Download Chemistry Reference Tables

PT 1: Relative Atomic Mass and Electron Configurations
NAME ___________________________________________________________________________________________
1
18
Hydrogen
Helium
184.002602
1.00794
1
H
1
22.989770
2
Lithium
Beryllium
6.941
9.012182
3
Li
4
Sodium
22.989770
11
Na
Be
Electron
Configuration
Potassium
13
14
Carbon
Nitrogen
Oxygen
Fluorine
Neon
10.811
12.0107
14.00674
15.9994
18.9984
20.1797
2-8-1
B
5
6
2-3
C
Silicon
3
K
20 Ca
2-8-8-2
4
5
6
Scandium
Titanium
Vanadium
Chromium
44.955910
47.867
50.9415
51.9961
21
Sc
2-8-9-2
V
Ti
23
22
2-8-10-2
24
8
Manganese
54.938049
Cr
2-8-13-1
2-8-11-2
7
25
Mn
10
11
Al
13
12
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
58.6934
63.546
65.39
69.723
72.61
74.92160
Fe
27
Co
28
2-8-15-2
Ni
29
2-8-16-2
Cu
30
2-8-18-1
Zn
31
2-8-18-2
Ga
32
2-8-18-3
Ge
Strontium
Yttrium
Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
87.62
88.90585
91.224
92.90638
95.94
(98)
101.07
102.90550
106.42
107.8682
112.411
114.818
118.710
Rb
Cesium
132.90545
55
Cs
**-18-8-1
38
Sr
2-8-18-8-2
Barium
137.327
56 Ba
-18-8-2
39
Y
40
Zr
2-8-18-9-2
2-8-18-10-2
Lanthanum
138.9055
57 La
41
Nb
42
2-8-18-13-1
Hafnium
Tantalum
178.49
180.9479
72 Hf
-18-9-2
-32-10-2
73Ta
-32-11-2
Rhenium
Osmium
Iridium
190.23
192.217
75 Re
76 Os
77 Ir
-32-12-2
-32-13-2
-32-14-2
-32-15-2
Rutherfordium
Dubnium
Seaborgium
(267)
(268)
(271)
89
Ac
104
Rf
105
Db
106
Sg
46
2-8-18-16-1
74W
(227)
Ra
Rh
186.207
Actinium
88
45
183.84
(226)
-32-18-8-2
Ru
Tungsten
Radium
Fr
44
2-8-18-15-1
(223)
87
43
2-8-18-14-1
Francium
-32-18-8-1
Tc
Mo
2-8-18-12-1
Pd
47
2-8-18-18
Ag
48
Cd
Platinum
Gold
Mercury
Thallium
195.078
196.96655
200.59
204.3833
78 Pt
79 Au
-32-17-1
-32-18-1
-32-18-2
Hassium
Meitnerium
Darmstadtium
Roentgenium
Copernicium
(270)
(276)
(281)
(280)
(285)
108
Hs
109
Mt
110
Ds
111
Rg
112
50
2-8-18-18-3
80 Hg
(272)
Bh
In
2-8-18-18-2
Bhorium
107
49
2-8-18-18-1
33
2-8-18-4
85.4678
37
P
58.933200
Rubidium
2-8-18-8-1
15
Sn
Uut
113
S
17
51
Cl
18
2-8-7
Se
Krypton
79.904
83.80
Br
36
2-8-18-7
Sb
Ar
2-8-8
Bromine
35
2-8-18-6
Kr
2-8-18-8
Tellurium
Iodine
Xenon
127.60
126.90447
131.29
Te
52
53
I
54
Xe
2-8-18-18-5
2-8-18-18-6
2-8-18-18-7
2-8-18-18-8
Lead
Bismuth
Polonium
Astatine
Radon
207.2
208.98038
(209)
(210)
(222)
83 Bi
-32-18-4
84 Po
-32-18-5
