Question

Consider the elements \(\mathrm{N}, \mathrm{F}, \mathrm{Si}, \mathrm{Rb},\) Te, and Ir. From this list, select the element that \((\mathbf{a})\) 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, (e) is a transition metal, \((\mathbf{f})\) forms four covalent bonds to achieve octet.

Short answer

(a) Fluorine (F) is the most electronegative element. (b) Tellurium (Te) exhibits a maximum oxidation state of +6. (c) Rubidium (Rb) loses an electron most readily. (d) Silicon (Si) forms π bonds most readily. (e) Iridium (Ir) is a transition metal. (f) Silicon (Si) forms four covalent bonds to achieve an octet.

Step-by-step solution

Identify the elements on the periodic table

First, locate the given elements on the periodic table. Knowing the periodic trends and the properties of different sections of the periodic table will help us in answering the questions.

Determine the most electronegative element

Electronegativity increases from left to right across a period and decreases from top to bottom down a group. Among the given elements, Fluorine (F) is the most electronegative element because it lies furthest to the right and the highest up in the periodic table. Answer (a): Fluorine (F)

Determine the element exhibiting a maximum oxidation state of +6

Elements from Group 16 (the chalcogens) are known to exhibit a maximum oxidation state of +6. Among the given elements, Tellurium (Te) belongs to Group 16. Answer (b): Tellurium (Te)

Determine the element that loses an electron most readily

The easiest element to lose an electron is the one with the lowest ionization energy. Ionization energy generally decreases from top to bottom down a group, and from right to left across a period. Among the given elements, Rubidium (Rb) is the most likely to lose an electron since it lies furthest to the left and the lowest down the periodic table. Answer (c): Rubidium (Rb)

Determine the element that forms π bonds most readily

Elements in Group 14 have the ability to form multiple bonds due to their ability to form empty p orbitals from their higher energy d orbitals, which can form π bonds with the elements they are bonded to. Among the given elements, Silicon (Si) belongs to Group 14. Answer (d): Silicon (Si)

Determine the transition metal element

Transition metals are elements that have partially filled d orbitals. They are located in groups 3-12 of the periodic table. Among the given elements, Iridium (Ir) is a transition metal, as it belongs to Group 9. Answer (e): Iridium (Ir)

Determine the element that forms four covalent bonds to achieve an octet

Elements from Group 14 can form four covalent bonds to achieve a complete octet, as they have four valence electrons. Among the given elements, Silicon (Si) belongs to Group 14. Answer (f): Silicon (Si)

Key concepts

Electronegativity

Electronegativity is a chemical property that describes the ability of an atom to attract a shared pair of electrons towards itself within a compound. It plays a crucial role in predicting the type of bond that will form between atoms. On the periodic table, electronegativity values usually increase from left to right across a period and decrease from top to bottom down a group. This is because elements on the right side of the periodic table are more inclined to gain electrons to fill their outer electron shell and become stable.
Fluorine (F), which is situated at the top right of the periodic table, is the element with the highest electronegativity. It is highly efficient at attracting bonding electrons due to its small atomic radius and a large effective nuclear charge. Fluorine's electronegativity value is 3.98, the highest of all elements, which makes it a strong attractor of electrons in chemical bonds.
Understanding electronegativity helps in predicting how atoms interact and bond with each other. An element with high electronegativity will tend to pull electrons towards itself in a bond, often resulting in polar covalent bonds if the electronegativity difference between two atoms is significant.

Oxidation State

The oxidation state of an element in a compound is a measure of the degree of oxidation of an atom. It is an important concept in chemistry, as it helps to determine the electron flow during chemical reactions. The oxidation state is often considered as an indicator of an atom's ability to lose, gain, or share electrons when forming chemicals bonds.
Elements in the periodic table exhibit different oxidation states depending on their group. For example, elements in Group 16, known as the chalcogens, can show a maximum oxidation state of +6. This is particularly notable in elements such as Tellurium (Te), which embodies this property.
Examining the oxidation state aids in writing chemical equations and understanding reaction mechanisms. It determines what elements are reduced or oxidized in a reaction, leading to the understanding of how electrons are transferred, which is crucial for grasping redox reactions.

Transition Metals

Transition metals are defined as elements found in Groups 3-12 of the periodic table. They are characterized by having partially filled d orbitals, which makes them unique in many ways. Transition metals like Iridium (Ir) belong to this category and possess distinctive properties such as forming various oxidation states, having a strong tendency to form coordination complexes, and displaying magnetic properties due to unpaired d electrons.
These metals are highly valuable in industrial processes, often used as catalysts due to their ability to change oxidation states easily. This flexibility allows them to facilitate numerous chemical reactions, making them indispensable in fields like chemistry and materials science.

• Generally have high melting and boiling points.
• Exhibit metallic properties such as conductivity and malleability.
• Can form complex ions with vibrant colors.

Understanding transition metals is vital to exploring the production of advanced materials and establishing innovative technological applications due to their unique properties.