Question

summary
atomic radius electronegativ i ionization energy
ionic radius
(stronger/weaker;
gains/loses)

• metals ions are

than metal
atoms, because the atom
electrons to
form the ion.

• nonmetal ions are

than
nonmetal atoms, because
the atom
electrons to form the ion.
compare the trends for
metals and nonmetals. use words such as smaller/bigger, higher/lower, more/less
metals nonmetals

• ion than its atom • ion than its atom
• ionization energy • ionization energy
• requires energy to • requires energy to

lose an electron lose an electron

• electronegative • electronegative

Explanation:

Ionic Radius Section

• For Metals: Metal atoms lose electrons to form cations. When an atom loses electrons, the remaining electrons experience a greater effective nuclear charge, pulling them closer to the nucleus. So metal ions are smaller than metal atoms, because the atom loses electrons to form the ion.
• For Nonmetals: Nonmetal atoms gain electrons to form anions. Gaining electrons increases electron - electron repulsion in the electron cloud, causing the electron cloud to expand. So nonmetal ions are bigger than nonmetal atoms, because the atom gains electrons to form the ion.

Compare the trends for metals and nonmetals Section

Metals

• Ion size: As explained above, metal ions are formed by losing electrons. The removal of electrons reduces electron - electron repulsion and increases the effective nuclear charge on the remaining electrons. So ion is smaller than its atom.
• Ionization energy: Metals have relatively low ionization energy. Ionization energy is the energy required to remove an electron from an atom. Since metals tend to lose electrons easily, they have lower ionization energy. And it requires less energy to lose an electron.
• Electronegativity: Electronegativity is the ability of an atom to attract electrons. Metals tend to lose electrons rather than attract them, so they are less electronegative.

Nonmetals

• Ion size: Nonmetal ions are formed by gaining electrons. The addition of electrons increases electron - electron repulsion in the electron cloud, making the ion larger. So ion is bigger than its atom.
• Ionization energy: Nonmetals have relatively high ionization energy because they tend to gain electrons rather than lose them. So they have higher ionization energy and it requires more energy to lose an electron.
• Electronegativity: Nonmetals have a strong tendency to attract electrons, so they are more electronegative.

Filling the Blanks

Ionic Radius

• 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.

Compare the trends for metals and nonmetals

Metals	Nonmetals
\(\boldsymbol{\text{Lower}}\) ionization energy	\(\boldsymbol{\text{Higher}}\) ionization energy
Requires \(\boldsymbol{\text{less}}\) energy to lose an electron	Requires \(\boldsymbol{\text{more}}\) energy to lose an electron
\(\boldsymbol{\text{Less}}\) electronegative	\(\boldsymbol{\text{More}}\) electronegative

Answer:

Ionic Radius Section

• For Metals: Metal atoms lose electrons to form cations. When an atom loses electrons, the remaining electrons experience a greater effective nuclear charge, pulling them closer to the nucleus. So metal ions are smaller than metal atoms, because the atom loses electrons to form the ion.
• For Nonmetals: Nonmetal atoms gain electrons to form anions. Gaining electrons increases electron - electron repulsion in the electron cloud, causing the electron cloud to expand. So nonmetal ions are bigger than nonmetal atoms, because the atom gains electrons to form the ion.

Compare the trends for metals and nonmetals Section

Metals

• Ion size: As explained above, metal ions are formed by losing electrons. The removal of electrons reduces electron - electron repulsion and increases the effective nuclear charge on the remaining electrons. So ion is smaller than its atom.
• Ionization energy: Metals have relatively low ionization energy. Ionization energy is the energy required to remove an electron from an atom. Since metals tend to lose electrons easily, they have lower ionization energy. And it requires less energy to lose an electron.
• Electronegativity: Electronegativity is the ability of an atom to attract electrons. Metals tend to lose electrons rather than attract them, so they are less electronegative.

Nonmetals

• Ion size: Nonmetal ions are formed by gaining electrons. The addition of electrons increases electron - electron repulsion in the electron cloud, making the ion larger. So ion is bigger than its atom.
• Ionization energy: Nonmetals have relatively high ionization energy because they tend to gain electrons rather than lose them. So they have higher ionization energy and it requires more energy to lose an electron.
• Electronegativity: Nonmetals have a strong tendency to attract electrons, so they are more electronegative.

Filling the Blanks

Ionic Radius

• 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.

Compare the trends for metals and nonmetals

Metals	Nonmetals
\(\boldsymbol{\text{Lower}}\) ionization energy	\(\boldsymbol{\text{Higher}}\) ionization energy
Requires \(\boldsymbol{\text{less}}\) energy to lose an electron	Requires \(\boldsymbol{\text{more}}\) energy to lose an electron
\(\boldsymbol{\text{Less}}\) electronegative	\(\boldsymbol{\text{More}}\) electronegative