chapter 6.1 introduction to chemical bonding molecule – smallest electrically neutral unit of a...
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Chapter 6.1 Introduction to Chemical Bonding Molecule – smallest
electrically neutral unit of a substance that still has the properties of the substance
Made up of two or more atoms
Molecular Compound Compounds
composed of molecules made up of different atoms
Molecular Compounds Usually low melting
and boiling points Usually liquids or
gases at room temperature
Usually made up of two or more nonmetals
Ions Atoms or groups of
atoms that have a positive or negative charge
Forms when an electron is lost or gained
Cation Any atom or group
of atoms that has a positive charge
Lose electrons Usually Metals
Anion Any atom or group
of atoms that has a negative charge
Gains electrons Usually Nonmetals
Ionic Compounds Compound
composed of anions and cations
Usually a metal cation and a nonmetal anion
Characteristic Molecular Compound
Ionic Compound
Representative Unit
Molecule Formula Unit
Type of Elements
Nonmetals Metal and Nonmetal
Physical State Solid, Liquid or Gas
Solid
Melting Point Low below 300 degrees Celsius
High above 300 degrees Celsius
Chapter 6.2 Representing Chemical Compounds Chemical Formulas Molecular Formulas Formula Units Laws of Proportions
Chemical Formulas Show the kinds and
numbers of atoms in the smallest representative unit of the substance
Monatomic Represent their
chemical formula by writing their symbol
Copper – Cu Helium - He
Diatomic If the molecules of
an element have more than one atom, use a subscript to indicate how many
Hydrogen – H2
Oxygen – O2
The Seven Diatomic Elements You must Memorize Hydrogen – H2
Fluorine – F2
Oxygen – O2
Nitrogen – N2
Chlorine – Cl2 Bromine – Br2
Iodine - I2
Molecular Formulas Shows the kinds
and numbers of atoms present in a molecule of a compound
Does not show anything about the structure
Ammonia
NH3
Formula Units (Ionic Compounds) Does not represent
a molecule No separate
molecular units Arranged in an
orderly pattern
Formula Unit Lowest whole
number ratio of ions in a compound
NaCl 1:1 MgCl2 1:2
The Law of Definite Proportions In samples of any chemical compound, the
masses of the elements are always in the same proportion.
The 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 elements are in small whole number ratios.
Chapter 6.3 Ionic Charges Monatomic Ions Polyatomic Ions
Monatomic Ions Ions consisting of
only one atom
Monatomic Ions – Cations Group 1A ions all
have a 1+ charge Group 2A ions all
have a 2+ charge Group 3A ions all
have a 3+ charge Only for metals
Monatomic Ions – Cations
? the group number from 8 to get number of the charge
Monatomic Ions - Anions Group 7A ions all
have a 1 – charge Group 6A ions all
have a 2 – charge Group 5A ions all
have a 3 – charge Only for nonmetals
Monatomic Ions - Anions Subtract group
number from 8 to get number of the charge
Naming ions with more than one oxidation numbers Stock System Use a roman
numeral after the symbol to indicate charge
Iron – Fe2+ - Iron (II) ion Fe3+ - Iron (III) ion
Polyatomic Ions Tightly bonded
group of atoms that behave as a unit and carry a charge
Sulfate – SO42-
Polyatomic Ions Most end in “ite” or
“ate” Look at table E Three exceptions
Ammonium Cyanide Hydroxide
Polyatomic Ions “ite” indicates one
less of oxygen “ate” indicates one
more of oxygen Does not tell how
many oxygens
Chapter 6.4 Ionic Compounds Writing Formulas Naming Binary
Compounds Ternary Ionic
Compounds
Anions Change ending to
“ide” Oxygen – Oxide Sulfur - Sulfide
Writing Formulas for Binary Ionic Compounds Binary Compound –
composed of two elements
The positive charge of the cation must balance the negative charge of the anion.
Writing Formulas for Binary Ionic Compounds The total net charge
must equal 0. Potassium Chloride
K+ and Cl-
KCl
Rust - Iron(III) Oxide Ions - ? Formula ?
Crisscross method Rust Iron(III) Oxide
Fe3+ and O2-
Naming Binary Ionic Compounds Cation first, anion
second Make sure charges
balance, if not, use subscripts to balance
If the cation has more than one oxidation number, use roman numerals to indicate charge (ONLY Positive)
Ternary Ionic Compounds Contains atoms of
three different elements
Calcium Carbonate CaCO3
Ternary Ionic Compounds “ate” or “ite” ending
indicates a polyatomic anion containing oxygen
Calcium Nitrate Ca2+ , NO3
-
Ca (NO3)2
Chapter 6.5 Molecular Compounds and Acids Binary Molecular
Compounds Naming Common
Acids
Binary Molecular Compounds Composed of two
nonmetallic elements
Prefixes are used to indicate the number of each atom present
Binary Molecular Compounds
Prefixes
Prefix Number
Mono- 1
Di- 2
Tri- 3
Tetra- 4
Penta- 5
Hexa- 6
Hepta- 7
Octa- 8
Nona- 9
Deca- 10
Binary Molecular Compounds All end with “ide” Drop the vowel at
the end of the prefix if the element begins with a vowel CO Carbon Monooxide Carbon Monoxide
Binary Molecular Compounds If the first element
has just one atom, drop the mono- CO Monocarbon
monoxide Carbon monoxide
Binary Molecular Compounds Tetraiodine
nonoxide ??
N20 ??
Naming Common Acids Compounds that
produce hydrogen ions when dissolved in water
Anions connected to as many H+ ions to make the molecule neutral
Naming Common Acids HCl
Hydrochloric Acid H2SO4
Sulfuric Acid HNO3
Nitric Acid HC2H3O2
Acetic Acid H3PO4
Phosphoric Acid H2CO3
Carbonic Acid
Chapter 6.6 Summary of Writing and Naming
PxQy
P = Hydrogen
P = Hydrogen