Final Exam Review Day 1 Name __________________

Classify the following matter as an element, a compound or a mixture.

1. ____HCl 3. ____ Cl2 (g) 5. ____ barium

2 ____ HCl (aq) 4. ____ diet coke 6. ____ calcium nitrate

Classify the following matter as a pure substance or a mixture

1. ____ Na2CO3 (s) 3. ____ air 5. ____ dirt

2. ____ Na2CO3 (aq) 4. ____ helium 6. ____ H2O (l)

Classify the following matter as homogeneous or heterogeneous.

1. ____ tossed salad 3. ____ stainless steel 5. ____ Ca(OH)2 (aq)

2. ____ Cl2 4. ____ saline solution 6. ____ MgSO4 (s)

Classify the following as a physical change or a chemical change.

1. __________ dissolving sugar into water

2. __________ burning gas

3. __________ decompose water into hydrogen and oxygen

4. __________ evaporate water

Units of measurement

cm3, L or mL is __________________

g is _______________________

g/cm3, g/l or g/mL are ________________

joules , calories, kcal is ______________________

K or ºC is _____________________________

Temperature conversions

ºC = K – 273 20º C = __________K

Metric Conversions

________ mm = 1 m ___________ cm = 1m __________ m = 1 km

Significant Figures

1. Reading Instruments Properly – give all figures known and estimate the last one

2. Determine the number of significant figures in the following measurements.

a) 87 000 000 000 __________

b) 0.000 607 0 __________

c) 320.00 __________

3. Calculate each of the following. Report answers using significant figures.

a) (4.15 × 105) m × (6.024 × 1023) m

b) __________3.56_g__________ 3.6 cm × 2.5 cm × 5.2215 cm

c) 18.63 g + 5.2 g

Density D = M /V

Calculate the density of an object measuring 21 cm by 6.0 cm by 2.12 cm and having a mass of 522.2 grams

A piece of granite has a mass of 55 g. When I place it into a graduated cylinder that has 50.0 mL of water in it the level changes to 70.0 mL. What is the density of this piece of granite?

Conversions

Given: 1 joule = 0.239 calorie. Convert 630 joules to calories.

Subatomic Particles and their Jobs

# protons = atomic number (identifies the element)neutrons define the mass of the atom # protons + neutrons = mass number# electrons determines the charge

Fill in the following table.

Symbol Atomic Number

Protons Neutrons Electrons Mass Number

Xe 77

Ba-137

27 33 27

Na+ 22

55Mn 25

17 18 36

15O-2

Write the complete chemical symbol for the ion with 31 protons, 39 neutrons, and 28 electrons.

Iron consists of four natural isotopes:

Isotope Mass (amu) Percent Abundance54Fe 53.9696 5.8256Fe 55.9349 91.6657Fe 56.9354 2.1958Fe 57.9333 0.33Calculate the atomic mass of iron to five significant digits.

Convert the following

1. 45.6 g Mg to atoms

2. 45.9 moles gold to g

3. 78.3 g Pb to atoms

Final Exam Review Day 2 Name_________________

Electron Configuration (shows where all the ______________ are located)Diagonal rule 1s2

2s2 2p6

3s2 3p6 3d10

4s2 4p6 4d10 4f14

5s2 5p6 5d10 5f14

6s2 6p6 6d10 6f14

7s2 7p6 7d10 7f14

Draw the electron configuration for the following:Potassium

Sulfur

Cobalt

P−3

Mg+2

Valence electrons are electrons in the outer shell.

Draw the dot diagrams for the following:

Potassium Sulfur P−3 Mg+2

Draw the shortcut electron configuration for each of the followingPotassium

Sulfur

Cobalt

P−3

Mg+2

Identify the following [Xe]4f 46s2

contains 3 electrons in its sixth and outer main energy level the element that has 2 electrons in the p sublevel in its second main energy level4s24p5

Be able to locate s, p, d, and f blocks on the periodic tableThe ___________ ____________ _____________ is the same as the period number.There are ________ main energy levels. The ____________ ___________ _________is caused when electrons emit energy as they fall back to a lower energy level.

