Unit 1: Atomic Structures & Properties

atom

neutral particle that is the fundamental building block of matter

ion

particle differing in number of electrons; may be positive or negative

isotope

particles that differ in amount of neutrons, making their mass different

mole

containing 6.022x10^23

atomic radius

the size of the atom, measured from the nucleus to the outermost electron

ionization energy

amount of energy required to remove an electron from an atom

electronegativity

ability for an atom to pull electrons close to itself in a molecule

electron affinity

amount of energy given off when an electron is added to an atom

mass spectroscopy measures the differences in (). along the x-axis () is graphed and along the y-axis () is graphed

ions, mass/charge ratio, abundance or relative intensity

photoelectron spectroscopy measures the differences in (). along the x-axis () is graphed and along the y-axis () is graphed.

electrons, binding energy, relative number of electrons

the relationship between the attractive force between the particles and their charge is ()

directly proportional

the relationship between the attractive force between the particles and their distance is ()

inversely proportional

pauli exclusion principal

electrons need to have different quantum numbers, and therefore should have electrons spinning in opposite direction within an orbital

hund’s rule

electrons within orbitals of the same energy need to spread out before the pair up

inert

does not react

law of definite proportions

the ratio of the masses of the elements in any pure sample of that compound is always the same

why does atomic radius increase as you go down

increasing energy level, the outermost electron is farther away in a greater energy level

why does atomic radius increase as you go across (left)

less protons, less coulombic attraction, protons don’t pull electrons as much so the radius is larger

why does ionization energy increase up and to the right

larger radius, less coulombic attraction, it takes less energy to remove the electron

what is the first exception to ionization energy

group 2 and 13 since the s orbital is closer to the nucleus than the p orbital

what is the second exception to ionization energy

group 15 and 16 since paired electrons are easier to remove than unpaired electrons because of e/e repulsion

isoelectric

same number of electrons, focus on number of protons

oxidation number

most common ion that forms for an element based on the amount of valence electrons