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periodicity
Trends or recurring variations in element properties with increasing atomic numbers
electronegativity
The tendency of an atom to attract electrons in a bond to itself
ionization energy
Energy required to remove an electron from a gaseous atom or ion/remove from the 1rst electron in the valence electron’s shell
Atomic Radius
One half of the distance between the nuclei of 2 identical atoms when they are joined by a covalent bond
Nuclear Charge
The pull exerted on a specific electron by the nucleus (# of protons)
sheilding
when another electron blocks the attraction of an additional electron to the nucleus
effective nuclear charge
the regular amount of protons, or the nuclear charge (z), with sheilding taken into account; zeff=z-sheilding
across a period, atomic radius __________ because ___________
decreases because the effective nuclear charge (zeff) increases while shielding remails constant (n is constant), and electrons are pulled closer by increasing atomic number/protons in the nucleus, causing more attraction and a smaller atomic radius
down a group, atomic radius __________ because ___________
increases because there are more energy levels; the principal quantum number (n, vertical numbers) increases as energy levels are added, giving rise to a larger atomic radius
Why Exceptions for atomic radius happen
a new subshell (s, p, d, f) is added to the outermost energy level; instead of decreasing, it increases
Exceptions for atomic radius
Mg—>Al
[Ne]s2—>[Ne]3s2,3p1
Zn—>Ga
[Ar] 4s2,3d10—>[Ar] 4s2,3d10, 4p1
across a period, ionization energy ___________ because ___________
increases because the effective nuclear charge (zeff) goes up with the increasing atomic number, causing more attraction; this makes it more difficult to remove a valence a valence electron, meaning more energy will be required
down a group, ionization energy __________ because ____________
decreases because more energy levels are present, meaning that there are more core electrons (electrons close to the center), giving rise to more sheilding; there is therefore less attraction, making it easier to remove a valence electron and causing more blockage; this blockage makes it easier to take an electron away with less energy required
why exceptions for ionization energy happe
when 1 orbital is full or half full, it is more stable and harder for an electron to be removed, making it decrease
exceptions for ionization energy
Be—>B
Mg—>Al
N→O
P—>S
Across a period, electronegativity ___________ because ___________
increases because there is more effective nuclear charge (zeff), meaning that it is more attractive to valence electrons
down a group, electronegativity _______ because ____________
decreases because there are more energy levels, meaning that there are more core electrons and therefore more sheilding; there is more distrance between valence electrons and the nucleusl it is less attractive to the electrons
why exceptions happen for electronegativity
electrons aren’t necessary because an atom is already stable with a full outer shell
exceptions for electronegativity
noble gases are already stable so they have very little electronegativity