Transcript Unit IV – Chemical Names and Formulas

NOTES: 9.1-9.2 –
NAMING & WRITING FORMULAS FOR
IONIC COMPOUNDS
Monatomic Ions:
• Monatomic ions = ions consisting of only 1 atom
• Charges can often be determined using the periodic
table – Table 9.1 p. 265
• Positive ions’ names – do not change
• Negative ions’ names – drop the ending and add ide
Monatomic Ions – METALS:
• Metals: form cations
• Group IA Metals: form 1+ ions
 Li+, Na+, K+
• Group IIA Metals: form 2+ ions
 Mg2+, Ca2+
• Group IIIA Metal (Al): forms 3+ ion
 Al3+
Monatomic Ions –
TRANSITION METALS:
• Transition metals: many have more than one common
ionic charge
• a Roman numeral in parentheses indicates the numerical
value of the ionic charge:
 iron(II) ion = Fe2+
 iron(III) ion = Fe3+
 copper(I) ion = Cu+
 copper(II) ion = Cu2+
Monatomic Ions –
TRANSITION METALS
**a few transition metals have only one ionic charge –
the names of these cations do NOT have a Roman
numeral:
 silver =
 cadmium =
 nickel =
 zinc =
Monatomic Ions –
TRANSITION METALS
**a few transition metals have only one ionic charge –
the names of these cations do NOT have a Roman
numeral:
 silver = Ag+
 cadmium =
 nickel =
 zinc =
Monatomic Ions –
TRANSITION METALS
**a few transition metals have only one ionic charge –
the names of these cations do NOT have a Roman
numeral:
 silver = Ag+
 cadmium = Cd2+
 nickel =
 zinc =
Monatomic Ions –
TRANSITION METALS
**a few transition metals have only one ionic charge –
the names of these cations do NOT have a Roman
numeral:
 silver = Ag+
 cadmium = Cd2+
 nickel = Ni2+
 zinc =
Monatomic Ions –
TRANSITION METALS
**a few transition metals have only one ionic charge –
the names of these cations do NOT have a Roman
numeral:
 silver = Ag+
 cadmium = Cd2+
 nickel = Ni2+
 zinc = Zn2+
Monatomic Ions – NONMETALS:
• Nonmetals: form anions
• Group VIIA nonmetals: form 1- ions
 F-, Cl-, Br • Group VIA nonmetals: form 2- ions
 O2-, S2-, Se2• Group VA nonmetals: form 3- ions
 N3-, P3-
What about GROUPS 4A and 0?
• the majority of elements in these groups do NOT
form ions
 noble gases rarely form compounds
 the nonmetals in 4A, C and Si, are found in
molecular compounds (not ionic)
POLYATOMIC IONS:
• tightly bound groups of atoms that behave as a unit
and carry a charge
• memorize the bold-faced ions on the list provided in
class!!
• table 9.3 on p. 268 for others
POLYATOMIC IONS:
• most are negative and end in –ite or –ate
EXAMPLES:
-ite:
-ate:
SO32-,
SO42-,
NO2-,
NO3-,
ClO2-,
ClO3-,
POLYATOMIC IONS:
• most are negative and end in –ite or –ate
EXAMPLES:
-ite:
-ate:
SO32-, sulfite
SO42-, sulfate
NO2-, nitrite
NO3-, nitrate
ClO2-, chlorite
ClO3-, chlorate
POLYATOMIC IONS:
• EXCEPTIONS! (of course…)
NH4+
(positive!)
CN-
(-ide ending)
OH-
(-ide ending)
POLYATOMIC IONS:
• EXCEPTIONS! (of course…)
NH4+
ammonium ion
(positive!)
