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NGSS Chemistry Curriculum Map
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NGSS Chemistry Pacing Guide
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Unit 1: Structure and Properties of Matter
( FREE Sample Unit )
Unit 2: Chemical Reactions
- 2-1 Atomic Combinations
- 2-2 Covalent Bonding
- 2-3 Ionic Bonding
- 2-4 Metallic Bonding
- 2-5 Writing Chemical Formula
- 2-6 Molecular Shape and the VSEPR Theory
Unit 3: Changes in Matter
- 3-1 Physical and Chemical Change
- 3-2 Conservation of Energy in Chemical Reactions
- 3-3 Conservation of Mass in Chemical Reactions
- 3-4 Law of Constant Composition
- 3-5 Chemical Change Representation
- 3-6 Balancing Chemical Equations
Unit 4: The Mole Concept
- 4-1 The Mole and Molar Mass
- 4-2 Mole Concept for Elements
- 4-3 Mole Concept for Molecules and Compounds
- 4-4 Molecular and Empirical Formula
- 4-5 Stiochiometry
Unit 5: Energy Changes in Chemical Reactions
- 5-1 Bond Energy and the Types of Reactions
- 5-2 Heat of Reaction
- 5-3 Spontaneous and Non-Spontaneous Reactions
Unit 6: Reaction Rate
- 6-1 Reaction Rate and Factors Affecting it.
- 6-2 Reaction Rate and Collision Theory
- 6-3 Measuring Reaction Rates
- 6-4 Catalysts and Reaction Rates
- 6-5 Chemical Equilibrium
Unit 7: Nuclear Processes
- 7-1 Nuclear Structure and Radiation
- 7-2 Types of Radiation
- 7-3 Half-Life
- 7-4 Sources of Radiation
- 7-5 Dangers and Uses of Radiation
- 7-6 Nuclear Fission
- 7-7 Nuclear Fusion
- 7-8 Nucleosynthesis
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NGSS High School Physical Sciences Standards:
1-1 Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.
1-2 Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.
1-3 Plan and conduct an investigation to gather evidence to compare the structure of substances at the bulk scale to infer the strength of electrical forces between particles.
1-4 Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.
1-5 Apply scientific principles and evidence to provide an explanation about the effects of changing the temperature or concentration of the reacting particles on the rate at which a reaction occurs.
1-6 Refine the design of a chemical system by specifying a change in conditions that would produce increased amounts of products at equilibrium.
1-7 Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction.
1-8 Develop models to illustrate the changes in the composition of the nucleus of the atom and the energy released during the processes of fission, fusion, and radioactive decay.
Next Generation Science Standards Chemistry Curriculum Map
| Unit | Lesson Outline | HS-PS |
| Unit 1:
Structure and Properties of Matter
|
1-1 Atoms and Molecules
1-2 The Kinetic Molecular Theory and Properties of Matter 1-3 Models of an Atom 1-4 Atomic Structure 1-5 Isotopes 1-6 Electron Configuration 1-7 The Periodic Table of Elements
|
1-1
1-2 1-3 |
| Unit 2:
Chemical Reactions
|
2-1 Atomic Combinations
2-2 Covalent Bonding 2-3 Ionic Bonding 2-4 Metallic Bonding 2-5 Writing Chemical Formula 2-6 Molecular Shape and the VSEPR Theory
|
1-1
1-2 1-4 |
| Unit 3:
Changes in Matter
|
3-1 Physical and Chemical Change
3-2 Conservation of Energy in Chemical Reactions 3-3 Conservation of Mass in Chemical Reactions 3-4 Law of Constant Composition 3-5 Chemical Change Representation 3-6 Balancing Chemical Equations
|
1-4 1-5 1-7
|
| Unit 4:
The Mole Concept
|
4-1 The Mole and Molar Mass
4-2 Mole Concept for Elements 4-3 Mole Concept for Molecules and Compounds 4-4 Molecular and Empirical Formula 4-5 Stiochiometry
|
1-7
|
| Unit 5:
Energy Changes in Chemical Reactions
|
5-1 Bond Energy and the Types of Reactions
5-2 Heat of Reaction 5-3 Spontaneous and Non-Spontaneous Reactions
|
1-4 1-5 1-6
|
| Unit 6:
Reaction Rate
|
6-1 Reaction Rate and Factors Affecting it.
