Question

Answer true or false. (a) To say that "energy is quantized" means that only certain energy values are allowed. (b) Bohr discovered that the energy of an electron in an atom is quantized. (c) Electrons in atoms are confined to regions of space called "principal energy levels." (d) Each principal energy level can hold a maximum of two electrons. (e) An electron in a 1 s orbital is held closer to the nucleus than an electron in a $2 s$ orbital. (f) An electron in a 2s orbital is harder to remove from an atom than an electron in a 1 s orbital. (g) An sorbital has the shape of a sphere, with the nucleus at the center of the sphere. (h) Each $2 p$ orbital has the shape of a dumbbell, with the nucleus at the midpoint of the dumbbell. (i) The three $2 p$ orbitals in an atom are aligned parallel to each other. (j) An orbital is a region of space that can hold two electrons. (k) The second shell contains one $s$ orbital and three $p$ orbitals. (1) In the ground-state electron configuration of an atom, only the lowest-energy orbitals are occupied. $(\mathrm{m}) \mathrm{A}$ spinning electron behaves as a tiny bar magnet, with a North Pole and a South Pole. (n) An orbital can hold a maximum of two electrons with their spins paired. (o) Paired electron spins means that the two electrons are aligned with their spins North Pole to North Pole and South Pole to South Pole. (p) $A n$ orbital box diagram puts all of the electrons of an atom in one box with their spins aligned. (q) An orbital box diagram of a carbon atom shows two unpaired electrons. (r) A Lewis dot structure shows only the electrons in the valence shell of an atom of the element. (s) A characteristic of Group 1A elements is that each has one unpaired electron in its outermost occupied (valence) shell. (t) A characteristic of Group 6A elements is that each has six unpaired electrons in its valence shell.

Name: Problem 42, Chapter 2: Introduction to General, Organic and Biochemistry
Uploaded: 2021-02-01T01:28:58-08:00
Duration: 22 min 57 s
Channel: Niamat Khuda

   Answer true or false.
(a) To say that "energy is quantized" means that only certain energy values are allowed.
(b) Bohr discovered that the energy of an electron in an atom is quantized.
(c) Electrons in atoms are confined to regions of space called "principal energy levels."
(d) Each principal energy level can hold a maximum of two electrons.
(e) An electron in a 1 s orbital is held closer to the nucleus than an electron in a $2 s$ orbital.
(f) An electron in a 2s orbital is harder to remove from an atom than an electron in a 1 s orbital.
(g) An sorbital has the shape of a sphere, with the nucleus at the center of the sphere.
(h) Each $2 p$ orbital has the shape of a dumbbell, with the nucleus at the midpoint of the dumbbell.
(i) The three $2 p$ orbitals in an atom are aligned parallel to each other.
(j) An orbital is a region of space that can hold two electrons.
(k) The second shell contains one $s$ orbital and three $p$ orbitals.
(1) In the ground-state electron configuration of an atom, only the lowest-energy orbitals are occupied.
$(\mathrm{m}) \mathrm{A}$ spinning electron behaves as a tiny bar magnet, with a North Pole and a South Pole.
(n) An orbital can hold a maximum of two electrons with their spins paired.
(o) Paired electron spins means that the two electrons are aligned with their spins North Pole to North Pole and South Pole to South Pole.
(p) $A n$ orbital box diagram puts all of the electrons of an atom in one box with their spins aligned.
(q) An orbital box diagram of a carbon atom shows two unpaired electrons.
(r) A Lewis dot structure shows only the electrons in the valence shell of an atom of the element.
(s) A characteristic of Group 1A elements is that each has one unpaired electron in its outermost occupied (valence) shell.
(t) A characteristic of Group 6A elements is that each has six unpaired electrons in its valence shell.

Introduction to General, Organic and Biochemistry

Frederick A.… 12th Edition

Chapter 2, Problem 42

Instant Answer

Solved by Expert Niamat Khuda

02/01/2021

Step 1

This is because electrons occupy orbitals of fixed energy and fractional values of orbitals are not possible. Therefore, the statement is **True**. Show more…

Show all steps

Thanks for your feedback!

