unit 5: bonding and inorganic nomenclature
DESCRIPTION
lithium nitrate. lead (II) sulfide. Outline. barium sulfide. lithium nitride. Chemistry. sulfur dioxide. lithium nitrite. Unit 5: Bonding and Inorganic Nomenclature. NO 2. NaClO 3. N 2 O 4. Fe(ClO 3 ) 2. N 2 O 5. Fe(ClO 3 ) 3. PowerPoint Presentation by Mr. John Bergmann. - PowerPoint PPT PresentationTRANSCRIPT
Unit 5: Bonding andInorganic Nomenclature
Chemistry
NaClO3
Fe(ClO3)2
lithium nitrate
lithium nitride
lithium nitrite
lead (II) sulfide
barium sulfide
sulfur dioxide
Fe(ClO3)3
NO2
N2O4
N2O5
Outline
PowerPoint Presentation by Mr. John Bergmann
Chemical Bonding Ionic Bonds: atoms give up or gain e– and
are attracted to each other by coulombic attraction
Na Na1+ Cl Cl1–loses e– gains e–
Na1+ + Cl1– NaCl
K1+ + NO31– KNO3
ionic compounds = salts
where NO31– is a polyatomic ion:
a charged group of atoms that stay together
Properties of Salts
1. very hard –
2. high melting points –
3. brittle –
each ion is bondedto several oppositely-charged ions
many bonds must be broken
with sufficient force,like atoms arebrought next toeach other and repel
calcite
Covalent Bonds …atoms share e– to get a full valence shell
Lewis structure:
1. Two shared e– make a single covalent bond,four make a double bond, etc.
2. unshared pairs: pairs of unbonded valence e–
3. Each atom needs a full outer shell, i.e., 8 e–. Exception: H needs 2 e–
a model of a covalent molecule that
shows all of the valence e–
1s2 2s2 2p2 (4 v.e–) 1s2 2s2 2p5 (7 v.e–)
both need 8 v.e– for a full outer shell (octet rule)
CF
x
x
H
x x
xx
x xF x
carbon tetrafluoride (CF4)
o
Co
o o
x
xxx
x xF x
o
Co
o ox
xxx
x xF x
x
xxx
xF x
x
xxx
x xF x
x
x
xxx
x xF x
x
xxx
x xF x
x
xxx
x xF x
methane (CH4)
o
Co
o o
H x
o
Co
o oH x
xH
x H
H x
H x
H x
ooo
oN o
nitrogen triiodide (NI3)
carbon dioxide (CO2)
x x
xx
x x I x
x
xxx
x x I x
x
xxx
x x I x
xxx
x x I x
x
x
xxx
x x I x
x
xxx
x x I xoo
o
oN o
o
Co
o o x
xxx
xO x
x
xxx
xO x
x
xxx
xO x
o
Co
o o O = C = O
x x
x x x x
x x
x
xxx
xO x
butter
(consist of twononmetal elements)
covalent compounds = molecular compounds
-- have lower melting points than do ionic compounds
In insulators (like wood),the v.e– are attachedto particular atoms.
Metallic Bonds
In metals, valence shells of atoms overlap, so v.e– are free to travel between atoms through material.
Not so in metals.
All due to free-moving
v.e–.
Properties of Metals
ductile conduct heat and electricity
malleable
These are much weaker than ionic, covalent, or metallic bonds, but very important in determining states of matter, boiling and melting points, and
molecular shape (among other things).
Other Types of Bonds
dipole-dipole forces hydrogen bonds London dispersion forces ion-dipole forces
DNA
boiling H2O
Writing Formulas of Ionic Compounds
chemical formula:
To write an ionic compound’s formula, we need:1. the two types of ions 2. the charge on each ion
Na1+ and F1–
Ba2+ and O2– Na1+ and O2– Ba2+ and F1–
shows types of atomsand how many of each
NaF
BaONa2OBaF2
(i.e., “pink” and “blue”)
has neutral charge;
charge on cation / anion“becomes” subscript of anion / cation
** Warning:
Al3+ and O2– Ba2+ and S2– In3+ and Br1–
Reduce to lowest terms.
Al O Ba S In Br 2 3 2 2 31
Al2O3 BaS InBr3
criss-cross rule:
Writing Formulas w/Polyatomic Ions
Parentheses are required only when you need morethan one “bunch” of a particular polyatomic ion.
