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Chapter 22: Problem 13

Consider the elements \(\mathrm{N}, \mathrm{F}\), Si, Rb, Te, and Ir. From this list, select the element that (a) is most electronegative, \((\mathbf{b})\) exhibits a maximum oxidation state of \(+6,(\mathbf{c})\) loses an electron most readily, (d) forms \(\pi\) bonds most readily, \((\mathbf{e})\) is a transition metal, (f) forms four covalent bonds to achieve octet.

Short Answer

Expert verified
(a) F, (b) Te, (c) Rb, (d) Si, (e) Ir, (f) Si.

Step by step solution

01

Identify the Most Electronegative Element

Electronegativity refers to the tendency of an atom to attract electrons. Among the given elements, fluorine ( F ) is known to be the most electronegative element on the periodic table.
02

Identify the Element with Maximum Oxidation State of +6

Elements that can exhibit a maximum oxidation state of +6 typically have a high number of valence electrons that can be paired with oxygen. Tellurium ( Te ), a chalcogen like sulfur ( S ), commonly exists in the +6 oxidation state in compounds such as TeO_3^2鈭� .
03

Identify the Element that Loses an Electron Most Readily

Elements that lose an electron most readily typically possess a single electron in their valence shell, like alkali metals. Rubidium ( Rb ) is an alkali metal and will lose its single valence electron easily to achieve a stable electron configuration.
04

Identify the Element that Forms 蟺 Bonds Most Readily

C0 bonds are formed when there is overlapping of p d-orbitals. Elements like silicon ( Si ) readily form C0 bonds by overlapping of orbitals, especially in compounds like silicones and silicates.
05

Identify the Transition Metal

Transition metals are elements that have partially filled d electron subshells. Iridium ( Ir ) is in the d -block of the periodic table, making it a transition metal.
06

Identify the Element that Forms Four Covalent Bonds to Achieve Octet

Atoms forming four covalent bonds often have four valence electrons and need four more to achieve an octet. Silicon ( Si ) has four valence electrons and forms four covalent bonds, like in silicon tetrachloride ( SiCl_4 ).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electronegativity
Electronegativity measures an atom's ability to attract and hold onto electrons. It's a key concept in understanding how different elements interact in chemical reactions. Fluorine ( F ) is famously known as the most electronegative element on the periodic table due to its high affinity for electrons. This characteristic means that fluorine will strongly attract electrons when forming chemical bonds. This property not only gives fluorine its reactive nature but also makes it a critical player in forming polar covalent bonds. Understanding electronegativity helps students grasp why certain molecules have specific shapes and characteristics due to electron distribution.
Oxidation States
An oxidation state represents the degree of oxidation or gain of an electron for an element in a compound. Elements can exhibit different oxidation states, depending on the number of electrons available for bonding or transfer. For instance, tellurium ( Te ) can exist in various oxidation states, but it notably shows a maximum oxidation state of +6. In compounds like TeO_3^{2-} , tellurium achieves its highest oxidation state. This capability results from tellurium's ability to make multiple bonds with oxygen and other elements, allowing for diverse chemical behavior and reactivity.
Transition Metals
Transition metals are elements located in the center of the periodic table, specifically those in the d -block. They are recognized by their ability to form complex ions, variable oxidation states, and colored compounds. Iridium ( Ir ) is a classic example of a transition metal, known for its durability and high melting point. Transition metals are unique because they have incompletely filled d electron subshells, which allow them to form a wide variety of compounds. These metals often exhibit intriguing properties like magnetism, conduction, and catalytic activity, making them invaluable in industries and technologies.
Covalent Bonds
Covalent bonds involve sharing electrons between atoms, allowing them to achieve full electron shells akin to a noble gas configuration. An excellent example is silicon ( Si ), which forms four covalent bonds to complete its octet configuration effectively. This characteristic enables silicon to form a vast array of compounds, such as silicon tetrachloride ( SiCl_4 ). Covalent bonding is central to molecular chemistry, as it determines the structure and properties of molecules. Students interested in covalent bonds will learn about molecular geometry, hybridization, and resonance, crucial for understanding chemical behavior.
蟺 Bonds
蟺 Bonds, or pi bonds, arise from the side-to-side overlap of p d-orbitals. Unlike sigma bonds, which involve end-to-end overlaps, 蟺 bonds provide added complexity to molecular structures. Silicon ( Si ), although primarily forming sigma bonds, can engage in 蟺 bonding particularly in complex structures like silicones and silicates. These bonds provide rigidity and facilitate the formation of conjugated systems, which have unique properties like delocalized electron clouds. Understanding 蟺 bonds is essential for grasping concepts like double and triple bonding in organic chemistry, influencing reactivity and stability.

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Most popular questions from this chapter

Complete and balance the following equations: (a) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(I)+\mathrm{O}_{2}(g) \longrightarrow\) (c) \(\mathrm{MnO}_{2}(s)+\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{AlP}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (e) \(\mathrm{Na}_{2} \mathrm{~S}(s)+\mathrm{HCl}(a q) \longrightarrow\)

Consider the elements \(\mathrm{Ba}, \mathrm{Na}, \mathrm{O}, \mathrm{B}, \mathrm{P},\) and \(\mathrm{Kr}\). From this list, select the element that (a) is most electronegative, (b) has the greatest metalliccharacter, \((\mathbf{c})\) most readily forms a positive ion, \((\mathbf{d})\) exhibits a maximum oxidation sate of +5 , (e) exists as monoatomic gas at room temperature, (f) has multiple allotropes.

Give the chemical formula for (a) copper(II) carbonate, (b) carbon monoxide, (c) magnesium hydrogen carbonate, (d) lithium acetylide, (e) carbon tetrafluoride.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium azide, (b) ammonium ion, (c) nitrous acid, (d) magnesium nitride, \((\mathbf{e})\) diazene, \((\mathbf{f})\) sodium nitrate, (g) nitrogen trifluoride, \((\mathbf{h})\) nitric acid.

What is the anhydride for each of the following acids: (c) \(\mathrm{HNO}_{2}\) (a) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (b) \(\mathrm{HClO}_{3}\), (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\), (e) \(\mathrm{H}_{3} \mathrm{PO}_{4} ?\)
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