Chemistry
Elements and Compounds
Molecular Mass

# How are the empirical and molecular formulas for a compound related?

A molecular formula is identical to the empirical formula, and is based on quantity of atoms of each type in the compound.

The relationship between empirical and molecular formula is that the empirical formula is the simplest formula, and the molecular can be the same as the empirical, or some multiple of it. An example might be an empirical formula of C3H8. Its molecular formula may be C3H8 , C6H16, C9H24, etc. Looking at it the other way, if the molecular formula is C6H12O6, the empirical formula would be CH2O.

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The molecular formula add the structure to a empirical formula.

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Molecular formula is integral multiple of empirical formula.

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The empirical formula is the lowest common denominator of the molecular formula.

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## Related Questions

Molecular formula is the integral multiple of Empirical formula.

An empirical formula is a brutto formula; a molecular formula explain the structure of a molecule.

Both formulas are possible molecular formulas for the same empirical formula, CH2.

the empirical formula only gives the amount of each element as a ratiothe molecular formula gives the actual number of atoms of each element in a molecule of the compoundFor example these compounds all have the same empirical formula (CH2) but different molecular formulas: ethylene C2H4butene C4H8cyclohexane C6H12cyclooctane C8H16cyclodecane C10H20etc.

The empirical formula is the lowest whole integer representation of the molecular formula. For example, the empirical formula for C6H12O6 would be CH2O.

The same as its molecular formula; CH4. See related question below for more details on how to find empirical formulas.

In order to find molecular formula from empirical formula, one needs to know the molar mass of the molecular formula. Then you simply divide the molar mass of the molecular formula by the molar mass of the empirical formula to find out how many empirical formulae are in the molecular formula. Then you multiply the subscripts in the empirical formula by that number.

The empirical formula for nitrogen dioxide is the same as its molecular formula - NO2. See related question below for more details on how to find empirical formulas.

Molecular.See the Related Questions to the left for how to determine if a molecule is molecular of ionic.

The chemical formula in which the subscripts are given in the smallest ratio.

Ca3P2 or Ca3(PO4)2 See related question below for more details on how to find empirical formulas.

Molecular mass and formula mass represent the mass of an individual molecule or formula unit of a compound.

Molecular formulas refer to covalently bonded substances (molecules). The molecular formula shows the exact number of atoms of each element present in the smallest unit of the substance. For example, benzene is a molecule composed of six carbon and six hydrogen atoms and has a formula C6H6.A formula unit refers to ionic compounds and network solids (both are crystals). Because in ionic crystals each ion is electrostatically bonded to every oppositely charged nearest neighbor, the ions in the whole crystal can be thought of as part of one single bonded entity. It is the same with network solids except that the bond is covalent. So rather than using a formula that shows all of the elements present in any one particular crystal, the formula unit shows the elements present in the smallest whole number ratio. In a common example, sodium chloride, the formula unit is NaCl since sodium and chloride are present in the crystal in a 1:1 ratio. The NaCl crystal itself, however, would have >>quintillians each of Na and Cl if it was big enough to see with the unaided eye. It is important to not confuse formula units with emprical formulas. Emprical formulas are simply the lowest whole number ratio of elements in a compound. Formula units are always empirical, whereas molecular formulas are usually not. For example, the empirical formula of benzene, C6H6, is CH, since there is a 1 to 1 ratio of C to H. Note that several molecules can have the same empirical formula. For example acetylene, with molecular formula C2H2, also has the same empirical formula as benzene, even though the two molecules are very different! Water, H2O, is an example of a molecular formula that is also empirical.A formula unit is the symbolic representation of an ionic compound or network solid, and a molecular formula is the symbolic representation of a molecular compound.See the Web Links and Related Questions links for more information.

The formula for ethyl alcohol, or ethanol, is C2H6O.See the Related Questions to the left to determine the molecular weight of any compound, such as ethanol.

You can't without more information. You cannot go from the molecular weight of a compound to its formula without more information about what atoms it contains.See the Related Questions link to the left for a more detailed discussion of this.

Molecular is defined as something of, related to, or consisting of molecules. Another definition of molecular is something of or related to a basic form or structure.

Molecular orbital is related to a molecule; atomic orbital is related to an atom.

You need additional information to go from the molar mass to the molecular formula. You need to know something about what elements are present in the compound and often you need to know what the percent composition of the compound is of each element. This is done by something called elemental analysis.For example, let's say you have a compound with molecular weight of 44 grams per mole. That could be C3H8 (propane) or CO2 (carbon dioxide). Without knowing more, there is no way to know which it is.Or if the molecular weight is 18 grams per mole, it could be water (H2O) or ammonium (NH4+). Again, no way to tell without some information about what elements the compound contains.From the molecular formula, you can always determine the molar mass. See the Related Questions link to the left for how to do that.

C6H12O6 is the empirical formula for a bunch of carbohydrate compounds. The empirical formula isn't enough to tell you exactly what substance it is; for that you'd need the structural formula, which shows exactly which atoms go where in the molecule. However C6H12O6 compounds do include ordinary glucose and if the question is related to high-school science homework, then that is probably what it's intended to mean.

The concentration is related to the volume of the atmosphere and the amount of the element your looking at.Molarity(concentration)= G/(Molecular weight)x Liters(volume)

MgCl2 is the correct formula, or two atoms of Cl for each 1 atom of Mg. You could also say 2 moles of Cl atoms for every 1 mole of Mg atoms. The empirical formula should be written with the subscripts in lowest whole number terms. Note that this formula is consistent with the fact that an Mg cation is Mg+2 and a Cl anion is Cl-1. Given these charges, a formula of MgCl2 is the one with the smallest whole number subscripts that will allow the charge of the compound to be zero. See related question below for more details on how to find empirical formulas.

The molecular shape of SCl2 is bent. Please see the related link below.

The molecular formula is (NH4)2SO4.See the Related Question link to the left for how to find the molecular weight using the molecular formula.