Names and Formulas
of Ionic and Covalent
Compounds
Ionic Compounds
Ionic Compounds
Names of some Ionic Compounds
• Magnesium phosphide
• Calcium bromide
• Lithium nitride
• Silver sulphide
• Lithium oxide
• Potassium chloride
Ionic Compounds
Formulas of some Ionic Compounds
• AlBr3
• MgBr2
• Na2O
• RbF
• CsF
• AgI
Ionic Compounds
Ionic Compounds
• I.C’s are always made of positive ions (cations)
and negative ions (anions).
Ionic Compounds
• I.C’s are always made of positive ions (cations)
and negative ions (anions).
• The positive ions is always first in the name
and formula.
Ionic Compounds
• I.C’s are always made of positive ions (cations)
and negative ions (anions).
• The positive ions is always first in the name
and formula.
• The positive ion is always a metal
Ionic Compounds
• I.C’s are always made of positive ions (cations)
and negative ions (anions).
• The positive ions is always first in the name
and formula.
• The positive ion is always a metal
• The second part is always a non-metal.
Ionic Compounds
• I.C’s are always made of positive ions (cations)
and negative ions (anions).
• The positive ions is always first in the name
and formula.
• The positive ion is always a metal.
• The second part is always a non-metal.
• The non-metal is always a negative ion.
Ionic Compounds
• I.C’s are always made of positive ions (cations)
and negative ions (anions).
• The positive ions is always first in the name
and formula.
• The positive ion is always a metal.
• The second part is always a non-metal.
• The non-metal is always a negative ion.
• The non-metal’s name always ends in “ide”
Ionic Compounds
Names of some Ionic Compounds
• Magnesium phosphide
• Calcium bromide
• Lithium nitride
• Silver sulphide
• Lithium oxide
• Potassium chloride
Ionic Compounds
Names of some Ionic Compounds
• Magnesium phosphide
• Calcium bromide
• Lithium nitride
• Silver sulphide
• Lithium oxide
• Potassium chloride
METALS
Ionic Compounds
Names of some Ionic Compounds
• Magnesium phosphide
• Calcium bromide
• Lithium nitride
• Silver sulphide
• Lithium oxide
• Potassium chloride
METALS
NON-METALS
Ionic Compounds
Names of some Ionic Compounds
• Magnesium phosphide
• Calcium bromide
• Lithium nitride
• Silver sulphide
• Lithium oxide
• Potassium chloride
METALS
NON-METALS
Ionic Compounds
Names of some Ionic Compounds
• Magnesium phosphide
• Calcium bromide
• Lithium nitride
“IDE” ENDING
• Silver sulphide
• Lithium oxide
• Potassium chloride
METALS
NON-METALS
Lesson 1
Lesson 1
Formula
Name
Lesson 1
Formula
Name
(The easy part)
Steps to naming Ionic Compounds
Steps to naming Ionic Compounds
Steps
Example
CaI2
Steps to naming Ionic Compounds
Steps
1. Name the metal ion
Example
CaI2
Steps to naming Ionic Compounds
Steps
1. Name the metal ion
Example
CaI2
• Ca is calcium
Steps to naming Ionic Compounds
Steps
1. Name the metal ion
2. Name the non-metal
ion and end the name
with “ide”
Example
CaI2
• Ca is calcium
Steps to naming Ionic Compounds
Steps
1. Name the metal ion
2. Name the non-metal
ion and end the name
with “ide”
Example
CaI2
• Ca is calcium
• I is iodine. Adding “ide”
gives iodide
Steps to naming Ionic Compounds
Steps
1. Name the metal ion
2. Name the non-metal
ion and end the name
with “ide”
3. Write the name of the
compound.
Example
CaI2
• Ca is calcium
• I is iodine. Adding “ide”
gives iodide
Steps to naming Ionic Compounds
Steps
1. Name the metal ion
2. Name the non-metal
ion and end the name
with “ide”
3. Write the name of the
compound.
