1.2-sruktur atom-2
DESCRIPTION
Chimical EngineeringTRANSCRIPT
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Pokok Bahasan Materi
1. Teori atom Dalton
2. Partikel dalam atom
3. Perkembangan teori / model atom
4. Spektrum Atom
5. Bilangan kuantum
6. Bentuk orbital
7. Aturan konfigurasi elektron dalam atom
8. Sifat periodik Unsur
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Teori Atom Dalton 1.Materi terdiri dari partikel yang tidak dapat dibagi-
bagi lagi, tidak dapat diciptakan dan dimusnahkan, yang disebut atom.
Ternyata atom dapat dibagi lagi menjadi partikel-partikel yaitu elektron (e), proton (p), dan neutron (n).
2. Atom suatu unsur tertentu adalah sama dan berbeda dengan atom unsur lain.
Ternyata ada isotop yaitu unsur dengan lambang sama yang mempunyai nomor atom sama tetapi nomor massa berbeda.
3. Jika atom-atom bergabung membentuk senyawa, maka perbandingan atom-atom ini merupakan angka sederaha.
Ternyata ada molekul rumit, mis. 3
18 35 2C H O Na
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Perkembangan Teori/Model Atom
1. Becquerel:
atom terdiri dari bagian bermuatan positif dan bagian bermuatan negatif.
2. Thomson (konsep elektron):
atom berupa awan muatan positif yang bulat (seperti bola kapas) dengan elektron-elektron pada permukaannya.
99,9 % massa atom terletak pada bagian bermuatan positif.
3. Rutherford (konsep inti atom):
atom terdiri dari inti yang keras dan kecil (r = 10−13 cm) dengan muatan +Ze dan hampir semua massa atom terpusatkan serta pada jarak relatif jauh terdapat elektron-elektron sebanyak Z yang mengelilingi inti. Z = nomor atom
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4. Bohr (konsep orbital & kulit elektron):
(a) tiap elektron hanya dapat bergerak dalam lintasan-lintasan berbentuk lingkaran (disebut orbit) dan momentum sudut elektron dalam lingkaran merupakan kelipatan bulat dari h/2π.
Lintasan elektron yang tidak memancarkan energi dinamakan keadaan stasioner.
(b) bila elektron mancarkan / menyerap energi (yaitu pindah dari keadaan stasioner satu ke keadaan stasioner lain), maka energi yang dipancarkan / diserap adalah
ΔE = hν
Dari konsep Bohr ini dapat meramalkan potensial ionisasi, yaitu: ΔE= Z2. ΔEH
dengan ΔEH = 1312 kJ/mol. Persamaan ini hanya berlaku untuk atom berelektron satu
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Absorption And Emission
Electrons that absorb energy are raised to a higher energy level
A particular frequency of light is emitted when an electron falls to a lower energy level
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Bohr’s (theoretical) equation explains the
experimental (empirical) Rydberg equation
The combination of constants, b/hc, has a
value which differs from the experimentally
derived value of RH by only 0.05%!
22
22
22
1111
11
or
with
)(
hl
hl
lh
nnhcb
lhnn
n
b
n
blh
hc
nnb
EEE
Bohr’s Model Predicts Energy Levels
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This equation allows the calculation of the energy,
E, of any orbit
b= Bohr’s constant
n is the orbit location
J 102.18b
nbE
18
2
Bohr Equation (1913)
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J 102.18b
nbE
18
2
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The Electron On A Wire- Uniting The Theories
Particle: the kinetic energy of the moving
electron is E=½ mv2
Standing wave, the half-wavelength must occur
an integer number of times along the wire’s
length n(λ/2)=L
de Broglie’s equation provides the link between
these.
m=mass of particle
v= velocity of particle
Combining these relationships:
mvh λ
2
22
8mL
hnE
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5. Louis de Broglie (azas dualisme partikel gelombang):
bila satu partikel bergerak dengan momentum p,
maka gerakan ini dapat digambarkan sebagai
suatu gerakan gelombang dengan λ = h/p =
h/mv.
