List Sn , Sn2+, Sn4+ in order of decreasing ionization energy
The ionization energy refers to the energy required to remove an electron from an atom or ion. In general, ionization energy increases as we move across a period from left to right in the periodic table, and decreases as we move down a group.
Based on this information, we can determine the order of decreasing ionization energy for Sn, Sn2+, and Sn4+:
1. Sn4+ (Tin IV ion): This ion has the highest ionization energy since it has lost all four of its valence electrons. It is more difficult to remove an electron from a positively charged ion compared to a neutral atom.
2. Sn2+ (Tin II ion): This ion has a lower ionization energy compared to Sn4+ because it has already lost two valence electrons. It is easier to remove electrons from a positively charged ion compared to a neutral atom.
3. Sn (Neutral Tin atom): This is the the most easily ionized state since it has all its valence electrons. It requires the least amount of energy to remove an electron from a neutral atom compared to any charged ion.
Therefore, the order of decreasing ionization energy is Sn4+ > Sn2+ > Sn.
To determine the order of decreasing ionization energy for Sn, Sn2+, and Sn4+, we need to understand the concept of ionization energy. Ionization energy refers to the energy required to remove an electron from an atom or ion in its gaseous state.
The general trend for ionization energy is that it tends to increase as we move across a period from left to right in the periodic table, and it tends to decrease as we move down a group. This is primarily due to the increasing effective nuclear charge (i.e., the attraction between the electrons and the nucleus) as we move across a period and the increasing distance between the outermost electron and the nucleus as we move down a group.
Now, let's apply this trend to Sn, Sn2+, and Sn4+:
1. Sn (tin): Tin (Sn) is an element in the periodic table. It has an atomic number of 50 and is located in Group 14. The electron configuration of Sn is [Kr]5s^24d^105p^2. Sn has a total of 50 electrons.
2. Sn2+ (tin cation with a 2+ charge): When Sn loses two electrons, it forms a 2+ cation. The electron configuration of Sn2+ becomes [Kr]5s^24d^10. Sn2+, with an atomic number of 50 and only 48 electrons, has a smaller electron cloud compared to Sn.
3. Sn4+ (tin cation with a 4+ charge): When Sn loses four electrons, it forms a 4+ cation. The electron configuration of Sn4+ becomes [Kr]5s^24d^8. Sn4+, with an atomic number of 50 and only 46 electrons, has an even smaller electron cloud compared to Sn and Sn2+.
Based on the trend of increasing ionization energy across a period and decreasing ionization energy down a group, we can rank the order of decreasing ionization energy as follows:
Sn > Sn2+ > Sn4+
This means that Sn has the highest ionization energy, followed by Sn2+, and Sn4+ has the lowest ionization energy among the three entities mentioned.
Ionization energy: the energy it takes to remove the outermost electron.
Sn4+ will be very difficult to remove the next energy
Sn2+ is difficult to remove next electrons
Sn is the easiest to rmove.