Name. Date

CHEMISTRY 1't Semester FINAL REVIEW- Fall 2014

Period

Measurement & Matter (Unit 1)

• Significant Figures

• Matter

• Heat

• Law of Conservation of Mass/Matter

• Density

Atomic Structure (Unit 2)

• Atom

• Ions

• Isotopes

• Atomic Mass Calculations

Nomenclature (Unit 3)

• Covalent Names and Formulas

• Ionic Names and Formulas

• Acid Names and Formulas

Moles (Unit 4)• Mass, Volume, and Particle conversions

• Empiricaland Molecular Formulas

Atomic Structure History (Unit 5)

Electrons (Unit 5)• History of the atomic model (Bohr, Shrodinger, etd)

• Orbitals, Sublevels, and Energy level basics

• Electron Configurations

• Rules (Hunds, Pauli's Exclusion, Aufbau)

• Frequency, wavelength and Energy of electrons calculations

• Valence Electrons/Dot Diagrams

Periodic Trends (Unit 6)• Atomic size

• Electronegativity

• Ionization energy

• Metal and nonmetal reactivity

• Ion size

Refer to the formula chart for other nÿeded equations

d constants!!!

SUBSTANCE SPECIFIC HEAT (JIB °C)Aluminum 0.90

Copper 0.38Gold 0.13Ice 2.06

Iron 0.45Lead 0.13

Steam 2.06Water 4.18

Measurement/Matter

1. Which measurement has 3 significant figures?

A. O.03 g

B. 300 g3.00 g

D. 0.030 g2. Which measurement has no zeroes that are significant?

A. 503 cm

B. 5.00 g

C. 670. m

0.02 ghase of matter has the greatest attractive forces?1. Which

2. Which

3. Which

4. Which

hase of matter has the least attractive forces?

hase of matter has the highest entropy (chaos)?

GOS

hase of matter has the lowest energy? ,)--

Liquid Gas ÿr)f(ÿ0lÿ ÿ1ÿ)7. Classify each of the following as either physical or chemical properties by checking the

appropriate box.

Property PhlYÿCal Chemical

Blue color

Density 'ÿ

Flammability j

Solubility J'<

Reacts with acid to form H2 v! ÿ'

Combustion ÿ VI

Melting point j

Solid Liquid

Gas Liquid

Gas Solid

Liquid Solid

Solid Gas

FinalPhase

Name of Phase Change

Ex: melting

Endothermic or Exothermic?

Endothermic

,erJo

InitialPhase

5. Which ÿhase of matter has the fastest moving particles? q ÿ'ÿ

6. Complete the chart below about the six possible phase changeÿ.

Reacts with water to form a gas

Reacts with a base to form water

Hardness

Jiling point

Can neutralize an acid

Luster

Odor

8. Classify each of the following as either a physical (P) or chemical (C) change.

a. Sodium hydroxide dissolves in water

b. Chlorine and hydrogen react to produce hydrochloric acid.

c. A pellet of sodium is sliced in two.

d. Water vaporizes into steam.

e. Iron rusts.

f. Evaporation.

g. Milk sours.

h. Ice melting.

i. Sugar dissolves in wafer.

j. Wood rotting.

k. Mirror cracking. ÿiÿI. Phase changes are ALWAYS ]ÿhUrÿ

9. What are the four signs of a chemical change.

b. £eoiOr" uc. rJ,- a e,

1o. The particle diagra.l below represents a sample of matter.

ChangesLIF

Which best describes the composition of the sample?

(ÿ mixture of compoundsb. a single compoundc. a single elementd. a mixture of elements and compounds

11. Circle the intensive prÿrties:

Mass Weight

12. Circle the extensive properties:

Malleability Freezing point density ÿ ÿ

13. Calculate the density of an object with a mass of 45.0g and a volume of 25.0mL (Show work, box

answer with units/labels)

v .o14. Calculate the volume of an object with a mass of 45.0g and a density of 1.5g/mL. (Show work, box

answer with units/labels)

v- - IV- 30. rnL

15. Calculate the mass of an object with a density of 2.0g/mL and a volume of 15.()mL. (Show work,

box answer with units/labels)

mÿ D.v :

Use the following graph to answer the next questions.

0

'"E

3O

o • 1¸. . ÿ • ÿ ÿ -. ,

me (mÿes)

16. Which segments represent an increase in kinetic energy? k} C') E17. Which segments represent an increase in potentigl energy. ÿ ÿ ÿ i

18 Which segments change with temperature? /4, C, ÿ-" - •19" Which segments represent phase changes? . ill ÿ ' ÿ! --

20. Which segment represents a: Solid? /'t'- .' Iÿiquid? C ÿ Gas?21. What is the melting point of this sÿbstance?ÿoiling point? ÿ0 ÿ freezing point? 5ÿuC,

22. How much heat is required to raise the temperature of 250.0 g of mercury from 48.0°C to100.0°C? Specific heat of Mercury = 0.140 J/gÿC (Show work, box answer with unÿs/labels)

• Is this process endothermÿ-ÿ-exothermic? Justify your answer (hint: what is the charge

of .)