6. Heisenberg (azas ketidakpastian):
penentuan yang bersamaan dari momentum dan
kedudukan suatu partikel tidak dapat diketahui
secara tepat, (Δpx)(Δx)≥ h .
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7. Schrodinger :
momentum dan kedudukan tidak diberikan
sebagai harga-harga tertentu melainkan
sebagai kebolehjadian memiliki harga tertentu
yang disebut fungsi gelombang, ψ.
Fungsi gelombang dinyatakan oleh Ψnlm
Note: 5, 6, 7 disebut mekanika kuantum (konsep subkulit, bilangan
kuantum, dan orbital)
Orbiatal adalah daerah kebolehjadian untuk menemukan elektron
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Radiant Energy Spectrum
high energy,
short waves
low energy,
long waves
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Electromagnetic Spectrum
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Flame Emission
Elements exhibit characteristic colors when
burned
The characteristic spectra are also observed
when elements are subject to strong
electrical fields as in gas discharge tubes.
Note that the light
from the discharge
tube is actually
several different
colored lines as
seen on the
surface of the CD
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Light emitted by excited atoms is comprised of
a few narrow beams with frequencies
characteristic of the element
Atomic spectra are unique for each element
Atomic Emission Spectra
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7.3
Line Emission Spectrum of Hydrogen Atoms
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For the hydrogen spectrum, a mathematical
pattern was noted and reported using the Balmer-
Rydberg equation
n1 and n2 are positive integers , where n1 <n2
Rydberg constant, RH, is an empirical
constant=109,678 cm-1
If n1=1, lines called “Lyman series”
If n1=2, called “Balmer series”
If n1 = 3 called “Paschen series”
Emitted light is quantized )( 2
221
11H
1
nnR
Patterns In Atomic Line Spectra
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Ephoton = E = Ef - Ei
Ef = -RH ( ) 1
n2 f
Ei = -RH ( ) 1
n2 i
i f
E = RH ( ) 1
n2
1
n2
nf = 1
ni = 2
nf = 1
ni = 3
nf = 2
ni = 3
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Ephoton = 2.18 x 10-18 J x (1/25 - 1/9)
Ephoton = E = -1.55 x 10-19 J
= 6.63 x 10-34 (J•s) x 3.00 x 108 (m/s)/1.55 x 10-19J
= 1280 nm
Calculate the wavelength (in nm) of a photon
emitted by a hydrogen atom when its electron
drops from the n = 5 state to the n = 3 state.
Ephoton = h x c /
= h x c / Ephoton
i f
E = RH ( ) 1
n2
1
n2 Ephoton =
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Chemistry in Action: Laser – The Splendid Light
Laser light is (1) intense, (2) monoenergetic, and (3) coherent
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Chemistry in Action: Electron Microscopy
STM image of iron atoms
on copper surface
e = 0.004 nm
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Chemistry Mystery: Discovery of Helium
In 1868, Pierre Janssen detected a new dark line in the solar emission spectrum
that did not match known emission lines
In 1895, William Ramsey discovered helium in a mineral of uranium (from alpha
decay).
Mystery element was named Helium
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Schrodinger Wave Equation
Y fn(n, l, ml, ms)
principal quantum number n
n = 1, 2, 3, 4, ….
