22/06/53 1 Dr. Weenawan Somphon Inorganic Chemistry I 01403312 Chemistry Division, Faculty of Liberal Arts and Science Kasetsart University, Kam Phaeng Saen Campus What is “Inorganic Chemistry”? The chemistry of all compounds that are not entirely made up from C, H, N and O includes the description of chemical and physical properties. includes theories and principles that can be used to predict or at least rationalize the formation and properties of compounds. Inorganic chemistry is very diverse use concepts from bonding theory, kinetics and thermodymanics to make sense of it all. Organic chemistry e.g. Catalysts in Organic synthesis Biochemistry/biology e g inorganic contained biological structures Inorganic Application*** in Wacker Process e.g. inorganic contained biological structures hemoglobin Material Science e.g. devices, coordination polymers Ferroelectric material: BaTiO 3 Environmental Science e.g. Cr(VI), As(V), Pb(II), Hg(II) Network of Inorganic Chemistry Outline of this lecture Atomic Structure Periodic Table Symmetry and point group Solid State C l t l l Covalent molecules Chemical force Acids-bases chemistry Nonaqueous chemistry Inorganic chains, rings, cages Nanomaterials Atomic Structure
Transcript
22/06/53
1
Dr. Weenawan Somphon
Inorganic Chemistry I 01403312
Chemistry Division, Faculty of Liberal Arts and ScienceKasetsart University, Kam Phaeng Saen Campus
What is “Inorganic Chemistry”?
The chemistry of all compounds that are not entirely made up from C, H, N and O
includes the description of chemical and physical properties.
includes theories and principles that can be used to predict or at least rationalize the formation and properties of compounds.
Inorganic chemistry is very diverse
use concepts from bonding theory, kinetics and thermodymanics to make sense of it all.
Organic chemistry e.g. Catalysts in Organic synthesis
Biochemistry/biology e g inorganic contained biological structures
Inorganic Application***
in Wacker Process
e.g. inorganic contained biological structures hemoglobin
Material Science e.g. devices, coordination polymers
Ferroelectric material: BaTiO3
Environmental Science e.g. Cr(VI), As(V), Pb(II), Hg(II)
Network of Inorganic Chemistry
Outline of this lecture
Atomic Structure Periodic Table Symmetry and point group Solid State
C l t l l Covalent molecules Chemical force Acids-bases chemistry Nonaqueous chemistry Inorganic chains, rings, cages Nanomaterials
รวบรวมแนวคดจาก Thomson ทสรปวาอนภาคประจลบภายในอะตอมคอ l t และ จาก R th f d ซงสรปวาอะตอมจะมอะตอมคอ electron และ จาก Rutherford ซงสรปวาอะตอมจะมสวนทวาง คอ electron ทลอมรอบนวเคลยสทอยตรงกลาง ทมประจบวก
เสนอภาพของอะตอมทมนวเคลยสลอมรอบดวย electrons ซงเคลอนทในวงโคจร (orbit) คลายกบดาวเคราะหรอบดวงอาทตย Proton at the
nucleus
electron
22/06/53
5
Bohr’s Atom
electrons in orbits
nucleus
Bohr Model
Niels Bohr followed Planck’s and Einstein’s lead by proposing that electron energy (En) was quantized.
