Chemistry Vocabulary [A to Z] Part - 4 (151 to 212)

Chemistry

Vocabulary [A to Z]

Part - 4 (151 to 212)

 151. Orbit

the path of an electron around the nucleus of an atom

152. Orbital

relating to the path of one body around another

153. Organic Compound

any compound of carbon and another element or a radical

154. Osmosis

diffusion of molecules through a semipermeable membrane

155. Oxidation

the process by which a substance combines with oxygen

156. Oxidation Number

the degree of oxidation of an atom or ion or molecule

157. Oxidation-Reduction

a reversible chemical reaction in which one reaction is an oxidation and the reverse is a reduction

158. Oxidize

enter into a combination with oxygen

159. Periodic Law

(chemistry) the principle that chemical properties of the elements are periodic functions of their atomic numbers

160. Periodic Table

arrangement of chemical elements according to atomic number

161. Ph

a measure of the acidity or alkalinity of a solution

162. Phase

a distinct state of matter in a system

163. Phase Change

a change from one state (solid or liquid or gas) to another without a change in chemical composition

164. Ph Scale

a measure of the acidity or alkalinity of a solution

165. Physical Change

a change from one state (solid or liquid or gas) to another without a change in chemical composition

166. Physical Property

any property used to characterize matter and energy and their interactions

167. Plasma

a fourth state of matter distinct from solid, liquid or gas

168. Polar

having a pair of equal and opposite charges

169. Polyatomic

of or relating to a molecule made up of more than two atoms

170. Polymer

a naturally occurring or synthetic compound

171. Polymerization

a chemical process that combines several monomers to form a polymer or polymeric compound

172. Precipitate

a substance separated from a solution or suspension

173. Precision

the quality of being reproducible in amount or performance

174. Product

a chemical substance formed as a result of a reaction

175. Property

a basic or essential attribute shared by members of a class

176. Proton

a stable particle with positive charge

177. Radiation

energy transmitted in the form of rays or waves or particles

178. Radioisotope

a radioactive isotope of an element

179. Reactant

a chemical substance present at the start of a process

180. Reaction

a process in which a substance is changed into another

181. Reagent

a substance for use in chemical reactions

182. Redox

a reversible chemical reaction in which one reaction is an oxidation and the reverse is a reduction

183. Rusting

the formation of reddish-brown ferric oxides on iron by low-temperature oxidation in the presence of water

184. Salinity

the relative proportion of salt in a solution

185. Saponification

a chemical reaction in which an ester is heated with an alkali (especially the alkaline hydrolysis of a fat or oil to make soap)

186. Solid

matter with definite shape at room temperature and pressure

187. Solubility

the quality of being easily dissolved in liquid

188. Solute

the dissolved matter in a solution

189. Solution

a homogeneous mixture of two or more substances

190. Solvent

a liquid substance capable of dissolving other substances

191. Specific Heat

the heat required to raise the temperature of one gram of a substance one degree centigrade

192. State Of Matter

(chemistry) the three traditional states of matter are solids (fixed shape and volume) and liquids (fixed volume and shaped by the container) and gases (filling the container)

193. Stoichiometry

(chemistry) the relation between the quantities of substances that take part in a reaction or form a compound (typically a ratio of whole integers)

194. Stp

standard temperature and pressure

195. Subatomic Particle

a body having finite mass and internal structure but negligible dimensions

196. Sublimation

a change directly from the solid to the gaseous state

197. Subscript

character printed slightly below and to the side of another

198. Substance

a particular kind of matter with uniform properties

199. Surface Tension

phenomenon at a liquid's surface from intermolecular forces

200. Suspension

a mixture in which fine particles are supported by buoyancy

201. Temperature

the degree of hotness or coldness of a body or environment

202. Test Tube

glass tube closed at one end

203. Thermochemistry

the branch of chemistry that studies the relation between chemical action and the amount of heat absorbed or generated

204. Thermodynamics

physics concerned with heat and other forms of energy

205. Titration

a measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete; the concentration of the unknown solution (the titer) can then be calculated

206. Valence

the combining power of an atom or radical

207. Valence Electron

an electron in the outer shell of an atom which can combine with other atoms to form molecules

