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Gen Chem part 3 ch 4
| Question | Answer |
|---|---|
| molecular equation | 1. Equations that describe the chemicals put into the water and the product molecules are called molecular equations. 2 KOH(aq) + Mg(NO3)2(aq) ® 2 KNO3(aq) + Mg(OH)2(s) |
| complete ionic equation | 1. Equations that describe the material’s structure when dissolved are called complete ionic equations. 2K+(aq) + 2OH−(aq) + Mg2+(aq) + 2NO3−(aq) ® 2K+(aq) + 2NO3−(aq) + Mg(OH)2(s |
| spectator ions | Ions that are both reactants and products are called spectator ions |
| net ionic equations: | An ionic equation in which the spectator ions are removed is called a net ionic equation |
| summarizing Aqueous equations:molecular equation- | is a chemical equation showing the complete, neutral formulas for every compound in a reaction. |
| summarizing Aqueous equations: complete ionic equation- | is a chemical equation showing all of the species as they are actually present in solution. |
| summarizing Aqueous equations:net ionic equation- | is an equation showing only the species that actually change during the reaction. |
| acid-base reaction or another name is a neutralizing reaction | it reacts with a base and the two neutralize each other, PRODUCING WATER! |
| gas-evolution reaction | A gase forms, resulting in bubbling. The reactions occur when the anion from one reactant combines with the cation of the other. |
| Arrhenius definitions: 1.acids form: 2. Bases: | 1.produces H+ ions in a solution 2. substance that produces OH- ions in awueneous solution. |
| know table 4.2 on page 156! | |
| what do you get when you mix an acid and a base? It's called an acid-base reaction | 1. You get water! 2. Acid+Base-->water+salt |
| titration: | 1.a substance in a solution of known concentration is reacted with another substance in a solution of UNKOWN concentration. |
| what is the end point: | In the titration, the unknown solution is added to a known amount of another reactant until the reaction is just completed. At this point, called the endpoint, the reactants are in their stoichiometric ratio. |
| equivalance point: | 1. At the endpoint of an acid-base titration, the number of moles of H+ equals the number of moles of OH a) also known as the equivalence point |
| indicator: | 1. the equivalence point is typically signaled by an indicator. 2. A dye whose color depend on the acidity or basicity of the solution. |
| titrant: | The titrant is the base solution in the burette. |
| gas-evolution reaction | 1. 2 aqueneous solutions mix to form a gaseous product that bubbles out of solution. 2.Other reactions form a gas by the decomposition of one of the ion exchange products into a gas and water |
| oxidation-reduction reactions or redox reactions: | Other kinds of reactions involve transferring electrons from one atom to another – these are called oxidation-reduction reactions 2. the reusting of iron, leaching of hair, and production of electiricity in batteries invove redox reactions. |
| oxidation and reduction | 1. oxidation: is the loss of electrons 2. reduction: is the gain of electrons. |
| oxidation states or oxidation number: | Chemists assign a number to each element in a reaction called an oxidation state that allows them to determine the electron flow in the reaction even though they look like them, oxidation states are not ion charges! |
| oxidation states (continued) | a)oxidation states are imaginary charges assigned based on a set of rules b)ion charges are real, measurable charges |
| Know rules for assigning oxidation states on page 164! | |
| rules for assigning oxidation states:(rule 1 and 2) | 1. free elements have an oxidation state = 0 Na = 0 and Cl2 = 0 in 2 Na(s) + Cl2(g) 2. monatomic ions have an oxidation state equal to their charge Na = +1 and Cl = −1 in NaCl |
| rules for assigning oxidation states (rules 3a) | 3.(a) the sum of the oxidation states of all the atoms in a compound is 0 Na = +1 and Cl = −1 in NaCl, (+1) + (−1) = 0 |
| rules for assigning oxidation states (rules 3b) | 3.(b)the sum of the oxidation states of all the atoms in a polyatomic ion equals the charge on the ion N = +5 and O = −2 in NO3–, (+5) + 3(−2) = −1 |
| rules for assigning oxidation states rules(4a & 4b) | 4. (a) Group I metals have an oxidation state of +1 in all their compounds Na = +1 in NaCl 4.(b) Group II metals have an oxidation state of +2 in all their compounds Mg = +2 in MgCl2 |
| rules for assigning oxidation states rules (rule 5) | in their compounds, nonmetals have oxidation states according to the table below nonmetals higher on the table take priority |
| oxidation and reduction must occur together. | 1. Oxidation and reduction must occur simultaneously a) if an atom loses electrons another atom must take them |
| oxidizing agent: is always reduced | 1. The reactant that oxidizes an element in another reactant is called the oxidizing agent a) the oxidizing agent contains the element that is reduced |
| reducing agent: is always oxidized | 1. The reactant that reduces an element in another reactant is called the reducing agent a) the reducing agent contains the element that is oxidized |
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