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InterviewSolution
This section includes InterviewSolutions, each offering curated multiple-choice questions to sharpen your knowledge and support exam preparation. Choose a topic below to get started.
| 451. |
Which of the following statement is falseA. `H_2` molecule has one sigma bondB. HCl molecule has one sigma bondC. Water molecule has two sigma bonds and two lone pairsD. Acetylene molecule has three sigma bond and three sigma bonds. |
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Answer» Correct Answer - D Acetylene molecule, `H-C^(sigma)-=C-H` has `3sigma` and two `pi` bonds |
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| 452. |
Which of the following is false ?A. 3s orbital is spherically symmetrical with two nodesB. `d_(x^2-y^2)` orbitals has lobes of electron density in XY plane along X and Y axisC. The radial probability curve of 1s. 3p and 5d have one, two and three regions of maximum probabilityD. `3d_z^2` has zero electron density in XY plane. |
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Answer» Correct Answer - D `d_z^2` orbital has two lobes along Z-axis and a collar of high electron density along XY-plane |
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| 453. |
One among the following is the incrorrect order of increasing ionisation energy :A. `Cl^-`lt Arlt `K^+`B. Klt Ca lt ScC. Au lt Ag lt CuD. Cslt Rblt K |
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Answer» Correct Answer - C The ionisation energy of Au gt Ag. It is because of the filling of (n-2) f-orbitals as a result of which the effective nuclear pull increases. |
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| 454. |
One among the following is the incrorrect order of increasing ionisation energy :A. `Cl- gt Ar gt K^+`B. `Klt Calt Se`C. `Au lt Ag lt Cu `D. `Cs lt Rb lt K` |
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Answer» Correct Answer - C Ionisation enrgy of `Au gt Ag` due to less shielding effect of `(n-2)` f-subshell. |
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| 455. |
Which of the following has a geometry different from others?A. `BF_4^(-)`B. `SO_4^(2-)`C. `PH_4^(+)`D. `XeF_4` |
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Answer» Correct Answer - D In `BF_4^(-)`, the central B has 4 valence electrons due to one unit of negative charge. All are used up to form 4 bonds with F atoms giving zero lone pair. In `SO_4^(2-)`, the central S atom has 8 valence electrons due to two units of `-ve` charge. All are used up to form bonds with 4 O atoms giving zero lone pair. In `PH_4^(+)`, the central P atom has 4 valence electrons due to one unit of positive charge. All are used up to form bonds with H atoms giving zero lone pair. In `XeF_4`, the central Xe has 8 valence electrons. Four `e^(-)s` are used up to form bonds with F atoms giving two lone pairs. Thus, `BF_4^(-)`, `SO_4^(2-)`, and `PH_4^(+)` all have octahedral geometry due to SN equal to 6. |
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| 456. |
In `H_(2)O_(2)` molecule, the angle between the two O-H planes isA. `90^(@)`B. `101^(@)`C. `103^(@)`D. `105^(@)` |
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Answer» Correct Answer - A `H_(2)O_(2)` contain bond angle between two O-H planes about `90^(@)` |
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| 457. |
Which one of the following oxides is expected to exhibit paramagnetic behaviour?A. `CO_(2)`B. `SO_(2)`C. `ClO_(2)`D. `SiO_(2)` |
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Answer» Correct Answer - C Due to unpaired `e^(-) ClO_(2)` is paramagnetic |
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| 458. |
Which of the following is not a correct statement ?A. Every `AB_5` molecule does in fact have square pyramind sructureB. Multiple bonds are always shorter than corresponding single bondsC. The electron-deficient molecules can act as Lewis acidsD. The canonical structures have non real existence |
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Answer» Correct Answer - A `I` in `IF_5` is `sp^3 d^2 `-hybridised and thus square pyramidal P in `PCl_5` is ` sp^3` d-hybridised and thus trigonal biuramid . |
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| 459. |
Which of the following is the correct electron-dot structure of `N_2O` molecule?A. `:N=N=overset(..)underset(..)O:`B. `:N-=overset(+)N-overset(..)underset(..)O:^(-)`C. `:N=N=overset(..)O:`D. `overset(..)underset(..)N=overset(..)N=overset(..)O:` |
