Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
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Chemistry RI10
Oxnard College
Week 14- Hydrogen Absorption and Emission
Fall 2020
The maximum amount of electrons you can place in a specific subshell depends on the shape of the
subshell (represented by the letters s, p. d, or f). Once a subshell is full (contains the maximum number of
electrons), the next subshell then begins filling. The maximum number of electrons that can be placed in a
specific subshell is shown below:
Махimum
Subshell Number of
Electrons
P
f
14
The number of electrons that are contained within a specific subshell are represented as a numerical
superscript. For example, the electron configuration for lithium (Li), which has 3 total electrons, is 1s'2s'.
This shows that 2 electrons exist in the 1s subshell and 1 electron exists in the 2s subshell.
Write the complete electron configuration for each of the following elements:
Practice
a) Si
1s'2s2p'3s*3p?
b) Co Is2s2p'3s²3p^4s°3d?
Example #2:
a) Na
b) Mn
Electron configurations can also be written in the shorthand noble gas form, which is especially useful for
larger atoms that have many electrons. If we take a look at the electron configuration for sodium (Na), for
example, it contains the electron configuration of the noble gas neon (Ne), plus one additional electron.
We can put this noble gas in brackets and then write the rest of the electron configuration next to it, as
shown below:
Is°2s*2p®3s! = [Ne] 3s'
Electrne
configuration of Ne
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