Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF a. Propane, CH3CH2CH3 b. Heptane, CH3(CH2)5CH3 c. Propanol, CH3CH2CH2OH d. Heptanol, CH3(CH2)6OH 2. For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed line to show any H-bonding. 3. For each compound, consider whether or not any polar bonds are present a. Use a different coloured pen to identify any polar bonds b. Which compounds are polar? Which compounds are nonpolar? Explain your reasoning 4. Compare your drawings for propanol and heptanol. a. Which compound has stronger dispersion forces? Explain your answer b. Which compound has a higher boiling point? Explain your answer 5. Compare your drawings of heptanes and heptanol
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
1. Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF
a. Propane, CH3CH2CH3
b. Heptane, CH3(CH2)5CH3 c. Propanol, CH3CH2CH2OH d. Heptanol, CH3(CH2)6OH
2. For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed line to show any H-bonding.
3. For each compound, consider whether or not any polar bonds are present
a. Use a different coloured pen to identify any polar bonds
b. Which compounds are polar? Which compounds are nonpolar? Explain your reasoning
4. Compare your drawings for propanol and heptanol.
a. Which compound has stronger dispersion forces? Explain your answer
b. Which compound has a higher boiling point? Explain your answer
5. Compare your drawings of heptanes and heptanol
a. Which compound is more polar? Explain your answer
b. Which compound is more soluble in water? Explain your answer
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