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IUPAC
BOHR DIAGRAMS FOR ATOMS
TYPES OF CHEMICAL BONDS
MOLECULAR COMPOUNDS
◦ TYPES
 SIMPLE COVALENT
 COMMON NAME

IONIC COMPOUNDS
◦
◦
◦
◦
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SIMPLE IONIC
MULTIVALENT
POLYATOMIC/COMPLEX
HYDRATED IONIC
ACIDS
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International Union of Pure and Applied Chemists
A global organization that sets the standards in
chemistry.
One job of the IUPAC is to give compounds SYSTEMIC
NAMES.
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AKA:ENERGY LEVEL
DIAGRAMS
These are a way of drawing atoms
in a 2-D manner.
Keep in mind that atoms are
actually 3-D, and there are more
complex representations of atoms.
Bohr models show the NUCLEUS
and the ELECTRON ENERGY
LEVELS of an atom.
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
3 types of SUBATOMIC PARTICLES
◦ PROTONS (p+)
 Positively charged particles – large mass
 Atomic Number = Number of Protons
◦ ELECTRONS (e-)
 Negatively charged particles – very small mass
 Number of Electrons = Number of Protons
◦ NEUTRONS (no)
 Neutral particles – large mass
 Number of neutrons = Atomic Mass – Atomic Number
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NUCLEUS
◦ center of the atom
◦ contains p+ and n0
◦ atomic mass is concentrated here
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ELECTRON ENERGY LEVELS
◦ areas around the nucleus where electrons may be found
◦ 3 LEVELS:
 FIRST LEVEL (Closest to Nucleus) maximum of 2 e SECOND LEVEL
maximum of 8e THIRD LEVEL
maximum of 8e-
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EXAMPLE:

Li – lithium atom
DRAW BOHR DIAGRAMS FOR:
◦ ATOMIC # =
_____________
◦ ATOMIC MASS =
_____________
◦ # p+ = ________________________
◦ # e- = ________________________
◦ # no = ________________________
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EXAMPLE:
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Ne – neon atom
DRAW BOHR DIAGRAMS FOR:
◦ ATOMIC # =
_____________
◦ ATOMIC MASS =
_____________
◦ # p+ = ________________________
◦ # e- = ________________________
◦ # no = ________________________
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EXAMPLE:
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S – sulfur atom
DRAW BOHR DIAGRAMS FOR:
◦ ATOMIC # =
_____________
◦ ATOMIC MASS =
_____________
◦ # p+ = ________________________
◦ # e- = ________________________
◦ # no = ________________________
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Do Bohr diagrams for the
first 18 elements.
Be sure to:
◦ Write in the atomic number
and mass number.
◦ Write the name of the atom.
◦ Show p+ and n0 in the nucleus
◦ Draw electrons in the energy
levels.
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VALENCE LEVEL
◦ The outermost energy level
◦ Electrons in this level are VALENCE ELECTRONS
◦ Atoms with FULL valence shells are STABLE,
meaning they do not normally react with other
atoms.
Which Group???
◦ Atoms that do not have full electron energy levels
are unstable and must GAIN, LOSE, or SHARE
electrons to become stable.
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A chemical bond is a force of attraction between
atoms.
 2 TYPES of Chemical bonds
1. COVALENT BONDS
◦ AKA: molecular bonds
◦ “co” – together/sharing , “valent” – outer shell
◦ Occur when 2 nonmetals share at least 1 pair of
electrons
◦ Molecules with covalent bonds are NONELECTROLYTES.
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ie. their solutions DO NOT CONDUCT electric
current
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2.
IONIC BOND
◦ Occur between a metal and a nonmetal
◦ Metals lose electrons to form CATIONS (+)
◦ Nonmetals gain electrons to form ANIONS (-)
◦ Ionic compounds are ELECTROLYTES.
 ie. their solutions CONDUCT electric current
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Form when 2 or more NONMETALS share
electrons in COVALENT BONDS.
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2 TYPES:
◦ BINARY Molecular Compounds
◦ TRIVIAL NAME Molecular Compounds
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Use these
IUPAC prefixes:

