Compare the magnitude of the lattice energy for each of the following two ion pairs. (a) Ni²+ and O²- separated by a distance of 394 pm (b) K+ and Br separated by a distance of 358 pm
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
![**Comparison of Lattice Energy Magnitude for Ion Pairs**
Examine the magnitude of lattice energy for each of the following ion pairs:
**(a)** \( \text{Ni}^{2+} \) and \( \text{O}^{2-} \) separated by a distance of **394 pm**.
\[ \text{Select an option: } \]
**(b)** \( \text{K}^{+} \) and \( \text{Br}^{-} \) separated by a distance of **358 pm**.
\[ \text{Select an option: } \]
This exercise involves comparing the lattice energy, which is the energy released when ions form a crystalline lattice. The ion pairs listed have different charges and distances, which affect the lattice energy. Use the dropdown to compare and analyze the effect of these factors.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cb3c08b-867c-49fa-a9fe-3ee9eddee973%2Fcf7bb182-2029-4c09-a2f4-752f187bda7f%2Filk47lh_processed.png&w=3840&q=75)
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