Course: Chemistry , The Physical Setting

Grade Level: 11

Hadley-Luzerne Central School

Main/General Topic:	Sub-topic:	essential questions:	what the students will Know	skills:	When Student Does it:	assessments:
The Science of Chemistry Key Ideas - 1,2,3.1,3.2,3.4,5 Standards – 1,6,4,7 Introductory, Mastery, & review lessons	- Substances, materials, and chemicals - Physical states of matter - “models”	· What is chemistry & how does it affect our lives? · What is the difference between a physical & chemical change? · What are the different characteristics of matter? · What are the physical and chemical properties of matter? · How is matter classified?	· How chemistry is part of their daily lives · The 3 states of matter and be able to describe them using “particle” models · What is evidence of a chemical change or physical occurring? Lab #3 “Physical & Chemical Changes” · The SI base units for measurement · Mathematics of Chemistry · Relationships between different classes of matter/ how matter is classified	1. Convert within the metric system using factor-labeling method (dimensional analysis) 2. Find density using the slope method – Lab #2 3. Use significant digits in calculations 4. Recognize measurement scales 5. Create graphs (direct & inverse) 6. Identify independent & dependent variables 7. Use scientific notation in calculations	Sept.	-quizzes -Text:p.9 #1-9 SR -p.9 #11-14 CT -Problems -Test #1 – “Math of Chemistry” -p.19 #1-11 SR -p.28 #1-8 SR -p.28 #9-14 CT -p.31-35 #1-41 -Test #2 – unit test
Matter and Energy Key Ideas: 3.1, 4.2, 5. Standards: 1,2,4,6,7 Introductory, Mastery, and Review lessons	-Energy and Change -Endothermic and Exothermic Processes	1. How does the Law of Conservation of Energy explain chemical and physical reactions? 2. How can energy be transferred in different form? 3. How is heat different from temperature? 4. What is the scientific method?	· The energy changes involved in boiling, condensation, freezing, evaporation, sublimation. · The differences between accuracy and precision in measurements · How one form of energy can be converted into another · Potential energy vs kinetic energy on the heating curve	- Be able to sketch a heating & cooling curve for water - Be able to calculate the heat needed to raise the temperature of water and to change phases. -Be able to calculate the heat of fusion of water – Lab # 4	October Weeks – 1 & 2	- Problem WS on Calculating heat in joules -Quizzes -p.45 #1-13 SR -p.53 # 1-13 SR -p.66-68 #1-27 -p.69 #28-35 -p.71 #39-42 -Unit Test: Matter and Energy
Atomic Theory Structure & Models Key Ideas: 3.1, 3.2, 3.4, 4.1, 4.2 Standards: 1,2,4,6,7 Introductory, Mastery, and Review lessons	- Dalton’s Atomic Theory - Law of Conservation of Mass - Law of Multiple Proportions - Sub-Atomic Particles - Valence electons - Avg.Isotopes - Mole Concept	1. What are the three laws that support the existence of atoms? 2. What are the principles of Dalton’s Atomic Theory? 3. What are the characteristics, location, and arrangement of electrons, protons, & neutrons? 4. What is the significance of Avogadro’s number? 5. How is the mole used to count particles?	· How Dalton’s Theory explains the Laws of Def. Composition, Conservation of Mass, & Multiple Proportions. · Be able to compare the Rutherford, Bohr, and Quantum models of the atom · Explain the relationship of the electron and the electromagnetic spectrum · The relationship between what they can see (beaker of chemicals) & what they cannot see (atoms that make up those chemicals)	- Sketch & explain Rutherford’s Gold Foil Experiment -Calculate the average mass of a given no. of isotopes of an atom -Use symbols to represent an atom’s structure - Find % of salt in a salt/sand mixture. Lab #5 - Be able to convert between mass, amount in moles, and number of particles using Avogadro’s number and molar mass.	October weeks 3,4 Nov. 1-7	- p.78 # 1-8 SR -p.89 #1-8 SR - Lab #5 “Flame Tests” & post-lab questions - Quizzes -Problem WS on moles -p.104 #1-13 -p.107-110 #1-45 Omit # 13,14,37,39,41-44 -Lab: “Finding Gram-Atomic Mass of Silver”
The Periodic Table Core Topics: 1.11,11.1,11.4,11.5,11.7. 11.8,11.9 Major Understandings 3.1l,3.1w,3.1x,3.1y,3.1z,3.1aa,3.1b Introductory & Mastery lessons	- Periodic Law - Trends in the table - Origin of elements	· How are the elements organized? · What elements make up the main groups? · What is ionization energy? · What is atomic and ionic radius? · How can electronegativity differences be used to predict the properties of a bond?	1. The organization of the modern periodic table according to periodic law. 2. To be able to locate the different families of the main-group elements of the periodic table, describe their characteristic properties, and relate them to their electron configurations. 3.Describe periodic trends in ionization energy, atomic radius, and electronegativity, and relate them to atomic structure. 4. Describe trends in ionic size, melting & boiling pts and relate them to atomic structure.	1. Students will be able to put together a hypothetical periodic table given the elements properties of density, atomic mass, reactivity with oxygen & formulas of oxides produced, and color of compounds.	Nov. 8 – Thanks-giving.	v Periodic Table Packet v Lab – making a periodic table. v Quizzes v Test – Holt Text: p.131 #1-13 p.141 #3,5-8,10-13,15 p.150-155 #1-55 (regents format) Lab – Calculating the % of Salt in a Sand/Salt mixture. Research project – ways of separating chemical mixtures: filtration, distillation, chromatography, density, polarity, melt. & boiling pts.

