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Mobile App Chapter 8: Problem 60
Write the electron configuration for potassium.
Short Answer
Expert verified
The electron configuration for potassium is: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^1 \]
Step by step solution
01
Find the atomic number of potassium
Potassium is a chemical element with the symbol K. Look at the periodic table to find the atomic number of potassium, which is 19. This means that potassium has 19 electrons.
02
Determine the order of subshell orbitals
To write the electron configuration, we need to follow the order of subshell orbitals. This order can be found using the aufbau principle or by following the diagonal rule:
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
An s subshell can hold a maximum of 2 electrons, a p subshell can hold a maximum of 6 electrons, a d subshell can hold a maximum of 10 electrons, and an f subshell can hold a maximum of 14 electrons.
03
Distribute electrons in the subshell orbitals
We will distribute 19 electrons of potassium in the subshell orbitals following the order found in step 2. Here is the electron configuration:
1s²: Two electrons in the 1s subshell (total: 2)
2s²: Two electrons in the 2s subshell (total: 4)
2p⁶: Six electrons in the 2p subshell (total: 10)
3s²: Two electrons in the 3s subshell (total: 12)
3p⁶: Six electrons in the 3p subshell (total: 18)
4s¹: One electron in the 4s subshell (total: 19)
Since we have now assigned all 19 electrons, we can write the electron configuration for potassium in a compact form:
04
Write the final electron configuration
The complete electron configuration for potassium is:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^1 \]
This represents the distribution of electrons in different subshell orbitals of potassium.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Understanding the Periodic Table
When you're looking at the periodic table, you're not just seeing a random collection of elements; you're observing a highly organized chart that reflects the elements' atomic structures. It's designed to group elements with similar properties and showcases their increasing atomic number, which leads us directly to the concept of electron configurations.
For instance, columns, known as 'groups', share chemical properties due to their similar valence electron configurations. Going across a row or 'period', elements have additional shells as their atomic number increases. You might notice that elements like potassium, which have a higher atomic number, sit further to the right in the periodic table. This position correlates with its electron configuration, as potassium's additional electrons fill higher energy orbitals.
For instance, columns, known as 'groups', share chemical properties due to their similar valence electron configurations. Going across a row or 'period', elements have additional shells as their atomic number increases. You might notice that elements like potassium, which have a higher atomic number, sit further to the right in the periodic table. This position correlates with its electron configuration, as potassium's additional electrons fill higher energy orbitals.
The Aufbau Principle
The aufbau principle is a fundamental guideline used to determine the electron configuration of an atom. The word 'aufbau' is German for 'building up' and refers to how electrons fill up orbitals starting from the lowest energy level to the higher ones.
Here's a simple way to think about it: Electrons are social butterflies that want their own space, but they're also energy-efficient, always picking the lowest energy 'seat' available. Whenever a new 'guest' arrives in an atomic 'party', it always takes the empty seat closest to the entrance (the nucleus). The room layout follows a specific pattern (1s, 2s, 2p, 3s, ...), and like a game of musical chairs, there is a set limit of seats (electrons) in each orbital type (s, p, d, f). Once an orbital is filled, the next electron moves to the next available space following the sequence.
Here's a simple way to think about it: Electrons are social butterflies that want their own space, but they're also energy-efficient, always picking the lowest energy 'seat' available. Whenever a new 'guest' arrives in an atomic 'party', it always takes the empty seat closest to the entrance (the nucleus). The room layout follows a specific pattern (1s, 2s, 2p, 3s, ...), and like a game of musical chairs, there is a set limit of seats (electrons) in each orbital type (s, p, d, f). Once an orbital is filled, the next electron moves to the next available space following the sequence.
Atomic Number and Electron Count
The atomic number isn't just a ranking on the periodic table; it tells us the number of protons in an atom's nucleus. Since atoms are electrically neutral in their elemental state, the number of protons is equal to the number of electrons.
In the case of potassium, with an atomic number of 19, you immediately know it has 19 electrons to house within its orbitals. This electron count determines how you'll distribute those electrons following the rules set by the aufbau principle. Each step in the aufbau sequence represents energy levels that the electrons fill in a specific order. The atomic number is like an RSVP list that tells you how many guests (electrons) you should expect at the party—the elemental party, that is.
In the case of potassium, with an atomic number of 19, you immediately know it has 19 electrons to house within its orbitals. This electron count determines how you'll distribute those electrons following the rules set by the aufbau principle. Each step in the aufbau sequence represents energy levels that the electrons fill in a specific order. The atomic number is like an RSVP list that tells you how many guests (electrons) you should expect at the party—the elemental party, that is.
