The%20Periodic%20Table%20and%20Naming%20Simple%20Compounds

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The Periodic Table and Naming Simple Compounds
Lecture 6

• Chemistry 142 B
• James B. Callis, Instructor
• Autumn Quarter, 2004

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Classification of the Elements

• Most of the elements are metals - metallic
  luster, ability to conduct electricity and heat,
  and malleability.
• The remaining elements are classified as
  nonmetals - no luster, poor conductors of
  electricity and heat and brittleness.

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Sub-Classes of Metals

• Alkali metals - (lithium, sodium, potassium,
  rubidium and cesium) - soft, low melting points,
  react with water to liberate hydrogen, form 11
  compounds with chlorine.
• Alkaline earths - (beryllium, magnesium, calcium,
  strontium, barium and radium) - react in a 12
  ratio with chlorine.
• Transition metals - (e.g. iron, copper, silver,
  gold, tungsten and cobalt) - structural metals
• Metalloids - (antimony, arsenic, boron, silicon
  and tellurium) - intermediate between metals and
  nonmetals.

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Non-Metals

• Chalcogens - (oxygen, sulfur, selenium and
  tellurium) - form 11 compounds with
  alkaline-earths, but 21 compounds with
  alkali-metals.
• Halogens - (fluorine, chlorine, bromine and
  iodine) - highly reactive and form 11 compounds
  with alkali-metals.
• Noble gases - (helium, neon, argon, krypton,
  radon) - virtually inert to chemical reactions.

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Periodic Variation

• When the properties of the elements are plotted
  against atomic number, we observe a periodic
  variation in their properties.
• The boundaries of the periods seem to be marked
  by the appearance of the noble gases at 2, 10,
  18, 36, 54 and 86 amu.
• The variations in both melting point and atomic
  radius seem to correlate (inversely).
• The different element classifications also appear
  cyclically in this periodic variation.

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The Periodic Table

• A two dimensional classification scheme for the
  elements. The columns or groups arrange the
  elements by chemical classification, as discussed
  above. The chemical variation across the rows or
  periods reflect the cyclic variation exhibited in
  the graphs above.
• The periodic table is not only an organizing
  principle, but it has (had) predictive power as
  well.
• As valuable as the periodic table is, the
  explanation of its organization was not obvious.
  It was not until the advent of quantum mechanics
  that the electronic structure of the atoms could
  be used to explain the periodic variation in
  properties.

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Groups in the Periodic Table
Main Group Elements (Vertical Groups) Group
IA - Alkali Metals Group IIA - Alkaline Earth
Metals Group IIIA - Boron Family Group
IVA - Carbon Family Group VA - Nitrogen
Family Group VIA - Oxygen Family (Calcogens)
Group VIIA - Halogens Group VIIIA - Noble
Gases Other Groups ( Vertical and Horizontal
Groups) Group IB - 8B - Transition Metals Period
6 Group - Lanthanides (Rare Earth
Elements) Period 7 Group - Actinides
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The Periodic Table of the Elements
H
He
O
N
C
B
Li
Be
Ne
F
S
P
Si
Al
Na
Mg
Ar
Cl
Se
As
Ge
Ga
Zn
Cu
Ni
Co
Fe
Mn
Cr
V
Ti
Sc
K
Ca
Kr
Br
Te
Sb
Sn
In
Cd
Ag
Pd
Rh
Ru
Tc
Mo
Nb
Zr
Y
Rb
Sr
Xe
I
Po
Bi
Pb
Tl
Hg
Au
Pt
Ir
Os
Re
W
Ta
Hf
La
Cs
Ba
Rn
At
Ac
Fr
Ra
Rf
Sg
Du
Bo
Ha
Me
The Halogens
The Alkali Metals
The Alkaline Earth Metals
The Noble Gases
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The Periodic Table of the Elements
H
He
Li
Be
F
Ne
B
C
N
O
Na
Mg
Ar
Cl
Al
Si
P
S
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Br
Kr
Ga
Ge
As
Se
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Xe
I
In
Sn
Sb
Te
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Rn
At
Tl
Pb
Bi
Po
Fr
Ra
Ac
Rf
Du
Sg
Bo
Ha
Me
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
Boron family
Nitrogen family
Carbon Family
Oxygen Family
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The Periodic Table of the Elements
H
He
O
N
C
B
F
Ne
Li
Be
S
P
Si
Al
Cl
Ar
Na
Mg
Se
As
Ge
Ga
Br
Kr
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Te
Sb
Sn
In
I
Xe
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Po
Bi
Pb
Tl
At
Rn
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Fr
Ra
Ac
Rf
Sg
Ha
Du
Bo
Me
The Transition Metals
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
Lanthanides The Rare Earth Elements
The Actinides
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Naming Binary Compounds (Type I Ionic)

