NEWARK PUBLIC SCHOOLS PUBLIC SCHOOLS SCHOOL ADVISORY BOARD MEMBERS 2013-2014 Ms. Antoinette Baskerville-Richardson, Chairperson Mr. Marques-Aquil Lewis, Vice Chairperson Mr. Rashon

NEWARK PUBLIC SCHOOLS

Curriculum Guide:

CHEMISTRY

Progressive Science Institute

Taken from New Jersey Center for Teaching and Learning: http://njctl.org/ Page 2


SCHOOL ADVISORY BOARD MEMBERS

2013-2014

Ms. Antoinette Baskerville-Richardson, Chairperson

Mr. Marques-Aquil Lewis, Vice Chairperson

Mr. Rashon K. Hasan

Mr. Alturrick Kenney

Ms. Eliana Pintor Marin

Ms. DeNiqua Matias

Dr. Rashied McCreary

Ms. Ariagna Perello

Mr. Khalil Sabu Rashidi

Mr. Jordan Thomas, Student Representative


NEWARK PUBLIC SCHOOLS ADMINISTRATION

2013-2014

Cami Anderson, State District Superintendent

Chief of Staff & General Counsel: Charlotte Hitchcock

Assistant Superintendent: Mitchell Center

Assistant Superintendent: Brad Haggerty

Assistant Superintendent: Tiffany Hardrick

Assistant Superintendent: Roger Leon

Assistant Superintendent: Aqua Stovall

Assistant Superintendent: Peter Turnamian

Special Assistant, Office of Curriculum and Instruction: Caleb Perkins

School Business Administrator: Valerie Wilson



SCHOOL ADVISORY BOARD

Program and Instruction Committee

Ms. DeNiqua Matias

Dr. Rashied McCreary

Ms. Ariagna Perello

Mr. Khalil Rashidi

Dr. Caleb Perkins, NPS Special Assistant of Curriculum

Valerie Merritt, NPS Director of Board Relations


PROGRESSIVE SCIENCE INITIATIVE: CHEMISTRY CURRICULUM

This course represents the first year in a comprehensive two year sequence of chemistry; students who elect to go on to the second year course, PSI AP Chemistry, will be prepared to take the AP Exam at the end of that course. PSI Physics and Algebra are pre-requisites to this course; the work done in PSI Physics is applied and expanded upon to explain macroscopic phenomenon through an understanding of the microscopic. The course is both quantitative and qualitative in nature, so mathematics will often be applied to the solving of problems. Throughout the year, students will be involved in problem-solving activities on an individual, small group and large group basis. Through this process the ability to read and understand problems, break them down into their component parts and then create and present solutions will be developed. These same skills will be developed with activities in the chemistry laboratory. In that case, problem solving will be done in real time with hands-on problems. Through this process both analytical techniques as well as technological capability will be developed. Integral to the teaching of this course is the use of SMART boards, notebooks and responders. Many of the curricular materials that support this course require that technology in order to develop effective learning on the part of students. Students who have successfully completed this course will be well prepared for PSI Biology. In fact the last two chapters of this course apply the principles of chemistry to biology. In the biology course, a similar approach of developing a microscopic understanding in order to explain macroscopic phenomena plays a key role.

Course Content Outline

Week 1: Nature of Matter, Dalton’s Atomic Theory, Physical and Chemical

Changes, Subatomic particles, Mass Spectroscopy

Week 2: Ions and Isotopes, Average Atomic Masses, Rutherford Models.

Nature of Light and development of Bohr Model, Bohr Model, PES

spectroscopy, Quantum Model, Electron Configurations, magnetism

1. Atomic Structure (Review from Physics)

a. The Wave Nature of Light b. The Double slit Experiment c. Photons and the photoelectric effect d. The Rutherford model of the atom


e. The Nature of Matter f. Dalton’s Atomic Theory g. Subatomic Particles h. Bohr model of the atom i. Rutherford Model j. Ions, Isotopes, and Average Atomic Mass

2. Models of the Atom and the Periodic Table

a. Emission Spectra and the Bohr Model of the Atom b. The Quantum Mechanical Model of the Atom c. Electron configurations and the Periodic Table

3. Periodic Trends

a. Review of Coulombic Attraction (from Physics) b. Periodic trends

i. Atomic size ii. Electronegativity iii. Ionization Energy

c. Valence electrons and periodic trends

4. Ionic Bonding and Ionic Compounds a. Formation of Cation and Anions b. Formation of Ionic Compounds c. Properties of Ionic Compounds d. Naming of Ionic compounds

