Chemistry
Chapter 9 – Chemical Names & Formulas Notes
Name ________________________
Date _________________________
Reminders



____________________ indicate how many atoms of an element are present.
o H2O = 2 Hydrogen, 1 Oxygen
o CO2 = 1 Carbon, 2 Oxygen
Note that subscripts only apply to the letter next to them (unless there are parentheses).
Cations (formed by metals) and anions (formed by nonmetals) attract one another and form
___________________ bonds.
Binary Ionic Compounds


Binary means a compound contains ____________ elements.
Ionic compounds are formed between a ____________________ and a ___________________.
Naming Binary Ionic Compounds
 Elements to Formulas
Example
Potassium and Fluorine
o Identify cation/anion (with charges)
o ___________________________________ are necessary for transition & other
multivalent metals!
o Put the __________________ symbol first, then the __________________.
o Drop & Cross to balance charges.
o Practice:
 Calcium and Bromine

Copper(II) and Oxygen

Lithium and Sulfur

Mercury(I) and Oxygen

Aluminum and Chlorine

Lead(IV) and Sulfur

Potassium and Sulfur

Beryllium and Bromine

Cobalt(II) and Phosphorus

Tin(IV) and Chlorine
 Formulas to Names
Example
KF
o Write the name of the ______________
 Uncross to find the Roman numerals with transition & multivalent metals.
o Write the name of the anion.
 Drop the ending
 Add _____________.
o Practice:
 CaBr2

Hg2O

NaCl

CoCl2

AlCl3

K2S

CrCl2

Na3P
Naming Ternary Ionic Compounds
 Elements/Polyatomics to Formulas
Example
Sodium and Carbonate
o Identify cation/anion (with charges)
o Identify the polyatomic ion (with charges)
o Put the __________________ or ______________________________symbol first, then
the __________________ or ___________________________________.
o Drop & Cross to balance charges.
 Put polyatomics in ( ) if more than 1.
o Practice:
 Ammonium and Oxygen

Potassium and Nitrate

Lead(IV) and Dichromate

Calcium and Hydroxide

Lithium and Sulfate

Calcium and Permanganate

Sodium and Chlorate

Magnesium and Phosphate
 Formulas to Names
Example
Na2CO3
o Look for the polyatomic – it can be first or second!
 Uncross to find charge of the polyatomic ion or the Roman numerals with
transition & multivalent metals.
o Write the name.
 If the polyatomic is 1st, end the anion with –ide
 If the polyatomic is 2nd, cation is written as normal and polyatomic is normal
o Practice:
 NH4Cl

KNO3

Ca(OH)2

Pb(Cr2O7)2

Li2SO4

Ca(MnO4)2

NaClO3

Mg3(PO4)2
 All Ionic Practice
o NaOH
o Beryllium Sulfate
o Tin(II) Iodide
o Aluminum Cyanide
o Zinc Hydroxide
o Co3N2
o Ag2SO3
o Mg3P2
o Beryllium Acetate
o Fe3N2
o Ga(NO2)3
o Silver Sulfide
Acids
 Formula to Name
o All acids contain 1 or more H atoms.
o H will be the first element listed!
Example
HCl
o If the anion ends with –ide (halogens)
 Acid name begins with _______________
 Stem of anion ends with __________
 End the name by writing __________
 Example:
o If polyatomics are present
 _____________ endings become ____________, followed by ____________.
 Example:
 ______________ endings become ____________, followed by ____________.
 Example:
 Names to Formulas
o H will be the first element listed!
 List H with a ___________ charge.
o Identify the anion (halogen or polyatomic)
 Write the formula with charge
o Drop & Cross
 Example:
o Practice:
 Bromic Acid

Hydroiodic Acid

Carbonous Acid

Nitrous Acid
 All Acid Practice
o H2CO3
o Hydroiodic acid
o HC2H3O2
o HBr
o Chloric acid
o H2CO3
o Hydrofluoric acid
o H3PO3
Example
Nitric acid
Binary Molecular Compounds




Binary means a compound contains ____________ elements.
Molecular compounds are formed between a ____________________ and a
___________________.
o Not IONS – No Charges!
_____________________ are used to indicate how many atoms of an element are present in the
compound.
Prefixes to Memorize
Prefix
Meaning
Mono –
1
Di –
2
Tri –
3
Tetra –
4
Penta –
5
Hexa –
6
Hepta –
7
Octa –
8
Nona –
9
Deca –
10
Naming Binary Molecular Compounds
 Formula to Name
Example
CO
o Confirm that the two elements are
nonmetals
o Name the 1st element
 If only 1 of the 1st element omit prefix
 If more than 1 of the 1st element use prefix
o Name the 2nd element (the more EN element)
 Always use a prefix
 Add -ide ending
o Practice:
 N2O4

SO3

NO

NO2

As2O5

PCl3

CCl4

SeF6
 Name to Formula
Example
Dinitrogen monoxide
o Write the symbol for the first element
 The prefix tells you what to write as a subscript
 If no prefix, the element symbol will not have a subscript
o Write the symbol for the second element
 The prefix tells you what to write as the subscript
o Practice:
 Dinitrogen triiodide

Diphosphorus pentoxide

Dinitrogen monoxide

Silicon dioxide

Carbon tetrabromide

Sulfur dioxide

Phosphorus pentabromide

Iodine trichloride
 All Molecular Practice
o PCl3
o Diphosphorus trioxide
o SF6
o Carbon dioxide
o C2H6
o CCl4
o Dichlorine octoxide
o N2O