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Norris Codes ---- SA = State Assessment, TO= Teacher Observation, Text = (Modern Chemistry - 2002 ) & related material
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Chemistry is a course that explores the properties of substances
and the
changes that substances undergo. The student will investigate
the following:
Atomic Structure --------------------------------------- Chapters 3-7,
22
Matter and Energy --------------------------------- Chapters
1-3, 8, 10, 13, 17
Interactions of Matter ------------------------------ Chapters
1-3, 6-11
Properties of Solutions and Acids and Bases ------ Chapters 7, 13-16
Students should explore chemistry through inquiry, hands-on
laboratory investigations, individual studies and group activities.
The student's experiences in chemistry should enable them to understand
the role of chemistry in their lives by investigating substances
that occur in nature, in living organisms and those that are created
by humans. Their study should include both qualitative and quantitative
descriptions of matter and the changes that matter undergo. Students
should practice the necessary precautions for performing safe
inquiries and activities and appreciate the risks and benefits
of producing and using chemical substances.
Atomic Structure
Standard Number: 1.0 Atomic Structure ------- Chapters 3, 4, 5, 6, 7, 22
Standard: The student will investigate atomic structure and its implications for physical and chemical properties.
Learning Expectations:
The student will:
1.1 compare and contrast various models of the atom as they have emerged historically, from the Greeks to the modern electron-cloud model. ----- 3.1, 3.2, 4.1, 4.2
1.2 investigate the basic organization of the modern periodic table, including atomic number and atomic properties.----- Chapter 5
1.3 describe models of the atom in terms of orbital, electron configuration, orbital notation, quantum numbers and electron-dot structures.----- 4.2, 4.3
1.4 investigate the composition of the nucleus so as to explain isotopes and nuclear reactions.----- 3.2, 3.3, 22.1
1.5 relate the spectral lines of an atom's emission spectrum to the transition of electrons between different energy levels within an atom.----- 4.1
Performance Indicators State: for Standard Number 1.0 Atomic Structure ------ Chapters 3 - 6
As documented through state assessment,
Level 1, the student is able to
Level 2, the student is able to
1.21SA- identify the
major characteristics of various models of the atom: Democritus,
Thomson, Rutherford, Bohr, and the modern quantum mechanical model.
----- 3.1-3.2,
4.1-4.2,
1.22SA- determine the number of protons, neutrons and/or
electrons in an atom or ion, given the symbol of the atom or ion
and a periodic table. --3.3
1.23SA- compare s and p orbitals in an energy level in
terms of general shape, energy and/or numbers of electrons possible.
----- 4.2-4.3
1.24SA- determine the Lewis electron-dot structure or number
of valence electrons for an atom of any main group element (1,
2, 13-18), given its atomic number or its position in the periodic
table.----- 6.2
Level 3, the student is able to
1.31SA - describe the trends
present in the periodic table with respect to atomic size, ionization
energy, electron affinity or electronegativity.----5.3
Performance Indicators Teacher: As documented through teacher
observation, Level 1, the student is
able to TO1.11 o identify an isotope when given the number of protons
and neutrons. ----- 3.3 Level 2, the student is
able to TO1.21 o write the arrangement of electrons in the following
three ways: Level 3, the student is
able to TO1.31 o compare s, p, d, and f orbitals in an energy level
in terms of Sample Task: Flame Test Demonstration Matter and Energy Standard Number: 2.0 Matter and Energy ------- Chapters 1, 2,
3, 8, 10, 13, 17 + Chemcard 3 & 6 Standard: The student will investigate the characteristics
of matter and the Learning Expectations: The student will: 2.1 The student will investigate the characteristics of matter.----- Chapters 1,
2, 3, 8, 13, 2.2 The student will explore the interactions of matter and
Performance Indicators State: for
Standard Number 2.0 Matter and Energy As documented through state assessment, Level 1, the student is able to 2.11SA- identify a pure substance
as element or compound, when given its chemical name or formula.
