Want this question answered?
Always the S and the P block.
Two- Since it has six valence electrons, it can form two covalent bonds, making the valence two. If it is easier to think about it this way, eight valence electrons would stabilize the element. Eight minus six is two, giving us the same answer as before.
The third energy level contains one s orbital and three p orbitals.
All alkaline earth metals have two valence electrons.
I assume you are referring to valence electrons (the "outermost" shell varies widely in the number of electrons it can hold, the valence electrons are a subset of this which are responsible for chemical bonding and reactivity).The number of valence electrons can only be from 1 electron to 8 electrons, these are divided between the s and p orbitals of a shell (each orbital can hold no more than 2 electrons).
Lead has 82 electrons. It also has four valence electrons, two s- electrons and two p- electrons in its orbitals.
Always the S and the P block.
All noble gases have completely filled orbitals. Helium has two valence electrons and its s-orbital is full and is stable. Other noble gases have completely fill p-orbitals as the valence orbitals.
Nitrogen has 5 valence electrons. Valence electrons are the electrons that are found in the outer most shell of an atom, and are consequently the electrons that move from atom to atom in the formation of compounds. The reason for this is a result of the electron configuration. A nitrogen atom has 3 orbitals; the 1s orbital, the 2s orbital, and the 2p orbital. In this case, the 2s and 2p orbitals are the valence orbitals, as they have the electrons with the most energy. With 7 protons, a neutral nitrogen atom has 7 electrons. The s orbitals can only hold 2 electrons, and the p orbitals can hold up to 6 electrons. The 1s orbital is filled first, leaving five electrons, then the 2s orbital is filled, leaving 3 electrons, and then these remaining electrons fill the 2p orbital halfway. There are a total of 5 electrons in the 2s and 2p orbitals, and since these orbitals have the most energy, there are 5 valence electrons.
Sulfur has two electrons in the 1s orbital, two electrons in the 2s orbital, and 6electrons in the 2 p orbitals. The electrons are part of the first and second energy levels, the electron core. The next energy level, the last one, is the outermost energy which comprises the valence shell.
6. Valence electrons are the electrons in the s and p orbitals. Keeping this in mind, Se has the 4s orbitals filled (2 electrons) and has 4 electrons filled in the 4p orbital (4p4). 2+4 = 6.
If I understand the theory correctly, then it is safe to assume that any molecular bond is based on the valence system. Valence bonding occurs when orbitals of electrons are slightly overlapped. Your question should rather be 'what kind of valence bond occured in the bond. There are 2 types namely sigma and pi. Sigma bonds occur when the orbitals of two shared electrons overlap head-to-head. Pi bonds occur when two orbitals overlap when they are parallel (wikipedia). So it is safe to assume that any bond that is covalent can be described using valence theory.
helium has completely filled valence orbitals and hence is stable
Two valence electrons.
Valence electrons are the total amount of electrons on the outermost shell of an atom. Meaning if the last shell has two, the valence electrons are two. But a complete valence shell would hold eight.
Two- Since it has six valence electrons, it can form two covalent bonds, making the valence two. If it is easier to think about it this way, eight valence electrons would stabilize the element. Eight minus six is two, giving us the same answer as before.
The third energy level contains one s orbital and three p orbitals.