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Intramolecular force vs Intermolecular force
Generally, Intramolecular forces are stronger than Intermolecular forces.
1
1. Covalent bonding- Between nonmetallic elements of similar
electronegativity.
2. Ionic bonding- Between metallic and nonmetallic elements of
different electronegativity.
3. Metallic bonding- Between metallic elements.
Types of Intramolecular Forces(Chemical Bonding)
2
Fill in the blanksubstance Type of bond substance Type of bond
S8 SiCHNO3 Cr2O3
CuCl TiCoSO4 SiH4
Na KICaHPO4 AuCH2O K4[Fe(CN)6]
3
Covalent bonding- Formed by sharing electron pairs
Examples; O2, CO2, C2H6, H2O, SiC , F2
H2 - bonding
The bond occure from the together attraction of 2 nuclei for the same electrons.
H + H H2
4
Lewis dot symbol of elements
5
Types of Covalent BondingTypes of Covalent Bonding can be determined from
the number of bond pair electrons. 1. single bond is covalent bond that two atoms use
one bond pair electrons to from chemical bonding. Give ( - ) for single bond such as Cl2 , NH3 etc.
6
bond pair electrons vs lone pair electrons
7
2. Double bond is covalent bond that two atoms use two bond pair electrons to from chemical bonding. Give ( = ) for double bond such as O2 , CO2 , C2H4
8
3. Triple bond is covalent bond that two atoms use three bond pair electrons to from chemical bonding. Give( ≡ ) for triple bond such as N2 , HCN , C2H2
9
Coordinate covalentbond is covalent bonding that one atom give one lone
pair electrons to other atom to form chemical bonding , following �Octet Rule� such as NH3 and H+ , SO2 , SO3
10
¨§e¢Õ¹¾ a¹¸ao¤ooà � ie¹µo¤eÇeŹµ � ¢o§oÁeÅ¡ uŵ �o仹Õé SO3 O3
HClO4 HNO3
HClO3 BF3 + NH3
11
Non-octet Molecules- Less octet molecules such as BeCl2 , BCl3
- More octet covalent molecules such as PCl5 , SF6
12
Nomenclature of Covalent Compound1. Covalent Elements ; using the name of this element.
Usually give the phase of this elements together O2
Cl2P2
Br2S8
2. covalent compounds are named by using prefixes to indicate how many atoms of each element are shown in the formula and the ending of the last element is changed to -ide.prefixes mono = 1 , di = 2 , tri = 3 , tetra = 4 , penta = 5
hexa = 6 , hepta = 7 , octa = 8 , nona = 9 13
ExampleCO2 named ���������.���������..���������...
BF3 named ���������.���������..���������...
Cl2O named ���������.���������..���������...
Si2Cl8 named ���������.���������..���������...
SF6 named ���������.���������..���������...
P4O10 named ���������.���������..���������...
Cl2Br7 named ���������.���������..���������...
C2H6 named ���������.���������..���������...
H2Se named ���������.���������..���������...
CS2 named ���������.���������..���������...
14
Writing the formula for covalent compounds1. Find the number of bonds that element want to form ;
Group 1 : H : form : 1 bondsGroup 2 : Be Mg : form : 2 bonds
Group 3 : B : form : 3 bonds Group 4 : C Si : form : 4 bonds
Group 5 : N : form : 3 bonds Group 6 : O S : form : 2 bonds Group 7 : F Cl Br I : form : 1 bond
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Ex formula(following rules)B and FSi and ClN and HC and SSi and ClCl and OSn and HSe and BrH and Te
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Bond length and Bond Energy
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Bond length (pm)
18
Bond Energies (kJ/mol)
19
summary
Comparison of Bond length between same elements
Comparison of Bond energy between same elements
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Calculating ΔH using bond energies.Form bond : Exothermic reaction : H = (-)
Break bond : Endothermic reaction : H = (+)
H is Heat
Form bond
e.g. 2Cl (g) Cl2 (g) ; H = 242 kJ/molBreak bond
e.g. Cl2 (g) 2Cl (g) ; H = -242 kJ/mol
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Example : Calculate the energy for breaking CO2 1 mol from molecule to atoms and this process is endothermic or exothermic reaction.
Example : Calculate the energy for breaking CCl4 2 mol from molecule to atoms and this process is endothermic or exothermic reaction.
