What is Element X from Part B? Identity Guide

In analytical chemistry, accurate substance identification is paramount, and spectroscopic techniques are frequently employed to determine the composition of unknown samples. The National Institute of Standards and Technology (NIST) maintains extensive databases that are crucial for identifying such elements. This guide addresses the question of what is the identity of element x from part b, often encountered when employing a methodology similar to the systematic qualitative analysis developed by Arthur Noyes, where meticulous separation and identification processes are standard practice. Understanding these processes is critical for researchers working to validate their results in certified laboratories.

The Quest to Identify Element X: A Systematic Approach

Identifying an unknown element, provisionally designated as Element X, presents a fundamental challenge in chemistry. Our objective is to pinpoint Element X within the parameters set forth in "Part B." This investigation will adhere to a defined "Closeness Rating" of 7 to 10, ensuring focus on the most probable candidates.

Defining the Scope and Objective

The primary goal is unequivocal: to determine the true identity of Element X. This task necessitates a rigorous examination of all available data. The problem requires methodical analysis and insightful deductions.

The Significance of Context: Decoding "Part B"

The term "Part B" alludes to a specific experimental setup, a data set, or perhaps a complex scenario outlined in a laboratory manual or research document. Understanding "Part B" is paramount. It provides the crucial context within which Element X exists. This context can be invaluable for narrowing down possibilities.

"Part B" could contain clues about the origin of the element, its potential reactivity, or the conditions under which it was observed. Without a thorough comprehension of "Part B," the task becomes significantly more challenging.

Utilizing the "Closeness Rating" Filter

The introduction of a "Closeness Rating" between 7 and 10 serves as a valuable filter. This suggests a pre-existing metric used to assess the likelihood of a match between Element X and various candidate elements. This rating system likely incorporates a range of factors, such as spectral similarities, reactivity patterns, or known physical properties.

By focusing on elements within this narrow range, we can streamline the identification process and prioritize the most promising leads. This selective approach enhances efficiency.

Embracing a Structured Methodology

The successful identification of Element X hinges on the application of a structured methodology. A haphazard approach is unlikely to yield accurate results. A systematic strategy ensures that all relevant data is considered and that conclusions are based on sound reasoning.

This methodology should encompass several key steps, including data collection, data analysis, hypothesis generation, and hypothesis testing. Each step must be performed with meticulous attention to detail. By employing a well-defined process, the identification of Element X can be achieved with confidence and precision.

Laying the Groundwork: Fundamental Concepts of Elements

Identifying an unknown element requires a firm grasp of core chemical principles. This section provides a necessary foundation, outlining key concepts such as atomic structure, isotopes, atomic mass, and the critical role of electronic configuration in defining an element's behavior. A comprehensive understanding of these principles is essential for successful element identification.

Defining an Element

At its most basic, an element is a pure substance consisting of only one type of atom. These atoms are characterized by a specific number of protons within their nucleus. This number is non-negotiable; altering the number of protons fundamentally changes the identity of the element. Elements cannot be broken down into simpler substances by chemical means, further solidifying their status as the foundational building blocks of matter.

The Significance of the Atomic Number

Atomic Number as a Unique Identifier

The atomic number is arguably the most crucial piece of information when identifying an element. It represents the number of protons found in the nucleus of every atom of that element.

This number acts as a unique identifier, akin to a fingerprint, definitively distinguishing one element from another. For instance, all atoms with an atomic number of 6 are carbon atoms, and all atoms with an atomic number of 79 are gold atoms.

The atomic number is typically denoted by the symbol Z. It dictates the element's position within the periodic table and underpins many of its chemical and physical properties.

Isotopes and Their Variations

While the number of protons defines an element, the number of neutrons can vary. Isotopes are variants of an element that have the same number of protons but different numbers of neutrons.

This difference in neutron count affects the mass number (total number of protons and neutrons) of the atom, but not its chemical properties. For example, carbon-12 (¹²C) and carbon-14 (¹⁴C) are both isotopes of carbon. They both have 6 protons, but carbon-12 has 6 neutrons, while carbon-14 has 8 neutrons.

