does reactivity increase down a group for metals

the atomic radius increases with increasing number of shells, so the outer electrons are further from the attraction of the nucleus.

We can explain this in terms of atomic radius, shielding and nuclear charge: It is clear from the data that we would expect reactivity to increase down the group as the energy required to remove the two outer shell electrons decreases and the 2+ ion becomes easier to form. It is the sum of these ionisation energies which determines the relative reactivity of the elements: Element Note that ionisation energies are defined for moles of atoms in the gaseous state, so this must be reflected in the state symbols: The energy required to remove the first of these electrons is the first ionisation energy, and the energy required to remove the second electron is the second ionisation energy. Group 2 elements react by losing two electrons to form M 2+ ions:

Sr 5s 2 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 5s 2īa 6s 2 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 6 6s 2Īll the atoms of Group 2 elements have two electrons in their outer shell. To understand the reactions of Group 2 it helps to consider their electron arrangements:Ĭa 4s 2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 *… except for beryllium which behaves differently because of its very small size, forming only covalent compounds.

conduct electricity when molten or in solution (when the ions are mobile and able to act as charge carriers).are colourless in solution ( white when solid).Its other properties closely resemble those of barium. Note: Radium is too radioactive to handle in a normal laboratory. have good conductivity of electricity (have delocalised electrons).are metals (beryllium is a semi-metal 0r metalloid).

Does reactivity increase down a group for metals