Polarity and intermolecular forces Flashcards
(16 cards)
Define electronegativity
Electronegativity is a measure of an atom’s ability to attract the shared electron pair in a covalent bond towards itself
Factors that affect electronegativity
- Atomic Radius
-Shielding - Nuclear charge
What type of bond (ionic or covalent) is formed between 2 atoms with a large difference in electronegativity?
Ionic - If the electronegativity difference between the atoms is small, a covalent bond is formed.
What is a polar covalent bond
A polar covalent bond is covalent bond in which the electron density is shared unequally between the bonded atoms due to their difference in electronegativity.
What is a dipole
A dipole is a difference in charge between two atoms caused by a shift in electron density in a bond
What is a polar molecule
A molecule in which the charge is not symmetrically distributed so that one area is slightly positively charged and another slightly negatively charged (a molecule is polar if it has a permanent dipole)
What is a non-polar molecule
A molecule where the polar bonds are arranged symmetrically so the dipoles don’t cancel each other out so the molecule doesn’t have an overall dipole
What are London forces
Weak intermolecular forces that exists between all molecules
What are the 3 main types of intermolecular forces
- London forces
- Permanent dipole-dipole
- Hydrogen bonding
How do London forces form
What factors determine the strength of London forces
What are permanent dipole-dipole interactions
What is a hydrogen bond
Why does ice float on water
Why does water have a higher melting and boiling point than other group 6 hydrides?