5. Covalent Bonding and Molecular Compounds

a. Covalent bonding b. Properties of Ionic Compounds and Molecular Compounds c. Naming of molecules d. Lewis Structures e. Multiple bonds f. Formal Charge* g. Resonance structures* h. Exceptions to the octet rule* i. Molecular shapes (the VSEPR model)* j. Polarity of molecules and symmetry

6. Moles and the Periodic Table

a. Avogadro’s Number b. Atomic Mass Unit c. Atomic Weight in AMU versus grams of NA atoms d. Converting between number of atoms and moles of an element e. Converting between volumes and moles of gas at STP f. Converting between mass and moles of an element g. Empirical Formulae h. Molecular Formulae

7. Chemical Reactions


a. Balancing chemical equations b. Precipitation reactions

I. Use of solubility tables to predict reaction II. Use of activity series to predict reaction

III. Net ionic equations c. Oxidation-Reduction reactions

I. Synthesis reactions II. Decomposition reactions

III. Combustion Reactions – completing and balancing

8. Gases, Liquids and solids a. The ideal gas law b. Gas density and molar mass c. Dalton’s law of partial pressures d. Kinetic – molecular Theory e. Average molecular speeds in relation to mass and temperature f. Graham's law of Effusion g. Non-ideal gases

9. Intermolecular Forces

a. Dipole-Dipole b. London Dispersion Forces c. Hydrogen Bonding d. Phase diagrams e. Critical and triple points f. Predicting the characteristics of a material from its molecular formula

i. Boiling points ii. Vapor pressure iii. Volatility

g. Structure of solids and lattice energy


10. Thermochemistry and Thermodynamics a. First Law: Conservation of Energy and its implications b. Exothermic versus Endothermic processes c. Energy as a state function d. Enthalpy of phase changes: fusion and vaporization e. Enthalpy of temperature changes f. Calorimetry g. Specific Heats h. Enthalpy changes during reactions i. Hess’s Law of Heat Summation j. Standard enthalpy and enthalpies of reaction and formation k. Second Law: Entropy and its implications l. Standard entropy m. Entropy of reactions n. Gibbs Free energy and spontaneity o. Free energy and temperature

11. Solutions

a. Concentration units b. Saturated solutions c. Factors affecting solubility d. Colligative properties

12. Chemical Kinetics

a. Reaction rates b. Dependence of rate on concentration c. Dependence of rate on concentration: the Collision Model d. First-order and Second-order reactions e. Potential energy diagrams: Activation energy and ΔH f. Catalysis

13. Chemical Equilibrium

a. The equilibrium constant: forward and reverse rates of reaction b. Calculating Kc c. Le Chatelier’s Principle d. The effects of changes in

i. pressure ii. concentration iii. temperature (in exothermic and endothermic reactions)

14. Acid-Base Equilibrium

a. The Arrhenius model b. The Bronsted-Lowry model c. Autoionization of water and the pH scale d. Strong acids and Strong bases e. Weak acids and Weak bases

15. Oxidation-Reduction Reactions

a. Assigning oxidation numbers


b. Determining oxidation numbers in a compound c. Identifying oxidized and reduced species d. Balancing oxidation-reduction reactions

Extra end of year preparation for Biology 16. Properties of Water

e. The effects of Hydrogen Bonding f. High specific heat: Moderation of temperature g. Polar solvent: role in life h. Density of solid versus liquid form: Insulation due to Floating Ice i. Adhesion and Cohesion j. Acids and bases

17. Organic Chemistry

a. Introduction to organic chemistry b. Carbon and its ability to form four bonds c. Classification of organic compounds: Alkanes, Alkenes and Alkynes d. Functional groups e. Amino Acids f. Aromatic compounds g. Naming organic compounds h. Polymers


Laboratory demos and practical: The laboratory work – Individual and group work. Colorimetry, calorimetry and electrochemistry experiments are performed in groups of two.

1. Observing Chemical Reactions 2. Atomic mass of beanium 3. Flame test – Identifying metal ions in compounds 4. Formation of ionic compounds- Formula of ionic compounds 5. Molecular geometry- A hands on activity using molecular model set-

VSEPR theory 6. Weighing as means of counting- Mole calculations 7. Empirical formula of copper sulfate hydrate 8. Single and double replacement reactions-Activity series 9. Classifying chemical reactions- Analyzing and predicting reaction products 10. Double replacement reactions- Solubility of the products and net ionic

equations 11. Limiting reagent- reaction stoichiometry and yield of a reaction 12. Ideal gas law- Mass of helium in the balloon 13. Heat of reactions and Hess’s law- Small scale calorimetry 14. Depression in freezing point and Molar Mass determination

Guiding Principles

Science Sequence – A fundamental principle of PSI, is that the courses are taught in the sequence of physics-chemistry-biology. This sequence allows students to learn the sciences in a way which minimizes memorization and maximizes understanding. In this sequence, each science becomes the foundation for the next.

