Question

two main - group elements are highlighted in the outline of the periodic table below: what can you say about these elements without knowing exactly which they are? use that knowledge to answer the questions in the fo important: do not try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific to. you will also be marked wrong for any answer, correct or not, that cant be determined from the rough location of each marked elem

Explanation:

Step1: Flame - test property

Metals (especially group - 1 and group - 2) tend to give colored flames. Element \(X\) is likely a metal (from the left - hand side of the periodic table, group - 1 or 2). Non - metals (where \(Y\) is likely from, right - hand side excluding noble gases) do not give such colored flames in the same way. So, element \(X\) is more likely to glow green or yellow in a flame.

Step2: Ionic compound formation with chlorine

Chlorine forms ionic compounds with metals. Element \(X\) (from the left, likely metal) will form an ionic compound with chlorine (by losing electrons to \(Cl\) which gains electrons). Element \(Y\) (non - metal) may form covalent compounds (by sharing electrons) rather than ionic with \(Cl\) (except for some polyatomic ions in complex cases, but from the position, metal - non - metal ionic is more straightforward here). So, element \(X\) is more likely to form an ionic compound with chlorine.

Step3: Anion in ionic compound

Anions are negatively charged ions, formed by non - metals (which gain electrons). Element \(Y\) (from the right - hand side, non - metal) is more likely to gain electrons (as non - metals have higher electron - affinity in general compared to metals on the left) and be an anion in an ionic compound.

Answer:

1. Element \(X\)
2. Element \(X\)
3. Element \(Y\)