Fundamentals of General, Organic, and Biological Chemistry (8th Edition)
Fundamentals of General, Organic, and Biological Chemistry (8th Edition)
8th Edition
ISBN: 9780134015187
Author: John E. McMurry, David S. Ballantine, Carl A. Hoeger, Virginia E. Peterson
Publisher: PEARSON
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Chapter 2.8, Problem 2.19P

(a)

Interpretation Introduction

Interpretation:

The electronic configuration of fluorine should be identified.

Concept introduction:

The periodic table is given below,

Fundamentals of General, Organic, and Biological Chemistry (8th Edition), Chapter 2.8, Problem 2.19P , additional homework tip  1

Electronic configuration:

The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

  1. (1) Electrons occupy in the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f. The lowest energy orbital is 1s. The order of energy of the orbital for the for the first three period is given below,

    1s, 2s, 2p, 3s,and 3p.

  2. (2) The orbital which is closer to the nucleus has lower energy, therefore the 2s is lower in energy than 3s. Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.
  3. (3) In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below, 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

s-Block element:

It is called as main group elements that result from the filling of an s orbital.

p-Block element:

It is also called as main group elements that result from the filling of an p orbital.

d-Block element:

It is called as transition metal elements that result from the filling of an p orbital.

f-Block element:

It is called as inner transition metal element that results from the filling of an p orbital.

(b)

Interpretation Introduction

Interpretation:

The electronic configuration of aluminium should be identified.

Concept introduction:

The periodic table is given below,

Fundamentals of General, Organic, and Biological Chemistry (8th Edition), Chapter 2.8, Problem 2.19P , additional homework tip  2

Electronic configuration:

The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

  1. (1) Electrons occupy in the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f. The lowest energy orbital is 1s. The order of energy of the orbital for the for the first three period is given below,

    1s, 2s, 2p, 3s,and 3p.

  2. (2) The orbital which is closer to the nucleus has lower energy, therefore the 2s is lower in energy than 3s. Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.
  3. (3) In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below, 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

s-Block element:

It is called as main group elements that result from the filling of an s orbital.

p-Block element:

It is also called as main group elements that result from the filling of an p orbital.

d-Block element:

It is called as transition metal elements that result from the filling of an p orbital.

f-Block element:

It is called as inner transition metal element that results from the filling of an p orbital.

(c)

Interpretation Introduction

Interpretation:

The electronic configuration of Arsenic should be identified.

Concept introduction:

The periodic table is given below,

Fundamentals of General, Organic, and Biological Chemistry (8th Edition), Chapter 2.8, Problem 2.19P , additional homework tip  3

Electronic configuration:

The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

  1. (1) Electrons occupy in the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f. The lowest energy orbital is 1s. The order of energy of the orbital for the for the first three period is given below,

    1s, 2s, 2p, 3s,and 3p.

  2. (2) The orbital which is closer to the nucleus has lower energy, therefore the 2s is lower in energy than 3s. Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.
  3. (3) In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below, 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

s-Block element:

It is called as main group elements that result from the filling of an s orbital.

p-Block element:

It is also called as main group elements that result from the filling of an p orbital.

d-Block element:

It is called as transition metal elements that result from the filling of an p orbital.

f-Block element:

It is called as inner transition metal element that results from the filling of an p orbital.

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Chapter 2 Solutions

Fundamentals of General, Organic, and Biological Chemistry (8th Edition)

