Arrange the following elements in terms of increasing reactivity:
1. Be, Ba, Sr, Mg
2. Na, K, Cs, Li
list in order down their column in the periodic table.
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To arrange the elements in terms of increasing reactivity, we need to consider their positions in the periodic table. Reactivity generally increases as we move down a group, and decreases as we move across a period from left to right.
1. Be, Ba, Sr, Mg:
To determine the order of reactivity for Be, Ba, Sr, and Mg, let's consider their positions in the periodic table:
- Be (Beryllium) is in Group 2, Period 2.
- Ba (Barium) is in Group 2, Period 6.
- Sr (Strontium) is in Group 2, Period 5.
- Mg (Magnesium) is in Group 2, Period 3.
Since all these elements are in the same group, their reactivity is primarily determined by their atomic radius, which increases down the group. Based on this, the order of increasing reactivity will be:
Be < Mg < Sr < Ba
2. Na, K, Cs, Li:
To determine the order of reactivity for Na, K, Cs, and Li, let's consider their positions in the periodic table:
- Na (Sodium) is in Group 1, Period 3.
- K (Potassium) is in Group 1, Period 4.
- Cs (Cesium) is in Group 1, Period 6.
- Li (Lithium) is in Group 1, Period 2.
Similar to the previous example, the reactivity of these elements will also increase as we move down Group 1. Based on this, the order of increasing reactivity will be:
Li < Na < K < Cs