Chemistry I Honors – Semester Exam Review – Fall 2000



Honors Chemistry 3rdQuarter cumulative test review – NO RETAKES (This is your SLO Test!)

It is recommended you study - this will be a comprehensive test

• FORMAT: 4 parts: Lecture and Lab multiple choice and extended response – combination of Honors and AP type questions

• RESOURCES THAT MAY BE USED DURING THE TEST: A Periodic table, solubility table, AP equation sheet and calculator may be used

• THINGS YOU NEED MEMORIZED: You must know how to name every compound we have used this year in Honors Chemistry – ionic, covalent, acids, ions. You must know equations not listed on AP equation sheet such as density; % yield; % error; (P1V1/T1) = (P2V2/T2); M1V1=M2V2

• RESOURCES FOR STUDYING: The first semester Test Review, AP Test Review, AP Test Retake Test corrections, Gas Law Test Review, VSEPR Test Review, and this review packet provide excellent study guides. Specific topics and some sample problems are listed below. It is strongly suggested you complete this packet. It will be graded.

• Lab equipment and safety

• Know lab safety

• Be able to identify the following lab equipment: Wire mesh, scoopula, test tube, ring stand, evaporating dish, test tube brush, crucible and lid, burner, test tube, watch glass, erlenmeyer flask, funnel, pipets, test tube tongs, crucible tongs, beaker tongs, clay triangle, beaker, scale, hot plate, weigh boat, well plate, volumetric flasks, iron ring

Atomic Structure

1. Identify scientists, their experiments, discoveries and models

Matter

• Be able to determine states of matter from a solubility table

Measurement

2. Know all sig fig rules

• Be able to record the appropriate sig figs

• Know the density equation D=m/v and be able to solve for each variable

• Be able to do metric conversions, for example L to mL or g to Kg

• Be able to write numbers in scientific notation

• Be able to convert C to K (know C + 273 = K)

• Be able to identify if a measurement is accurate or precise

Electrons Configuration and color

• Be able to draw orbital, short electron (1s2), and Nobel gas configuration

• Know the electron configuration exceptions

• Know what solutions are colorless and what solutions are colored and why

Chemical Bonding and Chemical equations

• Be able to write equations by predicting products

• Be able to provide the state of matter by using a solubility table

• Be able to balance equations

• Be able to identify the type of reaction that is taking place (synthesis, decomposition, combustion, single replacement, double replacement)

• Be able to identify covalent (non metal – non metal) and ionic compounds (metal – non metal)

• Be able to identify cations and anions

• Know that molecular compounds are compounds held together with covalent bonds

Molecular Structure

• Be able to determine valence electrons

• Be able draw Lewis dot structures for molecules, ions, and molecules with resonance structures

• Be able to write AXE formulas

• Be able to identify a 3D molecule by its AXE formula

• Be able to draw Ball and Stick structures and add vectors to determine polarity

• Be able to determine the geometry and bond angle of various molecules

• Explain the main idea of the VSEPR Theory.

Nomenclature

• Know all element names and symbols covered in class – specifically elements with atomic numbers 1-36 plus the first 2 columns, the last 2 columns (halogens and Nobel gasses), and Ag, Sb, Sn, Pb, Bi

• Memorize/ use crazy L common polyatomic ions and other common polyatomic ions we use in Honors Chemistry (acetate, ammonium, hydroxide)

• Know the charges on monatomic ions

• Know the following “AP” polyatomic ions:

CrO42- Chromate ion

Cr2O72- dichromate ion

C2O42- oxalate

HO3+ hydronium ion

• Memorize the transition metals that have multiple charges.

• Know all of the diatomic molecules Br2 I2 N2 Cl2 H2 O2 F2

• Write names and formulas for: ionic compounds (without Roman numerals), ionic compounds (with Roman numerals), Ionic compounds with polyatomic ions, acids (binary and with polyatomics), and 2 nonmetals (covalently bonded – this is when you use prefixes).

• Know the 7 strong acids:

HCl hydrochloric acid

HNO3 nitric acid

H2SO4 sulfuric acid

HBr hydrobromic acid

HI hydroiodic acid

HClO3 chloric acid

HClO4 perchloric acid

Gas Laws

• Know that you must convert C to K

• Be able to rearrange gas law equations: PV=nRT and (PV)/T = (PV)/T and solve for any of these variables

• Be able to determine the final pressure in a stopcock question

• Know standard temperature and pressure, abbreviated STP. Standard temperature is defined as zero degrees Celsius (0 0C), which translates to or 273.15 degrees kelvin (273.15 0K). Standard pressure is 1 atm.

