Unit 3 Chemistry

Continuous Spectrum

a unbroken range of frequencies, wavelengths. Happens when light from sun/ light bulb passes through prisim.

Balmer series

quantanized energy level transitions that give off visible light

crest

highest point of a wave

speed of light

speed of all electromagnetic radiation

quantized energy meaning

you can’t just stop in between, you have to stop in a certain point

ex: like an elevator, you can’t stop in between floors

trough

lowest point of a wave

ways to look at atoms location and movement

1) emission spectroscopy

2) ionization energy

electron light admission explanation

when electrons absorb heat, they get excited so the jump away from the nucleus

when they go back down is when the light is admitted

ion

a atom with a unequal amount of protons and electrons bc they gained or losses electrons

Cation

positive ion, when atom loses a electron

anion

negative ion, when a atom gains a electron

Photon

packet of energy with both particle and wave characteristics that travels at the speed of light. used in lasers for narrow wavelengths

High energy photons have…

short wavelengths

low energy photons have…

long wavelengths

atomic spectrum

light edmitted from heated elements through prisim. Lines of different colors separated by dark areas. This separation of colors indicates that only certain wavelengths of light are produced when an element is heated

lines in atomic spectrum mean…

there is a change in energy, electron drop

excited state

happens when atom absorbs energy, when an electron moves to higher state of energy. Less stable

when electron falls from excited state…

falls to a lower-energy state by emitting a photon of a specific energy. If the energy emitted is in the visible range, we see one of the colors of visible light

max number of electrons in energy level

2n²

sublevels

A group of orbitals of equal energy within energy levels. The number of sublevels in each energy level is the same as the principal quantum number (n).

ex: 2p, 3f, 4s, ect.

sublevel letters and order increasing energy

s,p,d,f

orbital

3 dimensional volume where electrons have highest probability of being found

ex: s, p, d, f

s orbital

sphere shape, most basic one and get progressively bigger as the number goes up

P orbitals

3 different types (x y and z axis) , looks like a balloon with tie in the middle

D orbital

looks like 4 leave clover, way weirder and 5 different types

F orbital

you dont need to know, 7 different orbitals

electrons per orbital

max 2, Pauli exclusion principle ( think arrows up and down )

orbital diagram

shows placement of electrons on orbitals with increasing energy

Hunds Rule

lowest energy state is attained when electrons are placed singly in available orbitals of the same sublevel with the same spin. fill up every orbital one by one before adding in more then one electron.

electron configuration

A list of the number of electrons in each sublevel within an atom, arranged by increasing energy.

valence electrons

electrons on the outer most shell, the same going down a group

atomic size

The distance between the outermost electrons and the nucleus

atomic size increases (group)..

going from the top to bottom, because the outer most electron shell is father from the nucleus, making it have less of a intense pull

atomic size increases(period)...

right to left because increase in protons means increase in positive charge, pulls in the electrons

Atomic size transition metals…

relatively the same because there is little change in the nuclear attraction for the valence electrons

ionization energy

The energy needed to remove the least tightly bound electron from the outermost energy level of an atom.

energy is required..

to remove a electron from a atom (more if closer to nucleus)

ionization energy decreases(group)…

going down the group because as those electrons are farther from the nucleus, attraction decreases

ionization energy increases(period)…

left to right, the positive charge of the nucleus increases because there is an increase in the number of protons.

metallic character

A measure of how easily an element loses a valence electron.

metallic character is more important..

on the left side of the periodic table, less so on the nonmetals because they do not easily loose electrons; less metallic

metallic character increases…(group)

top to bottom, more electron levels at the bottom making it easier to lose them

metallic character decreases…(period)

left to right, atoms gain more protons and a higher nuclear charge, pulling valence electrons closer and making it harder to lose electrons

frequency (v)

amount of waves that pass through a observer if standing still per second

wavelength (λ)

length of a wave from peak to peak (meter)

velocity constant

3×10^8 meters/sec

velocity equation

C = v x λ

(velocity)=(frequency)(wavelength)

electromagnetic radiation

a form of energy that moves through space or matter as a wave

ex: literally the entire spectrum we have been learning

Plancks constant

6.626×10^-34

used in equation as h

energy equation

E=h x v

(Energy)=(plancks constant)(frequency)

energy mesurement

Joules (J)

Color order of wavelengths

violet (400m), indigo, blue, green, yellow, orange, red (700nm)

High energy waves to low energy waves

1. X rays/gamma rays

2. Ultra violet

3. visible light

4. infared

5. microwaves

6. “water”

7. AM/FM/TV/phone

element used by bohr for light spectrum

hydrogen

organization order for orbitals ( least to most speicifc)

1. Principal energy levels

2. Sublevels

3. orbitals

each principal energy level has _ orbitals

n²

Aufbau Principal

Building up, when adding electrons, must occupy the orbital at the lowest energy level

Pauli Exclusion Principle

no 2 Es are the same, 2 electron in the same orbital must have equal but oposite spin (arrows)

FILL OUT/GO OVER

PERIODIC TABLE/IRREGS

goal for irreg configurations

to maintain symmetry or partial symmetry, and to benefit for energy

ions v atoms

ions are slightly smaller then atoms, but the pattern of size still holds