Important Naming rules to remember:
Ionic compound names Do NOT us prefixes.
- are neutral and the bonds transfer electrons.
- shortcut = criss-cross charges to from compounds.
Roman Numerals (I) = +1, (II) = +2, (III) = +3 ) represent the charge on transition metal.
- example = iron(II) chloride (FeCl2), or
Silver(I) Oxide (Ag2O
Covalent compound names use prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca).
- are neutral and the bonds share electrons.
- names end in ide (dichloride)
Acids:
- all acid formulas have H in front (HCl, HNO3, H2SO4).
- Binary acid names use hydro- prefix. (H + 1 element)
- Ternary acid names Do NOT use hydro- prefix. (H + a compound)
ate endings are changed to ic acids
Chlorate  Chloric acid
ite
Chlorite  Chlorous acid
endings are changed to
Oxyanions:
ous acids
Compounds with oxygen and a (-)charge . (oxide endings):
also called “polyatomic ions”
-ate
ending is used for 3 or 4 (more) oxygen atoms.
-ite
ending is used for 2 or 3 (less) oxygen atoms.
Per-
written in front used for 4 or 5 (most) oxygen atoms.
Hypo- written in front used for 1 (least) oxygen atoms.
Chemical Formulas:
- Are abbreviated names for compounds (like initials).
- Tells you what elements and how many of each are in a compound.
Example
=
(bottom right #) are the number of atoms, for each element.
H2O

- Subscripts
2 hydrogen atoms, 1 oxygen atoms
Vocabulary:
Monatomic = 1 atom …………………………….……. O
Diatomic
Binary
= only 2 atoms ……………………….……..
= only 2 elements ……………………………
O2
NaCl
Polyatomic = a Compound (3 or more atoms) ………………. H3PO4
Oxides are compounds containing oxygen
Ion – has a charge
Cation – has a positive charge
Anion – has a negative charge
Oxyanions - a compound containing oxygen
& has a negative charge.
Charge on ion (oxidation #)
+1 +2
+3
+4 -3 -2 -1 0
______________________________________________________________________________
# of Valence e1
2
3
4
5
6
7
8
Important to remember:
Elements name
~ monatomic Cations (+ metals) names end in _________
ion.
examples = hydrogen ion, magnesium ion, aluminum ion.
~ monatomic Anions (- nonmetals) names end in ~ide.
examples = oxide, chloride, nitride, fluoride
Covalent compounds are called…
“Molecules” Also called “molecular compounds”
• Form when 2
nonmetals elements bond by sharing electrons.
•
Water (H20)
dihydrogen monoxide
Methane (CH4)
carbon tetrahydride
Ammonia (NH3)
nitrogen trihydride
Rules for naming COVALENT Molecules:
sulfur dioxide
1st – write the name of the First element in the formula, First.
2nd – write the name of the second element. Change the ending to –ide
3rd – Add prefixes to indicate the number of atoms of each element.
(Do Not put mono in front of the 1st element named.)
“polyatomic
ions”, are compounds with an electrical charge.
- Polyatomic ion names end in ate or
ite
ate, refers to having more oxygen atoms.
ite, refers to having one less oxygen atom than ate.
Important to remember:
- Chlorate
- Nitrate
- Sulfate
- Carbonate
- Phosphate
Naming,
polyatomic ions with oxygen
………
Per-
means maximum amount of oxygen atoms
-ate
means 1 more oxygen atom than -ite
………
-ite
means 1 less oxygen atom than -ate
………
Hypo-
means one less oxygen atom than ite
= “Oxyanions”
………
4 oxygen atoms
3 oxygen atoms
2 oxygen atoms
1 oxygen atom
Forming Ionic Compounds
- Elements bond together, becoming ions and forming Neutral Compounds by transferring electrons.
- Ionic compounds form when a
Cation(metal) and Anion(non-metal) bond together.
- the Metal element loses electrons becoming positive.
- the Non-metal element gains electrons negative.
_________________________________________________________________________________________
Example showing valence electrons(dots) and bonding

