chem unit 3/4

cations became what when forming ions

smaller

anions become what when forming ions

larger

valence electrons

electrons in the outermost shell of an atom

frequency and wavelength are

direct

frequence and energy are

inverse

paramagnetic species

free electrons (attracted to magnetic forces)

diamagnetic species

no free electrons (not attracted to a magnetic field)

metals are

cations

nonmetals are

anions

atomic radius

size of an atom

why does atomic size increase going down

you gain electron shells

why does atomic radius go down going down a period

because there are more protons in the nucleus, which attract electrons further in

ionic radius

the center of the nucleus of an ion to its outermost electron shell

what does ionic radius do

decreases as atomic number increases

ionization energy

the energy required to remove an electron from the atom

where are electrons always removed

the outermost electron shell

how does ionization energy increase

going up and right

how does stability increase

going up and right

how does reactivity increase

going down and left

electronegativity

the ability of an atom to hold electrons

how does electronegativity increase

going up and right

properties of metals

shiny, malleable, ductile, good conductors of heat and electricity

nonmetals

dull, poor conductors

metalloids

semiconductors, properties of both

s sublevel

2

p sublevel

4

d sublevel

10

f sublevel

14

group 1

alkali metals

group 2

alkaline earth metals

d block (middle elements)

transition metals

group 17

halogens

group 18

noble gases

f block (top row)

lanthinides

f block (bottom row)

actinides

isoelectronic species

the element and ions have the same number of electrons

ionic radii

increases with negative charge and decreases with positive charge

1st energy level

up to 2 electrons

2nd energy level

up to 8 electrons

3rd energy level

up to 18 electrons

4-7th energy levels

up to 32 electrons

orbital

most likely place an electron can be found, can hold 2 electrons

aufbau principles

electrons fill orbitals from the least to greatest amount of energy

hunds rule (bus rule)

when electrons fill orbitals of equal energies, they fill one at a time before pairing up

pauli exclusion principle

when electrons fill the same orbital they rebel and move in opposite directions

frequency

how often a wave cycle passes a given point per second

wavelength

the distance from one wave cycle to the nextv

visible light

400-700 nm

under 300 nm

infrared, microwaves, radio waves

above 700 nm

ultraviolet, x-ray, gamma rays