Atom and Periodic Table §ãËÁ iºÒ iÁäÁ - Chemistry Kru Boy · 2017-05-11 · Chemistry...
Transcript of Atom and Periodic Table §ãËÁ iºÒ iÁäÁ - Chemistry Kru Boy · 2017-05-11 · Chemistry...
Chemistry M.4 Lesson 1
Atom and Periodic Table
by Angka Teprattananan
1angka teprattananan
Atomic Models¤ o Áo¹ÀÒ¾·Õè¹a¡Ç i·ÂÒÈÒʵà �ÊÃ�Ò§¢ é¹ ¨Ò¡¢�oÁÙÅ·Õèä �¨Ò¡¡ÒÃ
·´Åo§e¾ èo㪠�o¸ iºÒÂÅ a¡É³a¢o§oaµoÁ o´Â atomic models ·ÕèÊÃ�Ò§¢ é¹ÊÒÁÒö»Ã aº»Ãu§ËÃo
e»ÅÕè¹æ»Å§ä � ¶ �ÒÁռšÒ÷´Åo§ãËÁ�æ «è§o¸ iºÒÂo´Â㪠� atomic models 溺e iÁäÁ�ä �
2องคาร เทพรตนนนท
¨oË �¹ ´oŵ a¹ ( John Dalton )
Atomic�s Theory1. ¸Òµu»Ãa¡oº �ÇÂoaµoÁ«è§e»�¹Ë¹ �ÇÂeÅç¡·ÕèÊu äÁ�ÊÒÁÒö
æº�§æ¡Ëà o·íÒÅÒÂä´ �2. oaµoÁ¢o§¸Òµue ÕÂÇ¡ a¹¨aÁÕÊÁºaµieËÁo¹¡ a¹ oaµoÁ¢o§
¸Òµuµ�Ò§ª¹ i´¡ a¹¨aÁÕÊÁºaµiµ�Ò§¡ a¹3. ÊÒûÃa¡oºe¡ i´¨Ò¡¡ÒÃÃÇÁ¡ a¹¢o§¸Òµu¤¹Åaª¹ i´
e.g. H2O , CO2(Expect Na ,H2 , Br2 , P4 , S8)
3angka teprattananan
e¨ e¨ ·oÁÊ a¹ (J.J. Thomson)
4
J.J. Thomson È ¡ÉÒ¡ÒùíÒä¿¿�Ò¢o§æ¡ �Ê·Õèe¡ i´ã¹ cathode ray
tube ÀÒÂãµ�ÊÀÒÇa high voltage and low pressure.
angka teprattananan
Thomson�s Experiment
+‐voltage source
OFF
ON
+
‐eÁ èo¼ �ҹʹÒÁä¿¿ �Ò
¾ºo¹uÀÒ¤·ÕèÁÕ»Ãa¨ue»�¹Åº æÅaeÃÕ¡o¹uÀÒ¤¹ÕéÇ �Ò Electron
æÅaÇ a´¤ �Ò charge to mass ratio of the electron (q/me) = 1.76 x 108 coulombs/gram
5angka teprattananan
Discovery of the Proton– ¤ �¹¾ºo´Â Eugen Goldstein– ÁÕ¡Òþº �Canal rays� « è§ÁÕ»Ãa¨uºÇ¡æÅaeÃÕÂ¡Ç �Ò
Proton.
6
Eugen Goldstein
angka teprattananan
Cathode rays and Canal rays
7
__ cathode anode
+
angka teprattananan
¨Ò¡¡Ò÷´Åo§¢o§o¡Å �Êäµ¹ ÊÃu»ä �Ç�Ò - Ãa§ÊպǡËÃoo¹uÀÒ¤ºÇ¡e¡i´¨Ò¡æ¡�Ê « è§eºÕè§eº¹e¢�ÒËÒ¢aéÇźä �- Ãa§ÊպǡÁÕ¤�ÒoaµÃÒÊ �ǹ»Ãa¨uµ�oÁÇÅäÁ �¤§·Õè ¢é¹oÂÙ�¡aºª¹ i´¢o§æ¡ �Ê- ¶�Òe»ÅÕèÂ¹æ¡ �Êe»�¹äÎo´Ãe¨¹ ¨a¾ºÇ�Òo¹uÀÒ¤ºÇ¡·Õèe¡i´¢é¹¨aÁÕ¤�Ò»Ãa¨ue· �Ò¡ aº
oieÅ硵Ão¹¾o Õ ¨§eÃÕ¡o¹uÀÒ¤ºÇ¡¹ÕéÇ�Ò �o»Ãµo¹�
The oil drop apparatus
ÁiÅi桹·íÒ¡Ò÷´Åo§æÅa¾º»Ãa¨u¢o§oieÅ硵Ão¹ : 1.60 x 10-19 C æÅa¤íҹdzËÒÁÇÅ¢o§oieÅ硵Ão¹ä �e·�Ò¡ aº : 9.1 x 10-28 g
8angka teprattananan
Calculate mass of the Electron1. charge to mass ratio = 1.76x108 coulombs/gram2. charge of electron = 1.60 x 10-19 g
9angka teprattananan
Thomson�s Atomic Model(Plum Pudding Model)
�oaµoÁe»�¹·Ã§¡ÅÁ »Ãa¡oº �ÇÂo»Ãµo¹·ÕèÁÕ»Ãa uºÇ¡æÅaoieÅ硵Ão¹·ÕèÁÕ»Ãa uźoÂÙ�oÂ�Ò§¡Ãa a´¡Ãa¨Ò æÅaÊíÒËÃaºoaµoÁ·Õèe»�¹¡ÅÒ§·Ò§
ä¿¿ �Ò¨aÁÕ íҹǹo»Ãµo¹e·�Ò¡ aº íҹǹoieÅ硵Ão¹¾o Õ�10angka teprattananan
Discovery of Nucleus Tested Thomson�s model of atomic
structure with the �gold foil� experiment. ·íÒ¡Ò÷´Åo§Âi§Ã a§ÊÕæoÅ¿Òe¢�Òä»Âa§æ¼�¹·o§¤íÒ ¾ºÇ �Ò
Ernest Rutherford
11angka teprattananan
à a§ÊÕæoÅ¿ÒÊ �ǹãË�·aÅuoo¡ÁÒe» �¹eÊ �¹µÃ§ à a§ÊÕæoÅ¿ÒºÒ§Ê �ǹ ÁÕ¡ÒÃeºÕè§eº¹¨Ò¡æ¹Çe´ iÁ à a§ÊÕæoÅ¿ÒÊ �ǹ¹ �oÂÁÒ¡e¡ i´¡ÒÃÊa· �o¹¡Å aº
¨Ò¡¼Å¡Ò÷´Åo§ ·íÒãË �ÊÃu»ä´ �Ç �Ò : 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
12angka teprattananan
Rutherford's Atomic Model
�oaµoÁ»Ãa¡oº �ǹ iÇe¤ÅÕÂÊ« è§ÁÕ»Ãa¨uºÇ¡(o»Ãµo¹)oÂÙ�µÃ§¡ÅÒ§ ÁÕ¢¹Ò´eÅç¡ÁÒ¡æÅaÁÕÁÇÅÁÒ¡ Ê �ǹoieÅ硵Ão¹·ÕèÁÕ»Ãa¨uźæÅaÁÕÁÇŹ �o e¤Åèo¹·ÕèÃoº¹ iÇe¤ÅÕÂÊ
e»�¹ºÃ iedz¡Ç �Ò§"
13angka teprattananan
The Discovery of the Neutron ¡Òài§o¹uÀÒ¤æoÅ¿Òe¢ �Òä»Â a§æ¼�¹ Be ¾ºo¹uÀÒ¤¹ iǵÃo¹«è§ÊÒÁÒö·íÒãË�o»ÃµÃo¹ËÅu´¨Ò¡æ¼�¹
¾ÒÃÒ¿ �¹ä �Neutrons have mass similar to protons. No electrical charge.
