NOMENCLATURE and FORMULAS
112
Elements
millions of
Compounds
____________
______________
made
described
made
described
of
by
of
by
___________
____________ ______________ _____________
Cations
Anions
I. Molecular Compounds
A. Molecule
1)
____________________________________________________________________________________________
2)
____________________________________________________________________________________________
3)
____________________________________________________________________________________________
Examples: Molecular compounds of like
atoms: ________________________ _________________________
H2
_______________
N2
_______________
O2
________________
F2
________________
Cl2
________________
Br2
________________
I2
________________
More examples: Molecular compounds of different atoms:
CO
_____________
H2O
_______________
SO2
_____________ NH3
_______________
N2O
_____________
HBr _______________
C6H12O6
_____________
______ Dinitrogen trioxide
B. Three ways to represent Molecular Compounds
1.________________________ - shows how many atoms of each type and
how they are positioned next to each other
Examples:
**2. ___________________ - show how many atoms of each type**
Examples:
3. ___________________ - reduced form of the molecular formula
Examples:
_______________
________________
H2O2
_______
C2H4
_______
CO2
_______
II. Ionic Compounds
A. Ionic Compound
- composed of positive ions (_________) and negative ions (________)
- ____________________________; contain equal number of positive and
negative charges
- usually consists of a ________________ and _________________
B. Only one way to represent Ionic Compounds
________________________- lowest whole number ratio of ions in an ionic compound
Examples:
sodium chloride
__________
________________
MgCl2
________________
Fe2O3
Calcium
bromide
_________
III. Three Important Laws
A.
B.
C.
_________________ ___________: number of protons =
number of electrons
_________________ ___________: have (or feel like they
have) filled outer shell of electrons
To become stable an ATOM will react with another ATOM
to:
1. __________________________ to form a
_______________(______________)
2. __________________________ to form a
_______________(______________)
3. __________________________ to form a
______________________________
IV. How and Why Ions are formed
A. Cations
B. Anions
ex. Na atom - in Group 1 of the periodic table
____ protons
____ electrons (1 in outer shell)
____ neutrons
Overall charge on a Na atom:
_______________________________________
What will the Na atom do?
A Na atom _________ its outer electron to become a stable ________.
____ protons
____ electrons
____ neutrons
Overall charge on a Na ion:
_________________________
Na ion = Na cation = Na+
ex. Cl atom - in _________ of the periodic table
___ protons
___ electrons (7 are in the outer shell)
Overall charge on a Cl atom:
___________________
What will a Cl atom do?
A Cl atom _________ an electron to become a stable _______.
___ protons
___ electrons
Overall charge on a Cl ion:
_______________________
Cl ion = Cl anion = Cl -
C. Ionic Bonds
1. Ionic bond -
____________________________________________________________________________
2. _______________ _____________ used to represent the formation of an
ionic bond
a. Using words
___________ + __________ ---->
________________
b. Using chemical formulas and symbols
________________________________________
where s = ___________
g =
___________
IV. Naming Monatomic Ions
______________________ _____________ - single atom
with a positive or negative charge because it has lost or gained one or
more electrons
Examples:
Na
-------> Na+
+ e-
_________ yields ________ and
1 electron
More Examples:
A. CATION:
________________________________________________________________________________________________
Note: A variable charge element needs a stock name or
classical name
B. ANION:
________________________________________________________________________________________________
Examples:
Cl
+ e-
------> Cl-
___________ + 1 electron ------> ____________
O
+ 2 e- ------>
O2-
__________ + 2 electrons ------>
__________
C. POLYATOMIC IONS: GROUPS OF ATOMS THAT ACT AS A UNIT AND CARRY A CHARGE
1. Some have -ITE
endings
SO3 2-
__________
NO2 - _________
2. Some have -ATE
endings
SO42 -
__________ NO3 - _________
3. Other examples:
NH4 + ______________
OH - ______________
Naming and Writing formulas for IONIC COMPOUNDS
I. BINARY Ionic Compounds
A. Constant charge metals
1. To name the ionic compound from the formula:
Name = __________________ +
__________________________
Examples:
NaCl ___________
AlCl3 ___________
2. To write the formula from the name of the compound:
To write the formula: apply the _________________________________: the
net ionic charge of the formula unit is _______
Examples:
name = Barium chloride
a. Balanced charges method
Ba2+
Cl-
___ (+2) + ___ (-1) = 0
b. Criss-Cross Method
Ba2+
Cl-
Ba
Cl
BaCl2
Note: No ionic charges in the formula
Subscripts tell how many of each ion
Calcium sulfide
Ca2+
S2-
Using balanced charges methods:
_____ (+2) + _____ (-2) = 0
CaS
Using criss-cross method:
Ca2+
S2-
Ca2S2 must reduce to CaS because
____________ is the
____________ whole-number ratio of ions in an
_______________
Magnesium nitride
Mg2+
N3-
Using balanced charges methods:
____(+2) + ____ (-3) = 0
Mg3N2
Using balanced charges methods:
Mg2+ N3-
Mg N
B. Variable charge metals
1. Four common variable charge metals:
Copper
Cu+
Cu2+
Iron
Fe2+
Fe3+
Tin
Sn2+
Sn4+
Lead
Pb2+
Pb4+
2. Two ways to name variable charge metals: ____________ and
____________
Ion
Stock name
Classical name
Cu+
______________________
Cuprous ion
Cu2+
Copper (II)
ion
____________________
Fe2+
Iron (II)
ion
____________________
Fe3+
________________________
Ferric ion
Sn2+
_____________________
Stannous ion
Sn4+
Tin (IV)
ion
_____________________
Pb2+
Lead (II)
ion
_____________________
Pb4+
______________________
Plumbic ion
What pattern do you see in naming using the Classical system?
