Chapter 4. Atomic Structure
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1 Chapter 4 Atomic Structure
2 Warm Up We have not yet discussed this material, but what do you know already?? What is an atom? What are electron, neutrons, and protons? Draw a picture of an atom from what you know today.
3 History of the Atom 1. Democritus vs. Aristotle pg John Dalton and conservation of mass pg Cathode ray tube and Sir William Crookes pg Mass and charge of electron (J.J. Thompson) and oil drop experiment pg Plum pudding model vs. Rutherford s experiment pg
4 Democritus Greek philosopher who asked questions about matter. Can you divide matter infinitely? Democritus says no! Tiny particles called atoms, indivisible! Matter is composed of atoms, which move through empty space. Atoms are solid homogeneous, indestructible, and indivisible. Atoms have different sizes and shapes. These properties, and movement determine properties of matter
5 John Dalton Matter is composed of small particles called atoms that are indivisible and indestructible. Atoms of a given element are identical in size, mass, and chemical properties, and are different from those of another element. Different atoms combine in simple whole number ratios to form compounds. In a chemical reaction, atoms are separated, combined or rearranged.
6 Dalton s Inaccuracies Atoms are not the smallest type of matter! Subatomic particles electrons, protons, and neutrons Atoms of the same element can have slightly different masses! - isotopes
7 The Atom EXTREMELY small particle of an element that retains the properties of that element is an atom. If atom is the size of an orange, an orange would be the size of the EARTH
8 Subatomic Particles - Electron Cathode Ray Tube Thin beam of electrons travels from cathode to anode! Cathode rays are a Cathode Vacuum Anode stream of charged particles. Particles carry a negative charge now called electrons!
9 J.J. Thompson Determined that the mass of the charged particle (electron) was much less than that of the hydrogen atom. Dalton was WRONG about the atom being the smallest particle!
10 Millikan Oil-Drop Experiment Determined the charge of an electron. Charge up the oil particles with electrons. Change the electric field changes the rate of oil droplets! Charge of electron x coulombs Mass of electron = 9.1 x grams
11 Plum Pudding Model Matter isn t all negatively charged, so how do we have negatively charged subatomic particles without positively charged ones?? J.J. Thompson thought an atom was a positively charged sphere with electrons hanging out within.
12 Rutherford and the Nucleus Experiment proved that plum pudding model was incorrect! Atom is mostly empty space through which e - can move. Almost all of the positive charge and atomic mass resides in the center NUCLEUS! Nucleus is positively charged to deflect alpha particles and to balance electron charge.
13 Subatomic Particles Electron VERY tiny, negatively charged Proton located in the nucleus, charge opposite of an electron (positive!) Neutron located in the nucleus, same mass as a proton, neutral!
14 Warm Up! What experiment determined the mass and charge of an electron? Dalton concluded that the atom was the smallest particle of matter. Was he correct? What did the gold foil experiment prove?
15 Atomic Theory Today Quantum Mechanical Model All atoms are made up of electrons, protons, and neutrons. Electrons are located outside of the nucleus, protons and neutrons are located inside the nucleus. Electrons exist in a cloud surrounding the nucleus. Attracted to the nucleus so they hang around! Nucleus accounts for 99.97% of the atomic mass, and occupies a VERY small volume. A neutral atom has the same number of electrons and protons!
16 Current Atomic Model Neutral atom: # Protons = # Electrons
17 Make sure you can answer What are John Dalton s 4 theorems How does John Dalton s theory relate to conservation of mass? How was the electron discovered? Who discovered the mass of an e -? HOW? What was Rutherford s contribution? Describe the structure of the atom.
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