Question

electronegativity of noble gases

• what are the electronegativity values of neon, argon, and krypton?
• why do you think, in terms of valence electrons, why the noble gases are not electronegative?

summary
chart: periodic table with atomic radius, electronegativity, ionization energy boxes, and a table for ionic radius (metals ions... nonmetal ions...), and a table comparing metals and nonmetals with blanks: ion __ than its atom, ionization energy, requires energy to lose an electron, __ electronegative (for metals); same for nonmetals

compare the trends for metals and nonmetals. use words such as smaller/bigger, higher/lower, more/less

metals

• ion ____ than its atom
• ____ ionization energy
• requires ____ energy to lose an electron
• ____ electronegative

nonmetals

• ion ____ than its atom
• ____ ionization energy
• requires ____ energy to lose an electron
• ____ electronegative

Explanation:

1. Electronegativity values of Neon, Argon, and Krypton

Noble gases (Ne, Ar, Kr) typically have no defined electronegativity values (or are considered to have negligible/undefined electronegativity) because they have a full valence electron shell (octet, except He with duplet) and do not readily attract or share electrons.

2. Why noble gases are not electronegative (in terms of valence electrons)

Noble gases have a stable, full valence electron shell (e.g., Ne: 8 valence electrons, Ar: 8, Kr: 8). Electronegativity measures an atom’s ability to attract electrons in a bond. Since noble gases already have a complete octet (or duplet for He), they do not need to gain electrons to achieve stability. Thus, they have no tendency to attract electrons, making them non - electronegative.

3. Ionic Radius and Metal/Nonmetal Ion Trends

Metal Ions:

• Metal ions are smaller than metal atoms because the atom loses electrons to form the ion. When a metal atom loses electrons, the remaining electron cloud is pulled more tightly by the nucleus (fewer electrons, same nuclear charge), reducing the radius.

Nonmetal Ions:

• Nonmetal ions are bigger than nonmetal atoms because the atom gains electrons to form the ion. Gaining electrons increases electron - electron repulsion in the valence shell, causing the electron cloud to expand, increasing the radius.

Comparing Trends (Metals vs. Nonmetals)

Metals	Nonmetals

Answer:

s (Filling the Blanks):

Ionic Radius Section:

• Metals ions are \(\boldsymbol{\text{smaller}}\) than metal atoms, because the atom \(\boldsymbol{\text{loses}}\) electrons to form the ion.
• Nonmetal ions are \(\boldsymbol{\text{bigger}}\) than nonmetal atoms, because the atom \(\boldsymbol{\text{gains}}\) electrons to form the ion.

Metals Column (in the Table):

• Ion \(\boldsymbol{\text{smaller}}\) than its atom
• \(\boldsymbol{\text{Lower}}\) ionization energy
• Requires \(\boldsymbol{\text{less}}\) energy to lose an electron
• \(\boldsymbol{\text{Less}}\) electronegative

Nonmetals Column (in the Table):

• Ion \(\boldsymbol{\text{bigger}}\) than its atom
• \(\boldsymbol{\text{Higher}}\) ionization energy
• Requires \(\boldsymbol{\text{more}}\) energy to lose an electron
• \(\boldsymbol{\text{More}}\) electronegative