6-2 Reaction Rate and Collision Theory 6-3 Measuring Reaction Rates 6-4 Catalysts and Reaction Rates 6-5 Chemical Equilibrium
|
1-4
1-5 1-6
|
| Unit 7:
Nuclear Processes
|
7-1 Nuclear Structure and Radiation
7-2 Types of Radiation 7-3 Half-Life 7-4 Sources of Radiation 7-5 Dangers and Uses of Radiation 7-6 Nuclear Fission 7-7 Nuclear Fusion 7-8 Nucleosynthesis
|
1-8 |
NGSS Chemistry Pacing Guide
| Unit : 1 | Structure and Properties of Matter | Number of Instructional Days | |
| Common Core Standards Covered | Key Concepts | Total: 32 | |
| 1-1 | Atoms and Molecules
HS-PS1-1. |
· Atoms are the simplest building block of matter.
· Atoms bond together to form groups known as a molecule. · Molecules which contain different types of atoms are called compounds. |
2 |
| 1-2 | The Kinetic Molecular Theory and the Properties of Matter
HS-PS1-3. |
· Arrangement of particles in solids, liquids and gases
· Properties relating to each state · States of matter are reliant on the forces between particles · Define the temperature of a substance as a measure of the average kinetic energy of the particles. · Kinetic energy of each state of matter · Changes of state require energy to be added or removed. |
4 |
| 1-3 | Models of an Atom
HS-PS1-1. |
Outline the findings of:
· Solid Sphere - Dalton · Plum Pudding Model - Thomson · Nuclear Model – Rutherford · Planetary Model – Bohr · Quantum Model –Schrodinger Compare and contrast the models and identify key contributions to modern day atomic theory |
5 |
| 1-4 | Atomic Structure
HS-PS1-1. |
· Atoms are made of a nucleus consisting of protons and neutrons. The nucleus is surrounded by electrons.
· Protons and electrons are oppositely charged. · An atom has the same number of protons and electrons to making its overall charge zero (neutral). · Formation of Ions · Flame testing and identification of positive and negative ions |
6 |
| 1-5 | Isotopes
HS-PS1-1. |
· Isotopes are different forms of the same element.
· Change in mass number while the number of protons and electrons (atomic number) remains the same. · Examples: Hydrogen, Carbon and Chlorine |
4 |
| 1-6 | Electron Configuration
HS-PS1-1. HS-PS1-2. |
· Arrangement of electrons in orbitals
· First energy level is filled first - 1s orbital, · Second level, 2s and 2p orbital · Atoms are most stable when they have a full shell (reference to noble gases) · |
4 |
| 1-7 | The Periodic Table of Elements
HS-PS1-1. HS-PS1-2. |
· As proposed by Mendelev
· Elements are represented by symbols · Elements are sorted by atomic number starting with hydrogen. · Groups run vertically and show trends in properties (specific reference to Group I metals, Group II Alkali Earth Metals, Group 17 Halogens and Group 18 Noble Gases) · Transition metals · Rows determine the number of orbitals present · The ‘staircase’ separates metals and non-metals
|
7 |
| Unit : 2 | Chemical Reactions | Number of Instructional Days | |
| Common Core Standards Covered | Key Concepts | Total: 24 | |
| 2-1 | Atomic Combinations
HS-PS1-1. HS-PS1-2. HS-PS1-4 |
· Atoms join together to form compounds
· Different elements react, breaking and forming bonds · Forming bonds requires atoms giving, taking or sharing electrons · The properties of the compound are often very different to the individual atoms in the compound. |
2 |
| 2-2 | Covalent Bonding
HS-PS1-1. HS-PS1-2. |
· Occurs between non-metals
· Atoms share electrons in order to fill both outer (valence) shells · Properties of covalent molecules · Important examples: H2O, HCl, NH3, O2, CO2 · Giant covalent structures e.g. Graphite, Diamond |
4 |
| 2-3 | Ionic Bonding
HS-PS1-1. HS-PS1-2. |
· Forms from a metal (positive ion) losing it electron(s) and a non-metal (negative ion) gaining electron(s)
· Occurs to fill (or empty) the atoms valence shell · Properties of Ionic compounds · Ionic compounds occur as giant molecular lattices · Compounds have strong electrostatic forces holding them together · Important examples: NaCl, NaOH |
6 |
| 2-4 | Metallic Bonding
HS-PS1-1. HS-PS1-2.
