Compounds Binary Compounds Binary compounds that contain a metal of fixed oxidation number (group 1,...
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Transcript of Compounds Binary Compounds Binary compounds that contain a metal of fixed oxidation number (group 1,...
Compounds
Binary CompoundsBinary compounds that contain a metal of fixed oxidation number(group 1, group 2, Al, Zn, Ag, etc.), and a non-metal.
To name these compounds, give the name of metal followed by thename of the non-metal, with the ending replaced by the suffix –ide.
Examples:
NaCl sodium chloride (Na1+ Cl1-)
CaS calcium sulfide (Ca2+ S2-)
AlI3 aluminum iodide (Al3+ I1-)
Cations and Anions
Common Simple Cations and Anions
Cation Name Anion Name*
H 1+ hydrogen H 1- hydride Li 1+ lithium F 1- fluoride Na 1+ sodium Cl 1- chloride K 1+ potassium Br 1- bromide Cs 1+ cesium I 1- iodide Be 2+ beryllium O 2- oxide Mg 2+ magnesium S 2- sulfide Al 3+ aluminum Ag 1+ silver
*The root is given in color.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86
Example: Aluminum Chloride
Step 1:
Step 2:
Step 3: 1 3
Step 4: AlCl3
Criss-Cross Rule
Al Cl
Al Cl
3+ 1-
write out name with space
write symbols & charge of elements
criss-cross charges as subsrcipts
combine as formula unit(“1” is never shown)
Example: Aluminum Chloride
Step 1: Aluminum Chloride
Step 2: Al3+ Cl1-
Step 3: Al Cl1 3
Step 4: AlCl 3
Criss-Cross Rule
Example: Aluminum Oxide
Step 1: Aluminum Oxide
Step 2: Al3+ O2-
Step 3: Al O2 3
Step 4: Al2O3
Criss-Cross Rule
Example: Magnesium Oxide
Step 1: Magnesium Oxide
Step 2: Mg2+ O2-
Step 3: Mg O2 2
Step 4: Mg2O2
Step 5: MgO
Criss-Cross Rule
Naming Binary Compounds
Formula Name
1 BaO ____________________
2 ________________ sodium bromide
3 MgI2 ____________________
4 KCl ____________________
5 ________________ strontium fluoride
6 ________________ cesium fluoride
barium oxide
NaBr
magnesium iodide
potassium chloride
SrF2
CsF
Ternary Compounds
Ternary Compounds
Ternary compounds are those containing three different elements. (NaNO3, NH4Cl, etc.). The naming of ternary compounds involves the memorization of several positive and negative polyatomic ions, (two or more atoms per ion), and adding these names to the element with which they combine.
i.e., Sodium ion, Na1+ added to the nitrate ion, NO31-,
to give the compound, NaNO3, sodium nitrate.
Binary rules for indicating the oxidation number of metals and for indicating the numbers of atoms present are followed. The polyatomic ions that shouldbe learned are listed in a separate handout.
Ternary Compounds
NaNO2 sodium nitrite
KClO3 potassium chlorate
Ca3(PO4)2 calcium phosphate
Fe(OH)3 iron (III) hydroxide
NaHCO3 sodium bicarbonate ‘sodium hydrogen carbonate’
Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion Name Ion Name
NH4 1+ ammonium CO3 2- carbonate
NO2 1- nitrite HCO3 1- hydrogen carbonate NO3 1- nitrate (“bicarbonate” is a widely SO3 2- sulfite used common name) SO4 2- sulfate ClO 1- hypochlorite HSO4 1- hydrogen sulfateClO2 1- chlorite
(“bisulfate” is a widely ClO3 1- chlorate used common name) ClO4 1- perchlorate OH 1- hydroxide C2H3O2 2- acetate CN 1- cyanide MnO4 1- permanganate PO4 3- phosphate Cr2O7 2- dichromate HPO4 2- hydrogen phosphate CrO4 2- chromate H2PO4 1- dihydrogen phosphate O2 2- peroxide
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100
Ternary Compounds
1. ________________ calcium phosphate
2. ________________ ammonium carbonate
3. ________________ aluminum sulfate
4. Na2SO4 ____________________
5. LiCN ____________________
6. Ba(ClO3)2 ____________________
7. ________________ copper (II) hydroxide
Ca3(PO4) 2
(NH4)2CO3
Al2(SO4)3
sodium sulfate
lithium cyanide
barium chlorate
Cu(OH)2
Magnesium Phosphate
Step 1: Magnesium Phosphate
Step 2: Mg2+ PO43-
Step 3: Mg (PO4)3 2
Step 4: Mg3(PO4)2
phosphate
sulfate
carbonate
chlorate
nitrate
Polyatomic Ions - Memorize
phosphATE
sulfATE
carbonATE
chlorATE
nitrATE
PO43- ……………
SO42- ……………
CO32- …………..
