Guess Paper – 2009 Class – X Subject – Chemistry (P- Block Elements) Kalra sir 09460472649 kalra1977@rediffmail.com Group 15 elements: |Symbol |Atomic |Electronic configuration | | |number | | | |7 |[He]2s22p3 | |N | | | |P |15 |[Ne] 3s23p3 | |As |33 |[Ar]3d104s24p3
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PAGE 2 8. Which of the following represents an sp3 hybridized atomic orbital containing the lone pair of electrons of ammonia‚ NH3? (a) 1 (b) 2 (c) 3 (d) 4 9. How many electrons are there in the valence shell of the carbon atom of a methyl cation‚ CH3+? (a) 4 (b) 5 (c) 6 (d) 7 10. Which atomic orbitals overlap to form the C-H â bonding molecular orbitals of ethane‚ CH3CH3? (a) C2p + H1s (b) Csp + H1s (c) Csp2 + H1s (d) Csp3 + H1s 11. Which
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15. Benzene and Aromaticity • C-Phen DM Drops (Chlorpheniramine/Dextromethorp/Phenylephrine) • This combination medication is used to treat symptoms caused by the common cold‚ flu‚ allergies‚ hay fever‚ or other breathing illnesses (e.g.‚ sinusitis‚bronchitis). • One of the active ingredients is Phenylephrine –a decongestant that helps relieve stuffy nose symptoms. H HO OH H N CH3 . HCl What is the configuration at this chirality center? R or S ? www.primaryrx.com/pdf/C-PHEN%20DM%20DROPS
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1. (a)Correct the following statements. (i) The melting points of crystalline and amorphous solids are not definite. The melting point of an amorphous solid is not definite. OR The melting point of a crystalline solid is definite. P Ps X solute . Ps P Ps The equation for relative lowering of vapour pressure when solute remains normal is X solute P (iii)The degree of ionization decreases with dilution. The degree of ionisation increases with dilution. (iv) Tertiary butyl halide
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when forming the complex ions. The properties of lewis acid is to have high electron deficiency. For transition metals in this experiment‚ the high charge density‚ positive charge and their vacant bonding orbitals leads to tendency to attract lone pair electron by filling up their vacant orbitals. Metal acetylacetonates‚ formed by a metal and multiple acetylacetonate anions‚ are prime examples of coordination complexes. In this experiment‚ the metal use is copper (II) ion which is crystal blue
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9.1 Orbitals and Theories of Chemical Bonding 1. Which one of the statements concerning valence bond (VB) and molecular orbital (MO) bond theories is correct? a) MO theory predicts that electrons are localized between pairs of atoms. b) In VB theory‚ bonding electrons are delocalized over the molecule. c) MO theory accurately describes bonding in O2 and NO‚ VB theory does not. d) VB theory can describe molecular bonding in excited states. e) MO theory is used to accurately predict
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COrdination compounds Question 9.1: Explain the bonding in coordination compounds in terms of Werner’s postulates. =Werner’s postulates explain the bonding in coordination compounds as follows: (i) A metal exhibits two types of valencies namely‚ primary and secondary valencies. Primary valencies are satisfied by negative ions while secondary valencies are satisfied by both negative and neutral ions. (In modern terminology‚ the primary valency corresponds to the oxidation number of the metal
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Consider the cyclic molecule C8H8‚ the eight carbon analogue to benzene. a) Write the secular detrerminant corresponding to the pi-bonding in C8H8. b) Using the secular determinant‚ the following energies are found for the pi-bonding molecular orbitals: 1 = + 2 2 = + 1.41 (two states) 3 = (two states) 4 = - 1.41 (two states) 5 = - 2 Give the electron configuration for the pi-bonding for the ground state of C8H8. c) What is value for S (total spin quantum number)
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Name Period Date Molecular Geometry – Ch. 9 For each of the following molecules‚ draw the Lewis Diagram and tally up the electron pairs. Then‚ identify the correct the molecular shape and bond angle. molecule lewis diagram e- tally shape bond angle 1. SeO3 2. AsH3 3. NO2 - 4. BeF2 molecule lewis diagram e- tally shape bond angle 5. SiH4 6. SeH2 7. PF5 8. SCl6 Name:
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properties: This is connected to the effect of the electric field of the ligands on the metal d orbitals and the electrons in them. This effect is a repulsion‚ so it does not explain the bonding. But‚ it does explain the d orbital energies in a complex. In what follows‚ we concentrate on the second component only. © Drs. XO‚ PHB‚ CWR Octahedral Ligand Field (10.3.1 too detailed) Any electron in a d orbital is repelled by the ligand lone pairs (like charges…) and therefore has its energy increased
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