HCS Secondary Curriculum Document

HCS Curriculum: Science 6 – 12 Pre-AP Integrated Chemistry and Physics (High School)

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Hoover City Schools Secondary Curriculum Science, 2006-07

Course Information:

Course Title: Integrated Chemistry & Physics, Pre-AP Grade Level: 10,11

Course Description: This course is a study of chemistry as a microcosm of physics. The course includes the study of basic chemical and physical theories and principles that describe the interactions of matter and energy, the basic forces that exist in nature and the application of the conservation laws (as they apply to energy, momentum and matter). Honors Integrated Chemistry and Physics is designed for those students who possess exceptional mathematical and problem-solving skills as well as outstanding expository writing skills. Students who take this course need to be independent learners, readers with a very high ability to comprehend difficult concepts, and scholars who wish to pursue advanced science courses during the rest of their high school career. This course will focus on laboratory activities and problem solving.

State COS Correlate: Chemistry Core (all) & Physics Core (parts) Calendar Type: Year

Pre-requisite: Pre-AP Biology 9 or 10 Co-requisite: Pre-AP Algebra II or any math above this level

Textbook Title: Modern Chemistry (with Live Ink) Textbook Publisher: HRW

Textbook ISBN: 0-03-073546-7 Textbook Copy Year: 2006

(Supp) Textbook Title: Physics: Principles and Problems

(Supp) Textbook Publisher: Glencoe (Supp) Textbook ISBN: 0-07-845813-7

(Supp)Textbook Copy Year: 2005 Accountability Standards: None LEA Curriculum Authors: Jane Mahon

Date of LEA Approval: Spring 2006

Topical Scope and Sequence:

Unit # 1st Nine Weeks

1 Measurement, Basic Units, Unit Analysis, Dimensional Analysis, Scientific Method,


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Unit # 1st Nine Weeks

Nuclear Structure and Reactions, Basic Chemical Calculations (density, atomic mass, molar mass, mole concept, %composition)

2 Kinematics

3 Forces, Motion, and Statics

Unit # 2nd

Nine Weeks

4 Work Energy Cycle, Conservation of Momentum, and Gravity

5 Electrostatics

6 Atomic Structure and Periodicity

7 Chemical Bonding

Unit # 3rd

Nine Weeks

8 The Language of Chemistry

9 Gases, Liquids, Solutions, and Solution Stiochiometry

10 Thermochemistry and Thermodynamics

Unit # 4th

Nine Weeks

11 Currnet Electyricity and Circuits

12 Acids and Bases

13 Chemical and Physical Equilibrium

Units and Outcome-Based Objectives:

Unit 1- Measurement, Calculations, and Nuclear Chemistry

Essential Questions:

How is scientific knowledge discovered, verified and communicated?

How is the nucleus of the atom constructed, and how is this different from the

usual view of nuclear structure?

Conceptual Connections:

Discovery

Communication

Uncertainty and Analysis

Experimental Activities:

# Unit 1 Investigations Unit Obj

Correlation Type

(Dem, Exp, Inq)

1 Green Fire 3 Demo


Page 3 of 29


Correlation Type

(Dem, Exp, Inq)

2 Tea Bag Experiment 2,3,21 Inquiry

3 Standards Lab (Physics) 2,3,4,21 Inquiry

4 Reading and Constructing Graphs (Chemistry) 2 – 6,21 Experiment

5 Significant Figures/Accuracy and Precision

(Chemistry) 4,9,21 Experiment

6 Measurement (Chemistry) 3,4,21 Inquiry

7 Laboratory Procedures (Chemistry) 3,4,21 Experiment

8 Finding the Mass of Air in the Classroom

(Density) 2,4,21 Inquiry

9 Properties of Nuclear Particles (ASIM – Nuclear

Scalars) 19,20,21 Experiment

Outcome-Based Objectives:

# Unit 1 Objectives Mastery Level

(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1 Recall a group of specific elements and

symbols from the Periodic Table. Mastery A-3 NA

2 Use the scientific method to logically

approach the solution of a problem. Mastery

P-1

Through

P-11

NA

3 Perform basic laboratory procedures

safely. Mastery

P-1

Through

P-11

NA

4

Use significant digits, scientific

notation, S.I. units of measurement (both

fundamental and derived) and density to

perform calculations involving unit

analysis and dimensional analysis.

Mastery P-4 NA

5

Use mathematical and graphical

methods to express patterns and

relationships determined from sets of

scientific data.

Mastery P-2 NA

6

Distinguish between the relationships

represented by graphs that are linear,

hyperbolic or parabolic.

Mastery P-2 NA

7

Differentiate between: the three states

of matter, elements, mixture, and

compounds, extensive and intensive

properties of matter.

Mastery

A-1

A-5

A-1 a

A-1 c

NA

8

Solve for unknown quantities by

manipulating variables in a given

equation or mathematical formula.

Mastery P-9 NA

9 Distinguish between accuracy and Mastery P-10 NA


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(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

precision, and express accuracy as

percent error.

P-11

10 Define protons, electrons, and neutrons. Mastery A-3 b NA

11 Explain the different particles which

make up protons and neutrons Introduction A-9 a NA

12 Distinguish between mass number and

atomic number. Mastery A-3 b NA

13 Find elements on the Periodic Table

using atomic number. Mastery A-3 b NA

14

Differentiate between metals, non-

metals, and metalloids in the Periodic

Table and by property,

Mastery A-1 b NA

15

Define the term ‘isotope’ and calculate

its number of electrons, protons, and

neutrons.

