name: _____________ date: ...

Name: _________________________ Date: ____________ Period: ________

Study Guide (Semester 2)

To be able to name a compound based on its formula (IUPAC).

Directions: Hook together the following ions to write the correct formula and place the name of the resulting compound in the box

Fluorine Oxygen Phosphate

Lithium

Beryllium

Gallium

Ammonium

Directions: Name the following compounds:

1. FeCl3 ______________________________

2. CdSe ______________________________

3. TiO2 ______________________________

4. V2O5 ______________________________

5. ZnBr2 ______________________________

Directions: Name the following Molecules

1. CO _________________________________

2. PCl5 _________________________________

3. N2O _________________________________

4. P2O5 _________________________________

5. CS2 _________________________________

To be able to write the formula of a compound based on its name.

Directions: Write the formula:

1. Tin (IV) Chloride: ____________________________

2. Cobalt (III) Oxide: ____________________________

3. Vanadium (III) Chloride: ____________________________

4. Gold (I) Sulfide: ____________________________

5. Manganese (II) Sulfite: ____________________________

Directions: Write the Name:

1. Carbon Dioxide: _____________________

2. Dinitrogen TetraOxide: _____________________

3. Sulfur Hexachloride: _____________________

4. Oxygen Difluoride: _____________________

5. Phosphorus Tribromide: _____________________

To know the common polyatomic ions and be able to use them in formulas and names.

Directions: Write the formula.

1. Lead (II) Sulfite: __________________________

2. Copper (I) Acetate: __________________________

3. Ammonium phosphate: __________________________

4. Aluminum Hydroxide: __________________________

5. Magnesium Nitrate: __________________________

Directions: Write the name.

1. Au(HCO3)3 : _____________________________________

2. Be(NO3)2: _____________________________________

3. Pb(OH)2: _____________________________________

4. K(MnO4): _____________________________________

5. Zn(SO4): _____________________________________

To be able to write a skeleton chemical equation from words.

Directions: Write a complete balanced equation for each chemical reaction. Box your answer.

1. Tin foil will oxidize when exposed to oxygen forming tin (II) oxide.

2. When solid potassium is added to water, hydrogen gas and aqueous potassium hydroxide are produced.

3. Solid calcium hydrogen carbonate reacts with hydrochloric acid to produce aqueous calcium chloride, water, and carbon dioxide gas.

4. Mercury (II) Bromide decomposes into its elements when treated with electricity.

To be able to differentiate between the five types of reactions.

Directions: Identify the following reactions as a synthesis, decomposition, combustion, single-displacement, or a double displacement.

1. _________________________ 3Ag2SO4 (aq) + 2AlCl3 6AgCl (s) + Al2(SO4)3 (aq)

2. _________________________ C4H8 (g) + 6O2 4CO2 (g) + 4H2O (l)

3. _________________________ Zn (s) + 2AgNO3 (aq) Zn(NO3)2 (aq) + 2Ag (s)

4. _________________________ 2KClO3 (s) 2KCl (s) 3O2 (g)

5. _________________________ 4Fe (s) + 3O2 (g) 2Fe2O3 (s)

To be able to properly balance chemical equations

Directions: Balance the equation and re-write the balance equation on the line given.

1. C + H2O CO + H2

Balanced Equation: __________________________________________________

2. KClO3 KCl + O2


3. H3AsO4 As2O5 + H2O


4. KClO3 KClO4 + KCl


5. Al2(SO4)3 + Ca(OH)2 Al(OH)3 + CaSO4


Complete and Balance (where possible) the following reactions or label them No Reaction (Use activation series of metals)

1. Al(OH)3 + Mg2+ ___________________________

2. LiOH + Fe2+ ___________________________

3. K+ + H2O ___________________________

4. MgS + CaCl2 ___________________________

5. Pt2+ + O2 ___________________________

To understand the concept of the mole.1.What is a mole? (Give a complete explanation)

______________________________________________________________________________

______________________________________________________________________________

______________________________________________________________________________

2. One Mole of any gas at STP will occupy ________________.

3. One Mole equals _______________________ particles.

To be able to calculate the molar mass of a compound.

