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Molecules and Compounds
Compounds Display Constant
Composition
• Elements combine in fixed Proportions
• Law of Constant Composition
– H2O
– CO2
Molecules and Compounds
Compounds Display Constant
Composition
If we decompose water, we find 16.0 grams of
oxygen to every 2.00 grams of hydrogen. This
produces an Oxygen to Hydrogen mass ratio of
8.0.
Mass ratio = 16.0 grams = 8.0
2.00 grams
Water has a constant Mass Ratio of Oxygen to
Hydrogen of 8.0.
Molecules and Compounds
Chemical Formulas: How to
Represent Compounds
• Chemical Formula
– Elements present
– Relative numbers
• Subscripts
– Part of the definition
– Changing subscript changes compound
• Metals – Left-hand side of Periodic Table
– Listed first
• Nonmetals – Right-hand side of the Periodic Table
– Those to the left– More Metal-like
– Listed first
Significance of Chemical
Formulas
• A chemical formula indicates the relative
number of atoms of each kind in a
chemical compound.
• For a molecular compound, the chemical
formula reveals the number of atoms of
each element contained in a single
molecule of the compound.
– example: octane — C8H18
Molecules and Compounds
Writing Chemical Formulas
• Compound containing 2 aluminum atoms to
every 3 oxygen atoms
– Al2O3
• Compound containing 3 oxygen atoms to
every 1 sulfur atom
– SO3
Molecules and Compounds
Chemical Formulas: How to
Represent Compounds
• Water – H2O
– Hydrogen and
oxygen atoms
– 2:1 ratio
– Symbol and
subscript
– Dihydrogen
monoxide
Chemical Formulas and Compounds
Chemical Formulas: How to
Represent Compounds
• Carbon dioxide – CO2
–
–
–
–
–
Carbon and oxygen atoms
1:2 ratio
Symbol and subscript
Carbon dioxide
Two nonmetals
• Left-most listed first
• One carbon – not mono
• The chemical formula for an ionic
compound represents one formula unit—
the simplest ratio of the compound’s
positive ions (cations) and its negative
ions (anions).
– example: aluminum sulfate — Al2(SO4)3
– Parentheses surround the polyatomic ion
a unit. The subscript 3 refers to the unit.
SO42- to identify it as
Molecules and Compounds
Writing Chemical Formulas
Polyatomic Ions
• Contain several identical groupings of
atoms
• Polyatomic Ions
• Parenthesis
• Mg(NO3)2
• Magnesium nitrate
Molecules and Compounds
Writing Chemical Formulas
Polyatomic Ions
•
•
•
•
Mg(NO3)2
1 Mg
2N
6O
Molecules and Compounds
Molecular View of
Elements and Compounds
• Atomic Elements
– Single atoms
– Most Elements
• Molecular Elements
– Diatomic atoms
– Two atoms bonded together
– H2, N2, O2, F2, Cl2, Br2, I2
• Molecular Compounds
– Two or more Nonmetals
• Ionic Compounds
– Metal and nonmetal
Molecules and Compounds
Molecular View of
Elements and Compounds
Molecules and Compounds
Writing Formulas for
Ionic Compounds
•
•
•
•
Charge Neutral
Most elements form only one type of ion
Predictable charge
Sodium chloride
– Na  +1
– Cl  –1
– NaCl
• Magnesium chloride
– Mg  +2
– Cl  –1
– MgCl2
Common Monatomic Ions
(pg.221 in your textbook)
Common Monatomic Ions…
Molecules and Compounds
Writing Formulas for
Ionic Compounds
1.
2.
3.
4.
5.