Number
Prefix
1
mono
2
di
3
tri
4
tetra
5
penta
6
hexa
7
hepta
8
octa
9
nona
10
deca
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1. Write NAMES of elements, with the 2nd element
ending in “-ide”.
2. Use PREFIXES to indicate the number of each
atom.
3. Do NOT use the prefix “mono” for the 1st element.
DO use “mono” with the 2nd element.
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N2O4
________________________
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P2O5
________________________
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CCl4
________________________
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S2H2
________________________
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CO
________________________
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1. Write ELEMENT SYMBOLS for each element in
the compound.
2. Use each PREFIX to write the number of each
atom as a SUBSCRIPT next to the symbol
(omit the subscript 1).
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carbon monoxide
____________
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triphosphorus pentabromide ____________
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sulfur hexafluoride
____________
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dicarbon tetrahydride
____________
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AKA: COMMON NAME molecular
compounds.
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These must be memorized.
FORMULA
TRIVIAL/COMMON NAME
O3
ozone
H2O
water
H2O 2
hydrogen peroxide
NH3
ammonia
CH4
methane
CH3OH
methanol
C2H5OH
ethanol
C6H12O6
glucose
C12H22O11
sucrose
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Complete the NEXT THREE SHEETS in your
handout for HOMEWORK.
Refer to the following notes for help:
◦ FIRST SHEET
 Given Name, Write Formula Notes
◦ SECOND SHEET
 Given Formula, Write Name Notes
◦ THIRD SHEET
 Everything!
 Watch out for those common name molecular
compounds!!!
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 Atoms that are not NOBLE GASES will GAIN, LOSE,
or SHARE ELECTRONS to become more stable.
 SHARING electrons results in a COVALENT BOND
and a MOLECULAR COMPOUND.
 When an atom loses or gains electrons it forms
an ion.
 A ionic bond is a force of attraction between
positive and negative ions.

OCTET RULE
◦ Atoms that have an octet of valence electrons
are STABLE and UNREACTIVE.
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Cations
+
- POSITIVE ions that are formed from a
LOSS of electrons.
Cations have more PROTONS than ELECTRONS
and therefore has a net POSITIVE charge.
- METALS form cations.
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anions
re
eg
a
t
i
v
e
- NEGATIVE ions that are formed from
a GAIN of electrons.
Anions have more ELECTRONS than
PROTONS and therefore has a net
NEGATIVE charge.
- NONMETALS form anions.
Electron Blues
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METALS
◦ ATOMS of METALS will LOSE electrons to become CATIONS.
◦ ATOMS with 1, 2, or 3 VALENCE electrons will LOSE these
electrons to form 1+, 2+, or 3+ ions respectively.
◦ GROUP 1 ATOMS – ALKALI
 1 valence electrons(s) (will lose 1 to become stable)
 1 + ion
◦ GROUP 2 ATOMS – ALKALINE EARTH
 2 valence electrons(s) (will lose 2 to become stable)
 2 + ion
◦ GROUP 13 ATOMS
 3 valence electrons(s) (will lose 3 to become stable)
 3 + ion
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NONMETALS
◦ ATOMS of NONMETALS will GAIN electrons to become ANIONS.
◦ ATOMS with 5,6, or 7 VALENCE electrons will GAIN these electrons to form 3-,
2-, or 1- ions respectively.
◦ GROUP 15 ATOMS
 5 valence electrons(s) (will gain 3 to become stable)
 3 - ion
◦ GROUP 16 ATOMS
 6 valence electrons(s) (will gain 2 to become stable)
 2 - ion
◦ GROUP 17 ATOMS - HALOGENS
 7 valence electrons(s) (will gain 1 to become stable)
 1 - ion
◦ GROUP 18 ATOMS - NOBLE GASES
 FULL outer valence levels
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Made from a METAL and a NONMETAL
 Metals form CATIONS
 Nonmetals form ANIONS
 An IONIC BOND is the force of attraction
between cations and anions
(opposite charges attract)
 Ions are arranged in a CRYSTAL LATTICE.
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eg. NaCl crystal lattice
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eg. NaCl
Cl-
Na+
Na+
Cl-
Each cations is surrounded by
6 anions and vice versa
Cl-
Na+
Na+
Cl-
Cl-
Na+
Na+
Cl-
Cl-
Na+
Na+
Cl-
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
See Figure 4, p. 189
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• two types of ion (a cation and an anion)
• cations only have ONE possible charge
WRITE THE NAME FROM THE FORMULA
1.
Write the name of the CATION before the ANION
(Be positive before being negative 
2.
Change the ANION suffix to “-ide”
Do NOT
use
CAPITALS
Do NOT
use
PREFIXES
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MgBr2
KCl
_____________________________
_______________________________
Na2S
_____________________________
Mg3P2
_____________________________
Ba3N2 ______________________________
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What’s wrong with these for BaS?
barium sulfur
Barium Sulfide barium sulfuride
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Do the following sheet in the booklet for
homework:
Follow rules for:
◦ “GIVEN FORMULA, WRITE NAME” for Ionic
Compounds.
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WRITE THE FORMULA FROM THE NAME
1. Determine each ION CHARGE from the periodic
table.
2. Use the “crossover” method to write the formula for
the compound.
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The overall charge on a compound is “zero”.
Ion ratios must be reduced to lowest terms.
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EXAMPLE:
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sodium bromide
_____________________
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barium iodide
___________________
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EXAMPLE:
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magnesium oxide _____________________
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aluminum oxide ___________________
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Do the next two sheets
for homework!
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FIRST PAGE:
◦ Given NAME, Write
FORMULA
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SECOND PAGE:
