Download Chemistry M.4 Lesson 1 Atom and Periodic Table

Vocabulary
Chemistry M.4
Lesson 1
Atom and Periodic Table
by Angka Teprattananan
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conclude
conductivity
matter
divide
agree
made up
theory
compose
destroy
combine
definite
voltage
pressure
electric current
electric field
negative
charge to mass
appear
discover
positive
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Greek Model
 Over 2,000 years ago Democritus concluded that
matter could not be divided into smaller and smaller
pieces forever
 Named the smallest piece “atomos”
Democritus
¨oˏ¹ ´oŵa¹
( John Dalton )
(c460-371 BC)
Aristotle
(384-322 BC)
 But Aristotle didn’t agree with the concept of
atoms.
 Aristotle thought the earth was composed of
matter - which made up of four elements:
 “earth, air, fire, and water”.
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Dalton’s Atomic model
1. All elements are composed of atoms.
It is impossible to divide or destroy an atom.
2. All atoms of the same elements are
alike.
3. Atoms of different elements are
different.
4. Different atoms combine to form a
compound in definite whole number ratios.
e.g. H2O , CO2 (Expect Na ,H2 , Br2 , P4 , S8)
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(Dalton’s atomic model)
J.J. Thomson
e¨ e¨ ·oÁÊa¹
(J.J. Thomson)
oaµoÁÁÕû٠Ëҧe»š¹·Ã§¡ÅÁ ÁÕ¢¹Ò´eÅç¡
äÁ‹ÊÒÁÒö溋§æ¡æÅaÊÙ­ËÒÂ䴌
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Passing an electric current makes a beam appear to
move from the cathode to the anode end.
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‐
OFF
– Discovered by Eugen Goldstein
– He observed “Canal rays” and found that they
are composed of positive particles – Proton.
voltage source
+
6
Discovery of the Proton
Thomson’s Experiment
ON
Studied electrical conductivity of gases
by using a cathode ray tube in high voltage and
low pressure.
+
Eugen Goldstein
‐
By adding an electric field ,
he found that the moving pieces were negative.
And negative particle was called “Electron”
Thomson was able to measure the charge to
mass ratio of the electron
q/me = 1.76 x 108 coulombs/gram
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Canal Rays
¨Ò¡¡Ò÷´Åo§¢o§o¡Å´Êäµ¹ ÊÃu»ä´ŒÇ‹Ò
- Ãa§ÊպǡËÃืoo¹uÀÒ¤ºÇ¡e¡i´¨Ò¡æ¡Ê·ÕèºÃèuÀÒÂã¹ËÅo´Ãa§ÊÕ
æ¤o·´ «ึè§eºÕÂè §eº¹e¢ŒÒËÒ¢aéÇź䴌·aé§ã¹Ê¹ÒÁä¿¿‡ÒæÅaʹÒÁæÁ‹eËÅç¡
- Ãa§ÊպǡÁդҋ oaµÃÒʋǹ»Ãa¨uµ‹oÁÇÅäÁ‹¤§·Õè ¢ึé¹oÂً¡aºª¹i´¢o§
桍ʷÕèºÃèuoÂًÀÒÂã¹ËÅo´Ãa§ÊÕæ¤o·´
- ¶ŒÒe»ÅÕÂè ¹æ¡Êe»š¹äÎo´Ãe¨¹ ¨a¾ºÇ‹Òo¹uÀÒ¤ºÇ¡·Õèe¡i´¢ึ鹨aÁÕ
¤‹Ò»Ãa¨ue·‹Ò¡aºoieÅ硵Ão¹¾o´Õ ¨ึ§eÃÕ¡o¹uÀÒ¤ºÇ¡¹ÕéÇ‹Ò “o»Ãµo¹”
Canal Rays passed through holes, or channels, in
the reverse direction as the cathode ray.
_
cathode
_
anode
+
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Mass of the Electron
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Calculate mass of the Electron
1. charge to mass ratio = 1.76x108 coulombs/gram
2. charge of electron: = 1.60 x 10-19 g
The oil drop apparatus
Millikan determines the charge of the electron : 1.60 x 10-19 C
and the mass of the electron: 9.1 x 10-28 g
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Thomson’s Atomic Model
Vocabulary
(Plum Pudding Model)
“oaµoÁe»š¹·Ã§¡ÅÁ »Ãa¡oº´ŒÇÂo»Ãµo¹·ÕèÁÕ»Ãa¨uºÇ¡æÅaoieÅ硵Ão¹
·ÕèÁÕ»Ãa¨uźoÂًo‹ҧ¡Ãa¨a´¡Ãa¨Ò æÅaÊíÒËÃaºoaµoÁ·Õèe»š¹¡ÅÒ§·Ò§
ä¿¿‡Ò¨aÁÕ¨íҹǹo»Ãµo¹e·‹Ò¡aº¨íҹǹoieÅ硵Ão¹¾o´Õ”
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Discovery of Nucleus
Ernest Rutherford
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 Tested Thomson’s model of atomic
structure with the “gold foil” experiment.
 Bombarded thin gold foil with a beam of
“alpha” particles.
 If the positive charge was evenly
spread out, the beam should have easily.
passed through.
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bombarded
emit
experiment
symbol
gold foil
spread out
passed through
refract
reflect
empty space
distribute
occupy
atomic number
mass number
subatomic
particle
equal
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 Most of the particles passed through
 A few particles were refracted
 VERY FEW were greatly reflected
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 Based on his experimental
evidence:
 The atom is mostly empty
space
 All the positive charge, and
almost all the mass is in a small
area in the center. He called
this a “nucleus”
 The electrons distributed around
the nucleus, and occupy most of
the volume
 His model was called a “nuclear
model”
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Rutherford's Atomic Model
“oaµoÁ»Ãa¡oº´ŒÇ¹iÇe¤ÅÕÂÊ«ึè§ÁÕ»Ãa¨uºÇ¡(o»Ãµo¹)oÂًµÃ§¡ÅÒ§
ÁÕ¢¹Ò´eÅç¡ÁÒ¡æÅaÁÕÁÇÅÁÒ¡ ʋǹoieÅ硵Ão¹·ÕèÁÕ»Ãa¨uźæÅaÁÕÁÇŹŒoÂ
e¤Åืoè ¹·ÕèÃoº¹iÇe¤ÅÕÂÊe»š¹ºÃiedz¡ÇŒÒ§"
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The Discovery of the Neutron
 Chadwick bombarded alpha particles at
Beryllium.
