Chapter 3

Slide 1: Chapter 3 Substances are made of atoms

Slide 2: Natural Philosophy Heraclitus versus Parmenides  Heraclitus – everything is in the  process of change  Parmenides – Change is impossible

Slide 3: Natural Philosophy In 400 BCE, Democritus stated, All  matter consists of tiny particles called átomos, which are not created and cannot be destroyed.  This was the beginning of the atomism.

Slide 4: Natural Philosophy The fight wasn’t over. Plato disagreed.   He thought that the beauty of the world had to be caused by more than mere atoms.  He proposed a system of changing elements; water, fire, earth, air.

Slide 5: Natural Philosophy Aristotle disagreed with both  Democritus and Plato. He proposed a system called Hylomorphism. Hylomorphism is a system of ever  changing states of matter.

Slide 6: Natural Philosophy Atomism was lost until the 16th Century   Though it was still not a hard science, it was part of a belief system called alchemy.  Thankfully, Robert Boyle put an end to the mess when he wrote The Skeptical Chemyst.

Slide 7: “Nature works by means of bodies unseen.” Lucretius

Slide 8: The Elements

Slide 10: Atomic Theory Three laws provide supporting  evidence of atoms. Law of Definite Proportions – Law of Conservation of Mass – Law of Multiple Proportions –

Slide 11: Law of Definite Proportions  Every compound is composed of specific elements and whole- number ratios of those elements. Water H20 - 2 Hydrogen: 1 Oxygen

Slide 12: Law of Conservation of Mass  Matter cannot be create or destroyed by normal physical or chemical processes  i.e.- What goes in, must come out!

Slide 14: Law of Multiple Proportions  The same elements can bond in differing whole-number ratios to form different compounds. Methanol CH3O Ethanol C2H5O

Slide 16: Dalton’s Atomic Theory It contained five principles based on  current knowledge of atoms. We have summarized those principles  in the following statements:

Slide 17: Dalton’s Atomic Theory All matter is made up of tiny 1. indestructible particles called atoms. All atoms of one type (element) have 3. the same mass and properties. Atoms of different types (elements) 5. have different masses and properties.

Slide 18: Dalton’s Atomic Theory In Chemical reactions, atoms 1. rearrange, but are not changed, created, or destroyed. When different elements combine, 3. they do so in some ratio of whole numbers.

Slide 19: Chapter 3 Structure of Atoms

Slide 20: Atomic dessert In 1897 J.J. Thomson was able to control  light in a vacuum through the use of magnets. He concluded that the charge of the  beam was negative. He also new that the charge was due to  movement of something inside atoms He concluded that atoms contain  subatomic particles with + and - charges.

Slide 22: Atomic Dessert He created the  “plum pudding” model of the atom The Atom was a big  positive charge, with very small particles of negative charges embedded in it.

Slide 24: Radioactive Man In 1907, Ernest  Rutherford performed “The Gold Foil Experiment”

Slide 25: Radioactive Man Conclusion: Atoms have a hard, positively  charged center called a nucleus. The center was packed with tiny particles called  PROTONS. Most of the atom is empty space, while the tiny,  tiny electrons float around outside.

Slide 28: Subatomic Particles ATOM ATOM NUCLEUS ELECTRONS NUCLEUS ELECTRONS PROTONS NEUTRONS N E G A T I V E CHARGE NEGATIVE C H A R G E NEUTRONS PROTONS P O S IT IV E NEUTRAL POSITIVE NEUTRAL CHARGE CHARGE CHARGE CHARGE equal in a Atomic Number neutral atom equals the # of...

Slide 29: Elephants and Fleas Today, we believe that the atom has three subatomic parts: PROTON – positive charge in the nucleus NEUTRON – no charge in the nucleus ELECTRON – negative charge, orbiting the nucleus

Slide 30: Elephants and Fleas Atomic Number – number of protons   Atomic Mass – number of protons + number of neutrons Why aren’t electrons added into the  mass of the atom?

Slide 31: Isotopes ISOTOPE - atoms of the same element  that have a different number of neutrons  This happens rather frequently, that is why the atomic mass on the periodic table is not a whole number. It is an average of the different isotopes for that element.

Slide 32: Chapter 3 Electron Configurations

Slide 33: The not so great “greats” Dalton, Thomson, and Rutherford were  great men of science, but they had yet to understand the atom.  It wasn’t until Niels Bohr began to think about Hydrogen that were started to understand how complex an atom really is.

Slide 36: Bohr: What is it good for?! Bohr, using a technique called Line  Emission Spectrums, saw that electron didn’t just fly randomly around the nucleus. In fact, they are in distinct orbits called ENERGY LEVELS.

Slide 38: Bohr: What is it good for?! If you put energy into an electron, it will  change energy level into an EXCITED STATE. It will eventually drop back down to it’s GROUND STATE and give off energy in the form of light.

Slide 40: The colors of chemistry Electromagnetic Spectrum – radiation  moving at the speed of light ranging from low-energy radio waves to high- energy cosmic rays; includes visible light  It is often referred to as “light”  The spectrum is created by the “jumping” of electrons between orbits

Slide 41: Visible Spectrum The more energy a wave has, the  higher the frequency  Red has the lowest frequency, therefore it has the lowest energy  The most energetic color is violet  ROY G BIV

Slide 42: Electrons are wavicles. Bohr model of the atom shows  electrons orbiting a nucleus. Electrons are particles – When we attempt to observe an  electron, it changes position Electrons are waves –

Slide 43: De Broglie to the rescue In 1924, Louis De  Broglie suggested that electrons do not travel in perfect orbits, but rather in orbitals. The resulting image  was an “electron cloud.”

Slide 45: Electron Configuration Rules Take notes on Hog Hilton and work on  board.