Example
CaI2
• Ca is calcium
• I is iodine. Adding “ide”
gives iodide
• Calcium iodide
Try these
Try these
Formula
Name
Try these
Formula
• Li3N
Name
Try these
Formula
• Li3N
Name
• Lithium nitride
Try these
Formula
• Li3N
• Sr3P2
Name
• Lithium nitride
Try these
Formula
• Li3N
• Sr3P2
Name
• Lithium nitride
• Strontium phosphide
Try these
Formula
• Li3N
• Sr3P2
• AlBr3
Name
• Lithium nitride
• Strontium phosphide
Try these
Formula
• Li3N
• Sr3P2
• AlBr3
Name
• Lithium nitride
• Strontium phosphide
• Aluminum bromide
Try these
Formula
• Li3N
• Sr3P2
• AlBr3
• AgI
Name
• Lithium nitride
• Strontium phosphide
• Aluminum bromide
Try these
Formula
• Li3N
• Sr3P2
• AlBr3
• AgI
Name
• Lithium nitride
• Strontium phosphide
• Aluminum bromide
• Silver iodide
Try these
Formula
• Li3N
• Sr3P2
• AlBr3
• AgI
• CaI2
• MgBr2
• CsF
Name
• Lithium nitride
• Strontium phosphide
• Aluminum bromide
• Silver iodide
Try these
Formula
• Li3N
• Sr3P2
• AlBr3
• AgI
• CaI2
• MgBr2
• CsF
Name
• Lithium nitride
• Strontium phosphide
• Aluminum bromide
• Silver iodide
• Calcium iodide
• Magnesium bromide
• Cesium fluoride
Lesson 2
Lesson 2
Name
Formula
Lesson 2
Name
Formula
(The slightly harder part)
Steps to writing Formulas of Ionic
Compounds
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
Steps to writing Formulas of Ionic
Compounds
Steps
1. Identify each ion and its
charge.
Example aluminum fluoride
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
1. Identify each ion and its
charge.
• Al3+
and
F1-
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
1. Identify each ion and its
charge.
2. Determine total charges
needed to balance (+) and
(-)
• Al3+
and
F1-
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
1. Identify each ion and its
charge.
2. Determine total charges
needed to balance (+) and
(-)
• Al3+
and
• Al3+
F1- F1- F1-
F1-
= +3
= -3
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
1. Identify each ion and its
charge.
2. Determine total charges
needed to balance (+) and
(-)
3. Note ratio of (+) and (-)
• Al3+
and
• Al3+
F1- F1- F1-
F1-
= +3
= -3
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
1. Identify each ion and its
charge.
2. Determine total charges
needed to balance (+) and
(-)
3. Note ratio of (+) and (-)
• Al3+
and
F1-
• Al3+
= +3
F1- F1- F1= -3
• 1 Al3+ for every 3 F1-
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
1. Identify each ion and its
• Al3+ and F1charge.
2. Determine total charges
• Al3+
= +3
needed to balance (+) and
F1- F1- F1= -3
(-)
• 1 Al3+ for every 3 F13. Note ratio of (+) and (-)
4. Use subscripts to write the
formula.
Steps to writing Formulas of Ionic
Compounds
Steps
Example aluminum fluoride
1. Identify each ion and its
• Al3+ and F1charge.
2. Determine total charges
• Al3+
= +3
needed to balance (+) and
F1- F1- F1= -3
(-)
• 1 Al3+ for every 3 F13. Note ratio of (+) and (-)
4. Use subscripts to write the
formula.
AlF
3
Steps to writing Formulas of Ionic
Compounds
Steps
Example magnesium nitride
Steps to writing Formulas of Ionic
Compounds
Steps
1. Identify each ion and its
charge.
Example magnesium nitride
Steps to writing Formulas of Ionic
Compounds
Steps
1. Identify each ion and its
charge.
Example magnesium nitride
• Mg2+ and N3-
Steps to writing Formulas of Ionic
Compounds
Steps
1. Identify each ion and its
charge.
