ATOMIC STRUCTURE
PART I
1. Which one of the following experiment proves the particle nature of electron?
a. J.J.Thomson experiment
b. Photoelectric effect
c. scintillation
d. all of these
2. The kinetic energy of an electron that has been accelerated from rest through a potential
difference 1kV is ( in Joules)
a. 1.609 x 10-12
b. 1.609 x 10-16
c. 1.609 x 10-17
d. 1.609 x 10-18
3. Two particles A and B are in motion. If the wavelength associated with
B is 10-7m , calculate the wavelength of the particle A, if its momentum is twice that of B?
a. 5 x 10-8m
b. 2 x 10-7m
c. 2 x 10-6 m d. 5 x 10-16 m
4. The λ of an electron moving in a a stable orbit is related to its circumference of the orbit with
radius ‘a’ is
a. 2πa = nλ
b. 2πa = h/mv c. 2πa = λ/mvd. 2πa = hλ
5. The condition for a molecule to be stable is
a. Nb= Na
b. Nb˃Na
c. Nb ˂Na
d. both’ a’and ‘b’
6. The type of hybridization of I in ICl4- is
a. sp3
b. dsp3
c. d2sp3
d. dsp2
7. The energy of an electron present in first Bohr’s orbit of a Hydrogen atom is ( kJ mol-1)
a.1312
c. 6.626x 10-34
b. -1312
8. The shape of dz2 orbital is
a. dumb-bell shape
b.clover leaf shpe
c. dumb-bell shape with doughnut shape
d. -146
d. cloverleaf shape with doughnut shape
9. In which one of the following sp2 hybridization is not seen
a. NO2-
b. NO3-
c. CO3-,-
d. ClO2-
10. Which one of the following bond is the strongest
a. Ionic bond b. Covalent bond
c. Hydrogen bond
d. Vander waal’s bond
11. The energy of the electron in the Bohr’s second orbit of H atom is –E, what is the energy of
the electron in the Bohr’s third orbit is
a. -4/9 E
b. -9/4E
c.-4E
d.-9E
12.The strength of hydrogen bond is inversely proportional to the _______ of the combining
atom
a. Ionization energy b. Electronegativity
c. electron affinity
d. atomic radius
13. The intra molecular hydrogen bonding in molecules leads to
a. high boiling point
b. less boiling point
c. high solubility in water
d. both ‘b’ and ‘c’
14. The wavelength associated with a particle of mass 3.313 x 10-31 kg moving with a velocity
of 103m/s is
a. 2 x 106m
b. 2 x 10-6m
c. 2 x 106 cm d. 2 x 10-6 cm
PART II
15. What is the significance of negative electron energy?
16. Write short note on ‘p’ orbital
17. Explain bond length in terms of bond order
18. Diatomic Helium molecule is hypothetical one. Why?
19. Write a note on orbital
20. State uncertainty principle
21. Explain the hydrogen bond present in water?
22. Define hybridization
23. Calculate the energy needed to promote an electron from first energy level to third energy
level.
24. Calculate the product of uncertainty in position and velocity for an electron of mass 9.1 x 1031
kg according to Heisenberg uncertainty principle
PART III
25. Derive de-Broglie’s wavelength?
26. Write the salient futures of hybridization
27. Explain Davission – Germer method
28. Explain the formation of oxygen molecule by molecular orbital theory
29.Explain the shapes of ‘s’ and d orbital
PART IV
30. a. Give brief outline of molecular orbital theory
b. Calculate the wavelength of radiation emitted when the electron in hydrogen atom makes
transition from n=2 state to n=1state.
31. a. What is meant Hydrogen bond? Explain the strength of Hydrogen bond.
b. Explain the formation of Nitrogen molecule by molecular orbital theory
32. a. write the importance of Hydrogen bonding
b. Calculate the mass of photon in Kg of sodium light with a wave length of 5890 Ao ? (h =
6.626 x 10-34 Js?