 Neutrons were emitted and in turn hit parafin
and ejected protons from the parafin.
 Neutrons have mass similar to protons.
 No electrical charge.
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The Subatomic particles
Subparticle
James Chadwick
electron
proton
neutron
symbol
e
p
n
charge
-1
+1
0
mass(g)
9.1x10-27
1.67x10-24
1.67x10-24
mass(amu)
0.0005
1.0072
1.0086
THE MASS OF THE NEUTRON IS 1839 times greater than an electron.
Composition of the Nucleus:
• nuclei are composed of "nucleons": protons and neutrons
• atomic mass units: 1 amu = exactly 1/12 the mass of a carbon12 nucleus
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¤ÇÒÏ¡ ¤ืo o¹uÀÒ¤·ÕèeÅç¡·ÕèÊ´u e·‹Ò·ÕèÁÕ¡ÒÃÂoÁÃaº »˜¨¨uºa¹ÁÕ ¡Ò䌹¾º
¤ÇÒÏ¡ 6 µaÇ ¤ืo up quark, down quark, strange quark, charmed
quark, bottom quark æÅa top quark
- ¹iǵÃo¹ »Ãa¡oº´ŒÇ up quark 1 µaÇ æÅa down quark 2 µaÇ
- o»Ãµo¹ »Ãa¡oº´ŒÇ up quark 2 µaÇ æÅa down quark 1 µaÇ
Atomic Symbol (Nuclear Symbol)
• Contain the symbol of the element, the mass number
and the atomic number.
Mass
number
A
Atomic
number
Z
Element Symbol
X
• Atomic number = number of protons
– Same as the number of electrons in a neutral atom
• Mass number = the number of protons + neutrons
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9
4Be
14
6C
35
17Cl
74
33As
3- 44
20Ca
2+ 67
3+
31Ga
Atomic Number
Mass Number
# of Protons
# of Neutrons
• Isotope are atoms of the same element having
different masses, due to varying numbers of
neutrons.
1 H Subatomic particles
p=1 ,e=1 , n=0
1
2 H Subatomic particles
p=1 ,e=1 , n=1
1
• Isotone are atoms of the different element having
equal neutrons.
11 B Subatomic particles
p=5 ,e=5 , n=6
5
12 C Subatomic particles
p=6 ,e=6 , n=6
6
# of Electrons
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Isotope , Isotone , Isobar and Isoelectronic
Fill in the blanks for the following nuclear symbols:
Element
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For each of the following ,check the blank for
isotope , isotone , isobar or isoelectronic
• Isobar are atoms of the different element having
equal mass number.
36 S
mass no. of 3616S is 36
16
36 Ar mass no. of 36 Ar
is 36
18
18
Neclear symbols
14
20
10Ne
24 Mg2+
12
Subatomic particles
Subatomic particles
p = 10 , e = 10 , n = 10
p = 12 , e = 10 , n = 12
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&
excited State
electromagnetic
wave
relationship
wavelength
frequency
energy
ground State
describe
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Max Plank
energy levels
quantize
less-stable
absorbing
releasing
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isotone
isobar
isoelectronic
7N
19K
Vocabulary
spectrum
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& 4020Ca
35 Cl & 37 Cl
17
17
38 Ar & 32 S218
16
16 O & 18 O
8
8
40 Ar & 40 Ca
18
20
35 Cl- & 39 K+
17
19
31 P & 32 S
15
16
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• Isoelectronic are atoms of the different element
having equal electron.
6C
isotope
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Max Plank
studied a spectrum of Electromagnetic
Wave. The relationship among the wavelength
(λ), the frequency (ν), and the energy (E)
are:
or
where c is Speed of light = 3 x 108 m/s
h is Planck's Constant = 6.626 x 10-34 J.s
is Frequency (Hz)
λ is wavelength (m)
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Energy and frequency of Electromagnetic Wave
Color of spectrum
Violet
Blue
Green
Yellow
Orange
Red
Wavelength (nm)
400
420
490
580
590
650
-
420
490
580
590
650
700
Energy (kJ)
4.96x10-22
4.73x10-22
4.05x10-22
3.42x10-22
3.36x10-22
3.05x10-22
-
4.73x10-22
4.05x10-22
3.42x10-22
3.36x10-22
3.05x10-22
2.83x10-22
Calculate about Electromagnetic Wave
Ex1 Êe»¡µÃaÁÊÕÁ‹Ç§¤ÇÒÁÂÒǤÅืè¹ 500 nm ¨aÁÕ¤ÇÒÁ¶Õèe·‹Òã´
frequency(Hz)
7.49x1014 - 7.14x1014
7.14x1014 - 6.12x1014
6.12x1014 - 5.17x1014
5.17x1014 - 5.08x1014
5.05x1014 - 4.16x1014
4.61x1014 - 4.28x1014
Ex2 Êe»¡µÃaÁÊÕæ´§ÁÕ¤ÇÒÁÂÒǤÅืè¹ 500 nm ¨aÁÕ¤ÇÒÁ¶ÕèæÅa¾Åa§§Ò¹e·‹Òã´
Êe»¡µÃaÁ ¤ืo 涺ÊÕ·Õèe¡i´¨Ò¡¡ÒÃe»ÅÕè¹æ»Å§¾Åa§§Ò¹¢o§¤Åื¹è
æÁ‹eËÅç¡ä¿¿‡Ò
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Niels Bohr
 studied a spectrum of Hydrogen atom.
 discovered the four lines of Hydrogen
spectrums Violet , Blue , Blue-green ,and
Red.