114
85 At
-32-18-6
Flerovium
Cn
Argon
39.948
34
Antimony
82 Pb
-32-18-3
Chlorine
35.4527
2-8-18-6
2-8-18-18-4
81Tl
Sulfur
Selenium
121.760
Ne
10
2-8
32.066
2-8-6
As
F
9
2-7
16
2-8-5
Iron
2-8-14-2
O
8
30.973761
Si
14
17
2-6
Phosphorus
2-8-4
2-8-3
N
7
55.845
26
2-8-13-2
9
16
2-5
28.0855
Mg
15
2-4
Aluminum
12
He
Boron
Letter Symbol
26.98153
Calcium
40.078
19
Na
24.3050
39.0983
2-8-8-1
2
2
Magnesium
2-8-2
2-8-1
11
Atomic Number
2-2
2-1
Element
Name
Sodium
Atomic Mass
86
-32-18-7
Rn
-32-18-8
Livermorium
Fl
115
Uup
116
Lv
117
Uus
-32-18-9-2
These ** indicate that there are energy
levels of 2-8-18 for elements 55 & above
Key:
italicized symbols =
synthetic (human made)
an entry in ( ) indicates the
longest lived isotope of an
element for which the atomic
mass is indeterminate
Cerium
Praseodymium
Neodymium
Promethium
Samarium
Europium
Gadolinium
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
140.116
140.90765
144.24
(145)
150.36
151.964
157.25
158.92534
162.500
164.93032
167.259
168.93421
173.054
174.9668
58
Ce
59
Pr
60
Nd
61
Pm
Thorium
Protactinium
Uranium
Neptunium
232.038
231.03588
238.0289
(237)
Th
90
91
Pa
92
U
93
Np
62
Sm
Plutonium
(244)
94
Pu
63
Eu
Americium
64
Am
Tb
Dy
Curium
Berkelium
Californium
Einsteinium
Fermium
(247)
(247)
(251)
(252)
(257)
Cm
97
Bk
98
Cf
99
Es
68
Er
66
96
67
Ho
65
(243)
95
Gd
100
Fm
Tm
69
Mendelevium
(258)
101
Md
Yb
70
71
Lu
Nobelium
Lawrencium
(259)
(262)
102
No
103
Lr
PT 2: Categories of Elements and a Few Special "Family"
Group 18 = noble gas family
Group 1 =
alkali metal
family
Group 2 =
alkaline-earth metal
2
family
hydrogen
H
1
NM
1
1
lithium
beryilium
Li
Be
3
M
2-1
Na
11
M
name
symbol
atomic
number
Electron
Configuration
M
Metal
Metalloid
Nonmetal
Noble Gas
M
Me
NM
NG
2-8-1
K
magnesium
M
M
calcium
Ca
20
M
2-8-8-1
2-8-8-2
rubidium
strontium
Rb
37
M
3
16
17
boron
carbon
nitrogen
oxygen
fluorine
C
N
O
F
6
Me
scandium
6
7
8
9
10
11
12
titanium
vanadium
chromium
manganese
iron
cobalt
nickel
copper
zinc
Sc
21
M
22
2-8-9-2
2-8-10-2
2-8-11-2
zirconium
niobium
yttrium
Ti
M
2-8-18-8-1
2-8-18-8-2
2-8-18-9-2
2-8-18-10-2
cesium
barium
lanthanum
hafnium
M
Cs
55
M
Ba
56
M
2-8-18-18-8-1
2-8-18-18-8-2
2-8-18-18-9-2
francium
radium
actinum
Ra
88
M
La
57
M
Ac
89
M
Zr
40
M
Hf
72
M
**18-32-10-2
rutherfordium
Rf
104 M
23
V
Cr
24
M