14
James Chadwick
angka teprattananan
The Subatomic particlesparticle symbol charge mass(g) mass(amu)electron e -1 9.1x10-27 0.0005proton p +1 1.67x10-24 1.0072neutron n 0 1.67x10-24 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 carbon-
12 nucleus 15angka teprattananan
Atomic Symbol (Nuclear Symbol)
A
ZXMassnumber
Atomicnumber
Element Symbol
• Atomic number = ¨íҹǹo»Ãµo¹(ÁÕ¤ �Òe·�Ò¡ aº¨íҹǹoieÅ硵Ão¹ÊíÒËà aº¸Òµu·Õèe»�¹¡ÅÒ§)
• Mass number = ¼ÅÃÇÁÃaËÇ �Ò§¨íҹǹo»Ãµo¹æÅa¹ iǵÃo¹
16angka teprattananan
Fill in the blanks for the following nuclear symbols:
Element94Be 14
6C 3517Cl- 74
33As3- 4420Ca2+ 67
31Ga3+
Atomic Number
Mass Number
# of Protons
# of Neutrons
# of Electrons
17angka teprattananan
Isotope , Isotone , Isobar and Isoelectronic
• Isotope are atoms of the same element having different masses, (¨íҹǹ¹ iǵÃo¹äÁ�e·�Ò¡ a¹)
11H p = 1 , e = 1 , n = 021H p = 1 , e = 1 , n = 1
• Isotone are atoms of the different element having equal neutrons.
115B p = 5 , e = 5 , n = 6
126C p = 6 , e = 6 , n = 6
18angka teprattananan
• Isobar are atoms of the different element having equal mass number.
3616S mass no. of 3616S is 36
3618Ar mass no. of 3618Ar is 36
• Isoelectronic are atoms and ion having equal electron.
2010Ne p = 10 , e = 10 , n = 10
2412Mg2+ p = 12 , e = 10 , n = 12
19angka teprattananan
Neclear symbols isotope isotone isobar isoelectronic
146C & 147N
3919K & 4020Ca
3517Cl & 3717Cl
3818Ar & 3216S2-
168O & 188O
4018Ar & 4020Ca
3517Cl- & 3919K+
3115P & 3216S
For each of the following ,check the blank for isotope , isotone , isobar or isoelectronic
20angka teprattananan
Max Plank
È ¡ÉÒ spectrum ¢o§ Electromagnetic Wave Wave. The æÅa¤ÇÒÁÊ aÁ¾ a¹¸ �ÃaËÇ �Ò§ wavelength(λ), the frequency
(ν), and the energy (E)
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)
Max Plank
21angka teprattananan
Energy and frequency of Electromagnetic Wave
Color of spectrum
Wavelength (nm)
Energy (kJ)
Violet Blue Green Yellow Orange
Red
400 - 420420 - 490490 - 580580 - 590590 - 650650 - 700
4.96x10-22 - 4.73x10-22
4.73x10-22 - 4.05x10-22
4.05x10-22 - 3.42x10-22
3.42x10-22 - 3.36x10-22
3.36x10-22 - 3.05x10-22
3.05x10-22 - 2.83x10-22
22angka teprattananan
Calculate about Electromagnetic WaveEx1 Êe»¡µÃ aÁÊÕÁ�ǧ¤ÇÒÁÂÒÇ¤Å è¹ 500 nm ¨aÁÕ¤ÇÒÁ¶Õèe·�Òã´
Ex2 Êe»¡µÃ aÁÊÕæ´§ÁÕ¤ÇÒÁÂÒÇ¤Å è¹ 500 nm ¨aÁÕ¤ÇÒÁ¶ÕèæÅa¾Åa§§Ò¹e·�Òã´
23angka teprattananan
Ex3 The energy of electromagnetic wave is 3x10-22 KJ , Find the color
Ex4 The frequency is 5x1014 Hz , calculate the wavelength , energy and find the color of this spectrum.
