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ATOMIC STRUCTURE
AND PERIODIC
SYSTEM
LEVEL X SEMESTER 1
SMKN 7 BANDUNG
Standard competency
 Identifies atomic structure and periodic at
element periodic tables
Based competency
 Describing development of atomic theory
 Interprets data in tables periodic
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THE PURPOSE OF STUDY
 Student understands and solvent of description of proton,
neutron and electron based on relative charge and his(its relative
mass
 Solvent student of description of mass and charge in atom
 Solvent student of description of contribution of proton and
neutron at atomic nucleus based on atomic number and mass
number
 Solvent student of deduction number of protons, neutron and
electron which there is in atom and ion from atomic number and
mass number given
 Student can differentiate isotope based on neutron amounts
differs in the
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 Solvent student of description number of and orbital relative
energies of sulfur, p and d from principal quantum number
 Solvent student of deduction of atom electronic configuration
 Solvent student of description of periodic table based on
formation element at the height of atomic number, repetition of
character physical and character chemical in one periods and
character physical and the same chemical property in one
factions
 Solvent student of description element of third period, variation
electronic configuration, atom radius, electrical conductivity,
melting point and point boil, and explains its(the variation based
on structure and tying in element
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 Solvent student of description and explains various
energy first ionization of element increasing in one
periods based on improvement of nuclear charge
 Solvent student of description and explains various
energy first ionization of decline element in one
factions based on improvement of atom radius
 Student can interpret data based on configuration
electronic, atom radius, electrical conductivity, melting
point and boiling point for explains periodicity
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DEVELOPMENT OF ATOM MODEL
 Atom model John Dalton
 John Dalton explains that atom is smallest particle of element
indiscrete again, everlasting and cannot be annihilated that way
nor can be created.
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Atom model Joseph John
Thompson
 often is conceived of bun model with bread as atom which haves
positive charge and currant as electron which spread over
flattens in all parts of bread.
 Atom as a whole haves the character of neutral.
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Atom model Ernest Rutherford
 atom has core which haves positive charge and is
atom center of mass and electrons encircles it.
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Atom model Niels Bohr
Energy level
notation of Skin
Hal.: 9
1 2 3 4 5 ...
K L M N O ...
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Wave mechanics atom model
 that electron stays in orbital with certain energy
level.
 Orbital is an area the biggest possibility to find
electron is around atomic nucleus.
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 Electron is the elementary particle
composing a matter (atom)
 Mass e = 9,11 x 10-31 kg
 Charge e = ( - )
 Proton is a positively charged particle
which was discovered by Eugene Goldstein
 Mass proton = 1,67 x 10-27 kg
 Charged proton = + 1,6 x 10-19 C
 Neutron  is uncharged particle which has
mass ± 1,67 x 10-27 kg
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Atomic nucleus
 Ernest Rutherford finds atomic nucleus
 Radioactivity matter is matter what can transmit
off the cuff radiation, for example uranium, radium
and polonium.
 Radiation or what transmitted by radioactive
matter called as radioactivity.
 Familiar radioactivity is alpha rays ( α), beta rays
( β) and gamma (γ).
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ALPA RAYS,BETA AND GAMMA
Hal.: 13
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Atomic Number and Mass
Number of Atom
 In its relation to the atomic number and mass
number,
 hence the atom of an element is usually
expressed by the following symbol;
 X = the name of atom
 A = mass number of atom
 Z = atomic number
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Isotope
Isotope is on of two or more species of an
element atom having the same atomic
number, but differing in mass number
Examples;
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Isobar and Isotones
 Isobar is atom which come from different
element but having same mass number.
The example of the isobar;
14C and 14N , both are having the same mass
6
7
number, that is 14
 Isotones is atom which come from different
element but having same the number of
neutrons.
The example; 32S16 atom have the number of
neutrons of 16 that equal to the number of
neutrons of 31P15
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Electron in Atom
 if peripatetic electron encircles core, hence its the
energy loss electron would and energy electron
kinetic would continuously decrease.
 Atomic nucleus attractive force to electron will
become bigger than electron path centrifugal
forces and causes trajectory to become spiral and
finally fall electron into atomic nucleus.
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 If fall electron into atomic nucleus, hence atom
becomes do not stable.
 This thing is interferes in with common statement
that stable atom.
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LINE SPECTRUM
If beam
polychromatic like
electric light and
sunshine is overcome
through prism hence
will be obtained
continuous spectrum
consisted of various
its the compiler
colors.
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BOHR THEORY
 Niels Bohr does research and tries explains with
resolving approach of hydrogen line spectrum.
