mole and particles ppt f4

7/30/2019 Mole and Particles ppt f4

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At the beginning, all chemists agreed to use

atom hydrogen as a standard in determined

RAM and RMM with one atom hydrogen is given

as 1 units.

Then, chemists found that this standard is not

suitable because:

INTRODUCTION OF CARBON-12


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In 1860, chemists agreed to use atom oxygen

as a standard. This is because:

A problem occurred when there are two

standard of relative atomic mass.

Finally, in 1961 all scientists agreed to useisotope 126C as a standard. This is because:


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Hydrogen has isotopes, which is 11H,21H (deuterium)

and 31H (tritium). So, hydrogen is not 1 units.

Hydrogen existed as gases and its masses was very

difficult to determine. There are a lot of elements that is not react with

hydrogen.

WHY ATOM HYDROGEN IS NOT

SUITABLE AS A STANDARD:


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Atom oxygen can react with many elements.

Most of the compounds produced oxide is existed as

solid. The mass of this compound was easy to determine.

WHY ATOM OXYGEN USED AS A

STANDARD:


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Carbon existed is many kinds of materials and easy to

get.

Carbon occurred as a solid in room

temperature compare with oxygen gas. This element

doesnt need a stopper to keep it.

The existing of other isotope such as 126 C,13

6 C and14

6 C

are too little.

WHY CARBON-12 IS USED AS A

STANDARD FOR DETERMINING

RAM AND RMM


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RELATIVE ATOMIC MASS (RAM)

Definition

Then, relative atomic mass ofelement:

= mass of one element

1/12 x mass of one atom C-12

Example Try out


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RELATIVE ATOMIC MASS (RAM) of elements is

how much time one atom of element moreheavy than 1/12 mass of one atom C-12 with themass of one atom C-12 is 12.000.

DEFINITION OF RELATIVE

ATOMIC MASS (RAM)


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The mass of one atom potassium is 39 time more bigger

than 1/12 x mass of one atom C-12.

So, relative atomic mass for one atom potassium is 39.

K = 39

EXAMPLE:


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RELATIVE MOLECULAR MASS (RMM)

Definition

Relative molecular mass of

compound=

Mass of one molecule of compound

1/12 x mass of one atom C-12

Example Try out


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RELATIVE MOLECULAR MASS(RMM) is

how much time the mass of one molecule iscompound is more bigger than 1/12 mass of

one atom C-12 with the mass of one atom C-

12 is 12.000.

DEFINITION OF RELATIVE

MOLECULAR MASS (RMM)


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Relative molecular mass for water, H2O:

= 2 x (relative atomic mass H) + 1 x (relative atomicmass O)

= ( 2 x 1) + ( 1 x 16)=18

So, relative molecular mass for H2O is 18.

(RAM: H = 1; O = 16)

EXAMPLE:


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Relative molecular mass for HCl.

= 1 x (relative atomic mass H) + 1 x (relative atomic

mass Cl)

= (1 x 1) + (1 x 35.5)= 36.5

So, relative molecular mass for HCl is 36.5.

(RAM : H=1 ; Cl=35.5 )

EXAMPLE:


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C = ?

O = ?

N = ?F = ?

Br = ?

Na = ?

Al = ?

Fe = ?Ar = ?

Mn = ?

WHAT IS THE RELATIVE ATOMIC

MASS OF THESE ELEMENTS??


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C = 12O = 16

N = 14F = 19Br = 80Na = 23Al = 27Fe = 56Ar = 40Mn = 55


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Chlorine, Cl2

Nitrogen, N2 Ethanol, C2H205

Carbon dioxide, CO2

WHAT ARE THE RELATIVE

MOLECULAR MASSES OF THESE

MOLECULES??

(RAM: H=1; C=12; O=16;

Cl=35.5; N= 14)


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RELATIVE FORMULA MASS (RFM)

For IONIC SUBSTANCE

Example

Sodium chloride, NaCl= RAM of Na + RAM of Cl

= 23 + 35.5

= 58.5

Hydrated magnesium sulphate, MgSO4.7H2O

= RAM of Mg + RAM of S + 4(RAM of O) + 14(RAM

of H) + 7(RAM of O)

= 24 + 32 + 4(16) + 14(1) + 7(16)

= 246


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WHAT ARE THE RELATIVE

FORMULA MASSES OF THESE

ION??

Aluminium sulphate, Al2(SO4)3

Zinc chloride, ZnCl2

Sodium Oxide, Na2O Magnesium sulphate, MgSO4

(RAM: Al=27; Na=23; O=16;

Cl=35.5; Mg= 24; S=32; Zn=65)


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Mole Concept Avogadro Number, NA


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a) 1 dozen = 12 units b) 1 pair = 2 units

Daily life we used:

To delegate a big quantity:

Definition

Chemistry- mole concept:

Mole is a substance quantity that contain a number of particles

such as atom, ion, or molecule that have equal number of atom in

12 gram of 12C or 6.02 x 1023particles


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Example:

1 mole carbon atoms = 6.02 x 1023 carbon atoms

1 year = 12 months

1 kg = 1000 g

1 month = 30 days

1 km = 1000 m

1 dozen oxygen atoms = 12 oxygen atoms

1 mole oxygen atoms = 6.02 x 1023 oxygen atoms

1 mole sodium atoms = 6.02 x 1023

sodium atoms

Daily life

Chemistry
http://www.edhelper.com/logic_puzzles.htmhttp://www.edhelper.com/middle_school_math.htm


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Avogadros Number/ Avogadro's Constant,NA

1 Mole of Substance = 6.02 x 1023 Particles

NA=6.02 x 1023 mol-1


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Analogy:

Large Constant

1 mole = 6.02 x 1023 representative particles of a substance

Substance

NA = 6.02 x 1023 mole-1 Particles


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Amedeo

Avogadro

Avogadro's number has been experimentally determined to be 6.02 x 1023

molecules gram mole-1

Avogadro's number, NA= 6.02 x 1023 particles theorized by Amadeo Avogadro

later mathematically proven by Sanislao Canizzaro around the 1750's.

