Chemistry Chemical Bonding Online Mcqs Test

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Question 1

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

Answer

Microwave, infrared, visible, ultraviolet

Answer

Radio, visible, infrared, ultraviolet

Answer

X – radiation, visible, infrared, microwave

Answer

Visible, ultraviolet, infrared, gamma rays

Question 2

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

Answer

Remain same

Question 3

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

Answer

None of these

Answer

Electron affinity

Answer

Electro negativity

Answer

Ionization energy

Question 4

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

Answer

Move with speed as that of light

Answer

Can be deflected by magnetic fields

Answer

Charged particles

Answer

A stream of electrons

Question 5

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

Answer

First decreases then increases

Answer

First increases then decreases

Question 6

6. The carbon atoms in calcium carbide are held by

Answer

Ionic bonds

Answer

2π and one σ bond

Answer

2 covalent, one co-ordinate bond

Answer

2 sigma bonds

Question 7

7. The boiling point of heavy water is

Question 8

8. Which of the following is not isoelectronic?

Question 9

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

Question 10

10. 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 11

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

Answer

Trigonal bipyramidal

Question 12

12. Which of the following is a non-directional orbital?

Question 13

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

Answer

They are smaller than the atoms from which they were formed

Answer

They are larger than the atoms from which they were formed

Answer

They are also known as cations

Answer

They are formed when electros are formed from atoms

Question 14

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

Question 15

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

Answer

Boron trifluoride is pyramidal in shape while NH₃ is planar

Answer

NH₃ is pyramidal in shape while BF₃ is planar

Answer

Fluorides is more electronegative

Answer

Fluorides are more electronegative

Question 16

16. Number of π-bonds in naphthalene is

Question 17

17. Pick out the molecule which has zero dipole moment

Question 18

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

Question 19

19. 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 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

