Atomic Radius vs. Ionic Radius

In summary, atomic radius refers to the size of an atom, while ionic radius refers to the size of an ion. Generally, ionic radius is larger than atomic radius due to the change in electron distribution when an atom gains or loses electrons. Both atomic and ionic radius can vary depending on factors such as the element, its chemical environment, and its position on the periodic table. Atomic radius is typically measured using X-ray crystallography, while the factors that affect atomic and ionic radius include the number of energy levels, protons and electrons, charge, and chemical environment.
  • #1
moreovaltine
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Homework Statement



That's the problem statement (above). I basically need help knowing which fields to cover while talking about said topic in a 5-minute oral presentation. Pretty much, what I need to talk about (specifically).

Homework Equations



None.

The Attempt at a Solution



Asking you guys :P
 
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Have you started looking anywhere? Is there nothing said about this in your textbook or class notes? Have you tried looking on the internet anywhere?
 
  • #3


I would approach this topic by first defining the terms "atomic radius" and "ionic radius." Atomic radius refers to the size of an atom, specifically the distance from the nucleus to the outermost electron. Ionic radius, on the other hand, refers to the size of an ion, which is an atom that has gained or lost electrons and therefore has a different number of electrons than protons.

One of the main differences between atomic and ionic radius is that atomic radius is a physical property of an atom, whereas ionic radius is a chemical property that can change depending on the atom's environment. For example, if an atom gains an electron and becomes a negative ion, its ionic radius will be larger than its atomic radius. This is because the added electron increases the repulsive forces between the electrons, causing the outermost electron to be pushed further away from the nucleus.

Another important factor to consider when discussing atomic and ionic radius is the concept of effective nuclear charge. This refers to the attraction between the positively charged nucleus and the negatively charged electrons. As you move across a period in the periodic table, the atomic radius decreases because the effective nuclear charge increases, pulling the outermost electrons closer to the nucleus. On the other hand, as you move down a group in the periodic table, the atomic radius increases because the number of energy levels increases, shielding the outermost electrons from the attractive force of the nucleus.

In terms of ionic radius, the size of an ion is influenced by the same factors as atomic radius, but also by the charge of the ion. For example, a positively charged ion will have a smaller ionic radius than its parent atom because it has lost electrons and therefore has a higher effective nuclear charge. Conversely, a negatively charged ion will have a larger ionic radius because it has gained electrons and therefore has a lower effective nuclear charge.

It's also important to note that ionic radius can vary depending on the type of ion. For example, a monatomic ion (an ion made up of a single atom) will have a different ionic radius than a polyatomic ion (an ion made up of multiple atoms). This is because the arrangement and bonding between the atoms in a polyatomic ion can affect its overall size.

In conclusion, atomic and ionic radius are both important concepts in chemistry that help us understand the size and properties of atoms and ions. While atomic radius is a physical property that is influenced by the number of energy
 

1. What is the difference between atomic radius and ionic radius?

Atomic radius refers to the size of the atom itself, while ionic radius refers to the size of an ion. An ion is an atom that has gained or lost electrons, causing it to have a different number of protons and electrons. This change in the number of electrons affects the overall size of the ion, making it different from the size of its parent atom.

2. How do atomic and ionic radius compare?

In general, ionic radius is larger than atomic radius. This is because when an atom loses an electron to become a positively charged ion, the remaining electrons are more strongly attracted to the nucleus, causing the ion to become smaller. Conversely, when an atom gains an electron to become a negatively charged ion, the added electron repels the other electrons, causing the ion to become larger.

3. Can atomic radius and ionic radius change?

Yes, both atomic and ionic radius can change depending on the element and its chemical environment. Atomic radius can vary depending on the number of energy levels or electron shells an atom has. Ionic radius can also vary depending on the charge of the ion and its position on the periodic table.

4. How is atomic radius measured?

Atomic radius is typically measured using X-ray crystallography, which involves bouncing X-rays off of a crystal of the element and measuring the diffraction pattern. This can provide an accurate measurement of the distance between atoms in a crystal, which can then be used to calculate the atomic radius.

5. What factors affect atomic and ionic radius?

The main factors that affect atomic and ionic radius are the number of energy levels or electron shells an atom has, the number of protons and electrons in the atom, and the charge of the ion. Other factors such as the element's position on the periodic table and the presence of other atoms or molecules in its chemical environment can also impact atomic and ionic radius.

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