Chemistry: Notes Ssc

Radioactivity is the spontaneous disintegration of unstable atomic nuclei, discovered by . Marie and Pierre Curie discovered Radium and Polonium. Alpha ( ) Particles: Helium nuclei (

Crystalline form, hardest naturally occurring substance, bad conductor of electricity, three-dimensional network.

Introduced by , the pH scale measures acidity or alkalinity ranging from 0 to 14. : Neutral (Pure water) : Basic/Alkaline Common Chemical Indicators Color in Acid Color in Base Litmus Paper Blue turns Red Red turns Blue Phenolphthalein Methyl Orange Important Acids in Nature Citric Acid: Citrus fruits (lemons, oranges) Tartaric Acid: Tamarind, grapes Oxalic Acid: Tomatoes (used to remove ink stains) Lactic Acid: Sour milk, curd Formic Acid (Methanoic acid): Ant stings Acetic Acid: Vinegar 6. Metals, Non-Metals, and Metallurgy

): Carbon atoms arranged in the shape of a football (Buckminsterfullerene). Important Organic Gases Methane ( CH4cap C cap H sub 4 chemistry notes ssc

Chemistry Notes for SSC Exam Prep | PDF | Latent Heat - Scribd

Malleable (can be beaten into sheets) and ductile (can be drawn into wires).

Bitter to taste, soapy to touch, and turn . According to Arrhenius, they release Hydroxyl ions ( OH−cap O cap H raised to the negative power ) in aqueous solution. pH value is greater than 7 . Water-soluble bases are called Alkalis (e.g., NaOHcap N a cap O cap H KOHcap K cap O cap H The pH Scale Introduced by , the pH scale measures acidity

Protons (positive, nucleus), Neutrons (neutral, nucleus), Electrons (negative, shells). Atomic Number ( ): Number of protons. Mass Number ( ): Sum of protons and neutrons. Isotopes: Same atomic number, different mass numbers (e.g., Chapter 3: Acids, Bases, and Salts (High Yield) Acids: Taste sour, turn blue litmus red ( ). Examples: HCl (Stomach acid), H2SO4cap H sub 2 cap S cap O sub 4 (King of Chemicals). Bases: Taste bitter, turn red litmus blue ( ). Examples: NaOH (Caustic soda), (Slaked lime). pH Scale: Measures acidity/alkalinity ( is neutral (water). Common Salts: NaCl (Table salt), NaHCO3cap N a cap H cap C cap O sub 3 (Baking soda), Na2CO3cap N a sub 2 cap C cap O sub 3 (Washing soda). Chapter 4: Metals, Non-metals, and Alloys Metals: Malleable, ductile, good conductors. Non-metals: Poor conductors, brittle. Important Alloys: Brass: Copper + Zinc ( Bronze: Copper + Tin ( Stainless Steel: Iron + Chromium + Nickel ( Chapter 5: Periodic Table & Trends Modern Periodic Law: Arranged by atomic number. Groups: Vertical columns ( Periods: Horizontal rows (

: Indefinite shape. Indefinite volume. Low density. Highly compressible. Key Phase Changes

Discovered by Ernest Rutherford; positively charged. Neutron: Discovered by James Chadwick; neutral charge. Electron: Discovered by J.J. Thomson; negatively charged. Atomic Number (Z): Number of protons in the nucleus. Mass Number (A): Sum of protons and neutrons. Important Organic Gases Methane ( CH4cap C cap

Superheated gas composed of electrons and positive ions. Found in stars and neon signs.

Formed by the complete transfer of electrons from a metal to a non-metal (e.g., NaClcap N a cap C l MgOcap M g cap O

): Number of protons in the nucleus of an atom. It defines the element. Mass Number (

Separating liquids with close boiling points (e.g., Crude oil refining, separating liquid air).

An allotrope of carbon; the hardest naturally occurring substance. Key Ores of Common Metals Iron ( ): Hematite ( Fe2O3cap F e sub 2 cap O sub 3 ), Magnetite ( Fe3O4cap F e sub 3 cap O sub 4 ), Siderite ( FeCO3cap F e cap C cap O sub 3 Aluminum ( ): Bauxite ( ), Cryolite ( Na3AlF6cap N a sub 3 cap A l cap F sub 6 Copper ( ): Copper Pyrites ( CuFeS2cap C u cap F e cap S sub 2 ), Malachite Mercury ( ): Cinnabar ( HgScap H g cap S Lead ( ): Galena ( PbScap P b cap S Calcium ( ): Limestone ( CaCO3cap C a cap C cap O sub 3 ), Gypsum ( 7. Important Alloys and Their Composition