4. Calculate the molar mass (AKA molecular mass) for the following:

a) : Mg(C2H3O2)2

b) Sodium Sulfite: Na2SO3

To be able to convert between moles, mass, and particles

5. Determine the number of particles for the following:a) 3.2 moles CH4

b) 23.5 g BeCl2

6. Determine the mass for the following:a) 8.2 moles NO2

b) 1.36 x 1024 molecules PCl4

To be able to solve stoichiometric calculations

Directions: Solve and label the following problems. Box your answer. (To receive credit, work must be shown)

1. How many molecules of hydrogen are produced if 13.05 g of Zn reacts with excess hydrochloric acid?

Equation: Zn + HCl ZnCl2 + H2

2. If excess sulfuric acid reacts with 3.0 moles of sodium chloride, how many grams of hydrogen chloride are produced?

Equation: NaCl + H2SO4 HCl + Na2SO4

3. If 24.2 g chlorine gas reacts with a solution containing 32.8 g of potassium bromide, how many grams of bromine gas can be produced? (limiting reagent, honors only)

Equation: KBr + Cl2 KCl + Br2

4. How many grams of chlorine gas must be reacted with excess sodium iodide if 32.2g of sodium chloride are needed?

Equation: NaI + Cl2 NaCl + I2

5. Aluminum metal reacts with chlorine gas to produce aluminum chloride, AlCl3.

a) Write a balance equation for the reaction.

______________________________________________________________________

b) If 12.3 g of aluminum is combined with 23.6 g of chlorine, show by calculation which substance is the limiting reactant, and calculate the theoretical yield of aluminum chloride for the reaction.

To be able to solve Gas Law Calculations and understand the behavior of gases.

1. What happens to the velocity of gas when a. temperature increase?b. temperature decrease?c. when you reach absolute zero?

2. What is the value of absolute zero?

3. What does STP stand for?a. what values does it have for pressure in the units of kPa, atm, and

mmHg

b. what values does it have for temperature in the units of K and C°.

4. State Boyles Gas Law.

5. When temperature is held constant:a. what happens to the volume of the gas if you double the pressure?

(tip P1V1 = P2V2)

b. what relationship does volume and pressure have?

6. To increase pressure of a gas in a closed container, what would you have to do to the following?

a. the number of moles

b. the temperature

c. the volume

7. What would happen to the volume of balloon if the temperature increased as a constant pressure?

8. Name and list all the major gas laws.

9. Gas Law calculation:a. At constant pressure, the volume of a gas increased from 60.0L to 130.0 when heated from 85°C. What is the final temperature? (tip: Temp. must ALWAYS be in Kelvin for gas law calculations)

b. At constant temperature, the volume of the gas increased from 5 L to 10 L, the pressure was initially 100.0 kPa. What was the final pressure?

c. At constant volume, the pressure changed from 95.0 kPa to 105.0 kPa starting at 35°C. What was the final temperature in Kelvins?

d. 55.5 mL of a gas is collected at 30°C and 85.3 kPa. What volume would the gas occupy at STP? (tip: remember STP gives you 2 more given for the problem to use)

10. Ideal Gas Lawa. A gas has a volume of 35.4 L at a temperature of 30°C and a pressure of 88.5 kPa. If Its an ideal gas, how many moles are there in the sample? (tip: R = 8.31 kPa L/ mol K)

b. You have 0.56 moles of NaCl at STP. What is the volume?

________________________________________________

Name: _________________________ Date: ____________ Period: ________

Study Guide (Semester 1 Review) To be able to differentiate between an element, a compound, and a mixture.

1) Fill in the chart and give 2 examples of each.

Examples: Examples: Examples: Examples:

____________ ____________ ____________ ___________

____________ ____________ ____________ ___________

2) For each sample of matter below, correctly classify it as a substance or a mixture.

1. Table Sugar 1. ___________________

2. Pure Sand 2. ___________________

3. Kool Aid 3. ___________________

4. Calcium 4. ___________________

5. Asphalt 5. ___________________

3) For each sample of matter below correctly classify as a homogenous mixture or a heterogeneous mixture.

1. Salt Pepper 1. _______________________

________________________________________________

Pure SubstanceMixtures

Matter

2. Fruitopia Fruit Juice 2. _______________________

3. Oil Paint 3. _______________________

4. Air 4. _______________________

5. Brass 5. _______________________

To be able to differentiate between chemical and physical properties and chemical and physical changes.

Read the following properties and changes. Decide if each one is physical (P) or chemical (C), and whether it is a property (P), or a change (C). Thus, something that is a physical change would be labeled PC.

