The electronegativities of the elements are H=2.1, O=3.5, F=4.0, S=2.5, Cl=3.0. Determine (calculate) the electronegativity diffrences for the following molecules and explain how they are arranged in the order: H2, O2, HCl, HF, H2O and position them in the following designations.
Covalent bond-Polar Covalent Bond-Polar Bond. I have tried this question countless times and need help on how to calculate and determine the answers.
Answered above.
To determine the electronegativity difference and the type of bond (covalent bond, polar covalent bond, or polar bond), you need to understand the concept of electronegativity.
Electronegativity is a measure of the tendency of an atom to attract electrons in a chemical bond. The difference in electronegativity between two atoms in a compound determines the type of bond they form.
1. H2:
To calculate the electronegativity difference, subtract the electronegativity of hydrogen (H = 2.1) from itself: 2.1 - 2.1 = 0. The electronegativity difference is zero, suggesting a completely nonpolar covalent bond.
2. O2:
Subtract the electronegativity of oxygen (O = 3.5) from itself: 3.5 - 3.5 = 0. Again, the electronegativity difference is zero, indicating a nonpolar covalent bond.
3. HCl:
Subtract the electronegativity of hydrogen (H = 2.1) from chlorine (Cl = 3.0): 3.0 - 2.1 = 0.9. The electronegativity difference is 0.9, which falls within the range for a polar covalent bond. Chlorine is more electronegative than hydrogen, causing an uneven distribution of electrons in the bond.
4. HF:
Subtract the electronegativity of hydrogen (H = 2.1) from fluorine (F = 4.0): 4.0 - 2.1 = 1.9. The electronegativity difference is 1.9, which is also within the range of a polar covalent bond. Fluorine is more electronegative than hydrogen, resulting in an unequal sharing of electrons.
5. H2O:
Subtract the electronegativity of oxygen (O = 3.5) from hydrogen (H = 2.1): 3.5 - 2.1 = 1.4. The electronegativity difference is 1.4, falling within the range of a polar covalent bond. Oxygen is more electronegative than hydrogen, leading to the unequal sharing of electrons in the water molecule.
Arranging them in order:
H2 (Nonpolar covalent bond: electronegativity difference = 0)
O2 (Nonpolar covalent bond: electronegativity difference = 0)
HCl (Polar covalent bond: electronegativity difference = 0.9)
H2O (Polar covalent bond: electronegativity difference = 1.4)
HF (Polar covalent bond: electronegativity difference = 1.9)
Designations:
Covalent bond - H2, O2
Polar Covalent Bond - HCl, H2O
Polar Bond - HF
Remember, the designation "covalent bond" indicates a bond with equal sharing of electrons, "polar covalent bond" indicates an unequal sharing of electrons, and "polar bond" refers to a bond with a significant imbalance in electron distribution.