogen, or noblegas.

a. rubidium A \...I<A L I d. iodine HALOGe-A.l

b. bromine HALOGE"IJ e. radon

c. radium ALVALIN EEAll.n-IS f. lithium ALKAL I

-----.- --_.' -- ._------- _.- -_._--------- .._-_._. __._---_ _- -

37. State the trend for atomic radius.

T -'> (j

38. State the trend for ionization energy.

39. State the trend for electronegativity.

b£0CEY-lSt= T -7 (j) .rNe.R.€'fl~t: L -"> R40. Arrange these elements in order of decreasing atomic radius: sulfur, tellurim, and oxygen.

41. Arrange these elements in order of increasing ionization energy: TI, Ga, In, B.

T1 c .L f'\ < Gc.. <- (342. Arrange these elements in order of decreasing electronegativity: 0, F, C, N.

(-'>O>,.j>-(!;

43. Name the following ionic compounds:

a. MghMAGt-JESIljn'\ .roD \'\;)E"

f. Pb(NOZ)4

L8\iJ (I'J) NITI2\lt

g. (NH4)JP04

AMW\ONI v 1'\1) Pl-/oSPH4~

b.

h. Al(HC03)3

tlLU It! I /\/U YV1 e-I CAL.'()OA.i Arlf'

d. i. Ni(CN))

e. j. Zn(HC03)2

1- J'" C 81 CtJRSo;J 1-1 re:

OVER

---.~----- .------ .. --~----------

44. Write the formula for each of the following ionic compounds:

a. nickel (III) acetate f. iron (II) permanganate

Nt (CJ- 1-130.;)3 Fe (fYJr'104 );).

b. barium telluride g. manganese (III) carbonate

~Te fY/ Y) CJ (COS)3c. tin (Iv) cyanide h. gallium sulfide

SV\ (etJ) t( Gad. 3,3d. cobalt (Ill) sulfite I. radium iodide

Co;;. (503)3 ReA.. I a.e. copper(I) bicarbonate j. europium (II) phosphate

etA- HCO.3 E U3(fO tf) d,

MID-TERM TOPIC SUMMARY

Unit 1

rules for significant figuresrounding rulessr unitsUnit conversions (railroad tracks)Kilo-hecto-deca-base unit-deci-centi-milli

Unit 2

mattermixtures (homogeneous & heterogeneous)compoundselementsallotropesphysical changeschemical changesphysical propertieschemical propertiesallotropes

Unit 3

protons, electrons, neutronsmass numberisotopesisotopic symbolaverage atomic mass calculationsDemocritusDalton

- Rutherford- MiJliken- Thompson

Unit 4

UnitS

c='Ayamplitudefrequencyspeed of lightPlanck's constantE=hyground stateexcited statequantum numbers: n, I, rnr, m,electron configurations: complete and abbreviatedAufbau PrinciplePauli Exclusion PrincipleHund's Ruleorbital diagramsPlanckBohrde BroglieHeisenbergSchrodinger

MendeleevMoseleymetals, nonmetals, noble gases, metalloidsfamily namestrends in atomic radius, ionization energy, electronegativitydefinitions of atomic radius, ionization energy, electronegativitynaming ionic compounds containing monatomic ionswriting formulas for ionic compounds containing monatomic ionsnaming ionic compounds containing polyatomic ionswriting formulas for ionic compounds containing polyatomic ions

OVER