following truth table is correspond
S block elements- valence electrons are filling the s orbitals D block elements- valence electrons are filling the d orbitals P block elements- valence electrons are filling the p orbitals F block elements- valence electrons are filling the f orbitals
The elements of group 18 are known as inert because they havecompletelyfilled atomic orbitals.
The rows on the periodic table correspond to the highest energy level being filled by the elements in that row (period). For example, in period 3, the elements are filling their valence shell in the 3rd energy level from left to right across the period, from 3s1 in sodium to 3s23p6 in argon.
A possible last sublevel for an element in group 18 of the periodic table (noble gases) is f. The noble gases have completely filled s and p orbitals, and the f orbitals would be the next in line for additional electrons.
The d orbitals fill in elements starting from d-block transition metals, which are located in the center of the periodic table, specifically from scandium (Sc) to zinc (Zn). The d orbitals are part of the transition metal series in the periodic table.
The electron configuration kr 5s² 4d¹⁰ 5p⁴ corresponds to the element tellurium (Te). In this configuration, "kr" indicates that the configuration starts from krypton, followed by the filling of the 5s, 4d, and 5p orbitals. Tellurium has an atomic number of 52, placing it in group 16 of the periodic table.
The p-block on the periodic table is the chunk of mostly nonmetals starting at group 13 that ends at the Noble gases on the far right side.
Elements with full s and p orbitals in their highest electron shell are the noble, or inert, gases of the last column on the periodic table: He, Ne, Ar, Kr, Xe, and Rn.
Atomic radii increases moving down a group in the Periodic Table due to the increasing energy levels in the electron configuration and electrons filling in energy levels further away from the nucleus.
The group to which the element belongs and, therefore, its chemical properties.
Carbon, nitrogen, oxygen, and fluorine are elements that would most likely bond using sp3 hybrid orbitals. These elements have valence electrons in the 2s and 2p orbitals, which can hybridize to form four sp3 orbitals for bonding.
Block d contains transition metals, which include elements from group 3 to group 12 on the periodic table. These elements have partially filled d orbitals and exhibit similar chemical properties.