Chemistry Chemical Bonding Online Mcqs Test

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Question 1

1. Element having the smallest atomic radius among the following is

Question 2

2. By combining n atomic orbital, numbers of hybrid orbitals will be

Answer

Impossible to predict

Question 3

3. The relative attraction of the nucleus for the electrons in a chemical bond is called

Answer

Ionization energy

Answer

Electronegativity

Answer

Electron affinity

Answer

None of these

Question 4

4. In a double bond connecting two atoms there is a sharing of

Answer

6 electrons

Answer

4 electrons

Answer

1 electron

Answer

2 electrons

Question 5

5. The number and type of bonds between carbon atoms in calcium carbide are

Answer

Two sigma, one pi

Answer

One sigma, one pi

Answer

Two sigma, two pi

Answer

One sigma, two pi

Question 6

6. Which of the following molecules has no net dipole moment?

Question 7

7. In Millikan oil – drop experiment, the charges on several different oil drops were as: -5.92. – 4.44, -2.96, -8.88. The units are arbitrary. Choose the likely value of the electronic charge in these arbitrary units?

Question 8

8. The ionization energy

Answer

Generally increases from left to right in a period

Answer

Does not change in a group

Answer

Increase from top to bottom in a group

Answer

Does not change in a period

Question 9

9. Which of the following is not isoelectronic?

Question 10

10. Which of these molecules require more bond energy?

Question 11

11. Which of the following has zero depolemoment?

Question 12

12. Which one of these is weakest?

Answer

Metallic bond

Answer

Covalent bond

Answer

Van der Waal’s forces

Answer

Ionic bond

Question 13

13. Along a period the atomic radii

Answer

First decreases then increases

Question 14

14. Which of the sub – atomic particles is not charged?

Question 15

15. Which kinds of bonding can be found in a sample of H₂O(l)?

Answer

Nonpolar covalent bonds only

Answer

Hydrogen bonds only

Answer

Ionic and nonpolar hydrogen bonds

Answer

Both polar covalent and hydrogen bonds

Question 16

16. In OF₂, number of bond pairs and lone pairs of electrons are respectively

Question 17

17. Which of the following molecules does not have a net dipole moment?

Question 18

18. Fluorine molecule is formed by

Answer

The sidewise p-p overlap

Answer

The axial p-p overlap

Answer

The axial s-p overlap

Answer

The overlap of two sp² hybrid orbitals

Question 19

19. When 2 lone pair and 2 bond pair are around the central atom reduction in the bond angle is up to. (in degrees)

Question 20

20. Noble gases are most stable of all other elements because

Answer

They have high ionization energies

Answer

They do not react with one another

Answer

They have completely filled s and p orbitals

Answer

They are mono atomic gases

Question 21

21. Al become isoelectronic with Ne

Answer

By gaining three electrons

Answer

By losing three electrons

Answer

By losing two electrons

Answer

By gaining two electrons

Question 22

22. The relative attraction of the nucleus for the electrons in a chemical bond is called

Answer

Ionization energy

Answer

None of these

Answer

Electro negativity

Answer

Electron affinity

Question 23

23. Which of the following value of Electronegativity difference corresponds the formation of Ionic Bond?

Answer

Lesser then 1.7

Answer

Greater than 1.7

Answer

No specificity exist

Answer

Equal to 1.7

Question 24

24. Molecular orbital picture of N₂ indicates

Answer

One unpaired electron

Answer

None of these

Answer

Two unpaired electron

Answer

No unpaired electron

Question 25

25. On sp3 hybridization

Answer

Four p-orbitals are involved

Answer

One s and 3 p-orbitals are involved

Answer

All p-orbitals are involved

Answer

One p-orbital is involved

Question 26

26. Choose the correct statement about 2nd ionization energy

Answer

It is always greater than 1st ionization energy

Answer

It may be greater or less than the 1st ionization depending upon ht nature of the element

Answer

It is always less than 1st ionization energy

Answer

It is equal to the 1st ionization energy

Question 27

27. The atomic number of an element is 35. What is the total number of electrons present in all the p-orbitals of the ground state atom of that element?

