Chemistry Chemical Bonding Online Mcqs Test

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Question 1

1. According to VSEPR theory, the shape of the water molecule is

Answer

Planar triangle

Answer

Distorted tetrahedral

Answer

Octahedral

Question 2

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

Answer

Bonding molecular orbitals have low electron density between the two nuclei

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 possess less energy than atomic orbitals from which they are formed

Question 3

3. Shape of CIO₃¯ is

Answer

Triangular bipyramidal

Answer

Tetrahedral

Answer

Triangular pyramidal

Answer

Triangular planar

Question 4

4. Which of the following has maximum e/m value for positive rays?

Question 5

5. According to MO theory, the species O⁺₂ possesses

Answer

Diamagnetic character

Answer

Three unpaired electrons

Answer

Bond order of 2.5

Answer

Stability lower then O₂

Question 6

6. A lone pair of electrons in an atom implies

Answer

A pair of electrons involved in bonding

Answer

A pair of valence electrons

Answer

A pair of valence electrons not involved in bonding

Answer

A pair of electrons

Question 7

7. Choose the correct statement about 2nd ionization energy

Answer

It is always greater than 1st ionization energy

Answer

It is equal to the 1st ionization energy

Answer

It is always less than 1st ionization energy

Answer

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

Question 8

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

Answer

Remain same

Question 9

9. Geometry of molecule will be pyramidal if the outer post shell of the central atom has

Answer

2 bond pair 2 lone pair

Answer

3 bond pair one lone pair

Answer

1 bond pair 3 lone pair

Answer

3 lone pair 1 bond pair

Question 10

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

Question 11

11. Quantum umber values for 2p orbitals are

Answer

n = 1, l = 2

Answer

n = 1, l = 0

Answer

n = 2, l = 1

Answer

n = 2, l = 0

Question 12

12. Which of the following has more unpaired d-electrons?

Question 13

13. An oxygen atom has mass of

Answer

5.316 x 10¯²³ g

Answer

5.316 x 10¯²³ g

Answer

2.657 x 10¯²³ g

Question 14

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

Question 15

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

Question 16

16. The bond angle H – O – H in ice is closest to

Question 17

17. When potassium metal is exposed to violet light

Answer

There is no effect

Answer

The absorption of electrons takes place

Answer

Ejection of some potassium atoms occurs

Answer

Ejection of electrons takes place

Question 18

18. Fluorine has an atomic number 9 and Chlorine has 17. Which one has the highest electron affinity?

Answer

Both are equal

Answer

Cannot be determined

Question 19

19. Which one shows high % age of the ionic character?

Question 20

20. The ionization energy

Answer

Increase from top to bottom in a group

Answer

Generally increases from left to right in a period

Answer

Does not change in a period

Answer

Does not change in a group

Question 21

21. Energy of an atom in a compound is

Answer

Impossible to predict

Answer

Higher than individual

Answer

Lesser than individual

Question 22

22. The number of significant figures in 0.00200 is

Question 23

23. Atom with higher atomic number produces X-rays of

Answer

X-rays not produced

Answer

Gamma rays

Answer

Larger wavelength

Answer

Shorter wavelength

Question 24

24. Which of the following element’s outermost orbits last electron has magnetic quantum number m = 0?

Question 25

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

Answer

Ionization energy

Answer

Atomic size

Answer

Electron affinity

Answer

Electronegativity

Question 26

26. The carbon atoms in calcium carbide are held by

Answer

Ionic bonds

Answer

2π and one σ bond

Answer

2 sigma bonds

Answer

2 covalent, one co-ordinate bond

Question 27

27. The four quantum numbers of the valency electron of potassium are

Answer

4, 4, 0, ½

Answer

4, 1, 0, ½

Answer

4, 0, 0, ½

Answer

4, 1, 1, ½

Question 28

