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Chemistry
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a) How are the electron configurations of fluorine (F) and chlorine (Cl) are similar?

b) How are they different? 

c) How do you expect the electron configurations of bromine (Br) and iodine (I) to be similar to those of fluorine and chlorine?

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Related questions

On the basis of electron configurations, explain the following observations:
a) the electron affinity for nitrogen is lower than carbon
b) the electron affinity for sulfur is lower than chlorine
c) the electron affinity for iodine is lower than bromine

Consider the first ionization energy of neon and the electron affinity of fluorine. (a) Write equations, including electron configurations, for each process. (b) These two quantities have opposite signs. Which will be positive, and which will be negative? (c) Would you expect the magnitudes of these two quantities to be equal? If not, which one would you expect to be larger?

Please answer all questions

1. Which type of chemical bond involves the transfer of electrons?

A. Ionic

B. Polar covalent

C. Nonpolar covalent

2. A polar covalent bond will form between which two atoms?

A. Beryllium and fluorine (group 1 and group 7)

B. Hydrogen and chlorine (group 7)

C. Sodium and oxygen (group 1 and group 6)

D. Fluorine and fluorine (group 7)

3. A nonpolar covalent bond will form between which two atoms?

A. Potassium and chlorine

B. Hydrogen and chlorine

C. Sodium and bromine

D. Chlorine and chlorine

4. As the difference in electronegativity between two atoms increases, the polarity of a bond between those two atoms

A. increases.

B. decreases.

C. remains the same.

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