Syllabus and Summer Assignment
AICE Chemistry 2023-24
Syllabus and Relevant Info
Christopher Pabst
Christopher.pabst@marion.k12.fl.us
NOTE: Summer assignment starts on page 6
Introduction
AICE Chemistry is designed to give you a more complete experience of Chemistry that will
prepare you for both the AICE Chem examinations and future Chemistry college courses.
The only way to complete all the topics in this course is to move at a very rapid pace. I will try to
finish the lecture portion of the course shortly after the end of the third quarter so we can begin
reviewing for the exam.
Course Overview
The course is taught through a series of lectures and laboratories with homework problems,
practice exams/quizzes, and worksheets. Exams comprise the bulk of the grading criteria. It is
very important that you stay on top of your homework assignments (i.e. worksheets, packets, etc)
in order for you to succeed on your quizzes & tests. Please make your work absolutely authentic
and do not copy from some else, as this will severely affect you when it comes time to take a test.
Textbook
Chemistry for Cambridge International As & A level: Coursebook (Ryan, L.; Norris, R) and Practical
Workbook (Norris, R., Wooster, M.). Cambridge University Press 2020.
Physical Chemistry general topics
●
Atomic structure
●
Isotopes
●
Electrons in atoms
●
Periodic trends
●
The mole and Avogadro’s constant
●
Stoichiometry
●
Formula writing, Empirical and molecular formula
●
Reacting masses and volumes of solutions and gases
●
Chemical Bonding (ionic, covalent, metallic, coordinated bonding)
●
Intermolecular forces
●
States of matter and ideal gas law
●
Electrochemistry
●
Chemical Equilibrium
●
Acids and Bases
●
Reaction Kinetics
●
Catalysts
1
Syllabus and Summer Assignment
●
Chemical reactions and reactivity of chlorine, nitrogen and sulfur
Inorganic Chemistry general topics
●
The periodic table: chemical periodicity
●
Trends and properties of elements in period 3, group 2, group 17
Organic Chemistry general topics
●
Isomerism
●
Hydrocarbons: alkanes and alkenes
●
Halogen compounds
●
Hydroxy compounds
●
Carbonyl compounds
●
Carboxylic compounds and derivatives
●
Esters
●
Nitrogen Compounds
●
Polymerization
●
Organic Synthesis
●
Infrared spectroscopy
●
Mass spectrometry
The AICE Chem AS level course will have three examinations at the end of the year
●
PAPER 1 MULTIPLE CHOICE: Written paper, 1hour 15 min, 40 marks (40 Multiple
Choice Questions)
●
PAPER 2 AS LEVEL STRUCTURED QUESTIONS: Written Paper, 1 h 15 min, 60
marks (it includes short answers, explanations and calculations in which work must be
shown)
●
PAPER 3 ADVANCED PRACTICAL SKILLS: 2h, 40 marks (a practical lab must be
performed, data presented and questions are answered based on experimental skills)
Tips for succeeding in AICE Chem
●
Pre-Read!!!! Read the material carefully from the textbook (and notes) before each class.
●
Study AICE Chem every day for at least 30min. This means that if there are no formal
assignments, you should be using this time to review your class notes, read the text, give
yourself a practice quiz, make note cards (this is very helpful), etc. You must manage this
time carefully.
Choose a study partner that you can also use as a lab partner . This class is very difficult if
done alone. Pairs are better than larger groups. Get together at regularly scheduled times
for study and homework. DO NOT begin “splitting up” the work, as this will ultimately
hurt you.
Purchase a study guide and use it for each chapter studied. Sites such as chemguide.co.uk
are very helpful
Avoid getting behind in this course. If you get stuck on a concept or HW set, get help
immediately.
●
●
●
2
Syllabus and Summer Assignment
●
Come early in the mornings for extra help if you need it. I’m also available during lunch if
you let me know beforehand.
The Commitment:
If you’re taking this course, you have already enjoyed success in your academic career. Taking a
course such as AICE Chem will be very different from courses you have taken in the past. It will
involve a level of work and commitment that you may not have experienced before. Below is list
of realities that you must face:
●
Missing class will result in falling behind and extreme difficulty in getting caught up. You
may have been able to manage missing more than a few days each quarter in the past. In
this course multiple missed days will be very hard to make up.
●
Regardless of who teaches this course, it always follows the same pace, has the same
workload, and is the same difficulty level. There is a very specific amount of material that
must be covered for the AICE Test and there is no time to re-teach or slow down if some
students are falling behind. We absolutely must be ready for the AICE Tests in May and
June. You must accept the fact that you will have significant work outside of class and will
need to get help on assignments and lab work.