----- 1.2 Level 2, the student is able to 2.21SA- distinguish among gases,
liquids and solids in terms of particle spacing and relative movement,
given a diagram or scenario. ----- 1.2,
8.1, Chp. 12 Level 3, the student is able to 2.31SA- demonstrate an understanding
of the law of conservation of energy by equating heat loss and
heat gain in an interaction, given the formulas -q = q and q =
mcD t, and the specific heat. ----- 17.1,
Calorimetry lab
Performance Indicators Teacher: As documented through teacher
observation, Level 1, the student is
able to TO2.11 o estimate equivalent Fahrenheit and Celsius temperatures
and Level 2, the student is
able to TO2.21 o distinguish between accuracy and precision. ----- 2.3, chemcard 3.19 Level 3 , the student is
able to TO2.31 o using a calorimeter, identify an unknown metal by
determining its Sample Task: Bell, Jerry. "Mystery Powders: An Inquiry Activity."
Chemistry in the Interactions of Matter Standard Number: 3.0 Interactions of Matter ------- Chapters 1, 3, 6, 7, 8, 9,
11 Standard: The student will examine the interactions of matter. Learning Expectations: The student will: 3.1 investigate chemical bonding.---------
Chapter 6 3.2 analyze chemical reaction--------------
Chapters 1, 6, 7, 8, 9, 11, 15 3.3 explore the mathematics of chemical formulas and equations.
--------- Chapters 1, 6, 7,
8, 9, 11 Performance Indicators State: for
Standard Number 3.0 Interaction of Matter As documented through state assessment, Level 1, the student is able to 3.11SA- distinguish between
a chemical symbol and a chemical formula, given examples. ----- 1.3, 6.1, 7.1, 8.1, Chp.1, Teacher Level 2, the student is able to 3.21SA- distinguish between
ionic and covalent compounds, given binary formulas. -----
6.3, 7.1-7.2 mass, number of moles, number
of particles, molar volume (at STP) 3.27SA- determine molar ratios
expressed in balanced chemical equations. -----
9.1, Level 3, the student is able to 3.31SA- identify and solve
different types of stoichiometry problems (volume (at STP) to
mass, moles to mass, etc...) ----- 9.2,
11.1, 11.3
TO1.12 o draw Bohr models for the first 18 elements.----- 4.1 + teacher notes &direction
+ orbital notation ----- 4.3
+ electron configuration notation -----
4.3, 5.2
+ electron-dot notation ----- 6.2
TO1.22 o predict the charge of an ion usually formed by the
main-group
elements (1, 2, 13-18) using the periodic table. ----- Chp. 5 review, Chp. 7 review, chemcard
TO1.23 o organize atoms from the main- group elements (1,
2, 13-18) based
on atomic radii. ----- 5.3
TO1.24 o support the existence of the atom using the Laws
of Definite
Composition, Conservation of Matter and Multiple Proportion ----- 3.1, chemcard 1.10
TO1.25 o calculate the average atomic mass of an element from
the percent
distribution and masses of isotopes. -----
3.3
TO1.26 o identify and/or explain the formation of anions and
cations. ----- 5.3
TO1.27 o use the Bohr model to draw an electron moving from
its ground
state to an excited state, and/or represent the emission of energy
as it returns from an excited state to a lower energy state. ----- 4.1
TO1.28o recognize names of famous scientists and identify
their major
contributions: Neils Bohr, James Chadwick, John Dalton, Max
Planck, Ernest Rutherford, J.J. Thomson. -----
3.1-3.2, 4.1
TO1.29 o describe the differences between the Bohr model of
the atom and
the quantum mechanical (QM) electron-cloud model of the atom.
----- Chapter 4
TO1.210 o calculate wavelength, frequency or energy of a photon
of
electromagnetic radiation, given the formula and constants. ----- 4.1
TO1.211 o research careers that relate to atomic structure,
such as
astronomy, nuclear medical technician, research physicist,
chemist, etc.----- 1.1, p 19, p 220,
research
general shape, energy or number of electrons possible. ----- 4.2-4.3
TO1.32 o determine quantum numbers for elements given the
electron
configuration. ----- Chapter 4, teacher
notes
TO1.33 o explain in a paragraph why some elements do not have
the predicted
electron configuration; for example, copper tends to have an
electron configuration of [ Ar] 4s13d10 instead of [ Ar] 4s23d9
----- 4.3, (p 119)
TO1.34 o justify the quark combinations that make protons
and neutrons,
given the charges of the up and down quarks. -----
not in MC text, teacher provided or research
TO1.35 o write the nuclear equation involving alpha or beta
particles,
given the mass number of the parent isotope and complete symbols
for alpha or beta emissions.-----
Chp. 22 problems
interaction of matter and energy.
