Kimia anorganik ii
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Transcript of Kimia anorganik ii
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Kimia Anorganik II(2 SKS)
Johnson N. Naat, S.Pd., M.Si
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Ikatan yang terjadi karena adanya serah terima elektron
(IKATAN IONIS/ IKATAN IONIK/
IKATAN ELEKTROVALEN)
Senyawanya → Senyawa ion/ senyawa ionik/ senyawa ionis/ senyawa elektrovalen
Kadang-kadang disebut juga senyawa polar
INGAT!!! Senyawa ionik pasti polar…
Senyawa polar belum tentu ionik…..
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8 cells
CsCl Structure
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5 – Zinc Blende or ZnS Structure
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Zincblende (ZnS) Lattice
Zincblende LatticeThe Cubic Unit Cell
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A view of the tetrahedral coordination
& the 2 atom basisZincblende &
Diamond Lattices Face Centered Cubic (FCC) lattices with a
2 atom basis
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The Wurtzite Lattice
Wurtzite Lattice Hexagonal Close
Packed (HCP)Lattice + 2 atom basis
View of tetrahedral
coordination & the 2 atom basis.
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24
ABX3 Crystal Structures
Adapted from Fig. 12.6, Callister & Rethwisch 8e.
• Perovskite structure
Ex: complex oxide BaTiO3
CHARGE C.G. SEPARATE AT GEOMETRICAL CENTER
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Kristal terdiri atas kation2 dan anion2 yang tersusun teratur
Pola yang teratur & berulang menghasilkan kisi
Energi kisi : energi yang dibebaskan ketika sejumlah mol kation dan sejumlah mol anion didekatkan dari jarak tak terhingga sampai ke kedudukan setimbang dalam suatu kisi kristal 1 mol senyawa ionik pada 0 K
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Aspek Energi dalam Ikatan Ionik: Energi Kisi
• Misalkan ada suatu reaksi antara unsur logam yang reaktif (Li) dan mudah melepas elektron dengan gas halogen (F) yang cenderung menarik elektron:Li(g) Li+(g) + e- IE1 = 520 kJF(g) + e- F-(g) EA = -328 kJ
• Reaksi total:Li(g) + F(g) Li+(g) + F-(g) IE1 + EA = 192 kJ
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• Energi total yang dibutuhkan reaksi ini bahkan lebih besar karena kita harus mengkonversi Li dan F kedalam bentuk gas
• Akan tetapi eksperimen menunjukkan enthalpi pembentukan padatan LiF (∆H0
f) = -617 kJ• Jika kedua unsur dalam bentuk gas:• Li+(g) + F-(g) LiF(g) ∆H0 = -755 kJ• Energi kisi adalah perubahan enthalpi yang
menyertai ion-ion gas yang bergabung membentuk padatan ionik:
• Li+(g) + F-(g) LiF(s) ∆H0kisi LiF = energi kisi
= -1050 kJ
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Daur Born-Haber
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Nilai Energi Born-Haber• Ho
atom Li = 161 kJ• BE F2 = 159 kJ• IE1 (Li) = 520 kJ• EA (F) = -328 kJ• Ho
Lattice (LiF) = -1050 kJ• Ho
f LiF = -617 kJ• Total Energi :Ho
f LiF = Hoatom Li + ½ BE F2 + IE1 (Li) +
EA (F) + HoLattice
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Soal Latihan• Dengan menggunakan daur Born-Haber
untuk senyawa KF, hitung afinitas elektron fluorine jika diketahui data-data sebagai berikutK(s) K(g) ∆H0 = 90 kJK(g) K+(g) + e- ∆H0 = 419 kJF2(g) 2F(g) ∆H0 = 159 kJK(s) + ½ F2(g) KF(s) ∆H0
f = -569 kJK+(g) + F-(g) KF(s) ∆H0
kisi = -821 kJ
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Trend Periodik Energi Kisi• Menurut Hukum Coulomb:
Gaya elektrostatik ∞ (muatan A x muatan B) Jarak2
Karena energi = gaya x jarak, maka rumusan di atas dapat juga ditulis:Energi elektrostatik = (muatan A x muatan B)
JarakDidalam padatan ionik, A dapat berupa kation dan B anion dengan memperhitungkan jarak = jari-jari kation + jari-jari anion
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Trend pada Energi Kisi
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