chemistry 13th edition chapt 1,2,3,7,8

equilibrium

no observable changes as time goes by

reversible process sign

⇌

scientific method

1. create question
2. background research
3. create hypothesis
4. conduct experiment
5. test hypothesis
6. draw conclusions
7. report results

how to convert farenheit to celsius

(F-32)\*5/9

how to convert celsius to fareheit

9/5\*C+32F

how to convert celsius to kelvin

273\.15+C

dalton’s atomic theory

1. law of conservation of mass
2. reactions can be separated, rearranged, or combined
3. each element’s atom is identical and unique in size, mass, etc.
4. elements are composed of atoms

joseph proust

created law of definite proportions

law of definite proportions

no matter where you find a compound, the elements within it will always have fixed and consistent proportions by mass

law of multiple proportions

two elements can combine in different proportions to create various compounds, and the ratios of their masses in these compounds will be simple whole number ratios

radiation

the emission and transmission of energy through space in waves

JJ Thomson

discovered electrons

charge of an electron

\-1.602\*10^-19 coulombs

who discovered charge of an electron

Robert Milikan

mass of an electron

9\.10\*10^-28

Wilhelm Rontgen

discovered x-rays

Antoine Becquerel

discovered radioactivity

radioactivity

spontaneous emission of particles

plum pudding

equal protons and electrons

proton mass

1\.67\*10^-24

atomic radius number

100pm

molecule

two atoms held by chemical forces

ion

positive or negative charge

allotropes

one of two or more distinct forms of an element

molecular models

ball and stick or space filling

structural formula

shows how elements are bonded in a molecule

binary compounds

two element compounds

ternary compounds

three element compounds

oxoanions

anions of oxoacids

acid

substance that yields hydrogen ions when dissolved in water

oxoacids

acids that contain h,o, and central element

base

substance that yields OH- ions when disolved in water

hydrates

compounds that have a specific number of water molecules attached to them

hydrocarbons

simplest organic compound

functional groups

bonded in a specific way

atomic mass

mass of protons, neutrons, and electrons

F.W. Aston

developed mass spectrometer, discovered isotopes

percent composition formula

steps to find empirical formula

1. determine grams of element
2. convert grams to moles
3. divide by simplest ratio number if not whole

what do you need to know to calculate molecular formula

approx. molar mass of compound and empirical formula

ratio of molar and empirical mass

molar mass / empirical mass

theoretical yield

actual/percent \* 100%

percent yield

actual/theo \* 100%

quanta

atoms and molecules emit energy only in certain quantities

wave

periodic disturbance that moves through space

speed of wave

*v*=*f*⋅*λ, distance/time*

electromagnetic wave

contains electric and magnetic field

electromagnetic radiation

emission and transmission of energy in the form of electromagnetic waves

quantum

smallest quantity of energy that can be emitted in form of electromagnetic radiation

relationship formula between energy and frequency in the context of electromagnetic waves

E=hv

photoelectric effect

electrons are ejected from the surface of certain metals exposed to light of a certain frequency

photons

particles of light

how are electrons held together

attractive forces that requires light of certain frequency to break them free

relationship between the energy of a photon and kinetic energy

hv=KE + W

w = work function

the more intense the light

greater # of electrons emitted

higher frequency of light

greater kinetic energy

particle wave duality

light can be like wave or particles

emission spectra

continous spectra of radiation emitted by substances

line spectra

light emission at specific wavelengths

energy level of electrons in hydrogen

\-Rh(1/n^2)

Rh

2\.18 \* 10^-18J

free electron

electron that is infinitely far from nucleus

ground state

lowest energy state of a system

excited state

higher than ground

Rydberg formula

nodes

amplitude is 0

relationship between circumference and wavelength

2πr=hλ

Louis de Broglie

electrons have wavelike properties

De Broglie wavelength equation

h/mv

true or false: wave particles can be observed in submicroscopic and macroscopic

false

heisenburg uncertainty principle

impossible to know mass times volume and position of particle at the same time

schrodinger

created equation that describes behavior and energy of submicroscopic particles

wave function symbol

Ψ

electron density

probability that electron will be in particular region of atom

atomic orbital

wave function of electron

quantum numbers

describe distribution of electrons in hydrogen and other atoms

principal quantum number

integral values

angular momentum quantum number

shape of orbitals (l)

magnetic quantum number

orientation of orbital in space and depends on angular momentum quantum number

electron spin quantum number

value +1/2 or -1/2

electron configuration rules

pauli exclusion principle → two electrons per orbital with opp spin

hunds rule → when filling up the orbitals, place one electron in each orbital of a sublevel before pairing

aufbau principle → when more protons are added, electrons are added to atomic orbitals as well

paramagnetic substance

net unpaired spins attracted by magnet

diamagnetic substance

no net unpaired spins and repel

odd number of electrons useful rule

will always contain one or more unpaired spins

noble gas core

noble gas element that almost replaces element being considered

newlands

law of octaves

isoelectronic

same # of electrons and ground-state electron configuration

effective nuclear charge equation

Zeff = Z - *σ*

expression to remove first electron

3\.94 \* 10^-18J

expression to remove second electron

8\.72 \* 10^-18J

ionic radius

radius of cation or anion

higher the ionization energy

harder to remove electron

electron affinity

negative energy charge that occurs when electron is accepted by an atom in the gaseous state to form an anion

how is electron affinity determined

removing additional electrons from anion

electron affinity trend

increase left and right, decrease up and down

diagonal relationships

simiplarities between pairs of elements in diff groups and periods

charge density

charge of ion/volume

halides

anions derived from halogens

amphoteric

display both acidic and base properties