Respuesta :
An approximation of the power of the bonds in an ionic compound can be acquired by calculating the lattice energy of the compound, which is the energy given off when contrasting charged ions in the gas stage come collected to create a solid.The lattice energy of the following compounds are:CsBr -637CaO 3464KF 801
To arrange this from increasing:CsBr < KF < CaO.
The bigger the radius of an atom, the bigger the distance from one nucleus of the atom to the other in that molecule, therefore making a weaker bond which is a smaller magnitude lattice energy. This can be found in the periodic table.
To arrange this from increasing:CsBr < KF < CaO.
The bigger the radius of an atom, the bigger the distance from one nucleus of the atom to the other in that molecule, therefore making a weaker bond which is a smaller magnitude lattice energy. This can be found in the periodic table.
The correct increasing order of lattice energy is,[tex]\boxed{{\text{CsBr}<\text{KF}<\text{CaO}}}[/tex].
Further Explanation:
Lattice energy:
It is the amount of energy released when ions are combined to form an ionic compound or the energy required to break the ionic compound into its constituent gaseous ions. It cannot be measured directly and is denoted by [tex]{\mathbf{\Delta }}{{\mathbf{H}}_{{\mathbf{lattice}}}}[/tex]. Lattice energy can have both positive as well as negative values.
Lattice energy is used to determine the stability of ionic compounds.
The lattice energy of an ionic solid depends upon the following factors:
(1) The charge on the ions.
(2) The size or the radius of the ions.
The factor which must be check first is charge on the ions. The charge on the ions is directly related to the lattice energy, and therefore the lattice energy increases with increases in the charge on the ion. Then check for the second factor, the size of ions. The size of an ion is inversely proportional to the lattice energy. Therefore, when the size of an ion increases, the lattice energy decreases.
As we move down the group in the periodic table, the size of an atom increases and therefore the lattice energy decreases.
Given compounds are CaO, KF, and CsBr. Compound CaO contains [tex]{\text{C}}{{\text{a}}^{2 + }}[/tex] and [tex]{{\text{O}}^{2 - }}[/tex] ions. Compound KF contains [tex]{{\text{K}}^ + }[/tex] and [tex]{{\text{F}}^ - }[/tex] ions. Compound CsBr contains [tex]{\text{C}}{{\text{s}}^ + }[/tex] and [tex]{\text{B}}{{\text{r}}^ - }[/tex] ions. Since the charges on ions are higher in CaO thus it has higher lattice energy among three.
Between KF and CsBr, KF has smaller size thus it has higher lattice energy.
Hence the increasing order of lattice energy is,
CsBr<KF<CaO
Learn more:
1. Identify the chemical equation of the first ionization energy of the lithium: https://brainly.com/question/5880605
2. Arrange the elements, according to their first ionization energy: https://brainly.com/question/1550767
Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Lattice energy.
Keywords: Lattice energy, potassium fluoride, KF, CsBr, CaO, crystal lattice, s-block, periodic table and ionic size.
