The element with atomic number 62 belongs to the III B group and 6th period.

Explanation:

Atomic number:

The atomic number of an element represents the number of protons present in the nucleus of an atom. It is a unique identifier for each element on the periodic table.

Group and Period:

The periodic table is organized into groups and periods. Groups are the vertical columns, while periods are the horizontal rows. Each group contains elements with similar properties, and each period represents the number of electron shells or energy levels an atom has.

Determining the element:

To determine the element with atomic number 62, we need to locate it on the periodic table.

First, we find the period:

The atomic number of an element corresponds to the period it belongs to. In this case, the atomic number is 62, so the element belongs to the 6th period.

Next, we find the group:

To determine the group, we need to use the electron configuration of the element. The electron configuration is the arrangement of electrons in an atom's energy levels.

The electron configuration of the element with atomic number 62 is [Xe] 4f^7 5d^1 6s^2.

From this electron configuration, we can determine that the element belongs to the f-block, specifically the 4f subshell. The f-block elements are also known as the inner transition metals.

Now, we need to determine the group within the f-block. The number of electrons in the outermost s or d subshell determines the group number. In this case, the outermost s subshell has 2 electrons and the d subshell has 1 electron, so the element belongs to the III B group.

Therefore, the element with atomic number 62 belongs to the III B group and 6th period.