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Text Elements
energy
highest
waves
1
2
Lithium:
Helium:
energy
3.0 x 10^8 m/s
wavelength
frequency
higher
inverse
increases
direct
visible light
infrared
range
specific
individual
wavelengths
photons
absorbing
ground
releasing
Ultraviolet
emitted
metals
electrons
ground state
visible
7
shells
Charlotte
Electron cloud
neighborhood
energy levels
orbitals
your street
your house
electron
4
3
period = energy level
1
2
3
6
doubledumbell
5
10
sphere
flower
7
probability
2
subshell
orbitals ^MP32DvUv
Total e
orientations ^OiXB9ljv
s
1
3
2
6
p
d
5
10
f
7
14
address
overlap
4th
S
Energy level 3 sublevel p
1s
2
2s
2
3s
2
2p
6
3p
4
< - address of sulfur
2+2+6+2+4 = 16
16 electrons is correct so i did it right
1s
2
2s
2
3s
2
2p
6
3p
4
K
1s
2
2s
2
3s
2
2p
6
3p
6
4
4s
1
1s
2
2s
2
3s
2
2p
6
3p
6
4
4s
1
Ti
is formula for potassium
1s
2
2s
2
3s
2
2p
6
3p
6
4
4s
2
3d
2
2+2+6+2+6+1=19
is formula for titanium
2+2+6+2+6+2+2
= 22
1s
2
2s
2
3s
2
2p
6
3p
6
4
4s
2
3d
2
Valence electrons: Highest level ( 1 - 7 ) S sublevel and p ( sometimes just S ) ( highest level S and P ) for titanium ( NO D ) in this case your highest level is 4s^2 and your valence electrons are 2 for sulfur its 3s^2 and 3p^4 so its 4 + 2 = 6 for potassium its 4s^1 so its got 1 valence electron
Warmup: Nitrogen ( N ) Chlorine ( Cl ) Iron ( Fe )
N
1s
2
2s
2
2p
3
1s
2
2s
2
3s
2
2p
6
3p
5
Cl:
Fe:
1s
2
2s
2
3s
2
2p
6
3p
6
4s
2
3d
6
N:
5 valence electrons
7 valence electrons
2 valence electrons
mrs wotts does this before she does an orbital diagram:
s p d f
Sublevel
orbitals ^wD83VylW
1
3
5
7
4 electrons in 2p
they do not pair unless they have to they dont wanna sit together on the bus
spin
spin is designated with an up or down arrow
1s
2s
2p
1s
2s
2p
3s
3p
1s
2s
2p
3s
3p
4s
3d
noble gasses are group 18 ( or 8a ) are noble gasses. the reason they are noble ( or inert, meaning not reactive ) is because they have all the valence electrons they need and dont want anymore
[Ar] 4s2 3d10 4p5
[Ar] 4s2 3d6
[Xe] 5s2
Xe
Ar
As
Al
Atomic Radius
Electronegativity Defined as: Tendency of an atom to steal an electron when combining with another element
Ionization Energy
The Why:
atomic mass
patterns
atomic number
periods
groups
families
Atomic Number
Element Symbol
Average Atomic Mass
Nonmetals
same
least
1A or 1
reactive - most reactive
no
1
soft
Cesium
Rubidium
react violently and produce a base
2A or 2
less reactive but still reactive
no
2
7A or 17
nonmetals
salt former
salts
7
-1
8A or 18
2
8
no charge
have all 8 valence electrons
non metal
rare earth
radioactive
1+
2+
3+
3-
2-
1-
0
metals lose electrons and become cations ( + )
2
1
3
5
Across a period is left to right / right to left nuclear charge is increasing.
Down or up a group is vertically
+3 Li
10
Nuclear charge
Small -----------⇒ big
Across period ( left to R, R to L )
Energy levels going up
1
2
3
4
so does shielding
z
nuclear charge
increases
decreases
energy levels
nucleus
Li, K, Cs
Ba, Sr, Ca, Be
Na
increases
decreases
Defined as: The energy needed to remove the outermost electron from an atom
smaller
closer
electron shells
nucleus
Cs, K, Li
Be, Ca, Sr, Ba
Cl
increases
nucleus
decreases
shell
Cl, Br, I
positively
losing
gaining
negatively
protons
greater
electrons
weaker
1s
2
2s
2
3s
2
2p
6
3p
6
4s
2
3d
10
3p
6
5s
2
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