Neon
Sodium (Na) has the lowest first ionization energy in period 3.
The period an element is in affects the ionization energy because as you move across a period from left to right, the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the electrons in the outer shell. This increased attraction makes it harder to remove an electron, resulting in higher ionization energy.
The element that has a lower first ionization energy than aluminum (Al) is magnesium (Mg). Magnesium is one period above aluminum on the periodic table, and as you move down a group or family, the ionization energy tends to decrease.
Please provide the specific ionization values you are referring to so I can accurately identify the third period element.
Argon (#18). It's a noble gas, which means it doesn't react, which means it will be really hard to get it to lose an electron.
The element in the fifth period with the highest ionization energy is xenon. Ionization energy generally increases across a period from left to right, so xenon, being on the far right of the period, has the highest ionization energy.
Sodium (Na) has the lowest first ionization energy in period 3.
The period an element is in affects the ionization energy because as you move across a period from left to right, the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the electrons in the outer shell. This increased attraction makes it harder to remove an electron, resulting in higher ionization energy.
Carbon has the highest ionization energy in Group 4 of the periodic table. This is because as you move across a period from left to right, the ionization energy generally increases due to increase in effective nuclear charge. Among the elements in Group 4 (carbon, silicon, germanium, tin, lead), carbon has the highest ionization energy.
It's carbon. The trend for 1st ionization energy is that it increases as you move left-to-right across a period. As you move in that direction across period 2, ionization energy increases, and since carbon is the most to the right, it has the highest 1st I.E.
The element that has a lower first ionization energy than aluminum (Al) is magnesium (Mg). Magnesium is one period above aluminum on the periodic table, and as you move down a group or family, the ionization energy tends to decrease.
Please provide the specific ionization values you are referring to so I can accurately identify the third period element.
The element with the largest ionization energy in period 4 is argon. Argon has a full outer electron shell with 8 electrons, making it stable and more difficult to remove an electron compared to other elements in the same period.
Ionization energy increases as you go across a period, but as you go down a group it decreases.
Argon (#18). It's a noble gas, which means it doesn't react, which means it will be really hard to get it to lose an electron.
The trend in period 2 ionization energy across the elements increases from left to right.
Moving from left to right across a period, the first ionization energy increases because it becomes increasingly difficult to remove an electron.