1. Do Now Describe the structure of the atom… You must include….
The names of the subatomic particles.
Their charges.
Where in the atom they are located.

2. Atomic Structure
Protons- Positively charged particles located in the nucleus
Neutrons- Uncharged particles located inside the nucleus
Electrons- Negatively charged particles located outside the nucleus

3. Comparing subatomic particles…

4. Green – metals
Yellow – nonmetals
Blue - metalloids

5. Atomic Number # of protons # of electrons in a NEUTRAL atom
Always a whole number

6. Mass Number # of protons + neutrons in atomic mass units (amu)
Isotopes - atoms of the same element with different masses
differ in number of neutrons
Examples: Carbon-13 & Carbon-14

7. Give this a try Group Period Element Name Symbol P (+) N (0) E (-) 2 4
Calcium Ca 17 5 13 6

8. Do Now
Draw Lewis dot structures for Nitrogen, Calcium, Sulfur, and Potassium. (use the valance electron #)
Give the oxidation numbers for Sodium, Iodine, Phosphorus, Barium, Aluminum, and Oxygen.
Metals = valence electron number (with a (+) sign)
Nonmetals = - (8-valence electron #)
Give the formula for the compound formed between Magnesium and Nitrogen.

9. Oxidation Number
- The charge that the ion gets when it either loses or gains electrons is called the oxidation number.
The sum of the oxidation numbers for the atoms in a compound must be zero
In order for a compound to exist, it must be electrically neutral

10. ‘Criss - Cross’ Method
The formula for the compound composed of potassium and sulfur
K 1+ & S 2-
The formula for the compound composed of calcium and bromine
Ca 2+ & Br 1-
This becomes K2S
This becomes CaBr2

11. Steps to follow Step 1- write element symbols with the metal first
Step 2- write the oxidation numbers next to the elements
Metals = valence electron number (with a (+) sign)
Nonmetals = -(8-valence electron #)
Step 3- criss-cross numbers without signs
Step 4- don’t write 1’s for final compound
Step 5- Reduce the numbers

12. Do now
Q2Z is the formula of an ionic compound made from non-existent elements.
Which element is a non metal?
What are the oxidation numbers for each element?
How many valance electrons does each element have?
Draw a dot structure for each element.

13. DO NOW
What is the difference between a physical change and a chemical change?

14. Physical Change
A change in a material that does not create new substances.
Examples:
Melting, and other phase changes
Cutting
Shaving
Squashing

15. Chemical Change Creates new substances. Examples: Burning anything
(new substance=ash, energy, heat)
2 chemicals reacting.

16. Chemical Reaction
A reaction happens when two or more molecules interact and the molecules change.
A chemical change must occur. You start with one compound and turn it into another.

17. Counting Atoms in a Compound
Subscripts- small number next to an element
Example: Al₂ O₃
1 compound: Al₂O₃
2 elements: Al and O
5 atoms : 2 aluminum and 3 oxygen atoms

18. Compounds with parentheses
Multiply the number outside the parentheses by all of the subscripts inside
Example:
Ga₂ (SO₄)₃
Ga = 2 , S = 1x3 = 3 , O = 4x3 = 12

19. Find the number of atoms for each element in the following compounds:
AgNO3
Al(ClO3)3
(NH4)2SO3

20. Chemical Equations
Their Job: Depict the kind of reactants and products and their relative amounts in a reaction.
4 Al (s) O2 (g) ---> 2 Al2O3 (s)
The numbers in the front are called coefficients

21. Chemical Equations Reactants  Products
All chemical equations have reactants and products.
We express a chemical equation as follows:
Reactants  Products
The arrow is equivalent to an “=“ math. When we describe the equation we use the word “yields” or “produces” instead of equals
Example
C + O2  CO2
This reads “carbon plus oxygen react to yield carbon dioxide”

22. Subscripts vs. Coefficients
The subscripts tell you how many atoms of a particular element are in a compound. The coefficient tells you about the quantity, or number, of molecules of the compound.

23. Do Now: Copy this into your notes
_______________ F. _____________

24. Do now
Explain why coefficients are needed in a chemical equation.

25. Balancing Chemical Equations
Because of the law of the conservation of matter (matter can not be created or destroyed) an equation must be balanced.
It must have the same number of atoms of the same kind on both sides.

