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30 terms

Root test 1

Aqueous solutions. . .
STUDY
PLAY
Soluble or Insoluble?
Li⁺, Na⁺, K⁺
Exceptions
Soluble
No Exceptions
Soluble or Insoluble?
NO₃⁻
HCO₃⁻
ClO₃⁻
Exceptions?
Soluble
No Exceptions
Soluble or Insoluble?
Halides Cl⁻ Br⁻ I⁻

Exceptions?
Soluble . . . EXCEPT:
Ag⁺
Hg₂⁺²
Pb⁺²
Soluble or Insoluble?
Rb⁺
Cs⁺
NH4⁺

Exceptions?
Soluble

NO EXCEPTIONS
Soluble or Insoluble?
SO₄

Exceptions?
Soluble. . .EXCEPT
Ag⁺
Hg₂⁺²
Pb⁺²
Ca⁺²
Ba⁺²
Sr⁺²
Soluble or Insoluble?
CO₃⁻²

Exceptions?
INSOLUBLE
but SOLUBLE when with:
Alkali and NH₄
Soluble or Insoluble?
PO₄⁻³

Exceptions?
INSOLUBLE
but SOLUBLE when with:
Alkali and NH₄
Soluble or Insoluble?
CrO₄⁻²

Exceptions?
INSOLUBLE
but SOLUBLE when with:
Alkali and NH₄
Soluble or Insoluble?
S⁻²

Exceptions?
INSOLUBLE
but SOLUBLE when with:
Alkali and NH₄
Soluble or Insoluble?

OH⁻

Exceptions?
INSOLUBLE
but soluble when with:
Alkali and Ba⁺²
How many atoms in a:
Simple Cubic Cell
Body Centered Cubic Cell
Face Centered Cubic Cell
1 Atom
2 Atom
4 Atom
What are the four attractive force types in order of strong to weak?
Ionic
Hydrogen bond->Polar Molec.
Dipole-------->Polar Molec.
Dispersion
When dealing with intermolecular forces, the IONIC attractive force type has what characteristics?
High MP/BP
HIGH IMAF strength.
When dealing with intermolecular forces, the HYDROGEN BOND attractive force type has what characteristics?
ONLY POLAR Molecules
HIGH EN with FON elements
Moderate IMAF strength
Moderate BP/MP
When dealing with intermolecular forces, the DiPOLE-DiPOLE attractive force type has what characteristics?
ONLY POLAR molecules
Moderately Weak IMAF
Low MP/BP
When dealing with intermolecular forces, the London Dispersion attractive force type has what characteristics?
NONPOLAR substances
WEAK IMAF strength
LOW MP/BP
Define: Strong Electrolyte
A substance that dissolves in water to form a good conductor of electricity.
What are the characteristics of a Brønsted Acid?
An acid that Ionizes COMPLETELY in an aqueous solution.
React with some metals to produce Hydrogen Gas.
Also label as: Weak Acid or Strong Acid.
What do Monoprotic, Diprotic, and Triprotic refer to?
Brønsted Acids with one, two, or three Hydrogens.
A reaction with these characteristics is classified as what type of reaction:
-Gaining or losing of Oxygen Atoms (NOT IN H)
-On one side in elemental form, on the other as an ion or in a compound.
Redox Reaction

-Combination Reaction sl-s
-Decompostion Reaction ss-g
-Combustion Reaction sg-g
-Displacement reaction (halogen, Hydrogen, metal)
Do you recognize this reaction type?
The formation of a solid as a product from two aqueous solutions.
Precipitation Reaction
Do you recognize this reaction type?
Look for the formation of a salt (soluble or insoluble) AND H₂O.
Acid-Base Reaction
Do you recognize this reaction type?
Look for a metal carbonate, MetalCO₃, (or bicarbonate) and a strong acid as reactants and water and CO₂ gas as products
Gas Producting
When balancing the half reactions of a Redox Reaction equation, complete the following letter in the COHEB acronym :
C
Balance the compounds for all elements except O and H.
When balancing the half reactions of a Redox Reaction equation, complete the following letter in the COHEB acronym :
O
Balance O by adding OH(L)
When balancing the half reactions of a Redox Reaction equation, complete the following letter in the COHEB acronym:
H
Balance H⁺ by adding H⁺(aq)
When balancing the half reactions of a Redox Reaction equation, complete the following letter in the COHEB acronym:
E
Balance each half-reaction for charge by adding Electrons (e⁻)
When balancing the half reactions of a Redox Reaction equation, complete the following letter in the COHEB acronym :
B
Balance the total electrons e⁻ for both half reactions. Multiply each half reaction by the appropriate factor.

Finally: Check and BALANCE for MASS and CHARGE.
When balancing the half reactions of a Redox Reaction equation, complete the following letter in the COHEB - OH approach:
OH
Add OH on both sides of the equation to neutralize the H⁺(aq)
Research Relative Strength of IMF's
Ion-Ion (Ionic bond)
Covalent Bond
ion Dipole
Hydrogen Bond
Dipole-Dipole
Ion-Induced Dipole
Dipole Induced Dipole
Dispersion