Unit 7: Bonding and Naming
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Transcript Unit 7: Bonding and Naming
Unit 7: Bonding and Naming
A Quick Review…
Atoms are electrically neutral
Ions
Charged particles
Anion
Negative ion; gain electrons; nonmetals
Cation
Positive ion; lose electrons; metals
Unit 7 Objectives:
Distinguish between ionic, covalent, and metallic
bonds
Distinguish between ionic and molecular compounds
Name ionic and molecular compounds
Write formulas for ionic and molecular compounds
Bonds
A valence electron from one atom is attracted to
another atom’s nucleus
Remember…
Everything
wants a full valence shell
Everything wants to have lower Kinetic Energy
Can tell the type using the atoms’ electronegativities,
or by the type of atoms involved
Ionic Bonds
Electrons are donated from one
atom to the other
Very different
electronegativities (difference is
>1.7)
One atom is MUCH more
attracted to electrons than the
other
Which types of atoms are
involved?
Metals and non-metals – the metal
gives up electrons to the nonmetal
Covalent Bonds
Electrons are “shared” by
two atoms
Similar electronegativity
values (difference < 1.7)
Closer electronegativities
means more equal
sharing
What types of atoms are
involved?
2 nonmetals
Covalent Bonds
Atoms always share pairs of electrons
Type of Bond
Pairs Shared
Electrons
Shared
Single
1
2
Double
2
4
Triple
3
6
Metallic Bonds
What type of atoms?
2
metals
Metal cations
surrounded by a “sea of
electrons”
Determine the Bond Type
H-O
H-Cl
Na-Cl
K-Cr
Na-Br
C-H
Types of Compounds - Ionic
Ionic Compounds
Contain
ionic bonds
Electrically Neutral
A metal is joined to a non-metal or a polyatomic
ion
Polyatomic Ion
An ion made up of more than one element
Covalently Bonded
Almost always anions
Ex: SO42-
Types of Compounds - Ionic
Law of Definite Proportions
Small
whole number ratios
The formula represents a formula unit (NOT a
molecule)
Formula Units are always simplest ratio (REDUCE!)
Ions surround each other so you can’t see which is
hooked to which
Types of Compounds - Molecular
Contain covalent bonds
Non-metals are joined to other non-metals
Called molecules
Smallest electrically neutral unit that still maintains the
properties of the substance
Can be one type of atom – O2
Can be a compound – CO2
Distinguishing Between Ionic and Molecular
Ionic
Molecular
Bond Type
Ionic
Covalent
Smallest
Piece
Formula Unit
Molecule
Types of
Elements
State of
Matter
Metal-Nonmetal
Nonmetal - Nonmetal
Metal –Polyatomic Ion
Solid
Solid, liquid, or gas
Chemical Formulas
Show the kind and number of each type of atom in a
compound
For molecules you can also say molecular formula
Subscripts are used to tell you if there is more than
one of an atom. If there is only one, no subscript.
NaCl, BaS
CaCl2, C6H12O6
Diatomic Elements
Some elements are never found as a single atom
If they aren’t bonded to another type of atom, they
bond to themselves
There are 7:
1.
2.
3.
4.
5.
6.
7.
Hydrogen (H2)
Nitrogen (N2)
Oxygen (O2)
Fluorine (F2)
Chlorine (Cl2)
Bromine (Br2)
Iodine (I2)
Oxidation State
Remember the trend for the representative elements
Transition Metals don’t always have the same
oxidation state
Naming Ions
Two methods
Classical Method – uses root word (in Latin) +
suffixes (-ous, -ic).
Fe2+ = Ferrous
Doesn’t give the true value
Doesn’t work for everything
2. Stock System – uses Roman numerals in ( ) to
indicate the numerical value.
Fe2+ = Iron (II)
Much better because it works all the time. We’ll use
this one
1.
Roman Numerals
Number
Roman
Numeral
1
I
2
II
3
III
4
IV
5
V
6
VI
7
VII
8
VIII
9
IX
10
X
No, you don’t get
these on the test…
Use with
transition metals
Naming Ions - Cations
Use the stock system
If the charge is always the same (representative
elements, Cd, Ag, Zn), just say the name of the
element followed by “ion”
Example: Ca2+ = calcium ion
If it is a metal that varies (transitions, Sn, Pb) say the
name of the element, the oxidation state as a Roman
Number, followed by “ion”
Example: Mb2+ = molybdenum (II) ion
Naming Ions: Exceptions
Representative elements that need Roman Numerals
Pb
Sn
Transition metals that no not need a Roman
Numeral (bc they always have the same oxidation
state)
Ag1+
Cd2+
Zn2+
Naming Ions - Cations
Write the name of each cation
Na1+
Ca2+
Al3+
Fe3+
Li1+
Pb2+
W6+
Writing Formulas- Cations
Write the formula for each ion.