Boiling point _____ Melting point _____

Color _____ Texture _____

Getting a haircut _____ Density _____

Acidity _____ Ice cube melting _____

Lighting a candle _____ Formation of acid rain _____

Dry ice “smoking” at a concert _____ Alka-seltzer tablets fizzing _____

Malleability _____

Flammability – the ability of an object to support combustion _____

Combustibility – the ability of an object to burn or ignite _____

To be able to determine the numbers of protons, electrons, and neutrons based on the atomic number and atomic mass number.

Element SymbolNumber of

ProtonsNumber of Electrons

Number of Neutrons

Atomic Number

Mass Number

Lithium 4

26 56

47 108

2 2

Pd 105

For each isotope tell me how many electron, protons and neutrons.

a) Nitrogen – 14 b) Nitrogen – 15

Protons: ______ Protons: ______

Electrons: _____ Electrons: _____

Neutrons: _____ Neutrons: _____

To be able to describe the electron configuration for an atom.

1. Fill in the orbitals for the following elements, and state how many unpaired electron.

a) Copper (Cu): _________ unpaired electrons

b) Bromine (Br): __________ unpaired electrons

2. Write the complete electron configuration for the elements:

a) Chlorine (Cl)

b) Tin (Sn)

3. Write the short hand method (using the noble gas configuration) for the following elements.

a) Ruthenium (Ru)

b) Iodine (I)

c) Bromine (Br)

To be able to describe the characteristics of the representative elements and areas of the periodic table.

1. Explain why electronegativity decreases as you go down the periodic table. (Must include shielding effect, energy levels, and valence electrons in your response.)

2. Explain why electronegativity increase as you go from left to right on the periodic table.

3. Explain why the size of the atom decrease as you go from left to right in the periodic table.

4. Explain why the atom gets larger as you go down the periodic table.

To be able to explain how valence electrons are involved in bonding.

1. Define Valence Electrons.

______________________________________________________________________________

______________________________________________________________________________

______________________________________________________________________________

2. How do reactions occur, and what part of the atom interacts?______________________________________________________________________________

______________________________________________________________________________

3. Reactions between atoms involve only their __________________________.

4. Define octet rule.______________________________________________________________________________

______________________________________________________________________________

5. Elements become stable by achieving the same configuration of valence electrons as one of

the __________________________________.

6. How many valence electrons are in the following atoms.

a. Flourine: ____________________________

b. Carbon: ____________________________

c. Selenium: ____________________________

d. Gallium: ____________________________

7. The electron configuration of an element is 1s22s22p63s23p4. How many valence electrons

does it have?

_______________________

8. The noble gas configuration of an element is [Ar]4s23d104p5. How many valence electrons

does it have?

______________________

To be able to describe ionic and covalent bonding.

1. Define Covalent Bond.

______________________________________________________________________________

______________________________________________________________________________

2. Define Ionic Bond

______________________________________________________________________________

______________________________________________________________________________

3. Classify as Covalent (C) or Ionic(I).

________ Weak Interparticle force.

________ Strong Interparticle force.

________ Liquid or gas at room temperature

________ Solid at room temperature.

________ Less likely to dissolve in water.

________ Elements share electrons.

________ Dissolves in water.

________ Electrolyte

________ Transfer of electrons.

________ Ions

________ Molecules

________ The strong attractive force between ions of opposite charge.

________ The attraction of two atoms for a shared pair of electrons.

________ Non-metal + Non-metal

________ Non-metal + Metal

________ KCl

________ CH4

4. Use a table of electronegativity to find the electronegativity difference between each of the following pairs of elements and to predict the kind of bond that will be formed.

a. Calcium and Fluorine _____________________________

b. Carbon and Silicon _____________________________

c. Beryllium and Sulfur _____________________________

d. Hydrogen and Germanium _____________________________

e. Zinc and Bromine _____________________________

Nuclear Chemistry

1. Write the symbol, charge, and their properties for the following basic nuclear particles

a. Alphab. Betac. Positrond. Gamma

3. Write equations for the following nuclear decay reactions.

a. Decay of polonium-218 by alpha (a) emission.

b. Decay of carbon-14 by beta (b-) emission.

Misc. Answer the following questions.

a. being warmed as a solid ___________b. being warmed as a liquid __________c. being warmed as a gas ____________d. changing from a solid to a liquid _____e. changing from a liquid to a gas ______f. What is its boiling temperature? _________________g. What is its melting temperature? _________________h. Which resgions of the graph represents kinetic energy? ______________________i. Which regions of the graph represents potential energy? _____________________

name: _________________________ date: ____________...

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