Chem H units 3-4

electrons, PT trends

Coulomb’s law

the Force of attraction (f) between 2 charged particles depends on the individual charges (q1 q2) and the distance (d) between them

Coulomb’s law equation

F=q1xq2/d squared

Electromagnetic spectrum (low nrg to high)

Radio, Micro, IR, ROYGBIV, UV, Xray, Gamma Ray

Wavelength

distance between crests of a wave

Frequency

number of waves that pass a point per second

How to find speed of light ( c)

c= wavelength x frequency

As wavelength increases, energy…

decreases

as wavelength decreases, frequency…

increases

continuous spectrums

all wavelengths present

line spectrum

only some wavelengths present

Emission Spectrums

made when elem exposed to electricity/uv light.

Emission Spectrums: what do electrons do

Electrons jump to a higher n where it is unstable. Then release nrg as photons (light) and drop down to lower level. The farther they drop down, the more nrg released, the higher nrg light produced.

Drops to n 1

Uv light

drops to n2

visual light

drops to n3

IR light

Different types of orbitals

s,p,d,f

how many electrons in each orbital

2 with opposite spins

how many s orbitals on each n

1

N

energy level abbr.

F

force of attraction (between proton and e-)

NC

Nuclear charge abbr.

how many p orbitals on each n

3

how many d orbitals on each n

5

how many f orbitals on each n

7

allowed orbitals on n1

s

allowed orbitals on n2

s, p

allowed orbitals on n3

s,p,d

allowed orbitals on n4

s,p,d,f

hund’s rule

every orbital in a sublvl needs one e- before you can pair them.

Orbital type for group 1a,2a

s

Orbital type for group 3a - 8a

p

Orbital type for transition metals (10 middle columns)

d

Orbital type for inner transition metals (bottom 14)

f

filling order strat

do the diagonals

filling order exceptions

chromium, copper.

most stable n lvls (explains exceptions for filling order)

half full or full

Transition Metal ions

lose electrons from s sublevel before d sublevel

group

vertical columns. similar properties

period

horizontal rows. same n

metal properties

conductive, shine, malleable, ductile, cations

nonmetal properties

not conductive, dull, brittle, gases at room temp, anions

metalloid location

On the staircase

metalloid properties

both metallic and non metallic

alkali metals

group 1a

alkaline earth metals

group 2a

halogens

group 7a

noble gases

group 8a

valence electrons

e- in the highest n. Furthest away from nucleus. Involved in chemical bonding

core electrons

Inner e-. basically NOT valence

nuclear charge (NC)

number of protons. Positive charge attracting the e-

Energy level (n)

different lvls that e- can exist on. Higher lvls are farther away from the nucleus.

atomic radius

distance between nucleus and outermost electron

atomic radii trend ACROSS

radii decreases

atomic radii trend DOWN

radii increases

Electronegativity

how much an element attracts electrons when bonding

electronegativity trend ACROSS

EN increases

electronegativity trend DOWN

EN decreases

ionization energy (IE)

energy required to remove a valence electron from a gas

IE trend ACROSS

ie increases

IE trend DOWN

ie decreases

successive IE

energy required to remove successive e-. each one is bigger than the last. core e- requires way more successive IE.