Electronic Configuration Table for 1 to 30 Elements with Shells & Subshells
Electronic Configuration of First 30 Elements is essential in chemistry and helps students understand various practical and theoretical applications related to this topic. For exams like NEET, JEE, and school boards, being able to quickly write or recall the electronic configuration from Hydrogen to Zinc is a key skill. This topic helps in understanding atomic structure, periodic trends, and why elements behave the way they do in chemical reactions. With table formats and memory tips, you can master this fundamental concept for your chemistry journey.
What is Electronic Configuration of First 30 Elements in Chemistry?
A electronic configuration of first 30 elements refers to the systematic arrangement of electrons among different shells (K, L, M, N) and subshells (s, p, d, f) for each atom from Hydrogen (atomic number 1) to Zinc (atomic number 30). This concept appears in chapters related to atomic structure, periodic table, and chemical bonding, making it a foundational part of your chemistry syllabus. Knowing the order in which electrons fill the available orbitals reveals an element’s reactivity, valency, and position on the periodic table.
Molecular Formula and Composition
The molecular formula here is not for a single compound, but for each element H (Z=1) to Zn (Z=30) in their neutral atomic states. Each element consists of a nucleus containing protons and neutrons, surrounded by electrons arranged in specific configurations based on quantum rules. These configurations define each element’s group, period, and core chemical properties.
Preparation and Synthesis Methods
You do not chemically synthesize an electronic configuration; instead, you determine it by following principles such as the Aufbau Principle, Pauli Exclusion Principle, and Hund’s Rule. These rules help you fill electrons in increasing order of orbital energy. For real learning, educators at Vedantu teach stepwise filling and shortcut tricks to remember orders like 1s, 2s, 2p, 3s, etc.
Physical Properties of Electronic Configuration of First 30 Elements
Every element’s properties—such as metallic/nonmetallic behavior, magnetism, and valency—are controlled by its electronic structure. For example, Sodium (Na) with 1s2 2s2 2p6 3s1 is highly reactive due to its single outer electron, while Argon (Ar) is inert due to a filled shell. The structure determines stability, reactivity, and chemical bonding type.
Electronic Configuration of First 30 Elements Table
The electronic configuration of first 30 elements arranges electrons into shells and subshells, following the Aufbau principle. This compact table helps you review all configurations from Hydrogen to Zinc in both spdf notation and shell format.
| Atomic No. | Element | Symbol | Electronic Configuration (spdf) | Shells (KLMN) |
|---|---|---|---|---|
| 1 | Hydrogen | H | 1s1 | 1 |
| 2 | Helium | He | 1s2 | 2 |
| 3 | Lithium | Li | 1s2 2s1 | 2,1 |
| 4 | Beryllium | Be | 1s2 2s2 | 2,2 |
| 5 | Boron | B | 1s2 2s2 2p1 | 2,3 |
| 6 | Carbon | C | 1s2 2s2 2p2 | 2,4 |
| 7 | Nitrogen | N | 1s2 2s2 2p3 | 2,5 |
| 8 | Oxygen | O | 1s2 2s2 2p4 | 2,6 |
| 9 | Fluorine | F | 1s2 2s2 2p5 | 2,7 |
| 10 | Neon | Ne | 1s2 2s2 2p6 | 2,8 |
| 11 | Sodium | Na | 1s2 2s2 2p6 3s1 | 2,8,1 |
| 12 | Magnesium | Mg | 1s2 2s2 2p6 3s2 | 2,8,2 |
| 13 | Aluminium | Al | 1s2 2s2 2p6 3s2 3p1 | 2,8,3 |
| 14 | Silicon | Si | 1s2 2s2 2p6 3s2 3p2 | 2,8,4 |
| 15 | Phosphorus | P | 1s2 2s2 2p6 3s2 3p3 | 2,8,5 |
| 16 | Sulfur | S | 1s2 2s2 2p6 3s2 3p4 | 2,8,6 |
| 17 | Chlorine | Cl | 1s2 2s2 2p6 3s2 3p5 | 2,8,7 |
