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Atoms,
Elements,
The Periodic Table
&
Nomenclature
Democritus & Atomism
Developed a theory called
“Atomism.” This theory was
originally envisioned by his
teacher Leucippus to account
for the materialistic nature of
the world.
“The laughing philosopher”
c. 460 BCE (Abdera)
The Father of Atomism
The atomists held that
everything tangible is composed
of small indivisible bodies
which they called “atoms” and
that these atoms move about
in an infinite void space.
Antoine Lavoisier
Defined a chemical “element”
as a substance that cannot be
decomposed into simpler
substances by chemical means.
Created a table of 33 of
the then known elements.
1743 (Paris) – 1794 (Paris)
“The Father of
Modern Chemistry”
Grouped the elements into
four categories based on
their physical and chemical
properties. These categories
were gases, nonmetals,
metals, and earths.
Jöns Jakob Berzelius
Developed a table of atomic
weights in 1828.
Introduced the use of letters
as symbols for the elements.
Determined the atomic weight
of 43 elements.
First to isolate pure calcium,
barium, strontium, silicon,
titanium, and zirconium.
Swedish chemist
1779 – 1848
Discovered selenium, thorium,
and cesium.
Johann Döbereiner
In 1817, he proposed “triads,”
or groups of three elements
with similar properties. He
later published these ideas in
1829.
Examples of triads:
lithium, sodium, & potassium;
calcium, strontium, & barium;
chlorine, bromine, & iodine.
Discovered that the relative
atomic mass of the middle
element in each triad was
close to the average of the
relative atomic masses of the
other two elements.
German Scientist
1780–1849
John Newlands
Proposed the “Law of Octaves.”
In 1863, he arranged the 62 known
elements in order of their atomic
weights and observed similarities
between the first and ninth and
second and tenth elements, etc.
1837 (London) – 1898
H1
Li 2
Be 3
B4
C5
N6
O7
F8
Na 9
Mg 10
Al 11
Si 12
P 13
S 14
Cl 15
K 16
Ca 17
Cr 19
Ti 18
Mn 20
Fe 21
Newlands’ Periodic Table
Co & Ni 22
Cu 23
Zn 24
Y 25
In 26
As 27
Se 28
Br 29
Rb 30
Sr 31
Ce & La 33
Zr 32
Bi & Mo 34
Rh & Ru 35
Pd 36
Ag 37
Cd 38
U 40
Sn 39
Sb 41
Te 43
I 42
Cs 44
Ba & V 45
Ta 46
W 47
Nb 48
Au 49
Pt & Ir 50
Os 51
Hg 52
Tl 53
Pb 54
Bi 55
Th 56
Lothar Meyer
In 1869, he compiled
a periodic table of
56 elements based
on the “periodicity”
of their properties
(e.g., molar volumes)
when arranged in
order of increasing
atomic weight.
German chemist
1830 – 1895
Meyer’s Periodic Table for Molar Volume
Dmitri Mendeleev
“Father of the Modern
Periodic Table”
In 1869, he produced a
table based on the atomic
weights.
Russian Physicist and Chemist
1834 (Tobolsk, Siberia ) –
1907 (St. Petersburg)
He actually arranged them
such that elements with
similar properties were
located in the table
underneath each other;
thus, making it easier to
observe the “periodicity.”
Mendeleev’s Periodic Table
1
2
3
4
5
6
Periods are shown as horizontal rows.
All of the elements in a given period have
the same number of atomic shells.
Groups or families are shown as vertical columns.
There are 18 groups in the periodic table.
1
7
2
3 4
8
5 6
Elements in a group have similar electronic configurations
for their valence shell electrons. This is why elements in a
group have similar chemical properties.
William Ramsay
Discovered argon in
1894.
Discovered the noble
gases which formed a
new group in the
periodic table.
Awarded the Nobel
Prize for Chemistry
in 1904.
1852 (Glasgow) –
1916 (High Wycombe)
Henry Moseley
In 1914, he determined the
atomic number of each of
the elements
by x-ray scattering.
He modified the
“periodic law” to indicate
that the properties of the
elements vary periodically
with their atomic number
rather than atomic weight.
English physicist
1887 – 1915
Henry Moseley
He pointed out the
existence of missing
elements in the periodic
table for atomic
numbers 43, 61, 72,
and 75. Each of these
elements, Tc, Pm, Hf,
and Re were eventually
discovered.
He also showed that there are no elements lighter than
hydrogen (Z = 1) and that there is no possibility for
elements between hydrogen and helium (Z = 2).
