chemistry sl

sublimation

solid to gas transition

deposition

gas to solid transition

empirical formula

the simplest whole number ratio of atoms in a compound

molecular formula

the actual number of atoms in a molecule

percent composition

experimental yield

compare theoretical yeilds

find limiting reactant

starting excess amount - theoretical consumption

find excess reactant remaining

isotopes

different masses of the same element

relative atomic mass

weighted average of the natural isotope abundances

s, p, d, f

order of sublevels

ultraviolet

light emitted by big jumps/falls from n=1 emission spectra

visible light

light emitted by medium jumps/falls from n=2

infrared

light emitted by small jumps/falls from n=3+

exothermic

a reaction that releases heat

endothermic

a reaction that uses heat

ENF, outermost energy level, e to e repulsion

factors that affect periodic trends

ioniza

energy required to remove 1 mol e from 1 mol gaseous atoms

Na2O and MgO

basic oxides (2)

Al2O3

amphoteric oxide (1)

SiO2, P4O10 , SO3, Cl2O7

acidic oxides (4)

an electrostatic attraction between a cation lattice and a sea of delocalized electrons

describe metallic bonding

an electrostatic attraction between positive cations and negative anions in a lattice

describe ionic bonding

an electrostatic attraction between two nuclei and a shared pair of electrons

describe covalent bonding

resonance structures

when multiple lewis structures are possible, the “true” structure is an average of each