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| opposite charges attract hold atoms together |
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| Hydrogen sulfate or Bisulfate |
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| independent of the amount |
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| different number of electrons |
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| different number of neutrons |
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| Metals with More Than One Oxidation State |
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| If you are naming a metal cation that has more than one oxidation state, use a Roman numeral in the name. |
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| Nomenclature of Binary Ionic Compounds |
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Cation name = name of element.
Anion name = element name with the ending replaced by the suffix "ide".
Compound name = cation name + anion name
Compound Charge = 0 |
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| Nomenclature of Ionic Compounds with Oxo Anions |
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| Ionic compounds are named by stating the cation name and then the anion name. Oxo anions always have the suffix 'ate' or 'ite'. |
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| Find average, find difference from each number from the average, average those, and take the square roots |
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10(12)
(1,000,000,000,000) |
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Mass divided by volume
M/V |
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| Chlorate (ClO3- ), and perchlorate (ClO4-) salts |
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| SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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| SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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| SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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| SOLUBLE - - EXCEPT those also containing: hydrogen, calcium, silver, mercury (I), strontium, barium, or lead (Ca2+, Ag+, Hg22+, Sr2+, Ba2+, Pb2+) which are NOT soluble. |
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| Hydroxide (OH-) compounds |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, ammonium, or barium (Na+, K+, NH4+, Ba2+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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| Writing Net Ionic Equations |
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1. Write reactants.
2. Write products by exchanging cations.
3. Dissociate (write as ions) ALL soluble salts, strong acids, and strong bases (except Ca(OH)2)
Reminder: Do not break up polyatomic ions i.e.) K_2_SO_4_ --> 2 K^+ + SO4^2- NOT S2- + 4 O2-
4. Balance.
5. Cross out identical (spectator) ions on both sides of the equation.
6. Rewrite NET IONIC EQUATION. CHECK atom and charge balance. |
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There are two ways to name these compounds:
1. Molecular Name : Hydrogen + anion name
2. Acid Name : Hydro ____ ic acid. Used for aqueous solutions of the compound. |
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| hydrocyanic acid or hydrogen cyanide |
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ate anions form ic acids. HNO3 = nitric acid
ite anions form ous acids. HNO2 = nitrous acid |
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| HCl, HBr, HI, HNO3, HClO4, H2SO4 |
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| Strong Acids and Strong Bases in aqueous solution |
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| Assigning Oxidation Numbers Atoms in their elemental state |
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| LiOH, NaOH, KOH, Ca(OH)2 slightly soluble, Ba(OH)2, Sr(OH)2 |
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| "Filling up" or Aufbau Principle |
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| Electrons go into the lowest energy orbitals first. |
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| A maximum of 2 electrons can occupy an orbital. When 2 electrons occupy the same orbital, they must have paired spins, (or "ud" using our notation). |
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| When filling p or d orbitals with the same energy, electrons go into separate orbitals with parallel spins until all of the orbitals are occupied by one electron. Then they are paired. |
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| Drawing Lewis Structures 1 |
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Write the skeletal structure (the arrangement of atoms within the molecule):
Central atom = the atom with the lowest electronegativity (usually).
Hydrogen is always a terminal atom (on the end). |
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| Drawing Lewis Structures 2 |
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Count the total number of valence electrons:
Group number for each element = # valence electrons.
Add electrons for negatively charged ions.
Subtract electrons for positively charged ions. |
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| Drawing Lewis Structures 3 |
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Draw a bond between the central atom and each surrounding atom.
Single bond = 1 pair of electrons |
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| Drawing Lewis Structures 4 |
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Place lone pairs of electrons about each terminal atom to complete their octets.
Octet = 4 electrons pairs around an atom (eight electrons)
Hydrogen can only have 2 electrons. |
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| Drawing Lewis Structures 5 |
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If there are more electrons left, place them as lone pairs on the central atom.
This will sometimes lead to an "expanded octet" around the central atom.
Expanded octet = five or six electron pairs around an atom.
Only central atoms from the third period and above can have expanded octets. |
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| Drawing Lewis Structures 6 |
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If the central atom has an incomplete octet, use the electrons from surrounding atoms to make double or triple bonds.
Do not add electrons. "Borrow" them from surrounding atoms.
Double bond = 2 pairs of electrons
Triple bond = 3 pairs of electrons
Only C, N, O, P, and S form multiple bonds.
F and Cl do not form multiple bonds. |
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| Drawing Lewis Structures 7 |
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Sometimes you just can't complete the octet for a central atom.
If there is an odd number of electrons, give the central atom 7 electrons instead of 8.
Boron and Beryllium just don't have enough electrons to go around and often have incomplete octets. |
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| characterized by having ring systems in which the bonding can be described as alternating single and double bonds. |
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| subdivided into alkanes, alkenes and alkynes. |
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| compounds that contain only the elements H and C. They can be divided into two classes: aliphatic and aromatic. |
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| each C atom is bonded to four other atoms and all bonds are single bonds. |
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| contains a carbon-carbon double bond. |
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| carbon-carbon triple bond. |
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| Chlorate (ClO3- ), and perchlorate (ClO4-) salts |
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| SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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| SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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| SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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| SOLUBLE - - EXCEPT those also containing: hydrogen, calcium, silver, mercury (I), strontium, barium, or lead (Ca2+, Ag+, Hg22+, Sr2+, Ba2+, Pb2+) which are NOT soluble. |
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| Hydroxide (OH-) compounds |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, ammonium, or barium (Na+, K+, NH4+, Ba2+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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| NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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| Writing Net Ionic Equations |
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Definition
1. Write reactants.
2. Write products by exchanging cations.
3. Dissociate (write as ions) ALL soluble salts, strong acids, and strong bases (except Ca(OH)2)
Reminder: Do not break up polyatomic ions i.e.) K_2_SO_4_ --> 2 K^+ + SO4^2- NOT S2- + 4 O2-
4. Balance.
5. Cross out identical (spectator) ions on both sides of the equation.
6. Rewrite NET IONIC EQUATION. CHECK atom and charge balance. |
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There are two ways to name these compounds:
1. Molecular Name : Hydrogen + anion name
2. Acid Name : Hydro ____ ic acid. Used for aqueous solutions of the compound. |
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| hydrocyanic acid or hydrogen cyanide |
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ate anions form ic acids. HNO3 = nitric acid
ite anions form ous acids. HNO2 = nitrous acid |
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| HCl, HBr, HI, HNO3, HClO4, H2SO4 |
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| Strong Acids and Strong Bases in aqueous solution |
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| Assigning Oxidation Numbers Atoms in their elemental state |
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| LiOH, NaOH, KOH, Ca(OH)2 slightly soluble, Ba(OH)2, Sr(OH)2 |
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| Gases (ie methane) in order |
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| methane, ethane, propane, butane, pentane hexane, heptane, octane, nonane, decane |
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| 1 extra set 90, 120, 180 SF4 |
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| 2 extra set 90, 180 ClF3 |
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| extra pair 90, 180 ClF5 |
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| 2 extra pairs 90, 180 XeF4 |
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