energy. ----- Chapters 3, 8, 10, 13,
17
2.12SA- distinguish among
elements, compounds, solutions, colloids, and suspensions, given
examples. ----- 1.2, 13.1
2.13SA- classify changes in
matter as physical or chemical, given examples or scenarios. ----- Chapter 1
2.14SA- classify properties
of matter as physical or chemical when given
examples or scenarios. ----- 1.2
2.15SA- distinguish between
heat content and temperature when given a unit, a definition and/or
an example.----- 17.1
2.22SA- predict the effect
of changing one gas variable (volume, temperature or pressure)
on one of the others, given a scenario. -----
Chapter 10
2.23SA- demonstrate an understanding
of the law of conservation of matter, given experimental data.
----- 3.1
2.24SA- categorize a process
as endothermic or exothermic, given an example or scenario.----- 13.2, 17.1, 17.3
convert between Celsius and Kelvin temperature scales. ----- 10.3, + chemcard 3.16, Teacher notes
TO2.12 o measure the mass and volume of solids and liquids
using
appropriate equipment, methods and units. -----
Laboratory
TO2.13 o determine the density of solids and liquids. ----- 2.2, + labs
TO2.14 o read a thermometer and express the temperature accurately.----- Lab
TO2.22 o create data tables and graphs from experimental data.
----- throughout
TO2.23 o analyze data by computing a percentage error. ----- Chp. 2 + labs
TO2.24 o record measurements and results of calculations using
the correct
number of significant figures. -----
begin 2,
continue throughout, chemcard
# 6
TO2.25 o characterize a relationship between
two variables as directly or
inversely proportional.----- Labs
+ throughout text
TO2.26 o use conversion factors, dimensional analysis and/or
ratio and
proportion to convert between quantities. -----
Begin Chp. 2 + throughout
TO2.27 o express large and small numbers using scientific
notation and
perform calculations in scientific notation. -----
Begin Chp. 2 + throughout
TO2.28 o practice appropriate safety procedures when working
in the
laboratory. ----- throughout, cosmic
chemistry LD
TO2.29 o research careers that relate to matter and energy
such as,
surveyor, carpenter, structural engineer, HVAC technician,
pathologist, etc.----- throughout
specific heat. ----- LAB WORK - experiment
17-1
National
3.12SA- identify the parts
(reactants or products) of a chemical reaction, given a balanced
chemical equation. ----- Teacher, 1.2, 8.1
3.13SA- identify the types
of chemical reactions (composition, decomposition, double replacement,
single replacement), given a balanced equation. -----
8.2
3.14SA- determine the number
of atoms, formula units or molecules of a particular substance,
given a balanced equation.----- Teacher,
Chp. 8
3.22SA- identify the formula
for a compound using a periodic table and a list of common ions,
given the name of the compound ----- 7.1
3.23SA- identify the name
of compounds and common acids (sulfuric acid, nitric acid, hydrochloric
acid, acetic acid, and phosphoric acid), using a periodic table
and a list of common ions. ----- 7.1, 15.1
3.24SA- select a correctly
balanced chemical equation, when given examples. -----
Chp. 8
3.25SA- recognize a balanced
chemical equation using appropriate symbols, given a word equation.
----- Chp. 8
3.26SA- convert between any
two of the following quantities of a substance:-----
3.3, 7.3, 9.2, 11.1
3.28SA- analyze percent composition
of the elements in a compound, given the formula. -----
7.3,
3.29SA- solve mass to mass
stoichiometry problems----- 9.2
Performance Indicators Teacher:
As documented through teacher observation,
Level 1, the student is able to
TO3.11 o write a balanced equation and identify the reactants and products.--------- Chapter 8
Level 2, the student is able to
TO3.21 o draw models of atoms bonding ionically and covalently.
