1. “What are ATOMS?”

2. Leucippus and Democritus (400? BC)
Greek philosopher and his “student”
New idea:
- there is a limit to how far matter can be divided
- atomos:
“uncuttable” particles,
different shape/size

3. Robert Boyle (1627-1691) English scientist and philosopher
Hypothesis: everything made of corpuscles (tiny particles of various sizes/shapes).

4. Thinking about Atoms…

5. Some Definitions: Matter Classification
Element:
1) A pure substance that cannot be broken down into simpler substances by a chemical reaction.
2) A substance made of unique, (nearly) identical atoms.
Compound:
1) A pure substance that can be broken down into simpler substances by a chemical reaction.
2) A substance made in a chemical reaction by combining two or more different elements.

6. Start of Modern Era of Atoms: Dalton’s Atomic Theory
John Dalton
( )
British chemist,
lecturer, and
meteorologist

7. Dalton’s Atomic Theory (1803) - 1
All matter is made up of indivisible and indestructible basic particles called atoms.
All atoms of a given element are identical, both in mass and in properties. Atoms of different elements have different masses and properties.
Compounds are formed when atoms of different elements combine in the ratio of small whole numbers.

8. Dalton’s Atomic Theory (1803) - 2
Elements and compounds are composed of definite arrangements of atoms.
Chemical change occurs when the atomic arrays are rearranged.

9. Significance of Dalton’s Atomic Theory
Broke down 18th-century view of “elements”
Bridged gap between lab data and hypothetical atom.
- way of calculating relative atomic weights.
Explained Law of Conservation of Mass
- “Initial Mass = Final Mass”
- Only reorganizing of unchangeable atoms
occurs in chemical reaction.

10. Dalton: inconsistencies uncovered…
The basic state of an element is one atom?
Perhaps… basic natural state of an
element may be a molecule made of
2 or more atoms.
2) Dalton: “Thou knows…no man can split the atom.” Not so: radioactivity.
3) Atoms of given element have same mass and properties? Not so: isotopes exist…

11. More Definitions: Molecule: Allotropes: Isotopes: (more later…)
- any combination of 2 or more atoms.
- atoms can be same or different elements.
Allotropes:
- different molecular combinations of a
single element.
Ex] oxygen as O2 or ozone O3
Isotopes: (more later…)
- atoms of same element that differ in mass only

12. Identification of Elements
Physical properties
Chemical properties
Flame test for solids/solutions
Interaction with light:
line-absorption spectrum
line-emission spectrum

13. Flame Test for Element Identification
(From left) Sodium, potassium, lithium;
strontium, barium, potassium.

14. Elements: Ages of Discovery

15. Classification of the Elements: Development of the Periodic Table
Dobereiner: “Triads”
Newlands: “Octaves”
Mendeleev:
first-published “Period” definition
Meyer:
second-published “Period” definition

16. Dobereiner’s “Law of Triads” (1817)
Organized a few elements by
similar chemical properties
Hypotheses:
- Groups of three elements (triads) existed.
- In order of increasing atomic weight,
middle element’s properties were the
average of other 2 elements’ properties.

17. Newlands’ “Law of Octaves” (1863?)
Every eighth element repeats properties of first “Octave” element
[like middle-C to high-C on piano]

18. Dmitri Mendeleev (1834-1907) “Creator of the Periodic Table”
(probably formulated
periodic idea at same
time as Meyer)

19. Mendeleev’s
early notes
for the
Periodic Table
(1869)

21. Characteristics of Mendeleev’s Table
Organized 60+ known elements…
- in families (groups) with similar properties
- by valence = “combining number”
(split out elements with multiple valence)
- roughly by atomic weight (moved 17 elements based on properties rather than weight)
Could use to predict existence of new elements
(of 10, found 7; other 3 do not exist)
NOTE: at first, no “rare gases” were classified

22. Comparison of eka-silicon’s predicted properties and known Group 4 properties
Eka: “one beyond”

23. Discovery of Atomic Structure; Sub-atomic Particles
Thomson:
electron mass-to-charge ratio
Millikan: electron charge
Rutherford:
mass and charge of nucleus
Chadwick: neutron (1932).
(Nobel prize in 1935)
Bohr: electron energy levels (Topic 7)

24. (existence of electrons)
Joseph John Thomson
( )
British physicist
and mathematician
Nobel Prize in 1906
(existence of electrons)
1897: calc’d electron’s charge-to-mass
ratio in cathode-ray tube expt.

25. Robert Millikan (1868-1953) U.S. physicist Nobel Prize in 1923
(charge of electron: 1909 oildrop expt.)
With Thomson’s
result, this allowed
calculation of
electron mass.
Millikan’s experimental apparatus.

26. New Zealander teaching
Ernest Rutherford
( )
nuclear physicist,
New Zealander teaching
in Great Britain
Nobel Prize in 1908
(radioactive decay)
Gold foil experiments

27. Rutherford’s Experiments (1910-11) (done by undergrad Ernest Marsden/physicist Hans Geiger)
Fired beam of alpha particles [He+2] at gold foil.
Most particles went straight through,
some were deflected, BUT
a few were reflected straight back to source!

28. Rutherford’s Experiments (cont.)
Rutherford’s description:
“It was about as incredible as if you had fired a 15-inch shell at a piece of paper and it came back and hit you.”
Interpretation:
gold atom has small, dense, positively-charged nucleus surrounded by “mostly empty” space
in which the electrons must exist.
Calculated nuclear mass as mass of positively-
charged protons. Protons about half of actual mass:
suggests neutral particles of same mass as proton?

29. Known Properties of Subatomic Particles
Property
Particle
Mass (amu),
Mass (g)
Relative
Charge
Electron
x 10-28
- 1
Proton
x 10-24
+ 1
Neutron
x 10-24

30. Proton/Electron Count in Atoms
Every neutral atom has an equal number of
electrons and protons.
The number of protons, or “atomic number”,
is unique for each element.
If an atom has unequal numbers of
protons and electrons, it is called an ion
(which is a charged atom).
Example] Chlorine has atomic number 17. How many
protons & electrons are in one Cl atom? How many protons
& electrons are in one Cl- (chloride ion)?

31. Neutron Count in Atoms: Isotopes
For many elements, the atoms of that specific element are only “nearly identical” to each other: the number of neutrons may vary.
The “nearly identical” forms are called isotopes.
Example:
Chlorine atoms exist in nature as a mixture of two isotopes: Cl-35 and Cl-37.
3 in four Cl atoms are Cl-35; 1 in four is Cl-37. The “atomic mass” of Cl in Table is an average.

32. Modern “Periodic Table” Organization
Elements are NOW placed in order of
increasing atomic number (# of protons).
- Why? Refer to “isotopes”:
natural weight irregularities exist
This relationship between nuclear charge and
arrangement of elements in Table was
discovered by Henry Moseley in 1914.
In 1860s, Mendeleev / Meyer could NOT have
predicted a relationship to subatomic particles!