Chemistry Cycle 1

Dalton’s atomic theory

electrons have a charge of -1, mass 0, relative mass 5×10^-4 (0.0005) amu, quantity varies between ions

melting and boiling points peak

center of d block (transition metals)

intensive

property does not change based on amount of substance

ex: density bc it’s applied the same way no matter how much of a substance there is

extensive

changes based on amount of substance

reason for the atomic emission spectra of different elemnts

when e- go back to the ground state the give off energy that releases light

equation to find the energy of a particular level (n)

E = -B/n²

equation to calculate the change in energy when moving from one level to the next

_{E=(-Bn^2)final-(-Bn^2)initial}

Bohr’s constant

2.179×10^-18 J

Planck’s constant

6.626×10^-34

Speed of Light

3.00×10^8

nu

frequency

c=wavelength*frequency

The wave description of light

E = hv

the particle description of light

E = hc/lambda

energy of a photon

1 nanometer

10^-9 meter

1mm

10^-3 m

Avogadro’s number (1 mol)

6.022×10^23

Pauli exclusion principle

no two elecrons have the same set of quantum numbers

percentage error equation

value experimental - value accepted/ value accepted * 100

equation for total mass # of the isotopes

(mass number of isotope x abundance) + (mass number of isotope x abundance)

law of definite proportions

a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample/source of the compound

law of multiple proportions

if 2 or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first elements is always a ratio of small whole numbers.

µ

micro, 10^-6 (one millionth)

law of conservation of mass

mass is neither created nor destroyed during ordinary chemical reactions or physical changes

diffraction

the bending of a wave as it passes by the edge of an object or through a small opening

Aufbau principle

an electron occupies the lowest energy orbital that can receive it

ground state electron configuration

the lowest-energy arrangement of electrons for each element

hund’s rule

orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state

electron octet

when atoms have the s and p sublevels of their highest occupied level filled with eight electrons

every noble gas has this in its highest energy level except Helium