|
· Involves free electrons which produce the properties of unique to metals
· Outline the properties of metals · Electrons free to move through the structure to allow conduction of electricity, malleability etc · Electrons hold the metal together in a fixed shape through strong electrostatic forces. · Alloys are mixtures which make the new metal harder than the original elements. · Examples of alloys used in industry |
6 |
| 2-5 | Writing Chemical Formula
HS-PS1-1. HS-PS1-2.
|
· Shows the type and number of atoms in a substance
· Use of subscript numbers · Cancellation of charges (ionic formula) · Use of brackets · Correct naming conventions e.g. –ate, -ide, etc. |
4 |
| 2-6 | Molecular Shape and VESPR Theory
HS-PS1-1. HS-PS1-2. HS-PS1-4 |
· Electron pairs in bonds and lone pairs repel thus adopting the specific geometric shapes so that electron pairs are as far apart as possible.
· Linear (180o) E.g. CO2 · Bent (119.3o) E.g. SO2 · Trigonal pyramidal (106.7o) E.g. NH3 · Trigonal Planar (120o) E.g. BCl3 · T-shaped (86.2o) E.g. BrF3 |
2 |
| Unit : 3 | Changes in Matter | Number of Instructional Days | |
| Common Core Standards Covered | Key Concepts | Total: 22 | |
| 3-1 | Physical and Chemical Change
HS-PS1-4 HS-PS1-5
|
· Chemical change – permanent, involving new substances being made, indicated by color change, smell
· Physical Change – requires adding or removing heat to cause a change in state. · Physical changes are reversible · Identify chemical and physical change from experiments · Examples of chemical and physical Change |
4 |
| 3-2 | Conservation of Energy in Chemical Reactions
HS-PS1-4 HS-PS1-5 HS-PS1-7
|
· Chemical reactions involve energy which is used to break bonds in reactants.
· Energy is released when new bonds form in products. · Endothermic reactions absorb energy · Exothermic reactions release energy. · The law of conservation of energy – matter cannot be created or destroyed |
2 |
| 3-3 | Conservation of Mass in Chemical Reactions
HS-PS1-6. HS-PS1-7. |
· Mass is always conserved in a chemical reaction, due to no atoms being created or destroyed
· Same number and types of atoms will be present in the reactants as well as the products · Adding up relative formula masses on both sides of the equation to observe the conservation of mass. · Calculating mass in reactions · Using simplest ratios |
4 |
| 3-4 | Law of Constant Composition
HS-PS1-5 HS-PS1-7.
|
· Also known as Proust's law or the law of definite composition
· A given chemical compound always contains its component elements in fixed ratio (by mass) and does not depend on its source and method of preparation. |
2 |
| 3-5 | Chemical Change Representation
HS-PS1-7.
|
6 types of chemic al reactions
· Synthesis · Combustion · Decomposition · Single displacement · Double displacement · Acid-base |
6 |
| 3-6 | Balancing Chemical Equations
HS-PS1-7
|
· Placing numbers in from of the compounds (stiochiometric coefficients)
· Balancing one type of atom at a time · Reactants equal products |
4 |
| Unit : 4 | The Mole Concept | Number of Instructional Days | |
| Common Core Standards Covered | Key Concepts | Total: 18 | |
| 4-1 | The Mole and Molar Mass
HS-PS1-7
|
· Defining the mole as: One mole of a substance equals its Mr in grams
· Defining Avogadro number · One mole of gas occupies a volume of 24dm3 · Finding Relative atomic mass (Ar) · Calculating Relative formula mass (Mr · Number of moles = mass of substance (grams)/Mr
|
4 |
| 4-2 | Mole Concept for Elements
HS-PS1-7
|
· Number of moles = mass of element (grams)/Mr
· Calculating percentage mass of elements in compounds |
4 |
| 4-3 | Mole Concept for Molecules and Compounds
HS-PS1-7. |
· Number of moles = mass of compound (grams)/Mr
|
2 |
| 4-4 | Molecular and Empirical Formula
HS-PS1-7.
|
· Calculating empirical formulas from masses or percentages
|
2 |
| 4-5 | Stoichiometry
HS-PS1-7.
