PRINCIPLES OF CHEMISTRY I CHEM 1211 CHAPTER 2

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PRINCIPLES OF CHEMISTRY I CHEM 1211 CHAPTER 2

DR. AUGUSTINE OFORI AGYEMAN Assistant professor
of chemistry Department of natural
sciences Clayton state university
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CHAPTER 2 ATOMS, MOLECULES, AND IONS
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THE ATOMIC THEORY OF MATTER
Law of Constant Composition - The relative
numbers and kinds of atoms are constant in a
given compound - All samples of a given chemical
compound have the same elemental
composition Example - Water (H2O) always
contains 1 g of H for every 8 g of O Law of
Conservation of Mass (Matter) - The total mass of
materials after a chemical reaction is equal to
the total mass before the chemical reaction
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THE ATOMIC THEORY OF MATTER

• Law of Multiple Proportions
• - When two or more elements combine to form a
  compound, their masses in that
• compound are in a fixed and definite ratio
• - Elements combine in a ratio of small whole
  numbers
• - If two elements form more than one compound,
  the ratios of the masses of the
• second element combined with a fixed mass of
  the first element will be in ratios
• of small whole numbers

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THE ATOMIC THEORY OF MATTER
Law of Multiple Proportions - C and O can
combine to form CO and CO2 CO 1.33 g O combine
with 1.00 g C CO2 2.66 g O combine with 1.00 g
C - Ratio of O is 2.66 g 1.33 g 2 1
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THE ATOMIC THEORY OF MATTER
Daltons Atomic Theory 1. All matter (every
element) is made up of very small particles
called atoms - Atoms are indivisible and
indestructible 2. All atoms of a given element
are identical in mass and properties -
Atoms of a given element are different from atoms
of all other elements
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THE ATOMIC THEORY OF MATTER
Daltons Atomic Theory 3. Compounds are formed
from a combination of two or more different
kinds of atoms - A given compound always has
the same relative number and kind of
atoms 4. A chemical reaction is a rearrangement
of atoms - Atoms are neither created nor
destroyed in a chemical reaction
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THE ATOMIC THEORY OF MATTER
Modern atomic theory is more involved but based
on Daltons theory - Atoms can be destroyed by
nuclear reactions but not by chemical
reactions - There are different kinds of atoms
within an element (isotopes - different
masses, same properties)
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THE ATOMIC THEORY OF MATTER
Homework Read about the following and summarize
all in one page (double spaced) - Gas discharge
tubes (cathode rays) - Antoine Lavoisier - J. J.
Thompson - Robert A. Millikan (oil drop
experiment) - Ernest Rutherford - James Chadwick
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THE ATOMIC STRUCTURE
Atom - Is the smallest particle of an element
that retains the chemical identity of the
element - Is the basic building block of ordinary
matter - Made up of smaller particles (the
building blocks of an atom) called subatomic
particles Three Types of Subatomic
Particles Electron possesses a negative (-)
electrical charge Proton possesses a positive
() electrical charge Neutron has no charge (it
is neutral)
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THE ATOMIC STRUCTURE
Electronic Charge equals 1.602177 x 10-19 C (C
coulombs) - Charges are usually expressed as
multiples of the electronic charge Charge of an
electron -1.602177 x 10-19 C -1 Charge of a
proton 1.602177 x 10-19 C 1 Atoms have no
net electrical charge since they have equal
number of electrons and protons
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THE ATOMIC STRUCTURE
- Protons and neutrons have very large masses
(about 2000 x) as compared to electrons - Atoms
generally have extremely small masses - Atomic
Mass Unit (u) is used to express such small
masses 1 u 1.66054 x 10-24 g or 1 g
6.02212 x 1023 u
Mass (u) 5.486 x 10-4 1.0073 1.0087
Relative Mass 1 1837 1839
Charge Negative (-1) Positive (1) Neutral (0)
Particle Electron Proton Neutron
Mass (g) 9.109 x 10-28 1.673 x 10-24 1.675 x
10-24
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THE ATOMIC STRUCTURE
- The center of an atom is small, dense, and
positively charged called the nucleus - The
nucleus contains all protons and neutrons and are
referred to as necleons - The nucleus is,
therefore, positively charged and contributes
about 99.9 of the mass of an atom
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THE ATOMIC STRUCTURE

