CH 111:Inorganic Chemistry I

Module 1: Fundamentals of Chemistry (Part 2)

Textbook chapters: 1.3-1.9

The Greeks

Elements: fire, earth, water, air

Matter is

Continuous & infinitely divisible?

Composed of ultimate particles?

The Alchemists

Fake Alchemists: obsessed with turning metal to gold

Real Alchemists (scientists): discovered several elements & learned how to prepare mineral acids

Nicholas Flamel: famed Alchemist

Robert Boyle (1627-1691)

Boyles Law: 11 = 22

Boyles definition of an element: cannot be broken down into 2 or more simpler substance

Boyles mistake: Metals are not true elements; they can be changed from one metal to another

Combustion

Georg Stahl (1660-1734)

Phlogiston from burning metal stopped combustion

Joseph Priestly (1733-1804)

Discovered oxygen

Determined that oxygen sustains combustion

Note:

1. Oxygen was first discovered by Karl Scheele (1742-1786) but was late to publish

2. Oxygen was originally known as dephlogisticated air

Combustion & The Law of Conservation of Mass

Antoine Lavoisier (1743-1794) Explained the true nature of combustion

Named Oxygen (Oxygen from French oxygne meaning generator of acid) Combustion involved Oxygen and not Phlogiston

Law of Conservation of Mass Mass is neither created nor destroyed in a chemical reaction

Law of Definite Proportion

Joseph Proust (1754-1826) Copper Carbonate

5.3 parts copper, 4 parts oxygen ad 1 part carbon by mass

Law of Definite Proportion Originally called Proust

Law

A given compound always contains exactly the same proportion of elements by mass

Law of Multiple Proportions John Dalton (1766-1844)

Atoms as particles that compose elements Hypothesis: each element consisted a

certain type of atom and compounds were formed from specific combinations of atoms

Law of Multiple Proportions When two elements form a series of

compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole number ratios

Mass of Oxygen That Combines with 1 g of Carbon

Compound I 1.33 g

Compound II 2.66 g

Example: Law of Multiple Proportions

Hydrazine, Ammonia and Hydrogen azide all contain only nitrogen and hydrogen. Show how these data illustrate the Law of Multiple Proportions

Mass of Hydrogen That Contains 1 g of Nitrogen

Hydrazine 1.44 x 10^-1 g

Ammonia 2.16 x 10^-1 g

Hydrogen azide 2.40 x 10 ^-2 g

Daltons Atomic Theory

1. Each element is made up of tiny particles called atoms

2. Atoms of a given element are identical; atoms of different elements are different

3. Chemical compounds are formed when atoms of different elements combine with each other; a given compound always has the same relative numbers and types of atoms

4. Chemical Reactions involve reorganization of the atomschanges in the way they are bound together. The atoms themselves are not changed in a chemical reaction.

Joseph Gay-Lussac (1778-1850)

Gas volume experiments

Amadeo Avogadro (1776-1856)

Avogadros Hypothesis: at the same T & P, equal volumes of different gases contain the same number of particles

Jns Jakob Berzelius (1779-1848)

Discovered cerium, selenium, silicon, thorium

Developed modern symbols for elements

Reporting Guidelines

Groupings (to be done by the class president) Divide the whole class into 5 groups based on the order of

names on the class list (e.g. for class size of 45, first 9 in the class list is group 1)

Report (Aug. 9, 2014) Must run a maximum of 10 minutes Must be presented in a creative manner (should not be the

typical reporting style e.g. PowerPoint presentation) but must not sacrifice content

Must contain all important subtopics Must submit 5 questions about the assigned topic 1 day before

the day of reporting (Aug. 8, 2014)

Group Leader (to be elected by the group) Submit a detailed report on the contributions of each group

member

Group Reporting

Group 1: Cathode-Ray Tube Experiment J.J. Thomson Electron charge-to-mass ratio

Group 2: Millikan Experiment Robert Milikan Magnitude of the electron charge Mass of the electron

Group 3: Henri Becquerels Experiment ,

Group 4: Rutherfords Experiment Ernest Rutherford bombardment of foil

Group 5: Todays View of the Atomic Structure