duplet
octet
No. of particlesGas volume
Mass
No. of Mole
x Molar mass Molar mass
x NA
NA
24 dm3 (rc) @ 22.4 dm3 (stp)
x 24 dm3 (rc) @ 22.4 dm3 (stp)
INFORMATIVE PERIODIC TABLE OF ELEMENTS
Proton no. = no. of proton in nucleus of an atomNucleon no. = no. of proton + no. of neutronIn Atom : no. of proton = no. of electron (neutral)In Cation : no. of proton > no. of electronIn Anion : no. of proton < no. of electron
Atom – All metal elements & member of group 18.Molecular compound – comb. of non-metal atoms.Ionic compound – metal ions + non-metal ions.
ELECTROCHEMICAL SERIES
1H2H+
11
+ve ions (cation)K+ Co2+
Na+ Ni2+
Ca2+ Mn2+
Mg2+ Cr3+
Al3+
Zn2+
Fe2+ (/ 3+)
Sn2+
Pb2+
H+
Cu2+
Ag+
Au+
-ve ions (anion)F- CO3
2-
SO42- MnO4
-
NO3- CrO4
2-
Cl- Cr2O72-
Br- PO43-
I-
OH-
2He42
3LiLi+
72.1
Be HH is not the member of group 1. Mercury, Hg is a liquid metal. Si can be used to produce semiconductor.
- Going down groups ; - size of atoms increase.
- electropositivity of elements increase.
- Across periods to the right ;- size of atoms decrease.- electronegativity of elements increase.
BB
6C122.4
7N2
142.5
8O2O2
162.6
9F2F
192.7
10Ne2.8
11NaNa+
232.8.1
12MgMg2+
242.8.2
13Al27
2.8.3
14SiSi2828
2.8.4
15P31
2.8.5
16SS2
322.8.6
17Cl2Cl
35.52.8.7
18Ar
2.8.8
Metals MetaloidMetaloid Non-metals Basic oxides Transition elements Amphoteric Acidic oxides Inert
19K K+
392.8.8.1
20CaCa2+
402.8.8.2
Cr MnFe56
Co NiCu64
Zn65 GeGe AsAs
Br2Br
80Kr
RbAg108
Cd Sn SbSb TeTeI2I
127Xe
CsPt Au
Hg(l) Pb207 PoPo At2 Rn
INFORMATIVE PERIODIC TABLE OF ELEMENTS
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Noble
Formation of chemical bond in..A Ionic bond (in the ionic compound). metal atom (release e) + nonmetal atom (accept e)
(concept of transferring e)B Covalent bond (in the molecule compound). nonmetal atom + nonmetal atom (share e)
(concept of sharing e)
Tendency to discharge ions increases
7
Per I ods
18 Groups
Special features of Transition Metals
1. Form coloured ions / compounds / solutions.2. Varying oxidation numbers.
(eg: Fe : +2,+3 ; Cu : +1,+2)3. Show catalytic properties.4. Form complex (coloured) ions.
Pe
riod 3
AlkalineAlkaline metalsmetals
Halog
ensH
alogens
Avogadro N
o., NA
= 6.02 x
1023
Direction of electron movement in…
Electrolytic cellVoltaic cell andRedox cell…anode e- cathode
Earth-Earth- alkalinealkaline metalsmetals
Noble
gase
s
18 Groups AlkalineAlkaline metalsmetals
Halog
en H
alogen
Name : ……………………………………………..…………… Class : ………
duplet
octet
No. of particles Gas volume
Mass
No. of Mole
x Molar mass Molar mass
x NA
NA
24 dm3 (rc) @ 22.4 dm3 (stp)
x 24 dm3 (rc) @ 22.4 dm3 (stp)
Proton no. = no. of protonNucleon no. = no. of proton + no. of neutronAtom : no. of proton = no. of electron (neutral)Cation : no. of proton > no. of electronAnion : no. proton < no. of electron
Atom : All metal elements & member of group 18.Molecule compound : comb. of non-metal atoms.Ionic compound : metal ions + non-metal ions.