Potassium Ion
Magnesium Ion
Copper (II) Ion
Silver Ion
Mercury (II) Ion
Chromium (VI) Ion
Barium Ion
Naming Ions - Anions
Anions always have the same oxidation state (no
need for Roman Numerals)
Change the ending of the element to –ide
Ex: F = Fluorine
F - = Fluoride Ion
Naming Ions - Anions
Name the following ions
Cl 1 N 3 Br 1 O 2 Ga 3+
Writing Formulas - Anions
Write the formula for each ion
Sulfide Ion
Iodide Ion
Phosphide Ion
Strontium Ion
Polyatomic Ions
Ions containing more than 1 element
Almost always anions
See list on the back of your Periodic Table or Packet
No, You need not memorize them
To name them, just check the list and use the name.
No change to the ending
Naming Ionic Compounds
Binary Compounds only have 2 elements
To write the name, just name the 2 ions
NaCl - sodium chloride
MgBr2 – magnesium bromide
Naming Binary Ionic Compounds
A little harder with transition metals…
Don’t forget the Roman numerals
Ex: CuO
Overall, the compound is neutral
We know O is 2Copper must be 2+
Copper (II) Oxide
Ex: CoCl3
We know Cl is 1- and there are 3 of them
That makes 3Co must be 3+
Cobalt (III) Chloride
A Few More Examples
Cu2S
Sulfur is always:
The Copper needs to add up to:
There are 2 Copper atoms, so each one is:
Name:
Fe2O3
Oxygen is always:
There are 3 of them, which adds up to:
The 2 Iron atoms should add up to:
Each Iron is then:
Name:
Name some Binary Ionic Compounds
KCl
Na3N
CrN
Sc3P2
PbO
PbO2
Na2Se
Naming Ternary Ionic Compounds
These have polyatomic ions. Name the cation, then
name the polyatomic ion
Ex: NaNO3
Na = Sodium
NO3 = Nitrate
Sodium Nitrate
The hardest part is remembering to check your list!
Name the Ternary Ionic Compounds
LiCN
Fe(OH)3
(NH4)2CO3
NiPO4
Writing Formulas for Ionic Compounds
Remember, charges add up to ZERO
Get the oxidation state of each piece
Balance charges out by adding subscripts
Polyatomic ions need ( ) if there is more than 1 of it
Use the criss-cross method
Make the oxidation state of one the subscript of the other. Like
finding the least common multiple.
Calcium
Chloride
Ca2+ Cl 1CaCl2
Write the formulas for these
Lithium Sulfide
Tin (II) Oxide
Tin (IV) Oxide
Magnesium Fluoride
Copper (II) Sulfate
Iron (III) Phosphide
Gallium Nitrate
Iron (III) Sulfide
Ammonium sulfide
Keep in Mind…
If you see ( ) it’s telling you the oxidation state of the
cation
Anions generally end in –ide if it’s an element, and –
ate or –ite if it’s a polyatomic ion
Molecular Compounds
Made of only Non-metals
Electronegativities are similar, they aren’t being held
together by opposite charges
This means we can’t use the oxidation state to see
how many of each atom we have
The name will tell you the amount of each atom
using prefixes
Prefixes
1
Mono
2
Di
3
Tri
4
Tetra
5
Penta
6
Hexa
7
Hepta
8
Octa
9
Nona
10
Deca
Yes, memorize these!!
Naming Molecular Compounds
To write the name:
Prefix + first element then Prefix + second element
Only one exception this time: if the prefix on the first
element is “mono” we don’t write it
No double vowels (oa, oo)
Rule of thumb: if it sounds weird, you need to drop a vowel
Name the Molecular Compounds
N 2O
NO2
Cl2O7
CBr4
CO
BaCl2
Write the Formulas for Molecular Compounds
Diphosphorous pentoxide
Tetraiodide nonoxide
Sulfur hexafluoride
Nitrogen trioxide
Carbon trtrahydride
Phosphorous trifluoride
Aluminum chloride
Naming Acids
We will save the nomenclature for acids until we
start talking about them.
For now, here are a couple you should know:
Acid
Formula
Hydrochloric acid
HCl
Sulfuric Acid
H2SO4
Acetic Acid
CH3COOH