2. Determine total charges
needed to balance (+) and
(-)
Example magnesium nitride
• Mg2+ and N3-
Steps to writing Formulas of Ionic
Compounds
Steps
1. Identify each ion and its
charge.
2. Determine total charges
needed to balance (+) and
(-)
Example magnesium nitride
• Mg2+ and N3• Mg2+ Mg2+ Mg2+
= +6
Steps to writing Formulas of Ionic
Compounds
Steps
Example magnesium nitride
1. Identify each ion and its
• Mg2+ and N3charge.
• Mg2+ Mg2+ Mg2+
= +6
2. Determine total charges
N3- N3= -6
needed to balance (+) and
(-)
Steps to writing Formulas of Ionic
Compounds
Steps
Example magnesium nitride
1. Identify each ion and its
• Mg2+ and N3charge.
• Mg2+ Mg2+ Mg2+
= +6
2. Determine total charges
N3- N3= -6
needed to balance (+) and
(-)
3. Note ratio of (+) and (-)
Steps to writing Formulas of Ionic
Compounds
Steps
Example magnesium nitride
1. Identify each ion and its
• Mg2+ and N3charge.
• Mg2+ Mg2+ Mg2+
= +6
2. Determine total charges
N3- N3= -6
needed to balance (+) and
(-)
3. Note ratio of (+) and (-)
• 3 Mg2+ for every 2 N3-
Steps to writing Formulas of Ionic
Compounds
Steps
Example magnesium nitride
1. Identify each ion and its
• Mg2+ and N3charge.
• Mg2+ Mg2+ Mg2+
= +6
2. Determine total charges
N3- N3= -6
needed to balance (+) and
(-)
3. Note ratio of (+) and (-)
• 3 Mg2+ for every 2 N34. Use subscripts to write the
formula.
Steps to writing Formulas of Ionic
Compounds
Steps
Example magnesium nitride
1. Identify each ion and its
• Mg2+ and N3charge.
• Mg2+ Mg2+ Mg2+
= +6
2. Determine total charges
N3- N3= -6
needed to balance (+) and
(-)
3. Note ratio of (+) and (-)
• 3 Mg2+ for every 2 N34. Use subscripts to write the
formula.
Mg3N2
Or, the totally cheating
cross-over method!
Or, the totally cheating
cross-over method!
Al3+ F1-
Or, the totally cheating
cross-over method!
Al3+ F1-
Or, the totally cheating
cross-over method!
Al3+ F1-
Or, the totally cheating
cross-over method!
Al3+ F1-
Or, the totally cheating
cross-over method!
Al3+ F1-
Or, the totally cheating
cross-over method!
Al3+ F1-
Or, the totally cheating
cross-over method!
Al3+ F1-
AlF3
(we never write the 1)
Or, the totally cheating
cross-over method!
2+
3Mg N
Or, the totally cheating
cross-over method!
2+
3Mg N
Or, the totally cheating
cross-over method!
2+
3Mg N
Or, the totally cheating
cross-over method!
2+
3Mg N
Or, the totally cheating
cross-over method!
2+
3Mg N
Or, the totally cheating
cross-over method!
2+
3Mg N
Or, the totally cheating
cross-over method!
2+
3Mg N
Mg3N2
Try These!
Try These!
Na+ BrZn2+ IAl3+ S2Ca2+ O2Al3+ P3-
Try These!
Na+ BrZn2+ IAl3+ S2Ca2+ O2Al3+ P3-
NaBr (remember – don’t write 1’s)
Try These!
Na+ BrZn2+ IAl3+ S2Ca2+ O2Al3+ P3-
NaBr (remember – don’t write 1’s)
ZnI2
Try These!
Na+ BrZn2+ IAl3+ S2Ca2+ O2Al3+ P3-
NaBr (remember – don’t write 1’s)
ZnI2
Al2S3
Try These!
