Sort these elements into isoelectronic groups. Into three different boxes/sections.
Elements:
F-
O2-
Al3+
S2-
Ti4+
K+
He
Li+
B3+
David, you must be having an identity crisis.
Isoelectronic means the same number of electrons The easy way to do this is to write the electron configuration for each, then count to see which ones are in each "box" of the same number of electrons.
9F^- means 10e = 1s2 2s2 2p6
13Al^3+ means 10e = 1s2 2s2 2p6
So these two are isoelectronic (and there could be another with 10e. If so that would be isoelectronic with these two also). The others are done the same way.
Nope, just working in a study group. Each person asking a question. Thanks for the help. I thought about doing something like that but I was writing them with the noble gas first and that was making it difficult to see the pattern.
To sort these elements into isoelectronic groups, we need to compare their electronic configurations and find elements with the same number of electrons.
Isoelectronic Group 1:
F- (fluoride ion): Electronic configuration - 1s^2 2s^2 2p^6
O2- (oxide ion): Electronic configuration - 1s^2 2s^2 2p^6
Neon (Ne): Electronic configuration - 1s^2 2s^2 2p^6
F-, O2-, and Ne all have a filled electron shell with eight electrons, making them isoelectronic. These elements belong to the first isoelectronic group.
Isoelectronic Group 2:
Al3+ (aluminum ion): Electronic configuration - 1s^2 2s^2 2p^6
S2- (sulfide ion): Electronic configuration - 1s^2 2s^2 2p^6 3s^2 3p^6
Argon (Ar): Electronic configuration - 1s^2 2s^2 2p^6 3s^2 3p^6
Al3+, S2-, and Ar all have a filled electron shell with 18 electrons, making them isoelectronic. These elements belong to the second isoelectronic group.
Isoelectronic Group 3:
Ti4+ (titanium ion): Electronic configuration - 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^0
K+ (potassium ion): Electronic configuration - 1s^2 2s^2 2p^6 3s^2 3p^6
Ti4+ and K+ both have a filled electron shell with 10 electrons, making them isoelectronic. These elements belong to the third isoelectronic group.
Considering these comparisons, the elements can be arranged into three isoelectronic groups as follows:
Group 1: F-, O2-, Ne
Group 2: Al3+, S2-, Ar
Group 3: Ti4+, K+
To sort these elements into isoelectronic groups, we need to first determine the number of electrons each element has. Elements that have the same number of electrons are considered isoelectronic.
Let's determine the number of electrons for each element:
F-: Fluorine gains 1 electron to become an ion, giving it 10 electrons.
O2-: Oxygen gains 2 electrons to become an ion, giving it 10 electrons.
Al3+: Aluminum loses 3 electrons to become an ion, giving it 10 electrons.
S2-: Sulfur gains 2 electrons to become an ion, giving it 18 electrons.
Ti4+: Titanium loses 4 electrons to become an ion, giving it 22 electrons.
K+: Potassium loses 1 electron to become an ion, giving it 18 electrons.
He: Helium already has 2 electrons.
Li+: Lithium loses 1 electron to become an ion, giving it 2 electrons.
B3+: Boron loses 3 electrons to become an ion, giving it 6 electrons.
Now, let's group them based on the number of electrons:
Group 1 (10 electrons): F-, O2-, Al3+
Group 2 (18 electrons): S2-, K+
Group 3 (2 electrons): He, Li+
Group 4 (6 electrons): B3+
So, the elements are sorted into three isoelectronic groups as follows:
Group 1: F-, O2-, Al3+
Group 2: S2-, K+
Group 3: He, Li+