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Review Periodic Table

Review Periodic Table. Mendeleev - arranged in order of increasing atomic mass. Moseley – in order of increasing atomic number Atomic mass = #protons + # neutrons, atomic number = #protons Period - row of elements, properties change gradually

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Review Periodic Table

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  1. Review Periodic Table Mendeleev- arranged in order of increasing atomic mass. Moseley – in order of increasing atomic number Atomic mass = #protons + # neutrons, atomic number = #protons Period- row of elements, properties change gradually Group – column of elements, similar properties Electron configuration – all the elements in a group have the same configuration of electrons in their outer shell

  2. In the beginning When God started building the atoms of elements he began with a design. We may have discovered that design. He began adding electrons, protons and neutrons according to the design. The first element had 1 electron and 1 proton and either 0,1 or 2 neutrons. The second element had 2 electrons and 2 protons and either 1,2 or 3 neutrons. Simulation

  3. Uncertainty Principle The problem of defining the nature of electrons in atoms was solved by W. Heisenberg. We cannot simultaneously define the position and momentum (= m•v) of an electron. We can define e- energy exactly but we must accept the limitation that we do not know the exact position of the e-. W. Heisenberg 1901-1976

  4. Electron Configuration • Electrons within the electron cloud have different energy levels. • Each electron is assigned 4 different “quantum numbers”. No two electrons within an atom can have the same quantum numbers. • Energy Level quantum number, there are 7 levels (1-7) • Shape quantum number -suborbits for electrons s,p,d,f • Orientation quantum number • Spin quantum number- right handed or left handed

  5. QUANTUM NUMBERS Each orbital is a function of 3 quantum numbers: n, l,andml n the principal quantum number or shell (or size and energy level) l the angular momentum quantum number or subshell (or shape) ml the magnetic quantum number designates an orbitalwithin a subshell (or the orientation in space) In addition each electron has 1 of 2 Spins

  6. QUANTUM NUMBERS Symbol Values Description n (major) 1, 2, 3, .. Orbital size and energy (shell) l (angular) 0, 1, 2, .. n-1 Orbital shape or type (subshell) ml (magnetic) - l..0..+ l Orbital orientation # of orbitals in subshell = 2 l + 1

  7. Shells and Subshells When n = 1, then l = 0 and ml = 0 Therefore, in n = 1, there is 1 type of subshell and that subshell has a single orbital (ml has a single value  1 orbital) This subshell is labeled s Each n value (shell) has 1 orbital labeled s, and it is SPHERICALin shape.

  8. s Orbitals All s orbitals are spherical in shape.

  9. p Orbitals When n = 2, then l = 0 and 1 Therefore, in the n = 2 shell there are 2 types of orbitals — 2 subshells For l = 0 ml = 0 this is a s subshell For l = 1 ml = -1, 0, +1 this is a p subshellwith 3 orbitals

  10. p Orbitals When l = 1, there is a PLANAR NODE through the nucleus. 3 Orientations

  11. p Orbitals The three p orbitals lie 90o apart in space A p orbital

  12. d Orbitals When n = 3, l = 0, 1, 2 and so there are 3 subshells in the shell. For l = 0, ml = 0  s subshell with single orbital For l = 1, ml = -1, 0, +1  p subshell with 3 orbitals For l = 2, ml = -2, -1, 0, +1, +2 d subshell with 5 orbitals (orientations)

  13. d Orbitals s orbitals have no planar node (l = 0) and so are spherical. p orbitals have l = 1, have 1 planar node, and are “dumbbell” shaped. This means d orbitals (with l = 2) have 2 planar nodes

  14. d Orbitals

  15. f Orbitals When n = 4, l = 0, 1, 2, 3 so there are 4 types of subshells in the shell. For l = 0, ml = 0  s subshell with single orbital For l = 1, ml = -1, 0, +1  p subshell with 3 orbitals For l = 2, ml = -2, -1, 0, +1, +2  d subshell with 5 orbitals For l = 3, ml = -3, -2, -1, 0, +1, +2, +3  f subshell with 7 orbitals

  16. f Orbitals

  17. Arrangement of Electrons in Atoms Electrons are arranged in SHELLS (n) SUBSHELLS (l) ORBITALS (ml) Various Way of Describing Energy Levels {

  18. Arrangement of Electrons in Atoms Each orbital can be assigned no more than 2 electrons! This is tied to the existence of a 4th quantum number, the electron spin, ms.

  19. Electron Spin, ms Any spinning electric charge creates a magnetic field, comparable to N and S. There are two spin directions that are designated by ms = +1/2 and -1/2.

  20. Pauli Exclusion Principle No two electrons in the same atom can have the same set of 4 quantum numbers. That is, each electron has a unique address.

  21. Aufbau PrinciplePage 111 An electron occupies the lowest energy orbital that can receive it. Fill lower energy orbitals first Energy levels overlap 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d

  22. Electron Filling Order This is confusing- follow a listing of configurations to see just how it works.

  23. Hund’s Rule • Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state.

  24. Writing Atomic Electron Configurations There are two ways of writing configurations. One is called spectroscopic notation.

  25. Writing Atomic Electron Configurations The other method of writing e- configurations is called the orbital box notation. One electron has n = 1, l = 0, ml = 0, ms = + 1/2 Other electron has n = 1, l = 0, ml = 0, ms = - 1/2

  26. See Electron Configuration in ChemLand.

  27. Lithium Group 1A Atomic number = 3 1s22s1 3 total electrons

  28. Beryllium Group 2A Atomic number = 4 1s22s2 4 total electrons

  29. Boron Group 3A Atomic number = 5 1s2 2s2 2p1 5 total electrons

  30. Carbon Group 4A Atomic number = 6 1s2 2s2 2p2 6 total electrons Here we see for the first timeHUND’S RULE. When placing electrons in a set of orbitals having the same energy, we place a single electron in each orbital as long as possible.

  31. Nitrogen Group 5A Atomic number = 7 1s2 2s2 2p3 7 total electrons

  32. Oxygen Group 6A Atomic number = 8 1s2 2s2 2p4 8 total electrons

  33. Fluorine Group 7A Atomic number = 9 1s2 2s2 2p5 9 total electrons

  34. Neon Group 8A Atomic number = 10 1s2 2s2 2p6 10 total electrons Note that we have reached the end of the 2nd period, and the 2nd shell is full!

  35. Electrons in Atoms When n = 1, then l = 0 this shell has a single orbital (1s) to which 2e- can be assigned. When n = 2, then l = 0, 1 l = 0 is the 2s orbital which has 2e- l = 1 is the three 2p orbitals which have 6e- TOTAL = 8e- in 4 orbitals

  36. Electrons in Atoms When n = 3, then l = 0, 1, 2 l = 0 is the 3s orbital 2e- l = 1 is the three 3p orbitals 6e- l = 2 is the five 3d orbitals 10e- TOTAL = 18e- in 9 orbitals

  37. Electrons in Atoms When n = 4, then l = 0, 1, 2, 3 4s orbital 2e- three 4p orbitals 6e- five 4d orbitals 10e- seven 4f orbitals 14e- TOTAL = 32e- ChemLand: Atomic Structure Quantum Numbers

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