T2 - Bonding and structure Flashcards
Cation
A positively charged ion
Anion
A negatively charged ion
Sigma Bond
A bond that occurs from direct head-on overlap of two-orbitals
Pi Bond
A (double) bond that occurs from a sideways overlap
Define electronegativity
The ability for an atom to attract a pair of electrons towards itself in a covalent bond
How can we quantify how how electronegative an element is?
The Pauling scale
Why is fluorine the most electronegative element?
The futher up and right you go in the periodic table, the most electronegative the element is (Excluding noble gases)
The bigger the difference of electronegativity..
the more ionic the compound will be
What if the difference in electronegativity of a compound is zero?
The compound is purely covalent
How can covalent bonds become polar?
If the atoms attached to it have a difference in electronegativity
Polar bonds -
The bigger the difference in electronegativity, the more polar the bond will be
Polar bonds -
If bonds that are supposedly polar are arranged symmetrically, then there is no overall direction of polarity, therefore no overall polarity (this applies to hydrocarbons)
What are the 3 types of intermolecular forces?
Hydrogen bonding, permanent dipole-dipole and london
London forces -
Any molecule or atom with electrons can form a dipole when they move near to another atom or molecule, as electrons in a molecule/atom can move from one end to the other, which creates a temporary dipole
Why is a sigma bond stronger than a pi bond?
The overlap of a sigma bond is bigger than the overlap of a pi bond