Mastery A-3 b NA

16 Define the term ‘mole’ and ‘Avogadro’s

Number.’ Mastery A-6 NA

17

Define molar mass and be able to

calculate it for a given atom or

compound.

Mastery A-6 NA

18 Calculate equivalents among grams,

moles, and number of particles. Mastery A-6 NA

19

Identify the characteristics of alpha,

beta, and gamma radiation, and give the

general differences between fission and

fusion (nuclear reactions.)

Mastery A-9 c

A-9 d NA

20

Write nuclear equations and use the

half-life definition to solve problems.

Solve problems involving C-14.

Mastery A-9 b

A-9 e NA

21

Use written and oral communication

skills to present and explain scientific

phenomena and concepts individually or

in collaborative groups using scientific

and non-scientific language.

Mastery P-2 NA

Unit 2- Motion in One Dimension, Vectors, and Projectile Motion (This is a physics unit, so the COS Alignment is from the physics COS.)


How do you describe the motion of an object?



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Change vs consistency

Graphical Anslysis



Correlation Type

(Dem, Exp, Inq)

1 Constructing Motion Graphs 2.1,2.2,2,3 Experiment

2 Free Fall Lab 2.3,2.7,2.8,

2.9 Experiment

3 Projectile Motion Lab 2.8 – 2.12 Experiment/

Inquiry

4 Physical and Chemical Changes 1.7 and 1.14 Experiment



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1

Describe motion in terms of frames of

reference, displacement, time, and

velocity.

Mastery B-1, 4 NA

2 Distinguish between

distance/displacement, speed/velocity. Mastery B-1, 4 NA

3

Use physical data to construct and

analyze position and time, speed and

time, acceleration and time graphs for

both kinematics and free fall.

Mastery B-1, 4 NA

4

Relate average speed to distance

traveled and time elapsed to solve

problems involving such unknowns.

Mastery B-1, 4 NA

5 Define acceleration and suggest a way to

measure it. Mastery B-1, 4 NA

6

Apply kinematic equations to calculate

distance, time, or speed under conditions

of constant acceleration.

Mastery B-1, 4 NA

7

Write the value of the acceleration due

to gravity in both SI units and English

units.

Mastery B-1, 4 NA

8 Describe the behavior of an object in

free fall with and without air resistance. Mastery B-1, 4 NA

9

Calculate the position and velocity at

specific times for a body dropped from

rest, projected vertically downward or

vertically upwards with some initial

velocity.

Mastery B-1, 4 NA

10 Describe and discuss the trajectory of a Mastery B-1, 4 NA


Page 6 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

projectile in the earth’s gravitational

field.

11

Predict the range, maximum altitude,

and time of flight for a given position

for a given projectile when initial speed

and the angle of projection are given

Mastery B-1, 4 NA

12 Define scalar and vector. Mastery B-1 NA

13 Define vector sum and resultant of two

vectors at right angles. Mastery B-1 NA

14 Determine the x- and y- components of a

vector when the angle is given. Mastery B-1 NA

15

For a distance vs. time, velocity vs. time,

and acceleration vs. time graph, describe

what the slope (if it is a line) and the

area under the curve represent.

Mastery B-1 NA

Unit 3-Forces, Motion, and Statics


How does matter move and interact?

What is the relationship between force and motion?

How do forces maintain equilibrium?

How is friction beneficial?


Change

Force and Motion

Structure and Function

Consistency and change



Correlation Type

(Dem, Exp, Inq)

1 Dishes and Tablecloth 8 Demo

2 Newton’s Second Law 6,7 Inquiry

3 Newton’s Third Law and Rockets 9,10 Demo

4 Static and Kinetic Friction Lab 17 - 20 Experiment

5 Factors that Affect Friction 17 - 20 Inquiry

6 Flame Test (Chem. Lab will be done on assigned

day.) Experiment



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(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1

Identify the 4 basic forces that exist in

nature and cite examples of how and

where they are found. Describe Grand

Unification Theory.

Introduction B-1, 4 NA

2 Define net force and explain the effect

that a net force has on a body. Mastery B-1, 4 NA

3 Draw a free-body diagram for a body or

a system of bodies in motion or at rest. Mastery B-1, 4 NA

4

State and give an example of the

application of each of Newton’s Three

Laws of Motion.

Mastery B-1, 4 NA

5 Relate Newton’s first and second law to

kinematics. Mastery

B-1, 4

NA

6

Determine experimentally the

relationship between force, mass, and

acceleration.

Mastery B-1, 4 NA

7

Design an experiment that would show

the variations in acceleration caused by

a change in applied force on a given

mass.

Mastery

B-1, 4

NA

8 Define inertia and give several practical

examples. Mastery

B-1, 4

NA

9 Identify action-reaction pairs. Mastery B-1, 4 NA

10 Explain why action-reaction pairs do not

result in equilibrium. Mastery

B-1, 4

NA

11 Explain the cause of terminal speed. Mastery B-1, 4 NA

12 Distinguish between mass and weight. Mastery B-1 NA

13

Discuss the forces of kinetic and static

friction and suggest a means of

measuring them.

Mastery B-1 NA

14

State the two conditions for static

equilibrium in words and in equation

form.

Mastery B-1 NA

15 Find the normal force exerted on an

object by a rigid surface. Mastery B-1 NA

16

Identify the force of friction (including

direction) acting on an object in various

situations, given the coefficients of

friction between the object and a

surface.

Mastery B-1 NA


Page 8 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

17

Resolve the forces acting on an object

supported by an incline into components

parallel and perpendicular to the incline.

