Which atom or ion has the largest atomic radius?
Group of answer choices
a. I-
b. Xe
c. Na+
d. Cs+
e. F-
Is it d. Cs+?
Why don't you go to Google and type in
radius of Na ion
radius of Cs ion
etc
No, it is not d. Cs+. The atom or ion with the largest atomic radius among the given options is b. Xe, which is a noble gas. Noble gases have the largest atomic radii in their respective periods.
To determine which atom or ion has the largest atomic radius among the given answer choices, we need to understand the concept of atomic radius. Atomic radius refers to the size of an atom or ion, which is typically measured as the distance from the nucleus to the outermost electron shell.
Generally, the atomic radius decreases across a period or row from left to right on the periodic table, and it increases down a group or column. This trend is mainly due to the increase in effective nuclear charge (the positive charge from the nucleus that attracts the electrons) as you move across a period.
Now let's analyze the answer choices:
a. I- (Iodide ion): Iodide ion has gained one electron compared to a neutral iodine atom, making it larger than the neutral atom. This means that the ionic radius is larger than the atomic radius. Thus, I- has a larger atomic radius compared to neutral iodine (I).
b. Xe (Xenon): Xenon is a noble gas located in the last row of the periodic table. Noble gases have relatively large atomic radii compared to other elements because they have full electron shells. Thus, Xe has a larger atomic radius as compared to I-.
c. Na+ (Sodium ion): Sodium ion has lost one electron compared to a neutral sodium atom. The loss of an electron decreases the atomic radius. Thus, Na+ has a smaller atomic radius compared to neutral sodium (Na).
d. Cs+ (Cesium ion): Cesium ion has lost one electron compared to a neutral cesium atom. Similar to sodium, the loss of an electron decreases the atomic radius. Thus, Cs+ has a smaller atomic radius compared to neutral cesium (Cs).
e. F- (Fluoride ion): Fluoride ion has gained one electron compared to a neutral fluorine atom. Similar to iodide ion (I-), the addition of an electron increases the atomic radius. Thus, F- has a larger atomic radius compared to neutral fluorine (F).
Among the options provided, the atom or ion with the largest atomic radius is b. Xe (Xenon). Therefore, the answer is not d. Cs+, but rather b. Xe.