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- Núme Número ro quân quânti tico co prin princi cipa pal, l, n - Núm Número ero quâ quânti ntico co de momento momento ang angula ular, r, - Nú Núme mero ro qu quân ânti tico co ma magn gnéti ético co,, m
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- Nú Núme mero ro qu quân ântic ticoo pri princ ncipa ipal, l, n
Está relacionado com o tamanho da orb
Pode assumir os valores inteiros 1,
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- Nú Númer meroo quâ quânt ntic icoo de de mom momen ento to angular, está relacionado com forma da orbital (tipo de orbital) O número quântico ℓ, só pode assumir os valores inteiros compreendidos entre 0 e n -1 -1 Sign up to vote on this title
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- Nú Númer meroo quâ quânt ntic icoo de de mom momen ento to angular,
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- Nú Númer meroo quâ quânt ntic icoo de de mom momen ento to angular,
L o Tipo de orbital s
1 p
2 d
3 f
4 g
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- Nú Númer meroo quâ quânt ntic icoo mag magné néti tico co,, m
está relacionado com a orientação da orbital no espaço. Estes valores são os números inteiros de –ℓ a +ℓ. Para cada valor de ℓ há (2ℓ + 1) valores de mℓ. Sign up to vote on this title
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- Nú Númer meroo quâ quânt ntic icoo mag magné néti tico co,, m
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- Nú Núme mero ro qu quân ânti tico co de sp spin in,, ms ms Está relacionado com o sentido de rotação do electrão Pode ter o valor de
½ ou -½
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- Nú Núme mero ro qu quân ânti tico co de sp spin in,, ms ms
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Quanto maior for o número quântic principal (n ), ), maior é a energia
E 3s
> E 2s Sign up to vote on this title
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Em átomos monoelectrónicos a energia da orbital só depende de n.
E 2s
= E 2P Sign up to vote on this title
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Em átomos polielectrónicos para um dado valor de n , quanto maior o número quântico azimutal (ℓ ), ), maior é a energia.
E 2P
> E 2S
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Orbitais com iguais números quânticos principal e azimutal têm a mesma energia.
E 2px
= E 2py = E 2pz Sign up to vote on this title
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Para átomos diferentes a energia e o tamanho de um dado tipo de orbital são diferentes.
Ex.: A orbital 1s do sódio (11Na) tem maio energia que a orbital 1s do potássio (19K), pois sendo a carga nuclear do potássio maior, o electrão está mais atraído para o núcleo, sendo menos energético . Sign up to vote on this title Useful
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PRINCÍPIO DA ENERGIA MÍNIMA PRINCÍPIO DE EXCLUSÃO DE PAULI
REGRA DE HUND
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PRINCÍPIO DA ENERGIA MÍNIMA Os electrões deverão ocupar orbitais respeitando a orde crescente de energias até todas orbitais esta tarrem complet etaas. Sign up to vote on this title
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PRINCÍPIO DE EXCLUSÃO DE PAU Apenas dois electrões pode exist na mesma orbital atómica e est electrões têm de ter spins opostos. Sign up to vote on this title Useful
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REGRA DE HUND No preenchimento de orbitais com mesma energia distribui-se primeiro u electrão por cada orbital. Só seguida se faz o emparelhamento. Sign up to vote on this title Useful
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Nº de electrõ na orbital
Número quântico de momento angular, l
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2 2s2 2p6 3s1 – Na 1s 11
4 estados de energia
O electrão que requer menos energia para ser removido é o electrão 3s1, pois está mais fracamente ligado ao núcleo. Sign up to vote on this title
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Seguem-se por ordem decrescente d dificuldade os electrões 2p6 , 2s2 e 1
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