1) Write the electron configurations for the following atoms. Enter full electro
ID: 858528 • Letter: 1
Question
1) Write the electron configurations for the following atoms. Enter full electron configuration in order electrons fill the subshells. Enter subshells in parentheses followed by numbers of electrons in the exponent. For example you should enter "(1s)2(2s)2(2p)5" for atom of fluorine. The answer is case sensitive.
S:
K:
Ti:
Sn:
2) Give the correct electron configurations of Cr and Cu. Explain why they do not have the expected electron configurations.
These are the options for why they do not have the expected electron configurations:
3) What are the quantum numbers of the electrons that are lost by an atom of magnesium when it forms the ion Mg2+?
4) Imagine complete orbital diagrams for Mg and Ti. How many unpaired electrons are there in the ground state of each atom?
5) Which of the following atoms in their ground state are expected to be paramagnetic?
Mn
As
S
Sr
Ar
Half filled orbitals are more stable than partially filled orbitals.Explanation / Answer
1S16=(1s)2 (2s) 2 (2p)6 (3s)2 (3p)4
K19=(1s)2 (2s)2 (2p)6 (3s)2 (3p)6 (4s)1
Ti22=(1s)2 (2s)2 (2p)6 (3s)2 (3p)6 (4s)2(3d)2
Sn5o=(1s)2 (2s)2 (2p)6 (3s)2 (3p)6 (4s)2 (3d)10 (4p)6 (5s)2 (4d)10 (5p)2
2
Cr24=(1s)2 (2s)2 (2p)6 (3s)2(3p)6 (4s)1 (3d)5
Cu29=(1s)2 (2s)2(2p)6 (3s)2(3p)6(4s)1 (3d)10
because half filled& fully filled orbital are more stable
3>
Mg12=1s2,2s2,2p6,3s2
it losses its2 electron to form Mg2+
quantum no of these electron is given as
princple q. n. =3
angular q. n.l =0
magnetic q. n. =0
spin q. n.s -1/2,+1/2
4>
elec. configuration is given above .they have no unpaired electron
5>As, &S are paramagnetic
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