Ba2+ and SO42–
Mg2+ and NO21–
NH41+ and ClO3
1–
Sn4+ and SO42–
Fe3+ and Cr2O72–
NH41+ and N3–
BaSO4
Mg(NO2)2
NH4ClO3
Sn(SO4)2
Fe2(Cr2O7)3
(NH4)3N
Inorganic Nomenclature
potassiumnitrateKNO3
sodiumhydroxide
NaOH
dinitrogen monoxideN2O
copper (II)sulfateCu2SO4
Ionic Compounds (cation/anion combos)Single-Charge Cations with Elemental Anions
The single-charge cations are: groups 1, 2, 13, and Ag1+, Cd2+, and Zn2+
i.e., “pulled off the Table” anions
A. To name, given the formula:
2. Use name of anion (it has the ending “ide”).
1. Use name of cation.
NaF
BaO
Na2O
BaF2
sodium fluoride
barium oxide
sodium oxide
barium fluoride
Na
Ba
1. Write symbols for the two types of ions.2. Balance charges to write formula.
silver sulfide
zinc phosphide
calcium iodide
B. To write formula, given the name:
Ag1+ S2– Ag2S
Zn2+ P3– Zn3P2
I1– Ca2+ CaI2
CaAg
Zn
Multiple-Charge Cations with Elemental Anions
The multiple-charge cations are:
i.e., “pulled off the Table” anions
Pb, Sn, and the transition elements (but – of course! – not Ag, Cd, or Zn)
iron oxide
A. To name, given the formula:
1.Figure out charge on cation.2. Write name of cation.
3. Write Roman numerals in ( ) to show cation’s charge.4. Write name of anion.
FeO
Fe2O3
CuBr
CuBr2
iron oxide
CuFe
Stock Systemof nomenclature
Fe? O2– iron (II) oxide
Fe? O2– iron (III) oxide
copper bromide
copper bromide
Cu? Br1– copper (I) bromide
Cu2+ Br1– copper (II) bromide
Fe?
Br1–
O2– O2–
Fe2+
Fe3+ Fe3+
Cu1+
Cu?
B. To find the formula, given the name:1. Write symbols for the two types of ions.
2. Balance charges to write formula.
cobalt (III) chloride
tin (IV) oxide
tin (II) oxide
Co
Sn
Co3+ Cl1– CoCl3
Sn4+
O2–
O2–
Sn2+
SnO2
SnO
Compounds Containing Polyatomic Ions Insert name of ionwhere it should goin the compound’sname.
Write formulas:
iron (III) nitrite
ammonium phosphide
ammonium chlorate zinc phosphate lead (II) permanganate
iron (III) nitrite
ammonium phosphide
ammonium chlorate zinc phosphate lead (II) permanganate
Fe3+ NO31– Fe(NO3)3
NH41+
NH41+
P3– (NH4)3P
ClO31– NH4ClO3
Zn2+ PO43– Zn3(PO4)2
Pb2+ MnO41– Pb(MnO4)2
Write names:
(NH4)2S2O3
AgBrO3
(NH4)3N
U(CrO4)3
Cr2(SO3)3
(NH4)2S2O3
AgBrO3
(NH4)3N
U(CrO4)3
Cr2(SO3)3
ammonium thiosulfate
silver bromate
ammonium nitride
U? CrO42–
CrO42–
CrO42–
uranium (VI) chromate
Cr? Cr?
Cr3+ Cr3+ SO3
2– SO32–
SO32– chromium (III) sulfite
U6+
mono
Covalent Compounds -- contain two types of
** Key:
Use Greek prefixes to indicate howmany atoms of each element, but
don’t use “mono” on first element.
nonmetals nonmetals
FORGET CHARGES!
What to do:
1 –2 –3 –4 –5 –
6 –7 –8 –9 –
10 –
ditritetrapenta
hexaheptaoctanonadec
EXAMPLES:
carbon dioxide CO dinitrogen trioxide N2O5
carbon tetrachloride NI3
CO2 carbon monoxide N2O3
dinitrogen pentoxide CCl4
nitrogen triiodide
Dihydrogen Monoxide:A Tale of Danger and
Irresponsibility
-- major component of acid rain
-- found in all cancer cells-- inhalation can be deadly-- excessive ingestion results in acute physical symptoms:
e.g., frequent urination, bloated sensation, profuse sweating
-- often an industrial byproduct of chemical reactions; dumped wholesale into rivers and lakes
4. S F6
5. Fe (NO3)3
1. Ni2 S3
2. N F3
3. Na BrO3
6. Sr SO4
Writing Chemical NamesFormula RN/GP/neither
Use poly.ion sheet? Name
GPRN
RNGPneither
neither
noyes
nonoyes
yes
sulfur hexafluorideiron (III) nitrate
nickel (III) sulfidenitrogen trifluoridesodium bromate
strontium sulfate
10. oxygen difluoride
4. zinc arsenate5. silver nitride
1. copper (II) phosphide2. lithium phosphate3. phosphorus triiodide
7. dinitrogen pentasulfide8. tin (IV) nitride
6. sulfur dibromide
Writing Chemical Formulas
9. rubidium nitrite
11. iron (III) sulfite12. ammonium oxide
Name Charges matter?Use poly.
ion sheet? Formula
yesyes
yesyesno
noyes
no
yes
yesyes
no
yesno
noyesno
nono
no
yes
yesyes
no
Zn3(AsO4)2
Ag3N
Cu3P2
Li3PO4
PI3
N2S5
Sn3N4
SBr2
RbNO2
Fe2(SO3)3
(NH4)2O
OF2
Traditional System of Nomenclature
…used historically (and still some today) to name compounds w/multiple-charge cations
To use: 1. Use Latin root of cation. 2. Use -ic ending for higher charge; -ous ending for lower charge. 3. Then say name of anion, as usual.
