UNIT 3, waves and electron configurations

What is the Heisenberg uncertainty principle

states that it is impossible to know both the speed and position of a electron at the same time

what did schrodingers equations use to predict possible electron locations?

probability

What do schrodingers equations allow us to determine?

the shapes of the electron clouds or orbitals, where we will find electrons

what was not true about electrons orbital as bohr thought?

electrons do not travel around the nucleus in neat rings as bohr thought, instead they exist in certain regions called orbitals

what is an orbital?

a 3D region around a nucleus that indicates the probable location of an electron

Bohr model represents:

energy levels that electrons revolve around a nucleus

quantum theory :

circular lines on a bohr model represent 90% probability of finding an electron ( not orbit of electron)

what is electron configuration

describing where the electrons can be found around a nucleus

each element has its own unique __

electron configuration

there is a place for what in every atom

every electron

what does defining the area where an electron may be found do?

it is a cumulative process and builds as the number of electrons increase from one element to another

what are the 3 components of electron configurations?

• principal quantum number (n) or energy level

• energy levels are made of sublevels

• the superscript

explain the first component (n) - principle quantum number

• relates to the size and energy of the energy level

• n=1,2,3,4,5,6,7 (7 rows, so 7 energy levels ) n=1 IS THE CLOSEST TO THE NUCLEUS

• the principle number corresponds to the period on the periodic table

• the lower the number, the closer to the nucleus and LESS ENERGY

explain the 2nd component, energy levels are made of sub levels

• s, p ,d ,f, which describe its shape

• s= sphere , 1 orbital, hold maximum of 2 electors

• p= peanut , 3 orbitals, hold maximum of 6 electrons

• d= daisies, flowers , 5 orbitals, hold maximum of 10 electrons

• f= flowers with more petals , 7 orbitals, holds maximum of 14 electrons

• EACH ORBITAL MAY HOLD A MAXIMUM OF 2 ELECTRONS

explain the 3rd component, the superscript

• above the sub level letter

• indicates the number of electrons in each orbital

aufbau principle

the orbitals of Low energy are filled first with electrons and only then the orbitals of high energy are filled

pauli exclusion principle

when 2 electrons are in the same orbital they follow this principle. It states that only electrons with opposite spins can occupy the same orbital. we represent this with arrows pointing int he opposite directions

Friedrich hunds rule

an electron must be added to each orbital before the second electron is added ( so like Pauli’s except one up arrow in every orbital first then fill in with down arrows)

what are valence electrons

the outer most principal quantum level of an atom ONLY THE LAST RINGS

what are the core electrons

everything but the valence electrons

how do you do noble gas configuration

fill out the noble gas for the element in brackets and fill out all the energy levels after that noble gas NOT JUST VALENCE, EVERYTHING FROM NOBLE GAS TO THE ELEMENT INCLUDING THE ELEMNENT

• BASED OFF OF RINGS NOT LETTERS LIKE S P D F ITS BASED OF 1 2 3 4 5 6 7

What is the exception to the aufbau principle

you don’t have to filll up an energy level because you must take out an electron and add it when we have d4 and d9 to make it stable.

what is the constant for speed

3.00 × 10^8 m/s

what is the equation for speed

speed (m/s) = frequency - v (hz) x wavelength (m)

****WAVELENGTH IS ALWASY IN METERS

how many nanometers in a meter?

a billionnnnn ( 1×10^9)

what is electromagnetic radiation?

a type of energy that exhibits wavelike behavior as it travels through space.

• together, all of the forms of it from the electromagnetic spectrum

parts of a wave:

trough = local minimum

crest = local maximum

wavelength = space between 2 troughs or 2 crests METERS

as frequency of light increases wavelength of the light

decreases

as frequency increases, energy___

increases

as wavelength increases, energy ___

decreases

Higher energy levels are ____

further from the nucleus

what must an electron do to go to a higher energy level?

gain energy (absorb light energy)

what must an electron do to come back to ground state

emit that absorbed light energy to come back, so it actually loses energy while projecting a specific wavelength of light, giving it a color

what is light made out of

photons

photons interact with metals in?

metal like particles rather than a wave

energy is measured in :

joules

what is the constant of Planck ( h)

6.626×10^-34

why is the first energy level not always the ground state?

Because not all electrons are always in the first energy level boi

how can you tell whether its in ground or excited?

if an energy level isn’t full yet and theres still electrons in other energy levels = excited state bro is on a trampoline so it jumps in the ring of get air

define a photon

a discrete bundle of electromagnetic energy. photons are ALWASY in motion and in empty space have constant speed of light to all observers. they have zero mass and are NEUTRAL

• all electromagnetic energy is made is of photons

what is the unique characteristic of light?

behaves like both a wave and a particle at the same time

what happens to an orbiting electron when it gets hit by a photon?

It jumps to the excited state (cause it absorbs the light )

what must happen for the electron to return back to the first energy level?>

lose energy and emit the light absorbed

relationship between energy absorbed and the number of energy levels jumped?

direct, more energy absorbed = more energy levels jumped