Question

The position of the clement in the periodic table with its outer electronic configuration \(3 \mathrm{~s}^{2} 3 \mathrm{p}^{4}\) is (1) IV period, VIB group (2) IIl period, VIA group (3) IV period, IVB group (4) IIl period, IVB group

Short answer

(2) III period, VIA group

Step-by-step solution

- Determine the Period

Look at the principal quantum number of the outermost electrons. The configuration given is 3s² 3p⁴. The highest principal quantum number is 3, which means the element is in the 3rd period.

- Count Outer Electrons

Add the number of electrons in the outermost s and p orbitals. The configuration is 3s² 3p⁴, thus the total number of outer electrons is 2 + 4 = 6.

- Identify the Group

Elements with 6 outer electrons are in group 16 (VIA group) of the periodic table.

- Verify against Given Options

The element is in the III period and VIA group. Compare this information to the options given.

Key concepts

Electronic Configuration

Electronic configuration describes the arrangement of electrons in an atom. For our problem, the configuration given is 3s² 3p⁴. This notation tells us about the distribution of electrons in different energy levels and orbitals:

• 3s² means there are two electrons in the 3s orbital.
• 3p⁴ means there are four electrons in the 3p orbital.

The numbers before the letters (3 in this case) indicate the principal quantum number, which tells us about the energy level and the approximate distance of the electrons from the nucleus.
Understanding electronic configuration is essential for determining many properties of an element, such as its chemical reactivity and placement in the periodic table.

Period Determination

Determining the period of an element in the periodic table is straightforward once you understand the electronic configuration. The period of an element is indicated by the highest principal quantum number observed in its configuration.
In our example, the configuration is 3s² 3p⁴. The highest principal quantum number here is 3, which tells us that the element belongs to the 3rd period.
Each period on the periodic table corresponds to the filling up of a set of orbitals by electrons. Thus, knowing the principal quantum number directly helps us locate the element's period in the table.

Group Classification

Group classification involves determining which column (group) of the periodic table an element belongs to by looking at the number of outer electrons (valence electrons).
In our configuration 3s² 3p⁴, we count the valence electrons in both the s and p orbitals of the highest energy level:

• There are 2 electrons in the 3s orbital.
• There are 4 electrons in the 3p orbital.

Adding these gives us a total of 6 outer electrons.
Elements with 6 valence electrons are placed in Group 16, also known as Group VIA. This group includes oxygen, sulfur, and other similar elements known for their reactive properties.

Outer Electrons Counting

Counting outer electrons is key for determining the reactive properties and group placement of an element. The outer electrons, also known as valence electrons, are those located in the outermost shell of an atom, and they play a significant role in chemical bonding and reactions.
For the given configuration 3s² 3p⁴, we analyze:

• 3s² means 2 electrons in the 3s orbital.
• 3p⁴ means 4 electrons in the 3p orbital.

Add the electrons in these orbitals: 2 (from 3s) + 4 (from 3p) = 6 outer electrons.
These 6 valence electrons signify that this element will be in Group 16 (VIA), aligning it with elements that typically form -2 anions and participate in forming compounds with metals and nonmetals.