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. The reactivity of elements generally increases as you move from right to left across a period and from top to bottom within a group. Two reasons for this increase in reactivity are the decrease in effective nuclear charge and the increase in atomic size. As you move from neon to sodium, the effective nuclear charge decreases because there is an increase in the number of inner electron shells, which leads to a weaker attraction between the outermost electron and the nucleus. Additionally, sodium has a larger atomic size compared to neon, which means that its outermost electron is farther from the nucleus and is therefore easier to remove or interact with other atoms.
Moving from the element with atomic number 10 (neon, Ne) to atomic number 11 (sodium, Na) on the periodic table, there is a change from a non-reactive element to a reactive one. The direction of the change is towards increased reactivity. Two reasons for this change are the difference in electron configuration and the trend in electronegativity. Neon has a full valence shell with 8 electrons, making it stable and unreactive. Sodium, on the other hand, has one electron in its outermost shell, making it eager to lose that electron and become stable. Additionally, sodium has a lower electronegativity than neon, which means it is more likely to lose its electron 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 decrease in reactivity. This is because the reactivity of elements generally decreases as you move from left to right across a period in the periodic table. Two reasons for this change are the increasing number of protons in the nucleus and the increasing number of electrons in the outermost energy level. The increasing nuclear charge pulls the electrons closer to the nucleus, making it more difficult for the outermost electron to be easily gained or lost, thus decreasing reactivity. Additionally, the increasing number of electrons in the outermost energy level leads to a greater shielding effect, reducing the attraction between the outermost electron and the nucleus, and further decreasing reactivity.
