This document discusses the classification and properties of solids, solutions and colligative properties, chemical thermodynamics and energetics, electrochemistry, chemical kinetics, isolation of elements, p-block elements, and corrosion. Key points include the different types of unit cells and packing efficiency in crystalline solids, concentration units for solutions, lowering of vapor pressure and freezing point depression as colligative properties, spontaneity of reactions based on Gibbs free energy, electrode potentials and cells, temperature dependence of reaction rates by the Arrhenius equation, extraction of metals like zinc and iron from their ores, and properties of p-block elements.
Basic principles & questions and answers of organic chemistry Bryar Ali Rus
this is some basic principles and question & answers of previous years of organic chemistry with notes on dr.emad manhal's examination , school of pharmacy , university of sulaimani .
Basic principles & questions and answers of organic chemistry Bryar Ali Rus
this is some basic principles and question & answers of previous years of organic chemistry with notes on dr.emad manhal's examination , school of pharmacy , university of sulaimani .
B.Sc. Sem-I Unit-IV Mechanism of electrophilic aromatic substitution by Dr P...pramod padole
Mechanism of Electrophilic Aromatic Substitution: Nitration, Friedal Craft Alkylation and Acylation.Nuclear and Side Chain
Halogination, Birch Reduction
Basic principles in organic chemistry --exercise with solutionssuresh gdvm
Basic principles in organic chemistry. basics of organic chemistry, types of organic compounds, effects in organic compounds such as inductive effect, electromeric effect, resonance, hyperconjugation, IUPAC nomenclature
Organometallic Reactions and CatalysisRajat Ghalta
Organometallic compounds undergo a rich variety of reactions (oxidative addition, reductive elimination, cyclometalization, migratory insertion, carbonylation, hydrometallation hydrate elimination, etc ) that can sometimes be combined into useful homogeneous catalytic cycles. In this presentation, I have discussed organometallic reactions of particular importance for synthetic and catalytic processes like the oxo process (hydroformylation), heck coupling reaction, Wilkinson’s Catalyst
(Hydrogenation) etc.
A carbene is any neutral carbon species which contains a non-bonding valance pair of electrons.
Contributed by Alison Brown & Nathan Buehler, Undergraduates, University of Utah
Basic concepts of organic chemistry such as structural formulas, different kinds of representation, types of isomerism, examples, alkanes, alkenes, alkynes etc.
Its related to Study of gene metal-ligand stability constant of cefadroxil with cu2+ metal ion ph metrically at 0.1 m ionic strength. Also describe another Parameters.
B.Sc. Sem-I Unit-IV Mechanism of electrophilic aromatic substitution by Dr P...pramod padole
Mechanism of Electrophilic Aromatic Substitution: Nitration, Friedal Craft Alkylation and Acylation.Nuclear and Side Chain
Halogination, Birch Reduction
Basic principles in organic chemistry --exercise with solutionssuresh gdvm
Basic principles in organic chemistry. basics of organic chemistry, types of organic compounds, effects in organic compounds such as inductive effect, electromeric effect, resonance, hyperconjugation, IUPAC nomenclature
Organometallic Reactions and CatalysisRajat Ghalta
Organometallic compounds undergo a rich variety of reactions (oxidative addition, reductive elimination, cyclometalization, migratory insertion, carbonylation, hydrometallation hydrate elimination, etc ) that can sometimes be combined into useful homogeneous catalytic cycles. In this presentation, I have discussed organometallic reactions of particular importance for synthetic and catalytic processes like the oxo process (hydroformylation), heck coupling reaction, Wilkinson’s Catalyst
(Hydrogenation) etc.
A carbene is any neutral carbon species which contains a non-bonding valance pair of electrons.
Contributed by Alison Brown & Nathan Buehler, Undergraduates, University of Utah
Basic concepts of organic chemistry such as structural formulas, different kinds of representation, types of isomerism, examples, alkanes, alkenes, alkynes etc.
Its related to Study of gene metal-ligand stability constant of cefadroxil with cu2+ metal ion ph metrically at 0.1 m ionic strength. Also describe another Parameters.
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Postsecondary lesson for pre-u students or form 6th students on mole concept, stoichiometry, limiting reagent, spectrometry and percent yield and percent purity.