n=1 n=2 n=3
7.6
distance of e- from the nucleus
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Y = fn(n, l, ml, ms)
angular momentum quantum number l
for a given value of n, l = 0, 1, 2, 3, … n-1
n = 1, l = 0
n = 2, l = 0 or 1
n = 3, l = 0, 1, or 2
Shape of the “volume” of space that the e- occupies
l = 0 s orbital
l = 1 p orbital
l = 2 d orbital
l = 3 f orbital
Schrodinger Wave Equation
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l = 0 (s orbitals)
l = 1 (p orbitals)
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l = 2 (d orbitals)
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Y = fn(n, l, ml, ms)
magnetic quantum number ml
for a given value of l
ml = -l, …., 0, …. +l
orientation of the orbital in space
if l = 1 (p orbital), ml = -1, 0, or 1
if l = 2 (d orbital), ml = -2, -1, 0, 1, or 2
Schrodinger Wave Equation
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ml = -1 ml = 0 ml = 1
ml = -2 ml = -1 ml = 0 ml = 1 ml = 2 7.6
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Y = fn(n, l, ml, ms)
spin quantum number ms
ms = +½ or -½
Schrodinger Wave Equation
ms = -½ ms = +½
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Bilangan Kuantum
1. utama, n dengan n = 1, 2, 3,....
konsep: menunjukkan kulit elektron
fisik: menggambarkan ukuran orbital
2. momentum sudut / azimut, l dengan l = 0 s/d (n-1)
konsep: menunjukkan subkulit s, p, d, f, g,....
fisik: menggambarkan bentuk orbital
3. magnetik, m dengan m = (-l) s/d (+l)
konsep: menunjukkan orbital pada subkulit,
mis. px, py, pz
fisik: menggambarkan arah/orientasi orbital
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4. spin, s dengan s = ± ½
menunjukkan arah spin elektron
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Electron Spin: A Fourth Quantum Number
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Relationships between n, l, and m
Number of
n l ml Subshell Orbitals
1 0 0 1s 1
2 0 0 2s 1
1 -1, 0, 1 2p 3
3 0 0 3s 1
1 -1, 0, 1 3p 3
2 -2, -1, 0, 1, 2 3d 5
4 0 0 4s 1
1 -1, 0, 1 4p 3
2 -2, -1, 0, 1, 2 4d 5
3 -3, -2, -1, 0, 1, 2, 3 4f 7
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Schrodinger Wave Equation
Y = fn(n, l, ml, ms)
Shell – electrons with the same value of n
Subshell – electrons with the same values of n and l
Orbital – electrons with the same values of n, l, and ml
How many electrons can an orbital hold?
If n, l, and ml are fixed, then ms = ½ or - ½
Y = (n, l, ml, ½) or Y = (n, l, ml, -½)
An orbital can hold 2 electrons 7.6 11/09/2015 6:57:58 37 barnasholil/08122169961
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How many 2p orbitals are there in an atom?
2p
n=2
l = 1
If l = 1, then ml = -1, 0, or +1
3 orbitals
How many electrons can be placed in the 3d subshell?
3d
n=3
l = 2
If l = 2, then ml = -2, -1, 0, +1, or +2
5 orbitals which can hold a total of 10 e-
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Bentuk Orbital
1. Orbital s
n = 1, 2, .......
l = 0 z
m = 0
x
y
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Orbitals get larger as the principle quantum number n increases
Nodes, or regions of zero electron density, appear beginning with the 2s orbital
.
“s” Orbitals And Nodes
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s orbitals
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2. Orbital p
px py pz
n = 2, 3, ... n = 2, 3, ... n = 2, 3, ...
l = 1 l = 1 l = 1
m = +1 m =−1 m = 0
z z z
x x x
y y y
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Recall that there are three different
orbitals in each p subshell
Dot-density diagrams of the
cross section of the probability
distribution of a single (a) 2p
and (b) 3p orbital showing the
nodal plane.
The directions of maximum electron
density lie along lines that are mutually
perpendicular. It is convenient to label the
orbitals as px, py, and pz
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p Orbitals
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p Orbitals
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3. Orbital d
dxy dxz dyz
n = 3, 4, .. n = 3, 4, .... n = 3, 4, ...
l = 2 l = 2 l = 2
m = -2 m = +1 m = -1
z z z
x x x
y y y
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dx2−y2 dz2
n = 3, 4, ... n = 3, 4, ...
l = 2 l = 2
m = +2 m = 0
z z
x x
y y
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Shape and orientation of d orbitals are more complicated than for p orbitals.
