Chemistry Chemical Bonding Online Mcqs Test

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Question 1

1. Geometry of simple molecule having SP³ hybrid orbital is

Answer

Square planner

Answer

Tetrahedral

Answer

Triangular

Question 2

2. Choose the correct statement about 2nd 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 greater than 1st ionization energy

Answer

It is always less than 1st ionization energy

Question 3

3. 1 erg of energy corresponds to

Answer

6.02 x 10²³ J/mol

Answer

6.02 x 10¹⁶ J/mol

Answer

10¯⁷ J/mol

Question 4

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

Question 5

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

Question 6

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

Answer

Impossible to predict

Question 7

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

Answer

Electronegativity

Answer

Electron affinity

Answer

Activation energy

Answer

Ionization potential

Question 8

8. Lewis acids are

Answer

Electron rich

Answer

Octet is complete

Answer

No such acids exist

Answer

Electron deficient

Question 9

9. Bond order for N2 molecule is

Question 10

10. Molecular orbitals are filled according to

Answer

Hund’s rule

Answer

Aufbau principal

Answer

Pauli’s exclusion principle

Question 11

11. When potassium metal is exposed to violet light

Answer

The absorption of electrons takes place

Answer

Ejection of some potassium atoms occurs

Answer

Ejection of electrons takes place

Answer

There is no effect

Question 12

12. The velocity of photon is

Answer

Depends on its source

Answer

Independent of its wavelength

Answer

Equal to square

Answer

Depends on its wavelength

Question 13

13. Ionic radius in a period from left to right

Answer

First increases then decreases

Answer

First decreases then increases

Question 14

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

Question 15

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

Question 16

16. Anti-bonding MO is formed by

Answer

Addition of atomic orbitals

Answer

Multiplication of atomic orbitals

Answer

None of these

Answer

Subtraction of atomic orbitals

Question 17

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

Question 18

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

Answer

Tetrahedron

Question 19

19. 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 20

20. A lone pair of electrons in an atom implies

Answer

A pair of electrons involved in bonding

Answer

A pair of valence electrons not involved in bonding

Answer

A pair of valence electrons

Answer

A pair of electrons

Question 21

21. Pick out the molecule which has zero dipole moment

Question 22

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

Question 23

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

Answer

4, 1, 0, ½

Answer

4, 4, 0, ½

Answer

4, 1, 1, ½

Answer

4, 0, 0, ½

Question 24

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

Question 25

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

Question 26

26. Al become isoelectronic with Ne

Answer

By gaining three electrons

Answer

By losing two electrons

Answer

By losing three electrons

Answer

By gaining two electrons

Question 27

27. 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 28

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

Question 29

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

Answer

3 lone pair 1 bond pair

Answer

3 bond pair one lone pair

Answer

1 bond pair 3 lone pair

Answer

2 bond pair 2 lone pair

Question 30

30. The de-Broglie wavelength of a particle with mass 1 g and velocity 100 m/s is

Answer

6.63 x 10¯³⁵ m

Answer

6.65 x 10¯³⁵ m

Answer

6.63 x 10¯³³ m

Answer

6.63 x 10¯³⁴ m

Question 31

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

Question 32

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

Answer

Excited state of fluorine

Answer

Excited state of neon

Answer

Excited state of O¯₂

Answer

Ground state of fluorine atom

Question 33

33. Lateral overlapping expected in

Answer

Metallic bond

Answer

Ionic bond

Question 34

34. 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 35

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

Question 36

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

Question 37

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

Answer

Electro negativity

Answer

Electron affinity

Answer

Ionization energy

Answer

None of these

Question 38

38. Which of the following has zero depolemoment?

Question 39

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

Question 40

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

Answer

Triangular

Answer

Tetrahedral

Question 41

41. Energy of an atom in a compound is

Answer

Lesser than individual

Answer

Higher than individual

Answer

Impossible to predict

Question 42

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

Answer

Electro negativity

Answer

Electron affinity

Answer

Ionization energy

Answer

None of these

Question 43

43. Nuclear radiation is emitted by those elements whose

Answer

Molecules are unstable

Answer

Molecules are stable

Answer

Nuclei are stable

Answer

Nuclei are unstable

Question 44

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

Question 45

45. 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 46

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

Question 47

47. Which of the following species is paramagnetic?

Question 48

48. ____________ has their outermost shell complete in atomic form

Answer

Gun metals

Answer

Noble gases

Answer

Coinage metals

Answer

Alkali metals

Question 49

49. Which of the following orbitals have a dumb bell shape?

Question 50

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

Question 51

51. Shape of CIO₃¯ is

Answer

Triangular bipyramidal

Answer

Triangular pyramidal

Answer

Triangular planar

Answer

Tetrahedral

Question 52

52. Molecular orbital picture of N₂ indicates

Answer

None of these

Answer

No unpaired electron

Answer

One unpaired electron

Answer

Two unpaired electron

Question 53

53. 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

p orbitals

Answer

s orbitals

Question 54

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

Question 55

55. Which of the solid does not contain covalent bond

Question 56

56. Along a period the atomic radii

Answer

First decreases then increases

Question 57

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

Answer

Variable trend

Question 58

58. Which one of these is weakest?

Answer

Metallic bond

Answer

Ionic bond

Answer

Covalent bond

Answer

Van der Waal’s forces

Question 59

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

Answer

Lone pair – lone pair repulsion only

Answer

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

Answer

Lone pair – bond pair repulsion only

Answer

Bond pair – bond pair repulsion only

Question 60

60. XeF₄ has shape of

Answer

Square planar

Answer

Tetrahedral

Answer

Trigonal bipyramidal

Question 61

61. 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 62

62. 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

Hydrogen bond formation

Answer

Van der Waal’s forces

Answer

Covalent attraction

Question 63

63. Number of sigma bonds in P₄O₁₀ is

Question 64

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

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

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 121

Non-polar solvents

Answer 122

Concentrated acids

Answer 123

All solvents

Answer 124

Polar solvents

Answer 125

First increases then decreases

Answer 126

First decreases then increases

Answer 127

Double bond

Answer 128

Electrovalent bond

Answer 129

Covalent bond

Answer 130

Co-ordinate bond

Answer 131

A stream of electrons

Answer 132

Can be deflected by magnetic fields

Answer 133

Move with speed as that of light

Answer 134

Charged particles

Answer 135

4 electrons

Answer 136

1 electron

Answer 137

2 electrons

Answer 138

6 electrons

Answer 139

Octahedral

Answer 140

Distorted tetrahedral

Answer 141

Planar triangle

Answer 142

Two sigma bonds and one pi-bond

Answer 143

One sigma bond and two pi-bonds

Answer 144

Three sigma bonds

Answer 145

Three pi-bonds

Answer 146

Depends on the gas used in the discharge tube

Answer 147

Depends on the pressure in the discharge tube

Answer 148

Does not depend on the nature of 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

