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Chemistry Chemical Bonding and Molecular Structure

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Chemistry Chemical Bonding and Molecular Structure Molecular Orbital Theory

What are the major differences between valence bond theory & Molecular Orbital Theory?

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Chandra Pruthi

Beginner-Level 5

You can check the below given table for the comarative differences between valence bond theory and molecular orbital theory.

Feature	Valence Bond Theory (VBT)	Molecular Orbital Theory (MOT)
Basic Concept	Overlap of atomic orbitals.	Atomic orbitals combine to form molecular orbitals
Bond Formation	Due to head-on (? ) or sideways (? ) overlap of atomic orbitals.	Linear combination of atomic orbitals (LCAO) to form bonding and antibonding MOs.
Explanation of Magnetic Behavior	Often fails to explain magnetism of molecules (e.g., O? is paramagnetic).	Accurately explains paramagnetism/diamagnetism (O? is paramagnetic due to unpaired electrons in antibonding orbitals).
Bond Order	Not clearly defined.	Bond order = ½ (No. of bonding electrons - No. of antibonding electrons)
Electron Delocalization	Electrons are localized between two atoms.	Electrons may be delocalized over multiple atoms.
Energy Consideration	Considers only overlapping orbitals and their energy.	Considers combination and energy differences of atomic orbitals.
Applicability	Works well for simple molecules like H? , HF, etc.	Better for explaining molecules like O? , N? , and ions like NO? , CN?

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Chemistry Chemical Bonding and Molecular Structure Bond Parameters

Explain why the bond angle in ${N H}_{3}$ is larger than in ${P H}_{3}$ ?

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Himanshi Singh

Beginner-Level 5

The reason why bond angle is larger in ${N H}_{3}$ than ${P H}_{3}$ are given below.

In ${N H}_{3}$ , there is one lone pair on the nitrogen atom increases repulsion, while the lone pair on phosphorus is in a higher energy orbital and causes less repulsion.
Nitrogen is a small and electronegative atom whereas phosphorus is larger and less electronegative than nitrogen.
In ${P H}_{3}$ , the bonding orbitals are nearly pure p-orbitals, which are less directionals–p hybridization, on the other hand, the bond pairs remain fairly directed, leading to a larger bond angle.

Hence, the bond angle in ${N H}_{3}$ is about 107° ( less than the ideal tetrahedral 109.5°) due to lone pair pres

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The reason why bond angle is larger in ${N H}_{3}$ than ${P H}_{3}$ are given below.

In ${N H}_{3}$ , there is one lone pair on the nitrogen atom increases repulsion, while the lone pair on phosphorus is in a higher energy orbital and causes less repulsion.
Nitrogen is a small and electronegative atom whereas phosphorus is larger and less electronegative than nitrogen.
In ${P H}_{3}$ , the bonding orbitals are nearly pure p-orbitals, which are less directionals–p hybridization, on the other hand, the bond pairs remain fairly directed, leading to a larger bond angle.

Hence, the bond angle in ${N H}_{3}$ is about 107° ( less than the ideal tetrahedral 109.5°) due to lone pair presence and highly electronegative atom, and the bond angle in PH? ( 93.5°) is much smaller due to less repulsive lone pair, and less electronegative atom.

Hence, the bond angle in ${N H}_{3}$ (107°) is larger than in ${P H}_{3}$ (93.5°).

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Chemistry Chemical Bonding and Molecular Structure Bond Parameters

Why the bond length in NO? is shorter than in NO?

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Aayush Kumari

Beginner-Level 5

The NO (Nitric Oxide) has 11 valence electrons while the NO? (Nitrosonium ion) has 10 valence electrons due to removal of one antibonding electron. Due to this, the bond order of NO increases from? 2.5 to 3 in the NO? (Nitrosonium ion).

As per the NCERT, since the bond order of NO? (3) is higher than that of NO (2.5), the bond in Nitrosonium ion is stronger bond and the stronger the bond, the shorter bond length.

Hence bond length in NO? is shorter the NO.

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Chemistry Chemical Bonding and Molecular Structure Hydrogen Bonding

Why HF has a higher boiling point than HCl?

