Warm-Up Draw a picture of an atom. Be as specific as you can!

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Presentation transcript:

Warm-Up Draw a picture of an atom. Be as specific as you can!

History of the Atom

Democritus (400 B.C.) Greek philosopher Coined the word atom, meaning indestructible Atoms are solid, homogeneous, and indivisible Different types of matter existed due to changes in the atoms that composed them Problem: what holds the atom together?

John Dalton (19th century) English schoolteacher Modern Atomic Theory: All matter is composed of atoms All atoms of the same element have identical size, mass & chemical properties Different atoms combine in specific ratios to form compounds In chemical reactions, atoms are separated, combined or rearranged

Law of Multiple Proportions 2 H2 + O2  2 H2O H2 + O2  2 H2O2

Cathode Ray Tube

Sir William Crookes (1800s) Experimented with the CRD: No charged objects  ray is straight and flows from cathode to anode Positive charge near the tube  ray is deflected toward the charge Negative charge near the tube  ray is deflected away from the charge Conclusion: particles must be negatively charged

J.J. Thomson (1890s) English physicist Used CRT to determine charge-to- mass ratio of the electron Mass was much lighter than Hydrogen, the lightest atom Conclusion: Atoms must be divisible!

Plum Pudding Model Negative electrons evenly distributed throughout a uniform positive charge “Chocolate chip cookie model”

Robert Millikan (1909) American physicist (who shares a birthday with Ms. Breeze!) Determined charge & mass of an electron: Charge = 1- Mass = 9.1 x 10-28 g = 𝟏 𝟏𝟖𝟒𝟎 mass of H atom

Ernest Rutherford (1911) Gold Foil Experiment Prediction: particles would pass straight through (almost) Results: a few particles were deflected at large angles, some even straight back towards the source!

Nuclear Atomic Model Atom is made of mostly empty space Electrons move through this Tiny, dense region in the center called the nucleus Positively charged Almost all of the atom’s mass

James Chadwick (1932) English physicist Nucleus also contains neutrons: Neutral (no charge) Same mass as a proton

Relative Electrical Charge Subatomic Particles Particle Symbol Location Relative Electrical Charge Relative Mass Actual Mass (g)

Relative Electrical Charge Subatomic Particles Particle Symbol Location Relative Electrical Charge Relative Mass Actual Mass (g) Proton p+ In the nucleus +1 1 1.673x10-24 Neutron n0 Electron e- In the space surrounding the nucleus -1 1/1840 9.11x10-28

Information found on the Periodic Table 6 C Carbon 12.011 Atomic Number = number of protons Element’s Symbol Element’s Name Atomic Mass = protons + neutrons In elemental forms, the number of protons will be the same as the number of electrons. Carbon has 6 protons, 6 electrons, and an average of 6 neutrons.