Final Exam Review Day 1

Final Exam Review Day 1Name ______

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

1. ____HCl3. ____ Cl2 (g)5. ____ barium

2 ____ HCl (aq)4. ____ diet coke6. ____ calcium nitrate

Classify the following matter as a pure substance or a mixture

1. ____ Na2CO3(s)3. ____ air5. ____ dirt

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

Classify the following matter as homogeneous or heterogeneous.

1. ____ tossed salad3. ____ stainless steel5. ____ Ca(OH)2(aq)

2. ____ Cl24. ____ saline solution6. ____ MgSO4(s)

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

______dissolving sugar into water
______burning gas
______decompose water into hydrogen and oxygen
______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 – 27320º 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

DensityD = 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 Abundance
54Fe / 53.9696 / 5.82
56Fe / 55.9349 / 91.66
57Fe / 56.9354 / 2.19
58Fe / 57.9333 / 0.33

Calculate 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 2Name______

Electron Configuration (shows where all the ______are located)

Diagonal rule1s2

2s22p6

3s23p63d10

4s24p64d104f14

5s25p65d105f14

6s26p66d106f14

7s27p67d107f14

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:

PotassiumSulfurP−3Mg+2

Draw the shortcut electron configuration for each of the following

Potassium

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 level

4s24p5

Be able to locate s, p, d, and f blocks on the periodic table

The ______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 Table

Know 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 ______.

Trends

Atomic 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 Seis more reactive.

b)KNais the smaller atom.

c)COhas the higher ionization energy.

d)BaBhas only s electrons in its outer shell

e)SiIhas 4 valence electrons

f)NCsis a metal

g)MnCllast electron is d5

h)MgSgoes to a charge of −2

i)GeBrhas higher electronegativity

j)FeSbis a metalloid

k)BeFis a halogen

l)CaMgis more reactive

m)NaIis more likely to combine with oxygen

n)RbSrloses electrons more readily

o)AuPbis a transition metal

Chemical Bonding

The 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 Structures

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

CCl4SiO2

BaCl2H2O

CO3−2NH3

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

Final Exam Review Day 3Name______

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

H3AsO4H2Cr2O7

TiO2SO3−2

Calculate the molar mass of the following

CaCl2(NH4)2CO3Mn3(PO4)2

Convert each of the following.

a.5.6 × 1026 molecules NaOH to gramsNaOH

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 formulas

Binary IonicMgCl2

CuCl2

Tertiary IonicMgSO4

CovalentCO2

Binary acidsHI (aq)

OxyacidsHNO3(aq)

HNO2(aq)

Write the formula for each of the following substances:

Strontium hypobromitePhosphorus trichloride

Sodium chromitealuminum sulfite

Magnesium nitritechloride

Calcium sulfideiron (II) hydroxide

Sulfuric acidhydrosulfuric acid

Phosphorus trioxidehydrogen

Name the following substances

HCl (aq)CaO

F2NO

H3PO4(aq)NaClO3

SO2SO2−2

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?

Stoichiometry

1.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 C3H8react 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 4Name______

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 = P2V2PV = nRTPtot = 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 25C.

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 27C and 800 torr.

Gas Stoichiometry

1.Given:2 H2(g) + O2(g) → 2 H2O(g)

If this reaction occurs at 200C 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 500C 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∙∆TQ = 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 5Name______

Concentration

% by mass = g solute × 100Molarity (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?

CaBr2CH4Ca(OH)2Na3PO4HF

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 H2SO4b.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:

H2SO4KBrHNO3Ba(OH)2Na2SO4

Properties of acidProperties of base

1.1.

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 6Name______

EquilibriumKeq= 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 × 10−2M; [B] = 2.0 × 10−2M;

[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 BRemoving some A

Heatingdecreasing the pressure

Adding a catalystremoving 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 reactions

Refer 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.