Na+ BrZn2+ IAl3+ S2Ca2+ O2Al3+ P3-
NaBr (remember – don’t write 1’s)
ZnI2
Al2S3
CaO
Try These!
Na+ BrZn2+ IAl3+ S2Ca2+ O2Al3+ P3-
NaBr (remember – don’t write 1’s)
ZnI2
Al2S3
CaO Ca2O2
Try These!
Na+ BrZn2+ IAl3+ S2Ca2+ O2Al3+ P3-
NaBr (remember – don’t write 1’s)
ZnI2
Al2S3
CaO Ca2O2
AlP
Al3P3
Okay, now that you are an expert
write the formula for…
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Cobalt (III) oxide
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Cobalt (III) oxide
• These are multivalent
ions – they have more
than one ionic charge.
The (number) tells you
which one it is.
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Cobalt (III) oxide
• These are multivalent
ions – they have more
than one ionic charge.
The (number) tells you
which one it is.
• Mn4+ S2-
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Cobalt (III) oxide
• These are multivalent
ions – they have more
than one ionic charge.
The (number) tells you
which one it is.
• Mn4+ S2-
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Cobalt (III) oxide
• These are multivalent
ions – they have more
than one ionic charge.
The (number) tells you
which one it is.
• Mn4+ S2-
MnS2
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Mn4+ S2-
• Cobalt (III) oxide
• These are multivalent
ions – they have more
than one ionic charge.
The (number) tells you
which one it is.
• Co3+ O2-
MnS2
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Mn4+ S2-
• Cobalt (III) oxide
• These are multivalent
ions – they have more
than one ionic charge.
The (number) tells you
which one it is.
• Co3+ O2-
MnS2
Okay, now that you are an expert
write the formula for…
• Manganese (IV)
sulphide
• Mn4+ S2-
MnS2
• Cobalt (III) oxide
• These are multivalent
ions – they have more
than one ionic charge.
The (number) tells you
which one it is.
• Co3+ O2-
Co2O3
Steps for writing the name of
multivalent compounds
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
Steps for writing the name of
multivalent compounds
Steps
1. Is the metal multivalent?
Example
Au3N
Steps for writing the name of
multivalent compounds
Steps
Example
1. Is the metal multivalent?
1. Yes
Au3N
Steps for writing the name of
multivalent compounds
Steps
Example
1. Is the metal multivalent?
2. Determine ion charges
1. Yes
Au3N
Steps for writing the name of
multivalent compounds
Steps
Example
1. Is the metal multivalent?
2. Determine ion charges
1. Yes
2. Au+ and Au3+
Au3N
Steps for writing the name of
multivalent compounds
Steps
Example
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
1. Yes
2. Au+ and Au3+
Au3N
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
4. Find the charge of the
negative ion
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
4. Find the charge of the
negative ion
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
4. N3-
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
4. Find the charge of the
negative ion
5. The pos. and neg. must
balance out.
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
4. N3-
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
4. Find the charge of the
negative ion
5. The pos. and neg. must
balance out.
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
4. N35. For 3 Au to balance 1 N3the Au must be Au1-
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
4. Find the charge of the
negative ion
5. The pos. and neg. must
balance out.
6. Write the name
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
4. N35. For 3 Au to balance 1 N3the Au must be Au1-
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
4. Find the charge of the
negative ion
5. The pos. and neg. must
balance out.
6. Write the name
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
4. N35. For 3 Au to balance 1 N3the Au must be Au16. Gold (I) nitride
Steps for writing the name of
multivalent compounds
Steps
Example
Au3N
1. Is the metal multivalent?
2. Determine ion charges
3. Determine the ratio of ions
in the formula
4. Find the charge of the
negative ion
5. The pos. and neg. must
balance out.