Question 20

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

Question 21

21. 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

s orbitals

Answer

sp³ hybrid orbitals

Answer

p orbitals

Answer

sp² hybrid orbitals

Question 22

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

Question 23

23. Unit of dipole moment is

Question 24

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

Answer

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

Answer

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

Answer

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

Answer

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

Question 25

25. 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 26

26. Along a period the atomic radii

Answer

First decreases then increases

Question 27

27. XeF₄ has shape of

Answer

Tetrahedral

Answer

Trigonal bipyramidal

Answer

Square planar

Question 28

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

Answer

Bond pair – bond pair repulsion only

Answer

Lone pair – bond pair repulsion only

Answer

Lone pair – lone pair repulsion only

Answer

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

Question 29

29. Energy of an atom in a compound is

Answer

Lesser than individual

Answer

Higher than individual

Answer

Impossible to predict

Question 30

30. Unit of dipole moment is

Question 31

31. Covalent compounds are soluble in

Answer

All solvents

Answer

Non-polar solvents

Answer

Concentrated acids

Answer

Polar solvents

Question 32

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

Answer

One sigma, one pi

Answer

Two sigma, one pi

Answer

Two sigma, two pi

Answer

One sigma, two pi

Question 33

33. 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 34

34. Which hydrogen halide among the following has the highest percentage of ionic character?

Question 35

35. The shape of the molecule SF₂Cl₂ is

Answer

Octahedral

Answer

Trigonal bipyramidal

Answer

Tetrahedral

Question 36

36. Ionic radius in a period from left to right

Answer

First decreases then increases

Answer

First increases then decreases

Question 37

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

Answer

Octahedral

Answer

Planar triangle

Answer

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

Answer

1.7588 x 10¹¹

Answer

1.7588 x 10²⁰

Answer

9.1095 x 10¯³¹

Answer

6.02 x 10²³

Question 40

40. H-bonding is not present in

Answer

Hydrogen sulphide

Answer

Hydrogen fluoride

Question 41

41. Which of the following is the best explanation that CO₂ is a non-polar molecule?

Answer

SP hybridization

Answer

Linear geometry

Answer

Dipole moment is zero

Question 42

42. 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 electrons

Answer

A pair of valence electrons not involved in bonding

Question 43

43. In acetylene molecule, the two carbon atoms are linked by

Answer

Three pi-bonds

Answer

Two sigma bonds and one pi-bond

Answer

Three sigma bonds

Answer

One sigma bond and two pi-bonds

Question 44

44. Maximum hydrogen bonds in water are,

Question 45

45. The number of significant figures in 0.00200 is

Question 46

46. Which of these molecules require more bond energy?

Question 47

47. If the value of principal quantum number is 3, the total possible values for magnetic quantum number will be

Question 48

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

Question 49

49. Lewis acids are

Answer

Electron deficient

Answer

Electron rich

Answer

Octet is complete

Answer

No such acids exist

Question 50

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

Question 51

51. Which of the following has unchanged valency?

Question 52

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

Answer

None of these

Answer

Ionization energy

Answer

Electronegativity

Answer

Electron affinity

Question 53

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

Question 54

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

Answer

H – NH₂

Question 55

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

Answer

Ionization energy

Answer

Electronegativity

Answer

Electron affinity

Answer

Atomic size

Question 56

56. Sodium chloride imparts a yellow colour to the Bunsen flame. This can be interpreted due to the

Answer

Low ionization energy of sodium

Answer

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

Answer

Photosensitivity of sodium

Answer

Sublimation of metallic sodium to give yellow vapour

Question 57

57. Molecular orbitals are filled according to

Answer

Aufbau principal

Answer

Pauli’s exclusion principle

Answer

Hund’s rule

Question 58

58. Deflection of blue light is lesser than violet because

Answer

Blue is darker colour

Answer

Blue has more energy

Answer

Blue has higher wavelength

Answer

Blue is absorbed more easily

Question 59

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

Question 60

60. Inter molecular forces in solid hydrogen are

Answer

Hydrogen bonds

Answer

Van der Waal forces or London dispersion forces

Answer

All of these

Answer

Covalent forces

Question 61

61. The ionization energy

Answer

Does not change in a group

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

Question 62

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

Question 63

63. Bond order for N2 molecule is

Question 64

64. Which of the following species has lone pair of electrons on central atom?

Answer 129

Both polar covalent and hydrogen bonds

Answer 130

Nonpolar covalent bonds only

Answer 131

Hydrogen bonds only

Answer 132

Ionic and nonpolar hydrogen bonds

Answer 133

The overlap of two sp² hybrid orbitals

Answer 134

The sidewise p-p overlap

Answer 135

The axial s-p overlap

Answer 136

The axial p-p overlap

Answer 137

Equal to square

Answer 138

Depends on its source

Answer 139

Depends on its wavelength

Answer 140

Independent of its wavelength

Answer 141

No unpaired electron

Answer 142

Two unpaired electron

Answer 143

None of these

Answer 144

One unpaired electron

Answer 145

10.2340178

Answer 146

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

Answer 147

Depends on the pressure in the discharge tube

Answer 148

Depends on the gas used in the discharge tube

Answer 149

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

Answer 150

Ionization potential

Answer 151

Activation energy

Answer 152

Electron affinity

Answer 153

Electronegativity

Answer 154

Triangular planar

Answer 155

Triangular pyramidal

Answer 156

Tetrahedral

Answer 157

Triangular bipyramidal

Answer 158

Fourth Bohr orbit to the first Bohr orbit

Answer 159

Sixth Bohr orbit to the third Bohr orbit

Answer 160

