Chapter 16 Carbohydrates Classification Nomenclature Reactions.
Unit 2 Periodic Table, Chemical Formulas, Nomenclature, Simple Reactions, Balancing Reactions.
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Transcript of Unit 2 Periodic Table, Chemical Formulas, Nomenclature, Simple Reactions, Balancing Reactions.
Unit 2Periodic Table, Chemical Formulas, Nomenclature, Simple Reactions, Balancing Reactions
Periodic Table
Nomenclature: Molecular Compounds
Most are named by rules of Organic Chemistry
Simple Molecular compounds tend to be Binary nonmetallic
Use standard prefixes
2 kinds of elements
On the Right side of the periodic table
→ →
Nomenclature: Ionic Compounds
(–) ion(+) ion
Nomenclature: Simple Ions
Find patterns on the periodic table:
NO
BLE
GA
SESHH
–1
–2+2+
1 –3
–4
+3
+4
+ 5
Nomenclature: Ionic Compounds
Polyatomic ions may be involved… Let’s look at those…
A list appears in the appendix of your lab manual.
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
Cl
F
Br
I
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
Cl
F
Br
I
–1
–1
–1
–1
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
Cl
F
Br
I
Per ate - +1 oxygen ate - Most common ite - –1 oxygenHypo ite - –2 oxygens
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
ClO3–1
FO3–1
BrO3–1
IO3–1
Per ate - +1 oxygen ate - Most common ite - –1 oxygenHypo ite - –2 oxygens
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
ClO4–1
FO4–1
BrO4–1
IO4–1
Per ate - +1 oxygen ate - Most common ite - –1 oxygenHypo ite - –2 oxygens
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
ClO2–1
FO2–1
BrO2–1
IO2–1
Per ate - +1 oxygen ate - Most common ite - –1 oxygenHypo ite - –2 oxygens
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
ClO–1
FO–1
BrO–1
IO–1
Per ate - +1 oxygen ate - Most common ite - –1 oxygenHypo ite - –2 oxygens
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
S
O
Se
Te
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
S–2
O–2
Se–2
Te–2
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
SO4–2
O
SeO4–
2
TeO4–
2
The -ates
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
P
N
As
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
P–3
N–3
As–3
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
PO4–3
NO3–1
AsO4–
3
The -ates
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
Si
C
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
Si–4
C–4
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
SiO3–2
CO3–2The -ates
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
B
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
B+3
Yikes!
Nomenclature: Polyatomic Ions
Find patterns on the periodic table:
NO
BLE
GA
SES
BO3–3The -ates
Nomenclature: Ionic Compounds
On occasion, ionic compounds may exist as a hydrate.
A hydrate is when one or more water molecules (H2O) connect to a solid ionic compound.
Barium hydroxide octahydrate –
ZnCl2•6 H2O –
Ba(OH)2 • 8 H2OZinc chloride hexahydrate
Nomenclature: Ionic Compounds
Ionic compounds with transition metal ions – those that have multiple valences.
Nomenclature: Transition Metal Ions
Find patterns on the periodic table:
This area!
Nomenclature: Transition Metal Ions
Find patterns on the periodic table:
+1+2+3+4 +5 +1+2+3+4
+5+1+2+3+4
+1+2+3+4 +5+6
+3
+3
Notice the patternsLeft to right
AndRight to left
Nomenclature: Transition Metal Ions
Find patterns on the periodic table:
+1+2+3+4 +5 +1+2+3+4
+5+1+2+3+4
+1+2+3+4 +5+6
+3
+3+4
+3+5
+3+3+3 +3+3+3
What goes here?
Nomenclature: Transition Metal Ions
Find patterns on the periodic table:
+1+2+3 +1+2+3+4
+5+1+2+3+4
+1+2+3+4 +5+6
+3
+3+4
+3+5
+3+3+3 +3+3+3+3+2
+3+2
+3+2
+3+2
+3+2
Nomenclature: Transition Metal Ions
Find patterns on the periodic table:
+1+2+3 +1+2+3+4
+1+2+3
+1+2+3
+4
+4
+5
+5+6
+3
+3+4
+3+5
+3+3
+2+3
+2+3
+2+3
+2+3
+2+2
+1
+3+1
+4+2
+4+2
+5+3
+5+3
Nomenclature: Transition Metal Ions
Find patterns on the periodic table:
+1+2+3 +2+3+4
+1+2+3
+2 +3 +6
+3
+3+4
+3+5
+3+3
+2+3
+2+3
+2+3
+2+3
+2+2
+1
+3+1
+4+2
+4+2
+5+3
+5+3
mercury(I) = Hg2
+2
mercury(II) = Hg+2
Nomenclature: Transition Metal Ions
Stock system – Use a Roman numeral for the ionic charge (valence)
Nomenclature: Transition Metal Ions
Traditional system – Use the Latin roots with –ic or –ous endings.
mercur-
cobalt-
cupr-
ferr-
stann-
plumb-
aur-
Nomenclature: Transition Metal Ions
Traditional system – –ic ending
Considered the most common charge of the ions
–ous endingConsidered the second most common charge of the ions
Based on the trends shown on the periodic table, the most common charge is the highest charge listed; the second most common charges is the lower charge listed.