Bohr applies approach of Max Planck to explain
hydrogen line spectrum.
 According To Max Planck;
E = nhv
Description:
n = positive integer
h = Planck constant (6,63.10-34J.s)
v = frequency
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CONFIGURATION ELECTRON
What electron lapped over in the form of
trajectory trajectory in :
KULIT
SUB KULIT
Hal.: 21
KLMN
spdf
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Formation of Quantum number
Skin
Quantum number ( n)
accommodation
energy power of
Maximum electron
1
K
2 x 12 = 2
2
L
2 x 22 = 8
3
M
2 x 23 = 18
4
N
2 x 24 = 32
…
…
…
…
n
2n2
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Skin sub type which there is in atom;
 Skin sub s, contains orbital 1 ( can
accommodate 2 electron)
 Skin sub p, contains orbital 3 ( can
accommodate 6 electron)
 Skin sub d, contains orbital 5 ( can
accommodate 10 electrons)
 Skin sub f, contains orbital 7 ( can
accommodate 14 electrons)
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 Orbital admission filling sequence started from
orbital which its(the energy is lowest to orbital
which the energy is highest as according to
Aufbau Principe
 Orbital admission filling sequence is;
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p
6s 4f 5d 6p 7s 5f 6d 7p
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Example;
2 2s2 2p6 3s2 3p6 4s2 3d6
Fe
=
1s
26
What if Fe3+?
Reply :
means discharges 3 his outmost electron is thus the
electron total ( 23)
Fe3+ = 1s2 2s2 2p6 3s2 3p6 4s0 3d5
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Valence Electron
 Valence electron is number of electrons found on skin
outmost an element atom.
 valence electron so that electron valence can be told is
element atom chemical property determinant.
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Quantum Number
 To know correct position from at one particular
electron in atom, hence to every electron is given
[by] four of the price of quantum number.




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Principal quantum number ( n)
Azimuth quantum number ( l)
Magnetic quantum number ( m)
Spin quantum number ( s)
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Principal quantum number ( n)
 express skin number place of orbital location
electron or measure / distance / atom radius.






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Electron in skin first having the price of n = 1
Electron in skin second having the price of n = 2
Electron in having third skin the price of n = 3
Electron in skin fourth having the price of n = 4
Electron in skin ke-5 has the price of n = 5
Electron in skin ke-6 has the price of n = 6
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Azimuth quantum number (l)
express skin sub type place of location
electron. This number also express orbital
form.




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Electron in skin sub s has the price of l=0
Electron in skin sub p has the price of l=1
Electron in skin sub d has the price of l=2
Electron in skin sub f has the price of l=3
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As according to skin sub amounts which
implied in each skin hence the price of l
applying to every price n.
 n = 1, l = 0
 n = 2, l = 0,1
 n = 3, l = 0,1,2
 n = 4, l = 0,1,2,3
The price of l is integer from 0 until (n–1)
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Example;
 Electron at energy level 4s has the price of
n = 4, l = 0
 Electron at energy level 2p has the price of
n = 2, l = 1
 Electron at energy level 5d has the price of
n = 5, l = 2
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Magnetic quantum number ( m)
express is orbital place of location
electron. The price of m for electron in
every orbital is integer from - 1 until + 1




0
l=0, hence m=0
l=1, hence m=-1,0,+1 -1 0 +1
l=2, hence m=-2,-1,0,+1,+2 -2 -1
l=3, hence m=-3,-2,-1,0,+1,+2,+3
-3
Hal.: 32
-2
-1
0
0
+1 +2
+1 +2 +3
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Spin quantum number ( s)
 express direction of gyration of electron in
orbital. Two electron dwelling one having each
orbital the price of s = +½ and sulfur = -½
 Thereby inferential that;
 Electrons in one skins has the price of the same n
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 Electrons in one skin subs has the price of the
same n and
 Electrons in one orbital has the price of n, l
and the same m
 Electrons in one orbital has the price of
different s
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 Admission filling to four following above quantum
numbers is ground so-called Pauli Prohibition; “
There is no two electrons having quantum
number to four his its are same”
 Example; determines fourthly last electron
quantum number in admission filling of electron
from atom;
a. 7N
b. 17Cl
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Answer;
a. Configuration; 7N = 1s2 2s2 2p3
ll
ll
l
l
l
1s
2s
2p
hence;
n=2
l = 1 (remembers, skin sub p where l=1)
m = -1 (pays attention to orbital of p, for box tip of
right)
s = +½ (direction of rotation upward)
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b. Configuration,
ll
ll
2 2s2 2p6 3s2 3p5
Cl
=
1s
17
ll
ll
ll
ll
ll
ll
l
1s
2s
2p
3s
3p
hence;
n=3
l=1
m = 0 (pays attention to orbital of p, box which
is)
s = -½ (aims to under)
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Periodic System of Element
Triad Dobereiner
 Johann Wolfgang Dobereiner ( 1829) groups
elements in group of three element known as Triad.