Both possibilities had been advanced, with some proposals
demanding three elements between H and He.
Glenn Seaborg
Starting in 1940, he
synthesized several of the
transuranic elements that
occur after uranium in the
periodic table.
He won the Nobel Prize for
Chemistry in 1951 for the
discovery of plutonium.
American chemist
1912 – 1999
Seaborgium (element 106)
is named after him.
Periodic Table
Transition metals
Lanthanide Series
Actinide Series
Nomenclature Rules
Rules for naming three classes of compounds:
ionic compounds, binary covalent compounds & acids.
What type of compound is it?
IONIC COMPOUND:
Composed of cations
(metals or polyatomic
ions) and anions
(nonmetals or
polyatomic ions).
TYPE I:
Only one
type of
cation is
observed.
COVALENT COMPOUND:
Nonionic – not composed of
cations & anions.
Generally, only nonmetals
are present.
TYPE II:
More than
one type of
cation is
observed.
TYPE III:
Covalent,
nonionic.
ACID:
Produces H+ in water.
Typically the
hydrogen cation is
written first in the
chemical formula.
ACIDS:
Anion does
not contain
oxygen.
OXYACIDS:
Anion does
contain
oxygen.
Rules for Naming Ionic Compounds
1.) Determine whether or not the compound is ionic.
How do you know the compound is ionic in the first place?
a.) If the compound contains a metal, then it is
most likely an ionic compound. Metals readily lose
electrons to form positive ions, called cations. Ionic
compounds almost always contain a metal as a cation
and a nonmetal as an anion.
b.) However, not all ionic compounds will contain a
metal cation. The cation could be a polyatomic ions,
such as NH4+.
Rules for Naming Ionic Compounds
2.) Determine whether there is only one type of cation
possible (Type I) or whether there are several
cations possible (Type II).
a.) If the cation is a polyatomic ion (e.g., ammonium,
NH4+), then there is only one possible charge and
so it is a type I compound.
b.) If the cation is a metal, determine if it forms only
one type of cation.
Alkali metals (Group 1A)
+1 cation
Alkaline earth metals (Group 2A)
+2 cation
Transition metals (Group 1-8B)
often form more than one type of cation.
Rules for Naming Type I Compounds
1.) The cation is named first and the anion is named
second.
2.) The name of the cation is the same as the name
of the element. So both the element Mg and the cation
Mg2+ are called magnesium.
(Note: For polyatomic cations, you must memorize the names. )
3.) The anion is named by taking the root name of
the element and adding the suffix -ide. For example,
F is an atom of fluorine and F- is the anion fluoride.
(Note: For polyatomic anions, you must memorize the names. )
So MgF2 would be magnesium fluoride.
Rules for Naming Type I Compounds
with polyatomic ions
Polyatomic ions then resemble molecules in that they
contain at least two atoms bound together in a definite
arrangement.
The steps for naming compounds with polyatomic ions:
1.) The cation is listed first and the anion second.
2.) The polyatomic ion names must be memorized.
3.) No extra prefixes or suffixes are added.
Table of Polyatomic Ions
Symbol (root)
1
2
3
4
5
6
7
8
9
10
Cl (chlor)
Br (brom)
I (iod)
N (nitr)
C (carbon)
S (sulf)
Se (selen)
P (phosph)
As (Arsen)
Cr (Chrom)
per-root-ate
-
ClO4
BrO4 IO4 XXX
XXX
*
XXX
XXX
XXX
dichromate
2-
Cr2O7
MnO4-
11
12
Mn (mangan)
Ti (titan)
13
14
15
16
Acetate**
Formate**
Oxalate**
Cyanate
XXX
17
18
Thiocyanate***
Thiosulfate***
XXX
XXX
XXX
XXX
XXX
XXX
root-ate
-
root-ite
hypo-root-ite
ClO3
BrO3 IO3 NO3 CO3 2SO4 2SeO4 2PO4 3AsO4 3-
ClO2
BrO2 IO2 NO2 -
ClO BrO IO -
XXX
SO3 2SeO3 2PO3 3AsO3 3-
XXX
CrO4 2-
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
XXX
TiO3
2-
C2H3O2 CHO2 C2O4 2NCO SCN S2O3 2-
-
XXX
XXX
XXX
XXX
XXX
* Sulfur has two anions that are often referred to as persulfate. They are peroxomonosulfate (or
peroxymonosulfate) ion, SO5 2- and peroxodisulfate (or peroxydisulfate) ion, S2O8 2-.
