nucleus

An atom contains equal numbers of protons and electrons . Since protons and electrons have equal and opposite charges , this means that atoms are neutral overall.

Cation, atom or group of atoms that bears a positive electric charge. See ion. Positively charged ions are called cations; negatively charged ions, anions. Ions are formed by the addition…

If an atom, or atoms, has a balanced number of electrons (negative charge) and protons (positive charge) they are neutral overall….Cation vs anion chart.

Cations are positively charged ions. They are formed when a metal loses its electrons. They lose one or more than one electron and do not lose any protons. Some examples of cations are Calcium (Ca2+), Potassium (K+), hydrogen (H+).

Actually four resonance structures can be drawn for N−3, but the possible structures are only three, since in the structure IV, the N in the right most end does not fulfill the criteria of octet configuration.

There are seven resonance structures for SO3 .

In the Lewis Structure for N3- you’ll need to place a double bonds between the Nitrogen atoms to achieve full outer shells on all atoms while only using the valence electrons available for the molecule. There are 16 valence electrons for the Lewis structure for N3-.

F3 ion does not exist due to its small size and absence of vacant d-orbital to expand its covalency from one to two whereas Iodine have large size and vacant d orbital to form I3 ion. Note : Size is the major reason for non existence of F ion.

Lewis Dot of Triiodide Ion I3- I does not follow the octet rule. It will hold more than 8 electrons. Iodine having valence electrons in the 4th energy level, will also have access to the 4d sublevel, thus allowing for more than 8 electrons.

The central F atom is required to have a d orbital if F3- was to exist. This is not possible as F can not have an expanded octet, therefore F3- does not exist. The atom is too small (does not have d orbitals) to exceed the octet, therefore, it does not exist.

Although I3- is known, F3- is not. One of your classmates says F3- does not exist because it would violate the octet rule. SF6, ClF5, and XeF4 are three compounds whose central atoms do not follow the octet rule. Draw Lewis structures for these compounds.

BCl3 do not obey octet rule.It is a electron deficient molecule.As it share only three electron with chlorine atom . After forming a molecule boron has only six electrons I.e three from chlorine atom and three of its own. Nitrogen molecule will be achieving octet by sharing three electrons.

Octet rule: The concept that compounds containing carbon, nitrogen, oxygen, and fluorine are more stable if these atoms have eight valence electrons. When one of these atoms has less than eight valence electrons it has an open octet. Every carbon, nitrogen, oxygen, and fluorine atom in this molecule has a full octet.

The octet rule can be ‘expanded’ by some elements by utilizing the d-orbitals found in the third principal energy level and beyond. Sulfur, phosphorus, silicon, and chlorine are common examples of elements that form an expanded octet.

From the electron-in-box diagram we can see that oxygen has 2 unpaired electrons so can form 2 covalent bonds. In total oxygen will have 4 electrons from the 2 bonds and 4 electrons from its 2 lone pairs which adds up to 8 electrons. Hence oxygen is octet and obeys octet rule.