Term
| What are the three types of chemical reactions? |
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Definition
Oxidation-reduction (redox)
Precipitation reaction
Acid/Base reaction |
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Term
| Oxidation-reduction (redox) |
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Definition
| Oxidation numbers change in different atoms |
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Term
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Definition
| The combination of two liquids produces a solid (precipitate:ppt) |
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Term
| Acid/base neutralization reaction |
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Definition
| The combination of an acid and a base produces a neutral product and water (H2O) |
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Term
Is this reaction: redox, acid/base, or ppt?
Cu (s) + Ag1+NO3 (aq) --> Cu2+NO3 + 2 Ag(s) |
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Definition
| redox reaction (copper loses 2 e, silver gains 1e) |
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Term
Is this reaction: redox, acid/base, or ppt?
PbNO3 (aq) + KSO4 (aq) --> PbSO4 (s) + 2 KNO3 |
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Definition
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Term
Is this reaction: redox, acid/base, or ppt?
HNO3 (aq) + KOH (aq) --> KNO3 (aq) + H2O (l) |
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Definition
| acid base (1st is acid, 2nd is base, product is neutralized) |
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Term
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Definition
| A substance that separates into ions when dissolved in water. It conducts electricity. |
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Term
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Definition
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Term
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Definition
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Term
All bases are strong electrolytes except for:
******************** |
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Definition
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Term
Is it a: strong electrolyte, weak electrolyte, or non-electrolyte?
HI |
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Definition
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Term
Is it a: strong electrolyte, weak electrolyte, or non-electrolyte?
HF |
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Definition
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Term
Is it a: strong electrolyte, weak electrolyte, or non-electrolyte?
CH2OH |
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Definition
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Term
Is it a: strong electrolyte, weak electrolyte, or non-electrolyte?
HNO3 |
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Definition
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Term
Is it a: strong electrolyte, weak electrolyte, or non-electrolyte?
KBr |
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Definition
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Term
Is it a: strong electrolyte, weak electrolyte, or non-electrolyte?
NaCl |
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Definition
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Term
Is it a: strong electrolyte, weak electrolyte, or non-electrolyte?
HBr |
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Definition
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Term
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Definition
| the substance doesn't break up into ions entirely, most of it remains as the original substance. |
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Term
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Definition
| An equation that shows only the ions that are active in the reaction. |
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Term
| To produce a net-ionic equation: |
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Definition
First separate each separatable substance into its ions. (It is separatable only if: it is an aqeuous solution, and if it is a strong electrolyte) Next cross out ions that are the same on both sides of the reaction (spectator ions). Result is the net-ionic equation
*pay attention to the amount of a substance in the original reaction* |
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Term
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Definition
| the substance dissolves in a solvent, (usally water) |
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Term
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Definition
- the compound contains cations in group 1a (Li, K, Pb, Cs)
- Compounds contain anions in group 7 (halogens) [Br, Cl, I]
- **Except in conjunction w/ Ag, Hg2, and Pb**
- Compounds: NO3, ClO4, CH3CO2, NH4
- **Except in conjunction w/ Pb, Hg2, and Ba |
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Term
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Definition
A precipitate is formed
Compounds that appeal to the exceptions
Anything not in one of the categories of solubles |
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Term
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Definition
| Have weak bonds, and therefore fully dissociate into separate ions. As the elements "go down" on P.table, they become stronger |
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Term
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Definition
| Stronger bonds make it difficult to dissociate into separate ions, therefore there is only minimal separation. Strongly electro-negative and highly active |
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Term
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Definition
| The ability of an atom to gain electrons. This increases towards the right hand side of the periods, and weakens at the bottoms of the groups. |
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Term
| Reactions between acids and bases always produces: |
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Definition
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Term
| Reactions between strong acids and bases produces: |
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Definition
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Term
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Definition
| the loss of electrons to create a more positive charge |
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Term
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Definition
| the gain of electrons to create a more negative charge |
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Term
| 7 Rules for assigning oxidation numbers: |
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Definition
1. An atom in its elemental state always has an Ox # of 0.
2. Halogens have ox #'s of -1
3. Hydrogen has an ox # of +1 when it acts as a cation, and -1 when it acts as an anion
4. Oxygen has an ox # of -2, except for when it is found as a peroxide: then its ox # is -1
5. The sum of the oxidation numbers always equals the overal charge.
6. Molecules have ox #'s of 0.
7. Oxidation states are similar to ions (Ca2+(OH)^-1 2) |
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Term
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Definition
| the portion of the reaction that gets oxidized. (it causes reduction) |
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Term
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Definition
| The portion of the reaction that gets reduced (causes oxidation). |
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Term
| 6 Rules for using the Oxidation # method of balancing in acidic conditions: |
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Definition
1.Write out the unbalanced net-ionic equation
2. Balance the reaction for all atoms except for H and O
3. Assign oxidation numbers to all of the atoms
4. Figure out which ox. #'s change and how much they change
5. Make the total increase in electrons equal the total decrease in electrons by multipling one by the other
6. Add water to the side with less O and add H to the side with less H |
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