M
molybdenum
Nb
41
M
Mo
42
M
2-8-18-12-1
tantalum
Ta
73
M
-18-32-11-2
dubnium
NM
2-7
2-8
aluminum
silicon
sulfur
chlorine
argon
13
Si
14 Me
P
S
15 NM
16 NM
Cl
17 NM
Ar
18 NG
2-8-4
2-8-5
2-8-6
2-8-7
2-8-8
M
2-8-3
gallium
germanium
phosphorus
arsenic
Zn
30
M
Ga
31
M
Ge
32 Me
selenium
bromine
krypton
As
33 SM
Br
35 NM
Kr
36 NG
2-8-13-2
2-8-14-2
2-8-15-2
2-8-16-2
2-8-18-1
2-8-18-2
2-8-18-3
2-8-18-4
2-8-18-5
Se
34 NM
2-8-18-6
2-8-18-7
2-8-18-8
technetium
ruthenium
rhodium
palladium
M
Ru
44
M
Rh
45
M
2-8-18-15-1
2-8-18-161
tungsten
rhenium
osmium
iridium
Re
75
M
Os
76
M
-18-32-13-2
77
2-8-18-18-1
platinum
gold
Pt
M
78
meitnerium
Hs
108 M
Ag
47 M
2-8-18-18
-18-32-15-2
hassium
Bh
107 M
silver
Pd
46
M
Ir
-18-32-14-2
bohrium
Sg
106 M
9
Cu
29
M
2-8-18-13-2
seaborgium
Db
105 M
NM
2-6
neon
Ne
10 NG
Ni
28
M
2-8-18-131
-18-32-12-2
8
NM
2-5
18
Co
27
M
Mn
Tc
43
M
W
74
M
7
Mt
109 M
Au
79 M
M
-18-32-17-1
-18-32-18-1
damstadtium
roentgentium
Ds
110 M
Rg
111 M
cadmium
indium
Cd
48
M
tin
In
49
M
2-8-18-18-2
2-8-18-18-3
mercury
thallium
Hg
80
M
Sn
50
M
2-8-18-18-4
lead
Tl
81
-18-32-18-2
Pb
82
M
M
-18-32-18-3
copernicium
-18-32-18-4
Uut
Cn
112 M
flerovium
Fl
113
114
M
antimony
tellurium
iodine
xenon
Sb
51 Me
Te
52 Me
I
53 NM
Xe
54 NG
2-8-18-18-8
2-8-18-18-5
2-8-18-18-6
2-8-18-18-7
bismuth
polonium
astatine
radon
85 Me
Rn
86 NG
Bi
83
M
-18-32-18-5
Uup
Po
84 M
-18-32-18-6
livermorium
Lv
115
116 M
At
-18-32-18-7
-18-32-18-8
Uus
117 NM
Lanthanoid Series
cerium
praeseodymium
Ce
58
M
Pr
59
M
thorium
protactinium
Th
90
M
Pa
91
Actinoid Series
M
neodymium
Nd
60
M
uranium
U
92
M
NG
Fe
26
M
25
2-8-13-1
NM
2-4
Al
5
Y
39
M
15
5
4
Sr
38
M
Fr
87
14
B
Groups 3 -11 = the transition metal family
Mg
2-8-2
potassium
13
2-3
12
He
2
2
2-2
sodium
19
4
helium
Group 17 = halogen family
promethium
Pm
61 M
neptunium
Np
93
M
samarium
Sm
62
M
plutonium
Pu
94
M
europium
gadolinium
americium
curium
Eu
63
M
Am
95
M
Gd
64
M
Cm
96
M
terbium
dysprosium
Dy
66 M
Ho
67
M
Er
68
M
Tm
69
M
Yb
70
M
Lu
71
M
berkelium
californium
einsteinium
fermium
mendelevium
nobelium
lawrencium
98
99
Tb
65
M
Bk
97
M
Cf
M
holmium
Es
M
erbium
Fm
100 M
thulium
Md
101 M
ytterbium
No
102 M
lutetium
Lr
103 M
Uuo
118
Names & Formulas of
Some Monatomic Anions


Name
Formula
Bromide
Br-1
Chloride
Cl-1
Fluoride
F-1
Iodide
I-1
Hydride
H-1
