Download SEMESTER 1 EXAM Prblms/Short Ans

Chemistry EXAM – First Semester
Eq, S, U, SF – Equations; Show all equations used in all calculations.
Steps; show each step leading to each answer. Units; show the
appropriate units with each number used in all calculations. SF; Use
the correct significant figures when expressing all answers. Use
Scientific Notation for all numbers with values more than 3 decimal
places from the decimal point. ANSWER AT LEAST 10 QUESTIONS!
NAME: ______________________________________________
BLOCK: ________________ DATE: ________________________
ANSWER AT LEAST 10 QUESTIONS. You must answer 7, 8,
11, 15 & 16. You may not leave more than “2 in a row”
blank. (You may NOT leave the last several questions.
blank!)
1. The density of aluminum is 2.70 g/cm3. What is the mass of a solid piece of aluminum with a volume of 1.50 Cm3?
2. If 1 inch equals 2.54 cm, how many centimeters equal 1 yard (36 in = 1 yd)?
3. The mass of 2.0 mol of oxygen atoms (atomic mass = 16.00 amu) is:
4. A prospector finds 39.39 g of gold (Au), with a gram atomic mass = 196.9665g/mol. How many Au atoms does she
have?
5. Which lists the atomic orbitals in the correct order they are filled according to the Aufbau principle? Circle the correct
answer.
1s 2s 2p 3s 3p 4s 4p 3d 4d
1s 2s 2p 3s 4s 3p 3d 4p 5s
1s 2s 2p 3s 3p 4s 3d 4p 5s
1s 2s 2p 3s 3p 3d 4s 4p 5s
6. Write the electron configuration for Carbon (C).
Write the electron configuration for silicon (Si).
7. Illustration: In the boxes provided, draw and label a picture of the atomic model based on J.J. Thomson’s
experiment, Ernest Rutherford’s experiment, Niels Bohr’s experiment and the Quantum model of the atom. Show
protons, neutrons and electrons and their believed relationship to each other within the atom. DESCRIBE your
drawing with a complete sentence or two.
Thomson’s atom
Bohr’s atom
Rutherford’s atom
Quantum Model of the atom
8.Complete the orbital notation for S-32 atom. Label each sublevel.
Circle ALL sublevels with valence electrons.
___
___ ___ ___ ___ ___
___
___ ___ ___
___
Electron Configuration for S-32
___ ___ ___
___
Complete the electron configuration for S-32 here.
___
Number of protons
Number of neutrons
Number of electrons
Mass number
What is the highest occupied energy level?
Atomic #
How many valence electrons?
What is the highest occupied sublevel?
What is the tendency to gain or lose electrons
when bonding?
Write the symbol for the typical S-32 ion
9.Indicate the trends using up or down arrows as follows: ( ↑, → OR ↓ )
ACROSS through the Periods
DOWN through the Families
Atomic Radii
1st Ionization Energy
Electronegativity
Electron Affinity
10.Which radius is larger a chlorine atom ion or a chlorine ion?
Which radius is larger, a sodium atom or a sodium ion?
A
C
E
B
D
F
11A. According to the table above, where would you find the elements with the lowest electronegativity?
Where on the table would you find the highest electronegativity?
Explain your answer:
B. According to the table above, would you more likely find a larger atomic radius in the area labeled “A” or in the area
labeled “C”?
Would the atomic radius be larger in area “A” or area “B”?
Explain your answer:
C. According to the table above, would you more likely find a higher ionization energy in the area labeled “A” or in the
area labeled “B”?
Would the ionization energy be higher in area “A” or area “C”?
Explain your answer:
12.If the pairs of atoms below bonded, predict whether the bond would be ionic or covalent by placing an upper case
“C” or “I” after the pair. (SR # 3, p. 177)
Li and Cl _____
F and O ____
C and H _____
Mg and F _____
P and Cl ____
N and N _____
13.Write “Ionic” or “Covalent” after each description below. (SR# 4, p194)
a. higher melting and boiling points ___________________________
b. conductor of electricity when dissolved in water and melted. __________________________
c. forms a “crystal lattice” when solid ___________________________
d. composed of nonmetal bonded to nonmetal __________________________
14.Draw the Lewis structure, illustrating the molecular geometry of the following molecules. (SR#2, p.207)
a. SO2
b. CI4
c. Bl3
15.Draw FIVE water molecules, showing them in the proper orientation to each other. What forces are determining that
orientation? (SR #5 p. 207)___________________________
Draw 5 water molecules: Label force (use arrow) in your diagram below dictating the orientation.
16.Write the formulas for the following binary compounds formed between the following elements: (#1 p. 223)
a. Sodium and sulfur _______________________ d. aluminum and nitrogen __________________
Name the binary ionic compound as indicated by the following formulas: (#2 p. 223)
b. AgCl _____________________________ c. Na2O _______________________________
Write the formula and/or give the name for the following compounds: (#1 & 2, p.225)
c. Cu2+ and Br- __________________________ c. Fe2O3- _________________________________
Write the formulas and / or give the names for the following: (#1 & 2, p.227)
d. Sodium iodide ________________________ d. copper II sulfate _____________________________
e. NH4NO3 _____________________________ f. Ca(OH)2 _____________________________________
Give the names and / or write the formulas for the following molecular compounds. (#1 & 2, p. 229)
f.
SO3 ________________________________ d. N2O5 ________________________________________
g. Dinitrogen trioxide ___________________ f. dihydrogen monoxide ___________________________
Name each of the following: (#3 p. 231)
a. FeCl3 _______________________________ d. FeCl2 __________________________________________
Write formulas for the following; )#4, p. 231)
h. lead II nitrate ______________________ d. cobalt III sulfate __________________________________
i.
acetic acid ________________________ e. chloric acid _______________________________________
c. hydrochloric acid _____________________ f. sulfurous acid _____________________________________
Assign oxidation numbers to each atom in the following compounds: (#1, p. 235) Example: H = 1+, I + 1a. HI _________________________________ d. H2O _____________________________________________
b. SO42- _______________________________ e. H2SO4 ___________________________________________
17.For CaF2, calculate the following: (#1, p. 238)
Molar mass
Number of moles of CaF2 in the molar mass (p. 239)
Number of moles of Ca in the molar mass (p. 239)
17 Continued
Number of moles of F in the molar mass (p. 239)
Number of individual Ca atoms in the molar mass (p. 242)
Number of moles of CaF2 in a 47.06g sample of CaF2 (Show all calculations, steps, etc.) (p. 242)
Percent (by mass) Ca in CaF2
18.A compound is found to be 40..00% carbon and 6.727% hydrogen and 53.28% oxygen. Calculate the empirical
formula.
The molecular mass of the same compound is 180.18g / mol. Calculate the molecular formula.
19. Translate the word equation below into a balanced chemical equation.
Iron III combines with oxygen to form iron III oxide
What type of chemical reaction is the above reaction?
20. Write a chemical equation showing a balanced, double replacement reaction.
BONUS: Using the molar mass of Carbon 12, calculate the mass of 1 amu in grams.