●
In order for us to save some valuable time later in the course, everyone needs to be ready to
go. Carefully read the information on the packet in the pages that follow.
We are going to have an exciting, challenging and fun year. I look forward working with
you all this year.
Supplies: ** Bring the required items to class everyday**
●
Scientific (non-graphing) calculator (TI-30XIIS or TI-30Xa)
●
1-inch-ring binder or folder. You may share binder with another class.
●
Spiral or composition notebook (very important to take notes)
●
A few sheets of college ruled paper or copy paper for your personal use. You can use this
for note taking as well as for writing lab reports.
●
Pencils AND blue or black ink pens (Lab Reports must be written in black or blue ink only)
●
Highlighters for note taking.
Grading:
Grades will be WEIGHTED as follows:
●
●
●
●
Tests
Quizzes
Labs/Projects
Classwork/Homework
50%
20%
20%
10%
3
Syllabus and Summer Assignment
Grades will be based on:
●
●
●
●
●
●
●
●
UNIT TESTS: Unit tests will consist of a combination of multiple choice, match, true or
false premises, and free response questions. Expect a minimum of 4 per nine weeks. You
will also have and end of quarter exams, expect one each quarter.
Quizzes: Quizzes will be given through the progress of each unit to monitor progress of
learning. Expect one per week. Quizzes will be both announced and unannounced.
IN-CLASS ACTIVITIES: Each lesson includes a diversity of class activities in which all
students are expected to participate and assume an active role.
HOMEWORK: Homework is assigned nearly every day and will consist of
questions/problems that emphasize the concepts learned that day. It is pivotal that you show
all your work on each mathematical problem. Open-ended questions must be answered in
complete sentences. These assignments will be checked for completion at assigned dates.
Some homework will be graded by accuracy unannounced, so do your absolute BEST on
EACH worksheet.
LATE WORK: Each worksheet and assignment have a particular due date and is
EXPECTED that you turn it in the date assigned. A 10% of the grade will be deducted
for EACH day that the assignment is late. You will upload ALL LATE WORK into Google
classroom.
LAB REPORT: Complete a lab report after each experiment performed. Follow the format
on the practical workbook. Get familiar with it and follow all techniques discussed as you
will do a practical exam ON YOUR OWN at the end of the year. Lab reports must be typed
or written in blue or black ink. They are submitted as a group effort and so the grade is
awarded as so. You should become familiar with all the work related to each lab as the
Practical exam at the end of the year is done independently.
DO NOW/EXIT TICKET: A “Do Now” entry usually consists of a class opener or
reflection. A typical ‘Do Now’ will include one or two questions posted at the beginning of
the class to focus on the topic of the day or review a concept previously discussed. At the
end of class, students will be asked to reflect on what they have learned that day through a
variety of different methods. Students are expected to be on-task (answering the Do now)
as soon as they get in class.
INDEPENDENT RESEARCH TASK: Students will be given at least one independent
research task aligned to the standards for literacy in science. The task will involve both a
reading and writing component.
“Put it in the Tray or upload to CANVAS”
Students are expected to turn in assignments or projects via CANVAS or as a hard copy to the
teacher on the due date.
Course Policies and Procedures:
○
○
All Belleview High School policies will be enforced.
Respect all in school and classroom. This includes the teacher, your classmates, and school
property.
○
Clean up after yourself.
○
Refrain from personal hygiene. (i.e. combing hair, applying makeup, etc.)
4
Syllabus and Summer Assignment
○
○
○
○
○
○
○
○
Be in your seat ready to start before the tardy bell rings. This includes having supplies out,
pencils sharpened and homework turned in. We begin class when the bell rings. If you are late,
you will miss something!
Follow directions from the first time given.
Raise your hand and quietly wait to be called on. Please do not interrupt the teacher during
lectures/class discussion unless for a true emergency.
Please remain seated during class time and wait for me to dismiss you at the completion of
each class period. No line is to be formed for dismissal.
Although this is an electronic device friendly school, students using devices for
nonacademic purposes (texting playing games, surfing the net, doing work for another
class, etc.) will have verbal warning and further consequences per school policy.