22
Example : Calculate the energy of the reaction for the burning of methane in oxygen to form carbon dioxide gas and water gas, using heats of formation. The balanced equation is given below. Use the following list of bond energies
CH4(g) + 2O2(g) CO2(g) + 2H2O (g)
23
Ex Chlorine gas react with methane gas following below equation
CH4(g) + 2Cl2(g) CH2Cl2(g) + 2HCl (g) this process is endothermic or exothermic reaction and how many energies change.
24
ResonanceThe appearance of delocalized electrons within certain
molecules or polyatomic ions, so that the bonding cannot be expressed by one single Lewis formula.
25
Draw Resonance structure of O3, SO3, PO43-, -, SO3
2-, SO42-
26
- เปนทฤษฎทใชอธบายการเกดพนธะในโมเลกลของสารประกอบโคเวเลนต1. sp3 -hybrid orbital
ไดจากการรวมกนของ s-orbital 1 orbital และ p-orbital 3 orbitalExample CH4
พจารณาการจดอเลกตรอนของอะตอมกลาง 6C :1s22s2 2p2
• Four atomic orbitals (2s + 3 × 2p) mix to form four hybrid orbitals (4 × sp3)
ทฤษฏไฮบรดออรบทล
27
sp3 Hybrid Orbitals
28
พนธะทง 4 ใน CH4 เกดจาก 1s -orbital ของ H 4 อะตอม ซอนเหลอม(overlap) กบ 2sp3-orbital ของ C 1 อะตอม
sp3
C
29
2. sp2 -hybrid orbitalไดจากการรวมกนของ s-orbital 1 orbital และ p-orbital 2 orbital
Example BF3
พจารณาการจดอเลกตรอนของอะตอมกลาง 5B :1s22s2 2p1
พจารณาการจดอเลกตรอนของอะตอมขางเคยง 9F :1s22s2 2p5
Three atomic orbitals (2s + 2 × 2p) mix to form three hybrid orbitals (3 × sp2)
30
sp2 Hybrid Orbitals
31
พนธะทง 3 ใน BF3 เกดจาก 2p -orbital ของ F 3 อะตอม ซอนเหลอม(overlap) กบ 2sp2-orbital ของ B 1 อะตอม
2sp2
B B
32
Ethylene H
H
H
HC = C
1. Each C – H bond is a σ bond formed from the overlap of a C sp2 orbital with the H 1s orbital.
2. One of the C – C bonds is a σ bond formed from the overlap of C sp2 orbitals3. The second C – C bond is a π bond formed from the overlap of the unhybridized
C 2p orbitals.
sp2 -hybrid orbital
33
3. sp -hybrid orbitalไดจากการรวมกนของ s-orbital 1 orbital และ p-orbital 1 orbital
Example BeCl2
พจารณาการจดอเลกตรอนของอะตอมกลาง 4Be :1s22s2
พจารณาการจดอเลกตรอนของอะตอมขางเคยง 17Cl :1s22s22p63s22p5
Two atomic orbitals (2s + 2p) mix to form two hybrid orbitals (2 × sp)
2
34
sp Hybrid Orbitals
35
พนธะทง 2 ใน BeCl2 เกดจาก 3p -orbital ของ Cl 2 อะตอม ซอนเหลอม(overlap) กบ 2sp-orbital ของ Be 1 อะตอม
2spBe
36
Acetylene H - C ≡ C - H
1. Each C – H bond is a σ bond formed from the overlap of a C sp orbital with the H 1s orbital.
2. One of the C – C bonds is a σ bond formed from the overlap of C sp orbitals.3. The other two bonds are π bonds formed from the overlap of the C 2p orbitals.
sp -hybrid orbital
37
Molecular shapes(Molecular Geometry)
Valence-Shell Electron-Pair Repulsion (VSEPR) theory is a model in chemistry used to predict the shape of individual molecules based upon the extent of electron-pair electrostatic repulsion
• The "AXE method" of electron counting is commonly used when applying the VSEPR theory.