• The cation is always named first and the anion
  second.
• A monatomic cation takes its name from the name
  of the element, e.g. Na is called sodium in the
  names of compounds containing this ion.
• A monatomic anion is named by taking the first
  part of the element and adding ide, e.g. Cl- is
  chloride.

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Type I
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Problem 6-1 Give the Name and Chemical Formulas
of the Compounds formed from the following pairs
of Elements
a) Sodium and Oxygen
Na2O sodium oxide b) Zinc and
Chlorine c) Calcium and Fluorine
CaF2 calcium fluoride d)
Strontium and Nitrogen e) Hydrogen and Iodine
HI hydrogen
iodide f) Scandium and Sulfur
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Naming Binary Compounds (Type II Ionic)

• Applies to cations that can take on alternate
  charge states
• Using the principle of charge balance determine
  the cation charge.
• Include in the cation name a Roman numeral
  indicating the charge.

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Type II
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Determining Names and Formulas of Ionic
Compounds of Elements That Form More
Than One Ion.
Problem 6-2 Give the systematic names for the
formulas or the formulas for the names of the
following compounds.
a) iron (III) sulfide - Fe is 3, and S is 2-
therefore the compound is
Fe2S3 b)
CoF2 - c) stannic oxide - Stannic is the
common name for Tin (IV), Sn4, the
oxide ion is O2-, therefore the formula
of the compound is
SnO2 d) NiCl3 -
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Ionic Compounds with Polyatomic Ions

• Polyatomic ions are assigned special names that
  must be memorized.
• Special rules apply to anions that contain an
  atom of a given element and different numbers of
  oxygen atoms. These anions are called oxyanions.

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Start learning these boldface ones.
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Rules for Families of Oxoanions
Families with Two Oxoanions
The ion with more O atoms takes the nonmetal root
and the suffix -ate. The ion with fewer O
atoms takes the nonmetal root and the suffix
-ite.
Families with Four Oxoanions (usually a Halogen)
The ion with most O atoms has the prefix per-,
the nonmetal root and the suffix -ate. The
ion with one less O atom has just the suffix
-ate. The ion with two less O atoms has the
just the suffix -ite. The ion with three less
O atoms has the prefix hypo- and the suffix
-ite.
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NAMING OXOANIONS - EXAMPLES
Prefixes Root Suffixes
Chlorine Bromine Iodine
per ate
perchlorate perbromate periodate

ClO4- BrO4- IO4-
ate
chlorate bromate iodate

ClO3- BrO3- IO3-
ite
chlorite bromite iodite

ClO2- BrO2- IO2- hypo
ite
hypochlorite hypobromite hypoiodite

ClO - BrO - IO -
No. of O atoms
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Binary Compounds (Type III Covalent Contain
Two Nonmetals

• The first element in the formula is named first,
  using the full element name.
• The second element is named as if it were an
  anion.
• Prefixes are used to denote the numbers of atoms
  present.
• The prefix mono- is never used for naming the
  first element, e.g. CO is carbon monoxide.

