The electronegativity of plutonim (after Pauling tables) is 1,28.
The ionization energy of plutonium is 584,7 kJ/mol.
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.
Ionization energy and electronegativity are both periodic trends that help explain the behavior of elements in the periodic table. Generally, ionization energy increases across a period from left to right and decreases down a group, while electronegativity also increases across a period and decreases down a group. This relationship arises because elements with higher ionization energy tend to attract electrons more strongly, leading to higher electronegativity. Both properties reflect the effective nuclear charge experienced by valence electrons, influencing an element's reactivity and bonding characteristics.
They have high ionization energy and high electronegativity.
Boron has the greatest ionization energy among aluminum, boron, and carbon. This is because boron has a lower atomic size compared to aluminum and carbon, leading to increased electronegativity and stronger attraction for electrons in the atomic structure.
ionization potential energy. but remember the atom must be neutral .
When electronegativity decrease the first ionization energy also decrease.
Electronegativity and first ionization energy both increase going up the Periodic Table.
Ionization energy would be similar.
First ionization energy has a trend similar to that of electronegativity.
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.
Electronegativity and first ionization energy both increase as you move up the periodic table
Electronegativity and first ionization energy both increase going up the Periodic Table.
The electronegativity trend and the first ionization energy trend both increase as you move from left to right across a period in the periodic table due to the increasing effective nuclear charge. Higher electronegativity indicates a stronger pull on electrons, making it harder to remove an electron, thus increasing the first ionization energy.
Ionization energy, electronegativity, and atomic radius.
The trend for first ionization energy
As we move from left to right across Period 3 from Na to Cl, electronegativity and first ionization energy generally increase. This is due to the increasing effective nuclear charge as electrons are added, causing a stronger attraction between the nucleus and outer electrons. Chlorine, being closer to the right of the period, has a higher electronegativity and first ionization energy compared to sodium.
The trend for first ionization energy