Ex3 The energy of electromagnetic wave is 3x10-22 KJ ,
Find the color
Niels Bohr
Ex4 The frequency is 5x1014 Hz , calculate the wavelength ,
energy and find the color of this spectrum.
How did the spectrum appear ?
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Bohr used the term energy levels (or shells) to
describe. He said that the energy of an electron is
quantized, meaning electrons can have one energy
level or another but nothing in between.
The energy level an electron normally occupies
is called “ground state”. But it can move to a higherenergy (less-stable) by absorbing energy. This
higher-energy is called “excited state”.
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After it’s done being excited, the electron can
return to its original ground state by releasing the
energy it has absorbed, as shown in the diagram
below.
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35
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• Table show the energy of Hydrogen spectrum
Color of
Spectrum
Wavelength
(nm)
Energy
(kJ)
Red
656
3.02 x 10-22
Δ
E
10.6 x 10-23
Bluegreen
486
4.08 x 10-22
4.9 x 10-23
Blue
434
4.57 x 10-22
2.7 x 10-23
Violet
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410
4.84 x 10-22
Bohr’s Atomic Model
Electron Configuration (o¤Ã§æººoieÅ硵Ão¹)
Electrons orbit the nucleus in definite principle
energy levels (7 principle energy levels).
The principle energy level can hold only a specific
number of electrons.
Rule ; 2n2
n=
oaµoÁ»Ãa¡oº´ŒÇÂo»Ãµo¹æÅa¹iǵÃo¹ oÂًÀÒÂã¹¹iÇe¤ÅÕÂÊ
ʋǹoieÅ硵Ão¹Çi§è oÂًÃoº æ ¹iÇe¤ÅÕÂÊe»š¹ªa¹é æ ËÃืoe»š¹Ãa´aº¾Åa§§Ò¹«ึè§
ÁÕ¤‹ÒäÁ‹µ‹oe¹ืèo§¡a¹
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Principle energy levels
n
n
n
n
n
n
n
=
=
=
=
=
=
=
1
2
3
4
5
6
7
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Rule; Arrangements of electrons in an atom.
Maximum Electrons
1. Lowest levels are filled first.
2. Once a level is full, the electrons start filling
the next level.
3. Outer level (valence electrons) has maximum
electrons equal 8 and next outer level has maximum 8 or
18 electrons.
e.g. 11Na: has 11 electrons
2e
8e
18 e
32 e
50 e
72 e
98 e
 First energy level 1 (n =1)
can fill
2 electrons
 Second energy level 2 (n =2) can fill
8 electrons
 Third energy level 3 (n =3)
1 electron
 Or shot hand
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principle energy levels
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11Na
can fill
: 2,8,1
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Arrangements of electrons in an atom.
1. 3Li :
2. 12Mg :
3. 19K :
4. 33As :
5. 53I :
6. 55Cs :
7. 82Pb :
8. 88Ra :
9. 22Ti :
10. 28Ni :
Vocabulary
………………………………………
………………………………………
………………………………………
………………………………………
………………………………………
………………………………………
………………………………………
………………………………………
………………………………………
………………………………………
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explain
surround
electron cloud
closest
outermost
impossible
exact location
predict
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Electron Cloud Model
Modern Atomic model
 Electrons with the lowest
energy are found in the energy
level closest to the nucleus.
 Electrons with the highest
energy are found in the
outermost energy levels,
farther from the nucleus.
 It is impossible to determine
the exact location of an
electron only predict where is
could be based on how much
energy it has.
Bohr’s model could not explain complex atoms(can
explain Hydrogen atom only).
Atom has a small positively
charged nucleus surrounded
by a region of negatively
charged electrons to make
the entire atom neutral.
called the “electron cloud”.
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sub-energy
levels
exclusion
principle
spin
unpair
configuration
notation
indicate
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Erwin
Schrodinger
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The region of electrons move around the
nucleus in other shapes, called “Orbital”
There are 4 kind of orbitals (sub-energy levels)
e.g. s , p , d and f
s
p
d
f
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Arrangements of electrons in Orbital
principle energy levels
sub-energy levels
maximum electron
(shell)
n = 1
(subshell)
s
2
n = 2
s,p
8
n = 3
s,p,d
18
n = 4
s,p,d,f
32
n = 5
s,p,d,f
32
n = 6
s,p,d
18
n = 7
s,p
8
n = 8
s
2
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Electron configurations
By using ,
1. Pauli exclusion principle;
Each orbital can have only 2 electrons and have
not the same spin.
2. Aufbau principle;
Electron fill lowest energy levels first.
3. Hund’s Rule;
For atoms in ground state, the number of unpaired
electrons is the maximum possible and have the same
spin.
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Lower energy
Higher energy
1s 2s 2p 3s 3p 4s 3d 4p ….
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Ex. Give the full electron configuration of 27Co
Chemists use a standard notation to indicate the
electron configurations of atoms and molecules.
1) Orbital Diagram.
4d

1s
5S
4P
3d
2) Long notation or spdf configuration.
1s22s22p63s2....
3) Shorthand Notation or noble gas core.
[Ne]3s23p4
4S
3P
NOTE.
principle energy levels
Or 27Co;
3S
2P
2S
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1S
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Using Orbital Diagram
1. 3Li :
……
2S
12Mg
3.
18Ar
4.
19K
5.
25Mn
:
……………………………………………………
6.
26Fe
:
……………………………………………………
7.
24Cr
:
……………………………………………………
:
……………………………………………………
……………………………………………………
:
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Using Long Notation or spdf configuration
1. 12Mg : ……1s2 2s2 2p6 3s2………
2. 18Ar : ……………………………………………
3. 19K :
……………………………………………
4. 33As : ……………………………………………
5. 38Sr : ……………………………………………
6. 55Cs : ……………………………………………
7. 28Ni : ……………………………………………
8. 24Cr : ……………………………………………
9. 29Cu : ……………………………………………
………….…
2.