|
· Using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data
· Mass spectrometry and Relative isotopic abundance · Formula mass calculations · Percentage yield calculations |
6 |
| Unit : 5 | Energy Changes in Chemical Reactions | Number of Instructional Days | |
| Common Core Standards Covered | Key Concepts | Total: 14 | |
| 5-1 | Bond Energy and the Types of Reactions
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
· Calculating bond energy
· Calculating overall energy change of a reaction · -/+DH linked to energy released or absorbed · Endothermic vs. exothermic reactions
|
6 |
| 5-2 | Heat of Reaction
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
· Enthalpy of a reaction
· Enthalpy = internal energy + pressure x volume · Effect of temperature and pressure on enthalpy · Energy level diagrams – interpretation and drawing
|
4 |
| 5-3 | Spontaneous and Non-Spontaneous Reactions
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
· Entropy
· Spontaneous reactions (exothermic reactions) are favored when they result in a decrease in enthalpy and an increase in entropy of the system. Energy is released to the surroundings as heat. · Non-spontaneous reactions (endothermic reactions), decreases the entropy.
|
4 |
| Unit : 6 | Reaction Rate | Number of Instructional Days | |
| Common Core Standards Covered | Key Concepts | Total: 30 | |
| 6-1 | Reaction Rate and Factors Affecting It
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
Reaction rate is affected by changes in:
· Temperature · Catalysts · Concentration or pressure · Surface area
|
8 |
| 6-2 | Reaction Rate and the Collision Theory
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
· Particles are in constant motion
· Reactions occur when particles collide with sufficient force and in the correct orientation. |
2 |
| 6-3 | Measuring Reaction Rates
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
Reaction rate = amount of reaction used or product formed/ time
Observations of: · Precipitation · Change in mass · Volume of gas given off |
8 |
| 6-4 | Catalysts and Reaction Rates
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
· Does not participate in reaction
· Specific · Reduces energy requirement · Increases number of successful collisions |
2 |
| 6-5 | Chemical Equilibrium
HS-PS1-4 HS-PS1-5 HS-PS1-6
|
· The rate of a reversible reaction in a closed system
· Occurs when the forward and backward reactions occur at the same rate. · As reactants react concentration of these falls so forward reaction slows down. · Equilibrium position right vs. left based on the amounts of reactants and products · Factors which change equilibrium – temperature, pressure, concentration · The Haber process as an example of equilibrium · Using equilibrium tables and graphs
|
10 |
| Unit : 7 | Nuclear Processes | Number of Instructional Days | |
| Common Core Standards Covered | Key Concepts | Total: 22 | |
| 7-1 | Nuclear Structure and Radiation
HS-PS1-8
|
· Unstable nuclei release particles
· Ionisation
|
1 |
| 7-2 | Types of Radiation
HS-PS1-8
|
Compare and contrast types of radiation
· Alpha (helium nuclei) · Beta (electrons) · Gamma (short wavelength EM waves) · Balancing nuclear equations · Materials which block radiation · Effects of magnetic fields on radiation |
6 |
| 7-3 | Half-Life
HS-PS1-8
|
· Defined as the average time taken to halve the number of radioactive nuclei in an isotope
· Short vs. long half-life · Calculating number of half lives in a sample · Finding half-life using a graph
|
5 |
| 7-4 | Sources of Radiation
HS-PS1-8
|
· Unstable Isotopes
· Space · Human activity (nuclear fallout) · Background radiation |
2 |
| 7-5 | Dangers and Uses of Radiation
HS-PS1-8
|
Dangers:
· Harms living tissue Uses: · Smoke detectors · Medical tracers · Sterilisation · X-Rays · Radioactive dating · Radiotherapy/cancer treatment · Power stations |
2 |
| 7-6 | Nuclear Fission
HS-PS1-8
|
· Splitting/subdivision of nuclei into two nuclei of roughly even mass.
· Occurs in nuclear reactors |
2 |
| 7-7 | Nuclear Fusion
HS-PS1-8
|
· Joining of two or more nuclei together
· Requirements of a fusion reaction · Occurs in stars · Comparison with fission reaction |
2 |
| 7-8 | Nucleosynthesis
HS-PS1-8
|
· New nuclei formed from pre-existing nuclei
· Big Bang theory
|
2 |
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