Chemical Bonding: Key Concepts

• Electronic configurations of four atoms are given: L(1s²2s²2p¹), M(1s²2s²2p⁴), N(1s²2s²2p³), and O(1s²2s²2p⁵). O will readily form a diatomic molecule.

• The hybrid state of carbon in diamond, graphite, and acetylene (ethyne) is sp³, sp², and sp, respectively.

• Among the molecules listed, H₂CO is polar and has a central atom with an sp² hybrid state.

• The strongest hydrogen bond is present in HF.

• NaCl is soluble in water, but BaSO₄ is not because for BaSO₄, lattice energy is much more than hydration energy

• CO does not possess a dative bond.

• The bond lengths of H₂, F₂, Cl₂, and Br₂ are 74 pm, 144 pm, 199 pm, and 228 pm, respectively. The molecule with maximum bond energy is H₂.

• The bond angle in H₂O is 104.5° due to the repulsion between lone pairs.

• Elements O, P, Q, R, and S have specific electronic configurations. Q=1s²2s²2p¹ is most likely to form an electrovalent bond.

• The number of bonding electron pairs and non-bonding electron pairs in the NO₃⁻ ion is 3,1.

• According to the VSEPR model, the maximum repulsion between electron pairs is observed in lone pair & lone pair.

• SCI₂ is isostructural with H₂O.

• The increasing order of C-C bond length is C₂H₂ < C₂H₄ < C₂H₆.

• The strength of hydrogen bonding in N, F, and O is F > O > N.

• The combination with the most ionic compound is Cs & F.

• The F₂ molecule is formed by the overlap of p,p orbitals end to end manner.

• C-atoms in calcium carbide (CaC₂) are held together by 1σ, 2π.

• A molecule XY₂ contains two σ-bonds, two π-bonds, and one lone pair and has as a linear structure in the valence shell of X.

• In the OF₂ molecule, the total number of bond pairs and lone pairs in the molecule is 2, 8.

• The hybridization of N in NO₂⁺, NO₃⁻, and NH₄⁺ is sp, sp², and sp³, respectively.

• CH₃-CH=CH₂ has a bond formed by the overlap of sp-sp³ hybrid orbitals.

• The crystal structure of NaCl has an arrangement of ions in an octahedral fashion.

• Electrons involved in the Lewis structure of POCl₃ are 26.

• The bond energy of an H₂ molecule is 435 KJ/mol. Therefore, the energy required to dissociate 6.02x10²² molecules of H₂ is 43.5 KJ.

• The concept of a linear combination of atomic orbitals (LCAO) was given by the Molecular Orbital Theory.

• The weakest σ-bond is present in F₂.

• HCN contains both polar and non-polar bonds.

• The molecules possessing trigonal structure are SO₂ & BCl₃.

• The total number of electrons taking part in the formation of bonds in N₂ is 10.

• The pair of molecules that are isoelectronic is CO₂, N₂O.

• The number of electrons that are paired in the oxygen molecule is 12.

• In pyridine (N), the hybrid state assumed by N is sp².

• Hybridization of atomic orbitals in NO₂⁺, NO₂⁻, and NH₄⁺ is sp, sp², and sp³.

• The shape of gaseous SnCl₂ is angular.

• The geometry of the ClO₃⁻ ion, according to VSEPR theory, is Tetrahedral.

• H₂S has the least bond angle.

• CH2=CH-C≡CH represents the given mode of hybridization of sp², sp², sp, sp from left to right.

• Sulphate of a metal has the formula M₂(SO₄)₃. The formula of its phosphate will be M₂(PO₄)₃.

• In the following molecules/ions BF₃, NO₂, NH₂⁻ & H₂O the central aton sp³ hybridized is NH₂⁻ & H₂O.

• The element that could readily form a diatomic molecule with the electronic configuration 1s², 2s², 2p⁵ is B.

• The number of sigma & pi bonds in toluene is 15, 3.

• An element forms compounds of the formula ACl₃, A₂O₅ & Mg₃A₂ but does not form ACl₅. The A could be N

• Species with the same bond order include CN⁻ & NO⁺.

• An electron deficient molecule is C₂H₆.

• The correct set with reference to molecular formula, hybridization of the central atom, & shape of the molecule H₂O is sp³, pyramidal.

• Among the options, C₂H₄ possesses a planar shape.

• The diamagnetic species is C.

• The correct order of bond angles in H₂S, NH₃, BF₃ & SiH₄ is H₂S < NH₃ < BF₃ < SiH₄.

• H₂O is dipolar, but BeF₂ is not because the E.N of F is greater than that of O.

• The species in which sulphur undergoes sp³ hybridization are SF₄, SCl₂, SO₄⁻².

