Which of the following is least ionic ?
- \( BaCl_2 \)
- AgCl
- KCl
- \( CoCl_2 \)
The Correct Option is B
Approach Solution - 1
To determine which compound is the least ionic among the given options, we need to understand the concept of ionic character. The ionic character in a compound largely depends on the difference in electronegativity between the cation and the anion and the size of the ions comprising the compound.
The options provided are:
- \( \text{BaCl}_2 \)
- AgCl
- KCl
- \( \text{CoCl}_2 \)
Let's analyze each option considering the factors that affect ionic character:
- \( \text{BaCl}_2 \): Barium (Ba) is a Group 2 element, and Chlorine (Cl) is a halogen. The high electronegativity difference results in a strong ionic bond.
- AgCl: Silver chloride has lower ionic character due to the relatively smaller electronegativity difference between silver (Ag) and chlorine (Cl). Also, silver ions tend to form covalent bonds due to their filled d-orbitals, which reduce the overall ionic character.
- KCl: Potassium (K) is an alkali metal, and Chlorine (Cl) is a halogen, resulting in a large electronegativity difference and thus, a strong ionic character.
- \( \text{CoCl}_2 \): Cobalt (Co), a transition metal, forms ionic compounds with halogens. However, due to partial covalent character from its d-orbitals, it might be less ionic than simple alkali or alkaline earth metals, but more ionic than AgCl.
Based on the above analysis, AgCl is the least ionic compound among the given options due to the reasons mentioned, such as closer electronegativity and covalent character contributed by silver's orbital configurations.
Approach Solution -2
To determine which of the given compounds is the least ionic, we need to understand the concept of ionic character. Ionic character is influenced by several factors, including the differences in electronegativity between atoms and the charges on these atoms. Generally, compounds with greater differences in electronegativity between the bonded atoms tend to exhibit greater ionic character. Additionally, the type of ions involved and their ability to polarize each other also play a role.
- \(BaCl_2\) (Barium Chloride): Barium is an alkaline earth metal, and chlorine is a halogen. The ionic bond between a metal and a halogen is typically quite ionic due to the significant difference in electronegativity.
- AgCl (Silver Chloride): Silver, being a transition metal, differs from the typical behavior of alkaline or alkali metals. The bond between Ag and Cl is less ionic compared to other metal chlorides due to the smaller difference in electronegativity and the polarizability of Ag+ ions.
- KCl (Potassium Chloride): Potassium is an alkali metal, which typically forms highly ionic compounds with halogens due to the large electronegativity difference.
- \(CoCl_2\) (Cobalt(II) Chloride): Cobalt is a transition metal. While it has ionic character, the smaller size and higher charge density of Co2+ lead to some covalent character due to polarization, but it is still typically more ionic than AgCl.
Among these compounds, AgCl is the least ionic. This is primarily due to the lesser difference in electronegativity between Ag and Cl and the substantial covalent character introduced by the polarization effect of the larger, more polarizable silver cation, Ag+. This covalent character decreases the overall ionic characteristic of the compound.
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
- Number of compounds with one lone pair of electrons on central atom amongst following is
\(CIF_3, XeO_3, BrF_5, XeF_4, O_3, NH_3\),\( H_2O\)
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 ______.