ELECTROCHEMICAL SERIES
1H2H+
11
+ve ions (cation)K+ Co2+
Na+ Ni2+
Ca2+ Mn2+
Mg2+ Cr3+
Al3+
Zn2+
Fe2+/3+
Sn2+
Pb2+
H+
Cu2+
Ag+
Au+
-ve ions (anion)F- CO3
2-
SO42- MnO4
-
NO3- CrO4
2-
Cl- Cr2O72-
Br- PO43-
I-
OH-
2He42
3LiLi+
72.1
Be HH is not the member of group 1. Mercury, Hg is a liquid metal. Si can be used to produce semiconductor.
- Going down groups ; - size of atoms increase.
- electropositivity of element increase.
- Across periods to the right;- size of atoms decrease.- electronegativity of elements increase.
BB
6C122.4
7N2
142.5
8O2O2
162.6
9F2F
192.7
10Ne2.8
11NaNa+
232.8.1
12MgMg2+
242.8.2
13Al27
2.8.3
14SiSi2828
2.8.4
15P31
2.8.5
16SS2
322.8.6
17Cl2Cl
35.52.8.7
18Ar
2.8.8
Metals MetaloidMetaloid Non-metals Basic oxides Transition elements Amphoteric Acidic oxides Inert
19K K+
392.8.8.1
20CaCa2+
402.8.8.2
Cr MnFe56
Co NiCu64
Zn65 GeGe AsAs
Br2Br
80Kr
RbAg108
Cd Sn SbSb TeTeI2I
127Xe
CsPt Au
Hg(l) Pb207 PoPo At2 Rn
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Formation of chemical bond in..A Ionic bond (in the ionic compound). metal atom (release e) + nonmetal atom (accept e)
(concept of transferring e)B Covalent bond (in the molecule compound). nonmetal atom + nonmetal atom (share e)
(concept of sharing e)
Tendency to discharge ions increases
7
Per I ods
Special features of Transition Metals
1. Form coloured ions / compounds / solutions.2. Varying oxidation numbers.
(eg: Fe +2,+3 ; Cu +1,+2)3. Show catalytic properties.4. Form complex coloured ions.
Pe
riod 3
Avogadro N
o., NA
= 6.02 x
1023
Direction of electron movement in…
Electrolytic cellVoltaic cell andRedox cell…anode e- cathode
Earth-Earth- alkalinealkaline metalsmetals
IONIC FORMULAEIONIC FORMULAECATIONS ANIONSSodium ion Na+
Potassium ion K+
Silver ion Ag+
Hydrogen ion H+
Ammonium ion NH4+
Copper(II) ion Cu2+
Calcium ion Ca2+
Barium ion Ba2+
Zinc ion Zn2+
Iron(II) ion Fe2+
Iron(III) ion Fe3+
Lead(II) ion Pb2+
Aluminium ion Al3+
Chromium(III) ion Cr3+
Magnesium ion Mg2+
Mercury(I) ion Hg+
Chloride ion Cl¯Bromide ion Br¯Iodide ion I¯Hydroxide ion OH¯Nitrate ion NO3¯Hydride ion H¯Chlorate(V) ion ClO3¯Ethanoate ion CH3COO¯
Manganate(VII) ion MnO4¯Oxide ion O2¯Phosphate ion PO4
3¯Sulphide ion S2¯Sulphate ion SO4
2¯Carbonate ion CO3
2¯Chromate(VI) ion CrO4
2¯Dichromate(VI) ion Cr2O7
2¯
Charges in the positive ions (cations)Most of the metal ions have charges +2. You are only have to memorize the ions that have charges +1 and +3!.(a) Metal ions charged +1 are came from GROUP 1 which are Li+, Na+ and K+. Some others are Ag+, NH4
+, and H+.(b) Metal ions charged +3 are Al3+and Cr3+.(c) Roman numerals in brackets after the metal formulae to denote represent their charges. E.g.;, iron(II) = Fe2+ and ion chromium(III) = Cr3+.
Charges in the negative ions (anions)Most of the anions have charges -1. You are only have to memorize the ions that have charges -2 and -3!.(a) Some of the negative ions with -2 charged are O2-, SO4
2-, CO32-, CrO4
2-, and Cr2O72-.