Electronic Transitions in the Bohr Model for the Hydrogen Atom
Electron in H atom moves around the nucleus in certain allowed circular orbits.E = -2.718X10 -18 J (Z2/n2 )
n= integerZ = nuclear charge
Neil Bohr’s Model of Hydrogen
Bohr Explains Line Spectra
Bohr’s equation is most useful in determining the energy change (Elevel) that accompanies the leap of an electron from one energy level to another
For the final and initial levels:
f i2 2f i
B BE and E
n n
The energy difference between nf and ni is:
2 2 2 2f i i f
1 1B BE B
n n n n
Bohr Model
Bohr ไดทาการแทนทสมการชอง Balmer
4222 Z
22
11
hl
Hnn
RE
nucleuse mm
111
22
422
)4(
2
h
eZR
oH
22/06/53
6
De Broglie’s Equation
1924 Louis de Broglie: ไดเสนอวา สสาร (matter) มสมบตเปนทงคลน (wave) และอนภาค (particle)—ทดลองโดยการยนยนการหกเหของ electrons ในผลก
h
mv
h
Heisenberg’s Uncertainty Principle
1927 werner Heisenberg: เสนอหลกความไมแนนอนวา ในทางกลศาสตรควอนตม เราไมสามารถจะหาตาแหนง และโมเมนตมของอนภาคอยางถกตองแมนยาไดพรอมๆกน
1926 Erwin Schrödinger- เสนอสมการคลน เพออธบายฟฤตกรรมของอนภาคเลกๆ ใชในการอธบาย electron อะตอม และโมเลกล
H E =
= wave function = describes an electron wave in space = describes atomic orbital
= wave function = mathematical operatorH = the Hamiltonian Operator = calculus operation on
E = total energy of the atom
The Hamiltonian Operator = H
h = Planck’s constant, m = mass of the particleE = total energy of the system, e = charge of electron(x2 + y2 + z2)1/2 = r = distance to nucleusZ = charge of the nucleus, 4o = permittivity of vacuum
Bohr describe an orbit, the quantum-mechanical model uses 3 quantum, n, l, and ml to
describe an orbital
An atomic orbital is defined by 3 quantum numbers: n l ml
Electrons are arranged in shells and subshells of orbitals
n shelll subshell (describes shape of orbital
s, p, d, f corresponding to 0, 1, 2, 3 respectively
ml designates an orbital within a subshell
Quantum Numbers (QN) Principal Quantum Number (n)
The principal quantum number (n):
• Describes the energy level, orbital size as n increases, orbital size increases.
• Is independent of the other two quantum numbers.
• Can only be a positive integer (n = 1 2 3 4 )• Can only be a positive integer (n = 1, 2, 3, 4, …)
• The size of an orbital and its electron energy depend on the value of n.
• Orbitals with the same value of n are said to be in the same principal shell.
Angular Momentum Quantum Number (l)
Possible values = 0 to (n – 1); e.g., if n = 2, l can only be 0 or 1
22/06/53
9
Magnetic Quantum Number (ml)
Calculate the number of orbitals in the shells with principal quantum number = 1,2 and 3
s OrbitalsAll s orbitals are spherical in shape.
The 1s Orbital (Electron Probabilities) The 2s Orbital (Electron Probabilities)
The 2s orbital has two regions of high electron probability, both being spherical
The region near the nucleus is separated from the outer region by a spherical node ‐ a spherical shell in which the electron probability is zeroelectron probability is zero
22/06/53
10
Boundary surface for 1s orbital
Boundary Surface for Three 2p Orbitals
22/06/53
11
Boundary Surfaces of All of the 3d Orbitals
22/06/53
12
Boundary Surfaces of the 4f Orbitals
Quantum Numbers Summary Electron Spin Quantum Number (ms)
ออรบทลในชนเดยวกนจะมพลงงานแตกตางกนโดย s < p < d เนองจากมาจากความสามารถในการทะลผาน (penetrating ability) ของอเลกตรอนในแตละออรบทลเขาไปในกลมอเลกตรอนของออรบทลอนๆ ดงนน interaction กบนวเคลยสนนไมเทากน
Governs the arrangements of electrons in many-electron atoms.
No two electrons can have the same set of four b ( l l ) h fquantum numbers (n, l, ml, ms ). Therefore, no
atomic orbital can contain more than 2 e-.
An orbital can hold a maximum of two electrons and they must have opposite spins.
Aufbau Principle
Aufbau Principle: an e- occupies the lowest energy orbital that can receive it.
As protons are added one by one to the nucleus to build up the elements, electrons are similarly added t th h d lik bit lto these hydrogen-like orbitals.
Atomic State and Term Symbol
Term symbol--เปนการบอกสถานะพลงงาน โมเมนตมเชงมม และ spin multiplicity ของอะตอมหรอไอออน
spin multiplicityL = 0 S termL = 1 P termL = 2 D termL = 3 F term
2S+1LJ
orbital angular momentum
Russell Saunders Term Symbol
L = 0, 1, 2…total orbital angular momentum (l term)ML = -L…+L component of L (ML = ml)S = total spin quantum number (S = s)Ms = -S….+S component of S (MS = ms)