PERIODIC PROPERTIES
PART I
1. Which one of the following metal has the highest electron affinity value ?
a. Chlorine
b. Flourine
c. Iodine
d. Gold
2. Which one of the following element has the highest ionization energy?
a. Lithium
b. Carbon
c. Nitrogen
d. Flourine
3. The value of screening constant of the last electron of chlorine atom is
a. 6.1
b. 10.9
c. 2.2
d. 16.8
4. The covalent radii of bromine atom is (in Ao)
a. 2.28
b. 1.44
c. 1.24
d.1.54
5. The electron affinity value of an atom
a. directly proportional to the size
b. independent of size
c. inversely proportional to the size d. inversely proportional to nuclear charge
6. Which one has the highest ionization potential
a. Na
b. Cl
c. Si
d. Ar
7. The ionization potential and electron affinity value of fluorine atom is 17.4eV/atom and
3.62eV/atom respectively , then electronegativity value of fluorine atom is
a. 9.51
b. 3.75
c. 3.03 d. none of these
8. Which one of the following has the minimum ionization energy
a. noble gases
b. halogens
c. alkali metals
d. alkaline earth metals
9. Which one of the following has the negative electron affinity value
a. Zn
b. Cl
c. F
d. N
10. The order of ionization energy is
a. s˃p˃d˃f
b. s˂p˂d˂f
c. s˂p˂d˃f
d. both a and b
11. The element which has the highest electronegativity value
a. Chlorine
b. Flourine
c. Iodine
d. Bromine
12. If XA = XB then the molecule is
a. polar covalent
b. non polar covalent c. ionic
d. neutral
13. Which one of the following is the largest in size
a. Na
b. Na+
c. Cl
d. Cl-
14. Which one of the following is highly electro positive
a. Lithium
b. Sodium
c. Potassium d. Cesium
PART III
15. B and Al which one has the highest IE value? Why?
16. Fe, Fe2+, Fe3+ arrnge in increasing order of the size? Explain
17. Mention the disadvantage of Pauling and Mulliken scale
18. Write a note on successive electron affinity values
19. Electron affinity values of N and Ne are zero. Why?
20. Mg, Al which one has the lowest IE value? Why
21. Define second ionization potential
22. The experimental value of Si –C is 1.96Ao. Calculate the atomic radii of Silicon. (covalent
bond length of carbon is 1.54Ao
23 What are periodic properties? give example
24. Define atomic radii? How does it vary in the periodic table?
PART III
25. How is atomic radii calculated from covalent bond length?
26. How is electronegativity value is used to find out percentage of ionic character in polar
covalent bond?
27. Calculate the electronegativity value of chlorine atom from the following data EH-H =
104 K cal mol-1 ; Ecl – cl = 36 K cal mol-1; EH-Cl = 134 K cal mol-1
28. Explain Pauling’s method to determine ionic radii
29. Explain Mullikan’s method to determine electronegativity value
PART IV
30.a. Explain Ionization energy
b. How is electronegativity value is used to find out the nature of the bond
31. a. Explain electronaffinity ?
b. How is electronegtivity value determined by pauling’s method?
