What atoms ionization energy is greater than phosphorus

Ionization energy is defined as the minimum amount of energy required to knock out the electron from valence shell of an atom.

Trends in Period:

                           Ionization energy increases from left to right across the periodic table. This is because from left to right along the period the nuclear charge increases and the number of shells remain constant.

Trends in Groups:

                            Ionization energy decreases from top to bottom along the group. This is because down the group the number of shells increases and hence, the shielding effect increases shielding the valence electrons therefore, valence electrons are easily knocked out.

                     So, we can conclude that elements at right to Phosphorous and above Phosphorous will have greater Ionization energies as compared to Phosphorous. Examples,

At right to Phosphorous;

                                              Sulfur

                                              Chlorine

                                              Argon

At the top of Phosphorous;

                                             Nitrogen

                                              Oxygen

                                              Fluorine

                                              Neon

the answer would be b i believe

assuming that your periodic table has eighteen columns, you should highlight   the four elements in the third column from the left of the table.

neutral atoms of elements after calcium contain d electrons. the energy of d orbitals of a particular main shell lies between the energy of the s and p orbitals of the next main shell. for example, electrons in the have energy higher than those in the orbital while lower than those of the orbital.

by the aufbau principle, electrons fill orbitals one at a time, starting from those of the lowest energy. the orbital is therefore filled right after orbitals and before orbitals.  

potassium has electron configuration and calcium . the s orbital of a main shell holds a maximum of two electrons. the next element would thus have the electron configuration and satisfy the requirements.

a neutral atom of the element contains three electrons on top of the most recent noble gas element. it should thus be placed in the third column of the periodic table. both scandium and yttrium would satisfy the conditions. an aufbau diagram indicates that the 4f orbital is filled before the 5d. however, it appears that exceptions exists for both lanthanum and actinium. neutral atoms of the two d-block elements also demonstrate the and should be highlighted as well.