Chapter 1: Atomic Structure Flashcards
What does atomic mass refer to?
The sum of an elements protons + neutrons; The mass number.
What does atomic weight refer to?
The weighted average of an element’s naturally occurring isotopes.
What atomic measure does the periodic table represent, the atomic weight or atomic mass?
Atomic weight
What are isotopes?
Atoms of a given element (same atomic number) that have different mass (they differ in # of neutrons).
The principal quantum # n describes the energy state of _____.
The atomic shell
The azimuthal quantum number l describes the energy state of _____. What is the formula to determine l?
The atomic subshells. l= 0 - (n-1)
The magnetic quantum number m(l) describes the energy state of _____. What is the formula to determine m(l)?
The atomic orbitals. m(l) = (-l) - (+l)
Planck relation (frequency)
E=hf
E= energy
h= Planck’s constant = 6.626 x10^-34 J*s
f = lambda = frequency
Angular momentum of an electron (Bohr model):
E = (- R(H)/n^2
Max # of electrons within a subshell = ?
4l + 2
Max # of electrons within a shell = ?
2n^2
Heisenberg uncertainty principle
States that it is impossible to know an electron’s position and momentum exactly at the same time.
Hund’s rule
States that subshells with multiple orbitals (p, d, and f) fill electrons so that every orbital in a subshell gets one electron before any of them gets a second.
Atomic absorption spectrum
The energy absorbed by an electron when it jumps from a lower energy level to a higher one; it is equal to the energy difference between levels.
Atomic emission spectrum
The energy emitted by an electron when it jumps from a higher energy level to a lower one; it is equal to the energy difference between levels.
