PPT 2A Part 2 Flashcards
Atoms with the same atomic number but
different mass numbers
Isotopes
Atoms of different elements with the same mass number but different atomic numbers
Isobars
Atoms of different elements with the same number of neutrons but different mass numbers
Isotones
Atoms of different elements which have the same value of n - p
Isodiaphers
Who
Quantum mechanical model of the atom
- Louie de Broglie
- Erwin Schrodinger
- Werner Karl Heisenberg
Explains the manner of existence of electrons and their behavior in atoms
Quantum mechanical model of the atom
Helps us understand and predict the properties of atoms that are directly related to the behavior of the electrons
Quantum mechanical model of the atom
Orbital is AKA
Electron shell or Energy level
QUANTUM NUMBERS
* Location and energy of e- in an atom is determined by a set of ___ that describes different atomic ___
- 4 QN
- Orbitals
QN
- Main energy level occupied by the electron
- Integral values of 1, 2, 3 and so forth
Principal quantum number, n
Principal QN
Higher n, larger ___, e- has higher ___ and thus ___ from the nucleus
Orbital; energy; farther
QN
Defines the shape of the orbital or the type of subshell of an electron
Azimuthal quantum number (Angular momentum QN), l
QN
- Integral values from 0, 1, 2… (n-1)
- Generally designated by the letters s, p, d and f
Azimuthal quantum number (Angular momentum QN), l
Azimuthal QN Shapes
s (sharp)
Spherical
Azimuthal QN Shapes
p (principal)
Dumbbell
Azimuthal QN Shapes
d (diffuse)
Clover
Azimuthal QN Shapes
f (fundamental)
Complex
QN
Describes the orientation of the orbital in space (spatial arrangement)
Magnetic quantum number, ml
QN
Integral numbers between –l to l including 0
Magnetic quantum number, ml
QN
Either + 1⁄2 or – 1⁄2
Electron spin number, ms
QN
Denotes the direction of the spin of an electron that affects the direction of the magnetic field generated
Electron spin number, ms
Direction of spin (CCW or CW)
Arrow is up
Counterclockwise
Direction of spin (CCW or CW)
Arrow is down
Clockwise
The manner in which the electrons are distributed among the various orbitals of an atom
Electron configuration
“Aufbauen”
“to build”
Filling up energy sublevels with electrons starts with the lowest energy level available
Aufbau principle
No two electrons can have the same four quantum numbers
Pauli’s exclusion principle
An orbital can hold at most two electrons only if the electrons have opposite spins
Pauli’s exclusion principle
The lowest energy arrangement of electrons in a subshell is obtained by putting electrons into separate orbitals of the subshell with the same spin before pairing electrons
Hund’s rule
- Used to show how the orbitals of a subshell are occupied by electrons
- Represented by a circle/box/line
Orbital diagram
A substance with unpaired electrons is?
Paramagnetic
A substance composed only of paired electrons is?
Diamagnetic
