Electron configuration worksheet pdf: Unlock the secrets of atomic structure! This comprehensive guide simplifies the often-challenging world of electron configurations, making it easier to understand how electrons arrange themselves around an atom’s nucleus. From basic concepts to advanced problem-solving, this resource is your key to mastering this fundamental chemistry principle. Discover how electron configuration shapes the periodic table and drives chemical reactions.
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This resource meticulously Artikels the basics of electron configuration, from defining the concept to illustrating its significance in the periodic table. It delves into various worksheet formats, catering to different skill levels. Practical problem-solving strategies and illustrative examples make understanding the intricacies of electron configuration remarkably straightforward. The included PDF provides a structure for worksheets, complete with exercises and answers, ensuring a hands-on learning experience.
Introduction to Electron Configuration: Electron Configuration Worksheet Pdf
Electron configuration, a fundamental concept in chemistry, describes the arrangement of electrons within an atom. Understanding this arrangement is crucial for comprehending atomic properties, chemical bonding, and the periodic table’s structure. Imagine electrons as tiny particles orbiting the nucleus; their configuration dictates how atoms interact with each other.Electron configuration is like an atom’s address, telling us where each electron resides within the atom’s energy levels and sublevels.
This address impacts an atom’s behavior in chemical reactions. It’s the key to understanding why certain elements react in specific ways, form particular compounds, and exhibit unique properties.
Significance of Electron Configuration
Electron configuration is essential in chemistry because it explains the behavior of elements. It’s the basis for understanding reactivity, bonding, and the formation of molecules. Knowing an element’s electron configuration reveals its likely chemical behavior, enabling predictions about its interactions with other elements. This understanding is fundamental for advancements in materials science, medicine, and other fields.
Relationship Between Electron Configuration and the Periodic Table
The periodic table is a visual representation of electron configurations. Elements are arranged according to their electron configurations, reflecting the predictable patterns in atomic structure. Each element’s position in the periodic table corresponds to a specific electron configuration. Elements in the same group (vertical column) have similar outer electron configurations, leading to similar chemical properties.
Fundamental Principles Governing Electron Configuration
Several fundamental principles govern the filling of electron orbitals. The Aufbau principle states that electrons fill orbitals of the lowest energy first. The Pauli exclusion principle dictates that each orbital can hold a maximum of two electrons with opposite spins. Hund’s rule dictates that electrons occupy orbitals individually before pairing up. These principles guide us in predicting electron configurations.
Filling Order of Orbitals (s, p, d, f)
Understanding the order in which orbitals fill is crucial. The following table Artikels the filling order, a key concept for accurately determining electron configurations:
| Orbital | Filling Order | Example |
|---|---|---|
| 1s | First | Hydrogen (1s1) |
| 2s | Second | Lithium (1s22s1) |
| 2p | Third | Nitrogen (1s22s22p3) |
| 3s | Fourth | Sodium (1s22s22p63s1) |
| 3p | Fifth | Phosphorus (1s22s22p63s23p3) |
| 4s | Sixth | Potassium (1s22s22p63s23p64s1) |
| 3d | Seventh | Chromium (1s22s22p63s23p64s13d5) |
| 4p | Eighth | Selenium (1s22s22p63s23p64s23d104p4) |
This table demonstrates the sequence in which orbitals are populated. Knowing this order is essential for writing correct electron configurations for any element.
Types of Electron Configuration Worksheets
Electron configuration, a fundamental concept in chemistry, describes the arrangement of electrons within an atom. Mastering this concept is crucial for understanding chemical bonding, reactivity, and periodic trends. Different types of worksheets cater to various skill levels, ensuring a personalized learning experience for every student.Understanding electron configuration is like deciphering a secret code of atomic structure. Different worksheet formats allow learners to explore this code, building their confidence step-by-step, from basic understanding to advanced application.
This section will explore the diverse range of worksheets, highlighting the varying levels of difficulty and the skills each one targets.
Worksheet Formats
Various formats of electron configuration worksheets exist, each designed to reinforce different aspects of the subject. These formats, ranging from simple fill-in-the-blank exercises to more complex problem-solving tasks, cater to the diverse needs of students. These diverse formats enhance comprehension and reinforce understanding.