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Answer» Correct Answer - B The valence shell electron configuration of N and O are `2s^2 2p^3` and `2s^2 2p^4`, respectively. Thus, there are `(5xx2)+6=16`, valence electrons to account for in `N_2O`. Structure (3) is ruled out because it has 14 valence electrons while structure (4) is ruled out because it has 18 valence electrons. In structure (1), there are 16 valence electrons but the octet of terminal N is not complete. In structure (2), there are not only 16 valence electrons but the order of every atom is also satisfied. |
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| 460. |
The bond order in NO is 2.5 while that in `NO^+` is 3. Which of the following statements is true for these two species ?A. Bond length in `NO^+` is greater than in NOB. Bond length is unpredictableC. Bond length in `NO^+` is equal to that in NOD. Bond length in NO is greater than in `NO^+` |
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Answer» Correct Answer - D B.O. in NO is 2.5 while that `NO^+` is 3. As B.O. is inversely proportional to bond length, bond length in NO is more than in `NO^(+)` |
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| 461. |
Which one of the following compounds has bond angle close to `90^@` ?A. `NH_3`B. `H_2S`C. `C Cl_4`D. `CH_4` |
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Answer» Correct Answer - B Although S-atom in `H_2 S` molecule shows hybrid state of `sp^3`, but the presence of two lone pairs on sulphur atom, decreases the bond angle to `90^@` and the molecule becomes V-shaped |
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| 462. |
The maximum number of `90^(@)` angles between bond pair-bond pair of electrons is observed inA. `dsp^3`-hybridisationB. `sp^3-d^2`hybridisationC. `dsp^2`-hybridisationD. `sp^3`d-hybridisation |
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Answer» Correct Answer - B Maximum number of `90^@` angles between bond pair-bond pair of electrons is in `sp^3d^2` hybridisation |
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| 463. |
The bond angle and % of d-character in `SF_(6)` areA. `120^(@),20%`B. `90^(@),33%`C. `109^(@),25%`D. `90^(@),25%` |
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Answer» Correct Answer - B Sulphur hexafluoride involves `sp^(3)d^(2)` hybridisation and possesses octahedral geometry. % of d-character `=(2"(no. of d-orbitals)")/("6 (total hybridised orbitals)")xx100 =33%` Bond angle =`90^(@)` |
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| 464. |
Which one of the following compounds has bond angle close to `90^@` ?A. `H_(2)O`B. `H_(2)S` and `BeCl_(2)`C. `NH_(3)`D. `CH_(4)` |
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Answer» Correct Answer - B `H_(2)S` show bond angle nearly `90^(@)` |
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| 465. |
Bond angle between two hybrid orbitals is `105^@` Percentage of s-orbital character of hybrid orbital is betweenA. Between 20-21%B. Between 19-20%C. Between 21-22%D. Between 22-23% |
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Answer» Correct Answer - D Bond angle between two hybrid orbitals is `105^(@)` it means orbitals are `sp^(3)` hybridised but due to lone pair repulsion bond angle get charged from `109^(@)` to `105^(@)`. So its % of s-character is between 22-23% |
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| 466. |
In which of the following moleucles, all atoms are coplanar?A. `CH_(4)`B. `BF_(3)`C. `PF_(5)` and `BrF_(5)`D. `NH_(3)` |
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Answer» Correct Answer - B In `BF_(3)` molecule boron is `sp^(2)` hybridised so its all atoms are co-planar |
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| 467. |
Which orbital is not involved in the formation of `PCl_(5)` molecule :-A. sB. `d_(z^(2))`C. `d_(x^(2)-y^(2))`D. `P_(z)` |
| Answer» Correct Answer - C | |
| 468. |
Lattice energy of an ionic compound depedns upon :A. charge on the ions onlyB. size of the ions onlyC. packing of the ions onlyD. charge and size of the ions |
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Answer» Correct Answer - D Lattice nergy `prop (q_1 q_2 /(d^(2))` where ` q_(1)q_(2)` are chanrge on ions and d in `32` electrons . |
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| 469. |
Which of the following pair has same structure but different hybridisation ?A. `PH_(3)` and `BCl_(5)`B. `SO_(2)` and `NH_(3)`C. `PCl_(5)` and `SF_(6)`D. `NH_(4)^(+)` and `SO_(4)^(2-)` |
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Answer» Correct Answer - D `NH_(4)^(+)` and `SO_(4)^(2-)` both slow `sp^(3)`-hybridization and tetrahedral structure. |
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| 470. |
The correct order towards bond angle isA. `sp lt sp^(2)lt sp^(3)`B. `sp^(2)lt sp lt sp^(3)`C. `sp^(3) lt sp^(2)lt sp`D. Bond angle does not depends on hybridisation |
