Unit three notes s05
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This document provides a brief history of the atomic theory, from early philosophers' ideas to the modern quantum model. It describes Democritus' idea of indivisible atoms, Dalton's model of atoms as solid spheres, Thomson's discovery of electrons, Rutherford's gold foil experiment showing the nucleus, Bohr's planetary model, and the modern electron cloud/quantum model with protons and neutrons in the nucleus and electrons in clouds outside. It also discusses atomic structure, isotopes, ions, atomic mass, and calculating atomic properties using atomic number and mass number.
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- The document discusses the history and development of atomic models from Dalton to Bohr. It describes key discoveries and experiments.
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- Bohr incorporated Rutherford's nuclear model into his planetary model of the atom. He proposed that electrons orbit the nucleus in defined energy levels. This model had limitations when describing multi-electron atoms.
- The quantum mechanical model was developed based on discoveries that electrons can be described as waves using quantum physics principles like wave-particle duality and the uncertainty principle. This model uses atomic orbit
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Atomic Structure and Isotopes 7 (1).ppt
John Dalton suggested that all matter is made up of tiny spheres called atoms in the early 1800s. J.J. Thomson discovered electrons through cathode ray tube experiments in the late 1800s. Ernest Rutherford determined that the nucleus occupies a very small portion of the atom through nuclear scattering experiments. Niels Bohr developed the Bohr model of the atom to explain atomic spectra. Atoms have a small, dense nucleus containing protons and neutrons, surrounded by electrons in an electron cloud. The number of protons determines the element, and electrons normally equal protons for neutral atoms. Isotopes are atoms of the same element with different numbers of neutrons.
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Unit three notes s05
- 1. Chemistry Unit Three Atomic Structure
- 2. A Brief History of the Atomic Theory
- 7. Gold Foil Experiment Rutherford’s
- 12. Atomic Structure Found in the Nucleus Found in the Nucleus Found outside the nucleus Has 1 amu of mass Has 1 amu of mass Has 0 amu of mass Has a positive charge Has a negative charge Has no charge (neutral) Electrons (e-) Neutrons (n) Protons (p+)
- 13. Atomic Structure Atom The number of protons in an atom never changes. Isotope Atoms of the same element that have different numbers of neutrons. Ion An atom that has lost or gained electrons .
- 16. 6 C 12.011 Atomic Number = 6 6 protons = 6 electrons 6 p+ = 6 e- (atom is neutral) Atomic Mass = 12 12 p+ and n -6 p+ 6 neutrons Calculating Numbers of Protons, Neutrons and Electrons.
- 17. Practice Calculating p+, n, e- *Atomic # is number of protons so protons = 47 *number (+) charges (p+) must equal (–) charges to make the atom neutral so electrons = 47 *Mass Number is total particles with mass (p+ and n) so 47 + 61 = 108 47 47 108 61 47 Silver # neutron # electron # proton Mass Number Atomic number Element
- 18. B Practice Calculating p+, n, e- *number of protons is the atomic # so atomic number is 29 *number (+) charges (p+) must equal (–) charges to make the atom neutral so electrons = 29 *Mass Number is total of all particles with mass (p+ and n) so subtract away the atomic number (#p+) and you will have just neutrons (64 – 29 = 35) 35 29 29 29 64 Copper # neutron # electron # proton Mass Number Atomic number Element
- 21. Bohr Model of Lithium 3 4 e - e - e - 3 Li 6.941
- 22. Bohr Model of Argon 18 22 e - e - e - 18 Ar 39.948 e - e - e - e - e - e - e - e - e - e - e - e - e - e - e -
- 27. s and p Orbital Electrons
- 30. Periodic Table to remember order s 1 s 2 s 2 p 1 p 2 p 3 p 4 p 5 p 6 d 1 d 2 d 3 d 4 d 5 d 6 d 7 d 8 d 9 d 10 f 1 f 2 f 3 f 4 f 5 f 6 f 7 f 8 f 9 f 10 f 11 f 12 f 13 f 14 Sublevels (s,p,d,f) by columns - Energy levels by rows (1,2,3,4,5,6,7 except d(row-1) & f(row-2)) 1 2 3 4 5 6 7 X – 1s 2 2s 2 2p 6 3s 2 3p 4 (16 e-) Y – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 (36 e-) X Y
- 36. Lewis Dot Structures Con’t B B = Kernel (The protons, neutrons and full electron shells.) Valence shell electrons
- 40. Ne 1 2 3 4 5 6 7 8 So, it goes like this…
- 42. Average Atomic Mass (How the number ends up on the periodic table!!) 1 st Mass of one isotope x % abundance in decimal form (watch SIG FIGS!!) 2 nd Do this for each isotope of that element 3 rd Then add all individual isotopes together to get the average atomic mass.
- 43. 1. Calculate the average atomic mass of potassium using the following data: Potassium-39 38.964 amu x 0.9312 = 36.28 amu Potassium-41 40.962 amu x 0.0688 2.82 amu = + Average atomic mass for K = 39.10 amu 6.88 % 40.962 amu Potassium-41 93.12% 38.964 amu Potassium-39 % abundance Mass Isotope
- 44. 2. Calculate the average atomic mass of magnesium using the following data: Magnesium-24 23.985 amu x 0.7870 = 18.88 amu Magnesium-25 24.986 amu x 0.1013 2.531 amu = + Average atomic mass for K = 24.31 amu + Magnesium-26 25.983 amu x 0.1117 = 2.902 amu 11.17 % 25.983 amu Magnesium-26 10.13 % 24.986 amu Magnesium-25 78.70% 23.985 amu Magnesium-24 % abundance Mass Isotope