Chem 113

Universal Science College B.Sc. Biochemistry Second Term Examination - 2007 Semester: First Subject: Chem 113

F.M.: 100 Time: 3 hrs Date: 10th Feb 2007

Name: …………………………. 1.

Nature of alkali metals is a. + ve

2.

b.

c.

Neutral

Alkali metals are a. Most reactive c. Less reactive

b. d.

More reactive Non reactive

3.

Alkali metals are extracted by a. Carbon reduction process c. Electrolytic process

b. d.

Alumino thermite process None

4.

Chilli salt petre is a. Na2 CO3

c.

Na NO3

5.

Cohesive energy is equal in magnitude of a. Heat of atomization c. Heat of neutralization

b. d.

Heat of ionization Heat of dissociation

6.

Cohesive energy affects the a. Size of atom c. Electronegativity

b. d.

I.E. M.P. & B.P.

7.

Ionic bond is formed when electronegative difference between atoms is a. More than 1.7 ev b. Less than 1.7 ev c. Equal to 1.7 ev d. None of these

8.

Li – shows a. Ionic character c. Neutral character

9.

b.

-ve

Roll No. ………….

Na2 SO4

d.

None

d.

NaCl

The stability of Sodium chloride is ……………than sodium iodide a. Less b. More c. Equal

d.

None

10.

The solubility of Potassium iodide is …………….. than potassium chloride a. More b. Less c. Same

d.

None

11.

Density of sodium is less than water because it is a. High + ve in nature c. Neutral in nature

b. d.

High –ve in nature Large in size

12.

I.P. of Li in its own group is a. Highest

c.

Both a and b

d.

None

13.

Super conductivity is due to a. Paired electron c. Both-paired or unpaired elecron

b. d.

Unpaired electron None

b. d.

b.

Lowest

Covalent character None

14.

Critical temperature is that temperature where metal becomes a. Super conductor b. Good conductor c. Poor conductor d. None

15.

Substitutional alloys are formed when metallic radii difference is nearly a. 14 – 15% b. 20 – 22 % c. 10 – 12 %

16.

In interstitial alloy invading atom is present in a. Inter molecular space b. c. Atomic space d.

Molecular space Interstitial space

17.

Superoxide of alkali metal is formed by a. Li b. Na

c.

18.

Colorful compounds of alkali metals are due to the presence of a. Anions containing oxygen b. Anions containing sulphur c. Anions containing transition elements d. Anions containing nitrogen

19.

Lithium resembles to a. Ca

20.

b.

8 – 10 %

d.

None

c.

Al

d.

Si

Most stable compound among these is a. K–R b. Na – R

c.

Li – R

d.

Rb – R

21.

Crown has the structure a. Spherical

Dunb – bell

c.

Puckered

d.

None

22.

Na+ & Li + ion prefer to form a. Crown – 5 b.

Crown – 6

c.

Crown – 7

d.

Crown – 8

23.

Cryptates are a. Monocyclic

Dicyclic

c.

Tricyclic

d.

Polycyclic

24.

Coordination number of cryptates is a. 8 b. 6

c.

4

d.

10

25.

Metals are required to balance the electrical charge in the living cell with a. Negative charge macro organic molecule b. Positive charge organic molecule c. Neutral charge organic molecule d. None of these

26.

In biological functions the metal which expel out of cells is a. Li + b. Na+ c. K+

27.

Different ratio of Na+ to K+ inside & outside of cells are essential for the functioning of a. Nerve and blood b. Blood and muscle c. Bone & nerve d. Nerve & muscle

28.

Be and Mg has a structure a. B.C.C.

29.

Cohesive energy of 2nd group elements is greater than that of a. III rd group elements b. 1st group element c. 4th group elements d. None

30.

Conduction in metals is due to the presence of a. Empty conduction band c. Partially filled conduction band

b.

b.

b.

Mg

K

d.

H.C.P.

c.

b. d.

C.C.P.

d.

d.

Filled conduction band None

Rb+

none

31.

CO molecule has bonds a. 1 - σ bond & 2 - π bonds c. 1 - σ bond and 1 - π bond

32.

For σ bonding molecular orbital, along the internuclear line electron density is a. Maximum b. Minimum c. Zero

d.

None

33.

For π bonding molecular orbital, along the internuclear line electron density is a. Maximum b. Minimum c. Zero

d.

None

34.

Py– Py orbital giving the molecular orbital a. π bonding M.O. c. σ and π bonding M.O.

35.

When there is no overall change in energy, situation is termed as a. σ bonding b. π bonding c. Non bonding

d.

