Ionic Compound Formulation and Nomenclature
IONIC COMPOUND
IONIC COMPOUND
FORMULATION &
FORMULATION &
NOMENCLATURE
NOMENCLATURE
• All ionic compounds consist of two parts: a
cation
(a positive ion) and an
anion
(a negative ion).
• Ions are combined in simple, whole-number
ratios
to balance their
charges. This results in a
net charge
of
zero
, which all ionic compounds
MUST have.
• The “
cross technique
” is used to create the correct ratio of ions needed.
Example: aluminum (Al
+3
) and oxygen (O
-2
).
Al
O
+3
-2
1. Write the
symbols, then
write the charges
on each symbol
(from
ion list
)
2. Cross the charges,
dropping the
+
and
–
symbols
(
don’t write 1s
)
Al
O
2
3
Al
O
+3
-2
3. Clean up the
formula (completely
erase all charges)
and
reduce if
necessary
.
2
3
So when do you need to
reduce
?
•
Here’s two examples of when the ratio needs to be
reduced
:
Ca
O
+2
-2
Ca
O
2
2
C
C
a
a
O
O
Sn
S
+4
-2
Sn
S
2
4
S
S
n
n
S
S
2
2
2
•
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e
t
’
s
t
r
y
f
o
r
m
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l
a
t
i
n
g
s
o
m
e
c
o
m
p
o
u
n
d
s
(
p
u
t
t
i
n
g
t
h
e
m
t
o
g
e
t
h
e
r
)
:
•
Let’s try
formulating
some compounds (putting them together):
Let’s try
naming
some compounds:
MONATOMIC
1.
magnesium fluoride = ______________
2.
iron (III) bromide = ________________
3.
potassium chloride = ______________
4.
calcium chloride = ________________
5.
silver nitride = ____________________
6.
tin (II) sulfide = ___________________
7.
barium phosphide = _______________
8.
cobalt (III) oxide = _________________
9.
copper (I) iodide = _________________
10.
lead (IV) selenide= ________________
1.
FeO ___________________
2.
Al
2
O
3
__________________
3.
K
2
O____________________
4.
PbO
2
__________________
5.
K
2
S ___________________
6.
Mn
3
P
2
___________________
7.
Na
2
S____________________
8.
Ag
2
S
____________________
9.
Cu
3
N
____________________
10.
ZnCl
2
___________________
MgF
2
FeBr
3
KCl
CaCl
2
Ag
3
N
Mg
+2
F
-
Fe
+3
Br
-
K
+
Cl
-
Ca
+2
Cl
-
Ag
+
N
-3
•
Let’s try
formulating
some compounds (putting them together):
Let’s try
naming
some compounds:
MONATOMIC
1.
magnesium fluoride = ______________
2.
iron (III) bromide = ________________
3.
potassium chloride = ______________
4.
calcium chloride = ________________
5.
silver nitride = ____________________
6.
tin (II) sulfide = ___________________
7.
barium phosphide = _______________
8.
cobalt (III) oxide = _________________
9.
copper (I) iodide = _________________
10.
lead (IV) selenide= ________________
1.
FeO ___________________
2.
Al
2
O
3
__________________
3.
K
2
O____________________
4.
PbO
2
__________________
5.
K
2
S ___________________
6.
Mn
3
P
2
___________________
7.
Na
2
S____________________
8.
Ag
2
S
____________________
9.
Cu
3
N
____________________
10.
ZnCl
2
___________________
MgF
2
FeBr
3
KCl
CaCl
2
Ag
3
N
Sn
+2
S
-2
Ba
+2
P
-3
Co
+3
O
-2
Cu
+
I
-
Pb
+4
Se
-2
Sn
2
S
2
Ba
3
P
2
Co
2
O
3
CuI
Pb
2
Se
4
SnS
PbSe
2
• Ionic compounds are
named
with the following rules:
• The
cation
name goes first, the anion name goes
second
.
•
cations
are usually
metals
. The name of the cation does
not
change from the name of the element.
