Atomic Radius
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 133
- Joined: Wed Sep 30, 2020 9:45 pm
Atomic Radius
How do we know between ions of the same element, which ion may have a larger atomic radius?
Fe2+ vs. Fe3+
Also, do isoelectronic elements have the same size radius? I know they have the same number of electrons, but I am not sure if they have the same atomic radius.
Fe2+ vs. Fe3+
Also, do isoelectronic elements have the same size radius? I know they have the same number of electrons, but I am not sure if they have the same atomic radius.
-
- Posts: 101
- Joined: Wed Sep 30, 2020 9:49 pm
Re: Atomic Radius
The ion with the larger atomic radius would be the one with the less positive charge. In this case, it would be Fe 2+. The reason being is that the one with the lesser positive charge has more electron repulsion between the electrons which result in the radius to be slightly expanded. For the more positive charge, there is less of the repulsion allowing for the electrons to be more easily attracted to the nucleus thus decreasing the atomic radius. For isoelectronic elements, the atomic radius varies. Although the isoelectronic elements have the same number of electrons, the number of protons varies. So essentially, the elements that have more protons and less electron repulsion would have the smallest atomic radius. I hope this helps!
-
- Posts: 133
- Joined: Wed Sep 30, 2020 9:45 pm
Re: Atomic Radius
Rich Luong 1B wrote:The ion with the larger atomic radius would be the one with the less positive charge. In this case, it would be Fe 2+. The reason being is that the one with the lesser positive charge has more electron repulsion between the electrons which result in the radius to be slightly expanded. For the more positive charge, there is less of the repulsion allowing for the electrons to be more easily attracted to the nucleus thus decreasing the atomic radius. For isoelectronic elements, the atomic radius varies. Although the isoelectronic elements have the same number of electrons, the number of protons varies. So essentially, the elements that have more protons and less electron repulsion would have the smallest atomic radius. I hope this helps!
WOW thank you so much that cleared it up so much for me!!!
-
- Posts: 104
- Joined: Wed Sep 30, 2020 9:42 pm
Re: Atomic Radius
We know if the ions have a larger radius is they have a less positive charge. If they have a high positive charge then that means the ion lost electrons and electrons is a key part that makes the size of ions and atoms because of repulsion. Which is the electron cloud.
-
- Posts: 101
- Joined: Wed Nov 13, 2019 12:19 am
Re: Atomic Radius
The ion with the larger radius would be the ion that has a less positive charge, in this case, Fe2+.
-
- Posts: 102
- Joined: Wed Sep 30, 2020 9:32 pm
- Been upvoted: 1 time
Re: Atomic Radius
The larger the cation's charge the smaller the atomic radius as the loss of electrons reduces the size of the orbitals and increases the effective nuclear charge which pulls the electrons closer to the nucleus as a result. Hope this helps!
-
- Posts: 55
- Joined: Wed Sep 30, 2020 9:34 pm
Re: Atomic Radius
If the ion has a larger radius, it will also have a less positive charge. If it has a high positive charge then that indicates that the ion has lost some electrons. Electrons play an important part, making up the size of atoms and ions because of the repulsion they cause in the electron cloud.
-
- Posts: 124
- Joined: Wed Sep 30, 2020 9:43 pm
Re: Atomic Radius
how do we use the atomic radius to calculate the bond length? what information would we need to know?
-
- Posts: 109
- Joined: Fri Sep 24, 2021 6:54 am
Re: Atomic Radius
205323697 wrote:how do we use the atomic radius to calculate the bond length? what information would we need to know?
I think you need to actually know the covalent radii to calculate the bond length. Atomic radius is merely for a singular atom.
-
- Posts: 85
- Joined: Fri Sep 24, 2021 5:29 am
Re: Atomic Radius
The ion with the less positive charge would have a greater atomic radius. In this case, it would be Fe2+.
-
- Posts: 106
- Joined: Fri Sep 24, 2021 5:26 am
Re: Atomic Radius
Less positively charged ions tend to have a larger radius, so FE 2+ is the correct answer here.
-
- Posts: 52
- Joined: Fri Sep 24, 2021 5:09 am
Re: Atomic Radius
Hi!
Since Fe2+ has a lower effective nuclear charge than Fe3+, Fe2+ should have a bigger radius. Ions with lower effective nuclear charges tend to have bigger radii while ions with higher effective nuclear charges tend to have smaller radii. Effective nuclear charge is determined by the number of protons and electrons that an atom or ion has. Since Fe2+ has a lower effective nuclear charge, electrons aren't pulled in as close to the nucleus (in comparison to Fe3+), so it should have a larger radius.
I hope this helps!
Since Fe2+ has a lower effective nuclear charge than Fe3+, Fe2+ should have a bigger radius. Ions with lower effective nuclear charges tend to have bigger radii while ions with higher effective nuclear charges tend to have smaller radii. Effective nuclear charge is determined by the number of protons and electrons that an atom or ion has. Since Fe2+ has a lower effective nuclear charge, electrons aren't pulled in as close to the nucleus (in comparison to Fe3+), so it should have a larger radius.
I hope this helps!
-
- Posts: 106
- Joined: Fri Sep 24, 2021 7:20 am
Re: Atomic Radius
A general trend on the periodic table that I have found to be helpful conceptually for problems involving atomic radius is that atomic radius increases going vertically down the period table (from the top to the bottom) and atomic radius decreases going horizontally across the periodic table from the left to the right.
Return to “Trends in The Periodic Table”
Who is online
Users browsing this forum: No registered users and 3 guests