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Lewis Theory
Explains how atoms bond to form molecules.
Chemical Bond
Forms when bonded atoms' potential energy decreases.
Polar Covalent Bond
Unequal sharing of electrons between unlike atoms.
Electronegativity
Ability of an atom to attract electrons in a bond.
Electronegativity Trend
Increases left to right, decreases top to bottom.
Bond Polarity
Determined by the difference in electronegativity.
Dipole Moment
Measure of charge separation in polar bonds.
Percent Ionic Character
Percentage of bond's dipole compared to ionic bond.
Lewis Structure
Diagram showing bonding and arrangement of valence electrons.
Octet Rule
Atoms are most stable with eight valence electrons.
Central Atom
Least electronegative atom in a molecule.
Formal Charge
Charge assigned to an atom in a molecule.
Resonance Structures
Different ways to represent a molecule's electron distribution.
Bond Energy
Energy required to break a bond between atoms.
Bond Length
Distance between the nuclei of two bonded atoms.
Bond Strength
Energy needed to break a bond; related to bond length.
VSEPR Theory
Predicts molecular shapes based on electron repulsion.
Valence Electrons
Electrons in the outermost shell of an atom.
Anion
Negatively charged ion, gains electrons.
Cation
Positively charged ion, loses electrons.
Single Bond
One pair of electrons shared between two atoms.
Electron Deficiency
Condition where an atom has fewer electrons than needed.
Resonance
Delocalization of electrons across multiple structures.
Octet Rule
Atoms form bonds to achieve eight electrons.
Lewis Structure
Diagram showing electron arrangement in molecules.
Central Atom
Atom bonded to multiple other atoms.
Formal Charge
Charge if bonding electrons shared equally.
Expanded Octet
More than eight electrons around an atom.
Resonance Structures
Different Lewis structures for the same molecule.
Resonance Hybrid
Average of multiple resonance structures.
Bond Strength
Measured by bond enthalpy; energy to break bond.
Bond Length
Distance between nuclei of bonded atoms.
VSEPR Theory
Predicts molecular shape based on electron repulsion.
Bond Enthalpy
Energy required to break a chemical bond.
Single Bond
One pair of electrons shared between atoms.
Double Bond
Two pairs of electrons shared between atoms.
Triple Bond
Three pairs of electrons shared between atoms.
Electronegativity
Tendency of an atom to attract electrons.
Lone Pairs
Non-bonding pairs of electrons on an atom.
Connectivity
Arrangement of atoms in a molecule.
Molecule with Odd Electrons
Example: Nitric Oxide (NO) with unpaired electron.
Formal Charge Calculation
Valence electrons minus lone pairs and half bonding.
Charge Distribution
Preferred structures have fewer and smaller formal charges.
Bond Length Trends
Shorter bonds are generally stronger.
Molecular Shape
Determined by bond angles and electron pairs.
Electron Groups
Valence electron pairs around central atom.
Steric Number (SN)
Total number of electron groups on central atom.
Lone Pair
Non-bonding electron pair on central atom.
Bonding Pair
Electron pair shared between atoms in a bond.
Trigonal Planar Geometry
Three electron groups form a flat triangular shape.
Bent Molecular Geometry
Shape resulting from lone pairs in three groups.
T-shaped Molecular Geometry
Shape with three lone pairs and five groups.
Linear Molecular Geometry
Shape with four lone pairs and five groups.
Square Pyramidal Shape
Shape with one lone pair and six groups.
Square Planar Shape
Shape with two lone pairs and six groups.
Bond Angle
Angle between adjacent bonds in a molecule.
Polarity of Molecules
Molecule's asymmetrical shape and bond dipoles.
Electronegativity Difference
Measure of atom's ability to attract electrons.
Dipole Moment
Vector quantity representing bond polarity.
Vector Addition
Combining multiple dipole moments geometrically.
Polar Molecule
Molecule with net dipole moment due to shape.
Nonpolar Molecule
Molecule with symmetrical shape, dipoles cancel.
VSEPR Model
Predicts molecular shapes based on electron repulsion.
Glycine
Example of a molecule with multiple central atoms.
HCl Bond Polarity
H-Cl bond is polar due to electronegativity.
CO2 Nonpolarity
CO2 is nonpolar due to symmetrical shape.
Water Polarity
Water is polar due to bent shape and lone pairs.