Oxide
O-2
Phosphide
P-3
Sulfide
S-2
Telluride
Te-2
Name

Densities & Boiling Points of Various Molecular Gases
& Gas Mixtures
Name
Density
Normal
(kg/m3) @
Boiling Point
STP
(C)
Air
1.29
-194.5

Names & Formulas of Polyatomic Ions
Formula
Name
Formula
Acetate
Ammonium (not ammonia)
C2H3O2-1
NH4+1
Hypochlorite
Iodate
ClO-1
IO3-1
Arsenate
Carbonate
Chlorate
Chlorite
Chromate
Cyanide
Dichromate
Hydrogen Carbonate
Hydronium
Hydroxide
AsO4-3
CO3-2
ClO3-1
ClO2-1
CrO4-2
CN-1
Cr2O7-2
HCO3-1
H3O+1
OH-1
Nitrate
Nitrite
Perchlorate
Peroxide
Permanganate
Phosphate
Sulfate
Sulfite
Thiocyanate
Thiosulfate
NO3-1
NO2-1
ClO4-1
O22MnO4-1
PO4-3
SO4-2
SO3-2
SCN-1
S2O3 -2
Names & Formulas of Common Ionic Compounds
Ammonia (NH3)
0.771
-33
Carbon Dioxide (CO2)
1.98
-78
Formula
Li2CO3
Na2B4O7
NaCl
NaI
Carbon Monoxide (CO)
1.25
-191
NaHCO3
Sodium hydrogen carbonate (baking soda)
Chlorine (Cl2)
3.21
-35
Helium (He)
0.18
-269
Na2CO3
NaClO
Sodium carbonate (soda ash)
Sodium hypochlorite (chlorine bleach)
Hydrogen (H2)
0.089
-253
Hydrogen Chloride (HCl)
1.64
-85
Hydrogen Sulfide (H2S)
1.45
-60.2
KNO3
KCl
Potassium nitrate (saltpeter, fertilizer)
Potassium chloride (table salt substitute)
Methane (CH4)
0.716
-161.6
CaCO3
Calcium carbonate (TUMS, chalk, limestone)
Neon (Ne)
0.9002
-246.1
CaO
Nitrogen (N2)
1.25
-196
Nitrogen monoxide (NO)
1.34
-152
CaSO4
TiO2
Fe2O3
Oxygen (O2)
1.43
-183
Ag2S
Ozone (O3)
2.141
-111.3
Phosgene (CCl2O)
4.248
7.5
Sulfur Dioxide (SO2)
2.92
-10.1
Na2CO3·1.5 H2O2
Al2O3
Name and Synonyms
Lithium carbonate
Sodium Borate (borax)
Sodium chloride (table salt)
Sodium iodide (a salt in iodized salt)
Sodium percarbonate (oxiclean)
Aluminum oxide (corundum, ruby, sapphire)
Calcium oxide
(lime)
Calcium sulfate (gypsum, dry wall)
Titanium dioxide or Titanium (IV) oxide (pigment)
Iron (III) oxide (one form of iron rust)
Silver sulfide (silver tarnish)
TABLE OF SELECTED PROPERITES OF SELECTED ELEMENTS

Table of Ionic Compounds & Solubility in Water
s = soluble (dissolves)
i = nearly insoluble
➏
acetate
bromide
carbonate
chloride
chromate
CH3COO-1
Br-1
CO3-2
Cl-1
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
ss
s
i
s
s
i
s
i
i
i
i
i
i
i
i
i
s
s
s
s
s
s
s
s
ss
s
i
s
(possibly a precipitate)
ss = slightly soluble
(possibly a precipitate)
Alkali (Li+1, Na+1, K+1) etc.
