Sun Moon Mars Venus Saturn Jupiter Mercury Symbols used in the 16 th and 17 th Century Gold Silver Iron Copper Lead Tin Mercury Alchemical Symbols used in the 15 th Century Fire ID: 702361
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Slide1
Chemical Symbols
Ancient Astronomical Symbols
Sun
Moon
Mars
Venus
Saturn
Jupiter
Mercury
Symbols used in the 16
th
and 17
th
Century
Gold
Silver
Iron
Copper
Lead
Tin
Mercury
Alchemical Symbols used in the 15
th
Century
Fire
Air
Earth
WaterSlide2
Chemical Symbols
Symbols used in the 18
th
Century
Antimony
Water
Sulfuric acid
Copper
Sulfur
Symbols used by John Dalton
Carbon
Hydrogen
Oxygen
Silver
Sulfur
Nitrogen
S
Lead
Mercury
Copper
C
L
Gold
Potassa
Soda
G
Water
Carbon dioxide
AlcoholSlide3
Origin of the Names of Elements
Title Number of Elements
Pre-chemical Names 10Names from celestial bodies 8Names from mythology / superstition 10Names from minerals / ores, other than geographical names 13
Names from colors 9Names from properties other than color 8Geographical names from the domicile or workplace of the discoverer(s) 13Geographical names from minerals / ores 10
Constructed names 16Names from persons 10 Slide4
Names and Symbols of Selected Elements
Name* Symbol Name* Symbol
Aluminum Al Lead (
plumbum
) PbArgon Ar Lithium LiBarium Ba Magnesium MgBoron B Mercury (hydrargyrum
) HgBromine Br Neon NeCadmium Cd Nickel Ni
Calcium Ca Nitrogen NCarbon C Oxygen OChlorine Cl Phosphorus P
Cobalt Co Potassium (kalium) KCopper (
cuprum) Cu Silicon SiFluorine F Silver (
argentum) AgGold (aurum) Au Sodium (natrum) Na
Helium He Strontium SrHydrogen H Sulfur SIodine I Tin (stannum) SnIron (ferrum)
Fe Zinc Zn
*Names given in parentheses are ancient Latin or Greek words from which the symbols are derived.Slide5
Map of Elements DiscoveredSlide6
Several Synthetic Elements
Man-made
Bk = BerkeliumCf = CaliforniumAm = Americium
Synthetic
All made by nuclear bombardment
at Berkeley, California, U.S.A.Slide7
How to Organize Elements… Periodic Table DesignsSlide8
Dutch Periodic Table
106
107
108
109
110
111
112
113
114
115
116
117
118Slide9
“Mayan”
Periodic
TableSlide10Slide11
Stowe’s Periodic TableSlide12Slide13
Benfey’s Periodic TableSlide14
Law of Triads
Name
Atomic
Mass
Name
Atomic
Mass
Name
Atomic
Mass
Calcium 40Barium 137Average 88.5
Strontium 87.6
Chlorine 35.5Iodine 127
Average 81.3Bromine 79.9
Sulfur 32Tellurium 127.5
Average 79.8
Selenium 79.2
Johann Döbereiner ~1817
Elements could be classified into groups of three, or triads
based on trends in physical properties
such as density, melting point, and atomic mass were observed.Slide15
Newlands Law of Octaves
Newlands Law of Octaves
1
Li
Na
K
John Newlands
~1863
2
BeMg3
BAl4CSi
5
NP
6O
S
7F
Cl
Arranged the 62 known elements into groups of seven according
to
increasing atomic mass
and
proposed that an
eighth column
would then repeat the properties
of the first element in the previous group.Slide16
Dmitri Mendeleev
Russian
Invented periodic tableOrganized elements by properties
Arranged elements by atomic mass
Predicted existence of several unknown elementsNoted discrepancies
with atomic mass
Dmitri MendeleevSlide17
Mendeleev’s Early Periodic Table
GRUPPE I GRUPPE II GRUPPE III GRUPPE IV GRUPPE V GRUPPE VI GRUPPE VII GRUPPE VIII
___ ___ ___ ___
RH
4
RH
3
RH2 RH
R2O RO R2O
3 RO2 R2O5 RO3 R2O
7 RO4 REIHEN
1
2 3 4
5 6 7
8 910
1112
From
Annalen der Chemie und Pharmacie, VIII, Supplementary Volume for 1872, p. 151.