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Answer» Correct Answer - C Increasing order of bond angle is `underset(109^(@))(sp^(3))lt underset(120^(@))(sp^(2))lt underset(180^(@))(sp)` |
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| 471. |
The length of C-C bonds in benzene isA. TautomerismB. `sp^(2)` hybridisationC. IsomerismD. Inductive effect |
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Answer» Correct Answer - B All carbon atoms of benzne conists of alternate single and double bond and show `sp^(2)` hybridisation. |
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| 472. |
Which of the following will be octahedral ?A. `SF_6`B. `BF_4^-`C. `PCl_5`D. `BO_3^(3-)` |
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Answer» Correct Answer - A `SF_6` has octahedral structure because the central atom (sulphur) is `sp^3d^2` hybridised and due to the presence of d-orbitals sulphur may extend its covalency upto 6 |
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| 473. |
COVALENT BONDINGA. GermaniumB. Sodium chlorideC. Solid neonD. Copper |
| Answer» Correct Answer - A | |
| 474. |
Which of the following will be octahedral ?A. `SF_(6)`B. `BF_(4)^-`C. `PCl_(5)`D. `BO_(3)^(3-)` |
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Answer» Correct Answer - A S-atom in `SF_(6)` has `sp^(3)d^(2)` hybridisation. So, the structure of `SF_(6)` will be octahedral. |
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| 475. |
Which of the following contains both ionic and covalent bonding?A. `NaBr`B. `PCl`C. `Ba(CN)_2`D. `CH_3CH_2OH` |
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Answer» Correct Answer - C Barium cyanide contains `Ba^(2+)` and `[:C-=N:]^(-)` ions. The bonding between barium and cyanide ions is ionic while the bonding between C and N in cyanide ion is covalent. |
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| 476. |
P in `PCl_5` has `sp^3 d` hybridisation. Which of following statement is wrong about ` PCl_5` structure ?A. Two `P-Cl` bonds are strongest and three ` P -Cl` bonds weakerB. Two `P-Cl` bonds are axial and larger than three `P -Cl` equatorial bondsC. `PCl_5` has trigonal bipyramidal geometry with bond-polar natureD. All of these |
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Answer» Correct Answer - A In `PCl_5` two aixal bonda are larger and weaker and threfore `PCl_5` diassociates into `PCl_3` and `cl_2` . |
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| 477. |
Which one is false in the following statementsA. Each carbon in ethylene is in `sp^(2)` hybridisationB. Each carbon in acetylene in in `sp^(3)` hybridisationC. Each carbon in benzene is in `sp^(2)` hybridisationD. Each carbon in ethane is in `sp^(3)` hybridisation |
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Answer» Correct Answer - B In `C_(2)H_(2)` each carbon has sp-hybridisation `H-underset(sp)(C)-=underset(sp)(C)-H` |
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| 478. |
The `PCl_5` molecule is a result of the hybridisation ofA. `sp^(2)d^(2)`B. `sp^(3)d`C. `spd^(3)`D. `sp^2d^(3)` |
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Answer» Correct Answer - B The molecule of `PCl_(5)` has `sp^(3)d` hybridisation. Structure is trigonal bipyramidal. |
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| 479. |
Which type of bonding exists in `Li_(2)O` and `CaF_(2)` respectivelyA. respectivelyB. Ionic, ionicC. Ionic, covalentD. covalent, ionic |
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Answer» Correct Answer - A Lithium oxide and calcium fluoride show ionic characters. |
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| 480. |
Which of the following have both polar and non-polar bonds?A. `C_(2)H_(6)`B. `NH_(4)Cl`C. HClD. `AlCl_(3)` |
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Answer» Correct Answer - B `NH_(4)Cl` has both types of bonds polar and non polar `[H-overset(H)overset(|)underset(H)underset(|)(N)toH]^(+)Cl^(-)` |
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| 481. |
Which of the following statement is not true or ionic compoundsA. high melting pointB. least lattice energyC. least solubility in organic compoundsD. soluble in water |
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Answer» Correct Answer - B `BaCl_(2)` contain higher ionic character. |
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| 482. |
Which of the following bonds has the most polar character ?A. C-OB. C-BrC. C-SD. C-F |
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Answer» Correct Answer - D C-F bond has the most polar character due to difference of their electronegativity |