Social Constructivism – The core element of the teaching-learning process is an ongoing cycle of brief direct teaching episodes followed by student problem solving, often in groups of 4-5. Problems are designed to engage students in collaborative application of learned principles, maintain them in their zone of proximal development while developing their skills in collaborative teamwork. The use of SMART Responders has strengthened this component significantly.

SMART Notebooks and course materials – All PSI units have been developed by teachers at the Bergen County Technical High School in Teterboro, under the guidance of Robert Goodman, the founder of PSI and the Director of the NJCTL. Lessons are taught in SMART Board-equipped classrooms using SMART notebook technology. All curricular materials are hosted on www.njpsi.org, a site created and maintained by NJCTL. Free access to these materials is available to all students and teachers of science and mathematics for non-commercial purposes (student access to assessments is, of course, restricted). The site is constantly being updated and expanded by a cadre of NJCTL employees as well as participating PSI students and teachers.

http://www.njpsi.org/


SMART Responders – PSI requires all classes be equipped with SMART responders (clickers) that provide for real time formative assessment. Teachers do not have to guess whether students have mastered an assignment or wait until a test, to know whether they have mastered a concept; they know instantly. Frequent use of this technology every day facilitates differentiation of instruction and enhances student motivation. SMART Responder questions are embedded throughout the SMART Notebook units.


Unit Lesson Plan – Atomic Structure

Teacher: Click here to enter text. Time Frame: 10 days

Grade: 10

School:

Subject: PSI Chemistry

NJCCS/CPI 5.2.12.A1

Instructional Objective: (condition, behavior, standard)

SWBAT define and describe electromagnetic radiation and the experiments that describe the wave-particle nature of light.


SWBAT describe the relationship between wavelength, frequency and the speed of light to list givens, determine an unknown variable and correctly calculate the unknown variable.


SWBAT describe the relationship between energy and frequency to solve problems involving energy, frequency and wavelength.


SWBAT describe the wave nature of matter and given the de Broglie wavelength equation, calculate the wavelength of matter.


SWBAT explain historical timeline of the discovery and properties of atoms: Dalton’s Postulates, JJ Thomson’s CRT, Milikan’s Oil Drop, and Rutherford’s Gold Foil that lead to the nuclear model of the atom.


SWBAT describe the three subatomic particles, their charges and location in the atom.


SWBAT differentiate between atoms, ions, and isotopes, identify the atomic number and atomic mass of an element, and calculate average atomic mass

Essential Questions

(What questions will the student be able to answer as a result of the instruction?)

1. How do we describe the nature of light and matter?

2. How were the electron, proton and neutron discovered?

3. What are the properties of an atom and what is its structure?

4. What is an isotope and how is average atomic mass calculated?

http://www.ntuaft.com/njccs/home.html


Knowledge & Skills

(What skills are needed to achieve the desired results?)

By the end of this unit, students will know:

Light is both a wave and a particle

Matter is both a wave and a particle

Thomson’s discovered electrons and the mass-to-charge ratio of the electron in his cathode ray tube experiment (plum pudding model)

Milikan determined the mass and charge of an electron in his oil drop experiment

Rutherford’s Gold Foil Experiment lead to the discovery of a dense, positively charged nucleus (the nuclear atom)

The three subatomic particles that make up an atom are protons, neutrons - both bound together to make up the nucleus - and electrons, which are outside of the nucleus.

Protons are positively charged, electrons are negatively charged, and neutrons have no charge.

The number of protons determines the atomic number and identify of an element. The atomic number also represents the number of electrons in an electrically neutral atom. Atoms that have gained or lost electrons are called ions.

Atoms of an element can have different atomic masses, depending on the number of neutrons. Atoms of an element with different numbers of neutrons are called isotopes. The Average atomic mass of an element is calculated by taking a weighted average based on the relative abundance of each type of isotope found in nature.

By the end of this unit, students will be able to:

Apply the relationship between wavelength, frequency and the speed of light to make calculations for an unknown given two known values.

Given Plank’s constant, apply the relationship between energy and frequency to solve for an unknown variable.

Solve for the wavelength of matter given de Broglie's wavelength equation.

Solve for the average atomic mass of an element given relative abundance of each isotope of an element.

Assessment

(What is acceptable evidence to show desired results (rubrics, exam, etc.)?