Answer true or false. (a) To say that "energy is quantized" means that only certain energy values are allowed. (b) Bohr discovered that the energy of an electron in an atom is quantized. (c) Electrons in atoms are confined to regions of space called "principal energy levels." (d) Each principal energy level can hold a maximum of two electrons. (e) An electron in a 1 s orbital is held closer to the nucleus than an electron in a $2 s$ orbital. (f) An electron in a 2s orbital is harder to remove from an atom than an electron in a 1 s orbital. (g) An sorbital has the shape of a sphere, with the nucleus at the center of the sphere. (h) Each $2 p$ orbital has the shape of a dumbbell, with the nucleus at the midpoint of the dumbbell. (i) The three $2 p$ orbitals in an atom are aligned parallel to each other. (j) An orbital is a region of space that can hold two electrons. (k) The second shell contains one $s$ orbital and three $p$ orbitals. (1) In the ground-state electron configuration of an atom, only the lowest-energy orbitals are occupied. $(\mathrm{m}) \mathrm{A}$ spinning electron behaves as a tiny bar magnet, with a North Pole and a South Pole. (n) An orbital can hold a maximum of two electrons with their spins paired. (o) Paired electron spins means that the two electrons are aligned with their spins North Pole to North Pole and South Pole to South Pole. (p) $A n$ orbital box diagram puts all of the electrons of an atom in one box with their spins aligned. (q) An orbital box diagram of a carbon atom shows two unpaired electrons. (r) A Lewis dot structure shows only the electrons in the valence shell of an atom of the element. (s) A characteristic of Group 1A elements is that each has one unpaired electron in its outermost occupied (valence) shell. (t) A characteristic of Group 6A elements is that each has six unpaired electrons in its valence shell.

Play audio

Feedback

Niamat Khuda and 82 other subject Chemistry 101 educators are ready to help you.

Ask a new question

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Orbital Diagrams and Electron Configuration

Orbital diagrams are pictorial representations that show how electrons occupy orbitals in an atom. They incorporate principles like the Aufbau principle, Hund's rule, and the Pauli exclusion principle to indicate the distribution of electrons and their spins in various orbitals within an atom.

Periodic Table Groups and Valence Electrons

Elements in the periodic table are grouped based on similar properties, which are often related to the number of valence electrons in their outermost shell. The behavior of these electrons explains trends in reactivity, bonding patterns, and other chemical properties, making this concept critical in understanding the periodic table and chemical interactions.

Electron Spin

Electron spin is an intrinsic property of electrons that gives rise to a magnetic moment. It can be considered as a type of angular momentum with two possible orientations. The concept of electron spin is crucial for understanding magnetic properties and plays a role in the formation of electron pairs in orbitals.

Orbital Capacity and the Pauli Exclusion Principle

An orbital can hold a maximum of two electrons, provided they have opposite spins. This restriction is a result of the Pauli exclusion principle, which states that no two electrons in an atom can have the same set of quantum numbers, ensuring that electrons are arranged in a specific and structured way.

Lewis Dot Structures

Lewis dot structures are simplified diagrams that depict the valence electrons of an atom or a molecule. They are used to represent chemical bonds and the reactivity of atoms in compounds, focusing primarily on the electrons involved in bonding rather than the full electron configuration.

Electron Orbitals

Electron orbitals are regions in space where there is a high probability of finding an electron. Each orbital is characterized by distinct shapes and energies, and the type of orbital (e.g., s, p, d, f) impacts its geometry. This concept is essential for understanding chemical bonding, electron configuration, and the physical properties of atoms.

Atomic Models

Atomic models, such as the Bohr model, were developed to explain the behavior and arrangement of electrons in an atom. They incorporate the quantization of energy and introduce the idea that electrons occupy defined energy levels or shells, which was a major departure from classical models and helped lay the foundation for modern quantum theory.

Quantization of Energy

This concept refers to the idea that certain physical properties, like the energy of electrons in atoms, can only take on discrete values rather than a continuous range. It is fundamental in quantum mechanics and explains phenomena such as specific electron orbits, atomic spectra, and the stability of atoms.

Electron Shells and Subshells

Atoms have electron shells, denoted by principal quantum numbers, that correspond to different energy levels. Each shell contains one or more subshells (e.g., s, p, d, f) which consist of orbitals. These layers determine the electron configuration of an atom and are key to predicting chemical behavior and periodic trends.

Recommended Videos

Transcript

00:01 Hey guys, let's do problem 42.

00:04 In this problem, some statements are given.

00:07 We need to answer if these are true or false.

00:10 The first statement says energy is quantized, meaning that only certain energy values are allowed.

00:17 We know that electrons occupy orbitals of certain fixed energy.

00:24 Electrons occupy orbitals of fixed energy and the fractional value of orbitance is not possible.

00:41 Therefore, this is a true statement that energy is quantized.

00:46 Then the second one says, boat discovered that energy of an electron in an atom is quantized.

00:53 Since electron does not move freely around this space, which are around the nucleus, the electrons move in a fixed orbital, and these orbitals are having fixed energy.

01:08 So electrons move in fixed orbitals of certain energy.

01:28 Therefore, the energy of the electrons in an atom is quantized and this one is a true statement.

01:36 Then the third statement says, electrons in atom are confined to regions of space called principal energy level.

01:46 Now there is a large space outside.

