Chem Sat- Atomic Structure/periodic Table

Front 1

Dalton's theory

Back 1

all matter is made of atoms

all atoms of the same element have the same mass

atoms can't be divided/destroyed

atoms combine in whole number ratios

you can't destroy or make an atom in a reaction they only get rearranged

Front 2

how to figure out how many electrons are in each energy level

Back 2

2n^2

n=energy level

Front 3

Protium

Back 3

H 1/1

Front 4

Deuterium

Back 4

H 2/1

Front 5

Tritium

Back 5

H 3/1

Front 6

Calculating average atomic mass

Back 6

69.17% Cu63
30.83% Cu65

(.6917)(63)+ (.3083)(65)=63.5 AMU

Front 7

Where are the metals?

Back 7

to the left of the willis

Front 8

Where are the nonmetals?

Back 8

to the right of the willis

Front 9

When electrons move up....

Back 9

they absorb energy

Front 10

When electrons move down....

Back 10

they emit energy (in the form of photons)

Front 11

Lyman series

Back 11

electrons that fall from any level down to level 1 are within the lyman series (ultraviolet light)

Front 12

Balmer series

Back 12

electrons that fall from any level down to level 2 are in the balmer series (visible light)

Front 13

Paschen series

Back 13

electrons that fall from any level down to level 3 fall within the paschen series (infrared)

Front 14

Visible light spectrum

Back 14

ROYGBIV

R= long wavelength small frequency

V= Short wavelength high frequency

Front 15

Electromagnetic spectrium

Back 15

GXUVIMR

G= High frequency short wavelength

R= Low frequency long wavelength

Front 16

spdf

Back 16

s=2
p=6
d=10
f=14

Front 17

Pauli exclusion principle

Back 17

in each orbital you can't have 2 electrons spinning the same way- only 2 electrons fit in each orbital

s has one orbital= 2 electrons
p has 3 orbitals= 6 electrons
d has 5 oribtals= 10 electrons
f has 7 orbitals= 14 electrons

Front 18

Aufbau

Back 18

an electron will always occupy the lowest energy level first

it always goes to the s first

Front 19

Hund's rule

Back 19

orbitals will fill by filling the lower energy levels first

Front 20

D block funky rules

Back 20

in the d block it's either full, empty, or half full

The d block steals or gives electrons to its s block to achieve this

Front 21

Mendeleev

Back 21

made the first periodic table

Front 22

Moseley

Back 22

stated that properties of elements are a periodic function of their atomic numbers

Front 23

Atomic radius periodic trends

Back 23

Increases going down
Increases going left

Fattest element is in the bottom left corner

Front 24

Electronegativity trends

Back 24

increases going up
increases going right

the most electronegative is Fluorine (top right)

Front 25

Ionization energy trends

Back 25

increases going up
increases going right

the hardest to ionize (remove a valence electron) are the noble gasses in the top right corner

Front 26

Ionic radius

Back 26

radius of the atom when its an ion (when its reacted with something else to become the ion)

ex. NaCl vs. Cl

the CL in NaCl is bigger b/c it gained an electron to bond with Na