H = 1
Li = 7 Be = 9.4 B = 11 C = 12 N = 14 O = 16 F = 19
Na = 23 Mg = 24 Al = 27.3 Si = 28 P = 31 S = 32 Cl = 35.5
K = 39 Ca = 40 __ = 44 Ti = 48 V = 51 Cr = 52 Mn = 55 Fe = 56, Co = 59,
Ni = 59, Cu = 63
(Cu = 63) Zn = 65 __ = 68 __ = 72 As = 75 Se = 78 Br = 80
Rb = 85 Sr = 87 ? Yt = 88 Zr = 90 Nb = 94 Mo = 96 __ = 100 Ru = 104, Rh = 104, Pd = 106, Ag = 108
(Ag = 108) Cd = 112 In = 113 Sn = 118 Sb = 122 Te = 125 J = 127
Cs = 133 Ba = 137 ? Di = 138 ? Ce = 140 __ __ __ __ __ __ __
( __ ) __ __ __ __ __ __
__ __ ? Er = 178 ? La = 180 Ta = 182 W = 184 __ Os = 195, Ir = 197,
Pt = 198, Au = 199
(Au = 199) Hg = 200 Tl= 204 Pb = 207 Bi = 208 __ __
__ __ __ Th = 231 __ U = 240 __ __ __ __ __
TABELLE II
?
?
?Slide18
Elements Properties are Predicted
Property
Mendeleev’s
Predictions
in 1871
Observed
Properties
Molar Mass
Oxide formula
Density of oxide
Solubility of oxide
Scandium (Discovered in 1877)
44 g
M
2
O
3
3.5 g / ml
Dissolves in acids
43.7 g
Sc
2
O
3
3.86 g / ml
Dissolves in acids
Molar mass
Density of metal
Melting temperature
Oxide formula
Solubility of oxide
Gallium (Discovered in 1875)
68 g
6.0 g / ml
Low
M
2
O
3
Dissolves in ammonia solution
69.4 g
5.96 g / ml
30
0
C
Ga
2
O
3
Dissolves in ammonia
Molar mass
Density of metal
Color of metal
Melting temperature
Oxide formula
Density of oxide
Chloride formula
Density of chloride
Boiling temperature
of chloride
Germanium (Discovered in 1886)
72 g
5.5 g / ml
Dark gray
High
MO
2
4.7 g / ml
MCl
4
1.9 g / ml
Below 100
o
C
71.9 g
5.47 g / ml
Grayish, white
900
0
C
GeO
2
4.70 g / ml
GeCl
4
1.89 g / ml
86
0
C
O’Connor Davis, MacNab, McClellan,
CHEMISTRY Experiments and Principles
1982, page 119, Slide19
Modern Periodic Table
Determined the
atomic numbers of elements
from their
X-ray spectra (1914)Resolved discrepancies in Mendeleev’s arrangement.
Arranged elements by
increasing atomic number
Henry G.J. Moseley
1887 - 1915Slide20
Describing the Periodic Table
Periodic Law
– the properties of elements
repeat in a predictable pattern.
Periods are
ROWs; Numbered from 1 to 7.
NUMBER the PERIODS on your periodic tables
Group/Family are COLUMNs;
Numbered from 1 to 18 (share similar chemical properties),
NUMBER the GROUPS on your periodic tablesMain Group Elements:
Groups 1, 2, &
13 through 18
; “s” & “p” blockSlide21
Diatomic Elements
`
H
2
N
2
O
2
F
2
Cl
2
Br
2
I
2
Tl
At
S
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Rb
Sr
Y
Xe
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Pb
Bi
Po
Al
Si
P
4
B
C
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
S
8
Tl
Diatomic Molecules
Unable to stand alone; bonded to their identical twin
Sulfur
= 8 ; Phosphorus =
4
Sharks 8 Penguins 4 lunchSlide22
StationsSlide23
Metallic Characteristics
metallic character increases
nonmetallic character increases
metallic character increases
nonmetallic character increasesSlide24
Metals, Nonmetals, & Metalloids
1
2
3
4
5
6
7
Metals
Metalloids
Zumdahl, Zumdahl, DeCoste,
World of Chemistry
2002, page 349
Nonmetals
Pattern:
Metals = blank
Metalliods = diagonal
Nonmetals = dotSlide25
Properties of Metals
Good conductors
of heat and electricity.Lustrous
Ductile (stretched into thin wires)Malleable
(pounded into thin sheets)Chemical property: Reaction with water which
results in corrosionChemical Reactions:
lose electrons to form
positively charged ionsAll are solids except for mercurySlide26
Non-Metals Properties
Poor Conductors
of heat and electricity.