208. Vaporization

the process of becoming a suspension of particles in the air

209. Viscosity

resistance of a liquid to flowing

210. Volume

the amount of 3-dimensional space occupied by an object

211. Weight

the vertical force exerted by a mass as a result of gravity

212. Yield

an amount of a product

Chemistry Vocabulary [A to Z] Part - 3 (101 to 150)

 Chemistry

Vocabulary [A to Z]

Part - 3 (101 to 150)

101. Group

atoms bound together as a unit forming part of a molecule

102. Halogen

any of five related nonmetallic elements (fluorine or chlorine or bromine or iodine or astatine) that are all monovalent and readily form negative ions

103. Heat

a form of energy transferred by a difference in temperature

104. Heterogeneous

consisting of elements not of the same kind or nature

105. Homogeneous

all of the same or similar kind or nature

106. Hydrate

any compound that contains water of crystallization

107. Hydrocarbon

an organic compound containing only carbon and hydrogen

108. Hydrogen Bond

a chemical bond consisting of a hydrogen atom between two electronegative atoms (e.g., oxygen or nitrogen) with one side be a covalent bond and the other being an ionic bond

109. Hypertonic

having a higher osmotic pressure than a comparison solution

110. Hypotonic

having a lower osmotic pressure than a comparison solution

111. Ideal Gas

a hypothetical gas with molecules of negligible size that exert no intermolecular forces

112. Immiscible

(chemistry, physics) incapable of mixing

113. Indicator

a substance that changes color to show something's presence

114. Inorganic Compound

any compound that does not contain carbon

115. Ion

a particle that is electrically charged positive or negative

116. Ionic

containing or involving electrically charged particles

117. Ionic Bond

a chemical bond between oppositely charged ions

118. Isomer

a compound that exists in forms having different arrangements of atoms but the same molecular weight

119. Isotonic

having the same or equal osmotic pressure

120. Isotope

atom with same atomic number, different number of neutrons

121. Kelvin

British physicist who invented the Kelvin scale of temperature and pioneered undersea telegraphy (1824-1907)

122. Kinetic Theory

(physics) a theory that gases consist of small particles in random motion

123. Lattice

an arrangement of points in a regular periodic pattern

124. Law Of Conservation Of Matter

a fundamental principle of classical physics that matter cannot be created or destroyed in an isolated system

125. Law Of Definite Proportions

(chemistry) law stating that every pure substance always contains the same elements combined in the same proportions by weight

126. Le Chatelier'S Principle

the principle that if any change is imposed on a system that is in equilibrium then the system tends to adjust to a new equilibrium counteracting the change

127. Liquid

fluid matter having no fixed shape but a fixed volume

128. Litmus Test

material that changes color in acidic or alkaline solutions

129. Luster

the property of something that shines with reflected light

130. Malleable

capable of being shaped or bent

131. Mass

the property of a body that causes it to have weight

132. Mass Number

the sum of the number of neutrons and protons in an atomic nucleus

133. Matter

that which has mass and occupies space

134. Melting Point

the temperature at which a solid turns into a liquid

135. Meniscus

the curved upper surface of a liquid in a vertical tube

136. Metal

a chemical element or alloy that is usually a shiny solid

137. Metallic Bond

a chemical bond in which electrons are shared over many nuclei and electronic conduction occurs

138. Metalloid

of or being a nonmetallic element that has some of the properties of metal

139. Miscible

capable of being mixed, in chemistry

140. Mixture

a substance consisting of substances blended together

141. Molarity

concentration measured by molecular weight of a substance

142. Mole

the molecular mass of a substance expressed in grams

143. Molecule

the simplest structural unit of an element or compound

144. Monatomic

of or relating to an element consisting of a single atom

145. Neutral

having only a limited ability to react chemically

146. Neutralization Reaction

a chemical reaction in which an acid and a base interact with the formation of a salt; with strong acids and bases the essential reaction is the combination of hydrogen ions with hydroxyl ions to form water

147. Neutron

a subatomic particle with zero charge

148. Noble Gas

any of the chemically inert gaseous elements of the helium group in the periodic table

149. Nonpolar

not ionic

150. Nucleus

the positively charged dense center of an atom

Chemistry Vocabulary [A to Z] Part - 2 (51 to 100)

 Chemistry

Vocabulary [A to Z]

Part - 2 (51 to 100)