After a brief lesson using the SMART Board to introduce concepts, students will be questioned on these concepts using the SMART Response system. The teacher will demonstrate the problem solving skills needed for the topic and again, students will be questioned using the SMART Response system. Students will convene in small groups to complete problems. Then some students may volunteer to write their solutions on the board and explain their problem solving process. Quiz 1: Wavelength & Frequency Lab 1: Observing Chemical Reactions Quiz 2: Atomic Structure Lab 2: Average atomic mass Quiz 3: Subatomic Particles Unit Exam: Atomic Structure

(What is the sequence of activities, learning experiences, etc, that will lead to desired results (the plan)?


Day

Topic Presentation CW/HW

1 Review Light

Wave-Particle Duality

SMART Notebook Slide 1 – 50

CW 1-8; 22-26 HW 9-21; 27-31

2 Wave Nature of Matter

Dalton’s Postulates Slides 51-72

CW 32-36; 42-46 HW 37-41; 48-50

3

Wavelength and Frequency

Quiz Lab Safety Notebook

Lab Safety Notebook Slides

4 Lab Safety Quiz

Observing Chemical Reactions Lab

Observing Chemical Reactions Notebook

Observing Chemical Reactions Analysis

Questions

5

Observing Chemical Reactions Quiz

Discovery of the Electron, Proton, and Nucleus

Slides 74-119 CW 51-54; 58-63; 70-72 HW 55-57; 64-69; 73-76

6

Quiz Atomic Structure Discovery of Neutrons, Isotopes and Average

Atomic Mass

Slides 120-154 CW 77-81; 87-88 HW 82-86; 89-91

7 Average Atomic Mass Lab Quiz Subatomic Particles

Lab and Quiz

8

Average Atomic Mass Lab Quiz

Finish Notebook Quiz Atomic Structure

Slides 155-157

9 MC Review (Optional - Computer Lab phET Review Activity)

10 Atomic Structure Test


Unit Lesson Plan – Electron Configurations and the Periodic Table

Teacher: Click here to enter text. Time Frame: 7 days

Grade: 10

School:

Subject: PSI Chemistry

NJCCS/CPI 5.2.12.A1


SWBAT explain how Bohr developed a model of the atom using evidence from atomic spectra.


SWBAT explain the problem with the Bohr model of the atom and describe the currently accepted Quantum Mechanical model of the atom.


SWBAT describe 4 quantum numbers and explain how to find the probable location of an electron within an atom.


SWBAT create an electron orbital diagram following the Aufbau Principle, Pauli Exclusion Principle, and Hund’s Rule.


SWBAT write electron configurations and shorthand electron configurations


SWBAT derive the periodic table based on the quantum mechanical model of the atom and identify and describe similarities between groups of elements based on electron configurations.


SWBAT identify and describe properties of elements based on their electron configurations and locations on the periodic table including: Alkali Metals, Alkaline Earth Metals, the Oxygen Family, Halogens, and Noble Gases.

Essential Questions

(What questions will the student be able to answer as a result of the instruction?)

5. What is the Bohr Model of the atom?

6. What is the Quantum Mechanical Model of the atom?

7. What are electron configurations?

8. How was the Periodic Table derived?

(What is acceptable evidence to show desired results (rubrics, exam, etc.)?

After a brief lesson using the SMART Board to introduce concepts, students will be questioned on these concepts using the SMART Response system. The teacher will demonstrate the problem solving skills needed for the topic and again, students will be questioned using the SMART Response system. Students will convene in small groups to complete problems. Then some students may volunteer to write their solutions on the board and explain their problem solving process. Lab 1: Spectral Line Lab Lab 2: Flame Test Lab Quiz 1: Electron Orbital Diagram and Electron Configuration Unit Exam: Electron Configurations and the Periodic Table

(What is the sequence of activities, learning experiences, etc, that will lead to desired results (the plan)?

http://www.ntuaft.com/njccs/home.html


Day

Topic Presentation CW/HW

1 Bohr Model of the Atom and Emission Spectra

SMART Notebook Slide 1 – 42

CW 1 HW 2

2 Emission Spectral Lines

Lab Flame Test Lab

3 Quantum Numbers and the

Periodic Table

Slides 44-100 MC 1-12

4 Electron Orbital Diagrams

and Electron Configurations

Slides 101-154 CW 3-7, 13-15, 19-23, 29 HW 8-12, 16-18, 24-28, 30

5

Quiz Electron Orbital Diagram and Electron

Configuration

The Periodic Table

Slides 155-183

CW 31-32 HW 33-34

6

Multiple Choice Review *Point out Aufbau, Pauli

Exclusion and Hund’s Rule will be on the Quest

MC Review Slides 1-56

7 Electron Configurations and the Periodic Table Quest


Periodic Trends PSI chemistry

Essential questions

Why fluorine is very reactive than most of the nonmetals?

