Compare and/or predict the properties of selected elements by using their locations on the periodic table and known periodic trends. Explain how the periodic law can be used to predict the physical and chemical properties of elements. Define valence electrons, and determine the correlation between number of valence electrons and group number.Ģ1. Elements are characterized by the weight of their atoms 4. Atoms are indestructible and unchangeable 3. All matter consists of tiny particles called atoms 2. All elements are composed of tiny indivisible particles called atoms.2. Define periodic trends in atomic radii, ionization energy, electron affinity, and electronegativity.Ģ0. Timeline: 1800’s Scientist: John Dalton John Dalton was the first to adapt Democritus’ theory into the first modern atomic model. 1803: John Dalton and The Atomic TheoryHe was originally a meteorologist who switched to chemistry when he saw the applications for chemistry of his ideas about the atmosphere.Proposed the atomic theory in 1803.Atomic Theory:1. Describe how the elements belong to a group of the periodic table are interrelated in terms of atomic number.ġ9. Discuss the relationship between electron configuration of an element and its place on the period table.ġ8. Explain how the periodicity of chemical properties led to the arrangements of elements on the periodic table.ġ7. Compare Mendeleev's periodic table to the modern periodic table. Describe the electron configurations for atoms of any element using orbital notation, electron-configuration notation, and noble-gas notation.ġ6. Explain the relationship between the electron configuration and the atomic structure of a given atom or ion.ġ5. Explain how the Heisenberg uncertainty principle and the Schrodinger wave equation led to the idea of atomic orbitals.ġ4. Compare and contrast the Bohr model and quantum model of the atom.ġ3. George Zweig proposed the existence of quarks. To find this, he blasted high speed electrons into a hydrogen atom. He also found that all the elements of an atom are held together by quarks. Describe the Bohr model of the hydrogen atom.ġ2. Murray Gell- Mann was an American physicist who received a Nobel Prize for his theory on elementary particles. Correlate the observed line-emission spectrum of hydrogen to the progression of the atomic model.ġ1. Discuss the dual wave-particle nature of light.ġ0. Relate the existence of quantized energy levels to atomic emission spectra.ĩ. Differentiate between the mass number of an isotope and the average atomic mass of an element.Ĩ. Summarize the experiments carried out by Thomson and Rutherford that led to the discovery of atomic theory.ħ. Evaluate Dalton's atomic theory in terms of experimental proof and modern atomic theory.Ħ. Define the isotopes and utilize atomic and mass numbers to identify them.ĥ. Describe the properties of protons, neutrons, and electrons.Ĥ. Explain the law of conservation of mass, the law of definite proportions, and the law of multiple proportions.ģ. Describe the evolution of atomic theory leading to the current model of the atom based on the works of Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger.Ģ.
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