For strontium, which quantity will be greater, the difference between I1 and I2, or the
difference between I2 and I3? Explain
To compare the differences between I1 and I2, and I2 and I3 for strontium, we first need to understand what I1, I2, and I3 represent. In this context, I1, I2, and I3 stand for the ionization energy levels of the strontium atom.
Ionization energy is the amount of energy required to remove an electron from an atom or ion. The ionization energies of an atom typically increase as you remove more electrons because removing each subsequent electron requires more energy as you get closer to the nucleus, where the positive charge is concentrated.
To find these ionization energies, you can refer to the periodic table or use a reliable chemistry resource. Let's assume I1 is the first ionization energy, I2 is the second ionization energy, and I3 is the third ionization energy for strontium.
Now, if we consider the trend in ionization energies for strontium, we can make an inference. In general, as you move from left to right across a period in the periodic table, ionization energies tend to increase because the atomic radius decreases, making it harder to remove an electron due to increased attraction to the positively charged nucleus.
In the case of strontium, the first ionization energy (I1) is generally lower than the second ionization energy (I2) because removing the first electron is relatively easier compared to removing the second electron. This is due to the fact that removing the first electron results in a more stable electron configuration for the atom. Therefore, usually, the difference between I1 and I2 is greater than the difference between I2 and I3.
However, it's important to note that there can be exceptions or variations in this trend based on specific factors, such as electron shielding and electron subshells. So, for a precise comparison, it is best to consult the specific ionization energy values for strontium.