electronegativity is a calculated value for each element and is based upon the bonding behavior of each element. en is the ability of an element to pull electrons towards itself in a bond. depending upon the difference in electronegativity, $ \delta \mathrm{en} $, there may be partial charges assigned. the element with higher electronegativity is assigned a partial negative charge, $ \delta - $. the element with the lower en is assigned a partial positive charge, $ \delta + $. if the $ \delta \mathrm{en} $ is insignificant, 1.7, the bond is called ionic, the electrons are very unequally shared, and the individual ions act like strong magnets. consider fluorine, $ \mathrm{f}_{2} $. the en for fluorine is __1__. the $ \delta \mathrm{en} $ for the bond between f and f is __2__. this means that the bonding electrons are shared evenly between the f and the f atoms. thus, the bond in $ \mathrm{f}_{2} $ is a __3__ bond. also, since $ \mathrm{f}_{2} $ has no __4__ bonds, there is no dipole in the molecule and $ \mathrm{f}_{2} $ is a

Question

electronegativity is a calculated value for each element and is based upon the bonding behavior of each element. en is the ability of an element to pull electrons towards itself in a bond. depending upon the difference in electronegativity, $ \delta \mathrm{en} $, there may be partial charges assigned. the element with higher electronegativity is assigned a partial negative charge, $ \delta - $. the element with the lower en is assigned a partial positive charge, $ \delta + $. if the $ \delta \mathrm{en} $ is insignificant, < 0.5, the bond is called a nonpolar covalent bond, the electrons are shared fairly evenly, and en does not significantly affect the properties of the molecule. if the $ \delta \mathrm{en} $ is between 0.5 and 1.7, the bond is called a polar covalent bond, the electrons are not shared equally, partial charges are assigned to represent a dipole, and this may cause the molecule to behave like a magnet. if the dipoles cancel the molecule is nonpolar. if the dipoles dont cancel, the molecule is polar and acts like a magnet. if the $ \delta \mathrm{en} $ is > 1.7, the bond is called ionic, the electrons are very unequally shared, and the individual ions act like strong magnets. consider fluorine, $ \mathrm{f}_{2} $. the en for fluorine is __1__. the $ \delta \mathrm{en} $ for the bond between f and f is __2__. this means that the bonding electrons are shared evenly between the f and the f atoms. thus, the bond in $ \mathrm{f}_{2} $ is a __3__ bond. also, since $ \mathrm{f}_{2} $ has no __4__ bonds, there is no dipole in the molecule and $ \mathrm{f}_{2} $ is a

Accepted Answer

# Explanation:
## Step1: Determine electronegativity of fluorine
Fluorine has the highest electronegativity value. From the Pauling scale, the electronegativity of fluorine ($F$) is $4.0$.
## Step2: Calculate $\Delta EN$ for $F - F$ bond
The formula for $\Delta EN$ is $\Delta EN=\vert EN_1 - EN_2\vert$. For $F - F$ bond, $EN_1 = EN_2=4.0$. So $\Delta EN=\vert4.0 - 4.0\vert = 0$.
## Step3: Classify the bond type
Since $\Delta EN = 0<0.5$, according to the given criteria,  the bond is non - polar covalent.
## Step4: Analyze dipole formation
Since the bond in $F_2$ is non - polar covalent (no difference in electronegativity between the two $F$ atoms), there are no polar bonds.

# Answer:
1. $4.0$
2. $0$
3. non - polar covalent
4. polar

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Question

Explanation:

Step1: Determine electronegativity of fluorine

Step2: Calculate \(\Delta EN\) for \(F - F\) bond

Step3: Classify the bond type

Step4: Analyze dipole formation

Answer: