2º ENCONTRO UAB-UFPA (Polo Barcarena)

Apresentação em tema: "2º ENCONTRO UAB-UFPA (Polo Barcarena)"— Transcrição da apresentação:

1 2º ENCONTRO UAB-UFPA (Polo Barcarena)
QUÍMICA Prof. Pimentel/Tutora(Roseli) Barcarena (12/05/2018)

2 Wavelengths for Different States
O QUE É UM “ÁTOMO” ? O que são “Modelos Atômicos” ? Wavelengths for Different States

3 FÍSICA ≠ QUÍMICA Postulados da função de onda

4

5 Como “montar um átomo” ? “Simbolo do átomo”: neutro e íons (cation ou ânion)” ? VAMOS EXERCITAR!!!

6 Propriedades Periódicas

7 Propriedades Periódicas
Atomic Radii

8 Propriedades Periódicas
Níveis de energias e dependência do orbial

9 Pauli Repulsion in Ionic Molecules
LIGAÇÕES QUÍMICA INTERAÇÃO ATÔMICA Pauli Repulsion in Ionic Molecules An ionic bond may be modeled in terms of the ionization energy to produce the positive ion, the electron affinity associated with the negative ion, the dissociation energy for the molecule, the coulomb potential between the ions, and the repulsive force which limits the closeness of approach of the ions. This repulsive force is typically called Pauli repulsion. The energy balance of all these terms can be written in the form

10 LIGAÇÃO (Cloreto de sódio)
An atom of sodium has one 3s electron outside a closed shell, and it takes only 5.14 electron volts of energy to remove that electron. The chlorine lacks one electron to fill a shell, and releases 3.62 eV when it acquires that electron (it's electron affinity is 3.62 eV). This means that it takes only 1.52 eV of energy to donate one of the sodium electrons to chlorine when they are far apart. When the resultant ions are brought closer together, their electric potential energy becomes more and more negative, reaching eV at about 0.94 nm separation. This means that if neutral sodium and chlorine atoms found themselves closer than 0.94 nm, it would be energetically favorable to transfer an electron from Na to Cl and form the ionic bond.

11 LIGAÇÃO (Moléculas covalentes)
The exchange interaction (an entirely quantum mechanical effect) leads to a strong bond for the hydrogen molecule with dissociation energy 4.52 eV at a separation of nm. The potential energy of the anti-bonding orbital shown gives some insight into why a third hydrogen atom cannot bond to the two atoms of the hydrogen molecule. It would be in an anti-bonding situation with one of the other hydrogen atoms and would therefore be repelled. We say that the bond in the hydrogen molecule is "saturated" because it cannot accept another bond.

12 Diagrama do Orbital Molecular para CO e CO2

13 LIGAÇÃO (Metálica)

14 https://kaiserscience.wordpress.com/chemistry/atoms/compounds/

15 https://kaiserscience.wordpress.com/chemistry/atoms/compounds/

16 COMPARANDO: https://www.google.com.br
COMPARANDO:

17