Intro to Naming & Formula
Writing
Periodic Table Basics
And
Ionic VS Molecular Compounds
Systematic Naming
• There are too many compounds to
remember the names of them all.
• A compound is made of two or more
elements.
• Atoms of elements are joined together.
• The name should tell us how many and
what type of atoms.
Periodic Table- Repetitious arrangement
of elements according common chemical
and physical properties
• First table arranged by Dimitri Mendeleev.
• Arranged elements by atomic mass.
• Modern table arranged by Henry Mosely.
• Arranged elements by atomic number.
Periodic Table
• More than a list of elements.
• The elements are put in columns because of
•
•
•
•
similar chemical and physical properties.
All elements in a column have the same
number of valence electrons (outer shell
electrons).
Each column is called a group or family.
All elements in a row have the same number
of energy levels.
Each row has a periodic number that tells the
number of energy levels.
Representative elements
•
1A
2A
The group A elements
are called the
representative elements
because they represent
metals, non-metals,
metalloids and noble
gases.
8A
5A 7A
3A4A 6A
Hydrogen is
not a metal
Metals
Metals
• Luster – shiny.
• Ductile – drawn into wires.
• Malleable – hammered into sheets.
• Conductors of heat and electricity.
• Lose electrons when they form ions.
• Lose 1,2 or 3 electrons.
Transition metals
Inner transition
metals
Transition metals
• The Group B elements.
• Electrons in the shell underneath the valence
•
electrons may get involved in bonding.
This is why they may have more than one
ionic charge as an ion.
Inner Transition Metals
Lanthanide series – rare earth elements
Actinide series- man made elements
Non-metals
• Dull
• Brittle
• Nonconductorsinsulators
• Gain electrons
Metalloids or Semimetals
• Properties of both
• Semiconductors
Atoms and ions
• Atoms are electrically neutral.
• Same number of protons and electrons.
• Ions are atoms, or groups of atoms, with
a charge.
• Different numbers of protons and
electrons.
• Only electrons can move.
• Gain or lose electrons.
Anion
• A negative ion.
• Has gained electrons.
• Non metals can gain electrons.
• Charge is written as a super script on the
right.
-1
F
-2
O
Has gained one electron
Has gained two electrons
Cations
Positive ions.
 Formed by losing electrons.
 More protons than electrons.
 Metals form cations.

+1
Has lost one electron
K
+2
Has lost two electrons
Ca
Compounds and Law of Definite
Proportion
• Follow the Law of Definite Proportion.
• Have a constant composition.
• Have to add the same number of atoms
every time. (Keep the same ratio for
each atom.)
• Ex. NaCl always a 1:1 of sodium to
chlorine.
• Ex. C6H22O11 always a 6:22:11 ratio of
carbon to hydrogen to oxygen.
Two Types of Compounds
Molecular and Ionic
Molecular compounds
• Made by joining nonmetal atoms together to
•
•
•
•
•
make a molecule
Made of molecules.
Smallest piece is a molecule.
Molecules do not have charges. (NEUTRAL)
Diatomic Molecules- elements that are paired
when not joined with a different element.
H2;O2,N2;Cl2;Br2;I2;F2
Two Types of Compounds
Ionic Compounds
Made of cations and anions.
• Metals and nonmetals.
• The electrons lost by the cation are
gained by the anion.
• The cation and anions surround each
other.
• Ionic Compounds do not have charges.
(NEUTRAL)
• Smallest piece is a FORMULA UNIT.
Two Types of Compounds
Smallest
piece
Types of
elements
State
Melting
Point
Ionic
Molecular
Formula Unit
Molecule
Metal and
Nonmetal
Nonmetals
solid
Solid, liquid
or gas
High >300ºC
Low <300ºC
Chemical Formulas
• Shows the kind and number of atoms in
the smallest piece of a substance.
• Molecular formula- number and kinds of
atoms in a molecule. (Molecular
Compound)
• CO2
• C6H12O6
Formula Unit
• Formula Unit - The smallest whole number
ratio of atoms in an ionic compound.
• Ions surround each other so you can’t say
which is hooked to which.
Charges on ions
• For most of the Group A elements, the
Periodic Table can tell what kind of ion
they will form from their location.
• Elements in the same group have similar
chemical and physical properties.
• Including the charge when they are ions.
Group A metals – the group number is the charge .
Group A non-metals – (8 – the group number is the
charge.) Group 8A noble gases - have 8 valence
+1 electrons so they do not react or form ions.
+2
+3
-3 -2 -1
What about the others?
• We have to figure those out some other
way.
• More on this later.
Naming ions
• We will use the systematic way.
• Cation- if the charge is always the same
(Group A) just write the name of the
metal.
• Transition metals (Group B) can have
more than one type of charge.
• Indicate the charge with roman numerals
in parenthesis.
Roman Numerals
•1
•2
•3
•4
•5
•6
•7
•8
I
II
III
IV
V
VI
VII
VIII
Name these
• Na+1
• Ca+2
• Al+3
• Fe+3
• Fe+2
• Pb+2
• Li+1
Write Formulas for these
• Potassium ion
• Magnesium ion
• Copper (II) ion
• Chromium (VI) ion
• Barium ion
• Mercury (II) ion
Naming Anions
• Anions charges are always the same.
• Change the nonmetal’s name ending to –
ide
• F-1 Fluorine
Naming Anions
• Anions are always the same.
• Change the element ending to – ide
• F-1 Fluorin
Naming Anions
• Anions are always the same
• Change the element ending to – ide
• F-1 Fluori
Naming Anions
• Anions are always the same
• Change the element ending to – ide
• F-1 Fluor
Naming Anions
• Anions are always the same
• Change the element ending to – ide
• F-1 Fluori
Naming Anions
• Anions are always the same
• Change the element ending to – ide
• F-1 Fluoride
Naming Anions
• Anions are always the same
• Change the element ending to – ide
• F-1 Fluoride
Name these
• Cl-1
• N-3
• Br-1
• O-2
• Ga+3
Write these
• Sulfide ion
• iodide ion
• phosphide ion
• Strontium ion
Polyatomic ions
• Groups of nonmetal atoms that stay
together and have a charge.
• Made of nonmetals.
• Molecular Compounds
• are a group of nonmetal atoms without
a charge.
• Sulfate
Polyatomic ions
SO4-2
• Sulfite SO3-2
• Carbonate CO3-2
•
Chromate CrO4-2
• Dichromate Cr2O7-2
• Phosphate PO4-3
• Phosphite
PO3-3
• Nitrate NO3• Nitrite NO2• Ammonium NH4+1