Midterm Review: Random Shit Flashcards
states that building up the e- configuration of an atom. e-(s) are placed in orbitals, subshells, and shells in increasing order of energy
Aufbau Principle
states that the two e-(s) which share an orbital cannot have the same spin. one e- must spin clockwise, and the other must spin counterclockwise
Pauli Exclusion Principle
when an e- is added to a subshell, it will always occupy an empty orbital if one is available. e-(s) ALWAYS occupy orbitals singly if possible and pair up only if no empty orbitals are available
Hund’s Rule
based on e- configuration and how attractive an atom is to a magnet
paramagnetic
based on e- configuration and how PAIRED e-(s) are repelled by a magnet
diamagnetic
occurs when inner energy level e- (core e-) block some of the positive charge from the nucleus from reaching the outermost energy level
shielding
Z (effective) = Z (charge of nucleus) - S (core e-)
effective nuclear charge
the approximate distance from the nucleus of an atom to its valence e-
atomic radius
left to right in a period AR _______
decreases, p+ are being added but in the same shell
moving down in a group AR _______
increases, more shells of e-, more p+, but shielding cancels
cations are ______ than atoms
smaller; e- removed cause outer shell to be lost; e- lost = less repulsion
anions are ______ than atoms
larger; e- being added, valence being added; e- replusion increases
same as AR but metals differ from nonmetals; deals w/ cations and anions; cations are smaller while anions are larger
ionic radii
the same as binding energy; the energy required to remove an e- from an atom
ionization energy (IE)
moving across a period, IE _______
increases; p+ added to nucleus, valence e- more attracted, takes more energy
down a group IE ________
decreases; shells of e- are added, inner shells shields the distant ones, reducing pull; p+ being added but shielding cancels the p+
why is the second IE greater than the first?
e- removed causes repulsion to decrease and increase attractiveness of p+ to valence e-
as e- are being removed, IE increases 1. _______ until the shell is 2. _____, then makes a 3. _____ jump
- gradually
- empty
- big
when the valence shell is empty, the next e- must come from a shell much _____ to the nucleus; IE is larger than the previous one
closer
refers to how strongly the nucleus of an atom attracts the e-(s) of other atoms in a bond
electronegativity
electronegativity is affected by 2 factors
a) the 1. ______ the atom, the more effectively its 2. ______ _______ will be felt past its outer energy level
b) the 3. _______ the atom is to having 4. ___ energy level the more likely it is to 5. ________ the necessary e- to complete that level
- smaller
- nuclear charge
- closer
- full
- attract
left to right across a periodic table, EN ______
increases
down a group, EN _______
decreases
the amount of energy that an e- has depends on its distance from the atom
coulomb’s law
the greater the charge of an atom, the more energy it will have (e- have the same amount of charge)
basically coulombic potential energy is considered to be at 0 for a distance infinity, PE of 1s (more negative) brings the CPE to zero unlike 3s
for an e- to move from an energy level close to the nucleus to an energy level far from it needs to ______ energy (takes energy)
gain
for an e- to move from an energy level far away from the nucleus to an energy level close to it needs to ______ energy (easy to do)
lose
why can’t a single atom of hydrogen produce all four spectral lines simultaneously
a single atom of hydrogen cannot jump b/c it can’t get to the rest. it can only jump once and show one color