• - The electrons move rapidly around the nucleus
• - Outer region called the extranuclear region
• - Account for most of the volume of an atom
• Electron Cloud
• - Volume occupied by electrons
• - Negatively charged

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ATOMIC NUMBER (Z)
- The number of protons in the nucleus of an
atom - determines the identity of the element -
Since atoms have no net electrical charge number
of protons number of electrons Z number of
protons number of electrons
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MASS NUMBER (A)

• - The sum of the number of protons and
• the number of neutrons in the nucleus of an atom
• The total number of subatomic particles in the
  nucleus of an atom
• - The number of nucleons of an atom
• A number of protons number of neutrons
• number of neutrons mass number - atomic number
  A - Z

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ATOMIC AND MASS NUMBERS
MASS NUMBER
CHEMICAL SYMBOL
ATOMIC NUMBER
A
SYMBOL
Z
16
40
12
O
Ca
C
20
8
6
Mass number is the superscript to the left Atomic
number is the subscript to the left
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ATOMIC AND MASS NUMBERS
An atom has an atomic number of 56 and a mass
number of 138. What are the numbers of protons,
electrons, and neutrons present in the atom? What
is the number of subatomic particles present in
the nucleus of the atom? Number of protons
atomic number 56 Number of electrons atomic
number 56 Number of neutrons mass number
atomic number 138-56 82 Number of subatomic
particles in the nucleus mass number 138
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CHEMICAL PROPERTIES OF ATOMS
- The number of protons (the atomic number)
characterizes an atom - Electrons determine the
chemical properties of an atom - Atoms with the
same atomic number have the same chemical
properties - Atoms with the same atomic number
are atoms of the same element
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CHEMICAL PROPERTIES OF ATOMS
Chapter 1 definition of An Element - Is a pure
substance that cannot be reduced to a simpler
substance by normal chemical means Chapter 2
definition of An Element - Is a pure substance in
which all atoms present have the same atomic
number
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ISOTOPES
- Atoms of an element with the same atomic number
but different mass numbers - Atoms of an
element with the same number of protons and the
same number of electrons but different numbers
of neutrons - Isotopes of an element have the
same chemical properties but slightly different
physical properties - The atomic number is
usually omitted since it is the same for
isotopes of a given element
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ISOTOPES
11
12
13
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C
C
C
C
Most abundant is carbon-12
6
6
6
6
1
2
3
H
H
H
Most abundant is hydrogen-1
1
1
1
28
29
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Si
Si
Si
Most abundant is silicon-28
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14
14
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AVERAGE ATOMIC MASS
- Determined by using the masses of an elements
various isotopes and their respective natural
abundances Units 1 u 1.66054 x 10-24 g or 1 g
6.02214 x 1023 u u (amu) atomic mass unit u
is defined by assigning a mass of exactly 12 u to
an atom of carbin-12 (reference point)
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AVERAGE ATOMIC MASS
For an element with n isotopes which have atomic
masses in u (m1, m2, m3,.., mn) and natural
abundances expressed as fractions (x1, x2,
x3,,xn) Average Atomic Mass m1x1 m2x2
m3x3 . mnxn
The natural abundance is usually expressed as a
percentage Divide by 100 to convert to the
decimal form (fractional abundance)
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AVERAGE ATOMIC MASS
The mass spectrometer is an instrument used to
measure the masses and relative (natural)
abundances of the isotopes present in a sample
of an element Homework Describe the operation
and uses of the mass spectrometer One page
maximum and double spaced
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AVERAGE ATOMIC MASS
Naturally occurring copper is 69.09 63Cu, which
has a relative mass of 62.93 u, and 30.91 65Cu,
which has a relative mass of 64.93 u. Calculate
the average atomic mass of copper.
63Cu natural abundance 69.09 fractional
abundance 69.09/100 0.6909
65Cu natural abundance 30.91 fractional
abundance 30.91/100 0.3091
Average Atomic Mass (62.93)(0.6909)
(64.93)(0.3091) 63.5478
63.55 u
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PERIODIC TABLE OF ELEMENTS
- 117 known elements - 92 naturally occurring
elements - 25 are not found in nature but made in