The existence of isotopes introduces the concept of isotopic abundance, the relative amount of each isotope found naturally. This abundance is critical for accurately determining the average atomic mass of an element.

Atomic Mass/Weight Calculation

The atomic mass (or atomic weight) of an element is the weighted average of the masses of its isotopes, taking into account their natural abundance. It's typically expressed in atomic mass units (amu).

Calculating atomic mass requires knowing the mass of each isotope and its relative abundance. The formula is: Atomic Mass = (mass of isotope 1 × abundance of isotope 1) + (mass of isotope 2 × abundance of isotope 2) + ...

Understanding atomic mass is crucial for stoichiometric calculations and for relating macroscopic quantities of elements to the number of atoms present.

Chemical vs. Physical Properties

Elements exhibit a range of characteristics that can be broadly categorized as either chemical or physical properties. Distinguishing between these categories is essential for effective element identification.

Chemical Properties: Defining Reactivity

Chemical properties describe how an element interacts with other substances, including its tendency to form chemical bonds and undergo chemical reactions. These properties are determined by the element's electronic configuration, specifically the number and arrangement of valence electrons.

Examples of chemical properties include flammability, reactivity with acids or bases, oxidation state, and the types of chemical bonds an element is likely to form. Observing the chemical behavior of an unknown substance can provide critical clues about its elemental composition.

Physical Properties: Observable Characteristics

Physical properties, on the other hand, can be observed or measured without changing the chemical identity of the substance. These properties include characteristics like color, density, melting point, boiling point, hardness, and electrical conductivity.

Physical properties can be useful for narrowing down the list of potential elements, but they are generally less definitive than chemical properties. They are more easily influenced by external factors, like temperature and pressure.

Deciphering the Electronic Structure: Configuration and Valence

Laying the Groundwork: Fundamental Concepts of Elements Identifying an unknown element requires a firm grasp of core chemical principles. This section provides a necessary foundation, outlining key concepts such as atomic structure, isotopes, atomic mass, and the critical role of electronic configuration in defining an element's behavior. A comprehensive understanding of these principles is paramount for success in identifying Element X.

The Significance of Electron Configuration

Electron configuration, at its core, describes the arrangement of electrons within an atom. This seemingly simple arrangement dictates, to a large extent, how an atom will interact with other atoms.

Electron configuration is not merely a bookkeeping exercise; it is the key to unlocking an element's chemical personality.

The filling of electron shells and subshells follows specific rules, governed by the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Understanding these rules allows us to predict the electronic configuration of any element and, consequently, its expected behavior.

Electron Configuration and Chemical Behavior

The relationship between electron configuration and chemical behavior is direct and profound. Elements with similar valence electron configurations tend to exhibit similar chemical properties. This is why elements within the same group (vertical column) of the periodic table often behave alike.

Consider, for example, the alkali metals (Group 1). They all possess a single valence electron in their outermost shell. This shared electronic feature results in their high reactivity, readily donating that electron to form positive ions.

The arrangement of electrons defines how an atom will interact with its neighbors.

Conversely, the noble gases (Group 18) have completely filled electron shells, making them exceptionally stable and unreactive. Their reluctance to participate in chemical reactions stems directly from their stable electronic configuration.

Valence Electrons: The Architects of Chemical Bonds

Valence electrons are those electrons residing in the outermost electron shell of an atom. They are the primary players in chemical bonding. It is the interaction and redistribution of valence electrons that give rise to the myriad of chemical compounds that exist.

Valence electrons are the "hands" with which atoms reach out and grasp other atoms, forming the molecules that build our world.

The Role of Valence Electrons in Chemical Bonding

Atoms strive to achieve a stable electron configuration, often resembling that of a noble gas. This drive underlies the formation of chemical bonds.

