it is a group of elements and lots of explanation to understand. There are lots of definition to know about ionic bond and this PT is originally own by: Mister Flynn

1. CHAPTER 6: TIES THAT BIND

3. Learning objectives:
Identify the parts of an atom.
Identify the 3 types of atomic bonds.
Recognize the different group of elements in the periodic table
and its physical characteristics.
Determine the number of valence electrons in an atom based on
its position in the periodic table.
Draw electron dot structures of the representative elements.

4. ATOM

5.  ATOMS – COMBINE THROUGH
1.TRANSFER OF ELECTRONS – IONIC BOND
2.OVERLAP OF ORBITALS – METALLIC BOND
3.SHARING OF ELECTRONS – COVALENT BOND

9. GROUP OF ELEMENTS:
1. Non-Metals - is a chemical element that mostly lacks metallic attributes. Physically, nonmetals
tend to be highly volatile (easily vaporized), have low elasticity, and are good insulators of heat and
electricity; chemically, they tend to have high ionization energy and electronegativity values, and
gain or share electrons when they react with other elements or compounds.
2. Alkali Metals - are all shiny, soft, highly reactive metals at standard temperature and pressure.
They can all be cut easily with a knife due to their softness, exposing a shiny surface that tarnishes
rapidly in air due to oxidation by atmospheric moisture and oxygen.
3. Alkaline Earth Metals - The elements have very similar properties: they are all shiny, silvery-
white, somewhat reactive metals at standard temperature and pressure.

10. 4. Transition Metals (Early & Late)
They are good conductors of heat and electricity.
They can be hammered or bent into shape easily.
They have high melting points. (but mercury is a liquid at room temperature)
They are usually hard and tough.
They have high densities.
5. Basic/Poor Metals - Generally with higher electronegativity, lower melting and boiling points
and greater softness than the transition metals.

11. 6. Metalloids/ Semi-Metals - A metalloid is any chemical element which has properties in
between those of metals and nonmetals, or that has a mixture of them.
7. Halogens - They are reactive nonmetallic elements that form strongly acidic compounds with
hydrogen, from which simple salts can be made.
8. Noble Gases - are odorless, colorless, nonflammable, and monotonic gases that have low
chemical reactivity.
9. Lanthanides - are often collectively known as the rare earth elements.
They are soft metals and also have a lustrous nature. They have higher binding energy than other
elements. When added to acids, they dissolve quickly and produce a lot of energy when they
react with hydrogen.
10. Actinides - They are all radioactive, the heavier members being extremely unstable and not of
natural occurrence.

12.  LESSON 6.1: VALENCE ELECTRONS
 ELECTRONS IN THE OUTERMOST ENERGY LEVEL OF AN
ATOM ARE KNOWN AS VALENCE ELECTRONS.
 THESE ELECTRONS DETERMINE THE KIND OF CHEMICAL
BONDS (IF ANY) THAT THE ATOM CAN FORM.
 VALENCE COMES FROM THE LATIN WORD VALENTIA, WHICH
MEANS “CAPACITY”.
 FOR ATOMS, VALENCE REFERS TO THE CAPACITY OF
ATOMS TO FORM BONDS.

13.  ELECTRON CONFIGURATION CAN HELP DETERMINE THE
NUMBER OF VALENCE ELECTRONS OF AN ELEMENT. FOR
EXAMPLE, THE ELECTRONIC CONFIGURATION OF
HYDROGEN IS 1s1. THUS, IT HAS ONLY ONE VALENCE
ELECTRON BECAUSE ITS EXPONENT WHICH IS 1,
REPRESENTS THE NUMBER OF ELECTRONS IN THE
SUBSHELL.