Main/General Topic:

Sub-topic:

essential questions:

what the students will Know

skills:

When Student Does it:

assessments:

The Science of Chemistry

Key Ideas - 1,2,3.1,3.2,3.4,5

Standards – 1,6,4,7

Introductory, Mastery, & review lessons

- Substances, materials, and chemicals

- Physical states of matter

- “models”

· What is chemistry & how does it affect our lives?

· What is the difference between a physical & chemical change?

· What are the different characteristics of matter?

· What are the physical and chemical properties of matter?

· How is matter classified?

· How chemistry is part of their daily lives

· The 3 states of matter and be able to describe them using “particle” models

· What is evidence of a chemical change or physical occurring? Lab #3 “Physical & Chemical Changes”

· The SI base units for measurement

· Mathematics of Chemistry

· Relationships between different classes of matter/ how matter is classified

1. Convert within the metric system using factor-labeling method (dimensional analysis)

2. Find density using the slope method – Lab #2

3. Use significant digits in calculations

4. Recognize measurement scales

5. Create graphs (direct & inverse)

6. Identify independent & dependent variables

7. Use scientific notation in calculations

Sept.

-quizzes

-Text:p.9 #1-9 SR

-p.9 #11-14 CT

-Problems

-Test #1 – “Math of Chemistry”

-p.19 #1-11 SR

-p.28 #1-8 SR

-p.28 #9-14 CT

-p.31-35 #1-41

-Test #2 – unit test

Matter and Energy

Key Ideas: 3.1, 4.2, 5.

Standards:

1,2,4,6,7

Introductory,

Mastery, and Review lessons

-Energy and Change

-Endothermic and Exothermic Processes

1. How does the Law of Conservation of Energy explain chemical and physical reactions?

2. How can energy be transferred in different form?

3. How is heat different from temperature?

4. What is the scientific method?

· The energy changes involved in boiling, condensation, freezing, evaporation, sublimation.

· The differences between accuracy and precision in measurements

· How one form of energy can be converted into another

· Potential energy vs kinetic energy on the heating curve

- Be able to sketch a heating & cooling curve for water

- Be able to calculate the heat needed to raise the temperature of water and to change phases.

