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Why the ionization potential of 2-A group is more than the ionization potential of 1-A group?
Wiki User
∙ 10y ago
Completely filled s orbital is more stable than half filled s orbitals and it is difficult to remove electrons from the former due to extra stibility. Group IIA elements (or alkaline earth metals) have completely filled s orbitals, whereas group IA elements have half filled s orbitals.
Wiki User
∙ 10y ago
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Why are the elements in group 1 more reactive than the other groups?
Causes: very low ionization potential, very great electropositivity.
Which is more reactive sodium or barium?
sodium because it's the first group and first group are the most
Why does the second ionization energy of Group 1 Elements greater than the first ionization energy of Group 1 Elements?
It takes more energy to knock off two electrons
Why 2nd ionization potential is greter than 1st ionisation potential of element?
In the first ionization an electron is removed from a neutral atom. In the second ionization an electron is removed from a positively charged ion. Since electrons carry a negative charge and opposite charges attract it is more difficult (i.e. takes more energy) to remove.
What is the second ionization of energy and how does it work?
Imagine that one electron has already been removed from an atom, the energy used to accomplish this is the 1st ionization energy. Now more energy is needed to remove a 2nd electron. That is the 2nd ionization energy.
Why are the elements in group 1 more reactive than the other groups?
Causes: very low ionization potential, very great electropositivity.
Which is more reactive sodium or barium?
sodium because it's the first group and first group are the most
Why does the second ionization energy of Group 1 Elements greater than the first ionization energy of Group 1 Elements?
It takes more energy to knock off two electrons
Why 2nd ionization potential is greter than 1st ionisation potential of element?
In the first ionization an electron is removed from a neutral atom. In the second ionization an electron is removed from a positively charged ion. Since electrons carry a negative charge and opposite charges attract it is more difficult (i.e. takes more energy) to remove.
Why arsenic has larger ionization potential than cesium?
Due to smaller size of arsenic
Does antimony have a greater ionization energy level than tellurium?
Antimony. The higher an element is in a group, the smaller it is, requiring more energy (ionization energy) to remove an electron.
What is the second ionization of energy and how does it work?
Imagine that one electron has already been removed from an atom, the energy used to accomplish this is the 1st ionization energy. Now more energy is needed to remove a 2nd electron. That is the 2nd ionization energy.
What is niobium's ionization energy?
Niobium element has more than one electron to be removed, it will have more than one ionization Energy (IE) 1st ionization energy: 652.1 kJ mol-1,2nd ionization energy: 1381.7 kJ mol-1,3rd ionization energy: 2416 kJ mol-1
What is the trend for first ionization energy for the alkali metals?
Within the alkali metals, or group 1, the ionization energy trend is that ionization energy decreases as you move down the group from top to bottom. This is because with each step down, you add an energy level, therefore the one valence electron is farther and farther from the atom's nucleus. So, the attraction between the nucleus and that electron (its electronegativity) decreases. This makes it easier (requires less energy), making the element more reactive. For example, cesium is more reactive than rubidium, which is more reactive than potassium, which is more reactive than sodium...
Which has more ionizastion energy n2 or no?
n2 has more ionization energy than no.
Is cathode rays have maximum ionising power than alpha beta gamma rays?
Cathode (electron) rays have less ionizing potential than gamma, beta, and alpha rays (in increasing ionization potential).
Why is sodium more reactive than lithium?
Sodium is more reactive than Lithium because the metals of Group 1 become more reactive as we go down the group. The ionization energy of lithium is greater than the ionization energy of sodium, and thus sodium is more reactive.