Aluminum (Al+3)
Ammonium (NH4)+1
Barium
(Ba+2)
Calcium
(Ca+2)
Copper II (Cu+2)
Iron II
(Fe+2)
Iron III
(Fe+3)
Lead II
(Pb+2)
Magnesium (Mg+2)
Silver
(Ag+1)
Zinc
(Zn+2)
hydroxide
iodide
nitrate
phosphate
sulfate
CrO4-2
hydrogen
carbonate
HCO3-1
OH-1
I-1
NO3-1
PO4-3
SO4-2
s
i
s
i
s
i
i
i
i
s
ss
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
s
ss
i
i
i
i
i
i
i
s
s
s
s
s
i
s
i
ss
s
i
s
s
s
s
s
s
s
s
s
s
s
s
s
s
i
s
i
i
i
i
i
i
i
i
i
s
s
s
s
ss
s
s
ss
ss
s
ss
s
Vapor Pressure of Water
at Various Temperatures
➐
Temp
(C)
0
3
5
8
10
12
14
15
16
18
19
20
21
22
23
24
Pressure
(kPa)
0.6
0.8
0.9
1.1
1.2
1.4
1.6
1.7
1.8
2.1
2.2
2.3
2.5
2.6
2.8
3.0
Temp
(C)
25
26
27
28
29
30
32
35
37
40
50
60
70
80
90
100
Pressure
(kPa)
3.2
3.4
3.6
3.8
4.0
4.2
4.8
5.6
6.3
7.4
12.3
19.9
31.2
47.3
70.1
101.3
➑
Standard temperature
Standard pressure
Some Important Constants
0.0 C
or 273 Kelvin
1 atmosphere or 101.3 kiloPascals
Melting / Freezing point of water
Normal Boiling point of water
Specific Heat of water
Heat of Fusion constant of water
Heat of Vaporization constant of water
Density of water @ 3.98 C
0.0 C
100 C
4.18 J/g•C
334 J/
2,226J/g
1.00 g/mL
Avogadro’s Number
Molar Volume at STP
6.02 x 1023 species
22.4 Liters
8.314 J/molK
Universal Gas Constant (R)
0.082057 atmL/molK
➒
st
1 Ionization Energy
(kJ/mol)
Electronegativity*
Table of First Ionization Energies & Electronegativity Values
Group
1
Group
2
Group
13
Group
14
Group
15
Group
16
Group
17
H
1312
2.2
Li
520
1.0
Na
496
0.9
K
419
0.8
Rb
403
0.8
Cs
376
0.8
Fr
393
0.7
Group
18
He
2372
-
Be
900
1.6
Mg
736
1.3
Ca
590
1.0
Sr
549
1.0
Ba
503
0.9
Ra
509
0.9
B
C
N
O
F
801
1086
1402
1314
1681
2.0
2.6
3.0
3.5
4.0
Al
Si
P
S
Cl
578
787
1012
1000
1251
1.6
1.9
2.2
2.6
3.2
Ga
Ge
As
Se
Br
579
762
944
941
1140
1.8
2.0
2.2
2.6
3.0
In
Sn
Sb
Te
I
558
709
831
869
1008
1.8
2.0
2.1
2.1
2.7
Tl
Pb
Bi
Po
At
589
716
703
812
926
2.0
2.3
2.0
2.0
2.2
*based upon a scale in which 4.0 is the maximum value
Ne
2081
Ar
1521
Kr
1351
Xe
1170
Rn
1037
-

Atom
Temperature
Density
Equations
Mass # = # of protons + # of neutrons
K = C + 273
density = mass
volume
where K is Kelvin Temperature
C is Celsius Temperature in degrees
Molar Density(g)STP = 1mol mass
22.4 L
Percent
Composition
% composition by mass = mass of the Part you want x 100
mass of the Whole thing
Percent Error
% error = | measured value – accepted value | x 100
accepted value
Calorimetry
q = mc∆T
q = mHf
q = mHv
Hf is the heat of fusion constant in J/g
Hv is the heat of vaporization constant in J/g
Combined Gas
Law
P1V1 = P2V2
T1
T2
Ideal Gas Law
PV = nRT
Molarity (M)
Titration
(Neutralization)
Moles