• Be able to convert from atm to torr

• Know the relationships(direct or indirect) between the variables P, V, T, n and understand what direct and indirect mean

Solution/Dilution

• Know the definition of molarity and be able to calculate the concentration of solutions

• Be able to explain how to make a solution

• Be able to do the calculations: find the number of grams needed to make a certain volume with a specified molarity

• Be able to write step by step procedure using terms volumetric flask and distilled water

• Be able to determine how much water must be added to a solution

Stoichiometry – and other math type problems

• Be able to calculate the molar mass

• Be able to calculate the percent composition

• Be able to calculate percent error

• Be able to calculate percent yield

• Be able to calculate grams from moles and moles from grams

• Be able to calculate amount of product formed

• Know the difference between theoretical and experiment yield

• Be able to use stoichiometry to find the limiting reactant

• Be able to calculate the empirical and molecular formula

• Be prepared to complete a lab calculations for a formula for a hydrate

• Be prepared to do a comprehensive problem that begins with a naming compounds, then predicting the products of a reaction, determining the type of reaction it is, balancing the equation, including states of matter, determining the limiting reactant, determining the amount of product(s) formed, determining the percent error, determining the percent yield.

The following are some practice problems covering content. It is recommended you complete these and ask questions if you are unable to do them. Study by redoing missed problems several times to ensure you understand how to complete the problems. Study - this will be a comprehensive test

• Lab equipment and safety

No sample problems are provided

Atomic Structure

3. Identify the scientists who made the following discoveries.

a. Atoms contain negative particles called electrons.

b. The mass of an electron is 9.11 ( 10-28 g.

c. Atoms contain neutral particles called neutrons.

d. Atoms contain a dense, positive nucleus.

e. Atoms are indivisible and resemble billiard balls.

4. Describe the evolution of the atomic model from the billiard ball model to the electron cloud model.

5. Complete the table for the following isotopes.

|Symbol |Zn | | | |

|Atomic # | |20 | | |

|Mass # |65 | |74 |40 |

|# of protons | | |34 | |

|# of neutrons | |21 | | |

|# of electrons | | | |18 |

Matter

6. How many P atoms are there in Fe3(PO4)2?

7. Look at the solubility table

a. What state of matter are all nitrates?

b. What states of matter are hydroxides? Give examples

Measurement

8. In a lab, the average measured density for Pre-1982 pennies was 7.98 g/cm3. Given that the literature value for the density is 8.92 g/cm3, calculate the percent error.

9. How many sig figs are in the following numbers?

|2.35 |89.70 |

|34,000 |0.0052 |

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10. Convert the following numbers into or out of scientific notation.

|548,000 |1.200 × 10-3 |

|0.0000770 |9.25 × 107 |

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11. Osmium is the densest element with a density of 22.57 g/cm3. Find the mass of a 56.2 cm3 sample of osmium.

12. Perform the following SI prefix conversions.

|a. 65.2 mm = ? m |c. 65,000 L = ? mL |

| | |

|b. 2.3 kg = ?g |d. 0.502 g= ? Kg |

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Electrons Configuration and color

11. Give the electron configuration for the following.

|Symbol |Shorthand e- Configuration |

|Pd | |

|At | |

12. Explain why chromium’s electron configuration is [Ar] 4s13d5 instead of the expected configuration of [Ar] 4s23d4.

14. Draw orbital diagrams for the following elements.

|Symbol |Atomic # |Orbital Diagram |

|F | | |

| | | |

|V | | |

| | | |

13. Give some examples of colored and colorless solutions:

15. Predict the ions that will form from the following atoms and give the Nobel Gas configuration of the ion.

|Atom |Ion |Shorthand e- Configuration |

|Rb | | |

|Te | | |

| | | |

Chemical Bonding and Chemical equations

16. Based on what you know about ionic and covalent compounds and VSEPR theory are the bonds in the following substances IONIC, POLAR, or NONPOLAR?

a. MgO c. LiCl

b. H2O d. Br2

17. Use Lewis Diagrams to show the formation of MgO.

18. Use Lewis Diagrams to show the formation of H2O.

19. Predict the products and balance the equation:

a. K + HOH -->

b. Ca(C2H3O2)2 + Na2CO3 -->

20. For the following equations: Identify the type of reaction, balance the equation, and write in the states of matter

a. Cu + S8 --> CuS

b. C6H14 + O2 --> CO2 + H2O

c. BaCO3 --> BaO + CO2

d. AgNO3 + K3PO4 --> Ag3PO4 + KNO3

e. Ca + HCl --> CaCl2 + H2

21. Write formulas for the following compounds (HINT: First determine ionic/acid/covalent).

a. calcium bromide d. silicon dioxide

b. iron(III) sulfate e. dinitrogen tetroxide

c. hydrofluoric acid f. sulfurous acid

22. Write names for the following compounds (HINT: First determine ionic/acid/covalent).

a. CrCl3 d. MgSO4

b. Cu2CO3 e. P4O6

c. AsCl5 f. HClO3

Molecular Structure

23. For each of the following molecules, draw the Lewis electron dot diagram, give the shape and bond angle(s), and state whether the molecule is polar or nonpolar. Show your work in the spaces provided for counting valence e- and e- pairs.