Atoms may gain, lose, or share valence electrons to achieve a full outer shell, creating ionic, covalent, or metallic bonds. The number of valence electrons an atom possesses dictates the type and number of bonds it can form.

For instance, carbon, with four valence electrons, readily forms four covalent bonds, making it the backbone of organic chemistry. Oxygen, with six valence electrons, often forms two covalent bonds, crucial for the formation of water and many other essential molecules. Understanding valence electrons allows us to predict how elements will bond and form compounds. This knowledge is crucial for identifying Element X.

Harnessing the Power of Resources: The Periodic Table

Identifying an unknown element requires a firm grasp of core chemical principles. The periodic table stands as a cornerstone of chemistry, offering a wealth of information crucial for the successful identification of Element X. This section examines the periodic table as an indispensable tool, detailing its organization and demonstrating its practical application in deducing elemental properties.

The Periodic Table: A Map of the Elements

The periodic table is not merely a list of elements; it is a meticulously organized chart reflecting the underlying structure and behavior of matter. Understanding its layout is paramount to unlocking its potential as an identification resource.

Organization by Atomic Number

The foundation of the periodic table lies in the atomic number, which represents the number of protons within an atom's nucleus. Elements are arranged in ascending order of their atomic number, providing a logical progression across the table.

This arrangement is critical because the atomic number uniquely identifies each element. Knowing an element's atomic number immediately narrows down the possibilities and directs the investigation toward the correct location on the table.

Recurring Chemical Properties: Groups and Families

Beyond the atomic number, the periodic table reveals recurring chemical properties. Elements are grouped into vertical columns known as groups or families.

Elements within the same group share similar valence electron configurations, which directly influence their chemical reactivity. This shared characteristic makes groups incredibly useful for predicting how an element might behave in a given chemical reaction, providing invaluable clues for identification.

Periods: Trends Across the Table

In addition to groups, the periodic table exhibits trends across horizontal rows, known as periods. These trends include variations in electronegativity, ionization energy, and atomic radius.

Understanding these periodic trends provides insights into how an element's properties change as its atomic number increases, further refining the identification process. Analyzing these trends in conjunction with data from "Part B" and the Closeness Rating (7-10) enables a methodical approach to identifying Element X.

Using the Periodic Table Effectively

To effectively leverage the periodic table for element identification, consider the following:

• Start with the Atomic Number: If the atomic number is known or can be deduced, locate the corresponding element on the table.

• Examine Group Properties: Analyze the properties of the element's group to predict its chemical behavior.

• Consider Periodic Trends: Evaluate trends across the element's period to further refine the identification.

• Cross-Reference with Experimental Data: Compare the predicted properties with experimental data to confirm the identification.

By systematically employing the periodic table and its organization, coupled with the analytical methods discussed, the identification of Element X within Part B becomes an achievable and well-informed scientific endeavor. The periodic table becomes more than just a chart; it transforms into a powerful analytical tool.

Data Analysis: Interpreting Numerical Clues

Identifying an unknown element is akin to solving a puzzle, where the pieces are the data provided. This data, often numerical, serves as the key to unlocking the identity of Element X. This section delves into the crucial role of accessing and interpreting numerical data, such as mass, volume, and spectral data, in the quest for element identification.

Accessing Relevant Data

The first step in data analysis is ensuring access to all available information. This includes not only directly measured values like mass and volume but also derived data and spectral outputs. Data sources may include laboratory reports, instrument readouts, and online databases.

It is imperative to meticulously record and organize all data points, as even seemingly insignificant values can prove crucial in the later stages of analysis. Missing or improperly documented data can significantly hinder the identification process.

Understanding Numerical Data: Mass and Volume

Mass and volume measurements are fundamental properties that provide essential clues about the identity of an element. Understanding how to utilize these values is critical in the identification process.

Utilizing Molar Mass Calculations

The molar mass is the mass of one mole of a substance. Comparing the experimentally determined mass to expected molar masses helps narrow down the possible identities of Element X.

