In the long form of the periodic table, the valence shell electronic configuration of 5s²5p4 corresponds to the element present in:

The correct option is Group 16 and period 5.

To determine the group and period of the element from its valence shell electronic configuration, we analyze the configuration step-by-step:

1. Determining the Period:
The period of an element in the periodic table is given by the principal quantum number ($n$) of its outermost (valence) shell.
For the given electronic configuration $5s^{2}5p^4$, the principal quantum number of the outermost shell is $n=5$.
Therefore, the element belongs to Period 5.

2. Determining the Group:
The element has its valence electrons in the $s$ and $p$ subshells, which means it is a p-block element.
For p-block elements, the group number is calculated using the formula:
$\text{Group Number}=10+\text{number of valence electrons}$
Here, the number of valence electrons in the outermost shell ($n=5$) is:
$2\text{(from}5s\text{)}+4\text{(from}5p\text{)}=6$
Thus, the group number is:
$10+6=16$.
Therefore, the element belongs to Group 16.

Combining these findings, the element is present in Group 16 and period 5.