1. AP Ch2: Atoms, Molecules and ions

2. History of Chemistry
400 B.C: Democritus (greek philosopher) hypothesizes that all matter is composed of tiny particles called atoms.

3. Atoms vs Hyle

4. 1500’s: Georg Bauer-Germany, develops systematic metallurgy
1500’s: Georg Bauer-Germany, develops systematic metallurgy. How to extract metals from raw ore.

5. Robert Boyle-1st true chemist
Wrote: The Skeptical Chymist
Developed P1V1 = P2V2 Boyle’s Law

6. Joseph Priestly
1700’s: English clergyman discovers oxygen!

7. Priestly ROCKS!

8. Antoine Lavoisier
1700’s: French chemist, uses combustion reaction to verify the law of conservation of mass, mass cannot be created nor destroyed by ordinary chemical reactions.

9. Joseph Proust Proust’s Law: “The Law of Definite Proportions:
A given compound always contains exactly the same proportions of elements by mass”
Example: CuCO3 is always 51% Cu, 10% C and
39% O, by mass.

10. John Dalton….THE MAN!

11. John Dalton 1
Formulates the law of multiple proportions: Elements can combine to form a series of compounds.
Example: N2O dinitrogen monoxide
N O2 NO nitrogen monoxide NO2 nitrogen dioxide
NO1/2 cannot form

12. John Dalton 2 Formulates Atomic Theory:
Each element is made up of tiny particles called atoms.
The atoms of a given element are identical.
Chemical compounds are formed when atoms come together, in simple whole number ratios.
Chemical reactions involve the reorganization of the atoms; combined, separated or rearranged.

14. 1808: Gay-Lussac
Develops:
P1/T1 = P2/T2

15. 1903: J.J. THOMSON
Discovers the electron, using his famous Cathode Ray Tube (CRT), which turns out to be a primitive TV or computer monitor. He also calculated the charge of electron to be x 108 Coulombs per gram.

16. 1909 Millikan finds the charge of an electron.
Robert Millikan finds the charge on the electron to be -1.6 x Coulombs

17. Robert Millikan’s Oil Drop Experiment

18. CRT and TV

19. 1900’s Eugene Goldstein discovers that beams of particles travel in the opposite direction as cathode rays. These particles are protons.

20. 1911 Ernest Rutherford
Rutherford discovers the nucleus of an atom, using his famous gold foil experiment. His native New Zealand put his image on money.

21. Rutherford’s Gold Foil Experiment

22. Rutherford’s Gold Foil Experiment

23. James Chadwick
Chadwick, Rutherford’s assistant, later made the observation that when gold nuclei are radiated with alpha particles, they sometimes emit particles, which are not affected by a charge. This was the discovery of the neutron.

24. Nuclear Radiation Type symbol make-up mass penetrating power
Alpha a p+ & 2no amu low
Beta B high speed /1840 amu medium
electron
Gamma g high energy amu high
photon
Positron e beta antiparticle 1/1840 amu high

25. Penetrating Power

26. Periodic Table: The Basics

27. Classes of elements to know:
Group 1: Alkali metals
Group 2: Alkaline-earth metals
Groups 3-12: Transition Metals
B, Si, As, Te, Ge, Sb are metalloids
Group 17: Halogens
Group 18: Noble Gases
Elements #57-70: Rare-Earth Metals
Elements #89-102: Radioactive Series
*All elements with an atomic number greater than 83 and Tc have all radioactive isotopes.
**All elements on the periodic table on the wall which are outlined are synthetic.

28. Nomenclature: Naming Chemical Compounds
The types of chemical compounds you need to know for this chapter:
Covalent binary
Ionic binary
A) singlevalent cation (s-block)
B) multivalent cation (transition metal)
Ionic ternary (containing a polyatomic ion)
Ionic ternary hydrates
Acids

30. Binary Covalent: prefix___ prefix___ + ide (2 nonmetals)
# of atoms prefix examples
1 mono- CO2
2 di- CCl4
3 tri- NO2
4 tetra- N2O5
5 pent- P2O3
6 hex- SO3
7 hept- SO2

31. Binary ionic: cation anion+ide (metal + nonmetal)
Formula Name
KCl
magnesium chloride
NaBr
lithium oxide
Al2O3
calcium sulfide
BeF2
strontium nitride
NaH

32. Ionic w/ a multi-valent(transition metal) cation
The oxidation number of the cation is always given in roman numerals, in parethesis.
Common cations to memorize:
Cr 2+ = chromium (II) aka: chromous
Cr 3+ = chromium (III) aka: chromic
Fe 2+ = iron (II) aka: ferrous
Fe 3+ = iron (III) aka: ferric
Co 2+ = cobalt (II)
Co 3+ = cobalt (III)
Ni 2+ = nickel (II)
Ni 3+ = nickel (III)
Cu + = copper (I) aka: cuprous
Cu 2+ = copper (II) aka: cupric
Sn 2+ = tin (II) aka stannous
Sn 4+ = tin (IV) aka stannic
Pb 2+ = lead (II) aka plumbous
Pb 4+ = lead (II) aka plumbic
Indicates the most common form

33. Hydrates: Name ionic compound + _______ hydrate (prefix) Example:
CuSO4 . 5 H2O copper (II) sulfate pentahydrate

34. Acids Binary acids = hydro-_____-ic acid Ternary acids(oxyacids):
Name anion, ite = ous acid OR
Name anion, ate = ic acid

35. POP QUIZ!!!!! Name the following compounds: Na2S Fe(NO3)3
Mg(C2H3O2)2 NH4NO2
K2CO3 S2O5
CuCl Zn(ClO3)2
CuCl2 Zn(ClO4)2
CuCl2.3H2O Zn(ClO2)2
H2CO3 Zn(ClO)2
N2O3 HCl
HClO2 HClO4
HClO3

36. END OF CHAPTER 2