How IS The electronegativity trend relates to the first ionization energy trend?

Answer 1

Electronegativity and first ionization energy both increase going up the Periodic Table.

Answer 2

Electronegativity and first ionization energy both increase going up the Periodic Table.

Answer 3

The atomic radius, or the size of atom going from the nucleus to the outermost electron shell, is going to decrease going across periods and increase going down groups or families.

Explanation: The atomic radius decreases going across periods because as an electron is added, so does a proton. Since the electrons added going across periods all go within the same Principal Energy Level (PEL) or sublevel (parts within a Principal Energy Level [PEL]) to be more specific, the attraction between the protons in the nucleus and the valence electrons is going to become stronger, making the distance between the nucleus and the outermost electron shell smaller.

The atomic radius increases going down periods or families. While the same number of electrons and protons are added to atoms going down families and across periods, the electrons added going down families are added to entirely different Principal Energy Levels. This means that the distance between the outermost electrons and the nucleus is going to increase going down a family or a group.

Electronegativity, which is the ability of an atom to attract electrons in a given bond, tends to increase moving across a period and decreases going down a group (excluding the noble gases, due to their having 8 valence electrons [octet rule]). Related to ionization energy

Explanation: Going across a period, the number of valence electrons increases. This means that there is greater attraction between those valence electrons and the nucleus; this also means that as there are more valence electrons in an atom, the atom is more likely to gain more electrons to reach a noble gas configuration. Therefore, the electronegativity increasesgoing across a period.

Going down a group or family, the electronegativity decreases, as there is a greater distance between the outermost electrons and the nucleus. Because of this, there is a weaker attraction between the electrons and the nucleus, thus a smaller likelihood of actually attracting other electrons.

Ionization energy, or the amount of energy needed to remove an electron from an atom, tends to increasegoing across periods and decrease going down families or groups.

Explanation: Going across a period, the atomic radius decreases meaning a stronger attraction between that atom's electrons and the nucleus. Since that attraction is stronger going across a period, it will require more energy to remove an electron from that atom.

Going down a family or group, the atomic radius increases meaning a weaker attraction between that atom's electrons and the nucleus. Since that attraction is weaker going down a family or period, it will require less energy to remove an electron from that atom.

Answer 4

The trend of electronegativity and first ionization energy both increase from left to right across a period on the periodic table. This is because as you move across a period, the effective nuclear charge increases, leading to stronger attraction between the nucleus and electrons. Higher electronegativity values indicate a greater tendency to attract electrons, while higher first ionization energies indicate a greater energy required to remove an electron.

Answer 5

The more positive the ionization energy and the more negative the electron affinity, the greater the electronegativity of an element.

Answer 6

Electronegativity and first ionization energy both increase going up the periodic table.