# Mole definition chemistry quizlet

## isotope definition chemistry quizlet

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## High School

### Intrinsic and Extrinsic Properties

Properties of Matter &#; Part 2

One way to classify matter by properties is to use physical or chemical properties. But there is another way to look at properties: Does the property depend on how much matter you have? The answer determines whether you are working with an intrinsic or extrinsic property.

Intrinsic (AKA intensive) properties are properties that are within the substance. These properties do not depend on the amount of material that you have. For example, paper burns whether you have an entire sheet or whether you cut it in half. (Hint: focus on the prefix &#;in&#; to help you remember that it is within the substance)

Extrinsic (AKA extensive) properties are properties that depend on the amount&#;of the substance you have. All size measurements depend on amount, so all size measurements are extrinsic properties. For example, the length of a piece of wire depends on how much wire you have.

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## The mole - Higher

It is often useful in chemistry to know the number of atoms, ions or molecules involved in a chemical reaction. The mole is the unit for amount of substance. It is abbreviated to mol.

1 mol is the amount of substance that contains the same number of particles as there are atoms in g of carbon

Since atoms are so very small and have very little mass, the number of atoms in g of carbon is huge. It is equal to the Avogadro constant:

The Avogadro constant = × 1023 atoms per mole.

### Calculating the number of particles

The number of particles of a substance can be calculated using:

• the amount of substance in mole

number of particles = Avogadro constant × amount (mol)

Example

Calculate the number of water molecules in mol of water.

Number of water molecules = × 1023 ×

= × 1023

It is important to be clear about the particles involved. For example, × 1023 water molecules contain × 1023 atoms. This is because a water molecule, H2O, contains three atoms.

Question

Calculate the number of oxygen atoms in mol of oxygen molecules, O2.

Number of atoms = 2 × × × 1023

= × 1023

### Masses of atoms

The Avogadro constant can be used to calculate the mass of an atom in grams:

$mass\ of\ atom\ (g)\ =\ \frac{A_{r}\ of\ element}{Avogadro\ constant}$

Example

Calculate the mass of a magnesium atom.

(Relative atomic mass, Ar = )

$mass\ of\ Mg\ atom\ =\ \frac{}{ × 10^{23}}$

= × 10 g

It is important to give the final answer to the lowest number of significant figures used in the calculation. In this example, this is the same number of significant figures as the Ar value.

Question

Calculate the mass of a carbon atom. (Relative atomic mass, Ar = )

$mass\ of\ C\ atom\ =\ \frac{}{ × 10^{23}}$

= × 10 g

### Masses of molecules

The Avogadro constant can be used to calculate the mass of a molecule in grams:

$mass~of~molecule~(g) = \frac{M_{r}~of~substance}{Avogadro~constant}$

Example

Calculate the mass of a bromine molecule. (Relative formula mass, Mr = )

$mass\ of\ bromine\ molecule\ (g)\ = \frac{}{ × 10^{23}}$

= × 10 g

This answer is given to 4 significant figures because both numbers used in the calculation are given to 4 significant figures.

Question

Calculate the mass of a water molecule. (Relative formula mass, Mr = )

$mass\ of\ water\ molecule\ (g)\ = \frac{}{ × 10^{23}}$

= × 10g

One mole of any object contains the Avogadro number of that object, × 1023.

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What is a Mole? - #Extraclass #MoleConcept #Chemistry #Animation

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