Aromic Structure Flashcards
Isotopes
Nuclei that have the same number of protons but different number of neutrons = same physical and chemical properties
Binding energy
Energy needed to bind together the nucleus of atoms
Nuclear decay
The nucleus prior to nuclear decay is called the parent and the nucleus formed as a results of nuclear decay is called the daughter nucleus
Alpha particles
High velocity He atoms that are enmities by alpha decay, which steal two electrons and become helium
Beta particle
High velocity electrons
Alpha
Daughter has mass number 4 less than parent, atom mic number 2 less than parent
Beta
Daughter will always be a different element but will have the same mass number as parent
Gamma
Daughter is identical to parent, except it has less energy
First order decay
The probability that a nucleus will decay in a given time is constant and independent of the surrounding of the nucleus
Half life Equation
n = noe^-kt t(1/2) = ln2/k
Principal quantum number (n)
Describes the distinct energy levels or shells of the electron that orbits the nucleus; # of e- = 2n^2
Secondary quantum number (l)
Refers to the subshell with in each energy level; l=0:uses s, l=1:uses p, l=2:uses d, l=3:uses f
Magnetic quantum number (ml)
Refers to the electron orbitals with each subshell; every s has 1 orbital, every p has 3 orbitals, every d has 5 orbitals, every f has 7 orbitals
Magnetic quantum number possibilities
s: 1 ml =0
p: 3 ml = -1,0,+1
d: 5 ml = -2,-1,0,+1,+2
f: 7 ml = -3,-2,-1,0,+1,+2,+3
Spin quantum number (ms)
Can either be +(1/2) or -(1/2), for up or down arrows respectively, follows Pauli exclusion principle
Pauli exclusion principle
States that no two electrons in the same atom may ever have completely identical quantum numbers (n, l, ml, ms)
Aufbau principle
To find the correct ground state electron configuration of an atom, always completely fill all lower energy orbitals before filling any higher energy orbital
Hund’s rule
When partially filling degenerate orbitals of p, d, and f subshell a, always put on electron in each orbital before pairing them up; unpaired e- are orient so that their magnetic spins are all aligned
Violation of Aufbau principle
Extra stabilization is realized when an atom has a half filled or completely filled d orbital; Cr and Cu promote the 4s electron to the higher 3D subshell
Transition metal ions
Unlike other elements, transition metals always lose all their s electrons before losing any d electrons
