Chemical Bonding

1
Chemical Bonding

• Ionic, Covalent and Metallic Bonding
• Polar, Nonpolar Covalent, and
  Polar-Covalent Bonds
• Naming Chemical Compounds
• Writing Chemical Formulas

2

• Chemical Bond a mutual electrical attraction
  between the nuclei and valence electrons of
  different atoms that binds the atoms together.
• ..
  ..
• Na Cl NaCl
• .. ..
• NN NN

3

• Ionic Bonding chemical bonding that results
  from the electrical attraction between cations
  and anions.
• ..
  .. ..
• Na Cl NaCl Na1Cl-1
• .. .. ..

4

• Covalent Bonding results from the sharing of
  electron pairs between two atoms.
• NN NN

5

• Metallic Bonding the chemical bonding that
  results from the attraction between metal atoms
  and the surrounding sea of electrons.
• http//ithacasciencezone.com/chemzone/lessons/03bo
  nding/mleebonding/metallicbonding.htm

6

• Polar Bond (Ionic Bond) a bond in which there
  is a dramatically uneven distribution of charge
  due to a large difference in the
  electronegativities of the bonded atoms.
• 1.7 lt Ionic

7

• Is potassium chloride (KCl) an ionic compound?
• EN of Cl 3.0
• EN of K 0.8
• 2.2

8

• NonpolarCovalent Bond a covalent bond in which
  the bonding electrons are shared equally by the
  bonded atoms, resulting in a balanced
  distribution of electrical charge.
• Nonpolar lt 0.3

9

• Is Chlorine Monofluoride (ClF) a nonpolar
• covalent compound?
• EN of F 4.0
• EN of Cl 3.0
• 1.0

10

• Polar covalent bond is a covalent bond in
  which the bonded atoms have an unequal
  attraction for the shared electrons.
• 0.3 lt Polar Covalent lt 1.7

11

• Are the bonds in carbon dioxide (CO2) polar?
• EN of O 3.5
• EN of C 2.5
• 1.0

12

• Is the overall compound of carbon dioxide (CO2)
  polar?
• .. ..
• O C O
• . . . .
• ? ?

13
Naming Ionic Chemical Compounds

• Nomenclature (Naming System) a naming system
  for binary ionic compounds which involves
  combining the names of the compounds positive
  and negative ions.
• An ionic compound is composed of a cation ion and
  an anion.
• In an ionic compound, the cation (metal) is
  always written first and the anion (nonmetal) is
  always written second.

14
Type I Compounds (Binary Ionic Compounds)

• Binary Compound Compounds that are composed of
  two elements.
• Ionic Compound is composed of positive and
  negative ions that are combined so that the
  number of positive and negative charges are
  equal.

15
When naming the compound

• Name the cation as is.
• Part of the ending of the name for the anion gets
  dropped and ide is added.
• See the back of your periodic table.
• NaCl Sodium Chloride

16

• Name the following Compounds
• 1. CsI
• 2. Al2S3
• 3. Ba3N2
• 1. cesium iodide
• 2. aluminum sulfide
• 3. barium nitride

17
Writing Chemical Formulas

• Oxidation Numbers (Oxidation States) the number
  of electrons that have either been lost or gained
  by an ion or polyatomic ion.
• Calcium ion
• Ca2
• Chlorine ion
• Cl-1

18

• Chemical Formula indicates the relative number
  of atoms of each element in a chemical compound
  by using atomic symbols and numerical subscripts.
• Criss-cross the numbers from the charges.
• Potassium fluoride
• K1 F-1 KF
• Rubidium nitride
• Rb1 N-3 Rb3N

19

• Write the Formula for the following
• 1. Lithium Bromide
• 2. Calcium Oxide
• 3. Strontium Phosphide
• 1. LiBr
• 2. Ca2O2 CaO
• 3. Sr3P2

20
Type II Compounds (Binary Ionic Compounds with
Transition Metals)

• Most transition metals can have more than one
  type of charge.
• Example Pb2 or Pb4, Co2 or Co3, and
• Cu1 or Cu2
• Roman numerals are used, only in the name, to
  indicate what charge is on the transition metal.

21
Write the Formula for the following

• 1. Lead (IV) Oxide
• 2. Cobalt (III) Iodide
• 3. Chromium (II) Nitride
• 1. PbO2
• 2. CoI3
• 3. Cr3N2

22

• Name the following Compounds
• 1. NiCl3
• 2. FeS
• 3. AgF
• 1. Nickel (III) chloride
• 2. Iron (II) sulfide
• 3. Silver fluoride

23
Type III Compounds (Ternary Ionic Compounds)

• Ternary Compound a compound that contains three
  or more elements.
• Polyatomic ion a charged group of covalently
  bonded atoms.
• Oxyanions polyatomic ions that contain oxygen.

24
Polyatomic Ions

• (PO3)-3 phosphite
• (PO4)-3 phosphate
• (ClO4)-1 perchlorate
• (ClO3)-1 chlorate
• (ClO2)-1 chlorite
• (ClO)-1 hypochlorite
• F, Br, or I can replace Cl in any of these
  polyatomic ions.

25

• (CN)- 1 cyanide
• (OH)-1 hydroxide
• (NH4)1 ammonium
• (HSO3)-1 hydrogen sulfite
• (Cr2O7)-2 dichromate

26
List of Polyatomic Ions to Memorize

• Ammonium, Acetate, Chlorate, Chlorite, Cyanide,
  Bicarbonate, Hydroxide, Hypochlorite, Nitrite,
  Nitrate, Perchlorate, Permanganate
• ( F, Br or I can replace Cl in each)
• Carbonate, Chromate, Dichromate, Oxalate,
  Peroxide, Sulfite, Sulfate
• Phosphite, Phosphate

27
Write the names for the following

• 1. (NH4)2SO4
• 2. K(NO3)
• 3. CaCO3
• 1. Ammonium sulfate
• 2. Potassium nitrate
• 3. Calcium carbonate

28
Type IV Compounds (Covalent Compounds)

• Molecule is a neutral group of atoms that are
  held together by covalent bonds.
• Molecular Compound a chemical compound whose
  simplest units are molecules.
• Molecular Formula show the type and number of
  atoms combined in a single molecule of a
  molecular compound.

29
Naming Covalent Compounds

• Name the first nonmetal as is.
• Name the second nonmetal with the ide ending.
• Use Greek Prefixes to Name (The Greek Prefix
  indicates the number of each element in the
  compound)

30

• Do Not apply mono to the first element!
• Do Not Criss-Cross!
• Do Not use charges!
• Do Not reduce subscripts!

31
Greek Prefixes

• Mono 1
• Di 2
• Tri 3
• Tetra 4
• Penta 5
• Hexa 6
• Hepta 7
• Octa 8
• Nona 9
• Deca - 10

32

• Multiple Bonds refers to covalent bonds that
  share more than one pair of electrons (double or
  triple bonds)
• Double Bond is a covalent bond in
• which two pair of electrons are shared
• between two atoms.
• Triple Bond is a covalent bond in which
• three pair of electrons are shared between
• two atoms.

33
Name the following compounds

• 1. CO
• 2. CO2
• 3. N2O3
• 1. Carbon monoxide
• 2. Carbon dioxide
• 3. Dinitrogen trioxide

34
Write the formula for the following

• 1. Sulfur Hexafluoride
• 2. Tetraphosphorus decoxide
• 3. Boron trichloride
• 4. Disulfur dichloride
• 1. SF6
• 2. P4O10
• 3. BCl3
• 4. S2Cl2