26. Balance this equation! Na-1 Na-1 Cl-2 Cl-1 Na + Cl2 NaCl
Balance this equation!
Na + Cl NaCl
Na Na-1
Cl Cl-1
**note that the number of sodium atoms balance but the chlorine does not. We will have to use coefficients in order to balance this equation.

27. Do Now
Balance this equation
____ N2 + ____ F2  ____ NF3

29. Try this one
____ Na3PO4 + ____ KOH  ____ NaOH + ____ K3PO4

30. Do Now
Describe some pieces of evidence that would indicate a chemical reaction has taken place.

31. Types of Reactions: Single Replacement
A + BC B AC
Zn + 2HCl H ZnCl2
2Al + 3CuCl2 3Cu AlCl3

32. Types of Reactions: Double Replacement
AB + CD AD CB
Ag(NO3) + NaCl AgCl + Na(NO3)
2Ag(NO3) + K2(CrO4) Ag2(CrO4) + 2K(NO3)

33. Types of Reactions: Decomposition
AB A B
C12H22O C H2O

34. Types of Reactions: Synthesis
A + B AB
2Mg + O MgO

35. Exit Card: Classify Each Reaction

36. DO NOW Define an endothermic and exothermic reaction
A reaction that absorbs heat is called endothermic.
A reaction that releases heat is called exothermic.
An Endothermic reaction feels cold (because it is absorbing your heat)
An Exothermic reaction feels hot. (because it is giving off heat)

37. Do Now:
Describe the difference between an ionic and a covalent bond

38. Covalent Bonds A bond between two nonmetals.
Electrons are shared instead of transferred to make the compound stable.
ex: H + H  H2

39. Covalent Bonding
Remember that ionic compounds transfer electrons in order to attain a noble gas electron configuration
Covalent compounds form by sharing electrons to attain a noble gas electron configuration
Regardless of the type of bond, the Octet Rule still must be obeyed (8 valence electrons)

40. Single Covalent Bond
A Single Covalent Bond consists of two atoms held together by sharing 1 pair of electrons (2 e-)

41. Electron Dot Structure

42. Shared versus Unshared Electrons
A Shared Pair is a pair of valence electrons that is shared between atoms
An Unshared Pair is a pair of valence electrons that is not shared between atoms

43. Do Now Take out your homework Compare your answers to your partner’s.
Be prepared to share your answer on the board

44. Double Covalent Bonds
Sometimes atoms attain noble gas configuration by sharing 2 or 3 pairs of electrons
A Double Covalent Bond is a bond that involves 2 shared pairs of electrons (4 e-)

45. Triple Covalent Bond
A Triple Covalent Bond is a bond that involves 3 shared pairs of electrons (6 e-)

46. Covalent Bonds

47. Do Now Define the rule of octet
State how many bonds each atom can form
Oxygen, Sulfur, Nitrogen, Carbon, Chlorine, Phosphorus, Hydrogen, Fluorine, (hint) draw dot structures)

48. Naming Guidelines – PBr5
Name of first element (phosphorus)
Prefix needed if more than one atom
Name of second element (Bromine)
Prefix needed, even if 1 (mono)
Root name plus –ide (pentabromide)
PBr5 is phosphorus pentabromide

49. Possible Prefixes One is Two is Three is Four is Five is Six is
Seven is
Eight is
Nine is
Ten is
Mono-
Di-
Tri-
Tetra-
Penta-
Hexa-
Hepta-
Octa-
Nona-
Deca-

50. Name Covalent Compounds
SO2
SO4
SF6
NI3
P2O5
CCl4
Carbon monoxide
Carbon dioxide
Sulfur dioxide
Sulfur tetraoxide
Sulfur hexafluoride
Nitrogen triiodide
Diphosphorus pentoxide
Carbon tetrachloride

51. Endothermic/exothermic Reactions
A reaction that releases heat as it happens is called Exothermic.
A reaction that absorbs heat is called Endothermic.
An Endothermic reaction feels cold (because it is absorbing your heat)
An Exothermic reaction feels hot. (because it is giving off heat)