CONCEPTUAL PHYSICAL SCIENCE(LL)-PACKAGE
CONCEPTUAL PHYSICAL SCIENCE(LL)-PACKAGE
6th Edition
ISBN: 9780134560762
Author: Hewitt
Publisher: PEARSON
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Textbook Question
Chapter 15, Problem 1RCQ

How many electrons can occupy the first shell? How many can occupy the second shell?

Expert Solution & Answer
Check Mark
To determine

The number of electrons that can occupy first shell and second shell.

Answer to Problem 1RCQ

Solution:

Two electrons can occupy the first shell and eight electrons can occupy the second shell.

Explanation of Solution

In structure of Atom, electrons are found inside the shells. The shells represents the primary energy levels of an atom. Each shell has a set of sub-shells which represents various energy levels of the shells. Each sub-shell (except s-subshell) has further divided on the basis of energy levels – which are called “orbitals”.

Quantum numbers illustrates the possible energy levels and sub-energy levels of an atom. The four types of quantum numbers are – Principal quantum number, Angular quantum number, Magnetic quantum number and Spin quantum number.

Principal quantum number correlates to the possible number of shells in an atom. It is designated as ‘n’. The shells are represented as numerical positive integers 1, 2, 3, etc or alphabetically – K, L, M, N etc.

Angular quantum number gives the energy levels within the shell – which is also known as sub-shells. It also represents the shape of the sub-shells. Accordingly K-shell has only one sub-shell termed as‘s’. L-subshell has 2 sub-shells that are‘s’ and ‘p’. M-shell has 3 sub-shells that are termed as‘s’, ‘p’ and‘d’ and so on.

Magnetic quantum number explains about the possible energy levels of the sub-shells. They are called “orbitals”.

Spin quantum number represents the spin of the electron that occupy in the orbital.

According to Aufbau’s principle, electrons are occupied from the lowest energy level to highest energy level.

According to Hund’s rule, electrons are singly occupied in all the orbitals of the sub-shells and all those electrons have parallel spin. After the electrons are singly occupied, electrons further occupy the singly filled orbitals with opposite spin. This relates to Pauli’s exclusion principle which states an orbital can have only two electrons which must have opposite spins with respect to each other.

Each orbital can accommodate two electrons of opposite spins. The first shell has one s-orbital and 2 electrons are occupied in it. The second shell has 2 sub-shells – s and p. Six electrons are occupied in the 3 p-orbitals as two electrons per p-orbital. Further the p-subshell also has an s-orbital and 2 electrons can be occupied there. Totally 8 electrons can occupy the second shell.

Conclusion:

The number of electrons that can occupy first shell and second shell have been determined

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Chapter 15 Solutions

CONCEPTUAL PHYSICAL SCIENCE(LL)-PACKAGE

Ch. 15 - What is an alloy?Ch. 15 - What is a native metal?Ch. 15 - Prob. 13RCQCh. 15 - Prob. 14RCQCh. 15 - Within a neutral molecule, how many covalent bonds...Ch. 15 - Prob. 16RCQCh. 15 - Prob. 17RCQCh. 15 - Prob. 18RCQCh. 15 - Prob. 19RCQCh. 15 - How can a molecule be nonpolar when it consists of...Ch. 15 - Why do nonpolar substances boil at relatively low...Ch. 15 - Which is more symmetrical: a polar molecule or a...Ch. 15 - Why dont oil and water mix?Ch. 15 - Prob. 24RCQCh. 15 - Which is stronger: the ion-dipole attraction or...Ch. 15 - What is a hydrogen bond?Ch. 15 - Are induced dipoles permanent?Ch. 15 - Prob. 31TASCh. 15 - What is the electric charge on the calcium ion in...Ch. 15 - Prob. 33TASCh. 15 - Prob. 34TASCh. 15 - Rank these bonds in order of increasing polarity:...Ch. 15 - Prob. 36TARCh. 15 - Prob. 37TARCh. 15 - Prob. 38TARCh. 15 - Prob. 39ECh. 15 - Prob. 40ECh. 15 - How many more electrons can fit within the valence...Ch. 15 - Prob. 42ECh. 15 - What happens when hydrogens electron gets close to...Ch. 15 - Prob. 44ECh. 15 - Why does an atom with few valence electrons tend...Ch. 15 - Why is it so easy for a magnesium atom to lose two...Ch. 15 - Why doesnt the neon atom tend to lose or gain any...Ch. 15 - Why does an atom with many valence electrons tend...Ch. 15 - Sulfuric acid, H2SO4, loses two protons to form...Ch. 15 - Prob. 50ECh. 15 - Which should be more difficult to pull apart: a...Ch. 15 - Prob. 52ECh. 15 - Given that the total number of atoms on our planet...Ch. 15 - An artist wants to create a metal sculpture using...Ch. 15 - Two fluorine atoms join together to form a...Ch. 15 - How are metallic bonds similar to ionic bonds? How...Ch. 15 - What drives an atom to form a covalent bond: its...Ch. 15 - Atoms of nonmetallic elements form covalent bonds,...Ch. 15 - Prob. 59ECh. 15 - Prob. 60ECh. 15 - Write the electron-dot structure for the covalent...Ch. 15 - Prob. 62ECh. 15 - In each molecule, which atom carries the greater...Ch. 15 - Which is more polar: a sulfur-bromine (S-Br) bond...Ch. 15 - True or False: The greater the nuclear charge of...Ch. 15 - True or False: The more shells in an atom, the...Ch. 15 - Water, H2O, and methane, CH4, have about the same...Ch. 15 - In the figure on the next page, the molecule from...Ch. 15 - Prob. 69ECh. 15 - Three kids sitting equally apart around a table...Ch. 15 - Which is stronger: the covalent bond that holds...Ch. 15 - The charges with sodium chloride are all...Ch. 15 - Prob. 73ECh. 15 - Prob. 74ECh. 15 - Prob. 75ECh. 15 - A thin stream of water is pulled to a rubber...Ch. 15 - Prob. 77ECh. 15 - Prob. 1RATCh. 15 - Prob. 2RATCh. 15 - Which would you expect to have a higher melting...Ch. 15 - Why are ores so valuable? (a) They are sources of...Ch. 15 - In terms of the periodic table, is there an abrupt...Ch. 15 - A hydrogen atom does not form more than one...Ch. 15 - When nitrogen and fluorine combine to form a...Ch. 15 - Prob. 8RATCh. 15 - Prob. 9RATCh. 15 - Iodine, I2, has a higher melting point than...
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