--------- Chapter 6
TO3.22 o write the formulas for compounds, given the names
of compounds. ---------
Chapter 7.1-7.2
TO3.23 o write the names of compounds given
examples of chemical formulas
using the stock system. ---------
7.1-7.2
TO3.24 o write a balanced chemical equation and classify as
to type, given
a word description of a chemical reaction. --------- Chapter 8
TO3.25 o calculate and measure the actual molar mass of a
substance and
relate it to the number of particles. --------- 9.2 + Lab exercise
TO3.26 o predict the products of a single or double replacement
chemical
reaction, given an activity series and a solubility chart. --------- Chapter 8.2-8.3, Teacher
provided solubility charts (not in text)
TO3.27 o research careers that relate to interactions of matter,
such as
pharmacist technician, industrial chemist, chemical technician,
chemical engineer, etc.-----1.1-1.2,
7.2, videos, student research
Level 3, the student is able to
TO3.31 o draw shapes of molecules and label bond angles, bond
polarity and
molecule polarity, given a formula. --------- Chapter 6.5, video - "Atom Bond"
TO3.32 o predict amounts of product given mole or mass amounts
of reactants
in an actual lab experience and compare actual yield to
theoretical yield. ---------
Chapter 9.3, Lab Exp. 9-1 p. 816
TO3.33 o use percentage composition to determine the empirical
or molecular
formula of an unknown substance. ------- 7.3-7.4
Solutions and Acids/Bases
Standard Number: 4.0 Solutions and Acids/Bases ------ Chapters 7, 13-16
Standard: The student will investigate the characteristics
of solutions
including solutions of acids and bases.
Learning Expectations:
The student will:
4.1 The student will investigate the characteristics of solutions.------ Chapters 13, 14 , lab
4.2 The student will investigate the characteristics of acids
and
bases.------ Chapters 7, 15,
16, labs
Performance Indicators State: for Standard Number 4.0 Solutions and Acids/Bases
As documented through state assessment,
Level 1, the student is able to
4.11SA- classify substances
as acid or base, given the formula of an
inorganic acid or base.----- 7.1, Chp. 15
Level 2, the student is able to
4.21SA- identify the
solute and solvent in a solid, liquid or gaseous solution, given
its composition. ----- 13.1
4.22SA- classify a solution
as saturated, unsaturated or supersaturated, given the composition
of the solution and a solubility graph. -----
13.2
4.23SA- calculate the concentration
of a solution in terms of molarity or mass percent, given mass
of solute and mass or volume of solution. -----
13.3
4.24SA- classify a substance
as an acid or a base, given at least two of the following properties:
color of litmus, color of phenolphthalein, taste, pH and slippery
or non-slippery.----- 15.1, Chemcard
Level 3, the student is able to
4.31SA- predict the products
of a neutralization reaction involving inorganic acids and bases,
given the reactants. ----- 15.2-15.3
Performance Indicators Teacher:
As documented through teacher observation,
Level 1, the student is able to
TO4.11 o demonstrate the factors (temperature, stirring, particle
size and
concentration) that affect the rate at which a solute dissolves.
------ 13.2
TO4.12 o investigate the acidity/basicity of substances by
observing their
effect on various indicators.
------ 15.1, Exp16-3, Microlabs
Level 2, the student is able to
TO4.21 o describe how to prepare a dilute solution from a
concentrated
solution of known molarity. ------
13.3, Teacher, labs, Chem Guide to Prob. Solving pp. 180-183
TO4.22 o perform a neutralization reaction. ------ 15.3, labs
TO4.23 o research careers that relate to solutions, such as
cosmetologist,
environmental scientist, water quality control technician, artist,
etc.---- research
Level 3, the student is able to
TO4.31 o investigate colligative properties, i.e. the effect
on freezing
point and boiling point when a solute is added to a solvent. ----- 14.2
TO4.32 o demonstrate knowledge of neutralization reactions
by performing a
titration. -----
lab work
TO4.33 o calculate molality of solutions. ----- 13.3
TO4.34 o classify a solution as neutral, acidic, or basic,
or calculate its
pH, given the hydrogen ion concentration or hydroxide ion
concentration. ----- Chapter
16
Sample Task:
Students will classify various household substances as acid
or base using
various natural and synthetic indicators.
