Chemistry Chemical Bonding Online Mcqs Test

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Question 1

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

Answer

Planar triangle

Answer

Tetrahedral

Answer

Square planar

Question 2

2. The spectrum of He is expected to be similar to that of

Question 3

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

Question 4

4. 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 5

5. When a double bond is formed between two atoms, one of the bonds is a sigma bond and the other is a pi bond. The pi bond is created by the overlap of……

Answer

sp³ hybrid orbitals

Answer

sp² hybrid orbitals

Answer

s orbitals

Answer

p orbitals

Question 6

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

Answer

Vaporization

Answer

Crystallization

Answer

Colour spectrum

Answer

Distillation

Question 7

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

Answer

Triangular

Answer

Tetrahedral

Question 8

8. The correct set of quantum numbers (n, l and m) respectively of the unpaired electron of chlorine atom is:

Question 9

9. Fluorine molecule is formed by

Answer

The axial p-p overlap

Answer

The sidewise p-p overlap

Answer

The overlap of two sp² hybrid orbitals

Answer

The axial s-p overlap

Question 10

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

Answer

Electron affinity

Answer

Ionization energy

Answer

Electronegativity

Answer

Atomic size

Question 11

11. Ammonia has a net dipole moment while boron trifluoride has zero dipole moment because

Answer

NH₃ is pyramidal in shape while BF₃ is planar

Answer

Fluorides are more electronegative

Answer

Boron trifluoride is pyramidal in shape while NH₃ is planar

Answer

Fluorides is more electronegative

Question 12

12. The energy of the first electron in helium will be

Question 13

13. When 6d orbital is complete, the entering electron goes into

Question 14

14. 1 erg of energy corresponds to

Answer

6.02 x 10¹⁶ J/mol

Answer

10¯⁷ J/mol

Answer

6.02 x 10²³ J/mol

Question 15

15. The configuration 1s² 2s² 2p⁵ 3s¹ shows

Answer

Excited state of O¯₂

Answer

Excited state of fluorine

Answer

Ground state of fluorine atom

Answer

Excited state of neon

Question 16

16. 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 formed when electros are formed from atoms

