Question

State whether the following statements are true or false. \(" s^{n}\) and "p" block elements except zero group are known as representative elements.

Short answer

Answer: True.

Step-by-step solution

Understand the periodic table and the blocks

The periodic table is divided into four blocks: s, p, d, and f. The s block elements have their outermost electrons in "s" orbitals, the p block elements have their outermost electrons in "p" orbitals, and so on. The zero group, also known as the noble gases, are a part of the p block and have fully filled "p" orbitals.

Identify representative elements

Representative elements, or main group elements, are those that have their outermost electrons in either "s" or "p" orbitals. They display a wide range of physical and chemical properties and are often used to predict trends in the periodic table. One key characteristic of representative elements is that their group number matches the number of outermost (valence) electrons.

Determine if the statement is true

Now that we understand the blocks and representative elements, let's re-read the statement: \(" s^{n}\) and "p" block elements except zero group are known as representative elements. Both the s and p block elements belong to the main group (representative elements), as their valence electrons are in the "s" or "p" orbitals. The statement also mentions excluding the zero (noble gases) group, which is already a part of the p block. Therefore, the statement is accurate: elements in the s and p blocks, excluding the noble gases, are known as representative elements. The statement is #tag_math# \boxed{\text{True}} #tag_math#

Key concepts

Understanding the Periodic Table

The periodic table is the roadmap of the chemical elements, charting their symphony based on atomic number and electron configurations. It gives a visual structure to the entire field of chemistry, enabling students and scientists alike to predict how these elements will behave in reactions. Elements are divided into several blocks—these relate to the subshell in which the outermost electrons are found.

For example, hydrogen and helium are part of the s block because their electrons occupy the 's' orbital. Meanwhile, the p block is home to a diverse group of elements starting with boron and progressing through the table to the noble gases, but excluding them. The noble gases, while part of the p block, are distinct in their inertness and rarely engage in reactions due to their filled p orbitals—hence, they are not representative of the block's typical reactivity.

Taking this into account helps students understand the regular and repeating trends in the periodic table such as ionization energies, electron affinities, and atomic radii, all vital concepts in chemistry that are often presented in homework exercises.

s block Elements

The s block elements, comprising hydrogen, helium, and the elements in groups 1 and 2, are defined by their outermost electrons occupying s orbitals. Group 1 elements (alkali metals) and group 2 elements (alkaline earth metals) are highly reactive, each in their unique way. The reactivity comes from the desire to either lose one electron (in the case of alkali metals) or two electrons (for alkaline earth metals) to achieve a noble gas configuration.

Distinct Features of s block Elements

• They have a single electron (alkali metals) or two electrons (alkaline earth metals) in their outermost s orbital.
• Their valence shells are not completely filled, making them highly reactive.
• These elements tend to form ionic bonds by losing electrons.

Good to remember: since their group number matches the number of valence electrons, these s block elements are foundational in teaching how to predict chemical reactivity and bonding in introductory chemistry.

p block Elements

Meanwhile, the p block elements showcase much more variety in their chemistry. They include metals, nonmetals, and even metalloids, with their valence electrons in the p orbital. The group numbers for these elements are generally 13 to 18, except for helium, which has its distinct place despite having p orbital electrons.

Characterizing p block Elements

• Their valence shell can contain up to six electrons, filling the three p orbitals.
• They can share electrons to form covalent bonds, leading to a vast array of compounds.
• They exhibit multiple oxidation states, reflecting their versatility in forming different types of compounds.

Students often examine how these elements affect trends across the periodic table. For instance, electronegativity increases as you go from left to right across the p block, which is crucial for understanding why oxygen is far more electronegative than carbon.