A. Write the number of valence electrons below each formula. No points if valence electrons are incorrect. B. Draw the Lewis structure. No additional points if Lewis structure is incorrect. C. Determine the molecular polarity. Write “P” for polar and “NP” for nonpolar. D. Determine the dominant attractive force. Write “L” for London force, “D-D” for dipole-dipole interaction and “H-B” for hydrogen bond. E. Predict the H2O solubility of each compound. Write “H” if it is high. Write “L” if it is low. Compound Lewis Structure Polar or Nonpolar Dominant AF H2O Solubility H2S NH3 C2H6 OF2 C3H6O
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.
A. Write the number of valence electrons below each formula. No points if valence electrons are incorrect.
B. Draw the Lewis structure. No additional points if Lewis structure is incorrect.
C. Determine the molecular polarity. Write “P” for polar and “NP” for nonpolar.
D. Determine the dominant attractive force. Write “L” for London force, “D-D” for dipole-dipole interaction and “H-B” for hydrogen bond.
E. Predict the H2O solubility of each compound. Write “H” if it is high. Write “L” if it is low.
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Compound |
Lewis Structure |
Polar or |
Dominant |
H2O |
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H2S |
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NH3 |
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C2H6 |
|
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OF2 |
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C3H6O |
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