(b) The commonly -3 charged ion is PO43-
CHEMICAL FORMULAECHEMICAL FORMULAEAcids Gases Organic CompoundsHydrochloric acid HCl Oxygen O2 Carbon tetrachloride CCl4Sulphuric acid H2SO4 Hydrogen H2 Chloroform CHCl3Nitric acid HNO3 Carbon dioxide CO2 Hexane C6H14
Phosphoric acid H3PO4 Carbon monoxide CO Hexene C6H12
Ethanoic acid CH3COOH Ammonia NH3 Benzene C6H6
Alkalis Nitrogen N2 Methane CH4
Sodium hydroxide NaOH Hydrogen sulphide H2S Ethane C2H6
Potassium hydroxide KOH Nitrogen dioxide NO2 Ethene C2H4
Barium hydroxide Ba(OH)2 Sulphur dioxide SO2 Ethanol C2H5OHAmmonium hydroxide NH4OH Chlorine Cl2 Ethanoic acid CH3COOHCalcium hydroxide Ca(OH)2 Hydrogen chloride HCl Glucose C6H12O6
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IONIC FORMULAEIONIC FORMULAECATIONS ANIONSSodium ion Na+
Potassium ion K+
Silver ion Ag+
Hydrogen ion H+
Ammonium ion NH4+
Copper(II) ion Cu2+
Calcium ion Ca2+
Barium ion Ba2+
Zinc ion Zn2+
Iron(II) ion Fe2+
Iron(III) ion Fe3+
Lead(II) ion Pb2+
Aluminium ion Al3+
Chromium(III) ion Cr3+
Magnesium ion Mg2+
Mercury(I) ion Hg+
Chloride ion Cl¯Bromide ion Br¯Iodide ion I¯Hydroxide ion OH¯Nitrate ion NO3¯Hydride ion H¯Chlorate(V) ion ClO3¯Ethanoate ion CH3COO¯
Manganate(VII) ion MnO4¯Oxide ion O2¯Phosphate ion PO4
3¯Sulphide ion S2¯Sulphate ion SO4
2¯Carbonate ion CO3
2¯Chromate(VI) ion CrO4
2¯Dichromate(VI) ion Cr2O7
2¯
Charges in the positive ions (cations)Most of the metal ions have charges +2. You are only have to memorize the ions that have charges +1 and +3!.(d) Metal ions charged +1 are came from GROUP 1 which are Li+, Na+ and K+. Some others are Ag+, NH4
+, and H+.(e) Metal ions charged +3 are Al3+and Cr3+.(f) Roman numerals in brackets after the metal formulae to denote represent their charges. E.g.;, iron(II) = Fe2+ and ion chromium(III) = Cr3+.
Charges in the negative ions (anions)Most of the anions have charges -1. You are only have to memorize the ions that have charges -2 and -3!.(c) Some of the negative ions with -2 charged are O2-, SO4
2-, CO32-, CrO4
2-, and Cr2O72-.
(d) The commonly -3 charged ion is PO43-
CHEMICAL FORMULAECHEMICAL FORMULAEAcids Gases Organic
CompoundsHydrochloric acid HCl Oxygen O2 Carbon tetrachloride CCl4Sulphuric acid H2SO4 Hydrogen H2 Chloroform CHCl3Nitric acid HNO3 Carbon dioxide CO2 Hexane C6H14
Phosphoric acid H3PO4 Carbon monoxide CO Hexene C6H12
Ethanoic acid CH3COOH Ammonia NH3 Benzene C6H6
Alkalis Nitrogen N2 Methane CH4
Sodium hydroxide NaOH Hydrogen sulphide H2S Ethane C2H6
Potassium hydroxide KOH Nitrogen dioxide NO2 Ethene C2H4
Barium hydroxide Ba(OH)2 Sulphur dioxide SO2 Ethanol C2H5OHAmmonium hydroxide NH4OH Chlorine Cl2 Ethanoic acid CH3COOHCalcium hydroxide Ca(OH)2 Hydrogen chloride HCl Glucose C6H12O6
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PERIODIC TABLE OF ELEMENTSPERIODIC TABLE OF ELEMENTS1 18
7 Perio
ds
111HH
HydrogenHydrogen11 2
