Unsur gas mulia yang memiliki energi ionisasi terbesar adalah .... a. helium b. neon c. argon d. ...

Summary

The video discusses ionization energy in noble gases, explaining how atomic number and radius affect ionization trends. As you move down the group of noble gases (Helium, Neon, Argon, Krypton, Xenon, Radon), the atomic number and radius increase, making it easier for the atom to lose an electron and thus decreasing ionization energy. The video concludes that helium, being the smallest atom with the tightest electron binding, has the highest ionization energy among the noble gases.

Takeaways

• 😀 Noble gases include helium, neon, argon, krypton, xenon, and radon.
• 😀 Noble gases are highly stable, but some can react with elements of high electronegativity.
• 😀 As you move down the group of noble gases, the atomic number increases.
• 😀 With a larger atomic number, the atomic radius of noble gases also increases.
• 😀 A larger atomic radius results in outer electrons being farther from the nucleus.
• 😀 The farther the electrons are from the nucleus, the weaker the attractive force they experience.
• 😀 This weaker attraction makes it easier for noble gases to lose their outer electrons.
• 😀 As a result, ionization energy decreases as you go down the noble gas group.
• 😀 Helium has the smallest atomic radius among noble gases, making it the hardest to ionize.
• 😀 Therefore, helium has the largest ionization energy among the noble gases.

Q & A

What are the noble gases mentioned in the transcript?

The noble gases mentioned are helium, neon, argon, krypton, xenon, and radon.

Why do noble gases have high stability?

Noble gases have high stability because they have a full outer electron shell, making them less likely to react with other elements.

How does electronegativity affect the reactivity of noble gases?

Noble gases generally have low reactivity, but they can react with elements that have high electronegativity, as these elements can attract electrons from the noble gases.

What happens to the atomic radius as you move down the group of noble gases?

As you move down the group of noble gases, the atomic radius increases because additional electron shells are added, making the atoms larger.

What is the relationship between atomic number and atomic radius in noble gases?

As the atomic number increases, the atomic radius increases as well, due to the addition of more electron shells.

How does the distance between the outermost electron and the nucleus change as the atomic number increases?

As the atomic number increases, the outermost electron becomes farther from the nucleus because the atom's size increases.

Why do noble gases with larger atomic numbers have weaker attractive forces on their outermost electrons?

Noble gases with larger atomic numbers have weaker attractive forces on their outermost electrons because the electrons are farther from the nucleus, and the force of attraction decreases with distance.

What is the relationship between atomic number and ionization energy in noble gases?

As the atomic number increases in noble gases, ionization energy decreases because the outermost electrons are farther from the nucleus and are more easily removed.

Which noble gas has the highest ionization energy?

Helium has the highest ionization energy among the noble gases.

What trend in ionization energy is observed as you move down the group of noble gases?

Ionization energy decreases as you move down the group of noble gases because the outermost electron is farther from the nucleus and more easily removed.