You are responsible for make-up work. Consistent with school policy, you will be given
FIVE DAYS from your return to complete any make-up work (including worksheets, quizzes,
tests and labs). If you need to make-up a quiz, test or lab, you will need to SCHEDULE A
TIME WITH ME BEFORE/AFTER SCHOOL. It is YOUR responsibility to find out what
you missed while you were absent! Assignments, activities, or labs can be found in Google
classroom. I will not use class instructional time to “catch up” students that have been absent. If
special circumstances such as an extended absence or an overload of make-up work exists,
inform me prior to the five-day limit.
If you missed a lab/experiment, make arrangements with the teacher to make up for it as
soon as possible.
Students should adhere to these policies at all times. If policy violations occur, students can
expect: seat change, student/teacher discussion, phone call home, parent conference, detention,
class removal, and/or referral.
5
Syllabus and Summer Assignment
AICE Chemistry Summer Assignment
Study this packet. Complete all the mathematical calculations shown (pages 12-15) and memorize the
concepts shown below in tables (pages 5-8). It is stated clearly what you are expected to memorize.
You will have a test related to this packet during the first week of school (Thursday/Friday) that will go into
Gradebook.
This packet (pages 12-15) is worth a Quiz grade.
Memorize the following items. Know name, formula (or symbol) and
charges:
Positive Ions (Cations)
1+
2+
3+
4+
ammonium NH 4+
cesium Cs+
copper(I) Cu+
gold(I) Au+
hydrogen H+
lithium Li+
potassium K+
rubidium Rb+
barium Ba2+
beryllium Be2+
cadmium(II) Cd2+
calcium Ca2+
chromium(II) Cr2+
cobalt(II) Co2+
copper(II) Cu2+
iron(II) Fe2+
lead(II) Pb2+
magnesium Mg2+
manganese(II)Mn2+
mercury(I) Hg 2+
aluminum Al3+
antimony(III) Sb3+
bismuth(III) Bi3+
chromium(III) Cr3+
cobalt(III) Co3+
gallium Ga3+ gold(III)
Au3+ manganese(III)
Mn3+ nickel(III) Ni3+
iron(III) Fe3+
carbon C4+
lead(IV) Pb4+
silicon Si4+ tin(IV)
Sn4+
silver Ag+ sodium
Na+
2
mercury(II) Hg2+
nickel(II) Ni2+
strontium Sr2+
tin(II) Sn2+ zinc
Zn2+
6
5+
antimony(V) Sb5+
bismuth(V) Bi5+
Syllabus and Summer Assignment
Memorize the following items. Know name, formula (or symbol) and
charges:
Negative Ions (Anions)
-1
acetate CH3COO –
bromide Br -–
chlorate ClO3
chloride Cl- chlorite ClO2
cyanide CNdihydrogen
phosphate H2PO4fluoride Fhydride Hhydroxide OHhypochlorite ClOiodide Initrate NO3perchlorate ClO4permanganate
MnO4-
-2
-3
carbonate CO32chromate CrO42dichromate Cr2O72oxalate C2O42- oxide
O2peroxide
O222selenide Se
silicate SiO32sulfate SO42- sulfide
S2sulfite SO32Cyanamide, CN22carbide, C22-
7
arsenide As3nitride N3phosphate PO4
phosphide P3phosphite PO3
3-
3-
Syllabus and Summer Assignment
Memorize the following items. Know names and formulas:
Polyatomic
Elements
As2 arsenic
At2 astatine
Br2 bromine
Cl2 chlorine
F2 fluorine
H2 hydrogen
I2 iodine
N2 nitrogen
O2 oxygen
P4 phosphorus
S8 sulfur
Sb4 antimony
Se8 selenium
POLYATOMIC ELEMENTS, ACIDS and COMMON COMPOUNDS
Acids
Common
Compounds
DO NOT MEMORIZE
CH3COOH or C2H4O2
acetic(vinegar)
HBr hydrobromic
H2CO3 carbonic
H2C2O4 oxalic
HCl hydrochloric (muriatic)
HClO hypochlorous
HClO2 chlorous
HClO3 chloric
HClO4 perchloric
HF hydrofluoric
HI hydroiodic
HNO2 nitrous
HNO3 nitric
H2SO3 sulfurous
H2SO4 sulfuric
AlK(SO4)2·12H2O alum
CH4 methane
C6H6 benzene
C10H8 naphthalene (moth balls)
CHCl3 chloroform
CH3OH methyl alcohol or methanol (wood alcohol)
C2H5OH ethyl alcohol or ethanol (drinking alcohol)
CH3COCH3 acetone
C3H5(OH)3 glycerin
C6H8O6 L-ascorbic acid (vitamin C)
C6H12O6 monosaccharide (simple sugar)
C12H22O11 disaccharide (double sugar)
CaCO3 chalk, marble, limestone
CaO quicklime
Ca(OH)2 slaked lime (lime water)
CaSO4 gypsum, plaster of paris
Fe3O4 or Fe2O3 rust
HCHO formaldehyde
H2O water
Hg quicksilver
K2CO3 potash
MgO magnesia
MgSO4 epsom salts
NH3 ammonia
N2O laughing gas
Na2CO3 soda ash
NaCl table salt
NaHCO3 baking soda
NaNO3 saltpeter
NaOCl bleach
NaOH caustic soda or lye
Na2SO4 Glauber’s salt
Na2S2O3 hypo
SiO2 sand,quartz
8
Syllabus and Summer Assignment
Memorize the following items:
THE SOLUBILITY RULES
1.
