Electrons and Energy Levels - Chem

scientific notation

way of expressing very large or small numbers

how to covert to scientific notation

1. move decimal until you have number between 1 and 9.99999

2. place an x10 and an exponent equal to the number of time you moved the decimal

3. positive - left

4. negative - right

how to convert to standard notation

1. move decimal as many times as exponent

2. positive - right

3. negative - left

light

led to quantum mechanical model. kind of electromagnetic radiation (gamma rays, x-rays, radio waves)

speed of light

2.998 × 103 m/s

frequency

how frequent a wave passes through an object in a specific time, (v)

wavelength and frequency

inversely related (one goes up other down), different frequencies are different colors, range is called spectrum

Planck’s constant (h)

6.626 × 10-3 J*s

energy formula

E = hv

speed of light formula

c = wavelength v

excited state

atom with excess energy, ex. passing UV light through, heating up

ground state

atom is the lowest state possible

principle Quantum Number (energy level)

symbolized by n, detonates energy level in which the electron is located

atomic orbitals (sublevels)

regions where theres high probability of finding an electron, arranged in s, p, d, f

aufbau principle

electrons enter lowest energy level first

pauli exclusion principle

at most 2 electrons per orbital, different spins

hunds rule

when electrons occupy orbitals of equal energy

D (energy level)

5 versions, 10e- max

F (energy levels)

7 versions, 14e- max

S (energy levels)

3d sphere, 1 version, 2e- max

P (energy levels)

figure 8, 1 horizontal, 1 vertical, 1 diagonal on top of each other, 3 versions, 6 e- max

chromium and elements under

4s1 3d5 (d4 exception)

copper and elements under

4s1 3d10 (d9 exception)

horizontal rows

periods, 7 periods

vertical column

group (family), similar physical/chemical properties, identified by number and letter

metals

electrical conductors, have lusters, ductile, malleable, make up most of periodic table

nonmetals

generally brittle and non-lustrous, poor conductors of heat and electricity (due to covalent bonds), some gases (O,N,Cl), some solids (S), one fuming dark red liquid (Br)

metalliods

properties in between metals and nonmetals, does both ionic and covalent bonds

group 1

alkali metals, forms a base when reacting with water

group 2

alkaline earth metals, form bases with water, do not dissolve well

group 17

halogens, means salt-forming

group 18

noble gases, previously called “inert gases” because they rarely take part in a reaction, very stable