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Chapter 5: Problem 107

What is the most electronegative element in the periodic table? What is the least electronegative element? What kind of compound would form if these two elements were brought together?

Short Answer

Expert verified
The most electronegative element in the periodic table is Fluorine (F) with an electronegativity value of 3.98, while the least electronegative element is Francium (Fr) with an electronegativity value of 0.7. When these two elements are brought together, they form an ionic compound called Francium fluoride (FrF), where Fluorine gains an electron (F-) and Francium loses an electron (Fr+).

Step by step solution

01

Identify the most electronegative element

The most electronegative element can be found in the upper right corner of the periodic table, excluding the noble gases. This element is Fluorine (F) with an electronegativity value of 3.98 on the Pauling scale.
02

Identify the least electronegative element

The least electronegative element can be found in the lower left corner of the periodic table. This element is Francium (Fr) with an electronegativity value of 0.7 on the Pauling scale.
03

Determine the type of compound that would form between these two elements

Fluorine, being highly electronegative, will attract electrons and develop a negative charge. Francium, being least electronegative, will lose electrons and develop a positive charge. When these two elements are brought together, they will form an ionic compound with Fluorine gaining an electron (F-) and Francium losing an electron (Fr+). The compound formed is Francium fluoride (FrF).

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Most popular questions from this chapter

The acetate ion has the formula \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\). Draw a dot diagram for it given the following atomic connections. (Hint: Watch for resonance forms.)

Which one of the following statements is true about \(\mathrm{BeH}_{2} ?\) (a) It is ionic with \(\mathrm{H}\) as the anion. (b) It is ionic with \(\mathrm{H}\) as the cation. (c) It has polar covalent bonds with a partial negative charge on \(\mathrm{H}\). (d) It has polar covalent bonds with a partial positive charge on \(\mathrm{H}\).

Draw dot diagrams for \(\mathrm{Cl}_{2}\) and for \(\mathrm{MgCl}_{2}\) (put \(\mathrm{Mg}\) in the middle) that agree with the type of bonding occurring in each. (That is, show electrons as being shared or transferred, and if they are transferred, show the charges of the resulting ions.)

Without knowing the electronegativity values, in what situation can you be absolutely sure that the bonding between two atoms will be purely covalent?

Give the proper name for the following binary covalent compounds: (a) \(\mathrm{PCl}_{3}\) (b) \(\mathrm{SO}_{2}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{4}\) (d) \(\mathrm{P}_{5} \mathrm{O}_{10}\)
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