6. Write the name
1. Yes
2. Au+ and Au3+
3. Au3N means 3 Au for every
1N
4. N35. For 3 Au to balance 1 N3the Au must be Au16. Gold (I) nitride
Roman
Numeral
Polyatomic Ions
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
• Examples:
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
• Examples:
 CO32-
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
• Examples:
 CO32- carbonate
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
• Examples:
 CO32- carbonate
 PO43-
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
• Examples:
 CO32- carbonate
 PO43- phosphate
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
• Examples:
 CO32- carbonate
 PO43- phosphate
 Cr2O72-
Polyatomic Ions
• Polyatomic ions are ions made of more than
one type of atom.
• Examples:
 CO32- carbonate
 PO43- phosphate
 Cr2O72- dichromate
Writing Formulas of
Polyatomic Ions
Writing Formulas of
Polyatomic Ions
Steps
manganese (III) chlorate
Writing Formulas of
Polyatomic Ions
Steps
1. Identify each ion and charge
manganese (III) chlorate
Writing Formulas of
Polyatomic Ions
Steps
1. Identify each ion and charge
manganese (III) chlorate
1. Mn3+ ClO3-
Writing Formulas of
Polyatomic Ions
Steps
manganese (III) chlorate
1. Identify each ion and charge 1. Mn3+ ClO32. Determine total charges
needed to balance (+) and (-)
Writing Formulas of
Polyatomic Ions
Steps
manganese (III) chlorate
1. Identify each ion and charge 1. Mn3+ ClO32. Determine total charges
2. Mn3+
needed to balance (+) and (-)
ClO3- ClO3- ClO3-
= 3+
= 3-
Writing Formulas of
Polyatomic Ions
Steps
manganese (III) chlorate
1. Identify each ion and charge 1. Mn3+ ClO32. Determine total charges
2. Mn3+
needed to balance (+) and (-)
ClO3- ClO3- ClO33. Find ratio of ions
= 3+
= 3-
Writing Formulas of
Polyatomic Ions
Steps
manganese (III) chlorate
1. Identify each ion and charge 1. Mn3+ ClO32. Determine total charges
2. Mn3+
= 3+
needed to balance (+) and (-)
ClO3- ClO3- ClO3= 33. Find ratio of ions
3. 1 Mn3+ for every 3 ClO3-
Writing Formulas of
Polyatomic Ions
Steps
manganese (III) chlorate
1. Identify each ion and charge 1. Mn3+ ClO32. Determine total charges
2. Mn3+
= 3+
needed to balance (+) and (-)
ClO3- ClO3- ClO3= 33. Find ratio of ions
3. 1 Mn3+ for every 3 ClO34. Use brackets around ions to
show ratio.
Writing Formulas of
Polyatomic Ions
Steps
1. Identify each ion and charge
2. Determine total charges
needed to balance (+) and (-)
3. Find ratio of ions
4. Use brackets around ions to
show ratio.
manganese (III) chlorate
1. Mn3+ ClO32. Mn3+
= 3+
ClO3- ClO3- ClO3= 33. 1 Mn3+ for every 3 ClO34. (Mn)1(ClO3)3
Writing Formulas of
Polyatomic Ions
Steps
1. Identify each ion and charge
2. Determine total charges
needed to balance (+) and (-)
3. Find ratio of ions
4. Use brackets around ions to
show ratio.
5. Omit brackets if only one ion
is needed.
manganese (III) chlorate
1. Mn3+ ClO32. Mn3+
= 3+
ClO3- ClO3- ClO3= 33. 1 Mn3+ for every 3 ClO34. (Mn)1(ClO3)3
Writing Formulas of
Polyatomic Ions
Steps
1. Identify each ion and charge
2. Determine total charges
needed to balance (+) and (-)
3. Find ratio of ions
4. Use brackets around ions to
show ratio.
5. Omit brackets if only one ion
is needed.
manganese (III) chlorate
1. Mn3+ ClO32. Mn3+
= 3+
ClO3- ClO3- ClO3= 33. 1 Mn3+ for every 3 ClO34. (Mn)1(ClO3)3
5.
