Concept explainers
Interpretation:
The correct ground state electron configuration for
Concept Introduction:
General rules for writing electron configuration are asfollows:
Electrons will reside in the available orbitals of lowest possible energy.
Each orbital can accommodate a maximum of two electrons.
Electrons will not pair in degenerate orbitals if an empty orbital is available.
Orbitals will fill in order of increasing energy
s-orbital can have 0–2 electrons
p-orbital can have 0–6 electrons
d-orbital can have 0–10 electrons
f-orbital can have 0–14 electrons
In electron configuration, noble gas symbol in brackets represents core electrons.
The number of electrons in a neutral atom is equal to its
In ions, the number of electrons is not equal to the atomic number of that atom.
It may be lesser or greater than the atomic number.
A cation contains less number of electrons than the atomic number of the atom.
Anions contain more number of electrons than theatomic number of the atom.
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Chemistry
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- For each of the atoms below, 1) write its ground state electron configuration, 2) draw the diagram depicting the electron occupancy in the highest-energy subshell, and 3) predict whether it is paramagnetic or diamagnetic. Example: B 1) 1s2s22p! or [He]2s²sp! 2) 2p 3) It is paramagnetic. a) Si b) Ni c) Pd (Hint: the highest-energy subshell fills like Ag)arrow_forwardHow many valence electrons are present in the ground state electro configuration? 1s²2s²2p°3s?3p* O 2 0 6 16 04arrow_forwardWhich of the following electron configurations belongs to a diamagnetic species? * a) [Ar] 4s² 3d⁴ b) [Ne] 3s² 3p² c) [Ar] 4s² 3d¹⁰ d) [He] 2s² 2p³ e) None of these electron configurations belongs to a diamagnetic species.arrow_forward
- Question 4 For each of the atoms below, 1) write its ground state electron configuration, 2) draw the diagram depicting the electron occupancy in the highest-energy subshell, and 3) predict whether it is paramagnetic or diamagnetic. Example: B 1) 1s2s22p' or [He]2s²sp! 2) 2p 3) It is paramagnetic. a) Si (3 pt) b) Ni (3 pt) c) Pd (4 pt) (Hint: the highest-energy subshell fills like Ag)arrow_forward(ELECTRONIC STRUCTURE AND CHEMICAL BONDING Understanding periodic trends in effective nuclear charge Rank the effective nuclear charge Z experienced by a valence electron in each of these atoms: atom An atom of palladium. An atom of molybdenum. An atom of cadmium. An atom of niobium. z experienced by a valence electron. (pick one) (pick one) (pick one) ✓ (pick one) X Śarrow_forwardQuestion 41 Choose the elemental ground state electron configuration for P. O [Ne] 3s²3p4 O [Ne] 3s23p³ O [Ne] 3s¹3p4 O [Ne] 3s²3p²arrow_forward
- What is the ground-state electron configuration of Al (atomic number 13)? 15² 25² 2p 3s¹ 15²2² 2s²2p6 35³ 152² 25² 2p 3s² 3p¹ 2s²2p8 35² 3p¹ 25² 2p 3s² 3p³arrow_forwardQUESTION 28 Match the following elements/ions with the proper ground state electronic configurations Na A. 1s2 2s2 2p6 Ineon B. [Xe] fluoride C. calcium hafnium E. [Xej 6s2 4114 5a9 1s2 252 2p6 3s2 3d10 4p6 (Xe] 6s2 4f14 5d2 1s2 2p6 3s1 [ 1s2 252 2p6 11 K. [Kr] 5s2 4d10 5p6 QUESTION 29arrow_forwarddetermine the correct ground state electron configuration. I⁻arrow_forward
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