GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

UNIT 1—KMT and ENERGY

  1. The cylinder to the left contains water. An object with a mass of 21g and a volume of 15 cm3 is lowered into the water. Sketch the object and the new water level in the cylinder on the right.
  1. Calculate the density of the object from question 1.
  1. What property does the unit cubic centimeters (cm3)describe?

Use the graph on the previous page to answer the following questions:

  1. Calculate the density of Unknown A and Unknown B.
  1. Use Table 1 and Table 2 to determine the identity of the Unknown A and Unknown B.

Table 1 / Table 2
Substance - Liquids / Density g/mL / Substance - Solids / Density g/mL
Gasoline / 0.737 / Cork / 0.24
Cyclohexane / 0.779 / ParaffinWax / 0.898
Ethanol / 0.81 / Ice / 0.916
Kerosene / 0.820 / Nylon / 1.12
Coconut oil / 0.924 / Rubber / 1.52
Water / 1.00 / Sugar / 1.6
Sea water / 1.025 / Carbon / 2.15
Glycerin / 1.26 / Salt / 2.2
Maple Syrup / 1.37 / Aluminum / 2.7
Freon / 1.49 / Slate / 3.2
Carbon tetrachloride / 1.58 / Iron / 7.87
Copper / 8.9
Platinum / 21.4
  1. Sketch a line on the graph for liquid water.
  1. Plot the point (11 mL, 38 g) on the graph.

Could this substance be Unknown A or B or neither?

  1. Would Unknown A from the graph float or sink in water? Why did you choose your answer?
  1. What is the volume of 100 g of A? What is the volume of 100 g of B? Write at least one sentence to compare your answers.
  1. Draw a particle diagram to describe a liquid with some of the particles becoming a gas.
  1. How would you describe the attraction between the liquid particles?
  1. How would you describe the attraction between the gas particles?
  1. How does the motion of the liquid particles compare to the motion of the gas particles?
  1. State the PVTn relationships described by each of the following graphs.
  1. Define KMT.
  1. Define the term kinetic.
  1. What the relationship between kinetic energy and an increase in temperature?
  1. Define Pressure.
  1. How can pressure be increased?
  2. Use KMT to describe why the liquid in a thermometer rises when the thermometer is placed in warm water.
  1. Explain the difference between 0 °C and 0 K.

Why must Kelvin always be used in gas calculations?

  1. Fill in the chart below regarding the three states of matter and their relative volumes and shapes.

State of Matter / Volume / Shape
Solid
Liquid
Gas
  1. A container of carbon dioxide has a volume of 240. cm3 at a temperature of 22C. If the pressure remains constant, what is the volume at 44C? Show all of your work.
  1. Due to the friction between a tire and the road surface, the temperature of the air inside a tire increases as one drives. If the tire pressure is 26 psi when the car is in the driveway at 25˚C, what is the temperature of the air inside the tire when the pressure increases to 29 psi? Assume tire volume is constant. Show all of your work.
  1. The pressure of a 250 mL sample of gas is 105 kPa. What would be the pressure if the volume were increased to 375 mL? Show all of your work.

UNIT 2—ENERGY AND STATES OF MATTER

  1. Describe the change in state that occurs (from _____ to _____) for each of the following processes
  1. Boiling
  2. Melting
  3. Evaporation
  4. Freezing
  5. Condensation
  1. On the heating curve below:
  • label which phase or phases are present in each portion
  • label each region with either Eth or Eph
  • describe whether the thermal energy or phase energy is changing or staying constant at each region
  1. What happened to the energy that was released in the previous question (discuss using the words system and surroundings)?
  1. What type of process is this (endothermic or exothermic)?

UNIT 3 – DESCRIBING AND COUNTING SUBSTANCES

Write the letter of the box whose contents best match the description.

  1. Define element.
  1. Define compound.
  1. Matter can be described (or placed) in two categories. What are those two categories? Describe both.

Consider the four containers below.

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GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

  1. Which of these are mixtures?
  2. Which contain a diatomic molecule_____
  3. Which contain only compounds? _____
  4. Which contain only elements?_____

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GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

Consider the four containers below.

