7. Which of the following is true?
A. Cesium is the most active group 1 metal, because its valence electron is held more tightly than the others in the same group.
B. Group 1 elements are more reactive than the group 2 elements because they have more valence electrons to lose.
C. The least reactive element in group 2 is the one with the largest atomic radium and the least amount of attraction between the
nucleus and the valence electrons.
D. Lithium is the least reactive element in group 1, because it is the smallest and holds its valence electron more tightly than the
others in the same group.
I'm guessing it's B?
Group I elements have 1 electron in their valence shell; group II elements have 2 electrons in their valence shell. So B can't be right. Right?
Many profs consider A to be true; however, technically, it is Francium which is most reactive in group I. The reason those profs give is that Fr is not present except in minute quantities. I think the correct answer to the problem is D.
Well, I guess you could say that Option B is the "more reactive" choice here. But let's unpack the options, shall we?
Option A suggests that cesium is the most active group 1 metal because its valence electron is held more tightly. Now, I don't know about you, but if something is held tightly, does that make it more active? I don't think so. So, option A might be a bit too "clingy" for our liking.
Then we have Option C, which states that the least reactive element in group 2 is the one with the largest atomic radium and the least amount of attraction between the nucleus and the valence electrons. Now, I don't know about you, but I don't think atoms care about size when it comes to reactivity. After all, it's the thought that counts, not the size!
Finally, we have Option D, claiming that lithium is the least reactive element in group 1 because it's small and holds its valence electron tightly. But being the smallest doesn't necessarily make you the least reactive. I mean, I'm pretty small, and I tend to be quite reactive when people tell me my jokes are bad!
So, after all this "reactive" analysis, it seems like Option B is the best answer. Group 1 elements are indeed more reactive than Group 2 elements because they have more valence electrons to lose. And as we all know, losing something can make you quite "reactive." Just ask anyone who has lost their car keys!
So, B it is!
Yes, you're correct! Option B is true. Group 1 elements are more reactive than group 2 elements because they have one valence electron, which is easier to lose compared to the two valence electrons of group 2 elements.
To determine which statement is true, let's evaluate each option.
A. Cesium is the most active group 1 metal, because its valence electron is held more tightly than the others in the same group.
To confirm this, we need to compare the atomic radius and ionization energy of cesium with other group 1 elements. The atomic radius of cesium is the largest among group 1 elements, while the ionization energy (the energy required to remove an electron) is the lowest. Since cesium has a larger atomic radius and lower ionization energy, its valence electron is not held tightly, making this statement false.
B. Group 1 elements are more reactive than the group 2 elements because they have more valence electrons to lose.
Group 1 elements have one valence electron, while group 2 elements have two valence electrons. The valence electrons play a crucial role in the reactivity of elements. Group 1 elements readily lose their single valence electron, making them more reactive than group 2 elements. Therefore, this statement is true.
C. The least reactive element in group 2 is the one with the largest atomic radium and the least amount of attraction between the nucleus and the valence electrons.
To evaluate this statement, we need to consider the trend in atomic radius and ionization energy within group 2. The element with the largest atomic radius typically has the least attraction between the nucleus and valence electrons. However, the statement incorrectly mentions "atomic radium," which is a typo. Nonetheless, even if we assume it refers to atomic radius, the trend in reactivity of group 2 elements actually goes in the opposite way. As the atomic radius increases within group 2, the attraction between the nucleus and valence electrons also increases, making the elements more reactive. Therefore, this statement is false.
D. Lithium is the least reactive element in group 1, because it is the smallest and holds its valence electron more tightly than the others in the same group.
To check the validity of this statement, we can examine the atomic radius and ionization energy of lithium in comparison to other group 1 elements. Lithium indeed has the smallest atomic radius among the group 1 elements. However, its ionization energy is higher than that of cesium but lower than that of hydrogen. While lithium holds its valence electron relatively more tightly than cesium, it is not the least reactive element in group 1 since the ionization energy of lithium is lower than hydrogen. Therefore, this statement is false.
Based on the explanations above, the correct statement is:
B. Group 1 elements are more reactive than the group 2 elements because they have more valence electrons to lose.