The nature of residual gas

Answer 151

All of these

Answer 152

The nature of electrode

Answer 153

The nature of discharge tube

Answer 154

Covalent forces

Answer 155

Hydrogen bonds

Answer 156

All of these

Answer 157

Van der Waal forces or London dispersion forces

Answer 158

Ionic bonds

Answer 159

2π and one σ bond

Answer 160

2 sigma bonds

Answer 161

2 covalent, one co-ordinate bond

Answer 162

They are formed when electros are formed from atoms

Answer 163

They are also known as cations

Answer 164

They are larger than the atoms from which they were formed

Answer 165

They are smaller than the atoms from which they were formed

Answer 166

Two sigma, two pi

Answer 167

Two sigma, one pi

Answer 168

One sigma, one pi

Answer 169

One sigma, two pi

Answer 170

Increase from top to bottom in a group

Answer 171

Does not change in a period

Answer 172

Does not change in a group

Answer 173

Generally increases from left to right in a period

Answer 174

Boron trifluoride is pyramidal in shape while NH₃ is planar

Answer 175

Fluorides are more electronegative

Answer 176

NH₃ is pyramidal in shape while BF₃ is planar

Answer 177

Fluorides is more electronegative

Answer 178

They have completely filled s and p orbitals

Answer 179

They have high ionization energies

Answer 180

They do not react with one another

Answer 181

They are mono atomic gases

Answer 182

Hybrid orbitals

Answer 183

Atomic orbital and hybrid orbital

Answer 184

Un-hybrid orbitals

Answer 185

Hybrid and un hybrid orbitals

Answer 186

Electropositive character of elements

Answer 187

Electronegative character of elements

Answer 188

Octet rule

Answer 189

Pauli exclusion principle

Answer 190

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

Answer 191

Each bonding molecular orbital can accommodate only one electron

Answer 192

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

Answer 193

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

Answer 194

Attractive force

Answer 195

Interaction

Answer 196

All of above represent same entity

Answer 197

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

Answer 198

Remains constant

Answer 199

Shorter wavelength

Answer 200

X-rays not produced

Answer 201

Gamma rays

Answer 202

Larger wavelength

Answer 203

1.7588 x 10¹¹

Answer 204

9.1095 x 10¯³¹

Answer 205

1.7588 x 10²⁰

Answer 206

6.02 x 10²³

Answer 207

Water has higher molecular weight

Answer 208

Sulphure has high electronegativity than oxygen

Answer 209

Water molecules associate through hydrogen bonding

Answer 210

Hydrogen sulphide is a weak acid

Answer 211

Orbital overlap will not occur

Answer 212

Bonding will not occur

Answer 213

None of these

Answer 214

Both A and B are correct

Answer 215

Dispersion force

Answer 216

Chemical bond

Answer 217

London force

Answer 218

Van der Waal’s force

Answer 219

Four p-orbitals are involved

Answer 220

All p-orbitals are involved

Answer 221

One p-orbital is involved

Answer 222

One s and 3 p-orbitals are involved

Answer 223

Carbon dioxide

Answer 224

Carbon tetrachloride

Answer 225

Trigonal bipyramidal

Answer 226

Tetrahedral

Answer 227

Octahedral

Answer 228

10.2340178

Answer 229

Both are equal

Answer 230

Cannot be determined

Answer 231

Heisenberg’s uncertainty principle

Answer 232

Quarternization of angular members

Answer 233

Plank’s quantum theory

Answer 234

Quarternization of energy of electrons

Answer 235

Colour spectrum

Answer 236

Crystallization

Answer 237

Distillation

Answer 238

Vaporization

Answer 239

High, very negative

Answer 240

Low, positive or slightly negative

Answer 241

None of these

Answer 242

Low very negative

Answer 243

Liquid NH3

Answer 244

Liquid HCl

Answer 245

The axial p-p overlap

Answer 246

The axial s-p overlap

Answer 247

The sidewise p-p overlap

Answer 248

