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Pre-AP Chemistry

Fall 2013 Final Review

Name: Date: Period:

Instructor: Ms. Miranda Wysocki

Date:

Time:

Location: N226

Review Due Date:

2013 FALL SEMESTER EXAM SCHEDULE

|  |7:55 - 9:55 AM |10:05 AM - 12:05 PM | Dismissal |

|Tuesday, Dec. 17 |1st  Period Final |2nd Period Final |at 12:05 PM |

|Wednesday, Dec. 18 |3rd  Period Final |4th  Period Final |at 12:05 PM |

|Thursday, Dec. 19 |5th  Period Final |6th  Period Final |at 12:05 PM |

|Friday, Dec. 20 |7th  Period Final |0 or 8th Period Final |after your last exam |

You will be provided with: You will need to bring:

STAAR Chart **Calculator**

**You must use your own calculator for the final exam. No sharing, no exceptions.

Test Breakdown:

92 Multiple Choice Questions

Time Allowed: 2 hours

This review is designed to help you study for the Chemistry final but should not be used as the only study method. Make sure to study all notes, warm-ups, quizzes, tests, labs, etc. to prepare for this exam. Good Luck!

1) Define Precision vs. Accuracy.

2) How many significant figures are there in each of the following numbers?

a. 0.0020

b. 514000

c. 100.0

d. 0.0001

e. 7000

f. 0.01010

g. 10.01

h. 45

i. 0.0002300

j. 1.20 x 103

k. 1.0 x 10-3

l. 100

m. 100.

n. 102

3) Burning wood for fire is an example of a change.

4) Which of the following is a chemical property of butter?

a. Its yellow color

b. The fact that it melts at 110°C

c. Its greasy feel

d. The fact that it becomes rancid

5) What is the difference between a mixture and a substance?

6) Classify each of the following as: homogeneous mixture, heterogeneous mixture, compound or element

a. Gold

b. Steel

c. Salt water

d. Pizza

e. NaCl

f. Copper

g. Rust

h. Granite

i. Milk

j. Air

k. Neon

l. Alloy

7) What is the density of a metal with a mass of 20.0 g and a volume of 3.8 cm3?

8) Would the metal in the previous question (#7) sink or float in water?

9) The density of a metal is 2.54 g/cm3. What is the volume of 7.55 g of this metal?

10) Using skills in dimensional analysis, convert the following:

a. 445 km to mm

b. 88 mg to kg

c. 992 mL to L

d. 782 kg to mg

e. 8990 km to mm

f. 1.0 kg = ? g

g. 2.5 kg = ? mg

h. 5.0 cm = ? m

i. 4.75 cm = ? mm

j. 2.8 L = ? mL

k. 10,000Gm = ?m

11) What is the density (in g/cm3) of an object that has a volume of 50.3 cm3 and mass of 22.4 g?

12) What is the mass of a piece of copper that has a volume of 20.0 cm3? The density of copper is 8.92 g/cm3

13) What is the proper response to a discovery of cracked glassware during a lab?

14) Define physical change and physical property. Give 2 examples of each.

15) Compare and contrast intensive and extensive properties. Give 2 examples for each.

16) What are 5 characteristics of a chemical reaction?

17) Express the following numbers in scientific notation:

a. 622820000

b. 0.00385

c. 431700

d. 0.000020

18) Name the following laboratory equipment:

[pic] [pic] [pic] [pic]

19) What laboratory equipment is used to accurately measure the volume of a liquid?

20) Arrange the following atoms in order of increasing atomic radius:

a. O, S, Se, Te

b. P, S, Cl, Ar

21) Arrange the following atoms in order of increasing electronegativity:

a. O, S, Se, Te

b. P, S, Cl, Ar

22) Arrange the following atoms in order of increasing ionization energy:

a. O, S, Se, Te

b. P, S, Cl, Ar

23) Determine the number of protons, neutrons and electrons for each of the following:

a. Si-28

b. Na-23

c. Fr-223

d. Pd-106

e. Cr-52

f. Na

g. O

h. Zn

i. Na+1

j. O-2

k. U-235

l. H-3

24) Determine the value or symbol for x in each of the following:

a.

b.

c.

d.

25) Briefly describe what each of the following scientists’ contributions to atomic theory and structure:

a. John Dalton

b. J.J. Thomson

c. Earnest Rutherford

d. Niels Bohr.

26) Write the complete electron configuration for each of the following:

a. K

b. Cu

c. Mo

d. Cr2+

e. Br-

27) Define the following terms:

a. Cations

b. Anions

c. Isotopes

d. Valence electrons

28) For each of the following:

• Draw the Lewis structure

• Determine the molecular polarity

• Determine the molecular geometry and bond angles

a. CO2

b. BF3

c. CH3Cl

d. NH3

e. CH3OH

f. CCl4

g. HBr

h. H2O

i. H2

j. CO

29) Identify elements having the following electron configurations:

a. 1s22s22p63s23p3

b. [Ar]4s1

c. Contains four electrons in its third and outer main energy level

30) Draw the orbital diagram for the following:

a. Sulfur

b. Manganese

c. Calcium

31) List some characteristics of a metal.

32) List some characteristics of an ionic compound.

33) Identify metals, nonmetals, and metalloids on the Periodic table.