**The organic anions.
*** Thiocyanate and thiosulfate are formed by substituting a sulfur for an oxygen into the cyanate and
sulfate ions.
Nomenclature Mnemonic for Remembering “ates”
Nick the Camel Ate a Clam Supper and Crepes (for dessert) in Phoenix
Nomenclature Mnemonic for Remembering “ates”
Nick the Camel Ate a Clam Supper and Crepes (for dessert) in Phoenix
Consonants = Vowels =
Oxygen
Charge
Nick = Nitrate
Camel = Carbonate
Clam = Chlorate
3
3
3
-1
-2
-1
(Note: Bromate and Iodate are the same as Chlorate.)
Supper = Sulfate
Crepes = chromate
Phoenix = Phosphate
4
4
4
-2
-2
-3
Polyatomic
Ion
NO3 –
CO3 2ClO3 SO4 2CrO4 2PO4 3-
Rules for Naming Type II Compounds
Additionally for Type II Compounds:
4.) Use a roman numeral after the cation to indicate the
ionic charge of that cation.
So FeO would be called iron(II) oxide since the cation
is Fe2+ and Fe2O3 would be iron(III) oxide since the cation
is Fe3+.
5.) Alternatively, when using traditional names atoms
whose valence numbers vary, you add the suffix –ous to
the one with the lower valence state and –ic to the one
with the higher valence state.
So FeO would be called ferrous oxide since the cation
is Fe2+ and Fe2O3 would be ferric oxide since the cation is
Fe3+.
Table of Type II Compounds
IUPAC
copper (I) & copper (II)
Root
cupr-
Traditional
-ous
Cu+
-ic____
Cu 2+
gold (I) & gold (III)
aur-
Au+
Au3+
mercury (I) & mercury (II)
mercur-
Hg2 2+
Hg
chromium (II) & chromium (III)
chrom-
Cr2+
Cr3+
manganese (II) & manganese (III)
mangan-
Mn2+
Mn3+
iron (II) & iron (III)
ferr-
Fe2+
Fe3+
cobalt (II) & cobalt (III)
cobalt-
Co2+
Co3+
nickel(II) & nickel (III)
nickel-
Ni2+
Ni3+
tin (II) & tin (IV)
stann-
Sn2+
Sn4+
lead (II) & lead (IV)
plumb-
Pb2+
Pb4+
cerium (III) & cerium (IV)
cer-
Ce
Ce4+
arsenic (III) & arsenic (V)
arsen-
As3+
As5+
antimony (III) & antimony (V)
antimon-
Sb3+
Sb5+
bismuth (III) & bismuth (V)
bismuth-
Bi3+
Bi5+
3+
2+
Rules for Naming Binary Covalent Compounds
How do you recognize that something is a binary covalent
compound (versus an ionic compound)?
1.) If a compound contains only nonmetals (no metals),
then you can be reasonably sure that it is a covalent
compound.
Note: Some exceptions would be compounds that
contain polyatomic ions.
For example, ammonium bromide NH4Br and ammonium
sulfate (NH4)2SO4 are ionic compounds even though
they contain only nonmetals.
Type III Compounds: Binary Covalent Compounds
1.) The first element in the compound is named first
using the name of the element.
2.) The second element is named as though it were an
anion (the root name + suffix -ide); even though, we
know there are no anions in a covalent compound.
3.) Prefixes are used to denote the numbers of each
atom present. Since there are no formal charges on the
atoms in covalent compounds, it is more difficult to
predict the proportions that the atoms combine in.
(Note: the prefix mono is never used with the first
element).
Type III Compounds: Binary Covalent Compounds
Examples of binary covalent compounds include water (H2O), carbon monoxide
(CO), and carbon dioxide CO2.
Prefix
monoditritetrapentahexaheptaoctanonadeca-
meaning
one
two
three
four
five
six
seven
eight
nine
ten
The naming convention for binary covalent compounds is as follows:
(prefix)-nonmetal + (prefix)-nonmetal root + "-ide.
Try naming the compound P4O6.
Rules for Naming Simple Acids and Oxyacids
How do we determine if something is an acid?
The acids that we will be concerned with naming are really just a
special class of ionic compounds where the cation is always H+.
Recall that cations are written first in ionic formulas. So if the
formula has hydrogen written first, then this usually means that
the hydrogen is an H+ cation and that the compound is an acid.
When dissolved in water, acids produce H+ ions. These are also
called protons, because when the electron is removed from a
neutral hydrogen atom, it leaves behind one proton.