| 18 | Argon | Ar | 1s2 2s2 2p6 3s2 3p6 | 2,8,8 |
| 19 | Potassium | K | 1s2 2s2 2p6 3s2 3p6 4s1 | 2,8,8,1 |
| 20 | Calcium | Ca | 1s2 2s2 2p6 3s2 3p6 4s2 | 2,8,8,2 |
| 21 | Scandium | Sc | 1s2 2s2 2p6 3s2 3p6 3d1 4s2 | 2,8,9,2 |
| 22 | Titanium | Ti | 1s2 2s2 2p6 3s2 3p6 3d2 4s2 | 2,8,10,2 |
| 23 | Vanadium | V | 1s2 2s2 2p6 3s2 3p6 3d3 4s2 | 2,8,11,2 |
| 24 | Chromium* | Cr | 1s2 2s2 2p6 3s2 3p6 3d5 4s1 | 2,8,13,1 |
| 25 | Manganese | Mn | 1s2 2s2 2p6 3s2 3p6 3d5 4s2 | 2,8,13,2 |
| 26 | Iron | Fe | 1s2 2s2 2p6 3s2 3p6 3d6 4s2 | 2,8,14,2 |
| 27 | Cobalt | Co | 1s2 2s2 2p6 3s2 3p6 3d7 4s2 | 2,8,15,2 |
| 28 | Nickel | Ni | 1s2 2s2 2p6 3s2 3p6 3d8 4s2 | 2,8,16,2 |
| 29 | Copper* | Cu | 1s2 2s2 2p6 3s2 3p6 3d10 4s1 | 2,8,18,1 |
| 30 | Zinc | Zn | 1s2 2s2 2p6 3s2 3p6 3d10 4s2 | 2,8,18,2 |
*Chromium and Copper: Notice the special, more stable half-filled and fully-filled d-subshell exceptions.
Chemical Properties and Reactions
Elements with incomplete or partially filled outer shells tend to be more reactive, aiming to achieve stable noble gas configurations via chemical bonding. For example, sodium (Na) reacts readily to lose its single valence electron, while neon (Ne) does not react due to its full p-subshell. Transition metals (Sc to Zn) exhibit multiple valencies because of the close energy levels of 4s and 3d orbitals. For more on transition metals, see transition metals.
Frequent Related Errors
- Confusing shells (K/L/M/N) and subshells (s/p/d/f) when writing configuration.
- Forgetting exceptions: Chromium (Cr) and Copper (Cu) have unique configurations.
- Overlooking the 4s before 3d filling order and vice versa for ions.
- Misplacing valency—especially for transition metals with variable oxidation states.
Uses of Electronic Configuration of First 30 Elements in Real Life
Understanding the electronic configuration of the first 30 elements is widely used for predicting element reactivity, creating alloys (with transition metals), making fertilizers (using P, N, K, S), developing electronic materials, and understanding biological systems. In the lab, teachers at Vedantu use configuration to explain group behavior and bonding trends in elements.
Relevance in Competitive Exams
Students preparing for NEET, JEE, and Olympiads should be familiar with the electronic configuration of first 30 elements, as it helps them solve periodic table, atomic structure, and chemical bonding questions. Questions often test the knowledge of configuration exceptions, normal vs. shorthand notation, and trends across periods and groups.
Relation with Other Chemistry Concepts
Electronic configuration is closely related to topics such as Aufbau Principle, Hund's Rule, and Pauli Exclusion Principle, all of which are very important for correctly filling atomic orbitals. It also connects to Periodic Table Trends and concepts like atomic number.
Step-by-Step Reaction Example
1. Write the electronic configuration of Scandium (Z = 21):2. List orbitals in filling order – 1s, 2s, 2p, 3s, 3p, 4s, 3d
3. Fill 18 electrons as in Argon: [Ar] = 1s2 2s2 2p6 3s2 3p6
4. Add remaining 3 electrons: 4s2 3d1
5. Final Answer: [Ar] 3d1 4s2 (or full expanded as above)
Lab or Experimental Tips
Remember the “1s before 2s before 2p…” order using the diagonal rule (Aufbau diagram). For complete stability, look for full or half-filled subshells. Vedantu educators use colorful charts and shell models to explain difference between shell and subshell notation, making revision easier for students.
Try This Yourself
- Write the electronic configuration (spdf) for Manganese (Z=25).
- Identify which element has the configuration 1s2 2s2 2p6 3s2 3p6 4s1.
