Anorganik suatu kuliah singkat reaksi ki

INORGANIC CHEMISTRY 1

By :
Dina Kartika Maharani, M.Sc

Outline
 Ionic bonding
 Inorganic Reaction Principles
 Acid Base Chemistry

Syllabus
2

Memahami perbedaan jenis-jenis ikatan
kimia dan memahami pembentukan
senyawa kovalen, koordinasi, ionik.

Ikatan Kimia: Pendahuluan, Ikatan kovalen:
Teori ikatan valensi,teori tolakan elektron kulit
valensi, Teori orbital molekul, momen dipol.
Ikatan koordinasi: Teori ikatan valensi, teori

orbital molekul.
Ikatan
ion:
Sifat-sifat
senyawa
ionik,
pembentukan senyawa ionik, radius rasio,
energi kisi, kelarutan senyawa ionik, aturan
Fajan, penyimpangan struktur ionik sederhana.

4 x 3 x 50 ‘ tatap
muka

2

Memahami prinsip-prinsip dasar reaksi kimia, teori
asam basa, kekuatan asam, proses pelarutan, reaksi
dalam pelarut air dan non air.

Reaksi-reaksi kimia: Prinsip dasar reaksi kimia,

teori–
teori asam basa, kekuatan asam, proses pelarutan, reaksi
dalam pelarut air dan non air.

3 x 3 x 50’ tatap muka

Ionic Bonds
 One or more
electrons from 1
atom are removed
and attached to
another atom,
resulting in +ve
(cation) and –ve
(anion) ions which
attract each other

Ionic Bonds
The positive sodium
ion and the negative

chloride ion are
strongly attracted to
each other.

Covalent
Compounds

Ionic
Compounds

 Gases, liquids, or
solids
 Low melting and
boiling points
 Poor electrical
conductors
 Many soluble in
nonpolar liquids
but not in water

 Crystalline solids
 High melting and
boiling points
 Conduct
electricity when
melted
 Many soluble in
water but not in
nonpolar liquid

Struktur kristal fcc : NaCl

Struktur kristal bcc : CsCl

Ionic Crystal Formation

 M+ (g) + X- (g) → MX (s)

Electrostatic Approach
 Interaksi ion-ion menurut gaya

coulomb :

Electrostatic Approach

 Energi total = E tolakan + E tarik menarik

Coulomb Interaction in Ionic
Lattice
 Setiap ion M+ dikelilingi oleh

 Energi coulomb :

 Tetapan Madelung A
NaCl :
A= 6 – 12 + 8
√2 √3

Tetapan Madelung

Born Forces

 Energi kisi total melibatkan gaya tarik
menarik dan gaya tolak elektrostatik
antar ion

Persamaan Born Lande

 A = tetapan Madelung
 n = Born constant

Kapustinskii Equation
 Untuk kristal yang belum diketahui
strukturnya :

Born-Harber Cycle

ssolution of sodium chloride in water.
The hydrated ions slowly
diffuse away from the crystal
to become dissolved in

solution.
As the attraction
between the ions
weakens, the ions
move apart and
become
surrounded by
water
dipoles.
Polar water
molecules are
attracted to Na+ and Clions in the salt or crystal,
weakening the attraction
between the ions.

25

Solubility of Ionic Compound
 Ion size and charge : Hydration
energy

 Electronic configuration
 Crystal structure of solid
 HSAB
 Covalent character in ionic bond :
Polarization : Fajans rules

Fajans rules : Polarization
 High charge and small cation
polarizing power kation besar
mempolarisasi anion dengan kuat
 High charge and large anion
anion mudah terpolarisasi

 Electronic configuration of cation
kation dgn konf : (n-1)dx ns0 gol
transisi lebih mudah mempolarisasi
daripada kation dgn konf (n-1)s2 (n1)p6 ns0 (gol alkali dan alkali tanah)

Pengaruh polarisasi
 Peningkatan kelarutan dalam pelarut

polar seperti air
 AgF : sangat larut dalam air
 AgCl : larut dalam air dengan bantuan
ammonia
 AgBr : sedikit larut
 AgI : tidak larut

Penyimpangan Struktur Kristal

 Crystal defect atau cacat kristal

Schotky Defect

Frenkel

Transition
Transition Metal
Metal Gems
Gems
 Gemstone owe their color from trace

transition-metal ions
 Corundum mineral, Al22O33: Colorless

Cr  Al : Ruby

Mn  Al: Amethyst

Fe  Al:
Topaz

Ti &Co  Al: Sapphire
 Beryl mineral, Be33 Al 22Si66O18
: Colorless
18

Cr  Al : Emerald

Fe  Al : Aquamarine

Gemstones

 the colors of rubies and emeralds are
both due to the presence of Cr3+ ions –
the difference lies in the crystal
hosting the ion
Some
Al3+ ions
in Al2O3
are
replaced
by Cr3+

Some
Al3+ ions
in
Be3Al2(Si
O3)6 are
replaced
by Cr3+