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chem test
| Question | Answer |
|---|---|
| What is a redox reaction? | A reaction where electrons are transferred between substances. |
| What is oxidation? | Loss of electrons. |
| What is reduction? | Gain of electrons. |
| What does LEO says GER mean | Lose Electrons = Oxidation, Gain Electrons = Reduction. |
| What does OIL RIG mean? | Oxidation Is Losing, Reduction Is Gaining. |
| What is an oxidizing agent | A substance that causes another to be oxidized and is reduced itself. |
| What is a reducing agent? | A substance that causes another to be reduced and is oxidized itself. |
| In Mg + 2H⁺ → H₂ + Mg²⁺, what is oxidized? | Mg (it loses electrons). |
| In Mg + 2H⁺ → H₂ + Mg²⁺, what is reduced? | H⁺ (it gains electrons). |
| What is a half-reaction? | One part of a redox reaction showing either oxidation or reduction. |
| Write the oxidation half-reaction for Mg. | Mg → Mg²⁺ + 2e⁻ |
| Write the reduction half-reaction for H⁺. | 2H⁺ + 2e⁻ → H₂ |
| Why do oxidation and reduction always happen together? | Because electrons lost by one substance must be gained by another. |
| What is an oxidation number? | A number that shows the charge of an atom in a compound. |
| What is the oxidation number of elements by themselves? | 0 |
| What is hydrogen’s oxidation number? | +1 (usually) |
| Exception for hydrogen? | -1 in hydrides (like NaH) |
| What is oxygen’s oxidation number? | -2 (usually) |
| Exceptions for oxygen? | 1 in peroxides, +2 with fluorine |
| What is fluorine’s oxidation number? | Always -1 |
| What is the oxidation number of Group 1 elements? | +1 |
| What is the oxidation number of Group 2 elements? | +2 |
| What is the oxidation number of monatomic ions? | Equal to their charge |
| What must oxidation numbers add up to in a neutral compound? | 0 |
| What must oxidation numbers add up to in a polyatomic ion? | The charge of the ion |
| In covalent compounds, who gets the negative oxidation number? | The more electronegative element |
| What is the redox method used for? | A: Balancing equations that involve electron transfer. |
| Q: What is the first step in the redox method? | A: Assign oxidation numbers. |
| Q: What is the second step? | A: Write oxidation and reduction half-reactions. |
| Q: When balancing half-reactions, what do you balance first? | A: Atoms. |
| Q: What do you balance after atoms? | A: Charge (by adding electrons). |
| Q: Why are electrons added in half-reactions? | A: To balance the charge. |
| Q: What must be equal before combining half-reactions? | A: Electrons lost and electrons gained. |
| Q: How do you make electrons equal? | A: Multiply the half-reactions. |
| Q: What do you do after electrons are equal? | A: Combine the half-reactions. |
| Q: Should electrons appear in the final equation? | A: No. |
| Q: What is oxidation in a half-reaction? | A: Loss of electrons. |
| Q: What is reduction in a half-reaction? | A: Gain of electrons. |
| Q: In Al → Al³⁺, what is happening? | A: Oxidation. |
| Q: In Cu²⁺ → Cu, what is happening? | A: Reduction. |
| Q: Why do we check charge at the end? | A: To make sure both sides are equal. |
| whats a battery an example of | An electrochemical cell. Deep Dive: A battery is a device that turns chemical energy into electricity. "Electrochemical cell" is the broad category that includes both batteries (voltaic/galvanic) and electrolytic cells. |
| when it asks u whats being oxidized and whats the oxidizing agent its | the oxidizing agent is the one being reduced |
| when it asks u whats being reduced and whats the reducing agent its | reduceing agent is the one being oxidezed |
| elements that readily gain electrons tend to have | High ionization energies and high electronegativities. |
| what is the charge of a cathode in an electrochemical cell | positive |
| what is the charge of a anode in an electrochemical cell | negative |
| what is the pupose of a salt bridge in an electrochemical cell | To provide ions that flow between the two half cells and complete the electrical circuit. |
| what is not the same for an electrochemical cell and an electrolytic cell | They produce voltage and an electric current. Deep Dive: This is the big difference! Electrochemical (Voltaic) cells produce electricity. Electrolytic cells consume electricity (like charging a phone or plating jewelry). |
| a redox equation is a | single replacement reaction |
| red cat gets fat | reduction cathode gains mas |
| electrons flow from _____ to ____ | anode to cathode |
| where does the concentration increase | the anode |
| what will increase the voltage and current of a electrochemical cell | Increasing the concentration of the electrode solutions. |
| electroplating is an example of what type of chemical cell | electrolytic |
| how do you find the total electrons of an equation | count them up then multiply them buy tghe coeffiictiets |
| in a chemical reaction what is conserved | both charge and mass |
| negative ions flow where positive ions flow where | anions flow in to anodes cations flow into sthode |
| metals from which groups are obtained by the reduction or their fused salts | group 1 and group 2 |
| how do you act know what the reducing agent or oxidation agent is | its the one that is getting oxidized or reducted on the left |
| their might be some wierd questions like the corrosion or liek things peel of idk but how do u solve it | look at the answers and use table j to see which one is more spontatneous |
| when it asks u where electrons are transfered in a equation where is the answer | 2 electrons on the left |
| How is the type of reaction in an electrochemical cell (voltaic cell) described? | (B) Spontaneous oxidation-reduction reaction. These cells (like batteries) produce electricity naturally through a chemical reaction. |
| when theres a batery in the reaction you dont use table J just the fact that ____ | cathode is positive anode is negative |
| why is a battery usen in a electolytical reaction | used as a power sorce to provide enrgy to a non spontaneous reaction |
| for anode/oxidation what happens to mass | it decreaces but since it oxidation explain it as the equation |
| What is a voltaic (galvanic) cell? | An electrochemical cell that produces electricity from a spontaneous redox reaction. |
| What is an electrolytic cell? | A cell that uses electricity to force a nonspontaneous reaction. |
| In a voltaic cell, what happens at the anode? | Oxidation, mass decreases, concentration increases. |
| In a voltaic cell, what happens at the cathode? | Reduction, mass increases, concentration decreases. |
| What does spontaneous mean? | A reaction that occurs naturally without added energy. |
| What does nonspontaneous mean? | A reaction that requires energy to occur. |
| What type of reaction is always occurring in electrochemical cells? | Redox reactions. |
| What flows through the wire in a cell? | Electrons. |
| What happens to the mass of the cathode in a voltaic cell? | It increases because ions gain electrons and plate onto the electrode |
| What happens to the mass of the anode in a voltaic cell? | It decreases because metal atoms lose electrons and dissolve into solution. |
Created by:
Fernando.Quezada