All compounds containing alkali metal cations and the ammonium ion are soluble.
2.
All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble.
3.
All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb 2+, or Hg22+.
4.
All sulfates are soluble except those containing Hg22+, Hg2+, Ag+, Pb2+, Sr2+, Ca2+, or Ba2+.
5.
All hydroxides are insoluble except compounds of the alkali metals, Ca2+, Sr2+ and Ba2+.
6.
All compounds containing PO43-, S2-, CO 3 2-, and SO32- ions are insoluble except those that also contain
alkali metals or NH4+. 7. Rules above take precedent over rules below.
OXIDATION NUMBER RULES
Oxidation Number: A number assigned to an atom in a molecular compound or molecular ion that indicates
the general distribution of electrons among the bonded atoms. In some cases it is an actual charge of the atom
while in other cases it is a “perceived” charge if shared electrons were “given to” one atom or the other. Which
atom would “get” the electrons is based on electronegativity values.
1. The oxidation number of any uncombined element is 0 (zero). For example, the charge on elements
iron, Fe, is 0. The charge on each hydrogen in H2, a diatomic element, is also 0.
2. The oxidation number of a monatomic ion equals the charge on the ion.
3. The more electronegative element in a binary compound is assigned the number equal to the charge
it would have if it were an ion.
4. The oxidation number of fluorine in a compound is always –1
5. Oxygen has an oxidation number of –2 unless it is combined with F, when it is +2, or it is in a peroxide,
when it is –1.
6. The oxidation state of hydrogen is+1when combined with a nonmetal and is -1 when combined with a
metal.
7. In compounds, the elements of groups 1 and 2 as well as aluminum have oxidation numbers of +1, +2,
and +3, respectively
8. The sum of the oxidation numbers of all atoms in a neutral compound is 0 (zero).
9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the ion.
9
Syllabus and Summer Assignment
KNOW HOW TO NAME AND WRITE FORMULAS!!!
NAMING RULES
A flow chart for naming binary compounds
10
Syllabus and Summer Assignment
RULES FOR NAMING IONIC COMPOUNDS
1.
2.
3.
4.
5.
Balance Charges (charges should equal zero)
Cation is always written first (in name and in formula)
Change the ending of the anion to –ide
If cation has more than one oxidation number, use a Roman Numeral to indicate its charge
If anion is a polyatomic ion, name it.
Naming Review
Practice
NOMENCLATURE PRACTICE
AlCl3
lithium nitride sodium
hydroxide copper (II)
CH4
bromide copper (I)
bromide lead (II)
N3O5
CaO
VO2
Fe(OH)2
CrO2
CuCl2
SI6
H2O SrO
Ba(NO3)2
Ag2O
FeI3
Ni2O3
KBr
Na2O
Li3N
Al2O3
CuO
CuO2 Cu2O
SnBr4
P2O5
NH4OH
(NH4)2S
PbCO3
Sn(NO3)4
Sn(NO2)4
Pb(SO4)2
NaHCO3 sodium
carbonate
phosphate lead (IV)
oxide tetracarbon
octahydride_
ammonium oxide
dinitrogen tetroxide
cadmium (III) phosphide
hydrogen hydroxide
dihydrogen monoxide
iron (III) hydride
mercury (II) sulfate
mercury (I) sulfate lead
(II) carbonate
diphosphorous pentoxide
calcium hydroxide
aluminum nitride cobalt
(III) oxide acetic acid
sulfuric acid phosphoric
acid
11
Syllabus and Summer Assignment
tin (II) iodide phosphorus
trioxide
12
Syllabus and Summer Assignment
Directions:
• Complete the following questions carefully and turn the packet (pages 12-15) to
me the day of the test.