23. If a metal has a specific heat of 0.78 J/g °C and a mass of 28.8 g, how much heat is required to

raise its temperature by 2 °C? (Show work, b.ox answer with units/labels)

24. The temperature of a 95.4 g piece of metal increases from 25.0°C to 48.0°. The specific heat of

this metal is .3869 J/g°C? How much heat w[ the metal absorb?

• What is the identity of thisreference tables in the front of this packefl)

)at the specific heat and then compare on your

25. What number identifies an element?. ÿ,s J:ÿ26. What particles are represented by the atomic number?27. What particles are represented in the mass number?28. Chlorine-37 can be represented as

17a. 37Cl

Dr ultoP

d. 3735 CI

29. The diagram below represents the nucleus of an atom.

Key

Proton : 0)

Neutron : O

What are the atomic number and mass number of this atom?

(ÿÿ: atomic number is 9 and the mass number is 19.atomic number is 9 and the mass number is 20.c. The atomic number is 11 and the mass number is 19.d. The atomic number is 11 and the mass number is 20.

30. Which represents the most abundant isotope of sodium?a. sodium-11

b. sodium-22

sodium-24

31. What is the total number of electrons in an Mg2÷. ion?

A) 2 electrons

C) 12 electrons

D) 14 electrons

32. What is the total number of neutrons in an atom of26ÿe57ÿ ÿ.

A) 26 neutrons

C) 57 neutrons

D) 83 neutrons

33. Which phrase describes an atom?A) a positively charged electron cloud surrounding a positively charged nucleusBÿÿitively charged electron cloud surrounding a negatively charged nucleus

a neaaÿ1ÿely charged electron cloud surrounding a positively charged nucleusD) a negatively charged electron cloud surrounding a negatively charged nucleus

34. Complete the followin9 table.

Complete Atomic MassSymbol Number

i q

3., + iillJVa

Number

aÿ

Protons

II30

Neutrons

14

Jÿ18

Electrons

103b

Charge

O0

-3

35.Showing all your work,a) Calculate the atomic mass for the following element.

Isotope Mass Percent(ainu) Abundance

Isotope #1 27.98 92.22%Isotope #2 28.98 4.69%Isotope #3 29.97 3.09%

b) Identify this element.

i

36. Neon-20 accounts for 94.3% of naturally occurring neon. Neon-23 accounts for the remaining 5.7%.

Calculate the atomic mass of neon. SHOW ALL WORK!

i0o i00Nuclear Chemistry Review

37. Explain in one sentence why nuclei undergo radioactive decay. (Hint: stable vs unstable nucleus)

38. Complete the following table of radioactive decay parTicles:Particle Symbol Atomic Mass Charge Composition

Alpha, a

Beta,

O! i

0Gamma, VO

39. Which of the following paths will each of the following particles take? an alpha particlea beta particle, and a gamma ray.

RadioactiveSOtlfCe:

Detector

(+)40. Laÿel the following statements as either alpha, beta, or gamma radiation.

_ÿthe most dangerous type of radiation

l the largest of the radiation particles

have a positive charge

_ÿahaVe no mass (multiple answers)helium nucleus

)__an excited electron

lÿcannot penetrate paper or clothes

/ÿ harmful only when ingested

_ÿ_exception to transmutation reactions "

41. Write the nuclear equation for the alpha decay of 238.92u•

42. Write the nuclear equation for the beta decay of 1ÿC.

Iÿ 0

43. What type of decay does 237ÿrÿ9s,,ÿ, undergo if it produces 237pu')94. •

b7 ÿ7

44. If ]$7Cl undergoes beta andgamma decay, what atom is prodUl

45. Define fission:

46. Define fusionY

47. Label the diagrams below as fissmn or fusion.

tRONS

u ion

ult,ÿar-%, u.m

i ii

Nomenclature

Compound

48. NazO

49. NO

50. PbSO4

5l. AtÿCO3)3

52. N204

53. HCI

54. bromic acid

55. chromium(III) oxide

56. sulfur trioxide

57. pentaphosphorusdecoxide

58. ammonium sulfite

59. hydrosulfuric acid

Moles

I Moleculiÿr,l:.oniÿo n:° ÿrl.id?

Answer

MA

S.-A

61. Whatlÿ ttÿhÿram formulas mass

,,st

-I

i"iÿ# ,ÿ' .J 17

t'" 7" r, ÿs' ,..,Y..

