Question

question 4. for each pair of elements, identify which element is more reactive.
a) carbon (c), oxygen (o)
b) aluminum (al), rubidium (rb)
c) fluorine (f), chlorine (cl)
d) beryllium (be), barium (ba)

Explanation:

Step1: Analyze Carbon (C) and Oxygen (O)

Carbon and oxygen are non - metals. In the periodic table, for non - metals in the same period, reactivity increases from left to right. Carbon is in group 14 and oxygen is in group 16, and they are in the same period (period 2). So, oxygen is more reactive.

Step2: Analyze Aluminum (Al) and Rubidium (Rb)

Aluminum is a metal from group 13 and period 3. Rubidium is an alkali metal from group 1 and period 5. For metals, reactivity increases as we go down a group and from right to left across a period. Rubidium is lower in the group 1 (alkali metals) compared to lithium, sodium, etc., and is more reactive than aluminum. So, rubidium is more reactive.

Step3: Analyze Fluorine (F) and Chlorine (Cl)

Fluorine and chlorine are halogens (group 17). For non - metals in the same group, reactivity decreases as we go down the group because the atomic size increases, and it becomes harder to gain an electron. Fluorine is at the top of group 17, so fluorine is more reactive.

Step4: Analyze Beryllium (Be) and Barium (Ba)

Beryllium and barium are alkaline earth metals (group 2). For metals in the same group, reactivity increases as we go down the group because the atomic size increases, and it becomes easier to lose electrons. Barium is lower in group 2 than beryllium, so barium is more reactive.

Answer:

a) Oxygen (O)
b) Rubidium (Rb)
c) Fluorine (F)
d) Barium (Ba)