2. 1. Solid State
Classification of Solids
Classification of crystalline
solids
3. Unit cells, two and three dimensional
lattices and number of atoms per unit
cell and
Number of Atoms in the unit cell :
Unit cell scc bcc fcc hcp
Number of 1 2 4 3
atoms
5. Relation between radius (r) of an
atom and edge length (a) of cubic
unit cell :
scc bcc fcc
a 3 a
r r a r
2 4 2 2
6. Packing in solids
Density of unit cell
∙ Density of the crystal :
z M
d 3
a NA
7. Packing in voids of ionic solids
Defects in crystal structure
Electrical properties
Magnetic properties
8. 2. Solutions & Colligative
Properties
Types of solution
Concentration of solution of solids
in liquids
W
n
Number ofnmoles, M mol
Molarity = V mol dm-3 (or M)
Normality = gra m e q. gram eq.dm -3
V
9. Solubility of gases in liquids
Solid solution
Colligative properties and
molecular masses
Lowering of vapour pressure
10. n
Molality = W t. of solven t in kg
mol kg -1 (or m)
Raoult’s law: Psoln = x1 P0
P0 P W2 M 1
P0 W1M 2
11. Elevation of boiling point
Tb = Kbm and Tf = kf m
W2 1000
Tb = Kb
W1 M2
12. Depression of freezing point
W2 1000
Tf = Kf W1 M2
Osmotic pressure
2
C2
At constant temperature : C1
1
2
T2
At constant concentration : T1
1
17. 3. Chemical Thermodynamics
& Energetics
Basic concepts in thermodynamics
Nature of Heat and Work
Internal Energy
18. W = - P (V2 – V1) = -P V
(For expansion)
W = P (V2 – V1) – P V
(For compression)
V2
Wmax = - 2.303 nRT log10
V1
P1
Wmax = - 2.303 nRT log10 P2
19. First Law of Thermodynamics
Enthalpy
U=q+W
H = U + PV
H= U+P V
H = U + nRT
20. Enthalpy of physical changes
Thermo chemistry
Spontaneous processes
(Irreversible processes)
Gibbs free energy
S q rev H
T T
G = H – TS
21. G= H-T S
G0 = - 2.303 RT log10K
G = 0, the system is at
equilibrium
G < 0, the process is
spontaneous
G > 0, the process is non-
spontaneous.
Third law of thermodynamics.
23. Potential difference (V)
Resistance (R)
Electric current (I)
1 1
Electrical conductance (G)
R
or S
a
Resistivity ( ) R cm
1
24.
Cell constant = cm-1(or m– 1)
a
C e ll C o n s tan t
Conductivity (k)
R e s is tan ce
Molar conductivity (∧m) = (k in Ω-1
k
m-1 and C in mol m-3) OR C
25. k 1000
∧m
C
(k in Ω-1 m-1 and C in mol m-3)
0 0
Kohlarausch’s law : ∧0
m
Degree of dissociation ( )
0
2
m C
Dissociation constant (ka) (
0 0 m)
26. Electrochemical cells
Electrolytic cells
Galvanic or voltaic cells
Electrode potentials and cells potential
27. 0 0 0
E cell E red (cathode) E red (anode)
0 0.0592 n
EM n / M
E Mn log10 [M ]
/M
n
0 0 .0 5 9 2 [P r o d u c ts]
E c e ll E c e ll lo g1 0
n [R e a c ta n ts]
28. 0 0
G n FE cell
∆G = nFEcell
∆G0 = - RTln K
0 0.0592
E cell log10 K
n
For spontaneous cell reaction :
Ecell > 0; ∆G < 0
29. 5. Chemical Kinetics
Rate of reaction
For a reaction, aA + bB cC + dD
1 [A ] 1 [B] 1 [C] 1 [D ]
a t b t c t d t
Average rate =
Rate law : Rate = k [A]a [B]b
30. Dependence of rate on reactant
concentration
2 .3 0 3 [A ]0
k
t log0 [A ] t
(for first order reaction)
0.693
t ½ = k (for first order
reaction)
31. [A ]0 [A ]t
k=
t
(For zero order reaction)
[A ]0
t½= (For zero order reaction
2k
Molecularity of elementary reactions
Collision theory and activation energy
32. Temperature dependence of
reaction rates (Arrhenius equation)
K = Ae– Ea/RT (Arrhenius equation)
Ea
Log10k = log10A – 2 .3 0 3R T
Log10
33. Effect of catalyst on rates of
reactions
k2 E a ( T2 T1)
k1 2 .3 0 3R T1 T2
34. 6. General & Processes
of Isolation of Elements
Concentration of an ore
Oxidation – reduction
Refining of crude metal
35. Extraction of Zinc
Extraction of Iron
Extraction of Aluminium
Extraction of Copper
36. 7. p–Block Elements
Group 15 elements
Group 16 elements
Group 17 elements
Group 18 elements
37. Reference electrodes
Common types of cells
Fuel cells
Electrochemical series
Corrosion