Chemistry 20
Mrs. Rogers
Materials to Bring: Calculator, Pen, Pencil, Eraser
You will get a periodic table and ion chart to use during the final exam.
Unit 1: Introduction to Chemistry
1.
General Lab Safety Rules: Review procedures.
2.
WHMIS and MSDS – what they stand for and how they are used.
3.
Lab Equipment - Erlenmeyer Flask, test tube clamp, beaker, Bunsen burner, test tube holder, scoopula, evaporating dish, funnel, crucible tongs – identify pictures.
4.
Writing numbers in Scientific notation - round off a number to 2 significant figures and write the number in scientific notation.
5.
Quantitative and Qualitative Observations - be able to determine an example as quantitative or qualitative observation.
Unit 2: Atoms & Elements & the Periodic Table
1.
Arrangement of the modern periodic table – how is it organized?
2.
Elements – how are elements represented?
3.
Describe what an atom is and what it consists of
4.
Below are five models of the atom. Give a description of each and draw.
Drawing
Dalton
Thomspon (Plum Pudding)
Bohr
Description
Rutherford
Lavosier
5.
Electrons, protons and neutrons – know characteristics of each particle – charge, where it is located in the atom, mass, how it is determined, who discovered the particle.
6.
How did Mendeleev contribute to the development of the periodic table?
7.
Complete the following table:
Element Atomic # Mass # # electrons # protons # neutrons
O
Li
12
16
165 67
8.
What is an isotope?
9.
Write the isotope symbol for Carbon – 12 ________
How many protons does it have? _______
What is its mass number? _______
How many neutrons does it have? __________
4
12
5
4
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6.
7.
Chemistry 20
Mrs. Rogers
10.
Electron.
Give the electron configurations and orbital diagrams for each of the following atoms: a) P b) O c) Cr
11.
What are valence electrons and how do you determine the number of valence electrons an atom will have?
12.
Draw electron dot (Lewis dot) diagrams for potassium, chlorine and phosphorus.
13.
Know the following parts of the periodic table: groups, periods, representative elements, transition elements, inner transition elements, metals, non-metals, metalloids
14.
What are the characteristics of metals, non metals, and metalloids
15.
Alkali metals, Alkaline Earth Metals, Halogens, Noble Gases - location, group #, general properties (states, reactivity)
16.
What are the Pauli Exclusion Principle, Aufbau Principle and Hund’s rule?
Unit 3 : Molecules and Compounds
1.
Atoms that have a charge are called ________________. An atom with a positive charge is called a(n) ____________________, while an atom with a negative charge is called a(n) _______________
2.
Atoms, Ions, Cations, Anions, Monatomic Ions, Polyatomic ions - know what these are,
5. as well as naming and be able to write them properly.
3.
Naming ions both monatomic and polyatomic ions – know how to determine the charges of the monatomic ions using the periodic table.
4.
MAKE SURE THAT YOU KNOW HOW TO NAME AND WRITE THE
FORMULAS for ionic compounds, acids, organic compounds and molecular compounds.
Name the following ions: a) Li
+1 b) NH c) OH
4
+
-1 d) SO
4
-2 e) Mg f) Fe
+2
+2 g) CO
3
-2
Write the formulas for the following ions: a) Fluoride b) Aluminum ions c) Phosphate d) Phosphide e) f) g)
Sodium ion
Sulfide
Acetate
Give the formulas of the following compounds – there is a mixture of ionic and molecular. a) Potassium fluoride b) Aluminum hydroxide c) Sodium chloride d) Ammonium Phosphate
2

8. e) f) g)
Lithium Oxide
Copper (II) bromide
Carbon dioxide h) Phosphorus trioxide i) j)
Chemistry 20
Mrs. Rogers
Trinitrogen hexoxide
Sulfur pentabromide
Give the names for the following compounds – there is a mixture of ionic and molecular. a) b) Mg(OH)
2 c) K
2
CO
3 d) MgO e) f)
NaF
CuO
Fe
2
O
3 g) NH
4
CH
3
COO h) SO
2 i) CO j) CCl
4 k) N
2
O
5
9. Give names for the following compounds: a) HNO
3(aq) b) H
2
S
(aq) c) HNO
2(aq) d) HCl e) H(C
10 Give the names of each of the following compounds: a) C
4
H
8 b) C
2
H
6 c) C
6
H
14 d)
C
6
H
12
11. Give the formula for each of the following names: a) Pentane
(aq)
2
H
3
O
2
)
(aq) b) Ethene c) Heptane d) 2,4 – dimethyl – nonane e) 3, 6 – diethyl – 3 – decene f) Sufuric acid g) Phosphoric acid h) Hydrophosphoric acid
12. What are the prefixes used to name molecular compounds and organic compounds
(These will the molecular prefixes wil NOT be given on exam)? - List them all
Unit 3 (cont’d): Chemical Bonding
1.
List the properties of ionic compounds and molecular compounds.
2.
What is electronegativity – which element has the highest electronegativity value?
3.
Bonding: Describe each bond and how it is created.
Ionic Bonding (Ionic compounds)
Metallic bonding – description and properties
Covalent (molecular compounds)
4.
Know what Lewis Dot diagrams & structural diagrams are and how to draw them for compounds.
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Chemistry 20
Mrs. Rogers
5.
VSEPR Theory – know how to determine shape and draw the 3-D shape (stereodiagram)
6 In a _____________________ the electrons are shared equally and have an electronegativity difference of _________________. In a ____________________ the electrons are shared unequally and have an electronegativity difference of
______________. In an ionic compound – the difference in electronegativity is greater than ________________.
7.
8.
9.
Be able to determine if compound has polar covalent bonding or non polar covalent bonding - know what these are - be able to determine what type of bonding a compound will have by calculating with electronegativities.
Determine if a molecule is polar or not. (based on its shape)
Be able to determine which intermolecular bond will occur between two molecules
(London dispersion, hydrogen bond or dipole-dipole).
Unit 4 : Chemical Reactions
1. What are the signs of chemical changes (remember there are 6 signs) and make sure that you can distinguish between a chemical and a physical change.
2.
Know what the reactants are and products are in a chemical equation
3.
State the law of conservation of mass
4.
Be able to identify the types of chemical reaction when given an equation
5.
Be able to balance chemical reactions
6.
Writing chemical reactions from formulas into words and vice versa
Q – Write the following chemical reaction into words
2 Zn (s) + 2 AgNO
3
(aq)