Answer

They are smaller than the atoms from which they were formed

Answer

They are also known as cations

Question 17

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

Question 18

18. Hydrogen chloride molecule contains

Answer

Covalent bond

Answer

Co-ordinate bond

Answer

Double bond

Answer

Electrovalent bond

Question 19

19. Geometry of simple molecule having SP³ hybrid orbital is

Answer

Square planner

Answer

Tetrahedral

Answer

Triangular

Question 20

20. An electron has principal quantum number 3. The number of its (i) subshells and (ii) orbitals would be respectively

Question 21

21. The carbon atoms in calcium carbide are held by

Answer

Ionic bonds

Answer

2 sigma bonds

Answer

2 covalent, one co-ordinate bond

Answer

2π and one σ bond

Question 22

22. What happens to IP value if shielding effect is greater?

Answer

Remain same

Question 23

23. Bohr’s model atom is contradicted by

Answer

Quarternization of angular members

Answer

Quarternization of energy of electrons

Answer

Plank’s quantum theory

Answer

Heisenberg’s uncertainty principle

Question 24

24. According to VESPR Model the geometry of molecule having 5 bond pair in outer most shell will be

Answer

Trigonal bipyramidal

Answer

Triangular

Answer

Square planner

Answer

Octahedral

Question 25

25. When potassium metal is exposed to violet light

Answer

The absorption of electrons takes place

Answer

Ejection of some potassium atoms occurs

Answer

There is no effect

Answer

Ejection of electrons takes place

Question 26

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

Answer

Eight σ and eight π

Answer

Nine σ and seven π

Answer

Five π and nine σ

Answer

Nine σ and nine π

Question 27

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

Answer

Bonding molecular orbitals have low electron density between the two nuclei

Answer

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

Answer

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

Answer

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

Question 28

28. The nature of positive rays depends upon

Answer

All of these

Answer

The nature of discharge tube

Answer

The nature of electrode

Answer

The nature of residual gas

Question 29

29. H-bonding is not present in

Answer

Hydrogen fluoride

Answer

Hydrogen sulphide

Question 30

30. The shape of H₃O⁺ is

Answer

Triangular planar

Answer

Tetrahedral

Question 31

31. Along a period the atomic radii

Answer

First decreases then increases

Question 32

32. Electronic configuration of K is

Question 33

33. Number of π-bonds in naphthalene is

Question 34

34. 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 35

35. Unit of dipole moment is

Question 36

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

Question 37

37. ____________ has their outermost shell complete in atomic form

Answer

Noble gases

Answer

Alkali metals

Answer

Coinage metals

Answer

Gun metals

Question 38

38. Number of sigma bonds in P₄O₁₀ is

Question 39

39. Effective magnetic moment of Sc³ ion is

Question 40

40. A molecule in which sp² hybrid orbitals are used by the central atom in forming covalent bonds is

Question 41

41. In the ground state, an element has 13 electrons in its M shell. The element is

Question 42

42. Pi bonds are produced by overlapping of

Answer

Un-hybrid orbitals

Answer

Atomic orbital and hybrid orbital

Answer

Hybrid orbitals

Answer

Hybrid and un hybrid orbitals

Question 43

43. Outermost shells of two elements X and Y have two and six electrons respectively. If they combine, the expected formula of compound will be

Question 44

44. Nitrogen gas is chemically inert gas due to the reason that

Answer

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

Answer

It has high heat of dissociation

Answer

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

Answer

It has high electronegativity

Question 45

45. Which orbital of the following has a principal quantum number of 3 and an angular momentum quantum number of 27?

Question 46

46. Colour of the glow produced in the discharge tube

Answer

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

Answer

Depends on the gas used in the discharge tube

Answer

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

Answer

Depends on the pressure in the discharge tube

Question 47

47. Which of the following has zero depolemoment?

Question 48

48. When two ice cubes are pressed over each other, they unite to form one cube. Which of the following forces is responsible to hold them together?

Answer

Covalent attraction

Answer

Dipole interaction

Answer

Van der Waal’s forces

Answer

Hydrogen bond formation

Question 49

49. Which of the following is a non-directional orbital

Question 50

50. Ionic radius in a period from left to right

Answer

First increases then decreases

Answer

First decreases then increases

Question 51

51. In which one of the following does the central atom not possess can octet in its outer shell?

Question 52

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

Question 53

53. The value of e/m ratio of electron is:

Answer

1.7588 x 10¹¹

Answer

6.02 x 10²³

Answer

9.1095 x 10¯³¹

Answer

1.7588 x 10²⁰

Question 54

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

Question 55

55. Which of the following is the correct electron – dot formula of CO₂?

Question 56

56. The velocity of photon is

Answer

Depends on its wavelength

Answer

Independent of its wavelength

Answer

Depends on its source

Answer

Equal to square

Question 57

57. Which of these molecules require more bond energy?

Question 58

58. Molecular orbital picture of N₂ indicates

Answer

Two unpaired electron

Answer

None of these

Answer

One unpaired electron

Answer

No unpaired electron

Question 59

59. Which of the following equation represents the 1^st ionization energy of Na?

Question 60

60. 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 61

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

Question 62

62. The electronegativity of elements in a period from left to right

Answer

First increases then decreases

Answer

First decreases then increases

Question 63

63. The third line of the Balmer series, in the emission spectrum of the hydrogen atom, is due to the transition from the