the laboratory Periodic Table - Elements are
arranged in a tabular form (called the periodic
table) in order of increasing atomic number such
that elements with similar chemical properties
are positioned in vertical columns - A tool that
chemists use for organizing and remembering
chemical facts
Atomic number
SYMBOL
Atomic mass
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PERIODIC TABLE OF ELEMENTS
Period - The horizontal row of elements in the
periodic table - Labeled with Arabic numbers from
top to bottom - First row is period 1, second
row is period 2, etc Group - The vertical
column of elements in the periodic table - May
be labeled with Arabic numbers (1 through
18) Arabic numbers with letters A or B (1A, 1B,
2A, 3B, etc) Roman numerals with letters A or B
(IA, IB, IIA, IIIB, etc)
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PERIODIC TABLE OF ELEMENTS
Groups With Special Names Alkali Metals -
Elements in Group 1A (excluding hydrogen) Li, Na,
K, Rb, Cs, and Fr - Properties soft, shiny,
react readily with water - Reactivity increases
down the group Alkaline Earth Metals - Elements
in Group 2A Be, Mg, Ca, Sr, Ba, Ra - Properties
soft, shiny, react moderately with water
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PERIODIC TABLE OF ELEMENTS
Groups With Special Names Chalcogens - Elements
in Group 6A O, S, Se, Te, Po - Properties
commonly found as minerals Halogens (salt
formers) - Elements in Group 7A F, Cl, Br, I,
At - Properties reactive, colored, gas at room
temperature - Reactivity decreases down the group
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PERIODIC TABLE OF ELEMENTS
Groups With Special Names Noble Gases (inert
gases) - Elements in Group 8A He, Ne, Ar, Kr, Xe,
Rn - Properties unreactive gases
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PERIODIC TABLE OF ELEMENTS
Classification by Physical Properties Metals -
Elements on the left block of the periodic
table Characteristics - good conductors of
heat and electricity - ductile (capable of being
shaped or drawn into wire) - malleable (capable
of being rolled into sheets) - high luster
(shiny) - high melting points - high density -
solids at room temperature (except
mercury) (iron, aluminum, gold, silver, copper)
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PERIODIC TABLE OF ELEMENTS
Classification by Physical Properties Nonmetals -
Elements on the right block of the periodic
table Characteristics - poor conductors of
heat and electricity - good insulators (except
diamond) - no metallic luster - nonductile -
lower melting points - lower density - solids,
liquids or gases at room temperature (oxygen,
hydrogen, nitrogen, carbon, sulfur, bromine)
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PERIODIC TABLE OF ELEMENTS
Classification by Physical Properties Metals and
nonmetals on the periodic table are separated by
a bold steplike line running from Group 3A
through Group 6A Metalloids - Some elements
that lie along the line separating metals from
nonmetals Characteristics - Properties fall
between those of metals and nonmetals -
Semiconductors (weak conductors of electricity)
(B, Si, Ge, As, Sb, Te)
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CHEMICAL BOND
- The attractive force that holds atoms together
- The result of interactions between electrons
in the combining atoms - Two types of chemical
bonds covalent and ionic (electrovalent) bonds
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CHEMICAL BOND
Covalent Bond - Formed through the sharing of
one or more pairs of electrons between two atoms
- Always involve two nonmetals (electron
sharing) Ionic Bond - Formed by attraction
between two oppositely charged ions - Formed as
a result of the transfer of electron(s) from
atom(s) to another atom(s) - Often formed
between metal and nonmetal ions
through electrostatic attraction (electron
transfer)
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CHEMICAL COMPOUND
- A substance consisting of two or more different
elements chemically bonded together in a fixed
proportion by mass Two classes of chemical
compounds molecular and ionic compounds
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THE MOLECULE
- Two or more atoms tightly bound together and
behaving as a single unit - Basic structural
unit of molecular compounds - The molecule is
the limit of physical subdivision (the smallest
particle of a compound) - The atom is the limit
of chemical subdivision
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THE MOLECULE

• Homoatomic Molecule
• - All atoms present are of the same kind
  (element)
• Examples
• H2, O2, N2, Cl2, S8
• Heteroatomic Molecule
• - Two or more kinds of atoms are present
  (compound)
• - Two or more elements are present
• Examples
• H2O, CO2, CH4, HCl

