Topic 1 - Matter and Energy - Revsworld

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Topic 1 - Matter . and Energy 20. Phase change diagrams: Identify freezing, melting and boiling points, and other segments Concept Task: Be able to identify segments and interpret heating and cooling curves. Follow and study interpretations given below for the heating and the cooling curves. Temperature ( o C) -10 0 50 100 130 A solid solid/liquid B (melting/fusion) liquid liquid/gas D (boiling/evaporation) 0 2 4 6 8 10 12 14 16 18 20 22 24 26 28 30 32 34 36 38 40 42 44 46 Time ( minutes) Some important information about the above heating curve . Melting point / freezing point/ solid - liquid equilibrium occurs at : Boiling point / condensation point/ liquid-gas equilibrium occurs at : kinetic energy increases / potential energy remains constant during segments: The substance exists in one phase during segments: Potential energy increases / kinetic energy remains constant during segment: The substance exists in two phases during segments: Total time the substance goes through boiling (from 24 to 40 minutes) : Copyright © 2011 E3 Scholastic Publishing. All Rights Reserved. 13 gas 0 o C 100 o C A, C, and E A, C, and E B and D B and D 16 minutes The substance is likely water because solid water(ice) melts at 0 o C and boils at 100 o C Temperature ( o C) 20 30 40 50 60 70 80 90 MP gas A Boiling point (BP) BP gas/liquid (condensation) Freezing Point (FP) Melting Point (MP) Heating Curve C Cooling Curve liquid liquid/solid (freezing) solid 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 Time (minutes) Some important information about the cooling curve above: Melting point / freezing point/ solid - liquid equilibrium occurs at : Boiling point / condensation point/ liquid gas-equilibrium occurs at : kinetic energy decreases / potential energy remains constant during segments: Potential energy decreases / kinetic energy remains constant during segment: Total time for substance to freeze (from 13 to 18 minutes) : B E 40 o C 70 o C A, C, and E B and D 5 minutes The substance is not water because the freezing and boiling points are different from those of water. C D E
Topic 1 - Matter . and Energy 23. Heat calculations: Understanding heat equations and heat constants The amount of heat absorbed or released by a substance can be calculated using heat equations. There are three heat equations, and each heat equation contains a heat constant. The heat equations and the heat constants for water are given on the Reference Tables. Reference Table B: Heat constant for water Reference Table T: Heat equations Heat of fusion (Hf) Heat of Vaporization (Hv) Specific Heat Capacity of H 2 O(l) (C) 334J/g 2260 J/g 4.18J/g o C The notes below explain more about the heat constant and the heat equation, as well as when to use each heat equation. 24. Specific heat capacity: Understanding heat equation during temperature change A substance can change from one temperature to another by either absorbing or releasing heat. If heat is absorbed, the temperature of the substance will increase. If heat is released, the temperature of the substance will decrease. Heat absorbed 15 o C to warm 3 g to cool Heat released Heat(q) 20 o C 3 g q = mC∆T q = mHf q = mHv Heat = m x C x ∆ T If the specific heat capacity and the mass of a substance are known, the amount of heat absorbed or released by the substance to change from one temperature to another can be calculated using the equation below: m = mass of substance (g) Heat = m x C x ∆ T C = specific heat capacity (J/g. o C) ∆T = difference in temperature ( o C) (∆T = High temp - Low temp) Specific heat capacity (C) of a substance is the amount of heat needed to change the temperature of a 1 gram sample of a substance by just 1 o C. Specific heat capacity (C) for water = 4.18 J/g. o C See Reference Table B This value (4.18 J/g. o C) for water can be interpreted in the following ways: It takes 4.18 Joules (J) of heat energy to change the temperature of a one gram (g) sample of water by just one degree Celsius ( o C). Or A one gram sample of water must absorb (or release) 4.18 Joules of heat energy to change its temperature by just one Celsius degree ( o C) In heat equations, the specific heat capacity (C) serves as a conversion factor that allows you to calculate the amount of heat absorbed (or released) by any given amount (grams) of a substance to change from any given temperature to another. NOTE: Specific heat capacity for other substances are different from that of water. Copyright © 2011 E3 Scholastic Publishing. All Rights Reserved. 15
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Page 22 and 23: Introduction 4. The three types of
Page 24 and 25: . Topic 2 -The Periodic Table Atomi
Page 26 and 27: Topic 2 - The Periodic Table 18. Gr
Page 28 and 29: Concept Task: Be able to determine
Page 30 and 31: Topic 3 - The Atomic . structure To
Page 32 and 33: Topic 3 - The Atomic Structure . 10
Page 34 and 35: . Topic 3 - The Atomic Structure 17
Page 36 and 37: Lesson 3 - Electrons location and a
Page 38 and 39: 30. Spectral lines: Determining whi
Page 40 and 41: . Topic 3 - The Atomic Structure 36
Page 42 and 43: Topic 4 - Chemical . Bonding Topic
Page 44 and 45: . Topic 4 - Chemical Bonding 10. Co
Page 46 and 47: Topic 4 -. Chemical Bonding 18. Mol
Page 48 and 49: Topic 4 .- Chemical Bonding 25. Deg
Page 50 and 51: . Topic 4 - Chemical bonding 32. Le
Page 52 and 53: Topic 4 - Chemical . Bonding 38. Si