• The order that correctly describes the bond order is O₂⁺² > O₂ > O₂⁻² > O₂⁻².

• The total number of electrons involved in the Lewis structure of NO₃⁻ ion is 24.

• The angular shape of ozone (O₃) consists of 2ơ & 1π bond.

• The maximum bond angle at nitrogen is present in NO₂⁺.

• Species containing an equal number of sigma & pi bonds are N₂O₄.

• Ions that are isoelectronic and isostructural are ClO₃⁻, SO₄⁻².

• The following represents the correct description that is O₂⁺, O₂⁻² both paramagnetic.

• NH₄⁺ & H₃O⁺ ions both have tetrahedral geometry.

• The pair that contains both ionic & covalent compounds is KCN & NaOH.

• A molecule of acetylene contains 3σ, 2π bonds.

• In the sulfur dioxide (SO₂) molecule, the sulfur atom is in an sp² hybridized state.

• The C-C sigma bond in ethane is due to sp³-sp³ overlapping.

• The pair of compounds that is isostructural is BeCl₂, CS₂.

• A hybrid orbitals form σ-bond only is incorrect for hybridization.

• According to the VSEPR model, the shape of a molecule is determined by all of these.

• The correct order for bond angle in carbon compounds when carbon is present in different hybridized states is sp > sp² > sp³.

• In the compound CH≡C-CH=C=CH-CH₃, there are 2 C-atoms present in the sp² hybridized state.

• Among the statements, the correct one is that Lewis structure for CO₃⁻² has 24 electrons.

• π-bond is found in all except C₂H₆.

• The correct sequence for hybridization in the central atom of H₂S, PCl₃, CS₂, SO₃ is sp³, sp³, sp, sp².

• The total number of π electrons in half a mole of ethene is Nₐ.

• The formula XY₃ has a pyramidal shape which corresponds to 3 bonding pairs & 1 lone pair

• The hybrid state of C & N in CH₃NO₂ is sp³, sp2

• The only possible geometry for a molecule AB₂ with no lone pair on the central atom is Linear.

• The density of water is 1 g/cm³ at 4°C.

• Strongest attractive force is a Hydrogen bond

• The pair that can form the strongest & maximum number of hydrogen bonds is H₂O, HF.

• The CO molecule possesses: both σ and π bond

• The incorrect statement about π-bond is A C-atom containing a π-bond can rotate relative to other C-atom.

• The maximum bond angle can be found in: E CH₄

• Arrangement of water molecule in crystal structure of ice is: A Tetrahedral

• C-C bond length in sp Hybridized molecule is 1.10 À°

• The molecules that can poses maximum Lattice energy A MgO

• The reason for NH4 has dipole moment & BF3 has zero dipole moment A B has less EN than

• Interatomic distance in H2 & Cl2 is 74 & 198 so bond length between H-Cl is C 131

• The Geometry of H2S and its dipole moment ratio- Angular And non-zero

• Atoms obtain inert gas configuration to form chemical formula

• Ionic compound formation is favored in lower ionization energy and higher electron density of metal

• The ratio electronic configuration of Ionic bond formula is D A<3 B>2

• For a compound in lattice energy is less than solvation energy in D KsO4

• The multiple number of atomic bonds present with A.CCI4

• The molecule with chlorine presence is Purely covalent so it will be C chlorine

• For electronic configuration form more diatomic bond must contain A-B=A

• The dative bonds are found in Boron NH.

• A is 10-8esu is C-m.

• Bond energy orders depends on dipole bonds so its A HF <HO<HCI

• Dipoles and Dipole moment molecules must posses polar, geometrical and symmetry so options is B- polar

• The high co active factor of any given molecule contain is E. NO COVALENT character

• The first statement is false statement C is more polarized longer greater polarity

• A C==C contains possess bond energy so its E. 0-H

• Correct order for energy of different orbitals is: BMO>AO>ABMO

• Incorrect statements contain in bond are that it has nodal plane

• Summate of a metal has the formula MSO_4 The formula for is chloride would be A.MCl_2

• Electrons present in lewis structure. C.24

• Atoms contain equal and electron with same C a3 b6 - D A2B3 Stronger bond -E Cl-cl Compound that contains larger Lattice -C.NAF Paramagnetic -EO2 Total Number is electron pair - B.28 geometry A: angular , Dipole : zero Maximum Bond energy E: O2 Native Bond Is Present -C.(no3 Parameter valance theory a:bond. Bond increase B Energy Increased. Does not exist a H/20 The Most Bonded A; ICI Bond Angle B B<0<2 . Sigma bonds -15 Is c<b

Answer key's

171.B 172.A 173. O 174: C 175.A 176:D - NH4CI 177.Di 178Di 179Bi 180. c 181c 182Bi 183B 184 Di 185 A 186 A

187 D

2

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