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HCl: dipole-dipole interaction
HF: hydrogen bonding
TiCl4: ionic bonding?
CsCl:ionic bonding
To determine the type of bonding in each compound, we can use the electronegativity difference between the atoms involved.
1. HCl (Hydrogen Chloride): The electronegativity difference between hydrogen (H) and chlorine (Cl) is 0.9, which falls within the range of polar covalent bonds. Thus, the bonding in HCl is classified as a dipole-dipole interaction since the molecule is polar.
2. HF (Hydrogen Fluoride): The electronegativity difference between hydrogen (H) and fluorine (F) is 1.9, which is relatively larger than in HCl. This significant electronegativity difference creates a strong polarity in the HF molecule. Due to the presence of the highly electronegative fluorine atom, hydrogen bonding occurs in HF, which is a stronger form of dipole-dipole interaction.
3. TiCl4 (Titanium Tetrachloride): Titanium(IV) chloride consists of a central titanium (Ti) atom bonded to four chlorine (Cl) atoms. With the electronegativity difference less than 1.7 between Ti and Cl, the bonding in TiCl4 is considered as polar covalent bonds. It does not exhibit ionic bonding since the electronegativity difference is relatively small.
4. CsCl (Cesium Chloride): Cesium chloride contains a cesium (Cs) cation and a chloride (Cl) anion. With cesium being a metal and chlorine being a nonmetal, CsCl exhibits ionic bonding. The electrostatic attraction between the positively charged Cs ion and the negatively charged Cl ion leads to the formation of an ionic compound.
Therefore, the bonding type for each compound is:
- HCl: Dipole-dipole interaction
- HF: Hydrogen bonding
- TiCl4: Polar covalent bonding
- CsCl: Ionic bonding