AXmEn
38
39
Method to determine a molecular shapes
Covalent compound CF4Molecular shape
# valent ē of center atom
# ē of outside atom to form bond
# ē from charge
total e
# bond pair ē or # bond
# lone pair ēfomular
Hybrid Orbitals
Angle between atom 40
Method to determine a molecular shapes
Covalent compound CO32- Molecular shape
# valent ē of center atom
# ē of outside atom to form bond
# ē from charge
total e
# bond pair ē or # bond
# lone pair ē
fomular
Hybrid Orbitals
Angle between atom
41
Method to determine a molecular shapes
Covalent compound NH4+ Molecular shape
# valent ē of center atom
# ē of outside atom to form bond
# ē from charge
total e
# bond pair ē or # bond
# lone pair ē
fomular
Hybrid Orbitals
Angle between atom
42
Method to determine a molecular shapes Covalent compound I3
- Molecular shape
# valent ē of center atom
# ē of outside atom to form bond
# ē from charge
total e
# bond pair ē or # bond
# lone pair ē
fomular
Hybrid Orbitals
Angle between atom 43
Method to determine a molecular shapes Covalent compound AsH3
Molecular shape
# valent ē of center atom
# ē of outside atom to form bond
# ē from charge
total e
# bond pair ē or # bond
# lone pair ē
fomular
Hybrid Orbitals
Angle between atom 44
Method to determine a molecular shapes Covalent compound XeOF2
Molecular shape
# valent ē of center atom
# ē of outside atom to form bond
# ē from charge
total e
# bond pair ē or # bond
# lone pair ē
fomular
Hybrid Orbitals
Angle between atom 45
Polarity in Polyatomic MoleculesPolarity
Bond Molecule
- Polar bond - Polar molecule- Non-polar bond - Non-polar molecule
Determine polarity of bond by using EN
46
Non-polar bond- EN = 0 e.g. H2 , N2 , Cl2 - If the molecule has non-polar bond so this molecule
is also Non-polar molecule.
Polar bond - EN > 0 e.g. HCl, CO2 , N2O
- If the molecule has polar bond this molecule can be Non-polar molecule or Polar molecule.
47
Polar bond but Non-polar molecule
e.g. CO2 , BF3
Polar bond and Polar molecule e.g C2H2Cl2 , H2O
ᵟ-ᵟ+ᵟ- B
F
F F
48
� Polarity can use to predict a solubility of molecule in a solvent �Example Polar molecule can soluble in polar molecule
e.g. NH3 , C2H5OH , H2O are polar molecule
So NH3 and C2H5OH can soluble in water(H2O)
Non-polar molecule cannot soluble in polar molecule but can soluble in non-polar molecule.
Oil is non-polar molecule So Oil cannot soluble in water but oil can soluble in non-polar molecule such as Hexane(C6H12)
49
1. Van der Waals force1) Dipole-dipole interaction
Attractive forces between polar moleculese.g. I-Cl----- I-Cl2) Dipole-induced dipole interaction
Attractive forces between polar molecule and non-polar moleculee.g. H-Cl----- Cl-Cl
3) Dispersion force or London forceAttractive forces between non-polar molecules
e.g. F2-----F2
Intremolecular force
50
Hydrogen BondingA hydrogen bond is the attractive interaction of
a hydrogen atom with an electronegative atom, such as nitrogen, oxygen or fluorine
e.g. Hydrogen bonding in HF molecule
H — F ……. H — F
51
H O.. ..
HH O.. ..
H.. ..H OH
..
H O..H
H F.... ..H F.... ..
..
HF.. ..
Covalent bond
Hydrogen bond
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Effect of Hydrogen bond
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Network Structure - The structures of giant covalent substances like
diamond, graphite and silicon dioxide
1. Diamond
The physical properties of diamond- has a very high melting point (almost 4000oC). - is very hard. - doesn't conduct electricity. All the electrons are
held tightly between the atoms, and aren't free to move.
3D of Diamond
54
2. Graphite
The physical properties of graphite
- has a high melting point.
- has a soft, slippery feel, and is used in pencils and as a dry lubricant for things like locks.- has a lower density than diamond. - conducts electricity. The delocalised electrons are free to move throughout the sheets.
2D of Graphite
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Silicon dioxide, SiO2
Crystalline silicon has the same structure as diamond. each silicon atom is bridged to its neighbours by an oxygen atom.