62. Which substance has the greatest molecular mass, ÿNO ?

tg " _ Iÿ, oon x c

O -/s °lqÿ--'< ÿ'°°ÿ

1

63. List all seven diatomics:

I\.J! Oi

ot )

64. Determine the mass percent of oxygen in mÿgnesium hydroxide.

ig - 1, o 0 ÿ)XZ- !,01 to1J

qS,/fT. 0

65. C.ÿlculate the percent composition ÿ Ca(gH)z?

_ -, : ÿ "') :-, ÿ..ÿ 1

-'H ,oÿ z_

66. Draw the Mole Road Map! @: 1 ,ÿ ÿ'ÿ.ÿ

b,O2x I0;ÿD d Iÿ

U ,\:...;/ ,-.

Uÿ-I-GrS

, !

67. If there are 3.45 tools of Ca in a container, how many particles would there be?

6 ÿrÿÿ 0f4 Itÿ oÿt'o2ÿ "i]. I rrttcÿ,o -" -ÿÿc/ÿ tÿ])

68. What is the gram formula mass of 7,50 X 102ÿfoTmula units of Fe(NOa)ÿ? 7ÿ ÿ ÿ'ÿ--ÿ 7 ÿ' ÿ .i

q,9ox ÿoÿtfc,<-ÿvÿ-,t,, l>ÿu 1ÿ,ÿ:ÿ ÿ:- ',ÿ%414,tg'Yq4

6}. How many liters are there in 5.25g dOa at STP? l ÿ -- ed--ÿÿ ÿ ''

6,'Z6qO09-.) ! rrvoÿ ;;;¢, a ,,-_L._. " . G- la,oiÿ,<l =ÿ<,,-o!t- - /ÿ -ÿ " iÿ7-7.Lÿ£Lÿs ' (0 = 15,qqqxa= 5t,hcl2

70. There are 4.82X10aÿ f. units of FeaOa, what mass in grams is the equivalent to this?

"- "tÿ I t,,ÿ-.oc_.o. " /ÿ.cSqÿ<:ÿ-ÿ Fe_{<, 5,5,tÿs,,x:z-- I I,c,<

lco,oa.ÿ_coÿ-5 C',o,,.4s) i,o:v, co _____ <"" " - , -"

71, How many mols ?f Ne ate there in 5 50g of the gas7 _ÿ ÿ:\ ,GQÿ .l IO'ÿ,uÿ

5 ' 50 ÿ b"1 { ! I ÿa))ÿ ill .... ÿ: k 'C --

72. A sample of a compoundc0ntains 65.4 grams of zinc, 12.0 grams of carbon, and 48.0 grams of

oxygen. What is the mole ration of zinc to carbon to oxygen in this compound. (Hint: your

empirical tool to tool ration numbers you would use for #ÿbsÿip¢ÿ ..... ]

. O.ÿr, ÿ =, . iG©.;'Jÿ I' OOO /l'°°° ' =l(D'- it "ÿÿIQCÿ5 i ÿ

.,,;ÿ i!oÿ,oÿi,ÿ<_.- t, ,

6.00 0 t ryÿtÿ, :_ ,ooo/!,ooo

73. A compound contains 33.18 g C, 4.60 g H, 29.49 g O, 32.72 g CI, and a molar mass of 108.5g/tool.Determine the empirical and molecular formulas of the compounds.

k.X5( .... } { v'v'u>",..,.'-5fb, 1 "ÿ

1ÿ,4-t.,.ÿ ÿ -.-3 ""ÿ"

i iÿ"P,,4?<.<.L9 ÿ.i " ' .....

,.gÿR

g-- I !,',,ÿÿ-...... 7 ÿs,4.ÿc501 =

- 1"2.,Ot\X.B :- g:ÿ ,0:ÿ'ÿ

. = I, O0 0.ÿ, ... ÿ, 0-4

0 " I'@' q°ÿq x'2 ' "51..9q'ÿ

J'--- gosh< 1 -

74. A compound is 75.46% carbon, 4.43% hydrogen, and 20.10% oxygen by mass. It has a molecularweight of 318.31 g/tool. What is the empirical and molecular formula for this compound?

s.'Juÿ CI t ÿ'ÿtOO-

-ÿ-L<Z-:---'ÿ--qi .- ¢:,,ÿcÿ ÿ--'! cÿ b

-- ._- , _./

i,ÿ@

lO

_ =7% O.--!.'_.k2: Ix ,,...::--

12.,oItXÿO- la.O, II

is,qqg x 2.-_ -ÿ1 ,gq $

!i']

//i

i/

Electrons ....................................

75.If an electron moves farther from the nucleus, it has ÿOÿ ÿ S energy.