Hal.: 38
Triad
Relative
atomic
mass
Calcium
40
Strontium
88
Barium
137
Relative atom mass average
Third and first element
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Octave Law Newlands
 John Newlands ( 1864) groups element based on
increase of element relative atomic mass.
Resemblance of nature of shown by element
disagreeing one octaves namely element first and
element 8, element second with element 9.
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Periodic system of Mendeleev
 Dimitri Ivanovich Mendeleev ( 1869) express that element
character is periodic function from its the relative atomic
mass, certain would be recurring periodical if element is
compiled based on increase of its the relative atomic mass.
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Periodic system of Moseley
 Henry G Moseley ( 1914)
finds way is determining
atomic number based on
is element character
which is periodic function
of its(the atomic number
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Period and Faction
 Modern periodic system lapped over based on
increase of atomic number and resemblance of
nature and lapped over to 7 period and 18
factions.
 Horizontal column called as Period
 Vertical Column called as Faction, divided to
become :
 Element of Faction A ( Main)
 Element of Faction B ( Transition)
 Element of Faction Lanthanide and Actinide
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Modern Periodic system
Tables
Hal.: 43
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Main Faction elements
 It is element which admission filling of its the
electron ends at orbital of s or p, like at tables :
Faction Number
Hal.: 44
Faction Name
Outmost Electron
Structure
IA
Alkali
ns1
II A
Soil Alkali
ns2
III A
Boron
ns2 np1
IV A
Carbon
ns2 np2
VA
Nitrogen
ns2 np3
VI A
Oxygen
ns2 np4
VII A
Halogen
ns2 np5
VIII A
Noble gas
ns2 np6
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Faction Elements of Transition
 It is elements which admission filling of its(the electron
ends at orbital of d or called as block d.
 The Numbering of faction :
1. Faction number is given letter B
2. Faction number = number of electrons s +d ( number
of electrons in outmost skin is added with number of
electrons d filled last)
If:
Hal.: 45
s+d=9 hence faction VIII B
s+d=10 hence faction VIII B
s+d=11 hence faction I B
s+d=12 hence faction II B
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Faction Tables of Transition
Hal.: 46
Name Of Faction
Outmost Electron Structure
III B
ns2 nd1
IV B
ns2 nd2
VB
ns2 nd3
VI B
ns2 nd4
VII B
ns2 nd5
VIII B
ns2 nd6
VIII B
ns2 nd7
IB
ns1 nd10
II B
ns2 nd10
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Faction Elements Lanthanide
and Actinide
It is elements which admission filling of
its(the electron ends at orbital of f,
consisted of :
 Elements Lanthanide, ends at orbital of 4f
 Actinide Elements, ends at orbital of 5f
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Periodic of Element
 That is changing character in order according to
increase of atomic number from left of dextrose
in one periods and from the top (of) downwards
in one factions
 Atom Radius; That is distance from atomic
nucleus until outmost skin an atom
 In One Factions : From the top (of)
downwards more and more big
 In one periods : From left of dextrose more
and more small
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Determination of Atom radius
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The relation of atom radius
with atomic number
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Ionization energy
That is minimum energy required to
release neutral atom electron in
presentation of gas at outmost skin and
tied is feeblest
 In one factions : From the top (of) downwards
more and more small
 In one periods : From left of dextrose more
and more big
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The relation of ionization
energy with atomic number
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Electron affinity
 That is free energy or
permeated by neutral
atom in the form of gas
in the event of arrest of
one electrons placed at
his(its outmost skin and
atom becomes negative
ion
 In one periods : From
left of dextrose more
and more small
 In one factions: from the
top (of) downwards
more and more big
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Electro negativity
 That is ability of atom to be
interesting or catch's electron.
 Big electro negativity
( height) haves the character
of easy to catch electron
 Small electro negativity
( low) haves the character of
difficult to catch electron
 In one factions : From the top
(of) downwards more and
more small
 In one periods : From left of
dextrose more and more big
Hal.: 54
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THANKS
Hal.: 55
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