•
Note
: If the element is
polyionic
(meaning it can have more than
one type of charge), this must be indicated by placing a
roman
numeral
after the name to indicate the
size
of the charge.
•
anions
are a
single
negatively charged element
(monatomic)—name of element with ending taken off and
“-
ide
” added.
Zn
+2
= zinc
Sc
+3
= scandium
Fe
+2
= iron (II)
Fe
+3
= iron (III)
•
Let’s try
formulating
some compounds (putting them together):
Let’s try
naming
some compounds:
1.
magnesium fluoride = ______________
2.
iron (III) bromide = ________________
3.
potassium chloride = ______________
4.
calcium chloride = ________________
5.
silver nitride = ____________________
6.
tin (II) sulfide = ___________________
7.
barium phosphide = _______________
8.
cobalt (III) oxide = _________________
9.
copper (I) iodide = _________________
10.
lead (IV) selenide= ________________
1.
FeO ___________________
2.
Al
2
O
3
__________________
3.
K
2
O____________________
4.
PbO
2
__________________
5.
K
2
S ___________________
6.
Mn
3
P
2
___________________
7.
Na
2
S____________________
8.
Ag
2
S
____________________
9.
Cu
3
N
____________________
10.
ZnCl
2
___________________
MgF
2
FeBr
3
KCl
CaCl
2
Ag
3
N
Sn
2
S
2
Ba
3
P
2
Co
2
O
3
CuI
Pb
2
Se
4
SnS
PbSe
2
iron ( ) oxide
aluminum oxide
potassium oxide
lead ( ) oxide
potassium sulfide
II
IV
manganese ( ) phosphide
sodium sulfide
silver sulfide
copper ( ) nitride
zinc chloride
II
I
COVALENT BONDING
COVALENT BONDING
CHARACTERISTICS AND
CHARACTERISTICS AND
NOMENCLATURE
NOMENCLATURE
•
Covalent compounds
share
electrons, (ionic bonds transfer them).
•
Covalent bonds =
two nonmetals
,
or
a
nonmetal
and a
metalloid
.
•
Remember,
hydrogen
is
not
an alkali metal, it is a nonmetal.
•
Remember,
ionic
bonds always contain a
metal
. Metals
never
appear in
covalent compounds!!!
•
Covalent bonds rely on the “
octet rule
,” meaning that atoms in a
covalent bond need
8
electrons
around them (in most cases).
•
covalent bonds can be
single
,
double
, or
triple
, in order to satisfy the
octet rule.
•
Lewis-dot structures
show the arrangement of these eight electrons
F
F C F
O C O
N N
F
4 single
bonds
2 double
bonds
1 triple
bond
•
covalent compounds can involve the same elements with multiple
ratios (such as C
3
H
8
, C
2
H
4
, NO
2
, N
2
O), so the ratio in the compound
must be shown in the name.
•
to write the name of a covalent compound, we use
Greek prefixes
:
•
attach the appropriate
prefix
to the name of each
element in the compound.
(Note: if the
first
element in the compound is
single
, you do
not
need
the prefix “
mono-
.” “Mono-” is only used on the
second
element!)
•
the
ending
of the
second
element’s name is taken off,
and
“-ide”
is added.
•
if you get any of the following
vowel combinations
in
the name when you add the prefix:
“oo,” “ao,”
“oa,”
or
“aa,”
that’s not allowed!
Drop
the vowel off
of the
prefix
, and then add it to the name.
•
for
diatomic gases
, like O
2
, name the
element
, then
add the word “
gas
.” Therefore, O
2
=
oxygen gas
•
Let’s try a few:
1.
C
2
N
6
= _____________________
2.
P
3
O
7
= _____________________
3.
H
2
O = ______________________
4.
B
5
As = ______________________
5.
N
2
= _______________________
6.
trisulfur tetrachloride = ___________
7.
carbon monoxide = ___________
8.
chlorine gas = ____________
9.
silicon pentabromide = ___________
10.
tetrachlorine decabromide = ___________
Can you
tell the difference
between an
ionic
compound and
a
covalent
compound based on the name or formula alone?
