General info
What are valence electrons
The outermost electrons
What is Effective Nuclear Charge
The net positive charge from the nucleus that an electron experiences ( the higher the Z eff --> electrons are pulled more tightly to the nucleus)
What is the general trend for Atomic Radius on the periodic table
Atomic radius generally decreases from left to right
And get larger as you move down a group
Core electrons are involved in bonding (T/F)
False (valence electrons are involved in bonding)
What is shielding?
These inner electrons block, or "shield," the outer electrons from the full, positive pull of the protons.
What is ionization energy
is the energy required to remove an electron from a gaseous atom to produce a gaseous cation.
What is electron affinity
•the energy change when an electron is added to a gaseous atom to form a gaseous anion.
The sizes of atoms are determined by....
electronic structures and interactions between the nucleus and electrons
How do you calculate The Effective nuclear charge
Z eff=Z - S
Ionic Radius for Cations
1. electron
2. What happens to the attraction between the valence electrons and the nucleus
3. What happens to the radii compared to their corresponding neutral atoms
1. Removing an electron decreases the total negative charge of an atom.
2. This increases the attraction between the valence electrons and the nucleus.
3. All cations have smaller radii than their corresponding neutral atoms.
As atoms get larger-> what happens to the Inizatinenergy
IE decreases, making it easier to remove an electron.
What does a negative EA represent
decrease in energy when an electron is added to a gas-phase atom, an exothermic process.
(Most elements have negative EA values)
what is Z
Number of protons
Ionic radius for Anions
1. electron
2. What happens to the attraction between the valence electrons and the nucleus
3. That happens to the radius compared to their neutral atoms.
1. You are adding an electron --> making it more negatively charged
2. This decreases the attraction between the valence electrons and the nucleus and increases the repulsions between valence electrons.
3. All anions have larger radii than their corresponding neutral atoms.
What is First ionization energy vs Second Ionization energy
•The first ionization energy, is the energy required to remove an electron from a gases atom.
•The second ionization energy, is the energy required to remove the second electron fro the +1 gaseous ion.
•Second ionization energies (IE2) are always greater the first ionization energy(IE1).
What does a positive electron affinity represent
endothermic process: energy is required to add an electron to the gaseous atoms
•positive EA values have filled energy levels (noble gases) or sublevels (group 12).
How do you calculate shielding
S=# valence electrons(0.35)+# core electrons(0.85)
What is an Isoelectronic Series
A series of two or more species that have identical electron configurations, but different nuclear charges.
IE generally decreases down a group and increases going left to right across a period.
Excetion: When new subshells are occupied, the IE is lower; half-filled shbshells are particularly stable
what are some exceptions
Group 1 (ns1)--> more negative vs Group 2 (ns2)
and Group 4 (ns2np2)--> more negative vs Group 5 (ns2np3)