0
What happens to the energy needed to remove an electron as the atomic number increases down a family?
Wiki User
∙ 11y ago
The energy needed to remove an electron from an atom generally increases, decrease as you go across a period? Explain why ? please
Wiki User
∙ 14y ago
Add your answer:
Earn +20 pts
Why is the first ionization energy of aluminium is less than the first ionisation energy of silicon?
Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm
What increases as you move up a column of the periodic table?
Electronegativity, ionization energy, electron affinity, and atomic number are values that increase from left to right across a period.
What happens to ionization energy as atomic Number increases within a group?
and i thought answers could answer my question, this proofs that they're wrong
Why does ionization energy increase as atomic radius decreases?
Ionization energy is how much energy is needed to remove an electron from the valence shell (the outermost shell). When the atomic radius is smaller, you will need more energy to remove an electron because the pull from the nucleus on the electron is stronger. If the atomic radius is larger, then it will be much easier to remove an electron from the valence shell because there are more layers (shieldings) between the nucleus and valence shell.
Will electron lattice electron interaction lower the energy of electrons?
latice energy decreases as you move down a group. This is mostly due to the fact that, as you move down a group in the periodic table the atomic radius increases. It follows that since the square of the distance is inversely proportional to force of the attraction between charges (Coulomb's Law), latice energy will decrease as atomic radius increases.
What happens when the nuclear charge increases across a period?
The atomic size decreases (with some exceptions) , the ionization energy , electronegativity and electron affinity also increase from left to right.
What trend in atomic radius occurs going down on the periodic table and why?
Atomic radii increases moving down a group in the Periodic Table due to the increasing energy levels in the electron configuration and electrons filling in energy levels further away from the nucleus.
What happens as we move down columns on the periodic table?
As you move down a column (group) in the periodic table, the electronegativity decreases, the ionization energy decreases, the electron affinity decreases, and the atomic radius increases.
What happens to the energy that an electron has as its distance from the nucleus of the atom increases?
Physically put, the electron has more energy the farther ( higher ) it is from the nucleus. Simple potential energy. PE = mgh
What happened to the energyof an electron as it goes farther from the nucleus?
if an electron gains enough energy it jumps to a higher energy level. when this happens the atom is in an "excited" state.
How can you use the periodic table and electron configurations to predict relative atomic radii and ionization energies for two atoms?
in a periodic table1>from left to right across a periodic tableionization energy increases & atomic radii decreases2>from top to bottom along a groupionization energy decreases and atomic radii increaseswhen considering the periodic table from left to right the main energy level is the same,but the number of electrons and protons increases.so the nuclear attraction increases and thus the electrons are pulled closer towards the nucleus.this decreases the atomic radii and increases the amount of energy needed to remove the electron in the outer most shell from the strong attraction.that is the ionization energy increases and atomic radii decreases when going from left to right across the periodwhen going down the group in a periodic table the electronic configuration of elements increases by 1 shell.that is the number of main energy levels increases.so the nuclear attraction between the atomic nuclei and the last electron decreases due to the increase in the distance.therefore it is more easier to remove the electron in the outer most shell of an element than that of the element immediately above it.therefore the ionization energy increases down the group.and since number of energy levels increases the atomic radius increases.
What happens to the atomic structure as you go down any group?
Down a group, the atomic size (energy level / shells) increases.
How does the electron's energy change as the orbit of the electron increases?
The farther an electron is from the nucleus of an atom, the more energy it has.
When the atomic number increases what happens to the atomic radius?
When an electron absorbs a photon and therefore has more energy, it will move to a higher orbital and the radius of the atom will increase. This is generally a temporary state of affairs, since the electron will eventually re-emit the photon and fall back to its ground state.
Why is the first ionization energy of aluminium is less than the first ionisation energy of silicon?
Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm
What happens to atomic radius as you move from bottom to top of the periodic table?
atomic radius decreases from bottom to top of the periodic table.
What increases as you move up a column of the periodic table?
Electronegativity, ionization energy, electron affinity, and atomic number are values that increase from left to right across a period.