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:
1S

2s
……………………………………………………
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Using Short hand
1. 3Li :
2. 12Mg :
3. 18Ar :
4. 19K :
5. 33As :
6. 28Ni :
7. 37Rb :
8. 53I :
Notation or Noble Gas core.
………… [He]2s1 …………
………………………………………………
………………………………………………
………………………………………………
………………………………………………
………………………………………………
………………………………………………
………………………………………………
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The History of the
Periodic Table
(ÇiÇa²¹Ò¡Òâo§µÒÃÒ§¸Òµu)
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Vocabulary
similar property
conductor
middle element
roughly
publish
organize
increasing
regular
interval
according to
clear up
electricity
luster
ductile
malleable
reflect
except
semiconductor
stair step
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Johaun Dobereiner
Cl
Br
I
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He noticed that chlorine, bromine and iodine had
similar properties. And the atomic mass of the
middle element was roughly the average of the
masses of the others .
He called “Law of Triads”
Chlorine mass = 35.5
Bromine mass = 79.9
Iodine mass = 126.9
Average mass of chlorine and iodine
= (35.5 + 126.9) / 2
= 81.9 (close to Br!)
Dobereiner’s other triads included lithium (Li), sodium
(Na) and potassium (K), along with calcium (Ca), strontium (Sr)
and barium (Ba).
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He noticed that every 8th element had similar
properties, a bit like a musical scale. He listed some
of the known elements in rows of 7 as shown below.
He called “Law of Octaves” .
John Newlands
Dmitri Mendeleev
 In 1869 he published a table of the elements
organized by increasing atomic mass.
 Noticed similar properties appeared at regular
intervals --> “periodic”
Mendeleev
Lothar Meyer
 At the same time, he published his
own table of the elements
organized by increasing atomic
mass.
Lothar Meyer
His law of octaves work today with the first 20 elements.
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58
The table below compares Mendeleev’s prediction with
the actual data.
Mendeleev’s discovery
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Modern Periodic Table
Henry mosely
The Periodic Table was then arranged
according to increasing atomic number.
Henry mosely
The table was as it is now and cleared up the
Tellurium and Iodine problem.
 Periodic Law : the physical and chemical
properties of elements are periodic functions
of their atomic number and electrons
arrangement.
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Three classes of elements are Metals,
Nonmetals and Metalloids
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Metal Elements
Nonmetal Elements
 Good conductors of heat and electricity
 Have luster, are ductile , malleable , good reflect light
 All metals are solids at room temperature ,except for
mercury(Hg)
 Found on left side of periodic table and some on right
side of table
 Have properties that are opposite to those of metals
 Not good conductors of heat and electricity, poor
reflect light
 Usually brittle solids or gases ,except for bromine(Br)
 Found on right side of periodic table – AND hydrogen
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Gold
Sulphur
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Bromine
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Some properties of Metalloids , Al(metal) and I(nonmetal)
Metalloids




IE1
Sometimes called semiconductors
Form the “stairstep” between metals and nonmetals
Have properties of both metals and nonmetals
Examples: B, Si , Ge , As , Sb, Te and, At
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(kJ/mol)
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- B Si Ge As Sb Te Po At have high first
ionization energy(IE1) , electronegativity (EN) and can
form Ionic and Covalent compounds same nonmetals.
- High melting point and boiling point , high
density and can electrical conductivity same metals.
- So this elements will called “Metalloids”
(Po and At is radioactive element)
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Al
B
584
807
Si
793
Ge
As
Sb
I
768
951
840
1015
Type of
EN Density melting–boiling Electical
o
(g/cm3)
Conductivity
Compound
point( C)
1.61 2.70
660-2519
ionic
√
2.04 2.34
2075-4000
ionic and covalent
√
1.90 2.33
1414-3265
ionic and network
√
covalent
2.01 5.32
938-2833
ionic and covalent
√
2.18 5.75
358-603
ionic and covalent
√
2.05 6.68
631-1587
ionic and covalent
√
2.66 4.93
114-184
X
ionic and covalent
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Location of Hydrogen in the periodic table
Some properties of Hydrogen , group IA and
properties
Group IA
H
1. # valence electron
1
1
2. Oxidation number in
+1
+1 , -1
compounds
3. IE1 (kJ/mol)
382-526
1318
4. EN
0.7-1.0
2.1
5. phase
solid
gas
6. Electric conductivity
can
cannot
VIIA
group VIIA
7
+1 , +3 , +5
+7 , -1
1015-1687
2.2 -4.0
3 phase
cannot
chemist will arrange Hydrogen in group IA and VIIA
in the periodic table.
68
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Periodic Table
Vocabulary
vertical
gain
horizontal
consist
shiny
silvery
react
characteristic
flame
soluble
encounter
discharge
pale
diatom
monoatom
inert gases
incapable
synthesis
order
digit
The elements in same
group of the periodic table
have similar physical and
chemical properties!
The vertical columns of the periodic table are
called GROUP, or FAMILY. (18 groups)
69
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70
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Periodic Table
Periodic Table
The s and p block elements are called
“REPRESENTATIVE ELEMENTS (Group A)”
The d and f block elements are called
“TRANSITION ELEMENTS (Group B)”
s
p
d
The horizontal rows of the periodic table are
called PERIOD.(7 periods)
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71
f
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72
REPRESENTATIVE ELEMENTS
(Group A ; 8 groups)
Alkali Earth Metals
Halogens
Group IA (Alkali Metals)
Noble Gases
Inert Gases
Alkali Metals
73
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• Alkali Metals can react with oxygen to give
different oxide compounds :
4Li(s) + O2(g)  2Li2O(s)
Group I metals are shiny , silvery solids.