Write the symbol for the metal and its charge
Write the symbol for the nonmetal and its
charge
Charge (without sign) becomes subscript for
other ion
Reduce subscripts to smallest whole number
ratio
Check that the sum of the charges of the cation
cancels the sum of the anions
Molecules and Compounds
Writing Formulas for
Ionic Compounds
Ionic compound between aluminum and oxygen
Al3+
O2–
Al2O3
2 (+3) = +6
3 (–2) = –6
Molecules and Compounds
Writing Formulas for
Ionic Compounds
Ionic compound between magnesium and oxygen
Mg2+
O2–
MgO
1 (+2) = +2
1 (–2) = –2
Smallest whole number ratio is 1:1
Molecules and Compounds
Naming Ionic Compounds
• Metal and Nonmetal
• Two Types
– Type I
• Metal has constant predictable charge
• Inferred from group number in Periodic Table
– Type II
• Charge NOT always the same
• Transition Metals
Molecules and Compounds
Naming Ionic Compounds
Type I Binary Ionic Compounds
• Binary compounds
– Two different kinds of elements
– Cation + anion with IDE
• Metal
– Predictable constant charge
– Name of metal
• Nonmetal
– Name of nonmetal
– Ending  IDE
Molecules and Compounds
Naming Ionic Compounds
Type I Binary Ionic Compounds
• Binary compounds
– Two different kinds of elements
– Cation + anion with IDE
• Metal
– Predictable constant charge
– Name of metal
• Nonmetal
– Name of nonmetal
– Ending  IDE
Molecules and Compounds
Naming Ionic Compounds
Type I Binary Ionic Compounds
• MgF2
– Metal  Magnesium
– Nonmetal  Fluoride
– Magnesium fluoride
• KBr
– Metal  Potassium
– Nonmetal  Bromine
– Potassium bromide
Molecules and Compounds
Naming Ionic Compounds
Type I Binary Ionic Compounds
• CaCl2
– Metal  Calcium
– Nonmetal  Chlorine
– Calcium chloride
• Na2O
– Metal  Sodium
– Nonmetal  Oxygen
– Sodium oxide
Molecules and Compounds
Naming Ionic Compounds
Type II Binary Ionic Compounds
• Binary compounds
– Two different kinds of elements
– Cation + anion with IDE
• Metal
– Charge NOT always the same
– Transition metals and roman
numeral for charge
– Name of metal
• Nonmetal
– Name of nonmetal
– Ending  IDE
Molecules and Compounds
Naming Ionic Compounds
Type II Binary Ionic Compounds
• FeCl3
–
–
–
–
Metal  Iron
Nonmetal  Chlorine
Charge on Iron must be +3
Iron(III) chloride
• CrO
–
–
–
–
Metal  Chromium
Nonmetal  Oxygen
Charge on Chromium must be +2
Chromium(II) oxide
Molecules and Compounds
Naming Ionic Compounds
Type II Binary Ionic Compounds
• PbCl4
– Metal  Lead
– Nonmetal  Chlorine
– Charge on Lead must be +4
– Lead(IV) chloride
• Must determine charge of Cation
from the Formula
Molecules and Compounds
Naming Ionic Compounds
Polyatomic Ions
• Group of atoms with an overall charge
• Common Polyatomic Ions on pg. 226 in
textbook. MEMORIZE (flashcards?)
Molecules and Compounds
Naming Ionic Compounds
Polyatomic Ions
• KNO3
– Metal  Potassium
– Nonmetal  Nitrate
– Potassium nitrate
• FeSO4
– Metal  Iron
– Nonmetal  Sulfate
– Iron(II) sulfate
Ionic Compounds Containing
Polyatomic Ions….
• Write the formula for tin(IV) sulfate
• Sn(SO4)2
Molecules and Compounds
Naming Molecular Compounds
• Molecular Compounds
•Prefixes
• Two or more nonmetals
Mono – 1
• Right of the Periodic Table
Di – 2
Tri – 3
• Binary Molecular Compounds
Tetra – 4
Penta – 5
• Two elements
Hexa – 6
Hepta – 7
• Most “metal-like” first
Octa – 8
• Prefix [Element 1] Prefix [Element 2]
Nona – 9
Deca - 10
• Do not begin with “mono” and if
prefix is two syllables (& element
starts with vowel) then drop the
ending vowel of prefix.