24angka teprattananan
Niels Bohr È ¡ÉÒ Hydrogen Spectrum
Niels Bohr
25angka teprattananan
Color of Spectrum
Wavelength (nm)
Energy (kJ) ΔE
RedBluegreen
BlueViolet
656486434410
3.02 x 10-22
4.08 x 10-22
4.57 x 10-22
4.84 x 10-22
10.6 x 10-23
4.9 x 10-23
2.7 x 10-23
26angka teprattananan
Bohr�s Atomic Model
oaµoÁ»Ãa¡oº �ÇÂo»Ãµo¹æÅa¹ iǵÃo¹ oÂÙ�ÀÒÂã¹¹ iÇe¤ÅÕÂÊ Ê�ǹoieÅ硵Ão¹Ç iè§oÂÙ�Ãoº æ ¹ iÇe¤ÅÕÂÊe»�¹ªaé¹æ ËÃoe»�¹Ãa aº¾Åa§§Ò¹« è§ÁÕ¤ �Ò äÁ�µ�oe¹ èo§¡ a¹
27angka teprattananan
Electron Configuration(o¤Ã§æººoieÅ硵Ão¹)oieÅ硵Ão¹¨aoÂÙ�Ãoºæ ¹ iÇe¤ÅÕÂÊe» �¹ª aé¹æ eÃÕÂ¡Ç �Ò Ãa´ aº¾Å a§§Ò¹ËÅ a¡
�principle energy level�æµ �Åa principle energy level ¨aÁÕoieÅ硵Ão¹ã¹¨íҹǹ·Õè¨íÒ¡ ae» �¹ä»µÒÁ¡®
Rule ; 2n2
n = principle energy levels
28angka teprattananan
Rule; Arrangements of electrons in an atom.1. ¨ a´oieÅ硵Ão¹ã¹Ãa aºªaé¹¾Åa§§Ò¹æáæãË�eµçÁ¡ �o¹
2. eÁèoÃa aºæÃ¡æ ¨ �´eµçÁæÅ�ÇãË� a oieÅ硵Ão¹Å§ã¹Ãa aºªa鹶 a´ä»3. oieÅ硵Ão¹·ÕèÃa aº¹o¡Êu´ÁÕä � 1-8 æÅaÃa aº¶ a´e¢ �ÒÁÒ ÁÕ 8 æÅa 18
µÒÁÅíÒ aº(ÊíÒËà aº¸ÒµuËÁÙ�A)
e.g. 11Na: has 11 electrons 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) can fill 1 electron shot hand 11Na : 2 , 8 , 1
29angka teprattananan
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 : ���������������
30angka teprattananan
Electron Cloud Model
㨤ÇÒÁÊíÒ¤ a oieÅ硵Ão¹·ÕèÁÕ¾Åa§§Ò¹µèíÒ¨a¾ººÃ iedzã¡Å �
¹ iÇe¤ÅÕÂÊ oieÅ硵Ão¹·ÕèÁÕ¾Åa§§Ò¹ÊÙ§¡Ç �Ò¨a¾ºË�Ò§¨Ò¡
¹ iÇe¤ÅÕÂÊoo¡ÁÒ äÁ�ÊÒÁÒöºo¡µíÒæ˹ �§·Õèæ¹ �¹o¹¢o§oieÅ硵Ão¹
ä � ºo¡ä �e¾Õ§oo¡ÒÊã¹·Õè a¾ºoieÅ硵Ão¹ o´ÂºÃ iedz·ÕèÁÕ¡Åu�ÁËÁo¡oieÅ硵Ão¹Ë¹Òæ¹ �¹ÁÕ
oo¡ÒʾºoieÅ硵Ão¹ÁÒ¡¡Ç �Һà iedz·ÕèÁÕ¡Åu�ÁËÁo¡eºÒºÒ§
31Erwin Schrodinger angka teprattananan
Åa¡É³a¢o§ Electron Cloud Model ¨aeÃÕÂ¡Ç �Ò �Orbital� Ëà o subenergy levels «è§ÁÕ 4 ª¹i´ ä �æ¡ � s , p , d and f
s
p
d
f32angka teprattananan
Electron configurationsoÒÈ aÂËÅa¡¡Òô a§¹Õé1. 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.
33angka teprattananan
Arrangements of electrons in Orbital
principle energy levels
(shell)subenergy levels
(subshell)maximum electron
n = 1 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 234angka teprattananan
Lower energy Higher energy1s 2s 2p 3s 3p 4s 3d 4p �.
35angka teprattananan 1S
2S
3S2P
3P
4S
3d
4P5S
4d
Ex. Give the full electron configuration of 27Co
NOTE. principle energy levelsOr 27Co;
36angka teprattananan
»ÃaeÀ·¢o§ electron configuration æº �§e» �¹ 3 »ÃaeÀ·´ a§¹Õé
1) Orbital Diagram.
2) Long notation or spdf configuration.1s22s22p63s2....
3) Shorthand Notation or noble gas core.[Ne]3s23p4
s1
s2
37angka teprattananan
Using Orbital Diagram1. 3Li : �������������������� 2. 12Mg : ��������������������
3. 18Ar : ��������������������
4. 19K : ��������������������
5. 25Mn : ��������������������
6. 26Fe : ��������������������
7. 24Cr : ��������������������
38angka teprattananan
Using Long Notation or spdf configuration 1. 12Mg : ����������������� 2. 18Ar : �����������������3. 19K : �����������������4. 33As : �����������������5. 38Sr : �����������������6. 55Cs : �����������������7. 28Ni : �����������������8. 24Cr : �����������������9. 29Cu : �����������������
39angka teprattananan
Using Short hand Notation or Noble Gas core.1. 3Li : ����������������� 2. 12Mg : ������������������ 3. 18Ar : ������������������4. 19K : ������������������ 5. 33As : ������������������ 6. 28Ni : ������������������ 7. 37Rb : ������������������8. 53I : ������������������
40angka teprattananan
(Ç iÇ a²¹Ò¡Òâo§µÒÃÒ§¸Òµu)
The History of the Periodic Table
41angka teprattananan
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�
Cl Chlorine mass = 35.5Br Bromine mass = 79.9I 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).
Johaun Dobereiner
42angka teprattananan
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� .
His law of octaves work today with the first 20 elements.43
John Newlands
angka teprattananan
Dmitri Mendeleev In 1869 he published a table of the elements
organized by increasing atomic mass. Noticed similar properties appeared at regular
intervals --> �periodic�
Lothar Meyer At the same time, he published his
own table of the elements organized by increasing atomic mass.
44
Mendeleev
Lothar Meyer
angka teprattananan
Mendeleev’s discovery
45angka teprattananan
The table below compares Mendeleev�s prediction with the actual data.
