empirical vs molecular

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danielruiz1G
Posts: 62
Joined: Fri Apr 06, 2018 11:04 am

empirical vs molecular

Postby danielruiz1G » Sun Apr 15, 2018 11:36 pm

why when solved are the outcomes so different like in the example Dr. Lavelle gave us with glucose, CH2O(empirical) and C6H12O6(molecular)?

Chris Fults 1C
Posts: 27
Joined: Wed Nov 15, 2017 3:01 am

Re: empirical vs molecular

Postby Chris Fults 1C » Sun Apr 15, 2018 11:49 pm

Empirical formulas give us the basic structure of the covalently bonded molecule within the molecule. The molecular formula gives us the actual number of elements in a molecule. The Empirical formula tells us the ratio of elements in a compound which is helpful in

1. Calculating the percentage composition of the elements in a compound.

2. An elemental analysis of an unknown sample.

3. In the synthesis of a new compound.

Salena Chowdri 1I
Posts: 66
Joined: Fri Apr 06, 2018 11:02 am

Re: empirical vs molecular

Postby Salena Chowdri 1I » Wed Apr 18, 2018 9:08 pm

The empirical formula is the most simplified version of the formula, with the smallest ratio of whole numbers. So if glucose C6H1206 was divided by 3, we would get CH2O which is that most simplified formula. The molecular accounts for the actual state of the compound and its atomic binding.

Neha Divi 1K
Posts: 31
Joined: Fri Apr 06, 2018 11:02 am

Re: empirical vs molecular

Postby Neha Divi 1K » Thu Apr 19, 2018 11:31 am

Additionally, using the empirical formula and knowing the molar mass allows you to find the molecular formula by dividing the molar mass by the mass of the empirical compound to find the actual number of atoms in the molecular formula compared to the ratio.

ElizabethP1L
Posts: 59
Joined: Wed Nov 15, 2017 3:01 am

Re: empirical vs molecular

Postby ElizabethP1L » Thu Apr 19, 2018 9:02 pm

The empirical formula just gives us the relative number of atoms not the actual number. Therefore, usually the empirical formula will be much smaller than the molecular formula. If you notice however, multiplying each element of the empirical formula by the same number results in the molecular formula.

Endri Dis 1J
Posts: 33
Joined: Fri Apr 06, 2018 11:02 am

Re: empirical vs molecular

Postby Endri Dis 1J » Fri Apr 20, 2018 1:10 am

If this helps another example would be the formula for ethylene glycol which has a molecular formula of C2H602 which would give you the empirical formula when simplified by 2 ( a whole number) CH3O.


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