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Chemical Compounds
Molecular and Ionic Formulas
Organic Compounds
Naming Simple Compounds
Chemical Formula
• Shows the kinds and numbers of atoms in
the smallest representative unit of the
substance.
• If only one atom of the element in a
compound, you only write the element’s
symbol. (Ex: Lithium fluoride LiF)
• If the molecules or formula unit of the
element each have more than one atom, a
number is used as a subscript. (Ex:
Lithium oxide Li2O).
Molecular Formulas
• Chemical formula for a molecular compound
is called a molecular formula.
• Shows the kinds and numbers of atoms
present in a molecule of a compound.
• Examples: CO, CO2
• Tells nothing about the structure of the
molecule --- doesn’t show arrangement of
the various atoms.
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Molecular Formulas (continued)
• Use models and/or diagrams to show the
arrangements of molecules in a molecular
compound.
• IMPORTANT NOTE: Be familiar with the
various types of representations of molecular
compounds: Molecular formula, structural
formula, Ball-and-Stick Molecular Model,
Space-filling molecular model.
– Figure 2.18 Page 56
Formula Units
• Chemical formulas represent ionic
compounds.
• Formula units – lowest whole-number
ration of ions in the compound.
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Laws of Definite and Multiple
Proportions
• Law of Definite Proportions: in samples of any
chemical compound, the masses of the elements
are always in the same proportions.
• Law of Multiple Proportions: whenever two
elements form more than one compound, the
different masses of one element that combine with
the same mass of the other element are in the ratio
of small whole numbers.
Ionic Charges
• For most of the Group A elements, the
Periodic Table can tell what kind of ion they
will form from their location.
• Elements in the same group have similar
properties.
• Including the charge when they are ions.
+1
+2
+3
-3 -2 -1
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Naming ions
• We will use the systematic way.
• Cation- if the charge is always the same
(Group A) just write the name of the metal.
• Transition metals can have more than one
type of charge.
• Indicate the charge with roman numerals in
parenthesis.
Naming Anions
• Anions are always the same.
Change the element ending to – ide.
F-1 Fluorine
F-1 Fluoride
Polyatomic Ions
• Groups of atoms that stay together and have
a charge.
• Atoms in the polyatomic ion are bonded
covalently.
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Ions in Ionic
Compounds
Naming Binary Ionic Compounds
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Binary Compounds - 2 elements.
Ionic - a cation and an anion.
To write the names just name the two ions.
Easy with Representative elements.
Group A
NaCl = Na+ Cl- = sodium chloride
MgBr2 = Mg+2 Br- = magnesium bromide
Naming Binary Ionic Compounds
• The problem comes with the transition
metals.
• Need to figure out their charges.
• The compound must be neutral.
• same number of + and – charges.
• Use the anion to determine the charge on the
positive ion.
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Naming Binary Ionic Compounds
• Write the name of CuO
• Need the charge of Cu
– O is -2
– copper must be +2
– Copper (II) oxide
• Name CoCl3
– Cl is -1 and there are three of them = -3
– Co must be +3 Cobalt (III) chloride
Naming Binary Ionic Compounds
• Write the name of Cu2S.
• Since S is -2, the Cu2 must be +2, so each
one is +1.
• copper (I) sulfide
• Fe2O3
• Each O is -2
3 x -2 = -6
• 3 Fe must = +6, so each is +2.
• iron (III) oxide
Naming Binary Ionic Compounds
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Write the names of the following
KCl
Na3N
CrN
Sc3P2
PbO
PbO2
Na2Se
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Ternary Ionic Compounds
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Will have polyatomic ions
At least three elements
name the ions
NaNO3
CaSO4
CuSO3
(NH4)2O
Ternary Ionic Compounds
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LiCN
Fe(OH)3
(NH4)2CO3
NiPO4
Writing Formulas
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The charges have to add up to zero.
Get charges on pieces.
Cations from name of table.
Anions from table or polyatomic.
Balance the charges by adding subscripts.
Put polyatomics in parenthesis.
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Writing Formulas
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Write the formula for calcium chloride.
Calcium is Ca+2
Chloride is Cl-1
Ca+2 Cl-1 would have a +1 charge.
Need another Cl-1
Ca+2 Cl 2(-1)
Write the formulas for these
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Lithium sulfide
tin (II) oxide
tin (IV) oxide
Magnesium fluoride
Copper (II) sulfate
Iron (III) phosphide
gallium nitrate
Iron (III) sulfide
Write the formulas for these
• Ammonium chloride
• ammonium sulfide
• barium nitrate
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Things to look for
• If cations have (), the number is their charge.
• If anions end in -ide they are probably off the
periodic table (Monoatomic)
• If anion ends in -ate or -ite it is polyatomic
Molecular Compounds
Writing names and Formulas
Molecular compounds
• made of just nonmetals
• smallest piece is a molecule
• can’t be held together because of opposite
charges.
• can’t use charges to figure out how many of
each atom
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Easier
Ionic compounds use charges to determine how
many of each.
– Have to figure out charges.
– Have to figure out numbers.
• Molecular compounds name tells you the
number of atoms.