Ch. 2.4 - Prob. 2.9PCh. 2.5 - Prob. 2.10PCh. 2.5 - Prob. 2.11PCh. 2.5 - Prob. 2.12PCh. 2.5 - Prob. 2.13KCPCh. 2.5 - Prob. 2.3CIAPCh. 2.5 - Prob. 2.4CIAPCh. 2.6 - Prob. 2.14PCh. 2.7 - Prob. 2.15PCh. 2.7 - Write electron configurations for the following...Ch. 2.7 - Prob. 2.17PCh. 2.7 - Identify the atom with the following...Ch. 2.8 - Prob. 2.19PCh. 2.8 - Prob. 2.20PCh. 2.8 - Prob. 2.21PCh. 2.8 - Prob. 2.22KCPCh. 2.9 - Prob. 2.23PCh. 2.9 - Write electron-dot symbols for radon, lead, xenon,...Ch. 2.9 - Prob. 2.25PCh. 2.9 - Prob. 2.5CIAPCh. 2.9 - Prob. 2.6CIAPCh. 2 - Where on the following outline of a periodic table...Ch. 2 - Is the element marked in red on the following...Ch. 2 - Prob. 2.28UKCCh. 2 - What atom has the following orbital-filling...Ch. 2 - Use the following orbital-filling diagram to show...Ch. 2 - What four fundamental assumptions about atoms and...Ch. 2 - How do atoms of different elements differ?Ch. 2 - Prob. 2.33APCh. 2 - Prob. 2.34APCh. 2 - Prob. 2.35APCh. 2 - Prob. 2.36APCh. 2 - How many O atoms of mass 15.99 amu are in 15.99 g...Ch. 2 - Prob. 2.38APCh. 2 - What are the names of the three subatomic...Ch. 2 - Prob. 2.40APCh. 2 - Prob. 2.41APCh. 2 - Prob. 2.42APCh. 2 - Which of the following symbols represent isotopes...Ch. 2 - Prob. 2.44APCh. 2 - Prob. 2.45APCh. 2 - Prob. 2.46APCh. 2 - One of the most widely used isotopes in medical...Ch. 2 - Prob. 2.48APCh. 2 - Prob. 2.49APCh. 2 - Prob. 2.50APCh. 2 - Prob. 2.51APCh. 2 - Prob. 2.52APCh. 2 - Prob. 2.53APCh. 2 - Prob. 2.54APCh. 2 - Prob. 2.55APCh. 2 - For (a) rubidium (b) tungsten, (c) germanium, and...Ch. 2 - For (a) calcium, (b) palladium, (c) carbon, and...Ch. 2 - Prob. 2.58APCh. 2 - Prob. 2.59APCh. 2 - Prob. 2.60APCh. 2 - Prob. 2.61APCh. 2 - Prob. 2.62APCh. 2 - Prob. 2.63APCh. 2 - Prob. 2.64APCh. 2 - Prob. 2.65APCh. 2 - Prob. 2.66APCh. 2 - Prob. 2.67APCh. 2 - Prob. 2.68APCh. 2 - Prob. 2.69APCh. 2 - Prob. 2.70APCh. 2 - Prob. 2.71APCh. 2 - Determine the number of unpaired electrons for...Ch. 2 - Without looking back in the text, write the...Ch. 2 - Prob. 2.74APCh. 2 - Prob. 2.75APCh. 2 - Prob. 2.76APCh. 2 - Prob. 2.77APCh. 2 - Prob. 2.78APCh. 2 - Using n for the number of the valence shell and...Ch. 2 - What elements in addition to helium make up the...Ch. 2 - Prob. 2.81CPCh. 2 - What is the atomic number of the yet-undiscovered...Ch. 2 - Give the number of electrons in each shell for...Ch. 2 - Identify the highest-energy occupied subshell in...Ch. 2 - Prob. 2.85CPCh. 2 - Prob. 2.86CPCh. 2 - Germanium, atomic number 32, is used in building...Ch. 2 - Prob. 2.88CPCh. 2 - Prob. 2.89CPCh. 2 - What is wrong with the following electron...Ch. 2 - Prob. 2.91CPCh. 2 - Prob. 2.92CPCh. 2 - Prob. 2.93CPCh. 2 - Prob. 2.94CPCh. 2 - Prob. 2.95GPCh. 2 - Prob. 2.96GPCh. 2 - Prob. 2.97GPCh. 2 - Look again at the trends illustrated in Figures...
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