1.7- The Shrodinger model of the atom

Question 1

Three things Bohr’s model could not explain

Answer 1

1) cannot accurately predict the emission spectra of atoms with more than one electron.
2) is unable to explain why electron shells can only hold 2n squared electrons
3) does not explain why the fourth shell accepts two electrons before the third shell is completely filled

Question 2

what does the word quantum mean?

Answer 2

a specific amount

the energy of an electron is said to be quantised

Question 3

what is quantum mechanics?

Answer 3

describes the behaviour of extremely small particles like electrons, behaves as waves around the nucleus

Question 4

difference between the Schrodinger and Bohr’s model

Answer 4

• way they viewed electrons
• Bohr = tiny hard particles that revolves around the nucleus in circular orbitals
• Schrodinger = having wave like properties. electrons occupy three dimensional space around the nucleus known as the orbital.

Question 5

5 things Schrodingers theory on electrons having wave like properties helped find.

Answer 5

1) there are major energy levels in an atom that for historical reasons were called shells.
2) These shells contain separate energy levels of similar energy, called subshells (which he labelled s,p,d,f)
3) the first shell (n=1) contains only an s subshell, 2nd = s and p, 3rd = s,p,d and so on
4) each subshell is made up of smaller components called orbitals
5) the total number of shells in a shell I’m given by n squared

Question 6

two rules for subshell electronic configuration

Answer 6

1) lowest energy orbitals are always filled first

2) each orbital contains a maximum of two electrons

Question 7

what two elements are an exception to the electronic configuration

Answer 7

element 24 chromium

element 29 copper

Question 8

actual configuration of chromium Cr

Answer 8

1s(2), 2s(2) 2p(6) 3s(2) 3p(6) 3d(5) 4s(1)

Question 9

actual configuration of Copper Cu

Answer 9

1s(2) 2s(2) 2p(6) 3s(2) 3p(6) 3d(10) 4s(1)