If the counterion (the anion) to H+ in the acid is a polyatomic ion
that contains oxygen (like NO2- or PO43-), the acid is called an
oxyacid. If the anion does not contain oxygen (like F- or CN-),
then a different set of rules are used for naming the acid.
Binary acids are binary compounds that contain a hydrogen atom
and either a halogen (F, Cl, Br, I) or sulfur (S). It is important
to note that nitrogen, phosphorus, and oxygen do not form binary
acids with hydrogen.
The naming convention for binary acids is as follows:
“Hydro-” + nonmetal root + “-ic” + “acid”
The nonmetal roots are determined as follows. For the halogens,
simply remove the “ine” and for sulfur remove the “ur”. Thus,
the roots for fluorine, chlorine, bromine and iodine are fluor-,
chlor-, brom-, and iod- ; and for sulfur, sulf- .
So to determine the name for HCl:
hydro + chlor + ic + acid → hydrochloric acid
If the acid is in a gaseous form or an anhydrous form, the "-ic"
is replaced by "-ide" and the "acid" suffix is removed.
So, acids are formed by adding protons to atoms or radicals with
negative valence numbers. The names of acids that do not
contain oxygen are formed like those of binary acids by adding
the prefix hydro- to the root name for the element and adding
the suffix –ic and the word “acid”.
Formula
HF
HCl
HBr
HI
HCN
H2S
HN3
Acid Name_____
hydrofluoric acid
hydrochloric acid
hydrobromic acid
hydriodic acid
hydrocyanic acid
hydrosulfuric acid
hydrazoic acid
If only one type of oxygen acid is formed, then the name is that of the
characteristic element plus the suffix –ic and the word acid.
Formula
Acid Name___
H3BO3
boric acid
H2CO3
carbonic acid
H4SiO4
silicic acid
Acids formed from polyatomic ions have a naming system similar to
that of the polyatomic ions themselves. The difference being that for
“-ate” we substitute “-ic” and for “-ite” we substitute “ous” and
add the word acid.
For example, hypochlor-ite then becomes hypochlorous acid; and
perchlor-ate becomes perchloric acid.
Ion
Name
ClOClO2 ClO3 ClO4 -
Ion name
Acid Formula
hypochlorite
chlorite
chlorate
perchlorate
HClO
HClO2
HClO3
HClO4
Acid
hypochlorous acid
chlorous acid
chloric acid
perchloric acid
Note: The number of hydrogens added to the polyatomic ion is equal
to the charge on the cation.
Try naming the acids formed by nitrite and nitrate ions, NO2
respectively.
–
and NO3 -,
Organic Compounds
Organic compounds contain carbon.
All other compounds are defined as inorganic.
However, for the sake of convenience, some carbon
compounds are considered inorganic:
carbon monoxide (CO),
carbon dioxide (CO2),
carbon disulfide (CS2),
and those containing the anions:
cyanide (CN-),
carbonate (CO3 2-)
bicarbonate (HCO3-)
Organic Compounds
The alkanes consist only of carbon and hydrogen held together by single bonds.
The first four alkanes have common names. The higher ones have names
reflecting the Greek/Latin prefixes used in the covalent naming system.
Organic Compounds
CH4
C2H6
C3H8
C4H10
C5H12
C6H14
C7H16
C8H18
C9H20
C10H22
Names
methane
ethane
propane
butane
pentane
hexane
heptane
octane
nonane
decane
The alkenes have a double bond between two of the carbons. Every double
bonded carbon can only form two other bonds. So there are two less hydrogens
for every corresponding alkene. The alkynes have a triple bond between two of
the carbons. So every triple-bonded carbon can only form one other bond.
Listen here! Y’all know…
I Might Pass Maybe 0002
https://www.youtube.com/watch?v=WRlGwnxs-pM
Remember that “Ate Beats Ite!”…
…and hydroxide!
OH
-
Chemistry Song (to the tune of I Will Follow You Into the Dark by Death Cab for Cutie)
https://www.youtube.com/watch?v=pBxIGmlqr-s
For February 3-5
Read: The Statistical Analysis of Zinc Washers – Text pp 53-76
Due: Nomenclature – Packet pp 53-67 (pp 55-67 extra credit)
Dimensional Analysis 1 – Text pp 15-24
Problems 1, 3, 8, 11, 14, 15, 17, 19, 20, 21 & 22
Do not apply rules of significant figures.
Must show work to receive credit.
Significant Figures – Text pp41-2 & 51-52
Problem Set 1 & 2 – Do all problems.