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

Question 29

29. A chemist poured juice on soil. Which idea may he have in his mind?

Answer

Water should be preferred over lemon Juice for drinking

Answer

Lemon juice is dangerous for health

Answer

There may be a possibility of a chemical reaction

Answer

There may not be a possibility of chemical reaction

Question 30

30. Water (H₂O) is liquid while hydrogen sulphide (H₂O) is a gas because

Answer

Water molecules associate through hydrogen bonding

Answer

Water has higher molecular weight

Answer

Hydrogen sulphide is a weak acid

Answer

Sulphure has high electronegativity than oxygen

Question 31

31. The spectrum of helium is expected to be similar to that of

Question 32

32. XeF₄ has shape of

Answer

Trigonal bipyramidal

Answer

Square planar

Answer

Tetrahedral

Question 33

33. For principle quantum number, n = 4, the total number of orbitals having 1 = 3 is

Question 34

34. H-bonding is not present in

Answer

Hydrogen fluoride

Answer

Hydrogen sulphide

Question 35

35. Covalent compounds are soluble in

Answer

Non-polar solvents

Answer

All solvents

Answer

Concentrated acids

Answer

Polar solvents

Question 36

36. Molecular orbitals are filled according to

Answer

Pauli’s exclusion principle

Answer

Aufbau principal

Answer

Hund’s rule

Question 37

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

Answer

Triangular

Answer

Tetrahedral

Question 38

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

Question 39

39. Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers l = 1 and l = 2 are respectively

Question 40

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

Question 41

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

Question 42

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

Answer

One sigma, two pi

Answer

Two sigma, one pi

Answer

Two sigma, two pi

Answer

One sigma, one pi

Question 43

43. ____________ has their outermost shell complete in atomic form

Answer

Coinage metals

Answer

Gun metals

Answer

Alkali metals

Answer

Noble gases

Question 44

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

Answer

No specificity exist

Answer

Equal to 1.7

Answer

Greater than 1.7

Answer

Lesser then 1.7

Question 45

45. Unit of dipole moment is

Question 46

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

Question 47

47. Geometry of simple molecule having SP³ hybrid orbital is

Answer

Square planner

Answer

Triangular

Answer

Tetrahedral

Question 48

48. 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

Fifth Bohr orbit to the second Bohr orbit

Answer

Seventh Bohr orbit to the third Bohr orbit

Answer

Sixth Bohr orbit to the third Bohr orbit

Question 49

49. The velocity of photon is

Answer

Depends on its source

Answer

Equal to square

Answer

Depends on its wavelength

Answer

Independent of its wavelength

Question 50

50. In which of the following pairs, the numbers of electrons in the outermost shell are different?

Question 51

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

Question 52

52. Among the alkaline earth metals the element forming predominantly covalent compounds is

Question 53

53. Number of sigma bonds in P₄O₁₀ is

Question 54

54. In BrF₃ molecule, the lone pairs occupy equatorial positions to minimize

Answer

Bond pair – bond pair repulsion only

Answer

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

Answer

Lone pair – lone pair repulsion only

Answer

Lone pair – bond pair repulsion only

Question 55

55. If the radius of first Bohr orbit be ɜ₀, then the radius of third Bohr orbit would be

Answer

1/2 x ɜ₀

Question 56

56. Which of the bonds, shown by the ___________ has the greatest polarity?

Answer

H – NH₂

Question 57

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

Question 58

58. Effective magnetic moment of Sc³ ion is

Question 59

59. Which of the following is not isoelectronic?

Question 60

60. Elements with ________ first ionization energies and ________ electron affinities generally from cations. Choose the correct point

