What elements has the lowet ionization energy He C Rb Na and F?

Rubidium Rb has the lowest 1st ionization energy of these 4 elements.

The equation for the first ionization energy is: Na --> Na+ + e- The equation for the second ionization energy is:Na+ --> Na2+ + e-

Ionization energy increases as elements move to the right of the periodic table and up the periodic table. Na is weaker in energy level than Ne.

The ionization energy increase from sodium to fluorine.

The Pauling electronegativity and the first ionization energy increase from sodium to chlorine.

Na, sodium, should have the lowest first ionization energy of those four elements.

K Na C N F and Cs Na Al C O and K Na C N F

You are referring to the ionization enthalpy. The first ionization energy of sodium is the energy for the process Na(g) --> Na+(g) + e-(g).

The first ionization energy of Na is smaller than that of Mg. However, the second ionization energy of Na is larger than that of Mg. This is because the second ionization energy of metal M is the energy needed to to remove an electron from M+ to form M2+ . In the case of Na, Na+ is already a stable species. To take an electron away from Na+ , the electron has to be taken from one of the inner shells, where the electrostatic force from the nucleus is stronger, and thus it's more difficult. However, in the case of Mg, Mg2+ is the more stable species than Mg+ . Therefore, it takes less energy to remove one electron from Mg+ is easier than from Na+ .

I'm assuming you're referring to the problem Na(g)+Cl(g) -> Na+(g)+Cl-(g) Since, ionization energy is basically the amount of energy it takes to dislodge one electron from a neutral atom, Cl has to dislodge one electron to stabilize Na Thus, Na -> Na++e-

The order is: Cl,S, Si, Al, Na.

Na(g) --> Na+(g) + e- First ionisation energy is always: X(g) --> X+(g) + e- with X being an element

Simple answer: Because it is a smaller size, it take more energy to remove an electron.

No it has high ionization potential compared to Na, K. This is because it has a very small atomic radius so there is more attraction of the nucleus to the electrons. So it is not easy to remove electrons from it when compared to Na and K.

Sodium is more reactive then lithium because Na has a lower ionization energy.

The ionised energy is the amount of energy it takes to detach one electron from a neutral atom, thus it meaures how strong the otermost electron is attached to the atom. First Ionised Energy: Na -> Na+ + e-

K (lowest) Na Li B N (highest)

In general, you can pretty much predict that the second ionization energy will always be higher than the first ionization energy regardles of what atom you are looking at. This is because when you remove an electron, there is less electron-electron repulsion in the valence shell, which means that the electron cloud shrinks a bit. When it shrinks, the average distance from the nucleus for the remaining valence electrons decreases, increasing the amount of energy needed to remove them. This effect is magnified TREMENDOUSLY if you are looking at the group 1 elements (alkali metals), because after ionizing the first electron you remove a shell. This means that the valence shell is now closer to the nucleus and the effective nuclear charge that those valence electrons feel is increased. For instance, as a result, the 2nd ionization energy is very high. In the case of Na+, the 2nd ionization energy is higher than even helium, the atom that has the highest first ionization energy on the periodic table.

On a periodic table, Sodium onwards (Na)

I belive Radium (Ra, atomic number 88) ^It's not Ra, it's Na, aka Sodium

Na, as it's in group 1.

Ionisation energy of elements increases across periods. The ionisation energy of metals is the lowest as metal elements has a low electronegativity which means it tend to lose it's electrons easily. Ionisation energy increases in such a trend : Metals < Non-metals < Noble gases Therefore comparing sodium ( Na ) and copper (Cu), Cu is more on the right side of the periodic table, causing it to have a high ionisation energy.

Ionization energy of Na is less than that of Mg because Na gives only one electron but Mg gives two electrons as valency of magnesium is 2 and that of sodium is 1. And the I.E successor after 1st electron is always greater than the predecessor.i.e, 1st I.E < 2nd I.E <3rd I.E OR 3rd I.E > 2nd I.E > 1st I.E

The ionised energy is the amount of energy it takes to detach one electron from a neutral atom, thus it meaures how strong the otermost electron is attached to the atom. First Ionised Energy: Na -> Na+ + e- Read more: http://wiki.answers.com/Q/What_is_meant_by_the_term_first_ionization_energy#ixzz1atijGvlC

K Na Li B N