1. Covalent and Ionic Bonding
Chemical Bonding
Covalent and Ionic Bonding

2. Compound Review
Compound: a chemical combination of two or more elements
Why do elements chemically combine?
They want to achieve full energy levels
Full energy level = stability
Elements will move electrons for them to be satisfied

3. How do the electrons move?
Two ways:
Transferring electrons between two atoms
One atom is close to having a full level, while the other is close to emptying a level
Electrons are transferred from the almost empty atom to the almost full atom to make both satisfied
Sharing electrons between two atoms
Both atoms are close to having full levels
Electrons are shared back and forth between two atoms to make both feel satisfied

4. How do the electrons move?
Ionic Bonding
Transferring electrons between two atoms
One atom is close to having a full level, while the other is close to emptying a level
Electrons are transferred from the almost empty atom to the almost full atom to make both satisfied
Covalent Bonding
Sharing electrons between two atoms
Both atoms are close to having full levels
Electrons are shared back and forth between two atoms to make both feel satisfied

5. Ionic Bonding
Ionic Bond: a bond where the bonding electrons are transferred between two atoms
Typically occurs between a non-metallic and a metallic element
These are elements on opposite sides of the PT
The metallic elements are close to emptying a level
The non-metals are close to having a full level
The electron is transferred from the metal to the non-metal

6. Characteristics of Ionic Bonds
Ionic molecules are bound by charge
The transfer of electrons creates opposite charges
The atom that gains electrons is negative
The atom that loses electrons is positive
Ionic bonds form crystals
There is a lot of attraction between one set of bonding atoms and another
The attraction tends to create solids

7. Ions

8. Binary Ionic Nomenclature
Positive atom first, negative second
Charges must add up to zero
NO PREFIXES used in the written name
Ending of second element switched to “-ide”

9. Examples Magnesium bonds with bromine Chlorine bonds with potassium
Which comes first? ClK or KCl
How do we write the name?
Potassium chloride
Magnesium bonds with bromine
Which comes first? MgBr or Br2Mg
How do we write the name?
Magnesium bromide

10. Transition Metals
Transition metals are from Group 3 up to the dividing line that cuts through the “p” section
Remember that these metals have electrons in overlapping energy levels
Because of this overlap, the atom is often trying to fill two different levels instead of just one
This means that transition metals will often have more than one possible charge

11. Transition Metals (continued)
In the written name of a compound, the transition metals will have a Roman numeral that follows its name
The Roman numeral designates the charge of the transition metal
The Roman numeral does not need to be written in the molecular formula of the compound

12. Transition Metal Examples
Iron with a +3 charge bonds with chlorine
Molecular formula?
FeCl3
How do we write the name?
Iron (III) chloride
Copper with a +1 charge bonds with oxygen
Molecular Formula?
Cu2O
How do we write the name?
Copper (I) oxide

13. Polyatomic Ions “Poly-” means many
Polyatomic ion: an ion formed of more than one type of element
These types of ions are typically unsatisfied covalent bonds
Listed on back of PT

14. Polyatomic Ions (continued)
Polyatomic ions have names that typically end in “- ate” or “-ite”
When writing the molecular formula, you still make the charges neutral
If a polyatomic ion needs to be multiplied to make the charges neutral, it should be in parentheses
When writing the name, do not change the ending of the polyatomic ion; just use it as listed

15. Polyatomic Ion Examples
Calcium bonds with nitrate
Molecular formula? Ca(NO3)2
How do we write the name?
Calcium nitrate
Iron with a +3 charge bonds with carbonate
Molecular Formula? Fe2(CO3)3
How do we write the name?
Iron (III) carbonate

16. Ionic Practice TiI4 Na2CO3 NaOH FeCl2 FeCl3 Li3PO4 Lead (II) Sulfite
Beryllium Chloride
Gallium Nitride

17. Covalent Bond
Covalent Bond: a bond where the bonding electrons are shared between two atoms
Typically occurs between two non-metallic elements
These are elements to the right side of the PT
These elements are close to having full energy levels

18. Covalent Bonding

19. Covalent Molecules Covalent molecules are bound by proximity
The molecules must be close to each other to share the electron(s)
Covalent bonds form individual molecules

20. Lewis Structures
Each element in a group has the same number of electrons in their outer orbital, also known as “shells”.
The electrons in the outer shell are called “valence electrons”

21. Covalent Bond
Cl2
Chlorine will form a covalent bond with itself.

22. Cl Cl

23. Cl Cl

24. Cl Cl

25. Draw these bonds H2 F2 HF
H2O
NH3
CH4 I2
NF3

26. Covalent Nomenclature
Nomenclature: a system of naming
Lower electronegative atom first, highest second
Prefixes used in front of each element to show quantity of atoms that are sharing
Ending of second element switched to “-ide”

27. Covalent Nomenclature
One
Mono-
Six
Hexa-
Two
Di-
Seven
Hepta-
Three
Tri-
Eight
Octa-
Four
Tetra-
Nine
Nona-
Five
Penta-
Ten
Deca-

28. Examples
Example of a molecular comp:
CO2 CO
CCl4
Carbon tetrabromide

29. Practice PCl5 SF6 carbon trichloride N2O disulfur hexoxide NO2
nitrogen triiodide

30. Practice
CCl4
nitrogen triiodide
C2H6
DOUBLE BOND
SiO2

31. Prompt
Tell me about something that’s good in your life right now. It could be something at home, something related to school, or anything else that makes you happy.