P – block Elements
PART I
1. The element which exist as liquid at room temperature is
a. Thallium b. Indium c. Gallium d. Boron
2. Which is used in thermistors
a. Thallium b. Indium c. Gallium d. Aluminium
3. Litharge is
a. PbO
b. PbO2
c. Pb3O4
d. Cu O
4. Souring agent in the soft drinks is
a. H3PO3 b. H3PO4 c. H4P 2O7 d. HPO3
5. Which is used in Holme’s signal
a. CaC2 and Ca3P2
b. CaC2 and Ca2P3
c. Ca3(PO4)2 and Ca3P2
d. CaC2 and Ca3(PO4)2
6. Which is mixed with paints to make them damp-resistant
a. Silicone rubber b. Silicone resisns
c. Silicone oils
d. Straight chain silicones
7. Which one of the following ion is not existing
a. I3-
b. Br3-
c. Cl3-
d. F3-
8. The acidic character of HX is
a. HI˂HBr ˂ HCl ˂ HF
b. HI˃HBr ˃ HCl ˃ HF
c. HI˂HBr ˂ HCl ˃ HF
d. HI˃HBr ˂ HCl ˂ HF
9. Whcich is used as a preservative to prevent fermentation and also for preventing dental
cavities
a. NaF b. CaF2 c. SF6
d. UF6
10. Which one of the following mixture is used in the treatment of asthma
a. Oxygen & Helium
b. Oxygen & Neon
c. Oxygen & Krypton d. Oxygen & Xenon
11. Which one of the following light is used in botanical gardens
a. Helium
b. Neon
c. Krypton d. Xenon
12. The shape of ClF3 molecules without lone pair of electrons is
a. linear b. tetrahedral c. V-shaped d. T-shaped
13. During the laboratory preparing of phosphoric acid the catalyst used is
a. Platinum b. Iodine c. Nickel
d. Iron
14. When heated to 523K phosphoric acid gives
a. H3PO3 b. H3PO4 c. H4P 2O7 d. HPO3
PART II
15. How is potash alum prepred? Write its uses.
16. Write the uses of lead?
17. How does PCl3 reacts with O2 and SO3 respectively? Draw its electronic structure?
18. How does silver nitrate react with phosphene and phosphorous acid respectively?
19. Write a note on etching of glass? write the principle also.
20. What happens when BrF5 and ICl are hydrolyesed?
21. Discuss the oxidizing property of Fluorine?
22. Write the general characteristics of p – block elements?
23. What happens when phosphorous acid and phosphene are heated?
24. Write the uses of Neon?
PART III
25. Write the anomalous nature of Flourine?
26. How is Fluorine prepared from fluorides?
27. Give an account of various types of compounds which are formed by xenon?
28. How are the following compounds react with water?
i. P2 O3
ii. P2O5
iii. PCl5
29. How is phosphene prepared in Laboratory? How does it react with chlorine?
PART IV
30 a. How is noble gases are isolated from air.?
b. Explain interhalogen compounds of type AX3, AX5 and AX7
31a. How is Lead extracted from its ore?
b. What are silicones? How are they prepared?