The physical properties of silicon dioxide- has a high melting point
- is hard- doesn't conduct electricity
3D of SiO2
56
Ionic Bonding
Bond formed between two ions by the transfer of electronsIonic compounds result when metals react with nonmetals
- Metals lose electrons and form positive charge(cation)
- Nonmetals gain electrons and form negative charge(anions)note;
The Octet Rule: The �goal� of most atoms is to have an 8 electrons in their valence energy level.
Li+ N3- O2- F-
Na+ Mg2+ Al3+ P3- S2- Cl-
K+ Ca2+ Transition metal can form morethan one type of positive ion
Cr2+ Cr3+ Mn2+ Mn3+ Mn4+
Fe2+ Fe3+ Co2+ Co3+ Cu+
Cu2+
Ga3+ Ge4+ As3- Se2- Br-
Rb+ Sr2+ In3+ Sn2+
Sn4+
Sb3- Te2- I-
Cs+ Ba2+ Tl3+ Pb2+
Pb4+
Bi3+
H+
H-
Cation and anion
58องคาร เทพรตนนนท
Examples ; NaCl Ionic BondingBetween Ca and Cl to form CaCl2
Crystal structure of Ionic compound
Na+ : Cl-
:
:
Na+ has ���� nearest Cl- neighbors
Cl- has ���� nearest Na+ neighbors
61องคาร เทพรตนนนท
Ca2+
F-
Ca2+ has ���� nearest F- neighbors
F - has ���� nearest Ca2+ neighbors
Ca2+ : F-
:
:62องคาร เทพรตนนนท
Crystal structure of Ionic compound
Crystal structure of Ionic compound
63องคาร เทพรตนนนท
Cs+ has ���� nearest Cl- neighbors
Cl - has ���� nearest Cs+ neighbors
Cs+ : Cl-
:
:
o¤Ã§Êà �Ò§¢o§ÊÒûÃa¡oºäooo¹ i¡
64องคาร เทพรตนนนท
Writing Ionic Formula1. Always write cation and charge of this ion first.2. The net charge on an ionic compound is zero (sum of the positive charges equals the sum of the negative charges). 3. The formula of an ionic compound represents the simplest whole number ratio of ions present.
Na and Cl Na+ and Cl-
Mg and F Mg2+ and F-
Ba and OCH3COO- and CaNH4
+ and PO43-
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Write Ionic Formula
cationanion
Na Ca Al NH4
F
O
N
CN
CO3
PO466องคาร เทพรตนนนท
Naming Ionic CompoundsThe name of the positive ion is given first,
followed by the name of the negative ion.Naming Positive Ions(Cation)
1. For a monoatomic positive ion, that is, a metal cation, the name is that of the metal plus the word �ion.� For example,
Na+ is the Mg2+ is the Al3+ is the NH4
+ is the67องคาร เทพรตนนนท
2. Some cases occur, especially in the transition series, in which a metal can form more than one type of positive ion . The most common practice is to indicate the charge of the ion by a Roman numeral in parentheses immediately following the ion�s name. For example,
Co2+ is the Co3+ is the Sn2+ is the Sn4+ is the
Naming Negative Ions(Anion)1. A monatomic ion, the anion is named by
adding the suffix -ide to the root of the element name. For example,
Cl- is theO2- is the
2. Polyatomic negative ions, Most of these names must simply be learned. For example,
NO2- is the
NO3- is the
SO32- is the
CN- is the
ExampleNaCl :MgO :FeCl2 : CuO :MnO2 : (NH4)3PO4 : Li2NO3 :Cr2(SO4)3 :Mn(OH)4 :
70องคาร เทพรตนนนท
Naming Ionic Compound
1. NaBr2. GaAs3. K3N4. NH4Cl 5. Be(HCO3)26. Al(CN)37. Cu3P8. Pb3N2
9. AuClO3
10. Mn2(SO3)3
71องคาร เทพรตนนนท
Born-Harber cycleThe Born�Haber cycle involves the formation of an ionic
compound from the reaction of a metal with a non-metal. There are five steps.