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THE MOLECULE
Diatomic molecule contains two atoms (HCl, H2,
O2) Triatomic molecule contains three atoms
(H2O, CO2) Tetratomic molecule contains four
atoms (HNO2, SO3) Pentatomic molecule contains
five atoms (HNO3, CH4) ETC.
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THE MOLECULE
Chemical Formula - Tells which elements and how
many of those elements make up a
compound Example The chemical formula of
sulfuric acid is H2SO4 Conveys the information
that a sulfuric acid molecule contains - 3
different elements hydrogen (H), sulfur (S),
oxygen (O) - 7 atoms 2 hydrogen atoms, 1 sulfur
atom, 4 oxygen atoms - When a particular atom is
1 (as in S above) the subscript is not written
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THE MOLECULE
Chemical Formula - Note the difference between
CoCl2 and COCl2 CoCl2 - 2 different elements
cobalt (Co) and chlorine (Cl) - 3 atoms 1 Co
atom and 2 Cl atoms COCl2 - 3 different
elements carbon (C), oxygen (O), and chlorine
(Cl) - 4 atoms 1 C atom, 1 O atom, and 2 Cl atoms
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MOLECULAR COMPOUNDS
- Compounds composed of molecules - Contain more
than one type of atom - Atoms are joined through
covalent bonds -Generally composed of nonmetals
only (H2O, CO2, CH4, NH3) Physical Properties -
low melting points - poor conductors of
electricity - can be solids, liquids, or gases at
room temperature - low solubility in water
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MOLECULAR COMPOUNDS

Empirical Formula - Chemical formula indicating
the relative number of atoms of each type in a
molecule - Indicates the smallest possible whole
number ratios Molecular Formula - Chemical
formula indicating the actual numbers and types
of atoms in a molecule - Identifies multiples of
the smallest whole number ratios
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MOLECULAR COMPOUNDS
Substance Water Hydrogen Peroxide Methane Benzene
Hexane
Molecular Formula H2O H2O2 CH4 C6H6 C6H14
Empirical Formula H2O HO CH4 CH C3H7

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MOLECULAR COMPOUNDS
Structural Formula - Shows how atoms are arranged
(connected) - Shows chemical bonding within the
molecule (which atom is bonded or attached to
which) - Graphical representation of molecular
formula

H
H
O
O
C
H
H
O
H
H
H
H
Water
Hydrogen Peroxide
Methane
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MOLECULAR COMPOUNDS
1. Molecular (condensed) formula 2. Structural
formula 3. Perspective drawing - Depicts three
dimensional shape 4. Ball-and-stick model -
Shows atoms as spheres and bonds as sticks -
Shows angles at which bonds are attached 5.
Space-filling model - Shows relative sizes of
atoms
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IONS
- Positively or negatively charged particles -
Result from loss (positive) or gain (negative) of
electrons - Basic structural units of ionic
compounds - Charges are represented by
superscripts - Two types of ions Cation - An
ion with a positive charge (loss of
electrons) (H, Na, Al3, Ca2) Anion - An ion
with a negative charge (gain of electrons) (O2-,
Cl-, Br-, I-)

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IONS
Generally, metals form cations whereas nonmetals
form anions - Chemical properties of ions are
different from those of the atoms from which they
were derived - Atoms lose or gain electrons to
attain the same number of electrons as the noble
gas (Group 8A element) closest to
it Generally Group 1A elements form 1
ions Group 2A elements form 2 ions Group 6A
elements form 2- ions Group 7A elements form 1-
ions

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IONS
Monatomic Ion - An ion composed of one
atom (Br-, Na, Mg2, Al3, O2-) Polyatomic
Ion - An ion (charged particle) composed of two
or more atoms covalently bonded together -
behave as a single unit (OH-, NH4, SO42-, CO32-,
HCO3-)

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IONIC COMPOUNDS
- Compounds in which ionic bonds are present -
Contain both positively and negatively charged
ions - Generally composed of metals (positive
ions) and nonmetals (negative ions) (NaCl, KCl,
CaBr2, Na2O) Physical Properties - High melting
and boiling points - High hardness - Brittle
(easily cracked or fractured) - Good conductors
of electricity when molten (electrolytes) - Solid
at room temperature and pressure - High
solubility in water

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IONIC COMPOUNDS
- Ionic compounds do not contain discrete
molecules but ordered arrays of positive and
negative ions NaCl for example - The formula
unit indicates combining ratio (empirical
formula) - A given sodium ion has six immediate
chloride ion neighbors - A given chloride ion
has six immediate sodium ion neighbors
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IONIC COMPOUNDS