Zn (NO
3
)
2
(aq) + 2Ag (s)
Q – Write the word equation into the equation with the correct chemical formulas for each substance. a) When heat is added, solid calcium reacts with liquid water to produce Calcium hydroxide and hydrogen gas. b) Aqueous Silver nitrate reacts with aqueous potassium carbonate in the presence of the catalyst platinum to produce solid silver carbonate and aqueous potassium nitrate.
7. Finish the following reactions and balance: a) Mg(s) + O
2
(g)
 b) C
3
H
8
(g) + O
2
(g)
 c) KI(aq) + Pb(NO
3
)
2
(aq)

8.
Be able to complete the products when given the reactants for all the types of reactions.
9.
Net ionic Reactions – find the net ionic equation of a chemical reaction.
10.
Heat reactions – be able to write equations in ΔH notation for one mole of a substance in the reaction or be able to put the energy term back into the reaction.
Unit 5: Chemical Quantities and Stoiciometry
1.
Representative Particles - be able to identify the type of representative particle a
4

Chemistry 20
Mrs. Rogers substance is made up of [ atoms, ions, formula units, molecules ]
2.
Be able to calculate Molar Mass of elements and compounds – adding up the avg mass of each element in a compound (molar mass is the total mass of 1 mole of a substance) a) NaOH b) (NH
4
)
3
PO
4
3.
Calculate the number of moles when given certain number of atoms (representative particles)
How many moles are there is 5.2 x 10
24
molecules of oxygen.
4.
Calculate # of moles when given mass or calculate mass when given # moles.
How many moles are there in 15 grams of gold?
5.
Calculate volume when given moles
How many litres are there in 8 moles of oxygen gas (O
2
)
6.
Calculate volume when given grams or calculate grams when given volume:
How many litres are there in 5 grams of hydrogen gas (H
7.
Calculate % composition of a compound such as Ca
3
(PO
4
)
2
2
)
8.
Concentration: Be able to determine the concentration of a compound in a solution as well as determine how much of a compound it would take to produce a certain concentration of a chemical.
9.
Calculate various Stoichiometry Problems –

Remember to balance equation, identify wanted and given and show all your work.

You can either use the three step proportion method or the flow chart method. (note: flowchart will be given to you for this exam, nor will a blank copy be given to you – you will need to have whichever method memorized for the exam) a) In the reaction of methane gas (CH
4
) without oxygen, determine the mass of methane required to produce 23.0 g of water.
_____ CH
4
+ _____O
2

H
2
O + _______CO
2 b) How many moles of magnesium oxide will be produced when 54.2 g of magnesium react with excess oxygen
___ Mg + ______ O
2

_____ MgO c) What mass of candle wax (C
25
H
52
) must be burned to produce 12.5 L of CO
2
_____ C
25
H
52 +
_____
_
O
2

____ H
2
O + ____ CO
2 d) How many molecules of oxygen are required to completely react with 4.00 g of
5

Chemistry 20
Mrs. Rogers lithium bromide?
______ LiBr + _____ O
2

_____ Li
2
O + ____ Br
2
Preparing for you Final Exam
This review contains a lot of questions about knowledge, but only contains a limited number of calculation questions. The best practice for calculations is to go back in your notes and
REDO the numerous questions provided. Also, use your review time wisely and study over a period of several days. This will always produce better results than last minute cramming.
Please ask questions if you are having problems, but I will not just give you answers because you are too lazy to look them up.
One more suggestion – do not throw out your Chemistry 20 material – you might want it if you choose to take Chemistry 30 as the first unit is a review of the main concepts we covered in this course.
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