1. Heat of Sublimation ; S
2. Dissociation Energy ; D or bond enthalpy
3. Ionization energy ; IE
4. Electron Affinity ; EA
5. Lattice energy ; ΔHlatt
H0f = S + D + IE + EA + ΔHlatt
72องคาร เทพรตนนนท
The enthalpy of formation of Sodium chloride
73องคาร เทพรตนนนท
Step 1
Step 2
Step 3
Step 4
Step 5Net Reaction :
The Heat(enthalpy) of formation of Sodium chloride
Heat of Sublimation Dissociation Energy Ionization energy Electron Affinity Lattice energy
74องคาร เทพรตนนนท
Born-Haber cycle of NaCl
Na(s) + 1/2Cl2(g) NaCl(s)
Na(g) Cl(g)
Na+(g) + Cl-(g)
Hf
H1 H2
H3 H4
H5
Heat of formation NaCl : Hf = H1 + H2 + H3 + H4 + H5
75องคาร เทพรตนนนท
Draw a diagram and calculate the heat of formation of LiF
Give1. Heat of Sublimation of Li = 161 kJ/mol2. Dissociation Energy of F2 = 159 kJ/mol3. First Ionization energy of Li = 520 kJ/mol4. Electron Affinity of F= -328 kJ/mol5. Lattice energy of LiF = -1,047 kJ/mol
76องคาร เทพรตนนนท
The Heat(enthalpy) of formation of Lithium chloride
step 1
step 2
step 3
step 4
step 5
Net reaction
77องคาร เทพรตนนนท
Born-Haber cycle of LiF
78องคาร เทพรตนนนท
Draw a diagram and calculate the heat of formation of MgCl2
Give1. Heat of Sublimation of Mg = 148 kJ/mol2. Dissociation Energy of Cl2 = 234 kJ/mol3. First Ionization energy of Mg = 738 kJ/mol4. Second Ionization energy of Mg = 1,451 kJ/mol5. Electron Affinity of Cl = -349 kJ/mol6. Lattice energy of MgCl2= -2,524 kJ/mol
79องคาร เทพรตนนนท
The Heat(enthalpy) of formation of Magnesium chloride
Step 1
Step 2
Step 3(IE1+IE2)Step 4
Step 5
Net reaction :
80องคาร เทพรตนนนท
Born-Haber cycle of MgCl2
81องคาร เทพรตนนนท
Physical Properties of Ionic Compounds
Hard , crystalline solids but crack High melting point and boiling point Solid do not conduct electricity , when molten or dissolved in water , they can conduct electricity. Many ionic compound are soluble in water.
82องคาร เทพรตนนนท
Electrical Conductance of Ionic Compounds
83องคาร เทพรตนนนท
Physical Properties of Ionic Compounds
Compound Appearance Melting point
(C)
Boiling point
(C)
Soluble in water at 20C(g/water 100 g)
NaClLiF
CaCl2Al2O3
Fe2O3
White solidWhite solidWhite solidWhite solidRed Brown
solid
80184678220721565
1413171716002980
-
36.00.1374.5
Not solubleNot soluble
84องคาร เทพรตนนนท
Ionic compounds dissolve in water
Some ionic compounds (salts) dissolve in water, the salt's positive ions (e.g. Na+) attract the partially-negative oxygens in H2O. Likewise, the salt's negative ions (e.g. Cl−) attract the partially-positive hydrogens in H2O.
Dissolve in water of Ionic compounds relate with 2 steps
1. Lattice Energy2. Hydration Energy
องคาร เทพรตนนนท 85
Ionic compounds dissolve in water
86องคาร เทพรตนนนท
Heat of Solution Lattice energy is the energy required to break the
ions in their lattice arrangement into the ions in the gas phase , For example
NaCl(s) ---> Na+(g) + Cl-(g) Hydration energy is the energy released when the ion
dissolves in water forming an infinite dilute solution in the process, For example
Na+(g) + Cl-(g) ---> Na+(ag) + Cl-(ag) Heat of Solution is the energy required or released
when 1 mole ionic compound dissolves in solvent(water). Heat of Solution = Lattice energy - Hydration energy
Hsolution = Hlattice + Hhydration 87องคาร เทพรตนนนท
Example Dissolving NaCl in water
Lattice energy
NaCl(s) Na+(g) + Cl-(g) H = 776 kJ/mol
Hydration energy