◦ TOP HALF – Molecular
Compound Naming
◦ BOTTOM HALF – Ionic
Compound Naming
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Many transition metal
ions can have more
than one charge.
 These metals are
called MULTIVALENT.
 What are the 2
possible charges for
Cu
Fe
Au
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ROMAN NUMERALS
are used to show the
charge on these ions.
◦ 1+  I
◦ 2+  II
◦ 3+  III
◦ 4+  IV
◦ 5+  V
◦ 6+  VI
ONLY USE WITH
MULTIVALENT IONS!
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1. ROMAN NUMERALS show the ION
CHARGE of the MULTIVALENT ION.
2. If a ROMAN NUMERAL is NOT given, use
the charge found on the top in each box
on the table. (most common charge)
EXAMPLE:
copper (II) oxide
_________________________
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lead (IV) sulfide
_________________________
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tin sulfide
_________________________
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Do the sheet on the following page!
Remember to ONLY use the ROMAN NUMERAL
with the MULTIVALENT IONS!!!
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RULES
1. Write the names of the ions.
2. Write the ROMAN NUMERAL for the
MULTIVALENT ION. There are 2 METHODS:
1. METHOD 1
Charges must add up to zero.
1. METHOD 2
Charge of Anion X Subscript of Anion
Subscript of Cation
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PbI2
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Fe2O3
_________________________
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CuCl
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MnO2
_________________________
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Do the next 2 sheets for homework!
Remember, doing some workings can help
prevent any mistakes!!!
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A polyatomic ion is
a group of atoms
acting as 1 ION and
carrying a CHARGE.
On the back of your
periodic table, there is a
POLYATOMIC ION TABLE.
polyatomic ions usually
end in –ATE or –ITE,
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Examples:
◦
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nitrate
nitrite
cyanide
hydroxide
bicarbonate
chlorate
carbonate
sulfate
phosphate
ammonium
acetate
________
________
________
________
________
________
________
________
________
________
________
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lithium sulfate
_____________________
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ammonium carbonate
_____________________
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hydrogen dichromate
_____________________
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sodium acetate
_____________________
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lead (II) nitrate
_____________________
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calcium hydroxide
_____________________
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HNO3
_____________________
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NaOH
_____________________
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KMnO4
_____________________
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Cu2SO4
_____________________
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hydrogen carbonate is AKA bicarbonate HCO3-
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hydrogen sulfate is AKA bisulfate HSO4-
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tetraborate B4O72-
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silicate SiO32-
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glutamate C5NH8O4-
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Do the next 2 Sheets for homework!!!
Remember to use the crossover method for
charges.
You may find it helpful to use BRACKETS
around ALL polyatomic ions when writing the
formulae.
1.
Simple Ions
Names
Formulas
- write the name of the positive ion
- determine the charge on each ion
- write the name of the negative ion
followed by -ide
- cross over the charges to write the formula
eg.
eg.
NaCl
sodium chloride
Mg3N2
magnesium nitride
calcium phosphide
Ca 2+
P3Ca3P2
2.
Polyatomic Ions
Names
Formulas
- write the name of the positive ion
- determine the charge on each ion
- write the name of the negative ion
eg.
CaSO4 calcium sulfate
Al(OH)3
- cross over the charges to write the formula
eg.
magnesium nitrate
aluminum hydroxide
Mg2+
NO3Mg(NO3)2
3.
MultiValent Metals
- use Roman Numerals to indicate the ion charge(Stock System)
OR
- use the suffix -ic to indicate the smaller ion charge or -ous for the larger ion charge.
Names
eg.
Formulas
CoCl2 - cobalt(II) chloride
- cobaltous chloride
eg.
nickel(II) nitride
Ni2+
N3-
(cross over)
CoCl3 - cobalt(III) chloride
- cobaltic chloride
NOTE:
Ni3N2
After crossing over the charges to get the formula, make sure you are using the
simp lest ratio between the ions.
eg. magnesium oxide - Mg2 O2 becomes MgO
DON’T USE PREFIXES FOR IONIC COMPOUNDS.
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Hydrated ionic compounds have WATER
attached to their crystal lattice structure.
Solutions become hydrated when they are
crystallized from a water solution.
They are often recognizable by eye because
they are often SHINY and TRANSLUCENT.
Examples:
◦ Bluestone, Epsom salts, Rock salts

BLUESTONE  CuSO4 ∙5H2O
◦ 5 CuSO4 molecules attached to each H2Ocompound.
◦ The “dot” represents a weak bond.
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We indicate the presence of water with the
word HYDRATE and we indicate the number of
water molecules with our GREEK PREFIXES:
MONO 1, DI 2, TRI 3, TETRA 4, PENTA 5, HEXA
6, HEPTA 7, OCTA 8, NONA 9, DECA 10
ANHYDROUS: NO water attached
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barium chloride dihydrate
_____________________
potassium hydroxide hexahydrate
_____________________
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sodium carbonate octahydrate
_____________________
cobalt (II) chloride decahydrate
_____________________
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CaSO4 ∙2H2O
_____________________
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Na3PO4 ∙4H2O
______________________
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HCN ∙ 3H2O
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HOMEWORK:
_____________________
◦ DO THE SHEET ON HYDRATED IONIC COMPOUNDS
ON THE NEXT PAGE OF YOUR HANDOUT.