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Ionic Compounds
Nomenclature
Introduction
• We use the periodic table to tell us the most
•
commonly expected charges for the ions of
elements.
For example:
• Group 1 (1A) elements have a 1+ charge.
• Na becomes Na+
• Group 2 (2A) elements have a 2+ charge.
• Mg becomes Mg2+
• Group 13 (3A) elements have a 3+ charge.
• Al becomes Al3+
Introduction
• We use the periodic table to tell us the most
•
commonly expected charges for the ions of
elements.
For example:
• Group 15 (5A) elements have a 3- charge.
• N becomes N3-
• Group 16 (6A) elements have a 2- charge.
• O becomes O2• Group 17 (7A) elements have a 1- charge.
• Cl becomes Cl-
Forming Ionic Compounds
• We form ionic compounds by matching the
charges of the ions to form a neutral compound.
• For example:
• Combining Na+ with Cl- gives NaCl.
• Combining Ca2+ with S2- gives CaS.
• Combining Ga3+ with N3- gives GaN.
• Each of these combinations gives a neutral
compound.
Forming Ionic Compounds
• More complex combinations of ions also need to
be balanced to produce neutral compounds.
• For example:
• Combining Na+ with O2- gives Na2O.
• Combining Ca2+ with Br- gives CaBr2.
• Combining Al3+ with F- gives AlF3.
• Each of these combinations gives a neutral
compound.
Forming Ionic Compounds
• For even more complex combinations of ions we
use a trick to produce neutral compounds.
• For example:
2
2+
2+
3• Combining Ca with N : Ca
3
3N
2+, we
• We
To find
canthe
useproper
this “criss-cross”
number of Ca
when
ever
use
wethe
have
3
•
a complex
of
the N3-. combination of ions.
To find the proper number of N3-, we use the 2 of
the Ca2+.
Binary Ion Nomenclature
• When we name binary ionic compounds (ionic
compounds made from the ions of two elements),
we name the cation first followed by the anion.
• In general, cations that are metals are given the
name of the elemental metal.
• NaCl is named sodium chloride.
• BaF2 is named barium fluoride.
• Ca3P2 is named calcium phosphide.
Binary Ion Nomenclature
• When we name binary ionic compounds (ionic
compounds made from the ions of two elements),
we name the cation first followed by the anion.
• In general, anions are given the name of the
element followed by the suffix “-ide.”
• NaCl is named sodium chloride.
• BaF2 is named barium fluoride.
• Ca3P2 is named calcium phosphide.
Binary Ion Nomenclature
• The single element anions are:
nitride 3C
phosphide
N
P
oxide
21-
O
S
F
Cl
fluoride
sulfide
chloride
bromide
As
Se
arsenide
Br
I
selenide
iodide
Binary Ion Nomenclature
• Transition (d-block) metals most commonly have a
Sc2+
2+Fe
2+
3+
2+3+
3+ +
2+
2+
2+
3+
3+
4+
2+
Mn
,
Mn
Co
,
Fe
,
Co
V Cr
,TiV , Cr
,V
Cu ,
Cu2+
2+
Zn
2+ charge.
Mo
Sn2+, +Sn4+
Ag
Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Au+, Au3+
Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn
Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po
Lr Rf Db Sg Bh Hs Mt Ds Rg Uub
•
•
Pb2+, Pb4+
There are exceptions to this rule.
Some transition and main group metals have
two or
more common charges.
Binary Ion Nomenclature
• Since these cations can have different charges, we
need a nomenclature that will distinguish between
the different cations.
• The Stock system is used to identify different ions.
• We use the element name followed by the
charge of the ion in parenthesis.
• For example:
• Cu+ is written as copper(I)
• Cu2+ is written as copper(II)
• Pb2+ is written as lead(II)
Binary Ion Nomenclature
• Examples of Stock nomenclature:
• CuCl = copper(I) chloride
• CuCl2 = copper(II) chloride
• FeO = iron(II) oxide
• Fe2O3 = iron(III) oxide
• PbS = lead(II) sulfide
• PbS2 = lead(IV) sulfide
• VO = vanadium(II) oxide
• V2O3 = vanadium(III) oxide
Polyatomic Ion
Nomenclature
• Polyatomic ions are single ions that are made up
of several atoms.
• Examples of polyatomic ions include:
• nitrate: NO3• sulfate: SO42• phosphate: PO43• ammonium: NH4+
• nitrite: NO2-
Polyatomic Ion
Nomenclature
• Each of these units acts as a single ion.
• Nitrate (1-)acts in the same manner as chloride.
• Sodium nitrate is NaNO3.
• Calcium nitrate is Ca(NO3)2.
• Aluminum nitrate is Al(NO3)3.
• Sulfate (2-) acts in the same manner as oxide.
• Sodium sulfate is Na2SO4.
• Calcium sulfate is CaSO4.
• Cations:
•
Polyatomic Ion
Nomenclature
ammonium: NH4+
dimercury: Hg22+
Anions:
nitrate: NO3sulfate: SO42nitrite: NO2sulfite: SO32cyanide: CNcarbonate: CO32silicate: SiO32hydroxide: OHperchlorate: ClO4chromate: CrO42dichromate: Cr2O72chlorate: ClO32oxalate:
C
O
2 4
chlorite: ClO2
hypochlorite: ClOphosphate: PO43acetate: CH3COOphosphite: PO33hydrogen carbonate: HCO3-
Polyatomic Ion
Nomenclature
• When we form ionic compounds from polyatomic
•
ions, we treat the polyatomic ions as individual
units of charge.
For example:
• barium 2+ and nitrate 1Ba2+
(NO3)-
Ba(NO3)2
barium nitrate
We use the criss-cross trick to find the formula of the
compound.
Polyatomic Ion
Nomenclature
• When we form ionic compounds from polyatomic
•
ions, we treat the polyatomic ions as individual
units of charge.
For example:
• ammonium 1+ and sulfate 2(NH4)+
(SO4)2-
(NH4)2SO4
ammonium sulfate
We use the criss-cross trick to find the formula of the
compound.
Knowledge Check
• Determine the formulas of the following
compounds:
1.sodium carbonate
2.copper(II) sulfate
+ CO
2Na
Na
2 (CO
3 3)
2CuSO
Cu2+
(SO
4 4)
4+
3(PO
)
(PO
)
3.lead(IV) phosphate PbPb
4
3
4 4
4.aluminum nitrite
Al(NO
Al3+
(NO
2)3 2)
+
25.ammonium sulfide (NH4)(NH
4)2S S
Knowledge Check
• Determine the names of the following
compounds:
1.Fe2(CrO4)3
iron(III) chromate
2.VO2
vanadium(IV) oxide
3.Cr(CH3COO)2
chromium(II) acetate
4.AuPO4
gold(III) phosphate
5.NaClO
sodium hypochlorite