“f” orbitals are even more complex than the d orbitals
“d” Orbital Shape and Orientations
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d Orbitals
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Aturan konfigurasi elektron
1. Aturan Aufbau: (n+l)
pengisian elektron pada orbital dimulai dari
subkulit dengan energi terendah
tingkat energi
50
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 5g
n 1 2 2 3 3 3 4 4 4 4 5 5 5 5 5
l 0 0 1 0 1 2 0 1 2 3 0 1 2 3 4
n+l 1 2 3 3 4 5 4 5 6 7 5 6 7 8 9
urutan 1 2 3 4 5 7 6 8 10 13 9 11 14
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1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f 5g
6s 6p 6d 6f 6g 6h
7s 7p 7d 7f 7g 7h 7i
51
1
2 3
4 5
6
7
8
9
10
11
12
13
14
15
16
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Orbital Filling
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Order of orbitals (filling) in multi-electron atom
1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s
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How Do Quantum Numbers Relate to Each Other?
En
erg
y
2
3
4
p
p
s
4 5 p d
•n
•l
•ml 1
3
4
5
p s
s
s
s
2
3 d
0 -1 0 +1
-2 -1 0 +1 +2
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The approximate energies of the subshells in an
atom with more than one electron:
Electrons behave like tiny magnets
The quantum numbers
associated with the first
two shells are shown.
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2. Azas larangan Pauli
tiap orbital diisi paling banyak dua elektron dengan arah spin yang berlawanan
3. Aturan Hund
pengisian elektron pada subkulit yang sama diisi tidak berpasangan terlebih dahulu kemudian diisi kembali menjadi berpasangan
4. Aturan orbital penuh dan setengah penuh
konfigurasi elektron yang stabil terdapat pada pengisian penuh atau setengah penuh
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Electron Configurations
Aufbau process.
Build up and minimize energy.
Pauli exclusion principle.
No two electrons can have all four quantum
numbers alike.
Hund’s rule.
Degenerate orbitals are occupied singly first.
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Orbital Energies
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59
EPOT
1s
2s
3s
4s
2p
3p
3d
Each arrow represents an electron
1s2 2s2 2p6 3s2 3p6 4s2 3d3
Orbital Diagram & e-configurations - V
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Electron Configurations and the Periodic Table
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Outermost subshell being filled with electrons
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Sifat Periodik Unsur
1. Potensial ionisasi, IE, EI, I
adalah energi yang diperlukan untuk melepaskan satu elektron dari atom atau ion dalam keadaan gas.
M(g) → M+(g) + e− I1
M+(g) → M2+
(g) + e− I2
M2+(g) → M3+
(g) + e− I3
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Faktor-faktor yang mempengaruhi nilai potensial
ionisasi
jari-jari atom
muatan inti
efek sekatan orbital penuh atau setengah penuh
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64
unsur
konfigurasi
Potensial ionisasi, kkal/mol
I1 I2 I3
10Ne 1s2 2s2 2p6 497,2 947,2 1500,0
11Na 1s2 2s2 2p6 3s1
118,5 1091,0 1652,0
12Mg 1s2 2s2 2p6 3s2
176,3 346,6 1848,0
13Al 1s2 2s2 2p6 3s2 3p1 138,0 434,1 655,9
14Si 1s2 2s2 2p6 3s2 3p2 187,9 376,8 771,9
15P 1s2 2s2 2p6 3s2 3p3 254,2 453,2 695,5
16S 1s2 2s2 2p6 3s2 3p4 238,9 540,0 807,0
17Cl 1s2 2s2 2p6 3s2 3p5 300,0 548,9 920,2
18Ar 1s2 2s2 2p6 3s2 3p6 363,4 637,0 943,3
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Gol I A I, eV
Li 5,39
Na 5,14
K 4,34
Rb 4,18
Cs 3,89
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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
Variation of the First Ionization Energy with Atomic Number
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General Trend in First Ionization Energies
8.4
Increasing First Ionization Energy
Incre
asin
g F
irst
Ion
iza
tio
n E
ne
rgy
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Trends in IE
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Variations in
successive
ionization energies.