Question 28

28. Which one among the following does not have the hydrogen bond?

Answer

Liquid HCl

Answer

Liquid NH3

Question 29

29. Which is not true with respect to cathode rays?

Answer

A stream of electrons

Answer

Can be deflected by magnetic fields

Answer

Charged particles

Answer

Move with speed as that of light

Question 30

30. Bond order for N2 molecule is

Question 31

31. The twelve enter most electrons in O₂ molecule are distributed according to MOT as under. Find the correct one.

Answer

8 in bonding molecular orbitals, 4 in anti-bonding molecular orbitals

Answer

9 in bonding molecular orbitals and 3 in anti-bonding molecular orbitals

Answer

10 in bonding molecular orbitals and 2 in anti-bonding molecular orbitals

Answer

12 in bonding molecular orbitals, and zero in anti-bonding molecular orbitals

Question 32

32. Keeping in view the bonding molecular orbitals, find the incorrect statement

Answer

Bonding molecular possess less energy than atomic orbitals from which they are formed

Answer

Every electron in the bonding molecular orbital contributes to the attraction between atoms

Answer

Bonding molecular orbitals are formed when the electrons waves are undergo constructive interference

Answer

Bonding molecular orbitals have low electron density between the two nuclei

Question 33

33. According to VSPER theory, ammonia molecule has --------- shape

Answer

Triangular

Answer

Tetrahedral

Question 34

34. The relative attraction of the nucleus for the electrons in a chemical bond is called

Answer

Electro negativity

Answer

Electron affinity

Answer

None of these

Answer

Ionization energy

Question 35

35. Which of the following hydrides has the lowest boiling point?

Question 36

36. How many sigma and pi bonds are present in tetra cyano ethylene?

Answer

Eight σ and eight π

Answer

Five π and nine σ

Answer

Nine σ and seven π

Answer

Nine σ and nine π

Question 37

37. A student subtracted 0.00055 from 10.2345678 and reported the result as 10.23401. But his friend told him that result was wrong. What is the correct result?

Answer

10.2340178

Question 38

38. Geometry of simple molecule having sp3 hybrid orbital is

Answer

Tetrahedral

Answer

Triangular

Answer

Square planner

Question 39

39. Which of the following contains both polar and non-polar bonds?

Question 40

40. The number of significant figures in 0.00200 is

Question 41

41. With increasing principle quantum number, the energy difference between adjacent energy levels in H atom

Answer

Decreases for low value of Z and increases for higher value of Z

Answer

Remains constant

Question 42

42. The shape of ClO₃ according to valence shell electron pair repulsion theory will be

Answer

Planar triangle

Answer

Square planar

Answer

Tetrahedral

Question 43

43. Anti-bonding MO is formed by

Answer

Addition of atomic orbitals

Answer

None of these

Answer

Subtraction of atomic orbitals

Answer

Multiplication of atomic orbitals

Question 44

44. How many molecular orbitals may be constructed from the valence shell orbitals of the constituent atoms in CH₄?

Question 45

45. Which of the following is to isoelectronic with rest of three?

Question 46

46. The energy required to remove electron from an atom is called

Question 47

47. Unit of dipole moment is

Question 48

48. Azimuthal quantum number of last electron of ₁₁Na is

Question 49

49. Which molecule is polar among the following?

Answer

Carbon dioxide

Answer

Carbon tetrachloride

Question 50

50. The most suitable method of the separation of a mixture of ortho and para-nitrophenol mixed in the ratio of 1 : 1 is

Answer

Colour spectrum

Answer

Crystallization

Answer

Distillation

Answer

Vaporization

Question 51

51. If the molecule of HCl were totally polar, the expected value of dipole moment is 6.12 D (Debye) but the experimental value of dipole moment was 1.03 D. Calculate the percentage ionic character.

