Knowledge Booster

  INTERNATIONAL SPACE STATION(ISS) PC - NASA Five space agencies including NASA, JAXA, ROSCOSMOS, CSA, ESA have contributed to the space station assembly. The International Space Station is larger than a six-bedroom house with six sleeping quarters, two bathrooms, a gym, and a 360-degree view bay window. In 24 hours, the space station makes 16 orbits of Earth, traveling through 16 sunrises and sunsets. Peggy Whitson  set the U.S. record for spending the most total time living and working in space at 665 days on Sept. 2, 2017. To mitigate the loss of muscle and bone mass in the human body in microgravity, the astronauts work out at least two hours a day. The solar array wingspan (356 feet, 109 meters) is longer than the world’s largest passenger aircraft, the Airbus A380 (262 feet, 80 meters). pc-NASA The space station is 356 feet (109 meters) end-to-end, one yard shy of the full length of an American football field including the end zones. A spacecraft can arrive at the s...

  Titration - is a common laboratory method of quantitative chemical analysis to determine the concentration of an identified analyte. Purpose - Titration is the detection of the equivalence point,the point at which chemically equivalent amounts of the reactants have been mixed. The amount of reactants that have been mixed at the equivalence point depends on the stoichiometry of the reaction. Titration uses in Real Life -  Food Industry. Cosmetic Industry. Wine Industry. Pharmaceutical Industry Biodiesel Manufacturing. Waste water Management. Medical Diagnosis. Acid Rain Analysis.

  SALT ANALYSIS - What is Salt Analysis - Salt analysis is also known as systematic qualitative analysis or qualitative inorganic analysis involves the identification of the cation and anion of an inorganic salts. Most common salts NH4Br it contains Br- ion.                                   CaCl2 it contains Ca2+ ion.

https://drive.google.com/file/d/1GHv-rKtuTV1PQSFCWzSt2MH0XJ_N4m5z/view?usp=drivesdk p block

• General Characteristics of ionic Compounds : (i) Physical State: They generally exist as crystalline solids, known as crystal lattice. Ionic compounds do not exist as single molecules like other gaseous molecules e.g., H 2  , N 2  , 0 2  , Cl 2  etc. (ii) Melting and boiling points: Since ionic compounds contain high interionic force between them, they generally have high melting and boiling points. (iii) Solubility: They are soluble in polar solvents such as water but do not dissolve in organic solvents like benzene, CCl4etc. (iv) Electrical conductivity: In solid state they are poor conductors of electricity but in molten state or when dissolved in water, they conduct electricity. (v) Ionic reactions: Ionic compounds produce ions in the solution which gives very fast reaction with oppositely charged ions. For example, •  Covalent Bond—Lewis-Langmuir Concept : When the bond is formed between two or more atoms by mutual contribution and shar...

Modes of Chemical Combination — By the transfer of electrons: The chemical bond which formed by the complete transfer of one or more electrons from one atom to another is termed as electrovalent bond or ionic bond. — By sharing of electrons: The bond which is formed by the equal sharing of electrons between one or two atoms is called covalent bond. In these bonds electrons are contributed by both. Co-ordinate bond: When the electrons are contributed by one atom and shared by both, the bond is formed and it is known as dative bond or co-ordinate bond. Ionic or Electrovalent Bond Ionic or Electrovalent bond is formed by the complete transfer of electrons from one atom to another. Generally, it is formed between metals and non-metals. We can say that it is the electrostatic force of attraction which holds the oppositely charged ions together. The compounds which is formed by ionic or electrovalent bond is known as electrovalent compounds. For Example, , (i) NaCl is an electrovalent compou...

