Atomic radius and Ionization Energy Trends?

In summary, the trend for the radius of an atom is that the larger the atom, the more electrons it has. The trend for ionization energy is that the more electrons an atom has, the more energy it takes to remove them.
  • #1
hamza2095
28
1
My teacher was not too clear about this and from what I've gathered is if you're given two elements this is how you would figure out which one has a larger atomic radius or ionization energy, but I'm not sure if it's accurate

Radius: Whichever one is in a lower period (more energy levels) has a larger radius, if they're in the same period whichever one has the lower atomic number has a larger atomic radius
I.E - Whichever one is in the higher period (less energy levels) has more ionization energy, if they're in the same period the one with the higher atomic number is higher

Also, are Electronegativity and I.E the same thing except noble gases have an electronegativity of 0?
 
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  • #2
You should be able to easily find raw data (for example just google for periodic table trends atomic radius) and they will either confirm, or deny what you wrote.

To (mis)quote or paraphrase Feynman - in the end it is data (nature) that is right, doesn't matter what we think or predict.
 
  • #3
Hey there,

For the radius, whichever atom has the most electrons is the biggest. However, if you have two atoms with the same number of electrons, the atom with the LEAST PROTONS is the biggest. Ionization Energy is how much energy is required to remove an electron, so atoms with a full octet will require the most energy in order to remove an electron. So the more valence electrons = more I.E required.

Also, no, electronegativity and ionization energy aren't the same thing. Electronegativity is the attraction due to different charges.
 
  • #4
cazzuey said:
For the radius, whichever atom has the most electrons is the biggest.

Not necessarily. Check radii of lanthanides.
 
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  • #5
cazzuey said:
For the radius, whichever atom has the most electrons is the biggest.

Actually this holds well till we reach the f-block elements. Post this, the phenomenon of lanthanide contraction dominates and we observe deviations. Just like Borek said.
 
  • #6
Borek said:
You should be able to easily find raw data (for example just google for periodic table trends atomic radius) and they will either confirm, or deny what you wrote.

To (mis)quote or paraphrase Feynman - in the end it is data (nature) that is right, doesn't matter what we think or predict.

You do that thing. It's a matter for your judgment whether the data you will find could be called 'raw'. Until you understand how the conclusions called 'data' have been arrived at it is not fully scientific.

Here is an official explanation of the results, though not how they were obtaine, and you can find many others like it:. https://www.khanacademy.org/science...ic-table-trends-bonding/v/atomic-radius-trend

If you are intending to go much further in chemistry (or atomic physics) then I advise: always connect. Ionisation is the special extreme case of promotion or increase of energy of an electron. The more general case is jumping between different levels within the atom. If you have got at least as far as the Bohr atom, then Google for Mosley's law, and pick among what comes out according to your level.
 
  • #7
The Chemical Touch app, is an excellent reference for this sort of stuff and only costs a dollar and a half. There's also the free Merck PTE app that has this information laid out in a very elegant graphical form and it's free without ads!
 

1. What is atomic radius and how does it vary across the periodic table?

Atomic radius is the measure of the size of an atom. It is defined as the distance from the center of the nucleus to the outermost electron orbital. Atomic radius generally decreases from left to right across a period and increases from top to bottom within a group on the periodic table.

2. What factors influence the trend of atomic radius?

The trend of atomic radius is influenced by two main factors: the number of protons in the nucleus and the number of electron shells. As the number of protons increases, the positive charge in the nucleus increases, pulling the electrons closer and decreasing the atomic radius. On the other hand, as the number of electron shells increases, the size of the atom also increases, leading to a larger atomic radius.

3. What is ionization energy and how does it change across the periodic table?

Ionization energy is the energy required to remove an electron from an atom. Ionization energy generally increases from left to right across a period, as the atomic radius decreases and the electrons are held more tightly to the nucleus. It decreases from top to bottom within a group, as the atomic radius increases and the outermost electrons are further from the nucleus, making them easier to remove.

4. What are the implications of high and low ionization energy?

High ionization energy indicates that the electrons are tightly bound to the nucleus, making it difficult to remove them. This is characteristic of elements on the right side of the periodic table. Low ionization energy means that electrons are easily removed from the atom, which is common for elements on the left side of the periodic table. This can affect an element's reactivity and ability to form compounds.

5. How do atomic radius and ionization energy relate to each other?

Atomic radius and ionization energy have an inverse relationship. As atomic radius increases, ionization energy decreases. This is because the electrons are further from the nucleus, making them easier to remove. And as atomic radius decreases, ionization energy increases, as the electrons are held more tightly to the nucleus. This trend can be seen in the periodic table, with high ionization energy elements on the right side and low ionization energy elements on the left side.

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