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Chapter 4 Unit 2 Atomic Structure The students will learn what makes up atoms and how are atoms of one element different from atoms of another element. Explore the scientific theory of atoms (also known as atomic theory) by describing changes in the atomic model over time and why those changes were necessitated by experimental evidence. Students will be able to draw/identify each atomic model. Students will be able to compare/contrast the different atomic models. Students will be able to describe how results of experimental evidence caused the atomic model to change. proton electron neutron nucleus electron cloud Explore the scientific theory of atoms (also known as atomic theory) by describing the structure of atoms in terms of protons, neutrons and electrons, and differentiate among these particles in terms of their mass, electrical charges and locations within the atom. Students will compare/contrast the characteristics of subatomic particles. atomic number mass number isotope atomic mass unit (amu) atomic mass
Chapter 5 Electrons in Atoms The students will be able to describe the arrangement of electrons in atoms and predict what will happen when electrons in atoms absorb or release energy. Describe the quantization of energy at the atomic level. Students will participate in activities to view emission spectrums using a diffraction grating or a spectroscope. Students will be able to explain how the spectrum lines relate to electron motion. energy level atomic orbital quantum mechanical model Chapter 6 The Periodic Table The student will learn what information the periodic table provides and how periodic trends can be explained. Relate properties of atoms and their position in the periodic table to the arrangement of their electrons. Students will be able to compare and contrast metals, nonmetals, and metalloids. Students will be able to describe the traits of various families on the periodic table. Students will be able to explain periodicity. Students will write/represent electron configuration of various elements. Students will be able to use a periodic table to calculate the number of p + , e - , and n 0 . Students will be able to calculate the average weight of mass. periodic law halogen metals noble gas nonmetals transition metal metalloid atomic radius alkali metal ionization energy alkaline earth metal electronegativity
Page 1 and 2: Enmanuel’s Chemistry Notebook
Page 3 and 4: Unit 1 Measurement Lab Separation o
Page 5 and 6: Unit 5 (28 days) Chapter 10 Chemica
Page 7 and 8: 30. Always lubricate glassware (tub
Page 10 and 11: Chapter 1 Unit 1 Introduction to Ch
Page 12 and 13: Determine appropriate and consisten
Page 14 and 15: 2. One cereal bar has a mass of 37
Page 16 and 17: 1. How many meters are in one kilom
Page 18 and 19: The Learning Goal for this assignme
Page 20 and 21: RULE #3: To add/subtract in scienti
Page 24 and 25: Rule 3: A final zero or trailing ze
Page 26 and 27: For addition and subtraction, look
Page 28 and 29: Dimensional Analysis This is a way
Page 34 and 35: Looking at Ions We haven’t talked
Page 36 and 37: Neutron Madness We have already lea
Page 39 and 40: Electron Configuration Color the su
Page 41 and 42: Electron Configuration In order to
Page 44 and 45: Create groups for these Scientist a
Page 46 and 47: The Learning Goal for this Assignme
Page 48 and 49: Define Atomic Size: The size of the
Page 50 and 51: Electronegativity Define Electroneg
Page 52 and 53: Unit 3 Chapter 25 Nuclear Chemistry
Page 54 and 55: Enmanuel Garrido Name _____________
Page 56 and 57: Learning Goal for this section: Exp
Page 58 and 59: Beta Particle Decay Beta decay is a
Page 62 and 63: Ion Charge? What is the charge on f
Page 66 and 67: C 2 H 6 O Ethanol CH 3 CH 2 O Step
Page 68 and 69: Linear Molecular Geometry Orbital E
Page 70 and 71: Bent Molecular Geometry Orbital Equ
Page 72 and 73: Bent Molecular Geometry Orbital Equ
Page 74 and 75: Trigonal Bi Pyramidal Molecular Geo
Page 76 and 77: Octahedral Molecular Geometry Orbit
Page 78 and 79: Orbitals Equation Lone Pairs Angle
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Chapter 9 Unit 4 Chemical Names and
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http://www.bbc.co.uk/education/guid
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Chapter 12 Stoichiometry The studen
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www.youtube.com/watch?v=BTRm8PwcZ3U
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4) Double displacement: This is whe
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Determine the Type of Reaction for
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Step 3 Always leave hydrogen and ox
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1) ___ NaNO3 + ___ PbO ___ Pb(NO3)
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1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2
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we can determine that 2 moles of HC
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When there is no limiting reagent b
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Example 7 How much 5M stock solutio
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Theoretical and Actual Yields Key T
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Review Purposes To get an over
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Unit 6 Chapter 13 States of Matter
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The Learning Goal for this assignme
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Summary: In this chapter we learned
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P 1 : 1980 torr V 1 : 7730 ml P 2 :
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P 1 : 107 kPA T 1 : 41 C à 314 K P
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Ideal Gas Law: The gas law that inc
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7.Electrolyte: Is a compound that c
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Create and interpret potential ener
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Part 1: Mass Percent Mass percent (
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Glossary Concentration: Amount of d
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Specific Heat Here is the definitio
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Step One: solid ice rises in temper
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Step Three: liquid water rises in t
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Step Five: steam rises in temperatu
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then it is exothermic, meaning the
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Chemical Concepts: The chemical con
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A increasing the equilibrium consta
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Chemical Concepts: The chemical con
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Reduction Oxidation reduction react
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So far, the properties have an obvi
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The acid base theory of Brønsted a
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IV. Problems with the Theory This t
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Let's discuss significant figures a
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On your calculator you would input
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Ag+ + Cu ---> Ag + Cu2+ I have deli
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7. Half Reactions A half-reaction i
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Notice that each separate substance
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Table E Selected Polyatomic Ions Fo
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Table H Vapor Pressure of Four Liqu
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Table K Common Acids Table N Select
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Table R Organic Functional Groups C
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Table S Properties of Selected Elem
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Table T Important Formulas and Equa
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Activity Series of Metals Name Symb
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