VSPER Flashcards
VSEPR theory 3 points
- pairs of electrons surrounding a central atom of a molecule
-Arrange as far as possible to avoid electron electron repulsion
-Used to predict shapes of molecules and polarity of molecules
Shapes and names and angles
Linear 180
Planner 120
Tetrahedral 109.5
Bent 109.5
Pyramidal 107
Polar bond
Electrons shared unequally usually atom with a stronger electronegativity is slightly negative
Nonpolar bond
Electron shared equally
Electronegativity
Level of attraction
Caused by difference in electronegativity between atoms
Polarity
What does polarity results?
A dipole moment with a slightly negative and slightly positive end
Polar molecule
Asymmetrical distribution of charges
Symmetrical distribution
Nonpolar
Intramolecular forces, examples and meaning
Forces that holds atoms together within a molecule
Covalent ionic metallic bonds
Intermolecular forces
Forces that exist between molecules
London depression forces dipole, dipole, hydrogen bond
London diversion forces
Weakest force
Present in all substance ignore if there’s a stronger force
Momentarily uneven distribution of electrons
Strength increase electrons increase
Dipole dipole
Permanent dipole
Attractive forces which exist between polar molecules
Negative and will be attracted to the positive end of another
Stronger than LD F
Hydrogen bonding
Attractive for us between hydrogen attached to an electronegative Adam of one molecule and another different molecule
Strongest force
Hydrogen and oxygen
Hydrogen and nitrogen
Hydrogen and fluorine
Vanderwall forces
Term used to describe the weakest intermolecular attractions includes dipersion and dipole attractions