  1. Which of these are solid? pure substances?
  2. Which contain only compounds? only elements

Consider the four containers below.

  1. Which of these are possibly a gas? pure substances?
  2. Which contain only compounds? only elements
  1. How many atoms of sulfur are in aluminum sulfate? ______
  2. The molar mass of Na2CO3 is
    a. 51.0 g/mol b. 83.0 g/mol c. 96.0 g/mol d. 106.0 g/mol
  1. Find the molar mass of the following (make sure to include the correct unit):

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GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

KNO3

(NH4)2CO3

Ag2CrO4_____

Methane _____

FOR THE FOLLOWING PROBLEMS SHOW ALL OF YOUR WORK AND UNITS.

  1. How many moles are in 12.0 g iron?
  1. How many moles are in a sample of 0.476 g of ammonium sulfate?
  1. How many grams are in 0.15 moles sodium nitrate?
  1. How many grams are in 0.64 moles aluminum chloride?
  1. In one mole of magnesium oxidethere are ______grams of magnesium oxide.
  1. In one mole of iron (III) oxide there are ______grams of iron (III) oxide.
  1. In one mole of ammonia there are ______grams of ammonia.

UNIT 4—PERIODIC TABLE AND BONDING

  1. What is the name of the columns of the columns on the Periodic Table?
  1. What is the name of the periods on the Periodic Table?
  1. Know the trends in the periodic table: atomic radii, electronegativity and ionization energy
  • Identify these trends using the blank periodic table in question 4 below.
  • Which of the following elements has the largest atomic radius?

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GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

a.boron

b.aluminum

c.gallium

d.indium

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GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

  • Which of the following elements has the smallest ionization energy?

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GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

a.potassium

b.arsenic

c.nitrogen

d.bismuth

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GENERAL CHEMISTRY 1st SEMESTERFINAL REVIEW

  1. Place the names of each family on the Periodic Table below (make sure to include main group elements and transition elements) Indicate the charge formed for each ion in each group (at the top of that group).
  1. How are elements in a group alike and how are they different?
  1. What is the most common on the periodic table? Choose two of the below:

solidliquidgas

metalsmetalloidsnon-metals

  1. Which of the following elements has the greatest ionization energy?
    a. Lithium
    b. Calcium
    c. Neon
    d. Silicon
  1. Which of the following elements has the least ionization energy?
    a. Lithium
    b. Calcium
    c. Neon
    d. Silicon

Use the diagram below to answer question 10.

  1. Identify the charge of the ion formed by each element labeled in the above periodic table

a. ______b. ______c. ______d. ______

Use the diagram below to answer question 11.

  1. .In the diagram above, which arrow correctly represents each of the following trends?

a. Decreasing atomic size within a period

b. Increasing ionization energy within a group

  1. Which of the following would you predict to have the smallest radius (atomic size)?


Be.MgCaSr

In the diagram above, which arrow correctly represents each of the following trends?

  1. Decreasing ionization energy within a period
  1. Increasing atomic size within a group
  1. Which of the following would you predict to have the smallest radius?

.CNOF

Naming and Forming

WRITING IONIC COMPOUNDS

Ionic compounds are formed from a positive ion (cation) and a negative ion (anion).

The positive ion is always written first.

The resulting compound must be electrically neutral.

Use parentheses when you need two or more polyatomic ions in a formula.

Cl-1 / OH-1 / S2- / CO32- / PO43-
Na+
NH4+
Ca2+
Al3+
Sn4+
# / Name / Cation / Anion / Formula
1. / ammonium phosphate
2. / barium nitrate
3. / copper sulfide
4. / aluminum carbonate
5. / strontium hydroxide

Nomenclature - Write the names of the following compounds.

  1. BaCl2______
  1. Ni(OH)2______
  1. Na3PO4______
  1. SnBr4______
  1. (NH4)2CrO4______
  1. Li2O______
  1. FeS______

Write the formulas for the following compounds.

  1. copper (II) sulfate
  1. iron (III) chloride
  1. aluminum oxide______
  1. potassium phosphate
  1. ammonium carbonate
  1. chromium (III) oxide
  1. silver sulfide
  1. zinc nitrate
  1. strontium fluoride
  1. magnesium hydroxide

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