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Summary: In this chapter we learned about the specific states of matter and how they relate to liquids, and what particular characteristics they have. I also learned how kinetic energy plays a role in determining the nature of a substance. Fluids are not just limited to liquids, but also gases because they can flow if they are denser than air. Something unique was that vapor pressure requires a specialized balance to be at equilibrium. Boiling is not just about the increase in temperature of a liquid but also vapor pressure and external pressure. 13.3 The Nature of Solids A Model of Solids a. How are the structure and properties of solids related? The general properties of solids reflect the orderly arrangement of their particles and the fixed locations of their particles. Melting point (mp)- is the temperature at which a solid changes into a liquid. Freezing point (fp)- is the temperature at which a liquid changes into a solid. Crystal Structure and Unit Cell a. What determines the shape of a crystal? The shape of a crystal reflects the arrangement of the particles within the solid. Crystal- a solid in which the particles are arranged in an orderly, repeating, three-dimensional pattern called a crystal lattice. Unit cell- is the smallest group of particles within a crystal that retains the geometric shape of a crystal. Allotropes- are two or more different molecular forms of the same element in the same physical state. Amorphous solid- is a solid that lacks an ordered internal structure. Glass- is a transparent fusion product of inorganic substances that have cooled to a rigid state without crystalizing. Summary: In this chapter I learned about the changes a solid take on due to increase or decrease of temperature, melting, and how a liquid can change to a solid, freezing. I also learned about the different types of solids which are amorphous and crystalline. Each having different rules that alter their function and characteristics. 13.4 Changes of State Sublimation a. When can sublimation occur? Sublimation occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature. Sublimation- is the change of a substance from a solid to a vapor without passing through the liquid state. Dry ice. Phase Diagrams a. How are the conditions at which phases are equilibrium represented on a phase diagram? The conditions of pressure and temperature at which two phases exist in equilibrium are indicated on a phase diagram by a line separating the two regions representing the phases. Phase diagram- this gives the conditions of temperature and pressure at which a substance exists as solid, liquid, or gas (vapor). Triple point- this describes the only set of conditions at which all three phases can exist in equilibrium with one another. Summary: This section taught me how there are exceptions to how matter can change its state. For example, Dry Ice changes from a solid straight into a gas through sublimation, instead of going through a liquid phase. I also learned about different phases which can determine a substances state of matter based on different conditions. Triple point is when all three phases exist in equilibrium.
Name: Enmanuel G. Name: Robens T. Grade: 10 States of Matter Project You and you lab partner are going to create a study aid in the form of a game for the information in Chapter 13 States of Matter. First, each of you, independently from each other, will summarize the chapter on 3 pages of a pdf which will be submitted in Angel by the end of class on Wednesday Feb 22. Second, you and you lab partner will be given a game platform which you will use for your questions and answers, either Jeopardy or Kahoot. Third, you will fill in the information at the bottom of this page with your username, passwords and/or websites so that you do not forget this and I have a copy in case anything gets misplaced. This page will be submitted into Angel as a Word Document on Wednesday February 22 during class. Fourth, you will use your notes to generate the questions and answers. Finally you will give me access to your game by putting the website or Game Number on this page adding this page to your 3 pages of notes and resubmitting it in Angel as a pdf by the end of the class on Friday Feb 24. This page is due by the end of class on Wednesday February 22. This Project is due by the end of class on Friday February 24. Jeopardy (https://jeopardylabs.com) Password: Edit Link: Play Link: Kahoot (https://getkahoot.com) Username: EnmanuelG Email: Enmanuelg239@gmail.com Password: chemistry239 Game PIN: 847811
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Enmanuel’s Chemistry Notebook
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Unit 1 Measurement Lab Separation o
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Unit 5 (28 days) Chapter 10 Chemica
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30. Always lubricate glassware (tub
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Chapter 1 Unit 1 Introduction to Ch
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Determine appropriate and consisten
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2. One cereal bar has a mass of 37
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1. How many meters are in one kilom
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The Learning Goal for this assignme
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RULE #3: To add/subtract in scienti
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Rule 3: A final zero or trailing ze
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For addition and subtraction, look
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Dimensional Analysis This is a way
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Chapter 4 Unit 2 Atomic Structure T
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Looking at Ions We haven’t talked
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Neutron Madness We have already lea
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Electron Configuration Color the su
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Electron Configuration In order to
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Create groups for these Scientist a
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The Learning Goal for this Assignme
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Define Atomic Size: The size of the
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Electronegativity Define Electroneg
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Unit 3 Chapter 25 Nuclear Chemistry
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Enmanuel Garrido Name _____________
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Learning Goal for this section: Exp
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Beta Particle Decay Beta decay is a
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Ion Charge? What is the charge on f
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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
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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
Page 80 and 81: Chapter 9 Unit 4 Chemical Names and
Page 82: http://www.bbc.co.uk/education/guid
Page 85 and 86: Chapter 12 Stoichiometry The studen
Page 87 and 88: www.youtube.com/watch?v=BTRm8PwcZ3U
Page 89 and 90: 4) Double displacement: This is whe
Page 91 and 92: Determine the Type of Reaction for
Page 93 and 94: Step 3 Always leave hydrogen and ox
Page 95 and 96: 1) ___ NaNO3 + ___ PbO ___ Pb(NO3)
Page 97 and 98: 1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2
Page 99 and 100: we can determine that 2 moles of HC
Page 101 and 102: When there is no limiting reagent b
Page 103 and 104: Example 7 How much 5M stock solutio
Page 105 and 106: Theoretical and Actual Yields Key T
Page 107 and 108: Review Purposes To get an over
Page 110 and 111: Unit 6 Chapter 13 States of Matter
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Page 121 and 122: P 1 : 1980 torr V 1 : 7730 ml P 2 :
Page 123 and 124: P 1 : 107 kPA T 1 : 41 C à 314 K P
Page 125 and 126: Ideal Gas Law: The gas law that inc
Page 127 and 128: 7.Electrolyte: Is a compound that c
Page 129 and 130: Create and interpret potential ener
Page 131 and 132: Part 1: Mass Percent Mass percent (
Page 133 and 134: Glossary Concentration: Amount of d
Page 135 and 136: Specific Heat Here is the definitio
Page 137 and 138: Step One: solid ice rises in temper
Page 139 and 140: Step Three: liquid water rises in t
Page 141 and 142: Step Five: steam rises in temperatu
Page 143 and 144: then it is exothermic, meaning the
Page 145 and 146: Chemical Concepts: The chemical con
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Page 149 and 150: Chemical Concepts: The chemical con
Page 151 and 152: Reduction Oxidation reduction react
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Page 155 and 156: The acid base theory of Brønsted a
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Page 159 and 160: Let's discuss significant figures a
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Page 163 and 164: 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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