ClO31- …………..
NO31- ………..….
Eight “-ATE’s”
Exceptions:
ammonium
hydroxide
cyanide
NH41+ ……………
OH1- ……………
CN1- …………..
Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
BrO31-
Bromate ion
BrO21-
Bromite ion
BrO1-
Hypobromite ion
CO42- CO3
2-
Carbonate ion
CO22- CO2-
ClO41- ClO3
1-
Chlorate ion
ClO21- ClO1-
IO41- IO3
1-
Iodate ion
IO21- IO1-
NO41- NO3
1-
Nitrate ion
NO21- NO1-
PO53- PO4
3-
Phosphate ion
PO33- PO2
3-
SO52- SO4
2-
Sulfate ion
SO32- SO2
2-
1 more oxygen “normal” 1 less oxygen 2 less oxygen
Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
BrO31-
Bromate ion
BrO21-
Bromite ion
BrO1-
Hypobromite ion
CO42- CO3
2-
Carbonate ion
CO22- CO2-
ClO41- ClO3
1-
Chlorate ion
ClO21- ClO1-
IO41- IO3
1-
Iodate ion
IO21- IO1-
NO41- NO3
1-
Nitrate ion
NO21- NO1-
PO53- PO4
3-
Phosphate ion
PO33- PO2
3-
SO52- SO4
2-
Sulfate ion
SO32- SO2
2-
1 more oxygen “normal” 1 less oxygen 2 less oxygen
Write the total number of atoms that make up each compound.
Write the compound formed by the following ions:1) Al3+ S2-
2) Mg2+ PO43-
When a formula is given…write the proper name. When a name is given…write the proper formula.
3) BaO
4) lithium bromide
5) Ni2S3
6) triphosphorous heptaoxide
7) N2O5
8) molybdenum (VI) nitride
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)
Write the total number of atoms that make up each compound.
Write the compound formed by the following ions:1) Al3+ S2-
2) Mg2+ PO43-
When a formula is given…write the proper name. When a name is given…write the proper formula.
3) BaO
4) lithium bromide
5) Ni2S3
6) triphosphorous heptaoxide
7) N2O5
8) molybdenum (VI) nitride
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)
POP QUIZ
Write the total number of atoms that make up each compound.
Write the compound formed by the following ions:1) Al3+ S2-
2) Mg2+ PO43-
When a formula is given…write the proper name. When a name is given…write the proper formula.
3) BaO
4) lithium bromide
5) Ni2S3
6) triphosphorous heptaoxide
7) N2O5
8) molybdenum (VI) nitride
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)
Answer Key
Al2S3
Mg3(PO4)2
barium oxide
nickel (III) sulfide
LiBr
dinitrogen pentaoxide
MoN2
8
21
PbI4
P3O7
Polyatomic Ions - Quiz
oxalate
chromate
dichromate
permanganate
acetate
C2O42- ……………
CrO42- ……………
Cr2O72- …………..
MnO41- …………..
CH3COO1- …….
Exceptions!Two exceptions to the simple –ide ending are the diatomic oxide ions, O2
2- and O21-.
O22- is called peroxide
O21- is called superoxide.
Note the differences.
barium oxide __________barium peroxide __________
sodium oxide __________sodium peroxide __________
potassium oxide __________potassium superoxide __________
BaOBaO2
Na2ONa2O2 Do Not Reduce to lowest terms!
K2OKO2
Ba2+
Na1+
K1+
Ionic Compounds:Polyatomic Ions
KeysKeysKeysKeys
Ionic Compounds: Polyatomic Ions
Chart of the Ions and Polyatomic Ions
Polyatomic Ions Grid to Memorize Ionic Compounds: Polyatomic Ions
Ionic Binary Compounds:Multiple-Charge Cations
KeysKeysKeysKeys
Ionic Binary Compounds: Multiple-Charge Cations
Ionic Binary Compounds: Multiple-Charge Cations
Naming Chemical Compounds
Binary Compound?
Use the strategysummarized
earlier
Polyatomic ions present?
This is a compound for which naming procedures have not yet been considered.
Name the compound using procedures similar to those for naming binary ionic compounds.
