Useful Links
Chemistry
General Chemistry
Chemical Bonding
Ionic Bonds
Definition and Characteristics
Electrostatic attraction between oppositely charged ions
Typically formed between metals and nonmetals
Transfer of electrons from metal to nonmetal
Formation of Ionic Compounds
Cation and anion formation
Loss of electrons by metals to form cations
Gain of electrons by nonmetals to form anions
Lattice structure
Arrangement of ions in a repeating pattern
Influence on melting and boiling points
Properties of Ionic Compounds
High melting and boiling points
Electrical conductivity in molten state or when dissolved in water
Solubility in polar solvents
Covalent Bonds
Definition and Characteristics
Sharing of electron pairs between atoms
Typically formed between nonmetal atoms
Types of Covalent Bonds
Single Bonds
Sharing of one pair of electrons
Bond length and strength
Double Bonds
Sharing of two pairs of electrons
Comparatively shorter and stronger than single bonds
Triple Bonds
Sharing of three pairs of electrons
Shortest and strongest among covalent bonds
Polar and Nonpolar Covalent Bonds
Polar Covalent Bonds
Unequal sharing of electrons
Electronegativity differences between bonded atoms
Partial charges leading to dipoles
Nonpolar Covalent Bonds
Equal sharing of electrons
Similar electronegativity between bonded atoms
Resonance Structures
Concept of resonance
Alternate Lewis structures for molecules
Delocalization of electrons
Example cases
Benzene
Ozone
Metallic Bonds
Definition and Characteristics
Bonding in metals involving a sea of delocalized electrons
Metal cations surrounded by free-moving electrons
Properties of Metallic Bonds
High electrical and thermal conductivity
Malleability and ductility
Lustrous appearance
Intermolecular Forces
Overview of Intermolecular Forces
Forces of attraction between molecules
Weaker than intramolecular (covalent, ionic, metallic) bonds
Dipole-Dipole Interactions
Occur between polar molecules
Influence on boiling and melting points
Hydrogen Bonding
Strong type of dipole-dipole interaction
Occurs when hydrogen is bonded to electronegative atoms like N, O, or F
Critical in determining properties of water and biological macromolecules
London Dispersion Forces
Present in all molecules, especially nonpolar
Arises due to temporary dipoles
Greater influence in larger and heavier atoms/molecules
Molecular Geometry
VSEPR Theory (Valence Shell Electron Pair Repulsion)
Predicts geometry based on electron pair repulsion
Effect of lone pairs and bonds on molecular shape
Common Molecular Geometries
Linear
Bent
Trigonal planar
Tetrahedral
Trigonal bipyramidal
Octahedral
Hybridization
Concept of orbital mixing
sp, sp², sp³ hybrid orbitals
Relationship between hybridization and molecular geometry
Examples and applications in organic and inorganic chemistry
2. The Periodic Table
First Page
4. Stoichiometry