+
(Sodium a neutral atom)
+
(chlorine a neutral atom)

+1
-1
(Na – Cl )
0
bond becoming ions and forming neutral compounds.
Naming Ionic Compounds:
Step 1 – write the name of the Metal first and the Non-metal second.
Step 2 - All Anion element names end in –ide
(drop the last 2-3 letters of the non-metal elements name and change it to “ide”)
- keep polyatomic names the same, do NOT change ate or ite.
……. Sodium Bromide
……. Calcium Chloride
7. Sodium nitride
8. Lithium Oxide
9. Strontium Flouride
10. Aluminum Sulfide
11. Cesium phosphide
Naming Transition Metals
- Transition metals always use roman numerals to indicate the charge on that ion
-
The Roman Numerals after the elements name indicate the positive charge on that element(ion).
Example = Fe +2 charge …….. Iron (II)
Fe +3 charge …….. Iron (III)
Fe +4 charge …….. Iron (IV)
Iron (II) chloride (FeCl2)
Writing Ionic Compound
Formulas:
Step 1 – write the name of the Metal first and the Non-metal second.
Step 2 - Make the Metals positive charge number, into a subscript for the Anion.
(ignore the sign of the charge!)
Step 3 - Make the Non-metals negative charge number, into a subscript for the Cation.
(ignore the sign of the charge)
short cut:
Criss-Cross the charges of both ions to make the compound neutral.
 Aluminum oxide
Step 4 - Reduce all subscripts to lowest whole number ratios.
Writing Ionic Compound
Formulas:
******* Remember Compounds want to be Neutral! **********
(above) Aluminum oxide
(below) Calcium phosphate
• NH4I
• Ammonium iodide
• NaBrO3
• Sodium bromate
• Mg(NO3)2
• Magnesium nitrate
• KHSO4
• Potassium hydrogen sulfate
• NH4ClO4
• Ammonium perchlorate
• Al(ClO)3
• Aluminum hypochlorite
• FeF2
• Iron(II) flouride
Naming
Bases
&
Acids
Bases:
• Bases are aqueous ionic compounds that contain Hydroxide ions.
(Dissolves in water)
• Bases release Hydroxide ions into solution (when dissolved in water).
• Naming Bases: (name like ionic compounds)
– All bases have names that end in hydroxide.
• NaOH
=
sodium hydroxide
• KOH
=
potassium hydroxide
• Ca(OH)2 =
calcium hydroxide
Acids:
Acids are aqueous compounds that release Hydrogen Ions into solution.
Hydrogen is always written 1st
in the chemical formula for all
The general formula for all acids
Example of Binary
acids
=
Acids.
HnX
Examples of oxy-acids
HCl
= Hydrochloric acid
HNO3
= nitric acid
HF
= Hydrofluoric acid
HNO2
= nitrous acid
HBr
= hydrobromic acid
HBrO3 = bromic acid
H2S
= Hydrosulfuric acid
HBrO2 = bromous acid
H2Se = Hydroselenic acid
H2SO4 = Sulfuric acid
H3N
= Hydronitric acid
H2SO3 = sulfurous acid
H3P
= Hydrophosphoric acid
H3PO4 = phosphoric acid
Binary Acids:
•
Is an acid that contains hydrogen and 1 other element.
Naming Binary acids:
1.
To name, add the prefix hydro- for the hydrogen part of the molecule.
2.
To the root of the second element name, add the suffix –ic followed by the word acid.
Example:
HCl
=
Hydrochloric acid
H2S
=
Hydrosulfuric acid
H3P
=
Hydrophosphoric acid
• Oxyacids are acids that contains hydrogen and an oxyanion.
Naming =
– 1st
– 2nd
write the root name of the polyatomic oxy-anion. (no hydro)
add to the ending of the root…
-ate
changes to
–ic acid
Nitrate  Nitric acid
-ite
changes to
-ous acid
Nitrite  Nitrous acid