Periodic TableKnow the name and location of the following groups

Group 1 ___________________ Group 2 _____________________Group 3-13 ___________________ Group 17 _____________________Group 18 ___________________

The Noble gases are stable because they have ___ ______________ ____________.Elements are placed in order of ______________ _______________ and placed in groups according to their ___________________ __________________.

Rows = ______________ =___________ __________ _______Columns =______________ = _______________Metals are located _________________________________Nonmetals are located______________________________Metalloids are located __________________________________

Metals _____________ electrons. They form __________________.Nonmetals ______________________ electrons. They form __________.

TrendsAtomic radius (size)

ionization energy (energy to remove an electron)

Electronegativity (ability to gain an electron)

Reactivity for metal (metallic character)

Reactivity for nonmetal

a) F Se is more reactive.b) K Na is the smaller atom.c) C O has the higher ionization energy.d) Ba B has only s electrons in its outer shelle) Si I has 4 valence electronsf) N Cs is a metalg) Mn Cl last electron is d5

h) Mg S goes to a charge of −2i) Ge Br has higher electronegativityj) Fe Sb is a metalloidk) Be F is a halogenl) Ca Mg is more reactivem) Na I is more likely to combine with oxygenn) Rb Sr loses electrons more readilyo) Au Pb is a transition metal

Chemical BondingThe three types of chemical bonds are 1. _________________ usually between a ___________ and a ___________.

There is a __________ of electrons.2. _________________ usually between a ___________ and a ___________. The

electrons are _____________.a) _____________ _______________ between 2 same nonmetals. Electrons are ____________ shared.b) _____________ _______________ between 2 different nonmetals. Electrons are ____________ shared.

3. _________________ usually between a ___________ and a ___________. Many electrons are shared. They are ______________.

Characteristics of ionic vs covalent. Ionic bonds are strong. Ionic substances have orderly pattern and a high ____________ ___________. They form ______________.

Lewis StructuresPredict the type of bonding. Draw Lewis structures for molecules or polyatomic ion. Predict the shape names. Predict the intermolecular force for the molecules.

CCl4 SiO2

BaCl2 H2O

CO3−2 NH3

What is an intermolecular force? What are the three types of intermolecular forces? What is the strongest type?

Final Exam Review Day 3 Name_________________

Calculate the oxidation numbers of the atoms in each of the following compounds or polyatomic ions:

H3AsO4 H2Cr2O7

TiO2 SO3−2

Calculate the molar mass of the followingCaCl2 (NH4)2CO3 Mn3(PO4)2

Convert each of the following.a. 5.6 × 1026 molecules NaOH to grams NaOH

b. 45g KClO3 to moles KClO3

c. 7.4 moles Sn(SO4)2 to molecules

d. 3.25 moles (NH4)2CO3 to grams

Find the % composition by mass of each element in Fe3(PO4)2.

A compound contains 68.04 g N and 155.52 g O. Find its empirical formula.

A compound contains 68.04 g N and 155.52 g O. Its molar mass is 82 g. Find its molecular formula.

Naming Compounds and writing formulasBinary Ionic MgCl2

CuCl2

Tertiary Ionic MgSO4

Covalent CO2

Binary acids HI (aq)

Oxyacids HNO3 (aq)

HNO2 (aq)

Write the formula for each of the following substances:Strontium hypobromite Phosphorus trichloride

Sodium chromite aluminum sulfite

Magnesium nitrite chloride

Calcium sulfide iron (II) hydroxide

Sulfuric acid hydrosulfuric acid

Phosphorus trioxide hydrogen

Name the following substances

HCl (aq) CaO

F2 NO

H3PO4 (aq) NaClO3

SO2 SO2−2

Recognize an acid, a base a salt and other:

MgSO4 _____ C6H12O6 _____ HCl _____ NaOH _____

Chemical Reactions:Synthesis (element + element → compound) Mg (s) + O2 (g) →

Decomposition (compound → element + element) HgO (s) →

Single replacement (element + cpd→element + cpd) K + Ni(NO3)2 →

Double replacement (cpd + cpd → cpd + cpd) Pb(NO3)2 + NaBr →

Combustion (CxHy + O2 → CO2 + H2O) C3H8 + O2 →

Neutralization (acid + base → salt + water) LiOH + H2SO4 →

Classify and balance the following.________ 1. BaCl2 + (NH4)2CO3 → BaCO3 + NH4Cl

________ 2. KClO3 → KCl + O2

________ 3. Na2O + P4O10 → Na3PO4

________ 4. C6H6 + O2 → CO2 + H2O

________ 5. FeCl2 (aq) + Na3PO4 (aq) → Fe3(PO4)2 (s) + NaCl (aq)

What do the symbols (s), (l), (g) and (aq) mean?