Mastery B-1 NA

18 Solve motion problems by applying the

two conditions of equilibrium. Mastery B-1 NA

19 Demonstrate that the frictional force is

independent of the area of contact. Mastery B-1 NA

20

Demonstrate on a given set of surfaces

that the coefficient of static friction is

greater than the force of kinetic friction.

Mastery B-1 NA

Unit 4-Work-Energy Cycle, Conservation of Momentum, Gravity


If energy is always conserved, how can we speak of an energy crisis?

What does the conservation of energy mean?

How is momentum related to Newton’s Second Law?

How does the mass of an object affect the way it moves?

What holds the universe together?


Consistency and Change

Systems

Models




Correlation Type

(Dem, Exp, Inq)

1 Work and Conservation of Mechanical Energy 1 - 5 Experiment

2 Power Inquiry Lab 9,10 Inquiry

3 Hooke’s Law Lab 6 Experiment

4 Work and Power 1 -11 Demo

5 Conservation of Momentum Lab 13 - 18 Experiment

6 Intermolecular Forces (Chem. Lab) 7.19

(Chem.) Experiment

7 Ionic vs. Covalent Bonding (Chem. Lab)

7.3 – 7.5

and 7.13

(Chem)

Experiment



Page 9 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1

Recognize the difference between the

scientific and ordinary definitions of

work.

Mastery B-4 NA

2 Define the joule, erg, foot-pound as

units of work and energy. Mastery

B-4

NA

3

Recognize that the area beneath a Force

vs. Distance curve is work done over the

distance interval.

Mastery B-4 NA

4 Define and calculate kinetic and

potential energy. Mastery

B-4

NA

5

Demonstrate by example and

experiment the relationship between the

performance of work and the

corresponding change in kinetic or

potential energy.

Mastery

B-4

NA

6

Interpret and analyze Force vs.

Elongation experimental graph for a

Hooke’s Law Experiment. Include the

meaning of the slope of the line.

Mastery B-4 NA

7 Recognize and describe the forms that

conserved energy can take. Mastery

B-4

NA

8 Classify the different types of potential

energy. Mastery

B-4

NA

9 Define and calculate power. Mastery B-4 NA

10

Define and compare the units of watt,

kilowatt, and horsepower as they are

used to measure power.

Mastery B-4 NA

11 Identify situations in which conservation

of mechanical energy is valid. Mastery B-4 NA

12

Design an experiment to demonstrate the

use of the concept of power and a

procedure for computation.

Mastery B-4 NA

13 Define and relate impulse and

momentum. Mastery B-2 NA

14 Compare the momentum of the same

object moving with different velocities. Mastery B-2 NA

15

Derive an equation illustrating the

relationship of a change of momentum

to the impulse.

Mastery B-2 NA


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(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

16

Describe the interaction between two

objects in terms of the change in

momentum of each object.

Mastery B-2 NA

17

Using the Law of Conservation of

Momentum, predict the final velocity of

one object if the initial velocities of both

objects before the collision are known,

and the velocity of one of the objects is

known after the collision. Be able to use

other equations derived from the Law of

Conservation of Momentum.

Mastery B-2 NA

18 Identify collisions as elastic or inelastic. Mastery B-2 NA

19

Apply Newton’s Universal Law of

Gravitation to find the gravitational

force between two masses.

Mastery B-1 NA

20

Determine mass from weight and weight

from mass where a value for the

acceleration is known or can be

calculated from given data.

Mastery B-1 NA

Unit 5-Electrostatics


What is matter made of, and how does matter become charged?

What is electricity, and how is it different from electrical charge.


Change and Consistency




Correlation Type

(Dem, Exp, Inq)

1 Electrostatics Discovery Lab 1-7 Experiment

2 Electrostatics – Interactive Demonstrations 1-7 Demo



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1 Understand and be able to explain the

basic properties of electric charge. Introduction B-8,9 NA


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(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

2 Describe electrical forces between

objects. Mastery B-8,9 NA

3

Explain from the point of view of

electron transfer how an object becomes

charge.

Mastery B-8,9 NA

4

Explain, using the concept of induction,

how objects can attract and repel each

other.

Mastery B-8,9 NA

5 Write Coulomb’s Law in words and

express it in terms of an equation. Mastery B-8,9 NA

6 Relate that the coulomb (C) is the basic

unit of charge. Mastery B-8,9 NA

7 Calculate electric force using Coulomb’s

Law. Mastery B-8,9 NA

Unit 6-Atomic Structure and Periodicity


How do we know that matter has structure and order?

How does the organization of the Periodic Table reflect the structure of matter

and authenticate the quantum mechanical model of the atom?


Structure

Models

Organization



Correlation Type

(Dem, Exp, Inq)

1 Spectrum Tubes 3 Demo

2 Periodic Trends 19 Experiment

3 Wave Lab with Springs 1 Experiment

4 Diamagnetism and Paramagnetism (ASIM) 10,22,23 Experiment



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1

Explain the mathematical relationship

among speed, wavelength, and

frequency of electromagnetic radiation.

Mastery B-6 a NA


Page 12 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

2 Discuss the dual wave-particle nature of

light and electrons. Mastery B-6 c NA

3

Explain the benchmark discoveries that

led to the historical development of

atomic structure: Millikan’s Oil Drop

Experiment, Rutherford’s Gold Foil

Experiment, Thomson’s Cathode Ray,

the photoelectric effect, and atomic

spectra.

Mastery A-3 c NA

3 Describe the Bohr model of the

hydrogen atom. Mastery A-3 c NA

4

Discuss de Broglie’s role in the

development of the quantum mechanical

model of the atom.