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Jaya Sinha

Beginner-Level 5

The difference in boiling or melting point, even after nearly the same molecular geometry, is because opf the presence of hydrogen bond. HF forms intermolecular hydrogen bonds due to fluorine's high electronegativity. This intermolecular hydrogen bonding requires more energy due to break the hydrogen bonds and melt or boil. So, stronger intermolecular forces of HF result in a higher boiling point.

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Chemistry Chemical Bonding and Molecular Structure Hybridization

Determine the hybridisation and geometry of the central atom in ${X e F}_{2}$ .

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Nishtha Datta

Beginner-Level 5

Xenon has 8 valence electrons. In ${X e F}_{2}$ , it forms two bonds with fluorine, leaving three lone pairs. The steric number =2 bonds +3 lone pairs $= 5$ .
As per the VSEPR Theory the electron? pair geometry due to SN = 5 will be trigonal bipyramidal. The hybridization type will be ${s p}^{3} d$ hybridisation. However, the three lone pairs occupy equatorial positions, resulting in a linear molecular geometry.

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Chemistry Chemical Bonding and Molecular Structure Class 11th

Consider, PF₅, BrF₅, PCl₃, SF₆, ${[I C l_{4}]}^{-}$ , CIF₃ and IF₅.

Amongst the above molecule(s) / ion(s), the number of molecule(s) / ion(s) having sp³d² hybridisation is_____________.

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alok kumar singh

Contributor-Level 10

Following have the sp³d² hybridisation

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Chemistry Chemical Bonding and Molecular Structure Chemical Bonding and Molecular Structure

The number of molecule(s) or ion(s) from the following having non-polar structure is _________.

$N O_{3}^{-}, H_{2} O, B F_{3}, P C l_{3}, X e F_{4}, S F_{4}, X e O_{3}, P H_{4}^{+}, S O_{3}, {[A l {(O H)}_{4}]}^{-}$

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Vishal Baghel

Contributor-Level 10

SO₃ -> Sp² Planar

BF₃ -> Sp² Planar

$N O_{3}^{-}$ -> Sp² Planar

SF₄ -> Sp³d non-planar

H₂O₂ -> Sp³ Non-planar

PCl₃ -> Sp³ Non –planar

[Al (OH)₄]^{- ->} Sp³ Non-planar

XeF₄ -> Sp³d² planar

XeO₃ -> Sp³ Non-planar

$P H_{4}^{-}$ -> Sp³ Non-planar

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Chemistry Chemical Bonding and Molecular Structure Chemical Bonding and Molecular Structure

Why does MgO have a higher melting point than NaCl ?

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nitesh singh

Contributor-Level 10

Higher melting point means more energy is required to break the ionic bond. Since the ionic bonds in MgO are stronger than in NaCl due to various reasons, It have higher melting and even boiling point. Reasons are listed below:

In MgO, Magnesium and oxygen ions carry a +2 and -2 charge while sodium and in NaCl, chlorine ions carry a +1 and -1 charge. Due to higher charges more electrostatic attraction is involved.
The smaller ionic radius of Mg2+ are smaller compared to Na+, makes the bond stronger in MgO.
Due to larger elctrostatic force and smaller ionic radius, ionic bond in MgO are stronger, resulting in higher lattice energy.
The stro

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Chemistry Chemical Bonding and Molecular Structure Class 11th

According to MO theory, number of species / ions from the following having identical bond order is___________.

CN^-, NO⁺, O₂, $O_{2}^{+}, O_{2}^{2 +}$

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Payal Gupta

Contributor-Level 10

$C N^{-}, N O^{+} a n d O_{2}^{2 +}$ have bond order = 3

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Chemistry Chemical Bonding and Molecular Structure VSEPR Theory

What do you understand by bond pairs and lone pairs of electrons? Illustrate by giving one example of each type.

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Satyendra Dhyani

Beginner-Level 5

Molecules usually form chemical bond through either sharing or through rtransfering the electrons. During covalent bonding the electron pairs shared between atoms to form covalent bond are called shared pair or bond pair. At the same time, the electron pair which is not involved in sharing is called lone pair of electrons.

For example: CH₄ has 4 bond pairs but H₂O has 2 bond pairs and 2 lone pairs.

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