46angka teprattananan
Henry Mosely
¨ a´eÃÕ§ÅíÒ´ aº¸ÒµuµÒÁeÅ¢oaµoÁ(¨íҹǹo»Ãµo¹)¨Ò¡¹ �oÂä»ÁÒ¡ o´ÂeÃÕ§¨Ò¡« �ÒÂ仢ÇÒã¹µÒÃÒ§¸Òµu¡Òè a´µÒÃÒ§¸Òµu溺¹ÕéÊÒÁÒÃ¶æ¡ �» �ËÒ¢o§¸Òµu
Tellurium(Te) and Iodine(I) ä´ �¹o¡¨Ò¡¹Õé Mosely  a§µ aé§e» �¹¡®e¡ÕèÂÇ¡ aºµÒÃÒ§¸Òµu
Periodic Law : ÊÁº aµ i·Ò§¡ÒÂÀÒ¾æÅae¤ÁÕ¢o§¸Òµu ¢é¹oÂÙ�¡ aºeÅ¢oaµoÁæÅa¡Òè a´eÃÕ§oieÅ硵Ão¹
47
Henry Mosely
angka teprattananan
Three classes of elements are Metals, Nonmetals and Metalloids
Modern Periodic Table
48angka teprattananan
Metal 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
Gold
49angka teprattananan
Nonmetal Elements 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
SulphurBromine 50angka teprattananan
Metalloids Sometimes called semiconductors Form the �stairstep� between metals and nonmetals Have properties of both metals and nonmetals Examples: B, Si , Ge , As , Sb, Te , Po and At
51angka teprattananan
¡ÒÃe»ÃÕºe·ÕºÊÁº aµ i¢o§¡ è§oÅËa ¡ aº Al(oÅËa)æÅaI(ooÅËa)
IE1(kJ/mol)
EN Density(g/cm3)
melting�boiling point(oC)
ElecticalConductivity
Type of Compound
Al 584 1.61 2.70 660-2519 √ ionic
B 807 2.04 2.34 2075-4000 √ ionic and covalent
Si 793 1.90 2.33 1414-3265 √ ionic and network covalent
Ge 768 2.01 5.32 938-2833 √ ionic and covalent
As 951 2.18 5.75 358-603 √ ionic and covalent
Sb 840 2.05 6.68 631-1587 √ ionic and covalent
I 1015 2.66 4.93 114-184 X ionic and covalent
52angka teprattananan
Location of Hydrogen in the periodic table
Some properties of Hydrogen , group IA and VIIA
properties Group IA H group VIIA
1. # valence electron 1 1 7
2. Oxidation number in compounds
+1 +1 , -1 +1 , +3 , +5+7 , -1
3. IE1 (kJ/mol) 382-526 1318 1015-1687
4. EN 0.7-1.0 2.1 2.2 -4.0
5. phase solid gas 3 phase
6. Electric conductivity can cannot cannot
53angka teprattananan
¤ÇÒÁÊ aÁ¾ a¹¸ �ã¹æ¹Çµ aé§eÃÕÂ¡Ç �Ò ËÁÙ� æÅaËÁÙ�ã¹µÒÃÒ§¸ÒµuÁÕ·aé§ËÁ´ 18 ËÁÙ� æº �§e»�¹ËÁÙ� A 8 ËÁÙ� æÅaËÁÙ� B 8 ËÁÙ�(ËÁÙ� 8B «éíÒ¡ a¹ 3 ËÁÙ�)
¸Òµu·ÕèoÂÙ�ã¹ËÁÙ�e ÕÂÇ¡ a¹Áa¡¨aÁÕÊÁºaµi·Ò§¡ÒÂÀÒ¾æÅa·Ò§e¤ÁÕ¤Å�Ò¤ŧ¡ a¹
Periodic Table
54angka teprattananan
¤ÇÒÁÊ aÁ¾ a¹¸ �ã¹æ¹Ç¹o¹¢o§¸Òµu eÃÕÂ¡Ç �Ò ¤Òº « è§ÁÕ·aé§ËÁ´ 7 ¤Òºã¹µÒÃÒ§¸Òµu
Periodic Table
55angka teprattananan
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 pd
f
56
Periodic Table
angka teprattananan
REPRESENTATIVE ELEMENTS (Group A ; 8 groups)
57
Alkali MetalsAlkali Earth Metals Halogens
Noble GasesInert Gases
angka teprattananan
Group IA (Alkali Metals)
� e»�¹¢o§æ¢ç§ÊÕe§ i¹æÅaÊa·�o¹æʧä � Õ� o �o¹ÊÒÁÒöµ a´§ �Ò �ÇÂÁÕ´� ¤ÇÒÁ˹Òæ¹ �¹µèíÒ� e¡ i´» i¡ iÃiÂÒ¡ aºoÒ¡ÒÈä �§ �Ò µ �o§e¡çºäÇ �ã¹¹éíÒÁa¹� ·íÒ» i¡ iÃiÂÒ¡ aº¹éíÒ ä �ÊÒÃÅaÅÒ·ÕèÁÕÊÁº aµ ie»�¹eºÊe.g.
2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)
58angka teprattananan
� e¡ i´» i¡ iÃiÂÒ¡ aºoo¡« ie¨¹ ä �ÊÒûÃa¡oºoo¡ä« �ËÅÒÂ溺:4Li(s) + O2(g) 2Li2O(s) (oxide)
2Na(s) + O2(g) Na2O2(s) (peroxide)K(s) + O2(g) KO2(s) (superoxide)
� ¨aÁÕÊÕe©¾ÒaeÁèo¹íÒä»e¼Òã¹e»ÅÇä¿� ÊÒûÃa¡oº¢o§oÅËaËÁÙ� 1A ·u¡ª¹i´ÅaÅÒ¹éíÒä �� ¤ÇÒÁÇ �o§äÇ㹡ÒÃe¡ i´» i¡ iÃiÂÒe¾ ièÁ¨Ò¡º¹Å§Å�Ò§
59angka teprattananan
Group IIA (Alkali Earth Metals)
� ÁÕ¤ÇÒÁ˹Òæ¹ �¹ÁÒ¡¡Ç �Ò Alkali Metals� ÊÒûÃa¡oº carbonate , phosphate , sulphid , sulphite
¢o§ Alkali Earth Metal äÁ�ÅaÅÒ¹éíÒ� Be äÁ�e¡ i´» i¡ iÃiÂÒ¡ aº¹éíÒ , Mg e¡ i´» i¡ iÃiÂÒª �Òæ¡ aº¹éíÒ æÅa Ca e¡ i´» i¡ iÃiÂÒ¡ aº¹éíÒä � :
Mg(s) + 2H2O(l) Mg(OH)2(aq) + H2(g)Ca(s) + 2H2O(l) Ca(OH)2(aq) + H2(g)
60angka teprattananan
Group VIA (Chalcogen)
� Oxygen , Sulphur and Selenium are nonmetals , Tellurium is Metalloid and Polonium is radioactive element.
