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Chapter 7: Problem 77

Draw atomic orbital diagrams representing the ground-state electron configuration for each of the following elements. a. \(\mathrm{Na}\) b. \(\mathrm{Co}\) c. \(\mathrm{Kr}\) How many unpaired electrons are present in each element?

Short Answer

Expert verified
The ground-state electronic configurations for the given elements are as follows: a. Sodium (Na) has 1 unpaired electron in its 3s orbital. b. Cobalt (Co) has 3 unpaired electrons in its 3d orbitals. c. Krypton (Kr) has no unpaired electrons in its ground state.

Step by step solution

01

Determine the number of electrons for each element

Using the periodic table, we can find the atomic number of each element, which also represents the number of electrons in its neutral state. The atomic numbers are: a. Na: 11 b. Co: 27 c. Kr: 36
02

Determine the electron filling order using aufbau principle

Following the aufbau principle, determine the order in which the electrons will fill the orbitals. We can use the standard electron filling notation: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p... We will fill the electrons according to the elements we have (Na = 11, Co = 27, Kr = 36).
03

Construct the orbital diagrams

Using Hund's rule, construct the orbital diagrams for Na, Co, and Kr, filling electrons from lowest energy to highest. a. Sodium (Na: 11 electrons) 1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑ b. Cobalt (Co: 27 electrons) 1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑↓ 3p: ↑↓ ↑↓ ↑↓ 4s: ↑↓ 3d: ↑ ↑ ↑ ↑ ↑ ↑↓ ↑↓ c. Krypton (Kr: 36 electrons) 1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ 3s: ↑↓ 3p: ↑↓ ↑↓ ↑↓ 4s: ↑↓ 3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 4p: ↑↓ ↑↓ ↑↓
04

Count unpaired electrons

Now, count the unpaired electrons for each element: a. Sodium (Na): 1 unpaired electron b. Cobalt (Co): 3 unpaired electrons c. Krypton (Kr): 0 unpaired electrons The ground-state electronic configurations for these elements are as follows: a. Sodium (Na) has 1 unpaired electron in its ground state. b. Cobalt (Co) has 3 unpaired electrons in its ground state. c. Krypton (Kr) has no unpaired electrons in its ground state.

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Most popular questions from this chapter

The elements \(\mathrm{Cu}, \mathrm{O}, \mathrm{La}, \mathrm{Y}, \mathrm{Ba}, \mathrm{Tl}\), and \(\mathrm{Bi}\) are all found in high- temperature ceramic superconductors. Write the expected electron configuration for these atoms.

The electron affinities of the elements from aluminum to chlorine are \(-44,-120,-74,-200.4\), and \(-384.7 \mathrm{~kJ} / \mathrm{mol}\), respectively. Rationalize the trend in these values.

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. \(1 s^{2} 2 s^{2} 3 p^{1}\) b. \(1 s^{2} 2 s^{2} 2 p^{6}\) c. \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\) How many unpaired electrons are present in each of these species?

Write the expected electron configurations for each of the following atoms: \(\mathrm{Sc}, \mathrm{Fe}, \mathrm{P}, \mathrm{Cs}\), Eu, \(\mathrm{Pt}, \mathrm{Xe}, \mathrm{Br}\).

One bit of evidence that the quantum mechanical model is "correct" lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit paramagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for \(\mathrm{Li}, \mathrm{N}, \mathrm{Ni}, \mathrm{Te}, \mathrm{Ba}\), and \(\mathrm{Hg} .\) Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
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