NA


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Example 1:

Sodium, Na NaOH Water, H2O

RAM/ RMM

(g/mole)

Mole

Particles

23.0 23+16+1

= 40(2x1) + 16 = 18

11 1

6.02x1023mole-1molecule6.02 x 1023

mole-1molecules

6.02 x 1023

mole-1 atoms


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Helium (He) Hydrogen (H)

1(4 g/mole) = 4 g/mole

1 mole 6.02 x 1023 particles

4 (1 g/mole) = 4 g/mole

4 mole 4 (6.02 x 1023 particles)

Example 2:


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Mole is a quantity that contain a number of particles such as

atom, ion, or molecule that have equal number of atom in 12

gram of12C or 6.02 x 1023particles.

Question

1. Define the definition of

Mole concept:

Avogadro Number:

NA

= The number of particles in one mole of substances, 6.02 x 10


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2. If 1 mole of a substance contains 6.02 x 1023particles, then,

1 mole of Na contains

6.02 x 1023water molecules

6.02 x 1023sodium ions

6.02 x 1023sodium atoms

1 mole of Na+ contains

1 mole of H2O contains


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3. Calculate number of mole and a atomic number of each

substance given below and fill in the table with the correct

answers.

Substance Number of Mole Atomic Number

Iron 1.0 6.02 X1023

Potassium 2.0

Carbon 0.5 X 6.02 x 1023

Helium

Aluminium0.2

2.0 X 6.02 x1023

0.5

1.5 1.5 X 6.02 x 1023

0.2 X 6.02 x 1023


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Mole15 6.02 x 10233.01 x 1024

NA

X NA

4.816 x 10249

RELATIONSHIP BETWEEN THE NUMBER OF

MOLES AND THE NUMBER OF PARTICLES


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Particles MOLECULE

ION

ATOM

Number ofmoleatom

Number ofmole molecule

Number ofmoleion

C

C


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ExampleCount number of atom in 0.4 mole atomcarbon.

C

Solution:

0.4 mole ? Atom carbon

Number of moleatom carbon

= 0.4 mole

Get the information

from question

So, number ofatomcarbon is,

= 0.4 x Avogadro constant

= 0.4 x 6.02 x 1023atom

use the

relationship infigure 1

= 2.48 x 1023atoms


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Number ofmole

moleculeNumber ofmolecule Number ofatom

x NA x depending on formulas chemistry

depending on formulas chemistry NA

H

Relationship for

2mole molecule H2

2 x NA

MoleculeH2 = Atom H =

2 x NA x 2

Example


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There are 3 molegases hydrogen, H2 in one container,

a) Number ofmoleculehydrogen, H2

b) Number ofatomhydrogen

Example

Get the informationfrom the question

3mole moleculeof hydrogen, H2 ? Moleculehydrogen, H2

a) So, number ofmoleculehydrogen, H2 ;

= 3 x Avogadro Constant

= 3 x 6.02 x 1023molecule

= ___________ molecule

Use therelationship in

figure 2

Solution :

Number ofmole molecule hydrogen, H2 = 3 molemolecule hydrogen, H2

Count;

Th 3 l i i


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b) Every molecule hydrogen, H2 consist of2 atom hydrogen.

So, number ofatom hydrogen in the gas container;

3 x 6.02 x 10 moleculehydrogen, H2 ? Atom hydrogen

Use the

relationship in

figure 2

= 2 x number ofmolecule hydrogen, H= 2 x 3 x 6.02 x 1023atom

= ______________ atom

Analysis

formulae

molecule H2

There are 3 molegases in one container,

b) Number ofatom hydrogen

H H


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Molecule of water H2O

HO

Sample of water consist of 1.806 x 1024 molecules, count;

a) Number ofmole water molecule

b) Number ofatom oxygen

c) Number ofatom hydrogen in the sample.

EXAMPLE

H


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Solution;

1.806 x 1024 moleculewater ?Molecule water

So, number ofmole molecule water;

= 1.806 x 1024 NA

= 1.806 x 1024

= 3 mole molecule of water

a) Number ofmolecule water = 1.806 x 1024

Get the information from

question

6.02 x 1023


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1.806 x 1024molecule water ?Moleculewater

b) 1 molecule water consist 1 atom oxygen

So, 1.806 x 1024molecule of water consist of 1.806

x1024atomof oxygen

OH H


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c) Every molecule water, H2O consist of2 atom

hydrogen. So, number ofatom hydrogen in the sample;

= 2 x number ofmolecule hydrogen, H

= 2 x 3 x 6.02 x 1023atom

= 3.612 x 1024

atom

O

HH


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Number of mole

ion Number of unit Number of ion

x NA

x depending on formulas chemistry

depending on formulas chemistry NA

Relationship for


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Example

Count number ofunits in 4 mole NaCl.

Solution;

1 mole substance 6.02 x 1023units

So;

4 mole NaCl = ? units

4 mole NaCl = 4 x 6.02x 1023

= 2.408 x 1024unitsNaCl


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Count number ofionsofCl- in 4 mole NaCl.

One units of NaCl have 1 ion Cl-

So;

One mole unit of NaCl ? ion Cl-

1 mole units of NaCl = 6.02 x 1023ions

4 mole units of NaCl = 4 x 6.02 x 1023 ions

= 2.408 x 1024 ions


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