Periodic Table Trends/Bonding Theory Flashcards
Size of atoms
Positive Ions are smaller
Negative Ions are bigger
Electronegativity
The ability to attract electrons.
Electron Affinity
The energy released when an electron is added to form an ion
Ionization Energy
The minimum energy needed to remove an electron from an atom.
How small or large ionization energy should be
Electrons closer to the nucleus require more ionization energy in order to be removed then electrons further away from the nucleus
this is because the nucleus contains positive protons which attract the negative electrons
How will q1 q2 change the IE
if q1 q2 increases the ie increases, if q1 q2 decreases the ie decreases
how will d change the IE
if d increases, IE will decrease, if d decreases IE will increase
How to calculate the core charge of any atom
number of protons minus the inner shell electrons
relationship between core charge and valence electrons
the core charge is equal to the number of valence electrons
relationship between valence electrons and IE
how far the valence electrons are from the nucleus determines the minimum IE needed to remove an electron
how to hypothesize which atoms have a larger atomic radius
as you move down a group, atomic radius increases because electrons are added
as you move down the rows the the increasing amount of protons exerts a stronger pull on the electrons leading to a smaller atomic radius
hypothesize which ion would have a larger atomic radius based on its core charge and number of additional/less electrons.
as number of electrons decrease, radius decreases
how can a electron be knocked off by a photon
photons are packets of light
they bombard atoms and electrons are ejected off
they are ejected based on how strongly they are bonded
relationship between “energy levels” and the “rings” of a bohr diagram
energy levels of electrons differ on each ring, electrons closer to the nucleus have less energy
shell
shells are where the electrons “live”
