1. 12/13 Do Now Draw a Bohr model for Chlorine
Draw a Lewis Dot/Electron Dot diagram for Chlorine

2. HW: Pg 1, 2, 3 12/13 Agenda Do Now Begin Ch 13 Notes
Begin HW (If time)
HW: Pg 1, 2, 3

3. Chapter 13 Material on Midterm
Chemical Bonding
Chapter 13
Material on Midterm

4. Section 1: Electrons and Chemical Bonding
Combining Atoms through Chemical Bonding
Most atoms hate being alone…so they ________!
Chemical bonding is the ________________ of atoms to form molecules or ionic compounds
Properties of new substance are _______________ that the properties of the old substance
The _________________________ is the interaction that holds the two atoms together.
bond
combining
different
chemical bond

5. =
C6H12O6
aka
glucose

6. Section 1: Electrons and Chemical Bonding
Combining Atoms Through Chemical Bonding
It’s all about the electrons
When bonds form, electrons can…
…be ______________
…be _____________
…be ________
shared
gained
lost

7. Section 1: Electrons and Chemical Bonding
Electron Number and Organization
We need to organize the electrons so we know what they will do if bonds are formed
Review: How do I know how many electrons a neutral atom has?
Same as its ________________________(proton #)
atomic number

8. Section 1: Electrons and Chemical Bonding
What are the rules for where the electrons go? 8 2

9. Section 1: Electrons and Chemical Bonding
What are the rules for where electrons can go?
NNESWESW
EXCEPTION:
Group 14: ____outer electrons
Pattern: __________ 4
NESW

10. Section 1: Electrons and Chemical Bonding
Outer-Level Electrons and Bonding
Only the _____________ electrons are involved in forming chemical bonds
The valence electrons are the electrons found in the _________________ shell of an atom
valence
outermost
For group numbers over 10… subtract _____ to get valence electron number
EXCEPT: _______ which has ____ 10 He 2

11. Section 1: Electrons and Chemical Bonding

13. Section 1: Electrons and Chemical Bonding
Valence Electrons and the Periodic Table
Elements in the same __________ have the same number of ___________________________(generally)
If Lithium has 1…then Sodium, Potassium, rubidium, Cesium, and Francium all have…___!
group
valence electrons 1

15. Section 1: Electrons and Chemical Bonding
To Bond or Not to Bond
Not all atoms bond the _______
Group 18 have their outmost shell ____________.
WANT TO GET TO 8!
Group 8/18 already has ____ (except He), so they’re happy and DO NOT REACT
same
filled 8

16. Section 1: Electrons and Chemical Bonding
To Bond or Not to Bond
Filling the Outermost Level
Less than 8? More likely to ___________.
Will share, take, or lose electron(s) to get to the magic number
What about 2?
Some elements that are _________ (H, He, Li, Be), will try to get to ___ electrons for that first shell
Will share, take, or lose electron(s) to get to this number
react
small 2

17. Section 2: Ionic Bonds Forming Ionic Bonds
An ionic bond is a bond that form when electrons are ______________ from one atom to another atom
This creates ions, which are ___________ particles that form when atoms gain or lose electrons
As a result of an ionic bond, either _________ or ______________ ions can form
transferred
charged
positive
negative

18. Summary:

19. Section 2: Ionic Bonds Forming Positive ions
Positive ions (cations) form when ________ atoms _______ electrons
Na loses one electron---Na+ Sodium cation
Ca loses two electrons –Ca2+ Calcium cation
By losing electrons, metals can get to the ________ _________!
Usually 8, could be 2
metal
lose
magic
number

20. Summary:

21. Section 2: Ionic Bonds Forming Negative Ions
Negative ions (anions) form when ____________ atoms ______ electrons
Change ending to “ide”
Cl gains one electron – Cl- Chloride anion
O gains two electrons – O2- Oxide anion
By gaining electrons, nonmetals can get to the ____________________!
Usually 8, could be 2
nonmetal
gain
magic number

23. Predicting Ionic bonds
An ionic bond would / wouldn’t form with aluminum and sodium because…
An ionic bond would / wouldn’t form with Aluminum and oxygen because…

24. Predicting Ionic bonds
An ionic bond would / wouldn’t form with sulfur and oxygen because…
An ionic bond would / wouldn’t form with sulfur and neon because…
An ionic bond would / wouldn’t form with sodium and neon because…

25. Section 2: Ionic Bonds Ionic Compounds
When ionic bonds form, the number of electrons ________ by the metal EQUALS the number of electrons ____________ by the nonmetals
Everyone is _________!
The overall compound is neutral because the ions _________________
lost
gained
happy
cancel out

26. Full sentences for full credit!
Writing Prompt #2 (of 3)
Write the answer
What is the difference between how metals and nonmetals form ions? Even though positive and negative ions are formed, why is an atom overall neutral?
Full sentences for full credit!

