For the elements in row 2 of the PT discover the relationship between ionization and the family number of the element
Element. Family. Ionization Ener
Lithium. 1 13.6
beryllium. 2. 9.3
boron. 13. 8.3
carbon. 1 4. 11.27
nitrogen. 15 14.53
oxygen. 16. 13.62
fluorine. 17. 17.42
neon. 18. 21.56
Confused
The number of energy levels increases as you move down the group as the number of electrons increases.Each energy level is then further away from the nucleus, so atomic radiud decreases.
As you move across a period, the atomic radius decreases.
ionization energy tend to increase if you move left to right in a given period or up in the periodic table.
I understand all that, but why are the munbers all over the place? This is from the chart they gave us. I double checked the numbers and the only error is lithium. 5.39.
There is supposed to be a trend. There is no specific trend here unless it has something to do with the family number.
please help, I am lost.
<<ionization energy tend to increase if you move left to right in a given period or up in the periodic table. >>
your numbers certainly show that trend. Plot them on a graph if you can't see it.
I can understand why you're confused. While there is a general trend for ionization energy across the periodic table, there can be some exceptions and irregularities in specific cases. In this case, you're looking at the elements in row 2 of the periodic table, which includes the elements Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, Fluorine, and Neon.
The relationship between ionization energy and the family number of an element can be explained by their electron configuration. The number of valence electrons, which are the outermost electrons of an atom, generally determines the ionization energy.
As you move from left to right across a period, the ionization energy tends to increase. This is because the effective nuclear charge, which is the attractive force between the positively charged nucleus and the negatively charged valence electrons, increases. The increased nuclear charge makes it more difficult to remove an electron, hence higher ionization energy.
However, there can be exceptions to this trend. One such exception is found in the elements Lithium and Boron in Row 2. Lithium has an ionization energy of 5.39 eV (electron volts) and Boron has an ionization energy of 8.3 eV. This means that the ionization energy of Boron is higher than that of Lithium, even though Boron is to the right of Lithium in the periodic table.
The reason for this exception lies in the electron configuration of these elements. Lithium has a configuration of 1s²2s¹, which means it has only one valence electron in the 2s orbital. Boron, on the other hand, has 1s²2s²2p¹. In Boron, the 2p electron experiences electron-electron repulsion from the two paired electrons in the same orbital, making it easier to remove.
Overall, while there is a general trend for increasing ionization energy as you move from left to right across a period, there can be exceptions due to electron configuration and electron-electron repulsion. It's important to consider these factors when analyzing and understanding ionization energy trends in specific cases.