Chapter 11. What subatomic particles do you get to play with? Protons Neutrons Eletrons
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1 Chapter 11 What subatomic particles do you get to play with? Protons Neutrons Eletrons changes the element isotopes: only mass is different what we play with in chemistry
2 Bohr Model of the Atom electrons must circle the nucleus of an atom in certain paths Developed the concept of Energy Levels Connected H s electron with photon emission 1.e - reside in orbits 2.Lowest energy closest to nucleus, increase in energy farther from nucleus 3.Empty space between each orbit 4.Calculated energies of an e - in allowed energy levels; E photon = h 5.e - in higher-energy orbits, falls back to lower-energy orbit releasing a photon 6.Calculated energies agreed with line series 7.Only explained H atom
3 Quantum (definition from Webster s) 1) quantity, amount 2) any of the very small increments or parcels into which many forms of energy are subdivided Quantum Theory -describes mathematically the wave properties of electrons and other very small particles *electrons were determined to have a dual wave-particle nature *uses two principles
4 Heisenberg Uncertainty Principle -it is impossible to determine simultaneously both the position and velocity of an electron or any other particle Schrodinger Wave Equation -treats electrons as waves around the nucleus *Together these determine the probability of finding electrons.
5 I. Louis de Broglie Could electrons have a dual wave-particle nature as well? A.e - be considered waves confined to the space around an atomic nucleus B.e - could only exist at specific frequencies, correspond to orbit energies C. Experiments confirmed hypothesis
6 Orbital -three-dimensional region around the nucleus that indicates the probable location of an electron To describe orbitals, we use.. Quantum Numbers -specify the properties of atomic orbitals and the properties of electrons in orbitals *there are 4 quantum numbers
7 Principle Quantum Number (n) -the main energy level occupied by the electron *positive integers *ranges from 1 to 7 *equals to the period Angular Momentum Quantum Number (l) -shape of the orbital *orbitals possible is equal to n *values of l are all integers less than l = n-1
8 Angular Momentum Quantum Number (l) l letter 0 s 1 p 2 d 3 f
9 Angular Momentum Quantum Number (l)
10 Magnetic Quantum Number (m) -indicates the orientation of an orbital around the nucleus * m = ±l Spin Quantum Number -has only 2 possible values (+½, -½)
11
12 Electron Configurations -the arrangement of electrons in an atom *based on 3 rules Afbau Principle -electrons occupy the lowest energy level they can
13 Pauli Exclusion Principle -no two electrons in the same atom can have the same set of four quantum numbers 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
14 Relative Energies of Orbitals
15 Electron Configuration Notation - the order of orbitals is. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6
16 Electron Configuration Notation Boron 5 electrons Bromine 35 electrons 1s 2 2s 2 2p 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5
17 Electron Configuration Notation Can also use Noble Gases to show Electron Configurations since they have fulfilled the Octet Rule Noble Gas Notation Bromine 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 [Ar] 4s 2 3d 10 4p 5
18 Filling Electrons using Afbau s Principle, the Pauli Exclusion Principle, and Hund s Rule Fill e- for: N O Al Br
19 Using Quantum Numbers to Identify Elements n l m spin N O Al Br / /2
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