Chapter 4 Pt.2 Test Flashcards
greek philosopher did experimenting of cutting object in half called this the atomus (model is round and plain) he dissappeared, along with his theories
Democritus
british
all matter is made up of atoms
all atoms of an element are exactly alike
they’re different than the atomus of any other element
matter is neither created nor destroyed in a chemical reaction
model of atom = spherical
Dalton
realized there are + and - charges in an atom
he believed the whole atom was solid w/ all positives
called “-“ charges, electrons
J.J. Thomson
propelled alpha particles through gold foil
some alpha particles went through, or bounced back
ATOM IS EMPTY SPACE
DENSE CENTER
ELECTRONS MOVE RANDOMLY AROUND NUCLEUS
Rutherford
it acts like a wave.
it reflects and refracts
light
what does every element produce when being burned?
light
when light is passed through a prism, it separates into what?
wave-lengths
these wavelengths are ….
discrete
unique pattern
german
in an element, light is given off or absorbed as packets of energy
packets are “quantized”
they come in different sizes
Max Plank
a fan has 3 speeds
fast food meals come in regular or extra large sizes
Analogies for Quantize
example: “slider” for brightness on ipad -
nonanologies
packet of light energy -
Quantum
Quantum’s also know as …
photons
who created the Quantum Theory?
Max Plank
Albert Einstein
every electron has a fixed orbit
every electron has a location
every orbit has a # of electrons
farther from nucleus the more energy it takes to stay in orbits
Bohr
normal location of an electron =
ground state
farther from nucleus…. the __________________ it takes to stay in orbit
more energy
can higher orbits exists even if there are no electrons located there?
yes
what happens at step one of energy levels?
photon hits electron
electron absorbs and absorbs energy
Step two:
electron absorbs energy
electron jumps to higher energy level
Step three -
unstable electron loses energy & returns to ground state
published Heisenberg Uncertainty Principle
said you can know electrons location&momentum, but not at same time -
Heisenberg
showed that u can calculate the probability of an electron being in a certain location
- don’t know exactly the location of electron
- you can know probability of area where it should be
Schrodinger and Born?
Quantum mechanical model… also known as -
wave mechanical model
Quantum mechanical model combines ideas from ….
scientists
Quantum Mechanical Model:
electrons are in the ______ ________.
energy level
Quantum Mechanical Model:
-limited _________ in energy level
electrons
energy levels have sub levels called …
orbitals
what are the 4 different quantities -
n
l
m
s
n = ?
which energy level?
L = ?
shape of orbital
m = ?
where on x & y axis?
s = ?
spin up or down
Principle Energy Level = ….
N
n describes how ______ an electrons orbit is from the _________.
far
nucleus
N can be divided into sublevels ….
L
sub level … = ….
orbitals
it’s the region of space where there is 90% chance of finding the electron -
orbital
orbital and orbits do NOT mean the same thing.
true
energy level # of orbitals Orbital Names
n= 4 L=4 4s 4p 4u 4f
n=1 L=1 1s
just example
every energy level (n) has same number of _________ (l).
orbitals
s goes with the ______ orbital
1st
p goes with the _______ orbital
2nd
u goes with the _______ orbital
3rd
f goes with the _______ orbital
4th
who did Einstein disagree with??
Heisenberg and Bohr
they held conferences. and there was a lot of tension between who?
Bohr and Einstein
S looks like a ….
sphere
p = “pinched” so looks like….
8
d = “down on the ground” =
four leaf clover
f = …
far too complicated
1s…
small
2s…
medium
3s…
large
Px =
8 going sideways (acrossed the x-axis)
Py =
8
how many orbitals in “d” orbital?
5
how many f orbitals are therE?
7
what orbital tells u the orientation in space of each orbitals -
m
what orbital tells u the spin of the electrons movement?
s orbital
1/2 -
up
-1/2 =
down
each orbital can hold no more than ________ electrons
2
electrons must have ___________ spin
opposite
one _______, and one _________.
up / down
electrons fill in orbitals starting at the lowest energy level
“electrons are lazy”
Aufbau Principle
place one electron in each empty orbital in an energy level before you add a second electron to that orbital -
Hunds Rule
no more than 2 electrons may occupy an orbital & must have opposite spins -
Pauli Exclusion Act
a maximum of ______ electrons may occupy a single orbital, but only if the electrons have __________ spins
2
opposite
Quantum Mechanical Model of the Atom =
electrons located in energy levels
electrons are located by 4 _________ ___________.
different quantities
limited # of ___________ per energy __________.
electrons
level
its the fixed amount of energy -
energy levels
what are the 4 quantum #’s -
n
m
l
s
define orbitals -
sublevels in energy levels
what is the relationship between the principle energy level and the number of orbitals -
n = l
what orbitals are present if n = 3
s3
p3
u3
what orbitals are present if n = 4
4s
4p
4u
4f
