chemistry 40F info for october exam/test

EMR

release and transmission of energy in the form of electromagnetic waves

wavelength

shortest distance between equivalent points on a continous wave (m, cm, nm)

frequency

number of waves that pass a given point per second (Hz, /s)

how many nanometers in a meter

10^9

how many grams in a kilogram

1000

how many milometers in a meter

1000

how many cm in a meter

100 cm

how many meters in a kilometer

1000

what is the speed of light

3 × 10^8 m/s

how are wavelength and frequency related

inversely

how are energy and frequency related

proportionally

what unit must wavelength be in

meters

what unit must frequency be in

Hz (/s)

rabbits mate in very unusual Xtravagant gardens

radio, micro, infrared, visible, ultraviolet, x ray, gamma

in waht order

longest wavelength to shortest

what color order for visible light spectrum

ROYGBIV

what is a quanta

minimum amount of energy that can be gained or lost by an atom

according to planks theory, for a given frequency, matter can only..

emit or absorb energy in whole number multiples, not halves or anything. stairs

light can be thought of as a wave or..

as a stream of tiny particles called photons

photons

particle of EMR with no mass that carries a quanta of energy

what unit must energy be in

joules

a line spectrum consists of

distinct bright lines appearing on a dark background that occur in diff parts of the visible spectrum

why do elements have their own unique line spectrum

bc they have diff amounts of electrons and energy levels

what does the brightness of spectral lines depend on

how many photons of the same wavelength are emitted

what is the atomic emission spectrum

set of frequencies of EMR waves given off by atoms of an element; consists of fine lines of individual colors

what produces spectral lines

an atom being in the exicted state

how does an atom become excited

they must absorb energy and are the electrons are raised to a higher energy level by absorbing said energy

what happens when electrons fall back down after being exicted

releases color of light (photon), we see the color associated with the frequency and wavelength

what is the ground state

the default state when all electrons are in their lowest possible energy level

how many orbitals does the s sublevel have

1

how many orbitals does the p sublevel have

3

what energy level is the p sublevel first found in

second

how many electrons can one orbital hold

2

does the PQN (n) change the amount of orbitals in a sublevel?

no, it just makes the orbitals bigger

how many orbitals in the d sublevel

5

what energy level is the d sublevel first found in

3rd

how many orbitals in the f sublevel

7

what energy level does the f sublevel first appear in 

4

how to get number of electrons per energy level

2n²

what is the d sublevels relationship to the period number

one less than period number

what is the f sublevels relationship to the period number

two less than the period number (starts at 4f)

what is afbaus principle

each electron occupies the lowest energy level possible

what is pauli exclusion principle

a max of 2 electrons may occupy a single atomic orbital, but only if the electrons have opposite spin

what is hunds rule

single electrons with the same spin must occupy each equal-energy orbital before additional electrons can occupy the same orbital

when are sublevels the most stable and why

when half filled or fully fulled because each orbital has same amount of repulsion, np^6

what noble gas do u use for noble gas notation

for abbreviated, u use the noble gas of the previous period and then use electron configuration of the actual period to fill in the difference of remaining electrons  because it represents stable core 

order of sublevels and energy levels from low to high

1s, 2s, 2p, 3s, 3p, 4s, 3d, 5s, 4d, 5p