11Na
Sodium23 13 14 15 16 17
22HeHe
HeliumHelium44
23Li
Lithium7
4Be
Beryllium9 TRANSITION METALS
5B
Boron11
66CC
CarbonCarbon1212
77NN
NitrogenNitrogen1414
88OO
OxygenOxygen1616
99FF
FluorineFluorine1919
1010NeNe
NeonNeon2020
311Na
Sodium23
12Mg
Magnesium24 3 4 5 6 7 8 9 10 11 12
13Al
Aluminium27
14Si
Silicone28
1515PP
PhosphorusPhosphorus3131
1616SS
SulphurSulphur3232
1717ClCl
ChlorineChlorine35.535.5
1818ArAr
ArgonArgon4040
419K
Potassium39
20Ca
Calcium40
21Sc
Scandium
22Ti
Titanium
23V
Vanadium51
24Cr
Chromium52
25Mn
Manganese55
26Fe
Iron56
27Co
Cobalt59
28Ni
Nickel59
29Cu
Copper64
30Zn
Zinc65
31Ga
Gallium
32Ge
Germanium
33As
Arsenic75
3434SeSe
SeleniumSelenium
3535BrBr
BromineBromine8080
3636KrKr
KryptonKrypton8484
537Rb
Rubidium86
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
Silver108
48Cd
Cadmium112
49In
50SnTin119
51Sb
Antimony
52Te
5353II
IodineIodine127127
5454XeXe
XenonXenon131131
655Cs
Caesium133
56Ba
Barium137
57La
72Hf
73Ta
74W
75Re
76Os
77Ir
78Pt
Platinum195
79Au
Gold197
80Hg
Mercury201
81Ti
82Pb
Lead207
83Bi
84Po
8585AtAt
AstatineAstatine210210
8686RnRn
RadonRadon222222
787Fr
Francium223
88Ra
89Ac
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Unn
111Uuu
112Nam
LANTHANIDES58Ce
Cerium140
59Pr
60Nd
61Pm
62Sm
63Eu
64Gd
65Tb
66Dy
67Ho
68Er
69Tm
70Yb
71Lu
Lutetium175
ACTINIDES90Th
Thorium232
91Pa
92U
93Np
94Pu
95Am
96Cm
97Bk
98Cf
99Es
100Fm
101Md
102No
103Lr
Lawrencium260
IONIC FORMULAECATIONS (positive ions) ANIONS (negative ions)
Sodium ion Na+
Potassium ion K+
Hydrogen ion H+
Ammonium ion NH4+
Copper(II) ion Cu2+
Zinc ion Zn2+
Iron(II) ion Fe2+
Lead(II) ion Pb2+
Magnesium ion Mg2+
Aluminium ion Al3+
Silver ion Ag+
Calcium ion Ca2+
Barium ion Ba2+
Iron(III) ion Fe3+
Chromium(III) ion Cr3+
Mercury(I) ion Hg+
Chloride ion Cl¯
Bromide ion Br¯
Oxide ion O2¯
Hydroxide ion OH¯
Nitrate ion NO3¯
Sulphate ion SO42¯
Carbonate ion CO32¯
Manganate(VII) ion MnO4¯
Iodide ion I¯
Hydride ion H¯
Chlorate(V) ion ClO3¯
Ethanoate ion CH3COO¯
Phosphate ion PO43¯
Sulphide ion S2¯
Chromate(VI) ion CrO42¯
Dichromate(VI) ion Cr2O72¯
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Proton numberSymbol of elementName of elementRelative atomic mass
18 Groups
Charges in the positive ions (cations)Most of the metal ions have charges +2. You are only have to memorize the ions that have charges +1 and +3!.(g) Metal ions charged +1 are came from GROUP 1 which are Li+, Na+ and K+. Some others are Ag+, NH4
+, and H+.(h) Metal ions charged +3 are Al3+and Cr3+.(i) Roman numerals in brackets after the metal formulae to denote represent their charges. E.g.;, iron(II) = Fe2+ and ion chromium(III) = Cr3+.
Charges in the negative ions (anions)Most of the anions have charges -1. You are only have to memorize the ions that have charges -2 and -3!.(e) Some of the negative ions with -2 charged are O2-, SO4
2-, CO32-, CrO4
2-, and Cr2O72-.
