Podcast Beta
Questions and Answers
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Rate: The speed at which a chemical reaction takes place, usually expressed as the change in concentration of reactants or products per unit time.
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Reaction rate: The rate at which reactants are consumed or products are formed in a chemical reaction.
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Collision theory: A theory that explains how chemical reactions occur and proposes that chemical reactions happen when reacting particles collide with sufficient energy and proper orientation.
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Activation energy: The minimum amount of energy required for a chemical reaction to occur.
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Activated complex: Also known as transition state, it is a high-energy, unstable state formed during a chemical reaction in which old bonds are breaking and new bonds are forming.
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Reaction intermediate: A species formed during the course of a chemical reaction that is neither a reactant nor a product of the overall reaction.
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Catalyst: A substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with lower activation energy, without being consumed in the reaction.
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Reversible reactions: Chemical reactions that can proceed in both the forward and reverse directions.
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Chemical equilibrium: A state in which the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products over time.
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Equilibrium position: The relative concentrations of reactants and products at equilibrium.
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Le Chatelier’s principle: A principle stating that if a system at equilibrium is subjected to a stress (change in concentration, pressure, or temperature), the system will adjust to relieve the stress and restore a new equilibrium.
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Oxidation: The loss of electrons or an increase in oxidation state of an atom, ion, or molecule.
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Reduction: The gain of electrons or a decrease in oxidation state of an atom, ion, or molecule.
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Redox reaction: A chemical reaction in which one substance is oxidized (loses electrons) and another substance is reduced (gains electrons).
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Reducing agent: A substance that donates electrons and undergoes oxidation in a redox reaction, causing another substance to be reduced.
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Oxidizing agent: A substance that accepts electrons and undergoes reduction in a redox reaction, causing another substance to be oxidized.
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Oxidation number: A number assigned to an atom in a chemical compound that indicates the number of electrons lost or gained by the atom.
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Half reaction: Either the oxidation or reduction part of a redox reaction, showing the transfer of electrons.
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Oxidation-number-change method: A method for balancing redox reactions by tracking changes in oxidation numbers.
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Half-reaction method: A method for balancing redox reactions by writing separate equations for the oxidation and reduction half-reactions.
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Electric potential: The amount of work done per unit charge in moving a positive test charge from a reference point to a specific point in an electric field.
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Electrochemical process: A chemical reaction that involves the transfer of electrons between species.
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Electrochemical cell: A device that converts chemical energy into electrical energy, consisting of two electrodes immersed in an electrolyte solution.
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Voltaic cell: An electrochemical cell that generates electrical energy from spontaneous chemical reactions.
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Half-cell: One of the two compartments of an electrochemical cell containing either the oxidizing or reducing species.
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Electrode: A conductor through which electric current enters or leaves an electrolyte or other non-metallic medium.
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Anode: The electrode where oxidation occurs in an electrochemical cell, attracting negatively charged ions.
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Cathode: The electrode where reduction occurs in an electrochemical cell, attracting positively charged ions.
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Reduction potential: The tendency of a species to gain electrons and be reduced, measured relative to a standard hydrogen electrode.
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Oxidation potential: The tendency of a species to lose electrons and be oxidized, measured relative to a standard hydrogen electrode.
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Standard reduction potential: The reduction potential of a half-reaction under standard conditions (1 M concentration, 1 atm pressure, and 25°C temperature).
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Standard cell potential: The potential difference between the two half-cells of an electrochemical cell under standard conditions.
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Electrolyte cell: An electrochemical cell in which an electric current is generated or consumed through an electrolytic process.
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Electrolysis: The process of using electrical energy to drive a non-spontaneous chemical reaction.
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Electroplating: The process of coating an object with a thin layer of metal using electrolysis.
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Fuel cell: An electrochemical cell that converts the chemical energy of a fuel directly into electrical energy.
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Organic compound: A compound containing carbon atoms.
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Hydrocarbon: A compound consisting of hydrogen and carbon atoms only.
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Structural formula: A representation of the molecular structure of a compound, showing the arrangement of atoms and bonds.
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Alkane: A saturated hydrocarbon with single bonds between carbon atoms.
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Straight-chain alkane: An alkane in which the carbon atoms are arranged in a continuous chain with no branching.
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Branched-chain alkane: An alkane in which carbon atoms are arranged in a chain with one or more side chains branching off.
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Substituent: An atom or group of atoms that can replace a hydrogen atom in an organic compound.
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Condensed structural formula: A simplified version of a structural formula in which certain groups of atoms are represented by specific symbols.
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Alkene: A hydrocarbon containing at least one carbon-carbon double bond.
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Alkyne: A hydrocarbon containing at least one carbon-carbon triple bond.
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Saturated compound: A compound containing only single bonds between carbon atoms. (only alkane)
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Unsaturated compounds: Compounds containing multiple bonds (double or triple bonds) between carbon atoms.
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Degree of saturation: The extent to which a compound contains multiple bonds relative to the maximum possible number of bonds.
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Isomers: Compounds with the same molecular formula but different structural arrangements or spatial orientations of atoms.
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Structural isomers: Isomers with different arrangements of atoms in their molecular structure.
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Stereoisomers: Isomers with the same molecular formula and the same connectivity of atoms but different spatial arrangements of atoms.
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Geometric isomers: Stereoisomers that differ in the spatial arrangement of atoms around a double bond or a ring.
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Optical isomers: Stereoisomers that are non-superimposable mirror images of each other.
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Cyclic hydrocarbons: Hydrocarbons in which the carbon atoms form a ring structure.
