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Answered 2009-11-13 07:01:19

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.

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The second ionization energy of calcium is higher than its first ionization energy. You are, after all, removing an electron from a positively charged ion; however, the Ca+ ion does not have a noble gas configuration, so it easily loses a second electron to achieve one. If you were to look up calcium's 3rd ionization energy, you would find it to be tremendously higher than the second, just as potassium's second ionization energy is much higher than its first.


Ionization energy is an atoms ability to hold on to its valence electrons. Flourine (F) has the highest, and Francium (Fr) has the lowest. This value decreases from top to bottom and from right to left.


Helium (He) has the highest 1st ionization energy.


Because there is no such atom. Every second IE is greater than the first IE for the same element/isotope.


First pull out your periodic table. If you know their are 18 groups on the periodic table, you know then that their is a specific order on how to find the ionization number of an element. As shown: Ionization for Group 1 is +1 Ionization for Group 2 is +2 Ionization for Group 3 is +3 Ionization for Group 4 is +4 Ionization for Group 5 is +5 Ionization for Group 6 is +6 Ionization for Group 7 is +7 Ionization for Group 8 is +8 Ionization for Group 9 is +9 Ionization for Group 10 is +10 Ionization for Group 11 is +11 Ionization for Group 12 is +12 Ionization for Group 13 is +3 Ionization for Group 14 is +4 or -4 Ionization for Group 15 is -3 Ionization for Group 16 is -2 Ionization for Group 17 is -1 Ionization for Group 18 is 0


Just see where there is a significant jump in the ionization energies. For example, if the first ionization is 456 and the second is 4996, you know that there is one valence electron. Then you have to check the others, consecutively, for any other valence electrons. Hope this helps!


Ok, to find the first ionization equation you have to start with the neutral calcium ion and then write the equation for the removal of one electron: Ca(s) -----> Ca+(s) + e- So the second ionization energy is just the removal of one more electron: Ca+(s) ------> Ca2+(s) + e- Good luck!


To find that, you multiply the first element of the first row by the second element of the second row. You also multiply the first element of the second row with the second element of the first row. Then you subtract the products not add them.


It is rare to find a 4 plus ion of carbon because of the increasing energy required to ionize carbon. Ionization energy increases with each time.


Helium is a very light atom, and it is difficult for it to hold a charge. You will find a periodic trend down the periodic table of lower and lower first ionization energies.


Find the element's period number on the periodic table.


Your element as it pertains to Wicca is the element you feel the most energy from, or feel the most balanced in. It is the element you would rather be in or observe above all others.


There are many in just one atom and vary between atoms, and it is the level at which you find an electron, and electrons can jump between levels, and escape them (ionization).


It is called as ionization energy.To find the ionisation energy, use the formula:- 13.6 x Z2 (1/(n1)2 - 1/(n2)2)eVWhereZ is atomic no.n1 is initial energy level.n2 is the energy level to be transferred.


The number of electrons in the outermost energy shell is usually used in finding the valency of a given element. For instance elements that have two electrons in the outermost energy shell have valency 2.


Ionization detectors respond to fast burning fires like stove grease flare-ups or burning newspapers


it very easy: whatever row the element is in is the number of energy levels it has. Example: hydrogen in the first row, it has 1 energy level.Read more: How_do_you_find_number_of_energy_levels_in_an_element


They are both sets such that a function maps each element of the first set to a unique element in the second. The first set is called the domain and the second is called the codomain or range.


Super easy way: whatever row the element is in is the number of energy levels it has. Example: hydrogen in the first row, it has 1 energy level. actually, the easiest way to find the number of energy levels to the nucleus is to look at the top right hand corner and see the number in the chart of the element, however many numbers there are in that right hand corner of the elemnt is your answer. Example: Radium, see radium has 6 levels because there are 6 numbers


Find the element's period number on the periodic table.


Horsepower = (number of joules of energy every second) divided by (746).


This is a chemical element. You can find the how many electron in a single atom by using a periodic table.


This is a chemical element. You can find the how many electron in a single atom by using a periodic table.


This is a chemical element. You can find the how many electron in a single atom by using a periodic table.


Marie Curie discovered that by taking bitumen tar, and breaking it down into seperate components thereby eliminating substances , the end result was to produce a 1 substance or element. this was Radium and it was seen to emit light. The emission of light was interprated as an example of natural energy. the conclusion from this was that a substance or element has a form of energy within it and the energy can be derived from within the substance. the energy given off, in the form of light showed that it was a pure element.



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