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Naming Compounds Handout
IONIC COMPOUNDS versus MOLECULAR COMPOUNDS
ionic compound: consist of cations (positive ions) and anions (negative ions) held together by electrostatic attraction – usually metal + nonmetal(s) – made of monatomic ions, polyatomic ions, and/or both
– monatomic ions: consist of a single atom
molecular compound: consist of nonmetal atoms bonded together byshared electrons (covalent bonding)
NAMING MONATOMIC CATIONS:
Metal atoms lose valence electrons to form positively charged ions, called cations.
An ion formed from an individual atom is a monatomic (or monoatomic) cation.
I. Groups IA, IIA, IIIA elements silver (Ag), and zinc (Zn) form only one type of ion: + + + +
– Group IA elements form +1 ions: H , Li , Na , K+2 +2 +2 +2 +2
– Group IIA elements form +2 ions: Be , Mg , Ca , Sr , Ba– Group IIIA elements form +3 ions: Al
+3
– silver ion = Ag+; zinc ion = Zn
+2
When a Group IA, IIA, IIIA element, silver, or zinc forms an ion, it is named:
element name + ion
e.g. Na+ = sodium ion Sr+2 = strontium ion Zn+2 = zinc ion
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II. The Stock system is used to name transition metals and other metals that form more than one ion:
– iron (Fe) forms two ions: Fe+2
and Fe+3
– lead (Pb) forms two ions: Pb+2
and Pb+4
When a metal can form more than one ion, each ion is named:
element name (charge in Roman numerals) + ion
e.g. Fe+2
= iron (II) ion Pb+2
= lead (II) ion Cu+
= copper (I) ion Fe
+3 = iron (III) ion Pb
+4= lead (IV) ion Cu
+2= copper (II) ion
Name each of the following monatomic cations:
Li+
= _________________________ Ba+2
= _________________________
Ag+
= _________________________ Cu+2
= _________________________
Al+3
= ________________________ Mg+2
= _________________________
Mn+2
= ________________________ Sn+4
= _________________________
H+
= _________________________ Co+3
= _________________________
Fe+3
= ________________________ Na+
= _________________________
K+
= ________________________ Ti+4
= _________________________
Ca+2
= ________________________ Ni+2
= _________________________
NOTE: ONLY USE ROMAN NUMERALS WHEN DESCRIBING IONIC COMPOUNDS MADE FROM THE 9 ATOMS ON THE PERIODIC TABLE THAT CAN FORM MORE THAN 1 POSITIVE ION
HINT: Only use Roman numerals for the schitzophrenic atoms
lithium ion
silver ion
manganese (II) ion
aluminum ion
hydrogen ion
ion (III) ion
potassium ion
calcium ion
bariunion
copper (II) ion
tin ion
magnesium ion
cobalt (III) ion
sodium ion
titanium ion
nickel ion
NAMING MONATOMIC ANIONS:
Nonmetal atoms gain valence electrons to form negatively charged ions called anions.
When a nonmetal forms an ion, it is named:
element stem name + “ide” + ion
O–2 e.g. O = oxygen atom = oxide ion
N = nitrogen atom N–3 = nitride ion
Name each of the following monatomic anions:
– – F = _________________________ Cl = _________________________
– –2 Br = _________________________ S = _________________________
–3 I–
= _________________________ P = _________________________
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________________________
________________________
________________________
Nitride Ion
Sul�de Ion
Carbide Ion
Write the chemical formula for the most common ion for the following::
�uoride ion
bromide ion
iodide ion
chloride ion
sul�de ion
phosphide ion
N-3
S-2
C-4
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2a. If two monatomic ions have different chargesuse crossover rule to get formula of the compound
– superscript for cation becomes subscript for anion – superscript for anion becomes subscript for cation – simplify subscripts to get lowest ratio of atoms
(Note: Only the numbers cross down, not the signs!)
Na+ 2–S BaNa2S Ba3N2
2+ 3–N> Ti4+ 2–> O>> >
TiO2Ti2O4 is simplified!
Combine each pair of ions to get the formula of the compound they form:
+ –2 +2 – + –3 Cu O Mg F K P
+ – +2 –2 Ag Cl Ca S
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Cu2O MgF2 K3P
AgCl CaS
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CHEMICAL FORMULAS AND NAMES FROM INDIVIDUAL IONSCompounds are named from the individual ions they come from.