Mastery A-3 c NA

5

Compare and contrast the Bohr model of

the atom and the quantum mechanical

model of the atom.

Mastery A-3 c NA

6

Explain how the Heisenberg Uncertainty

Principle and Schrödinger wave

equation led of the idea of atomic

orbitals.

Mastery A-3 c NA

7 List the 4 quantum numbers and their

significance. Mastery NA NA

8

Relate the number of sublevels

corresponding to each of an atom’s main

energy levels, the number of orbitals per

sublevel, and the number of orbitals per

main energy level.

Mastery NA NA

9 List the total number of electrons needed

to fully occupy each main energy level. Mastery NA NA

10

Use the Aufbau Principle, the Pauli

Exclusion Principle and Hund’s rule to

write electron configurations and orbital

notations for any element.

Mastery A-3 a NA

11 Describe the modern Periodic Table Mastery A-3 NA

12

Explain how the Periodic Law can be

used to predict the physical and

chemical properties of the elements.

Mastery A-3 NA

13

Describe how the elements belonging to

a group of the Periodic Table are

interrelated in terms of atomic number.

Mastery A-3 NA

14

Describe the relationship between

electrons in sublevels (orbitals) and the

length of each period on the Periodic

Mastery A-3 NA


Page 13 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

Table.

15

Locate and name the four blocks of the

Periodic Table. Explain reasons for

these names.

Mastery A-3 NA

16 Discuss the relationship between group

configurations and group numbers. Mastery

A-3

NA

17

Describe the locations in the Periodic

Table and the general properties of the

alkali metals, the alkaline earth metals,

the halogens, and the Noble Gases.

Mastery A-3 NA

18 Define atomic and ionic radii, ionization

energy, and electronegativity. Mastery

A-3

NA

19

Compare the periodic trends of atomic

radii, ionization energy and

electronegativity, and explain the

reasons for each.

Mastery A-3 NA

20

Define valence electrons, and state how

many are present in atoms of each main

group element.

Mastery A-3 NA

21

Compare the atomic radii, ionization

energies and electronegativities of the d-

block elements with those of the main-

group elements.

Mastery A-3 NA

22 Write electron configurations and orbital

notations for ions. Mastery

A-3

NA

23

Define the words paramagnetism and

diamagnetism. Classify a metal as

paramagnetic or diamagnetic from its

orbital notation.

Mastery A-3 NA

Unit 7-Chemical Bonding


How does matter interact on an atomic level?


Change

Form and Function

Models


Page 14 of 29

Symmetry



Correlation Type

(Dem, Exp, Inq)

1

Intermolecular Forces (ASIM)

Listed with a physics unit because of the timing,

but will be referred to and the write-up and post-

lab discussion possibly completed during this unit

19 Experiment

2

Ionic vs. Covalent Bonding

Listed with a physics unit because of the timing,

but will be referred to and the write up and post-

lab discussion possibly completed during this

unit.

3-5, 13 Experiment

3 Covalent Bonding Manipulative (models) 9-11, 21 -

23 2 Experiments



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1 Define chemical bond. Mastery A-5 NA

2 Explain why most atoms form chemical

bonds. Mastery A-5 NA

3 Describe ionic and covalent bonding. Mastery A-5 NA

4 Explain why most chemical bonding is

neither purely ionic nor purely covalent. Mastery A-5 NA

5 Classify bonding type according to

electronegativity difference. Mastery

A-3

A-5 NA

6 Define molecule and molecular formula. Mastery A-5 NA

7

Explain relationships between potential

energy, distance between approaching

atoms, bond length, and bond strength.

Mastery B-4 NA

8 State the octet rule. Mastery A-3 a NA

9 Draw Lewis structures (Lewis dot

structures) for molecules. Mastery A-3 a NA

10

Draw Lewis structures for resonance

structures and use these structures in the

explanation of the molecular structure.

Mastery A-3 a NA

11 Explain why some molecules are non-

polar and some are polar. Mastery NA NA

12 Define lattice energy and its significance

With regard to ionic bonding. Mastery NA NA

13 List and compare distinctive properties

of ionic compounds and molecular Mastery A-6 a NA


Page 15 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

compounds.

14

Explain the difference between

empirical formulas and molecular

formulas.

Mastery A-6 a NA

15

Write the Lewis structure for a

polyatomic ion given the formula and

the charge on the ion.

Mastery A-6 b NA

16

Describe the electron-sea model, and use

it to explain the properties of metals:

good conductors of heat and electricity,

shiny, malleable, and ductile.

Mastery

A-1 b

NA

17

Explain the VSPER theory and use it to

predict molecular shapes and shapes of

polyatomic ions.

Mastery NA NA

18

Explain how the shapes of molecules

and polyatomic ions are accounted for

by hybridization theory. Know the

shapes and bond angles for molecules

and polyatomic ions containing 5 or

fewer atoms.

Mastery NA NA

19

Describe the intermolecular forces:

dipole-dipole, London dispersion, and

hydrogen bonding.

Mastery A-5 NA

20 Describe the structure of carbon chains,

branched chains and rings. Introduction

A-2

NA

21

Name and write molecular formulas and

structural formulas for compounds with

up to 10 carbon atoms in alkane series or

the alkene series.