You need to be able to do so!
Place an “I” or a “C” in the blank:
1.
Fe
3
N
2
2.
K
2
S
3.
NH
3
4.
Br
2
5.
Mn
2
O
3
6.
CaO
7.
Li
2
O
8.
carbon dioxide
9.
aluminum nitride
10.
tin (II) sulfide
11.
chlorine gas
12.
calcium sulfide
13.
cobalt (III) oxide
14.
sodium phosphide
___
___
___
___
___
___
___
___
___
___
___
___
___
___
I
I
C
C
I
I
I
C
I
I
C
I
I
I
Ionic compounds consist of cations and anions combined in simple ratios to balance charges. The cross technique helps determine the correct ratio of ions. Reduction of ratios may be necessary in certain cases. Formulation and naming examples are provided to illustrate these concepts.
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Presentation Transcript
IONIC COMPOUND FORMULATION & NOMENCLATURE
All ionic compounds consist of two parts: a cation (a positive ion) and an anion (a negative ion). Ions are combined in simple, whole-number ratios to balance their charges. This results in a net charge of zero, which all ionic compounds MUST have. The cross technique is used to create the correct ratio of ions needed. Example: aluminum (Al+3) and oxygen (O-2). AlO 1. Write the symbols, then write the charges on each symbol (from ion list) +3 -2 +3 -2 Al O 2 3 3. Clean up the formula (completely erase all charges) and reduce if necessary. AlO 2 3 2. Cross the charges, dropping the + and symbols (don t write 1s) So when do you need to reduce?
Heres two examples of when the ratio needs to be reduced: +2 -2CaO -2SnS CaO SnS 22CaO 24SnS2 2 +4 Let s try formulating some compounds (putting them together):
Lets try formulating some compounds (putting them together): MgF2 FeBr3 KCl CaCl2 Ag3N Mg+2F- Fe+3Br- Ca+2Cl- 6. tin (II) sulfide = ___________________ 7. barium phosphide = _______________ 8. cobalt (III) oxide = _________________ 9. copper (I) iodide = _________________ 10. lead (IV) selenide= ________________ K+Cl- Ag+N-3 1. magnesium fluoride = ______________ 2. iron (III) bromide = ________________ 3. potassium chloride = ______________ 4. calcium chloride = ________________ 5. silver nitride = ____________________ Let s try naming some compounds: 1. FeO ___________________ 6. Mn3P2 ___________________ 2. Al2O3 __________________ 7. Na2S____________________ 3. K2O____________________ 8. Ag2S____________________ 4. PbO2 __________________ 9. Cu3N____________________ 5. K2S ___________________ 10.ZnCl2 ___________________ MONATOMIC
Lets try formulating some compounds (putting them together): MgF2 FeBr3 KCl CaCl2 Ag3N Sn+2S-2 Ba+2P-3 Cu+I- Sn2S2 Ba3P2 Co2O3 CuI Pb2Se4 PbSe2 SnS 6. tin (II) sulfide = ___________________ 7. barium phosphide = _______________ 8. cobalt (III) oxide = _________________ 9. copper (I) iodide = _________________ 10. lead (IV) selenide= ________________ Co+3O-2 Pb+4Se-2 1. magnesium fluoride = ______________ 2. iron (III) bromide = ________________ 3. potassium chloride = ______________ 4. calcium chloride = ________________ 5. silver nitride = ____________________ Let s try naming some compounds: 1. FeO ___________________ 6. Mn3P2 ___________________ 2. Al2O3 __________________ 7. Na2S____________________ 3. K2O____________________ 8. Ag2S____________________ 4. PbO2 __________________ 9. Cu3N____________________ 5. K2S ___________________ 10.ZnCl2 ___________________ MONATOMIC
Ionic compounds are named with the following rules: The cation name goes first, the anion name goes second. cations are usually metals. The name of the cation does not change from the name of the element. Zn+2 = zinc Sc+3 = scandium Fe+2 = iron (II) Fe+3 = iron (III) Note: If the element is polyionic (meaning it can have more than one type of charge), this must be indicated by placing a roman numeral after the name to indicate the size of the charge. anions are a single negatively charged element (monatomic) name of element with ending taken off and -ide added.
