General Chemistry First Semester Final Exam Review
Partial Key
You will have an opportunity to improve your scores from previous exams.
In order to do so, you must complete all of the review questions for that particular unit.
Also, you may have a one quarter sheet of notes (back and front) to use on the final.
Your notes must be handwritten and you may not share them with another student.
Good Luck and happy studying!
Unit 1: Particles
1. Matter Classification
2. Subatomic Particles
3. Atomic Models
4. Periodic Trends
Unit 2: Bonding
1. Ionic Bonding
2. Covalent Bonding
3. Shape & Polarity
4. Nomenclature
Unit 3: Measurement & Calculation
1. Measuring Sig Figs
2. Calculating Sig figs
Unit 4: Moles
1. Dimensional Analysis
2. Mole Definitions
(3. Calculating Moles)
Unit 1: Particles
Objective 1.1: Matter Classification
1. What is the difference between counting the atoms and counting the elements?
2. What is the difference between atoms and molecules?
3. What is the difference between the three states of matter?
4. Use the picture of hydrogen peroxide (wound disinfectant) to answer the following questions:
a. How many atoms are in the picture?
b. Is hydrogen peroxide a compound or an elemental molecule?
c. How many different elements are in hydrogen peroxide?
d. The hydrogen peroxide you buy from the store is diluted with water to contain only 3% of the hydrogen
peroxide molecule. Is this hydrogen peroxide solution a pure substance or a mixture?
e. What state of matter is hydrogen peroxide? What is happening to the molecules that define its state of
matter?
Objective 1.2: Subatomic Particles
5.
What are three things you know about each of the following subatomic particles?
a. Protons
b. Neutrons
c. Electrons
6. What do the two numbers provided for each element on the periodic table mean?
7. How do you find the number of neutrons an element has?
8. Complete the following table regarding the number of subatomic particles in NEUTRAL atoms:
Element
Protons Average Mass Neutrons Electrons
Phosphorus
27
19
9. Complete the following table regarding the charge of atoms:
Element Protons Electrons Net Charge
20
18
Chlorine
-1
18
+7
Objective 1.3: Atomic Models
10. How do you draw a bohr model?
11. How do you draw a lewis structure?
12. Draw the bohr models for Helium, Boron and Sulfur (without looking at the bohr models in your notes)
13. Draw the lewis structures for Helium, Boron and Sulfur (without looking at the lewis structures in your notes)
Objective 1.4: Periodic Trends
14. On the blank periodic table below, label the 7 families:
15. On the periodic table above, write the element symbols of any metalloids.
a. Are the metals to the right or left of the metalloids?
b. Are the non-metals to the right or left of the metalloids?
i. What element is also a non-metal but is not in the non-metal section?
16. Regarding states of matter…
a. Which elements are in a liquid state of matter at room temperature?
b. What state of matter are most of the non-metals?
i. What elements are an exception to this and what state of matter are they?
c. What state of matter are most of the metals?
17. On the periodic table below:
a. Label the pattern for number of valence electrons.
b. Label the pattern for number of electron shells/energy levels.
18. Considering elements in the same row, which side has a smaller sized atom? WHY?
Remember, atoms decrease in size from left to right.
19. Considering elements in the same column, which end has a smaller sized atom? WHY?
Remember, atoms increase in size proceeding down the Periodic Table.
20. Considering elements in the same row, which side has a larger electronegativity? WHY?
21. Considering elements in the same column, which end has a larger electronegativity? WHY?
Unit 2: Bonding
Objective 2.1: Ionic Bonds
22. On the periodic table below, label which side gains electrons to meet the octet rule and which side loses. Also label the
resulting ionic charges for each column.
23. Draw the Lewis structure and show the electron transfer and molecular formula for the bonding of:
a. Potassium and fluorine
b. Beryllium and bromine
24. Show the ionic charges canceling out to a net zero charge and the molecular formula for the bonding of:
a. Magnesium and sulfur
(+2)
+ (-2) = 0, therefore MgS
b. Lithium and nitrogen
25. Show the molecular formula created from the ionic bonding of the following elements using the shortcut:
a. Calcium and chlorine
Ca +2
Cl -1  CaCl2
b. Aluminum and oxygen
Objective 2.2: Covalent Bonds
26. What are the steps for drawing a Lewis structure?
1. Make sure that you know all the steps. Refer to
the Notes: “Objective 2.2 Covalent Bonding”
2
3a.
3b.
4.
27. Draw the Lewis structure for the following molecules:
a. CCl4
b. O2
Requires double bonds.
