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# Chemistry

Formulae and Isomerism

by

Tweet## Jamie Dawes

on 28 April 2010#### Transcript of Chemistry

Chemistry-Formulae and Isomerism

. What types of formulae are there in unit 1?

. The explanation of isomerism What will this include? Firstly, Formulae... Empirical formula, the simplest whole-numbered ratio of atoms of each element present

How to approach a queation... Analysis of a compound showed the following percentage composition by mass: Na: 74.19%, O: 25.81% [Ar: Na, 23.0 ; 0, 16.0] Find the molar ratio of atoms...

Step 1: Find the ratio, in this case, Na:O Step 2: Percentage of Element 74.19 25.81

---------------------, in this case ----- : ----- (3.226:1.613)

23.0 16.0

Atomic number

Step 3: Divide both sides of the ratio by the lowest amount, in this case 3.226 1.613

----- : ----- (2:1)

1.613 1.613 Step 4: Use the Ratio to form the chemical formula, in this case 2:1 Na2O Molecular Formula: The atual number of atoms of each element in a molecule A compound has the same Empirical formula of CH2 and a relative formula mass, Mr, of 56.0. What is the Molecular formula?

How to approach a queation... Step 1: Find the Empirical formula mass of the compound, by adding all the atomic numbers. In this case, 12.0 + (1.0 x 2) = 14.0 Relative Molecular Mass 56.0

Step 2: Find the number of units in a molecule: ----------------------- In this case ---- (4)

Empirical Formula Mass 14.0 Step 3: Use the number of units in a molecule to find formula mass. In this case (4 x CH2)=C4H8

Full transcript. What types of formulae are there in unit 1?

. The explanation of isomerism What will this include? Firstly, Formulae... Empirical formula, the simplest whole-numbered ratio of atoms of each element present

How to approach a queation... Analysis of a compound showed the following percentage composition by mass: Na: 74.19%, O: 25.81% [Ar: Na, 23.0 ; 0, 16.0] Find the molar ratio of atoms...

Step 1: Find the ratio, in this case, Na:O Step 2: Percentage of Element 74.19 25.81

---------------------, in this case ----- : ----- (3.226:1.613)

23.0 16.0

Atomic number

Step 3: Divide both sides of the ratio by the lowest amount, in this case 3.226 1.613

----- : ----- (2:1)

1.613 1.613 Step 4: Use the Ratio to form the chemical formula, in this case 2:1 Na2O Molecular Formula: The atual number of atoms of each element in a molecule A compound has the same Empirical formula of CH2 and a relative formula mass, Mr, of 56.0. What is the Molecular formula?

How to approach a queation... Step 1: Find the Empirical formula mass of the compound, by adding all the atomic numbers. In this case, 12.0 + (1.0 x 2) = 14.0 Relative Molecular Mass 56.0

Step 2: Find the number of units in a molecule: ----------------------- In this case ---- (4)

Empirical Formula Mass 14.0 Step 3: Use the number of units in a molecule to find formula mass. In this case (4 x CH2)=C4H8