Chemical Bond The force that holds different atoms in a molecule is called chemical bond. Octet Rule Atoms of different elements take part in chemical combination in order to complete their octet or to attain the noble gas configuration. Valence Electrons It is the outermost shell electron which takes part in chemical combination. Facts Stated by Kossel in Relation to Chemical Bonding •  In the periodic table, the highly electronegative halogens and the highly electro-positive alkali metals are separated by noble gases. • Formation of an anion and cation by the halogens and alkali metals are formed by gain of electron and loss of electron respectively. •  Both the negative and positive ions acquire the noble gas configuration.  The negative and positive ions are stabilized by electrostatic attraction Example,

        QUESTIONS   Question 1. Give the uses of freon 12, DDT, carbon tetrachloride and iodoform. Question 2. p-Dichlorobenzene has higher m.p. and lower solubility than those of o- and m-isomers. Discuss.

QUESTIONS Question 1:  Write the isomers of the compound having formula C4H9Br. Question 2:  Write the equations for the preparation of 1−iodobutane from (i) 1-butanol (ii) 1-chlorobutane (iii) but-1-ene Question 2:  How will you bring about the followin g conversions? (i) Ethanol to but-1-yne (ii) Ethane to bromoethene (iii) Propene to 1-nitropropane (iv) Toluene to benzyl alcohol (v) Propene to propyne (vi) Ethanol to ethyl fluoride (vii) Bromomethane to propanone (viii) But-1-ene to but-2-ene  (ix) 1-Chlorobutane to n-octane  (x) Benzene to biphenyl. Question 3:  Explain why?  (i) the dipole moment of chlorobenzene is lower than that of cyclohexyl chloride? (ii) alkyl halides, though polar, are immiscible with water? (iii) Grignard reagents should be prepared under anhydrous conditions?

PRACTICE QUESTIONS Question  1. Write the structures of the following organic halogen compounds. (i) 2 -Chloro-3 -methylpentane (ii) p -Bromochlorobenzene (iii) 1 -Chloro-4-ethylcyclohexane (iv) 2 – (2 -Chlorophenyl) -1 -iodooctane (v) Perfluorobenzene (vi) 4 – tert – Butyl -3 -iodoheptane (vii) 1 – Bromo – 4 – sec – butyl – 2 – methylbenzene (viii) 1 ,4 – Dibromobut – 2 – ene Question  2. Which one of the following has the highest dipole moment? (i) CH2Cl2 (ii) CHCl3 (iii) CCl4 Question 3. A hydrocarbon C5H10 does not react with chlorine in dark but gives a single monochloro compound C5H9Cl in bright sunlight. Identify the hydrocarbon.

            PRACTICE QUESTIONS Question 10.1: Name the following halides according to IUPAC system and classify them as alkyl, allyl, benzyl ( primary, secondary, tertiary ), vinyl or aryl halides : (i) (CH 3 ) 2 CHCH(Cl)CH 3 (ii) CH 3 CH 2 CH(CH 3 )CH(C 2 H 5 )Cl (iii) CH 3 CH 2 C(CH 3 ) 2 CH 2 I (iv) (CH 3 ) 3 CCH 2 CH(Br)C 6 H 5 (v) CH 3 CH(CH 3 )CH(Br)CH 3 (vi) CH 3 C(C 2 H 5 ) 2 CH 2 Br (vii) CH 3 C(Cl)(C 2 H 5 )CH 2 CH 3 (viii) CH 3 CH=C(Cl)CH 2 CH(CH 3 ) 2 (ix) CH 3 CH=CHC(Br)(CH 3 ) 2 (x) p-ClC 6 H 4 CH 2 CH(CH 3 ) 2 (xi) m-ClCH 2 C 6 H 4 CH 2 C(CH 3 ) 3 (xii) o-Br-C 6 H 4 CH(CH 3 )CH 2 CH Question 10.2:Give the IUPAC names of the following compounds: (i) CH3 CH(Cl) CH(Br) CH3 (ii) CH F2 CBr ClF (iii) Cl CH2 C ≡ C CH2 Br (iv) ( CCl 3) 3 CCl (v) CH3 C (p – Cl C6 H4 )2 CH(Br) CH3 (vi) (CH3 )3 C CH = C Cl C6 H4 I 