where q is energy in joules
m is mass in grams
c is specific heat in J/gram•C
∆T is change in temperature in C
where P is pressure
V is volume
T is Kelvin Temperature
where P is pressure in atmospheres or kPa
V is volume in Liters
T is temperature in Kelvin
R = 8.314 J/molK when kPa is used
0.082057 atmL/molK when atm is used
Molarity = moles of dissolved material
Liters of solution
(#H1+ ) (Macid)(Vacid) = (Mbase )(Vbase) (#OH1-)
moles =
grams of substance
mole mass of substance
where M is molarity and V is volume

Acid / Base Indicators & pH
Range / Color
Color Change
In That Range
Methyl Orange
3.2-4.4
Red (below 3.2)
orange
Yellow (above 4.4)
Bromothymol
6.0-7.6
Yellow (below 6.0)
Blue
green
Blue (above 7.6)
Phenolphthalein
8.2-10
Colorless (below 8.2)
(phth)
pink
Deep Pink (above 10)
Litmus
5.5-8.2
Red (below 5.5)
purple
Blue (above 8.2)
Bromcresol Green
3.8-5.4
Yellow (below 3.8)
green
Blue (above 5.4)
Thymol Blue
8.0-9.6
Yellow (below 8.0)
green
Blue (above 9.6)
Indicator


pH Scale
9
10
11
12
13
DRANO
8
TUMS
7
Baking soda
6
BASE
Egg white
5
Blood 7.3
4
Tap water
3
Black coffee
2
Orange juice
1
Vinegar
0
NEUTRAL
Pure water
ACID
14
Names & Formulas of Common
Arrhenius Acids
HBr(aq)
Hydrobromic acid
HF(aq)
Hydrofluoric acid
HCl(aq)
Hydrochloric acid
H2S(aq)
Hydrosulfuric acid
HNO3(aq)
Nitric acid
H2SO4(aq)
Sulfuric acid
H3PO4(aq)
Phosphoric acid
H2C2O4(aq)
Oxalic acid
HSO3NH2(aq)
Sulfamic acid
H2CO3(aq)
Carbonic acid
HC2H5O2(aq) or
Ethanoic acid
CH3COOH(aq)
(a.k.a. acetic acid)
Names & Formulas of Common
Arrhenius Bases
NH4OH(aq)
Ammonium hydroxide
(a.k.a. ammonia in
water)
Ba(OH)2(aq)
Barium hydroxide
Ca(OH)2(aq)
Calcium hydroxide
Mg(OH)2(aq)
Magnesium hydroxide
KOH(aq)
Potassium hydroxide
NaOH(aq)
Sodium hydroxide
Other names/types of acids
Amino acids (e.g. leucine, valine, serine...)
Ascorbic acid
Citric acid
Other names/types of bases
Amines (e.g. CH3NH2)
Carbonates (e.g. CaCO3, Na2CO3)
Hydrogen Carbonates (NaHCO3)

Various Standard & Qualitative Tests
A POSITIVE TEST …
Test for:
Test
oxygen gas
O2(g)
Flaming splint
causes the flame to flare up and to burn more brightly than before
oxygen gas
O2(g)
carbon dioxide gas
CO2(g)
Glowing splint
causes the glowing ember to re-light and to burn
Bubble gas into Ca(OH)2(aq)
produces a white precipitate (solid). Addition of more carbon dioxide reverses
the reaction
hydrogen gas
H2(g)
Flaming splint
in the presence of atmospheric oxygen, the hydrogen gas ignites, causing a
popping sound (like uncorking a champagne bottle)
metal (active)
React with acid
creates bubbles filled with hydrogen gas. Often the un-reacted metal will
darken in color.