Page 54 and 55: . Topic 5 - Chemical formulas and e
Page 56 and 57: Lesson 3 - Writing and naming chemi
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Topic 5 - Chemical . formulas and e
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Topic 5 - Chemical . formulas and e
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. Topic 6 - Mole interpretation : M
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6. Mass - mole relationship: Unders
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12. . Percent composition of hydrat
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16. Mole - mole problems: Calculati
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Topic 6 - Mole interpretation: Math
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4. Properties of solution: Facts To
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Topic 7 - Solutions . 10. Soluble a
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Topic 7 - Solutions . 15. Saturated
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Topic 7 - Solutions . 21. The solub
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Topic 7 - Solutions . Lesson 5 : Bo
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Topic 7 - Solutions . 32. Effect of
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Topic 8 - Acids, . Bases and Salt T
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Topic 8 - Acids, . Bases and Salt 8
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Topic 8 - Acids, Bases . and Salt I
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Topic 9 - Kinetics and . equilibriu
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Topic 9 - Kinetics . and equilibriu
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Concept Terms . Topic 9 - Kinetics
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Topic 10 - Organic . Chemistry 3. B
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Topic 10 - Organic . Chemistry 9. A
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Topic 10 - Organic . Chemistry 17.
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25. Ketones: Definitions, facts, an
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Topic 10 - Organic . Chemistry Less
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Topic 10 -. Organic Chemistry 39. c
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Topic 10 .- Organic Chemistry 42. A
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Topic 11 - Redox . and Electrochemi
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Topic 11 - Redox and Electrochemist
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14. Redox equations Topic 11 - Redo
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Topic 11 - Redox and . Electrochemi
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Topic 11 - Redox . and Electrochemi
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33. Electrolytic cells: Diagram and
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37. Electroplating: How does it wor
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Concept Terms Topic 11 - Redox . an
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Topic 12: Nuclear Chemistry . 4. Nu
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Topic 12: Nuclear . Chemistry 11. B
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Topic 12: Nuclear . Chemistry 17. F
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Topic 12: Nuclear . Chemistry 22. N
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Topic 12: Nuclear . Chemistry 26. R
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Topic 12: Nuclear . Chemistry 30. H
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. Topics Review Questions 317
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Constructive Response Questions Top
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Constructed Response Questions Topi
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. Topic 3 - The Atomic Structure Co
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Topic 4 - Chemical Bonding Construc
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. Topic 6 - Mole interpretation: Ma
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. Topic 7 - Solutions 23. According
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. Topic 8 - Acids, Bases, and Salts
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. 20. A potential energy diagram fo
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. 28. Given the reaction below: C 4
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Topic 11 - Redox and Electrochemist
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Topic 12: Nuclear . Chemistry Const
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Table G: Solubility Curves . Refere
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Table P: Organic Prefixes . Referen
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. Reference Tables 373
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C Glossary Calorimeter a device use
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Glossary . H cont. Half-reaction a
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P Glossary . Parts per million conc
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Index . Absolute zero 10 Accelerato
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Index . Law of conservation 113 - 1
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