Nomenclature: Acid Compounds
Binary AcidsContain only hydrogen (H+) and one other element – a nonmetal
These are named with ‘hydro’ ‘ic acid’
Nomenclature: Acid Compounds
Ternary Acids (oxyacids)– Contain hydrogen and a polyatomic ion (a
oxyradical) that either ends in –ate or –ite.• -ate goes to –ic• -ite goes to –ous• Ponder gum… “If you ate it it is icky; but if
you bite it, it is delicious.”
Nomenclature: Practice
1. Decide which of the following are expected to be ionic and which are expected to be molecular:a) KF
b) N2O5
c) SiCl4
2. What is the formula of magnesium nitride?
3. What is the formula of calcium phosphate?
ioniccovalentcovalent
Mg3N2
Ca3(PO4)2
Nomenclature: Practice
4. Give the formula of carbon disulfide.
5. Give the formula of dinitrogen tetrafluoride.
6. Calcium chloride hexahydrate is used to melt snow from roads. What is the formula of this compound?
CS2
N2F4
CaCl2•6 H2O
Nomenclature: Practice
7. Name BaO.
8. Name Cr2(SO4)3.
9. Name OF2.
10.Name S4N4.
11.Bromine has an oxyacid HBrO2, whose name is bromous acid. What is the name and formula for the corresponding ion?
chromium(III) sulfate
barium oxide
oxygen difluoride
tetrasulfur tetranitride
BrO2–1 = bromite
Nomenclature: Practice
12.Name HIO.
13.Name H3PO4.
14.A compound whose common name is green vitriol has the chemical formula FeSO4•7 H2O. What is the chemical name of this compound?
hypoiodous acid
phosphoric acid
iron(II) sulfate heptahydrate
General Reactions
• Synthesis– Two elements makes a Binary compound
• Fe + O2 Fe2O3
– Two oxides makes a Ternary compound• Metal oxide + water makes metal hydroxide
– BaO + H2O Ba(OH)2
• Nonmetal oxide + water makes acid
– N2O5 + H2O HNO3
• Metal oxide + Nonmetal oxide makes ternary compound
– BaO + N2O5 Ba(NO3)2
→
→
→
→
General Reactions
• Notice the ions are staying the same!!!– Oxygen is O–2
– Barium is Ba+2
– Hydroxide is OH–1
– Nitrate is NO3–1 and familiar
General Reactions
• Decomposition (the opposite of synthesis)– Binary compound will make two elements– Metal hydroxide makes metal oxide and water– Ternary acid makes nonmetal oxide and water– Ternary compound (many) makes nonmetal oxide
and metal oxide.• One of the most common is that of a metal
carbonate:
• MgCO3 MgO + CO2
– Metal chlorate makes metal chloride and oxygen gas
• Ba(ClO3)2 BaCl2 + O2
→
→
General Reactions
• Single Replacement– A metallic element + a compound switches
the positive ions.
• MgCO3 + Li Li2CO3 + Mg
– A nonmetallic element (usually a halogen) + a compound switches the negative ions.
• Cl2 + FeBr3 FeCl3 + Br2
→
→
General Reactions
• Double Replacement– Positive ions and Negative ions switch
positions.– Take time to identify these ions.
• MgCO3 + Sn(ClO3)4
→
Mg+2 CO3–2 Sn+4 ClO3
–1
Sn(CO3)2 Mg(ClO3)2+
General Reactions
• Double Replacement– Try another
• Sb(OH)3 + Zn3P2→
Sb+3 OH–1 Zn+2 P–3
SbP + Zn(OH)2
General Reactions
• Combustion– Typically a hydrocarbon burns in the
presence of oxygen to create water and carbon dioxide• Hydrocarbons are made of –• On occasion, they include oxygen, as
well. • CH4 + O2
• C2H5OH + O2
→ CO2 + H2O
hydrogen + carbon
→ CO2 + H2O
General Reactions
• Acid-Carbonate– There must be an acid and a metal
carbonate – check for these BEFORE presuming double replacement.
– These will create water, carbon dioxide, and an ionic salt.• Li2CO3 + HNO2→ CO2 + H2O
Li+1 CO3–2 H+1 NO2
–1
+ LiNO2
Balancing Reactions• Based on the Law of Conservation, is present
must be preserved. In other words, whatever happens to the reactants must occur to the products.– Choose a chemical – insert a coefficient
(multiplier) in front of it. Never change the subscripts!
– Treat ions (radicals) that appear on both sides as single chunks.
– ½’s can be used for diatomic elements.– It is helpful to think of water as HOH, rather
than H2O.
Balancing Reactions• Whatever happens to the reactants must occur to the
products.• Choose a chemical – insert a coefficient (multiplier) in
front of it. Never change the subscripts!• Treat ions (radicals) that appear on both sides as single
chunks.• ½’s can be used for diatomic elements.• It is helpful to think of water as HOH, rather than H2O.
MgCO3 + Sn(ClO3)4 Mg(ClO3)2 + Sn(CO3)2
→ 2 1 2 1
Balancing Reactions• Whatever happens to the reactants must occur to the
products.• Choose a chemical – insert a coefficient (multiplier) in
front of it. Never change the subscripts!• Treat ions (radicals) that appear on both sides as single
chunks.• ½’s can be used for diatomic elements.• It is helpful to think of water as HOH, rather than H2O.
C4H8OH + O2 CO2 + H2O→ 1 23/2
8 ? 2 9
4 C4H8OH + 23 O2 16 CO2 + 18 H2O
→