ECAT Chemistry Chapter 4 Liquids & Solids Online Test With Answers

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ECAT Chemistry Chapter 4 Liquids & Solids Online Test

Sr. # Questions Answers Choice
1 Trend of boiling point of halogens from fluorine to Iodine is that it Decreases Is negligible Increases Remains constant
2 Heat of vapourization for liquids with strong dipole-dipole forces will have Negligible Values Reasonably high values Very high values very low values
3 The boiling point of NH3is maximum among the hydrides of group V elements due to Enhanced electronegative character of Nitrogen Pyramidal structure of NH<sub>3</sub> Very small size of Nitrogen Enhanced electropositive character of Nitrogen
4 Which of the following liquids has low vapour pressure at 250C Diethyl ether Acetone Water Ethyl alochol
5 Escape of high energy molecules from the surface of a liquid is called Sublimation Distillation Condensation Evaporation
6 A liquid on evaporation causes Heating effect Cooling effect Suffication All of above
7 At sea level and at 1000C the vapour pressure of water in an open system is 1000 mm Hg 760 mm Hg 730 mm Hg 670 mm Hg
8 Rate of evaporation and rate of condensation at equilibrium Become very low Become very high Become equal Can never be equal
9 Evaporation of water is possible at Above 100<sup>0</sup> 0<sup>0</sup> 100<sup>0</sup> At all temperature
10 H2S is a gas which H2O is liquid at room temperature. it is due to Less intermolecular forces in water Covalent bond in H-O in water molecule Hydrogen bonding in water molecules Ionic characters in water molecules
11 Hydrogen bonding is present between the molecules of NH<sub>3</sub> H<sub>2</sub>O HF All of above
12 Debye forces are present in one of the following pairs Na<sup>+</sup>ion and water Argon and water Argon and Na<sup>+</sup>ion Ne and Water
13 The strongest forces are Debye forces London dispersion forces Dipole-dipole attraction Hydrogen
14 Polypeptide chains are coiled about one another into a spiral by Ionic bonds Covalent bonds Van der Waal's forces Hydrogen bonds
15 HF has exceptionally low acidic strengths due to Smaller size of fluorine Strong polar bond between H and F Electronegativity of fluorine Strong hydrogen bonding
16 Hydrocarbon molecules with large chain lengths experience Weaker attractive forces Stronger attractive forces Repulsive forces No attractive forces
17 In a group on going downward, polarizability generally Decreases Increases Remains constant Negligible
18 London dispersion forces are also called Hydrogen bonding Debye forces Van de Waal's forces Instantaneous dipole-induced dipole forces
19 The intermolecular forces in liquids are Negligible Very weak Very strong Reasonably strong
20 The gases can be converted into liquids by increasing the pressure only Lowering temperature and increasing pressure Increasing pressure and bringing temperature below critical point Lowering temperature only
21 Which one of the following is the weakest intermolecular force Dipole induced dipole forces Ionic dipole forces Electrostatics forces between ions Dipole-dipole forces
22 The density of water decreases, when it is freezed at 0oC because of Change of bond lengths Change of bond angles Cubic structure of ice Empty spaces present in the structure of Ice
23 The only forces are London dispersion forces among the Atoms of He in gaseous state at high temperature Molecules of water in liquid state Molecules of solid I<sub>2</sub> Molecular of hydrochloric acid gas
24 Force of attraction between atoms of He is London dispersion forces Hydrogen bondign Coordinate covalent bond Covalent bond
25 Chloroform and acetone are soluble in each other due to Instantaneous dipole interactions Dipole-dipole interactions Intermolecular hydrogen bonding All of above
26 Diamond is a bad conductor because It has a tight structure It has a high density there is no free electron present in the crystal of diamond of conduct electicity Is transparent to light
27 Which of the following is a pseudo solid CaF<sub>2</sub> Glass NaCl All
28 The molecules of CO2in dry ice from the Ionic crystalls Covalent crystals Molecular crystals Any type of crystal
29 Amorphous solids Have sharp melting point Undergo clean cleavage when cut with knife Have perfect arrangement of atoms Can possesses small regions of orderly arrangement of atoms
30 Ionic Solids are characterized by Low melting points Good conductivity in solid state High vapour pressure Solubility in polar solvents
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