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. 2 th Ed., John Wiley & Sons. Inc. New York. 2. Umland, Jean B., 1993. General Chemistry. West publishing company. 3. Zumdahl, Steven S. 1995. Chemical Principal. 2 th Ed. DC. Health & company. Toronto. 4. http://www.chemistry.msu.edu/Courses/http://www.chemistry.msu.edu/Courses/ 5. http://antoine.frostburg.eduhttp://antoine.frostburg.edu 6. http://chemed.chem.purdue.eduhttp://chemed.chem.purdue.edu 7. http://www.chem1.com/chemed/genchem.htmlhttp://www.chem1.com/chemed/genchem.html 8. http://www.cbu.edu/~mcondren/lectures.htmhttp://www.cbu.edu/~mcondren/lectures.htm 9. http://ull.chemistry.uakron.edu/GenChem/index.htmlhttp://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. Particle Mass (g)Charge Proton 1.6727 x10 -24 +1 Neutron 1.6750 x10 -24 0 Electron 9.110 x 10 -28 - 1

6. Atomic Structure

8. Electromagnetic Radiation

10.  c Where:  frequency  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. the emission of electrons by substances, especially metals, when light falls on their surfaces.

14. Photoelectric Effect

15. Quantum Mechanics Quantum theory 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. Absorption Spectrum  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

24. The Atomic Spectrum of Hydrogen and the Bohr Model Bohr Model for the Hydrogen Atom mvr = nh/2  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. 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. 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 absorbedemitted not involved

42. Orbitals region of probability of finding an electron around the nucleus region of probability of finding an electron around the nucleus 4 types: s, p, d, f 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. The shorthand representation of the occupancy of the energy levels (shells and subshells) of an atom by electrons.

58. Hund's Rules

59. Electronic Configuration H atom (1 electron): 1s 1 He atom (2 electrons):1s 2 Li atom(3 electrons):1s 2, 2s 1 Cl atom (17 electrons):1s 2, 2s 2, 2p 6, 3s 2, 3p 5

60. Electronic Configuration As atom 33 electons: 33 electons: 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 3 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 3or [Ar] 4s 2, 3d 10, 4p 3

62. Mn: [Ar]4s 2 3d ? How many d electrons does Mn have? 4, 5, 6

64. Electronic Configuration Negative ions : add electron(s), 1 electron for each negative charge S -2 ion: (16 + 2)electrons: 1s 2, 2s 2, 2p 6, 3s 2, 3p 6

65. Electronic Configuration Positive ions remove electron(s), 1 electron for each positive charge Mg +2 ion: (12-2) electrons 1s 2, 2s 2, 2p 6 1s 2, 2s 2, 2p 6

66. How many valence electrons are in Cl, [Ne]3s 2 3p 5 ? 2, 5, 7

67. For Cl to achieve a noble gas configuration, it is more likely that electrons would be added electrons would be removed

69. Regions by Electron Type

75. Trends in the Periodic Table atomic radius atomic radius ionic radius ionic radius ionization energy ionization energy electron affinity electron affinity

76. Atomic Radius decrease left to right across a period Z eff = Z - S where Z eff = effective nuclear charge Z = nuclear charge, atomic number S = shielding constant

77. Atomic Radius  Increase top to bottom down a group  Increases from upper right corner to the lower left corner

78. Atomic Radius

79. Atomic Radius vs. Atomic Number

80. Ionic Radii

81. Ionic Radius Same trends as for atomic radius Same trends as for atomic radius positive ions smaller than atom positive ions smaller than atom negative ions larger than atom negative ions larger than atom

82. Comparison of Atomic and Ionic Radii

83. Ionic Radius Isoelectronic Series series of negative ions, noble gas atom, and positive ions with the same electronic confiuration series of negative ions, noble gas atom, and positive ions with the same electronic confiuration size decreases as “positive charge” of the nucleus increases size decreases as “positive charge” of the nucleus increases

84. Ionization Energy energy necessary to remove an electron to form a positive ion energy necessary to remove an electron to form a positive ion low value for metals, electrons easily removed low value for metals, electrons easily removed high value for non-metals, electrons difficult to remove high value for non-metals, electrons difficult to remove increases from lower left corner of periodic table to the upper right corner increases from lower left corner of periodic table to the upper right corner

85. Ionization Energies first ionization energy energy to remove first electron from an atom. energy to remove first electron from an atom. second ionization energy energy to remove second electron from a +1 ion. energy to remove second electron from a +1 ion.etc.

86. Ionization Energy vs. Atomic Number

87. Electron Affinity energy released when an electron is added to an atom energy released when an electron is added to an atom same trends as ionization energy, increases from lower left corner to the upper right corner same trends as ionization energy, increases from lower left corner to the upper right corner metals have low “EA” metals have low “EA” nonmetals have high “EA” nonmetals have high “EA”

88. Magnetism Result of the spin of electrons Result of the spin of electrons diamagnetism - no unpaired electrons diamagnetism - no unpaired electrons paramagnetism - one or more unpaired electrons paramagnetism - one or more unpaired electrons

89. Magnetism Without applied fieldWith applied field