d – block elements
PART- I
1. Which one of the following pairs have almost equal atomic radii?
a. Mo, W
b. Y, La
c. Zr, Hf
d. Nb, Ta
2. Which one of the following is colourless?
a. Ti4+
b. Ti3+
c.V3+
d. Fe2+
3. Which one of the following ion has high magnetic moment value?
a. Ti4+
b. Mn2+
c.Cr3+
d. Fe2+
4. The composition of alloy bronze is
a. Cu=60-80%, Sn= 20-40%
b. Cu=60-80%, Zn= 20-40%
c. Cu=75-90%, Sn= 10-25%
d. Cu=75-90%, Zn= 10-25%
5. Which is used in making ointment for curing skin diseases?
a. ZnCO3
b. AgNO3
c. CuSO4
d. K2Cr2O7
c. Ru, Os
d. Mn, Os
6. Metals exhibiting +8 oxidation state is
a. Ru, Mo
b. Rh, At
7. When copper reacts with carbondioxide in presence of moisture and air is
a. Cu(OH)2, CuO
b. Cu(OH)2, CuCO3
c. CuO, CuCO3
d. Cu2O, CuCO3
8. Colour of cuprous iodide is
a. white
b. bluec. yellow
d. Red
9. Purple of cassius is a colloid of
a. Silver, colloidal stannic acid
c. tin, colloidal silver
b. Gold, Colloidl stannic hydroxide
d. colloidal tin, copper
10. When heated to 720oC copper sulphate pentahydrate gives
a. CuSO4.H2O b. CuSO4
c. CuO, SO3 d. CuO, SO2
11. When chloride salt is treated with potassium dichromate and Con.H2SO4 it gives reddish
brown vapours of
a. CrCl3
b. CrOCl2
c. CrO2Cl2
d. Crcl2
12. Spitting of silver can be prevented by using
a. Charcol
b. Borax
c. Aluminium d. copper
13. percentage of gold in 22 carrot gold is
a. 75%
b. 25%
c. 91.6%
d. 100%
14. The alloy which is used in resistance wires for electrical heating is
a. Ferrochrome
b. Nichrome c. Stellite
PART II
d. Chrome steel
15. Write a note on chrome plating?
16. Why transition elements is used as catalyst?
17. Write a note on magnetic properties of d- block elements
18. How does copper react with nitric acid?
19. Which is known as philosopher’s wool? How is it prepared?
20. How is silver obtained from silver coins?
21. How does gold react with Gold?
22. Write the uses of Lunar caustic
23. How is zinc carbonate prepared? What happens when it is heated?
24. How is purple of cassius prepared?
PARTIII
25. How is silver extracted from its ore?
26. Explain alumino thermic process?
27. How does copper sulphate react with the following?
i. NH4OH
ii. KI
iii. KCN
28. Explain any three oxidizing property of potassiumdichromate?
29. How does zinc react with nitric acid and alkalies?
PART IV
30a. How is copper extracted from its ore?
b. How is silver nitrate prepred? What happens when it is heated? How does it react with
NaCl.
31 a. How is Gold extracted from its ore?
b. Write a note on alloys of chromium
32. How is zinc extracted from its ore?
b. Why do d block elements form coloured ions and variable oxidation states
f- BLOCK ELEMENTS & NUCLEAR CHEMISTRY
PART I
1. The number of α and β particles emitted when
a. 4, 3 b. 2,4
218
84X
is changing to a stable 82Y206
c. 3, 4 d. 4,6
2. The average of life of U238 having half life period is 140 days is
a. 20.02 days b. 70 days
c. 202.02 days d. 30 days
3. The isotope which is used in location of blood clots and circularity disorders is
a. Iron 59
4.
235
92U
b. Sodium 24 c. iodine 131 d. mercury 197
nucleus absorbs a neutron and disintegrates into 54Xe139,
a. α particle
b. βparticle
94
38Sr
and X. Then X is
c. 3 neutrons d. 2 neutrons
5. 1gram of radioactive isotope is reduced to 0.125grams in 24 hours, then its half life period is
a. 12hours
b. 10 hours
c. 8 hours
d. 6 hours
6. Uranium series belongs to
a. 4n
b. 4n+1
c. 4n+2
d. 4n+3
7. Which one of the following do not form complexes easily?
a. lanthanides b. transition elements c. actinides
d. none of these
8. The maximum oxidation state of actinide is
a. 6
b. 4
c.3
d.2
9. Which is used in the preparation of toys, tracer bullets?
a. ceria
b. thoria c. mish metals
d. pyrophoric alloys
10. Pure lanthanide metals are obtained by heating the trifluride s of lanthanides with
a. calcium
b. lithium
c. sodium
d. both ‘a’ &’b’
11. One of the consequence of lanthanide contraction is
a. regular increase in their ionic radii
b. irregular increase in their ionic radii
c. regular decrease in their ionic radii d. irregular decrease in their ionic radii
12. Which is used as a power source in long mission space probes?
a. U-235
b. U-232
c. Pu-238
d. Pu-241
13. Which one will form oxocations?
a. lanthanides b. actinides
c. noble gases d. alkalimetals
14. Which is used in gas lamp materials?
a. ceria
b. thoria
c. magnesia
d. both ‘a’ and ‘b’
PART II
15. What is Q value of a nuclear reaction?
16. Explain the principle involved in Hydrogen bomb?
17. What is meant by spallation reaction?
18. What is meant by binding energy?
19. Complete the following reactions
i.
ii.