Answer

Fourth Bohr orbit to the first Bohr orbit

Answer

Sixth Bohr orbit to the third Bohr orbit

Answer

Fifth Bohr orbit to the second Bohr orbit

Answer

Seventh Bohr orbit to the third Bohr orbit

Question 64

64. When two hydrogen atoms approach to form a chemical bond

Answer

The repulsive force dominate the attractive forces

Answer

The two atoms start ionization

Answer

They energy of atoms increases

Answer

The attractive forces dominate the repulsive forces

Answer 126

2 electrons

Answer 127

6 electrons

Answer 128

1 electron

Answer 129

4 electrons

Answer 130

Impossible to predict

Answer 131

Tetrahedron

Answer 132

Ionization energy

Answer 133

None of these

Answer 134

Electron affinity

Answer 135

Electronegativity

Answer 136

Dispersion force

Answer 137

Dipole-dipole interaction

Answer 138

Ion-dipole interaction

Answer 139

Nuclei are unstable

Answer 140

Molecules are unstable

Answer 141

Molecules are stable

Answer 142

Nuclei are stable

Answer 143

Dipole moment is zero

Answer 144

Linear geometry

Answer 145

SP hybridization

Answer 146

It is always greater than 1st ionization energy

Answer 147

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

Answer 148

It is equal to the 1st ionization energy

Answer 149

It is always less than 1st ionization energy

Answer 150

Electron affinity

Answer 151

Ionization energy

Answer 152

None of these

Answer 153

Electro negativity

Answer 154

1/2 x ɜ₀

Answer 155

Remains constant

Answer 156

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

Answer 157

Blue has more energy

Answer 158

Blue is darker colour

Answer 159

Blue is absorbed more easily

Answer 160

Blue has higher wavelength

Answer 161

2.657 x 10¯²³ g

Answer 162

5.316 x 10¯²³ g

Answer 163

5.316 x 10¯²³ g

Answer 164

Tetrahedral

Answer 165

Trigonal bipyramidal

Answer 166

Octahedral

Answer 167

Liquid HCl

Answer 168

Liquid NH3

Answer 169

Both are equal

Answer 170

Cannot be determined

Answer 171

Van der Waal forces or London dispersion forces

Answer 172

Hydrogen bonds

Answer 173

All of these

Answer 174

Covalent forces

Answer 175

Hydrogen sulphide is a weak acid

Answer 176

Sulphure has high electronegativity than oxygen

Answer 177

Water has higher molecular weight

Answer 178

Water molecules associate through hydrogen bonding

Answer 179

Charged particles

Answer 180

Move with speed as that of light

Answer 181

Can be deflected by magnetic fields

Answer 182

A stream of electrons

Answer 183

Bond length in NO⁺ is greater than in NO

Answer 184

Bond length in NO⁺ is equal to that in NO

Answer 185

Bond length is unpredictable

Answer 186

Bond length in NO is greater than in NO⁺

Answer 187

One sigma, one pi

Answer 188

One sigma, two pi

Answer 189

Two sigma, two pi

Answer 190

Two sigma, one pi

Answer 191

They do not react with one another

Answer 192

They are mono atomic gases

Answer 193

They have completely filled s and p orbitals

Answer 194

They have high ionization energies

Answer 195

Electron affinity

Answer 196

None of these

Answer 197

Electro negativity

Answer 198

Ionization energy

Answer 199

Three unpaired electrons

Answer 200

Stability lower then O₂

Answer 201

Bond order of 2.5

Answer 202

Diamagnetic character

Answer 203

Variable trend

Answer 204

Square planar

Answer 205

Octahedral

Answer 206

Trigonal bipyramidal

Answer 207

1 bond pair 3 lone pair

Answer 208

2 bond pair 2 lone pair

Answer 209

3 lone pair 1 bond pair

Answer 210

3 bond pair one lone pair

Answer 211

always same irrespective of its hybrid state

Answer 212

sp³-hybridized carbon

Answer 213

sp²- hybridized carbon

Answer 214

sp- hybridized carbon

Answer 215

A pair of valence electrons

Answer 216

A pair of electrons

Answer 217

A pair of valence electrons not involved in bonding

Answer 218

A pair of electrons involved in bonding

Answer 219

4, 4, 0, ½

Answer 220

4, 1, 0, ½

Answer 221

4, 0, 0, ½

Answer 222

4, 1, 1, ½

Answer 223

Three pi-bonds

Answer 224

Three sigma bonds

Answer 225

Two sigma bonds and one pi-bond

Answer 226

One sigma bond and two pi-bonds

Answer 227

Sublimation of metallic sodium to give yellow vapour

Answer 228

Low ionization energy of sodium

Answer 229

Photosensitivity of sodium

Answer 230

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

Answer 231

H – NH₂

Answer 232

Shorter wavelength

Answer 233

Larger wavelength

Answer 234

