1 / 11

The History of Chemistry

Law of Conservation of Matter: states that mass can neither be created or destroyed during a chemical reaction. The History of Chemistry. About 960 BCE- the Chinese monk Li Tian invented gunpowder (saltpeter- potassium nitrate, sulfur and charcoal)

levi
Download Presentation

The History of Chemistry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Law of Conservation of Matter: states that mass can neither be created or destroyed during a chemical reaction

  2. The History of Chemistry About 960 BCE- the Chinesemonk Li Tian invented gunpowder (saltpeter- potassium nitrate, sulfur and charcoal) which also brought about the invention of fireworks Democritus (465 BCE)First to propose that matter exists in the form of particles. Coined the term 'atoms'. Aristotle (348- 315 BCE) Established the subject of science in his school- thought matter was composed of earth, water, air and fire- these were the 4 elements that made up everything- his knowledge was renowned and respected for over a 1000 years Alchemistry ( 1000 to 1650 CE) A group of individuals throughout the world that would try to convert common elements into gold 1100 CE- Evidence of a loadstone used in a compass Boyle, Sir Robert (1637-1691)Formulated the fundamental gas laws. First to propose the combination of small particles to form molecules. Differentiated between compounds and mixtures. Priestley, Joseph (1733-1804)Discovered oxygen, carbon monoxide, and nitrous oxide. Proposed electrical inverse-square law (1767). Lavoisier, A.L. (1743-1794)Discovered nitrogen. Described the composition of many organic compounds. Sometimes regarded as the Father of

  3. Elements , Atomic Structure and the Periodic Table Mass number: the atomic mass rounded to a whole number- also the sum of protons + neutrons Elements are made up of atoms- atoms are composed of protons, neutrons and electrons

  4. Avogadro, Amedeo (1776-1856)Proposed principle that equal volumes of gases contain the same number of molecules. Gay-Lussac, J.L. (1778-1850)Discovered boron and iodine. Discovered acid-base indicators (litmus). Improved method for making sulfuric acid. Researched behavior of gases. Mendeléev, Dmitri (1834-1907)Discovered periodicity of the elements. Compiled the first Periodic Table with elements arranged into 7 groups (1869). Le Chatelier, H.L. (1850-1936)Fundamental research on equilibrium reactions (Le Chatelier’s Law), combustion of gases, and iron and steel metallurgy. Thomson, Sir J.J. (1856-1940)Research on cathode rays proved existence of electrons (1896). Nobel Prize in 1906 Rutherford, Sir Ernest (1871-1937)Discovered that uranium radiation is composed of positively charged 'alpha' particles and negatively charged 'beta' particles (1989/1899). First to prove radioactive decay of heavy elements and to perform a transmutation reaction (1919). Discovered half-life of radioactive elements. Established that the nucleus was small, dense, and positively charged. Assumed that electrons were outside the nucleus. Nobel Prize in 1908.

  5. Isotopes: Atoms of the same element with different number of neutrons- some can be radioactive Calculating average atomic mass (weighted average): BoronB(10) 10.012938 19.80B(11) 11.009305 80.20

  6. CH 24 Nuclear Chemistry History- Curie, Marie (1867-1934) With Pierre Curie, discovered and isolated radium and polonium (1898). Studied radioactivity of uranium. Nobel Prize in 1903 (with Becquerel) in physics; in chemistry 1911. Roentgen, Wilhelm (1895)Discovered that certain chemicals near a cathode ray tube glowed. Found highly-penetrating rays that were not deflected by a magnetic field, which he named 'x-rays'. Becquerel,Henri (1896)While studying effects of x-rays on photographic film,he discovered that some chemicals spontaneously decompose and emit very penetrating rays.

  7. Radioactive Decay: radioactive elements and radioisotopes are unstable and will emit radiation to form a more stable atom Elements with 82 protons or more are radioactive

  8. Half- Life:is what radioactive decay is measured inand is the time required for one half of the radioactive isotope’s nuclei to decay into it’s products. • Carbon 14’s half-life is 5730 years. If a bone which originally had 36 g of C-14 was found with 9g of C-14 remaining, how old is the bone?

  9. Uses and Concerns of nuclear reactionz • Used as an energy source- nuclear reactors use fission • Used in weapons • Used in medicine for both diagnostic and to kill cancerous tumors • Used to date objects • Radioactive material never goes away it will always be here • Radioactivity can cause cancer and death not just in humans but any living thing

  10. Definition-a pure substance made up of 2 or more chemically combined elements Law of Definite Proportion: states that a compound is always composed of the same elements in the same proportion by mass, no matter the size of the sample ex: water is always H2O Law of Multiple Proportions: states that when different compounds are formed by a combination of the same elements, different masses of one element in a ratio of small whole numbers ex: H2O is water H2O2 is hydrogen peroxide Formula and what it tells you: the elements in the combined and the atom to atom ratio Hydrates: A compound that has a specific number water molecules bound to its atoms Determining Formula Mass What is the formula mass of table sugar? C12H22O11 Calculating % by mass A 28.0 g sample of nitrogen gas combines completely with 6.0 g of hydrogen gas to form ammonia. What is the mass of ammonia? If 3.5 g of element X reacts with 10.5g of element Y to form the compound XY, what is the percent by mass of each element? Compounds

More Related