Basic Worksheets
These worksheets focus on the foundational principles of electron configuration. Students typically practice writing the electron configurations of atoms using the Aufbau principle, Hund’s rule, and the Pauli exclusion principle. They often involve simple elements, with the main goal being to build a solid understanding of the rules and principles governing electron distribution. Examples include determining the electron configuration for elements like Lithium (Li) or Beryllium (Be).
These worksheets are like stepping stones, helping learners grasp the basics before moving on to more challenging tasks.
Intermediate Worksheets
Moving beyond the basics, intermediate worksheets introduce more complex elements and scenarios. Students will likely encounter elements with a greater number of electrons and more nuanced electron distributions. They often involve identifying the number of valence electrons, predicting the ionization energy of different atoms, and understanding the relationships between electron configuration and the periodic table. Examples include determining the electron configuration of elements like Phosphorus (P) or Sulfur (S) and applying the concepts to predict properties.
These worksheets are designed to challenge students’ understanding and encourage them to connect the dots between electron configuration and chemical properties.
Advanced Worksheets
These worksheets push the boundaries of electron configuration mastery. They delve into more intricate concepts such as exceptions to the Aufbau principle, the relationship between electron configuration and magnetism, and the application of electron configuration in understanding complex chemical bonding. Students will encounter elements with higher atomic numbers, exploring the more nuanced electron arrangements and relationships. Examples include predicting the magnetic properties of transition metal ions or understanding the impact of electron configuration on bonding in complex molecules.
These worksheets are for students who are ready for a more in-depth and rigorous understanding of the subject.
Worksheet Difficulty Levels
| Worksheet Type | Targeted Skill Level | Example Elements |
|---|---|---|
| Basic | Beginner | Li, Be, B, C |
| Intermediate | Intermediate | P, S, Cl, Ar |
| Advanced | Advanced | Transition Metals, Lanthanides, Actinides |
These diverse worksheets provide a comprehensive learning path for students of all levels. By progressing through the various levels, students can develop a thorough and nuanced understanding of electron configuration, enabling them to tackle more complex chemical concepts.
Common Electron Configuration Problems
Electron configurations, while seemingly straightforward, can sometimes trip up even the most seasoned students. Understanding the rules and common pitfalls is key to mastering this fundamental concept in chemistry. This section delves into typical challenges and provides practical solutions, ensuring a robust grasp of electron configurations.Electron configuration, essentially the arrangement of electrons within an atom, follows specific rules.
These rules, while seemingly rigid, are surprisingly intuitive once understood. Mastering these rules is crucial for predicting atomic behavior and understanding chemical bonding. Misinterpretations often stem from overlooking these rules, or getting lost in the complexity of higher atomic numbers. Let’s navigate these common challenges and emerge confident in your understanding.
Identifying the Correct Order of Filling Electron Shells
A fundamental hurdle is remembering the order in which electron shells and subshells are filled. The Aufbau principle, a crucial concept, guides this process. The principle dictates that electrons initially fill the lowest energy levels first. This order, often visualized as a diagonal pattern, ensures stability and minimizes energy. Remembering this order is critical for accurately determining the electron configuration of any element.
Understanding Exceptions to the Aufbau Principle
Certain elements deviate from the predicted Aufbau order. These exceptions, while less frequent, are essential to acknowledge. These exceptions often arise due to the subtle interplay of electron-electron repulsion and the stability gained by half-filled or fully filled subshells. Recognizing these exceptions is crucial for accurately predicting the electron configurations of these special cases.
Addressing Electron Configuration of Ions
Determining the electron configuration of ions involves an extra step. When an atom gains or loses electrons to form an ion, the outermost electrons are the first to be affected. The loss of electrons results in a reduction in the overall negative charge, and the removal of electrons changes the electron configuration. For example, consider the electron configuration of sodium (Na).
Sodium’s electron configuration is 1s 22s 22p 63s 1. When sodium becomes a sodium ion (Na +), it loses its single 3s electron, resulting in the electron configuration 1s 22s 22p 6.