___________________________________
___________________________________
Example:
Name the compound Fe2O3
O ion is a _____________ ion so its charge is ______
Fe ion is a _______________ ion: Is it _____ or _____ ?
Use ___________ to find out:
2 ( _____ ) + 3 (-2) = 0
2 ( 3 ) + 3 ( -2) = 0
So:
Stock name: _________________
Classical name: _________
Examples:
Name the ionic compound: Fe2S3
Balanced charges: 2 (____) + 3 (-2) = 0
So: _______
Name: ___________________
___________________
Name the compound: FeS
Balanced charges: 1 ( ____ ) + 1 ( -2 ) = 0
________________
________________
II. TERNARY Ionic Compounds
__________________ - a compound containing atoms of three different elements, usually containing at least one polyatomic ion
examples of ternary compounds:
Na2CO3
Mg(OH)2
A. To name the ternary ionic compound
Name = _________________ + __________________
Na2CO3
Mg(OH)2
B. To write the formula given the name
Examples:
Sodium nitrate:
Use balanced charges or criss-cross method:
_________
Sodium nitrite:
Barium nitrate:
Calcium phosphate
III. BINARY Molecular Compounds
__________________ - substance composed of two (or more) nonmetal
elements
A. To name a molecular compound given its formula
1) Use the names of the two elements in the formula
2) Use prefixes before the name of the element to tell the subscript of each element in the formula
3) Give the second element in the name the -ide ending
Prefixes Number
______ 1
______ 2
______ 3
______ 4
______ 5
______ 6
______ 7
______ 8
______ 9
______ 10
Some common molecular compounds:
C O 2 C
O N
2 O C
Cl 4
________________
___________________
____________________ ____________________
Compounds of carbon and oxygen:
Compounds of sulfur and oxygen:
Compounds of nitrogen and oxygen:
Examples: Name the following compounds.
Element name Number of atoms
Prefix
N2O
Nitrogen
2
di-
Oxygen
1
mono-
_______________
N2O5
Element name Number of atoms
Prefix
_________________ (note: the a in penta- becomes the o in oxide)
Element name Number of atoms
Prefix
OF2
_________________
Cl2O8
_________________ (note: a in octa- becomes octo-)
B. To write the formula given its name
1) Use the chemical symbols for the names of the elements
2) Use the prefixes to determine the subscripts of the elements
3) Do NOT use ionic charges (these are NOT ions)
Examples:
nitrogen triflouride
_______
disulfur dichloride
_______
dinitrogen tetroxide
_______
Name the following pairs of compounds:
1) PBr3 and CrBr3
2) N2O and Na2O
3) P2O3 and Fe2O3
III. Naming Common ACIDS
Properties of acids:
1) compounds that produce
___________________________ in solution
2) are _______________________
3) cause certain _________________ to change colors
4) react with ________________ to produce
__________________
5) react with compounds containing
____________________ to form water and a salt
6) _______________________
HCl (aq)
___________________
H2SO4 (aq) ___________________
HNO3 (aq) ___________________
HC2H3O2 (aq) ___________________
H3PO4 (aq) ___________________
H2CO3 (aq) ___________________
IV. Naming HYDRATES
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