All are soft and can easily cut with a knife.
Have low density.
react easily in air. They are kept under oil.
Group I elements are called “alkali metals” because
they react with water to give alkaline solution.
e.g.
2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
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Group IIA (Alkali Earth Metals)
• Alkali Earth Metals have higher density than Alkali
Metals
• carbonate , phosphate , sulphid , sulphite compounds
of Alkali Earth Metal cannot soluble in water.
• Be does not react with water , Mg react slowly with
water and Ca and the elements below it react
readily with water:
Mg(s) + 2H2O(l)  Mg(OH)2(aq) + H2(g)
Ca(s) + 2H2O(l)  Ca(OH)2(aq) + H2(g)
(oxide)
2Na(s) + O2(g)  Na2O2(s) (peroxide)
K(s) + O2(g)  KO2(s) (superoxide)
• Alkali Metals emit a characteristic color when
placed in a flame.
• All alkali compounds can soluble in water.
• Group I elements become more reactive down the
group.
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•
•
•
•
•
75
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76
Group VIIA (Halogens)
Group VIA (Chalcogen)
• Oxygen , Sulphur and Selenium are nonmetals ,
Tellurium is Metalloid and Polonium is radioactive
element.
• Oxygen is encountered in two molecular forms , O2
and O3.
• O3 is also formed from O2 in electrical discharges,
such as in lightning storms:
3O2(g)  2O3(g) H = +284.6 kJ
• Ozone is toxic.
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• Halogen always gain one electron to form anion:
X2 + 2e-  2X• Fluorine is most reactive in the group:
2F2(g) + 2H2O(l)  4HF(aq) + O2(g)
• Each element consists of diatom molecules ; F2 , Cl2
, Br2 and I2
• Fluorine gas is pale yellow , Chlorine gas is yellowgreen , Bromine liquid is red-brown and solid iodine is
black (violet vapor)
77
Group VIIIA(Noble gases)
• Fluorine and Chlorine are more reactive than
Bromine and Iodide
• Noble gases are monoatom (He Ne Ar Kr Xe Rn)
• Noble gases have completely filled s and p
subshell.
• 1960s the elements were called the “inert gases”
because they were thought to be incapable of
forming chemical compounds.
• Today we can synthesis some of noble gas
compounds ; XeF2 XeF4 XeF6 KrF2 and HArF
2Cl-(aq) + F2(g)
 2F-(aq) + Cl2(g)
2Br-(aq) + Cl2(g)  2Cl-(aq) + Br2(g)
2I-(aq) + Br2(g)  2Br-(aq) + I2(g)
 X
2F-(aq) + Cl2(g)
 X
2Cl-(aq) + Br2(g)
2Br-(aq) + I2(g)  X
In fact, fluorine removes electrons from almost any
substance with which it come into contact.
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80
TRANSITION ELEMENTS
(Group B ; 8 groups)
Electron Configuration and Properties
Transition Metals
InnerTransition Metals
Rare-earth elements
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81
82
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Oxidation Number of Transition Metals
Phisical Properties of Potassium - Zinc
(Stable Oxidation Number in red)
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Nomenclature of Elements
with Atomic Numbers Greaterer than 100
Write the element symbol and name :
The Rules for Naming Elements
1. Name directly from the atomic number of the element
using the following numerical roots
0 = nil , 1 = un , 2 = bi , 3 = tri , 4 = quad , 5 = pent ,
6 = hex , 7 = hept , 8 = oct , 9 = enn
2. The roots are put together in the order of the digits
and terminated by “ium” to spell out the name.
Example
Atomic Number : 112
Element Name: Ununbium
Element Symbol: Uub
85
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Location of atoms in the periodic table
17Cl
:
:
17Cl
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3. Atomic Number : 115
4. Atomic Number : 118
5. Atomic Number : 120
Name :
Symbol
Name :
Symbol
Name :
Symbol
Name :
Symbol
Name :
Symbol
___________
: ___________
___________
: ___________
___________
: ___________
___________
: ___________
___________
: ___________
86
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e.g.
Outer level
21Sc
1s2 2s2 2p6 3s2 3p5
valence electron
2,8,7
: 1s2 2s2 2p6 3s2 3p6 4s2 3d1
/2+1 = 3
4 principle
energy levels
So, Sc is in group 3B and period 4.
Three shells
So,
2. Atomic Number : 110
Element
Element
Element
Element
Element
Element
Element
Element
Element
Element
For Transiton metals (group B)
group no. = sum of two last sub-energy levels
(subshell)
period no. = no. of principle energy levels
For representative elements (group A)
group no. = no. of valence electron
= sum of electron outer level
period no. = no. of principle energy levels
Ex.
1. Atomic Number : 102
is in group 7A and period 3
87
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88
Vocabulary
Fill in the blank , Determine Group No. and Period No.
1. 7N : ……………………………………
group ………… period …………
2. 11Na : …………………………………
group ………… period …………
3. 18Ar : …………………………………
group ………… period …………
4. 20Ca : …………………………………
group ………… period …………
5. 35Br : …………………………………
group ………… period …………
6. 25Mn : ……………………………………
group ………… period …………
7. 26Fe : ……………………………………
group ………… period …………
8. 22Ti : ……………………………………
group ………… period …………
9. 53I : ……………………………………
group ………… period …………
10. 29Cu : …………………………………
group ………… period …………
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Radioactive
turned into
unstable
falls down
radiation
equation
Ionising ability
Balancing
Penetrating
half life
behavior
undergo
electric field
decrease
excessive
collide
repulsion
Fission
Decay
Fussion
90
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Properties of radiation
Radioactive Elements
A radioactive elements are an elements with an
unstable nucleus, which radiates alpha, beta or gamma radiation
and gets converted to a stable element.