Table of Common Problems and Solutions
| Problem | Solution |
|---|---|
| Incorrect order of filling subshells | Refer to the Aufbau principle and the periodic table’s order. |
| Misunderstanding exceptions to the Aufbau principle | Recognize the special stability of half-filled and fully filled subshells. |
| Difficulty determining electron configuration of ions | Identify the number of electrons lost or gained and adjust the configuration accordingly. |
| Calculating electron configurations of high atomic number elements | Use the periodic table as a visual guide for filling orbitals. |
Electron Configuration Worksheet PDF Structure
Unlocking the secrets of electron arrangements is like discovering a hidden code! Electron configurations, those fascinating recipes for where electrons reside in atoms, are essential for understanding chemistry’s intricate dance. This structured worksheet will guide you through the journey, making the process both engaging and educational.A well-designed worksheet should mirror the complexity of the electron configuration itself, guiding learners through the concepts in a logical, step-by-step fashion.
Clear instructions, relevant examples, and a thoughtful progression of difficulty are crucial for student success. The structure should not just convey information, but also foster understanding and problem-solving skills.
Worksheet Template Design, Electron configuration worksheet pdf
This template aims to present electron configuration in a clear, structured format. The worksheet will use a logical progression, starting with the basics and gradually increasing complexity. The design will include sections that are clearly defined and easy to follow.
Content and Layout
The worksheet will feature a variety of exercises to solidify understanding. Each section will include clear instructions and example problems, ensuring students have the support they need. It will start with fundamental principles, then gradually introduce more challenging concepts. The worksheet will emphasize visual aids and clear explanations to help learners grasp the core concepts.
- Section 1: Fundamentals
-This initial section introduces the basics of electron configurations, outlining the Aufbau principle, Hund’s rule, and the Pauli exclusion principle. This section also includes a table of the periodic table, highlighted with key elements to assist students in visualizing the patterns in electron arrangement. Examples of basic configurations for common elements are included. - Section 2: Building Configurations
– Here, learners apply the principles learned in the first section. They will practice writing electron configurations for various elements, progressively increasing in atomic number. This section includes diagrams depicting orbital filling sequences. Visual aids are essential for learners to visualize the filling process. - Section 3: Exceptions and Special Cases
– This section introduces exceptions to the standard rules, like chromium and copper, which have unique electron configurations. This provides context for the non-standard behavior of some elements. It also introduces condensed electron configurations, using noble gas shorthand to simplify complex configurations. This section will also discuss elements with incomplete subshells and their importance. - Section 4: Practice Exercises
– This crucial section will include a diverse range of exercises, including multiple-choice questions, fill-in-the-blanks, and short-answer questions. Examples of practice exercises include: determining the electron configuration of an element given its atomic number, identifying the element given its electron configuration, and explaining the significance of Hund’s rule. These exercises are designed to reinforce the concepts introduced throughout the worksheet.
Sample Worksheet Structure
This table presents a sample structure of the worksheet, illustrating the layout and content.
| Column Heading | Exercises | Expected Answers |
|---|---|---|
| Element | Nitrogen (N) | 1s22s22p3 |
| Element | Potassium (K) | 1s22s22p63s23p64s1 |
| Element | Chromium (Cr) | [Ar]3d54s1 |
| Explanation | Explain Hund’s Rule | Electrons occupy separate orbitals within a subshell before pairing up in the same orbital. |
Generating Practice Problems
Unlocking the secrets of electron configurations requires practice, just like mastering any new skill. This section provides a diverse range of practice problems, from straightforward applications to more challenging scenarios, designed to solidify your understanding. These exercises will equip you with the tools to tackle any electron configuration challenge with confidence.
Element and Configuration Pairs
A crucial step in mastering electron configurations is memorizing the patterns. This section provides a set of elements and their corresponding electron configurations. Understanding the relationship between the element’s position on the periodic table and its electron arrangement is key to predicting configurations for other elements.
- Hydrogen (H): 1s 1
- Helium (He): 1s 2
- Lithium (Li): 1s 22s 1
- Beryllium (Be): 1s 22s 2
- Boron (B): 1s 22s 22p 1
- Carbon (C): 1s 22s 22p 2
- Nitrogen (N): 1s 22s 22p 3
- Oxygen (O): 1s 22s 22p 4
- Fluorine (F): 1s 22s 22p 5
- Neon (Ne): 1s 22s 22p 6
Orbital Diagrams
Visualizing electron arrangements using orbital diagrams provides a clear picture of electron distribution within atomic orbitals. This approach emphasizes the concept of electron spin, a fundamental aspect of quantum mechanics. The diagrams below illustrate the arrangement for the same elements listed above, providing a spatial representation of the electrons.
