Atomic Orbitals and Electron Arrangement
Number that specifies the properties of the
atomic orbitals
Tells us the distance from the nucleus and
the shape of the orbital
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Main level or shell
These are the Bohr energy levels
n
= 1,
n
= 2,
n
= 3
As
n
increases, the distance from the nucleus
increases
Each main level is divided into sublevels
Four types of sublevels
s
p
d
f
Each sublevel is made of orbitals
Every orbital can hold 2 electrons
s – 1 orbital – 2 electrons
p – 3 orbitals – 6 electrons
d – 5 orbitals – 10 electrons
f – 7 orbitals – 14 electrons
One spherical
shaped orbital
Three dumbbell shaped
One dumbbell in each axis
Arrangement of electrons in an atom
Aufbau Principle – electrons fill into an atom
starting with the lowest energy levels
Way which the electrons rotate on their axis
Pauli Exclusion Principle – in order for two
electrons to occupy the same orbital, they
must have opposite spin
Hund’s Rule – electrons occupy orbitals
singly first before doubling up
Write the configuration for each of the below
C
S
Br
Na
Cl
Kr
Electrons in the last main energy level
These are the electrons farthest out on the
atom
These will interact with other atoms
These are the electrons involved in chemical
reactions
There are a maximum of 8 valence electrons
Write configuration and count electrons in
last
main
energy level
Examples: Find valence electrons for
C
Na
P
Fe
Ar
Atoms will give up, accept, or share electrons
in order to achieve a filled valence shell (8
valence electrons)
Metals become more reactive (more metallic
in character) as you go down a group
Most metallic elements bottom left corner of
the periodic table
Least metallic, top right corner
Energy required to remove the most loosely
held electron from an atom
The greater the ionization energy, the more
strongly the atom holds onto its electrons
M + energy
→ M
+
+ e
Ionization energy increases as moving
across a period
Ionization energy decreases as moving
down a group
Half of the distance between two adjacent
nuclei
Radius decreases across a period (atoms hold
the electrons tightly in)
Radius increases down a group
Learn about the properties of atomic orbitals and how they determine the distance from the nucleus and the shape of orbitals. Explore the main energy levels, sublevels, and the arrangement of electrons following the Aufbau Principle within an atom.
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Presentation Transcript
Number that specifies the properties of the atomic orbitals Tells us the distance from the nucleus and the shape of the orbital
Main level or shell These are the Bohr energy levels n = 1, n = 2, n = 3 As n increases, the distance from the nucleus increases
Each main level is divided into sublevels Four types of sublevels s p d f
Each sublevel is made of orbitals Every orbital can hold 2 electrons
s 1 orbital 2 electrons p 3 orbitals 6 electrons d 5 orbitals 10 electrons f 7 orbitals 14 electrons
One spherical shaped orbital
Three dumbbell shaped One dumbbell in each axis
Main Level Main Level Sublevels Sublevels Number of Sublevels Number of Sublevels Electrons in sublevels Electrons in sublevels Total Electrons in Main Level Total Electrons in Main Level 1 s 1 2 2 2 s p 1 3 2 6 8 3 s p d 1 3 5 2 6 18 10 4 s p d f 1 3 5 7 2 6 32 10 14
Arrangement of electrons in an atom Aufbau Principle electrons fill into an atom starting with the lowest energy levels
Way which the electrons rotate on their axis Pauli Exclusion Principle in order for two electrons to occupy the same orbital, they must have opposite spin
File:Orbital diagram nitrogen.svg Hund s Rule electrons occupy orbitals singly first before doubling up
Write the configuration for each of the below C S Br Na Cl Kr
Electrons in the last main energy level These are the electrons farthest out on the atom These will interact with other atoms These are the electrons involved in chemical reactions There are a maximum of 8 valence electrons
Write configuration and count electrons in last main energy level Examples: Find valence electrons for C Na P Fe Ar
Atoms will give up, accept, or share electrons in order to achieve a filled valence shell (8 valence electrons)
Metals become more reactive (more metallic in character) as you go down a group Most metallic elements bottom left corner of the periodic table Least metallic, top right corner
Energy required to remove the most loosely held electron from an atom The greater the ionization energy, the more strongly the atom holds onto its electrons M + energy M+ + e Ionization energy increases as moving across a period Ionization energy decreases as moving down a group
Half of the distance between two adjacent nuclei Radius decreases across a period (atoms hold the electrons tightly in) Radius increases down a group
