SIMPLY-The element Oxygen can either capture two electrons or share two elect
so just for the more techy side......ns.
The Electron Structure of Oxygen
Oxygen atoms have 8 protons and therefore 8 electrons in their neutral state. If we follow the subshell filling guide for elements, we end up with this: 1s2 2s2 2p4. This tells us that Oxygen has two shells of electrons. The first is holds only two electrons and is completely filled. The second contains six electrons, with space for another two electrons to make the full complement of 8 which is necessary for stability. As these outer shell electrons are arranged in pairs, we get the electron dot diagram for Oxygen as shown to the left. We can see from this that Oxygen will want to either capture two electrons or share two electrons to achieve stability.
We can see a more detailed image of the electron structure of the Oxygen element below. Subshells are indicated by the black horizontal lines. The numbers in brackets show the maximum number of electrons that can be placed in that subshell is the number given in brackets.
The lone pair electron region is the place around the central atom where electrons not bonding with another atom can be found. A lone pair of electrons are electrons that are not bonded with other atoms.
Repulsion of the unshared electron pairs (2)and the bonded pairs (2) around the central oxygen atom. Repulsion of these 4 electron pairs attempts to form a tetrahedral shape. Describing the molecular shape, we ignore the unshared electrons and just describe the shape of the molecule based on the location of the atoms, thus bent.
Chlorine (nucleus) has 1 lone pair and 3 polar-covalent bonding pairs (the shared pairs with O). Each oxygen (nucleus) has 3 lone pairs and 1 polar-covalent bonding pair (the shared pair with Cl)
The molecular geometry of NH4+ is tetrahedral. This is because NH4+ has four bonding regions (four hydrogen atoms bonding with the central nitrogen atom) and no lone pairs of electrons on the central nitrogen atom.
If an atom has five valence electrons, it will have one lone pair of electrons.
ONE!
Electrons exist as pairs. Although, electrons hate each other, and only go as pairs as a last resort.
H-O-H Well, the hydrogens bring a total of two valance electrons to the mix and the oxygen contributes six, so the total valance electrons = 8 4 are used in the two bonds, so 8 - 4 = 4 Two lone pair, one above and one below the oxygen in the Lewis dot structure.
There are four electrons, which is two pair.
The Central atom has no lone pairs in CH4
They share two pairs of electrons and have 2 lone pairs
4 pairs
One lone pair. The central atom is N (nitrogen) which has 5 valence electrons. Three of them are shared with 3 hydrogen atoms, leaving 2 electrons (1 lone pair) on the N.
These pairs of electrons are referred to as lone pairs.
lone pairs
The answer is not 6 as said here before! The number of valence electrons in O2 (oxygen molecule) is: 12 valence electrons. 6 of them from each oxygen (O) atom. 4 valence electrons make up the double bond between the two oxygen atoms, and the remaining 8 valence electrons form lone pairs (non-bonding pairs) on the oxygen atoms, 2 lone pairs on each. I hope there is some help in this.
Cl4 doesn't exist. It should be Cl2 and there will be 4 pairs of non bonding electrons on each chlorine.