- Hydrogen (H): 1s ↑
- Helium (He): 1s ↓↑
- Lithium (Li): 1s ↓↑ 2s ↑
- Beryllium (Be): 1s ↓↑ 2s ↓↑
- Boron (B): 1s ↓↑ 2s ↓↑ 2p ↑
- Carbon (C): 1s ↓↑ 2s ↓↑ 2p ↑ ↑
- Nitrogen (N): 1s ↓↑ 2s ↓↑ 2p ↑ ↑ ↑
- Oxygen (O): 1s ↓↑ 2s ↓↑ 2p ↑ ↑ ↓
- Fluorine (F): 1s ↓↑ 2s ↓↑ 2p ↑ ↑ ↑ ↓
- Neon (Ne): 1s ↓↑ 2s ↓↑ 2p ↓↑ ↓↑ ↓↑
Electron Configuration Problems
These problems will challenge you to apply your understanding of electron configurations in different scenarios.
- Determine the electron configuration of Magnesium (Mg). This problem emphasizes the filling order of orbitals.
- What is the electron configuration of Phosphorus (P)? This focuses on the understanding of the periodic table and the filling order of sublevels.
- Predict the electron configuration of a hypothetical element with atomic number 20. This problem focuses on the relationship between atomic number and electron configuration.
- Describe the electron configuration of a neutral atom with 17 electrons. This problem helps understand how the number of electrons relates to the electron configuration.
- Illustrate the electron configuration of Iron (Fe). This example demonstrates how to deal with exceptions to the filling order of electrons.
Identifying Elements from Configurations
These problems test your ability to decipher the electron configuration of an element and determine the element itself.
- Determine the element represented by the configuration 1s22s 22p 63s 23p 5. This focuses on recognizing patterns.
- What element corresponds to the electron configuration 1s 22s 22p 63s 23p 64s 23d 104p 3? This problem helps recognize the complexities of the filling order.
- Identify the element with the configuration [Ar]4s 13d 5. This problem emphasizes the use of shorthand notation.
- What element has the electron configuration 1s 22s 22p 63s 23p 64s 23d 104p 65s 24d 105p 66s 24f 145d 106p 4? This problem focuses on complex configurations.
- Determine the element associated with the configuration [Kr]5s 24d 105p 5. This problem emphasizes using shorthand notation and recognizing patterns.
Table of Element Configurations
This table provides a concise overview of the elements and their corresponding configurations. This reference table is helpful for checking answers or gaining a comprehensive understanding.
| Element Symbol | Atomic Number | Electron Configuration |
|---|---|---|
| H | 1 | 1s1 |
| He | 2 | 1s2 |
| Li | 3 | 1s22s1 |
| Be | 4 | 1s22s2 |
| B | 5 | 1s22s22p1 |
| C | 6 | 1s22s22p2 |
| N | 7 | 1s22s22p3 |
| O | 8 | 1s22s22p4 |
| F | 9 | 1s22s22p5 |
| Ne | 10 | 1s22s22p6 |
Visual Representation of Electron Configuration
Electron configuration, a fundamental concept in chemistry, describes the arrangement of electrons within an atom. Visual representations, like orbital and box diagrams, make this intricate structure easier to grasp and understand. These diagrams aren’t just pretty pictures; they offer a powerful tool for predicting atomic properties and understanding chemical behavior. Let’s explore how these visual aids illuminate the electron world.Orbital diagrams and box diagrams are invaluable tools for visualizing the electron configuration of atoms.
They provide a clear picture of how electrons populate the various energy levels and sublevels within an atom. This visual clarity allows for a deeper understanding of the relationships between electrons and their interactions, paving the way for a more intuitive understanding of chemical bonding and reactivity.
Illustrating Electron Configuration with Orbital Diagrams
Orbital diagrams use boxes to represent atomic orbitals. Each box represents an orbital, and an arrow within the box signifies an electron. The direction of the arrow (up or down) represents the electron’s spin. Electrons in the same orbital must have opposite spins, a fundamental principle known as the Pauli Exclusion Principle.
Illustrating Electron Configuration with Box Diagrams
Box diagrams, a simpler variation, use boxes to represent orbitals, but they don’t explicitly show electron spin. They are still useful for representing the distribution of electrons across orbitals and sub-orbitals. The number of boxes in a given energy level corresponds to the number of orbitals in that level (1 for s, 3 for p, 5 for d, and 7 for f).