Questions 34-37 refer to the following elements

A) Br

B) K

C) Ba

D) Cs

E) Ca

34) The element with the lowest ionization energy

35) The smallest atom

36) The element with the lowest electronegativity

37) The alkaline earth element with the smallest atomic radius

Question 38-41 refer to atoms for which the occupied atomic orbitals shown below.

[pic]

38) Represents a noble gas

39) Represents a carbon atom

40) Represents an atom that has four valence electrons.

41) Represents a transition metal.

42) Using the SHORT HAND notation, write the electron configuration for the following:

a. Nitrogen

b. Calcium

c. Zinc

43) Draw orbital diagrams for the elements in #42.

44) Calculate the average atomic mass (amu) of an element with the following percent abundance:

|Mass |Abundance |

|19.38 amu |38.4% |

|18.75 amu |17.2% |

|17.69 amu |44.4% |

45) Assume chromium has 4 isotope forms. Calculate the average atomic mass based on the natural abundance and weights indicated below:

Form A: 33% - 22 grams

Form B: 13% - 25 grams

Form C: 35% - 20 grams

Form D: 19% - 34 grams

46) What are some exceptions to the Octet Rule?

47) Compare and contrast ionic and covalent substances.

48) Write the formula for the following substances:

a. Potassium nitrate

b. Iron (III) chloride

c. Lead (II) iodide

d. Calcium chloride

e. Magnesium hydroxide

f. Diphosphorus trioxide

g. Ammonium acetate

h. Barium permanganate

i. Copper (II) nitrate

j. zinc sulfate

k. Lithium sulfide

l. Tin (IV) oxide

m. Magnesium nitride

n. Aluminum sulfide

o. Carbon tetrachloride

p. Diphosphorus trioxide

q. Calcium phosphate

r. Lithium nitride

s. Sodium hydroxide

49) Name the following substances:

a. NaCl

b. HCl

c. CO

d. Fe2O3

e. K2S

f. H2

g. CaCO3

h. SiO2

50) What is the wavelength of a photon that has a frequency of 5.47 x 1013 Hz?

51) What is the energy of light emitted at the frequency of 3.57 x 1021 Hz?

52) The energy of a photon is 5.87 x 10-20 J. What is its wavelength in nm?

53) Calculate the wavelength of the following:

a. A green traffic sign with a frequency of 6.10x1014 Hz

b. A yellow flower with an energy of 3.40x10-19 J

54) Draw and label the parts of a wave.

55) List examples of diatomic gases.

56) What is the most precise value that can be measured by using the Ruler A? What is the most precise value that can be measured by using the Ruler B?

[pic]

57) Explain the Law of Conservation of Mass.

58) A chemistry student’s investigation is described below.

| |

|The student obtains 15 g of an unknown substance. |

|The student notes that at room temperature the substance is a solid and is colored white. |

|The student determines that the density of the substance is 2.17 g/cm3 |

|The student then determines that the substance is soluble in water. |

The student determines that the unknown substance is sodium chloride. Which of the following is an extensive property of sodium chloride?

A) Mass of 15 g B) White color C) Density of 2.17 g/cm3 D) Solubility in water

FIRST SIX WEEKS LEARNING TARGETS

|# |Student Learning Target |

|1 |The student is able to demonstrate lab safety rules |

|2 |The student is able to take measurements with precision |

|3 |The student is able to express numbers and perform calculations using scientific notation |

|4 |The student is able to use the rules for significant figures in calculations |

|5 |The student is able to perform metric conversions using conversion factors and dimensional analysis |

|6 |The student is able to calculate the density of an object |

|7 |The student is able to distinguish between the accuracy and precision of a measurement |

|8 |The student is able to distinguish between intensive and extensive properties |

|9 |The student is able to distinguish between physical and chemical changes and properties |

|10 |The student is able to apply the Law of Conservation of Mass |

|11 |The student is able to classify substances as elements, compounds, or mixtures |

|12 |The student is able to understand the experimental design and conclusions used in the development of modern atomic theory |

|13 |The student is able to calculate the subatomic particles for neutral and charged atoms |

|14 |The student is able to practice calculations involving isotopes and atomic mass |

|15 |The student is able to write electron configurations, orbital diagrams, and quantum numbers for atoms and ions |

|16 |The student can identify and explain the properties of chemical families, including alkali metals, alkaline earth metals, halogens, noble gases, |

| |and transition metals |

|17 |The student is able to explain periodic trends such as ionization energy, atomic radii, and electronegativity |

SECOND SIX WEEKS LEARNING TARGETS

|# |Student Learning Target |

|1 |The student is able to explain the relationship between wavelength, frequency, and energy |

|2 |The student is able to use Planck’s constant and the speed of light to calculate wavelength, frequency, and energy |

|3 |The student is able to explain periodic trends such as atomic radii, ionic radii, ionization energy, electron affinity, and electronegativity |

|4 |The student is able to use experimental data to explain periodic trends such as atomic radii, ionic radii, ionization energy, electron affinity, |

| |and electronegativity |

|5 |The student is able to distinguish between ionic, covalent, and metallic substances |

|6 |The student is able to name and write the formula for ionic and covalent substances |

|7 |The student is able to describe and/or illustrate the formation of ionic and covalent bonds |

|8 |The student is able to draw Lewis structures for molecules and ions |

|9 |The student is able to apply the VSEPR Theory to predict the molecular geometry and bond angles for molecules and ions |

|10 |The student is able to predict the bond and molecular polarity for molecules and ions |

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

31

P

X

108

Ag+

X

48

X

22

127

X-

53

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