Using only the periodic table arrange the following elements in order of increasing kontration energy carbon, silicon, lead, germanium Lowest Highest Please awwer this question according to the general nales you have learned regarding periodic tren DO NOT base your answer on tabulated values since exceptions may occur. Submit Answer Retry Endre Group more group attempts remaining Clearning Centre Tcheca MacBook Air 5 6 3 Y P. T G F H K V B N M command option Using only the periodic table arrange the following elements in order of increasing ionization energy: selenium, potassium, bromine, krypton Lowest Highest Please answer this question according to the general rules you have learned regarding periodic trends DO NOT base your answer on tabulated values since exceptions may occur. Submit Answer Retry Entire Group more group attempts remaining Pro Ne Can Learning Ceng Technical support MacBook Air B R T T Y P G ? IK v > V B N M 92 command option
The correct answer and explanation is:
To answer the question about arranging the elements in order of increasing ionization energy (Selenium, Potassium, Bromine, Krypton), we need to consider periodic trends.
General Rules for Ionization Energy:
- Ionization Energy tends to increase as we move across a period (from left to right) on the periodic table. This is because elements on the right side of the table have more protons and a greater effective nuclear charge, which holds their electrons more tightly.
- Ionization Energy tends to decrease as we move down a group (from top to bottom) on the periodic table. This is due to the increase in atomic radius, which means the outermost electrons are farther from the nucleus and are less tightly held.
Analysis of the Elements:
- Potassium (K): Potassium is in Group 1 and Period 4. It has a single electron in its outermost shell, and it’s located in the leftmost part of the periodic table. Due to its large atomic radius and low effective nuclear charge on the outermost electron, it will have the lowest ionization energy.
- Selenium (Se): Selenium is in Group 16 and Period 4. Being on the right side of the periodic table compared to potassium, it has a higher effective nuclear charge, but its outer electrons are still somewhat shielded by inner electrons. Its ionization energy will be higher than potassium’s.
- Bromine (Br): Bromine is in Group 17 and Period 4. It is a halogen, and halogens tend to have relatively high ionization energies because they are close to having a full outer shell. Bromine will have a higher ionization energy than selenium.
- Krypton (Kr): Krypton is in Group 18 and Period 4. As a noble gas, krypton has a full outer electron shell, which makes it highly stable and results in the highest ionization energy among the four elements. Noble gases have the highest ionization energies in their respective periods.
Correct Order (Lowest to Highest Ionization Energy):
- Potassium (K) < Selenium (Se) < Bromine (Br) < Krypton (Kr)
Explanation:
- Potassium (K) has the lowest ionization energy because it is an alkali metal with a large atomic radius and only one electron in its outermost shell.
- Selenium (Se) has a higher ionization energy than potassium because it is a non-metal and is to the right of potassium, where the effective nuclear charge increases.
- Bromine (Br), being a halogen, has even higher ionization energy due to its proximity to a stable octet.
- Krypton (Kr), as a noble gas, has the highest ionization energy, since it has a full outer shell and is stable, making it harder to remove an electron.
Thus, the order of increasing ionization energy is: K < Se < Br < Kr.