water
H2O (l)
Blue Cobalt Chloride Paper
acid
Various indicators
causes a color change in selected indicators (see Table 11)
base
(hydroxide containing)
Various indicators
causes a color change in selected indicators (see Table 11)
carbonate
React with an acid
creates fizzing due to bubbles of carbon dioxide gas
monosaccharides
(reducing sugar)
Tollen’s test using
AgNO3(aq) + KOH(aq)
causes the precipitation/deposition of silver metal on glass
monosaccharides
(reducing sugar)
Benedict’s Solution
Causes the color of the Benedict’s solution to change from blue to yellow or
red
polysaccharides (starch)
React with a solution of iodine
protein
Biuret Test
turns a chemically treated blue paper a pinkish color
causes the color to change from red to blue/black
causes a color change from blue to violet or pink for small polypeptides

Reaction Type
Example
Comment(s)
Acid Base Neutralization
HNO3(aq) + KOH(aq)  H2O(l) + KCl(aq) + energy kJ
an acid
a base
water a salt
Titration
Saponification
C51H88O6(s) + 3 NaOH(aq)  3 CH3(CH2)14CO2Na(s) + C3H8O3
a fat
a base
a soap
glycerol (-ine)
Making soap
Complete Combustion
(of an organic compound)
CH4(g)
+
an organic
compound
Esterification
CH3COOH(aq) + CH3CH2OH(l)  CH3COOCH2CH3(aq) + H2O(l)
an organic acid
an alcohol
an ester
water
Nonmetal Oxide in Water
O2(g ) 
oxygen
CO2(g) + H2O(l) + energy kJ
carbon water
dioxide
CO2(g) + H2O(l)  H2CO3(aq)
carbon water
carbonic acid
dioxide
Metal Oxide in Water
Na2O(s) +
H2O(l)  2 NaOH
sodium oxide water
sodium hydroxide
Active Metal in Acid
2 Li(s) + 2 H2O(l)  2 LiOH(aq) + H2(g)
a metal water
a base
hydrogen gas
Carbonate in Acid
CaCO3(s) + 2 HCl(aq)  CaCl2(aq) + CO2(g) + H2O(l)
a carbonate an acid
a salt
carbon
water
dioxide
Burning
associated with flavorings
A nonmetal oxide in water
produces an acidic solution
associated with acid
precipitation and soda water
A metal oxide in water produces
a basic solution
A form of neutralization;
The old Volcano Reaction;
associated with the acidification
of lakes
Measurement
➊➏
Common units used in Chemistry
Unit
Abbreviation
Length
Mass
Volume
meter
gram
Liter
Pressure
Pascal
or
Atmosphere
m
g
L
or
3
dm (cubic decimeter*)
Pa
or
atm
*In 1964, the 12th General Conference on Weights and Measures voted on the equivalence and use of 1 L = 1 dm3
http://www.nist.gov/pml/wmd/pubs/upload/appc-13-hb44-final.pdf
Prefix
Prefixes and interpretations for commonly used units
Meaning
Example, using meter
Alternate Example, using meter
milli-
one-thousandth 1 millimeter = 1 meter
1,000
1 mL = 0.001 meter
cent-
one-hundredth
1centimeter = 1 meter
100
1 cm = 0.01 meter
deci-
one-tenth
1 decimeter = 1 Meter
10
1 dm = 0.1 meter
deka-
ten
1 dekameter = 10 meters
1 dam = 10 meters
hecto-
one hundred
1 hectometer = 100 meters
1 hm = 100 meters
one thousand
1 kilometer = 1,000 meters 1 kL = 1,000 meters
kilo-
http://physics.nist.gov/Pubs/SP811/sec06.html and
http://www.nist.gov/pml/wmd/pubs/upload/appc-13-hb44-final.pdf
❶➐
Organic Prefixes
# of carbons
Prefix
1
2
3
4
5
6
7
8
9
10
12
16
➊➑ The Hydrocarbons
Family
General Formula
Formula
Name
alkane
CnH2n+2
C4H10
butane
alkene
CnH2n
C4H8
1-butene
alkyne
CnH2n-2
C4H6
1-butyne
18
20
meth
eth
prop
pron: prōp
but
(pron like beaut-y)
pent
hex
hept
oct
non
dec
dodec
(laur-yl)
Hexadec
(cet-yl or myrist-ic)
octadec (stear-yl)
eicos (arachid-ic)
Examples
Structure
Other Views
H H H H
| |
| |
H—C—C—C—C—H
| |
| |
H H H H
H H
| |
H—C—C—C  C—H
| |
|
|
H H H
H
H H
| |
H—C—C—C  C—H
| |
H H
CH3CH2CCH
arene
(aromatic
hydrocarbon)
CnH2n-6
C6H6
benzene
note: the term
aromatic refers to
a closed ring with
C or N with
alternating double
bonds
where "n" equals the number of carbons in the longest (parent) chain
❶➒ Organic Compounds with Functional Groups
Class
Description
a
Examples of
molecular or
condensed formula
a
Alcohol
R-OH
(Monohydroxy)
1 (O-H) group
bonded to a carbon.
