Notes from slides Flashcards
What happens to the distance between orbits from the nucleus
The distance between orbits decreases with distance from the nucleus
What happens to the energy as the distance increases from the nucleus
more energy
Name the waves on electromagnetic spectrum
gama, X ray, UV VBGYOR IR micro radio
highest to lowest energy
short to long wavelength
Rank the subshells in order of their energy
s < p < d < f
Does subshell s have multiple orientations
No, all other except for s do. they can exist in x y z plane
How many electrons in each orbital
2, spins up and down
What are three rules for electron filling in an atom
Pauli principle - describes the carrying capacity of orbitals. No two electrons can be identical. This limits the occupancy to max of 2 electrons
Aufbau principle - electrons are added to orbitals from lowest to highest energy . electrons are removed from valence orbitals first with highest to lowest energy
Hund’s rule - electrons fill degenerate orbitals one per orbital before pairing. paramagnetic and dimagnetic.
According to Aufbau principle, what are the rules to fill electrons in subshells 4s and 3d
Even though 3d is higher in energy than 4s, the valence electrons are removed from 4s first before 3d.
What are the rules for excited state electron configurations
make sure the configuration has the correct total number of electrons
the electrons can be in any orbital as long as that orbital exists.
Difference between the Aufbau principle and Hund’s rule
Aufbau principle describes how electrons are added/removed from orbitals of different energy however Hund’s rule describes how electrons are added/removed from the orbitals of the same energy
Half filled/fully filled orbitals are higher in energy?
false, lower in energy
Define paramagnetic
at least one unpaired electron
Define diamagnetic
all the electrons are paired
What are the 7 element groups
group 1 - alkali metals
group 2 - alkaline earth metals
group 7 - halogen
group 8 - noble gases
the d block - transitional metal
the s and p blocks - representative elements
the f block - rare earth metals
Describe the shielding effect
core electrons shield the valence electrons from the full nuclear charge
more core electrons, less attracted the valence electron is to nucleus
What is effective nuclear charge
the nuclear charge experienced by a valence electron
moving down a group, what happens to electrostatic force (F e), size and nuclear charge (Z eff)
F e decreases, Z eff is constant because core electrons are added at the same rate as protons, r increases
moving across a period, what happens to electrostatic force (F e), size and nuclear charge (Z eff)
F e increases, size remains constant, Z eff increases because core electrons remain constant while protons are added.
moving from positive to negative charge, what happens to electrostatic force (F e), size, charge (C) and nuclear charge (Z eff)
F e decreases with increasing negative charge, C becomes negative, size doesnt change much, Z eff remains constant because core electrons and protons remain the same
Atomic radius moving from left to right
decreases (Fe increases)
Atomic radius form top to bottom
increases
How does ionic radius change with charge
ionic radius increases with negative charge
Ionization energy
minimum amount of energy required to remove the outer most electron from an atom in its gaseous state. depends on F e
left to right, ionization energy
F e increases so IE increases
Top to bottom, ionization energy
Fe decreases, IE decreases
What are the rules for multiple ionizations
- more positive charge on an ion (cation), more ionization energy
- second IE is greater than first IE
- pulling off electron from a half full/full orbital require more IE
Define electron affinity
energy change when adding an electron to valence shell of an atom in its gaseous state. exothermic. More Fe, more energy is released
Electron affinity left to right
F e increases left to right, more negative because more energy is released
Electron affinity top to bottom
Fe decreases top to bottom, therefore less negative EA because less energy is released.
Electronegativity and Fe
As Fe increases ENV increases, from left to right and bottom to top
Pneumonic for ENV
FONClBrISCH
acidity from left to right
as stability increases of the anion (conjugate base) produced increases, the acidity increases. as the size of the anion increases, the stability increases. Left to right, size increases and acidity also increases
Acidity top to bottom
top to bottom the size increases and so does the acidity