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Examples of Names and Formulas of Oxoanions and
Their Compounds - I

• KNO2
  BaSO3 barium sulfite
• Mg(NO3)2 magnesium nitrate Na2SO4
• LiClO4 lithium perchlorate Ca(BrO)2
  calcium hypobromite
• NaClO3
  Al(IO2)3 aluminum iodite
• RbClO2 rubidium chlorite KBrO3
• CsClO
  LiIO4 lithium periodate

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Examples of Names and Formulas ofOxoanions and
their Compounds - II

• calcium nitrate
  ammonium sulfite (NH4)2SO3
• strontium sulfate SrSO4
  lithium nitrite
• potassium hypochlorite KClO lithium
  perbromate LiBrO4
• rubidium chlorate
  calcium iodite Ca(IO2)2
• ammonium chlorite NH4ClO2 boron
  bromate
• sodium perchlorate
  magnesium hypoiodite Mg(IO)2

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Problem 6-3 Determining Names and Formulas of
Ionic Compounds Containing Polyatomic Ions
a) magnesium perchlorate
b) (NH4)2SO3
c) calcium nitrate
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Naming Acids
1) Binary acids solutions form when certain
gaseous compounds dissolve in water. For
example, when gaseous hydrogen chloride
(HCl) dissolves in water, it forms a solution
called hydrochloric acid. Prefix hydro-
anion nonmetal root suffix -ic the word acid

hydrochloric acid
2) Oxoacid names are similar to those of the
oxoanions, except for two suffix changes
Anion -ate suffix becomes an -ic suffix in
the acid. Anion -ite suffix becomes an
-ous suffix in the acid. The oxoanion
prefixes hypo- and per- are retained. Thus,
BrO4- is perbromate, and HBrO4 is perbromic
acid IO2- is iodite, and HIO2 is iodous
acid.
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Determining Names and Formulas ofAnions and Acids

• Problem 6-4 Name the following anions and give
  the names and
• formulas of the acid
  solutions derived from them
• a) I - b) BrO3- c) SO3 2-
  d) NO3- e) CN -
• Solution
• a) The anion is
• b) The anion is bromate and the acid is
  bromic acid, HBrO3
• c) The anion is
• d) The anion is nitrate and the acid is
  nitric acid, HNO3
• e) The anion is

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Names and Formulas of Binary Covalent
Compounds
1) The element with the lower group number in the
periodic table is the first word in the name
the element with the higher group number is the
second word. (Important exception When the
compound contains oxygen and a halogen, the
halogen is named first.) 2) If both elements are
in the same group, the one with the higher
period number is named first. 3) The second
element is named with its root and the suffix
-ide. 4) Covalent compounds have Greek
numerical prefixes to indicate the number of
atoms of each element in the compound. The first
word has a prefix only when more than one atom of
the element is present the second word always
has a numerical prefix.
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Determining Names and Formulas of Binary
Covalent Compounds
Problem 6-5
What are the name or chemical formulas of the
following chemical compounds
a) carbon dioxide b) PCl3 c) Give the name and
chemical formula of the compound formed from two
P atoms and five O atoms.
Solution
a) carbon dioxide b) PCl3 c) The compound
formed from two P atoms and five O atoms
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Answers to Problems in Lecture 6

• (b) ZnCl2 , Zinc Chloride (d) Sr3N2 , Strontium
  Nitride (f) Sc2S3 , Scandium Sulfide
• (b) Cobalt (II) Fluoride (d) Nickel (III)
  Chloride
• (a) Mg( ClO4)2 (b) Ammonium Sulfite (c)
  Ca(NO3)2
• (a) iodide, hydroiodic acid, HI (c) sulfite,
  sulfurous acid, H2SO3 (e) cyanide, hydrocyanic
  acid, HCN
• (a) CO2 (b) phosphorous trichloride (c)
  diphosphorous pentaoxide