01:49 The nucleus but the electrons are confined to specific regions so electrons are confined to specific region and they do not freely move around the nucleus and these specific regions these are called principal energy level therefore this is also a true statement then d says each principal energy level can hold a maximum of two electrons.

02:29 We know that each principal energy levels they have different sub -shells and the subshells of the principal energy levels are s p d f where s can have maximum of two we can have six the d can have ten and if can have maximum of 14 electrons therefore the principal energy level can hold a maximum of 32 electrons and this statement is false.

03:05 Then e says an electron in 1s orbital is held closer to the nucleus than an electron in the 2s orbital.

03:15 The 1s orbital is the lies in the first principal energy level.

03:25 1 s orbital is in the principle is in the principle is in the first principal energy level and the 2 s orbital is in the second principal energy level the first principal energy level is closer to the nucleus compared to the second principal energy level therefore the 1 s orbital is closer to the nucleus then the then the electrons in the second orbital so this one is a true statement then f says an electron in a 2s orbital is harder to remove from an atom than an electron in the 1s orbital.

04:31 Since the 1s electrons, these are closer to the nucleus, therefore nucleus attracts these electrons in the 1s orbital way more strongly.

04:46 Since 1s orbital is closer to the nucleus.

04:55 Then the 2s orbital therefore electrons in 1s orbital is attracted more strongly than electrons in 2s orbital and due to this strong attraction for electrons in the 1s orbital one s electrons are harder to remove therefore the statement f that is actually false then g says an s orbital has the shape of a spear with the nucleus at the center of this pair the shape of the orbiters they represent the electron density so shape of orbitals represent the electron density so shape of orbitals represent the electron density and this electron density is the probability of which is the probability of finding electrons now for s orbital the electron density is spherical around the nucleus for s orbital the electron density is spherical around the nucleus.

07:17 Therefore the shape of the s orbital is spherical and this one is a true statement.

07:25 Then h says that each 2p orbital has the shape of a dumbbell with the nucleus at the midpoint of the dumbbell.

07:35 Now for 2 orbital the electron density is dumbbell shaped and the nucleus remains at the middle.

07:43 So this statement is a true statement.

07:49 So for 2p orbitals, the electron density is a dumbbell shaped and the nucleus is on the midpoint.

08:10 Therefore, the 2p orbital is dumbled shaped.

08:15 Then the 3 2p orbitals in an atom are aligned parallel to each other.

08:20 This one is a false statement.

08:25 The 2p orbitals, they are not parallel to each other, they are at right angle to each other.

08:35 2p orbitals are right angle to each other.

08:48 So it is a false statement.

08:52 Then j says an orbital is a region of space that can hold two electrons.

08:59 In an atom, shells are divided into subshells and within these subshells, electrons are grouped in orbitals.

09:07 So within the sub -shells, electrons are grouped in orbitals.

09:25 And these orbitals hold can hold a maximum of two electrons.

09:33 Can hold maximum of two electrons.

09:37 Therefore, this one again is a true statement.

09:40 Then case is the second shell contains 1s orbital and 2 p orbitals the second shell it can hold a maximum of 8 electrons it can hold a maximum of 8 electrons and these electrons can occupy the 2s and the 2 p orbitals 2 s orbital is a single s orbital and it can hold 2 electrons and 2 p orbitals it consists of three sets of orbitals and can hold six electrons therefore the second shell can contain a maximum of two plus six which is the eight electrons it can hold maximum of eight electrons and therefore the second shell contains one s orbital and three p orbitals and this one is a true statement.

11:14 Then l says in the ground state electron configuration of an atom only the lowest energy orbitals are occupied.

11:23 The electron configuration of an atom, it gives the description of the orbitals in which the electrons occupy.

11:31 So, electron configuration gives the description of the orbital in which the electrons occupy.

11:55 In the ground state electron configuration electrons occupy the orbitance which are having the lowest energy and all the orbitals of higher energy remain empty.

12:09 In ground state, in electron configuration electron occupy orbitals of lower energy.

12:31 Therefore this one is the true statement.

12:36 Then the statement m says that and spinning electron behave as a tiny bar magnet with a north pole and a south pole.

12:48 A spinning electron produces a tiny magnetic field around it and aligns itself in the north and south direction.

12:59 So, spinning electron creates a tiny magnetic field and align itself in the north and south direction.

13:31 And south direction.

13:35 Therefore a spinning electron is considered as a tiny magnet with a north pole and a south pole and m is a true statement...

Ace is your personal tutor. It breaks down any question with clear steps so you can learn.

Start Using Ace

Continue solving this problem

Create a free account to:

View full step-by-step solution
Ask follow-up questions with Ace AI
Save progress and study later

Please give Ace some feedback