Note that it is
extremely difficult to
break into the noble
gas core (2nd
through 8th
ionizations for Li
through F,
respectfully.
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Irregularities in I.E.
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2. Jari-jari atom ... ditentukan dengan sinar X
adalah setengah jarak antara dua atom yang
terikat oleh ikatan tunggal kovalen
atau
jarak antara inti atom dengan elektron paling
luar
Jari-jari ion positif lebih kecil dari jari-jari atomnya
(berkurangnya sangat besar)
Jari-jari ion negatif lebih besar dari jari-jari atomnya
(bertambahnya sangat besar)
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Ion vs. Atom Radii
Positive ions are always
smaller than the atoms from
which they are formed
due to decreased shielding
effects
Negative ions always larger
than the atoms from which
they are formed
due to increased electron
repulsion
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Trends In Atomic and Ionic Radii (pm)
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Atomic Radii
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8.3
Comparison of Atomic Radii with Ionic Radii
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Cation is always smaller than atom from
which it is formed.
Anion is always larger than atom from
which it is formed.
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8.3
The Radii (in pm) of Ions of Familiar Elements
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3. Afinitas elektron, EA, AE, A
adalah energi yang dilepaskan / diperlukan bila suatu atom atau ion dalam keadaan gas menerima satu elektron.
X(g) + e− → X−(g) A1
X−(g) + e− → X2−(g) A2
Addition of one electron to a neutral atom is exothermic for nearly all atoms
Addition of subsequent electrons always requires energy
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In general, electron affinity:
increases (as an exothermic value) from left to
right in a period
increases (as an exothermic value) bottom to
top in a group
Trends in Electron Affinity
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8.5
Variation of Electron Affinity With Atomic Number (H – Ba)
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A, kJ/mol
Cl(g) + e− → Cl−(g) −349
O(g) + e− → O−(g) −141
O−(g) + e− → O2−(g) +844
Jika suatu atom/ion mempunyai nilai afinitas besar maka atom/ion tersebut makin stabil
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A, eV
F 3,45
Cl 3,61
Br 3,36
I 3,06
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4. Kemagnetan
sifat magnet ditentukan oleh jumlah elektron
tidak berpasangan.
Diamagnetik: tidak ditarik magnet bahkan
kadang-kadang agak ditolak (tidak memiliki elektron
yang tidak berpasangan / semua elektron berpasangan)
Paramagnetik: ditarik magnet dengan lemah.
Feromagnetik: ditarik magnet dengan kuat.
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Perkiraan nilai momen magnetik
μ =
μ = momen magnetik, dalam Bohr magneton
n = jumlah elektron tidak berpasangan
1 BM = 9,273 erg/gauss
88
n n 2
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Paramagnetic
unpaired electrons
2p
Diamagnetic
all electrons paired
2p
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.
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Group 1A Elements (ns1, n 2)
M M+1 + 1e-
2M(s) + 2H2O(l) 2MOH(aq) + H2(g)
4M(s) + O2(g) 2M2O(s)
Incre
asin
g r
eactivity
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Group 1A Elements (ns1, n 2)
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Group 2A Elements (ns2, n 2)
M M+2 + 2e-
Be(s) + 2H2O(l) No Reaction
Incre
asin
g r
eactivity
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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Group 2A Elements (ns2, n 2)
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Group 3A Elements (ns2np1, n 2)
8.6
4Al(s) + 3O2(g) 2Al2O3(s)
2Al(s) + 6H+(aq) 2Al3+
(aq) + 3H2(g)
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Group 3A Elements (ns2np1, n 2)
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Group 4A Elements (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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Group 4A Elements (ns2np2, n 2)
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Group 5A Elements (ns2np3, n 2)
8.6
N2O5(s) + H2O(l) 2HNO3(aq)
P4O10(s) + 6H2O(l) 4H3PO4(aq)
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Group 5A Elements (ns2np3, n 2)
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Group 6A Elements (ns2np4, n 2)
8.6
SO3(g) + H2O(l) H2SO4(aq)
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Group 6A Elements (ns2np4, n 2)
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Group 7A Elements (ns2np5, n 2)
X + 1e- X-1
X2(g) + H2(g) 2HX(g)
Incre
asin
g r
eactivity
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Group 7A Elements (ns2np5, n 2)
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Group 8A Elements (ns2np6, n 2)
8.6
Completely filled ns and np subshells.
