Chemical Reaction Rates and Collision Theory

1. Rate: The speed at which a chemical reaction takes place, usually expressed as the change in concentration of reactants or products per unit time.

2. Reaction rate: The rate at which reactants are consumed or products are formed in a chemical reaction.

3. 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.

4. Activation energy: The minimum amount of energy required for a chemical reaction to occur.

5. 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.

6. Reaction intermediate: A species formed during the course of a chemical reaction that is neither a reactant nor a product of the overall reaction.

7. 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.

8. Reversible reactions: Chemical reactions that can proceed in both the forward and reverse directions.

9. 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.

10. Equilibrium position: The relative concentrations of reactants and products at equilibrium.

11. 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.

12. Oxidation: The loss of electrons or an increase in oxidation state of an atom, ion, or molecule.

13. Reduction: The gain of electrons or a decrease in oxidation state of an atom, ion, or molecule.

14. Redox reaction: A chemical reaction in which one substance is oxidized (loses electrons) and another substance is reduced (gains electrons).

15. Reducing agent: A substance that donates electrons and undergoes oxidation in a redox reaction, causing another substance to be reduced.

16. Oxidizing agent: A substance that accepts electrons and undergoes reduction in a redox reaction, causing another substance to be oxidized.

17. Oxidation number: A number assigned to an atom in a chemical compound that indicates the number of electrons lost or gained by the atom.

18. Half reaction: Either the oxidation or reduction part of a redox reaction, showing the transfer of electrons.

19. Oxidation-number-change method: A method for balancing redox reactions by tracking changes in oxidation numbers.

20. Half-reaction method: A method for balancing redox reactions by writing separate equations for the oxidation and reduction half-reactions.

21. 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.

22. Electrochemical process: A chemical reaction that involves the transfer of electrons between species.

23. Electrochemical cell: A device that converts chemical energy into electrical energy, consisting of two electrodes immersed in an electrolyte solution.

24. Voltaic cell: An electrochemical cell that generates electrical energy from spontaneous chemical reactions.

25. Half-cell: One of the two compartments of an electrochemical cell containing either the oxidizing or reducing species.

26. Electrode: A conductor through which electric current enters or leaves an electrolyte or other non-metallic medium.

27. Anode: The electrode where oxidation occurs in an electrochemical cell, attracting negatively charged ions.

28. Cathode: The electrode where reduction occurs in an electrochemical cell, attracting positively charged ions.

29. Reduction potential: The tendency of a species to gain electrons and be reduced, measured relative to a standard hydrogen electrode.

30. Oxidation potential: The tendency of a species to lose electrons and be oxidized, measured relative to a standard hydrogen electrode.

31. Standard reduction potential: The reduction potential of a half-reaction under standard conditions (1 M concentration, 1 atm pressure, and 25°C temperature).

32. Standard cell potential: The potential difference between the two half-cells of an electrochemical cell under standard conditions.

33. Electrolyte cell: An electrochemical cell in which an electric current is generated or consumed through an electrolytic process.

34. Electrolysis: The process of using electrical energy to drive a non-spontaneous chemical reaction.

35. Electroplating: The process of coating an object with a thin layer of metal using electrolysis.

36. Fuel cell: An electrochemical cell that converts the chemical energy of a fuel directly into electrical energy.

37. Organic compound: A compound containing carbon atoms.

38. Hydrocarbon: A compound consisting of hydrogen and carbon atoms only.

39. Structural formula: A representation of the molecular structure of a compound, showing the arrangement of atoms and bonds.

40. Alkane: A saturated hydrocarbon with single bonds between carbon atoms.

41. Straight-chain alkane: An alkane in which the carbon atoms are arranged in a continuous chain with no branching.

42. Branched-chain alkane: An alkane in which carbon atoms are arranged in a chain with one or more side chains branching off.

43. Substituent: An atom or group of atoms that can replace a hydrogen atom in an organic compound.

44. Condensed structural formula: A simplified version of a structural formula in which certain groups of atoms are represented by specific symbols.

45. Alkene: A hydrocarbon containing at least one carbon-carbon double bond.

46. Alkyne: A hydrocarbon containing at least one carbon-carbon triple bond.

47. Saturated compound: A compound containing only single bonds between carbon atoms. (only alkane)

48. Unsaturated compounds: Compounds containing multiple bonds (double or triple bonds) between carbon atoms.

49. Degree of saturation: The extent to which a compound contains multiple bonds relative to the maximum possible number of bonds.

50. Isomers: Compounds with the same molecular formula but different structural arrangements or spatial orientations of atoms.

51. Structural isomers: Isomers with different arrangements of atoms in their molecular structure.

52. Stereoisomers: Isomers with the same molecular formula and the same connectivity of atoms but different spatial arrangements of atoms.

53. Geometric isomers: Stereoisomers that differ in the spatial arrangement of atoms around a double bond or a ring.

54. Optical isomers: Stereoisomers that are non-superimposable mirror images of each other.

55. Cyclic hydrocarbons: Hydrocarbons in which the carbon atoms form a ring structure.

56. Aromatic compound: A type of cyclic hydrocarbon with alternating double and single bonds, often possessing a distinctive odor.