1. Pearson Prentice Hall Physical Science: Concepts in Action
Chapter 6
Chemical Bonds

5. 6.1 Ionic Bonding Objectives:
1. Explain when an atom is unlikely to react
2. Indicate one way in which elements can achieve a stable electron configuration
3. Express how the structure of an ionic compound affects its properties

6. How atoms bond - George Zaidan and Charles Morton

7. When Atoms are Unlikely to React
When the highest occupied energy level (the outer shell) is filled with electrons (valence electrons), the atom is stable and unlikely to react

10. Because pf sp3 hybridization, 8 electrons is a full valence orbital

11. Electron dot diagram
The valence electrons can be represented by a special drawing called an electron dot diagram (8 electrons is full)

12. How to draw dot diagrams
Electrons do not pair until they must

13. Concept Question
Draw the electron dot diagram for  Ca S P C Cl

14. Achieving Stable Electron Configurations
Atoms can become stable by obtaining a full valence orbital
Some elements achieve stable electron configurations by transferring electrons between atoms
The gain or loss of electrons between the atoms then produces full shells & stability

15. Giving and taking electrons  Ionic compounds
NaCl
MgO

16. Concept Question
Use electron dot diagrams to predict the ratio of the ionic compound
Ex: Na + Cl  NaCl 1:1
Na + O  Na2O 2:1
Na + N _______
Ca + Cl _______
Al + S ________

17. The gain or loss of electrons also produces an atom with a net positive charge (lost one or more electrons) or a net negative charge (gained one or more electrons)

18. Definition: an ion is an atom with a net positive or net negative charge
Definition: an anion is an ion with a net negative charge
Definition: a cation is an ion with a net positive charge

19. Definition: a chemical bond is the force that holds atoms or ions together as a unit
Definition: an ionic bond is the force that holds cations and anions together
Definition: an ionic bond is the bond that forms when electrons are transferred from one atom to another

21. Definition: a chemical formula is a notation that shows which elements a compound contains & the ratio of atoms or ions of the elements that make up the compound

22. Cations form when electrons gain enough energy to escape from atoms
Electrons must overcome the natural attraction to the protons in the nucleus

23. Definition: ionization energy is the amount of energy used to remove an electron from an atom
The lower the ionization energy is, the easier it is to remove an electron

24. Ionization generally increases in the periodic table from left to right and decreases from the top down

25. Structure and Properties
Many ionic compounds are solid at room temperature
IONIC COMPOUNDS GENERALLY CONSIST OF A METAL + A NONMETAL
Their molecular structure has an orderly repeating three dimensional structure called a lattice

26. Definition: solids whose particles are arrange in a lattice are called crystals
The properties of an ionic compound can be explained by the strong attractions among the ions in a crystal lattice

27. Ionic cmpds are brittle

28. 6.1 Ionic Bonding When is an atom least likely to react?
Describe one way an element can achieve a a stable electron configuration.
What characteristic of ionic bonds can be used to explain the properties of ionic compounds?
Use ioniation energy to explain why metals lose electrons more easily than nonmetals.
Why is a rock salt crystal likely to shatter when struck?
What will the ratio of ions be in any compound formed from a Group 1 metal and a Group 7 (Halogen) nonmetal? Explain.
Why do ionic compounds include at least one metal?
Based on their chemical formulas, which of these compounds is not likely to be an ionic compound: KBr, SO2, or FeCl3? Explain.

31. 6.2 Covalent Bonding Objectives:
1. Explain how atoms are held together in a covalent bond
2. Describe what happens when atoms don’t share electrons equally
3. Discuss what factors determine whether a molecule is polar
4. Compare the attractions between polar molecules with the attractions between nonpolar molecules

33. How Atoms Are Held Together in a Covalent Bond
Definition: a covalent bond is a chemical bond in which two atoms share a pair of valence electrons
Definition: a molecule is a neutral group of atoms that are joined together by one or more covalent bonds

34. The attractions between the shared electrons & the protons in each nucleus hold the atoms together in a covalent bond
It is possible for more than one pair of electrons to be shared producing a double or triple covalent bond