Why potassium is more reactive than sodium? Content

Atomic size/radius

Ionization energy

Electronegativity

Ionic size

Metallic character Skills

They will study the trend in the atomic size across and down the period and group.

They will understand the trend in metallic character.

They will study the variation in ionization energy and size of ions.

They will discuss the trend in electronegativity. Activities

They will graphically interpret the trend (atomic size, IE or EN) across periods and discuss the variations.

Bring the elemental sample kit to the class and introduce wherever it fits to the discussion (Flinn scientific)

Assessments

Quiz – on each trend

Quest- Test


Pacing guide

Day Topic Class work Home work

1 Introduction to ENC, shielding, size

1-21

2 Ionization energy Quiz 1

HW help 22-40

3 Electronegativity Quiz-2 or Quiz 1+2

HW help 41-47

4 Metallic character

HW help 48-50

5 Ion formation and size of ions

51-59

6 HW Rev including FR

7 Final quest or test


Ionic Bonding and Ionic Compounds PSI chemistry

Essential questions

What are ions?

What are ionic compounds? Content

Formation and naming of ionic compounds

Naming ionic compounds

Polyatomic ions Skills

They will study the formation of anions and cations.

They will learn the formation of ionic compounds by electron transfer between them.

They will understand the properties of ionic compounds. Activities

They will use the harpoon method to determine the formula of ionic compounds.

Assessments

Quiz – Ions

Quest- Ionic bonding Pacing guide


1 Introduction to periodic Table of elements Formation of ions

1-34

2 Formation of ionic compounds

35-46

3 Naming ionic compounds Quiz

47-60 + practice problems

4 Polyatomic ions and compounds

Home work help 61-70 Practice problems

5 Rev Quiz


Covalent bonding and geometry PSI chemistry

Essential questions

What are molecular compounds?

What elements will form covalent compounds>

What is electron domain geometry?

How do we determine the shape of a molecule?

What make a molecule polar or nonpolar? Content

Formation and naming of molecular compounds.

Drawing Lewis dot structure of molecules and complex ions

VSEPR theory and predicting the geometry of molecules. Skills

They will study the formation of covalent compounds by sharing electron pairs between the atoms. They will distinguish the difference between multiple covalent bonds and coordinate covalent bonds. They will learn to draw the Lewis dot structure for molecules and ions and use it to derive the VSEPR number and then to predict the geometry of the compound. They will understand how the geometry and polarity of the molecules are related and will be able to predict the molecule is going to be polar or not from the molecular geometry.

Activities

They will use the molecular model set to study the geometry of the molecules.

Assessments

Quiz – covalent bonding

Quiz- VSEPR number and geometry


Pacing guide


1 Introduction to covalent bond Lewis dot structure of atoms

1-8

2 Multiple covalent bonds

9-16

3 Lewis dot structure of polyatomic ions and molecules and exceptions to octet rule VSEPR number

22-26 17-33

4 Quiz 1

Home work help

5 VSEPR number and geometry of the molecule

Group work with models Practice Rev

34-55

6 VSEPR number and geometry continued

Class work with models Practice Rev

56-72

7 resonance Practice Rev 73-80

Bond polarity and polar molecules End with naming?

Practice rev 81-106

8 Review Home work help

9 Quiz-final


Mole calculations PSI chemistry

Essential questions

How many atoms are there in 1 g of sugar?

What is the mass of 100ml of Hydrogen?

What is the percent composition of table salt?

How do we determine the formula of a compound from the percent composition?

Content

Avogadro number of particles

Mass – mol, mole-volume, particles –mole problems

Percent composition

Empirical and molecular formula calculation Skills

They will study the relationship between Avogadro number and mass of a substance. They will learn to solve converting moles – particles, mole-mass, mole –volume of different atoms and molecules. They will learn to calculate percent composition of substances and then to calculate the empirical and molecular formula of it.

Activities

They will do problem solving in class.