NATURE OF C-X BOND :  •  Halogens is more electronegative than carbons.  •  Carbon atom has partial positive charge •  The nature of C-X bond depends on both the nature of carbon in the aromatic ring and the halogen attached.  •  Florine has the highest electronegative element of halogens.  •  The halogens elements(17th group) are just one electron short of completing their nearest novel gas configurations.  •  Electronegativity increased across a period from left to right.      (F>Cl>Br>I)  •  The C-X bond in haloarenes is polarised as 'X' are more electronegative than carbon.  •  The only one sigma bond is formed between one carbon and one halogen.  •  The atomic size has increased Florine to down the period.  •  The C-X bond length in haloarenes increases from Florine(F) to Astetine(As) and bond dissociated strength decreases....

Question . Discuss the structure of Side chain halogen Compounds.  Question . How do you to identify aromatic compounds. Discuss. 

Question 1.  How to explain 1°, 2°, and 3° Alkile Halides. Give the examples.  Question 2.  Give the molecular structure of given below compounds: •  CH 3-CH=C=C=O •  CH2-Cl-CH2-CH=CH-OH

IUPAC NOMENCLATURE -  •   CH2=CH-CH3 •  CH3-CH2-CH2-CH=CH2-Br •    CH3-CH2-CH2-CH=CH-CH2-Cl •   CH2=CH-OH •   CH3-CH2-OH

IUPAC NOMENCLATURE -  •   CH3-CH2-CH-Br2 •   CH3-CH2-CH2-CH2Cl •   CH3-CH2-CH2-CH2-CH3 •   CH-F2-CH2-CH3 •   CH3-CH2-CH2-CH2-CH2-Br2

Question 1. How to explain halogens in details.  Question 2. Give the physical & chemical properties of halogens.  Question 3. What is the characteristics of halogens. Give their uses.  Question 4. Give some Reactions with halogenic compounds to other metallic compounds.  Question 5. Why we called halogen of 17th group in the periodic table.                             **************

Exercising Questions :  Question 1.  Give the structural formula of following compounds : a) CCl4 b) CH2Cl2 c)   CH3CH2OH d) CHCl3 e) CH3Br f) CH3CH3CH2-I g) C6H4Br2 h) C6H50H Question 2.  Give the IUPAC name of following compounds: a) CH2-Cl-CH2-CH-Cl-OH b) CH3-CH2-CH-Br-CH3 c) C6H6

Exercise Questions for Haloalkanes Question  1. Give the structural formula of the following compounds.  a) Butane.  b) Butene.  c) Propylene.  d) Hexenon. e) 3-Pentanol. f) 2,4,5-Trimethyl Hexane.  Question 2.  Give the IUPAC name of the following compounds.  a) CH3-CH2-CH2-CH2-OH b) CH2-OH-CH2-CH2-CH2-OH c) CH2-O-CH-OH-CH2-CH3 d) C6H5OH e) C6H5CH3.  Question 3. What do you understand by aliphatic compounds. Give examples.                    

Topics that which we learn in further discussion as following : •  Heloalkanes.  •  Haloarenes.  •  Alifatic Halogen Compounds.  •  Aromatic Halogen Compounds.  •  IUPAC Nomenclature.  •  Nomenclature of Haloalkanes.  •  Isomerism in Haloalkanes.  •  Methods of Preparation of Haloalkanes.  •  Physical Properties of Haloalkanes •  Chemical Properties of Haloalkanes.  •  Nucleophilic Substitution Reactions.  •  Elimination Reactions.  •  Satyzeff's Rule.  •  Stereochemical aspects of Nucleophilic Substitution Reactions of Haloalkanes.  •  Chirality.  • Elementry of Symmetry.  •  Uses of Haloalkanes.                                   Thank you   !