Number of compounds with one lone pair of electrons on central atom amongst following is
\(CIF_3, XeO_3, BrF_5, XeF_4, O_3, NH_3\),\( H_2O\)
\(CIF_3, XeO_3, BrF_5, XeF_4, O_3, NH_3\),\( H_2O\)
Correct Answer: 4
Approach Solution - 1
1. CIF₃ (Chlorine trifluoride)
Chlorine (Cl) has 7 valence electrons. It forms 3 bonds with F atoms → uses 3 electrons. Remaining = 7 – 3 = 4 electrons = 2 lone pairs.
→ **2 lone pairs on Cl**
2. XeO₃ (Xenon trioxide)
Xenon (Xe) has 8 valence electrons. Each oxygen forms a double bond, using 6 electrons in total (3 × 2). Used 6 electrons → 8 – 6 = 2 electrons = 1 lone pair.
→ **1 lone pair on Xe**
3. BrF₅ (Bromine pentafluoride)
Bromine (Br) has 7 valence electrons. Forms 5 bonds with F → uses 5 electrons. Remaining 7 – 5 = 2 electrons = 1 lone pair.
→ **1 lone pair on Br**
4. XeF₄ (Xenon tetrafluoride)
Xenon (Xe) has 8 valence electrons. Forms 4 bonds with F → uses 4 electrons. Remaining 8 – 4 = 4 electrons = 2 lone pairs.
→ **2 lone pairs on Xe**
5. O₃ (Ozone)
Central O has 6 valence electrons. It forms one single and one double bond (resonance). Bonds use 3 pairs = 6 electrons → 6 – 4 = 2 electrons = 1 lone pair.
→ **1 lone pair on central O**
6. NH₃ (Ammonia)
Nitrogen has 5 valence electrons. Forms 3 bonds with H → uses 3 electrons. Remaining 2 electrons = 1 lone pair.
→ **1 lone pair on N**
7. H₂O (Water)
Oxygen has 6 valence electrons. Forms 2 bonds with H → uses 2 electrons. Remaining 4 electrons = 2 lone pairs.
→ **2 lone pairs on O**
Step 5: Count of Compounds with One Lone Pair
Compounds with exactly one lone pair on central atom: \[ \text{XeO}_3, \; \text{BrF}_5, \; \text{O}_3, \; \text{NH}_3 \] Total = **4**
Final Answer:
\[ \boxed{4} \]
Approach Solution -2
To determine the number of compounds with one lone pair on the central atom, let’s examine each compound:
- O3: Contains one lone pair on the central oxygen atom.
- H2O: Contains two lone pairs on the central oxygen atom.
- SF4: Contains one lone pair on the sulfur atom.
- ClF3: Contains two lone pairs on the chlorine atom.
- NH3: Contains one lone pair on the nitrogen atom.
- BrF5: Contains one lone pair on the bromine atom.
- XeF4: Contains two lone pairs on the xenon atom.
From the above, the compounds with exactly one lone pair on the central atom are: O3, SF4, NH3, and BrF5.
Total: 4 Compounds
So, the correct answer is: 4
Top JEE Main Chemistry Questions
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- At equilibrium the concentrations of and in a sealed vessel at . What will be for the reaction
- Find out the major products from the following reactions
Cobalt chloride when dissolved in water forms pink colored complex $X$ which has octahedral geometry. This solution on treating with cone $HCl$ forms deep blue complex, $\underline{Y}$ which has a $\underline{Z}$ geometry $X, Y$ and $Z$, respectively, are
- The correct order of atomic radii is:
Top JEE Main Chemical bonding and molecular structure Questions
- Statement I: Since fluorine is more electronegative than nitrogen, the net dipole moment of NF3 is greater than NH3.
Statement II: In NH3, the orbital dipole due to the lone pair and the dipole moment of NH bonds are in opposite directions, but in NF3, the orbital dipole due to the lone pair and the dipole moments of N-F bonds are in the same direction.
In light of the above statements, choose the most appropriate from the options given below: - What is the structure of Mn2(CO)10?
- Consider the following two statements Statement I: \(π\) \(2p\) bonding molecular orbital has low electron density above & below internuclear axis Statement II: \(π\times2p\) antibonding molecular orbital has only one nodal plane
- Consider the following two statements Statement I: \(SiO_2\) and GeO₂\(GeO_2\) are acidic, \(SnO\) and \(PbO\) are amphoteric Statement II: Allotropes of carbon are formed due to catenation and \(dπ - ρπ\) bond
- The order of relative stability of the contributing structure is:
Choose the correct answer from the options given below:
Top JEE Main Questions
- In a hydrogen like atom, when an electron jumps from the $M$ - shell to the $L$ - shell, the wavelength of emitted radiation is $\lambda$. If an electron jumps from $N$-shell to the $L$-shell, the wavelength of emitted radiation will be :
- Two masses $m$ and $\frac{m}{2}$ are connected at the two ends of a massless rigid rod of length $l$. The rod is suspended by a thin wire of torsional constant $k$ at the centre of mass of the rod-mass system(see figure). Because of torsional constant $k$, the restoring torque is $\tau =k\theta$ for angular displacement $\theta$. If the rod is rota ted by $\theta_0$ and released, the tension in it when it passes through its mean position will be:
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- The value of is
- The number of terms of an is even. The sum of the odd terms is and of the even terms is . The last term exceeds the first by . Then the number of terms in the series is ______.
Concepts Used:
Chemical Bonding and Molecular Structure
Such a group of atoms is called a molecule. Obviously, there must be some force that holds these constituent atoms together in the molecules. The attractive force which holds various constituents (atoms, ions, etc.) together in different chemical species is called a chemical bond.
Types of Chemical Bonds:
There are 4 types of chemical bonds which are formed by atoms or molecules to yield compounds.
- Ionic Bonds - Ionic bonding is a type of chemical bonding which involves a transfer of electrons from one atom or molecule to another.
- Covalent Bonds - Compounds that contain carbon commonly exhibit this type of chemical bonding.
- Hydrogen Bonds - It is a type of polar covalent bonding between oxygen and hydrogen wherein the hydrogen develops a partial positive charge
- Polar Bonds - In Polar Covalent chemical bonding, electrons are shared unequally since the more electronegative atom pulls the electron pair closer to itself and away from the less electronegative atom.
Factors Affecting Bond Enthalpy in Chemical Bonding:
- Size of the Atom
- Multiplicity of Bonds
- Number of Lone Pair of Electrons Present
- Bond Angle