chapter 4: periodic table - the great chemistrythegreatchemistry.yolasite.com/resources/lecture...
TRANSCRIPT
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CHAPTER 4:
PERIODIC TABLE
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LEARNING OUTCOMES
At the end of the lesson the students should be
able to :
(a) Indicate period, group and block (s, p, d, f).
(b) Specify the position of metals, metalloids and
non-metals in the periodic table.
(c) Deduce the position of elements in the
periodic table from its electronic
configuration.
LECTURE 1
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4.1 Period, Group and
Block(s,p,d,f)
The periodic table is a table that arranges
all the known elements in order of
increasing proton number.
A vertical column of elements is called a
group.
A horizontal row of elements is known as a
period.
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The groups in the Periodic Table are numbered from 1 to 18.
Elements in the same group have the same number of valence electrons.
Example: Sodium and potassium are both found in group 1 which means that they both have 1 valence electron
Group number = number of valence electron, if the
element is in block s and d
OR
Group number = number of v.e. + 10, if the element is in
block p
4.1.1 Groups
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Periodic Table
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Main group ( Representative Group ) in
periodic table
Group 1 : alkali metals
Group 2 : alkaline earth metals
Group 3-12: transition metals
Group 16 : chalcogens
Group 17 : halogens
Group 18 : inert / noble gases
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Alkali metal
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Alkaline earth metal
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Halogens
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Noble Gases
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The atoms of the elements in each period posses an identical number of quantum levels.
Are numbered 1 to 7.
Example: Sodium and chlorine are in row 3 or Period 3 because their principal quantum number of the valence electron shell is 3.
Na: 1s22s22p63s1
Cl: 1s22s22p63s23p5
4.1.1 Period
Period number = principle quantum number, n, of the
electrons in valence shell
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4.1.1 Blocks
All the elements in the periodic table can
be classified into 4 main blocks according
to their valence electron configuration.
These main blocks are block s, p, d and f.
}
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s Block :
Groups 1 and 2
Filling of valence electron only involve s
orbital
Configuration of valence electron : ns1 to
ns2
Example:
11Na: 1s2 2s2 2p6 3s1 3s1
20Ca: 1s2 2s2 2p6 3s2 3p6 4s2 4s2
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p Block :
Groups 13 to 18
Configuration of valence electrons:
ns2 np1 to ns2 np6.
Example:
13Al: 1s2 2s2 2p6 3s2 3p1
52Te: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p4
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d Block
Also known as a transition elements.
Groups 3 to 12.
Configuration of valence electron:
(n-1)d1 ns2 to (n-1)d10 ns2
Example:
23V : 1s2 2s2 2p6 3s2 3p6 3d3 4s2
= [ Ar ] 3d3 4s2 , where [ Ar ] = 18 electrons
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f Block
Involve elements in the series of
lanthanides (Ce to Lu) and actinides (Th to
Lr) in which the filling of valences electron
happens in the subshell of 4f and 5f
Lanthanides actinides
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Periodic Table
}
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4.1.2 Metal, nonmetal and
metalloids
All the elements on the left side and in the
middle of the periodic table (except for
hydrogen) are metallic elements, or
metals.
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The metals are separated from the non-metallic
elements by the diagonal step-like line that runs from
boron (B) to Astatine (At) as shown:
Further across the period towards the right, elements
gradually lose their metallic character and gained
nonmetallic features.
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Many of the elements that lie along the line that
separates metals from non-metals, such as
antimony (Sb) have properties that fall between
those of metals and non-metals.
These elements are often referred to as
metalloids.(semi-metals)
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4.1.3 Position of elements from its
electron configuration:
E.g:
Classify the following elements into its
appropriate group, period and block.
P : 1s2 2s2 2p6 3s2 3p6
Q: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
R : 1s2 2s2 2p6 3s2 3p6 4s2
S : 1s2 2s2 2p6 3s2 3p6 3d34s2
T : 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
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Answer
Element Group Period Class/block
P
Q
R
S
T
18
17
2
5
18
3
4
4
4
4
Inert gas/block p
Block p
Block s
Transition element/
block d
Inert gas/block p
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End of lecture 1…