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

Classification of Matter State Composition

Four states of Matter Solid Liquid Gas Plasma

Composition of Matter Elements Compounds Mixtures

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

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

Average Elemental Composition of Human Body Mass % Oxygen 65.0 Carbon 18.0 Hydrogen 10.0 Nitrogen 3.0 Calcium 2.0 Phosphorus 1.0 Traces of other elements

Elements’ Distribution (earth, sea, atmosphere) Mass % Oxygen 49.20 Chlorine 0.19 Silicon 25.67 Phosphorus 0.11 Aluminum 7.50 Manganese 0.09 Iron 4.71 Carbon 0.08 Calcium 3.39 Sulfur 0.06 Sodium 2.63 Barium 0.04 Potassium 2.40 Nitrogen 0.03 Magnesium 1.93 Fluorine Hydrogen 0.87 Titanium 0.58 All others 0.47

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

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

Elements that Exist as Diatomic Molecules Symbol Molecular Formula Normal State Hydrogen H H2 Colorless gas Nitrogen N N2 Oxygen O O2 Fluorine F F2 Pale yellow gas Chlorine Cl Cl2 Yellow-green gas Bromine Br Br2 Reddish-brown liquid Iodine I I2 Bluish-black solid

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

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

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

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

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

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

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

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

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

Energy Heat: Quantitative Measurement Energy in Chemical Changes

Law of Conservation of Energy: Is the energy available but not being used or is it in use? Forms of Energy Types of Energy Radiant (light) Kinetic Energy (Motion Energy) 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

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.

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. 1C = 1kcal = 103 cal 1kcal = 4.3184kJ 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

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

The specific heat of a substance changes when the physical state of the substance changes Ex. Water (ice) Water (steam) Water (liquid) 2 .1 J / g °C 2 . 0 J / g °C 4 . 18 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.

Solving problems q = m x Cs x ∆T 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:

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