X-rays not produced

Answer 235

Gamma rays

Answer 236

Metallic bond

Answer 237

Covalent bond

Answer 238

Van der Waal’s forces

Answer 239

Ionic bond

Answer 240

6.65 x 10¯³⁵ m

Answer 241

6.63 x 10¯³⁴ m

Answer 242

6.63 x 10¯³³ m

Answer 243

6.63 x 10¯³⁵ m

Answer 244

Lone pair – lone pair repulsion only

Answer 245

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

Answer 246

Bond pair – bond pair repulsion only

Answer 247

Lone pair – bond pair repulsion only

Answer 248

Equal to 1.7

Answer 249

No specificity exist

Answer 250

Greater than 1.7

Answer 251

Lesser then 1.7

Answer 252

Distorted tetrahedral

Answer 253

Planar triangle

Answer 254

Octahedral

Answer 255

10.2340178

Answer 256

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

Answer 257

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

Answer 258

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

Answer 259

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

Answer 260

Interaction

Answer 261

Attractive force

Answer 262

All of above represent same entity

Answer 263

High, very negative

Answer 264

Low, positive or slightly negative

Answer 265

Low very negative

Answer 266

None of these

Answer 267

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

Answer 268

Each bonding molecular orbital can accommodate only one electron

Answer 269

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

Answer 270

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

Answer 271

Ionic bond

Answer 272

Metallic bond

Answer 273

By gaining two electrons

Answer 274

By losing three electrons

Answer 275

By gaining three electrons

Answer 276

By losing two electrons

Answer 277

Tetrahedral

Answer 278

Trigonal bipyramidal

Answer 279

Square planar

Answer 280

Carbon dioxide

Answer 281

Carbon tetrachloride

Answer 282

Triangular bipyramidal

Answer 283

Triangular pyramidal

Answer 284

Triangular planar

Answer 285

Tetrahedral

Answer 286

Bonding will not occur

Answer 287

Orbital overlap will not occur

Answer 288

None of these

Answer 289

Both A and B are correct

Answer 290

Van der Waal’s force

Answer 291

Chemical bond

Answer 292

Dispersion force

Answer 293

London force

Answer 294

Tetrahedral

Answer 295

Square planner

Answer 296

Triangular

Answer 297

Non-polar solvents

Answer 298

Concentrated acids

Answer 299

Polar solvents

Answer 300

All solvents

Answer 301

There may be a possibility of a chemical reaction

Answer 302

Water should be preferred over lemon Juice for drinking

Answer 303

Lemon juice is dangerous for health

Answer 304

There may not be a possibility of chemical reaction

Answer 305

Ionization potential

Answer 306

Electronegativity

Answer 307

Electron affinity

Answer 308

Activation energy

Answer 309

Generally increases from left to right in a period

Answer 310

Does not change in a group

Answer 311

Increase from top to bottom in a group

Answer 312

Does not change in a period

Answer 313

Both polar covalent and hydrogen bonds

Answer 314

Nonpolar covalent bonds only

Answer 315

Ionic and nonpolar hydrogen bonds

Answer 316

Hydrogen bonds only

Answer 317

Trigonal bipyramidal

Answer 318

Multiplication of atomic orbitals

Answer 319

Subtraction of atomic orbitals

Answer 320

Addition of atomic orbitals

Answer 321

None of these

Answer 322

Electropositive character of elements

Answer 323

Electronegative character of elements

Answer 324

Octet rule

Answer 325

Pauli exclusion principle

Answer 326

Octet is complete

Answer 327

Electron rich

Answer 328

Electron deficient

Answer 329

No such acids exist

Answer 330

Impossible to predict

Answer 331

Lesser than individual

Answer 332

Higher than individual

Answer 333

Four p-orbitals are involved

Answer 334

One p-orbital is involved

Answer 335

One s and 3 p-orbitals are involved

Answer 336

All p-orbitals are involved

Answer 337

Radio, visible, infrared, ultraviolet

Answer 338

X – radiation, visible, infrared, microwave

Answer 339

Visible, ultraviolet, infrared, gamma rays

Answer 340

Microwave, infrared, visible, ultraviolet

Answer 341

Aufbau principal

Answer 342

Hund’s rule

Answer 343

Pauli’s exclusion principle

Total Questions:	187
Time Allowed:	60 Minutes
Total Marks:	187
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Important Chemistry Chemical Bonding Question and Answer

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