Which of the following molecules of has the highest boiling point?
Question 3 options:
a) C3Cl8
b) C3H8
c) C3I8
d) C3F8
e) C3Br8
The highest boiling point is generally associated with molecules that have stronger intermolecular forces, such as hydrogen bonding or dipole-dipole interactions.
In this case, the molecule with the highest boiling point would be the one with the strongest intermolecular forces.
Among the given options, the molecule with the highest boiling point would be C3I8 because iodine (I) atoms are larger and have more electrons, resulting in stronger London dispersion forces between molecules.
To determine which of the given molecules has the highest boiling point, we need to consider the intermolecular forces between the molecules. The strength of intermolecular forces increases with increasing polarity and molecular weight.
Let's analyze each option:
a) C3Cl8: This molecule consists of carbon (C) and chlorine (Cl) atoms. Chlorine is more electronegative than carbon, which leads to a polar molecule. The molecular weight is relatively high. Thus, this molecule has strong intermolecular dispersion forces.
b) C3H8: This molecule consists of carbon (C) and hydrogen (H) atoms. Neither carbon nor hydrogen is very electronegative, so there is no significant polarity within the molecule. Additionally, the molecular weight is lower than in option a). As a result, this molecule has weaker intermolecular forces compared to C3Cl8.
c) C3I8: This molecule consists of carbon (C) and iodine (I) atoms. Iodine is even more electronegative than chlorine, leading to a more polar molecule. Furthermore, the molecular weight is higher due to iodine being larger than chlorine. Consequently, this molecule has stronger intermolecular forces than C3Cl8.
d) C3F8: This molecule consists of carbon (C) and fluorine (F) atoms. Fluorine is highly electronegative, resulting in a large polarity within the molecule. However, the molecular weight is lower due to fluorine being smaller than chlorine, which decreases the strength of the intermolecular forces.
e) C3Br8: This molecule consists of carbon (C) and bromine (Br) atoms. Bromine is less electronegative than chlorine, so this molecule has a slightly lower polarity than C3Cl8. However, the molecular weight is higher due to bromine being larger than chlorine, resulting in stronger intermolecular forces than in option a).
In summary, the molecule with the highest boiling point is C3I8 (option c) since it has both a high molecular weight and significant polarity.
To determine which molecule has the highest boiling point among the given options, we need to consider the intermolecular forces of attraction between the molecules.
Intermolecular forces are the attractive forces between molecules, and they play a significant role in determining the boiling point of a substance. The main types of intermolecular forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding.
Among the given options, C3F8, C3Cl8, C3Br8, and C3I8 are all halogenated hydrocarbons. These molecules experience London dispersion forces, which increase with increasing molecular size and surface area.
Among these options, the one with the highest boiling point is likely to be the molecule with the largest halogen atom. As we move down the halogen group in the periodic table (from fluorine to chlorine, bromine, and iodine), the size of the halogen atom increases, resulting in stronger London dispersion forces and higher boiling points.
Therefore, the molecule with the highest boiling point among the given options is likely to be C3I8 (option c).
Note: C3H8 is a nonpolar molecule and experiences only London dispersion forces. However, the halogenated hydrocarbons have larger halogen atoms, resulting in stronger intermolecular forces than C3H8.