The Significance of Arrows in Orbital Diagrams
The arrows in orbital diagrams are crucial. They indicate the spin of the electrons. A single arrow in a box represents an electron with one spin direction, and a pair of arrows (one up, one down) represents two electrons with opposite spins in the same orbital. This crucial detail is essential for understanding the stability and properties of atoms.
Filling Order of Electrons in Different Orbitals
Understanding the filling order of electrons is key. Electrons fill orbitals following Hund’s rule, which states that electrons first occupy separate orbitals within a subshell before pairing up. This filling order is often depicted using a diagram that shows the relative energies of orbitals. For example, the 2p orbitals will each receive one electron before any of them get a second electron.
This minimizes electron-electron repulsion, contributing to atomic stability. The diagram below illustrates this concept.
↑↓ ↑↓ ↑
1s 2s 2p 3s
The above diagram visually represents the filling order, with arrows signifying electrons and their spins. The 1s orbital fills first, followed by 2s, then the 2p orbitals.
Visualizing Electron Configuration in Complex Atoms
Visualizing the electron configuration of complex atoms, like those with multiple electron shells, involves representing each electron’s placement within the various orbitals. For example, the electron configuration of Oxygen (atomic number 8) is 1s 22s 22p 4. A visual representation would depict two electrons in the 1s orbital, two in the 2s orbital, and four in the 2p orbitals. This detailed depiction illustrates the atom’s electronic structure, crucial for understanding its chemical interactions.
Illustrative Examples for Electron Configuration
Unlocking the secrets of atomic structure involves understanding how electrons populate the different energy levels and sublevels within an atom. Electron configuration is like a blueprint, detailing the arrangement of these tiny particles. Let’s explore some concrete examples to visualize this fascinating concept.
Electron configuration provides a roadmap of how electrons are distributed within an atom’s various energy levels and sublevels. This knowledge is fundamental to understanding chemical behavior and bonding.
Electron Configuration of Oxygen (O)
Oxygen, with its eight electrons, showcases a fundamental principle of electron filling. The electrons fill the lowest energy levels first, following the Aufbau principle.
- Oxygen’s atomic number is 8, indicating 8 electrons.
- The first energy level (n=1) can hold a maximum of 2 electrons, filling the 1s orbital.
- The remaining 6 electrons fill the second energy level (n=2). This level has two sublevels, 2s and 2p. The 2s orbital holds 2 electrons, and the 2p orbitals (three in total) hold the remaining 4 electrons.
The electron configuration of Oxygen (O) is 1s 22s 22p 4.
Electron Configuration of Sodium (Na)
Sodium, with its 11 electrons, demonstrates the progression of electron filling across different energy levels and sublevels.
- Sodium’s atomic number is 11, meaning it has 11 electrons.
- Following the Aufbau principle, the lowest energy levels are filled first. The first energy level (n=1) holds 2 electrons in the 1s orbital.
- The second energy level (n=2) accommodates 8 electrons, with 2 in the 2s orbital and 6 in the 2p orbitals.
- The remaining electron goes into the 3s orbital of the third energy level (n=3).
Thus, the electron configuration of Sodium (Na) is 1s 22s 22p 63s 1.
Electron Configuration of Iron (Fe)
Iron, with its 26 electrons, presents a more complex but still predictable pattern.
- Iron’s atomic number is 26, corresponding to 26 electrons.
- The filling follows the Aufbau principle, progressively filling lower energy levels. Key to understanding Iron’s configuration is the fact that 3d orbitals are slightly higher in energy than 4s orbitals.
- The configuration is 1s 22s 22p 63s 23p 64s 23d 6
This demonstrates the nuanced interplay of energy levels and sublevels.
Electron Configuration of a Transition Metal
Transition metals, like Iron, exhibit interesting patterns in their electron configurations. The filling of the d orbitals often deviates from the strict Aufbau principle.
- Transition metals often have incomplete d orbitals. This is due to the subtle energy differences between the d and s orbitals.
- Iron’s electron configuration is a typical example, demonstrating how the d orbitals are filled in certain elements.
Iron’s electron configuration highlights the subtleties within the electron filling process.
