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), there is an increase in reactivity. Firstly, sodium has one less electron in its outermost shell compared to neon, making it more likely to lose this electron and form a positive ion. This makes sodium more reactive than neon, which has a full outer shell and is stable. Secondly, sodium has a larger atomic radius compared to neon due to the addition of an extra energy level. This larger atomic radius allows sodium to interact more easily with other elements, increasing its reactivity.
Moving from the element with atomic number 10 (neon) to atomic number 11 (sodium) on the periodic table, there is an increase in reactivity. This change is because sodium has one more electron in its outermost energy level compared to neon. Firstly, the additional electron in sodium's outermost energy level increases the likelihood of forming chemical bonds with other elements, making it more reactive. Secondly, the electron configuration of sodium makes it easier for the outermost electron to be removed, resulting in greater reactivity in terms of electron donation.
Moving from the element with atomic number 10 (neon) to atomic number 11 (sodium) on the periodic table, there is an increase in reactivity. This is because sodium has one more valence electron than neon, making it more likely to engage in chemical reactions due to its desire to achieve a stable electron configuration. Additionally, sodium's larger atomic size compared to neon allows for easier interaction with other atoms. These factors result in sodium being more likely to readily form compounds and react with other substances compared to neon.
