What is the increasing dipole moment for CO,CS, and SiS?
My answer: SiS<CO<CS
Is this correct?
I would not rank them that way.
To determine the order of increasing dipole moment for CO, CS, and SiS, we need to consider the electronegativity difference between the atoms in each molecule.
The dipole moment of a molecule depends on the polarity of the bonds within it. A bond becomes polar when there is an electronegativity difference between the atoms involved. The greater the electronegativity difference, the stronger the polarity.
First, let's determine the electronegativity of each element:
- Carbon (C): 2.55
- Oxygen (O): 3.44
- Sulfur (S): 2.58
- Silicon (Si): 1.90
Now, let's compare each molecule.
1. CO (carbon monoxide) consists of a carbon atom bonded to an oxygen atom. Oxygen is more electronegative than carbon, creating a polar molecule. The dipole moment of CO is the highest among the three molecules.
2. CS (carbon disulfide) contains a carbon atom bonded to two sulfur atoms. Sulfur has a similar electronegativity to carbon, so the bond isn't as polar as in CO. CS has a lower dipole moment compared to CO.
3. SiS (silicon sulfide) consists of a silicon atom bonded to a sulfur atom. Silicon has a lower electronegativity than carbon, making the bond less polar in SiS. Therefore, SiS has the lowest dipole moment among these three molecules.
Based on this analysis, the correct order of increasing dipole moment is SiS < CS < CO. So, your answer is incorrect.