2. the Atom & Bohr/Lewis Diagrams

REVIEW STATIONS

1. PERIODIC TABLE & TRENDS

2. THE ATOM & BOHR/LEWIS DIAGRAMS

3. MOLECULAR/IONIC COMPOUNDS

4. NAMING - IONIC COMPOUNDS

5. NAMING MOLECULAR COMPOUNDS

6. BALANCING

7. LAW OF CONSERVATION OF MASS

8. PHYSICAL AND CHEMICAL CHANGE

9. TYPES OF REACTIONS - GENERAL

10. ACIDS AND BASES

11. PUTTING IT ALL TOGETHER - PART 1

12. PUTTING IT ALL TOGETHER - PART 2

13. PUTTING IT ALL TOGETHER - PART 3

STATION 1 - THE PERIODIC TABLE & TRENDS

Use the periodic tables provided to answer the questions on your review handout.

STATION 2 - THE ATOM & BOHR & LEWIS DIAGRAMS

1. Name the three sub-atomic particles of the atom. What charges do they have?

2. What is meant by "valence electrons"?

3. Draw either a Bohr OR Lewis diagram for the following elements/ions (note - Lewis diagram shows only the outermost shell, with valence electrons only as opposed to Bohr diagrams which shows all the shells, including the valence electrons)

a. Silicon atom

b. Magnesium ion

STATION 3 - MOLECULAR AND IONIC COMPOUNDS

1. What does "ion" mean? What does it mean if you see Al3+ or S2−?

2. How do you know if a compound is ionic or molecular?

3. Using NaF and CO2 as examples, draw either Bohr or Lewis diagrams to show how their bonds are formed. What is the difference?

4. Why does magnesium chloride (MgCl2) have a weaker smell compared to candle wax (C25H52)?

STATION 4 - NAMING IONIC COMPOUNDS

1. Complete the following chart by writing the correct chemical formula or name in the space. Use the periodic tables provided. Remember to take note of multivalent metals and polyatomic ions!

FORMULA / NAME
K2S
magnesium phosphide
tin(IV) oxide
CaCO3
copper(II) bicarbonate

Note: A periodic table will be provided to you on test day, including a polyatomic ion chart as well as ionic charges for the elements. But no names will be given on the periodic table. You are responsible for knowing the names/symbols of the 40 elements that were discussed!

STATION 5 - NAMING MOLECULAR COMPOUNDS

1. Complete the following chart by writing the correct chemical formula or name in the space. Use the periodic tables provided.

FORMULA / NAME
SO3
triphosphorus hexachloride
carbon monoxide
P2O5
dinitrogen tetroxide

STATION 6 - BALANCING CHEMICAL EQUATIONS

Balance the 5 skeleton equations on your review handout. Always double check your work by counting the number of atoms of each element on both sides of the arrow! Remember, do not put 1 as a coefficient!

STATION 7 - LAW OF CONSERVATION OF MASS

Is the Law of Conservation of Mass applicable to the following scenarios? Justify your answers.

1. The mass of a rusty bicycle is found to be slightly greater than the mass of the same bicycle before it rusted.

2. 0.51 g of aqueous solution of copper(II) chloride and 0.62 g of sodium hydroxide were mixed in a test tube with a stopper. After the reaction, the products were weighed to be a total of 1.10 g.

STATION 8 - PHYSICAL AND CHEMICAL CHANGE

Read the following scenarios. Identify whether a physical and/or chemical change has occurred and how you know.

1. A student adds a piece of magnesium metal to a solution of sulphuric acid (H2SO4). The test tube fizzes and is warmer at its base. The student also puts a flaming split inside the test tube and hears a pop sound.

2. A scoop of copper(II) chloride powder, which is light blue, is added to distilled water. The result is a translucent blue homogeneous solution.

3. Aluminum foil is added to a beaker containing a solution of copper(II) sulphate and heated up. After 15 minutes, the solution turns darker and there are reddish flakes floating in the solution and deposited on some pieces of the foil.

STATION 9 - TYPES OF CHEMICAL REACTIONS

1. Consider the six reaction types discussed in class. All involve elements and compounds. Identify the type(s) of reaction that has the following reactant(s) or product(s):

Reactant(s) / Product(s) / Type of Reaction
Two elements
An element and a compound
Water and a salt
Two compounds
Only one compound
Carbon dioxide and water

STATION 10 - ACIDS AND BASES

1. Classify the compound as an ACID or a BASE or BOTH based on the following properties:

a) pH = 4.0 / b) reacts with carbonates to produce CO2 gas / c) slippery texture
d) litmus paper stays red / e) unreactive with metals / f) pH = 13.0
g) contain hydrogen ions / h) reacts with metals to produce H2 gas / i) bitter tasting
j) electrolyte in solution (conducts electricity) / k) corrosive / l) contain hydroxide ions
m) turns blue with bromothymol blue (BTB) / n) sour tasting / o) phenolphthalein turns pink

2. Name or write the formulas for the following acids and bases:

a) HF / HNO2
b) magnesium hydroxide / hydroiodic acid

3. A scientist walked into a lab and discovered a clear puddle on the floor. Taking precautions, he discovers from his analysis using different pH indicators and equipment:

· Bromothymol blue: BLUE

· Universal pH indicator paper: 11.0

· Cabbage Juice: TURQUOISE

· Electronic pH meter (see image): 11.4

a) What is meant by "pH"?

b) Is the chemical in the puddle acidic, basic or neutral?

c) How can he safely clean the spill up? What type of reaction is this?

STATION 11 – PUTTING IT ALL TOGETHER

PART 1

A student wishes to see the reaction between an aqueous solution of phosphoric acid and an aqueous solution of magnesium hydroxide. One of the products will be a solid compound that contains magnesium ions as part of it.

a) Write a balanced chemical equation for this chemical reaction and predict its products. Include the states of matter notations.

b) Classify this type of reaction.

STATION 12 - PUTTING IT ALL TOGETHER

PART 2

When a copper wire is placed in an aqueous solution of silver nitrate, a solid layer appears on the copper wire and the solution turns blue due to the Cu2+ ions and there are solids flaking off into the solution.

a) Write a balanced chemical equation for this chemical reaction and predict its products. Include the states of matter notations.

b) Classify this type of reaction.

c) How do you know that a chemical change has occurred?

STATION 13 - PUTTING IT ALL TOGETHER

PART 3

A scientist reacts an aqueous solution of cobalt(II) chloride and an aqueous solution of sodium carbonate. Only one of the products that formed in this reaction will be a solid (see image) and it is a pink solid that is due to the Co2+ ions present in the compound.

a) Write a balanced chemical equation for this chemical reaction and predict its products. Include the states of matter notations.

b) Classify this type of reaction.