Chemistry Curriculum Presentation

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Chemistry Curriculum Study

International Chemistry Education

Faculty Mathematics and Natural Science

State University of Surabaya

2012


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Standard Competence Basic Competences

Understanding the

periodic system

Writing the simple electron

configuration

Explaining periodic system

arrangement based on electron

configuration


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After learning this chapter, you are expected to be able to :

1. Explain the development of periodic table2. Explain basic particle of elements (proton, neutron, electron)3. Explain the basic of element grouping in the periodic table4. Determine the electron configuration and valence electron


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Periodic System

The development of

Periodic System

Element Grouping

Electron Configuratio

Basic Particle of Elements


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History of Periodic

Table Development

Johann Wolfgang

Dobereiner

(Triads)

John A. R. Newlands

(Law of Octaves)

Dmitry Mendeleyev andJulius Lothar Meyer

(Periodic Law)

Short-Form Periodic

Table

Henry G.J Moseley

(Modern Periodic

Table)


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The examples of triads are:

Chlorine, bromine and iodine.

Calcium, strontium, and barium.

Iron, cobalt, and manganese

Mass of Strontium =(Mass of Calcium + Mass of Barium) : 2


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John A. R. Newlands (Law of Octaves)

He listed the elements in the order based on the increase

of atomic weights and he noted that a given properties of

the elements in the list, recurs at every eighth element

called law of octaves.

1H 2Li 3Be 4B 5C 6N 7O

8F 9Na 10Mg 11Al 12Si 13P 14S

15Cl 16K 17Ca 18Ti 19Cr 20Mn 21Fe

22

Co&Ni 23

Cu24

Zn25

Y26

In27

As28

Se


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Mendeleyevs Periodic Table

They proposed a chemical law that the properties of all the

elements are periodic functions of their atomic mass called

periodic law.

Mendeleyev and Meyer grouped about 66 elements based on the

increase of their atomic mass.


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Short-Form Periodic Table

In 1930 the scientists developed the new periodic

table which is the development of Mendeleyevs

periodic table called short-form periodic table.


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Long-Form Periodic Table (ModernPeriodic Table)

Henry G. J. Moseley found that the propeties of elements are

periodic function of their atomic number.

In modern periodic table:

Period is the placement row of the elements is in the horizontal

lines.

Group is the placement of the elements is in the vertical

columns.


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Modern Periodic Table
http://www-tech.mit.edu/cgi-bin/imagemap/Projects/Chemicool/pertable.map


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XA

ZAtoms

name

Atomic

number

Atomic

mass


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ZNumber of

protons = numberof electrons

A

Number of proton+ number of

neutrons

A-Z

Number ofneutrons


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Sample Problem !

Determine the number of protons, electrons,

and neutrons for :

O168 F199


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For Oxygen,

A = 16

Z = 8

A-Z = 8

Thus, number of :

Protons = 8Electrons = 8

Neutrons = 8

For Fluor,

A = 19

Z = 9

A-Z = 10

Thus, number of :

Protons = 9Electrons = 9

Neutrons = 10


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A. PeriodIn modern periodic table, elements are grouped into 7 periods that consist of :

Period 1, consist of 2 elements

Shortest Period

Period 2 and 3, each consist of 8 elements

Short Period

Period 4 and 5, each consist of 18 elements

Long Period

Period 6, consist of 32 elements

Longest Period

Period 7

Uncomplete Period


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B. GROUPElements which take placed in one group are the elements having the similar propertied

of one another. The group of element in periodical table is distinguish into principal group

(A) and transition group (B)

Group

Principal

Transition

Alkali Metals (IA)

Alkaline Earth

Metals (IIA)

Halogen (VIIA)

Noble Gases

(VIIIA)

I B VIII B (Principal

transition metals)


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Atom is consist of protons, neutrons, and electrons.

The nucleus of atom consist of protons and neutrons, while the electrons

revolving the nucleus on a certain path.

The path of the electrons in atom is often called shell of atom.


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HELIUM ATOM

+N

N+

--

proton

electron neutron

Shell

What do these particles consist of?

He42


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The maximum number of electrons on each atom shell

Shell n Maximum

electrons (2n2)

K 1 2

L 2 8

M 3 18

N 4 32

O 5 50

.... .... ....


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Electron

Configuration

Electron configuration is a method to depict

the electron spreading in a atom.

Electron spreading on the shells of atom

done by filling of each shell from K, L, M,N,O and so forth.


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The shell of atoms


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Example: Electron configuration for principal group in onegroup (group VII A)

ElementAtomicNumber

Electron Configuration

K L M N O

F 9 2 7 - - -

Cl 17 2 8 7 - -

Br 35 2 8 8 7 -

I 53 2 8 18 18 7


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The number of valence electrons in an atom is

determine properties of the atom, especially for its

chemical properties.

The number of valence electrons of a given elementatom represent the number element group, especially

for the principal group elements.

The number of an element atom shell express the

element period number.


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Electrons of the first elements atom will occupy one shell only, that is K

shell (n =1). For example :

Helium which having atomic number of 2, then two electron of helium will

occupy K shell only.

2He = 2Means that He is in first period

and IIA group.


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In the second period elements, their electrons will occupy 2 shells, those are

K (n = 1) and L (n = 2). For example: Fluorin having the atomic number of 9.

9F = 2, 7Means that F is in second

period and VIIA group.


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In the third period elements, their electrons will occupy 3 shells, those are K

(n = 1), L (n = 2), and M(n =3). For example:

Sulfur having the atomic number of 16.

16S = 2, 8, 6

Means that S is in thirdperiod and VIA group.


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In the fourth period elements, their electrons will occupy 4 shells, those are

K (n = 1), L (n = 2), M(n = 3) and N(n = 4). For example:

As having the atomic number of 33.

33As = 2, 8, 18, 5Means that As is in fourth period and

IVA group.


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Sample Problem

Determine the electron configuration, period,

and group of :

a.17

Cl

b. 20 Ca

c. 35 Br

YOU HAVE 1 MINUTES TO DO THIS PROBLEM


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Chemistry Curriculum Presentation

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