Matter and Energy

1. Matter and Energy Preparation of College Chemistry Columbia University Department of Chemistry

2. State Composition Classification of Matter

3. Four states of Matter Solid Liquid Gas Plasma

4. Composition of Matter Elements Compounds Mixtures

5. Matter Classification Matter Mixtures Pure Substances Compounds Homogeneous One Phase (Solutions) Elements Heterogeneous More than one phase

6. Organelle Cell Organ Tissue System Organism Protons Neutrons Molecule Macromolecule Electrons Atom (Elements) Object Levels of Organization Leptons Quarks,... http://www.bnl.gov/RHIC/

7. Average Elemental Composition of Human Body

8. Elements’ Distribution (earth, sea, atmosphere)

9. H 1 He 2 Li 3 Be 4 5 B C 6 7 N 8 O F 9 Ne 10 Na 11 12 Mg 13 Al Si 14 P 15 S 16 Cl 17 Ar 18 K 19 20 Ca 21 Sc Ti 22 V 23 Cr 24 25 Mn Fe 26 Co 27 Ni 28 Cu 29 Zn 30 31 Ga 32 Ge 33 As Se 34 Br 35 36 Kr Rb 37 Sr 38 39 Y 40 Zr Nb 41 42 Mo Tc 43 44 Ru Rh 45 46 Pd Ag 47 Cd 48 49 In 50 Sn 51 Sb 52 Te 53 I Xe 54 Cs 55 Ba 56 57 La Hf 72 Ta 73 W 74 75 Re 76 Os 77 Ir 78 Pt Au 79 80 Hg 8l Tl Pb 82 83 Bi Po 84 85 At Rn 86 Fr 87 88 Ra Ac 89 104 Rf Ha 105 Sg 106 107 Bh Hs 108 Mt 109 Ce 58 Pr 59 Nd 60 Pm 61 62 Sm 63 Eu 64 Gd Tb 65 Lu 71 70 Dy Yb Tmi Ho 67 69 66 68 Er Th 90 91 Pa 92 U Np 93 94 Pu Am 95 96 Cm Bk 97 102 103 Cf Es Fm Md 101 99 100 Lr 98 No , Nonmetals, Metals Metalloids Main-Group Elements Main-Group Elements Transition Metals Inner-Transition Metals Lantanides Actinides

10. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr B C N Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Al Si P He Li Be Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Ga Ge As O F Na Ne Mg Fr Ra Ac Rf Ha Sg Bh Hs Mt In Sn Sb S Cl Ar K Ca Ce Pr Nd Pm Sm Eu Gd Tb Ho Yb Er Tmi Lu Dy Tl Pb Bi Se Br Rb Kr Sr Th Pa U Np Pu Am Cm Bk No Cf Md Es Lr Fm Te I Cs Ba Xe Po At Ra Fr Rn 8A Noble Gases 1A Alkali metals 7A Halogens 2A Alkaline earth metals 6A Chalcogens 4A 3A 5A

11. Elements that Exist as Diatomic Molecules

12. Allotropic Forms (Allotropes) Berzelius, 1841 Graphite Carbon Diamond Buckyballs (C60 ) Nanotubes Oxygen (O2 ) Oxygen Ozone (O3 ) Oxygen Singlet (O2*)

13. Allotropic Forms (Allotropes) Monoclinic (S8 ) Sulfur Rhombic (S8 ) Amorphous (Sn ) White phosphorus, (P4 ), d =1.82 Red phosphorus, (Pn ), d = 2.20 Phosphorus Violet phosphorus, (Pn ), d = 2.32 Black phosphorus, (Pn ), d = 2.70

14. Compounds Contain two or more elements with fixed mass percents Covalent: Glucose: 40.00% C 6.71% H 53.29% O Ionic: Sodium chloride: 39.34% Na 60.66% Cl

15. Depending Upon Bonding Type Compounds Ionic (Coulombic forces) Molecular (Covalent bonds) Molecules Cations Anions

16. Intensive vs. Extensive: density vs. mass Chemical vs. Physical Properties of Substances

17. Chemical vs. Physical Properties Chemical Properties Molecules or ions undergo a change in structure or composition Physical Properties Can be studied without a change in structure or composition

19. Intensive vs. Extensive: density vs. mass Chemical vs. Physical Properties of Substances

20. Extensive Properties Vary with the amount of material • Mass • Volume • Internal Energy • Enthalpy • Entropy

21. Intensive Properties Independent of the amount of material Density (mass per unit volume) Temperature (average energy per particle)

22. Energy in Chemical Changes Heat: Quantitative Measurement Energy

23. Is the energy available but not being used or is it in use? Types of Energy Forms of Energy Kinetic Energy (Motion Energy) Radiant (light) Thermal (heat) Energy Chemical (Capacity to do work) Potential Energy (Stored Energy) Electrical • Position, • Composition • Condition Mechanical Law of Conservation of Energy: In any chemical or physical change, energy can be converted from one form to another, but it is neither created nor destroyed

24. Heat Energy and Specific Heat Units of Energy: Joule : Amount of kinetic energy possessed by a 2kg object moving at a speed of 1m/s. Substituting these values in the equation that defines kinetic energy: Equivalent to the amount of energy you will feel if you drop 4.4 lb from about 4 in. onto your foot. calorie (cal) : Amount of heat energy needed to raise the temperature of one gram of water by one degree Celsius measured between 14.5 and 15.5°C.

25. Units of Energy 1 cal = 4.3184 J The joule and calorie are rather small units. The large calorie (Cal, C) is used to express the energy content of foods. 1kcal = 4.3184kJ 1C = 1kcal = 103 cal 140,000 cal of energy is released when the soft drink is metabolized within the body. Sprite™ contains 140 C: 1 BTU (British Thermal Unit): Amount of heat needed to raise the temperature of a lb of water one °F 1BTU =.818 kcal

26. Heat Capacity and Specific Heat Joseph Black (~1750): “Amount of heat needed to raise the temperature of a substance by the same amount depends on the substance” Amount of heat needed to raise the temperature of a given quantity of substance in a specific physical state. Heat Capacity Amount of heat needed to raise the temperature of 1 g of a substance in a specific physical state by 1°C Specific Heat • Units: cal /g °C or J/g °C

27. The specific heat of a substance changes when the physical state of the substance changes Ex. Water (ice) Water (liquid) Water (steam) 2 .1 J / g °C 4 . 18 J / g °C 2 . 0 J / g °C The higher the specific heat of a substance, the less its temperature will change when it absorbs a given amount of heat. • metals heat up quickly, but cool quickly At the beach, sand has a lower specific heat than water, so it heats up while water stays cool.

28. Solving problems Heat transferred = mass x Specific heat x ∆T q = m x Cs x ∆T Amount of heat energy needed to cause a fixed amount of a substance to undergo a specific temperature change without causing a change of state. Transfer of heat from one body to another. Heat always flows from the warmer body to the colder body. The heat loss by the warmer body is equal to the heat gained by the colder body. Generalizations:

29. Potential energy Potential energy H2 H2 O2 O2 + + time time Heat in Chemical Change Electrolysis Direct synthesis H2O H2O Potential Energy Diagrams