(f) The common -3 charged ion is PO43-
CHEMICAL FORMULAEAcids Gases Organic Compounds
Hydrochloric acid HCl Oxygen O2 Carbon tetrachloride CCl4
Sulphuric acid H2SO4 Hydrogen H2 Chloroform CHCl3
Nitric acid HNO3 Carbon dioxide CO2 Hexane C6H14
Phosphoric acid H3PO4 Carbon monoxide CO Hexene C6H12
Ethanoic acid CH3COOH Ammonia NH3 Benzene C6H6
Alkalis Nitrogen N2 Methane CH4
Sodium hydroxide NaOH Hydrogen sulphide H2S Ethane C2H6
Potassium hydroxide KOH Nitrogen dioxide NO2 Ethene C2H4
Barium hydroxide Ba(OH)2 Sulphur dioxide SO2 Ethanol C2H5OH
Ammonium hydroxide NH4OH Chlorine Cl2 Ethanoic acid CH3COOH
Calcium hydroxide Ca(OH)2 Hydrogen chloride HCl Glucose C6H12O6
[email protected] : Jadual Perkalaan Unsur Berinformasi
duplet
octet
No. of particles Gas volume
Mass
No. of Mole
x Molar mass Molar mass
x NA
NA
24 dm3 (rc) @ 22.4 dm3 (stp)
x 24 dm3 (rc) @ 22.4 dm3 (stp)
INFORMATIVE PERIODIC TABLE OF ELEMENTS
Proton no. = no. of protonNucleon no. = no. of proton + no. of neutronAtom : no. of proton = no. of electron (neutral)Cation : no. of proton > no. of electronAnion : no. proton < no. of electron
Atom – All metal elements & member of group 18.Molecule compound – comb. of non-metal atoms.Ionic compound – metal ions + non-metal ions.
ELECTROCHEMICAL SERIES
1H2H+
11
+ve ions (cation)K+ Co2+
Na+ Ni2+
Ca2+ Mn2+
Mg2+ Cr3+
Al3+
Zn2+
Fe2+/3+
Sn2+
Pb2+
H+
Cu2+
Ag+
Au+
-ve ions (anion)F- CO3
2-
SO42- MnO4
-
NO3- CrO4
2-
Cl- Cr2O72-
Br- PO43-
I-
OH-
2He42
3LiLi+
72.1
Be HH is not the member of group 1. Mercury, Hg is a liquid metal. Si can be used to produce semiconductor.
- Going down groups ; - size of atoms increase.
- electropositivity of element increase.
- Across periods to the right;- size of atoms decrease.- electronegativity of elements increase.
BB
6C122.4
7N2
142.5
8O2O2
162.6
9F2F
192.7
10Ne2.8
11NaNa+
232.8.1
12MgMg2+
242.8.2
13Al27
2.8.3
14SiSi2828
2.8.4
15P31
2.8.5
16SS2
322.8.6
17Cl2Cl
35.52.8.7
18Ar
2.8.8
Metals MetaloidMetaloid Non-metals Oxide bases Transition elements Amphoteric Oxide acids Inert
19K K+
392.8.8.1
20CaCa2+
402.8.8.2
Cr MnFe56
Co NiCu64
Zn65 GeGe AsAs
Br2Br
80Kr
RbAg108
Cd Sn SbSb TeTeI2I
127Xe
CsPt Au
Hg(l) Pb207 PoPo At2 Rn
IONIC FORMULAEIONIC FORMULAECATIONs ANIONsSodium ion Na+ Potassium ion K+ Silver ion Ag+ Hydrogen ion H+
[email protected] : Periodic Table + Chemical Formulae Dengan berusaha gigih, pastinya kimia itu mudah!
Noble
gase
s
Formation of chemical bond in..A Ionic bond (in the ionic compound). metal atom (release e) + nonmetal atom (accept e)
(concept of transferring e)B Covalent bond (in the molecule compound). nonmetal atom + nonmetal atom (share e)
(concept of sharing e)
Tendency to discharge ions increase
7
Per I ods
18 Groups
Special features of Transition Metals
5. Form coloured ions / compounds / solutions.6. Varying oxidation numbers.
(eg: Fe +2,+3 ; Cu +1,+2)7. Show catalytic properties.8. Form complex coloured ions.
