Question

How many \(2 p\) electrons are in an atom of each element? (a) \(\mathrm{C}\) (b) \(\mathrm{N}\) (c) \(\mathrm{F}\) (d) \(\mathrm{P}\)

Short answer

The number of 2p electrons for each element is: (a) Carbon (C) - 2, (b) Nitrogen (N) - 3, (c) Fluorine (F) - 5, (d) Phosphorus (P) - 6.

Step-by-step solution

Recall the electron configuration principle

The electron configuration of an element describes the distribution of electrons in the atomic orbitals. For elements in the periodic table, electrons fill from lower to higher energy orbitals in the sequence 1s, 2s, 2p, 3s, 3p, and so on.

Identify the 2p electrons for Carbon (C)

Carbon has an atomic number of 6, which means it has 6 electrons. The electron configuration of Carbon is 1s^2 2s^2 2p^2. The number of 2p electrons in a Carbon atom is the exponent of 2p in its electron configuration, which is 2.

Identify the 2p electrons for Nitrogen (N)

Nitrogen has an atomic number of 7, which means it has 7 electrons. The electron configuration of Nitrogen is 1s^2 2s^2 2p^3. Therefore, the number of 2p electrons in a Nitrogen atom is 3.

Identify the 2p electrons for Fluorine (F)

Fluorine has an atomic number of 9, meaning it has 9 electrons. The electron configuration of Fluorine is 1s^2 2s^2 2p^5. Thus, the number of 2p electrons in a Fluorine atom is 5.

Identify the 2p electrons for Phosphorus (P)

Phosphorus has an atomic number of 15, which means it has 15 electrons. The electron configuration of Phosphorus is 1s^2 2s^2 2p^6 3s^2 3p^3. All 2p orbitals are filled with electrons, so the number of 2p electrons in a Phosphorus atom is 6.

Key concepts

Atomic Orbitals

The wonders of chemistry often begin with understanding the intricate patterns of electrons as they occupy specific areas around an atom's nucleus, known as atomic orbitals. These represent the probable locations where electrons may be found. It’s beneficial to think of them as defined spaces within an atom that accommodate electron pairs. The most basic types are designated as s, p, d, and f orbitals, each with a unique shape and energy level.

To visualize this, imagine the s orbital as a sphere around the nucleus, while the p orbitals resemble dumbbells extending in three dimensions which are mutually perpendicular. Electrons fill these orbitals, starting at the lowest energy, which is the 1s orbital, followed by the 2s, 2p, and so on, moving to higher energy orbitals as the atom becomes larger. The concept of atomic orbitals is vital when mapping out an element's electron structure, and understanding how these orbitals are filled is key to grasping the behavior of different elements.

2p Electrons

Moving one step further in electron configuration, 2p electrons are those that occupy the second energy level's p orbital. The p orbital can hold up to six electrons, with three sub-orbitals (2p_x, 2p_y, and 2p_z) hosting a pair each. These electrons play a significant role in chemical bonding and reactions.

For instance, in the Steps of Solution, the number of 2p electrons in elements like Carbon (C), Nitrogen (N), and Fluorine (F) was determined by the exponent of 2p in their electron configuration. This knowledge is crucial as the chemical properties of an element, such as its valency and the type of bonds it can form, are largely determined by the arrangement of its 2p electrons.

Periodic Table Elements

The Periodic Table is a master chart of elements, meticulously organized based on atomic number, electron configurations, and recurring chemical properties. Elements in the same column, or group, typically share similar characteristics. Periodic Table Elements are not just mere listings but a gateway to understanding the behaviors and relationships between different atoms.

As you delve into the table, you’ll notice it’s divided into blocks corresponding to the outer electron configurations – with the p-block including elements which have their last electron entering a p orbital. The steps to determine how many 2p electrons are present in various elements are guided by the principles that this table lays down. Fluorine (F), in the exercise given, is a p-block element and follows the configuration patterns typical for that section of the table.

Atomic Number

At the very heart of the Periodic Table lies the Atomic Number, a fundamental characteristic of an element. It is the total number of protons found in the nucleus of an atom and is unique for each element. The atomic number not only identifies the element but also dictates the number of electrons in a neutrally charged atom, which in turn influences the electron configuration.

As seen in the solution steps, the atomic numbers for Carbon (6), Nitrogen (7), Fluorine (9), and Phosphorus (15) dictated the total number of electrons and helped to establish their respective electron configurations. Knowing the atomic number immediately gives you a head start on predicting the electron arrangement and the properties of an element that follow from it.