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Study Notes/NMAT/Chemistry

NMAT Chemistry

Comprehensive guide to Inorganic Chemistry, Organic Chemistry & Biochemistry

Estimated: 50 min readPart 2 of 5

In This Lesson

1. Inorganic Chemistry2. Organic Chemistry3. Biochemistry4. Important Reactions
Section 1

Inorganic Chemistry

Atomic Structure

Key Concepts

  • Protons: Positive charge, determines element identity (atomic number)
  • Neutrons: No charge, affects mass and isotopes
  • Electrons: Negative charge, determines chemical behavior
  • Atomic Number (Z): Number of protons
  • Mass Number (A): Protons + Neutrons

Electron Configuration

Order of filling: 1s β†’ 2s β†’ 2p β†’ 3s β†’ 3p β†’ 4s β†’ 3d β†’ 4p β†’ 5s β†’ 4d β†’ 5p β†’ 6s β†’ 4f β†’ 5d β†’ 6p

Aufbau Principle: Electrons fill lowest energy orbitals first

Pauli Exclusion: Maximum 2 electrons per orbital (opposite spins)

Hund's Rule: Electrons fill orbitals singly before pairing

Periodic Table Trends

Increases Left to Right β†’
  • β€’ Electronegativity
  • β€’ Ionization energy
  • β€’ Electron affinity
Increases Top to Bottom ↓
  • β€’ Atomic radius
  • β€’ Metallic character
  • β€’ Number of electron shells

Chemical Bonding

Ionic Bonds
  • Metal + Nonmetal
  • Electron transfer
  • High melting point
  • Conducts electricity when dissolved
Covalent Bonds
  • Nonmetal + Nonmetal
  • Electron sharing
  • Lower melting point
  • Poor conductor
Metallic Bonds
  • Metal + Metal
  • "Sea of electrons"
  • Good conductor
  • Malleable, ductile

Acids and Bases

Acids
  • Donate H⁺ (protons)
  • pH < 7
  • Sour taste
  • React with metals to produce Hβ‚‚
  • Examples: HCl, Hβ‚‚SOβ‚„, HNO₃
Bases
  • Accept H⁺ / Donate OH⁻
  • pH > 7
  • Bitter taste, slippery
  • React with acids (neutralization)
  • Examples: NaOH, KOH, NH₃

pH Scale

pH = -log[H⁺]
0-6: Acidic | 7: Neutral | 8-14: Basic
Each pH unit = 10Γ— difference in H⁺ concentration

Section 2

Organic Chemistry

Organic chemistry is the study of carbon-containing compounds. Carbon's ability to form four bonds makes it uniquely suited for creating complex molecules essential for life.

Functional Groups

Functional GroupStructureExample
Alcohol-OHEthanol (Cβ‚‚Hβ‚…OH)
Aldehyde-CHOFormaldehyde
KetoneC=O (middle)Acetone
Carboxylic Acid-COOHAcetic acid
Ester-COO-Ethyl acetate
Amine-NHβ‚‚Methylamine
Amide-CONHβ‚‚Acetamide

Hydrocarbons

Alkanes (Saturated)

Single bonds only, C-C

General formula: Cβ‚™Hβ‚‚β‚™β‚Šβ‚‚

Methane, Ethane, Propane, Butane

Alkenes (Unsaturated)

Contains C=C double bond

General formula: Cβ‚™Hβ‚‚β‚™

Ethene, Propene, Butene

Alkynes

Contains C≑C triple bond

General formula: Cβ‚™Hβ‚‚β‚™β‚‹β‚‚

Ethyne (Acetylene)

Aromatics

Contains benzene ring

Alternating double bonds

Benzene, Toluene, Phenol

Isomerism

  • Structural Isomers: Same molecular formula, different connectivity
  • Geometric Isomers (cis/trans): Different arrangement around double bond
  • Optical Isomers (Enantiomers): Mirror images, chiral center
Section 3

Biochemistry

Biomolecules

Carbohydrates

  • Monosaccharides: Glucose, Fructose, Galactose
  • Disaccharides: Sucrose, Lactose, Maltose
  • Polysaccharides: Starch, Glycogen, Cellulose
  • Function: Energy source, storage, structural support

Lipids

  • Fatty acids: Saturated vs Unsaturated
  • Triglycerides: Glycerol + 3 fatty acids
  • Phospholipids: Cell membrane structure
  • Steroids: Cholesterol, hormones
  • Function: Energy storage, insulation, hormones

Proteins

  • Building blocks: 20 amino acids
  • Peptide bond: Links amino acids
  • Structure levels: Primary, Secondary (Ξ±-helix, Ξ²-sheet), Tertiary, Quaternary
  • Function: Enzymes, transport, structure, immunity

Nucleic Acids

  • DNA: Deoxyribose, A-T, G-C, double helix
  • RNA: Ribose, A-U, G-C, single strand
  • Types of RNA: mRNA, tRNA, rRNA
  • Function: Genetic information storage and expression

Enzymes

  • Definition: Biological catalysts (proteins) that speed up reactions
  • Lock and Key Model: Substrate fits into active site
  • Factors Affecting Activity: Temperature, pH, substrate concentration
  • Inhibitors: Competitive (binds active site) vs Non-competitive (binds elsewhere)
Section 4

Important Reactions

Synthesis (Combination)

A + B β†’ AB

Two or more substances combine

Decomposition

AB β†’ A + B

One substance breaks apart

Single Replacement

A + BC β†’ AC + B

One element replaces another

Double Replacement

AB + CD β†’ AD + CB

Two compounds exchange partners

Combustion

Fuel + Oβ‚‚ β†’ COβ‚‚ + Hβ‚‚O

Rapid reaction with oxygen

Neutralization

Acid + Base β†’ Salt + Hβ‚‚O

Acid-base reaction

Balancing Equations Tip

Remember the Law of Conservation of Mass: Atoms are neither created nor destroyed. Balance one element at a time, starting with the most complex molecule.

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