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Covalent Bond
A bond formed from atoms sharing electrons.
Molecule
A covalent compound made up of two or more atoms.
Formula Unit
The lowest whole number ratio of ions in an ionic compound.
Octet Rule
Atoms become stable by having eight electrons in their valence shell.
Diatomic Elements
Elements that naturally bond to themselves, like H2 or O2.
Single Covalent Bond
A bond formed by the sharing of one pair of electrons.
Double Covalent Bond
A bond formed by the sharing of two pairs of electrons.
Triple Covalent Bond
A bond formed by the sharing of three pairs of electrons.
Bond Length
The distance between the nuclei of two bonded atoms.
Bond Dissociation Energy
The amount of energy required to break a specific covalent bond.
Endothermic Process
A process that absorbs energy, such as breaking bonds.
Covalent Compound Naming Rule
Use prefixes based on subscripts, change the ending of the second element to -ide.
Hydro_ic Acid
Naming convention for binary acids that end in -ide.
Monocyclic Hydrocarbons
Simple hydrocarbons with carbon and hydrogen only.
Alkane Formula
CnH2n+2, where C is the number of carbon atoms.
Alkene Formula
CnH2n, indicating double bonds present.
Alkyne Formula
CnH2n-2, indicating triple bonds present.
Unsaturated Hydrocarbons
Hydrocarbons with double or triple bonds.
Saturated Hydrocarbons
Hydrocarbons that contain only single bonds.
Cyclic Hydrocarbons
Hydrocarbons that form a ring structure.
Alcohol Naming Rule
Drop the -ane from the alkane name and add -anol.
Lewis Structure
Diagram showing the arrangement of valence electrons around atoms.
Central Atom Rule
The least electronegative atom is generally the central atom.
VSEPR Theory
Valence Shell Electron Pair Repulsion, predicts molecular shapes.
Trigonal Planar Geometry
Molecular shape with 3 bonding pairs and 0 lone pairs.
Tetrahedral Geometry
Molecular shape with 4 bonding pairs and 0 lone pairs.
Resonance
Occurs when two or more valid Lewis structures can represent a molecule.
Polar Covalent Bond
A bond where electrons are shared unequally due to electronegativity differences.
Nonpolar Covalent Bond
A bond where electrons are shared equally.
Ionic Bond
A bond formed by the complete transfer of electrons.
Electronegativity
A measure of an atom's ability to attract and hold electrons.
Intermolecular Forces
Forces that occur between molecules, which are generally weak.
Hydrocarbons
Compounds made solely of hydrogen and carbon.
Aromatic Compounds
Compounds that contain a benzene ring.
Square Planar Geometry
Molecular shape with 4 bonding groups and 2 lone pairs.
Seesaw Geometry
Molecular shape with 4 bonding groups and 1 lone pair.
Straight-chain Hydrocarbons
Hydrocarbons with carbon atoms connected in a linear arrangement.
Cyclic Alkanes
Cyclic hydrocarbons following specific bonding patterns.
Bond Character Dependence
Determined by the electronegativity difference of bonded atoms.
Alcohols in Chemistry
Compounds with a hydroxyl group (-OH) bonded to a carbon atom.
Naming Binary Acids
Use the prefix 'hydro' for acids not containing oxygen.
Forces in Covalent Compounds
Covalent bonds are strong, but intermolecular forces are weak.
Shape Symmetry in Molecules
Symmetrical shapes tend to be nonpolar if terminal atoms are identical.
Lowest Melting/Boiling Points
Covalent compounds usually have lower melting and boiling points due to weak intermolecular forces.
Lone Pairs and Bonding
Unshared pairs of electrons impact molecular geometry and polarity.
Hydrogen as a Central Atom
Hydrogen can never be the central atom in a Lewis structure.
Diatomic Element Examples
H2, N2, O2, F2, Cl2, Br2, I2 are all diatomic elements.
Shape Determinants
The geometry and symmetry of a molecule impact its polarity.
Organic Compound Naming Rules
Name compounds starting with carbon and containing many hydrogens.
Acid Naming Rule
Compounds starting with H follow specific acid naming rules.
Electronegativity Difference Importance
Determines whether a bond is ionic, polar covalent, or nonpolar covalent.
Bonding Energy Relation
Shorter bond lengths correspond to greater bond dissociation energy.
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