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Chapter 22: Problem 14

Consider the elements \(\mathrm{Li}, \mathrm{K}, \mathrm{Cl}, \mathrm{C}, \mathrm{Ne},\) and \(\mathrm{Ar}\). From this list select the element that (a) is most electronegative, (b) has the greatest metallic character, (c) most readily forms a positive ion, (d) has the smallest atomic radius, (e) forms \(\pi\) bonds most readily, (f) has multiple allotropes.

Short Answer

Expert verified
(a) Cl (b) K (c) K (d) Ne (e) C (f) C

Step by step solution

01

(a) Most Electronegative Element)

Electronegativity is the ability of an atom to attract electrons in a chemical bond. Elements on the right and upper side of the periodic table have higher electronegativity values, with Fluorine having the highest value. From the given elements, chlorine (Cl) has the highest electronegativity.
02

(b) Element with Greatest Metallic Character)

Metallic character refers to an element's ability to lose electrons and form positive ions or cations. Elements on the left and lower side of the periodic table have higher metallic character. From the given elements, potassium (K) has the greatest metallic character.
03

(c) Element that Most Readily Forms a Positive Ion)

The formation of positive ions occurs when elements lose electrons. Elements with lower ionization energies, usually located on the left and lower side of the periodic table, tend to form positive ions more readily. Potassium (K) has the lowest ionization energy among the given elements, so it most readily forms a positive ion.
04

(d) Element with the Smallest Atomic Radius)

Atomic radius tends to decrease from left to right across a period and increases down a group. In this case, the element with the smallest atomic radius is helium (He), which is not on the list, but among the given elements, the smallest atomic radius belongs to neon (Ne).
05

(e) Element that Forms π Bonds Most Readily)

π bonds are formed by sideways overlap of p orbitals. Elements that commonly form π bonds have valence electrons in the p orbital. The ability to form such bonds depends on the element's bonding requirements. Carbon (C) commonly forms π bonds, as it can make double (C=C) and triple (C≡C) bonds with other carbon atoms.
06

(f) Element with Multiple Allotropes)

Allotropy is the property of some chemical elements to exist in two or more different forms in the same physical state. In this case, carbon (C) has multiple allotropes, such as diamond, graphite, and fullerenes like C60, also known as Buckminsterfullerene.

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