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Which could represent the empirical and the formula of a given compound?
Wiki User
∙ 9y ago
The empirical formula is representative for the chemical composition of a compound; the structural formula is representative for the spatial structure of the compound.
Wiki User
∙ 9y ago
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Would ionic or covalent molecules use the molecular formula or empirical formula?
What you write for an ionic compound is called the formula unit, but the formula unit is almost always the same as the empirical formula. The answer to your question could not be the molecular formula because an ionic compound is not a molecule.
Explain why the percent composition of certain compounds are not sufficient to determine the compounds molecular formulas?
Because unlike the empirical formula, the molecular formula does not have to be the simplest ratio.If by chance you are given the percent composition of the elements in a substance, you could calculate the empirical formula and then the empirical formula's mass. However, the molecular formula equation is molecular formula= (empirical formula)n, where n is the mass of the molecular formula divided by the mass of the empirical formula. You would, therefore, need to know the mass belonging to the molecular formula, which you are not given.
Could 2 3-dimethylpentane have the molecular formula as C7H16?
Yes, 2,3-dimethylpentane has the empirical formula C7H16.
What is the empirical formula for magnesium oxide?
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.
What is the formula unit of molecular compounds?
The molecular formula is the formula of a discrete (single) molecule of the substance.The formula unit is generally defined in the same way as the empirical formula, which is the simplest whole number ratio of the elementsChemical formula includes both molecular and formula units.Examples:-Benzene a molecule consisting of a ring of 6 carbon atoms each with a hydrogen attached:-molecular formula C6H6formula unit CH (which is the result you would get if you analysed the compound and worked out the atomic ratio of carbon to hydrogen.NaCl is ionic so you cannot write a molecular formula you express the compound simply as the formula unit (empirical formula)- in its simplest case NaCl (never Na2Cl2 or some such)How can you tell whether a formula is molecular formula or a formula unit. Well if the formula could be "simplified" like benzene C6H6 could be simplified to CH then you know its a molecular formula. Something like SO2 and TiO2, well you need to be told. (SO2 is molecular, TiO2 is ionic)
What is the molecular formula of a compound with an empirical formula of CH?
CH could represent the moleculaes H-C///C-H (Ethyne/Acetylene) Or Benzene , which is C6H6
Would ionic or covalent molecules use the molecular formula or empirical formula?
What you write for an ionic compound is called the formula unit, but the formula unit is almost always the same as the empirical formula. The answer to your question could not be the molecular formula because an ionic compound is not a molecule.
How are molecular and empirical formulas related?
An empirical formula may or may not be the same as a molecular formula. The empirical formula of a compound shows the smallest whole-number ratio of the atoms compound. The molecular formula tells the actual number of each kind of atom present in a molecule of the compound.
How do you calculate Molecular formula from empirical formulaWhat could you do with that information to determine that the empirical and molecular formulas are related to one another by a factor of 6?
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.
Which could be an empirical formula aN2O4 bN2H6 cN2O5?
N2O5
What could be a molecular formula for the empirical formula C2H2?
Anything really. C4H4, C8H8, C100H100....
Explain why the percent composition of certain compounds are not sufficient to determine the compounds molecular formulas?
Because unlike the empirical formula, the molecular formula does not have to be the simplest ratio.If by chance you are given the percent composition of the elements in a substance, you could calculate the empirical formula and then the empirical formula's mass. However, the molecular formula equation is molecular formula= (empirical formula)n, where n is the mass of the molecular formula divided by the mass of the empirical formula. You would, therefore, need to know the mass belonging to the molecular formula, which you are not given.
Is KOH a molecular or ionic?
"KO" does not exist as the formula for any chemical compound that is stable at standard temperature and pressure. It could be the empirical formula for potassium peroxide, for which the actual formula is K2O2. More likely, however, the questioner intended it to represent potassium oxide, for which the proper formula is K2O. Potassium oxide is ionic.
Could 2 3-dimethylpentane have the molecular formula as C7H16?
Yes, 2,3-dimethylpentane has the empirical formula C7H16.
Is ch3o a compound?
CH3O is not the formula of any compound but could be a formula for a hydroxymethyl radical.
How do you determine the molecular formula of a compound from its empirical formula?
If you are given the empirical formula and are asked for the actual formula, then the molecular mass of the compound will be given too. Take this example problem: Empirical Formula: CH2O Molecular Mass: 180.0 First you have to find the empirical mass. Just find the atomic masses of all the elements in the empirical formula and add them together. If there are multiple atoms of the same element, then you have to add the element's atomic mass for every multiple. In the example, you have to add hydrogen twice because there are two hydrogen atoms in the empirical formula. C- 12.0 H- 1.00 H- 1.00 O- 16.0 + _________ 30.0 The empirical formula is some multiple of the actual formula. The empirical formula shows the ratio of atoms as 1:2:1. This means that the actual formula could be 2:4:2 or 3:6:3 or 4:8:4 etc. In order to find what multiple it is, divide the molecular mass by the empirical mass. An easier way to think of it is: x(empirical mass) = molecular mass Use this formula to find x: x(30.0) = 180.0 x = 6 In this example, x turned out to be exactly 6, but in some cases (especially in lab results) the answer will be close to a whole number but not exact. There is usually a standard +/- .02 for your result. If the x value was 6.02 or 5.98, we would just round up or down as long as it is within .02 Take the x value and multiply it with the number of atoms in the original empirical formula. C1H2O1 * 6 = C6H12C6 The final result is the actual molecular formula.
How do you find the molecular and empirical formulas?
There is no easy answer to this question. First, it depends what information you have to start with. Do you have the name? Do you know what elements are found in the substance?If you are given the name of the molecule, you can often find the molecular structure of that compound by simply using the Google search engine online and searching for the name. It is often give you the answer! There are certain compounds that you should be familiar with also. Also, there is a set of official rules that determine the name of a specific compound, so that if you have the formula, you can name it correctly, and if you have the name, you can determine the formula. Unfortunately, many chemicals also have common names that do not follow these rules, and you just have to memorize those, or look them up with Google.See the Related Questions and Web Links to the left for some information about how compounds are named and how to go from a formula to a name and vice versa.
