Intermolecular Forces and more Flashcards
Covalent bonds
bonds that are formed by electrostatic attraction between a shared pair of electrons and the positively charged nuclei
The octet rule
The tendency of atoms to gain a valence shell with a total of 8 electrons
A coordination bond
A covalent bond in which both the electrons of the shared pair originate from the same atom
VSEPR
The valence shell electron repulsion model enables the shapes of molecules to be predicted from the repulsion of electron domains around a central atom
What are the structures and properties of Si, SiO2, and carbon’s allotropes?
Intermolecular forces
The nature of the force that exists between molecules is determined by the size and polarity of the molecules. Intermolecular forces include London (dispersion), dipole-dipole, dipole-induced dipole, and hydrogen bonding.
–London forces between all molecules and are the weakest, whereas H bonding is the strongest
Resonance structures
occur when there is more than 1 possible position for a double bond in a molecule
Benzene (C6H6) structure
- A cyclic hydrocarbon, with 6 C atoms arranged in a hexagonal ring
- has a stable resonance structure due to delocalized pi electrons over the entire ring
- the circle in a hexagon symbolizes delocalized pi electrons
- sp2 hybridization
- all C-C bonds are equal
Formal Charge
- used to determine which of several possible Lewis formulas is preferred
- can be calculated for each atom in a species
Sigma bonds
- form by the head-on (axial) combination of atomic orbitals where the electron density is concentrated along the bond axis
Pi bonds
- form by the lateral (sideways) combination of p-orbitals where the electron density is concentrated on opposite sides of the bond axis
Hybridization
- the concept of mixing atomic orbitals to form new hybrid orbitals for bonding
