The force of attraction between two charges is described by Coulomb's law: F=k(q1q2/r^2), where q1 and q2 are the magnitudes of the charges, r is the distance between them, and k is a constant
The strength of any electrostatic attraction is directly proportional to the charges involved
The strength of any electrostatic attraction is inversely proportional to the distance between the charges squared (as the distance of the force of attraction decreases)
Corecharge
A measure of the attractive force between the valence electrons and the nucleus
Atomic radius
The distance from the nucleus to the valence shell electrons
Ionisation energy
The process of moving an electron from an atom
Happens when the atom is given sufficient energy
The energy required to move one electron from an element in its gas phase
If sufficient energy is supplied, all other electrons can be ionised, and the energy required to do this is successive ionisation energy
Electronegativity
The ability of an atom to attract electrons in a covalent bond
The atomic radius decreases
Because the increase in nuclear charge pulls the electrons closer to the nucleus
Ionisation energy is the energy needed to move one electron
Ionisation energy increases because of increasing nuclear charge, which results in stronger attraction between the valence electrons and nucleus
Electrostatic force
A force that acts between charges
Factors impacting electrostatic force
Quantity of charge (more charge = more force)
Distance between charges (more distance = less force)
Quantity of charge
Directly proportional to electrostatic force
Distance between charges
Inversely/indirectly proportional to electrostatic force
An atom of Lithium has 3p+, 4n°, 3e-
Large core charge + small distance
Large electrostatic force
Smaller core charge + further away from nucleus
Small electrostaticforce
Full electron shells
Shield valenceelectrons from the electrostatic force
Going down a group
Electrons experience moreshielding
Going left to right in a period
Electrons experience moreshielding
Atomic radius
Increases down the group (more shells)
Decreases going across the period (larger core charge)
More electrostatic force pulling electrons in
Larger core charge
Ionisation energy
The energy required to remove an electron from an atom
Going down the group
Ionisation energy decreases
Going across the period
Ionisation energy increases
Removing more electrons
Higher ionisation energy required
Electronegativity
The ability of an atom to attract an electron towards itself
Going down a group
Electronegativity goes down (bigger core charge)
Going across a period
Electronegativity increases (closer to the nucleus more force)
Fluorine is the most electronegative and has the highest ionisation energy
Francium is easy to remove an electron but hard to gain one
Electron affinity
Change in energy of an atom when an electron is added to its valence shell
Going up the group
Electronaffinity increases (decreasing energy)
Going across a period
Electron affinity increases (decreasing energy)
Chlorine has the highest electron affinity
Formation of ions
Atoms with a positive or negative charge, trying to become the most stable (least electronaffinity)
Overall netcharge isn't 0 so there is imbalance in protons and electrons