2O. O denotes atom of oxygen. 2O denotes two atoms of oxygen. O2 denotes a molecule of oxygen gas.

Ozone is an alternative version of oxygen. Oxygen or (O2) in the air we breathe is actually two molecules of oxygen attached together. Ozone is three atoms of oxygen attached together forming a molecule that is O3.

Ozone (O3) is a triatomic molecule, consisting of three oxygen atoms. It is an allotrope of oxygen that is much less stable than the diatomic O2 (oxygen gas)….Comparison chart.

So, to reiterate, the difference between oxygen (O) and oxygen (O2) is that the former is an oxygen atom while the latter consists of two O atoms bound together, forming a molecule also called oxygen.

Answer: 3O is three molecules of oxygen but O3 shows 3 atom of oxygen in its one molecule.

We breathe in oxygen and some of this carbon dioxide. When we exhale, we breathe out less oxygen but more carbon dioxide than we inhale. The carbon we breathe out as carbon dioxide comes from the carbon in the food we eat.

O2− is larger than O because the increase in electron repulsions that accompany addition of an electron causes the electron cloud to expand. O2− is larger than O because O is neutral but O2− has a charge 2−.

The K+ ion has its outermost electrons on the third energy level now and is size is smaller than that of K ion. Hence, K is larger than K+.

Answer. Answer: o has a largest size.

(d) K+ is larger than Ca2+ Isoelectronic; Ca2+ has more protons to pull e- inward.

Br – will have the largest atomic size because Br- has one extra electron in its valence shell which due to its unbalanced negative charge will be repelled and hence the atomic radius of Br- will increase.

Ca2+ has smaller ionic radius than K+ because it has more nuclear charge. In a given period, on moving from left to right, the nuclear charge increases without addition of shell. The increased nuclear charge attracts the electrons more strongly towards the nucleus. This decreases the ionic size.

The atomic numbers of the ions are S (16), Cl (17), K (19), and Ca (20). Thus, the ions decrease in size in the order S2– > Cl– > K+ > Ca2+.

Metallic, Covalent and Ionic Radii(r)*

Generally, electron affinities become more negative across a row of the periodic table. Fluorine, therefore, has a lower affinity for an added electron than does chlorine. Consequently, the elements of the third row (n = 3) have the most negative electron affinities.

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Explanation: And for NEUTRAL atoms, reasonably, atomic size decreases across a Period, from left to right as we face the Table, and INCREASES down a Group. With respect to the parent atoms, potassium would be larger than argon, the which would be smaller than chlorine.

The ionic radii of cations follow the same trends as atomic radii. They increase from top to bottom and from right to left in the Periodic Table. Thus, the ion with the largest radius is closest to the lower left corner of the Periodic Table, and that is the K+ ion.

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francium

Atomic Radius The radius of an atom can only be found by measuring the distance between the nuclei of two touching atoms, and then halving that distance. As you can see from the diagrams, the same atom could be found to have a different radius depending on what was around it.

Atomic radius decreases across a period because valence electrons are being added to the same energy level at the same time the nucleus is increasing in protons. The increase in nuclear charge attracts the electrons more strongly, pulling them closer to the nucleus.

As electrons are added to the valence shell, an extra proton (i.e fundamental, positively charged nuclear particle) is added to the element’s nucleus. As electrons add and Z the atomic number increases 1 by 1, nuclear charge WINS, and electronic radii contract.

Why does the atomic radius decrease from left to right? Electrons enter the same energy level, as protons and electrons are added the force between the protons and electrons increase. The electrons are pulled closer to the nucleus making the atom smaller.

In general, atomic radius decreases across a period and increases down a group. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.

Yes,Atomic radius increases due to increase in their atomic number. Because, Due to increase in atomic number, No. of electrons increase. of electrons, Shells automaticaly,Increase.By Increase in shell, radius also Increase From top to bottom on Group 7.

(i) Atomic size increases as we move from top to bottom because each time one new shell is added and electrons in the outermost shell move away from the nucleus.

As you move down a column or group, the ionic radius increases. Ionic radius decreases moving from left to right across a row or period. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly.

Ionic radii increases down a group. In a group, all the ions have the same charge as they have the same valency (that is, the same number of valence electrons on the highest energy level sub-orbital). Therefore, ionic radii increase down a group as more shells are added (per period). 2.

Ionic radius is determined by measuring the atom in a crystal lattice. Removal of electrons results in an ion that is smaller than the parent element. Addition of electrons results in an ion that is larger than the parent atom.