Chemistry Chemical Bonding Online Mcqs Test

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Question 1

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

Question 2

2. Lateral overlapping expected in

Answer

Metallic bond

Answer

Ionic bond

Question 3

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

Answer

Trigonal bipyramidal

Answer

Octahedral

Answer

Square planner

Answer

Triangular

Question 4

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

Question 5

5. 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 6

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

Question 7

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

Answer

Impossible to predict

Question 8

8. Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to the highest energy

Answer

Radio, visible, infrared, ultraviolet

Answer

Microwave, infrared, visible, ultraviolet

Answer

X – radiation, visible, infrared, microwave

Answer

Visible, ultraviolet, infrared, gamma rays

Question 9

9. Unit of dipole moment is

Question 10

10. Bond order for N2 molecule is

Question 11

11. A long a period E.N __________ from left to right

Answer

Variable trend

Question 12

12. ____________ has their outermost shell complete in atomic form

Answer

Gun metals

Answer

Noble gases

Answer

Alkali metals

Answer

Coinage metals

Question 13

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

Answer

Hydrogen bonds only

Answer

Ionic and nonpolar hydrogen bonds

Answer

Both polar covalent and hydrogen bonds

Answer

Nonpolar covalent bonds only

Question 14

14. H-bonding is not present in

Answer

Hydrogen sulphide

Answer

Hydrogen fluoride

Question 15

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

Answer

They have completely filled s and p orbitals

Answer

They have high ionization energies

Answer

They are mono atomic gases

Answer

They do not react with one another

Question 16

16. The structure of ICl₂¯ is

Answer

Square planar

Answer

Trigonal bipyramidal

Answer

Octahedral

Question 17

17. The central atom in BrF₅ has _?_ bonding pairs of electrons and _?_ non-bonding pairs of electrons.

Question 18

18. 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 19

19. The carbon atoms in calcium carbide are held by

Answer

Ionic bonds

Answer

2 covalent, one co-ordinate bond

Answer

2π and one σ bond

Answer

2 sigma bonds

Question 20

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

Answer

Planar triangle

Answer

Tetrahedral

Answer

Square planar

Question 21

21. Find the magnetic moment of a divalent ion in aqueous solution if its atomic number is 25

Question 22

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

Answer

Distorted tetrahedral

Answer

Octahedral

Answer

Planar triangle

Question 23

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

Question 24

24. Which one of the following molecules shows high percentage of ionic character?

Question 25

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

Question 26

26. The number of d-electrons retained in Fe²⁺ (At. No. of Fe = 26) ions is

Question 27

27. Maximum hydrogen bonds in water are,

Question 28

28. Which of the following molecule has Ā bond

Question 29

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

Answer

Lone pair – bond pair repulsion only

Answer

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

Answer

Bond pair – bond pair repulsion only

Answer

Lone pair – lone pair repulsion only

Question 30

30. Which has the minimum bond angle?

Question 31

31. XeF₄ has shape of

Answer

Tetrahedral

Answer

Trigonal bipyramidal

Answer

Square planar

Question 32

32. Pick out the molecule which has zero dipole moment

Question 33

33. On sp3 hybridization