- The charges of ions can be used to depict the
empirical formula for ionic compounds - For
equal magnitude of charges on cation and anion
the subscript on each ion is 1 NaCl Na and
Cl- KBr K and Br- MgO Mg2 and O2-
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IONIC COMPOUNDS
- The charges of ions can be used to depict the
empirical formula for ionic compounds - For
unequal magnitude of charges the charge on one
ion is the subscript on the other ion (without
the positive or negative sign) AlCl3 Al3 and
Cl- CaCl2 Ca2 and Cl- Na2S Na and S2- Fe2O3
Fe3 and O2-

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IONIC COMPOUNDS
- The charges of ions can be used to depict the
empirical formula for ionic compounds - For
polyatomic ions each ion is considered as one
unit NH4NO3 NH4 and NO3- (NH4)2CO3 NH4 and
CO32- Na2CO3 Na and CO32- Sr3(PO4)2 Sr2 and
PO43- Ca(OH)2 Ca2 and OH-

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BINARY COMPOUNDS
- Only two elements are present - Any number
of atoms of the two elements may be
present Examples NaCl, H2O, CaCl2, NH3, Al2O3
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BINARY COMPOUNDS
Binary Molecular Compounds - Both elements are
nonmetals Examples H2O, CO2, NO2, SO2, HCl, NH3
Binary Ionic Compounds - One of the two elements
is a metal (cation) and the other is a nonmetal
(anion) Examples Al2S3, NaCl, KCl, KBr
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FORMULA MASS
- The sum of atomic masses of all the atoms
present in the chemical formula of a
substance - Relative mass based on the carbon-12
relative-mass scale - It is advisable to use two
decimal places for atomic masses For molecular
compounds - Formula mass is obtained from the
molecular formula - Also known as molecular
mass For ionic compounds - Formula mass is
obtained from the empirical formula
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FORMULA MASS
Calculate the formula mass of H2O H 2 x 1.01 u
2.02 u O 1 x 16.00 u 16.00 u Formula mass
(2.02 16.00) u 18.02 u
Calculate the formula mass of H2SO4 H 2 x 1.01 u
2.02 u S 1 x 32.06 u 32.06 u O 4 x 16.00 u
64.00 u Formula mass (2.02 32.06 64.00) u
98.08 u
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FORMULA MASS
Calculate the formula mass of CaCO3 Ca 1 x 40.08
u 40.08 u C 1 x 12.01 u 12.01 u O 3 x 16.00
u 48.00 u Formula mass (40.08 12.01
48.00) u 100.09 u
Calculate the formula mass of Fe2(SO4)3 Fe 2 x
55.85 u 111.70 u S 3 x 32.07 u 96.21 u O 12
x 16.00 u 192.00 u Formula mass (111.70
96.21 192.00) u 399.91 u
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NAMING SIMPLE COMPOUNDS

Positive Ions (Cations) - Cations have the same
name as the metal atom from which they were
formed Na sodium ion Al3 aluminum ion K
potassium ion
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NAMING SIMPLE COMPOUNDS

Positive Ions (Cations) - The positive charge is
indicated by a Roman numeral (in parenthesis) if
the metal can form different cations - Usually
seen in transition metals Fe2 iron(II)
ion Fe3 iron(III) ion Pb2 lead(II)
ion Pb4 lead(IV) ion Sn2 tin(II) ion Sn4
tin(IV) ion Cu copper(I) ion Cu2 copper(II)
ion
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NAMING SIMPLE COMPOUNDS

Positive Ions (Cations) - Older method for
naming differently charged ions of the same
metal Fe2 ferrous ion Fe3 ferric ion Pb2
plumbous ion Pb4 plumbic ion Sn2 stannous
ion Sn4 stannic ion Cu cuprous ion Cu2
cupric ion
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NAMING SIMPLE COMPOUNDS
Positive Ions (Cations) - If you have any doubt
whether a metal forms more than one cation, just
use the Roman numeral (never wrong to do so) -
The charge on the nonmetal and charge neutrality
can be used to identify the charge on the
metal - Cations formed from nonmetal atoms end
in -ium (polyatomic ions) NH4 ammonium
ion H3O hydronium ion

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NAMING SIMPLE COMPOUNDS
Negative Ions (Anions) - Monatomic anions are
formed by replacing the ending of the name of
the element with -ide Br- bromide ion Cl-
chloride ion O2- oxide ion S2- sulfide ion

