Compounds & Molecular Structures Flashcards
(30 cards)
Ionic Bonds
Electrostatic force between oppositely charged particles
Crystal Lattice
The formation of large numbers of positive and negative ions existing together in a ratio
Disassociate
Break into ions
Electrolytes
Ions free to move in a solution and can conduct electricity well
Malleable
Able to be hammered into a thin sheet
Ductile
Able to be drawn out into a thin wire
Metallic Bonds
The attraction of a metallic cation for delocalized electrons
Alloy
A mixture of elements that have metallic properties
Covalent bond
A result of non metals sharing valence electrons
Molecule
Formed when 2 or atoms bond covalently.
Sigma bond
Electron pair is shared in an area centred between the 2 atoms
Pi Bond
When parallel orbitals overlap to share electrons
Multiple covalent bonds
Contains 1 sigma bond and at least 1 Pi bond
Bond length
Distance between nuclei
Bond disassociation energy
Amount of energy required to break a specific covalent bond
London dispersion forces
Weak force caused by temporary shifts of electron density in electron clouds between NON POLAR molecules
DIPOLE DIPOLE
An attraction between positive and negative regions of POLAR MOLECULES
Hydrogen Bonding
Dipole dipole attraction between hydrogen atoms and highly electronegative fluorine, nitrogen, and oxygen atoms
Intermolecular
The weak forces of attraction between individual molecules
London dispersion, dipole dipole, hydrogen bonding
INTRAMOLECULAR
Polar, non polar, ionic
Attractive forces
Non-polar covalent
Symmetrical, equal sharing of electrons
Polar covalent
Unsymmetrical, unequal sharing of electrons
Ionic compounds
- most are salts
- exothermic reaction bc resulting compound is so stable
- can conduct electricity while aqueous or liquid
- high melting points
PRACTICE LEWIS STRUCTURES FOR POLYATOMICS RIGHT NOW
5 NOW