Electron Configuration for an Element with More Than 30 Electrons
Elements beyond the first 30 electrons become more complex, but the principles remain consistent.
- The Aufbau principle, Hund’s rule, and the Pauli exclusion principle continue to guide the filling process.
- Understanding the order of filling orbitals and sublevels is crucial for accurate electron configuration.
- Advanced elements require careful consideration of the subtle energy differences among orbitals, especially when approaching the transition metals.
The electron configurations of larger atoms become more intricate, but the fundamental principles of electron filling remain constant.
Problem Solving Techniques for Worksheets
Unlocking the secrets of electron configurations is like deciphering a cosmic code. This section will equip you with powerful strategies to tackle these fascinating problems, turning you into a master code-breaker. We’ll delve into the periodic table’s role, explore electron shell distribution, and master Hund’s rule, all while offering step-by-step guides to complete worksheets with confidence.
Electron configurations, while seemingly complex, are built on a foundation of logical steps. Understanding these steps will transform you from a bewildered student to a confident problem solver. This section provides a structured approach to conquering these challenges, making the process less daunting and more enjoyable.
Strategies for Solving Electron Configuration Problems
Electron configuration problems often seem daunting, but with the right approach, they’re quite manageable. A systematic strategy is key to success. Breaking down the problem into smaller, more digestible parts can make the process much smoother.
- Start with the Periodic Table: The periodic table is your best friend. It’s a roadmap to the electronic structure of elements. Notice the arrangement of elements according to their atomic number and electron configurations. The periodic table shows the order in which electrons fill atomic orbitals. For instance, elements in the same column (group) often have similar outer electron configurations, reflecting their chemical properties.
Using this as a reference will simplify your task greatly.
- Determine the Atomic Number: The atomic number dictates the number of electrons in a neutral atom. Knowing this is the first step towards understanding the electron configuration. The atomic number is the key to unlocking the puzzle of electron distribution.
- Fill Orbitals Systematically: Electrons fill orbitals in a specific order, following the Aufbau principle. This principle describes the filling order of orbitals, starting with the lowest energy levels. Think of it like filling a building, starting with the ground floor. Understanding the order of filling will allow you to build up the electron configuration correctly.
Significance of the Periodic Table
The periodic table isn’t just a chart; it’s a powerful tool for understanding electron configurations. The table’s structure reflects the filling order of atomic orbitals. Each row corresponds to a principal energy level (n), and each block corresponds to a specific type of orbital (s, p, d, f). Recognizing these patterns allows you to quickly predict electron configurations for various elements.
- Orbital Filling Order: The periodic table’s arrangement provides a visual guide to the order in which orbitals are filled. This order, determined by the principle quantum number (n) and the azimuthal quantum number (l), is crucial for accurate electron configurations.
- Electron Configuration Trends: Notice how elements in the same column (group) often exhibit similar outer electron configurations. This reflects their similar chemical properties. For example, alkali metals (group 1) all have one electron in their outermost shell, making them highly reactive.
Determining the Number of Electrons in Each Shell
Each shell or energy level can hold a specific maximum number of electrons. Understanding these limits is essential for completing electron configurations.
- Shell Capacity: The maximum number of electrons that can occupy a given shell is determined by the formula 2n 2, where ‘n’ represents the principal quantum number (shell number). For example, the first shell (n=1) can hold a maximum of 2 electrons, the second shell (n=2) can hold a maximum of 8 electrons, and so on. Understanding this will help you quickly determine the capacity of each shell.
Hund’s Rule in Electron Configuration
Hund’s rule provides an additional crucial guideline for filling orbitals. It ensures maximum multiplicity by distributing electrons across orbitals within a subshell before pairing them up. This principle helps ensure the most stable electron configuration.
- Electron Pairing: Hund’s rule dictates that electrons will individually occupy each orbital within a subshell before pairing up in the same orbital. This is a crucial step in determining the correct electron configuration, ensuring maximum stability.
Step-by-Step Guide to Completing a Worksheet
Follow these steps to master electron configurations:
- Identify the element. Locate the element on the periodic table and determine its atomic number.
- Use the periodic table to identify the order in which orbitals fill.
- Fill the orbitals according to the Aufbau principle.
- Apply Hund’s rule to ensure maximum multiplicity.
- Check your work to make sure the total number of electrons matches the atomic number.