Introduction A-2 NA

22 Name an alkane or an alkene when

given the structural formula. Introduction A-2 NA

23 Draw the structural formula of benzene

and describe its unique properties. Introduction A-2 NA

24 Demonstrate at least 3 applications of

organic compounds in every day life. Introduction

A-2

NA

25

Determine empirical and molecular

formulas for a compound using percent

composition data

Introduction A-6e NA


Page 16 of 29

Unit 8-The Language of Chemistry and Its Quantitative Nature


How do scientists systematically name various types of substances?

How does matter interact on an atomic or molecular level?

How are the interactions of matter expressed quantitavely?


Classification

Organization

Form and Function

Balance

Systems

Symmetry

Ratio



Correlation Type

(Dem, Exp, Inq)

1 Types of Reactions/Evidence of Chemical

Change 17 Experiment

2 Law of Conservation of Mass/Matter 4.7

(Physics) Inquiry

3 Kinetics – The NEW Blue Bottle Reaction 20 Demo

4 S’mores 22 Experiment

5 Mole and Mass Relationships 21 Experiment

6 Limiting Reagent/Reactant 22 Experiment



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1 Explain the significance of a chemical

formula. Mastery A-6 c NA

2

Determine the formula of an ionic

compound formed between two given

ions.

Mastery A-6 b NA

3 Name an ionic compound given its

formula. Mastery A-6 c NA

4 Using prefixes, name a binary molecular

compound from its formula. Mastery A-6 c NA


Page 17 of 29


(Int, Rev, Mas)

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Alignment

Accountability

Alignment

5 Write the formula of a binary molecular

compound given its name. Mastery A-6 c NA

6 Memorize the list of polyatomic ions. Mastery A-6 c NA

7 Use the rules for assigning oxidation

numbers. Mastery A-6 b NA

8 Name ionic compounds of transition

metals using the Stock sytem. Mastery A-6 c NA

9 Calculate the formula mass of molar

mass of any given compound. Review A-6 NA

10

Use molar mass to convert between

mass in grams and moles of a chemical

compound.

Review A-6 NA

11

Classify chemical reactions as

composition, decomposition, single

replacement, double replacement or

combustion

Mastery A-6d NA

Unit 9-Gases, Liquids, and Solution Stiochiometry


How does the motion of matter affect its properties?


Models

Order

Time

Ratio



Correlation Type

(Dem, Exp, Inq)

1 Gas Laws 3-7 Experiment

2 Phase Changes 1 Experiment

3 Exploding Tennis Ball Can 3-7 Inquiry

4 Design to investigate one of the factors which

affect solubility. 14 Inquiry



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1 State the kinetic molecular theory of

matter, and describe how it explains Mastery A-5 NA


Page 18 of 29


(Int, Rev, Mas)

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certain properties of matter and how it

explains phase changes.

2

Explain the difference between a real

gas and an ideal gas in terms of Kinetic

Molecular Theory.

Mastery A-5 NA

3 Define pressure and relate it to force. Mastery A-7 NA

4 Convert units of pressure. Mastery A-7 NA

5

Relate that STP means standard

temperature and pressure, which are

1.00 atm and 273 K

Mastery A-7 NA

6

Define and apply Dalton’s Law of

Partial Pressures using the example of

gases collected over water.

Mastery A-7 NA

7 Use the ideal gas equation to solve for

any of its variables: PV = nRT Mastery A-6 NA

8

Use the ideal gas equation to solve for

the molar mass of a gas or the density of

a gas.

Mastery A-6

A-7 NA

9 Use the Law of Combining Volumes to

solve problems. Mastery

A-6

A-7 NA

10 Use the standard molar volume of a gas

(22.4 l/mol at STP) to solve problems. Mastery

A-6

A-7 NA

11 Calculate stoichiometric problems that

involve both mass and volume. Mastery A-6 NA

12

Use Graham’s Law of Effusion of

determine the relative rates of effusion

of two gases of known molar mass.

Mastery A-7 NA

13

Given the mass of the substance

dissolved (solute) and the volume of the

solvent (dissolving medium, usually

water), calculate the molarity of a

solution.

Mastery A-4 c NA

14 Describe the factors that affect the rate

of solution. Mastery A-4 d NA

15 Use solubility curves to interpret

saturation levels. Mastery A-4 a NA

16

Given the molarity of a solution,

determine the amount of solute in a

given amount (volume in liters) of

solution.

Mastery A-4 e NA

17

Given the concentration of a solution,

determine the amount (volume in L) of

the solution.

Mastery A-4 e NA

18 Given the concentration of a solution, Mastery A-4 e NA


Page 19 of 29


(Int, Rev, Mas)

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Accountability

Alignment

determine how to dilute it to obtain a

solution with a lower molarity.

19

Use solution concentrations in

stoichiometric calculations involving

both masses of substances and volumes

of gases.

Mastery A-6

A-4 e NA

20 Explain the conductivity of electrolytic

solutions Introduction A-4b NA

Unit 10-Thermochemistry and Thermodynamics


What is energy and how does it relate to changes in matter?

How is heat transferred?

What is entropy?



Expansion

Force and Energy



Correlation Type

(Dem, Exp, Inq)

1 Endo- and Exothermic Reactions 10 Experiment

2 Specific Heat of an Unknown Metal 11 Experiment

3 Heat of Fusion 4 Experiment



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1 Distinguish between energy, heat, and

temperature. Mastery

B-4

B-5 a NA

2

Calculate the quantity of heat absorbed

or released during temperature and

phase changes.

Mastery B-5 a NA

3

Explain the conditions required for a

spontaneous physical or chemical

change. (enthalpy and entropy)

Mastery B-5 NA

4 Relate the definition of heat of Mastery B-5 a NA


Page 20 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

formation, ∆Hf, and use ∆Hf to find

∆Hrxn.