The overlap of two sp² hybrid orbitals

Answer 249

Hydrogen sulphide

Answer 250

Hydrogen fluoride

Answer 251

Water should be preferred over lemon Juice for drinking

Answer 252

There may not be a possibility of chemical reaction

Answer 253

There may be a possibility of a chemical reaction

Answer 254

Lemon juice is dangerous for health

Answer 255

Blue has higher wavelength

Answer 256

Blue is absorbed more easily

Answer 257

Blue is darker colour

Answer 258

Blue has more energy

Answer 259

Trigonal bipyramidal

Answer 260

Atomic size

Answer 261

Electronegativity

Answer 262

Ionization energy

Answer 263

Electron affinity

Answer 264

It has high electronegativity

Answer 265

It has high heat of dissociation

Answer 266

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

Answer 267

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

Answer 268

Electronegativity

Answer 269

Electron affinity

Answer 270

Ionization energy

Answer 271

None of these

Answer 272

Square planar

Answer 273

Planar triangle

Answer 274

Tetrahedral

Answer 275

Linear geometry

Answer 276

SP hybridization

Answer 277

Dipole moment is zero

Answer 278

Triangular

Answer 279

Square planner

Answer 280

Tetrahedral

Answer 281

Eight σ and eight π

Answer 282

Nine σ and seven π

Answer 283

Nine σ and nine π

Answer 284

Five π and nine σ

Answer 285

Triangular planar

Answer 286

Tetrahedral

Answer 287

The attractive forces dominate the repulsive forces

Answer 288

The repulsive force dominate the attractive forces

Answer 289

The two atoms start ionization

Answer 290

They energy of atoms increases

Answer 291

always same irrespective of its hybrid state

Answer 292

sp- hybridized carbon

Answer 293

sp³-hybridized carbon

Answer 294

sp²- hybridized carbon

Answer 295

Bond length in NO⁺ is greater than in NO

Answer 296

Bond length is unpredictable

Answer 297

Bond length in NO⁺ is equal to that in NO

Answer 298

Bond length in NO is greater than in NO⁺

Answer 299

Trigonal bipyramidal

Answer 300

Triangular

Answer 301

Octahedral

Answer 302

Square planner

Answer 303

1/2 x ɜ₀

Answer 304

Hydrogen bonds only

Answer 305

Both polar covalent and hydrogen bonds

Answer 306

Ionic and nonpolar hydrogen bonds

Answer 307

Nonpolar covalent bonds only

Answer 308

Square planar

Answer 309

Octahedral

Answer 310

Trigonal bipyramidal

Answer 311

Dipole-dipole interaction

Answer 312

Ion-dipole interaction

Answer 313

Dispersion force

Answer 314

Stability lower then O₂

Answer 315

Diamagnetic character

Answer 316

Three unpaired electrons

Answer 317

Bond order of 2.5

Answer 318

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

Answer 319

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

Answer 320

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

Answer 321

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

Answer 322

Greater than 1.7

Answer 323

No specificity exist

Answer 324

Equal to 1.7

Answer 325

Lesser then 1.7

Answer 326

Sublimation of metallic sodium to give yellow vapour

Answer 327

Low ionization energy of sodium

Answer 328

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

Answer 329

Photosensitivity of sodium

Answer 330

Fourth Bohr orbit to the first Bohr orbit

Answer 331

Fifth Bohr orbit to the second Bohr orbit

Answer 332

Sixth Bohr orbit to the third Bohr orbit

Answer 333

Seventh Bohr orbit to the third Bohr orbit

Answer 334

Remain same

Answer 335

Visible, ultraviolet, infrared, gamma rays

Answer 336

X – radiation, visible, infrared, microwave

Answer 337

Microwave, infrared, visible, ultraviolet

Answer 338

Radio, visible, infrared, ultraviolet

Answer 339

H – NH₂

Answer 340

n = 1, l = 0

Answer 341

n = 1, l = 2

Answer 342

n = 2, l = 1

Answer 343

n = 2, l = 0

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