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| 483. |
Which of the following is a polar compound ?A. HFB. HClC. `HNO_(3)`D. `H_(2)SO_(4)` |
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Answer» Correct Answer - A We know that greater the difference in electronegativity of two atoms forming a covelent bond. More Is its polar nature. In HF there is a much difference in the electronegatives of hydrogen and fluorine. Therefore (HF) is a polar compound. |
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| 484. |
The hydrogen bond is the strongest inA. HFB. HIC. `CH_(4)`D. `PH_(3)` |
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Answer» Correct Answer - A compound containing highly electronegative element show hydrogen bonding. Fluorine (F) is highly electronegatively and has smaller size. So hydrogen fluorine shows the strongest hydrogen bonding in the liquid phase. |
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| 485. |
The first IP lithium is `5.41eV` and electron gain enthalpy of `Cl` is `-3.61eV` . Calculate `Delta H` in `KJ mol^(-1)` for the reaction: `Li_(g) +Cl_(g) rarr Li_(g)^= +Cl_(g)^(-)`. |
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Answer» `Delta H//`molecule of `Li^+` and `Cl^- =IF_1 +` Electron gain enthaply . ` = 5.41 - 3. 61 =1. 80 eV` ` :. Li rarr Li^+ +e , IP_1 +ve` and ` Cl + e rarr Cl^(-1) ,` Electron gain enthalpy `= -ve` ` :. Delta H//mol=1.8 xx 6. 023xx 10^(23) eV` `=1.8xx 6. 023 xx 10^(233) xx 1.602 xx 10^(19) J` ` =1. 8 xx 6.023 xx 10^(23) xx 1. 602 xx 10^(19) xx 10^(-3) kJ` ` = 173. 7 kJ`. |
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| 486. |
The shape of `ClO_3^-` according to valence shell electron pair repulsion theory will beA. Planar triangleB. PyramidalC. TetrahedralD. Square planar |
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Answer» Correct Answer - B `.^(-)O-underset(O)underset(|)(ddot(Cl))-O` |
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| 487. |
The total number of lone pairs in a chlorine molecule isA. sixB. threeC. fourD. two |
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Answer» Correct Answer - A `:underset(..)overset(..)Cl*+*underset(..)overset(..)Cl:rarr:underset(..)overset(..)Cl:underset(..)overset(..)Cl:` A formula using dots to represent valence electrons is called a Lewis electron-dot formula. An electron pair (represented by a pair of dots) shared between two Cl atoms in a bonding pair while an electron pair that remains on one Cl atom and is not shared is a lone or nonbonding pair. Thus, there are 6 lone pairs, 3 on each Cl atom. |
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| 488. |
Pairs of nonmetal atoms share electron pairs to form covalent bonds because the result of this sharing is that each atom attains a more stable electron configuration, frequently the same as that of theA. following noble gasB. preceding noble gasC. nearest noble gasD. inert gas |
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Answer» Correct Answer - C This results in a more stable arrangement for the bonded atoms. |
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| 489. |
The bond between two identical nonmetal atoms has a pair of electronsA. If both assertion and reason are true and the reason is the correct explanation of the assertionB. if both assertion and reason are true but reason is not the correct explanation of the assertionC. if assertion is true but reason is falseD. if the assertion and reason both are false |
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Answer» Correct Answer - D Both assertion & reason are false because pairs of electrons will have different spins. Electrons are equally shared between them |
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| 490. |
How many `Cs` atoms can be converted to `Cs^+` ions by ` 1` joule energy , If `IE_1` for `Cs` si `376kJ mol^(-1)` ? |
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Answer» `376 xx10^3 J` energy porduces ` 6.023 xx10^(23)` ions . `:.1 J` energy produces `(,0623 xx10^(23)) /(376xx10^3)` ions `=1.60 xx10^(18) C s^+` ions. |
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| 491. |
Which of the following is incorrect about sigma bonds?A. They result from the end-to-end overlap of orbitals.B. In `sigma` bonds, the electron density is concentrated above and below the bond axis.C. The shape of the molecule is determined by the orientation of `sigma` bonds.D. All of these |
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Answer» Correct Answer - B In sigma bond, the `e^(-)` density is concentrated between the nuclei of bonded atoms. |
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| 492. |