Lab- counting particles activity Assessments

Quiz – mole-particles

Quiz- mole-mass in grams

Quiz-mole-volume

Quiz- percent composition, empirical and molecular formula

Chapter test


Pacing guide


1 Introduction to Avogadro number Mole and particles connection

1-5 questions 6-18

2 Molar mass of elements and compounds Mole to molar mass connection

19-25 26-36

3 Mole to molar volume at STP Mole to molar volume and mixed type conversions

Group work solving problems Quiz 1and 2 ( can be given together)

37-51

4 Percent composition of compounds Empirical formula

Group work 52-55 56-63

5 Empirical formula and Molecular formula

Quiz 3 64-74

6 Home work review Quiz 4- % composition, EF,MF Open ended questions ( from HW)

7 Quest - Chapter


Reactions PSI Chemistry

Essential questions

How do we describe a chemical reaction?

Why there is a need to balance a chemical reaction?

How many different reactions are there?

What are double replacement reactions?

What are spectator ions? What is a net ionic equation? Content

Writing word equations

Balancing chemical equation

Different types of reactions

Net ionic equation and spectator ions Skills

They will learn how to transform word equation to chemical equation. They will study how to balance a chemical reaction equation. They will discuss different types of reactions. They will learn to identify the insoluble precipitate and spectator ions in double replacement reactions. They will learn to predict the net ionic equation.

Activities

Balancing equations- class practice

Lab- single replacement reactions. ( Activity series)

Lab/Demo - Double replacement reactions

Paper lab- Identify the precipitate in double replacement reactions. Assessments

Quiz- Reactions and balancing reactions

Quiz-Types of reactions

Test- reactions


Pacing Guide

Day Topic Class work HW

1 Word to Skeleton equation

From the practice HW pack

Rest of the questions in the pack on skeleton equation

2 Balancing equations HW help

Smart response questions

MC HW-1-12 4 each from the practice HW pack

3 Types of reactions 5 types

Formation and Decomposition reactions- in detail

13- 25 Selected ones from the practice pack

4 Quiz skeleton equation and types of reactions Single replacement reaction Activity series HW help

Smart response and Questions from practice pack

31-32 Writing and balancing SR from the pack 33-43

5 Combustion reaction

Class practice Practice pack- questions 49-53

6 Double replacement reaction

Smart response

54-62 Practice pack - problems

7 Quiz- combustion, replacement reactions Net ionic equation

Class practice from the HW pack.

Practice pack

8 Review and HW help

9 Test Review

10 Chapter test


Stoichiometry PSI Chemistry

Essential questions

How do we interpret a chemical equation?

What is stoichiometry?

What is a limiting reagent?

How do we calculate the yield in a reaction? Content

Interpreting a balanced equation

Apply law of conservation of mass in chemical equation

Solve mole-mole, mole- mass, mole-volume stoichiometric problems based on balanced equation

Identify limiting and excess reagents in a reaction

Calculate the theoretical yield and percent yield of a reaction Skills

They will learn to interpret a balanced equation and to apply law of conservation of mass in terms of moles, atoms and mass. They will solve problems to calculate the moles, mass and volume of product produced or reactants needed using stoichiometric relationship in a chemical equation. They will learn to identify the limiting and excess reagent in reaction. They will learn to calculate the theoretical yield and percent yield of a reaction.

Activities

Problem solving related to moles, mass and volume.

Lab-Limiting reagent Assessments

Quiz- Stoichiometric calculation mixed type

Chapter Test- stoichiometry


Pacing guide

Day Topics Class work HW

1 Interpreting chemical equations Conservation of mass, atoms in a chemical reaction

Senteo questions and explain how to interpret the reaction of N2+3H2 2NH3

1-11

2 Mole –mole relationship in chemical reactions Proportion method and setting up the ratio using the given/wanted and the values in the reaction equation

Senteo questions. 12-15 group work

16-26

3 HW help Mass –mole proportion method for problem solving

Guiding to set the proportion based on the reaction equation. Senteo 27-29

30-38

4 Quiz mole- mole HW help on mass-mole

38-42

5 Mass –liter Mass – mass relationships and problem solving

43-47 48-52

6 Quiz mass-mass-liter Limiting and excess reagent Determining limiting reagent

Smart response questions 60-63 Class work- from practice set

53-59

7 Limiting reagent- and maximum amount of the product

Selective problems with mole-mole, grams – gram And mole-grams ratio set up 64, 72, 74

65-71, 73, 75, 77-79

8 Yield of a reaction- Theoretical yield of product and excess reagent left over

Smart response 80-82, 76

83-90 5, 6 from practice set( limiting regt)

9 Practice set -problems to review and class work

Class work Set 5-10 Set 7-10 from % yield

10 Chapter test


Intermolecular forces PSI Chemistry

Essential questions

Why water has a high boiling point?

Why ice floats on water?

Why hydrocarbons are not soluble in water?

