Redox Reactions and Engineering Materials Quiz

<p>It loses electrons and is oxidized (C)</p> Signup and view all the answers

<p>Hypothetical charges for tracking electrons (D)</p> Signup and view all the answers

<p>Combustion of methane (D)</p> Signup and view all the answers

<p>It gains electrons and is reduced (B)</p> Signup and view all the answers

<p>Typically +1 (B)</p> Signup and view all the answers

<p>To withstand applied loading without breaking or deforming excessively (A)</p> Signup and view all the answers

<p>Nickel-Cadmium Battery (C)</p> Signup and view all the answers

<p>Cathodic Protection (A)</p> Signup and view all the answers

<p>2H₂O (A)</p> Signup and view all the answers

<p>Acidic environments (A)</p> Signup and view all the answers

<p>Aerospace parts (B)</p> Signup and view all the answers

<p>They are costly despite being efficient (D)</p> Signup and view all the answers

<p>Titanium (B)</p> Signup and view all the answers

<p>They require external energy to proceed. (A)</p> Signup and view all the answers

<p>ΔG &gt; 0 (B)</p> Signup and view all the answers

<p>It enhances the reaction rate by lowering activation energy. (D)</p> Signup and view all the answers

<p>By increasing the temperature and pressure appropriately. (C)</p> Signup and view all the answers

<p>Increasing the activation energy required. (B)</p> Signup and view all the answers

<p>The reduction at the cathode is unfavorable. (C)</p> Signup and view all the answers

<p>Increasing product concentrations. (A)</p> Signup and view all the answers

<p>Non-ferrous metals (A)</p> Signup and view all the answers

<p>Radioactive isotopes like carbon-14 (A)</p> Signup and view all the answers

<p>Achieving and maintaining extreme temperatures and pressures (A)</p> Signup and view all the answers

<p>Uncontrollable nuclear chain reactions (C)</p> Signup and view all the answers

<p>Clean, nearly limitless energy (B)</p> Signup and view all the answers

<p>Proper waste disposal and recycling (A)</p> Signup and view all the answers

<p>Positive ions gain electrons (B)</p> Signup and view all the answers

<p>Copper (Cu) (B)</p> Signup and view all the answers

<p>Zinc (Zn) (A)</p> Signup and view all the answers

<p>To coat a surface with metal (B)</p> Signup and view all the answers

<p>Chemical change induced by electrical energy (A)</p> Signup and view all the answers

<p>Copper (Cu) (C)</p> Signup and view all the answers

<p>To allow ions to migrate between the half-cells (A)</p> Signup and view all the answers

<p>Nuclear Fission (B)</p> Signup and view all the answers

<p>They are non-rechargeable batteries (B)</p> Signup and view all the answers

<p>Alpha Decay (D)</p> Signup and view all the answers

<p>E=mc² (D)</p> Signup and view all the answers

<p>Nuclear Fusion (A)</p> Signup and view all the answers

<p>They often require careful disposal due to radioactivity (B)</p> Signup and view all the answers

<p>Technetium-99m (A)</p> Signup and view all the answers

<p>It provides a consistent and low-carbon energy source (D)</p> Signup and view all the answers

<p>Beta Decay (B)</p> Signup and view all the answers

A chemical process involving the transfer of electrons between reactants, resulting in changes in oxidation states.

The process of losing electrons, leading to an increase in oxidation state.

The process of gaining electrons, leading to a decrease in oxidation state.

A species that accepts electrons in a redox reaction, causing its own reduction.

A species that donates electrons in a redox reaction, causing its own oxidation.

A hypothetical charge assigned to an atom in a molecule or ion to track electron movement in redox reactions.

A chemical reaction where oxidation and reduction occur simultaneously, with equal electron transfer.

Redox reactions are crucial for various processes like energy production (cellular respiration, photosynthesis), corrosion (rusting), environmental processes (water purification, soil formation), and industrial applications (electroplating, batteries).

The process where electrical energy drives a chemical change, like decomposing substances or plating metals.

A container with an electrolyte, cathode (negative) and anode (positive) electrodes, used for electrolysis.

In electrolysis, positive ions gain electrons at the cathode, becoming neutral atoms.

In electrolysis, negative ions lose electrons at the anode, becoming neutral atoms.

Devices that produce electrical energy from spontaneous redox reactions.

A measure of a substance's tendency to gain electrons (be reduced) in a half-reaction.

Metals with high SRP are strong oxidizing agents, readily accepting electrons.

Metals with low SRP are strong reducing agents, easily losing electrons.

A chemical reaction where oxidation and reduction occur simultaneously, with equal electron transfer.

A method for dating fossils and artifacts by analyzing the decay of radioactive carbon-14.

The use of controlled nuclear reactions to produce electricity.

The process involving uncontrolled nuclear reactions (fission or fusion) with immense destructive power.

A potential energy source that utilizes the fusion of atomic nuclei, producing clean energy with minimal radioactive waste.

The potential environmental impact of radioactive materials from nuclear processes, requiring careful management and proper disposal methods.

The spontaneous emission of particles or radiation by unstable nuclei to become stable.

The process by which a neutron transforms into a proton (or vice versa) with the emission of an electron or positron.

The release of high-energy photons from an unstable nucleus as it transitions to a lower energy state.

Nuclear reactions release significantly more energy than chemical reactions due to the strong nuclear force.

A small amount of mass is converted into a large amount of energy in nuclear reactions, as described by Einstein's equation E=mc².

Byproducts of nuclear reactions are often radioactive and require careful management and disposal to minimize environmental and health risks.

A chemical reaction that requires an external energy input to occur. This energy can overcome thermodynamic or kinetic barriers that prevent it from happening spontaneously.

The free energy change of a reaction indicates whether it will occur spontaneously. A positive value means the reaction is non-spontaneous and requires energy to proceed.

A reaction's cell potential is a measure of its tendency to occur. A negative standard cell potential (E°cell < 0) indicates that the reduction at the cathode is unfavorable, making the overall reaction non-spontaneous.

The initial energy required to start a reaction. A high activation energy makes a reaction slow or non-spontaneous, as it requires a substantial push to begin.

A catalyst speeds up a reaction by providing an alternate pathway with lower activation energy. If a catalyst is absent or inhibited, the reaction may be much slower or non-spontaneous.

The concentration of reactants plays a crucial role. Low concentrations can prevent the reaction from happening efficiently.

High product concentrations can drive the reaction backward due to the equilibrium shift.

Changes in pressure can influence the feasibility of a reaction, especially for reactions involving gases. Non-optimal pressure can make the reaction non-spontaneous.