Study ionic, covalent, and metallic bonds.
The type of bond formed when electrons are shared between atoms
The type of bond formed when electrons are transferred from one atom to another
A weak bond that occurs between molecules due to partial charges
The rule that states atoms tend to form bonds to achieve a full outer shell of electrons
A type of bond where the electron pair is shared unequally between atoms
The measure of the ability of an atom to attract electrons
A bond where one pair of electrons is shared between two atoms
A bond where two pairs of electrons are shared between two atoms
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The type of bond formed when electrons are shared between atoms
Covalent Bond
The type of bond formed when electrons are transferred from one atom to another
Ionic Bond
A weak bond that occurs between molecules due to partial charges
Hydrogen Bond
The rule that states atoms tend to form bonds to achieve a full outer shell of electrons
Octet Rule
A type of bond where the electron pair is shared unequally between atoms
Polar Covalent Bond
The measure of the ability of an atom to attract electrons
Electronegativity
A bond where one pair of electrons is shared between two atoms
Single Covalent Bond
A bond where two pairs of electrons are shared between two atoms
Double Covalent Bond
A bond where three pairs of electrons are shared between two atoms
Triple Covalent Bond
The electrons in the outermost shell of an atom that are involved in forming bonds
Valence Electrons
A type of chemical bond that forms between positively charged metal ions and the electrons around them
Metallic Bond
The energy required to break a chemical bond and form neutral isolated atoms
Bond Energy
Forces of attraction between molecules
Intermolecular Forces
Attractive forces that occur between positive ends of polar molecules and negative ends of other polar molecules
Dipole-Dipole Interactions
The weakest intermolecular force that occurs as a result of momentary changes in electron density in a molecule
London Dispersion Forces
The process of forming ions by gaining or losing electrons to achieve a full outer electron shell
Ion Formation
The three-dimensional arrangement of atoms in a molecule
Molecular Geometry
The various forms that a molecule can take when multiple Lewis structures are possible
Resonance Structures
A measure of how equally or unequally the electrons in any covalent bond are shared
Bond Polarity
The energy required to separate one mole of an ionic compound into its gaseous ions
Lattice Energy
Applications of chemical bonds include the formation of water, salt, sugar, and diamond among others
Real-World Materials
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