27. Writing Ionic Compounds
Write the metal with its charge
Write the nonmetal with its charge
Criss- Cross the charges
Only bring down the #, NOT the charge
Examples:
Sodium and Chlorine
Barium and Fluorine
Potassium and Oxygen
Lithium and Sulfur

28. Naming Ionic Compounds
-ide
Name of Metal + nonmetal w/ ending ______
Examples:
Sodium and Chlorine
Barium and Fluorine
Potassium and Oxygen
Lithium and Sulfur

29. Write and name me! Lithium and oxygen Aluminum and phosphorus
Magnesium and fluorine
Calcium and sulfur

30. Section 2: Ionic Bonds crystal lattice
When ions bond, they form a repeating 3D pattern called a ____________________
crystal lattice

31. Name and Draw!
Sodium and sulfur
Aluminum and Iodine

32. Section 3: Covalent and Metallic Bonds
Atom v. molecule
Atom
Molecule
______ type of element
_____ or more types of elements
Smallest particle into which an ____________ can be divided and still be the same element
Smallest particle into which a covalently bonded _____________ can be divided and still be the same compound
One
Two
element
compound

33. Section 3: Covalent and Metallic Bonds
Covalent Bonds and Molecules
A molecule is the smallest unit of a substance that keeps all the physical and chemical ______________ of that substance
2 or more atoms joined in a definite ratio
properties

34. Section 3: Covalent and Metallic Bonds
The Simplest Molecules
Must have at least two covalently bonded atoms
2 of the same element? ________________ molecules
Remember: HONClBrIF
Hydrogen Oxygen Nitrogen Chlorine Bromine Iodine Fluorine
Diatomic

35. Section 3: Covalent and Metallic Bonds
More Complex Molecules
Many different elements
Many based on ___________
carbon

36. Section 3: Covalent and Metallic Bonds
What are Covalent Bonds
A covalent bond forms when atoms __________ one or more pairs of electrons
Occurs between ________________
Helps them get to their MAGIC NUMBER (8 or 2)
share
nonmetals

37. Section 3: Covalent and Metallic Bonds
Covalent Bonds and Molecules
Easier way to draw them– _______________ Diagrams
Remember, only the valence electrons are important for bonding!
Electron-Dot

38. Covalent Compounds
How to draw covalent molecules using electron dot diagrams
Combine the elements where they can share electrons so each have a full outer shell. (The shared electrons are the covalent bond)
Examples:
Hydrogen + Chlorine
Fluorine + Fluorine
Water
Oxygen + Oxygen

39. Naming Covalent Compounds
Prefixes
One = _______
Two = _______
Three = ______
Four = ________
Five = ________
Six = _______
Seven = ________
Eight= _______
Nine = ________
Ten = _______
Rules:
Prefix + name Prefix + name –ide
Rule: Do NOT use mono- on the first element
Examples: CO
CO2
C2H4
P2O5
N3P6
mono di
tri
tetra
penta
hexa
hepta
octa
nona
deca

40. Name and Draw!
3 Hydrogen and 1 Nitrogen
Sulfur and 2 fluorine

41. 88

42. Section 3: Covalent and Metallic Bonds
Metals have properties like malleability and ductility because of their ___________________
______________________ are bonds from between the attraction of positively charged metal ions and the electrons around them
special bonds
Metallic bonds

43. Section 3: Covalent and Metallic Bonds
Movement of Electrons Throughout a Metal
Bonding in metals is a result of the metal atoms being so close to another that their outermost energy levels _____________
Metals surrounded in a “sea” of _____________
overlap
electrons

44. Section 3: Covalent and Metallic Bonds
Properties of Metals
Conducting Electric Current
Valence electrons that are __________
Reshaping Metals
Electrons free to move around…makes it easy to shape
____________
________________
Bending without breaking
Electrons can ________ in response to pressure so they can bend without breaking
moving
Ductility
Malleability
move

45. Full sentences for full credit!
Writing Prompt #3 (of 3)
Write the answer.
How do metallic bonds explain ductility and malleability in metals?
Full sentences for full credit!