Atomic structure- IONISATION ENERGY AND PERIODICITY Flashcards
What is the definition for the fist ionization energy
ionization energy is the amount of energy needed to remove a mole of electrons forms a mole of atom, in the gaseous state
when an atom is ionized where is the first electron removed from
the outer most shell
what is the unit for ionization energy
kjmol-1
what do the periods tell you about an atom and how does it change down a group
periods tell you the number of shells; increasing down a group
the number of sells increase down the group. how does this affect shielding
shielding increases
how does the number of shells affect the electrostatic attraction
more shell, more shielding, less electrostatic attraction between the nucleus and the outer electrons,
less shells, less shielding, more electrostatic attraction between the nucleus and the outer electron
how is the nuclear charge changing across a period
increasing nuclear charge
which has ore shielding Boron or Aluminum
Al as it has more shells
what is happing to the radius across period
shielding stays the same ( same number of shells), the nuclear charge is increasing(amount of protons), stronger electrostatic attraction, between the nucleus ad outermost electrons. radius is decreasing
what is happing to the radios down the group
shielding increases (more shells), less attraction between the nucleus and the outer electron, radius increases
what is happing to the IE across a period
shielding stays the same ( same number of shells), the nuclear charge is increasing(amount of protons), stronger electrostatic attraction between the nucleus and the outermost electron, more energy required to remove the outermost electron
what is happing to IE down a group
shielding increases , less electrostatic attraction between the uncles and the outermost electron, less energy to remove the outermost electron. IE decreases
why does the first ionization energy decrease down the group
shielding increases( more shells), less electrostatic attraction between the nucleus and the outermost electron, less energy to remove the outermost electron
what is the trend in IE from Li to Ne
shielding is the same, the nuclear charge is increasing, stronger electrostatic attraction between the nucleus and the outermost electrons, more energy is required to remove the outermost electron
the second electron of K is removed from an ion that already has a positive charge what will this mean for IE
the second ionization would be higher
which has a grater first IE, Be or Mg
Be has less shielding than Mg, stronger electrostatic attraction between the nucleus and the outermost electrons, more energy is required to remove the outermost electron
from Na to Ar the ionization energy is increasing why
shielding is the same, the nuclear charge is increasing so stronger electrostatic attraction between the nucleus and the outermost electron so more energy is required to remove the outermost electron
the electro static attraction with changing shielding why
more shells, more shielding, less electrostatic attraction between the nucleus and the outer electrons
less shells, less shielding more electrostatic attraction between the nucleus and outer electron
why does the first IE increase across a period
shielding is the same, the nuclear charge is increasing, stronger electrostatic attraction between the nucleus and the outermost electrons, more energy is required to remove the outermost electron
which is the smaller ion Be2+ or O2-
Be2+ ion only has one shell, its electrons are closer to the nucleus and there is less shielding so the outer electrons are more strongly attracted to the nucleus
