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You question is not very clearly stated but I think I know what you are asking. As you go down the column of any family of elements in the Periodic Table, you move to increasingly heavier and larger atoms. Their outer electrons are therefore farther from the nucleus, and even though the nucleus is larger and has a larger positive charge, the increased distance is the predominant influence, making the outermost electrons less tightly bound, and therefore more easily ionized, with a lower ionization energy.
Wiki User
∙ 14y ago
Wiki User
∙ 11y agoBackground: to start off, atomic radius depends on the number of orbitals around a nucleus. The number of orbitals depends on how many valence electrons a certain element has. The more valence electrons, the bigger the size of the atomic radius. As the atomic number gets larger, the number of orbitals also increases; therefore, the atomic radius gets larger as one goes down a family of the periodic table. Now, ionization energy is the amount of energy it takes to take electrons out of an orbital. This is determined by how close they are to the nucleus. Since the protons (positive charge) is in the nucleus, the closer the electrons (negative charge) are to the nucleus, the stronger the attraction, and the harder it is to get the electrons out.
Answer: As the atomic radius gets larger, it is easier to take the electrons out, and so the ionization energy decreases because you don't need as much energy.
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When energy is removed what does the decrease in energy causes the particles in that state to do?
When energy is removed, the particles involved lose kinetic energy-they slow down.
What can you do to decrease the thermal energy of a metal block?
Putting it in the fridge works pretty well.
What happens to the particles of a liquid in a can as it cools down after heating?
The particles will have lower kinetic energy, which will slow them down, and the pressure inside the can will decrease as a result.
How IS The electronegativity trend relates to the first ionization energy trend?
Electronegativity and first ionization energy both increase going up the Periodic Table.
Why does the loudness of a sound wave decrease as the wave travels away from its source?
The energy in the sound's vibration dies down, until it is no longer audible.
In ionization energy how does the property varies within a group?
The ionization energy decrease moving down in a group.
Which element has a higher first ionization energy than chlorine Cl?
Ionization energy decrease down the group.So in halogens,Fluorine has highest 1st ionization energy.
Does the first ionization energy increase or decrease when you go down a group?
it increases
What is ionization energy and how does it relate to the periodic table?
The ionization energy is the energy needed to extract an electron from an atom.The value of the ionization energy increase from left to right in a period of the periodic table and decrease in a group from the above to down.
How does the first ionization energy change going down and across the periodic table?
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
What is the group trend in the first ionization energies and why?
1. The ionization energy decrease down in the group.2. The cause is that the distance between the nucleus and the electron shell increase and the needed energy to extract an electron decrease.
Why ionization energies of alkaline earth metals decrease from Be to Ba?
as we know that there are 7 periods and 18 groups ,as we go down a group the size of the atom decreases therefore there is a decrease in ionization energy for
What are the metallic trends concerning electronegativity and ionization energy?
Electronegativity decrease going down in a group and increase from left to right; but this isn't a general rule.A similar situation is also with the ionization energy.
Elements belong in upper ionization energy?
All of the elements on the top half of the periodic table belong in upperionizationenergy because the trend is top to bottom. Top being lowest and getting bigger as it goes down.------------------------------------------------------* In a group: the ionization energy decrease from the lighter elements to heavier elements.* In a period: the ionization energy increase from the left elements to the elements of the right.* When the atomic radius decrease the ionization energy increase.
What is the general trend of ionization energy as you go across the periodic table?
Across a period, first ionization energy increases. However, when going down a group, first ionization energy generally decreases. As you go down a group, atoms hove more total electrons so they don't really care that much about their outermost ones.
Is the pattern in ionization energy always true or generally true?
there is always a decrease in ionization energies down a group, and there is always a general increase across each period. this is always true.
If you go down a group on the periodic table does the first ionization level increase?
Decrease, due to less nuclear attraction from the nucleus. There are more energy levels which causes less pull on the outer shells, making it easier to remove electrons from those outer shells.
