Name ______________________________

Period _______

HONORS CHEMISTRY FINAL REVIEW

Final Exam: approximately 75 multiple choice questions (scantron) worth 20% of

your semester grade

x Ch.3 - Scientific Measurement

x Ch. 1 & 2 - Matter and Change

x Ch. 4 & 6 - Atomic Structure

x Ch. 25 - Nuclear Chemistry

x Ch. 9 - Naming Compounds

x Ch. 10 - The Mole

x Ch. 11 – Chemical Reactions

On the final exam day, you will need:

x a pencil with a good eraser

x a scientific calculator

On the final exam day, you will be given:

x a periodic table

x scrap paper

Study Tips: 1) Complete the review packet.

2) Find all old tests and quizzes. Read them, study them, and correct mistakes.

3) Read and highlight important topics in your notes.

4) Make a list of things you must memorize for the final: equations (density, radioactivity,

avogadro’s number, etc.) polyatomic ions, vocabulary.

Chapter 3: Scientific Measurement Perform the following conversions:

a. How many kilometers are in 22.4 cm? __2.24x10-4

______________

b. How many microliters are in 5.662 L? __5.662x106______________

c. How many milligrams are in 3.4 ng? __3.4x10-6

______________

d. How many nanometers are in 230 cm? __2.3x109______________

Perform the following temperature conversions:

a. 36ºC = __309_______K c. 962K = ___689______ ºC

b. 112 ºC = _385________K d. 1134K = __861_______ ºC

Determine how many sig figs are in each number:

a. 3300.2 __5______ c. 0.00005003 ___4_____ e. 10,000 __1______

b. 2,000,000 _1_______ d. 30 ___1_____ f. 400.0 ___4_____

Using the rules of significant figures, calculate the following:

a. 22.44 + 3.8 _26.2______ c. 12.6 x 0.53 _6.7_______ e. 6.112 x 7.1 __43______

b. 672.55 – 3.18 669.37______ d. 298.4/0.6 __500______ f. 25.36-4.15 _21.21____

Put the following numbers in standard scientific notation:

a. 357 ___3.57x102__ c. 0.000403 __4.03x10

-4___________

b. 238,000 ___2.38x105______ d. 510,000,000 _5.1x10

8____________

What is accuracy? ________________________________________________________________

What is precision? ________________________________________________________________

Look at the dart boards below. Determine if the person has good accuracy or precision. (Circle all that apply)

accuracy accuracy accuracy

precision precision precision

What is the formula used to calculate density? __d = m/v_______

What is the density of a metal that weighs 24.888g and displaces 2.810mL of water? 8.857g/mL

What is the mass of a substance with a volume of 56.0mL and a density of 23.1g/mL? 1290g

What is the volume of a substance that weighs 15.8g and has a density of 0.81g/mL? 20.mL

Use dimensional analysis to convert 32.8 in to nanometers (1 in = 2.54cm) 8.33x108nm

Ch. 1 & 2 Matter & Energy What is a physical change? _______________________________________________________

What is a chemical change? ______________________________________________________

Identify each of the following as a physical(P) or chemical(C) change:

a. iron metal is melted ___p___ c. burning wood __c____ e. water evaporating _p_____

b. iron rusts ___c___ d. breaking a pencil __p____ f. dissolving Kool-aid __p____

What is the difference between heterogeneous and homogeneous mixtures? _________________________

_____________________________________________________________________________________

Identify each of the following as an element, compound, homogeneous, or heterogeneous mixture:

Potting soil hetero window glass homo

Aluminum metal element your sock drawer hetero

List the seven diatomic elements:

Define heat:

Define specific heat:

Convert the following: 63.4 cal = 265 J 833 J = 199 cal

How much energy (in joules) is required to heat a piece of aluminum weighing 1.30g from 25.0oC to 46.0

oC?

24.3J

Ch. 4 & 6: Atomic Structure List the three parts of an atom. Include their location, charge, and relative mass.

Subatomic Particle Location Charge Relative

Mass

Proton Nucleus +1 1

Neutron nucleus 0 1

electron Electron cloud -1 0

Which two subatomic particles contribute to an atom’s mass? __proton_____________ & __neutron________

Complete the following atom table:

Symbol Atomic

Number Mass Protons Electrons Neutrons

S 16 32 16 16 16

Ba 56 137 56 56 81

K 19 39 19 19 20

Hg 80 201 80 80 121

Mg 12 24 12 12 12

Complete the following isotope table:

Isotope

Name

Isotope

Symbol

Atomic

Number Mass Protons Neutrons

Cu-65 65

Cu 29 65 29 36

Po-210 210

84Po 84 210 84 126

U-234 234

U 92 234 92 142

C-14 14

C 6 14 6 8

Complete the following ion table:

Atom # Electrons

(atom) change in e-

# electrons

(ion) Formula Ion Name

O 8 Gains 2 10 O-2

Oxide

F 9 Gain1 10 F-1

Fluoride

Ba 56 Lose 2 54 Ba+2

Barium ion

K 19 Lose 1 18 K+

Potassium ion

Al 13 Lose 3 10 Al+3

Aluminum ion

Cl 17 Gain1 18 Cl-

chloride

Ca 20 Lose 2 18 Ca+2

calcium ion

Elements in group 1A(1) are called: ________alkali metals___________________

Elements in group 2A(2) are called: ________alkaline earth metals___________________

Elements in group 7A(17) are called: ________halogens___________________

Elements in group 8A(18) are called: ________noble gases___________________

Where are the inner transition metals located on the periodic table? ____bottom 2 rows_________________

Give 3 examples of transition metals: ______________, ______________, ______________

Give 3 examples of inner transition metals: ______________, ______________, ______________

Cations are atoms that have ____lost__________ electrons. They have a ___positive____________ charge.

