Moving from the element with atomic number 10 to atomic number 11 on the periodic table, there is a change in reactivity. In three to five sentences, identify the direction of the change, and give two reasons for the change.
Moving from the element with atomic number 10 (neon) to atomic number 11 (sodium) on the periodic table, there is an increase in reactivity. Sodium is more reactive than neon for two main reasons. Firstly, as we move across a period from left to right, the number of valence electrons increases. In the case of neon, it has a full valence shell with 8 electrons, while sodium only has one valence electron. This makes sodium more eager to lose that electron and form a positive ion, increasing its reactivity. Secondly, the atomic radius decreases as we move across a period. The smaller atomic size of sodium compared to neon leads to a higher electronegativity, making sodium more likely to attract electrons and react with other elements.
Moving from the element with atomic number 10 (neon) to atomic number 11 (sodium) on the periodic table, there is a change in reactivity. The direction of the change is an increase in reactivity. This is because sodium has only one valence electron, making it relatively unstable and eager to lose that electron and achieve a stable electron configuration. Additionally, sodium is located in Group 1 (alkali metals) of the periodic table, and alkali metals are known for their high reactivity due to the low ionization energy required to remove their valence electron.
To identify the direction of the change in reactivity while moving from the element with atomic number 10 (neon) to atomic number 11 (sodium), we need to understand some key factors. Reactivity generally increases as you go down a group and decreases as you go across a period on the periodic table. Since neon is found in the noble gases group (Group 18), it has a full valence shell and is stable, resulting in low reactivity. However, sodium is found in Group 1 (alkali metals), which only has one valence electron. This makes sodium highly reactive, as it easily loses that one electron to achieve a stable electron configuration. So, in moving from neon to sodium, the direction of change in reactivity is an increase. The two reasons for this change are the difference in valence electrons (sodium has one valence electron while neon has eight) and the tendency to lose that one electron to attain stability.