5

Use Hess’s Law to find ∆Hrxn when

given a set of equations, or write a set of

equations and look up ∆Hf to find ∆Hrxn

for a reaction that has no data.

Mastery B-4 NA

6

Explain qualitatively that all energy

cannot be converted into useful work,

Second Law of Thermodynamics.

Mastery B-5 NA

7

Explain the relationship between

enthalpy and entropy in the equation ∆G

= ∆Hrxn + T∆S. A change is

spontaneous only if ∆G is negative.

Mastery B-5 a NA

8

Discuss how the temperature of a

chemical or physical change can be

changed to make the change

spontaneous.

Mastery B-5 a NA

9

Draw Potential Energy Diagrams to

show that reactions are endothermic or

exothermic.

Mastery B-5 a

A-8 NA

10 Distinguish between changes that are

endothermic and exothermic. Mastery A-8 NA

11

Use the equation q = m x c x ∆T to

determine any one of the four variables

when the other three are known. Mastery B-5 a NA

12 Calculate the specific heat using a

change in temperature Mastery A-8a NA

Unit 11 – Current Electricity and Circuits Essential Questions:

How does electricity get to my house?

How can Ohm’s Law be used to regulate circuits?


Power




Correlation Type

(Dem, Exp, Inq)


Page 21 of 29


Correlation Type

(Dem, Exp, Inq)

1 Circuit Discovery Lab 3, 7-12 Inquiry

2 Electrical Equivalent of Heat (Joule’s

Experiment) 10, 11 Experiment



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1 Define the ampere as the unit of

electrical current. (Coulomb/second) Mastery

B-9

NA

2

Distinguish be definition and example

between potential energy, electric

potential, and electrical potential

difference.

Mastery B-9 NA

3 Describe the conditions for flow of

electrical change. Mastery B-9 NA

4 Distinguish between conventional flow

and electron flow. Mastery B-9 NA

5

Define the unit of resistance as the

ohm. This is a derived unit and its

more basic units are J/C.

Mastery B-9 NA

6 Define the factors that determine the

resistance of a wire. Mastery B-9 NA

7

Calculate the resistance across a bank

of resistors in series, in parallel, and in

combinations of series and parallel.

Mastery B-9 NA

8 Define emf and its role in DC electrical

theory and circuits. Mastery B-9 NA

9

Define and describe voltage, current

and equivalent resistance of resistors

connected in series, parallel, and

combination.

Mastery B-9 NA

10 Calculate the power loss for a given

DC circuit. Mastery B-9 NA

11

Connect resistors in series, in parallel

and combined. Draw circuit diagrams

for each circuit.

Mastery B-9 NA

12

Design and conduct an experiment

using series/parallel resistors in

conjunction with ammeters and

voltmeters (multimeters).

Mastery B-9 NA

13 Summarize similarities in the

calculation of electrical, and Mastery B-9 NA


Page 22 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

gravitational forces between objects.

Unit 12- Acids and Bases


How are substances classified as acids or bases?


Function

Strength

Taste



Correlation Type

(Dem, Exp, Inq)

1 MOM to the Rescue 1 Demo

2 pH/Acid Base Titration 4 Experiment

3 Properties of Acids and Bases 1 and 2 Inquiry



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1

Describe acids and bases in terms of

strength, concentration, and

neutralization reactions.

Mastery A-4 c NA

2 Relate that pH = -log [H

+]. This is

called the power of the hydrogen ion. Mastery A-4 c NA

3

Relate that [ H+

] x [ OH1-

] = 1 x 10-14

.

This is known as the ionization constant

for water. It can also be written pH +

pOH = 14.

Mastery A-4 c NA

4

Calculate the [ H+

], the [ OH1-

], the pH

and the pOH for any acid or base when

the concentration is given. The [ ] mean

concentration in moles/L or M.

Mastery A-4 c NA

5 Compare and contrast the three theories

of acids and bases. Mastery NA NA

6 Label conjugate acid base pairs in a

given chemical equation. Mastery NA NA

7 Explain why some specific molecules or Mastery NA NA


Page 23 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

ions act only as acids or bases according

to the Lewis definition.

8 Identify common weak acids, such as

vinegar (acetic acid, CH3COOH). Mastery NA NA

9 Identify common weak bases such as

ammonia (NH3). Mastery NA NA

10

Identify the following strong acids:

HClO4, H2SO4, HNO3, HClO3, HCl,

HBr, HI. All other acids are weak. The

strong bases are the hydroxides of the

group I metals. All other hydroxides or

derivatives of ammonia are weak acids.

Mastery NA NA

Unit 13- Chemical Equilibrium


Do reactions ever go to completion?


Equal rates

Ratios

Constancy



Correlation Type

(Dem, Exp, Inq)

1 LeChatelier’s Principle 8,9 Experiment

2 2 NO2(g) ↔ N2O4(g) 1-9 Demo



(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

1

Describe chemical and physical

equilibrium as a dynamic state which

exists when the rate of the forward

reaction equals the rate of the reverse

reaction.

Mastery NA NA

2

Explain why the vapor pressure of a

liquid in a closed system depends only

on the temperature and the nature of the

liquid. Give examples of liquids that

would have different vapor pressures

Mastery NA NA


Page 24 of 29


(Int, Rev, Mas)

COS

Alignment

Accountability

Alignment

and explain in terms of intermolecular

forces of attraction.

3

Write equilibrium constant expressions

for homogeneous reactions and

heterogeneous reactions.

