In $BrCl$, on the other hand, both bromine and chlorine are halogens and tend to accept electrons. So they share an electron and form a covalent bond.
BrCl is an interhalogen compound. The bond between BrCl is polar covalent with the negative end on Cl. This bond is formed because of the electronegativity difference between bromine and chlorine.
At room temperature it decomposes to bromine and chlorine gases. BrCl is a covalent compound because the constituents are halogens and share an electron to form a covalent bond.
The bond between chlorine and bromine in BrCl is polar with the negative end on Cl. The bond is polar due to the electronegativity difference between bromine and chlorine.
Bromchlorid | BrCl – PubChem.
In $RbCl$ rubidium forms a cation and chlorine an anion and an ionic bond is formed. Whereas in $BrCl$ both bromine and chlorine are halogens and tend to accept electrons. So they share an electron and form a covalent bond. So we can say that $RbCl$ is the more ionic compound.
Why is the BrCl molecule polar? The shared electrons are closer to Cl due to chlorine’s greater electronegativity. Diatomic molecules are nonpolar when a pair of shared electrons is closer to one atom than to the other.
Consequently, BrCl is polar, with chlorine carrying the partial negative charge. This molecule also has a dipole moment of 0.57 D .
In NaF sodium completely donates its electrons to the fluorine atom since fluorine is the most electronegative element and sodium is one of the most electropositive elements in the periodic table. From the above evidence it is clear that NaF is an ionic compound.
Some examples are NaCl (common salt), KCl, CsF and RbBr.
(CaS), barium selenide (BaSe) or strontium oxide (SrO). They have the same structure as sodium chloride, with each atom having six neighbors.
The solubility of bromine chloride is a function of polarity; it thus shows greater solubility in polar solvents. The solubility of BrCl in water is 2.5 times that of bromine, i. H. 8.5g/100g at 20°C.
The charge of Pb in PbCl2 is +2 and PbCl4 is +4. According to Fajan’s rule, the greater the charge of the cation, the greater its ability to self-polarize the bonding electrons, giving the compound a higher covalent character.
The three types of intramolecular forces are covalent, ionic and metallic bonds. Covalent bonds occur between two nonmetals. In this type of bond, the atoms share electrons. There are two types of covalent bonds: polar and non-polar.