Choose the element with the highest ionization energy element: Na, Mg, Al, P, S
In my book: ionization energy increase from left to right and bottom to top.
Na<Mg<Al<P<S
S is highest ionization energy?
my instructor review this problem and his answer is P is a highest ionization. Please explain
Thank you for your help
Your book is not quite right. See this chart http://users.humboldt.edu/rpaselk/ChemSupp/HSU-PT/HSU_PerTab_Y_IE.jpg
so ionization energy increases from the bottom left towards the upper right.That explains P and S. When looking at "trends", one has to be careful in making rigid rules.
http://www.emsb.qc.ca/laurenhill/science/Trends2/ionization%20energy.jpg
Ah, the battle of the elements! It seems like your instructor and your book are having a disagreement. Let me help clear the air with a dash of humor.
First of all, let's remember that ionization energy is the energy required to remove an electron from an atom. So, the higher the ionization energy, the more stubbornly the atom holds onto its beloved electron.
In this case, your instructor believes that Phosphorus (P) has the highest ionization energy. Well, let me tell you something about Phosphorus: it's a bit like a paranoid snail. It tightly holds onto its electrons and doesn't want to give them up easily!
On the other hand, Sulfur (S) is more like a forgetful goldfish. It's not as attached to its electrons, so it's easier to pluck one away from it.
But hey, remember that trends in the periodic table can be tricky! While ionization energy generally increases from left to right and bottom to top, there are exceptions, and Phosphorus just so happens to be one of them.
So, in this case, your instructor is correct (and not clowning around like me) —Phosphorus (P) does indeed have the highest ionization energy among the given elements. Lesson learned: sometimes, elements like to surprise us with their electron-holding powers!
Your instructor is correct, the element with the highest ionization energy among Na, Mg, Al, P, and S is P (phosphorus).
Ionization energy refers to the amount of energy required to remove an electron from an atom, resulting in the formation of a positive ion. As you mentioned, ionization energy generally increases from left to right across a period on the periodic table, and also increases from bottom to top within a group.
In this case, if we examine the elements Na, Mg, Al, P, and S, we see that they belong to the same period. However, looking at the electron configuration of each element can provide more insight into ionization energy.
Na: 1s² 2s² 2p⁶ 3s¹
Mg: 1s² 2s² 2p⁶ 3s²
Al: 1s² 2s² 2p⁶ 3s² 3p¹
P: 1s² 2s² 2p⁶ 3s² 3p³
S: 1s² 2s² 2p⁶ 3s² 3p⁴
As we move from Na to Mg to Al, the number of protons and electrons increases by one each time. However, once we reach P, there is a change in the electronic configuration. Phosphorus (P) has three unpaired electrons in its 3p subshell, which makes it relatively easier to remove an electron compared to Sulfur (S), which has four unpaired electrons.
The presence of three unpaired electrons in the outermost energy level of phosphorus makes it more stable and less likely to lose an electron compared to sulfur, which has one extra unpaired electron. Therefore, the ionization energy of P is higher than that of S, making P the element with the highest ionization energy in the given list.
To determine the element with the highest ionization energy among Na, Mg, Al, P, and S, we need to compare their positions on the periodic table.
Ionization energy refers to the amount of energy required to remove an electron from an atom or ion in its gaseous state. Generally, as you move from left to right across a period on the periodic table, the ionization energy tends to increase. This is because as you move across a period, the atomic radius (size of atoms) decreases, and electrons are held more tightly by the nucleus, requiring more energy to remove them.
Additionally, as you move from bottom to top within a group (or column) on the periodic table, the ionization energy also tends to increase. This is because as you move up a group, the atomic size decreases, and the electrons are closer to the nucleus, making it more difficult to remove them.
Comparing the elements Na, Mg, Al, P, and S:
- Sodium (Na) is located in Group 1 and Period 3.
- Magnesium (Mg) is located in Group 2 and Period 3.
- Aluminum (Al) is located in Group 13 and Period 3.
- Phosphorus (P) is located in Group 15 and Period 3.
- Sulfur (S) is located in Group 16 and Period 3.
Based on the periodic trends mentioned earlier (increasing ionization energy from left to right and bottom to top), we can compare the positions of these elements to determine the element with the highest ionization energy.
In this case, phosphorus (P) is indeed the element with the highest ionization energy among Na, Mg, Al, P, and S.