Soluble in water
(polar molecule)
a
C3H7OH
b
C4H9OH
Alcohol
(Glycol or
Dihydroxy)
Aldehyde
Ester
2 O-H groups (or OH
groups) bonded to
carbon. Water soluble
(polar molecule)
a product of an
alcohol & carboxylic
acid reaction.
Ketone
C3H6(OH)2
a
HCOH
b
CH3OOCCH3
a
CH3OOCCH3
b
C2H5OOCC2H5
O
||
R— C—R'
a carbonyl group on
an "interior" or nonterminal carbon
Carboxylic
Acid
(the most
common form
of organic acid)
Amine
(simple)
O
||
R—C—O-H
a carboxyl group
(COOH) bonded to a
carbon R-Group.
RNH
|
H
a derivative of NH3
At least one H is
replaced with an
organic group. A
weak base (B-L)
a
C3H6O
b
C6H12O
CH3COOH
b
C2H5COOH
a
b
(also called a
halocarbon)
R-X
a
2-propanone (acetone)
Halogen(s) {X} are
substituted onto a
hydrocarbon, by
removing hydrogen(s)
b
C3H6F2
H H H H
| |
| |
H—C—C—C—C—H
| |
| |
H OH H H
1,2-propanediol (propylene glycol)
H H H
| |
|
H—C—C—C—H
| |
|
H O-H O-H
b
ethanal (acetaldehyde)
H O
| ||
H—C—C—H
|
H
b
ethyl propanoate
H H
O H H
|
|
|| | |
H—C— C—O—C—C—C—H
| |
|
|
H H
H H
b
3-hexanone
H H H O H H
| | |
|| | |
H—C—C—C—C—C—C—H
| |
|
| |
H H H
H H
H O H
| || |
H—C—C—C—H
|
|
H
H
ethanoic acid (acetic acid)
b
propanoic acid
H H O
| | ||
H—C—C—C—O—H
| |
H H
b
phenylamine (aniline)
H O
| ||
H—C—C—O—H
|
H
a
1-propanamine (1-propylamine)
H H H
| |
|
HCCCNH
| |
| |
H H H H
C6H5NH2
C3H7Br
methanal (formaldehyde)
methyl ethanoate
H
O H
|
|| |
H—C—O—C—C—H
|
|
H
H
C3H7NH2
a
b
a
a
Halide
1,2-ethanediol (ethylene glycol)
1-bromopropane
Br H H
| |
|
H—C—C—C—H
| |
|
H H H
Example Name / Structure
2-butanol
O
||
H—C—H
a
a
b
H H
| |
H—C—C—H
| |
OH OH
a
O
||
R—C—H
A carbonyl group on
a terminal C with
carbon or hydrogen as
the "R" group
O
||
R—O—C—R'
C2H4(OH)2
b
1-propanol
H H H
| |
|
H—C—C—C—O-H
|
|
|
H H H
a
a
b
Example Name / Structure
NH
|
H
b
1,2-difluoropropane
H H F
| |
|
H—C—C—C—H
| |
|
H F H