Arrangement of Electrons in Atoms (Honors Chemistry)

electromagnetic radiation

energy that exhibits wave-like behavior as it travels through space

electromagnetic spectrum

all forms of electromagnetic radiation, which all move at a constant speed (the speed of light).

the speed of light (c)

3.00 x 10⁸ meters per second (m/s)

wavelength (λ)

the distance between corresponding points on adjacent waves

meters (m) / nanometers (nm)

how wavelength is measured

frequency (ν)

the number of waves that pass a given point in a specific time

hertz (Hz) / 1 wave per second

how frequency is measured

c = λν

the relationship between frequency (ν) and wavelength

inversely proportional

as one value goes up, the other goes down (ex. wavelength and frequency)

photoelectric effect

the emission of electrons from a metal when light shines on it

quantum

the minimum amount of energy that can be lost or gained by an atom

Planck's constant (h)

6.626 x 10⁻34 J*s (joule-seconds)

energy (E)

measured in J (joules)

E = hν

the relationship between a quantum of energy (E) and the frequency of radiation (ν)

directly proportional

as one value goes up, the other does as well (ex. energy and frequency)

photon

a particle of electromagnetic radiation with zero mass carrying a quantum of en energy

ground state

the lowest energy state of an atom

excited state

a state higher than the ground state of an atom

photon emission

occurs when an electron drops from a higher energy state to a lower one

photon absorption

occurs when an electron rises from a lower energy state to a more excited one

electron orbital

the three-dimensional space where an electron is found 90% of the time

electron shell

an energy level representing the distance of an electron from the nucleus of an atom.

electron sublevel

grouping of orbitals found within an energy level; s, p, d and/or f

s sublevel

spherical, holds 2 electrons, only 1 type

p sublevel

dumbbell shaped, holds 6 electrons, 3 types

d sublevel

clover shaped, holds 10 electrons, 5 types

f sublevel

complex, holds 14 electrons, 7 types

electron configuration

describes the arrangement of electrons in atoms at ground state (# on the left is the sublevel, exponent is the # of electrons)

noble gas notation

an abbreviated electron configuration of an element in which filled inner shells are represented by the symbol of the noble gas before

orbital notation

a diagramic representation that uses dashes and arrows to show the principal energy levels and sublevels for all the electrons in an atom

Aufbau Principle

an electron occupies the lowest-energy orbital that can receive it

Hund's Rule

orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron

Heisenberg's Conclusion

determining the velocity and position of an electron simultaneously is impossible

Pauli's Exclusion Principlee

no two electrons have the same quantum number

quantum number

a number that describes the properties of atomic orbitals and the electrons in them

principal quantum number (n)

the energy level of the electron (only positive integers)

n²

the amount of orbitals in one shell

2n²

total electrons possible in one energy level

angular momentum quantum number (l)

indicates the shape of the orbital (0, 1, 2, or 3)

magnetic quantum number (mₗ)

indicates the orientation of the orbital (ranges from -l to l)

spin quantum number (mₛ)

indicates the spin of the electron (either 1/2 [↑] or -1/2 [↓])