Consider the scenario where one has measured the volume of gas produced from a reaction involving the unknown Element X. By knowing the stoichiometry of the reaction, one can then calculate the number of moles of gas produced.

This allows for the experimental determination of the molar mass of Element X, and it can then be compared to the molar masses of possible elemental candidates in the periodic table.

Density as a Tool

Density, defined as mass per unit volume, can also be a very helpful physical property. Measuring mass and volume of an Element X sample enables density determination.

This provides another physical parameter for comparison with known elemental densities. Notably, this also requires one to account for temperature and pressure when dealing with gases, as these external conditions can greatly affect measured densities.

Spectroscopic Data Analysis

Spectroscopy provides a powerful means of identifying elements through their interaction with electromagnetic radiation. Each element possesses a unique spectral "fingerprint," making this technique invaluable in elemental analysis.

Interpreting Emission Spectra

Emission spectra are produced when excited atoms release photons of specific wavelengths. The wavelengths of emitted light are unique to each element and can be used for identification.

The presence of specific spectral lines can confirm the presence of a particular element in the sample. Conversely, the absence of expected spectral lines can effectively rule out elements from consideration.

Decoding Absorption Spectra

Absorption spectra are generated when atoms absorb photons of specific wavelengths. These absorbed wavelengths correspond to transitions between energy levels within the atom.

The pattern of absorption lines is unique to each element, providing another "fingerprint" for element identification. Analyzing both emission and absorption spectra provides a more comprehensive understanding.

Unlocking Contextual Clues: Analyzing "Part B"

Identifying an unknown element is akin to solving a puzzle, where the pieces are the data provided. This data, often numerical, serves as the key to unlocking the identity of Element X. This section delves into the crucial role of accessing and interpreting numerical data, such as mass, volume, and spectral readings, and how this impacts the identification process.

The Significance of "Part B"

In the quest to identify Element X, “Part B” emerges as a pivotal source of contextual clues. It represents more than just supplementary information; it is the framework within which the element exists.

The information provided in Part B is essential for understanding the chemical environment and any interactions Element X might be undergoing. This context is paramount for narrowing down the possibilities and making informed deductions.

Decoding Experimental Design

Analyzing the experimental design detailed in Part B provides valuable insights into the conditions under which Element X is being observed. This includes the experimental apparatus used, the presence of specific reagents, and the overall setup.

These details can directly hint at the properties and potential reactions that Element X might exhibit. Understanding the experimental design provides a framework for interpreting the results obtained.

Analyzing Reagents and Chemical Interactions

The reagents employed in the experiment play a crucial role in determining the behavior of Element X. Identifying the reagents and understanding their properties can reveal potential reactions and interactions.

For example, the presence of a strong oxidizing agent might indicate that Element X is susceptible to oxidation. Similarly, the use of a specific catalyst might suggest the involvement of Element X in a particular type of chemical reaction.

Furthermore, consideration of potential chemical reactions based on the reagents can lead to understanding the compounds Element X may form. This includes potential products and intermediates. Understanding the roles of all these substances is crucial.

Deciphering Available Information

Beyond the experimental setup and reagents, Part B often contains a wealth of additional information that can aid in the identification process. This might include:

• Observations recorded during the experiment, such as color changes or the formation of precipitates.
• The purpose of the experiment and the objectives it aims to achieve.
• Any assumptions or limitations that were considered during the design of the experiment.

By carefully analyzing all the available information, a clearer picture of Element X begins to emerge. The clues scattered throughout Part B, when pieced together, provide a solid foundation for the subsequent steps in the identification process.

Experimental Investigations: Setup, Reactions, and Procedures

Identifying Element X requires a meticulous examination of the experimental context outlined in "Part B." This section focuses on dissecting the experimental setup, the reagents employed, and the procedures followed. By carefully analyzing these elements, we can significantly narrow down the range of potential candidates for Element X.