Mn(ClO3)3
Writing Formulas of
Polyatomic Ions
Name
Formula
Writing Formulas of
Polyatomic Ions
Name
Formula
1. Sodium chromate
1.
2.
2. Fe(OH)3
3.
3. Ca(HCO3)2
4. lead (II) perchlorate
4.
5.
5. (NH4)3PO4
6. ammonium nitrate
6.
Writing Formulas of
Polyatomic Ions
Name
Formula
1. Sodium chromate
1. Na2CrO4
2.
2. Fe(OH)3
3.
3. Ca(HCO3)2
4. lead (II) perchlorate
4.
5.
5. (NH4)3PO4
6. ammonium nitrate
6.
Writing Formulas of
Polyatomic Ions
Name
Formula
1. Sodium chromate
1. Na2CrO4
2. Iron (III) hydroxide
2. Fe(OH)3
3.
3. Ca(HCO3)2
4. lead (II) perchlorate
4.
5.
5. (NH4)3PO4
6. ammonium nitrate
6.
Writing Formulas of
Polyatomic Ions
Name
Formula
1. Sodium chromate
1. Na2CrO4
2. Iron (III) hydroxide
2. Fe(OH)3
3. Calcium bicarbonate
3. Ca(HCO3)2
4. lead (II) perchlorate
4.
5.
5. (NH4)3PO4
6. ammonium nitrate
6.
Writing Formulas of
Polyatomic Ions
Name
Formula
1. Sodium chromate
1. Na2CrO4
2. Iron (III) hydroxide
2. Fe(OH)3
3. Calcium bicarbonate
3. Ca(HCO3)2
4. lead (II) perchlorate
4. Pb(ClO4)2
5.
5. (NH4)3PO4
6. ammonium nitrate
6.
Writing Formulas of
Polyatomic Ions
Name
Formula
1. Sodium chromate
1. Na2CrO4
2. Iron (III) hydroxide
2. Fe(OH)3
3. Calcium bicarbonate
3. Ca(HCO3)2
4. lead (II) perchlorate
4. Pb(ClO4)2
5. Ammonium phosphate
5. (NH4)3PO4
6. ammonium nitrate
6.
Writing Formulas of
Polyatomic Ions
Name
Formula
1. Sodium chromate
1. Na2CrO4
2. Iron (III) hydroxide
2. Fe(OH)3
3. Calcium bicarbonate
3. Ca(HCO3)2
4. lead (II) perchlorate
4. Pb(ClO4)2
5. Ammonium phosphate
5. (NH4)3PO4
6. ammonium nitrate
6.
NH4NO3
Names and Formulas of
Covalent Compounds
Names and Formulas of
Covalent Compounds
Covalent compounds:
Names and Formulas of
Covalent Compounds
Covalent compounds:
• Form only between non-metals
Names and Formulas of
Covalent Compounds
Covalent compounds:
• Form only between non-metals
• Do not need to “balance charges” because
they share electrons instead of exchanging
them.
Names and Formulas of
Covalent Compounds
Covalent compounds:
• Form only between non-metals
• Do not need to “balance charges” because
they share electrons instead of exchanging
them.
• Instead, C.C’s use prefixes in the formula to
show how many atoms of each element are in
a molecule.
Names and Formulas of
Covalent Compounds
Prefix
Number
Names and Formulas of
Covalent Compounds
Prefix
MonoDiTriTetraPentaHexaHepta-
OctaNonaDeca-
Number
Names and Formulas of
Covalent Compounds
Prefix
Number
Mono-
1
Di-
2
Tri-
3
Tetra-
4
Penta-
5
Hexa-
6
Hepta-
7
Octa-
8
Nona-
9
Deca-
10
Steps to Writing the Names of
Binary Covalent Compounds
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
CO
Steps to Writing the Names of
Binary Covalent Compounds
Steps
1.
Name the left element first.
Example
CO
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
1.
Name the left element first.
Carbon
CO
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
Name the left element first.
Name the second element – use
the “ide”.
