which element will have the greater metallic character?
Cs or Sr
Ge or In
Al or K
Sr or Rb
Left to right on periodic table metallic character decreases (K is more metallic than Br.
Top to bottom in periodic table metallic character increases.
Cs is the most electropositive element in the table; F is the most electronegative element in the table.
To determine the element that has greater metallic character, we need to consider a few factors. Metallic character generally refers to the ability of an element to exhibit metallic properties, such as metallic luster, high electrical conductivity, and malleability.
To compare the metallic character between two elements, we need to look at their relative positions in the periodic table. Moving from left to right across a period, metallic character generally decreases, whereas it increases from top to bottom down a group.
1. Cs or Sr:
Both cesium (Cs) and strontium (Sr) are located in Group 1 (the alkali metals) of the periodic table. As we move down Group 1, metallic character increases. Therefore, cesium has greater metallic character than strontium.
2. Ge or In:
Germanium (Ge) is a metalloid located in Group 14 of the periodic table, whereas indium (In) is a metal located in Group 13. Metallic character increases down a group, so indium has greater metallic character than germanium.
3. Al or K:
Aluminum (Al) is a metal located in Group 13, while potassium (K) is an alkali metal located in Group 1. Similar to the previous comparison, metallic character increases down a group. Therefore, potassium has greater metallic character than aluminum.
4. Sr or Rb:
Both strontium (Sr) and rubidium (Rb) are located in Group 1, but rubidium is located below strontium. Thus, rubidium has greater metallic character than strontium.
In summary:
- Cs > Sr
- In > Ge
- K > Al
- Rb > Sr
To determine which element will have a greater metallic character, we need to compare their positions on the periodic table. In general, metallic character increases as you move down a group or to the left across a period on the periodic table.
Comparing Cs (Cesium) and Sr (Strontium):
Both Cs and Sr are in the same group (Group 1) and period (Period 5). As we move down the group, metallic character increases. Therefore, Cs will have a greater metallic character than Sr.
Comparing Ge (Germanium) and In (Indium):
Ge is located to the left of In on the periodic table. As we move to the left across a period, metallic character increases. Therefore, Ge will have a greater metallic character than In.
Comparing Al (Aluminum) and K (Potassium):
Al is located to the right of K on the periodic table. As we move to the left across a period, metallic character decreases. Therefore, K will have a greater metallic character than Al.
Comparing Sr (Strontium) and Rb (Rubidium):
Both Sr and Rb are in the same group (Group 2) and period (Period 5). As we move down the group, metallic character increases. Therefore, Sr will have a greater metallic character than Rb.