Answer

All p-orbitals are involved

Answer

One p-orbital is involved

Answer

Four p-orbitals are involved

Answer

One s and 3 p-orbitals are involved

Question 34

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

Answer

Seventh Bohr orbit to the third Bohr orbit

Answer

Fifth Bohr orbit to the second Bohr orbit

Answer

Fourth Bohr orbit to the first Bohr orbit

Answer

Sixth Bohr orbit to the third Bohr orbit

Question 35

35. Effective magnetic moment of Sc³ ion is

Question 36

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

Question 37

37. Which of the following will have highest value of electron affinity

Question 38

38. Which of the following is not isoelectronic?

Question 39

39. The ionization energy

Answer

Does not change in a group

Answer

Generally increases from left to right in a period

Answer

Increase from top to bottom in a group

Answer

Does not change in a period

Question 40

40. Ionic radius in a period from left to right

Answer

First increases then decreases

Answer

First decreases then increases

Question 41

41. Al become isoelectronic with Ne

Answer

By losing two electrons

Answer

By gaining three electrons

Answer

By gaining two electrons

Answer

By losing three electrons

Question 42

42. Molecular orbital picture of N₂ indicates

Answer

One unpaired electron

Answer

No unpaired electron

Answer

None of these

Answer

Two unpaired electron

Question 43

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

Question 44

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

Answer

None of these

Answer

Electro negativity

Answer

Ionization energy

Answer

Electron affinity

Question 45

45. The bond order in NO is 2.5 while that is NO⁺ is 3. Which of the following statements is true for these two species?

Answer

Bond length is unpredictable

Answer

Bond length in NO⁺ is greater than in NO

Answer

Bond length in NO is greater than in NO⁺

Answer

Bond length in NO⁺ is equal to that in NO

Question 46

46. Which of these molecules require more bond energy?

Question 47

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

Answer

Move with speed as that of light

Answer

A stream of electrons

Answer

Charged particles

Answer

Can be deflected by magnetic fields

Question 48

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

Answer

High, very negative

Answer

Low very negative

Answer

None of these

Answer

Low, positive or slightly negative

Question 49

49. 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

Dipole interaction

Answer

Covalent attraction

Answer

Hydrogen bond formation

Answer

Van der Waal’s forces

Question 50

50. Choose the correct statement

Answer

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

Answer

Each bonding molecular orbital can accommodate only one electron

Answer

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

Answer

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

Question 51

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

Question 52

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

Question 53

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

Answer

None of these

Answer

Electronegativity

Answer

Ionization energy

Answer

Electron affinity

Question 54

54. The total number of possible values of magnetic quantum number for the value of l = 3 is

Question 55

55. Which of the following geometry is associated with the compound in which the central atom assumes sp³ d hybridization?

Answer

Trigonal bipyramidal

Question 56

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

Answer

H – NH₂

Question 57

57. Which of the following phenomena will occur when two atoms of the elements having same spin of electron approach for bonding?