Question 52

52. Quantum umber values for 2p orbitals are

Answer

n = 1, l = 2

Answer

n = 1, l = 0

Answer

n = 2, l = 0

Answer

n = 2, l = 1

Question 53

53. A lone pair of electrons in an atom implies

Answer

A pair of valence electrons

Answer

A pair of electrons involved in bonding

Answer

A pair of electrons

Answer

A pair of valence electrons not involved in bonding

Question 54

54. Lewis acids are

Answer

Octet is complete

Answer

Electron rich

Answer

No such acids exist

Answer

Electron deficient

Question 55

55. The energy of a photon is given as, ∆ E/atom = 3.03 x 10¯¹⁹ J atom¯¹ then, the wavelength (λ) of the photon is

Question 56

56. Which of the following has the greatest covalent character?

Question 57

57. Which of the following is not absolute term of element?

Answer

Electronegativity

Answer

Atomic size

Answer

Ionization energy

Answer

Electron affinity

Question 58

58. An oxygen atom has mass of

Answer

2.657 x 10¯²³ g

Answer

5.316 x 10¯²³ g

Answer

5.316 x 10¯²³ g

Question 59

59. The boiling point of heavy water is

Question 60

60. In O2 each oxygen atom is hybridized

Question 61

61. Electronic configuration of K is

Question 62

62. Which quantum number is sufficient to describe the electron is hydrogen atom?

Question 63

63. The structure of ICl₂¯ is

Answer

Square planar

Answer

Octahedral

Answer

Trigonal bipyramidal

Question 64

64. Which of the following statements about positive ions is incorrect?

Answer

They are larger than the atoms from which they were formed

Answer

They are also known as cations

Answer

They are smaller than the atoms from which they were formed

Answer

They are formed when electros are formed from atoms

Answer 128

H – NH₂

Answer 129

Higher than individual

Answer 130

Impossible to predict

Answer 131

Lesser than individual

Answer 132

All solvents

Answer 133

Concentrated acids

Answer 134

Polar solvents

Answer 135

Non-polar solvents

Answer 136

Hund’s rule

Answer 137

Aufbau principal

Answer 138

Pauli’s exclusion principle

Answer 139

Ion-dipole interaction

Answer 140

Dispersion force

Answer 141

Dipole-dipole interaction

Answer 142

Electron affinity

Answer 143

Electronegativity

Answer 144

Ionization potential

Answer 145

Activation energy

Answer 146

Octahedral

Answer 147

Planar triangle

Answer 148

Distorted tetrahedral

Answer 149

Depends on its wavelength

Answer 150

Equal to square

Answer 151

Independent of its wavelength

Answer 152

Depends on its source

Answer 153

All of above represent same entity

Answer 154

Interaction

Answer 155

Attractive force

Answer 156

The nature of residual gas

Answer 157

All of these

Answer 158

The nature of electrode

Answer 159

The nature of discharge tube

Answer 160

Quarternization of energy of electrons

Answer 161

Heisenberg’s uncertainty principle

Answer 162

Plank’s quantum theory

Answer 163

Quarternization of angular members

Answer 164

Tetrahedron

Answer 165

4, 0, 0, ½

Answer 166

4, 4, 0, ½

Answer 167

4, 1, 0, ½

Answer 168

4, 1, 1, ½

Answer 169

Fluorides is more electronegative

Answer 170

Fluorides are more electronegative

Answer 171

NH₃ is pyramidal in shape while BF₃ is planar

Answer 172

Boron trifluoride is pyramidal in shape while NH₃ is planar

Answer 173

6.02 x 10¹⁶ J/mol

Answer 174

10¯⁷ J/mol

Answer 175

6.02 x 10²³ J/mol

Answer 176

None of these

Answer 177

Bonding will not occur

Answer 178

Both A and B are correct

Answer 179

Orbital overlap will not occur

Answer 180

2π and one σ bond

Answer 181

Ionic bonds

Answer 182

2 sigma bonds

Answer 183

2 covalent, one co-ordinate bond

Answer 184

Dipole interaction

Answer 185

Van der Waal’s forces

Answer 186

Hydrogen bond formation

Answer 187

Covalent attraction

Answer 188

X-rays not produced

Answer 189

Gamma rays

Answer 190

Larger wavelength

Answer 191

Shorter wavelength

Answer 192

They energy of atoms increases

Answer 193

The two atoms start ionization

Answer 194

The attractive forces dominate the repulsive forces

Answer 195

The repulsive force dominate the attractive forces

Answer 196

Bond order of 2.5

Answer 197

Stability lower then O₂

Answer 198

Diamagnetic character

Answer 199

Three unpaired electrons

Answer 200

Trigonal bipyramidal

Answer 201

Triangular

Answer 202

Square planner

Answer 203

Octahedral

Answer 204

Electropositive character of elements

Answer 205

Pauli exclusion principle

Answer 206

Octet rule

Answer 207

Electronegative character of elements

Answer 208

Un-hybrid orbitals

Answer 209

Hybrid and un hybrid orbitals

Answer 210

Hybrid orbitals

Answer 211

Atomic orbital and hybrid orbital

Answer 212

Cannot be determined

Answer 213

Both are equal

Answer 214

Nuclei are stable

Answer 215

Molecules are stable

Answer 216

Nuclei are unstable

Answer 217

Molecules are unstable

Answer 218

Blue is darker colour

Answer 219

Blue has higher wavelength

Answer 220

Blue has more energy

Answer 221

Blue is absorbed more easily

Answer 222

Hydrogen sulphide

Answer 223

Hydrogen fluoride

Answer 224

It has high electronegativity

Answer 225

