1)Which of the following single bonds has the greatest bond energy?
B-F
B-Cl
B-I
B-Br
2)What is the % ionicity of the bond you chose above? (answer in full percent, not a fraction)
3)What is the % ionicity of the weakest single bond above? (answer in full percent, not a fraction)
Do you have a table of electronegativity differences?
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To determine the bond with the greatest bond energy among B-F, B-Cl, B-I, and B-Br, we need to compare the electronegativities of the atoms involved in each bond.
1) First, let's define bond energy. Bond energy represents the energy required to break a bond, and it is influenced by the strength of the bond. Stronger bonds have higher bond energies.
To compare the bond energies, we need to look at the electronegativities of the atoms involved. Electronegativity is the measure of an atom's ability to attract electrons towards itself in a chemical bond.
2) The electronegativity values of the atoms involved in the given bonds are as follows:
Boron (B) - 2.04
Fluorine (F) - 3.98
Chlorine (Cl) - 3.16
Iodine (I) - 2.66
Bromine (Br) - 2.96
To calculate the difference in electronegativity for each bond, subtract the electronegativity of the atom closer to fluorine from the electronegativity of the other atom.
Difference in electronegativity:
B-F = 3.98 - 2.04 = 1.94
B-Cl = 3.16 - 2.04 = 1.12
B-I = 2.66 - 2.04 = 0.62
B-Br = 2.96 - 2.04 = 0.92
The greater the difference in electronegativity, the more polar the bond, and typically, the stronger it is.
From the given options, B-F has the largest electronegativity difference of 1.94. Therefore, B-F has the greatest bond energy among these bonds.
3) Now, let's calculate the % ionicity of the B-F bond.
To determine the % ionicity of a bond, we use the equation:
% ionicity = (0.5 × difference in electronegativity) / average electronegativity
For B-F:
Average electronegativity = (2.04 + 3.98) / 2 = 3.01
% ionicity = (0.5 × 1.94) / 3.01 = 0.647 * 100 = 64.7%
Therefore, the % ionicity of the B-F bond is approximately 64.7%.
4) To find the % ionicity of the weakest single bond above, we need to calculate the difference in electronegativity and apply the same formula.
The smallest difference in electronegativity is for B-I:
% ionicity = (0.5 × 0.62) / 2.35 (average electronegativity of B and I) = 0.131 * 100 = 13.1%
Therefore, the % ionicity of the weakest single bond (B-I) is approximately 13.1%.