• You will have a test on the material of these pages as well as the tables expected
to be MEMORIZED (the tables and information to be memorized is clearly
labeled (pages 5-8).
• You should be able to write correct names and formulas for ionic and covalent
compounds as well.
I.
Atomic Structure and Isotopes
a. Complete the following table for the isotopes shown
Element
Atomic
Mass Number
Protons
Symbol
Number
Electrons
56
𝑀𝑛
40
55
50
129
56
II.
70
82
139
b. Calculate the average atomic mass for the following fake elements
i. 182Sf atomic mass 182. 00 amu (38% abundant)
184
Sf atomic mass 184.00 amu (35 % abundant)
186
Sf
atomic mass 186.00 amu (27 % abundant)
ii.
Neutrons
77
Pn atomic mass 77.22 amu (39 % abundant) 79Pn
atomic mass 79.18 amu (25 % abundant)
81
Pn atomic mass 81.31 amu (36 % abundant)
Electrons, energy levels and atomic orbitals
a. How many electrons can fill these each subshell?
i. s ______
ii. p ______ iii. d ______
b. Write the electron configuration for the following atoms and ions i. Sr
13
Syllabus and Summer Assignment
ii. Br1- iii.
Fe3+ iv. Ag
v. Ag1+
vi. Te2c. Draw the orbital diagram (
i. Sr2+
) for the following atoms and ions
ii. As iii. Fe
iv. Mn
d. Write the shorthand electron configuration (noble gas notation) for the following i.
V
ii. Rb
iii. In
III.
Write formulas and names for the following compounds
a. Cr(N3)2
b. Fe(IO2)2
c. C3N5
d. Ga2(CrO4)3
e. N3O7
f. I6O10
g. CuMnO4
h. AgOH
i. Lead (IV) sulfite
j. Aluminum telluride
k. Tetraphosphorus octochloride
l. Carbon monosulfide
m. Cadmiun nitride
n. Chromium (VI) nitride
o. lithium oxalate
p. Nickel (II) dichromate
IV.
Classify and Balance the following chemical equations
________a. ___CaCO3 + ___H3PO4  ___Ca3(PO4)2 + __ H2CO3
________b. ___Cr(OH)6 + ___H3PO3  __Cr(PO3)2 + ___H2O
________c. ___Al(OH)3 + ___Ca3N2  ___AlN + ___Ca(OH)2
________d. ___Ga2O3  ___Ga + ____O2
14
Syllabus and Summer Assignment
________e. ____CO(g)
+
___H2(g) 
____C8H18(l) +__H2O (l)
_______f. ___C5H8O + ____O2  ___CO2
_______g. ___C5H8O + ____O2 🡪 ___CO2
+ ___H2O
+ ___H2O
IV. Perform the following conversions and round to the answer to the correct number of significant figures and
round accordingly.
1. Convert 3.7 moles of FeCl3 to grams of it.
2. Convert 286 g Mn2(S2O3)3 to moles of it.
3. How many moles are in 312 g of of Lead (IV) sulfite?
V. Stoichiometry. Perform the following stoichiometry conversions. Report answer with the correct number of
significant figures and round accordingly.
1. Given the following equation:
Al2(SO3)3 + NaOH  Na2SO3 + Al(OH)3
a) If 88 g of Al2(SO3)3 react with 40 grams of NaOH, which one is the limiting reactant and how many
grams of the Al(OH)3 will be formed?
2. Given the following equation:
Al2O3 +
Cr 
CrO2 +
Al
a) 201 grams of Al2O3 react with 65 grams of Cr, which one is the limiting reactant and how many
grams of Al will be produced?
b) If 21 grams of Al are produced what will be the percent yield?
15
Syllabus and Summer Assignment
VI. Indicate which compounds are soluble or insoluble in water.
a. NaOH
b. NaCl
c. KClO4
d. CuSO4
e. BaSO4
f. SrSO4
g. Mg(OH)2
h. Ba(OH)2
i. K2CO3
j. CaCO3
k. AgI
l. AgCl
m. AgBr
n. NaNO3
o. NH4NO3
VII. Indicate the oxidation number for each of the underlined elements in the following substances
a. Cl2
b. KMnO4
c. MnO2
d. Mn
e. CaCO3
f. CH4
g. Cr2O7-2
h.
i.
j.
k.
l.
Na2CrO4
Cr
CrO3
HBr
Br2
16