PRINCIPALS OF CHEMISTRY I (CEM 141) Dr. BÙI THỊ BỬU HUÊ College of Science Cantho University

1. PRINCIPALS OF CHEMISTRY I (CEM 141) Dr. BÙI THỊ BỬU HUÊ College of Science Cantho University

2. Chapter 1. MATTER AND MEASUREMENT Chapter 2. ATOMS, MOLECULES AND IONS Chapter 3. STOICHIOMETRIC Chapter 4. ATOMIC STRUCTURE AND THE PERIODIC TABLE Chapter 5. CHEMICAL BONDS AND MOLECULAR STRUCTURE Chapter 6. STATES OF MATTER Chapter 7. ENERGY AND CHEMICAL REACTIONS Chapter 8. SOLUTIONS Chapter 9. CHEMICAL EQUILIBRIA

3. References • 1. Brady and Holum. 1996. Chemistry: the Study • of Matter and its Changes. • 2th Ed., John Wiley & Sons. Inc. New York. • 2. Umland, Jean B., 1993. General Chemistry. • West publishing company. • 3. Zumdahl, Steven S. 1995. Chemical Principal. • 2th Ed. DC. Health & company. Toronto. • 4. http://www.chemistry.msu.edu/Courses/ • 5. http://antoine.frostburg.edu • 6. http://chemed.chem.purdue.edu • 7. http://www.chem1.com/chemed/genchem.html • http://www.cbu.edu/~mcondren/lectures.htm • http://ull.chemistry.uakron.edu/GenChem/index.html

4. Chapter 4. ATOMIC STRUCTURE AND THE PERIODIC TABLE • Objectives • Understand atomic structure of an atom including its mass number, isotopes and orbitals. • Know how to account for the structure of the periodic table of the elements based on the modern theory of atomic structure. • Understand general trends of several important atomic properties.

5. Chapter 4. ATOMIC STRUCTURE AND THE PERIODIC TABLE Atomic Structure An atom is composed of three types of subatomic particles: the proton, neutron, and electron.

6. Atomic Structure

7. Atomic Structure

8. ElectromagneticRadiation

10. Electromagnetic Radiation nl= c Where: n: frequency l: wavelength c: speed of light

11. Electromagnetic Spectrum

12. Dispersion of White Light

13. Photoelectric Effect • the emission of electrons by substances, especially metals, when light falls on their surfaces.

14. Photoelectric Effect

15. Quantum Mechanics • Quantum theory the theory of the structure and behavior of atoms and molecules.

16. Photons The quantum of electromagnetic energy, generally regarded as a discrete particle having zero mass, no electric charge, and an indefinitely long lifetime. E = hν = hc/λ h = Planck's constant = 6.626 × 10−34 J.s

21. Line Emission Spectrum

22. Light shinning on a sample causes electrons to be excited from the ground state to an excited state wavelengths of that energy are removed from transmitted spectra Absorption Spectrum

24. The Atomic Spectrum of Hydrogen and the Bohr Model Bohr Model for the Hydrogen Atom mvr = nh/2p n = quantum number n = 1, 2, 3, 4, 5, 6, 7, etc

25. Bohr Atom

26. Ground State The state of least possible energy in a physical system, as of elementary particles. Also called ground level.

27. Excited State Being at an energy level higher than the ground state.

28. Electron Transition in a Hydrogen Atom Lyman series → ultraviolet n > 1 → n = 1 Balmer series → visible light n > 2 → n = 2 Paschen series → infrared n > 3 → n = 3

29. Knowing diamond is transparent, which curve best represents the absorption spectrum of diamond (see below)? A, B, C

30. According to the energy diagram below for the Bohr model of the hydrogen atom, if an electron jumps from E1 to E2, energy is absorbed emitted not involved

42. Orbitals • region of probability of finding an electron around the nucleus • 4 types: s, p, d, f

43. Atomic Orbitals, s-type

44. Atomic Orbitals, p-type

45. Atomic Orbitals, d-type

48. Pauli Exclusion Principle

49. Electronic Configurations • The shorthand representation of the occupancy of the energy levels (shells and subshells) of an atom by electrons.