CN-
cyanide ion
(-ide ending)
OH-
hydroxide ion
(-ide ending)
Naming Binary and Ternary IONIC
COMPOUNDS:
• Binary Compounds – composed of two kinds of
elements
• Ternary Compounds – compounds of three kinds
elements
***Polyatomic ions are included!
Ionic Compound Naming Rules:
● Binary compounds with only two elements:
● Remember, the cation is always named first
● Name the cation (usually the metal ion) using the same name as
the element
● If the cation forms more than one ion, use a Roman numeral
following the element name to indicate the charge
(all metals except group 1A, group 2A, Al3+, Zn2+, Ni2+, Cd2+,
Ag+)
● Name the anion by usually using the first syllable of the element
followed by the suffix -ide (it is pretty obvious where more than
one syllable of the element name is needed).
IONIC COMPOUNDS: Naming Rules Continued…
● Other Ionic compounds (those with multiple
elements):
 Name the cation or anion as in binary
compounds
 Name the polyatomic ion
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
lithium bromide
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
lithium bromide
calcium oxide
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
lithium bromide
calcium oxide
strontium nitrite
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
lithium bromide
calcium oxide
strontium nitrite
rubidium sulfate
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
lithium bromide
calcium oxide
strontium nitrite
rubidium sulfate
iron(III) oxide
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
lithium bromide
calcium oxide
strontium nitrite
rubidium sulfate
iron(III) oxide
calcium dichromate
Name the following ionic compounds:
● LiBr:
● CaO:
● Sr(NO2)2:
● Rb2SO4:
● Fe2O3:
● CaCr2O7:
● NaHCO3:
lithium bromide
calcium oxide
strontium nitrite
rubidium sulfate
iron(III) oxide
calcium dichromate
sodium bicarbonate
IONIC COMPOUNDS: Writing
Formulas…
● the positive charge of the cation must balance the
negative charge of the anion
● the NET IONIC CHARGE of the formula must be
ZERO.
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES:
K+
&
Cl-:
Ca2+
&
Br- :
Mg2+
&
S2- :
Fe3+
&
O2-:
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES:
K+
&
Cl-:
Ca2+
&
Br- :
Mg2+
&
S2- :
Fe3+
&
O2-:
KCl
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES:
K+
&
Cl-:
KCl
Ca2+
&
Br- :
CaBr2
Mg2+
&
S2- :
Fe3+
&
O2-:
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES:
K+
&
Cl-:
KCl
Ca2+
&
Br- :
CaBr2
Mg2+
&
S2- :
MgS
Fe3+
&
O2-:
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES:
K+
&
Cl-:
KCl
Ca2+
&
Br- :
CaBr2
Mg2+
&
S2- :
MgS
Fe3+
&
O2-:
Fe2O3
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES: polyatomic ions
Ca2+
&
NO3- :
K+
&
SO42- :
NH4+
&
PO43- :
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES: polyatomic ions
Ca2+
&
NO3- :
K+
&
SO42- :
NH4+
&
PO43- :
Ca(NO3)2
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES: polyatomic ions
Ca2+
&
NO3- :
Ca(NO3)2
K+
&
SO42- :
K2SO4
NH4+
&
PO43- :
IONIC COMPOUNDS: Writing
Formulas…
EXAMPLES: polyatomic ions
Ca2+
&
NO3- :
Ca(NO3)2
K+
&
SO42- :
K2SO4
NH4+
&
PO43- :
(NH4)3PO4
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Na2O
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Na2O
Cu2S
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Na2O
Cu2S
CuSO4
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Na2O
Cu2S
CuSO4
Ca(ClO2)2
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Na2O
Cu2S
CuSO4
Ca(ClO2)2
Al(OH)3
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Na2O
Cu2S
CuSO4
Ca(ClO2)2
Al(OH)3
(NH4)3P
Write the formula for the following
compounds:
● Sodium oxide:
● Copper(I) sulfide:
● Copper(II) sulfate:
● Calcium chlorite:
● Aluminum hydroxide:
● Ammonium phosphide:
● Iron(III) nitrate:
Na2O
Cu2S
CuSO4
Ca(ClO2)2
Al(OH)3
(NH4)3P
Fe(NO3)3