8.5 Atomic Structure
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1 Views of the Atom Democritus (Greek philosopher from 460 BC to 370 BC) Believed that atoms were indivisible and indestructible. His approach was simply philosophy and was not based upon the scientific method. Aristotle (Greek philosopher from 384 BC to 322 BC) Did not believe in the atomic theory but believed all materials on Earth were composed of four elements - earth, fire, water, and air. John Dalton ( ) Used the scientific method to transform Democritus ideas into a scientific theory. Dalton s atomic theory 1. All elements are composed of tiny indivisible particles called atoms. 2. Atoms of the same element are identical. 3. Atoms of different elements can chemically combine in simple whole-number ratios to form compounds. 4. Chemical reactions occur when atoms are separated, joined, or rearranged, however atoms are never changed into atoms of another element as a result of a chemical reaction.
2 JJ Thompson Used cathode ray tube to find electrons are inside atom (Chocolate-Chip Cookie Model) Robert Millikan Used Oil-Drop Experiment to calculate the charge of an electron. Earnest Rutherford Used Gold-Foil Experiment to discover the tiny positive central core called a nucleus. The rest of the atom was mostly empty space where the electrons reside.
3 Niels Bohr Electrically charged Hydrogen gas to find that there are energy levels called orbits (n=1, n=2, etc.). Heisenberg s Uncertainty Theory Impossible to know both the position and velocity of an electron at a particular instant. Electron-Cloud Theory Used Heisenberg s Uncertainty Theory to show that electrons were in orbitals (gave the probability of the location of an electron).
4 Subatomic Particles Particle Mass Charge Proton 1 +1 Neutron 1 0 Electron 0-1 Nucleus positively charged center of the atom that has most of the mass. It is made up of protons and neutrons Distinguishing Among Atoms Atomic Number = number of protons (the protons identifies the element) (Atomic Number = #P) Atomic Weight = number of protons and neutrons (Atomic weight = #P + #N) Ionic Charge = number of protons minus electrons (Ionic Charge = #P - #e) Isotope = same number of protons (same element), different number of neutrons (a different mass) Element Squares on the Periodic Table
5 Example: Fill in the table below. Bolded information would be given. Element Protons Neutrons Atomic Weight Electrons Ionic Charge Carbon-12 O F Answer: Element Protons Neutrons Atomic Weight Electrons Ionic Charge Carbon O Ag F Mg Example: If the atomic mass of chlorine is 35.5, which isotope will be more abundant Cl-35 or Cl-37? Answer: Cl-35 will be more abundant because the average is closer to the mass of 35 than 37. Electron Configurations Example: What is the electron configuration of oxygen? Answer: 1s 2 2s 2 2p 4 Example: What is the electron configuration of titanium? Answer: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2
6 Orbital Diagrams (Boxes) Aufbau Principle Electrons are filled in lowest energy orbitals first (Start with 1s first) Pauli-Exclusion Principle Each orbital can have a maximum of two electrons with opposite spins (Each box can only hold two arrows one up and one down) Hund s Rule One electron in each box before pairing (when it comes to the p-orbital, fill one in each box before pairing) Example: Draw the orbital diagrams (boxes) for Oxygen. Answer: The electron configuration of Oxygen is 1s 2 2s 2 2p 4 The first orbital diagram is incorrect because it goes against Hund s Rule which states that one electron must go in each box before pairing. The second orbital diagram is correct. Emission Spectrum Emission Spectra The step of frequencies in the electromagnetic spectrum that an element gives off when an electron goes from an excited state (higher energy) back down to a lower energy state. Example: Which two elements are found in the star using the emission spectra below?
7 Answer: Helium and Hydrogen 8.5 Atomic Structure
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