Answer

Low very negative

Answer

Low, positive or slightly negative

Answer

High, very negative

Answer

None of these

Question 61

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

Question 62

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

Question 63

63. Which one of these is weakest?

Answer

Metallic bond

Answer

Covalent bond

Answer

Ionic bond

Answer

Van der Waal’s forces

Question 64

64. Energy released or absorbed when electrons are added in atom is

Answer

Ionization potential

Answer

Activation energy

Answer

Electron affinity

Answer

Electronegativity

Answer 128

1.7588 x 10²⁰

Answer 129

1.7588 x 10¹¹

Answer 130

9.1095 x 10¯³¹

Answer 131

6.02 x 10²³

Answer 132

Double bond

Answer 133

Covalent bond

Answer 134

Co-ordinate bond

Answer 135

Electrovalent bond

Answer 136

A stream of electrons

Answer 137

Can be deflected by magnetic fields

Answer 138

Move with speed as that of light

Answer 139

Charged particles

Answer 140

Interaction

Answer 141

Attractive force

Answer 142

All of above represent same entity

Answer 143

Planar triangle

Answer 144

Square planar

Answer 145

Tetrahedral

Answer 146

First decreases then increases

Answer 147

Electron affinity

Answer 148

None of these

Answer 149

Electronegativity

Answer 150

Ionization energy

Answer 151

NH₃ is pyramidal in shape while BF₃ is planar

Answer 152

Boron trifluoride is pyramidal in shape while NH₃ is planar

Answer 153

Fluorides are more electronegative

Answer 154

Fluorides is more electronegative

Answer 155

Five π and nine σ

Answer 156

Eight σ and eight π

Answer 157

Nine σ and seven π

Answer 158

Nine σ and nine π

Answer 159

London force

Answer 160

Dispersion force

Answer 161

Chemical bond

Answer 162

Van der Waal’s force

Answer 163

Triangular planar

Answer 164

Tetrahedral

Answer 165

Blue is absorbed more easily

Answer 166

Blue has higher wavelength

Answer 167

Blue is darker colour

Answer 168

Blue has more energy

Answer 169

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

Answer 170

It has high heat of dissociation

Answer 171

It has high electronegativity

Answer 172

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

Answer 173

6.02 x 10¹⁶ J/mol

Answer 174

10¯⁷ J/mol

Answer 175

6.02 x 10²³ J/mol

Answer 176

Impossible to predict

Answer 177

The repulsive force dominate the attractive forces

Answer 178

They energy of atoms increases

Answer 179

The two atoms start ionization

Answer 180

The attractive forces dominate the repulsive forces

Answer 181

Octahedral

Answer 182

Trigonal bipyramidal

Answer 183

Triangular

Answer 184

Square planner

Answer 185

Bond length in NO⁺ is greater than in NO

Answer 186

Bond length in NO is greater than in NO⁺

Answer 187

Bond length in NO⁺ is equal to that in NO

Answer 188

Bond length is unpredictable

Answer 189

Square planner

Answer 190

Triangular

Answer 191

Tetrahedral

Answer 192

Excited state of fluorine

Answer 193

Ground state of fluorine atom

Answer 194

Excited state of O¯₂

Answer 195

Excited state of neon

Answer 196

sp² hybrid orbitals

Answer 197

p orbitals

Answer 198

s orbitals

Answer 199

sp³ hybrid orbitals

Answer 200

2 electrons

Answer 201

1 electron

Answer 202

4 electrons

Answer 203

6 electrons

Answer 204

First decreases then increases

Answer 205

First increases then decreases

Answer 206

None of these

Answer 207

Addition of atomic orbitals

Answer 208

Subtraction of atomic orbitals

Answer 209

Multiplication of atomic orbitals

Answer 210

Dipole moment is zero

Answer 211

Linear geometry

Answer 212

SP hybridization

Answer 213

Octet rule

Answer 214

Pauli exclusion principle

Answer 215

Electronegative character of elements

Answer 216

Electropositive character of elements

Answer 217

Carbon tetrachloride

Answer 218

Carbon dioxide

Answer 219

Tetrahedron

Answer 220

One unpaired electron

Answer 221

No unpaired electron

Answer 222

Two unpaired electron

Answer 223

None of these

Answer 224

Trigonal bipyramidal

Answer 225

Tetrahedral

Answer 226

Octahedral

Answer 227

Liquid NH3

Answer 228

Liquid HCl

Answer 229

Nuclei are stable

Answer 230

Molecules are stable

Answer 231

Nuclei are unstable

Answer 232

Molecules are unstable

Answer 233

X – radiation, visible, infrared, microwave

Answer 234

Visible, ultraviolet, infrared, gamma rays

Answer 235

Radio, visible, infrared, ultraviolet

Answer 236

Microwave, infrared, visible, ultraviolet

Answer 237

always same irrespective of its hybrid state

