1. A Brief History of Chemistry
Ancient Greece
~_____ BCE
____________
Atomos-_________
Thought matter was discreet

2. A Brief History of Chemistry
Aristotle
Thought matter was ________________
Credited with 4 Greek elements
Earth
Air
Fire
Water

3. A Brief History of Chemistry
The Middle Ages
________________
Europe-Convert base metals to ________
Asia- ____________

4. A Brief History of Chemistry
Robert Boyle
The Skeptical Chemist
The beginnings of chemistry as an __________________________________

5. A Brief History of Chemistry
Antoine Lavoisier
The father of modern chemistry
Law of ______________ of Mass
Helped develop the ____________________
Made first comprehensive list of _______________

6. A Brief History of Chemistry
John Dalton
_________________

7. A Brief History of Chemistry
1867
Dmitri Mendeleev
_________________

8. A Brief History of Chemistry
1897
J. J. Thomson
Discovers ______________

9. A Brief History of Chemistry
1911
Ernest Rutherford
Gold Foil Experiment
Discovered __________________
Discovered __________ in 1919
James Chadwick discovered the _______________ in 1932

10. A Brief History of Chemistry
The Manhattan Project
1940’s
The Atomic Bomb

11. The Law of Conservation of Mass
Matter is neither _________ nor _________ during chemical reactions or during physical changes.

12. The Law of Definite Proportions
A chemical compound contains the same _________ in exactly the same _________________by mass regardless of the _________ of the sample or _________ of the compound.

13. The Law of multiple Proportions
If two or more different compounds are composed of the __________________, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of __________________.

14. Dalton’s Atomic Theory
All matter is made up of _______________ called atoms.
Atoms of a given element are identical in ______, ______, and other properties.
Atoms of different elements _______ in size, mass, and other properties.

15. Dalton’s Atomic Theory
Atoms cannot be _________, _________, or _________.
Atoms of different elements can combine in simple, _________________ to form chemical compounds.

16. Dalton’s Atomic Theory
In chemical reactions (rxns), atoms are _________, _________, or _________.

17. Modern Atomic Theory
All matter is composed of __________________particles called atoms.
Atoms of the same element have the same chemical properties, while atoms of different elements have different __________________.

18. Modern Atomic Theory
While individual atoms of a given element may not all have the same _________ (due to differences in nuclear structure), any natural sample of the element will have a definite __________________that is characteristic of that element as compared to any other element.

19. Modern Atomic Theory
_________ are formed when atoms of 2 or more elements unite, with each atom losing its characteristic _________ as a result of this combination.
Atoms are not _________ in physical or chemical rxns.

20. Discovery of the Electron
1897
JJ Thomson
Cathode Ray Tube Experiment
Discovered the electron

21. Discovery of the Electron
Air was evacuated from the tube and an electric current was passed through it.
A _________was seen.
When Thomson held a magnet to the glow, it was _________________ the magnet.

22. Discovery of the Electron
This meant that the glowing field had an _________________.
Thomson had to work out whether the glow was _________________.
He placed a ________________ inside of the tube.

23. Discovery of the Electron
If the wheel moved, the glow was __________________.
If the wheel did not move, the glow was _________.
The wheel moved, so Thomson knew that ___________________________were produced by the current.

24. Mass of the electron 1909 Robert Millikan Oil Drop Experiment
Mass of electron
9.109 x 10-31kg

25. Plum Pudding Model

26. Rutherford’s Gold Foil Experiment
1911
Ernest Rutherford
Gold Foil Experiment
Discovered the atomic nucleus

28. The atom
An atom is the smallest particle of an element that retains the _______________ of that element.
The ___________ is a very small region located at the center of an atom.
The nucleus is made up of at least one positively charged particle called a ___________ and usually one or more neutral particles called ___________.

29. The atom
Surrounding the nucleus is a region occupied by negatively charged particles called ______________.
Protons, neutrons, and electrons are often referred to as _______________________.

30. Properties of Subatomic particles

31. Forces in the Nucleus
When two protons are extremely close to each other, there is a _______________ between them.
A similar attraction exists when _______ are very close to each other or when protons and neutrons are very close together.
The short-range proton-neutron, proton-proton, and neutron-neutron forces that hold the nuclear particles together are referred to as _________________.

32. Nuclear Forces

33. Atomic Number
Atoms of different elements have different numbers of __________.
Atoms of the same element all have the _______ number of protons.
The atomic number (Z) of an element is the number of _________ of each atom of that element.

34. Mass Number
The mass number is the total number of _________________ that make up the nucleus of an isotope.

35. Isotopes
Isotopes are atoms of the same element that have different __________.
The isotopes of a particular element all have the ________ of protons and electrons but _________ numbers of neutrons.
Most of the elements consist of ________ of isotopes.

36. Relative Atomic Mass
The standard used by scientists to compare units of atomic mass is the ______________ atom, which has been arbitrarily assigned a mass of exactly 12 atomic mass units, or 12 amu.
One __________________, or 1 _____, is exactly 1/12 the mass of a carbon-12 atom.
The atomic mass of any atom is determined by comparing it with the mass of the ___________ atom.

37. Average Atomic Mass
Average atomic mass is the weighted average of the atomic masses of the naturally occurring _________ of an element.
Calculating Average Atomic Mass
The average atomic mass of an element depends on both the _______ and the ___________________of each of the element’s isotopes.

38. The mole
A mole (abbreviated mol) is the amount of a substance that contains as many particles as there are atoms in exactly _______ of carbon-12.
The mole is the SI unit for amount of ___________.
Avogadro’s number— × 1023—is the number of particles in ___________ of a pure substance.

39. Molar Mass
The mass of __________ of a pure substance is called the molar mass of that substance.
Molar mass is usually written in units of _______.
The molar mass of an element is numerically equal to the atomic mass of the element in _________________.

40. Molar Conversions
What is the mass in grams of 3.50 mol of the element copper, Cu?

41. Molar Conversions
How many moles of silver, Ag, are in  1023 atoms of silver?