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Aromatic compound: A type of cyclic hydrocarbon with alternating double and single bonds, often possessing a distinctive odor.
Rate: The speed at which a chemical reaction takes place, usually expressed as the change in concentration of reactants or products per unit time.
Reaction rate: The rate at which reactants are consumed or products are formed in a chemical reaction.
Collision theory: A theory that explains how chemical reactions occur and proposes that chemical reactions happen when reacting particles collide with sufficient energy and proper orientation.
Activation energy: The minimum amount of energy required for a chemical reaction to occur.
Activated complex: Also known as transition state, it is a high-energy, unstable state formed during a chemical reaction in which old bonds are breaking and new bonds are forming.
Reaction intermediate: A species formed during the course of a chemical reaction that is neither a reactant nor a product of the overall reaction.
Catalyst: A substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with lower activation energy, without being consumed in the reaction.
Reversible reactions: Chemical reactions that can proceed in both the forward and reverse directions.
Chemical equilibrium: A state in which the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products over time.
Equilibrium position: The relative concentrations of reactants and products at equilibrium.
Le Chatelier’s principle: A principle stating that if a system at equilibrium is subjected to a stress (change in concentration, pressure, or temperature), the system will adjust to relieve the stress and restore a new equilibrium.
Oxidation: The loss of electrons or an increase in oxidation state of an atom, ion, or molecule.
Reduction: The gain of electrons or a decrease in oxidation state of an atom, ion, or molecule.
Redox reaction: A chemical reaction in which one substance is oxidized (loses electrons) and another substance is reduced (gains electrons).
Reducing agent: A substance that donates electrons and undergoes oxidation in a redox reaction, causing another substance to be reduced.
Oxidizing agent: A substance that accepts electrons and undergoes reduction in a redox reaction, causing another substance to be oxidized.
Oxidation number: A number assigned to an atom in a chemical compound that indicates the number of electrons lost or gained by the atom.
Half reaction: Either the oxidation or reduction part of a redox reaction, showing the transfer of electrons.
Oxidation-number-change method: A method for balancing redox reactions by tracking changes in oxidation numbers.
Half-reaction method: A method for balancing redox reactions by writing separate equations for the oxidation and reduction half-reactions.
Electric potential: The amount of work done per unit charge in moving a positive test charge from a reference point to a specific point in an electric field.
Electrochemical process: A chemical reaction that involves the transfer of electrons between species.
Electrochemical cell: A device that converts chemical energy into electrical energy, consisting of two electrodes immersed in an electrolyte solution.
Voltaic cell: An electrochemical cell that generates electrical energy from spontaneous chemical reactions.
Half-cell: One of the two compartments of an electrochemical cell containing either the oxidizing or reducing species.
Electrode: A conductor through which electric current enters or leaves an electrolyte or other non-metallic medium.
Anode: The electrode where oxidation occurs in an electrochemical cell, attracting negatively charged ions.
Cathode: The electrode where reduction occurs in an electrochemical cell, attracting positively charged ions.
Reduction potential: The tendency of a species to gain electrons and be reduced, measured relative to a standard hydrogen electrode.
Oxidation potential: The tendency of a species to lose electrons and be oxidized, measured relative to a standard hydrogen electrode.
Standard reduction potential: The reduction potential of a half-reaction under standard conditions (1 M concentration, 1 atm pressure, and 25°C temperature).
Standard cell potential: The potential difference between the two half-cells of an electrochemical cell under standard conditions.
Electrolyte cell: An electrochemical cell in which an electric current is generated or consumed through an electrolytic process.
Electrolysis: The process of using electrical energy to drive a non-spontaneous chemical reaction.
Electroplating: The process of coating an object with a thin layer of metal using electrolysis.
Fuel cell: An electrochemical cell that converts the chemical energy of a fuel directly into electrical energy.
Organic compound: A compound containing carbon atoms.
Hydrocarbon: A compound consisting of hydrogen and carbon atoms only.
Structural formula: A representation of the molecular structure of a compound, showing the arrangement of atoms and bonds.
Alkane: A saturated hydrocarbon with single bonds between carbon atoms.
Straight-chain alkane: An alkane in which the carbon atoms are arranged in a continuous chain with no branching.
Branched-chain alkane: An alkane in which carbon atoms are arranged in a chain with one or more side chains branching off.
Substituent: An atom or group of atoms that can replace a hydrogen atom in an organic compound.
Condensed structural formula: A simplified version of a structural formula in which certain groups of atoms are represented by specific symbols.
Alkene: A hydrocarbon containing at least one carbon-carbon double bond.
Alkyne: A hydrocarbon containing at least one carbon-carbon triple bond.
Saturated compound: A compound containing only single bonds between carbon atoms. (only alkane)
Unsaturated compounds: Compounds containing multiple bonds (double or triple bonds) between carbon atoms.
Degree of saturation: The extent to which a compound contains multiple bonds relative to the maximum possible number of bonds.
Isomers: Compounds with the same molecular formula but different structural arrangements or spatial orientations of atoms.
Structural isomers: Isomers with different arrangements of atoms in their molecular structure.
Stereoisomers: Isomers with the same molecular formula and the same connectivity of atoms but different spatial arrangements of atoms.
Geometric isomers: Stereoisomers that differ in the spatial arrangement of atoms around a double bond or a ring.
Optical isomers: Stereoisomers that are non-superimposable mirror images of each other.
Cyclic hydrocarbons: Hydrocarbons in which the carbon atoms form a ring structure.
Aromatic compound: A type of cyclic hydrocarbon with alternating double and single bonds, often possessing a distinctive odor.
