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

2. Classification of Matter
State
Composition

3. Four states of Matter
Solid
Liquid
Gas
Plasma

4. Composition of Matter
Elements
Compounds
Mixtures

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

6. Levels of Organization
Organism
System
Cell
Organ
Organelle
Tissue
Molecule
Macromolecule
Protons
Atom (Elements)
Neutrons
Electrons
Object
Leptons
Quarks,...

7. 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

8. 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

9. , Nonmetals, Metals Metalloids Main-Group Elements Main-Group Elements47 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

10. 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

11. 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

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: % C
6.71% H
53.29% O
Ionic:
Sodium chloride: % Na
60.66% Cl

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

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

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

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
Heat: Quantitative Measurement
Energy in Chemical Changes

23. 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

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 = 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 = kJ
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 (steam)
Water (liquid)
2 .1 J / g °C
2 . 0 J / g °C
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 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:

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