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Ionisation energy increases as you go down a group. The reactivity increases on descending the group from lithium to caesium. As you go down the group the period number is increasing so the number of electron shells is also increasing so the forces between the oppositely charged electrons and nucleus are lower. This makes it easier for the elements such as rubidium and caesium to react and gain electrons. All group one metals have one electron in their outer shell which makes it easy for them to react with other elements.
What else can I help you with?
Does the first ionization energy increase or decrease when you go down a group?
it increases
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.
Can ionization energies determine an element group?
Yes, ionization energies can be used to determine the group of an element on the periodic table. Elements in the same group have similar trends in ionization energy, with a general decrease moving down a group due to the increase in atomic size. This pattern allows us to predict an element's group based on its ionization energy values.
How does the first ionization energy change going down and across the periodic table?
As you move down a group on the periodic table, the first ionization energy generally decreases due to the increasing atomic size and shielding effect of inner electrons. Across a period, the first ionization energy generally increases because the effective nuclear charge increases, making it harder to remove an electron.
What trend does the ionization energy follow in the periodic table?
It decreases when going down a group.
In ionization energy how does the property varies within a group?
The ionization energy decrease moving down in a group.
Does the first ionization energy increase or decrease when you go down a group?
it increases
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.
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.
Is the pattern in ionization energy always true or generally true?
The pattern in ionization energy is generally true, but there can be exceptions due to factors such as electron-electron repulsions or orbital hybridization. In most cases, ionization energy tends to increase across a period and decrease down a group on the periodic table.
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.
Can ionization energies determine an element group?
Yes, ionization energies can be used to determine the group of an element on the periodic table. Elements in the same group have similar trends in ionization energy, with a general decrease moving down a group due to the increase in atomic size. This pattern allows us to predict an element's group based on its ionization energy values.
How does the first ionization energy change going down and across the periodic table?
As you move down a group on the periodic table, the first ionization energy generally decreases due to the increasing atomic size and shielding effect of inner electrons. Across a period, the first ionization energy generally increases because the effective nuclear charge increases, making it harder to remove an electron.
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.
What trend does the ionization energy follow in the periodic table?
It decreases when going down a group.
Why does the ionization energy tend to decrease from top to bottom within a group?
there is an increase in atomic number and atomic size down the group due to addition of extra shells.this increase in the atomic size overcomes the effect of an increase in the nuclear charge.Therefore ionisation energy decreases with an increase in atomic size i.e.,it decreases as one moves down a group..
Which property has a trend similar to that of electronegativity?
First ionization energy has a trend similar to that of electronegativity.
