(2) SCH3U Matter and Chemical Bonding – September 8th to September 12th 2014 (FLIP WEEK)
Date
Mon
Sept
8th
Tues
Sept
9th
Topic/Activities
1. Junior Chemistry Review DUE TODAY!
2. Optional ClassNet PRINT: Fundamental Atomic
Particles (PPT)
a. Atomic Number
b. Mass Number
c. Standard Atomic Notation
Learning Goals
 I can explain the
relationship between the
atomic number and the
mass number of an
element

I can state the periodic
law, and explain
patterns in the electron
arrangement

I can explain the
relationship between
isotopic abundance of
an element's isotopes
and the relative atomic
mass of the element
3.
Fundamental Atomic Particles Practice (ws)
1.
Ion Formation (PPT)
a. Metals vs. Nonmetals
b. The Octet Rule
c. The Duet Rule
d. Positive Ions – Cations
e. Negative Ions – Anions
f. Multivalent Ionic Charges
g. Polyatomic Ions
Ion Formation and Internet Research Practice (ws)
Complete Ion Formation
and Internet Research
Practice (ws)
ClassNet PRINT: Isotopes, Radioisotopes, and
Atomic Mass (PPT)
a. Isotopes
b. Isotopic abundance and average atomic mass
c. Radiation and Radioisotopes
d. Half-lives
p. 32 Practice
UC # 9, 12, 13 (calculate
only do NOT graph), 14
2.
Wed
Sept
10th
Homework
Complete Fundamental
Atomic Particles Practice
(ws)
1.
2.
Isotope and Radioactive Practice (ws)
Study for Junior
Chemistry Review
Quiz Thursday
September 11th
p. 29 Practice
UC # 1, 2, 3, 4, 5, 6, 7, 8
Success Criteria
 key vocabulary: atom, electron, proton, neutron,
energy level, valence shell, valence electrons, atomic
number, mass number
 standard atomic notation includes elements symbol,
mass number (rounded), and atomic number
 describe the evolution of the atomic theory and
describe the structure of an atom as represented by
several different models
 describe how the Bohr-Rutherford diagram represents
electrons as orbiting the nucleus of an atom and how
it helps us to predict the properties of an element
 identify the atomic number of an element as the
number of protons in the nucleus and the number of
electrons in a neutral atom
 identify the mass number as the sum of the protons
and neutrons in the nucleus of an atom
 represent atoms using each of three methods that
incorporate the mass number of the atom
 key vocabulary: full or stable octet, octet rule, duet
rule, cation, valence, anion, multivalent,
polyatomic ion
 state the octet rule by describing that atoms tend to
gain or lose electrons to achieve the arrangement of
electrons, known as a stable octet, of the nearest
noble gas
 identify metals as likely to lose electrons to form
positively charged ions called cations
 identify non-metals as likely to gain electrons to
form negatively charged ions called anions
 distinguish the ions formed by multivalent
elements using classical names and IUPAC names
 identify polyatomic ions as being composed of
more than one atom
 describe the roles of various ions in the human
body
 key vocabulary: isotope, isotopic abundance, mass
spectrometer, radioactive decay, nuclear radiation,
alpha particle, beta particle, gamma ray,
radioisotope, radioactive, atomic mass
 describe how isotopes of an element are alike and
how they differ through a comparison of the
compositions of the atoms
 relate the instability of radioisotopes to the
Date
Topic/Activities
Homework
Learning Goals
 I can explain the
relationship between
the atomic number and
the mass number of an
element, and the
difference between
isotopes and
radioisotopes of an
element
Thurs
Sept
11th
QUIZ: Junior Chemistry Review
Seeing Periodic Table
Trends Activity
a. Atomic/ionic radius
b. Ionization energy
c. Electronegativity

The Modern Periodic Table
1.
2.
3.
Students to read p. 17 – 18 “Mendeleev &
Periodic Table”
Video – “The Periodic Table: Properties of
Elements”
Read pp. 14 – 20 “Organizing the Elements” and
complete questions p. 17 UC #11, p. 19 UC #15,
16, 18, 19 and p.21 UC #4

(Graphing Activity)
DUE Tuesday
September 16th

I can graph data related
to the properties of
elements within a
period (e.g., ionization
energy, atomic radius,
electronegativity, etc.)
and identify general
trends in the periodic
table
p. 42 Practice
UC # 1, 2, 3, 4

p.45 Practice
UC # 5, 6, 7

I can draw BohrRutherford diagrams of
atoms and ions
I can explain why
colours of produced
when metals are
burned (flame test)
Developing a Model of the Atom
4.
5.
Fri
Sept
12th
Read and Summarize pp. 22 – 26 “Developing a
Model of the Atom” – include contributions made
by Democritus, Dalton, Thomson, Rutherford, and
Chadwick in summary
Complete questions p. 26 UC # 1, 2, 3, 5
Developing a Model of the Atom
1. Review Bohr-Rutherford diagrams of atom vs. ion
2. Bohr’s Proposal of Energy Levels - Bohr Model of
the Atom- Demonstration – visible light spectrum,
p.40 discharge tubes and atomic spectra – p. 637 –
line spectra “hydrogen” “neon” – Application of
emission spectra – flame test
3. Introduce Lewis Dot Diagrams
4. Electron Configurations (ws)
I can state the periodic
law, and explain how
patterns in the electron
arrangement
I can explain each
scientists major
contribution to atomic
theory
Electron Configurations
(ws)
Success Criteria
spontaneous generation of other elements,
radiation, and energy
 identify three types of radiation: alpha radiation,
beta radiation, and gamma radiation
 describe the properties of each type of radiation
 calculate the relative atomic mass of an element
from the atomic masses of all its isotopes and the
relative abundance of each isotope
 explain how much of a radioisotope remains
provided ½ life
 describe the evolution of the atomic theory and
describe the structure of an atom as represented by
several different models
 describe how the Bohr-Rutherford diagram
represents electrons as orbiting the nucleus of an
atom and how it helps us to predict the properties
of an element
 identify the atomic number of an element as the
number of protons in the nucleus and the number
of electrons in a neutral atom

identify the mass number as the sum of the protons
and neutrons in the nucleus of an atom
 represent atoms using each of three methods that
incorporate the mass number of the atom
 relate the basis of the atomic mass unit (u) to the
mass of one carbon-12 atom
 Can place atomic theory discovers on a time line
and summarize each scientists contribution(s)





Bohr-Rutherford diagrams include protons,
neutrons, and electrons
Use appropriate symbols for protons and neutrons
Energy levels
Ion charges are include on all Bohr-Rutherford
diagrams of ions
Atom have a neutral charge