1. Chemical Bonds
by Mehmet Okuyucu

2. Intramolecular Intermolecular Ionic bond Covalent Bond CHEMICAL BONDS
Hydrogen
Ionic bond
Dipole-Dipole
Covalent
Bond
Van Der Waals
Polar
Crystal structure
What ıs a chemıcal bond and how are they formed?
Nonpolar
Metallic Bond
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3. Bonds between atoms are caused by electrons in outermost shells
What causes atoms to form bonds? Why atoms make dıfferent compounds or bonds?
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4. Why do almost all atoms want to form a chemical bond under conditions???
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5. HAPPY ATOMS
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6. Each atom ends up with 8 electrons in its outer most shell that is called octet rule
Atoms that complete their octet will be happy or satisfied
Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons
C would like to
N would like to
O would like to
Gain 4 electrons
Gain 3 electrons
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Gain 2 electrons

7. ELECTRONEGATIVITY
Electronegativity is the tendency of an atom to attract the bonding electrons within a compound to itself.
Depends upon the nuclear charge (proton
number) and the atomic radius of the atom.
how and why it varies around the Periodic Table? electronegativity differences affect the bond type of atoms
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8. As you follow arrow above you will see that electrogeativity of elements usually increases due to increasing nuclear charge of atoms
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9. electron shells
Electrons vary in the amount of energy they possess, and they occur at certain energy levels or electron shells.
Electron shells determine how an atom behaves when it encounters other atoms
Note that valence electrons are very ımportant ın determınıng how atoms bonds wıth other atoms!!!
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10. Electrons are placed in shells according to rules:
The 1st shell can hold up to two electrons, and each shell thereafter can hold up to 8 electrons.
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11. Why are electrons important?
Elements have different electron configurations
different electron configurations mean different levels of bonding
What particles play the most active role in chemical bonding?
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12. by Mehmet Okuyucu

13. Representation of Chemical bonds
Chemical bonds can be represented in many ways.
Orbital representation
Lewis symbols(Dot representatıon)
Line representation
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14. The electron configuration of fluorine is 1s22s22p5
1-Orbital Representation of Chemical Bonds:
F2 molecule
The electron configuration of fluorine is 1s22s22p5
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15. 2-Electron Dot Representation (Lewis Symbol) of Chemical Bonds:
Symbols of atoms with dots to represent the valence-shell electrons
1A A 3A A A A A A
H He:
          
Li Be  B   C   N   O  : F  :Ne :
       
          
Na Mg  Al  Si  P S :Cl  :Ar :
       
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16. by Mehmet Okuyucu

17. 3- Line Representation of Chemical Bonds:
Two electrons (:) are shown by a line (–).
The line representation of fluorine molecule is;
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18. INTRAMOLECULAR FORCES
intermolecular
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19. IONIC BOND bond formed between two ions by the transfer of electrons
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20. Formation of Ions from Metals
Ionic compounds result when metals react with nonmetals
Metals lose electrons to match the number of valence electrons of their nearest noble gas
Positive ions form when the number of electrons are less than the number of protons
Group 1 metals  ion 1+
Group 2 metals  ion 2+
Group 13 metals  ion 3+
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21. Formation of Sodium Ion
Sodium atom Sodium ion
Na  – e  Na +
( = Ne)
11 p p+
11 e e-
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22. Ions from Nonmetal Ions
In ionic compounds, nonmetals in 15, 16, and 17 gain electrons from metals
Nonmetal add electrons to achieve the octet arrangement
Nonmetal ionic charge:
3-, 2-, or 1-
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23. Fluoride Ion     1 - : F  + e : F :     2-7 2-8 (= Ne)
unpaired electron octet
   
: F  e : F :
   
(= Ne)
9 p p+
9 e e-
ionic charge
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24. Ionic Bond
Between atoms of metals and nonmetals with very different electronegativity
Bond formed by transfer of electrons
Produce charged ions all states. Conductors and have high melting point.
Examples; NaCl, CaCl2, K2O
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25. by Mehmet Okuyucu

26. Ionic Bonds: One Big Greedy Thief Dog!
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27. 1). Ionic bond – electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.
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28. by Mehmet Okuyucu

29. COVALENT BOND bond formed by the sharing of electrons
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30. Covalent Bond
Between nonmetallic elements of similar electronegativity.
Formed by sharing electron pairs
Stable non-ionizing particles, they are not conductors at any state
Examples; O2, CO2, C2H6, H2O, SiC
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31. Covalent Bonds
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32. Bonds in all the polyatomic ions and diatomics are all covalent bonds
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33. when electrons are shared equally
NONPOLAR COVALENT BONDS
when electrons are shared equally
H2 or Cl2
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34. 2. Covalent bonds- Two atoms share one or more pairs of outer-shell electrons.
Oxygen Atom
Oxygen Atom
Oxygen Molecule (O2)
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35. when electrons are shared but shared unequally
POLAR COVALENT BONDS
when electrons are shared but shared unequally
H2O
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36. Polar Covalent Bonds: Unevenly matched, but willing to share.
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37. - water is a polar molecule because oxygen is more electronegative than hydrogen, and therefore electrons are pulled closer to oxygen.
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38. METALLIC BOND bond found in metals; holds metal atoms together very strongly
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39. Metallic Bond Formed between atoms of metallic elements
Electron cloud around atoms
Good conductors at all states, lustrous, very high melting points
Examples; Na, Fe, Al, Au, Co
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40. Metallic Bonds: Mellow dogs with plenty of bones to go around.
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41. Metallic Bond, A Sea of Electrons
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42. Metals Form Alloys Metals do not combine with metals. They form
Alloys which is a solution of a metal in a metal.
Examples are steel, brass, bronze and pewter.
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43. by Mehmet Okuyucu

44. Hope you got it!!!
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