Yes
YesNo
No
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 102
Oxidation Numbers and Ionic Compounds
KeysKeysKeysKeys
Oxidation Numbers and Ionic Compounds
Oxidation Numbers and Ionic Compounds
Names and Formulas of Compounds
KeysKeysKeysKeys
Names and Formulas of Compounds
Names and Formulas of Compounds
Subscripts, Superscripts and Coefficients
1
2
3
4
5
6
1
2
3
4
5
6
Electronegativities
7
Be
1.5
Al
1.5
Si
1.8
Ti
1.5
V
1.6
Cr
1.6
Mn
1.5
Fe
1.8
Co
1.8
Ni
1.8
Cu
1.9
Zn
1.7
Ga
1.6
Ge
1.8
Nb
1.6
Mo
1.8
Tc
1.9
Ag
1.9
Cd
1.7
In
1.7
Sn
1.8
Sb
1.9
Ta
1.5
W
1.7
Re
1.9
Hg
1.9
Tl
1.8
Pb
1.8
Bi
1.9
1.5 - 1.9
N
3.0
O
3.5
F
4.0
Cl
3.0
3.0 - 4.0
C
2.5
S
2.5
Br
2.8
I
2.5
2.5 - 2.9
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Ba
0.9
Fr
0.7
Ra
0.9
Below 1.0
H
2.1
B
2.0
P
2.1
As
2.0
Se
2.4
Ru
2.2
Rh
2.2
Pd
2.2
Te
2.1
Os
2.2
Ir
2.2
Pt
2.2
Au
2.4
Po
2.0
At
2.2
2.0 - 2.4
Per
iod
Actinides: 1.3 - 1.5
Li
1.0
Ca
1.0
Sc
1.3
Sr
1.0
Y
1.2
Zr
1.4
Hf
1.3
Mg
1.2
La
1.1
Ac
1.1
1.0 - 1.4
Lanthanides: 1.1 - 1.3
1A
2A
3B 4B 5B 6B 7B 1B 2B
3A 4A 5A 6A 7A
8A
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373
8B
Interpretation of a Chemical Formula
Sulfuric Acid
H2SO4
Two atomsof hydrogen
One atom of sulfur
Four atoms of oxygen
HH
O
S
OO
O
Chemical Formulas
C8H18 Subscript indicates that there are 8 carbon atoms in a molecule of octane.
Subscript indicates thatthere are 18 hydrogen atoms
In a molecule of octane.
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 203
Stock System of Nomenclature
CuCl2 Name of Roman cation numeral
indicating charge
Name of anion+
copper (II) chloride
Chemical Formulas
Al2(SO4)3Subscript 2
refers to2 aluminum
atoms.
Subscript 4refers to4 oxygenatoms in
sulfate ion.
Subscript 3 refers toeverything inside parentheses.Here there are 3 sulfate ions, with a total of 3 sulfur atoms
and 12 oxygen atoms.
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 204
Naming Binary Ionic Compounds
Al2O3
Name of cation Name of anion
aluminum oxide
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 207
The Stock System of Nomenclature
CuCl2Name of Name of anion cation
Copper (II) chloride
Romannumeral
indicatingcharge
+
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 208
Bonding Activity
Common Polyatomic Ions
O2-
K1+
K1+
Mg2+
Br1-
Br1-
K Br
potassium atom bromine atom
e- e- Br1-K1+
potassium ion bromide ionpotassium bromide
K Br
potassium atom bromine atom
e-
Br1-K1+
potassium ion bromide ion
KBr
MgBr2 K2Omagnesium bromide potassium oxide
Ca2+
Al3+
K1+
Pb4+
Br1-
O2-
N3-
K1+
K1+
Mg2+
Br1-
Br1-
PO43-
S2-
Cu2+
OH1-
OH1-NH41+
NO31-
?
Chemical Bonding Activity
Ca2+
Al3+
Na1+
Pb4+
OH1-
N2-
N3-
M1+
Mg2+
OH1-
OH1-
N3-
Pb4+
N3-
N3-
Pb4+
N3-
Pb4+
N3-
?
(nonmetal)M1+
(metal)
Pb4+ N3-
(metal)(metal)
M2+
(metal)
Pb3N4
lead (IV) nitrideor
plumbic nitride
Chemical Bonding Activity
KeysKeysKeysKeys
Chemical Bonding Activity (pink/blue)Chemical Bonding Activity Pieces
Chemical Bonding Activity (pink/blue)Chemical Bonding Activity Pieces
Key
Cu2+
Al3+
K1+ Pb4+Br1-
O2-
N3-
K1+
K1+
Mg2+
Br1-
Br1-
N3-
N3-
Pb4+
N3-
Pb4+
N3-
1.
2.
3.
4. 5.
6. OH1-
OH1-
NH41+
NO31-
7.
KBr
K2O
MgBr2
AlN
Cu(OH)2
NH4NO3
Pb3N4
http://www.unit5.org/christjs/4bondingact.doc
Key
Fe2+
8. 9. 10.
Ca2+
Ca2+
Ca2+
PO43-
PO43-
PO43-
NH41+
NH41+
NH41+
O2-
Al3+
Al3+
O2-
O2-
O2-
11.
Ca3(PO4)2
(NH4)3PO4
FeOAl2O3
Key
12.
