Ionic Compounds and Acid
Nomenclature
Chemical Bonds
The force that holds two elements together.
- Bonds form to seek the lowest energy state and to meet the
maximum number of valence electrons.
Lewis Dot Compounds
Ionic Compounds
Ions= atoms or groups of atoms that have a positive or
negative charge.
The difference in charge holds the two atoms together
Negative= gaining an electron (-)
Positive= losing or donating an electron (+)
1. Have high melting and boiling points
2. Forms Solids
3. Made from a metal and non-metal.
Ionic Compounds
If an atom is normally neutral
(same # of Protons and Electrons)
And
It donates one electron away it is no longer neutral but positive.
So the Sodium becomes Positive known as a Cation
Chlorine becomes Negative known as a Anion
Cation wrote as Na⁺
Anion wrote as Cl¯
Cation=Metals and Positive
Anions=Non-Metals and Negative
MONOATOMIC IONS- ONLY HAVE ONE ATOM AND
HAVE A SPECIFIC (+) OR (-) CHARGE.
OXIDATION NUMBER OR IONIC CHARGE- CHARGE OF
A MONOATOMIC ION AND IS EQUAL TO THE NUMBER
OF ELECTRONS TRANSFERRED FROM OR TO AN ATOM.
Ions
Oxidation Numbers
Oxidation numbers are written as
superscripts to indicate charge but
are not included in the formula.
Ex: Li1+ or O2-
NAMING MONOATOMIC IONS
Cations
Name the element and add the word Ion.
Example: Na⁺= Sodium Ion
Anions
Drop the ending off the element name and adding
“ide”
Example: O²¯= Oxide
Naming Transition Metal Ions
Transition Metals have more than one Ionic charge.
Example: Iron can form two Cations
Fe²⁺ or Fe³⁺
Fe²⁺= Iron (II) ion
Fe³⁺= Iron (III) ion
Practice
Lithium=
Fluorine=
Oxygen=
Carbon=
Barium=
Cesium=
Au2+=
Gold (III) Ion =
Binary Ionic Compounds
Binary Ionic Compound- made of two ions/elements;
Naming Binary Ionic Compounds
The cation keeps the normal name from periodic table
and the Anion receives an –ide ending.
Example:
NaCl= Sodium Chloride
KI= Potassium Iodide
Writing a formula for Ionic Compounds
1.
2.
Binary Ionic Compounds = cation + anion
Determine the oxidation number of each cation
and anion.
The net charge of the compound must equal “0”
Example: Sodium Chloride
Na⁺ and Cl¯
+1 and -1 =0
Formula = NaCl
Naming Simple Binary Ionic
Compounds
Example 2
Calcium Chloride
Ca²⁺ and Cl¯
2+ and -1 = +1
Add one more Cl to = 0
Formula= CaCl₂
Naming Simple Binary Ionic
Compounds
Practice!!!
Potassium Iodide=
Calcium Phosphide=
Magnesium Chloride=
Magnesium Oxide=
Li₂O=
KBr=
Metals Always Placed Before Non-Metals!!!!!!
Polyatomic Ions
Polyatomic Ions-Tightly bound group of atoms that
behave as a unit and carry a charge.
Ex. SO₃²¯, ClO₂⁺
Names for Polyatomic Ions
Most of the names end with –ite or –ate but not all.
The –ite ending indicates one less oxygen than the
-ate ending.
But –ite and –ate does not determine the actual
number of oxygen atoms.
Cations and Polyatomic Ions
When adding Cations (metals) to polyatomic ions add
the basic element name to the Polyatomic Ion.
Example: CaSO₄ = Calcium Sulfate
Writing Formulas
The charge for the whole compound must equal “0”.
Example: Magnesium Chlorate
Writing Formulas with Cations and
Polyatomic Ions
The charge for the whole compound must equal “0”.
Example: Magnesium Chlorate
Magnesium= +2 and Chlorate = -1
We must have 2 chlorate for the compound to equal
Zero.
Formula= Mg(ClO₃)₂
When adding an extra Polyatomic Ion Use
Parenthesis and add desired amount behind.
Ionic Compounds with Transition Metals
Naming
1. Recognize the metal is a transition metal.
FeCl₂
Fe = Iron a transition metal unknown charge
2. Use the Non-metal to determine the charge of the
transition metal.
Chlorine charge = -1 x 2 = -2
3. The charge of the whole compound must equal zero.
Iron must have a +2 Charge
Name of FeCl₂ = Iron (II) Chloride
Naming Acid
Rules
Anion Ends In –ide
Hydro- stem-ic Acid
Example with Chlorine = Hydrochloric Acid
Anion Ends In –ite
Stem of Anion –ous Acid
Example with Sulfite= Sulfurous Acid
Anion Ends In –ate
Stem of Anion-ic Acid
Example with Nitrate= Nitric Acid
Acids
Acids- compounds that produce hydrogen ions when
dissolved in water
Acids to Know
Hydrochloric Acid=HCl
Sulfuric Acid= H₂SO₄
Nitric Acid= HNO₃
Acetic Acid= HC₂H₃O₂
Phosphoric Acid= H₃PO₄
Carbonic Acid= H₂CO₃
END OF Unit 4!!!
Naming Covalent/Molecular
Compounds
Covalent Compounds are made of two non-metals.
Pre-fixes are used to indicate the number of atoms in
each compound.
Naming Covalent/Molecular
Compounds
1.
2.
3.
Rules
The first element name is given followed by the
second with an “ide” ending.
The first element gets a prefix if more than one.
The second element always gets a prefix.
Examples
NO=Nitrogen Monoxide
N₂O= Dinitrogen Monoxide
N₂O₄=Dinitrogen TetraOxide
Naming Covalent/Molecular Compounds
Formula
Copper(II) Sulfate = CuS
Roman Numeral = Charge of your Metal
Use the Roman Numeral to figure out the charge on your
non-metal.
Copper (II) equals + 2 Charge
The total charge on the whole compound must still equal
0.
Molecular Compounds
Molecular Compounds or when two atoms of different
elements create bonds.
Examples: CO₂, H₂O, PCL₃
1.
Characteristics:
Low melting points and Low boiling points
2.
Form liquids or gases.
3.
Made from two or more non-metals
MOLECULE-MADE UP OF TWO OR
MORE ATOMS OF THE SAME
ELEMENT.
EXAMPLES: 0₂ (OXYGEN YOU BREATHE)
O₃ (OZONE)
Molecules and Bonds
Ionic Bonds Vs. Covalent Bonds
Ionic Bonds
Bonded together by the attraction of
opposite charges (+ and -)
Covalent Bonds
Bonded together by the sharing of
electrons
Electrons are donated/transferred and
taken giving one atom a (+) charge and
the other a (-) charge.
Electrons are shared between both atoms
charges remain the same.
Polar Molecule
Non-Polar Molecule
Made of a metal and non-metal
Made up of two non-metals
Weaker Bonds
Stronger Bonds