-Be able to calculate the heat of fusion of water – Lab # 4

October

Weeks –

1 & 2

- Problem WS on

Calculating heat in joules

-Quizzes

-p.45 #1-13 SR

-p.53 # 1-13 SR

-p.66-68 #1-27

-p.69 #28-35

-p.71 #39-42

-Unit Test: Matter and Energy

Atomic Theory Structure & Models

Key Ideas: 3.1,

3.2, 3.4, 4.1, 4.2

Standards:

1,2,4,6,7

Introductory,

Mastery, and Review

lessons

- Dalton’s Atomic Theory

- Law of Conservation of Mass

- Law of Multiple Proportions

- Sub-Atomic Particles

- Valence electons

- Avg.Isotopes

- Mole Concept

1. What are the three laws that support the existence of atoms?

2. What are the principles of Dalton’s Atomic Theory?

3. What are the characteristics, location, and arrangement of electrons, protons, & neutrons?

4. What is the significance of Avogadro’s number?

5. How is the mole used to count particles?

· How Dalton’s Theory explains the Laws of Def. Composition, Conservation of Mass, & Multiple Proportions.

· Be able to compare the Rutherford, Bohr, and Quantum models of the atom

· Explain the relationship of the electron and the electromagnetic spectrum

· The relationship between what they can see (beaker of chemicals) & what they cannot see (atoms that make up those chemicals)

- Sketch & explain

Rutherford’s Gold Foil Experiment

-Calculate the average mass of a given no. of isotopes of an atom

-Use symbols to represent an atom’s structure

- Find % of salt in a salt/sand mixture. Lab #5

- Be able to convert between mass, amount in moles, and number of particles using Avogadro’s number and molar mass.

October

weeks 3,4

Nov. 1-7

- p.78 # 1-8 SR

-p.89 #1-8 SR

- Lab #5 “Flame Tests” & post-lab questions

- Quizzes

-Problem WS on moles

-p.104 #1-13

-p.107-110 #1-45

Omit # 13,14,37,39,41-44

-Lab: “Finding Gram-Atomic Mass of Silver”

The Periodic Table

Core Topics: 1.11,11.1,11.4,11.5,11.7. 11.8,11.9

Major Understandings

3.1l,3.1w,3.1x,3.1y,3.1z,3.1aa,3.1b

Introductory & Mastery lessons

- Periodic Law

- Trends in the table

- Origin of elements

· How are the elements organized?

· What elements make up the main groups?

· What is ionization energy?

· What is atomic and ionic radius?

· How can electronegativity differences be used to predict the properties of a bond?

1. The organization of the modern periodic table according to periodic law.

2. To be able to locate the different families of the main-group elements of the periodic table, describe their characteristic properties, and relate them to their electron configurations.

3.Describe periodic trends in ionization energy, atomic radius, and electronegativity, and relate them to atomic structure.

4. Describe trends in ionic size, melting & boiling pts and relate them to atomic structure.

1. Students will be able to put together a hypothetical periodic table given the elements properties of density, atomic mass, reactivity with oxygen & formulas of oxides produced, and color of compounds.

Nov. 8 – Thanks-giving.

v Periodic Table Packet

v Lab – making a periodic table.

v Quizzes

v Test –

Holt Text:

p.131 #1-13

p.141 #3,5-8,10-13,15

p.150-155 #1-55

(regents format)

Lab – Calculating the % of Salt in a Sand/Salt mixture.

Research

project – ways of separating chemical mixtures: filtration, distillation, chromatography, density, polarity, melt. & boiling pts.

Main/General Topic:

Sub-topic:

essential questions:

what the students will Know

skills:

When StudentDoes it:

assessments:

Ionic Compounds

Core Topics

I.11,III.1,IV.1-3,6-9,13,V.24

Major Understandings

3.1I,3.1cc,dd,5.2

Simple ions

Ionic bonding & salts

Names & Formulas of ionic compds.

· What is the difference between an atom and an ion?

· How do metals react with non-metals to form an ionic bond?

· What are the properties of ionic compounds?

· How are ionic formulas written and named w/ 2 or more oxidation states for the metal?

1.Metal lose electrons and become positive ions.

