flask Chemical Bonding & Structure
Chemical bonding explains why table salt shatters, metals bend, and water flows. From Lewis structures to VSEPR shapes to intermolecular forces, this topic connects atomic structure to the properties of everything around you.
What you will learn
- Distinguish ionic, covalent, and metallic bonding
- Draw Lewis structures
- Predict molecular geometry with VSEPR
- Explain bond and molecular polarity
- Describe intermolecular forces
High School concepts
Bond Polarity: Unequal Sharing of Electrons
How electronegativity differences create polar covalent bonds with partial charges, and the 0.5 and 1.7 cutoffs that separate bond types.
Dipole–Dipole Forces: Polar Molecules Attracting
How the positive end of one polar molecule attracts the negative end of another, and how these forces raise boiling points of polar compounds.
Formal Charge: Bookkeeping for Electrons
How to calculate formal charge on each atom in a Lewis structure and use it to pick the most plausible structure among alternatives.
Hydrogen Bonding: The Strongest Dipole Attraction
When hydrogen bonds form between molecules, why they need N, O, or F, and how they give water its strange and life-supporting properties.
Intermolecular Forces: Attractions Between Molecules
An overview of the forces between molecules — hydrogen bonding, dipole-dipole, and London dispersion — and how they control boiling points and solubility.
Lewis Structures: Drawing Molecules on Paper
A step-by-step method for drawing Lewis dot structures, counting valence electrons, placing bonds and lone pairs, and checking the octet rule.
London Dispersion Forces: Attraction in Every Molecule
How fleeting, random electron shifts create temporary dipoles that attract all molecules, and why bigger molecules boil at higher temperatures.
Molecular Geometry: The Shapes of Molecules
From linear to octahedral: how VSEPR predicts the actual 3D shapes of molecules and how to assign each molecule its geometry name.
Resonance: When One Drawing Is Not Enough
Why some molecules need several Lewis structures, what delocalized electrons really mean, and how resonance explains bond lengths and stability.
VSEPR Theory: Electrons Repel, Shapes Emerge
How the repulsion between electron domains around a central atom determines electron geometry, and why lone pairs squeeze bond angles.
Beginner concepts
Covalent Bonding: Sharing Electrons in Molecules
How atoms share electron pairs to form molecules, why shared pairs lower energy, and how single, double, and triple bonds differ in length and strength.
Ionic Bonding: Electron Transfer and Salt Crystals
How metals donate and nonmetals accept electrons to form ions, and how those ions pack into crystalline lattices with high melting points and brittleness.
Metallic Bonding: The Electron Sea Model
How delocalized electrons glue metal cations together, explaining conductivity, malleability, luster, and why metals behave so differently from salts.
Introductory College concepts
Hybridization: Mixing Orbitals to Explain Shapes
A gentle introduction to sp, sp2, and sp3 hybrid orbitals: why carbon mixes its orbitals and how hybridization connects to molecular geometry.
Molecular Polarity: Does the Whole Molecule Have a Dipole?
How to combine bond polarities with 3D shape to decide whether a molecule is polar, using vector addition and symmetry arguments.