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Golden Rules Of Investment

12 GOLDEN RULES OF INVESTMENT Live by these 12 rules and let your money grow!  1) The past is irrelevant –   Do not rely on past performances and build castles in the air. Invest for tomorrow and live for today.  2) Opinions can hurt. Don’t ask too many people –   just don’t!! To each, his own. What works for someone else, may not work for you and vice-versa. Your investment plan should be as unique as the back of your hand. More importantly, it must suit you best.  3) Everyone’s journey is different. Understand yours. –   Do not invest if you’re not clear on the purpose. Do not draw parallels with other investors. Your need for investing, risk appetite, and nature of investments is of utmost importance. You need to understand what you are doing.  4) Don’t allow your ego to engage with professional advice –   Trust your financial advisor! Google can give you lots of information but your advisor will tell you what’s best for you. Listen and then act!  5) Overthinking will never allow
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PAULI EXCLUSION PRINCIPLE

Electronic configuration. Pauli exclusion principle 

There are a number of " rules" that determine the way in which the electrons of an atom may be distributed, that is, that determines the electronic configuration of an atom. 

The most fundamental of these rules is the Pauli exclusion principle: only two electrons can occupy any atomic orbital, and to do so these two must have opposite spins. These electrons of opposite spins are said to be paired. Electrons of like spin tend to get as far from each other as possible. This tendency is the most important of all the factors that determine the shapes and properties of molecules. 

The exclusion principle, advanced in 1925 by Wolfgang Pauli, Jr. (of the Institute for Theoretical Physics, Hamburg, Germany), has been called the cornerstone of chemistry 

We see that an orbital becomes occupied only if the orbitals of lower energy are filled (e.g., 2s after 1s, 2p after 2s). We see that an orbital is not. occupied by a pair of electrons until other orbitals of equal energy are each occupied by one electron (e.g., the 2p orbitals). The 1s electrons make up the first shell of two, and the 2s and 2p electrons make up the second shell of eight. For elements beyond the first ten, there is a third shell containing a 3s orbital, 3p orbitals, and so on

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