Question 1: 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 towards increased reactivity. This is because sodium has one valence electron in its outer shell, which makes it more likely to lose that electron and form a positively charged ion. Neon, on the other hand, has a full outer shell of electrons and is therefore very stable and unreactive. Additionally, sodium's larger atomic radius compared to neon allows for easier electron loss and greater reactivity.
Question 2: The periodic table does show a pattern with regard to ionic charge. Elements in the same group or column on the periodic table often exhibit similar ionic charges. This is because elements in the same group have the same number of valence electrons. For example, all elements in group 1A (alkali metals) have one valence electron and commonly form +1 ions. Similarly, elements in group 2A (alkaline earth metals) have two valence electrons and commonly form +2 ions. This pattern continues throughout the periodic table, with the number of valence electrons influencing the ionic charge of an element.
Writing question’s for chemistry
Questions 1: 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.
Question 2:The periodic table is arranged by various patterns. Is there a pattern with regard to ionic charge? In three to five sentences, explain your reasoning and provide specific examples.
1 answer