P Block

To solve the problem of identifying the atomic number of the element in the VA group that comes after nitrogen, we begin with understanding the periodic table groups.

The nitrogen group, also known as group 15 or VA, includes nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). The elements in this group share similar properties, such as forming -3 charges, due to having five valence electrons.

Nitrogen (N) is the first element in this group, with an atomic number of 7. The subsequent element in the VA group is phosphorus (P). The atomic number of phosphorus is 15.

Thus, the atomic number of the element in the VA group, coming after nitrogen, is 15.

To determine the element that belongs to the 2nd group and 3rd period, we need to understand the organization of the periodic table. The periodic table is arranged in periods (horizontal rows) and groups (vertical columns).

• Periods: The 3rd period includes elements in the third row of the periodic table. These elements have their outermost electrons in the third energy level.
• Groups: The 2nd group, also known as Group 2 or the alkaline earth metals, consists of elements that have two electrons in their outermost shell.

Let's analyze the given options:

• Na (Sodium): Located in the 3rd period but in the 1st group, which contains alkali metals with one electron in their outermost shell.
• Al (Aluminum): Located in the 3rd period but in the 13th group, with elements from group 13 having three electrons in their outermost shell.
• Mg (Magnesium): Located in the 3rd period and the 2nd group, fitting the criteria of having two electrons in their outer shell.
• Cl (Chlorine): Located in the 3rd period but in the 17th group, with elements from group 17 having seven electrons in their outermost shell.

Based on this analysis, the correct element that belongs to the 2nd group and 3rd period is Mg (Magnesium).

The question asks us to identify the correct statement regarding the periodic table blocks. The options are related to the characteristics of elements within the s and p blocks.

Understanding the s Block: The s block of the periodic table consists of two groups: Group 1 (alkali metals) and Group 2 (alkaline earth metals). These elements have their outermost electrons in the s subshell. A key feature of these elements is that they are all metals. Typical properties of metals include high electrical and thermal conductivity, malleability, ductility, and a lustrous appearance. Given these properties, the statement that "all s block elements are metals" is indeed correct.

Understanding the p Block: The p block includes Groups 13 to 18 on the periodic table. This block is distinctive because it contains a mix of metals, non-metals, and metalloids. Therefore, not all p-block elements are metals, nor are they all non-metals. This variability in composition makes the remaining options incorrect.

Conclusion: Based on these explanations, the only correct statement is that "all s block elements are metals."