chemical bonding
TRANSCRIPT
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Chemical Bonding
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CHEMICAL BONDS
• A chemical bond is the force that holds atoms together.
• There are 3 types of bonds:
• Ionic bond
• Covalent bond
• Metallic bond
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Chemical bond
• Chemical bonds can form :
• A) By the attraction between opposite charged ions
• B) By the sharing of electrons between atoms
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Positive Ion Formation
• A positive ion forms when an atom loses one or more valence electrons in order to attain a noble gas configuration (octet rule).
• A positively charged ion is called a cation
• Ex.
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Metal Ions
• Metals atoms are reactive because they lose valence electrons easily, have Low ionization energy and low electron affinity
• The group 1 and 2 metals are the most reactive metals in the P.T.
• Metals in group 1 form +1 ions• Metals in group 2 form +2 ions• Metals in group 13 form +3 ions• Transition metals: is difficult to predict
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Negative Ion Formation
• Nonmetals, located on the right side of the P.T., easily gain electrons to attain a stable outer configuration(octet rule) and form an anion.
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Nonmetal Ions
• Elements in group 15 gain 3 electrons and form -3 ions
• Elements in group 16 gain 2 electrons and form -2 ions
• Elements in group 17 gain 1 electron and form -1 ions
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Lewis dot diagrams for Ions
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Practice
• Write the symbol of the ion and the dot structure of the following :
• a)calcium ion
• b) germanium ion
• c) phosphide
• d) oxide
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The Ionic Bond
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Na
e.c. 2,8,1
(Na +)
Ion
Atom
e.c. (2,8)+
The Sodium loses 1 electron to leave a complete outer shell.
It is now a Sodium ion with a charge of 1 +
The Sodium atom has 1 Electron in it’s outer shell.
+
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Cl
e.c. 2,8,7
(Cl - )
Ion
Atom
e.c. (2,8,8)-
The Chlorine gains 1 electron to gain a complete outer shell.
It is now a Chlorine ion with a charge of 1 -
The Chlorine atom has 7 electrons in it’s outer shell.
-
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Sodium atom
Na
Sodium ion
(Na +)
Chlorine atom
Cl
Chlorine ion
(Cl -)
The Ionic Bond
The sodium atom loses one electron to attain a complete outer shell and become a positive ion (Na +). The Chlorine atom gains one electron to attain a complete outer shell and become a negative ion (Cl –).Strong electrostatic forces attract the sodium and chlorine ions.
+ -
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Ionic Bonds
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Ion Cartoon
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Covalent Bonds
• Atoms in nonionic compounds share electrons.
• A molecule is formed when 2 or more atoms bond covalently.
• The majority of covalent bonds form between atoms of nonmetallic elements.
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Covalent Bonds
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Covalent Bonds
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Covalent bonds can be single, double or triple
• Single covalent bond: atoms share 1 pair of electrons
• Double covalent bond: atoms share 2 pairs of electrons
• Triple covalent bond: atoms share 3 pairs of electrons
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Covalent bonds
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Covalent bonds
• The halogens, group 17, form single covalent bonds with atoms of other nonmetals. They can only form 1 bond since they have 7 valence electrons.
• The chalcogens, group 16, have 6 valence electrons, can form a total of 2 bonds. These can be single or double.
• The group 15 elements, have 5 valence electrons, can form a total of 3 bonds. These can be single, double or triple.
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Practice
• Draw the Lewis structures for each molecule:
• a) PH3
• b) H2S
• c) HCl
• d) CCl4
• e) SiH4
• f) OBr2
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Electronegativity and Polarity
• The type of bond formed is related to each atom´s attraction for electrons.
• Electronegativity indicates the relative ability of an element´s atoms to attract electrons in a chemical bond.
• Nonmetals have higher electronegativities than do metals.
• Each element is assigned a value:
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Electronegativity
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Types of Bonds
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Types of bonds
• Bond can be: polar covalent, nonpolar covalent and ionic.
• Polar bond: a bond in which electrons are shared unequally.
• Nonpolar bond: a bond in which electrons are shared equally.
• Ionic bond: a bond in which electrons are transferred.
• The character of a bond depends on how strongly each of the bonded atoms attracts electrons.
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Practice
• Use electronegativities to classify each of the following bonds as nonpolar covalent, polar covalent or ionic:
• a) O-H
• b) O-K
• c) Cl- As
• d) N -N
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POLARITY OF MOLECULES
• Nonpolar molecules: are molecules that have a symmetrical arrangement and the dipoles cancel each other.
• Polar molecules: one end of the molecule is more negatively charged than the other end, have a dipole.
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POLARITY OF MOLECULES
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PRACTICE
• Indicate if each of the following molecules is polar or nonpolar:
• a) BF3
• b) CH3F
• c) CCl4
• d) NF3
• e) Br2
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IONIC AND COVALENT COMPOUNDS
IONIC COVALENT METALLIC
TYPE OF PARTICLE
PHYSICAL STATE
MELTING POINT
ELECTRIC CONDUCTIVITY
SOLUBILITY
EXAMPLES