Deconstructing the Experimental Setup

The experimental setup serves as the initial framework for understanding the context in which Element X exists and reacts. A thorough analysis of this setup can provide valuable insights into the element's potential properties and behavior.

Pay close attention to the following aspects of the experimental setup:

• Apparatus: The type of equipment used can indicate the nature of the experiment and the properties being investigated (e.g., distillation apparatus suggesting volatility).
• Conditions: Temperature, pressure, and presence of a controlled atmosphere can reveal the stability and reactivity of Element X under specific conditions.
• Physical State: Observing the initial and final physical states of the substances involved (solid, liquid, gas) gives clues regarding phase changes and reactions.

Deciphering Chemical Reactions and their Products

Understanding the chemical reactions that occur within "Part B" is paramount to identifying Element X. This involves identifying the reactants, the conditions under which the reaction proceeds, and the products formed.

Key Considerations for Analyzing Chemical Reactions:

• Reaction Type: Identifying the type of reaction (e.g., oxidation-reduction, acid-base, precipitation) can help predict the chemical behavior of Element X.
• Stoichiometry: Analyzing the stoichiometric ratios of reactants and products can provide clues about the element's valence and bonding capabilities.
• Reaction Conditions: Factors like catalysts or heat applied can significantly affect reaction pathways and outcomes.
• Expected products: By analyzing the chemical reaction, you can predict expected products and determine if they are consistent with the element identified.

Evaluating the Reagents

Reagents are substances added to cause a chemical reaction. The reagents used in the experiments can help give insight to Element X.

Some key areas to focus on:

• Role of Reagents: Understanding the purpose and function of each reagent.
• Known properties of Reagents: Understanding the properties of the reagent will allow to better determine properties of Element X.
• Identify reaction of Reagents: Use the reaction created by reagents to determine elements properties.

Interpreting Experimental Observations

Careful observation and interpretation of experimental results provides insight into the chemical and physical properties of Element X.

Types of experimental observations to be aware of:

• Color Changes: Color alterations during a reaction can suggest the formation of new complexes or compounds containing Element X.
• Phase Transitions: Changes in physical state (e.g., melting, boiling, sublimation) can indicate the element's physical properties and phase transition temperatures.
• Gas Evolution: The production of gases (e.g., oxygen, hydrogen, carbon dioxide) can indicate the occurrence of specific reactions involving Element X.
• Precipitate Formation: The appearance of a solid precipitate from a solution can suggest the formation of insoluble compounds containing Element X.

Strategic Problem Solving: Textbook Problems and Lab Reports

Building upon the foundation of experimental understanding, the next crucial step involves strategically leveraging existing knowledge repositories. Textbook problems and laboratory reports serve as invaluable resources, offering pre-existing analyses and data sets that can significantly accelerate the identification of Element X. This section details how to effectively utilize these resources.

Textbook Problem Analysis

Textbooks, often overlooked as simple repositories of information, are meticulously curated collections of solved problems and conceptual explanations. These problems are not merely exercises; they are carefully crafted scenarios designed to reinforce key concepts.

Identifying Relevant Chapters and Examples

The initial step is to pinpoint the chapters and example problems that directly correlate with the experimental conditions outlined in "Part B." Pay close attention to chapters focusing on:

• Stoichiometry: Essential for understanding quantitative relationships.
• Chemical Reactions: Providing insights into potential reactions.
• Spectroscopy: Allowing you to interpret spectral data effectively.

Within these chapters, example problems often showcase step-by-step solutions that can serve as models for analyzing the data related to Element X.

Extracting Key Concepts and Methodologies

Carefully dissect the methodology employed in the textbook's example problems. Note the specific equations, assumptions, and problem-solving strategies used.

Adapt these approaches to the unique challenges presented by "Part B," focusing on identifying any parallels or deviations that might offer clues about the identity of Element X.

Laboratory Report Analysis

Laboratory reports provide a wealth of empirical data, including observations, measurements, and conclusions drawn from similar experiments. Properly analyzing these reports is crucial.