None

36.

Pentagonal bipyramidal have hybridization a. SP3 d b. SP3d2

d.

SP3

37

For combination of atoms during formation of molecule, they must have a. More energy b. Highest energy c. Lower energy d. Same energy

38.

Oxygen is a. Paramagnetic

b.

Diamagnetic c.

Ferromagnetic

d.

None

39.

Bond order in O-2 ion is a. 1

b.

2

c.

3

d.

None

40.

The force between atoms in metallic lattice is a. Van der waal force c. Cohesive force

b. d.

Electrostatic force None

41.

Structure of alkali metals is a. C.C.P.

c.

H.C.P.

d.

None

42.

Band theory explains a. Properties of metals c. Properties of metalloids

b. d.

Properties of non metals None

43.

Conductivity of metals ………….. with increase in temperature a. Decreases b. Increases c. Remains same

d.

None

44.

Conductivity of semiconductors ………….. with increase in temperature a. Decreases b. Increases c. Remains same

d.

None

45.

The bonding energy of metals depends on the average number of unpaired a. Electrons b. Protons c. Neutrons

d.

Mesons

46.

Crystal structure adopted by metal depends on the number of a. S & P orbitals b. SP & d orbitals c. S, P, & f orbitals d. P & d orbitals

47.

Cohesive force increases from a. Left to right in period c. Moving down a group

48.

Lustre of metal is due to a. Bonding electrons

d.

None

b.

b.

b. d.

B.C.C

b. d.

c.

b. d. Free electrons c.

2 - σ bonds and 1 - π bonds 2 - π bonds – 2 - σ bonds

σ bonding M.O. None

SP3d3

Right to left in period Ascending up a group No electrons

49.

Which molecule does not exist? b. a. He2

50.

C.N. of pentagonal bipyramidal molecule is a. 4 b. 5

51.

d-block elements form colored ions, because they absorb some energy for a. d – s transition b. p – d transition c. d – d transition d. None of them

52.

Paramagnetic property is the property of a. Paired electrons c. Completely vacant electric sub-shell

b. d.

Unpaired electrons Completely filled electronic sub-shell

53.

Electronic configuration of platinum is a. ……… 4d10 5 s0 c. ……… 5d10 6 s0

b. d.

……… 5d9 b s1 ……… 5d8 6 s2

54.

In 3d - transition series, with the increase in nuclear charge, the screening effect a. First increases & then decreases b. Decrease c. Dirst decreases & then increases d. Increases

55.

The maximum oxidation state of Mn is a. +6 b. +5

56.

Covalent character of a given metal increases with a. Decrease in the oxidation state b c. Decrease in the ionization energy d.

57.

Energy associated with a wave length

li2

c.

H2

d.

N2

c.

6

d.

7

c.

+7

d.

+8

Increase in the oxidation state None of them

is given by

a.

10 5 KJ mol −1 0 83.7 × λ ( A )

b.

10 6 KJ mol −1 0 83.7 × λ ( A )

c.

10 8 KJ mol −1 83.7 × λ ( A)

d.

None

58.

Which one of the following ligands is π bonding ligand ? a. Clb. NH3 c.

H2O

d.

CO

59.

Which one of the oxides of V is acidic in nature? a. VO b. V2O3

VO2

d.

V2O5

60.

Zegler – Natta catalyst is used for the manufacture of a. Nylon 6 b. c. Polythene d.

TNT None of these

61.

B.M (Bohr magneton) is the unit of a. Density c. Magnetic moment

b. d.

Volume Wave length

62.

Paramagnetism is the property of a. Paired electron c. Completely filled electronic sub-shell

b. d.

Unpaired electrons Completely vacant electronic sub-shell

63.

1st I.E. of Hg is higher than that of Cd, due to the presence of 4f orbitals which brings a. Repulsion b. Attraction c. Poor – shielding effect d. Perfect shielding effect

c.

64.

Which of the following has Frankel defect? a. NaCl b. Cs Cl

65.

The electromagnetic value of A & B is 0.7 & 3 respectively. Predict the nature of bond a. Co-valent bond b. Ionic bond c. Co-ordinate covalent bond d. Metallic bond

66.

With the increase in the value of lattice energy, stability of an ionic solid a. Decreases b. Remains same c. Increases d. None

67.

Born exponent "n" can be measured by the a. Expansion measurement c. Cryoscopic measurement

68.

Lattice energy becomes stronger when inter – ionic distance a. Increases b. Decreases c. Remains constant d. None of them

69.