3 Types of Radiation
Type of Radiation
Alpha particle
Beta particle
Gamma ray
Symbol



(can look different,
depends on the font)
Mass (atomic mass
units)
4
1/2000
0
Charge
+2
-1
0
Speed
slow
fast
very fast (speed of
light)
Ionising ability
high
medium
0
Penetrating power
low
medium
high
paper
aluminium
lead
Stopped by:
Penetrating power
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92
The behavior of three types of radioactive emissions in
an electric field.
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93
Beta Decay
Alpha Decay
The reason alpha decay occurs is because the
nucleus has too many protons which cause excessive
repulsion.
94
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Gamma Decay
Beta decay occurs when the neutron to proton ratio
is too great in the nucleus and causes instability. In basic
beta decay, a neutron is turned into a proton and an
electron. The electron is then emitted.
Gamma decay occurs because the nucleus is at too
high an energy. The nucleus falls down to a lower energy
state and, in the process, emits a high energy photon known
as a gamma particle.
3
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95
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2He*
3
2He
+ γ
96
Symbol charge and mass
Nuclear equation
Partical
Symbol
Charge
mass(amu)*
Alpha
α , 42He
+2
4.00276
Beta
β,
-1
0.000540
0
0
+1
0.000540
0
-1e
γ
Gamma
Positron
β+ ,
Neutron
n ,
1
0n
0
1.0087
Proton
P ,
1H
1
+1
1.0073
Deuteron
D ,
2H
1
+1
2.0136
Tritron
T ,
3H
1
+1
3.0219
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0
+1e
Balancing Nuclear Equations
Ex. 1:
1
66
29Cu
C.
27
13Al
_______
97
+ 42He
D. 146C
E.
226
F.
226
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30
13
6C
14Si
98
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G.
213
-1e
H.
209
+ _______
I.
23
J.
238
+
0
+ ________
83Bi
_______ + 42He
81Tl
209
11Na
+ 42He
92U
+
16
90
+
L. 23592U +
1
99
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+ _______
0n
87Fr
__________
12Mg
239
16
222
26
8O
K. 23892U +
89Ac
+ _______
________ +510n
+ ________
226
82Pb
8O
88Ra
89Ac
9
6
4
1H + 4Be ---> 3Li + 2He
Rule: The sum of the mass numbers of the reactants equals the
sum of the mass numbers of the products.
Balancing Nuclear Equations
_______ + 0-1e
A. 2714Si
B.
A nuclear equation shows how a nucleus gains
or loses subatomic particles.
94Pu + ________
38Sr +
143
54Xe
+ ________
100
Radioactive Elements
Half life ; t½
is the period of time it takes for the amount of
a substance undergoing decay to decrease by half.
Ex. P-32 has a half life 14 days
100 g
14 วัน
14 วัน
50 g
25 g
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101
µaÇo‹ҧ ¶ŒÒ·ié§äoo«o·»¡aÁÁa¹µÃa§ÊÕª¹i´Ë¹ึè§ 20 ¡ÃaÁ änj¹Ò¹ 28 Ça¹ »ÃÒ¡¯
NjÒÁÕäoo«o·»¹aé¹eËÅืooÂً 1.25 ¡ÃaÁ ¤Ãึ觪Õǵi ¢o§äoo«o·»¹ÕéÁÕ¤‹Òe·‹Òã´
Half life
Radiation
U-235 7.1x109 years Alpha Gamma
C-14
5,760 years
Beta
Co-60
5.26 years
Gamma
Au-198
2.7 days
Beta Gamma
I-125
60 days
Gamma
I-131
8.07 days
Beta Gamma
P-32
14.3 days
Beta
Pu-239 24,000 years Alpha Gamma
K-40
1x109 years
Beta
Ra-226
1,600 years Alpha Gamma
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Benefit
Treatment of Cancers
Archeology
Treatment of Cancers
Medical Diagnostics
Medical Diagnostics
Medical Diagnostics
Treatment of Cancers
Generation of Electricity
Archeology
Treatment of Cancers
102
1. After 42 days a 2.0 g sample of phosphorus-32 contains only 0.25 g
of the isotope. What is the half-life of phosphorus-32?
2. In 5.49 seconds, 1.20 g of argon-35 decay to leave only 0.15 g.
What is the half-life of argon-35?
µaÇo‹ҧ ¨§ËÒ»ÃiÁÒ³ I-131 eÃièÁµŒ¹ eÁืèo¹íÒ I-131 ¨íҹǹ˹ึè§ÁÒÇÒ§änj
e»š¹eÇÅÒ 40.5 Ça¹ »ÃÒ¡¯Ç‹Ò ÁÕÁÇÅeËÅืo 0.125 ¡ÃaÁ ¤Ãึ§è ªÕÇiµ¢o§ I-131
e·‹Ò¡aº 8.1 Ça¹
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Elements
103
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104
Calculations base on half life
5. Polonium-214 has a half-life of 164 seconds. How many seconds
would it take for 8.0 g of this isotope to decay to 0.25 g?
Nt = N0
2n
n = T / t1/2
=
=
=
=
=
number remaining
initial number
time
no. time of decay
half life
µaÇo‹ҧ ¨§ËÒ»ÃiÁÒ³¢o§ Tc-99 ·ÕèeËÅืoeÁืèoÇÒ§ Tc-99 ¨íҹǹ 18 ¡ÃaÁänj¹Ò¹
24 ªaèÇoÁ§ æÅa Tc-99 ÁÕ¤Ãึ觪ÕÇiµ 6 ªaèÇoÁ§
6. How many days does it take for 16 g of palladium-103 to
decay to 1.0 g? The half-life of palladium-103 is 17 days.
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Nt
N0
T
n
t1/2
105
106
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Nuclear Reaction
1. After 42 days a 2.0 g sample of phosphorus-32 contains only 0.25 g
of the isotope. What is the half-life of phosphorus-32?
Nuclear Reaction is process in which two nuclei,
or else a nucleus of an atom and a subatomic particle
(such as a proton, or high energy electron) from
outside the atom, collide to produce products different
from the initial particles.
