The reactivity trends of inorganic compounds within a group and across a period on the periodic table are influenced by several factors related to their electronic configuration. These factors include:1. Atomic size: As you move down a group, the atomic size increases due to the addition of electron shells. This causes a decrease in the effective nuclear charge experienced by the valence electrons, making it easier for them to be lost or gained in a chemical reaction. Conversely, as you move across a period, the atomic size decreases due to an increase in the effective nuclear charge, making it harder for the valence electrons to be lost or gained.2. Ionization energy: Ionization energy is the energy required to remove an electron from an atom. As you move down a group, ionization energy decreases due to the increased atomic size and shielding effect. This makes it easier for elements to lose electrons and participate in chemical reactions. Across a period, ionization energy increases, making it more difficult for elements to lose electrons and react.3. Electron affinity: Electron affinity is the energy change associated with the addition of an electron to an atom. As you move down a group, electron affinity decreases due to the increased atomic size and shielding effect, making it less favorable for elements to gain electrons in a reaction. Across a period, electron affinity generally increases, making it more favorable for elements to gain electrons and react.4. Electronegativity: Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. As you move down a group, electronegativity decreases due to the increased atomic size and shielding effect. This results in a lower tendency for elements to attract electrons and form bonds. Across a period, electronegativity increases, leading to a higher tendency for elements to attract electrons and participate in chemical reactions.5. Valence electrons: The number of valence electrons in an element's electronic configuration determines its reactivity. Elements with a full or nearly full valence electron shell are less reactive, while elements with only a few valence electrons or nearly empty valence shells are more reactive. This is because elements with a full or nearly full valence shell require more energy to lose or gain electrons, while elements with only a few valence electrons can easily lose or gain electrons to achieve a stable electronic configuration.In summary, the reactivity trends of inorganic compounds within a group and across a period on the periodic table are influenced by factors such as atomic size, ionization energy, electron affinity, electronegativity, and the number of valence electrons in their electronic configuration. These factors collectively determine the ease with which elements can lose or gain electrons and participate in chemical reactions.