What is the trend in ionization energy as you move down the group in s-block elements?
Practice Questions
1 question
Q1
What is the trend in ionization energy as you move down the group in s-block elements?
Increases
Decreases
Remains constant
Varies irregularly
Ionization energy decreases as you move down the group in s-block elements due to increased atomic size.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the trend in ionization energy as you move down the group in s-block elements?
Solution: Ionization energy decreases as you move down the group in s-block elements due to increased atomic size.
Steps: 6
Step 1: Understand what ionization energy is. It is the energy required to remove an electron from an atom.
Step 2: Identify what s-block elements are. They are found in Group 1 (alkali metals) and Group 2 (alkaline earth metals) of the periodic table.
Step 3: Recognize that as you move down a group in the periodic table, the number of electron shells increases.
Step 4: Realize that with more electron shells, the size of the atom increases. This means the outermost electron is further from the nucleus.
Step 5: Understand that the further an electron is from the nucleus, the less tightly it is held by the positive charge of the protons.
Step 6: Conclude that because the outermost electron is held less tightly, it requires less energy to remove it, leading to a decrease in ionization energy.