Molecules and Compounds
Nomenclature: Naming
Compounds
• Systematic ways to name compounds
• Common names
• Water
– H2O
– Common name  Water
– Systematic name  Dihydrogen monoxide
Molecules and Compounds
Naming Molecular Compounds
• CO2
• Most “metal-like” – Carbon
• Nonmetal – Oxygen
• Carbon dioxide
• N2O
• Most “metal-like” – Nitrogen
• Nonmetal – Oxygen
• Dinitrogen monoxide
• Give name for As2O5:
• Write formula for oxygen difluoride:
Molecules and Compounds
Naming Acids
•Acids
–Molecular Compounds
–Form H+
–Sour Taste
•Binary Acids- acids that consist of two
elements (usually hydrogen and a
halogen)
•Oxyacids – acids that contain
hydrogen, oxygen and a third element
(usually a nonmetal)
Binary Acids…
If anion ends in “ide” then acid name is
“hydro—ic”
• HCl hydrochloric acid
• HBr hydrobromic acid
• HI hydroiodic acid
Naming Oxyacids
• No “hydro” in name
• If anion ends in “ate” then acid name is “—
ic”
• If anion ends in “ite” then acid name is “—
ous”
Oxyacids
Anion
sulfate SO42sulfite SO32nitrate NO3phosphate PO43-
Acid _____
sulfuric acid H2SO4
sufurous acid H2SO3
nitric acid HNO3
phosphoric acid H3PO4
Salts
• An ionic compound composed of a cation
and the anion from an acid is often
referred to as a salt.
– examples:
• Table salt, NaCl, contains the anion from
hydrochloric acid, HCl.
• Calcium sulfate, CaSO4, is a salt containing the
anion from sulfuric acid, H2SO4.
Oxidation Numbers
• The charges on the ions in an ionic compound
reflect the electron distribution of the compound.
• In order to indicate the general distribution of
electrons among the bonded atoms in a molecular
compound or a polyatomic ion, oxidation numbers
are assigned to the atoms composing the
compound or ion.
• Unlike ionic charges, oxidation numbers do not
have an exact physical meaning: rather, they serve
as useful “bookkeeping” devices to help keep track
of electrons.
Assigning Oxidation Numbers
In general when assigning oxidation numbers,
shared electrons are assumed to “belong” to
the more electronegative atom in each bond.
More-specific rules are provided by the
following guidelines.
1. The atoms in a pure element have an
oxidation number of zero.
examples: all atoms in sodium, Na,
oxygen, O2, phosphorus, P4, and sulfur,
S8, have oxidation numbers of zero.
Assigning Oxidation Numbers,
continued..
2. The more-electronegative element in a
binary compound is assigned a
negative number equal to the charge it
would have as an anion. Likewise for
the less-electronegative element.
3. Fluorine has an oxidation number of –1
in all of its compounds because it is
the most electronegative element.
Assigning Oxidation Numbers,
continued..
4. Oxygen usually has an oxidation number of –2.
– Exceptions:
• In peroxides, such as H2O2,
oxygen’s oxidation number is –1.
• In compounds with fluorine, such as OF2, oxygen’s oxidation
number is +2.
5. Hydrogen has an oxidation number of +1 in all
compounds containing elements that are more
electronegative than it; it has an oxidation number
of –1 with metals.
Assigning Oxidation Numbers,
continued..
6. The algebraic sum of the oxidation numbers
of all atoms in an neutral compound is equal
to zero.
7. The algebraic sum of the oxidation numbers
of all atoms in a polyatomic ion is equal to
the charge of the ion.
8. Although rules 1 through 7 apply to
covalently bonded atoms, oxidation
numbers can also be applied to atoms in
ionic compounds similarly.
Assigning Oxidation Numbers,
continued..
Assign oxidation numbers to each atom
in the following compounds or ions:
a. UF6
b. H2SO4
c. ClO3-
Molecules and Compounds
Nomenclature Summary
Molecules and Compounds
Formula Mass & Molar Mass
• Formula Mass - Average mass of the
Molecules that compose a compound
(in a.m.u.’s)
• Molar Mass – Average mass of the
molecules that compose a mole
(6.02x1023) of the compound (in
grams/mole)
Same values different units!
Molar Mass Calculation
• What is the molar mass of barium
nitrate, Ba(NO3)2?
• 262.35 g/mol