Chapter 6- Electronic Structure & Periodic Table Flashcards
electromagnetic radiation
radiation consisting of electric and magnetic waves that travel at the speed of light
wavelength
- distance between two consecutive peaks in a wave
- unit: m
frequency
- number of waves (cycle) per second that pass a given point in space
- unit: 1/s = hertz (Hz)
- frequency = speed of light (c)/ wavelength
Max Planck’s Quantum Theory
- light must be emitted and absorbed in discrete amounts
- light was before considered as a continuous electromagnetic wave
Equation for light
- E = hv
- h = 6.63 x 10^-34 J-s
v = frequency
de Broglie’s wave equation
wavelength = h / mv (mass x velocity)
Lyman’s Series
- results in ultraviolet emission of lines
- electron goes from n>=2 to n=1
Balmer series
- results in visible emission of lines
- electron goes from n>=3 to n=2
Paschhen series
- results in infrared emission of lines
- electron goes from n>=4 to n=3
Brackett series
- results in infrared emission of lines
- electron goes from n>= 5 to n=4
Schrodinger Equation
predicts analytically and precisely the probability of events or outcome, predicts the probability of finding the particle
Heisenberg Uncertainty Principle
it is impossible to calculate both the momentum and the speed of an electron in an atom, only possible to calculate the probability of finding an electron
orbital
indicates electron’s probable location
node
an area of an orbital having zero electron probability
ground state
lowest possible energy state of an atom or molecule
excited state
any state of a particle or system of particles that has a higher energy than that of its ground state
Pauli Exclusion Principle
no two electrons can have the same set of four quantum numbers
Aufbau Principle
electrons fill orbitals starting at the lowest available energy state before filling higher states
Hund’s Rule
single electron with the same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbital
paramagnetic
- atom has unpaired electrons
- attracted to a magnetic field due to unpaired electron
diamagnetic
- all electrons are paired
- weakly repelled by magnetic fields
principal quantum number (n)
as n increases, the orbital becomes larger- electron has a higher energy level and is less tightly bounded to the nucleus
angular momentum number (l)
- values from 0 to n-1
- defines shape of orbitals
- 0 is S. 1 is P, 2 is D, and 3 is F
magnetic quantum number
- determines orientation of orbital
- values from -l to +l
spin quantum number
either -1/2 or +1/2
atomic radius
- increases as you move down
- decreases as you move right
shielding effect
lessening of attractive electrostatic charge difference between the nuclear protons and valence electrons by partially or fully filled inner shells
effective nuclear charge
attractive positive charge of nuclear protons acting on valence electrons
anion radius
- larger than respective atoms
- electron electron repulsion forces them to spread further apart
cation radius
- smaller than respective atoms
- less electron electron repulsion, come closer together
first ionization energy
energy required to remove the most loosely bound electron from a neutral atom in its GASEOUS state
ionization energy
- decreases as you move down (larger atomic radius)
- increases as you move right (smaller atomic radius)
electron affinity
- energy released when an atom gains an electron and becomes a negative ion
- decreases as you move down (atomic radius increases)
- increases as you move right (atomic radius decreases)
- greater electron affinity = more negative
