The text delves into various concepts related to atomic properties and behaviors. It begins by explaining atomic structure and the differences between isotopes and radioisotopes, noting that radioisotopes can decay due to lower nuclear charge.
The electron affinity is the potential energy change of the atom when an electron is added to a neutral gas
shielding
The more electron shells there are, the greater the shielding effect
the shielding effect, describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell.
electron negativity
The tendency of an atom in a molecule to attract the shared pair of electrons towards itself
the closer you move to the top right corner of the periodic table the more electron negativity it has.
effective nuclear charge
increases when you move left to right on the periodic table
The Effective nuclear charge is the actual amount of positive charge experienced by an electron
ionization enrgy
increases when you move up and left to right on the periodic table
the minimum amount of energy required to remove the most loosely bound electron, the valence electron
atomic mass/number and isotopes
Each isotope of an element has an atomic mass. The average of all the atomic masses of an element's isotopes gives an element's atomic weight
The difference between isotopes and radioisotopes is that a radioisotope can decay because the isotope has less nuclear charge and protons escape
The atomic number and atomic mass can be used in equations to find the unknown one. To get the atomic mass is neutrons + atomic number and to get atomic number is neutrons - atomic mass