2. Polonium-214 has a half-life of 164 seconds. How many seconds
would it take for 8.0 g of this isotope to decay to 0.25 g?
2 Types of nuclear reaction
1. Nuclear Fission
2. Nuclear Fussion
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107
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108
Nuclear Fission
A heavy nucleus such as Uranium-235 absorbs an extra
neutron, it becomes unstable and splits into two lighter
nuclei. The energy is released as kinetic energy of the
fission products.
109
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Nuclear Fussion
When two light nuclei such as Hydrogen or Deuterium are
forced to combine forming a new, heavier nucleus. The energy is
released as kinetic energy of the fusion products.
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110
Atomic Properties and Periodic Trends
Atomic Properties
 Atomic radius (¢¹Ò´oaµoÁ)
 Ion size (ÃaÈÁÕäooo¹)
 Ionization energy (IE) (¾Åa§§Ò¹äoooä¹e«ªa¹)
 Electron affinity (EA) (ÊaÁ¾ÃäÀÒ¾oieÅ硵Ão¹)
 Electronegativity (EN) (oieÅç¡o·Ãe¹¡ÒµiÇiµÕ)
 Melting point(m.p.) (¨u´ËÅoÁeËÅÇ)
and Boiling point(b.p.) (¨u´e´ืo´)
 Oxidation Number(O.N.) (eÅ¢oo¡«ie´ªa¹)
and
Periodic Trends
(ÊÁºaµi¢o§¸ÒµuæÅaæ¹Ço¹ŒÁ¢o§¸ÒµuµÒÁµÒÃÒ§¸Òµu)
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111
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112
Atomic Radius (Atomic Size)
Vocabulary
distance
discontinuity
repulsion
endothermic
attraction
exothermic
trend
tendency
Cation
combine
anion
require
Network
structure
indicate
inversely
giant molecules
 The atomic radius is one half of the distance
between the nuclei of two atoms of the same
element when the atoms are joined.
proportional
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113
A Kind of Radius
1. Covalent Radius(ÃaÈÁÕo¤eÇeŹµ) used for Covalent
compounds. e.g. H2 , F2 , Cl2 , O2
Atomic Radius
Group trends :
The atoms get bigger as we go down a group.
Because the increase in the principal energy levels.
Cl - Cl
2. Van der Waals Radius(ÃaÈÁÕæǹe´oÏÇÒÅʏ) used for
Noble gases. e.g. He , Ne , Ar
Period Trends :
The atoms get bigger as we go from right to left
in a period at same energy level. Because the
decrease of nucleus attraction.
3. Metallic Radius(ÃaÈÁÕoÅËa) used for Metal atoms.
e.g. Li , Mg , Cu
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114
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115
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116
Atomic Radius
1. Which element in each pair has the larger atoms?
1.2 3Li or 8O
1.1 12Mg or 20Ca
1.3
17Cl
or
35Br
1.4
11Na
or
16S
2. Arrange these atoms in order of increasing size?
11Na , 13Al , 6C , 20Ca
3. Arrange these atoms in order of increasing size?
33As , 37Rb , 18Ar , 15P
117
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6.3
The Octet Rule
118
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Ions size
 Metals elements lose valence electrons to form cation.
Cation radius are always smaller than atomic radius.
The “goal” of most atoms is to have an
octet or group of 8 electrons in their valence
energy level.
Metals generally give(lose) electrons,
Nonmetals take(gain) electrons from other
atoms.
 Non-metal elements gain valence electrons to form anion.
Anion radius are always larger than atomic radius.
Atoms that have gained or lose electrons
are called “ion”.
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119
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120
Group trends
The ions get bigger as we go down a group.
Because the increase in the principal energy
levels.
Period Trends
The ions get bigger as we go from right to
left in a period at same energy level. Because the
decrease of nucleus attraction.
Atoms and Ions size
B3+
Li+
Be2+
C4+
N3-
O2-
F121
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4.
+
11Na
or 12Mg2+
2. Arrange these atoms and ions in order of increasing size?
2+ ,
3+ ,
3- ,
12Mg
13Al
15P
17Cl
3. Arrange these atoms and ions in order of increasing size?
+
+
23Li , 11Na , 12Mg , 16S
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Ionization Energy(IE)
1. Which atoms or ions in each pair are larger?
2. 8O or 8O21. 12Mg or 12Mg2+
3. 7N3- or 9F-
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 The energy required to remove an electron from
an atom in gas phase.
 Ionization energy and atomic radius are inversely
proportional.
 e.g.
First Ionization Energy(IE1)
Na(g) --> Na+(g) + e
Second Ionization Energy(IE2)
Na+(g) --> Na2+(g) + e
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124
Find the group number from ionization of following element ?
Write IE1 – IE5 of Boron
______
______
______
______
______
__________________
__________________
__________________
__________________
__________________
:
:
:
:
:
IE1 = 807 KJ/mol
IE2 = 2,433 KJ/mol
IE3 = 3,666 KJ/mol
IE4 = 25,033 KJ/mol
IE5 = 32,834 KJ/mol
IE1
IE2
IE3
IE4
IE5
(MJ/mol)
(MJ/mol)
IE6
IE7
IE8
(MJ/mol)
(MJ/mol)
(MJ/mol)
(MJ/mol)
(MJ/mol)
(MJ/mol)
0.744 1.457
7.739
10.547 13.636 18.001
1.687
3.381
6.057 8.414
11.029 15.171
1.093
2.359
4.627 6.229
37.838 47.285
0.906
1.763
14.855 21.013
group
21.710 25.663
17.874 92.047
IE3 and IE4 is more different , why ?
125
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Trends in First Ionization Energies of First 20 Elements
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126
Trends in First Ionization Energies of Elements
 First ionization
energy tends to
increase from bottom
to top within a group.
 And increase from
left to right across a
period.
However, there are two apparent discontinuities in
this trend.
