100 Basic Chemistry Terminology
1. Atom: The tiny building block of matter.
2. Element: A pure substance made of only one type of atom.
3. Molecule: A group of atoms held together by chemical bonds.
4. Compound: A substance made of two or more different elements chemically combined.
5. Proton: A positively charged particle in the nucleus of an atom.
6. Neutron: A neutral particle in the nucleus of an atom.
7. Electron: A negatively charged particle that orbits the nucleus of an atom.
8. Nucleus: The central core of an atom where protons and neutrons are located.
9. Periodic Table: A chart that organizes elements based on their properties.
10. Atomic Number: The number of protons in an atom's nucleus.
11. Atomic Mass: The total mass of an atom, including protons, neutrons, and electrons.
12. Isotope: Atoms of the same element with different numbers of neutrons.
13. Ion: An atom with a positive or negative charge due to the loss or gain of electrons.
14. Chemical Bond: The force that holds atoms together in compounds.
15. Covalent Bond: A bond formed when atoms share electrons.
16. Ionic Bond: A bond formed by the transfer of electrons from one atom to another.
17. Valence Electrons: Electrons in the outermost energy level of an atom.
18. Mixture: A combination of two or more substances that are not chemically bonded.
19. Solution: A homogeneous mixture where one substance dissolves in another.
20. Solvent: The substance in a solution that does the dissolving.
21. Solute: The substance in a solution that gets dissolved.
22. Concentration: The amount of solute dissolved in a solvent.
23. Chemical Reaction: A process where substances change into new substances.
24. Reactant: A substance that participates in a chemical reaction.
25. Product: A substance formed as a result of a chemical reaction.
26. Catalyst: A substance that speeds up a chemical reaction without being consumed.
27. Chemical Equation: A representation of a chemical reaction using symbols and formulas.
28. Acid: A substance that releases hydrogen ions (H+) in a solution.
29. Base: A substance that releases hydroxide ions (OH-) in a solution.
30. pH Scale: A scale used to measure the acidity or basicity of a solution.
31. pH: A measure of the concentration of hydrogen ions in a solution.
32. Salt: A compound formed by the reaction between an acid and a base.
33. Oxidation: A chemical reaction where a substance loses electrons.
34. Reduction: A chemical reaction where a substance gain electrons.
35. Combustion: A rapid chemical reaction between a fuel and oxygen, producing heat and light.
36. Hydrocarbon: A compound made up of hydrogen and carbon atoms.
37. Polymer: A large molecule made up of repeating smaller units.
38. Monomer: The basic building block of a polymer.
39. Chemical Formula: A shorthand notation that represents the composition of a compound.
40. Molecular Formula: A chemical formula that shows the actual number of atoms in a molecule.
41. Empirical Formula: A chemical formula that shows the simplest whole-number ratio of atoms in a compound.
42. Avogadro's Number: The number of atoms or molecules in one mole (6.022 x 10^23).
43. Stoichiometry: The study of the quantitative relationships in chemical reactions.
44. Endothermic: A reaction that absorbs heat from its surroundings.
45. Exothermic: A reaction that releases heat to its surroundings.
46. Ligands: The molecules or ions which are coordinated to the central atom or ion in the coordination compound are called ligands.
47. Rate of Reaction: The speed at which a chemical reaction occurs.
48. Synthesis Reaction: A reaction where two or more substances combine to form a more complex product.
49. Decomposition Reaction: A reaction where a compound breaks down into simpler substances.
50. Single Replacement Reaction: A reaction where one element replaces another in a compound.
51. Double Replacement Reaction: A reaction where the positive and negative ions in two compounds switch places.
52. Precipitate: A solid formed in a double replacement reaction.
53. Chemical Equilibrium: A state in which the forward and reverse reactions in a system occur at the same rate.
54. Kinetic Energy: The energy of motion of particles in a substance.
55. Potential Energy: The stored energy in an object.
56. Exothermic Reaction: A chemical reaction that releases energy in the form of heat.
57. Endothermic Reaction: A chemical reaction that absorbs energy from the surroundings.
58. Activation Energy: The minimum energy required to start a chemical reaction.
59. Law of Conservation of Mass: Matter is neither created nor destroyed in a chemical reaction.
60. Law of Conservation of Energy: Energy cannot be created or destroyed, only converted from one form to another.
61. Sublimation: The change of a substance directly from a solid to a gas.
62. Deposition: The change of a substance directly from a gas to a solid.
63. Condensation: The change of a gas into a liquid.
64. Evaporation: The change of a liquid into a gas.
65. Melting: The change of a solid into a liquid.
66. Freezing: The change of a liquid into a solid.
67. Boiling Point: The temperature at which a substance changes from a liquid to a gas.
68. Melting Point: The temperature at which a substance changes from a solid to a liquid.
69. Density: The mass per unit volume of a substance.
70. Buoyancy: The upward force exerted by a fluid that opposes the weight of an object.
71. Viscosity: The resistance of a liquid to flow.
72. Solubility: The ability of a substance to dissolve in a solvent.
73. Saturation: When a solution can no longer dissolve more solute at a given temperature.
74. Supersaturation: A solution that contains more solute than it should be able to dissolve.
75. Insoluble: A substance that does not dissolve in a particular solvent.
76. Filtration: A method for separating solid particles from a liquid by using a porous barrier.
77. Distillation: A process for separating liquids based on differences in their boiling points.
78. Chromatography: A technique used to separate and analyze the components of a mixture.
79. Acid Rain: Rainfall with a low pH due to the presence of pollutants like sulfur dioxide and nitrogen oxides.
80. Greenhouse Effect: The trapping of heat in Earth's atmosphere by greenhouse gases.
81. Oxidation State: The charge of an atom in a compound, indicating its ability to gain or lose electrons.
82. Radioactive Decay: The spontaneous breakdown of unstable atomic nuclei, releasing radiation.
83. Isomer: Compounds with the same molecular formula but different structures or arrangements.
84. Electrolyte: A substance that conducts electricity when dissolved in water.
85. Redox Reaction: A chemical reaction that involves the transfer of electrons.
86. Half-Life: The time it takes for half of a radioactive substance to decay.
87. Chemical Kinetics: The study of reaction rates and mechanisms.
88. Thermodynamics: The study of the relationships between energy, heat, work, and matter.
89. Solvation: The process of surrounding solute particles with solvent molecules.
90. Neutralization: A reaction between an acid and a base to produce salt and water.
91. Inhibitor: A substance that slows down or inhibits a chemical reaction.
92. Coordination Chemistry: The branch of chemistry which deals with the study of coordination compounds or complex compound is known as coordination chemistry.
93. Alloy: A mixture of two or more elements, at least one of which is a metal.
94. pH Indicator: A substance that changes colour in response to changes in pH.
95. Quantum Mechanics: The branch of physics that deals with the behaviour of particles at the atomic and subatomic level.
96. Bond Energy: The amount of energy required to break a chemical bond.
97. Entropy: A measure of the disorder or randomness of a system.
98. Chemical Equilibrium: A state in which the concentrations of reactants and products remain constant over time.
99. Heat Capacity: The amount of heat required to raise the temperature of a substance by a certain amount.
100. Vaporization: The change of a liquid to a gas at a temperature below its boiling point.
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