Atom Models & Atomic Structure PDF

Atomos-Indivisible  Louis de Werner Erwin Broglie Heisenberg Schrodinger, WAVE-PARTICLE DUALITY OF UNCERTAINTY QUANTUM MATTER PRINCIPLE...

Atomos-Indivisible  Louis de Werner Erwin Broglie Heisenberg Schrodinger, WAVE-PARTICLE DUALITY OF UNCERTAINTY QUANTUM MATTER PRINCIPLE MECHANICAL ThereMODEL is a region of De Broglie Hypothesis: It is impossible to know No one can predict the space where the position and exact path of an electron electrons are most momentum of an electron as it moves around the likely to be found. at the same time  ELECTRON CONFIGURATI ON It is the  a. PERIODIC TABLE b. ENERGY LEVEL distribution of c. SUBLEVEL d. ORBITAL e. ELECTRIC electrons to CONFIGURATION track where is the probable location of electrons in an atom ENERGY LEVEL (shell/principal energy level) - Indicates the relative size and energy of an orbital -Contains the certain number of sublevels  SUB ENERGY LEVEL/ SUBLEVEL - Has fixed number of atomic orbitals -The name of the sublevel is also same as the name of orbitals (s, p, d, f)  ORBITAL (s, p, d, f) -Region around the nucleus where electrons are most likely to be found - serves as the house of electrons - Can accommodate maximum of 2 electrons  ORBITAL (s, p, d, f) -Region around the nucleus where electrons are most likely to be found orbital No. of orbital No. of - serves as the house electrons of electrons s 1 2 - Can accommodate p 3 6 maximum of 2 d 5 10 electrons f 7 14  The principal energy levels are broken down into sublevels. These sublevels define the orbital shape (s, p, d, f)  The principal energy levels are always equal to the number of sublevels.  TWO WAYS OF WRITING ELECTRON CONFIGURATIONS Unabbreviated Electron Abbreviated Electron Configuration Configuration CALCIU M  3 RULES IN WRITING ELECTRON CONFIGURATION 1. Aufbau’s Principle 2. Pauli’s Exclusion principle 3. Hund’s Rule of Multiplicity  Aufbau’s principle - “Building up principle” - Electrons must occupy first the orbitals with lower energies Aufbau’s principle 2 1 1s 2s Valence electron: 1  Pauli’s exclusion principle -Only a maximum 2 electrons can occupy an orbital and they must have opposite spin to minimize repulsion Pauli’s exclusion principle 2 1s 2s 2 2p6 3s 1  Hund’s Rule of multiplicity -When electrons enter a sublevel with more than one orbital, they will spread out to the available orbitals with the same spin before pairing Hund’s Rule of Multiplicity 2 1s 2s 2 2p3  Quantum numbers The position and energy of every electron in an atom is determined by a set of 4 quantum numbers. Four quantum numbers can be used to completely describe all the attributes of a given electron belonging to an atom, these are:  ATOMIC ELEMENT PRINCIPAL ORBITAL MAGNETIC SPIN QN NUMBER QUANTUM QN QN NUMBER +1/2 (shell s=0 s= 0 period) P=1 p= -1,0,+1 -1/2 d=2 d= -2,-1,0,+1,+2 F=3 f= -3,-2,- 1,0,+1,+2,+3 1 HYDROGEN 1 0 0 +½ 2 HELIUM 1 0 0 -½ 3 LITHIUM 2 0 0 +½ 4 BERYLLIUM 2 0 0 -½ 5 BORON 2 1 -1 +½ 6 CARBON 2 1 0 +½ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.