Which substances in question 5 are solutions?

What are the reactants in question 5?

What are the products in question 5?

What is the subscript of oxygen in question #4?

What is the coefficient of oxygen in question #4?

Stoichiometry1. Given the following: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)

a) How many moles of C3H8 are needed to produce 9 moles of CO2?

b) How many grams of CO2 are produced when 2.0 moles of C3H8 react with excess oxygen?

c) How many grams of oxygen are needed to react with 22.0 g C3H8?

d) How many grams of oxygen are needed to react with 3.48 liters of C3H8 at STP?

2. Given the following: 2 Na + Cl2 → 2 NaCl

(a) If 23.0 g Na and 71.0 g Cl2 react, what is the theoretical mass of NaCl produced? Why? What is the limiting reactant? What is the

excess reactant?

b) An excess of sodium is reacted with 142 g Cl2. If 199 g of NaCl are actually produced, what is the percent yield?

3. Aluminum reacts with hydrochloric acid according to the following unbalanced equation: 2 Al + 6 HCl → 2 AlCl3 + 3 H2

(a) If 18 g Al are combined with 75 g HCl, which reactant is the limiting reactant?

(b) What mass of AlCl3 is theoretically formed?

(c) An excess of HCl is reacted with 52 g of Al. If 5.0 g H2 are actually produced, what is the percent yield?

Final Exam Review Day 4 Name_________________

Gas Laws

Kinetic Molecular Theory assumes gases are made up of _________ ___________moving in _____________ ___________, colliding into each other with ______________ collisions.

Ideal vs Real : Non-ideal behavior occurs when gases stop moving (or move slowly)That is at _________ temperatures and __________ pressures.

P1V1 = P2V2 PV = nRT Ptot = P1 + P2 + P3 … T1 T2

STP means 1 atm (760 mm Hg) and 273 K

1. A sample of gas occupies 400.0 mL at a pressure of 1 atm. What will the volume be if the pressure is changed to 2 atm while the temperature remains constant?

2. Calculate the volume occupied by 64.0 grams of O2 at a pressure of 850 torr and a temperature of 25C.

3. A gas occupies 250 mL at STP. It expands to 375 mL as it is heated to 75ºC. What is the new pressure?

4. A gas sample is collected over water when at a pressure of 760 mm Hg. What is the pressure of the dry gas if the partial pressure of the water vapor is 11.5 mm Hg?

5. Calculate the number of grams of N2 in a 6.0 liter cylinder at 27C and 800 torr.

Gas Stoichiometry

1. Given: 2 H2(g) + O2(g) → 2 H2O(g)

If this reaction occurs at 200C and 1500 torr, how many liters of O2 will react with 20.0 L of H2?

2. Given: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)

How many liters of CO2 at 500C and 850 torr are produced from 6.60 g C3H8?

Phases and Phase Diagrams

Solids Liquids Gases

Definite shape

Definite Volume

Fluidity

Particle movement (KE)

Particle arrangement

Attractive forces

Density

Diffusion rate

Compressibility

Heat Calculations

Q = m∙Cp∙∆T Q = m∙∆H

1. What quantity of heat, in joules, is required to raise the temperature of 22.5 g of lead from 18°C to 30°C? The specific heat of lead is 0.129 J/g·°C.

2. Calculate the quantity of heat energy (to the nearest calorie) required to convert 50.0 g of ice at 0°C to steam at 110°C. Be sure to draw a diagram showing the temperature and phase changes and the heat energy increases.

