MDCAT Chemistry Online Test With Answers

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MDCAT Chemistry Online Test

Sr. # Questions Answers Choice
1 The reason that diamond and graphite have different physical properties is density color bonding hardness
2 Diamond and graphite are isomorphous polymorphous allotropes none of these
3 The amount of energy released when gaseous ions of opposite charges combine to give one mole of a crystalline ionic compound is called bond energy heat of formation lattice energy ionization energy
4 The system in which two out of three axes are of equal length and angles are all 90° cubic system hexagonal system trigonal system tetragonal system
5 The system in which all the three axes are unequal and are at righ angle to each other is called cubic hexagonal orthorhombic tetragonal
6 If a = b = c and x = y = z 90° then crystal structure is Cubic Tetragonal Orthorhombic Triclinic
7 Two substances that have the same crystal structure are said to be isomorphous anisotropic isotropic polymorphous
8 A temperature at which two cyrstalline forms of a substances coexist in equilibrium is called standard temperature critical temperature transition temperature absolute temperature
9 Diamond is a bad conductor because it has light structure it has a high density there are no free electron present in the crystal of diamond to conduct electricity it transparent to light
10 The molecules of CO2is dry ice form the ionic crystals covalent crystals molecular crystals any type of crystal
11 Amorphous solids have sharp melting points undergo clean cleavage when cut with knife have perfect arrangement of atoms can possesses small regions of orderly arrangements of atoms
12 Ionic solids are characterized by low melting points good conductivity in solid state high vapour pressure solubility in polar solvents
13 Intermolecular forces are _________ than binding forces stronger Equal Weaker None
14 On the basis of intermolecular forces diamond is a ionic solid covalent solid metallic solid molecular solid
15 Which of the following is not a property of crystalline solid geometric shape cleavage plane anisotropy isomerism
16 Dipole-dipole forces and London forces are collectively called hydrogen bonding Vander Waals forces Covalent bonding Ionic bonding
17 Which forms metallic cyrstals Cu NaCl Diamond None
18 If there are weak intermolecular forces in a liquid, it will be more volatile less volatile more dense less heavy
19 At room temperature, the vapour pressure of water and ether will be equal different zero almost same
20 Which of the following liquid has high vapour pressure? H<sub>2</sub>O ether CH<sub>3</sub>OH C<sub>2</sub>H<sub>5</sub>OH
21 Which of the following liquid has higher boiling point? HCl HBr H<sub>2</sub>O Br<sub>2</sub>
22 Which liquid is more volatile? water mercury benzene honey
23 When vapour pressure is equal to atmospheric pressure than it is called Evaporation M.P B.P Freezing point
24 Which does not affect vapour pressure Nature of liquid intermolecular forces Temp None of these
25 The pressure exerted by the vapours in equilibrium with its pure liquid at given temperature is called the equilibrium pressure atmospheric pressure vapour pressure external pressure
26 The amount of heat required to vaporize one mole of liquid at its boiling point without change in temperature is called molar heat of vaporization molar heat of sublimation molar heat of fusion none of these
27 Vapour pressure of a liquid increasing with increase of temperature increases with decrease of temperature increases with size of container increases with volume of liquid
28 Which order of vapour pressure in the following liquids is correct water &gt; ethanol &gt; acetone &gt; ether ether &gt; acetone &gt; ethanol &gt; water ether &gt; ethanol &gt; acetone &gt; water water &gt; ether &gt; acetone &gt; ethanol
29 Vapour pressure of a liquid is more if the intermolecular forces between the molecules of the liquid are strong the intermolecular forces between the molecules of the liquid are weak more liquid is present in a container liquid has more surface area to evaporate
30 NH3can form only one hydrogen bond per molecule though it has three partially positively charged hydrogens nitrogen in NH<sub>3</sub>has only one ions pair of electrons which can make one H-bond ammonia is a base ammonia is a weak acid it ionizes to give one H<sup>+</sup>
31 H2O is liquid at room temperature whereas H2S is a gas because H<sub>2</sub>O used as drinking water, but H<sub>2</sub>S has rotten egg smell H<sub>2</sub>O is neutral. H<sub>2</sub>S is a weak acid stronger hydrogen bonding in H<sub>2</sub>O than in H<sub>2</sub>S H<sub>2</sub>O occurs abundantly than H<sub>2</sub>S
32 Boiling point of H2O is higher than that of HF although F is more electronegative than O. It is due to stronger dipole dipole forces in H<sub>2</sub>O H<sub>2</sub>O is neutral HF is acidic H<sub>2</sub>O is angular, but HF is linear number of hydrogen bonds more in H<sub>2</sub>O<sub></sub>than in HF
