No. 3/3/2018-CS.II(A)
Government of India
Ministry of Personnel, Public Grievances and Pension
Department of Personnel & Training
(CS.II Division)

3^{rd } Floor, Lok Nayak Bhavan, Khan Market, New Delhi-110003, Dated, the 5^{th } October, 2018.

OFFICE MEMORANDUM

Subject: Vigilance Clearance and Major/ Minor Penalty Certificate in respect of PS of CSSS – Zone of consideration for the pending Select Lists of PPS-reg.

The undersigned is directed to refer to this Department’s OM No. 3/3/2016-CS.II(A) dated 11.09.2018 vide which vigilance clearance & major/minor penalty certificate for the last 10 years was sought in respect of 311 PSs and to say that this Department is in the process of the exercise of promotion from Private Secretary (PS) grade of CSSS to the post of Principal Private Secretary (PPS) grade of CSSS for the pending Select Lists. In this regard, vigilance clearance and major/ minor penalty certificate (during the last 10 years) in respect of 586 more officers are required. A list of 586 officers is attached at Annexure-I.

2. Concerned cadre units are requested to provide the vigilance clearance and major/minor penalty certificate for the last 10 years (at Annexure-II) in respect of the eligible officers, positively by \mathbf{1 8 . 1 0 . 2 0 1 8} otherwise it would be difficult to consider their names for promotion. The same may also be sent via email: chirabrata.sarkar@nic.in and sumit.k13@nic.in . It may be ensured that personal particulars of these officials have been uploaded in the Web Based Cadre Management System of CSSS.
3. Cadre units may also ensure that complete ACR/APAR grading, as required as per existing instructions, of the officers concerned have been sent to this Division, if not, the same may be made available immediately otherwise in the absence of ACR/APAR, it would be difficult to consider their names for promotion.
4. The list of officers may be seen/downloaded on/from the website of this Department: http://dopt.gov.in > About Us > Central Secretariat> CSSS> Promotions > Regular> PS to PPS.
   (Chirabrata Sarkar)
   Under Secretary to the Government of India
   24623157
   To
   (i) All concerned cadre units of CSSS.
   (ii) The officers concerned.

Chemistry

Chemical Reactions

Balancing Chemical Equations

1. Write the unbalanced equation:

• Example: C3H8 + O2 \rightarrow CO2 + H_2O

1. Balance the equation:

• Balance carbon atoms first.
• Then balance hydrogen atoms.
• Finally, balance oxygen atoms.
• Balanced equation: C3H8 + 7O2 \rightarrow 3CO2 + 4H_2O

1. Balance the equation:

• Balance oxygen atoms first.
• Then balance oxygen oxygen atoms.
• Balanced equation: C3H8 + 7O2 \rightarrow 3CO2 + 4H_2O

Types of Reactions

1. Combination Reaction:

• Example: 2H2 + O2 \rightarrow 2H_2O

1. Decomposition Reaction:

• Example: 2H2O2 \rightarrow 2H2O + O2

1. Single Displacement Reaction:

• Example: Zn + 2HCl \rightarrow ZnCl2 + H2

1. Double Displacement Reaction:

• Example: AgNO3 + NaCl \rightarrow AgCl + NaNO3

1. Combustion Reaction:

• Example: CH4 + 2O2 \rightarrow CO2 + 2H2O

Stoichiometry

Mole Concept

• Mole (mol): The amount of substance containing as many particles (atoms, molecules, ions) as there are atoms in exactly 12 grams of carbon-12.
• Avogadro’s Number: 6.022 \times 10^{23} particles per mole.

Molar Mass

• Molar Mass: The mass of one mole of a substance.
• Example: The molar mass of water (H_2O) is 18.015 g/mol.

Calculations

1. Moles to Mass:

• Formula: n = \frac{m}{M}
• Example: Calculate the number of moles of H_2O in 18 grams of water.
• n = \frac{18.015 \, g}{18.015 \, g/mol} = 2 \, mol

1. Moles to Mass:

• Formula: m = n \times M
• Example: Calculate the mass of 18.015 g of water.
• m = 18.015 \, g/mol = 2 \, mol

Gas Laws

Ideal Gas Law

• Equation: PV = nRT
• Variables:
• P = Pressure (atm)
• V = Volume (L)
• n = Number of moles (mol)
• R = Ideal gas constant (0.0821 L·atm/mol·K)
• T = Temperature (K)

Boyle’s Law

• Equation: P1V1 = P2V2
• Variables:
• P₁ = Pressure (atm)
• P₂ = Volume (L)
• P₃ = Ideal gas constant (0.0821 L·atm/mol·K)
• P₃r = Ideal gas constant (0.0821 L·atm/mol·K)

Charles’s Law

• Equation: V1 = P1V_2
• Variables:
• V₁ = Volume (L)
• V₂ = Ideal gas constant (0.0821 L·atm/mol·K)
• V₃ = Ideal gas constant (0.0821 L·atm/mol·K)
• P2V2 = P3V3
• V₁/V₂ = V2V2

Thermochemistry

Enthalpy (H)

• Definition: The heat content of a system at constant pressure.
• Equation: \Delta H = q_p
• Variables:
• q_p = Heat transferred at constant pressure.
• \Delta H = Heat transferred at constant pressure.

Hess’s Law

• Statement: The enthalpy change for a reaction is the same whether it occurs in one step or multiple steps.
• Example:
  C3H8 + 7O2 \rightarrow 3CO2 + 4H_2O

Electrochemistry

Oxidation and Reduction

• Oxidation: Loss of electrons.
• Reduction: Gain of electrons.