Highest ionization energy of all elements.
No tendency to accept extra electrons.
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Properties of Oxides Across a Period
basic acidic
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Chemistry in Action: Discovery of the Noble Gases
Sir William Ramsay
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Reaksi yang memiliki perubahan entalpi standar, ΔHo,
paling kecil adalah
(A) Li(g) → Li+(g) + e−
(B) Na(g) → Na+(g) + e−
(C) K(g) → K+(g) + e−
(D) Mg(g) → Mg+(g) + e−
(E) Ca(g) → Ca+(g) + e−
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Urutan energi-energi ionisasi (pertama, kedua,
dst) dalam kJ/mol untuk unsur X adalah 740,
1500, 7700, 10500, 13600, 18000, 21700. Ion
manakah yang akan terbentuk jika X bereaksi
dengan klor ?
(A) X2−
(B) X−
(C) X+
(D) X2+
(E) X3+
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Jika energi ionisasi atom hidrogen adalah 13,6
eV/atom, maka energi ionisasi kedua atom helium
adalah
(A) 13,6 eV
(B) 54,4 eV
(C) 122,4 eV
(D) 217,6 eV
(E) 340,0 eV
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Jika energi ionisasi atom hidrogen adalah 13,6
eV/atom, maka energi ionisasi kelima bagi atom
boron adalah
(A) 27,2 eV
(B) 68,0 eV
(C) 136,0 eV
(D) 272,0 eV
(E) 340,0 eV
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Potensial ionisasi Li2+ → Li3+ + e− adalah 11.810
kJ/mol. Nilai potensial ionisasi F8+ → F9+ + e−
adalah
(A) 83.982 kJ/mol
(B) 47.240 kJ/mol
(C) 106.290 kJ/mol
(D) 115.862 kJ/mol
(E) 64.299 kJ/mol
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Energi ionisasi X(g) → X+(g) + e−
O 4700 kJ/mol
S 3260 kJ/mol
Ca 1740 kJ/mol
Energi ionisasi untuk Se adalah
(A) 1410 kJ/mol
(B) 3020
(C) 3280
(D) 4240
(E) 6260
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Ujian-1: 8 Oktober 2010
Berikut adalah tabel energi ionisasi pertama,
kedua, dan ketiga dari beberapa unsur pada
perioda ketiga yang belum teridentifikasi. Gunakan
informasi pada tabel ini untuk menjawab soal-soal
dibawah.
114
Unsur Energi Ionisasi I
(kJ/mol)
Energi Ionisasi II
(kJ/mol)
Energi Ionisasi III
(kJ/mol)
W 1251 2300 3820
X 496 4560 6910
Y 738 1450 7730
Z 1000 2250 3360
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a. Tuliskan unsur yang karakter logamnya paling
tinggi.
b. Perkirakan termasuk dalam golongan berapa
unsur Y pada tabel periodik modern.
c. Tuliskan lambang unsur X.
d. Manakah dari keempat unsur diatas yang
memiliki jari-jari atom paling kecil.
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Afinitas elektron pertama unsur Cl berkaitan dengan proses
(A) Cl2(g) + 2e− → 2Cl−(g)
(B) ½Cl2(g) + e− → Cl−(g)
(C) Cl(g) + e− → Cl−(g)
(D) Cl2(g) + 2e− → Cl2−(g)
(E) Cl2(g) + 2e− → 2Cl−(l)
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