• Uses prefixes to tell you the number
Prefixes
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1 mono2 di3 tri4 tetra5 penta6 hexa7 hepta8 octa-
Prefixes
• 9 nona• 10 deca• To write the name write two words
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Prefixes
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9 nona10 decaTo write the name write two words
Prefix name Prefix name -ide
Prefixes
• 9 nona• 10 deca• To write the name write two words
• One exception is we don’t write mono- if
there is only one of the first element.
Prefixes
• 9 nona• 10 deca• To write the name write two words
• One exception is we don’t write mono- if there is
only one of the first element.
• No double vowels when writing names (oa oo)
– Not wrong if you do not eliminate a vowel
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Name These
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N2O
NO2
Cl2O7
CBr4
CO2
BaCl2
Write formulas for these
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diphosphorus pentoxide
tetraiodide nonoxide
sulfur hexafluoride
nitrogen trioxide
Carbon tetrahydride
phosphorus trifluoride
aluminum chloride
Acids
Writing names and Formulas
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Acids
• Compounds that give off hydrogen ions when
dissolved in water.
• Indicated by (aq)
– HCl (g) vs HCl (aq)
– Hydrogen chloride vs Hydrochloric acid
• Must have H in them.
• will always be some H next to an anion.
• The anion determines the name.
Naming Binary acids
• If the anion attached to hydrogen is ends in ide, put the prefix hydro- and change -ide to ic acid
• HCl - hydrogen ion and chloride ion
• hydrochloric acid
• H2S hydrogen ion and sulfide ion
• hydrosulfuric acid
Naming OxyAcids
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If the anion has oxygen in it
it ends in -ate of -ite
change the suffix -ate to -ic acid
HNO3 Hydrogen and nitrate ions
Nitric acid
change the suffix -ite to -ous acid
HNO2 Hydrogen and nitrite ions
Nitrous acid
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Name these
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HF
H3P
H2SO4
H2SO3
HCN
H2CrO4
Writing Formulas
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Hydrogen will always be first
name will tell you the anion
make the charges cancel out.
Starts with hydro- no oxygen, -ide
no hydro, -ate comes from -ic, -ite comes
from -ous
Write formulas for these
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hydroiodic acid
acetic acid
carbonic acid
phosphorous acid
hydrobromic acid
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Hydrates
Writing Formulas and
Naming Hydrates
Hydrates
• Compound that contains water molecules
weakly bound in its crystals.
• They are named for the anhydrous
compound followed by the word hydrate with
a prefix to indicate the number of water
molecules per formula unit.
• A dot (•)separates the ionic formula for the
anhydrous compound from the water
molecules
– Example: CuSO4•5H2O
– Copper sulfate pentahydrate
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Name these Hydrates
• MgSO4•7H2O
• Na2CO3•10H2O
• CoCl2•6H2O
Write Formulas for these
Hydrates
• Calcium sulfate dihydrate
• Sodium thiosulfate pentahydrate
• Nickel (II) chloride hexahydrate
Organic Compounds
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Organic Compounds
• Class of molecular substances that contain
carbon combined with other elements
(hydrogen, oxygen, nitrogen)
• Identified by their functional group
– Functional group – the reactive portion of the
organic molecule
• Common organic compounds
– Methane – CH4
– Ammonia – NH3
Organic Functional Groups
Name
Functional Group
Carboxylic Acid
-COOH
Structural
Formula
Molecular
Formula
CH3CH2COOH
Organic Functional Groups
Structural
Formula
Molecular
Formula
Name
Functional Group
Carboxylic Acid
-COOH
CH3CH2COOH
Aldehyde
-CHO
CH3CH2CHO
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Organic Functional Groups
Structural
Formula
Molecular
Formula
Name
Functional Group
Carboxylic Acid
-COOH
CH3CH2COOH
Aldehyde
-CHO
CH3CH2CHO
Alcohol
-COH
CH3CH2OH
Organic Functional Groups
Structural
Formula
Molecular
Formula
Name
Functional Group
Carboxylic Acid
-COOH
CH3CH2COOH
Aldehyde
-CHO
CH3CH2CHO
Alcohol
-COH
CH3CH2OH
Ether
-CH2OC-
CH3CH2OCH3
Organic Functional Groups
Structural
Formula
Molecular
Formula
Name
Functional Group
Carboxylic Acid
-COOH
CH3CH2COOH
Aldehyde
-CHO
CH3CH2CHO
Alcohol
-COH
CH3CH2OH
Ether
-CH2OC-
CH3CH2OCH3
Ketone
-COC-
CH3COCH3
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Incorrect Formulas
For which formula is the name
given correctly?
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H2SO4 – hydrogen sulfide
MgCl2 – manganese chlorine
Al2O3 – aluminum (II) oxide
P2O5 – diphosphorus tetraoxide
CoCO3 – cobalt (II) carbonate
Which name is correct for the
given formula?
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Ca(OH)2 – calcium hydroxate
CH4 – ammonia
BeF2 – beryllium difluoride
CoSO4 – cobalt (II) sulfate
NO2 – nitrogen oxide
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For the given formula, which
name is completely correct?
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K2O – dikrypton monoxide
NiSO4 – nickel sulfate
NO3-1 – nitroxide ion
SO2 – sulfur (II) oxide
Mg3N2 – magnesium nitride
PF3 – phosphorus tetrafluoride
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