� Oxygen 㹸ÃÃÁªÒµi¾º 2 ÃÙ» ¤ o O2 and O3. � O3 e¡ i´¨Ò¡ O2 o´Â㪠�¡ÃaæÊä¿¿�Ò, eª �¹»ÃÒ¡¯¡Òó �¿ �Ò¼�Ò:
3O2(g) 2O3(g) H = +284.6 kJ� O3 e»�¹æ¡ �ʾ iÉ.
61angka teprattananan
Group VIIA (Halogens)� Halogen ÊÒÁÒöà aºoieÅ硵Ão¹æÅa¡ÅÒÂe»�¹äooo¹Åº ä �:
X2 + 2e- 2X-
� Fluorine e»�¹¸Òµu·ÕèÇ �o§äÇ㹡ÒÃe¡ i´» i¡ iÃiÂÒÁÒ¡·ÕèÊu´:
2F2(g) + 2H2O(l) 4HF(aq) + O2(g) • Halogen 1 oÁeÅ¡uŨa»Ãa¡oº �Ç 2 oaµoÁ ; F2 , Cl2 , Br2
and I2� Fluorine gas is pale-yellow , Chlorine gas is yellow-
green , Bromine liquid is red-brown and solid iodine is black (violet vapor)
62angka teprattananan
• ¤ÇÒÁÇ �o§äÇ㹡ÒÃe¡ i´» i¡ iÃiÂÒŴŧ¨Ò¡º¹Å§Å�Ò§ ¸ÒµuËÁÙ� 7A
2Cl-(aq) + F2(g) 2Br-(aq) + Cl2(g) 2I-(aq) + Br2(g) 2F-(aq) + Cl2(g) 2Cl-(aq) + Br2(g) 2Br-(aq) + I2(g)
63angka teprattananan
Group VIIIA(Noble gases)• Noble gases oÂÙ�e»�¹oaµoÁe ÕèÂÇ(He Ne Ar Kr Xe Rn)• ºÃèuoieÅ硵Ão¹eµçÁã¹ s æÅa p orbital• »� 1960 eÃÕ¡¸Òµu¡Åu�Á¹ÕéÇ �Ò �inert gases� e¾ÃÒaäÁ�ÊÒÁÒöe¡ i´» i¡ iÃiÂÒe¤ÁÕ¡ aº¸Òµuo è¹æ
• »�¨ uº a¹ÊÒÁÒöeµÃÕÂÁÊÒûÃa¡oº¢o§¸Òµu¡Åu�Á¹Õéä � ; XeF2XeF4 XeF6 KrF2 and HArF
64angka teprattananan
TRANSITION ELEMENTS (Group B ; 8 groups)
65
Transition Metals
InnerTransition MetalsRare-earth elements
angka teprattananan
Electron Configuration and Properties
66angka teprattananan
Phisical Properties of Potassium - Zinc
67angka teprattananan
Oxidation Number of Transition Metals(Stable Oxidation Number in red)
68angka teprattananan
Nomenclature of Elements with Atomic Numbers Greaterer than 100
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 69angka teprattananan
Write the element symbol and name :1. Atomic Number : 114 Element Name : ___________
Element Symbol : ___________2. Atomic Number : 115 Element Name : ___________
Element Symbol : ___________3. Atomic Number : 116 Element Name : ___________
Element Symbol : ___________4. Atomic Number : 117 Element Name : ___________
Element Symbol : ___________5. Atomic Number : 118 Element Name : ___________
Element Symbol : ___________70angka teprattananan
Prediction located of atoms in the periodic table
71
For representative elements (group A)group no. = ¾ i¨ÒóҨҡ¨íҹǹoieÅ硵Ão¹ª aé¹¹o¡Êu´
= ËÃo¼Å¨Ò¡ªaé¹¹o¡Êu´¨Ò¡Ãa aº¾Åa§§Ò¹Â �oÂperiod no. = ¾ i¨ÒóҨҡ¨íҹǹÃa aº¾Åa§§Ò¹
Ex. 17Cl : 1s2 2s2 2p6 3s2 3p5
: 2 , 8 , 7
So, 17Cl is in group 7A and period 3
valence electron
Outer level
Three shells
angka teprattananan
For Transiton metals (group B)group no. = ¾ i¨ÒóҨҡ¼Å¢o§oieÅ硵Ão¹ 2 Ãa aºÊu´·�ÒÂperiod no. = ¾ i¨ÒóҨҡ¨íҹǹÃa aº¾Åa§§Ò¹
e.g. 21Sc : 1s2 2s2 2p6 3s2 3p6 4s2 3d1
So, Sc is in group 3B and period 4.
72
/2+1 = 3
4 principle energy levels
angka teprattananan
Fill in the blank , Determine Group No. and Period No.
1. 7N : �������������� 6. 25Mn : ��������������group ���� period ���� group ���� period ����
2. 11Na : ������������� 7. 26Fe : ��������������group ���� period ���� group ���� period ����
3. 18Ar : ������������� 8. 22Ti : ��������������group ���� period ���� group ���� period ����
4. 20Ca : ������������� 9. 53I : ��������������group ���� period ���� group ���� period ����
5. 35Br : ������������� 10. 29Cu : �������������group ���� period ���� group ���� period ����
73angka teprattananan
e»�¹¸Òµu·Õè¹ iÇe¤ÅÕÂÊäÁ�eʶÕÂà ¨aÁÕ¡ÒÃæ¼� alpha, beta or gamma radiation æÅae»ÅÕè¹e»�¹¸Òµu·ÕèeʶÕÂÃÁÒ¡¢ é¹
Radioactive Elements
74angka teprattananan
Properties of radiation
Type of Radiation Alpha particle Beta particle Gamma ray
Symbol
Mass (amu) 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
Stopped by: paper aluminium lead
Penetrating power
75angka teprattananan
The behavior of three types of radioactive emissions in an electric field.
