Bonding

The electrostatic attraction between oppositely charged ions • between a metal and a non metal • electrons are transferred from a non metal to a metal to achieve a full outer shell • oppositely charged particles attract through electrostatic forces to form giant ionic lattice

a shared pair of electrons. the electron pair is attracted by both nuclei so resists seperation • forms between two non-metals • electrons are shared between the two outer shells to achieve a full outer shell.

a covalent bond where both electrons in the shared pair originate from the same atom

the attraction between positive metal ions and the surrounding sea of delocalised electrons

to get as far apart from each other as possible

linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral

because they’re closer to the nucleus and repel more strongly than bonding pairs

2.5

The power of an atom to attract the pair of electrons in a covalent bond

• as nuclear charge increases so does electronegativity • as atomic radius increases, so does shielding, so electronegativity decreases

the nuclear charge increases meaning the outer electrons are more attracted to the nucleus, reducing the atomic radius

as there are fewer energy levels so the outer electron is more attracted to the nucleus

one in which the electron density across the whole molecule is unevenly distributed • polar is non-symmetrical • non polar is symmetrical

they’re between polar molecules

between a lone pair and H • only N,O,F • strongest intermolecular force

• weakest intermolecular force • exists between all molecules at all times and are in addition to any other intermolecular forces • the more electrons the stronger they are as they’re caused by the movement of electrons

vaporisation - the energy needed to boil a liquid - enthalpy of vaporisation

fusion- the energy needed to melt a solid - enthalpy of fusion

sublimation

giant ionic, giant metalic, simple covalent, giant covalent

they have strong electrostatic attractions between oppositely charged ions

• ions are free to move around in solution or molten but fixed when solid and can’t move freely

• a force can move the ions and produce contact between like charges causing them to repel (break)

ions become surround by the water molecules and pull apart the positive and negative ions in the crystal lattice through electrostatic attraction