Final Exam Review Section 2

Zeff = (# of protons) - (# of core electrons) Remains constant as we move down in Groups Increases by 1 as we move L->R in periods

As we move left to right Radius decreases As we move down radius increases

Cations: (+) charge - radius is smaller Anions: (-) charge - radius is larger

series of elements with same # of electrons O^(2-) F^(1-) Ne Na^(1+) Mg^(2+)

Increases as we move down the table Decreases as we move left to right on table Anions are more polarizable than cations

energy required to remove an electron from atom (g) Al (g) –> Al+(g) + e-

Moving left to right the ionization energy will increase Moving down the ionization energy will decrease

Group 2 has greater IE than Group 13 Group 15 has greater IE than group 16

energy change when electron is added to neutral atom (g) X (g) + e- –> X- (g)

Moving from left to right EA will increase Moving down the EA will decrease

3p elements have greater EA than 2p elements In group 2 EA increases as you go down group In group 15 EA increases as you go down group Noble gasses have EA that’s equal to zero Group14 has greater EA than group 15

Increases from left to right on PT Decreases moving down on PT F is most EN and Cs is least EN

a. fill subshells in order b. completely fill subshell before moving to next c. any single orbital w/ two electrons must spin opposite d. place one electron in each orbital first all with same spin, then fill orbitals with opposite spin

Chromium, Molybdenum, Copper, Silver, & Gold

When an atom absorbs energy it sends electron from a lower subshell to a higher one -Change in energy will be positive (ENDO)

When an atom emits energy it sends electron from a higher subshell to a lower one -Change in energy will be negative (EXO)

-n -1 to infinity -Energy level and the size of electron shell

-l -0 to (n-1) -type of subshell & the shape of the orbital

-ml - from -l to +l -number of orbitals in subshell

-ms - (-1/2) to (+1/2) -direction of electron spin

States that no two electrons within in atom can have the same set of 4 quantum numbers

Orbitals are filled from lower principal quantum number (n) values to higher (n) values

In an excited state, electrons will move from a lower energy subshell to a higher energy subhell