In dry ice , there are :A. ionic bondB. covalent bondC. hydrogen bondD. none of these |
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Answer» Correct Answer - B Dry ice is ` CO_2` having ` C-O` covalent bonds . |
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| 493. |
`CO_2` has the same geometry as :A. A and CB. B and DC. A and DD. C and D |
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Answer» Correct Answer - C Both ` HgCl_2` and `C_2H_2` are linear like ` CO_2` because of sp-hybridisation . |
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| 494. |
How many resonating structures can be drawn for `NO_2`?A. SixB. FourC. FiveD. Two |
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Answer» Correct Answer - B Since `NO_2` has `5+(2xx6)=17` valence electrons, an odd number, not all of its atoms can have complete octets. Without considering nonbonding electrons, we can write two structures: `O=N-OiffO-N=O` In distributing the nonbonding electrons, we can write structures in which N atom has an incomplete octet and has the unpaired (or odd) electron: `overset(..)underset(..)O=underset(I)overset(.)N-overset(..)underset(..)O:iff:overset(..)underset(..)O-overset(.)underset(II)N=underset(..)overset(..)O` or structures in which the O atoms have incomplete octet, such as `overset(.)underset(..)O=underset(III)overset(..)N-overset(..)underset(..)O:iff:overset(.)underset(..)O-underset(IV)overset(..)N=overset(..)underset(..)O` The first two structures, in which the N atom has an incomplete octet, make the most important contribution. Structures such as the last ones, in which the O atom has incomplete octet, are less important, since the most electronegative element usually has the completed octet. |
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| 495. |
Bond angle is minimum forA. `H_(2)Te`B. `H_(2)Se`C. `H_(2)O`D. `H_2S` |
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Answer» Correct Answer - A Bong angle of hydrides decreases down the group |
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| 496. |
Which contains both polar and non-polar bonds ? .A. `H_2O_2`B. `CH_4`C. `HCN`D. `NH_4Cl` |
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Answer» Correct Answer - A Such bonds are present in polar covalent compounds only. `NH_4Cl` is ionic, `CH_4` is covalent, but all the bonds between C and H are polar due to electronegativity difference. The Lewis structure of `HCN` is `H-C-=N:`, it also has only polar bonds. In `H_2O_2`, having the Lewis structure `H-overset(..)underset(..)O-underset(..)overset(..)O-H` the bond between like O atoms is nonpolar while the bond between unlike H and O atoms is polar. |
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| 497. |
Which moleucle is T-shaped ?A. `BeF_2`B. `BCl_3`C. `NH_3`D. `ClF_3` |
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Answer» Correct Answer - D `ClF_3` has ` sp^3` d-hybridisation with two lone pairs of electron on ` Cl`. |
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| 498. |
Which of the following has the minimum bond length ?A. `O_2^-`B. `O_2^(2-)`C. `O_2`D. `O_2^+` |
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Answer» Correct Answer - D Bond order of `O_2^(+)=(10-5)/2=2.5` Bond order of `O_2^(-) =(10-7)/2=1.5` Bond order of `O_2^(2-)=(10-8)/2=1` Bond order of `O_2 =(10-6)/2=2` `because` Maximum bond order = minimum bond length `therefore` Bond length is minimum for `O_2^(+)` |
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| 499. |
Which fomulae does not correctluy represents the bonding capacity of the atom involued ?A. B. C. D. |
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Answer» Correct Answer - D One carbon has three bonds and other five wherease each should have four bonds . |
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| 500. |
In which of the following pairs of molecules/ ions, the central atoms have `sp^2`-hybridization ?A. `NO_2^-` and `NH_3`B. `BF_3` and `NO_2^-`C. `NH_2^-` and `H_2O`D. `BF_3` and `NH_2^-` |
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Answer» Correct Answer - B Key Idea For `sp^3` hybridisation , there must be `3 sigma` bonds or `2 sigma` bonds along with a lone pair of electrons. `(i)NO_2^(-) rArr 2 sigma + 1 lp =3 i.e. sp^2` hybridisation `(ii)NH_3 rArr 3 sigma + 1 lp =4 i.e. sp^3` hybridisation `(iii)BF_3 rArr 3 sigma + 0 lp =3 i.e. sp^2` hybridisation `(iv)NH_2^(-) rArr 2 sigma + 2 lp =4 i.e. sp^3` hybridisation `(v)H_2O rArr 2 sigma + 2 lp =4 i.e. sp^3` hybridisation Thus , among the given pairs, only `BF_3` and `NO_2^-` have `sp^2` hybridisation. |
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