Answer

None of these

Answer

Orbital overlap will not occur

Answer

Both A and B are correct

Answer

Bonding will not occur

Question 58

58. Fluorine molecule is formed by

Answer

The axial s-p overlap

Answer

The overlap of two sp² hybrid orbitals

Answer

The axial p-p overlap

Answer

The sidewise p-p overlap

Question 59

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

Answer

Tetrahedral

Answer

Triangular

Question 60

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

Question 61

61. In CCl₄, the four valencies of carbon are directed towards the corners of a

Answer

Tetrahedron

Question 62

62. Which carbon is more electronegative?

Answer

always same irrespective of its hybrid state

Answer

sp²- hybridized carbon

Answer

sp³-hybridized carbon

Answer

sp- hybridized carbon

Question 63

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

Answer

Remain same

Question 64

64. Bohr’s model atom is contradicted by

Answer

Quarternization of angular members

Answer

Heisenberg’s uncertainty principle

Answer

Quarternization of energy of electrons

Answer

Plank’s quantum theory

Answer 121

Covalent bond

Answer 122

Metallic bond

Answer 123

Van der Waal’s forces

Answer 124

Ionic bond

Answer 125

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

Answer 126

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

Answer 127

It has high electronegativity

Answer 128

It has high heat of dissociation

Answer 129

Shorter wavelength

Answer 130

X-rays not produced

Answer 131

Gamma rays

Answer 132

Larger wavelength

Answer 133

2.657 x 10¯²³ g

Answer 134

5.316 x 10¯²³ g

Answer 135

5.316 x 10¯²³ g

Answer 136

6.63 x 10¯³⁴ m

Answer 137

6.65 x 10¯³⁵ m

Answer 138

6.63 x 10¯³⁵ m

Answer 139

6.63 x 10¯³³ m

Answer 140

Carbon tetrachloride

Answer 141

Carbon dioxide

Answer 142

Van der Waal forces or London dispersion forces

Answer 143

Hydrogen bonds

Answer 144

All of these

Answer 145

Covalent forces

Answer 146

Triangular planar

Answer 147

Triangular bipyramidal

Answer 148

Triangular pyramidal

Answer 149

Tetrahedral

Answer 150

Activation energy

Answer 151

Ionization potential

Answer 152

Electronegativity

Answer 153

Electron affinity

Answer 154

1/2 x ɜ₀

Answer 155

10.2340178

Answer 156

Triangular planar

Answer 157

Tetrahedral

Answer 158

Electron deficient

Answer 159

Octet is complete

Answer 160

No such acids exist

Answer 161

Electron rich

Answer 162

Dispersion force

Answer 163

Ion-dipole interaction

Answer 164

Dipole-dipole interaction

Answer 165

Lesser than individual

Answer 166

Impossible to predict

Answer 167

Higher than individual

Answer 168

Ground state of fluorine atom

Answer 169

Excited state of O¯₂

Answer 170

Excited state of neon

Answer 171

Excited state of fluorine

Answer 172

None of these

Answer 173

Electron affinity

Answer 174

Electro negativity

Answer 175

Ionization energy

Answer 176

First decreases then increases

Answer 177

4, 1, 0, ½

Answer 178

4, 0, 0, ½

Answer 179

4, 4, 0, ½

Answer 180

4, 1, 1, ½

Answer 181

Colour spectrum

Answer 182

Distillation

Answer 183

Vaporization

Answer 184

Crystallization

Answer 185

Liquid HCl

Answer 186

Liquid NH3

Answer 187

All of these

Answer 188

The nature of residual gas

Answer 189

The nature of discharge tube

Answer 190

The nature of electrode

Answer 191

Ionization energy

Answer 192

Atomic size

Answer 193

Electronegativity

Answer 194

Electron affinity

Answer 195

Tetrahedral

Answer 196

Triangular

Answer 197

Square planner

Answer 198

Equal to 1.7

Answer 199

No specificity exist

Answer 200

Greater than 1.7

Answer 201

Lesser then 1.7

Answer 202

Molecules are unstable

Answer 203

Molecules are stable

Answer 204

Nuclei are unstable

Answer 205

Nuclei are stable

Answer 206

Bond order of 2.5

Answer 207

Diamagnetic character

Answer 208

Three unpaired electrons

Answer 209

Stability lower then O₂

Answer 210

Water should be preferred over lemon Juice for drinking

Answer 211

There may not be a possibility of chemical reaction

Answer 212

There may be a possibility of a chemical reaction

Answer 213

Lemon juice is dangerous for health

Answer 214

Fluorides is more electronegative

Answer 215

NH₃ is pyramidal in shape while BF₃ is planar

Answer 216

Boron trifluoride is pyramidal in shape while NH₃ is planar

Answer 217

Fluorides are more electronegative

Answer 218

Aufbau principal

Answer 219

Pauli’s exclusion principle

Answer 220

Hund’s rule

Answer 221

2 electrons

Answer 222

4 electrons

Answer 223

6 electrons

Answer 224

1 electron

Answer 225

One sigma, two pi

Answer 226

One sigma, one pi

Answer 227

Two sigma, two pi

Answer 228

Two sigma, one pi

Answer 229

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

