Ch 6 Atomic Structure

Frequency/Wavelength equation

v = c/λ

Energy/Frequency relation

E = hv

Equation for energy of an electron at base state

E = -R/n²

Equation for energy absorbed/emitted by an electron

E = -R/(1/n_f² - n_i²)

Planck’s constant

h = 6.626 × 10^-34 J/Hz^-1

Ryberg’s constant

2.179 × 10^-18 J

Ionization energy of an atom

Energy required for an electron to jump to nth shell as n → ∞

Quantified Energy

For an electron to jump to some higher energy level, you must add at least enough energy

(think of this like a floor function for what shell it can be in)

wave/particle duality

all small particles may behave as waves when not observed and as particles when observed

Heisenberg uncertainty principle

it is impossible to determine both the position and velocity of an electron or any other particle in motion with any great degree of certainty

An electron in an orbital has __ quantum numbers which tell you its probable position

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quantum number n

range of [0, ∞)

Tells you the relative distance and energy level of an electron from the nucleus

quantum number l

range of [0, n-1]

tells you the type of sub-shell an electron is in

quantum number m_l

range of [-l, l]

tells you the orientation of the orbital of an electron

quantum number m_s

always either -1/2 or +1/2

tells you if the electron is spinning up (positive) or down (negative)

node

region within an orbital where the probability of finding an electron is 0

each subshell has __ orbitals

l = 0 → 1 (1 s orbital)

l = x → l(x-1) + 2

*recursive definition

there are __ orbitals in the nth shell

n²

AKA Σ_i=0^n-1 nsub(i) where nsub(i) is the number of orbitals in that subshell

__ electron(s) can have the same 4 quantum numbers in an atom

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