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26 Cards in this Set
- Front
- Back
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What states do (g), (l), (s), and (aq) stand for? |
(gaseous), (liquid), (solid), and (aqueous). |
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Synthesis Reaction |
A+B→C |
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Decomposition Reaction |
AB→A+B |
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Single Replacement/Desplacement Reaction |
A+BC→AB+C |
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Double Replacement/Displacement Reaction |
AB+CD→AD+BC |
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Combustion Reaction |
CxHy+O2→CO2+H2O |
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Hydrolysis Reaction |
X(aq)+H2O→HX(aq)+OH(aq) |
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Panda... Panda... Panda Panda Panda Panda Panda |
BRARARARARARARARARARARARARARARAUGH... I got broads in Atlanta. |
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Net Ionic Equations |
Only show the Ions changed in the reaction; emits spectator ions. |
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Solubility rule of alkali metal compounds and NH4? |
They are usually soluble. |
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Solubility rules for Cl, I, and Br compounds? |
They are soluble except when they contain Ag, Hg or Pb2. |
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Solubility rules for F compounds? |
Soluble unless they contain alkali earth metals. |
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Solubility rules for NO3, ClO3, ClO4, and CH3COO compounds? |
Soluble. |
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Solubility rules for SO4 compounds? |
Soluble except when they include Ca2, Sr2, Ba2, Ag, and Pb2. |
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Solubility rules for OH salts? |
Insoluble for all compounds except with the alkali metals. |
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Which compounds are usually insoluble? |
CO3, PO4, C2O4, CrO4, S2, and O2. |
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Alkali earth metal compounds save what odd solubility property? |
They are mostly insoluble, yet still classified as strong bases. |
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To form a net ionic equation, which compounds will you keep? |
The compounds that form the percipitate. |
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Six strong acids? |
HCL, H2SO4, HNO3, HI, HBr, and HClO4. |
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Arrhenius acid and base definition: |
Increase H+ or OH- concentrations. |
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Bronsted Lawry acid and base definition: |
Proton donors and acceptors. |
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Lewis acid and base definition: |
Acids accept electron pairs, bases donate electron pairs. |
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Define monoprotic, diprotic and polyprotic. |
Can donate one, two, or any number greater than 2 H+. |
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Amphiprotic definition: |
Can be either acid or base. |
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Amphiprotic compound examples: |
HCO3, HSO4, HPO4. |
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Conjugate acids and bases: |
XH + H2O → H3O+ + X- |