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NAMING SIMPLE COMPOUNDS

Negative Ions (Anions) - Some polyatomic anions
also end in -ide OH- hydroxide ion CN- cyanide
ion O22- peroxide ion
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NAMING SIMPLE COMPOUNDS

- Polyatomic anions containing oxygen end in -ate
or -ite - The -ite ion has one less oxygen atom
than the -ate ion - The pair carry the same
charge SO42- sulfate ion SO32- sulfite
ion NO3- nitrate ion NO2- nitrite ion ClO3-
chlorate ion ClO2- chlorite ion PO43-
phosphate ion
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NAMING SIMPLE COMPOUNDS
- Prefix is used in some cases per- indicates
one more O atom than the -ate (ClO3- chlorate
ClO4- perchlorate) hypo- indicates one less O
atom than the -ite (ClO2- chlorite ClO-
hypochlorite - Some pairs differ by the
presence of hydrogen CO32- (carbonate) and HCO3-
(hydrogen carbonate or bicarbonate)

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NAMING SIMPLE COMPOUNDS
Ionic Compounds - Names consist of the cation
name followed by the anion name NaCl sodium
chloride KOH potassium hydroxide NH4Br ammonium
bromide CaCO3 calcium carbonate - Parenthesis
are used for compounds containing two or more
polyatomic ions Mg(OH)2 magnesium
hydroxide Pb(NO3)2 lead(II) nitrate

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NAMING SIMPLE COMPOUNDS
Acids - Hydrogen containing compounds -
Substance whose molecules yield hydrogen ions
(H) when dissolved in water A 1) names
ending in -ide change to -ic 2) the prefix
hydro- is added to the anion 3) the word acid
follows HCl anion is chloride hydrochloric
acid HBr anion is bromide hydrobromic acid HCN
anion is cyanide hydrocyanic acid

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NAMING SIMPLE COMPOUNDS
Acids - Hydrogen containing compounds -
Substance whose molecules yield hydrogen ions
(H) when dissolved in water B 1) names
ending in -ate change to -ic and -ite change to
-ous 2) the word acid follows HNO3 anion is
nitrate nitric acid HNO2 nitrous acid H2SO4
anion is sulfate sulfuric acid H2SO3 sulfurous
acid H3PO4 anion is phosphate phosphoric acid

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NAMING SIMPLE COMPOUNDS
Binary Molecular Compounds - Compounds with two
elements but any number of atoms - Some
molecular compounds with nonsystematic common
names H2O water NH3 ammonia CH4 methane

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NAMING SIMPLE COMPOUNDS
Binary Molecular Compounds - The name of the
element farther to the left in the periodic
table is usually written first (oxygen is an
exception) - For elements in the same group of
the periodic table the one with higher atomic
number (to the bottom) is named first - The name
of the second element ends in -ide

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NAMING SIMPLE COMPOUNDS
Binary Molecular Compounds - The number of atoms
of each element is indicated by Greek
prefixes - The prefix mono- is not written for
first elements - If the element begins with a
vowel, the a or o of prefix is not written

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NAMING SIMPLE COMPOUNDS
Binary Molecular Compounds CO2 carbon
dioxide PCl3 phosphorus trichloride PCl5
phosphorus pentachloride SF6 sulfur
hexafluoride P4O10 tetraphosphorus
decoxide O2F2 dioxygen difluoride CO carbon
monoxide N2O4 dinitrogen tetroxide N2O5
dinitrogen pentoxide CBr4 carbon
tetrabromide IF7 iodine heptafluoride

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NAMING SIMPLE COMPOUNDS
Organic Compounds - Compounds containing carbon
and hydrogen, and in combination with oxygen,
nitrogen and other elements Hydrocarbons -
Contain only carbon and hydrogen - Each carbon
is bonded to four other atoms Alkanes One carbon
atom methane Two carbon atoms ethane Three
carbon atoms propane Four carbon atoms
butane Five carbon atoms pentane

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NAMING SIMPLE COMPOUNDS
Alcohols - When one H atom is replaced by an -OH
group One carbon atom methanol Two carbon
atoms ethanol Three carbon atoms propanol Four
carbon atoms butanol Five carbon atoms
pentanol etc. The position of the -OH group can
be specified (2-pentanol, 2-butanol, 1-pentanol,
1-propanol)