Carbon
CO
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
Name the left element first.
Name the second element – use
the “ide”.
CO
Carbon
Oxygen becomes “oxide”
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
3.
Name the left element first.
Name the second element – use
the “ide”.
Add a prefix to each element’s
name to show how many atoms
are present in the molecule.
Exception: if the first element
has only one atom do not add a
prefix.
CO
Carbon
Oxygen becomes “oxide”
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
Carbon
Oxygen becomes “oxide”
3.
Carbon monoxide
3.
Name the left element first.
Name the second element – use
the “ide”.
Add a prefix to each element’s
name to show how many atoms
are present in the molecule.
Exception: if the first element
has only one atom do not add a
prefix.
CO
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
Carbon
Oxygen becomes “oxide”
3.
Carbon monoxide
3.
Name the left element first.
Name the second element – use
the “ide”.
Add a prefix to each element’s
name to show how many atoms
are present in the molecule.
Exception: if the first element
has only one atom do not add a
prefix.
CO
Not: monocarbon mono-oxide
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
N2O3
Steps to Writing the Names of
Binary Covalent Compounds
Steps
1.
Name the left element first.
Example
N2O3
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
1.
Name the left element first.
Nitrogen
N2O3
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
Name the left element first.
Name the second element – use
the “ide”.
Nitrogen
N2O3
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
Name the left element first.
Name the second element – use
the “ide”.
Nitrogen
Oxide
N2O3
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
3.
Name the left element first.
Name the second element – use
the “ide”.
Add a prefix to each element’s
name to show how many atoms
are present in the molecule.
Exception: if the first element
has only one atom do not add a
prefix.
Nitrogen
Oxide
N2O3
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
Nitrogen
Oxide
3.
2 nitrogens = “di-”
3 oxygens = “tri-”
3.
Name the left element first.
Name the second element – use
the “ide”.
Add a prefix to each element’s
name to show how many atoms
are present in the molecule.
Exception: if the first element
has only one atom do not add a
prefix.
N2O3
Steps to Writing the Names of
Binary Covalent Compounds
Steps
Example
1.
2.
1.
2.
Nitrogen
Oxide
3.
2 nitrogens = “di-”
3 oxygens = “tri-”
3.
Name the left element first.
Name the second element – use
the “ide”.
Add a prefix to each element’s
name to show how many atoms
are present in the molecule.
Exception: if the first element
has only one atom do not add a
prefix.
N2O3
dinitrogen trioxide
Practice These
Practice These
Formula
Name
Practice These
Formula
1. N2O
Name
Practice These
Formula
Name
1. N2O
1. Dinitrogen monoxide
Practice These
Formula
Name
1. N2O
1. Dinitrogen monoxide
2. P4S10
2.
3.
3. Oxygen difluoride
4. S2F9
4.
5.
5. Dichlorine monoxide
Practice These
Formula
Name
1. N2O
1. Dinitrogen monoxide
2. P4S10
2.
3.
3. Oxygen difluoride
4. S2F9
4.
5.
5. Dichlorine monoxide
tetraphosphorus decasulphide
Practice These
Formula
Name
1. N2O
1. Dinitrogen monoxide
2. P4S10
2.
3. OF2
3. Oxygen difluoride
4. S2F9
4.
5.
5. Dichlorine monoxide
tetraphosphorus decasulphide
Practice These
Formula
Name
1. N2O
1. Dinitrogen monoxide
2. P4S10
2.
3. OF2
3. Oxygen difluoride
4. S2F9
4. Disulphur nonafluoride
5.
5. Dichlorine monoxide
tetraphosphorus decasulphide
Practice These
Formula
Name
1. N2O
1. Dinitrogen monoxide
2. P4S10
2.
3. OF2
3. Oxygen difluoride
4. S2F9
4. Disulphur nonafluoride
5. Cl2O
5. Dichlorine monoxide
tetraphosphorus decasulphide
Comparing Ionic and
Covalent Compounds
Comparing Ionic and
Covalent Compounds
• It is crucial that you are able to tell the
difference between Ionic and Covalent
Compounds. Here’s the easiest way.
