How do atomic structures vary across the periodic table?

Atomic structures vary across the periodic table in terms of their atomic number, electron configuration, and chemical properties.

The atomic structure of an element is determined by its atomic number, which is the number of protons in its nucleus. As you move across the periodic table from left to right, the atomic number increases. This means that the number of protons in the nucleus, and hence the positive charge of the nucleus, increases. This also increases the number of electrons in the neutral atom, which are arranged in energy levels or shells around the nucleus.

The electron configuration of an atom, which describes the distribution of electrons in its atomic orbitals, also changes across the periodic table. The periodic table is structured so that elements with similar electron configurations are grouped together. For example, all elements in group 1 (the first column of the periodic table) have one electron in their outermost energy level, while all elements in group 18 (the last column) have a full outermost energy level.

The variation in atomic structure across the periodic table also leads to differences in chemical properties. Elements in the same group (vertical column) of the periodic table have similar chemical properties because they have the same number of electrons in their outermost energy level. As you move from left to right across a period (horizontal row), the elements become less metallic and more non-metallic in their properties. This is because the number of electrons in the outermost energy level increases, making the element less likely to lose electrons and form positive ions.

In summary, the atomic structure of elements varies across the periodic table in terms of their atomic number, electron configuration, and chemical properties. This variation is what gives each element its unique set of properties and determines its position in the periodic table.