| |Number of valence |Lewis Diagram |AXE formula |Ball and Stick |Molecular Shape |Molecular Polarity (vectors) |

| |e( | | | |& Bond Angle(s) | |

|SiO2 | | | | | | |

| | | | | | | |

|OF2 | | | | | | |

| | | | | | | |

24. Draw the vectors for each bond in the following molecules and circle whether the molecule is polar or nonpolar. Write the AXE formula for each molecule.

|TeCl2 bent |BCl3 trigonal planar |CH2Cl2 tetrahedral |

|AXE = |AXE = |AXE = |

|polar nonpolar |polar nonpolar |polar nonpolar |

Nomenclature

No review problems – just be sure you can name, for example silver nitrate, magnesium sulfate

Gas Laws

25. You fill up a balloon with air and it has a volume of 4.00 L at 25.0 C and a pressure of 1.01 atm. You submerge the balloon in a tank of water and it now is under a pressure of 2.05 atm and a temperature of 5.00 C. Calculate the new volume of the balloon.

26. A sample of chlorine gas occupies 1.00 L at 26.0 C and 1.00 atm. What volume will it occupy at 50.0 C and 1.50 atm?

27. At STP what is the volume of 142 g of chlorine gas

28. 5.00 g of water evaporates into a bag. The final volume of the bag is about 3.00 L at 298 K. What is the pressure of the gas in the bag

29. A gas occupies 100. L at 1.5 atm pressure and 26.85°C. How many moles of gas are present in the sample?

30. A container with a volume of 5.6 mL and a pressure of 2.3 atm is connected to another container with a volume of 3.6 mL and a pressure of 3.4 atm. If the stop cock between the container sis open what is the final pressure of the system?

Solution/Dilution

31. How much sodium chloride is needed to make 500 ml of 1.0M SOLUTION?

32. Explain how to make the sodium chloride solution

33. You have 50. mL of a 0.50 M solutions, who much water must be added to make a 0.25 M solution?

34. What volume of a 2.0 M NaOH solution is needed to make 150.mL of a 1.50M solution?

35. How many grams of NaOH are in 250mL of a 1.5M solution of sodium hydroxide?

Stoichiometry – and other math type problems

36. What is the molar mass of acidic acid?

37. What is the percent composition of O in CO2?

38. What is the percent error if the Experimental Value: 1.24 g and the Theoretical Value: 1.30 g

39. What is the percent yield for a reaction if you predicted the formation of 21. grams of C6H12 and actually recovered only 3.8 grams?

40. Given 18 grams of hydrogen gas, how many moles is this?

41. Given 3 moles of chlorine gas, how many grams is this?

42. What Mass of NaCl Can Be Produced by reacting 12.0 grams of sodium, Na, with

an excess of chlorine gas, Cl2

43. A 50.6 g sample of Mg(OH)2 is reacted with 45.0 g of HCl to form magnesium chloride and water. What is the limiting reactant?

44. What is the empirical formula for a compound with the following elemental composition: 40.00% C, 6.72% H, 53.29% O.

45. The empirical formula C4H4S has a molar mass of 84 g/mol. If the molecular weight of the actual compound is 168 g/mol, what is the molecular formula?

46. Example of a comprehensive problem:

a. What is the element symbol for Aluminum?

b. Write the ion with the correct charge for an aluminum ion.

c. Write the ion with the correct charge for a chlorine ion

d. What is the molecular formula for chlorine gas?

e. What is the formula for aluminum chloride?

f. Assume aluminum chloride can be made by the reaction of solid aluminum metal with chlorine gas. Write the balanced equation, including states of matter.

g. What type of reaction is this?

h. What is the molar masses for Aluminum?

i. What is the molar mass for the molecule chlorine gas?

j. What is the limiting reactant if 20.0 grams of aluminum and 30.0 grams of chlorine are used, what is the limiting reactant?

k. What is the molar mass for aluminum chloride?

l. How much aluminum chloride can theoretically be made?

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m. If 36.2 grams of aluminum chloride was made in the lab what is the percent yield?

n. What is the percent error?

47. Example of lab calculations for formula for a hydrate:

Assume a15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass after heating several times and re-massing after cooling remained the same and it was 7.58 grams. Find the formula for the hydrate by answering the following questions.

a. Write the formula for water.

b. Determine the mass of water driven off by heating.

c. What is the molar mass for water?

d. Determine the moles of water.

e. Write the formula for magnesium carbonate.

f. What is the molar mass for magnesium carbonate

g. Determine the moles of magnesium carbonate.

h. Find the whole number mole ratios:

i. Write the formula for the hydrate

j. Name this hydrate

-----------------------

Cl

Cl

H

H

C

Cl

Cl

Cl

B

Te

Cl

Cl

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