Atomic Radius/ Ionic Radius/ Electronegativity/ Ionisation Energy/ Solubity Flashcards
What is Atomic Radius?
The distance from the nucleus to the outer most electron
Moving Across the Periodic Table Atomic Radius ____________
Moving Across the Periodic Table Atomic Radius DECREASES
Why does Atomic Radius DECREASE as you move ACROSS the periodic table?
Atomic Radius decreases as you move across the table as there are more protons and electrons at the same distance, resulting in a stronger attraction, pulling the electrons closer.
Moving down the Periodic Table the Atomic Radius_________
Moving down the Periodic Table the Atomic Radius INCREASES
Why does Atomic Radius INCREASE as you move DOWN the periodic table?
The outer electron are further away from the nucleus
What is Ionic Radius?
The space occupied by an ion in the crystal lattice
Positive Ions have a __________ ionic radii than corresponding atomic radii.
Positive Ions have a SMALL ionic radii than corresponding atomic radii.
Why do POSITIVE ions have a SMALLER ionic radii than corresponding atomic radii?
The larger positive draws the negative electrons in. Therefore a smaller ionic radius.
Negative ions have a __________ ionic radii than corresponding atomic radii.
Negative ions have a LARGER ionic radii than corresponding atomic radii.
Why do NEGATIVE ions have a LARGER ionic radii than corresponding atomic radii?
The smaller positive electrons are unable to pull of the negative electrons in; also there is a increase in repulsion between the negative electrons. This results in a overall increase in size.
What is Electronegativity?
The power of an atom to attract electrons
As you move ACROSS a period the electronegativities ___________________
As you move ACROSS a period the electronegativities INCREASE
Why do electronegativities INCREASE as you move ACROSS the periodic table?
There is a stronger attraction because of the stronger nuclear charger, because the have more protons and electrons.
As you move DOWN a group the electronegativities ___________________
As you move DOWN a group the electronegativities DECREASE
Why do electronegativities DECREASE as you move DOWN the periodic table?
The valence electrons a further away from the nucleus, due to the screening effect caused by the electron orbitals there is a weaker attraction.
What is Ionisation Energy?
The amount of energy required to remove one electron from an atom
As you move ACROSS a Period there is an _____________ in the first ionisation energy.
As you move ACROSS a Period there is an INCREASE in the first ionisation energy.
Why does first ionisation energy INCREASE as you move ACROSS the periodic table?
First Ionisation Energy increase because the nuclear charges on the right side of the table are stronger, making them reluctant to loss electrons.
As you move DOWN a Period there is an _____________ in the first ionisation energy.
As you move DOWN a Period there is an DECREASE in the first ionisation energy.
Why does first ionisation energy DECREASE as you move DOWN the periodic table?
The is a weaker attraction between the nucleus and its valence electrons, caused by the screening effect of electron orbitals as the distance is greater.
Why does ionisation energy increase as you lose more electrons?
Ionisation energy increase because as you lose electrons the positive ion becomes stronger pulling the electrons closer; therefore requiring more energy to remove.
Why do atom with Nobel Gas Configurations have highest ionisation energies?
Since they have a full shell they are stable, making them reluctant to lose more; resulting in a higher ionisation energy.
What identifies a full shell (ionisation energy)?
The biggest jump in ionisation energy.
____________Highest 1st ionisation energy
____________ Lowest 1st Ionisation energy
NOBLE GASES Highest 1st ionisation energy
ALKALI METALS Lowest 1st Ionisation energy