51. Cohesion

the force that holds together molecules in a solid or liquid

52. Colloid

a mixture with properties between those of a solution and fine suspension

53. Combustion

a reaction of a substance with oxygen to give heat and light

54. Composition

the way in which someone or something is put together

55. Compound

a substance formed by chemical union of two or more elements

56. Concentration

the strength of a solution

57. Condensation

process of changing from a gas to a liquid or solid state

58. Conductivity

the property of transmitting heat, electricity, or sound

59. Conductor

a substance that readily serves as a medium for transmission

60. Covalent Bond

a chemical bond that involves sharing a pair of electrons between atoms in a molecule

61. Crucible

a vessel used for high temperature chemical reactions

62. Crystal

a solid having a highly regular atomic structure

63. Crystalline

consisting of or containing or of the nature of crystals

64. Decomposition Reaction

(chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance

65. Density

the amount per unit size

66. Deposition

the natural process of laying something down

67. Desalination

the removal of salt

68. Diatomic

of or relating to a molecule made up of two atoms

69. Dilution

a solution reduced in strength or concentration

70. Dissolve

pass into a solution

71. Distillation

purifying a liquid by boiling it and condensing its vapors

72. Dmitri Mendeleev

Russian chemist who developed a periodic table of the chemical elements and predicted the discovery of several new elements (1834-1907)

73. Double Bond

a covalent bond in which two pairs of electrons are shared between two atoms

74. Double Replacement Reaction

a chemical reaction between two compounds where the positive ion of one compound is exchanged with the positive ion of another compound

75. Ductile

capable of being shaped or bent or drawn out

76. Electrolysis

(chemistry) a chemical decomposition reaction produced by passing an electric current through a solution containing ions

77. Electron

an elementary particle with negative charge

78. Electronegativity

(chemistry) the tendency of an atom or radical to attract electrons in the formation of an ionic bond

79. Element

a substance that cannot be separated into simpler substances

80. Empirical Formula

a chemical formula showing the ratio of elements in a compound rather than the total number of atoms

81. Endothermic

occurring or formed with absorption of heat

82. Endothermic Reaction

a chemical reaction accompanied by the absorption of heat

83. Energy

any source of usable power

84. Entropy

energy in a system no longer available for mechanical work

85. Enzyme

a complex protein produced by cells that acts as a catalyst

86. Equilibrium

a chemical reaction and its reverse proceed at equal rates

87. Evaporation

the process of becoming a suspension of particles in the air

88. Exothermic

occurring or formed with the release of heat

89. Exothermic Reaction

a chemical reaction accompanied by the evolution of heat

90. Family

a collection of things sharing a common attribute

91. Fermentation

breaking down an organic substance, as sugar into alcohol

92. First Law Of Thermodynamics

the fundamental principle of physics that the total energy of an isolated system is constant despite internal changes

93. Fission

splitting a massive nucleus with the release of energy

94. Flammable

easily ignited

95. Free Energy

(physics) a thermodynamic quantity equivalent to the capacity of a physical system to do work; the units of energy are joules or ergs

96. Freezing

the withdrawal of heat to change something from a liquid to a solid

97. Freezing Point

the temperature below which a liquid turns into a solid

98. Fusion

reaction in which nuclei combine to form more massive nuclei

99. Gas

state of matter distinguished from solid and liquid states

100. Gay-Lussac'S Law

(physics) the density of an ideal gas at constant pressure varies inversely with the temperature

201. Temperature

the degree of hotness or coldness of a body or environment

202. Test Tube

glass tube closed at one end

203. Thermochemistry

the branch of chemistry that studies the relation between chemical action and the amount of heat absorbed or generated

204. Thermodynamics

physics concerned with heat and other forms of energy

205. Titration

a measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete; the concentration of the unknown solution (the titer) can then be calculated

206. Valence

the combining power of an atom or radical

207. Valence Electron

an electron in the outer shell of an atom which can combine with other atoms to form molecules

208. Vaporization

the process of becoming a suspension of particles in the air

209. Viscosity

resistance of a liquid to flowing

210. Volume

the amount of 3-dimensional space occupied by an object

211. Weight

the vertical force exerted by a mass as a result of gravity

212. Yield

an amount of a product

Boyle’s Law
The volume of gas depends on its temperature and pressure. According to Boyle’s law, the volume (V) of a definite quantity of gas is inversely proportional to its pressure (P), at constant temperature (T).

V œ 1/P (Temperature constant)
V = K/P K = constant
PV = K