Mastery NA NA

4

Calculate the numerical value of the

equilibrium constant if the equilibrium

concentrations are given or can be

calculated.

Mastery NA NA

5 Write equilibrium constant expressions

for weak acids and weak bases. Mastery NA NA

6

Calculate the pH of a weak acid or a

weak base if its equilibrium constant is

known.

Mastery NA NA

7 Calculate the Ka or Kb if the pH is given. Mastery NA NA

8

Relate how Le Chatelier’s Principle

states that if a change is made in an

equilibrium system, the system will

move to moderate or use up the change.

Mastery A-8 b NA

9

Use Le Chatleier’s Priniciple to predict

which way a reaction will move when a

change in the reaction conditions is

made.

Mastery A-8 b NA

Alabama Course of Study Correlation: Science

COS Title Chemistry Core (all) &

Physics Core (parts) Bulletin 2005, No. 20

Std.

# COS Standard

HCS Unit-

Objective

CONTENT STANDARDS, Chemistry (all)

A-1

Differentiate among pure substances, mixtures, elements, and

compounds. 1.7

a) Distinguishing between intensive and extensive properties

of matter

1.7

1.14

b) Contrasting properties of metals, nonmetals, and metalloids 7.16

c) Distinguishing between homogeneous and heterogeneous

forms of matter 1.7

A-2 Describe the structure of carbon chains, branched chains, and

rings. 7.20 – 7.24

A-3 Use the periodic table to identify periodic trends, including atomic

radii, ionization energy, electronegativity, and energy levels.

1.1

6.11 – 6.23


Page 25 of 29



Std.

# COS Standard

HCS Unit-

Objective

7.5

a) Utilizing electron configurations, Lewis dot structures, and

orbital notations to write chemical formulas

6.10

7.8 – 7.10

b) Calculating the number of protons, neutrons, and electrons

in an isotope

1.10

1.12

1.13

1.15

c) Utilizing benchmark discoveries to describe the historical

development of atomic structure, including photoelectric

effect, absorption, and emission spectra of elements

(Example: Thompson’s cathode ray, Rutherford’s gold foil,

Millikan’s oil drop, and Bohr’s bright line spectra

experiments)

6.3 – 6.6

A-4

Describe solubility in terms of energy changes associated with the

solution process.

a) Using solubility curves to interpret saturation levels 9.15

b) Explaining the conductivity of electrolytic solutions 9.20

c) Describing acids and bases in terms of strength,

concentration, pH, and neutralization reactions

9.13

12.1 – 12.4

d) Describing factors that affect the rate of solution 9.14

e) Solving problems involving molarity, including solution

preparation and dilution 9.16 – 9.19

A-5

Use the kinetic theory to explain states of matter, phase changes,

solubility, and chemical reactions. (Example: water at 25 degrees

Celsius remains in the liquid state because of the strong attraction

between water molecules while kinetic energy allows the sliding of

molecules past one another)

1.7

7.1 – 7.6

7.19

9.1 – 9.2

A-6

Solve stoichiometric problems involving relationships among the

number of particles, moles, and masses of reactants and products

in a chemical reaction.

1.16 – 1.18

8.9 – 8.10

9.7 – 9.11

9.19

a) Predicting ionic and covalent bond types and products

given known reactants 7.13 – 7.14

b) Assigning oxidation numbers for individual atoms of

monatomic and polyatomic ions

7.15

8.2

8.7

c) Identifying the nomenclature of ionic compounds, binary

compounds, and acids

8.1

8.3 – 8.6

8.8

d) Classifying chemical reactions as composition,

decomposition, single replacement, or double replacement 8.11

e) Determining empirical or molecular formulas for a 7.25


Page 26 of 29



Std.

# COS Standard

HCS Unit-

Objective

compound using percent composition data

A-7

Explain behavior of ideal gases in terms of pressure, volume,

temperature, and number of particles using Charles’s law, Boyle’s

law, Gay-Lussac’s law, the combined gas law, and the ideal gas

law.

9.3 – 9.6

9.8 – 9.10

9.12

A-8

Distinguish among endothermic and exothermic physical and

chemical changes. (Examples: endothermic physical—phase

change from ice to water, endothermic chemical- reaction between

citric acid solution and baking soda, exothermic physical- phase

change from water vapor to water, exothermic chemical-

formation of water from combustion of hydrogen and oxygen)

10.9

10.10

a) Calculating temperature change by using specific heat 10.12

b) Using Le Châtelier’s principle to explain changes in

physical and chemical equilibrium 13.8 – 13.9

A-9

Distinguish between chemical and nuclear reactions.

a) Identifying atomic and subatomic particles, including

mesons, quarks, tachyons, and baryons 1.11

b) Calculating the half-life of selective radioactive isotopes 1.20

c) Identifying types of radiation and their properties 1.19

d) Contrasting fission and fusion 1.19

e) Describing carbon-14 decay as a dating method 1.20

CONTENT STANDARDS, Physics (parts)

B-1

Explain linear, uniform circular, and projectile motions using one-

and two-dimensional vectors.

2.1 – 2.15

3.1 – 3.20

4.19 – 4.20

a) Explaining the significance of slope and area under a curve

when graphing distance-time or velocity-time data

(Example: slope and area of a velocity-time curve giving

acceleration and distance traveled)

b) Describing forces that act on an object (Example: drawing

a free-body diagram showing all forces acting on an object

and resultant effects of friction, gravity, and normal force

on an object sliding down an inclined plane)

B-2

Define the law of conservation of momentum. 4.13 – 4.18

a) Calculating the momentum of a single object

b) Calculating momenta of two objects before and after

collision in one-dimensional motion

B-3 Explain planetary motion and navigation in space in terms of

Kepler’s and Newton’s laws.

