SCH 3U
Unit 1: Matter, Chemical Trends, Chemical Bonds
Unit 1 Test Study Guide
The Unit 1 Test will be held on Thursday 8 October 2015.
 You will need (at least) a pencil, an eraser and a dedicated, non-programmable calculator. i-pods, phones and other
non-dedicated “calculators” will not be permitted. A clean periodic table will be provided.
 For the test, you need to KNOW the formulas and charges for the polyatomic ions listed at the bottom of the
nomenclature quizzes.
 If you will not be in class on test day and know ahead of time, it is your responsibility to work something out with
your teacher. If you experience an unforeseen absence on test day, you will be writing the missed test during class
the 1st day you are back at school. If a parent has not already called in to verify the absence, a parent will be
contacted.
 You may choose to keep writing until 12:10 p.m. to make up for travel time and time given over to handing out
the test. At this time, all papers will be collected and no further extra time granted. Questions that remain
unfinished will score zero.
 If you have an IEP and wish to write in Resource it is YOUR responsibility to make your teacher aware of this
request PRIOR to the test date so that alternate arrangements can be made well ahead of time. If your
arrangements mean you will miss a portion of another class, it is YOUR responsibility to speak with the other teacher
involved and to catch up on any missed work.
 Please be aware that the unit test is designed to be completed within the period by the well prepared student.
Atomic Theory
Review terms. Examples: element, compound, atom, nucleus, proton, neutron, electron, valence electron, orbits
or shells, atomic number, mass number, isotope, radioisotope, ion, cation, anion, Bohr Diagram, Lewis Dot
Diagrams for the representative elements. Be sure you understand how the standard notation for atoms works
(eg. 146C and carbon-14) and what the letters A and Z represent.
(Most of these terms were covered in your grade 10 review package. They are also in your textbook.
Accuracy, Precision and Significant Digits
Review the handout we took up in class and pages 614-615 of the textbook. You need to use the established
rules in any and all math problems in this course.
Models of the Atom – Review page 11 of the textbook and the handout completed on this topic.
Trends in the Periodic Table – Review the typed notes on this topic from class and on the website. Review the
Assignment (answer key on website). Review the quiz that dealt with this topic.
IUPAC nomenclature

Give formulae and proper IUPAC names for binary and diatomic molecules and binary and oxoacids ; for
binary ionic compounds; for ionic compounds containing polyatomic ions and/or for any ionic compound
containing mono- or multivalent metals; for hydrates. Use classical names for binary and oxoacids (both
are molecules).

There are many extra nomenclature and formulae practice questions listed under this topic on your unit
outline. Please practice! You now need to KNOW the formulas and charges for the polyatomic ions listed
at the bottom of the nomenclature quizzes.
Intramolecular forces

How is ΔEN calculated? What does it tell us about the type of bonds forming between two atoms?

What is a bond dipole?

How do we represent single, double and triple covalent bonds using Lewis Dot Diagrams? Using structural
diagrams?

How do we represent an ionic bond using Lewis Dot Diagrams?
Drawing Lewis Structures for Molecules and Ionic Compounds

Review how to write out Lewis dot structures to show the formation of molecules and ionic compounds
from their elements (see the model building lab completed in class).
Intermolecular forces

How is the term “intermolecular force” defined?

Be sure you review London dispersion forces, dipole-dipole forces and the special dipole-dipole force
called hydrogen bonding and can determine the type of force(s) present between neighboring molecules.

What kinds of effects do intermolecular forces have on properties of molecules?
Comparing ionic compounds to molecules
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Compare in terms of how we draw the formation equation for each one.
Compare in terms of whether they contain covalent bonds, ionic bonds or both types of bonding (as in
polyatomic ions).
Compare the physical properties of ionic compounds and molecules.
Be sure you can define the term “electrolyte”. Identify whether each of the following substances is
generally considered to be an electrolyte or a non-electrolyte: non-polar molecules, slightly polar
molecules, polar molecules, acids, bases, ionic compounds.
Under what conditions are ionic compounds electrolytes?
Sample problem: Identify which of the following will be held together by ionic bonds and which will be
held together with covalent bonds. Be prepared to state your reasoning.
Na2SO4(s), SO42-, H2SO4,
HCl, C6H12O6
Suggested Textbook Review Questions
- Several questions are provided on your unit outline for each section of the course covered in this unit.
- A list of some of the significant review questions for the unit appears below. The answers to these questions are
posted on the class website, accessible through othspanthers.ca under the staff directory for math and science
and your teacher’s name.
Question Set 1
Periodic table, isotopes, radioisotopes, mass no., atomic no., average atomic mass
Do pg. 19 #1 – 10 (answers are at back of the text for these); pg. 21 #4 – 11;pg. 45 #4, 5; pg. 46 #18, 19;pg.
49 #11, 13, 16; pg. 97 all; pg. 98 #11, 12, 13, 15, 16, 17, 18, 29; pg. 101 #57; pg. 102 #2, 12, 13 (answers are at
back of the text for these)
Question Set 2: Models of the Atom pg. 98 #11, 43;pg. 100 #55; pg. 103 #1
Question Set 3: Nomenclature
Review nomenclature rules, practice sheets and quizzes. You can also do pg. 75 #5, 6, 8, 9, 10;
pg. 89 #4 – 6, 11; pg. 92 #2, 6, 16-19; pg. 98 #31-36, 39; pg. 102 #9, 10
Question Set 4 Periodic Law – page 49 #18
Question Set 5:
Trends in the Periodic Table – review the notes on this topic from class and on the website; review the Assignment
(answer key on website); review the quiz; try pg. 40 #1 – 13; pg. 45 #3, 6-8; pg. 46#12, 13, 15, 16, 20; pg. 47 #24;
pg. 48 #6-8,10; pg. 49 #17, 21, 23, 25; pg. 98 #15, 30; pg. 102 #3 – 5, 11, 15, 17
Question Set 6
Lewis Dot Diagrams and Models of molecules and ionic compounds – page 21 #2; page 59 #3,6; page 75 #12, 14; pg.
89 #12; pg. 90 #18, 21, 33; pg. 93 #12, 13; pg. 98 #18, 36; pg. 101 #58, 59; pg. 103 #18 and the molecule building
assignment
Question Set 7 Electronegativity differences and the bonding continuum – see class note and do the assigned
questions on the back. Also pg. 89 #1 – 3; pg. 89 #13; pg. 90 #28; pg. 92 #1, 3, 4, 5, 8, 9, 15; pg. 101 #60; pg. 102
#7, 8.
Question Set 8 Intramolecular vs intermolecular forces; Effect of forces on properties of a ionic compounds and
molecules
pg. 90 #25; pg. 91 #30, 31, 35 – 37; pg. 92 #7, 10, 21, 22, 23, 24, 25; pg. 99 #37; pg. 101#61, 64, 66; pg. 103 #19,
20, 23, 24, 25