The correct statement about ionization energy is: "refers to the energy required to lose one electron".

Here's why:

1. Metals tend to have less ionization energy, not more. This is because their electrons are generally further from the nucleus and thus easier to remove.

2. Ionization energy and electronegativity both increase across a period (from left to right) on the periodic table, so they do not have opposite trends.

3. More ionization energy does not mean less attraction between protons (p+) and electrons (e-). In fact, it's the opposite: more ionization energy means there is a stronger attraction, making it harder to remove an electron.

4. Nonmetals tend to have higher ionization energies, not less. This is because their outermost electrons are closer to the nucleus and more tightly bound.

Question

The correct statement about ionization energy is: "refers to the energy required to lose one electron".

Here's why:

1. Metals tend to have less ionization energy, not more. This is because their electrons are generally further from the nucleus and thus easier to remove.

2. Ionization energy and electronegativity both increase across a period (from left to right) on the periodic table, so they do not have opposite trends.

3. More ionization energy does not mean less attraction between protons (p+) and electrons (e-). In fact, it's the opposite: more ionization energy means there is a stronger attraction, making it harder to remove an electron.

4. Nonmetals tend to have higher ionization energies, not less. This is because their outermost electrons are closer to the nucleus and more tightly bound.

Knowee AI · Accepted Answer

The correct statement about ionization energy is: "refers to the energy required to lose one electron".

Here's why:

1. Metals tend to have less ionization energy, not more. This is because their electrons are generally further from the nucleus and thus easier to remove.

2. Ionization energy and electronegativity both increase across a period (from left to right) on the periodic table, so they do not have opposite trends.

3. More ionization energy does not mean less attraction between protons (p+) and electrons (e-). In fact, it's the opposite: more ionization energy means there is a stronger attraction, making it harder to remove an electron.

4. Nonmetals tend to have higher ionization energies, not less. This is because their outermost electrons are closer to the nucleus and more tightly bound.

22. Which of the following is true about ionization energy?1 pointmetals tend to have more ionization energyhas opposite trends of electronegativitymore energy means less attraction between p+ and e-refers to the energy required to lose one electronnonmetals tend to have less ionization energy

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