28. Are the bonds in CCl4 polar? What about the bonds in O2? WHY? Label partial positive/negative where applicable.
CCl4 is polar covalent. Referring to the
electronegativity table, Cl has the greater
electronegativity so it would be partial
negative.
O2 is “purely” covalent since each oxygen has
the same electronegativity (3.5)
Objective 2.3: Shape & Polarity
29. What are the shape symbols (AX2E) for the following shapes? Also draw the 3-D line structures for each.
a. Linear AX2
b. Bent
c. Trigonal Planar
AX3
d. Trigonal Pyramidal
e. Tetrahedral
30. What is the shape of these lewis structures? Are they polar or non-polar molecules?
Bent:
(AX2E)
Objective 2.4: Nomenclature
31. What elements follow type I nomenclature and what are the naming rules?
32. What elements follow type II nomenclature and what are the naming rules?
33. What elements follow type III nomenclature and what are the naming rules?
34. Name the following formulas:
a. Mg3P2
b. There was a mistake, it should be CCl4
Carbon tetrachloride (Type III)
c. CuBr2
Copper (II) bromide (Type II)
35. Write the formulas for the following names:
a. Nickel (II) nitride
b. Potassium oxide
K2O (Type I)
c. Phosphorus trichloride
Unit 3: Measurement & Calculation
Objective 3.1: Measuring Sig Figs
36. Regarding the Sig Fig Rules:
a. Rule 1… Do all these digits count as significant? 9.43 (WHY?)
Again, make sure that you know all the rules – then apply.
b. Rule 2… Does this zero count as significant? 8703 (WHY?)
c. Rule 3… Do these zeros count as significant? 0.074 (WHY?)
d. Rule 4… Does this zero count as significant? 90 (WHY?)
e. Rule 4… Does this zero count as significant? 5.70 (WHY?)
37. Provide the number of significant figures for the following masses:
a. 0.00305 g
3 significant figures (all four rules apply)
b. 90010 gc. 8.00 g
Remember the significance of the decimal for Rule 4.
38. Round these measurements to the indicated number of significant figures:
a. 4589.540325 (to 4 SF) - 4590.– round up (5 or above), the decimal is necessary for 4 SF’s
b. 599.999 (to 5 SF)
c. 778390 (to 2 SF)
Remember to round up and that trailing zeroes do not count if there is no decimal.
39. Record a measurement to the proper number of significant figures for the following graduated cylinders:
Objective 3.2:
40. What are the
Calculating Sig Figs
Sig Fig Calculation Rules:
a. Adding/Subtracting:
b. Multiplying/Dividing:
41. Provide the proper significant figure answers to the following problems:
a. 8542 / 524 = 16.301526, three significant figures are allowed (524 is the limiting factor), therefore 16.3
b. 1.06 + 54.3 = 55.36, one decimal place is allowed (54.3 is the limiting factor), therefore 55.4 (round up)
c. 97 x 0.164 x 4.00 =
d. 9765.87 – 5.3498 – 764.385 =
42. Convert the following numbers into or out of scientific notation
a. 4.83 x 104 = 48,300
b. 8245000 = 8.245 x 106
c. 9.17 x 10-3
d. 0.000491
Unit 4: Moles
Objective 4.1: Dimensional Analysis
43. Perform the following unit conversions showing your work using dimensional analysis:
a. 1.25 inches to feet
b. 2.12 quarts to liters
c. 2640 ft to kilometers
44. At the mall, you decide to try on a pair of French jeans. Naturally, the waist size of the jeans is given in centimeters.
What does a waist measurement of 52 cm correspond to in inches?
45. Calculate how many seconds you spend in class in 1 school year. Each school year has 180 days and each day you
spend 5 hours in class.
Objective 4.2: Mole Definitions
46. What are the three ways to measure 1 mole of oxygen gas?



47. How many phosphorus atoms are there is 1.75 moles of phosphorus?
1.054 x 10 24
There are 6.02 x 10 23 atoms in one mole (Avogadro’s number)
Therefore you multiply Avogadro’s number by 1.75 to get the number of atoms in 1.75 moles.
48. A man made the mistake of heating old dental fillings on his stove to get the gold and silver. He forgot that silver
fillings actually contain some mercury. He died when he inhaled 0.375 mol of mercury. How many grams is that?
Look up the atomic mass of Hg then convert moles to grams using dimensional analysis.
49. A small inflatable toy contains 2.15 L of gas, how many moles is this?
Remember, for any gas at STP (Standard Temperature and Pressure), there are 22.4 L of gas in one mole. Solve using
dimensional analysis.