Anions are atoms that have ____gain___________ electrons. They have a ___negative____________ charge.

Calculate the atomic mass for an element that has the following isotopes:

S-32 (95.02%) S-33 (0.75%) S-34 (the rest of the time)

32.10

Ch 25: Nuclear Chemistry

What is radioactivity? __________________________________________________________________

Write the correct symbol for each type of radioactive decay:

Alpha Emission: __4He_or α______ Beta Emission: _-1e or β_________

Positron Emission: __+1e__or β+______ Gamma Emission: __γ________

Which type of decay consists of pure energy released from the nucleus? ____γ______________________

Show the alpha and gamma emission of Ra-222: __222

Rn → 218

Ra + α + γ_____________________

Show the beta decay of C-14: __14

C → 14

N + β______________________________

Show the positron and gamma reaction of O-18: __18

_O → β+ +

18N

+ γ___________________________

Cu-66 converts to Zn-66 through what type of emission? Show your work. __________β______________

Describe the type of materials needed to shield each type of radiation:

ALPHA __paper & clothing______ BETA __wood & Al_________ GAMMA __Pb & concrete_________

What is the resulting atom made from the following transmutations?

a. 246

Am +

18

O ---------) ___

260Lr_____ + 4 (

1

0 n)

b. 9Be +

4He ---------)

12C + _

1n____

The half-life of Sr-90 is 80 days. Calculate the amount remaining of a 250g sample after 560 days have passed.

1.95

How much Po-210 remains if 8.0 grams of Po-210 decays over 690 days? The half-life of Po-210 is 136 days.

0.25

What is half-life? _________________________________________________________________________

What is the half-life when 12.0g of an isotope decays into 0.75g over a period of 340 days?

85 days

What is fusion? __________________________________________________________________________

What is fission? __________________________________________________________________________

Ch. 9 Nomenclature Name the following compounds. *Use roman numerals when appropriate.

a. NaF __sodium fluoride___ b. Ca(HCO3)2 __calcium bicarbontae_____

c. PbO _lead(II) oxide____________ d. Fe3N

2 __iron(III) nitride_________

e. KNO2

_potassium nitrite_________ f. Sr3(PO4) 2 __strontium phosphate_____

i. AgClO2 _silver chlorite______________ j. KOH _potassium hydroxide________

k. BaC2O4 _barium oxalate_________________ l. SnSO4 _tin(II) sulfate_________________

Write formulas for the following ionic compounds:

a. lithium phosphide _Li3P__________ b. chromium (VI) sulfite _Cr(SO3)3__________

c. barium nitrate __Ba(NO3)2________ d. silver chloride _AgCl__________

e. aluminum selenide __Al2Se3_________ f. copper(I) oxalate _Cu2C2O4__________

g. zinc iodide __ZnI2_________ h. manganese(VII) nitride _Mn3N7__________

Name or write the formula of the following molecular compounds:

a. N2O5 dinitrogen pentaoxide b. PO8 phosphorus octaoxide

c. CO carbon monoxide d. S3O6 trisulfur hexaoxide

e. carbon tetrachloride CCl4 f. tribromine nonaiodide Br3I9

Name or write the formula for these acids: HClO3 __chloric acid___________ H2SO3 _sulfurous acid______________

hydrophosphoric acid _H3P__________ phosphorous acid _H3PO3________ HBr__hydrobromous acid__________

Know organic compound names and formulas (alkanes)

Ch. 10 The Mole Define each of the following:

gram molar mass

mole

Avagadro’s number Percent composition

Empicial formula

1 mole = 22.4 L , molar mass , 6.02x1023

particles

Determine the mass of one mole of each of the following:

K = 39 (NH4)2SO3 = 116

H2SO4 = 98 Al(NO3)3 = 213

How many sodium ions are in 117g of sodium oxide?

2.27x1024

ion

How many atoms of zinc are in 9.3g?

8.6x1022

atoms

What are the mass percents of each element in iron(III) acetate heptahydrate?

Fe = 15.6%, C = 20.1%, H = 6.4%, O = 57.9%

Determine the molecular formula of the compound with an empirical formula of CH and a formula mass of 78.110g.

C6H6

Ch. 11 Writing and Balancing Reactions

x You must know your FORMULAS of any possible compound; ionic, molecular, organic, or acid

1. Write and balance the following reactions:

a. propane gas burns in oxygen

3CO2 + 4H2O

b. magnesium and sulfuric acid mix

MgSO4 + H2

c. sodium metal reacts with water

2NaOH + H2

d. silver carbonate is heated

Ag2O + CO2

e. tin(+2) is dropped in water

no reaction

f. sodium carbonate and barium chlorate mix

BaCO3↓ + 2NaClO3

g. ammonium hydroxide and hydrobromic acid mix

NH4Br + H2O

h. phosphorus combines with magnesium metal

Mg3P2

g. aluminum hydroxide is heated

Al2O3 + 3H2O

i. lithium reacts with barium carbonate

Li2CO3 + Ba