Atomic Structure

higher frequecy = ? wavelenght

Shorter wavelength

higher frequency = ? energy

Higher energy

higher wavelegthn = ? energy

Lower energy

represent each itema s the correct letter

• speed

• energy

• frequency

• planks constant

• c

• E

• v

• h

what si th ephoto electric effect

The photoelectric effect is the phenomenon where electrons are emitted from a material when it is exposed to light of sufficient frequency.

what must happen for electros to escape a surface?

the energy of th eshining light must overcome the threshold of the material

Photoelectrict effect: as wavelength decreases

energy increases and you ebcome closer to overcming the threshold

Photoelectrict effect: how many photoelectrons are mmited from the surface for every electorn?

one

Photoelectrict effect: what happens of the energy of the light or photon is greater tan the threshold?

the excess energy is tunred into kenetic energy and speed up the mitted photelectron

Photoelectrict effect: what heppns if the intensity/brightness increases?

more photoelectrons are emmited

Photoelectrict effect: how do you fidn the kenetic energy of an emited electorn?

manipulate the energy of a photon equation and other basic equations

is inoization absoption or emmision?

absorption

what happens in emission vs absoption

emmision: the release of energy by an atom, resulting in the emission of a photon (light, colours ect.)

absorption: the process where an atom takes in energy and promotes an electron to a higher energy level.

a sample is excited and produces a coloured flams, thi woulld be an example of?

emission

when a mlecule of sunscreen absobs radiation, the molecule is ionized

false

ionized = removal of electron

does have a transition but doesnt necessarily lose and elctron

what si the wave particle duality?

particels have wavelike properties

wvaes have particle like properties

do small particles have large or small wavelenghts?

large

what is defraction?

when radiation adn object psacing are similar. we will usually look at how close the wavelengths are. This allows us to find the wavelenght of of a particle like a photoelectron

what are orbitals

regions where there is a high probabaility of an electron being. 3 quantum numbers describe it

what does n describe in quantum numbers?

• orbital eneergy

• priciple shell

what does (fancy) L describe in quantum numbers?

• orbital shape

• number of subshelss

• n-1

• 0=s, 1=p, 2=d, 3=f

what does m (little l) describe in quantum numbers?

• orbital oreintation

• -facy L , 0, to positive fancy l

• you can ahve as many as 2(fancy) L +1 numbers values for m

s orbitals

spherical

p orbitals

1 angular node where you can not fidn the electorn

only possible with nis greter than or equal to 2

looks like 2 bubbles

3 types of p orbitals: px, py, pz.

d orbitals

2 angular nodes where you cna find electorns

only possible when n is greater or equal to 3

looks like 4 bubbles and sometimes a bit more weird

5 types of d orbitals: dxy, dyz, dzx, dx2-y2, dz2.

what does it mean when we say hydrogen subshells are degenrate?

the subshelss have the same energies

what does ht eleectrom spin quantum number tell us?

the generating megnetic field, +1/2 or -1/2

if electron are paried they have no spin since they cancle out

whata re atoms / ions that have all spins paried called?

diamagentic

what are atoms with uncpaired electrons called?

paramagnetic

if an atom is in an excited state what happens ot its configuration?

an electron would move to higehr orbital

most halogens/gasses have their last few eelectron in which orbital?

p orbital

transitions metals have most of thier valence leectron in which orbital?

d orbital

most alakli mtals have thier valence electrons in which orbital?

s orbital

helium has its valence electrons in which orbital?

s orbital

last bottom row ont he periodics table has its valence electrons in whihc orbital?

f orbital