23
11Na
23
11Na
(n , β) …………
+ ………→ 12Mg23 + 0n1
20. Write the mechanism of photosynthesis in plants
21. Write theuses of radioactive isotopes?
22. What are mish metals? Write the uses?
23. Write the various oxidation states of lanthanides and actinides
24. Write a note on radioactive decay series?
PART III
25. How are lanthanides extracted from its ore?
26. Write the consequences of lanthanide contraction?
27. Explain carbon dating method?
28. Explain the principle involved in nuclear fission reaction?
29. Differentiate nuclear reaction and chemical reaction?
PART IV
30. a. Write the differences between lanthanides and actinides?
b. Write the uses of lanthanides and actinides?
31. a. Explain nuclear reactions taking place in sun?
b.Write a note on lanthanide and actinide contraction?
COORDINATION COMPOUNDS
PART – I
1. The magnetic moment value of [Fe(F)6] molecule is
a. zero
b. 4.90BM
c. 2.83BM
d.1.732BM
2. The isomerism exhibited by [Co(NH3)4SO4]Br and [Co(NH3)4Br] SO4is
a. coordination isomerism
b. ionization isomerism
c. linkage isomerism
d. ligand isomerism
3. [Fe(CN)6] is diamagnetic because
a. CN- is a weaker ligand
b. CN- is a strong ligand
c. CN- is a flexidentate ligand
d. CN- is a chelating ligand
4. The colour of [Cr(H2O)6]Cl3 is
a. bright green
b. grey green c. Red d.Violet
5. The IUPAC name of [Cr(en)3]Cl3 is
a. triethylenediammine chromium III chloride
b. trisethylenediamine chromium VI chloride
c. trisethylenediamine chromium III chloride
d. trisethylenediamine chromium IV chloride
6. An example for neutral ligand is
a. en
b.CO
c. NO
d. all of these
7. The coordination number of Co in [Co(NH3)4SO4]Br is
a. 4
b. 2
c. 6
d.3
8. An example for ambidentate ligand is
b. CN- c. Cl-
a.en
d. NO2-
9. The oxidation number of Ni in [Ni(CN)4]2- is
a.2
b.4
c.6
d. 3
10. Coordination number of a molecule is 4 then its structure is
a. linear
b. trigonal
c. square planar
d. octahedral
11. The primary and secondary valency of the central metal ion in [Fe(NH3)6]Br3 is
a. 4,6
b.3,6
c.2,4
d2,6
12. Which one of the following is an example for anionic complex
a. [Fe(NH3)6]Br3
b. [Cu(NH3)4]SO4
c. K4 [Fe(CN)6]
d. [Pt(H2O)4]Br2
13. The isomerism seen in the complexes [Pt(NH3)4][CuCl4] is
a. ionization isomerism
b. Linkage isomerism
c. coordination isomerism
d. optical isomerism
14. The shape and magnetic moment value of [Ni(NH3)4]2+ is
a. square planar, 2.83
b. tetrahedral. 2.83
c. square planar, zero
d. tetrahedral, zero
PART II
15. Write the differences between simple salt and coordination complex?
16. What is meant by chelating ligand? give example
17. Write a note on solvate isomerism
18. Write a note on optical isomerism present in coordination compounds?
19. Write the structural formula of
i. tris(ethylenediamine) cobalt (III)ion
ii. pentaamminesulphatocoblt(III) chloride
20. How is coordination compounds used in complexometric titrations?
21. What is meant by central metal ion?
22. Write the central metal ion, coordination number, shape, IUPAC name of
[Cu(NH3)4]SO4.
23. Explain the structure of Hemoglobin and myoglobin?
PART III
24. Write the postulates of valence bond theory about coordination complex?
25. [Ni(CN)4]2- is diamagnetic wheres [Ni(NH3)4] 2+ is paramagnetic. Why? Explain
26. Explain the importance of chlorophyll in environmental chemistry? Mention its function
27. What are ligands ? How are they classified? Explain with examples
PARTIV
28.a. Explain Werner’s coordination theory?
b. Explain cis, trans isomerism present in coordination compounds?
29. a. Explain the structures of [Fe(F)6]4-, and [Fe(CN)6]4- based on valence bond theory?
b. Explain i. coordination isomerism ii. ionization isomerism and linkage isomerism