76angka teprattananan
Alpha Decaye¡ i´¡ aº¹ iÇe¤ÅÕÂÊ·ÕèÁÕo»Ãµo¹ÁÒ¡e¡ i¹ä» ·íÒãË�e¡ i´æç¼Å a¡ã¹¹ iÇe¤ÅÕÂÊÁÒ¡
¨ §¨íÒe»�¹µ�o§Å´ íҹǹo»Ãµo¹Å§
77angka teprattananan
Beta Decaye¡ i´¡ aº¸Òµu·ÕèÁÕoaµÃÒÊ �ǹ¹ iǵÃo¹µ�oo»Ãµo¹ÁÒ¡e¡ i¹ä» ¨ §ÁÕ¡ÒÃe»ÅÕè¹
¹ iǵÃo¹ãË�e»�¹o»Ãµo¹o´Â¡ÒûŴ»Å�oÂoieÅ硵Ão¹ËÃoà a§ÊÕºÕµÒoo¡ÁÒ
78angka teprattananan
Gamma Decay
e¡ i´¡ aº¹ iÇe¤ÅÕÂÊ¢o§¸Òµu·ÕèÁÕ¾Åa§§Ò¹ÊÙ§e¡ i¹ä» ¨ §ÁÕ¡ÒûŴ»Å�o¾Åa§§Ò¹oo¡ÁÒã¹ÃÙ» high energy photon Ëà oo¹uÀÒ¤æoÅ¿Ò.
32He* 32He + γ
79angka teprattananan
Partical Symbol Charge mass(amu)*
Alpha α , 42He + 2 4.00276
Beta β , 0-1e - 1 0.000540
Gamma γ 0 0
Positron β+ , 0+1e + 1 0.000540
Neutron n , 10n 0 1.0087
Proton P , 11H + 1 1.0073
Deuteron D , 21H + 1 2.0136
Tritron T , 31H + 1 3.0219
Symbol charge and mass
80angka teprattananan
Nuclear equatione»�¹ÊÁ¡Ò÷ÕèæÊ´§¡ÒÃe»ÅÕè¹æ»Å§ÀÒÂã¹¹iÇe¤ÅÕÂÊ¢o§¸Òµu
¡ aÁÁa¹µÃa§ÊÕËÃo¡ÃaºÇ¹¡ÒÃæ¼ �Ãa§ÊÕBalancing Nuclear EquationsEx1:
11H + 94Be ---> 63Li + 42He
Rule: The sum of the mass numbers of the reactants equals the sum of the mass numbers of the products.
81angka teprattananan
Balancing Nuclear Equations
A. 2714Si _______ + 0-1e
B. 6629Cu _______ + 0-1e
C. 2713Al + 42He 30
14Si + _______D. 14
6C 136C + ________
E. 22689Ac 226
88Ra + ________
F. 22689Ac 222
87Fr + __________
82angka teprattananan
G. 21383Bi _______ + 42He
H. 20981Tl 209
82Pb + _______I. 23
11Na + 42He 2612Mg + _______
J. 23892U + 16
8O ________ +510n
K. 23892U + 16
8O 23994Pu + ________
L. 23592U + 10n 90
38Sr + 14354Xe + ________
83angka teprattananan
100 g 50 g 25 g14 วน 14 วน
Half life ; t1/2¤ o ÃaÂaeÇÅÒ·Õè radioactive elements e¡ i´¡ÒÃÊÅÒµ aÇ
æÅaÁջà iÁҳŴŧ¤Ã è§Ë¹ 觢o§·ÕèÁÕoÂÙ�e´ iÁEx. P-32 has a half life 14 days
84angka teprattananan
Elements Half life Radiation Benefit
U-235 7.1x109 years Alpha Gamma Treatment of Cancers
C-14 5,760 years Beta Archeology
Co-60 5.26 years Gamma Treatment of Cancers
Au-198 2.7 days Beta Gamma Medical Diagnostics
I-125 60 days Gamma Medical Diagnostics
I-131 8.07 days Beta Gamma Medical Diagnostics
P-32 14.3 days Beta Treatment of Cancers
Pu-239 24,000 years Alpha Gamma Generation of Electricity
K-40 1x109 years Beta ArcheologyRa-226 1,600 years Alpha Gamma Treatment of Cancers
85angka teprattananan
µaÇo �Ò§ ¶ �Ò· ié§äoo«o·»¡ aÁÁa¹µÃ a§ÊÕª¹ i´Ë¹è§ 20 ¡Ã aÁ äÇ �¹Ò¹ 28 Ç a¹ »ÃÒ¡¯Ç �ÒÁÕäoo«o·»¹ aé¹eËÅooÂÙ� 1.25 ¡Ã aÁ ¤Ã 觪ÕÇ iµ¢o§äoo«o·»¹ÕéÁÕ¤ �Òe·�Òã´
µaÇo �Ò§ ¨§Ëһà iÁÒ³ I-131 eà ièÁµ�¹ eÁèo¹íÒ I-131 íҹǹ˹ è§ÁÒÇÒ§äÇ �e»�¹eÇÅÒ 40.5 Ç a¹ »ÃÒ¡¯Ç �Ò ÁÕÁÇÅeËÅo 0.125 ¡ÃaÁ ¤Ã 觪ÕÇ iµ¢o§ I-131 e·�Ò¡ aº 8.1 Ç a¹
86angka teprattananan
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?
87angka teprattananan
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?
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.
88angka teprattananan
Calculations base on half life
Nt = N0 2n
n = T / t1/2
Nt = number remainingN0 = initial numberT = timen = no. time of decayt1/2 = half life
µaÇo �Ò§ ¨§Ëһà iÁÒ³¢o§ Tc-99 ·ÕèeËÅoeÁèoÇÒ§ Tc-99 ¨íҹǹ 18 ¡Ã aÁäÇ �¹Ò¹ 24 ª aèÇoÁ§ æÅa Tc-99 Áդà 觪ÕÇ iµ 6 ªaèÇoÁ§
89angka teprattananan
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. 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?