Why dry ice sublimes at room temperature without melting? Content

Different types of IMF

Dipole-dipole, London dispersion, Hydrogen bonding, Ion- dipole interaction

Structure, polarity and volatility of compounds

Phase changes and diagrams Skills

The students will learn about different types of intermolecular forces. They will study the dependence of structure, polarity and volatility of compounds. They will learn about the phase changes and phase diagrams of compounds.

Assessments

Quiz on IMF

Quiz on vapor pressure and phase diagram

Quiz on free response questions Activities

Problem solving in class

IMF of different liquids- Volatility and polarity evaluation


Pacing guide

1 Introduction to IMF Polarity and dipole moment. London dispersion forces

In class practice: 1-5

1-2 18-20

2 Hydrogen bonding , ion- dipole interaction

15-18 3-15 21-27

3 Phase changes And phase pressure

28-30 35-37

31-34 38-44

4 Phase diagrams 45-46 47-52

5 Liquids and solids Chapter review

6 Test


Thermochemistry PSI Chemistry

Essential questions

What are system and surroundings?

How do we measure the heat absorbed or released in a reaction? Content

Internal energy of a system and surroundings

Enthalpy of a reaction

Heating and cooling curve

Calorimetric determination of heat exchange in a process

Hesse’s law of heat summation

Enthalpy of a reaction Skills

They will learn heat work done by a system and surroundings. They will study the heating and cooling pattern and enthalpy of a reaction. They study Hesse’s law of heat summation and apply this concept to determine the enthalpy of a reaction. They will learn to calculate the enthalpy of reaction from the enthalpy of formation.

Assessments

Quest – Heat and first law of thermodynamics

Quiz – heating curve and Calorimetry

Quiz- Enthalpy and Hess’s law

Chapter test Activities

Problem solving in class – Heating and cooling curve/calorimetry

Demo- Exothermic and endothermic reactions

Hesse’s law Lab

Calorimetry- determination of specific heat


Pacing guide

Day Topic Class work Homework

1 Introduction to internal energy System and surroundings Exo and endothermic reactions Senteo questions from the notebook

Senteo questions from the notebook

1-10

2 Enthalpy, q=msDt 20-25 11-20, 26-28

3 Calorimetry, heating curves Quest

Analyzing the heating curve segments- practice problem in the notebook

29-36

4 Enthalpy of reactions- stoichiometric aspect

40-45

37-39 45-55

5 Quiz- heating curves and calorimetry Hess’s law-lesson

Senteo problems and 58-60

56-57 61-64

6 Hess’s law HW help Heat of formation of reactions

Senteo problems and 65-67

68-78

7 Quiz – Hess’s law Help on Heat of formation

79-84

8 Chapter test

Thermodynamics –Second law PSI Chemistry


Essential questions

What is entropy?

How Gibbs free energy and entropy related?

When will be a process become spontaneous? Content

Entropy and randomness

Entropy in change in reactions

Calculating entropy change in reactions

Gibbs free energy

Free energy, temperature and spontaneity Skills

They will learn entropy changes in reactions. They will study what is Gibbs free energy and the relationship of it to entropy and temperature. They will apply Dg= Dh –TDs to solve for entropy or Free energy. They will learn to identify when a reaction will become spontaneous.

Assessments

Entropy and free energy –Quiz

Thermodynamics test

Activities

Demo- spontaneous reactions



Pacing Guide


1 Entropy and 2nd law

Senteo problems 1-15

2 Change in entropy Senteo questions, 16-20

21-34

3 Help with Dh HW Gibbs free energy

38, 39 35-38, 39-42

4 Quiz –entropy and Gibbs free energy Dg and Temperature

46-50 43-46 47-54

5 HW help Calculation of Temperature at which DG becomes spontaneous

Class practice and Review

6 Chapter test


Solutions and Properties of matter PSI Chemistry

Essential Questions

What is an electrolyte?

How do we distinguish chemical and physical changes?

How do we express the concentration of a solution and how can we make a solution?

What are colligative properties and how do they affect the solution properties?

Content

Physical and chemical changes

Solute, solvent interactions.

Concentration units of solutions

Colligative properties Skills

The students will learn physical and chemical changes. Student will learn the solvation process and the factors affecting the solubility of solutes in solvents. They will learn the different ways of expressing the concentration of solutions and preparing them. They will study the properties of solutions that are affected by the solute particles in the solution such as, elevation in boiling point, freezing point depression, etc. They will learn following terms such as, molality, mole fraction, molarity, lowering of vapor pressure, electrolyte, saturated and super-saturated.