35. Unequal Sharing of Electrons
IN GENRAL, COVALENT MOLECULES CONSIST OF TWO NONMETALS
Definition: a polar covalent bond is a covalent bond in which the electrons are not shared equally
When atoms form a polar covalent bond, the atom with the greater attraction for electrons has a partial negative charge (written δ-)
The other atom has a partial positive charge (written δ+)
Water is an example

36. Polar molecules

37. Polar bonds - Electrons can be shared “unequally”

38. Polar bonds

40. Polar vs. non molecules

42. Factors that Determine Polarity
The electronegativity of atoms in the molecule and its geometric shape are factors that determine whether a molecule is polar or nonpolar
Example: CO2 is linear, while the water molecule is bent

43. Lewis dot diagrams activity

44. Polar Attractions
Attractions between polar molecules are stronger than attractions between nonpolar molecules
“Like attracts like”: polar molecules are attracted to polar molecules; nonpolar molecules are attracted to nonpolar molecules

45. 6.2 Covalent bonds What hold atoms together in a covalent bond?
What happens to the charge on atoms when they form a polar covalent bond?
Name the two factors that determine whether a molecule is polar.
Compare the strength of attractions between polar molecules to the attrition between nonpolar molecules.
What is a molecule?
Which of these elements do not bond? Oxygen, chlorine, neon, or sulfur?
Why is the boiling point of water higher than chlorine (Cl2)?
Using electron diagrams, what is the chemical formula for nitrogen bonded with hydrogens?

47. 6.3 Naming Compounds & Writing Formulas
Objectives:
1. Explain what information the name and formula of an ionic compound provide
2. Describe the information that the name and formula of a molecular compound provide

48. Ionic Compound Formulas
The name of an ionic compound (usually a metal plus a nonmetal) must distinguish the compound from other ionic compounds containing the same elements
The formula of an ionic compound describes the ratio of the ions in the compound

49. Definition: a binary compound is a compound made of only 2 elements
The name of a binary compound follows a pattern
The cation (+ charge, usually the metal) is named first followed by the anion (- charge, usually the nonmetal)
The cation states its name
There is a special suffix for the anion
The anion uses the stem of its name plus –ide ex: chlorine becomes chloride (-ide means it’s an ion)

50. Many transition metals can form more than one ion
Ex: iron can be Fe2+ or Fe3+ & is called “iron two ion” or “iron three ion”
The name of transition metal ions will have a Roman numeral after the name that states the charge
Ex: CuO is copper(II) oxide because copper can be Cu+ or Cu2+
Definition: a polyatomic ion is a covalently bonded group of atoms acting as a single unit that carries a charge
Compounds with polyatomic ions are ionic compounds

51. If you know the name, you can write the formula
The total charges of the cations and anions must add up to zero
Sodium ion is Na+ while sulfide is S2-
You will need 2 sodium ions to make the charges add up to zero
It is written Na2S and is called sodium sulfide

52. Molecular Compound Formulas
The name and formula of a molecular compound describe the type and number of atoms in a molecule of that compound
Molecular compounds are made from nonmetals (upstairs to the right in the periodic table)
To name the compounds, the most metallic element, farthest to the left on the table is named first
If the elements are in the same group, the element closest to the bottom of the group is named first

53. The suffix of the second element is changed to –ide
It is possible to for 2 elements to combine in different amounts to produce a molecular compound such as N2O4 and NO2
Prefixes are used to tell the amount of each except when there is only one atom of the first element
Do not use –mono on the first element only
1=mono- 2=di- 3=tri- 4=tetra- 5=penta- 6=hexa- 7=hepta- 8=octa- 9=nona- 10=deca-

54. To write the formula for a molecular compound, write the symbols of the elements in the name
Then add the appropriate subscript to the element
Ex: diphosphorus tetrafluoride is P2F4
Q: What is a polyatomic ion?
Q: What is the formula for calcium chloride?
Q: Is calcium chloride an ionic or molecular compound? How do you know?