2. Non-metals gain electrons and become negative ions.

3. Valence electrons are involved in bonding.

4. Ionic substances are made of unit cells w/crystal lattice.

1.Be able to name and write chemical formulas for monatomic and polyatomic ions.

2. Be able to tell the difference between binary and ternary compounds.

3.Be able to calculate the electronegativity difference and identify an ionic bond.

End of Nov. – early Dec.

3 problem sheets on formula writing

Quiz-writing & naming ionic formulas

Holt:p.183-185

#1-28

Covalent Compounds & Bonding

Core Topics:

III.1,IV.2-5,7-13

Major Understanding:

3.1cc,5.2

-Covalent bonds

-Molecular orbitals

-Nonpolar covalent bonds

-Polar covalent bonds

v What is the difference between a single, double, & triple covalent bond?

v How do properties of substances depend on bond type?

1. Covalent bonds form when atoms share pairs of electrons.

2. Atoms have less P.E. and more stability after they form a bond.

3. Greater the electronegativity difference, the greater % ionic character.

4. Physical & chemical properties are related to compound’s bond type.

5. “Stuff” is matter and it is divided into metallic, ionic, & covalent compounds.

6. Covalent compounds involve non-metal bonding w/ another non-metal.

7. Element w/highest electroneg. Is written second.

1. Students will be able to draw Lewis-dot structures of polar & nonpolar compounds.

2. Students will be able to build models of molecular structures.

3. Students will be able to recognize the polarity of a molecule by its shape & structure.

4. Students will be able to predict the shape of covalent molecules.

5. Students will be able to write and name covalent compounds.

1^ST TWO WEEKS OF DEC.

Lab on “Building Molecular Models”

Problem sheet on naming and writing covalent compounds.

Holt:p.216-220

#1-42

2Quizzes

Test – will combine all types of bonding and formula writing.

Main/General Topic:

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essential questions:

what the students will Know

skills:

When StudentDoes it:

assessments:

Formulas and Percent Composition

Core Topics:

III.2,III.3,III.7

Major Understandings:

3.1ee,3.3d,3.3f

*Empirical Formulas

*Molecular Formulas

*Percent composition of elements in compounds

* Percent of Water of Hydration

· What is the relationship between empirical formula and molecular formula?

· What does % mean?

· What is water of hydration?

· How to calculate the % by mass of any element in a compound.

· How to calculate the empirical formula given the % of each element.

· How to calculate the molecular formula given the empirical formula and the molecular mass.

· How to determine the percent of water of hydration.

· Students will know how to perform the mathematical functions stated in “what they will know.”

Dec.

v Quiz

v Lab – “Determining % of Water of Hydration in CuSO₄·5H₂O”

v Holt:p.251-253 #1-39

v P.243 PP #1,2

v P.245 PP #1,2

v P.248 PP #1,3

v Find % water of hydration in BaCl₂·2H₂O

v Test

v December Review of all material to date.

Main/General Topic:

Sub-topic:

essential questions:

what the students will Know

skills:

When StudentDoes it:

assessments:

Chemical Equations and Reactions

Core Topics:

III.4,III.5,III.8,V.20

Major Understandings:

3.3a,3.3c,3.2b,3.2a

· 5 Types of Chemical Reactions

· What is evidence that a chemical reaction has occurred?

· What are the reactants and products?

· What is the energy change in various chemical reactions?

· What are the 5 types of chemical reactions?

1. Students will be able to relate the conservation of mass to the rearrangement of atoms in a chemical equation.

2. Students will be able to identify reactants and products.

3. Students will know how to classify and identify chemical reactions into synthesis, decomposition, single and double displacement, and combustion.

1. Students will be able to write and balance the 5 types of chemical equations.

2. Using Holt, p.284, students will be able to identify type of reactions and predict products in their lab.

3. In a net-ionic equation, students will be able to identify the precipitate & spectator ions.

Mid- Dec through

Christmas vacation

· Lab – “Types of Chemical Reactions”

· Equation worksheets.