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Ionization, Electronegativity, and Bonds

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Presentation on theme: "Ionization, Electronegativity, and Bonds"— Presentation transcript:

1 Ionization, Electronegativity, and Bonds
Chemical bonding Ionization, Electronegativity, and Bonds

2 Chemical Formulas and Units
A chemical formula shows the kinds of atoms in the molecule as well as the amount of atoms in the molecule A formula unit is expressed in the smallest whole number ratio for the molecule Examples: NaCl TiO2 VCl5 Ca3(PO4)2

3 All about Valence Electrons
Electrons located in the outer shell Readily available for bonding Always s or p sublevel Follows the Octet Rule Modeled by the Lewis Dot Diagram

4 The two biggest indicators
Electronegativity Big Difference = Ionic Character Small Difference = Covalent Character Atom Type M + NM = Ionic M + M = Metallic NM + NM = Covalent

5 Formed from an exchange in electrons forming two charged ions
Ionic Bonding Formed from an exchange in electrons forming two charged ions Result of large difference in electronegativity Strongest type of bond

6 Ionic Bond Characteristics
Solid at room temperature High Melting point & High Boiling Point Become conductive when melted or dissolved Create network, crystalline solids that are hard and brittle

7 Common Anions ( -1) F- Fluoride NO- Nitrate I- Iodide C2H3O2- Acetate
OH- Hydroxide MnO4- Permanganate Cl- Chloride CN- Cyanide ClO- Hypochlorite Br- Bromide ClO2- Chlorite BrO3- Bromate ClO3- Chlorate HCO3- Hydrogen Carbonate

8 Common Anions (-2) O-2 Oxide S-2 Sulfide SO4-2 Sulfate CO3-2 Carbonate Cr2O7-2 Dichromate CrO4-2 Chromate

9 Common Anions (-3) N-3 Nitride P-3 Phosphide PO4-3 Phosphate

10 The Octet Rule – Determining the charge
States that an atom will lose or gain electrons in order to fill the outer sublevels (s and p) to achieve noble gas configuration Modeled by the Lewis Dot Diagram >4 valence electrons = Gain of electrons = anion <4 valence electrons = Loss of electrons = cations =4 valence electrons = could go either way (metalloid)

11 Binary Ionic Compounds
A Bicycle has how many wheels? A biplane has how many wings? A binary compound has how many elements? A binary ionic compound has two elements where electrons are exchanged NaCl MgBr2 Ca3N2 Sodium Chloride Magnesium Bromide Calcium Nitride

12 Polyatomic Ions What is polytheism? What is a polygon?
How about polyatomic ions? Polyatomic ions are IONS that consist of multiple atoms Polyatomic ions are used in ionic bonding because there is still an exchange in electrons PAGE 7 OF REFERENCE PACKET!!!

13 Electrons are shared between atoms
Covalent Bonding Electrons are shared between atoms Result of similar electronegativities Two non-metal atoms Each bond represents a pair of electrons

14 Covalent Bonding characteristics
Bonds can occur as single, double, or triple bonds Excellent insulators Composed by Non-metals Low melting point & Low boiling point Polarity Volatile Can achieve all states of matter, commonly found as liquids or gases Solubility depends on polarity “like dissolves like”

15 VSPER Theory Lewis Dot diagrams help make pairs!
Valence Shell Electron Pair Repulsion Theory Depends on number of bonding (ligands) and nonbonding (lone pairs) groups around the central atom. Lewis Dot diagrams help make pairs! Atoms and lone pairs want to be as far apart from one another as possible = geometry of a molecule

16 VSEPR Shapes

17 Linear Arrangement 180°  2 LIGANDS, 0 LONE PAIRS

18 Bent type 1 <120°  2 LIGANDS, 1 LONE PAIRS

19 Bent type 11 <109.5°  2 LIGANDS, 2 LONE PAIRS

20 Trigonal Planar 120°  3 LIGANDS, 0 LONE PAIRS

21 Trigonal Pyramidal <109.5°  3 LIGANDS, 1 LONE PAIRS

22 Tetrahedral Tetrahedron 109.5°  4 LIGANDS, 0 LONE PAIRS

23

24 Electron movement allows for all of the unique properties
Metallic Bonds Electrons are shared through empty orbitals across ALL metal atoms (delocalized) Electron movement allows for all of the unique properties Weakest type of bond

25 Transition Metal Cations

26 Metallic Bonding Attraction of free floating electrons in the cloud
Flow of electrons allows for great conductivity Often arranged in a crystalline structure Alloys are a mixture of metals that take advantage of their properties

27 Metallic Bonding Characteristics
Conductive of heat Insoluble Conductive of electricity Malleability Luster (shiny) High melting & high boiling point (due to structure) Ductile Crystalline Structures

28 Forces – Attraction between compounds
Hydrogen Bonds Only occur between O, N, or F Dipole-Dipole Attraction Only occur between polar substances Responsible for adhesion and cohesion London Dispersion Forces Weakest attraction between electrons and protons of any compound Also called universal attraction

29 Use the electronegativity trend
Determining the Bond Use the electronegativity trend If they are close = covalent If they are far = ionic If they are both metals = metallic If there are multiple atoms that are close and far = covalent and ionic

30 Ionic Covalent Metallic NaCl NaNO3 CO4 Ag2CrO4 K2O N2O2 Fe2O3 TiC PCl5
What would the bond be? NaCl NaNO3 CO4 Ag2CrO4 K2O N2O2 Fe2O3 TiC PCl5 CuZn Ionic Covalent Metallic


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