B-4 Describe quantitative relationships for velocity, acceleration,

force, work, power, potential energy, and kinetic energy.

2.1 – 2.11

3.1 – 3.11

4.1 – 4.12


Page 27 of 29



Std.

# COS Standard

HCS Unit-

Objective

7.7

10.1

10.5

B-5

Explain the concept of entropy as it relates to heating and cooling,

using the laws of thermodynamics.

10.3

10.6

a) Using qualitative and quantitative methods to show the

relationship between changes in heat energy and changes

in temperature

10.1 – 10.2

10.4

10.7 – 10.9

10.11

B-6

Describe wave behavior in terms of reflection, refraction,

diffraction, constructive and destructive wave interference, and

Doppler effect.

a) Explaining reasons for differences in speed, frequency, and

wavelength of a propagating wave in varying materials 6.1

b) Describing uses of different components of the

electromagnetic spectrum, including radio waves,

microwaves, infrared radiation, visible light, ultraviolet

radiation, X rays, and gamma radiation

c) Demonstrating particle and wave duality using Einstein’s

theory for explaining the photoelectric effect 6.2

d) Describing change of wave speed in different media

B-7

Describe properties of reflection, refraction, and diffraction.

(Examples: tracing the path of a reflected light ray, predicting the

formation of reflected images through tracing of rays)

a) Demonstrating the path of light through mirrors, lenses,

and prisms (Example: tracing the path of a refracted light

ray through prisms using Snell’s law)

b) Describing the effect of filters and polarization on the

transmission of light

B-8

Summarize similarities in the calculation of electrical, magnetic,

and gravitational forces between objects. 5.1 – 5.7

a) Determining the force on charged particles using

Coulomb’s law

B-9

Describe quantitative relationships among charge, current,

electrical potential energy, potential difference, resistance, and

electrical power for simple series, parallel, or combination direct

current (DC) circuits.

5.1 – 5.7

11.1–11.13

PROCESS AND APPLICATION STANDARDS

P-1 Observing: Using one or more of the senses to gather information

about one’s environment

1.2

1.3

P-2 Communicating: Conveying oral or written information verbally

as well as visually through models, tables, charts, and graphs

1.2 – 1.3

1.5 – 6


Page 28 of 29



Std.

# COS Standard

HCS Unit-

Objective

1.21

P-3 Classifying: Utilizing simple groupings of objects or events based

on common properties 1.2 – 1.3

P-4 Measuring: Using appropriate metric units for measuring length,

volume, and mass 1.2 – 1.4

P-5

Predicting: Proposing possible results or outcomes of future

events based on observations and inferences drawn from previous

events

1.2 – 1.3

P-6 Inferring: Constructing an interpretation or explanation based on

information gathered 1.2 – 1.3

P-7

Controlling Variables: Recognizing the many factors that affect

the outcome of events and understanding their relationships to

each other whereby one factor (variable) can be manipulated while

others are controlled

1.2 – 1.3

P-8 Defining Operationally: Stating definitions of objects or events

based on observable characteristics 1.2 – 1.3

P-9 Formulating Hypotheses: Making predictions of future events

based on manipulation of variables

1.2 – 1.3

1.8

P-10

Experimenting (Controlled): Conducting scientific

investigations systematically, including identifying and framing

the question carefully, forming a hypothesis, managing variables

effectively, developing a logical experimental procedure,

recording and analyzing data, and presenting conclusions based

on investigation and previous research

1.2 – 1.3

1.9

P-11 Analyzing Data: Using collected data to accept or reject

hypotheses

1.2 – 1.3

1.9

EXPLORE / PLAN / ACT Standards for Transition Correlation: Science

Score

Range EPAS Standard

HCS Unit-

Objective

24 to 27

Compare data from a complex table, graph, or

diagram

Interpolate between data points in a table or graph

Identify or use a simple mathematical relationship

that exists between data

Identify a direct or inverse relationship between

variables in a complex table, graph, or diagram

Compare or combine data from two simple data sets

Combine new, simple information (data or text) with


Page 29 of 29

Score

Range EPAS Standard

HCS Unit-

Objective

given information (data or text)

Understand moderately complex lab procedures

Understand simple experimental designs

Select a simple hypothesis, prediction, or conclusion

that is supported by one or more data sets or

viewpoints

Inv 12.3

Identify strengths and weaknesses in one or more

viewpoints

Post-Lab

discussion

of Inv 12.3

Identify similarities and differences in two or more

viewpoints

Inv 11.1

Class

Discussion

Identify key issues or assumptions in an argument or

viewpoint

Inv 10.2

Class

discussion

of sources

of error.

Determine whether new information supports or

weakens a viewpoint or hypothesis

Inv 9.3

Discussion

of

differences

in results.

28 - 32

Identify or use a complex mathematical relationship

that exists between data

Obj 5.5 and

4.19

Extrapolate from data points in a table or graph 2.1

Compare or combine given text with data from

tables, graphs, or diagrams 2.1

Understand complex lab procedures

Determine the hypothesis for an experiment

Understand moderately complex experimental

designs

Identify an alternate method for testing a hypothesis

Select a complex hypothesis, prediction, or

conclusion that is supported by a data set or

viewpoint

Select a set of data or a viewpoint that supports or

contradicts a hypothesis, prediction, or conclusion

Predict the most likely or least likely result based on

a given viewpoint

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HCS Secondary Curriculum Document

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