Pe
riod 3
AlkalineAlkaline metalsmetals
Halog
en H
alogen
Avogadro N
o., NA
= 6.02 x
1023
Direction of electron movement in…
Electrolytic cellVoltaic cell andRedox cell…anode e- cathode
Earth-Earth- alkalinealkaline metalsmetals
Ammonium ion NH4+
Copper(II) ion Cu2+
Calcium ion Ca2+
Barium ion Ba2+
Zinc ion Zn2+
Iron(II) ion Fe2+
Iron(III) ion Fe3+
Lead(II) ion Pb2+
Aluminium ion Al3+
Chromium(III) ion Cr3+
Magnesium ion Mg2+
Mercury(I) ion Hg+
Chloride ion Cl¯Bromide ion Br¯
Iodide ion I¯Hydroxide ion OH¯Nitrate ion NO3¯Hydride ion H¯Chlorate(V) ion ClO3¯Ethanoate ion CH3COO¯Manganate(VII) ion MnO4¯
Oxide ion O2¯Phosphate ion PO4
3¯Sulphide ion S2¯Sulphate ion SO4
2¯Carbonate ion CO3
2¯Chromate(VI) ion CrO4
2¯Dichromate(VI) ion Cr2O7
2¯
Charges in the positive ions (cations)Most of the metal ions have charges +2. You are only have to memorize the ions that have charges +1 and +3!.(j) Metal ions charged +1 are came from GROUP 1 which are Li+, Na+ and K+. Some others are Ag+, NH4
+, and H+.(k) Metal ions charged +3 are Al3+and Cr3+.(l) Roman numerals in brackets after the metal formulae to denote represent their charges. E.g.;, iron(II) = Fe2+ and ion chromium(III) = Cr3+.
Charges in the negative ions (anions)Most of the anions have charges -1. You are only have to memorize the ions that have charges -2 and -3!.(g) Some of the negative ions with -2 charged are O2-, SO4
2-, CO32-, CrO4
2-, and Cr2O72-.
(h) The commonly -3 charged ion is PO43-
CHEMICAL FORMULAECHEMICAL FORMULAEAcids Gases Organic CompoundsHydrochloric acid HCl Oxygen O2 Carbon tetrachloride CCl4Sulphuric acid H2SO4 Hydrogen H2 Chloroform CHCl3Nitric acid HNO3 Carbon dioxide CO2 Hexane C6H14
Phosphoric acid H3PO4 Carbon monoxide CO Hexene C6H12
Ethanoic acid CH3COOH Ammonia NH3 Benzene C6H6
Alkalis Nitrogen N2 Methane CH4
Sodium hydroxide NaOH Hydrogen sulphide H2S Ethane C2H6
Potassium hydroxide KOH Nitrogen dioxide NO2 Ethene C2H4
Barium hydroxide Ba(OH)2 Sulphur dioxide SO2 Ethanol C2H5OHAmmonium hydroxide NH4OH Chlorine Cl2 Ethanoic acid CH3COOHCalcium hydroxide Ca(OH)2 Hydrogen chloride HCl Glucose C6H12O6
[email protected] : Periodic Table + Chemical Formulae Dengan berusaha gigih, pastinya kimia itu mudah!
1 Ion +ve (kation)K+ Co2+
Na+ Ni2+
Ca2+ Mn2+
Mg2+ Cr3+
Al3+
Zn2+
Fe2+/3+
Sn2+
Pb2+
H+
Cu2+
Ag+
Au+
Ion -ve (anion)F- CO3
2-
SO42- MnO4
-
NO3- CrO4
2-
Cl- Cr2O72-
Br- PO43-
I-
OH-
18
1
H21
2 13 14 15 16 172
He2
3Li
2.1Be B
6C
2.4
7
N22.5
8
O22.6
9
F22.7
10Ne2.8
11Na
2.8.112Mg
2.8.2
13Al
2.8.3
14Si
2.8.4spara logam
15P
2.8.5
16S
2.8.6
17
Cl22.8.7
18Ar
2.8.8
Logam Bukan logam<Oksida Bes> Unsur Peralihan <Amfoterik> < Oksida Asid > Lengai
19K
2.8.8.1
20Ca
2.8.8.2Cr Mn Fe Co Ni Cu Zn Br2 Kr
Rb Ag Cd Sn I2 XeCs
Pt Au Hg(ce) Pb At Rn
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1. Membentuk sebatian bewarna2. Lebih dari satu no. pengoksidaan ( eg: Fe +2,+3 ; Cu +1,+2 )3. Sebagai mangkin4. Membentuk ion kompleks
Kala 3
Oktet
AsidHClH2SO4 -dwibes
HNO3
CH3COOH-lemah
AlkaliNaOHKOH
NH3 - lemah
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Duplet
Semakin mudah dinyahcaskan
4 OH- 2H2O + O2 + 4e-
Terminal –ve e- Terminal +ve