- Give two real-life uses of transition metals found among the first 30 elements.
Final Wrap-Up
We explored the electronic configuration of first 30 elements—their arrangement, memory tips, exceptions, and impact on property trends. For more detailed explanations and exam-specific guidance, join the interactive classes at Vedantu or try topic notes for chemistry.
FAQs on Electronic Configuration of First 30 Elements (With Table & Valency)
1. What is the electronic configuration of the first 30 elements in Chemistry?
The electronic configuration describes how electrons are arranged in the shells and subshells (s, p, d, f) of atoms for elements Hydrogen (Z=1) to Zinc (Z=30). Each element has a unique configuration determined by the Aufbau principle, Pauli exclusion principle, and Hund's rule. This arrangement dictates an element's chemical and physical properties.
2. How do you write the electronic configuration for elements 1 to 30?
Follow these steps: 1. Determine the atomic number (number of electrons). 2. Use the Aufbau principle to fill orbitals in increasing energy order (1s, 2s, 2p, 3s, etc.). 3. Apply the Pauli exclusion principle (maximum two electrons per orbital) and Hund's rule (fill orbitals singly before pairing). Remember exceptions like Chromium and Copper.
3. What are the exceptions to the Aufbau principle in electronic configuration (elements 1-30)?
Chromium (Cr) and Copper (Cu) are notable exceptions. To achieve greater stability, they deviate from the expected filling order, resulting in half-filled or completely filled d-subshells. Cr is [Ar] 3d5 4s1 instead of [Ar] 3d4 4s2, and Cu is [Ar] 3d10 4s1 instead of [Ar] 3d9 4s2.
4. What is the significance of electronic configuration in determining chemical properties?
Electronic configuration directly determines an element's valency and chemical reactivity. The number of electrons in the outermost shell (valence electrons) dictates how an atom will bond with other atoms. Elements with similar valence electron configurations exhibit similar chemical behaviors.
5. How does Hund's rule affect electron configuration?
Hund's rule states that electrons will individually occupy each orbital within a subshell before doubling up in any one orbital. This maximizes the total spin and leads to greater stability. For example, in Nitrogen (N), the three 2p electrons occupy three separate orbitals with parallel spins.
6. What is the difference between shells and subshells in electronic configuration?
Shells (e.g., K, L, M) represent principal energy levels, while subshells (s, p, d, f) are sub-levels within a shell. Shells determine the overall energy level, and subshells specify the shape and orientation of orbitals within that shell. Each subshell can hold a specific maximum number of electrons.
7. Explain the Pauli Exclusion Principle and its role in electron configuration.
The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of four quantum numbers. This means that each orbital can hold a maximum of two electrons, which must have opposite spins (one spin-up and one spin-down).
8. How does electronic configuration relate to the periodic table?
The periodic table is organized based on the electronic configurations of elements. Elements in the same group (vertical column) have similar valence electron configurations, leading to similar chemical properties. The periods (horizontal rows) reflect the filling of electron shells.
9. What is the electronic configuration of Zinc (Zn)?
The electronic configuration of Zinc (Zn, atomic number 30) is [Ar] 3d10 4s2. Note the filled d-subshell contributes to its relatively low reactivity.
10. How can I use electronic configuration to predict the valency of an element?
The valency of an element is often determined by the number of electrons in its outermost shell (valence electrons). Elements tend to gain, lose, or share electrons to achieve a stable configuration, often resembling a noble gas. For example, elements in Group 1 (alkali metals) have a valency of +1 because they readily lose one electron.
11. What are orbital diagrams, and how are they used to represent electronic configuration?
Orbital diagrams visually represent electron configurations using boxes to represent orbitals and arrows to represent electrons. The direction of the arrow indicates the spin of the electron. Orbital diagrams help visualize the filling of orbitals according to Hund's rule and the Pauli exclusion principle.
12. How does electronic configuration help in understanding chemical bonding?
Understanding electronic configuration is crucial for predicting the type and strength of chemical bonds. Atoms interact to achieve stable electron configurations, often by sharing (covalent bonds), transferring (ionic bonds), or forming coordinate covalent bonds. The number and arrangement of valence electrons dictate the bonding behavior.