Seventh Bohr orbit to the third Bohr orbit

Answer 161

Fifth Bohr orbit to the second Bohr orbit

Answer 162

6.63 x 10¯³⁵ m

Answer 163

6.65 x 10¯³⁵ m

Answer 164

6.63 x 10¯³³ m

Answer 165

6.63 x 10¯³⁴ m

Answer 166

The two atoms start ionization

Answer 167

They energy of atoms increases

Answer 168

The attractive forces dominate the repulsive forces

Answer 169

The repulsive force dominate the attractive forces

Answer 170

6.02 x 10¹⁶ J/mol

Answer 171

10¯⁷ J/mol

Answer 172

6.02 x 10²³ J/mol

Answer 173

Bonding molecular orbitals have low electron density between the two nuclei

Answer 174

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

Answer 175

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

Answer 176

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

Answer 177

Three unpaired electrons

Answer 178

Bond order of 2.5

Answer 179

Stability lower then O₂

Answer 180

Diamagnetic character

Answer 181

Triangular

Answer 182

Tetrahedral

Answer 183

Five π and nine σ

Answer 184

Eight σ and eight π

Answer 185

Nine σ and seven π

Answer 186

Nine σ and nine π

Answer 187

Tetrahedral

Answer 188

Triangular

Answer 189

Square planner

Answer 190

Liquid NH3

Answer 191

Liquid HCl

Answer 192

Covalent attraction

Answer 193

Hydrogen bond formation

Answer 194

Dipole interaction

Answer 195

Van der Waal’s forces

Answer 196

There may not be a possibility of chemical reaction

Answer 197

Lemon juice is dangerous for health

Answer 198

There may be a possibility of a chemical reaction

Answer 199

Water should be preferred over lemon Juice for drinking

Answer 200

Carbon tetrachloride

Answer 201

Carbon dioxide

Answer 202

Variable trend

Answer 203

Pauli exclusion principle

Answer 204

Electropositive character of elements

Answer 205

Electronegative character of elements

Answer 206

Octet rule

Answer 207

Interaction

Answer 208

Attractive force

Answer 209

All of above represent same entity

Answer 210

By losing three electrons

Answer 211

By gaining two electrons

Answer 212

By losing two electrons

Answer 213

By gaining three electrons

Answer 214

Triangular planar

Answer 215

Tetrahedral

Answer 216

Cannot be determined

Answer 217

Both are equal

Answer 218

Gun metals

Answer 219

Noble gases

Answer 220

Coinage metals

Answer 221

Alkali metals

Answer 222

sp³-hybridized carbon

Answer 223

sp²- hybridized carbon

Answer 224

sp- hybridized carbon

Answer 225

always same irrespective of its hybrid state

Answer 226

Double bond

Answer 227

Covalent bond

Answer 228

Electrovalent bond

Answer 229

Co-ordinate bond

Answer 230

Van der Waal’s force

Answer 231

Dispersion force

Answer 232

London force

Answer 233

Chemical bond

Answer 234

Vaporization

Answer 235

Distillation

Answer 236

Crystallization

Answer 237

Colour spectrum

Answer 238

Van der Waal’s forces

Answer 239

Covalent bond

Answer 240

Ionic bond

Answer 241

Metallic bond

Answer 242

Hydrogen sulphide is a weak acid

Answer 243

Water molecules associate through hydrogen bonding

Answer 244

Water has higher molecular weight

Answer 245

Sulphure has high electronegativity than oxygen

Answer 246

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

Answer 247

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

Answer 248

It has high electronegativity

Answer 249

It has high heat of dissociation

Answer 250

5.316 x 10¯²³ g

Answer 251

5.316 x 10¯²³ g

Answer 252

2.657 x 10¯²³ g

Answer 253

Square planar

Answer 254

Tetrahedral

Answer 255

Planar triangle

Answer 256

n = 1, l = 0

Answer 257

n = 2, l = 1

Answer 258

n = 2, l = 0

Answer 259

n = 1, l = 2

Answer 260

Square planner

Answer 261

Triangular

Answer 262

Tetrahedral

Answer 263

Trigonal bipyramidal

Answer 264

Octahedral

Answer 265

Square planar

Answer 266

Greater than 1.7

Answer 267

Equal to 1.7

Answer 268

Lesser then 1.7

Answer 269

No specificity exist

Answer 270

4, 0, 0, ½

Answer 271

4, 4, 0, ½

Answer 272

4, 1, 0, ½

Answer 273

4, 1, 1, ½

Answer 274

X-rays not produced

Answer 275

Larger wavelength

Answer 276

Shorter wavelength

Answer 277

Gamma rays

Answer 278

Hybrid and un hybrid orbitals

Answer 279

Un-hybrid orbitals

Answer 280

Atomic orbital and hybrid orbital

Answer 281

Hybrid orbitals

Answer 282

Impossible to predict

Answer 283

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

Answer 284

Remains constant

Answer 285

Subtraction of atomic orbitals

Answer 286

Addition of atomic orbitals

Answer 287

None of these

Answer 288

Multiplication of atomic orbitals

Answer 289

Tetrahedron

Answer 290

The nature of discharge tube

Answer 291

The nature of residual gas

Answer 292

All of these

Answer 293

The nature of electrode

Answer 294

3 bond pair one lone pair

Answer 295

1 bond pair 3 lone pair

Answer 296

2 bond pair 2 lone pair

Answer 297

3 lone pair 1 bond pair

Answer 298

Ionic bond

Answer 299

Metallic bond

Answer 300

Ion-dipole interaction

Answer 301

Dipole-dipole interaction

Answer 302

Dispersion force

Answer 303

All p-orbitals are involved

Answer 304

One p-orbital is involved

Answer 305

One s and 3 p-orbitals are involved

Answer 306

Four p-orbitals are involved

Answer 307

Octahedral

Answer 308

Square planner

Answer 309

Triangular

Answer 310

Trigonal bipyramidal

Answer 311

1/2 x ɜ₀

Answer 312

Quarternization of angular members

Answer 313

Heisenberg’s uncertainty principle

Answer 314

Quarternization of energy of electrons

Answer 315

Plank’s quantum theory

Answer 316

The absorption of electrons takes place

Answer 317

There is no effect

Answer 318

Ejection of electrons takes place

Answer 319

Ejection of some potassium atoms occurs

Answer 320

Bond length in NO⁺ is greater than in NO

Answer 321

Bond length in NO⁺ is equal to that in NO

Answer 322

Bond length in NO is greater than in NO⁺

Answer 323

Bond length is unpredictable

Answer 324

None of these

Answer 325

Electro negativity

Answer 326

Electron affinity

Answer 327

Ionization energy

Answer 328

None of these

Answer 329

Both A and B are correct

Answer 330

Orbital overlap will not occur

Answer 331

Bonding will not occur

Answer 332

Nuclei are unstable

Answer 333

Nuclei are stable

Answer 334

Molecules are stable

Answer 335

Molecules are unstable

Answer 336

Ground state of fluorine atom

Answer 337

Excited state of fluorine

Answer 338

Excited state of neon

Answer 339

Excited state of O¯₂

Answer 340

1 electron

Answer 341

6 electrons

Answer 342

4 electrons

Answer 343

2 electrons

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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