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Matter Classification
Matter
Mixtures Pure Substances
HeterogeneousMore than one phase
HomogeneousOne Phase(Solutions)
Elements Compounds
SystemOrgan Tissue
Macromolecule
CellOrganelle
Protons
Neutrons
Atom (Elements)
Levels of Organization
Organism
Object
Leptons
Quarks,... http://www.bnl.gov/RHIC/
Molecule
Electrons
Average Elemental Composition of Human Body
1.0Traces of other elements
1.0Phosphorus
2.0Calcium
3.0Nitrogen
10.0Hydrogen
18.0Carbon
65.0Oxygen
Mass %Element
Elements’ Distribution (earth, sea, atmosphere)
0.47All others0.58Titanium
0.87Hydrogen
0.03Fluorine1.93Magnesium
0.03Nitrogen2.40Potassium
0.04Barium2.63Sodium
0.06Sulfur3.39Calcium
0.08Carbon4.71Iron
0.09Manganese7.50Aluminum
0.11Phosphorus25.67Silicon
0.19Chlorine49.20Oxygen
Mass %ElementMass %Element
Metalloids
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
Inner-Transition Metals
Transition Metals
Main-Group Elements Main-Group Elements
Lantanides
Actinides
Metals, Nonmetals,
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
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
8A Noble Gases
Ga
Al
Tl
In
B
Pb
Sn
Ge
Si
C N
Bi
As
Sb
P
Po
Te
O
Se
SBr
I
At
F
Cl
Ne
Kr
Ar
Rn
Xe
He
7A Halogens
6A Chalcogens5A4A3A
1A Alkali metals
2A Alkaline earth metals
Na
Rb
K
Fr
Cs
Li
Mg
Sr
Ca
Ra
Ba
Be
Elements that Exist as Diatomic Molecules
Bluish-black solidI2IIodine
Reddish-brown liquidBr2BrBromine
Yellow-green gasCl2ClChlorine
Pale yellow gasF2FFluorine
Colorless gasO2OOxygen
Colorless gasN2NNitrogen
Colorless gasH2HHydrogen
Normal StateMolecular FormulaSymbolElement
Allotropic Forms (Allotropes) Berzelius, 1841
CarbonGraphite
Diamond
Nanotubes
Buckyballs (C60 )
OxygenOxygen (O2 )
Ozone (O3 )
Oxygen Singlet (O2* )
Allotropic Forms (Allotropes)
Sulfur
Monoclinic (S8 )
Amorphous (Sn )
Rhombic (S8 )
Phosphorus
White phosphorus, (P4 ), d =1.82
Red phosphorus, (Pn ), d = 2.20
Violet phosphorus, (Pn ), d = 2.32
Black phosphorus, (Pn ), d = 2.70
Compounds
Contain two or more elements with fixed mass percents
Sodium chloride: 39.34% Na60.66% Cl
Glucose: 40.00% C6.71% H53.29% O
Covalent:
Ionic:
Depending Upon Bonding Type
Compounds
Ionic (Coulombic forces)
Molecular(Covalent bonds)
MoleculesCations Anions
Chemical vs. Physical Properties
Chemical Properties
Physical Properties
Molecules or ions undergo a change instructure or composition
Can be studied without a change instructure or composition
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)
Radiant (light)
Thermal (heat)
Chemical
Electrical
Mechanical
In any chemical or physical change, energy can be convertedfrom one form to another, but it is neither created nor destroyed
Law of Conservation of Energy:
Is the energy available but not being used or is it in use?
Forms of Energy Types of Energy
Kinetic Energy (Motion Energy)
Energy(Capacity to do work)
Potential Energy (Stored Energy)
o Position,o Compositiono Condition
†
Ek =12
mv2
Heat Energy and Specific HeatUnits of Energy:
Amount of kinetic energy possessed by a 2kg object moving at a speed of1m/s. Substituting these values in the equation that defines kinetic energy:
Joule :
Equivalent to the amount of energy you willfeel 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 ofwater by one degree Celsius measured between 14.5 and 15.5°C.
†
Ek =12
mv2
†
Joule =kgm2
s2
1kcal = 4.3184kJ1C = 1kcal = 103 cal
Sprite™ contains 140 C:
1 BTU (British Thermal Unit):
140,000 cal of energy is released when thesoft drink is metabolized within the body.
Amount of heat needed to raise thetemperature of a lb of water one °F
1 cal = 4.3184 J
The joule and calorie are rather small units.
The large calorie (Cal, C) is used to express the energycontent of foods.
Units of Energy
1BTU =.818 kcal
Specific HeatAmount of heat needed to raise the temperature of 1 g ofa substance in a specific physical state by 1°C
Units: cal /g °C or J/g °C
“Amount of heat needed to raise the temperature of asubstance by the same amount depends on the substance”
Amount of heat needed to raise the temperature of agiven quantity of substance in a specific physical state.
Joseph Black (~1750):
Heat Capacity and Specific Heat
Heat Capacity
The specific heat of a substance changes when thephysical state of the substance changes
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 itstemperature will change when it absorbs a given amount of heat.
At the beach, sand has a lower specific heat thanwater, so it heats up while water stays cool.
metals heat up quickly, but cool quickly
Water (ice) Water (steam) Water (liquid)Ex.
Solving problemsHeat transferred = mass x Specific heat x ∆T
q = m x Cs x ∆T
1. Amount of heat energy needed to cause a fixed amount of a substanceto undergo a specific temperature change without causing a change ofstate.
2. Transfer of heat from one body to another.
I. Heat always flows from the warmer body tothe colder body.
II. The heat loss by the warmer body is equal tothe heat gained by the colder body.
Generalizations: