1. Metric Conversions king henry died by drinking chocolate milk
k h da b d c m
king henry died by drinking chocolate milk
k h da base d c m

2. Metric System Conversions
Example: cm= _____________ km

3. TRY THIS:
1000 mg = ______ g 1

4. TRY THIS:
0.15 m = __________ mm
150

5. TRY THIS:
kg = __________ cg
6400

6. TRY THIS:
89 ds = __________ das
0.89

7. What is density? m ÷
ALWAYS REMEMBER UNITS! × D V

8. Let’s try a density problem together
Frank’s paper clip has a mass of 9 g and a volume of 3 mL. What is its density?
Density = Mass  Volume
Density = 9 g  3 mL = 3 g/mL
9 g
= 3 g
3 mL mL m ÷ × D V

9. Let’s try a density problem together
Frank’s eraser has a density of 6 g/mL and a volume of 2 mL. What is its mass?
Mass = Density × Volume
Mass = 6g/mL × 2mL = 12g
6 g
x 2 mL
= 12 g mL m ÷ × D V

10. Let’s try a density problem together
Frank’s shot-put has a mass of 500 g and a density of 100 g/mL. What is its volume?
Volume = Mass  Density
Volume = 500 g  100 g/mL
= 5 mL m ÷ × D V

11. Significant Figures 56,400,000 Is there a decimal? PACIFIC (Present)
ATLANTIC (Absent)
Start from LEFT & count all #s from first nonzero
Start from RIGHT & count all #s from first nonzero
56,400,000
4 sig figs
3 sig figs

12. You Try! How many sig figs in the following: Examples: a) 1001 km
b) m
c) 129,870 m
d) km
e) L
f) 6.02 x 1023 atoms
g) 20,000 cm
h) g
Number of Significant Figures:
a) 4
b) 4
c) 5
d) 1
e) 4
f) 3
g) 1
h) 2

13. CALCULATIONS WITH SIG FIGS Summary
Multiplying or dividing: round to the measurement with the smallest number of significant figures.
2.6 cm x 3.78 cm = cm2
Adding or subtracting: round the answer to the smallest number of decimal places.
165.5 cm + 8 cm cm = cm
= 9.8 cm2
= 178 cm

14. PARTS OF THE ATOM Nucleus: Contains protons and neutrons VERY tiny
Contains all the atom’s mass
Electron Cloud:
Contains electrons
Makes up the atom’s volume
No mass

15. Isotope Naming

16. Electron Configurations7p

17. Electron Configurations
Electrons fill sublevels in the order on the chart.
Read it like a book – from left to right. Every sublevel to the left and above is filled.
Boron (B)
1s22s22p1
Oxygen (O)
1s22s22p4 7p

18. Electron Configurations
Electrons fill sublevels in the order on the chart.
Read it like a book – from left to right. Every sublevel to the left and above is filled.
Silicon (Si)
1s22s22p63s23p2
Gallium (Ga)
1s22s22p63s23p64s23d104p1 7p

19. 2A: Alkaline Earth Metals
Periodic Table
ROWS: Periods
COLUMNS: Families or Groups
8A: Noble Gases
1A: Alkali Metals
7A: Halogens
2A: Alkaline Earth Metals

20. Trends in Electronegativity
Ability of an atom to attract electrons in another atom *
Fluorine has the highest electronegativity,
Noble gases have ZERO electronegativity

21. Trends in Ionization Energy
The energy required to remove an electron from an atom

22. Trends in Atomic Size
Atomic Size
The distance between the nucleus and the outer edge of the electron cloud

23. Ionic Bonds – electrons transferred
Metals lose electrons and
Nonmetals gain electrons to form an ionic bond.
Properties of Ionic Compounds
Crystal lattice structure
High melting points
Conducts electricity when melted or dissolved in water

24. Predicting Ionic Charges
Group 1A:
Lose 1 electron to form 1+ ions H+
Li+
Na+ K+
Rb+

25. Predicting Ionic Charges
Group 2A:
Loses 2 electrons to form 2+ ions
Be2+
Mg2+
Ca2+
Sr2+
Ba2+

26. Predicting Ionic Charges
Loses 3
electrons to form
3+ ions
Group 3A:
B3+
Al3+
Ga3+

27. Predicting Ionic Charges
Neither! Group 4A elements rarely form ions
EXCEPTION: Sn and Pb!! Treat like transition metals
Do they lose 4 electrons or gain 4 electrons?
Group 4A:

28. Predicting Ionic Charges
Nitride
Gains 3
electrons to form
3- ions
Group 5A:
P3-
Phosphide
As3-
Arsenide

29. Predicting Ionic Charges
Oxide
Gains 2
electrons to form
2- ions
Group 6A:
S2-
Sulfide
Se2-
Selenide

30. Predicting Ionic Charges
Gains 1 electron to form
1- ions
Group 7A:
F1-
Fluoride
Br1-
Bromide
Cl1-
Chloride
I1-
Iodide

31. Predicting Ionic Charges
Stable noble gases do not form ions!
Group 8A:

32. Covalent Bonds – electrons shared
Bond between two nonmetals.
Properties of Covalent Compounds
Lower melting points
Does not conduct electricity when dissolved in water

33. Metallic Bonds – “sea” of electrons
Bond between two metals.
Bond is the attraction between electrons and positive nucleus.
Properties of Metallic Compounds
Malleable (pounded into shapes)
Ductile (pulled into wires)
Conducts electricity as a solid.

34. NAMING COMPOUNDS Use roman numerals for transition metals
IONIC COMPOUNDS:
Name the CATION then the ANION
Use roman numerals for transition metals
Example: Cu(NO3)2
copper (II) nitrate
COVALENT COMPOUNDS (molecules):
Use prefixes to match the subscript.
Second atom name ends in “ide”
Example: N2O4
dinitrogen tetroxide

35. WRITING FORMULAS Example: iron (II) chloride Fe2+ Cl- Fe 1 Cl 2 FeCl2
IONIC COMPOUNDS:
USE THE CROSS RULE:
Example: iron (II) chloride
Fe2+ Cl-
Fe 1 Cl 2
FeCl2
COVALENT COMPOUNDS (molecules):
Use prefixes to identify the subscripts.
Example: trichloro tetrafluoride
Cl3F4

36. Lewis Structure of Molecules
Add up all the valence electrons. This is the number of dots in the final structure.
Place least electronegative element in center. (Never H)
Place two electrons between central and outer atoms
Fill up outer atom octets.
Fill up central atom octet.
Make double or triple bonds if necessary so all atoms meet the octet rule.
Br2
2(7) = 14

37. Lewis Structure of Molecules
Add up all the valence electrons. This is the number of dots in the final structure.
Place least electronegative element in center. (Never H)
Place two electrons between central and outer atoms
Fill up outer atom octets.
Fill up central atom octet.
Make double or triple bonds if necessary so all atoms meet the octet rule.
H2O
6 + 2(1) = 8

38. Lewis Structure of Molecules
Add up all the valence electrons. This is the number of dots in the final structure.
Place least electronegative element in center. (Never H)
Place two electrons between central and outer atoms
Fill up outer atom octets.
Fill up central atom octet.
Make double or triple bonds if necessary so all atoms meet the octet rule.
CO2
4 + 2(6) = 16

39. Balancing Reactions
Balance reactions so that the same number of atoms are on both sides.
ONLY change coefficients, NOT subscripts.
_____C3H ____O2  ____CO ____H2O
____ Pb(NO3) ____ HCl  ____ PbCl ____ HNO3
Balance in the following order
Polyatomic ions (as a group, only if they appear on both sides)
Metals
Nonmetals
Hydrogen
5.Oxygen

40. Calculating Percent Composition Example
Determine the percent composition of each element in Mg(NO3)2
Determine the contribution of each element
Molar mass
On a per mol basis

41. Mole Conversions 1 mole = 6.02  1023 particles 1 mole = _______ g
*particles could be molecules, ions, atoms, formula units
1 mole = _______ g
*1 mole equals the molar mass of the atom or compound
1 mole = 22.4 L
* for gases only at STP (Standard Temperature (0˚C and Standard Pressure (1 atm))

42. Mole Conversions a. What is the number of moles of CaS in 120 g?
1 mole =72.2 g CaS
= 1.7 moles
120 g CaS
1 mole
72.2 g CaS
b. What is the mass in grams of 1.81 x 1023 molecules of CO2?
1 mole =6.02  1023 particles, 1 mole =44.0 g CO2
= 13.2 g
1.81 x molecules CO2
1 mole
72.2 g CO2
6.02 x molecules

43. Mole Conversions c. How many molecules of CO2 are in 0.50 moles?
1 mole = 6.02  1023 particles
= 3.01x1023 molecules
0.50 moles CO2
1 mole
6.02 x molecules
d. How many liters do 7.87×1023 molecules of H2S occupy at STP?
1 mole =6.02  1023 particles, 1 mole =22.4 L at STP
= 29.3 L
7.87 x molecules CO2
1 mole
22.4 L
6.02 x molecules

44. Mole Conversions
e. What is the number of liters that 27 g of oxygen gas occupies at STP?
1 mole =32.0 g O2, 1 mole =22.4 L at STP
= 18.9 L
27 g O2
1 mole
22.4 L
32 g O2

45. Stoichiometry Calculations
Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g)
38a. How many moles of H2 if 4 moles of HCl react?
CONVERSION FACTOR:
mole ratio: ___ mole _____ = ___ mole ______
2 mol HCl = 1 mol H2
4 mol HCl
1 mol H2
= 2 mol H2
2 mol HCl

46. Stoichiometry Calculations
Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g)
38b. How many grams of Zn if 3 moles of ZnCl2 are formed?
CONVERSION FACTORS:
mole ratio: ___ mole _____ = ___ mole ______
molar mass: 1 mole ____ = _____ g ______
1 mol Zn = 1 mol ZnCl2
1 mol Zn = g Zn
3 mol ZnCl2
1 mol Zn
65.34 g Zn
= g Zn
1 mol ZnCl2

47. Stoichiometry Calculations
Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g)
38c. How many grams of HCl if 6.87 g Zn react?
CONVERSION FACTORS:
mole ratio: ___ mole _____ = ___ mole ______
molar mass: 1 mole ____ = _____ g ______
1 mol Zn = 2 mol HCl
1 mol Zn = g Zn
1 mol HCl = g HCl
6.87 g Zn
1 mol Zn
2 mol HCl
36.45 g HCl
= 7.7 g HCl
65.34 g Zn
1 mol HCl

48. Stoichiometry Calculations
Mg + 2 HNO3  Mg(NO3)2 + H2
39a. If 40 g Mg react, how many grams H2 form?
CONVERSION FACTORS:
mole ratio: ___ mole _____ = ___ mole ______
molar mass: 1 mole ____ = _____ g ______
1 mol Mg = 1 mol H2
1 mol Mg = 24.3 g Zn
1 mol H2 = 2.0 g H2
40 g Mg
1 mol Mg
1 mol H2
2.0 g H2
= 3.3 g H2
24.3 g Mg

49. Stoichiometry Calculations
Mg + 2 HNO3  Mg(NO3)2 + H2
39b. If 1.7 g H2 was ACTUALLY produced, what was the percent yield?
Actual Yield: Given in problem (1.7 g H2)
Theoretical Yield: Calculated in part a (3.3 g H2)

50. Stoichiometry Calculations
Mg + 2 HCl  ZnCl2 + H2
40a. If 40 g Zn and 40 g HCl react, how many grams H2 form?
This is a limiting reactant problem. Do 2 calculations.
CONVERSION FACTORS:
mole ratio: ___ mole _____ = ___ mole ______
molar mass: 1 mole ____ = _____ g ______
First Calculation:
1 mol Zn = 1 mol H2
1 mol Zn = 65.4 g Zn
1 mol H2 = 2.0 g H2
40 g Zn
1 mol Zn
1 mol H2
2.0 g H2
= g H2
65.4 g Zn

51. Stoichiometry Calculations
Mg + 2 HCl  ZnCl2 + H2
40a. If 40 g Zn and 40 g HCl react, how many grams H2 form?
This is a limiting reactant problem. Do 2 calculations.
CONVERSION FACTORS:
mole ratio: ___ mole _____ = ___ mole ______
molar mass: 1 mole ____ = _____ g ______
Second Calculation:
2 mol HCl = 1 mol H2
1 mol HCl = 35.5 g HCl
1 mol H2 = 2.0 g H2
40 g HCl
1 mol HCl
1 mol H2
2.0 g H2
= g H2
36.5 g HCl

52. Stoichiometry Calculations
Mg + 2 HCl  ZnCl2 + H2
40b. If 40 g Zn and 40 g HCl react, how many grams H2 form?
What is the limiting reactant?
First Calculation (Zn is reactant): Produced 1.22 g H2.
Second Calculation (HCl is reactant): Produced 1.10 g H2.
HCl produced the LEAST amount of product so it is the limiting reactant. You can only produce 1.10 g H2.