Cu
Au Pb
Sn
Fe
(i.e., NOT the Stock System)
Write formulas: cuprous sulfide
auric nitrite
ferrous fluoride
Write names: Pb3P4
Pb3P2
Sn(OH)4
Cu1+ S2– Cu2S
Au3+ NO21– Au(NO2)3
Fe2+ F1– FeF2
cuprous sulfide
auric nitrite
ferrous fluoride
Pb3P4
Pb3P2
Sn(OH)4
Pb? P3– Pb? Pb?
Pb? Pb? Pb?
P3– P3– P3–
P3– P3– Pb2+
Pb4+
Pb2+
Pb4+ Pb4+
plumbic phosphidePb2+
plumbous phosphideOH1– Sn4+ Sn? OH1–
OH1– OH1–
stannic hydroxide
Element Latin root -ic -ous
gold, Au aur- Au3+
Au1+
lead, Pb plumb- Pb4+
Pb2+
tin, Sn stann- Sn4+
Sn2+
copper, Cu cupr- Cu2+
Cu1+
iron, Fe ferr- Fe3+
Fe2+
10. oxygen difluoride
4. zinc arsenate5. silver nitride
1. copper (II) phosphide2. lithium phosphate3. phosphorus triiodide
7. dinitrogen pentasulfide8. tin (IV) nitride
6. sulfur dibromide
Writing Chemical Formulas
9. rubidium nitrite
11. iron (III) sulfite12. ammonium oxide
Name Charges matter?Use poly.
ion sheet? Formula
yesyes
yesyesno
noyes
no
yes
yesyes
no
yesno
noyesno
nono
no
yes
yesyes
no
Zn3(AsO4)2
Ag3N
Cu3P2
Li3PO4
PI3
N2S5
Sn3N4
SBr2
RbNO2
Fe2(SO3)3
(NH4)2O
OF2
7. S O3
8. Sn Br4
Writing Chemical Names
9. K3 PO4
11. C S2
12. Cu F
10. NH4 OH
Formula RN/GP/neitherUse poly.
ion sheet? Name
GPneitherneither
GPRN
neither
nonoyes
nono
yes
sulfur trioxidetin (IV) bromide
potassium phosphate
carbon disulfidecopper (I) fluoride
ammonium hydroxide
Traditional System of Nomenclature
…used historically (and still some today) to name compounds w/multiple-charge cations
To use: 1. Use Latin root of cation. 2. Use -ic ending for higher charge; -ous ending for lower charge. 3. Then say name of anion, as usual.
Element Latin root -ic -ous
gold, Au aur- Au3+
Au1+
lead, Pb plumb- Pb4+
Pb2+
tin, Sn stann- Sn4+
Sn2+
copper, Cu cupr- Cu2+
Cu1+
iron, Fe ferr- Fe3+
Fe2+
Write formulas: cuprous sulfide
auric nitrite
ferrous fluoride
Write names: Pb3P4
Pb3P2
Sn(OH)4
Cu1+ S2– Cu2S
Au3+ NO21– Au(NO2)3
Fe2+ F1– FeF2
cuprous sulfide
auric nitrite
ferrous fluoride
Pb3P4
Pb3P2
Sn(OH)4
Pb? P3– Pb? Pb?
Pb? Pb? Pb?
P3– P3– P3–
P3– P3– Pb2+
Pb4+
Pb2+
Pb4+ Pb4+
plumbic phosphidePb2+
plumbous phosphideOH1– Sn4+ Sn? OH1–
OH1– OH1–
stannic hydroxide
Empirical Formula and Molecular Formula
Compound Molecular Formula
EmpiricalFormula
glucose C6H12O6
propane C3H8
butane C4H10
naphthalene C10H8
sucrose C12H22O11
octane C8H18
lowest-termsformula
shows the true numberand type of atoms in a
m’cule
CH2O
C3H8
C2H5
C5H4
C12H22O11
C4H9
0 0
0 0
Resources - Nomenclature
Objectives
Worksheet - binary cmpds: single charge cation
Worksheet - ions in chemical formulas
Worksheet - ionic cmpds: polyatomic ions w multiple-charge cation
Worksheet - ionic formulas (binary, polyatomic, transition)
Worksheet - traditional system of nomenclature
Worksheet - covalent binary cmpds: non-metal - non-metal
Worksheet - ionic cmpds: polyatomic ions
Outline (general)
Worksheet - empirical and molecular
Worksheet - vocab (bonding)
Activity - bonding pieces
Activity - molecular models
Activity - mole pattern
Worksheet - binary compounds
Worksheet - ions in chemical compounds
Textbook - questions
Worksheet - ionic binary cmpds: multiple charge cation
Worksheet - oxidation numbers and ionic cmpds
Worksheet - names and formulas of cmpds
Worksheet - errors in chemical formulas and nomenclature