Chemistry: Ionization Energy And Nuclear Charge Quiz

1. True or false: As you go across, there are the same number of outer electrons in the entire row.

True

False

False. As you go across a row in the periodic table, the number of outer electrons does not remain the same. The number of outer electrons increases by one from left to right across a row, except for the transition metals. The transition metals have a variable number of outer electrons, which can be different for each element in the row.

Explanation

False. As you go across a row in the periodic table, the number of outer electrons does not remain the same. The number of outer electrons increases by one from left to right across a row, except for the transition metals. The transition metals have a variable number of outer electrons, which can be different for each element in the row.

2. True or False: The proccess of when an atom GAINS electrons to become an ion, is called Ionization.

True

False

The process of when an atom GAINS electrons to become an ion is actually called reduction, not ionization. Ionization refers to the process of when an atom or molecule loses or gains electrons to form ions.

Explanation

The process of when an atom GAINS electrons to become an ion is actually called reduction, not ionization. Ionization refers to the process of when an atom or molecule loses or gains electrons to form ions.

3. Ionization energies generally _____________ as you move from left to right across a _________

As you move from left to right across a period, the ionization energies generally increase. This is because the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the electrons in the outermost energy level. As a result, more energy is required to remove an electron, resulting in higher ionization energies.

Explanation

As you move from left to right across a period, the ionization energies generally increase. This is because the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the electrons in the outermost energy level. As a result, more energy is required to remove an electron, resulting in higher ionization energies.

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4. Nuclear charge is ....

The increased hold on the valence electrons

The energies that generally increase as you move from left to right on a period

When electricity is plugged in a nuclear plant and charged until 100%

The total charge of all protons in the nucleus

Nuclear charge refers to the total charge of all protons in the nucleus of an atom. Protons carry a positive charge, and their total charge determines the overall charge of the nucleus. This charge influences the behavior of the valence electrons and the energies of the electrons in an atom. As the number of protons increases, the nuclear charge also increases, leading to a stronger attraction between the nucleus and the valence electrons. This increased hold on the valence electrons is responsible for the energies that generally increase as you move from left to right on a period in the periodic table.

Explanation

Nuclear charge refers to the total charge of all protons in the nucleus of an atom. Protons carry a positive charge, and their total charge determines the overall charge of the nucleus. This charge influences the behavior of the valence electrons and the energies of the electrons in an atom. As the number of protons increases, the nuclear charge also increases, leading to a stronger attraction between the nucleus and the valence electrons. This increased hold on the valence electrons is responsible for the energies that generally increase as you move from left to right on a period in the periodic table.

5. As you go down a group, atoms have more total _________electrons, so they don't really care that much about their outermost ones.

As you move down a group (vertical column) in the periodic table, atoms have more electron shells, increasing the distance between the outermost electrons (valence electrons) and the positively charged nucleus. This greater distance reduces the attractive force between the nucleus and the valence electrons, making them less tightly held and more likely to participate in chemical reactions.

Explanation

As you move down a group (vertical column) in the periodic table, atoms have more electron shells, increasing the distance between the outermost electrons (valence electrons) and the positively charged nucleus. This greater distance reduces the attractive force between the nucleus and the valence electrons, making them less tightly held and more likely to participate in chemical reactions.

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