If the limiting radius value is 0.732 – 0.999 for a compound them the coordination number is a. 3 b. 4 c. 6 d. 8

70.

The inter metallic compound Li Ag crystallizes into cubic lattice in which both lithium and silver have coordination number of light. The crystal class is a. Simple cubic b. Face centered cubic c. Body centered cubic d. None of them

71.

An ion occupying a tetrahedral hole has co-ordination number a. 3 b. 4 c. 6

72.

If the coordination number for a certain ionic compound is 6 : 3, then the structure is a. Linear b. Tri-angular c. Rectile d.

Fluorite

73.

F – centered defects are associated with a. Structure b. Color

c.

Density

d.

All of them

74.

Promoted iron is used as catalyst to prepare a. Halogens b. HNO3

c.

H2SO4

d.

NH3

75.

Boron and aluminium are a. s – block elements c. d – block elements

b. d.

p- block elements f – block element

76.

Which one of the following elements shows the most stable +1 oxidation state? a. Al b. Ga c. In

d.

Tl

77.

Inert pair effect is exhibited by a. B b.

Al

c.

C

d.

None

78.

Aluminium chloride exist as a. Momomer b.

Dimer

c.

Polymer

d.

None

79.

BF3 is a. Lewis base c. Amphoteric

b. d.

Lewis acid Proton acceptor

80.

Icosahedron is a regular shape with a. 20 corners and 12 face c. 12 corners & 20 face

b. d.

14 corners and 20 faces 16 corners and 20 face

c.

b. d.

K Br

d.

None

Compressibility measurement All of them

d.

8

81.

Born Lande equation is used to determine the a. Ionization energy c. Lattice energy

82.

Which one of the following ions gives colored compound? a. T14+ b. Ti 3+ c. Sc3+

83.

The color of [Ti (H2O)6]3+ ion is due to a. Presence of water molecules c. Excitation of electrons from t2g to eg orbital

b. d.

Intra – atomic transfer of electrons None

84.

Which of the following compound is not colored? a. Na2 [Cu Cl4] c. K4 [Fe (CN)6]

b. d.

Na2 [Cd Cl4] K3[Fe (CN)6]

85.

The no. of unpaired electron is the [Co (NH3)6 ] 3+ ion a. 5 b. 6 c.

4

d.

3

86.

The correct electronic configuration of Mo a. 4d6 5s0 b. 4d3 5s2

4d4 5S2

d.

None

87.

Compounds of the transition elements containing highest oxidation state shows a. Ionic nature b. Covalent nature c. Co-ordinate co-valent d. All of them

88.

The element with the highest density is a. Y b. Tl

Pd

d.

Os

89.

Which of the oxides of Cr is amphoteric in nature? a. CrO b. Cr O3 c.

Cr O5

d.

None

90.

Transition elements have greater tendency to form complexes because a. They have two electrons in their outer most shell b. They have large size c. They have vacant d- orbitals d. They have fully filled d – orbitals

91.

The polarization effect produces a. Electrovalence c. Co-ordinate co-valence

92.

NaCl is more ionic them cuprous chloride because a. Cu+ has less polarizing power b. c. Cu+ has ionizing power d.

Cu+ has greater polarizing power Na+ has greater polarizing power

93.

BCl3 is a. Ionic compound c. Electron deficient compound

Lewis base Electron donor

94.

Melting point of boron is exceptionally high, the reason is a. It being an ionic substrate b. c. Due to its unusual structure d.

Due to its simple structure None of them

95.

Due to Frankel defect, the density of ionic solids a. Increases c. Does not change

Decreases Changes

96.

Schottky defect in crystals is observed when a. An ion leaves its normal site & occupies an interstitial site b. Density of the crystals is increased c. Unequal number of cations and anions are missing from the lattice d. Equal number of cations & anions are missing from the lattice.

b. d.

c.

c.

b. d.

b. d.

b. d.

Hydration energy Solvation energy d.

All of them

Co- valence All of them

97.

The lanthanide contraction is responsible for the fact that a. Zr & Y have about the same radius b. c. Zr & Hf have about the same radius d.

Zr & Zn have similar oxidation state None of them

98.

Cluster compounds in transition elements contain a. Non – metal to metal bonding c. Metal to hydrogen bonding

Metal to metal bonding Metal to oxygen bonding

99.

Titanium shows magnetic moment of 1.73 BH in its compound. What is the oxidation number of Ti in the compound? a. +2 b. +3 c. +4 d. None of above

100.

Which one is most electronegative? a. F b. Cl

b. d.

c.

***

Br

d.

I