76. To emit energy, electrons move to a lower energy level, which is to the

nucleus. ÿ,

77. Who developed the quantum mechanical model? -_ÿ ÿfÿ fÿ O ÿ ÿ ÿl ÿ

78. Who developed the planetary model? ÿ2 .O ÿ ÿ , ÿ •79. Wÿt was incorrect about Bohr's model? ÿ! O_ÿC-ÿD[ÿ ÿ dÿO!ÿ-]ÿ'i "ÿ-ÿÿ/ÿ:;1ÿ:ÿ:ÿÿ_.,,,_

8 0. E Z pl' a ÿ. t h" quantum mechanical model. _ÿ ÿ-ÿtrÿ.

8L How many electrons can occupy each atomic orbital? ÿ <ÿ i ÿ-ÿ_ÿ

82. What percent chance do you have of f nd ng an electro, orb,tal,

83. How many orbitals are found ÿin a d-sublevel? 584. The letter, n, is used to represent theÿlÿerÿ, i...ÿ. ÿ -! In other words, n =2 is

the same thing as saying the second energy levee

85. How many electrons can occupy a f-sublevel? !/-ÿ.

86. Which sublevel has a spherical shape, ÿ' Dumb bell shape, p87. For the electron configuration, ls2;ÿ;ÿ)how many electrons are in the second energy level? -ÿ

88. For the electron configuration, ts22ÿ3s(ÿ4sÿ3d5, how many electrons are in p sublevels? ÿ_ÿ

89. State Hund's Rule.

90. State Pauli's Exclusion Principle.P, e tec-+ s,

91. State the Aufbau Principle.

92. Which two elemÿs have eÿeectron conVÿiguratiÿnÿnat are exceptions to the rules, Write theiri

name AND &ymbo[ 7 -' - :ÿ ÿ'' "> zÿ l <: I "ÿ'1 l ÿ ÿn,,-, ÿ -ÿ-q,ÿ -ÿ,,

"9 ""ÿ %ÿ " | "-7 .

93. Write the electron configuration for each of the following elements.

/S#ÿ) a. Titanium (Ti)

-ÿg[)b. Tungsten (W)

'?__..C[)c. Copper (Cu) - - i - "

%

36. Which has more energy: red light or violet light?

37. What element has an electron configuration that ends in 5p2?

38. What element has an electron configuration: [Xe]6s24f145d47

39. What element has the electron configuration, 1s22s22p63sZ3p2?

40. How many energy levels are found in a potassium atom?

(

41. Write the complete electron configuration for radon.

42. Write the noble gas electron configuration (short hand) for indium.

l: nr] J

a. How many electrons are on the outermost energy level of indium?

343. Draw the orbital diagram for Lithium.

Iÿÿ' ÿ /ÿ,85

44. Draw the orbital diagram for Chlorine.

45. What is

5,'so x lo'') :ÿ 3,'sv :ÿ ,dÿ'JÿI'

46. A mercury lamp emits radiation with a frequency of 5.62 xIOz4 Hz. Calculate the wavelength of

this radiation.

coÿ;L

4'

o¢: 5,ooxÿO_..ÿ

:,5,6 3x ÿ (.:,'ÿ

Periodic Trends

107. Oxygen and tellurium are both in Group 16. What two things will they have in common?

cl C- 3. nonmcNls

108. Why are noble gases not assigned an electronegativity value?

uJI.

109.

110.

111.

What is the family name for group 17 elements?

t4aloÿosWhat is the ?amily name for the elements in group 2Aÿ

@ltÿali ¢arLhOrder the elements Fo Seo S and Cs in order of increasing ionization energy.

Os112. Which of the following groups has the highest electronegativity?

a. 1A

b. 2A

113.

114.

Rank the elements in order of decreasing electronegativity: Ru, CI, Na, Te, F

Circle all of the trends going down a group of the periodic table that are correct?a. atomic size decreases

b. reactivity of metals decreases

c. electronegativity increases

Q ionization energy decreasestOmic size increaseslectronegativity decreases

g. ionization energy increaseshÿ. reactivity of nonmetals decreases

eactivity of metals increasesj. reactivity of nonmetals increases

115.

116.

kthe following atoms in order of decreasing atomic radi s: F, Rb, Br, Sr, I

What element is found in group 14 and on period 4 of the periodic table?

117. Ions aren't the same size as the atoms they come from. Compare the sizes of sodium and

chloride ions with the sizes of sodium and chlorine atoms.

Cations (gain,lose)electrons causing the atom to get (larger,smaller) while anions (gain,lose)electrons, causing the atom to get (larger,smaller).

With this !nformation, waulÿr p-3, be smaller?

woulÿr K -1, be smaller?

IWith this information,

118.

119.120.121.

Circle the element with the largest radius: Ca,ÿJor MÿCircle the element that is the most reactive: CI, O, or FÿCircle the element with the greatest ionization energy: Na, MgCircle the element with the smallest electronegativity: Be, Mg, oÿ

LUC QoelGreat Job!!!! NOW STUDY...and Good kllll

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