Search results
Results from the WOW.Com Content Network
Methanol and its vapours are flammable. Moderately toxic for small animals – Highly toxic to large animals and humans (in high concentrations) – May be fatal/lethal or cause blindness and damage to the liver, kidneys, and heart if swallowed – Toxicity effects from repeated over exposure have an accumulative effect on the central nervous system, especially the optic nerve – Symptoms may ...
Chemical formula Boiling point Dielectric constant Density Dipole moment Polar protic solvents: formic acid: HCO 2 H: 101 °C 58 1.21 g/mL 1.41 D n-butanol: CH 3 CH 2 CH 2 CH 2 OH: 118 °C 18 0.810 g/mL 1.63 D isopropanol (IPA) (CH 3) 2 CH(OH) 82 °C 18 0.785 g/mL 1.66 D nitromethane: CH 3 NO 2: 101°C 35.87 1.1371 g/mL 3.56 D ethanol (EtOH) CH ...
Note that the dipole moments drawn in this diagram represent the shift of the valence electrons as the origin of the charge, which is opposite the direction of the actual electric dipole moment. The bond dipole moment [5] uses the idea of electric dipole moment to measure the polarity of a chemical bond within a molecule. It occurs whenever ...
Here is a similar formula from the 67th edition of the CRC handbook. Note that the form of this formula as given is a fit to the Clausius–Clapeyron equation, which is a good theoretical starting point for calculating saturation vapor pressures: log 10 (P) = −(0.05223)a/T + b, where P is in mmHg, T is in kelvins, a = 38324, and b = 8.8017.
The polarizability of an atom or molecule is defined as the ratio of its induced dipole moment to the local electric field; in a crystalline solid, one considers the dipole moment per unit cell. [1] Note that the local electric field seen by a molecule is generally different from the macroscopic electric field that would be measured externally.
The reaction field method is used in molecular simulations to simulate the effect of long-range dipole-dipole interactions for simulations with periodic boundary conditions. Around each molecule there is a 'cavity' or sphere within which the Coulomb interactions are treated explicitly.
The polarity, dipole moment, polarizability and hydrogen bonding of a solvent determines what type of compounds it is able to dissolve and with what other solvents or liquid compounds it is miscible. Generally, polar solvents dissolve polar compounds best and non-polar solvents dissolve non-polar compounds best; hence " like dissolves like ".
Chemical formula Boiling point Dielectric constant Density Dipole moment Comment Polar aprotic solvents: acetone: C 3 H 6 O 56.05 °C 21.83 0.7845 g/cm 3: 2.91 reacts with strong acids and bases acetonitrile : CH 3 CN 81.3 - 82.1 °C 38.3 0.776 g/cm 3: 3.20 reacts with strong acids and bases dichloromethane: CH 2 Cl 2: 39.6 °C 9.08 1.3266 g/cm ...