90angka teprattananan
Nuclear Fission¡ÃaºÇ¹¡Ò÷ÕèoaµoÁ¢o§¸Òµu˹ a¡e¡ i ¡ÒÃÊÅÒµ aÇãË�oaµoÁ¢o§¸Òµu·ÕèeºÒ
¡Ç �Ò ¾Ã �oÁ»Å´»Å�o¾Åa§§Ò¹oo¡ÁÒ
91angka teprattananan
Nuclear ReactionNuclear Fussion
¡ÃaºÇ¹¡Ò÷ÕèoaµoÁ¢o§¸ÒµueºÒ ÃÇÁµ aÇ¡ a¹e»�¹oaµoÁ¢o§¸Òµu·ÕèËÅa¡¢ é¹æÅaÁÕ¡ÒûŴ»Å�o¾Åa§§Ò¹oo¡ÁÒ
92angka teprattananan
Atomic Properties and
Periodic Trends
93angka teprattananan
Atomic size (¢¹Ò´oaµoÁ) Ion size (¢¹Ò´äooo¹) Ionization energy (IE) (¾Å a§§Ò¹äoooä¹e«ª a¹) Electron affinity (EA) (Ê aÁ¾ÃäÀÒ¾oieÅ硵Ão¹) Electronegativity (EN) (oieÅç¡o·Ãe¹¡Òµ iÇ iµÕ) Melting point(m.p.) (¨u´ËÅoÁeËÅÇ)
and Boiling point(b.p.) (¨u´e´ o´) Oxidation Number(O.N.) (eÅ¢oo¡« ie´ª a¹)
94
Atomic Properties and Periodic Trends
angka teprattananan
95
¡Òþ i¨ÒóҢ¹Ò´oaµoÁ ¨a¾ i¨ÒóҨҡ atomic radius « è§atomic radius ¤ o ÃaÂa·Ò§¤Ã è§Ë¹è§ÃaËÇ �Ò§¨u´¡ 觡ÅÒ§¢o§oaµoÁ 2 oaµoÁ ·ÕèoÂÙ�µ i´¡ a¹
Atomic Size
angka teprattananan 96
ª¹ i´¢o§Ã aÈÁÕoaµoÁ1. Covalent Radius(à aÈÁÕo¤eÇeŹµ �) used for Covalent
compounds. e.g. H2 , F2 , Cl2 , O2
2. Van der Waals Radius(à aÈÁÕæǹe´oà �ÇÒÅÊ �) used for Noble gases. e.g. He , Ne , Ar
3. Metallic Radius(Ã aÈÁÕoÅËa) used for Metal atoms. e.g. Li , Mg , Cu
Cl - Cl
angka teprattananan
Trends of Atomic size
Group trends :The atoms get bigger as we go down a group.
Because the increase in the principal energy levels.
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.
97angka teprattananan 98angka teprattananan
1. Which element in each pair has the larger atoms? 1.1 12Mg or 20Ca 1.2 3Li or 8O
1.3 17Cl or 35Br 1.4 11Na or 16S
2. Arrange these atoms in order of increasing size?
11Na , 13Al , 6C , 19K
3. Arrange these atoms in order of increasing size?
33As , 37Rb , 18Ar , 15P
99angka teprattananan
The Octet Rulee»�¹¡ÃaºÇ¹¡Ò÷ÕèoaµoÁ¢o§¸Òµu¾ÂÒÂÒÁ¨ a´eÃÕ§ãË �ÁÕoieÅ硵Ão¹
ª aé¹¹o¡Êu´ e·�Ò¡ aº 8 eËÁo¹æ¡ �ÊËÁÙ� VIII o´ÂMetals generally give(lose) electrons, Nonmetals take(gain) electrons from other atoms.oaµoÁ·ÕèoÂÙ�ã¹ÃÙ»»Ãa¨uä¿¿ �Ò eÃÒeÃÕÂ¡Ç �Ò �ion�.
100angka teprattananan
Ions size Metals elements lose valence electrons to form cation.
Cation radius are always smaller than atomic radius.
Non-metal elements gain valence electrons to form anion. Anion radius are always larger than atomic radius.
6.3
101angka teprattananan
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.
Li+
Be2+
B3+
C4+N3- O2- F-
102angka teprattananan
Atoms and Ions size
103angka teprattananan
1. Which atoms or ions in each pair are larger? 1. 12Mg or 12Mg2+ 2. 8O or 8O2-
3. 7N3- or 9F- 4. 11Na+ or 12Mg2+
2. Arrange these atoms and ions in order of increasing size?
12Mg2+ , 13Al3+ , 15P3- , 17Cl-
3. Arrange these atoms and ions in order of increasing size?
3Li+ , 11Na+ , 12Mg , 16S2-
104angka teprattananan
Ionization Energy(IE) ¤ o ¤ �Ò¾Åa§§Ò¹·ÕèoaµoÁ Ù´e¢ �Òä»e¾ èoãª�´§oieÅ硵Ão¹oo¡¨Ò¡oaµoÁã¹Ê¶Ò¹a
æ¡ �Ê «è§æ¹Ço¹�Á¢o§ IE ¨a¼¡¼a¹¡ aºæ¹Ço¹�Á¢o§¢¹Ò´oaµoÁ
e.g.First Ionization Energy(IE1)
Na(g) --> Na+(g) + eSecond Ionization Energy(IE2)
Na+(g) --> Na2+(g) + e
105angka teprattananan
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
106angka teprattananan
IE3 and IE4 is more different , why ?
Find the group number from ionization of following element ?
IE1(MJ/mol)
IE2(MJ/mol)
IE3(MJ/mol)
IE4(MJ/mol)
IE5(MJ/mol)
IE6(MJ/mol)
IE7(MJ/mol)
IE8(MJ/mol)
group
0.744 1.457 7.739 10.547 13.636 18.001 21.710 25.663
1.687 3.381 6.057 8.414 11.029 15.171 17.874 92.047
1.093 2.359 4.627 6.229 37.838 47.285
0.906 1.763 14.855 21.013
107angka teprattananan
ABCD
Trends in IE1 of First 20 Elements
First ionization energy tends to increase from bottom to top within a group. And increase from
left to right across a period.
108angka teprattananan
109angka teprattananan
1. Which element in each pair has the greater ionization energy?
1. 12Mg or 13Al 2. 4Be or 5B
3. 6C or 14Si 4. 2He or 53I
2. Arrange these atoms in order of increasing IE1 ?
33As , 37Rb , 18Ar , 15P , 16S 3. Arrange these atoms in order of increasing IE1 ?
