Chap._2-Atoms_and_Elements

Chap._2-Atoms_and_Elements - Atoms and Elements Chapter 2...

Info iconThis preview shows pages 1–10. Sign up to view the full content.

View Full Document Right Arrow Icon
Atoms and Elements Chapter 2
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Chapter 2 Topics Atomic Theory Nature of matter. Structure of the Atom Electrons, Protons and Neutrons. Periodic Table Atomic Mass Mole Concept
Background image of page 2
Law of the Conservation of Matter Mass is conserved in chemical changes. Mass is neither created nor destroyed in chemical reactions. Reactant mass equals product mass (plus unchanged reactants). Mass in equals mass out. Antoine Lavoisier 1789
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Law of Definite Proportions A pure chemical substance will always contain the same elements in the same relative amounts. Different samples of the same compound have the same mass ratios of constituent elements. Chemical compounds contain specific proportions of elements. Not random. Joseph Proust 1799
Background image of page 4
Law of Multiple Proportions If two elements form more than one compound between them, then the ratios of the masses of the second element which combine with a fixed mass of the first element will be ratios of small whole numbers. Different compounds of the same elements have different ratios of the elements John Dalton 1803
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Dalton’s Atomic Theory The smallest identifiable unit of an element is an atom. Each element has a unique atomic mass. Different elements have atoms with different masses. Not true. Instead each element has a unique number of protons. Elements combine in small whole number ratios to make different substances. In a chemical reaction atoms are unchanged. They are only rearranged. John Dalton 1808
Background image of page 6
Structure of the Atom: Electrons J. J. Thompson: Cathode Ray Experiment Thompson proposed: Tiny negatively charged particles called electrons. Electrons are common to all elements. Thompson calculated charge/ mass ratio for the electron.
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Structure of the Atom: Electrons R. Millikan: Oil Drop Experiment Calculated the mass and charge of an electron.
Background image of page 8
Structure of the Atom: Electrons Charge: - 1.60 x 10 - 19 C (coulombs) Mass: 9.109 x 10 - 28 g Electrons occupy the outer portions of the atom.
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 10
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 02/19/2009 for the course CHEM 101 taught by Professor Rillings during the Spring '06 term at Clemson.

Page1 / 39

Chap._2-Atoms_and_Elements - Atoms and Elements Chapter 2...

This preview shows document pages 1 - 10. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online