14. 1s¹

15. Valence electrons of elements in the 1st three periods
Element Group no. Electron
configuration
No. of valence
electrons
H 1 1s1 1
He 2 1s2 2
Li 1 [He]2s1 1
Be 2 [He]2s2 2
B 3 [He]2s2 2p1 3
C 4 [He]2s2 2p2 4
N 5 [He]2s2 2p3 5
O 6 [He]2s2 2p4 6
F 7 [He]2s2 2p5 7

16. Element Group no. Electron configuration No. of valence
electrons
Ne 8 [He]2s2 2sp6 8
Na 1 [Ne]3s1 1
Mg 2 [Ne]3s2 2
Al 3 [Ne]3s2 3p1 3
Si 4 [Ne]3s2 3p2 4
P 5 [Ne]3s2 3p3 5
S 6 [Ne]3s2 3p4 6
Cl 7 [Ne]3s2 3p5 7
Ar 8 [Ne]3s2 3p6 8
K 1 [Ar]4s1 1
Ca 2 [Ar]4s2 2
Sc 3 [Ar]4s2 3d1 3

17. Lesson 6.2
Lewis Electron-Dot Structures of Representative Elements
> Dots are often used to represent the valence electrons in atoms
and molecules.
The resulting structures are referred to as Lewis structures,
electron-dot structures, Lewis electron-dot structures.
These structures were named after Gilbert Newton Lewis (1857-
1946) who pioneered the explanation on the relationship between
electron structure and chemical bonding.

18. > Thus, Lewis structures are being used to monitor
the valence electrons and assure that the number of
electrons does not change before and after a
chemical bond has been formed.

19. LEWIS ELECTRON-DOT STRUCTURE OF SOME REPRESENTATIVE ELEMENTS
1A(1) 2A(2) 3A(13) 4A(14) 5A(15) 6A(16) 7A(17) 8A(18)
H . He:
Li .
.
Be .
.
.B.
.
.C.
.
..
.N.
.
..
.O.
..
..
:F.
..
..
:Ne:
..
Na .
.
Mg.
.
.Al.
.
.Si.
.
..
.P.
.
..
.S.
..
..
:Cl.
..
..
:Ar:
..

21. 6.4 IONIC BOND
You have learned that noble gases have stable electron configurations and that atoms gain or
lose electrons to achieve such configurations. All atoms, in general, are neutral; that is, they have
an equal number of protons and electrons.
An ion is formed whenever a neutral atom gains or loses an electron.
Cation is a positive ion, while a negative ion is Anion.
For example, sodium atoms have a tendency to lose one electron to form sodium ion, thereby
achieving a neon core. A neutral sodium atom has (Na) has 11 protons (p) and 11 electrons (e-).
Its electron configuration is 1s22s22p63s1. Neon (Ne) has an electron configuration of
1s22s22p6. Therefore, another way of writing the electron configuration of Na is [Ne]3s1.
Since Na has only one electron in its outermost shell, it will lose this outermost electron to a
nonmetal to form a cation with an electron configuration the same as that of Ne.

22. Na . Na+ + e-
(11p, 11e-) (11p, 10e-)
[Ne]3s1 [Ne]
METALLIC GROUP

23. .
Mg . Mg2+ + 2e-
(12p, 12e-) (12p, 10e-)
[Ne]3s2 [Ne]

24. .
.Al. Al3+ + 3e-
(13p, 13e-) (13p,10e-)
[Ne]3s23p1 [Ne]

25. .. ..
:F. + e- :F:-
.. ..
(9p, 9e-) (9p, 10e-)
[He] 2s2 2p5 [Ne]
NON METALLIC

26. .. ..
.P. + 3e- : P: 3-
. ..
(15p, 15e-) (15p, 18e-)
[Ne] 3s2 3p3 [Ar]

27. Atoms may combine in ratios other than 1:1. For example, one atom of
magnesium & two atoms of chlorine can combine to form the ionic compound
magnesium chloride, MgCl2+ Magnesium loses two electrons form a +2 cation, but
chlorine can add only one electron to form a -1 anion. Two chlorine atoms are
needed to accept the two electrons lost by one atom of magnesium.
Mg + 2Cl MgCl2
Magnesium Chloride
..
. Cl:
. .. ..
Mg. Mg²+ 2(:Cl:-)
.. ..
. Cl:
..
METAL & NON
METAL

28. 2Al + 3O Al2O3 (Aluminum Oxide)
.
. .O:
Al. ..
. . ..
. .O: 2(Al³+)3(:O:²-)
Al. .. ..
. .
.O:
..

29. END OF THE CHAPTER
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