15.
O2-
O2-
Fe3+
Fe3+
O2-
O2-
O2-
13.
Pb4+
S2-
S2-
Pb4+
S2-
S2-
Pb2+ S2-
14.
Cu2+
Cu1+
Cu1+
16.
Fe2O3
Pb2S3
PbS
CuO
Cu2OPb2S4PbS2
Molecular Models Activity
KeysKeysKeysKeys
Molecular Model's Activity
Molecular Model's Activity
Molecular Models Activity
ammonia
hydrogen monochloride
trichloromethane
urea
propane
butane
nitrogen triiodide (video)
carbon tetrachloride
methane
water
ethane
ethyne
dihydrogen monosulfide
carbon dioxide
supplies
Bonding and Shape of Molecules
Number of Bonds
Number of Unshared Pairs Shape Examples
2
3
4
3
2
0
0
0
1
2
Linear
Trigonal planar
Tetrahedral
Pyramidal
Bent
BeCl2
BF3
CH4, SiCl4
NH3, PCl3
H2O, H2S, SCl2
-Be-
B
C
N
:
O
:
:
CovalentStructure
Carbon tetrachloride
C ClClCl
Cl
CCl4
C109.5o
Cl
ClClCl
Carbon tetrachloride – “carbon tet” had been used as dry cleaning solventbecause of its extreme non-polarity.
Tetrahedral geometry
Methane
CHH
HH
C109.5o
H
HHH
Methane –The first member of the paraffin (alkane) hydrocarbons series. a.k.a. (marsh gas, CH4).
Tetrahedral geometry
Water
....
H HOBent
geometry
SO2
(-)
(+)
Polar molecule
Ethane
CH
CHH
HHH
space-filling molecule
ball-and-stickLewis dot notation
C2H4
molecular formula
C = 1s22s22p2
Ethane
CH
CHH
HHH
space-filling molecule
ball-and-stickLewis dot notation
C2H4
molecular formula
Ethyne
CCH H CCH H
No octet
Stable octet
6 electrons = triple bond
CCH H
C2H2
CCH H
each C “feels” 6 electrons
each C “feels” 7 carbons
Ethyne – a.k.a. “acetylene”
Dihydrogen monosulfide
....
H HS
Bent
SO2
Carbon dioxide
O OC
Lineargeometry
C OOCO2
C OO
Ammonia
NH HH
N107o HH
H
..
NH3
..
HH
H
N
TrigonalPyramidalgeometry
NH HH
Hydrogen monochloride
H ClHCl
H Cl
(-)(+)
H Cl
Polar molecule
HCl(g) + H2O(l) HCl(aq)
hydrogenchloride
water hydrochloric acid
Trichloromethane
C ClClCl
H
CHCl3
C109.5o
H
ClClCl
C ClClCl
H
(-)
(+)
Polar molecule
Tetrahedral geometry
Urea
CON HH
NH H
CON HH
NH H
CO(NH2)2
NOT “di-urea”
Urea – The first organic compound to be synthesized (Wohler, 1828).
Propane
CH
CHH
CH
HHHH
C C C
HH
H
HH H H
H
C3H8
Butane
CH
CHH
CH
C HH
HHHHH - C - C - C - C - H
H H H H
H H H H
C4H10 C C C
HH
H
HH H H
HC
H
H
Nitrogen triiodide
NI II N
107o III
..
NI3
TrigonalPyramidalgeometry
Video clip:
(slow motion)
detonation of NI3
Supplies
15 black (carbon) 8 green (chlorine and iodine) 1 yellow (sulfur) 4 blue (oxygen) 4 red (nitrogen) 42 hydrogen (hydrogen) 67 bonds (bonds)
C Cl I S O N H
C ClClCl
ClCH
H HH
C OO
SH HC C HH
C ClClCl
H
H Cl
CCl4 CH4
CO2
C2H2
HClCHCl3
SH2
CH
CHH
CH
C HH
HHHHCH
CHH
CH
HHHH
NH HH
NI II
Decomposition of Nitrogen Triiodide
Decomposition of Nitrogen Triiodide
2 NI3(s) N2(g) + 3 I2(g)
NI3 I2
N2
C109.5o
H
HHH
N107o HH
H
..
O104.5o H
H
..
..
CH4, methane NH3, ammonia H2O, water
..
O
O
O
lone pairelectrons
OOO
O3, ozone
......
The VSEPR Model
O OC
Linear
The Shapes of Some Simple ABn Molecules
O OS
BentO O
S
O
Trigonalplanar
FF
F
N
Trigonalpyramidal
T-shaped Squareplanar
F FCl
F
F F
Xe
F FF
F
FP
F
F
Trigonalbipyramidal
Octahedral
FF
F
S
F
F
F
AB6
SO2
Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 305