Name the cation and the anion, then remove “ion” from each name:
e.g. Na+ = sodium ion
Cl– = chloride ion � NaCl = sodium chloride
K+ = potassium ion
Fe+3
= iron (III) ion–
Ag+ = silver ion
S–2
= sulfide ion � Ag2S = silver sulfide
Combine each pair of ions to get the chemical formula, then name the compound:
Individual ions Compound Formula Compound Name
Mg+2 F – _____MgF2______ ______magnesium fluoride_____
Ni+2 S–2 _______________ ___________________________
Ca+2 Br– ________ ___________________________
Al+3 P–3 _______________ ___________________________
Co+2 O _______________ ___________________________
_______________ ___________________________
Fe+3 O–2 _______________ ___________________________
–2
Ag+1 S–2
NiS
CaBr2
AlP
CoO
Ag2S
Fe2O3
nickel sul�de
calcium bromide
aluminum phosphide
cobalt (II) oxide
silver sul�de
iron (III) oxide
GIVEN THE CHEMICAL FORMULA, NAME THE COMPOUND
1. If the metal is in Groups IA–IIIA, silver, cadmium, or zinc, then just name the metal cation and the anion:
e.g. NaCl Na = sodium and Cl = chloride sodium chloride
BaI2 Ba = barium and I = iodide barium iodide
2. If the metal can form more than one ion, a. Determine the charge on the cation using the charge on the anion. b. Name the cation and the anion, then remove “ion” from both
e.g. FeBr2 Since the ion formed is Br–, then 2 Br’s have an overall negative charge of –2. To get an overall charge of zero for the compound, the overall positive charge must be +2. Thus, Fe must have a charge of +2, so the ion iron forms is Fe+2 .
+2 Fe = iron (II) ion Br– = bromide ion FeBr2 = iron (II) bromide
Copper (II) oxide = _____________________________
Copper (I) oxide = _____________________________
cobalt (II) sul�de= _____________________________
CoP = _____________________________________
CuF= _____________________________________
PbO= _____________________________________
CuO
Cu2O
CoS
cobalt (III) phosphide
copper (I) �uoridelead (II) oxide
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Give the name for each compound given its chemical formula:
Formula Individual Ions Name of Compound
MgCl2 Mg+2 Cl– magnesium chloride
LiF
ZnO
K2S
SnO2
CuBr2
Ag3N
WRITING CHEMICAL FORMULAS GIVEN THE COMPOUND NAME
Get the individual ions from the name, then combine them using the crossover rule:
e.g. barium chloride � barium = Ba+2 chloride = Cl
–
Ba+2 Cl– � BaCl2
KCl 2
ZnF2
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Give the chemical formula for each compound given its name:
Name of Compound individual ions Formula
lithium chloride Li+ Cl
– LiCl
iron (III) sulfide
calcium iodide
mercury (IV) chloride
silver chloride
copper (II) oxide
zinc bromide
lead (II) phosphide
potassium iodide
cobalt (II) nitride
nickel (II) sulfide
NAMING COVALENT COMPOUNDSIndicate number of atoms of each element with Greek prefix before element name:
# of atoms Greek Prefix # of atoms Greek Prefix
1 mono (usually omitted) 6 hexa
2 di 7 hepta
3 tri 8 octa
4 tetra 9 nona
5 penta 10 deca
For the first element: prefix + element nam eFor the second element: prefix + element name stem + “-ide ”
Note: Mono is generally omitted, except in common names like CO = carbon monoxide
P2O5 SF6
diphosphorus pentaoxide sulfur hexafluoride
Name the following molecular compounds:
SO3 = _____________________ SiBr4 = ______________________
XeF6 = ______________________ ClF3 = ______________________
N2O4 = ______________________ Cl2O7= ______________________
PCl5 = ______________________ P4O10 = _____________________
DETERMINING FORMULAS OF COLVALENT COMPOUNDS Use Greek prefix(es) to determine number of atoms of each element in formula.
Get elements and number of atoms of each from name:
tetraphosphorus hexasulfide
P4S6
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Name each of the following covalent compounds:
PUTTING IT ALL TOGETHER:Name each of the following compounds and indicate ionic (I) or covalent (C) bond:
BaCl2 _____________________ NiBr2 ____________________
_____________________ N S2 ____________________
silver fluoride: _____________ SiO
2
____________________
SBr _____________________ PF5 ____________________
FeP _____________________
N 3 = _____________________ P S4
= ______________________
IF5 = ______________________ ClO2 = ______________________
N2O
= ______________________
SF6 = ______________________
Pl 3 = ______________________ P4O5 = _____________________
2O 5
= ______________________ antimony tribromide
hydrogen iodide
3 = ______________________
sodium sulfide: _____________
2
oxygen difluoride: __________
copper (II) sul�de
magnesium �uoride __________________
sodium phosphide ___________________
zinc chloride ________________________