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CHM 130
Naming & Writing Chemical Formulas
PRE - LAB
Section 1: Naming Monatomic Cations – Group IA and IIA cations form only one stable charge and are named for the parent metal followed by the word “ion.” Many other metals, especially the transition metals, can form cations with variable charges (oxidation states) so it is necessary to include a Roman numeral in parentheses to indicate the charge of the cation. Copper, for example, can form either Cu+, which we name copper (I), and Cu 2+, which we name copper (II). The aluminum ion (Al3+), zinc ion (Zn2+) and silver ion (Ag+) are exceptions for transition metals and do not require the Roman numeral to be added to the name of the cation.
Cr2+_______________________ Al 3+^ ____________________
Co3+^ _____________________ Cu1+^ _____________________
Ca2+^ ___ __________________ Sn 4+^ ____________________
K+________________________ Ni3+^ _____________________
Fe2+_______________________ Pb2+^ _____________________
Ag+_______________________ Zn2+^ ____________________
Section 2: Naming Monatomic Anions – Nonmetal ions are named using the nonmetal stem plus the suffix
– ide. For example, Cl-^ is named chloride ion; N3-^ is named nitride ion.
O2-_______________________ Br -^ _______________________
H-^ _______________________ I-^ _________________________
S2-_______________________ P3-^ ________________________
Section 3: Naming Polyatomic Ions – Polyatomic anions generally contain one or more elements combined
with oxygen and are often called oxyanions. The most common oxyanions have the name ending in – ate (root
form)
SO 4 2-^ _________________________ PO 4 3-__________________________
CO 3 2-^ __________________________ NO 3 - _________________________
BrO 3 1-^ ________________________________________^ IO 3 1-^ _____________________________________
ClO 3 1-^ ________________________________________
The prefix hypo- with ending - ite indicates two less oxygen atom than the oxyanion ending in – ate (the root form);
The ending ite indicates one less oxygen atom than the oxyanion ending in – ate (the root form);
The root form of the oxyanions as listed in the section 3 ending with -ate ;
The prefix per- with ending -ate indicates one more oxygen atom than the oxyanion ending in – ate (the root form)
ClO 4 -^ __________________________ SO 4 2-_________________________
ClO 3 -^ __________________________ SO 3 2-_________________________
ClO 2 -^ __________________________ SO 2 2-_________________________
ClO-^ ___________________________
Anions derived by adding H+^ to an oxyanion are named by adding as a prefix the word hydrogen or dihydrogen,
as appropriate. The charge on the ion will increase by + 1 for each hydrogen added to the base oxyanion.
HSO 4 -^ __________________________ HCO 3 -^ ________________________
HPO 3 2-^ __________________________ H 2 PO 4 -^ _________________________
Polyatomic anions that are exceptions and do not fit into any of the above:
CN -^ ____________________________ OH -^ ____________________________
C 2 2-^ ___________________________ O 2 2-_____________________________
There is only one polyatomic cation we need to know for now: NH 4 +^ _________________________
Name the following ionic compounds. Watch out for metals that can take a variable oxidation state.
NH 4 Br _________________________________ NaHSO 4 __________________________
CrO 3 _________________________________ Mg(NO 3 ) 2 ________________________
Co(NO 2 ) 2 ______________________________ CuSO 5 ____________________________
CaCO 3 _________________________________ NaHCO 3 __________________________
KCl ___________________________________ NiBr 3 _____________________________
FeSO 4 _________________________________ Be(NO 3 ) 2 __________________________
MgCl 2 _________________________________ AuCl 3 _____________________________
FeCl 3 __________________________________ Cu 3 P ______________________________
Zn 3 (PO 5 ) 2 ______________________________ NH 4 NO 2 ___________________________
Al(OH) 3 _______________________________ Cu(C 2 H 3 O 2 ) 2 ________________________
CuC 2 H 3 O 2 ______________________________ PbSO 3 _____________________________
NaClO ________________________________ SnS 2 _______________________________
Fe 2 O 3 __________________________________ (NH 4 ) 3 PO 4 ___________________________
Write the chemical formula for the following ionic compounds:
magnesium sulfate ________________________ barium hydrogen carbonate _______________
silver sulfide _____________________________ lead (II) nitrate _________________________
ammonium perphosphate ___________________ iron (II) oxide __________________________
iron (III) oxide ___________________________ calcium chloride ________________________
potassium nitrite _________________________ magnesium hydroxide ___________________
aluminum hyposulfite _________________________ copper (II) hypochlorite __________________
lead (IV) peroxide ________________________ potassium carbide _______________________
aluminum sulfite __________________________ lithium cyanide _________________________
Binary Molecular Compounds
Section 6: Name the Following Binary Molecular Compounds. A binary molecular compound is composed of two nonmetal elements. (Nonmental elements usually found to the right of the staircase in the periodic table)
The first element in the compound is named using the parent name and the second element in the formula
uses the stem of the parent name with the suffix ending with – ide. The number of atoms of each element is indicated by Greek prefixes with an exception being the prefix mono- is never used in naming the first element. For example, P 4 S 7 is named tetraphosphorus heptasulfide.
Write the name of each binary molecular compound.
SO 3 ___________________________________ N 2 O _____________________________
NO ____________________________________ N 2 O 4 ____________________________
N 2 O 5 ___________________________________ PCl 3 ___________________________
PCl 5 __________________________________ NH 3 _____________________________
SCl 6 ___________________________________ P 2 O 5 ____________________________
CCl 4 ___________________________________ SiO 2 ____________________________
CS 2 ___________________________________ OF 2 _____________________________
Write the chemical formula for the following binary molecular compounds:
carbon monoxide ________________________ boron trichloride ____________________
dinitrogen pentoxide _____________________ silicon dioxide ______________________
tetraphosphorous decoxide ________________ disulfur hexaiodide ___________________
nitrogen tribromide ______________________ triiodine nonafluoride _________________
octaselenium pentoxide ___________________ dibromine tetroxide __________________
tetraiodine decoxide _____________________ dioxygen heptafluoride _______________