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128
Electron Affinity(EA)
1. Which element in each pair has the greater ionization
energy?
1. 12Mg or 13Al
2. 4Be or 5B
3. 6C or
14Si
 Electron affinity is the energy change when an
atom gains one electron.
 Where ionization energy is always endothermic,
electron affinity is usually exothermic, but not
always.
4. 2He or 53I
2. Arrange these atoms in order of increasing IE1 ?
33As , 37Rb , 18Ar , 15P , 16S
Example ;
3. Arrange these atoms in order of increasing IE1 ?
19K , 13Al , 11Na , 12Mg , 20Ca
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129
in Electron affinity of Elements
 If the atom has more tendency to accept an
electron then the energy released will be large
and electron affinity will be high.
 Atoms with large ionization energy have negative
electron affinity.
 If there are no empty spaces, a new orbital, making
the process endothermic (Group IIA and VIIIA).
e.g.
2 2 6 2
Group IIA
12Mg : 1s 2s 2p 3s
2 2 6 2 6
Group VIIIA
18Ar : 1s 2s 2p 3s 3p
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131
O(g) + e
O-(g) + e
O- (g) : EA = -142 KJ/mol
O2- (g) : EA = 780 KJ/mol
130
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Trends in Electron Affinity
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132
Electronegativity (EN)
1. Which element in each pair has the greater electron
affinity?
1. 12Mg or 13Al
2. 3Li or 8O
3. 6C or
5.
11Na
or
32Ge
19K
4.
18Ar
 Electronegativity is the tendency for an atom to
attract electrons to itself when it is chemically
combined with another element.
 High electronegativity means it pulls the
electron toward it.
or 53I
6. 9F or
53I
2. Arrange these atoms in order of increasing EA ?
19K , 20Ca , 11Na , 15P , 9F
133
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6.3
Trends in Electronegativity of Elements
 Electronegativity tends to increase from bottom
to top within a group.
 And increase from left to right across a period.
Because the increase of nucleus attraction.
 Note; Noble gases are NOT assigned
electronegativities
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134
Trends in Electronegativity
Representative Elements in Groups 1A through 7A
135
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136
1. Which element in each pair has the greater
electronegativity?
1. 11Na or 15P
2. 3Li or 8O
4. 9F or 53I
3. 6C or 32Ge
2. Draw arrow to show the bond polarity in each pair elements
N---F
C---Br
O----Cl
Br---Br
C---S
C----I
3. Arrange these atoms in order of increasing EN ?
12Mg , 20Ca , 17Cl , 9F
137
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For metals ;
The melting point and boiling point tends to
increase from bottom to top within a group
(the increase metallic bond).
Melting Point and Boiling Point
 The melting point is the temperature at which the
transition from the solid phase to the liquid phase.
- Helium has the lowest melting point (-272.2oC).
- Carbon has the highest melting point (3550oC).
 The boiling point is the temperature at which the
transition from the liquid to the gas phase.
- Helium has the lowest boiling point (-268.9oC).
- Tungsten has the highest boiling point (5927oC).
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For nonmetals ;
The melting point and boiling point tends to
increase from top to bottom within a group.
And increase from right to left across a period.
(the increase van der waals' forces)
And increase from left to right across a period
(the metallic bond increase when increase of outer
electrons or valence electron).
But, the group IVA ; high melting point and boiling point
because they have giant molecules(Network structure).
angka teprattananan
139
angka teprattananan
140
Arrange these atoms in order of increasing
melting – boiling point ?
Electron affinity
17Cl
, 13Al
11Na
, 3Li
4. 9F , 53I ,
11Na
5. 7N , 14Si , 9F ,
m.p. and b.p. of metal
, 13Al
10Ne
141
angka teprattananan
Oxidation number
angka teprattananan
Atomic radius
metallic character
m.p. and b.p. of nonmetal142
3. The oxidation number of some elements in their compounds
is fixed
E.g. Hydrogen in most of its compound = +1
Oxygen in most of its compound = -2
all group I elements
= +1
all group II elements
= +2
4. The sum of the oxidation numbers of the elements in a
molecule or ion is equal to the charge on the molecule or ion.
E.g. OH- (-2) + (+1) = -1
The oxidation number of an element indicates the
number of electrons lost, gained, or shared as a
result of chemical bonding.
Rules of Oxidation Number
1. Elements have an oxidation number of zero.
E.g. Na , K , Pb , H2 , O2 , P4
2. The oxidation number of simple ion is the charge on the
ion.
E.g. Li+ = +1 , Fe3+ = +3 , O2- = -2 , Cl- = -1
angka teprattananan
m.p. and b.p. of metal
10Ne
Electronegativity
metallic character
3. 6C ,
Ionization energy
Atomic radius
2. 3Be ,
,
Electronegativity
15P
Electron affinity
,
Ionization energy
19K
summary
m.p. and b.p. of nonmetal
1.
Periodic trends
143
angka teprattananan
144
Determine the oxidation number of underline element :
Find the Oxidation Number of S in SOCl4 ?
O.N. of Oxygen =
O.N. of Chlorine =
1. SO2
2. CaSO4
3. PO434. NH4+
Oxidation numbers of
C in HCO3- ?
5. Pb(OH)4
HCO3O=
6. KMnO4
H=
7. Cu(NO3)
8. K2[Fe(CN)3H2O]
angka teprattananan
145
Determine the oxidation number of underline element :
3. SO3
1. CO
2. CH4
4. Al2O3
5. S2Cl2
6. BaSO4
7. MgCrO4
8. Sr(NO3)2
9. IF3
10. K2MnO4
11. [Fe(CN)6]3- 12. Cr(OH)3
13. NiCl2.6H2O
14. K3[Fe(CN)6]
15. [Cu(NH3)4]SO4
16. [Mn(H2O)6]3+
17. (NH4)2[NiCl4]
angka teprattananan
147
angka teprattananan
146