MDCAT Chemistry Online Test With Answers

MDCAT Chemistry Online Test

Sr. # Questions Answers Choice
1 The geometry of diamonds is tetragonal cubic rhombohedral none of these
2 The molecules of CO2, in dry ice form the covalent crystals molecular crystals none of these crystals ionic crystals
3 The nature of crystal of diamond is metallic molecular covalent ionic
4 The crystals formed due to London forces of interaction are ionic covalent molecular metallic
5 In most of the cases the molecular crystals are very soft soft extremely hard sufficiently hard
6 The crystal of diamond is ionic molecular covalent metallic
7 Substance that does not show the process of sublimation is K2Cr2O7 iodine naphthalene NH4CI
8 The number of Na+, ions which surround each Cl- ion in the NaCl crystal lattice is 8 12 6 10
9 NaCI has face centered cubic structure. The Na ion at the face of the unit cell is shared by 2-unit cells 4-units cells only one unit cell 8-unit cells
10 The Cl- ion present at the corner of the unit cell is NaCl crystal, contributes 1/8 th 1/4 th 1/2 th 1
11 The number of Cl- ions per unit cell of NaCl are 6 4 2 8
12 lonic solids don't conduct the electrical current because ion do not have translatory motion free electrons are less the coordination number of the ion is very high strong covalent bonds are present in their structure
13 lonic solids are characterized by which one of the following properties moderately low pressure high vapour pressure good conductivity in solid state solubility in polar solvents
14 Some of crystals are good conductors of heat and electricity, they may be ionic in nature of metallic character covalent in nature of molecular nature
15 LiF is a crystalline substance and has ionic crystal metallic crystal covalent crystal molecular crystal
16 One of the following is a ionic solid. Which is that? Fe KBr Diamond Cr
17 An element from the given below exists as discrete small molecules in the solid state. Which is that? Sodium Silicon lodine lron
18 The structure of sodium chloride is simple cube body centered cubic face centered cubic depends upon conditions
19 Which property is associated with ionic solids? Solubility in polar solvents Low melting points Good conductivity in solid state High vapour pressure
20 In crystal of sodium chloride, a Cl-1 ion present at the corner of cube is shared between how many cubes? 8 4 6 10
21 What is the co-ordination number of face centered cubic structure? 12 8 6 10
22 A crystal system in which all three angles and all three edges are different is called triclinic rhombohedral cubic hexagonal
23 Structure of CrO4(-2) is' triclinic cubic octahedral tetrahedral
24 The most unsymmetrical one in crystal system is triclinic Li, Na, K monoclinic hexagonal
25 The hexagonal closed packing is associated with Ag, Cu, Au Zn, Cd, Hg Li, Na, K NaCl, KBr
26 Which impurity makes the shape of NaCl crystal needle like MgSO4 urea glucose MgCO3
27 K2SO4, and K2Cr2O4, are isomorphous solids and exist in cubic form orthorhombic form trigonal form tetragonal
28 The transition temperature of tin is 95.5 C° 13.2 C° 13.2°C 128.5°
29 The existence of an element in more than one form is called allotropy isomorphism polymorphism isotropy
30 The transition temperature of KNO3, is 13.2°C 95.5°C 128°C 32.02°C
31 Polymorphism is shown by AgNO3. Which one of the following options is true for AgNO3? Orthorhombic and rhombohedral Cubic and orthorhombic Cubic and tetragonal Monoclinic and hexagonal
32 Which one is an isomorphic pair? NaNO3, CaCO3, NaF, MgO K2SO4 ,K2Cr2O7 Zn, Cd
33 The examples of a hexagonal system is sugar graphite(a=b not equal to c) {Alpha =beta. not equal to gamma} sulphur diamond
34 In diamond, the carbon atoms are arranged in a tetrahedral manner hexagonal manner square planar manner octahedral manner
35 Hardness of diamond is attributed to the strength of the ionic bonds in the structure three-dimensional network of covalent bonds three-dimensional network of covalent bonds absence of valence electrons in carbon atoms
36 How many allotropic forms are present in carbon? Two Four Three Five
37 Which among the following will show anisotropy? Wood Glass Paper BeCl2
38 Crystals can be classified into 7 crystal systems 4 crystal systems 3 crystal systems 14 crystal systems
39 Amount of heat absorbed when one mole of a solid melts into liquid form at its melting point is called: heat of vaporization latent heat of fusion molar heat of fusion molar heat of sublimation
40 The boiling point of glycerin at 1 atmospheric pressure is: 290°C 390°C 190C° 210°C
41 In order to maintain the boiling point of water at 110 C°, the extemal pressure should be 550 torr between 500 and 760 tor between 760 and 1500 torr any pressure can be maintained
42 Which of following factor affect vapour pressure of a liquid? temperature inter molecules forces size of the molecules all of these
43 The boiling of water may be 120°C, when the external pressure is greater than 760 torr less than 760 torr equal to 760 torr variable
44 Liquids evaporate at every temperature. When the temperature becomes constant for a liquid, then: rate of evaporation is greater than the rate of condensation the rate of condensation is greater than the rate of evaporation The rate of condensation and evaporation become equal it depends upon the nature of the liquid
45 Point out the substance which has maximum vapour pressure at a given temperature? Acetone Water Ethanol Acetic acid
46 Vapour pressure of a substance does not depend upon: physical state of matter temperature intermolecular forces surface area
47 Which of the following liquid has highest bolling point HCI HBr H2O Br2
48 The B.P. of compound is mostly raised by dipole-induced dipole interactions london dispersion forces intramolecular H-bonding intermolecular H-bonding
49 The vapour pressure of a liquid depends upon amount of the liquid surface area temperature size of container
50 The B.P of glycerine at 760 torr pressure is 200°C 290C° 250C° 262C°
51 lce occupies more space than liquid water 9% 10% 11% 12%
52 At freezing point of water, the density decreases due to change of bond angles change of bond lengths cubic structure of ice empty spaces present in the structure of ice
53 The long chains of amino acids are coiled around one another into a spiral by ionic bond Van der Waal's forces hydrogen bonding overlapping of orbitals
54 H2O and HF are the hydrides of the second period. Fluorine is more electronegative than oxygen. Anyhow, the boiling point of water is greater than that of HF. This is due to: water is more polar than HF water has a bent structure HF has a zig zag structure after making hydrogen bonding the number of hydrogen bonds produced by water are greater than that of HF
55 Hydrogen bonding is extensively present in proteins which form the spiral. The hydrogen bond being produced is between nitrogen and hydrogen atom oxygen and hydrogen atom carbon and hydrogen atom oxygen and carbon atom
56 Halogens form halogen acids. HF is the weakest among all of them This is due to the reason that fluorine is a very small-sized atom fluorine is highly electronegative atom there is strong hydrogen bonding in HF the polarity of HF bond is less
57 The boiling point of H2O is 100°C while that of C2H5-OH is 78.5C°. The reason is that: H2O molecules are small-sized the bond angles at oxygen atom are different C2H5-group is electron donating the number of H-bonds are greater in H20, than C2H5-OH
58 Oxygen and sulphur are present in VI-A group of the periodic table The hydride of oxygen i.e., H2O is liquid at room temperature but the hydride of sulphur (H2S) is a gas. This is due to greater bond angle of water than Hs greater bond lengths in HS than H2O hydrogen bonding in water acidic character of HS
59 Ice floats on water because the hydrogen bonding in ice is stronger than that of in water empty spaces are left in ice ice has two-dimensional structure the bond length of the oxygen and hydrogen bond is different in water and ice
60 H-bonding is maximum in: ethanol benzene diethyl ether water
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