Answer 230

Low ionization energy of sodium

Answer 231

Sublimation of metallic sodium to give yellow vapour

Answer 232

Photosensitivity of sodium

Answer 233

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

Answer 234

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

Answer 235

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

Answer 236

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

Answer 237

Blue has more energy

Answer 238

Blue has higher wavelength

Answer 239

Blue is darker colour

Answer 240

Blue is absorbed more easily

Answer 241

Three pi-bonds

Answer 242

Three sigma bonds

Answer 243

Two sigma bonds and one pi-bond

Answer 244

One sigma bond and two pi-bonds

Answer 245

Cannot be determined

Answer 246

Both are equal

Answer 247

Triangular

Answer 248

Square planner

Answer 249

Tetrahedral

Answer 250

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

Answer 251

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

Answer 252

Depends on the pressure in the discharge tube

Answer 253

Depends on the gas used in the discharge tube

Answer 254

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

Answer 255

It is always less than 1st ionization energy

Answer 256

It is always greater than 1st ionization energy

Answer 257

It is equal to the 1st ionization energy

Answer 258

10¯⁷ J/mol

Answer 259

6.02 x 10²³ J/mol

Answer 260

6.02 x 10¹⁶ J/mol

Answer 261

Electronegative character of elements

Answer 262

Pauli exclusion principle

Answer 263

Octet rule

Answer 264

Electropositive character of elements

Answer 265

1.7588 x 10²⁰

Answer 266

9.1095 x 10¯³¹

Answer 267

6.02 x 10²³

Answer 268

1.7588 x 10¹¹

Answer 269

A pair of valence electrons not involved in bonding

Answer 270

A pair of electrons involved in bonding

Answer 271

A pair of valence electrons

Answer 272

A pair of electrons

Answer 273

Atomic orbital and hybrid orbital

Answer 274

Hybrid and un hybrid orbitals

Answer 275

Hybrid orbitals

Answer 276

Un-hybrid orbitals

Answer 277

First increases then decreases

Answer 278

First decreases then increases

Answer 279

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

Answer 280

Bonding molecular orbitals have low electron density between the two nuclei

Answer 281

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

Answer 282

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

Answer 283

Ejection of some potassium atoms occurs

Answer 284

The absorption of electrons takes place

Answer 285

Ejection of electrons takes place

Answer 286

There is no effect

Answer 287

Depends on its source

Answer 288

Depends on its wavelength

Answer 289

Independent of its wavelength

Answer 290

Equal to square

Answer 291

Subtraction of atomic orbitals

Answer 292

None of these

Answer 293

Addition of atomic orbitals

Answer 294

Multiplication of atomic orbitals

Answer 295

sp³ hybrid orbitals

Answer 296

sp² hybrid orbitals

Answer 297

p orbitals

Answer 298

s orbitals

Answer 299

Interaction

Answer 300

Attractive force

Answer 301

All of above represent same entity

Answer 302

Dispersion force

Answer 303

Chemical bond

Answer 304

Van der Waal’s force

Answer 305

London force

Answer 306

Nine σ and nine π

Answer 307

Nine σ and seven π

Answer 308

Five π and nine σ

Answer 309

Eight σ and eight π

Answer 310

n = 2, l = 1

Answer 311

n = 2, l = 0

Answer 312

n = 1, l = 0

Answer 313

n = 1, l = 2

Answer 314

Water has higher molecular weight

Answer 315

Sulphure has high electronegativity than oxygen

Answer 316

Hydrogen sulphide is a weak acid

Answer 317

Water molecules associate through hydrogen bonding

Answer 318

Double bond

Answer 319

Electrovalent bond

Answer 320

Co-ordinate bond

Answer 321

Covalent bond

Answer 322

Dipole moment is zero

Answer 323

Linear geometry

Answer 324

SP hybridization

Answer 325

They energy of atoms increases

Answer 326

The two atoms start ionization

Answer 327

The repulsive force dominate the attractive forces

Answer 328

The attractive forces dominate the repulsive forces

Answer 329

They are smaller than the atoms from which they were formed

Answer 330

They are larger than the atoms from which they were formed

Answer 331

They are also known as cations

Answer 332

They are formed when electros are formed from atoms

Answer 333

Tetrahedral

Answer 334

Octahedral

Answer 335

Trigonal bipyramidal

Answer 336

3 bond pair one lone pair

Answer 337

1 bond pair 3 lone pair

Answer 338

2 bond pair 2 lone pair

Answer 339

3 lone pair 1 bond pair

Answer 340

Concentrated acids

Answer 341

Polar solvents

Answer 342

All solvents

Answer 343

Non-polar solvents

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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