33 NaCl is completely ionized in water due to presence of hydrogen bonding dipole dipole forces ion dipole forces London dispersion forces
34 The attractive forces which exist between ionic compounds and water molecules are dipole-dipole forces ion diopole forces istantaneous dipole-induced dipole forces dipole-induced dipole forces
35 The attractive forces which are created due to repulsion of electronic cloud of the molecules are dipole-dipole forces ion dipole forces instantaneous dipole-induced dipole forces dipole-induced dipole forces
36 The boiling point of Kr is higher (-152.23°C) than that of helium (-268.6°C) due to Kr forms greater number of covalent bonds greater polarizability of Kr than He Kr has lowest freezing point Kr is in liquid state at ordinary temperature
37 CO2gas is dissolved in water due dipole-dipole interactions higher molecular mass of CO<sub>2</sub> ion dipole attractive forces hydrogen bonding
38 For the purpose of interacts which one of the following arrangements represents the correct of increasing stability? covalent &lt; hydrogen bonding &lt; London forces &lt; dipole-dipole London forces &lt; hydrogen bonding &lt; dipole-dipole &lt; covalent London forces &lt; dipole-dipole &lt; hydrogen bonding &lt; covalent Dipole-dipole &lt; London forces &lt; hydrogen bonding &lt; covalent
39 In which of the following molecules strongest hydrogen bond is shown water ammonia hydrogen fluoride hydrogen sulphide
40 Which one of the following molecules show maximum hydrogen bonding? H<sub>2</sub>O H<sub>2</sub>Se H<sub>2</sub>S HF
41 The maximum possible number of hydrogen bonds in which a H2O molecule can participate is 1 2 3 4
42 In which of the following compounds hydrogen bonding is not present water ethanol ether ammonia
43 Water has high boiling point which is due to weak dissociation hydrogen bonding high specific heat high dielectric constant
44 When two ice cubes are pressed together they unite to form one cube. Which of the following forces is responsibles for holding them together Van der Waal's covalent bonding hydrogen bonding dipole-dipole interaction
45 London forces are more affective at low temperature high temperature low pressure low temperature and high pressure
46 The bonding which occurs among polar covalent molecules containing H and one of the small electronegative element such as O, F or N is called bridge bonding metallic bonding hydrogen bonding Ionic bonding
47 When water freezes at 0°C, its density decreases due to cubic structure of ice empty spaces present in the structure of ice change of bond lengths change of bond angles
48 NH3shows a maximum boiling point among the hydrides of Vth group elements due to very small size of nitrogen hydrogen bonding between its molecules enhanced electronegative character of nitrogen pyramidal structure of NH<sub>3</sub>
49 Acetone and Chloroform are soluble in each other due to intermolecular hydrogen bonding ion-dipole interaction instantaneous dipoles dipole-induced dipole interaction
50 In which system hydrogen bonding is not present solution of ethanol in water linking of helix in protein molecule structure of ice solution of NaCl in benzene
51 The boiling point of radon (211 K) is higher than boiling point of Helium (4.4 K) because the atomic number of Rn is larger than that of the He the atomic mass of Rn is larger than that of He the dispersion forces between Rn atoms are more prominent that between He atoms Rn atoms are joined by dipole-dipole force whereas He atoms are joined by hydrogen bonding
52 An example of ion-dipole force is solution of NaCl in water Glucose in water Bromine in benzene Ethanol in water
53 Which of the following molecules have a permanent dipole CH<sub>4</sub> CHCl<sub>3</sub> CCl<sub>4</sub> CO<sub>2</sub>
54 Which of the following may be called London dispersion forces dipole-dipole forces ion-dipole forces dipole-induced dipole forces instantaneous dipole-induced dipole forces
55 Diffusion of different species is due to difference of potential energy temperature density all the above
56 Which one the following gases is ideal at -200°C? N<sub>2</sub> He both none
57 Real gases deviate from the ideal behaviour at very high pressure low temperature low pressure both a and b
58 The phenomenon in which sudden expansion of a gas causes cooling is called evaporation cooling Joule Thomson effect sublimation
59 Joule is a unit of energy which is defied as Kgm<sup>-2</sup>s<sup>-2</sup> Kgm<sup>2</sup>s<sup>-1</sup> Kgms<sup>-2</sup> Kgm<sup>2</sup>s<sup>-2</sup>
60 Equal volumes of all gases at STP contain equal no of molecules is called Dalton's law of partial pressure Graham'a law of diffusion Avogadro's law None
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