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19 Cards in this Set
- Front
- Back
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A single headed arrow |
Indicates the net forward reaction, formation of products is highly favoured. |
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Two half arrows |
Indicate all the chemical species are present in relative quantities. called and equilibrium arrow |
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Molecular equations |
each compound is written as a neutral species |
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Complete ionic equation |
each compound is written as if it were present in solution. as ions or solids. |
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Net ionic equation |
Only the changing chemical species are written |
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Precipitation reactions |
Occur when two soluble ions combine to form an insoluble ionic compound. |
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Strong electrolytes |
Ionic compounds which completely dissociate in solution readily conduct electricity |
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Weak electrocytes |
Ionic compounds which partially dissociates in solution do conduct electricity butnot very well |
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Non electrolytes |
Compounds which do not dissociate into ions, and do not conduct electricity. |
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Rules for determining solubility |
a) Ionic compounds of group 1 compounds (Li+, Na+, K+) and NH4+ are generally soluble b) Nitrates (NO3-), acetates (CH3COO-), chlorates (ClO3-) and perchlorates (ClO4-) aregenerally soluble c) Ionic compounds containing Ag+, Pb2+ and Hg22+ ions are insoluble d) Chlorides, bromides, and iodides are soluble e) Sulfates (SO42-) are soluble except for those combined with Ca2+, Ba2+, Sr2+ ions f) Carbonates (CO32-), phosphates (PO43-), oxides (O2-), Sulfides (S2-) and hydroxides (OH-) are “insoluble” |
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Spectator ions |
Ions that do not participate in the reaction |
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Acid |
A substance which produces protons in aqueous solution. |
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Base |
A substance that produces hydroxide ions in an aqueous solution. |
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Redox reactions |
chemical reactions which involve the transfer of electrons between two or more chemical species. |
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Oxidation |
when an atom loses one or more electrons. |
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Reduction |
When an atom gains one or more electrons |
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Limiting reagent |
The first reactant to get consumed in a reaction. The reactant that would produce the least amount of product. |
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equivalence point |
both reagents combine in exact stoichiometric quantities. |
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End point |
When the indicator changes colour |