Assessments

Quiz on solvation, solubility – section ABC

Quiz on polar/nonpolar interaction of solutes and solvents

Quiz on solution concentrations

Quest on colligative properties Activities

Problem solving in groups

Demo experiment on electrolytes

Preparing solutions

Freezing point depression – investigation


Pacing guide

Day Topic Classwork Home work

1 Introduction to mixtures and solutions

1-6 7- 18

2 Electrolytes and solubility 22-26 19-21, 27-28

3 Temperature and solubility, Polar nonpolar interaction of solute and solvent- quiz

29-32 Quiz on AB

33-39

4 Concentration units. Mole fraction and mass %

Practice problems in the handout

40-47

5 Molarity and molality 51-54 Quiz on C

48-50 55-68

6 Colligative properties- Dissociation of solutes- particles Lowering of vapor pressure Elevation in boiling point,

70-71 72-77

7 Depression in freezing point and osmosis

73-76 Quiz on DEF section

FR rev

8 Free response rev Practice in class

9 Lab demo, making solution, depression in freezing point.

10 Test


Acids and Bases PSI chemistry

Essential questions

What is an acid?

What are conjugate acid and base?

What is pH? Content

Various definitions of acid and base

Conjugate acid and base

Measurement of pH Skills

The students will learn various aspects of acid base reactions. They will learn to calculate the acid /base strength in terms of pH.

Assessments

Acids and bases quiz

Acid bases quest Activities

Problem solving

Demo- pH measurement of various acids and bases Pacing guide


1 Introduction to acid and bases Conjugate acid and base

5-10, senteo questions

1-5, 11-24

2 Auto-ionization of water Help on HW

Problem solving pH calculation

27-38

3 Ph problem help Quiz-acid and bases

39-47

4 review

5 Quest

.

Kinetics and Equilibrium


PSI Chemistry Essential questions

How do we measure the speed of a reaction?

What factors will affect the rate of a reaction?

What is meant by dynamic equilibrium?

How does equilibrium compromise to changes in conditions? Content

The rate /speed of a reaction.

Understanding the dynamic equilibrium

Potential energy diagram

Equilibrium constant expression

Le Chateleir’s Principle

Effect of concentration, pressure, and temperature at equilibrium

Effect of catalyst Skills

They will learn about the factors that affect the speed of a reaction. The students will study the energy requirements in a chemical reaction. They will understand the nature of potential energy diagram of a reaction and the effect of catalyst on the activation energy. They will understand the relationship between speed and concentration of a reaction. They will study to analyze the rate law expression and to interpret the order of a reaction. They will learn about dynamic equilibrium. They will study on different factors that could change the rate of a reaction. They will understand the chemical equilibrium constant expression. They will learn about Le Chatelier’s principle. They will study the effect of change in concentration, volume, pressure and temperature at equilibrium.

Assessments

Quiz- Rate and potential energy diagram

Quiz- Kinetics and rate law

Quest- Kinetics and equilibrium Activities


Smart response

Demo

Simple Bunsen burner flame with different setting of airhole.

Hydrogen peroxide /Manganese dioxide reaction

Temperature effect on equilibrium-Cobalt chloride /HCl reaction Pacing guide


Day topic Class work HW

1 Rate of reaction and rate law

Senteo questions demo

1-10

2 Potential energy diagram and catalyst action on activation energy.

Smart response 11-16

3 Quiz Equilibrium expression

18, 19 smart response

17, 20-26

4 Le Chatelier’s Effect of concentration and volume-pressure

Smart response 27-32

5 Effect of Temperature

Smart response Hw help

33-36

6 Review of chapter

7 Chapter quest


Organic chemistry PSI Chemistry

Essential questions

What is organic chemistry?

What are macromolecules?

What are hydrocarbons?

What are functional groups? Content

Introduction to carbon containing compounds.

Classification of hydrocarbons

Functional groups and compounds

Macromolecules in related to life Skills

They will learn why study of carbon compounds is a major branch of chemistry. They study the classification of carbon compounds based on hydrocarbons, functional groups. They study the important macromolecules related to life and their importance.

Assessments

Quiz Activities:

They will use molecular models to create different structure and isomers of hydrocarbons and other molecules.

Pacing guide

Day topic Class work HW

1 Introduction to organic chemistry- hydrocarbons

1-16

2 Functional groups. Smart response 17-25

3 macromolecules 26-46

4 rev Quiz

Documents

NEWARK PUBLIC SCHOOLS PUBLIC SCHOOLS SCHOOL ADVISORY BOARD MEMBERS 2013-2014 Ms. Antoinette Baskerville-Richardson, Chairperson Mr. Marques-Aquil Lewis, Vice Chairperson Mr. Rashon