Problem 85 Write each element's orbital not... [FREE SOLUTION]

Chapter 5: Problem 85

Write each element's orbital notation and complete electron configuration. $$\begin{array}{ll}{\text { a. beryllium }} & {\text { c. nitrogen }} \\\ {\text { b. aluminum }} & {\text { d. sodium }}\end{array}$$

Short Answer

Expert verified

Beryllium: 1s虏 2s虏; Aluminum: 1s虏 2s虏 2p鈦� 3s虏 3p鹿; Nitrogen: 1s虏 2s虏 2p鲁; Sodium: 1s虏 2s虏 2p鈦� 3s鹿.

Step by step solution

Understanding Orbital Notation and Electron Configuration

Orbital notation represents electrons using arrows to indicate their spin within each orbital, while electron configuration describes the distribution of electrons among the orbitals using numbers and letters. Each element has a unique electron arrangement based on its atomic number.

Beryllium (Be)

Beryllium has an atomic number of 4, meaning it has 4 electrons. - **Orbital Notation**: The electrons fill the 1s, then 2s orbitals. - 1s: 鈫戔啌 - 2s: 鈫戔啌 - **Electron Configuration**: 1s虏 2s虏

Aluminum (Al)

Aluminum has an atomic number of 13, meaning it has 13 electrons. - **Orbital Notation**: The electrons fill the 1s, 2s, 2p, 3s, and part of 3p orbitals. - 1s: 鈫戔啌 - 2s: 鈫戔啌 - 2p: 鈫戔啌鈫戔啌鈫戔啌 - 3s: 鈫戔啌 - 3p: 鈫� - **Electron Configuration**: 1s虏 2s虏 2p鈦� 3s虏 3p鹿

Nitrogen (N)

Nitrogen has an atomic number of 7, meaning it has 7 electrons. - **Orbital Notation**: The electrons fill the 1s, 2s, and part of 2p orbitals. - 1s: 鈫戔啌 - 2s: 鈫戔啌 - 2p: 鈫� 鈫� 鈫� - **Electron Configuration**: 1s虏 2s虏 2p鲁

Sodium (Na)

Sodium has an atomic number of 11, meaning it has 11 electrons. - **Orbital Notation**: The electrons fill the 1s, 2s, 2p, and part of 3s orbitals. - 1s: 鈫戔啌 - 2s: 鈫戔啌 - 2p: 鈫戔啌鈫戔啌鈫戔啌 - 3s: 鈫� - **Electron Configuration**: 1s虏 2s虏 2p鈦� 3s鹿

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Orbital Notation

Orbital notation is a way to represent the arrangement of electrons in an atom. It visually illustrates where each electron may be located and includes information about their energy levels and spin direction.

Electrons are represented by arrows. Each arrow indicates an electron's spin, either upwards or downwards. For example, a spin-up electron is depicted as 鈫�, while a spin-down electron is shown as 鈫�.

In orbital notation:

Each box corresponds to an orbital (a space where electrons are likely to be found).
Electrons are filled into orbitals in a specific order based on increasing energy, known as the Aufbau principle.
Orbitals are filled singly first before pairing up, which is guided by Hund's rule.

Atomic Number

The atomic number is a unique identifier for each element on the periodic table. It denotes the number of protons in the nucleus of an atom. Remarkably, it's also equal to the number of electrons in a neutral atom.

Understanding the atomic number is crucial for determining the electron configuration of an element:

The atomic number determines an element's place in the periodic table.
It allows chemists to predict the chemical behavior of an element.
As the atomic number increases, it translates to more electrons, which occupy higher energy levels around the nucleus.

Each change in the atomic number results in the presence of a new element with unique properties.

Electron Distribution

Electron distribution, or electron configuration, refers to the way electrons are situated around the nucleus of an atom. Electrons occupy orbitals, and each orbital can hold a certain number of electrons: s can hold 2, p can hold 6, d can hold 10, and f can hold 14.

Key points about electron distribution:

Electrons fill orbitals starting from the lowest energy level to the highest.
The arrangement follows the principle of the Aufbau process, with electrons filling 3s before 3p and so forth.
Electron configurations dictate the chemical, magnetic, and structural properties of atoms.

This distribution is pivotal in predicting how an atom will bond or interact with others chemically.

Quantum Chemistry

Quantum chemistry involves the application of quantum mechanics to chemical systems, providing insights into the underlying principles that govern the behavior of electrons in atoms and molecules.

Quantum chemistry helps us understand:

Why electrons occupy specific orbitals and how these relate to the energy levels.
The dual nature of electrons, behaving both as particles and waves.
The probability distribution of electrons within an atom, which allows us to predict the likelihood of finding an electron in a particular zone around the nucleus.

Through quantum chemistry, we can predict reactions, the energy required to disrupt bonds, and the shape of molecules.

91影视

Write each element's orbital notation and complete electron configuration. $$\begin{array}{ll}{\text { a. beryllium }} & {\text { c. nitrogen }} \\\ {\text { b. aluminum }} & {\text { d. sodium }}\end{array}$$

Short Answer

Step by step solution

Understanding Orbital Notation and Electron Configuration

Beryllium (Be)

Aluminum (Al)

Nitrogen (N)

Sodium (Na)

Key Concepts

Orbital Notation

Atomic Number

Electron Distribution

Quantum Chemistry

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