chem unit 3 - quantum theory

who was the father of the periodic table

mendeleev

how did moseley correct the periodic table

he rearranged the elements by atomic number

what are the 2 terms given for vertical columns

family and group

horizontal rows are called

periods

group A elements are called

representative elements

group B elements are called

transition metals

the main 3 groups of elements are

metals, metalloids, non-metals

group I-A

alkali

group II-A

alkaline-earth

group VII-A

noble gas

group VIII-A

halogens

the inner transition metals are also called

lanthanides and actinides

atomic radius

size of the atom

the atomic radius increases which way

down and left

ionic radius

size, electrons repell each other

adding an electron makes the atom

bigger

removing an electron makes the atom

smaller

ionization energy

the energy needed to pull and electron away from the nucleus

the ___ away an electron is from the nucleus the easier it is to pull away

farther

group 1 will lose electrons __

easily

an atom with a ____ will need more energy

full shell

electronegativity

the ability of an atom to attract an electron when the atom is in a compound, opposite of ionization energy

electronegativity _____ when you move down

decreases

electronegativity _____ when you move to the right

increases

speed of light equation

C=Av

energy equation

E=hv

C stands for

speed of light

E stands for 

energy

C is measured in

m/s

E is measured in

joules

A stands for

wavelength

A (wavelength) is measured in

meters

v stands for

frequency

v (frequency) is measured in

Hz/1/seconds

C (speed of light) equation is

3.0 × 10^8

h equations is

6.626 × 10^-34

h is measured in

joules x seconds

wavelength and frequency is 

inverse

frequency and energy is

direct

wavelength and energy is

inverse

what is the far left group

S

what is the middle group

D

what is the far right group

P

what is the bottom group

F

how many electrons can block S hold

2

how many electrons can block D hold

10

how many electrons can block P hold

6

how many electrons can block F hold

14

how many orbitals are in block S

1

how many orbitals are in block D

5

how many orbitals are in block P

3

how many orbitals are in block F

7

d block =

n-1

f block =

n-2

aufbau principle

electrons occupy the lowest energy level possible (closest to the nucleus)

hunds rule

electrons will occupy each orbital with the same spin (direction) before occupying an orbital with a different spin (direction)

pauli exclusion principle

no two electrons can have the same quantum number, they must be traveling opposite directions if they are in the same orbital 

heisenberg uncertainty principle

it is impossible to know precisely both the position and the momentum/speed of an electron