Flashcards
Chapter 5- Electrons and bonding: electronic structure
Cards in this deck (22)
- 1number of electrons that can fit in each shell-shell 1 = 2e
-shell 2 = 8e
-shell 3 = 18e
-shell 4 = 32e - 2atomic orbitalregion around the nucleus that can hold
up to two electrons, with opposite spins - 3s orbital shape
- 4p orbital shape
- 5subshellsgroups of the same type of orbitals within a shell
- 6order of filling subshells1s 2s 2p 3s 3p 4s 3d 4p 4d 4f
- 7why does the 4s subshell come before the 3d sub shell?because the orbitals are filled according to increasing energy, and the 4s sub shell has a lower energy than the 3d subshell
- 8how many orbitals can be filled up in a s subshell?1
- 9so how many electrons can be held in a s subshell?2
- 10how many orbitals can there be in a p subshell?3
- 11so how many electrons can be held in a subshell?6
- 12how many orbitals can there be in a d subshell?5
- 13so how many electrons can occupy a d sub shell?10
- 14how many orbitals can there be in a f subshell?7
- 15so how many electrons can occupy a f subshell?14
- 16how do electrons fill a subshell up?a subshel has one energy because its same orbital, so electrons occupy each orbital singularly before pairing
- 17why do the electrons occupy shells singularly first?to prevent repulsion between paired electrons until theres no further orbital available at same energy level
- 18state the 3 ways you can write electronic configuration-subshell notation
-electrons in boxes
-shorthand notation (except cr or cu) - 19can use these methods for upto atomic number=36 (krypton). write subshell notation for kr36 e so:
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 - 20write box notation for kr
- 21write shorthand notation for kr[Ar] 3d10 4s2 4p6
- 22how would you wor out electronicconfig of ions?just add or substract however many electrons gained/loss
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- A level Chemistry (Module 2 Foundations in Chemistry) Flashcards on Chapter 5- Electrons and bonding: electronic structure, created by Mehak Zahrah Faheem on 02/12/2018.
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- Mehak Zahrah Faheem
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