Specific heats: water = 1.00 cal/g·°C steam = 0.480 cal/g·°C

∆Hvap = 540 cal/g; ∆Hfus = 80 cal/g

Final Exam Review Day 5 Name_________________

Concentration% by mass = g solute × 100 Molarity (M) = moles solutes g solution Liter solution

1. Calculate the molarity of 95.0 grams of Al(OH)3 dissolved in 500. mL of solution.

2. Calculate the % of a solution containing 35 g NaCl in 110 g H2O.

3. Calculate the % concentration by mass of a solution in which 20 g Mg(OH)2 is dissolved in 80 g H2O.

Solubility

1. What is the solubility of KCLO3 at 30 ºC?

2. 50 g of KCl are added to 100 g of water at 40°C. Is the solution saturated or unsaturated?

If saturated, how many more grams of KCl remain undissolved?

If unsaturated, how many more grams of KCl could be dissolved?

3. How does temperature affect the solubility of a solid in a liquid?

Dilutions: C1V1 = C2V2

How many mL of a 12.0 M HCl solution are needed to make 100 mL of a 1.0 M HCl solution?

Ions in solution

1. Write an equation showing the dissociation of AlCl3 in water.

2. For the following write (a) the ionic equation; and (b) the net ionic equation.

formula equation: 2 AlCl3(aq) + 3 Na2CO3(aq) → Al2(CO3)3(s) + 6 NaCl (aq)

ionic equation:

net ionic equation:

3. Write an equation showing the ionization of H3PO4 in water.

4. Which of the following are electrolytes?

CaBr2 CH4 Ca(OH)2 Na3PO4 HF

Acids and Bases

Be able to identify a neutralization reaction.

1. Calculate the Normality of: Normality (N) = M × Subscript of H+ or OH−

a. 0.45 M H2SO4 b. 0.82 M Ca(OH)2

2. Calculate the pH of a 0.0052 M solution of HCl. pH = − log (N of acid)

3. In an aqueous solution if H3O+ = 1 10 −5, then OH− = ________, pH=

______, and pOH =______. pH + pOH = 14

Know pH scale |-----------------|-----------------|

acid ← 7 → base

Acids donate a proton. Bases accept a proton.

Indicate each of the following as an acid, base, or salt:

H2SO4 KBr HNO3 Ba(OH)2 Na2SO4

Properties of acid Properties of base1. 1.

2. 2.

3. 3.

4. 4.

5. 5.

Titration: N1V1 = N2V2

How many mL of 0.15 N KOH are needed to neutralize 50.0 mL N H2S, if both completely break into ions?

Final Exam Review Day 6 Name____________________

Equilibrium Keq= Products reactants

1. Given: A(g) + 2 B(g) → AB2(g) + heat

Write the equation for the equilibrium constant, Keq.

If at equilibrium the concentrations are: [A] = 1.2 × 10−2 M; [B] = 2.0 × 10−2 M;[AB2] = 1.5 × 10−5 M ; calculate the value of the equilibrium constant.

Is the reaction endothermic or exothermic?

2. For the same equation given above, predict the effect of the following (get more products, get more reactants, or no effect on the amount of products or reactants)

Adding more B Removing some A

Heating decreasing the pressure

Adding a catalyst removing AB2

3. Ksp = products The higher the Ksp the greater the solubility.

For the reaction: Al(OH)3 (s) → Al+3 (aq) + 3 OH−1(aq)

Write the expression for the solubility product, Ksp.

4. Name 4 ways to increase reaction rate.

5. What must you have in order for a reaction to occur?

Heat in reactionsRefer to the following diagram for the hypothetical reactions:

1. Is the reaction endothermic or exothermic?

(a) (b)

2. What is the value for the activation energy for the forward reaction?

(a) (b)

3. What is the value of ∆H for the reaction?

(a) (b)

Oxidation and Reduction

Oxidation = _______ of electrons

Reduction = _______ of electrons

The oxidizing agent caused the oxidation. (It was reduced)The reducing agent caused the reduction. (It was oxidized)

KNO3 + CO → CO2 + NO2 + K2O

Assign oxidation numbers to the elements in each substance.

___________ was oxidized.

___________ was reduced.

___________ was the reducing agent.

___________ was the oxidizing agent.

Time

Energy

Time

Energy