Question

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

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:

To solve this, we analyze the trends for metals and nonmetals regarding their ions, ionization energy, and electronegativity:

For Metals:

1. Ion Size vs. Atom Size: Metals typically form positive ions (cations) by losing electrons. Removing electrons reduces electron - electron repulsion and the ion has fewer electron shells (or the remaining electrons are pulled in more tightly by the nucleus). So the ion is smaller than its atom.
2. Ionization Energy: Metals have relatively low ionization energy because they tend to lose electrons easily. So they require lower energy to lose an electron.
3. Electronegativity: Metals have a tendency to lose electrons rather than gain them, so they are less electronegative.

For Nonmetals:

1. Ion Size vs. Atom Size: Nonmetals typically form negative ions (anions) by gaining electrons. Adding electrons increases electron - electron repulsion and the ion has more electrons, so the ion is bigger than its atom.
2. Ionization Energy: Nonmetals have relatively high ionization energy because they tend to gain electrons (and holding onto their own electrons is difficult to lose). So they require higher energy to lose an electron.
3. Electronegativity: Nonmetals have a tendency to gain electrons, so they are more electronegative.

Filling the Table:

Category	Ion (compared to atom)	Ionization Energy (to lose an electron)	Electronegativity
Nonmetals	bigger	higher	more

Final Answers (Filling the Blanks):

• Metals:
• Ion: smaller than its atom
• Ionization energy: lower energy to lose an electron
• Electronegative: less electronegative

• Nonmetals:
• Ion: bigger than its atom
• Ionization energy: higher energy to lose an electron
• Electronegative: more electronegative

Answer:

To solve this, we analyze the trends for metals and nonmetals regarding their ions, ionization energy, and electronegativity:

For Metals:

1. Ion Size vs. Atom Size: Metals typically form positive ions (cations) by losing electrons. Removing electrons reduces electron - electron repulsion and the ion has fewer electron shells (or the remaining electrons are pulled in more tightly by the nucleus). So the ion is smaller than its atom.
2. Ionization Energy: Metals have relatively low ionization energy because they tend to lose electrons easily. So they require lower energy to lose an electron.
3. Electronegativity: Metals have a tendency to lose electrons rather than gain them, so they are less electronegative.

For Nonmetals:

1. Ion Size vs. Atom Size: Nonmetals typically form negative ions (anions) by gaining electrons. Adding electrons increases electron - electron repulsion and the ion has more electrons, so the ion is bigger than its atom.
2. Ionization Energy: Nonmetals have relatively high ionization energy because they tend to gain electrons (and holding onto their own electrons is difficult to lose). So they require higher energy to lose an electron.
3. Electronegativity: Nonmetals have a tendency to gain electrons, so they are more electronegative.

Filling the Table:

Category	Ion (compared to atom)	Ionization Energy (to lose an electron)	Electronegativity
Nonmetals	bigger	higher	more

Final Answers (Filling the Blanks):

• Metals:
• Ion: smaller than its atom
• Ionization energy: lower energy to lose an electron
• Electronegative: less electronegative

• Nonmetals:
• Ion: bigger than its atom
• Ionization energy: higher energy to lose an electron
• Electronegative: more electronegative