1. Chapter 6
ATOMS AND BONDING

3. New Chapter New Notebook
Unit 2 Chapter 6 Day 1
OBJECTIVE: Describe how ionic bonds form. Predict the composition of a ionic compound.
Do Now:
Vocabulary Word Windows-Chapter 6
Today:
Chapter 6 – Atoms and Bonding notes
Practice – Ionic and Covalent Bonds
Homework:
Everyday Elements
Missing Assignments?
New Chapter New Notebook

4. Unit 2 Chapter 6 Day 2
OBJECTIVE: Predict the composition of a ionic and covalent compound.
Do Now:
R & R – Ionic Bonding
Today:
Finish Notes and Practice – Ionic and Covalent Bonds
Bonding Basics – Ionic and Covalent
Homework:
Read Chapter 6.1 and 6.1 GRWS

5. Unit 2 Chapter 6 Day 3
OBJECTIVE: Name and Determine chemical formulas for ionic, covalent and molecular compounds.
Do Now:
Charting Oxidation Numbers
Today:
Homework check and review 6.1 GRWS
Bonding and Chemical Formulas
The Criss-Cross method
Writing and Naming Compounds
Homework:
Read Chapter 6.2 and 6.2 GRWS

6. Unit 2 Chapter 6 Day 4 OBJECTIVE: Model the structure of ionic and covalent molecules. Predict and classify and name ionic and covalent bonds.
Do Now:
Counting Atoms
Today:
Homework check and review 6.2 GRWS
Continue Writing and Naming Compounds
Bond with a Classmate Activity
Homework:
Read Chapter 6.3 and 6.3 GRWS

7. Unit 2 Chapter 6 Day 5
OBJECTIVE: Model the structure of ionic and covalent molecules. Predict and classify and name ionic and covalent bonds.
Do Now:
Word Wise Chap 6
Today:
Molecule Models: Model to Formula
Homework check and review 6.3 GRWS
Modeling Molecules Lab
Homework:
Counting Naming Writing Formula review

8. Unit 2 Chapter 6/7 transition
OBJECTIVE: Model the structure of ionic and covalent molecules. Predict and classify and name ionic and covalent bonds.
Star Trek and the Silicon Creature
Modern Marvels Video – Carbon
CSI Online

9. CHEMICAL BONDING
when atoms combine
to form new substances

10. Examples of COMPOUNDS
SALT
SUGAR
WATER
VINEGAR
BLEACH
BAKING SODA

11. REMEMBER!!
in an atom
# protons = # electrons
NEUTRAL (no charge)

12. ELECTRONS
attract the
PROTONS
Atoms are like
Tiny MAGNETS
THIS ATTRACTION
KEEPS THE ATOM
TOGETHER!

13. ELECTRONS are in Energy Levels around the Nucleus
1st Level can hold up to
2 ELECTRONS
2nd Level can hold up to
8 ELECTRONS
3rd Level can hold up to
18 ELECTRONS

14. (in the level farthest away from the nucleus)
Outermost Electrons
(in the level farthest away from the nucleus)
*VALENCE ELECTRONS*
Valence Electrons
are most IMPORTANT
ELECTRONS!!
they CAUSE bonding

15. # of valence electrons
tells HOW
that atom
will bond
with others!

16. outermost energy level
When an atom has
FILLED
outermost energy level
it is VERY stable
(Noble Gases have filled
outermost energy levels)

18. Every atom
HOPES
that one day
it will have a
filled outermost
energy level

19. Some atoms
TAKE Electrons
to be stable!
Some atoms
GIVE AWAY Electrons
to be stable!
Some atoms
SHARE Electrons
to be stable!

20. THERE ARE
2 TYPES OF BONDS
Ionic and Covalent

21. IONIC bonding

22. IONIC BONDING
Atoms
GIVE AND TAKE
Electrons
(they don't SHARE them!)

23. charged atom
(positive or
negative charge)
ION
Not like a
NORMAL, NEUTRAL atom

24. Na 1+ Na
atom
ion

26. Ionic Bonding” also called “electron transfer bonding”
IN IONIC BONDING
one atom
TAKES electrons
from another atom
Ionic Bonding” also called “electron transfer bonding”

27. Ions are either “+” (positive) Or Ions are “-” (negative)
Ions are charged atoms
Ions are either “+” (positive)
Or Ions are “-” (negative)

28. Atoms that undergo ionic bonding either gain or lose electrons
If an atom gains an electron it becomes “-” negatively charged ion Why?
If an atom loses an electron, the overall charge on the ion is positive.

29. When 2 ions bond the over all charge on the atom is
Neutral
Ex: Sodium Fluoride Na¹+ (more positive) F¹¯ (more negative) YieldsNaF (neutral)

30. Ion Formation
The process of removing electrons and forming ions is called Ionization
Energy is needed for ionization This energy is called Ionization energy

31. Ionization energy is directly related to number of valence electrons

32. Less valence electrons = Less ionization energy
EX: Li has 1 valence electron = LOW ionization energy
Other elements with LOW Ionization energies Alkali metals and Alkaline metals

33. More valence electrons= HIGH ionization energy
EX: Fluorine has 7 valence electrons = Very HIGH ionization energy
Other elements with HIGH Ionization energies Halogens

34. Why ? It is easier to gain 1 electron then to lose 7
Electron Affinity:
The tendency of an atom to attract electrons.

35. Fluorine has a strong electron affinity
Why?
Because it only needs one more electron to have a “full” outer electron shell All Halogens have strong electron affinities

36. Ionic Bonds produce crystal lattice structures
have repeatable patterns
Lattice structure makes ionic molecule more stable

37. Example: NaCl (table salt)
Gives physical property of shape example= cubic crystals in salt Gives a physical property of high melting point
Example: NaCl (table salt)

38. One Last word about Ions…
Polyatomic Ions
A special group of covalently bonded atoms that acts like a single atom
Example: OH- (hydroxide)

40. Covalent bonding

41. Covalent Bonds Usually non metals.
(You will need TWO different colored pencils for today’s lesson) Covalent Bonding occurs when atoms SHARE electrons.
Usually non metals.
Both of the non metals want to GAIN electrons.
The elements will SHARE electrons in an effort to fill their outer shells.

42. NON-METALS
METALS

43. Covalent Bonds
The forces holding covalent molecules together are weaker than ionic bonds
Covalent compounds are often gases or liquids
They do not conduct electricity
They do not dissolve in water

44. Covalent Bonds
A good example of a covalent bond is between two Hydrogen atoms. H
Hydrogen has one electron in its electron shell.
Since this shell can have TWO, each hydrogen will try to gain a second electron.
A single atom will react with another to form the compound H2

45. This is called a SINGLE covalent bond
Covalent Bonds
The atoms share each other’s single electron forming a covalent bond and BOTH atoms have a full electron shell H H
This is called a SINGLE covalent bond

46. Covalent Bonds
Draw a single covalent bond for Chlorine:
Cl Cl

47. Covalent Bonds
Draw two covalent bonds in water:
H O H

48. This is called a DOUBLE covalent bond
Covalent Bonds
Atoms can share more than one electron. Oxygen atoms share two electrons to form oxygen molecules:
O O
This is called a DOUBLE covalent bond