The ionization energy increase from sodium to fluorine.
Na, sodium, should have the lowest first ionization energy of those four elements.
Potassium (K) has a lower ionization energy than sodium (Na).
The amount of energy needed to remove the most loosely held electron is referred to as the ionization energy. It is the energy required to remove an electron from a gaseous atom or ion.
Element Rb (Rubidium) has the lowest ionization energy among Rb, Na, C, and F. This is because as you move down a group on the periodic table, the ionization energy typically decreases due to the increase in atomic size. Rubidium is located below sodium (Na) in the same group, so it has a lower ionization energy.
Within a group, first ionization energy generally decreases as you move down the group due to increasing atomic size and shielding effects. Across a period, first ionization energy generally increases due to increasing nuclear charge and effective nuclear charge. For example, within Group 2 (alkaline earth metals), the first ionization energy decreases as you move down the group from Be to Ra. Across Period 3, the first ionization energy increases from Na to Cl.
The order from highest to lowest ionization energy is Cl > Al > Si > Na > S. This is because ionization energy generally increases from left to right and from bottom to top in the periodic table.
Na, sodium, should have the lowest first ionization energy of those four elements.
Potassium (K) has a lower ionization energy than sodium (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 NaThus,Na -> Na++e-
As we move from left to right across Period 3 from Na to Cl, electronegativity and first ionization energy generally increase. This is due to the increasing effective nuclear charge as electrons are added, causing a stronger attraction between the nucleus and outer electrons. Chlorine, being closer to the right of the period, has a higher electronegativity and first ionization energy compared to sodium.
K (lowest) Na Li B N (highest)
The amount of energy needed to remove the most loosely held electron is referred to as the ionization energy. It is the energy required to remove an electron from a gaseous atom or ion.
Sodium (Na) has the lowest first ionization energy in period 3.
Element Rb (Rubidium) has the lowest ionization energy among Rb, Na, C, and F. This is because as you move down a group on the periodic table, the ionization energy typically decreases due to the increase in atomic size. Rubidium is located below sodium (Na) in the same group, so it has a lower ionization energy.
The dissociation is:NaHCO3-------------Na+ + (HCO3)-
Within a group, first ionization energy generally decreases as you move down the group due to increasing atomic size and shielding effects. Across a period, first ionization energy generally increases due to increasing nuclear charge and effective nuclear charge. For example, within Group 2 (alkaline earth metals), the first ionization energy decreases as you move down the group from Be to Ra. Across Period 3, the first ionization energy increases from Na to Cl.
Rb has the least