Answer 238

sp- hybridized carbon

Answer 239

sp²- hybridized carbon

Answer 240

sp³-hybridized carbon

Answer 241

Electro negativity

Answer 242

None of these

Answer 243

Ionization energy

Answer 244

Electron affinity

Answer 245

Variable trend

Answer 246

By gaining two electrons

Answer 247

By losing two electrons

Answer 248

By gaining three electrons

Answer 249

By losing three electrons

Answer 250

Low ionization energy of sodium

Answer 251

Sublimation of metallic sodium to give yellow vapour

Answer 252

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

Answer 253

Photosensitivity of sodium

Answer 254

Hybrid and un hybrid orbitals

Answer 255

Un-hybrid orbitals

Answer 256

Atomic orbital and hybrid orbital

Answer 257

Hybrid orbitals

Answer 258

Heisenberg’s uncertainty principle

Answer 259

Quarternization of energy of electrons

Answer 260

Quarternization of angular members

Answer 261

Plank’s quantum theory

Answer 262

Colour spectrum

Answer 263

Vaporization

Answer 264

Crystallization

Answer 265

Distillation

Answer 266

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

Answer 267

Remains constant

Answer 268

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

Answer 269

Each bonding molecular orbital can accommodate only one electron

Answer 270

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

Answer 271

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

Answer 272

10.2340178

Answer 273

Van der Waal’s forces

Answer 274

Covalent attraction

Answer 275

Dipole interaction

Answer 276

Hydrogen bond formation

Answer 277

First increases then decreases

Answer 278

First decreases then increases

Answer 279

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

Answer 280

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

Answer 281

Depends on the pressure in the discharge tube

Answer 282

Depends on the gas used in the discharge tube

Answer 283

Trigonal bipyramidal

Answer 284

Octahedral

Answer 285

Square planar

Answer 286

One s and 3 p-orbitals are involved

Answer 287

Four p-orbitals are involved

Answer 288

One p-orbital is involved

Answer 289

All p-orbitals are involved

Answer 290

Covalent forces

Answer 291

Van der Waal forces or London dispersion forces

Answer 292

Hydrogen bonds

Answer 293

All of these

Answer 294

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

Answer 295

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

Answer 296

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

Answer 297

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

Answer 298

Dipole-dipole interaction

Answer 299

Dispersion force

Answer 300

Ion-dipole interaction

Answer 301

They do not react with one another

Answer 302

They are mono atomic gases

Answer 303

They have high ionization energies

Answer 304

They have completely filled s and p orbitals

Answer 305

Electron affinity

Answer 306

Electro negativity

Answer 307

Ionization energy

Answer 308

None of these

Answer 309

The axial s-p overlap

Answer 310

The sidewise p-p overlap

Answer 311

The overlap of two sp² hybrid orbitals

Answer 312

The axial p-p overlap

Answer 313

All of these

Answer 314

The nature of residual gas

Answer 315

The nature of electrode

Answer 316

The nature of discharge tube

Answer 317

6.65 x 10¯³⁵ m

Answer 318

6.63 x 10¯³⁵ m

Answer 319

6.63 x 10¯³³ m

Answer 320

6.63 x 10¯³⁴ m

Answer 321

Trigonal bipyramidal

Answer 322

Both polar covalent and hydrogen bonds

Answer 323

Ionic and nonpolar hydrogen bonds

Answer 324

Hydrogen bonds only

Answer 325

Nonpolar covalent bonds only

Answer 326

Both A and B are correct

Answer 327

Orbital overlap will not occur

Answer 328

Bonding will not occur

Answer 329

None of these

Answer 330

One sigma bond and two pi-bonds

Answer 331

Three sigma bonds

Answer 332

Two sigma bonds and one pi-bond

Answer 333

Three pi-bonds

Answer 334

They are smaller than the atoms from which they were formed

Answer 335

They are formed when electros are formed from atoms

Answer 336

They are also known as cations

Answer 337

They are larger than the atoms from which they were formed

Answer 338

Ionic bond

Answer 339

Metallic bond

Answer 340

Electron rich

Answer 341

No such acids exist

Answer 342

Electron deficient

Answer 343

Octet is complete

Total Questions:	187
Time Allowed:	60 Minutes
Total Marks:	187
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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