19K , 13Al , 11Na , 12Mg , 2He
110angka teprattananan
Electron Affinity(EA) ¤ o ¤ �Ò¾Åa§§Ò¹·Õè¤ÒÂoo¡ÁÒ eÁèooaµoÁ¢o§¸Òµuã¹Ê¶Ò¹aæ¡ �Ê ÃaºoieÅ硵Ão¹ 1 o¹uÀÒ¤. ¤ �Ò EA Ê�ǹãË�ÁÕ¤ �Òe»�¹Åº e¹èo§¨Ò¡e»�¹» i¡ iÃiÂÒ ¤Ò¤ÇÒÁà �o¹Example ;
O(g) + e O- (g) : EA = -142 KJ/mol
O-(g) + e O2- (g) : EA = 780 KJ/mol
111angka teprattananan 112angka teprattananan
1. Which element in each pair has the greater electron affinity? 1. 12Mg or 13Al 2. 3Li or 8O
3. 6C or 32Ge 4. 18Ar or 53I
5. 11Na or 19K 6. 9F or 53I
2. Arrange these atoms in order of increasing EA ?
19K , 20Ca , 11Na , 15P , 9F
113angka teprattananan
Electronegativity (EN) ¤ o ¤ �ÒæÊ´§¤ÇÒÁÊÒÁÒö㹡ÒÃæ �§ª i§oieÅ硵Ão¹¢o§oaµoÁã¹
ÊÒûÃa¡oº ·ÕèÁÕ¡ÒÃÊà �Ò§¾ a¹¸ae¤Áի觡 a¹¸Òµu·ÕèÁÕ¤ �Ò EN ÁÒ¡ ¨aÁÕ¤ÇÒÁÊÒÁÒö㹡ÒÃæ �§ª i§
oieÅ硵Ão¹ä´ � Õ
114angka teprattananan
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
115angka teprattananan
6.3
116angka teprattananan
1. Which element in each pair has the greater electronegativity?
1. 11Na or 15P 2. 3Li or 8O 3. 6C or 32Ge 4. 9F or 53I
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
117angka teprattananan
Melting Point and Boiling Point
melting point o u³ËÀÙÁi·ÕèÊÒÃe»ÅÕè¹ʶҹa¨Ò¡¢o§æ¢ç§e»�¹¢o§eËÅÇ- Helium has the lowest melting point (-272.2oC).- Carbon has the highest melting point (3550oC).
boiling point o u³ËÀÙÁi·ÕèÊÒÃe»ÅÕè¹ʶҹa¨Ò¡¢o§eËŧe»�¹æ¡ �Ê- Helium has the lowest boiling point (-268.9oC). - Tungsten has the highest boiling point (5927oC).
118angka teprattananan
For metals ;The melting point and boiling point tends to increase from
bottom to top within a group (e¹ èo§ÁÒ¨Ò¡¤ÇÒÁæ¢ç§æç¢o§¾ a¹¸aoÅËa).And increase from left to right across a period
(e¹ èo§ÁÒ¨Ò¡¤ÇÒÁæ¢ç§æç¢o§¾ a¹¸aoÅËaæÅa¨íҹǹoieÅ硵Ão¹ªaé¹¹o¡·Õèe¾ ièÁ¢é¹).
119angka teprattananan
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.
(e¹ èo§ÁÒ¨Ò¡¤ÇÒÁæ¢ç§æç¢o§æçæǹe´oà �ÇÒÅ�Ç)
¢ �o¡eÇ �¹ ¤ oËÁÙ� IVA eª�¹ C Si (high melting point , boiling point)e¹ èo§¨Ò¡ÊÒÁÒöe¡ i´e»�¹oÁeÅ¡uÅ¢¹Ò´Â a¡É �·ÕèeÃÕÂ¡Ç �Òo¤Ã§¼Å¡Ã �Ò§µÒ¢ �ÒÂ
120angka teprattananan
Arrange these atoms in order of increasing melting � boiling point ?
1. 19K , 15P , 17Cl
2. 3Be , 10Ne , 13Al
3. 6C , 11Na , 3Li
4. 9F , 53I , 11Na , 13Al
5. 7N , 14Si , 9F , 10Ne
121angka teprattananan
Periodic trendssummary
Ioni
zatio
n en
ergy
Elec
tron
affi
nity
Elec
tron
egat
ivity
m.p
. and
b.p
. of m
etal
Electron affinity
Ionization energy
Electronegativity
m.p. and b.p. of metal
Atom
ic radius
metallic character
m.p. and b.p. of nonm
etal
Atomic radius
metallic character
m.p. and b.p. of nonmetal122angka teprattananan
123
Oxidation numberThe oxidation number of an element indicates the number of electrons lost, gained, or shared as a result of chemical bonding.
angka teprattananan
e¡³± �¡íÒ˹´¤ �ÒeÅ¢oo¡« ie´ªa¹¢o§¸Òµuµ�Ò§æ1. O.N. ¢o§¸ÒµuoiÊÃaÁÕ¤ �Òe»�¹Èٹ � eª�¹ S8 O2 Si Br2 Zn 2. O.N. ÁÕ¤ �Òe·�Ò¡ aº»Ãa¨u¢o§äooo¹ eª�¹ Na+ , Cl- ÁÕ¤ �Ò +1 , -13. O.N. ¢o§¸ÒµuËÁÙ� IA æÅa IIA ã¹ÊÒûÃa¡oºÁÕ¤ �Ò +1 æÅa +24. O.N. ¢o§äÎo´Ãe¨¹ã¹ÊÒûÃa¡oºÁÕ¤ �Ò +1 ¡eÇ �¹ äÎä´Ã´ � e»�¹ -15. O.N. ¢o§oo¡« ie¨¹ã¹ÊÒûÃa¡oºÁÕ¤ �Ò -2 ¡eÇ �¹ OF2 e»�¹ +2 ,
e»oà �oo¡ä« � (Na2O2 , BaO2 , H2O2) ÁÕ¤ �Ò -1 æÅa«u»e»oà �oo¡ä« �( NaO2 , KO2) ÁÕ¤ �Ò -1/2
HCO3-
O = H =
Oxidation numbers of C in HCO3
- ?
124
Find the Oxidation Number of S in SOCl4 ?O.N. of Oxygen = O.N. of Chlorine =
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