Fundamental Concepts of Organic and Inorganic Chemistry

Fundamentals of Organic Chemistry

Hydrocarbons

Alkanes

These are saturated hydrocarbons with single carbon-carbon bonds.

• General Formula: CnH2n+2
• Suffix: -ane
• Prefixes by Carbon Count:
  • 1C: meth-
  • 2C: eth-
  • 3C: prop-
  • 4C: but-
  • 5C: pent-
  • 6C: hex-

Alkenes

Unsaturated hydrocarbons containing at least one carbon-carbon double bond (C=C).

• General Formula: CnH2n
• Suffix: -ene
• Prefixes by Carbon Count:
  • 2C: eth-
  • 3C: prop-
  • 4C: but-
  • 5C: pent-
  • 6C: hex-

Alkynes

Unsaturated hydrocarbons containing at least one carbon-carbon triple bond.

• General Formula: CnH2n-2
• Suffix: -yne
• Prefixes by Carbon Count:
  • 2C: eth-
  • 3C: prop-
  • 4C: but-
  • 5C: pent-
  • 6C: hex-

Common Functional Groups

• Carboxylic Acids: Suffix is -anoic acid.
• Aldehydes: Suffix is -anal.
• Ketones: General structure R-CO-R', where R can be a hydrogen atom or a radical. The suffix is -one.

Introduction to Inorganic Chemistry

Classification of Metals

Alkali Metals (Group IA)

Elements include Li, Na, K, Rb, Cs, and Fr.

• High metallic character.
• Solid at room temperature.
• Very reactive.

Alkaline Earth Metals (Group IIA)

Elements include Be, Mg, Ca, Sr, Ba, and Ra.

• Less reactive than alkali metals.

Transition Metals (Groups IB - VIIIB)

Examples include Au, Ag, Fe, Zn, and Cu.

• High density and melting points (except for Hg, which is a liquid).
• Some exhibit magnetic properties.

Inner Transition Metals (Group IIIB)

These belong to two series:

1. Lanthanides: Soft, gray-colored metals that are good electrical conductors.
2. Actinides: Have radioactive properties similar to actinium. Elements with atomic numbers greater than 92 do not exist naturally.

Metalloids or Semimetals (Groups IIIA to VIIA)

Elements include B, Si, Ge, As, Sb, Te, Po, and At.

• They have properties intermediate between metals and non-metals.

Reactions of Metals

Formation of Basic Oxides

A metal reacts with oxygen to form a basic oxide (Metal + O₂).

• 4Na + O₂ → 2Na₂O
• 2Ca + O₂ → 2CaO

Formation of Hydroxides (Bases)

A basic oxide reacts with water to form a hydroxide. Hydroxides are identified by the OH group.

• Na₂O + H₂O → 2NaOH
• CaO + H₂O → Ca(OH)₂

Formation of Halide Salts from Acids

A metal reacts with an acid to produce a salt and hydrogen gas (Metal + Acid → Salt + H₂).

• Mg + 2HCl → MgCl₂ + H₂
• 2Na + 2HBr → 2NaBr + H₂

Non-Metals and Their Reactions

Groups of Non-Metals

• Carbon Group (IVA): C, Si, Ge, Sn, Pb
• Nitrogen Group (VA): N, P, As, Sb, Bi
• Oxygen Group (VIA): O, S, Se, Te, Po
• Halogen Group (VIIA): F, Cl, Br, I, At

Formation of Acidic Oxides (Anhydrides)

A non-metal reacts with oxygen.

• 2C + O₂ → 2CO (Incomplete combustion)

Formation of Oxyacids

An acidic oxide reacts with water.

• SO₃ + H₂O → H₂SO₄
• CO₂ + H₂O → H₂CO₃

Formation of Hydracids

A halogen or sulfur reacts with hydrogen.

• S + H₂ → H₂S
• Cl₂ + H₂ → 2HCl

The key difference between oxyacids and hydracids is the presence of oxygen in oxyacids.

Formation of Halide Salts from Elements

A metal reacts with a halogen.

• 2Na + Cl₂ → 2NaCl

Neutralization Reactions

An acid reacts with a base to produce a salt and water.

• Acid + Base → Salt + H₂O
• Example: HCl + NaOH → NaCl + H₂O