Download - Tabel Periodik
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Tabel Periodik
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8.1
Kapan unsur-unsur ditemukan?
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8.2
ns
1
ns
2
ns
2n
p1
ns
2n
p2
ns
2n
p3
ns
2n
p4
ns
2n
p5
ns
2n
p6
d1
d5
d1
0
4f
5f
Konfigurasi elektron unsur-unsur pada keadaan dasar
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8.2
Penggolongan unsur-unsur
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Konfigurasi Elektron Kation dan Anion
Na [Ne]3s1 Na+ [Ne]
Ca [Ar]4s2 Ca2+ [Ar]
Al [Ne]3s23p1 Al3+ [Ne]
Atom kehilangan elektron
shg kation memiliki
konfigurasi gas mulia pada
elektron terluarnya.
H 1s1 H- 1s2 or [He]
F 1s22s22p5 F- 1s22s22p6 or [Ne]
O 1s22s22p4 O2- 1s22s22p6 or [Ne]
N 1s22s22p3 N3- 1s22s22p6 or [Ne]
Atom memperoleh
elektron shg anion
memiliki konfigurasi gas
mulia pada elektron
terluarnya.
8.2
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+1
+2
+3
-1
-2
-3
Kations dan Anion dari Unsur-unsur
8.2
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Na+: [Ne] Al3+: [Ne] F-: 1s22s22p6 atau [Ne]
O2-: 1s22s22p6 or [Ne] N3-: 1s22s22p6 atau [Ne]
Na+, Al3+, F-, O2-, dan N3- seluruhnya merupakan
isoelektronik dg Ne
Apakah atom netral isoelektronik dengan H- ?
H-: 1s2 Konfigurasi elektron yg sama dg He
8.2
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Kation yang Dihasilkan dari Logam Transisi
8.2
Ketika kation terbentuk dr suatu atom logam transisi, elektron
pd awalnya selalu dipindahkan dari orbital ns dan kemudian
dari orbital (n – 1)d.
Fe: [Ar]4s23d6
Fe2+: [Ar]4s03d6 or [Ar]3d6
Fe3+: [Ar]4s03d5 or [Ar]3d5
Mn: [Ar]4s23d5
Mn2+: [Ar]4s03d5 or [Ar]3d5
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Muatan inti efektif (Zeff) adalah “muatan positif” yang
mempengaruhi suatu elektron.
Na
Mg
Al
Si
11
12
13
14
10
10
10
10
1
2
3
4
186
160
143
132
Zeff Inti Z Jari2
Zeff = Z - s 0 < s < Z (s = konstanta perisai)
Zeff Z – muatan inti sebenarnya
8.3
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Muatan Inti Efektif (Zeff)
8.3
Zeff meningkat
Zeff m
enin
gkat
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8.3
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8.3
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Plot jari2 atom unsur2 terhadap nomor atomnya
8.3
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8.3
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Kation selalu lebih kecil dari atom yg
membentuknya.
Anion selalu lebih besar dari atom yang
membentuknya.
8.3
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8.3
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Kimia dalam kehidupan: Unsur Cair ke-3? L
iqu
id?
113 unsur, 2 unsur cair pada 250C – Br2 dan Hg
223Fr, t1/2 = 21 menit
8.3
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Energi Ionisasi adalah energi minimum yang diperlukan
untuk melepaskan satu elektron dari atom berwujud gas
pada keadaan dasarnya.
I1 + X (g) X+
(g) + e-
I2 + X (g) X2+
(g) + e-
I3 + X (g) X3+
(g) + e-
I1 energi ionisasi pertama
I2 energi ionisasi kedua
I3 energi ionisasi ketiga
8.4
I1 < I2 < I3
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8.4
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Filled n=1 shell
Filled n=2 shell
Filled n=3 shell Filled n=4 shell
Filled n=5 shell
8.4
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Trend Umum pada Energi Ionisasi Pertama
8.4
Energi Ionisasi Pertama meningkat
En
erg
i Io
nis
asi P
ert
am
a m
en
ing
ka
t
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Afinitas Electron adalah negatif dari perubahan energi
yang terjadi ketika suatu elektron diterima oleh atom suatu
unsur dalam keadaan gas.
X (g) + e- X-(g)
8.5
F (g) + e- X-(g)
O (g) + e- O-(g)
DH = -328 kJ/mol EA = +328 kJ/mol
DH = -141 kJ/mol EA = +141 kJ/mol
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8.5
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8.5
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8.6
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Unsur-unsur Golongan 1A (ns1, n 2)
M M+1 + 1e-
2M(s) + 2H2O(l) 2MOH(aq) + H2(g)
4M(s) + O2(g) 2M2O(s) R
eaktifita
s m
enin
gkat
8.6
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Unsur-unsur Golongan 2A (ns2, n 2)
M M+2 + 2e-
Be(s) + 2H2O(l) Tidak Bereaksi
Reaktifita
s m
enin
gkat
8.6
Mg(s) + 2H2O(g) Mg(OH)2(aq) + H2(g)
M(s) + 2H2O(l) M(OH)2(aq) + H2(g) M = Ca, Sr, or Ba
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Unsur-unsur Golongan 3A (ns2np1, n 2)
8.6
4Al(s) + 3O2(g) 2Al2O3(s)
2Al(s) + 6H+(aq) 2Al3+
(aq) + 3H2(g)
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Unsur-unsur Golongan 4A (ns2np2, n 2)
8.6
Sn(s) + 2H+(aq) Sn2+
(aq) + H2 (g)
Pb(s) + 2H+(aq) Pb2+
(aq) + H2 (g)
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Unsur-unsur Golongan 5A (ns2np3, n 2)
8.6
N2O5(s) + H2O(l) 2HNO3(aq)
P4O10(s) + 6H2O(l) 4H3PO4(aq)
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Unsur-unsur Golongan 6A (ns2np4, n 2)
8.6
SO3(g) + H2O(l) H2SO4(aq)
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Unsur-unsur Golongan 7A (ns2np5, n 2)
X + 1e- X-1
X2(g) + H2(g) 2HX(g)
Reaktifita
s m
enin
gkat
8.6
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Unsur-unsur Golongan 8A (ns2np6, n 2)
8.6
ns dan subkulit np terisi sempurna.
Memiliki energi ionisasi tertinggi dari
seluruh unsur.
Tidak menunjukkan kecenderungan untuk
menerima ekstra elektron.
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Sifat-sifat Oksida dalam Satu Periode
basa asam
8.6
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Kimia dalam Kehidupan: Penemuan Gas Mulia
Sir William Ramsay 8.6
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1.
2.
3.
4.