DullNot ductile Not malleable
Solid non-metals are brittleCan be gases, liquids or solids.Tend to gain electrons to form negatively charged ions
Share electrons in reaction with other non-metals.
SulfurSlide27
Metalloids Properties
Metalloids (metal-like)
Exhibit properties of both metals and non-metals
Solids that can be shiny or dull.
Conduct heat and electricity better than non-metals but not as well as metals.Ductile and malleable.
SiliconSlide28
Hydrogen
is in a
class of its own.only needs 2 electrons to complete its valence shell.
Characteristics Gas
at room temperature. FlammableSlide29
Alkali Metals
Most REACTIVE metals.
Characteristics Soft (Clay consistency)
Dull Silver color Low Density Low Melting Point
React violently with water React w/ halogens to form saltns1
valence electron configurationSlide30
Alkaline Earth Metals
Characteristics
Soft
Shiny silver color Low Density Found naturally as a compound
Glow different colors “
ns2” valence electron configurationSlide31
Transition Metals
“d” block
Column 11: “Coinage metals” contains Cu, Ag & AuSlide32
Transition Metals
usually
brightly colored often used to
color paints.Characteristics
High Density High Melting/Boiling Pt Good Catalysts
Hard, Tough & Strong
Multiple oxidation
(charge) statesForm compounds called oxides
Group 11 know as “coinage metals” contains Cu, Ag & AuSlide33
Group 13: Boron Family
3 valence electrons
forms +3 charged ions
.Family includes a metalloid (boron), and the rest are metals.Family includes the most abundant metal in the earth’s crust; aluminum.
Highly reactive & form stable compounds with oxygen“
ns2np1
” valence electron configurationSlide34
Group 14:
Carbon Family
4 valence electrons forms 3 oxidation states
-4, +4 & +2 (loss of two np2
gives a filled ns2 subshell)Family includes a non-metal, metalloids, and metals.
Carbon is called the “basis of life.”
“
ns2np2
” valence-electron configuration.Slide35
Group 15:
Nitrogen (Pnicogen
) Family
5 valence electrons forms 3 oxidation states -3, +5 & +3
(three np electrons lost to give a filled ns2 subshell)Family includes non-metals, metalloids and metals
Nitrogen makes up 79% of our atmosphere.
“ns
2np3” valence electron configurationSlide36
Group 16:
Oxygen (Chalcogens
) Family
6 valence electrons forms 3 oxidation states
-2, +6 & +4 (four np electrons lost give filled ns2 subshell)
Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements.
“
ns2np
4” valence-electron configuration
O
8
S
16
Se
34
Te
52
Po
84Slide37
Group 17: Halogen (Salt Makers)
Family
Most active non-metals. - never found free in natureOnly group in all 3 states of matter
React with alkali metals to form SALTS
High electronegativityNon-metal qualities – dull, brittle, non-conductor“ns2np5” valence electron configurationSlide38
Group 18: Noble Gases
Characteristics
Inert (Non-reactive) due to their filled octet
Colorless gas Odorless Tasteless
Nonflammable Non-metal qualities – dull, brittle, non-conductorFound in small amounts in the earth's atmosphere.
“ns2
np6” valence electron configurationSlide39Slide40Slide41
Rare Earth (Inner Transition) Elements
Rare earth elements
not particularly rare but long & tedious processes were required to purify the metals from their oxides prior to 1945
One element of the lanthanide series & most of the elements in the actinide series are called
trans-uranium, which means synthetic or man-made.
Characteristics
High melting points Reactivity varies Usually bonded to non-metals
Tarnish readily in air High electrical conductivity