Atomic structure/properties Flashcards
radioactive decay types
alpha - decreases mass number by 4 and atomic number by 2
beta - adds 1 to atomic number
positron emission - subtracts 1 from atomic number
electron capture - subtracts 1 from atomic number
gamma decay - doesn’t change mass or electron number
exponential decay formula
N= N0(1/2)^(T/t/.5)
t/.5 = half life
T=total time sampled has decayed
mass defect formula
total mass of separate nucleons - mass of nucleus
nuclear binding energy formula
Eb= deltaM kg *9 *10^16J or Eb (in electrovolts) = deltaM(in amu) * 931.5 MeV
photon energy
EPhoton= hf = h(c/wavelength)
h=6.63 *10^-34 J/s
How are wavelength and energy related
They are inverses of each other
s orbital
has one spherically symmetrical orbital
p orbital
has three orbitals
three rules of electron configuration
electrons occupy lowest available energy orbital, electrons in same sub shell occupy available orbitals singly, before pairing up, there can be no more than two electrons in any given orbital
rules for adding and removing electrons
electrons are added to lowest energy orbital and removed from highest n level
S electrons are lost before d electrons
Atomic radius trends
decrease left to right across and period and increases down a group
Ionization energy trend
increases to the right across a period and up a group
electron affinity trend
usually becomes more negative as we move to right across a row or up a group but there are exceptions
electronegativity trend
increases to right across a period and decreases down a group
F>O>N=Cl>Br>I>S>C>H
fawn cull brish
acidity trend
increase down a group and to the right across a period