Chemistry - Atomic structure

1. 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. 2. Explain the law of conservation of mass, the law of definite proportions, and the law of multiple proportions. 3. Describe the properties of protons, neutrons, and electrons. 4. Define the isotopes and utilize atomic and mass numbers to identify them. 5. Evaluate Dalton's atomic theory in terms of experimental proof and modern atomic theory. 6. Summarize the experiments carried out by Thomson and Rutherford that led to the discovery of atomic theory. 7. Differentiate between the mass number of an isotope and the average atomic mass of an element. 8. Relate the existence of quantized energy levels to atomic emission spectra. 9. Discuss the dual wave-particle nature of light. 10. Correlate the observed line-emission spectrum of hydrogen to the progression of the atomic model. 11. Describe the Bohr model of the hydrogen atom. 12. Compare and contrast the Bohr model and quantum model of the atom. 13. Explain how the Heisenberg uncertainty principle and the Schrodinger wave equation led to the idea of atomic orbitals. 14. Explain the relationship between the electron configuration and the atomic structure of a given atom or ion. 15. Describe the electron configurations for atoms of any element using orbital notation, electron-configuration notation, and noble-gas notation. 16. Compare Mendeleev's periodic table to the modern periodic table. Explain how the periodicity of chemical properties led to the arrangements of elements on the periodic table. 17. Discuss the relationship between electron configuration of an element and its place on the period table. 18. Describe how the elements belong to a group of the periodic table are interrelated in terms of atomic number. 19. Define periodic trends in atomic radii, ionization energy, electron affinity, and electronegativity. 20. Define valence electrons, and determine the correlation between number of valence electrons and group number. 21. Explain how the periodic law can be used to predict the physical and chemical properties of elements. Compare and/or predict the properties of selected elements by using their locations on the periodic table and known periodic trends.

Atomic Mass

Atomic Mass

Protons + Neutrons

Atom

Smallest unit of matter

Nucleus

the positively charged dense center of an atom made up of protons and neutrons

Neutron

A subatomic particle that has no charge and that is found in the nucleus of an atom

Proton

A subatomic particle that has a positive charge and that is found in the nucleus of an atom.

electron

a subatomic particle that has a negative charge