2. SCHROEGINDER WAVE EQUATION
Wave-particle duality of electrons
The position of an electron is described in terms of
probability density
Orbital
region (volume of space around the nucleus) where
there is a high probability of finding an electron of a
given energy
Atomic model
3-D
3 quantum numbers (principal, angular, magnetic)
3. QUANTUM NUMBERS
Describe the size, shape and orientation in space of
the orbitals
Principal Quantum Number (n)
Energy level of the electron
Maximum number of electrons at n level is 2n2
Energy Level No. of electrons
n = 1 2
n = 2 8
n = 3 18
n = 4 32
4. QUANTUM NUMBERS
Angular Quantum Number (l)
Sublevels in n & Shape of the orbitals
s, p, d, f
Each energy level has n sublevels
Energy Level No. of
Sublevels
Sublevels
n = 1 1 1s
n = 2 2 2s, 2p
n = 3 3 3s, 3p, 3d
n = 4 4 4s, 4p, 4d, 4f
5. QUANTUM NUMBERS
Magnetic Quantum Number
Number of orbitals within a sublevel
Sublevel No. of Orbitals Max. Electrons
s 1 2
p 3 6
d 5 10
f 7 14
6. QUANTUM NUMBERS
Fourth Quantum Number????????
Spin Quantum Number
Each electron has a magnetic field and a spin
associated with that electron
Pauli Exclusion Principle
No more than two (2) electrons can occupy an orbital
Two (2) electrons in the same orbital must have
opposite spins
NO TWO ELECTRONS IN AN ATOM HAVE THE SAME
FOUR QUANTUM NUMBERS
8. SHAPES OF ORBITALS
s orbital
Each energy level has one s orbital
Maximum number of electrons = 2
Spherical
1s and 2s orbitals are similar in shape however electron
density is closer to the nucleus for the 1s orbital
9. SHAPES OF ORBITALS
p orbitals
Each energy level has three (3) degenerate p orbitals
i.e. 3 orbitals of EQUAL ENERGY
Dumb-bell shape
11. ELECTRONIC CONFIGURATIONS
s orbitals have slightly lower energy than the p
orbitals at the same energy level i.e. 2s < 2p
s orbital will ALWAYS fill before corresponding p
orbitals
s orbital have the lowest energy then p, d, f
s < p < d < f
12. ELECTRONIC CONFIGURATIONS
Anomaly
Irregularity in the position of the 3d and 4s orbitals
3d has slightly more energy than 4s
4s fills first then 3d orbitals followed by 4p orbitals
13. ELECTRONIC CONFIGURATIONS
Describes the arrangement of electrons in the
orbitals of an atom
How are electronic configurations worked out?
Electrons are added one at a time, starting with the
lowest energy orbital (Aufbau Principle)
No more than two electrons can occupy an orbital (Pauli
Exclusion Principle)
Electrons fill degenerate orbitals one at a time with
parallel spin before a second electron is added with
opposite spin (Hund’s Rule)
14. ELECTRONIC CONFIGURATIONS
How do we write electronic configurations?