There is triple bond between nitrogen atoms which make the molecule quite stable

Answer 226

It has high heat of dissociation

Answer 227

Some of the electrons are also present in anti-bonding molecular orbitals

Answer 228

3 bond pair one lone pair

Answer 229

1 bond pair 3 lone pair

Answer 230

2 bond pair 2 lone pair

Answer 231

3 lone pair 1 bond pair

Answer 232

Low, positive or slightly negative

Answer 233

Low very negative

Answer 234

High, very negative

Answer 235

None of these

Answer 236

Square planner

Answer 237

Tetrahedral

Answer 238

Triangular

Answer 239

Sixth Bohr orbit to the third Bohr orbit

Answer 240

Fifth Bohr orbit to the second Bohr orbit

Answer 241

Fourth Bohr orbit to the first Bohr orbit

Answer 242

Seventh Bohr orbit to the third Bohr orbit

Answer 243

6.63 x 10¯³⁴ m

Answer 244

6.63 x 10¯³³ m

Answer 245

6.65 x 10¯³⁵ m

Answer 246

6.63 x 10¯³⁵ m

Answer 247

Water has higher molecular weight

Answer 248

Water molecules associate through hydrogen bonding

Answer 249

Sulphure has high electronegativity than oxygen

Answer 250

Hydrogen sulphide is a weak acid

Answer 251

Trigonal bipyramidal

Answer 252

Tetrahedral

Answer 253

Trigonal bipyramidal

Answer 254

Octahedral

Answer 255

Excited state of fluorine

Answer 256

Ground state of fluorine atom

Answer 257

Excited state of O¯₂

Answer 258

Excited state of neon

Answer 259

X – radiation, visible, infrared, microwave

Answer 260

Visible, ultraviolet, infrared, gamma rays

Answer 261

Microwave, infrared, visible, ultraviolet

Answer 262

Radio, visible, infrared, ultraviolet

Answer 263

Noble gases

Answer 264

Alkali metals

Answer 265

Gun metals

Answer 266

Coinage metals

Answer 267

Ionic bond

Answer 268

Metallic bond

Answer 269

First decreases then increases

Answer 270

First increases then decreases

Answer 271

Ejection of electrons takes place

Answer 272

The absorption of electrons takes place

Answer 273

There is no effect

Answer 274

Ejection of some potassium atoms occurs

Answer 275

Lone pair – lone pair repulsion only

Answer 276

Bond pair – bond pair repulsion only

Answer 277

Lone pair – bond pair repulsion only

Answer 278

Lone pair – lone pair repulsion and lone pair – bond pair repulsion

Answer 279

sp²- hybridized carbon

Answer 280

sp- hybridized carbon

Answer 281

sp³-hybridized carbon

Answer 282

always same irrespective of its hybrid state

Answer 283

1.7588 x 10²⁰

Answer 284

6.02 x 10²³

Answer 285

9.1095 x 10¯³¹

Answer 286

1.7588 x 10¹¹

Answer 287

Does not depend on the nature of the gas used in the discharge tube

Answer 288

Does not depend on the nature of the gas used in the discharge tube

Answer 289

Depends on the gas used in the discharge tube

Answer 290

Depends on the pressure in the discharge tube

Answer 291

Remain same

Answer 292

Triangular bipyramidal

Answer 293

Triangular pyramidal

Answer 294

Tetrahedral

Answer 295

Triangular planar

Answer 296

Tetrahedral

Answer 297

Triangular planar

Answer 298

Each bonding molecular orbital can accommodate only one electron

Answer 299

As bonding molecular orbitals become more stable, anti-bonding molecular orbital become equally less stable

Answer 300

In molecular orbitals, the number of bonding electrons equals the number of anti-bonding electrons

Answer 301

The molecular orbitals in a molecule equals twice the number of constituent atomic orbitals

Answer 302

SP hybridization

Answer 303

Dipole moment is zero

Answer 304

Linear geometry

Answer 305

First decreases then increases

Answer 306

First increases then decreases

Answer 307

Double bond

Answer 308

Covalent bond

Answer 309

Co-ordinate bond

Answer 310

Electrovalent bond

Answer 311

sp³ hybrid orbitals

Answer 312

s orbitals

Answer 313

sp² hybrid orbitals

Answer 314

p orbitals

Answer 315

Variable trend

Answer 316

Two sigma bonds and one pi-bond

Answer 317

Three sigma bonds

Answer 318

One sigma bond and two pi-bonds

Answer 319

Three pi-bonds

Answer 320

Covalent forces

Answer 321

Van der Waal forces or London dispersion forces

Answer 322

All of these

Answer 323

Hydrogen bonds

Answer 324

Bond length is unpredictable

Answer 325

Bond length in NO⁺ is greater than in NO

Answer 326

Bond length in NO⁺ is equal to that in NO

Answer 327

Bond length in NO is greater than in NO⁺

Answer 328

Photosensitivity of sodium

Answer 329

Emission of excess energy absorbed as a radiation in the visible region

Answer 330

Sublimation of metallic sodium to give yellow vapour

Answer 331

Low ionization energy of sodium

Answer 332

Water should be preferred over lemon Juice for drinking

Answer 333

Lemon juice is dangerous for health

Answer 334

There may not be a possibility of chemical reaction

Answer 335

There may be a possibility of a chemical reaction

Answer 336

1/2 x ɜ₀

Answer 337

Chemical bond

Answer 338

Van der Waal’s force

Answer 339

Dispersion force

Answer 340

London force

Answer 341

Trigonal bipyramidal

Answer 342

Square planar

Answer 343

Tetrahedral

Total Questions:	187
Time Allowed:	60 Minutes
Total Marks:	187
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