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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.
How are the empirical and molecule formulas for a compound related?
The empirical formula of a compound represents the simplest whole-number ratio of the elements present, while the molecular formula indicates the actual number of atoms of each element in a molecule of the compound. The molecular formula can be a multiple of the empirical formula, meaning that it may contain the same elements in a proportion that is a whole number multiple of the empirical ratio. For example, if the empirical formula is CH₂, the molecular formula could be C₂H₄, C₃H₆, etc., depending on the actual number of atoms in the molecule.
Could 2 3-dimethylpentane have the molecular formula as C7H16?
Yes, 2,3-dimethylpentane has the empirical formula C7H16.
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.
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 molecular formula of a compound with an empirical formula of CH?
The molecular formula of a compound with an empirical formula of CH is likely to be CH, as there is only one carbon atom and one hydrogen atom in the empirical formula. In this case, the empirical formula is also the molecular formula.
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 the empirical and molecule formulas for a compound related?
The empirical formula of a compound represents the simplest whole-number ratio of the elements present, while the molecular formula indicates the actual number of atoms of each element in a molecule of the compound. The molecular formula can be a multiple of the empirical formula, meaning that it may contain the same elements in a proportion that is a whole number multiple of the empirical ratio. For example, if the empirical formula is CH₂, the molecular formula could be C₂H₄, C₃H₆, etc., depending on the actual number of atoms in the 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.
What could be a molecular formula for the empirical formula C2H2?
The molecular formula for the empirical formula C2H2 is also C2H2. The empirical formula gives the simplest whole number ratio of atoms present in a compound, whereas the molecular formula provides the actual number of atoms of each element in a molecule.
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.
In the compound X2O the X could be what?
The X in compound X2O could represent elements such as calcium, strontium, or barium as they form oxides in the formula X2O.
Which could be an empirical formula aN2O4 bN2H6 cN2O5?
N2O5
Could the empirical formula determined from chemical analysis be used to tell the difference between propane C3H8 and butene C4H8?
No, because both propane (C3H8) and butene (C4H8) have the same empirical formula (CH4), which is the simplest ratio of the elements present in the compound. To differentiate between propane and butene, one would need additional information such as molecular formula or structural information.
Could 2 3-dimethylpentane have the molecular formula as C7H16?
Yes, 2,3-dimethylpentane has the empirical formula C7H16.
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.
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.