Principal Quantum number (1, 2, 3 etc)
Symbol for the orbital (s, p, d, f)
Superscript that shows the number of electrons in the
sublevel
number of electrons in orbital
energy level1s2
type of orbital
15. ELECTRONIC CONFIGURATIONS
Atomic Number Symbol Electronic
Configuration
1 H 1s1
2 He 1s2 or [He]
3 Li [He] 2s1
4 Be [He] 2s2
5 B [He] 2s2 2p1
6 C [He] 2s2 2p2
7 N [He] 2s2 2p3
8 O [He] 2s2 2p4
9 F [He] 2s2 2p5
10 Ne [He] 2s2 2p6 or [Ne]
16. ELECTRONIC CONFIGURATIONS
Atomic Number Symbol Electronic
Configuration
11 Na [Ne] 3s1
12 Mg [Ne] 3s2
13 Al [Ne] 3s2 3p1
14 Si [Ne] 3s2 3p2
15 P [Ne] 3s2 3p3
16 S [Ne] 3s2 3p4
17 Cl [Ne] 3s2 3p5
18 Ar [Ne] 3s2 3p6 or [Ar]
19 K [Ar] 4s1
20 Ca [Ar] 4s2
17. ELECTRONIC CONFIGURATIONS
Atomic Number Symbol Electronic
Configuration
21 Sc [Ar] 4s2 3d1
22 Ti [Ar] 4s2 3d2
23 V [Ar] 4s2 3d3
24 Cr [Ar] 4s1 3d5
25 Mn [Ar] 4s2 3d5
26 Fe [Ar] 4s2 3d6
27 Co [Ar] 4s2 3d7
28 Ni [Ar] 4s2 3d8
29 Cu [Ar] 4s1 3d10
30 Zn [Ar] 4s2 3d10
18. ELECTRONIC CONFIGURATIONS –
ABBREVIATED
He, Ne and Ar have electronic configurations with
filled shells of orbitals
Abbreviated electronic configurations
He = 1s2 or [He]
Ne = 1s2 2s2 2p6 or [Ne]
Ar = 1s2 2s2 2p6 3s2 3p6 or [Ar]
19. ELECTRONIC CONFIGURATIONS - SPECIAL
After 3p orbitals are filled, 4s orbital is filled before
the 3d orbital
4s orbital is at a slightly lower energy than the 3d
K is [Ar] 4s1
Ca is [Ar] 4s2
Sc is [Ar] 4s2 3d1
20. ELECTRONIC CONFIGURATIONS - SPECIAL
After Sc, the 3d orbitals are filled
Irregularity is seen in the electronic configuration of
Cr and Cu
Cr is [Ar] 4s1 3d5
Cu is [Ar] 4s1 3d10
21. ELECTRONIC CONFIGURATIONS - SPECIAL
One electron has been transferred from the 4s
orbital to the 3d orbital
Half-filled and filled sublevels of 3d orbitals decreases
Energy
Spin pairing of the 4s orbital increases
Energy
23. IONIZATION ENERGY
1st Ionization Energy of an element
Energy needed to convert 1 mole of its gaseous atoms
into gaseous ions with a single positive charge
M(g) M+
(g) + e-
Energy required to remove each successive
electron is called the 2nd, 3rd, 4th, etc. ionization
energy
Ionization energies are positive because it requires
energy to remove an electron
24. IONIZATION ENERGY –
INFLUENCING FACTORS
Magnitude of ionization energy
how strongly the electron to be lost is attracted to the
nucleus
Factors that influence ionization energy
Atomic Radii
Nuclear Charge
Shielding (Screening)
25. IONIZATION ENERGY – ATOMIC RADII
Atomic Radii
Distance of the outer electron is from the nucleus
As distance increases ( ), nuclear attraction for the
outer electron decreases ( ), ionization energy
decreases( )
26. IONIZATION ENERGY – ATOMIC RADII
Successive Ionization Energies of Sodium (Na)
Ionization
Energy
Energy Orbital
Electron Lost
From
1st 496 3s
2nd 4562 2p
3rd 6912 2p
4th 9543 2p
5th 13353 2p
6th 16610 2p
7th 20114 2p
27. IONIZATION ENERGY – NUCLEAR CHARGE
Nuclear Charge
As nuclear charge increases, attraction of the nucleus
for the outer electron increases, ionization energy
increases
Atomic Radii and Electron Shielding (Screening) can
outweigh the effect of nuclear charge
Cs has a larger nuclear charge than Na, loses electron more
readily than Na
28. IONIZATION ENERGY –
SHIELDING (SCREENING)
Screening Effect of Inner Electrons
Electrons experience repulsion by other electrons
Outer electrons are shielded from the attraction of the
nucleus by repelling effect of inner electrons
Screening effect of electrons in lower energy levels is
more effective than electrons in higher energy levels
29. IONIZATION ENERGY –
SHIELDING (SCREENING)
Screening Effect of Inner Electrons
Electrons in same energy level has negligible screening
effect on each other
As screening effect becomes more effective, ionization
energy decreases