Comparing Ionic and
Covalent Compounds
• It is crucial that you are able to tell the
difference between Ionic and Covalent
Compounds. Here’s the easiest way.
1. Look at the first element and determine if it
is a metal or NH4+ (ammonium ion).
Comparing Ionic and
Covalent Compounds
• It is crucial that you are able to tell the
difference between Ionic and Covalent
Compounds. Here’s the easiest way.
1. Look at the first element and determine if it
is a metal or NH4+ (ammonium ion).
2. If it is a metal (or NH4+ ) then it is an Ionic
Compound.
Comparing Ionic and
Covalent Compounds
• It is crucial that you are able to tell the
difference between Ionic and Covalent
Compounds. Here’s the easiest way.
1. Look at the first element and determine if it
is a metal or NH4+ (ammonium ion).
2. If it is a metal (or NH4+ ) then it is an Ionic
Compound.
3. If it is not a metal (or NH4+ ) it is a Covalent
Compound.
Try These
Try These
Ionic or Covalent
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2
SBr2
N2O3
Na2Cr2O7
FeF2
SO3
Li2SO4
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2 Ionic
SBr2
N2O3
Na2Cr2O7
FeF2
SO3
Li2SO4
• V is vandium – a metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3
Na2Cr2O7
FeF2
SO3
Li2SO4
• V is vandium – a metal
• S is sulpher – a non-metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3 Covalent
Na2Cr2O7
FeF2
SO3
Li2SO4
• V is vandium – a metal
• S is sulpher – a non-metal
• N is nitrogen – a non-metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3 Covalent
Na2Cr2O7 Ionic
FeF2
SO3
Li2SO4
•
•
•
•
V is vandium – a metal
S is sulpher – a non-metal
N is nitrogen – a non-metal
Na is sodium – a metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3 Covalent
Na2Cr2O7 Ionic
FeF2 Ionic
SO3
Li2SO4
•
•
•
•
•
V is vandium – a metal
S is sulpher – a non-metal
N is nitrogen – a non-metal
Na is sodium – a metal
Fe is iron – a metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3 Covalent
Na2Cr2O7 Ionic
FeF2 Ionic
SO3 Covalent
Li2SO4
•
•
•
•
•
•
V is vandium – a metal
S is sulpher – a non-metal
N is nitrogen – a non-metal
Na is sodium – a metal
Fe is iron – a metal
S is sulphur – a non-metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3 Covalent
Na2Cr2O7 Ionic
FeF2 Ionic
SO3 Covalent
Li2SO4 Ionic
•
•
•
•
•
•
•
V is vandium – a metal
S is sulpher – a non-metal
N is nitrogen – a non-metal
Na is sodium – a metal
Fe is iron – a metal
S is sulphur – a non-metal
Li is lithium – a metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3 Covalent
Na2Cr2O7 Ionic
FeF2 Ionic
SO3 Covalent
Li2SO4 Ionic
(NH4)2S
•
•
•
•
•
•
•
V is vandium – a metal
S is sulpher – a non-metal
N is nitrogen – a non-metal
Na is sodium – a metal
Fe is iron – a metal
S is sulphur – a non-metal
Li is lithium – a metal
Try These
Ionic or Covalent
•
•
•
•
•
•
•
•
VO2 Ionic
SBr2 Covalent
N2O3 Covalent
Na2Cr2O7 Ionic
FeF2 Ionic
SO3 Covalent
Li2SO4 Ionic
(NH4)2S Ionic
•
•
•
•
•
•
•
V is vandium – a metal
S is sulpher – a non-metal
N is nitrogen – a non-metal
Na is sodium – a metal
Fe is iron – a metal
S is sulphur – a non-metal
Li is lithium – a metal
• NH4+ (ammonium) is the one
exception: an ionic non-metal
The End