Galvanic Cells

• Definition: A cell that converts chemical energy into electrical energy.
• Components:
• Anode: Oxidation occurs.
• Cathode: Reduction occurs.
• Salt Bridge: Connects the two half-cells.

Nernst Equation

• Equation: E = E^\circ – \frac{RT}{nF} \ln Q
• Variables:
• E = Energy (K)
• E^\circ = Cell potential (V)
• E^\circ = Standard cell potential (V)
• E = Standard cell potential (V)
• R = Ideal gas constant (0.0821 L·atm/mol·K)
• T = Temperature (K)
• n = Number of moles of electrons transferred
• F = Faraday constant (96,485 C/mol)
• Q = Reaction quotient
  

  S.No.	CSL No. in PS	NameShri/Ms./Smt.	Cadre	Gen/SC/ ST	Date of Birth	SLY	Chemistry

  Chemical Reactions

  Balancing Chemical Equations

  1. Write the unbalanced equation:
  • Example: C3H8 + O2 \rightarrow CO2 + H_2O
  1. Balance the equation:
  • Balance carbon atoms first.
  • Then balance hydrogen atoms.
  • Finally, balance oxygen atoms.
  • Balanced equation: C3H8 + 7O2 \rightarrow 3CO2 + 4H_2O
  1. Balance the equation:
  • Balance oxygen atoms first.
  • Then balance oxygen oxygen atoms.
  • Balanced equation: C3H8 + 7O2 \rightarrow 3CO2 + 4H_2O

  Types of Chemical Reactions

  1. Combination Reaction:
  • Example: 2H2 + O2 \rightarrow 2H_2O
  1. Decomposition Reaction:
  • Example: 2H2O2 \rightarrow 2H2O + O2
  1. Single Displacement Reaction:
  • Example: Zn + 2HCl \rightarrow ZnCl2 + H2
  1. Double Displacement Reaction:
  • Example: AgNO3 + NaCl \rightarrow AgCl + NaNO3
  1. Combustion Reaction:
  • Example: CH4 + 2O2 \rightarrow CO2 + 2H2O

  Stoichiometry

  Mole Concept

  • Mole (mol): The amount of substance containing as many particles (atoms, molecules, ions) as there are atoms in exactly 12 grams of carbon-12.
  • Avogadro’s Number: 6.022 \times 10^{23} particles per mole.

  Molar Mass

  • Molar Mass: The mass of one mole of a substance.
  • Example: The molar mass of water (H_2O) is 18.015 g/mol.

  Calculations

  1. Mass to Moles:
  • Formula: n = \frac{m}{M}
  • Example: Calculate the number of moles of H_2O in 18 grams of water.
  • n = \frac{18.015 \, g}{18.015 \, g/mol} = 2 \, mol
  1. Moles to Mass:
  • Formula: m = n \times M
  • Example: Calculate the mass of 2 moles of H_2O.
  • m = 2 \, mol \times 44.01 \, g/mol = 88.01 \, g

  Gas Laws

  Ideal Gas Law

  • Equation: PV = nRT
  • Variables:
  • P: Pressure (atm)
  • V: Volume (L)
  • n: Number of moles (mol)
  • R: Ideal gas constant (0.0821 L·atm/mol·K)
  • T: Temperature (K)

  Boyle’s Law

  • Equation: P1V1 = P2V2
  • Variables:
  • P₁: Pressure (atm)
  • P₂: Volume (L)
  • P₃: Pressure (atm)
  • P₁: Pressure (atm)
  • P₂: Volume (L)
  • P₃: Pressure (atm)
  • P₁: Pressure (atm)

  Boyle’s Law (Boyle’s Law)

  • Equation: \frac{P1V1}{P2V2} = \frac{P2V2}{T1} = \frac{P1}{T_2}

  Thermochemistry

  Enthalpy (H)

  • Definition: The heat content of a system at constant pressure.
  • Equation: \Delta H = q_p
  • Variables:
  • q_p: Heat transferred at constant pressure.
  • q_p^2: Heat transferred at constant pressure.

  Hess’s Law

  • Statement: The enthalpy change for a reaction is the same whether it occurs in one step or multiple steps.
  • Equation: \Delta H = qp + \Delta H0
  • Variables:
  • q_p: Heat transferred at constant pressure.
  • q_p^2: Heat transferred at constant pressure.

  Hess’s Law (Hess’s Law)

  • Statement: The enthalpy change for a reaction is the same whether it occurs in one step or multiple steps.
  • Equation: \Delta H = qp + \Delta H0
  • Variables:
  • H: Heat transferred at constant pressure.
  • q_p^2: Heat transferred at constant pressure.

  Electrochemistry

  Oxidation and Reduction

  • Oxidation: Loss of electrons.
  • Reduction: Gain of electrons.

  Galvanic Cells

  • Definition: A cell that converts chemical energy into electrical energy.
  • Components:
  • Anode: Oxidation occurs.
  • Cathode: Reduction occurs.
  • Salt Bridge: Connects the two half-cells.

  Nernst Equation

  • Equation: E = E^\circ – \frac{RT}{nF} \ln Q
  • Variables:
  • E: Energy (K)
  • E^\circ: Standard deviation of the energy (J)
  • R: Ideal gas constant (0.0821 L·atm/mol·K)
  • T: Temperature (K)
  • n: Number of moles of electrons transferred
  • F: Faraday constant (96,485 C/mol)
  • Q: Reaction quotient