Na+(g) + Cl-(g) Na+(aq) + Cl-(aq) H = - 771 kJ/mol
Heat of solution
NaCl(s) Na+(aq) + Cl-(aq)
Hsolution = 776 - 771 = 5 kJ/mol
88องคาร เทพรตนนนท
H2O
H2O
Diagram of dissolving NaCl in water
89องคาร เทพรตนนนท
If ΔHlatt > ΔHhyd so, ΔHsoln is + (Endothermic process)If ΔHlatt < ΔHhyd so, ΔHsoln is - (Exothermic process)
90องคาร เทพรตนนนท
Ionic compound
Mass(g)
Temperature of water (0C)
Temperature of solution (0C)
Process
CuSO4 1 31.0 35.0
NH4Cl 1 31.0 29.0
NaCl 1 31.0 30.5
KCN 1 31.0 32.5
Ionic compounds dissolve in water
Dissolving KCl in water1. Hlatt = +690 kJ/mol
2. Hhyd = -686 kJ/mol
Write the equation when KCl dissolved in water and calculate Hsoln
Lattic equation (ÊÁ¡ÒÃæÊ´§¾Å a§§Ò¹æŵ· i«)
:
Hydration equation (ÊÁ¡ÒÃæÊ´§¾Å a§§Ò¹äÎe´Ãª a¹)
:
Solution (ÊÁ¡ÒáÒÃÅaÅÒÂ)
:
91องคาร เทพรตนนนท
Diagram of dissolving KCl in water
92องคาร เทพรตนนนท
Write the equation to show the dissolving Ionic compound in water
1. MgBr2
Lattic equation :
Hydration equation :
Solution equation :
2. Na2O
Lattic equation :
Hydration equation :
Solution equation :
องคาร เทพรตนนนท 93
3. AlCl3
Lattic equation :
Hydration equation :
Solution equation :
4. NH4F
Lattic equation :
Hydration equation :
Solution equation :
5. K2CO3
Lattic equation :
Hydration equation :
Solution equation :องคาร เทพรตนนนท 94
Solubility of Ionic compound
95องคาร เทพรตนนนท
- Less than 0.1 g of the substance will dissolve in 100 g of water, the substance is considered insoluble.
- Between 0.1 - 1 g of a substance will dissolve in 100 g of water, the substance is considered moderately soluble.
- More than 1 g of a substance will dissolve in 100 g of water, the substance is considered soluble.
Solubility rules
Writing Net Ionic EquationsNet ionic equations indicate only the substance that
undergo a change and are very important in our study of chemistry.
steps for write net ionic reactions :1. balance the chemical equation. 2. write out the dissolved species as they exist in
solution. Precipitates, liquids and gases are not written as ions. This is called a total ionic equation.
3. remove common aqueous ions, ( ions that are in both the reactant and product) . The resulting equation is called the net ionic equation.
องคาร เทพรตนนนท 98
A solution of Barium chloride combines with a solution of Sodium carbonate to form a precipitate of Barium carbonate and a solution of Sodium Chloride
1. Write the chemical equations and balance BaCl2(aq) + Na2CO3(aq) --> BaCO3(s) + 2NaCl(aq)
2. Write the species as they exist in solution. Leave solids, liquids and gases unchanged.
Ba2+(aq) + 2Cl-(aq) + 2Na+(aq) + CO32-(aq)
---> BaCO3(s) + 2Na+(aq) + 2Cl-(aq) 3. Remove common aqueous ions. (Net Ionic Equations )
Ba2+(aq) + CO32-(aq) ---> BaCO3(s)
องคาร เทพรตนนนท 99
Writing Net Ionic Equations
1. KCl and AgNO3
Chemical Equation :
Ionic Equation :
Net Ionic Equation :
2. KBr and Mg(NO3)2
Chemical Equation :
Ionic Equation :
Net Ionic Equation :
องคาร เทพรตนนนท 100
3. Na2O and AlCl3
Chemical Equation :
Ionic Equation :
Net Ionic Equation :
4. MgBr2 and Pb(ClO3)2
Chemical Equation :
Ionic Equation :
Net Ionic Equation :
5. (NH4)2S and (CH3COO)2Ca
Chemical Equation :
Ionic Equation :
Net Ionic Equation :
องคาร เทพรตนนนท 101
¾ a¹¸aoÅËa ¤o ¾ a¹¸a·Õèe¡ i´¨Ò¡æç´§ Ù´ÃaËÇ �Ò§äooo¹ºÇ¡·ÕèeÃÕ§ª i´¡ a¹¡ aºo ieÅ硵Ão¹·ÕèoÂÙ�o´ÂÃoº
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