Lets try formulating some compounds (putting them together): 1. magnesium fluoride = ______________ 2. iron (III) bromide = ________________ 3. potassium chloride = ______________ 4. calcium chloride = ________________ 5. silver nitride = ____________________ Ag3N Sn2S2 Ba3P2 Co2O3 CuI PbSe2 SnS MgF2 6. tin (II) sulfide = ___________________ 7. barium phosphide = _______________ 8. cobalt (III) oxide = _________________ 9. copper (I) iodide = _________________ 10. lead (IV) selenide= ________________ Pb2Se4 FeBr3 KCl CaCl2 1. FeO ___________________ iron ( ) oxide II manganese ( ) phosphide II Let s try naming some compounds: 2. Al2O3 __________________ aluminum oxide potassium oxide lead ( ) oxide potassium sulfide 6. Mn3P2 ___________________ sodium sulfide silver sulfide copper ( ) nitride zinc chloride 7. Na2S____________________ 3. K2O____________________ IV 8. Ag2S____________________ I 4. PbO2 __________________ 9. Cu3N____________________ 5. K2S ___________________ 10.ZnCl2 ___________________
COVALENT BONDING CHARACTERISTICS AND NOMENCLATURE
Covalent compounds share electrons, (ionic bonds transfer them). Covalent bonds = two nonmetals, or a nonmetal and a metalloid. Remember, hydrogen is not an alkali metal, it is a nonmetal. Remember, ionic bonds always contain a metal. Metals never appear in covalent compounds!!! Covalent bonds rely on the octet rule, meaning that atoms in a covalent bond need 8 electrons around them (in most cases). covalent bonds can be single, double, or triple, in order to satisfy the octet rule. CF4 CO2 F F C F O C O N N F N2 1 triple bond 4 single 2 double bonds Lewis-dot structures show the arrangement of these eight electrons bonds
covalent compounds can involve the same elements with multiple ratios (such as C3H8, C2H4, NO2, N2O), so the ratio in the compound must be shown in the name. to write the name of a covalent compound, we use Greek prefixes: attach the appropriate prefix to the name of each element in the compound. (Note: if the first element in the compound is single, you do not need the prefix mono-. Mono- is only used on the second element!) the ending of the secondelement s name is taken off, and -ide is added. if you get any of the following vowel combinations in the name when you add the prefix: oo, ao, oa, or aa, that s not allowed! Drop the vowel off of the prefix, and then add it to the name. for diatomic gases, like O2, name the element, then add the word gas. Therefore, O2 = oxygen gas # 1 2 3 4 5 6 7 8 9 Prefix mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- 10
Lets try a few: C2N6 = _____________________ dicarbon hexanitride triphosphorus heptaoxide dihydrogen monooxide pentaboron monoarsenide nitrogen gas 1. no AO combo! no OO combo! no OA combo! heptoxide monoxide monarsenide (diatomic gas!) 2. P3O7 = _____________________ H2O = ______________________ 3. 4. B5As = ______________________ N2 = _______________________ 5. S3Cl4 6. trisulfur tetrachloride = ___________ CO carbon monoxide = ___________ 7. Cl2(diatomic gas!) 8. chlorine gas = ____________ SiBr5 9. silicon pentabromide = ___________ Cl4Br10 10. tetrachlorine decabromide = ___________
Can you tell the difference between an ionic compound and a covalent compound based on the name or formula alone? You need to be able to do so! Place an I or a C in the blank: 1.Fe3N2 2.K2S 3.NH3 4.Br2 5.Mn2O3 6.CaO 7.Li2O ___ ___ I I C C I C I I C I ___ ___ ___ ___ ___ ___ I I ___ ___ ___ ___ ___ ___ I I 8. carbon dioxide 9. aluminum nitride 10.tin (II) sulfide 11.chlorine gas 12.calcium sulfide 13.cobalt (III) oxide 14.sodium phosphide