Sourcing and Selecting Relevant Reports

Identifying reports that align with "Part B" is key. Prioritize reports that detail experiments involving:

• Similar reactions or compounds.
• Comparable analytical techniques.
• Elements within the "Closeness Rating" range of 7-10.

Dissecting the Data and Analysis

The core of a laboratory report lies in its data and subsequent analysis. Scrutinize the following elements:

• Experimental Procedure: Understanding the exact steps taken can reveal crucial details.
• Raw Data: Examine the original measurements for anomalies or patterns.
• Data Analysis: Evaluate the statistical methods employed and the conclusions drawn.
• Error Analysis: Identify potential sources of error that could influence the results.

Comparing and Contrasting with "Part B"

The ultimate goal is to compare and contrast the findings in the laboratory reports with the data and observations from "Part B." Look for similarities and differences in:

• Reaction Rates: Suggesting elements with similar reactivity.
• Spectral Signatures: Providing direct elemental identification.
• Physical Properties: Narrowing down the list of possibilities.

By meticulously cross-referencing textbook examples and analyzing laboratory reports, it becomes easier to systematically narrow down the list of potential candidates for Element X, paving the way for a definitive identification.

Strategic Approaches: Elimination and Detail

Building upon the foundation of experimental understanding, the next crucial step involves strategically leveraging existing knowledge repositories. Textbook problems and laboratory reports serve as invaluable resources, offering pre-existing analyses and data sets that can significantly aid in identifying Element X. However, to effectively navigate these resources and apply them to the problem at hand, a strategic approach is essential. This involves meticulous attention to detail, employing a process of elimination, and understanding the required level of granularity for the analysis.

The Importance of Careful Instruction Review

A critical first step in any scientific endeavor is a thorough review of all available instructions and guidelines. These instructions often contain explicit clues, constraints, or specific parameters that can significantly narrow the range of possibilities.

Ignoring seemingly minor details can lead to misinterpretations and wasted effort, emphasizing the need for a meticulous approach. Careful attention to detail can reveal hidden assumptions or specific directives that are crucial for successful element identification.

Employing the Process of Elimination

The periodic table, while comprehensive, presents a wide array of potential candidates for Element X. Therefore, a systematic process of elimination is vital to efficiently narrow down the possibilities.

This involves leveraging known properties of elements, such as physical state at a given temperature, characteristic reactions with specific reagents, and expected spectral signatures. By comparing these known properties with the observed behavior of Element X, elements that demonstrably do not match can be systematically excluded.

This process of elimination requires a strong understanding of elemental properties and the ability to correlate them with experimental observations.

Determining the Required Level of Detail

Not all scientific inquiries demand the same level of precision or depth of analysis. It is crucial to evaluate the specific research problem or question to determine the appropriate level of detail required.

Overly detailed analysis can be time-consuming and resource-intensive, while insufficient detail can lead to inaccurate conclusions. Striking a balance between thoroughness and efficiency is paramount.

Understanding the specific objectives and constraints of the analysis will guide the determination of the appropriate level of detail. For example, a preliminary analysis might focus on identifying the group or family to which Element X belongs, before delving into more specific characteristics to pinpoint the exact element.

Harnessing Analytical Techniques: Spectroscopic Methods

Transitioning from strategic problem-solving, we now delve into the realm of analytical techniques, specifically spectroscopic methods. These techniques provide a powerful means of identifying elements based on their unique interactions with electromagnetic radiation. A thorough understanding of these interactions and the ability to interpret spectral data are crucial for accurate elemental identification.

Spectroscopy: A Window into Elemental Identity

Spectroscopy encompasses a range of techniques that analyze the interaction of electromagnetic radiation with matter. Each element possesses a unique electronic structure, which dictates how it absorbs, emits, or scatters radiation at specific wavelengths. This unique spectral "fingerprint" allows for definitive identification.

The fundamental principle behind spectroscopy lies in the quantization of energy levels within atoms. Electrons can only occupy discrete energy states, and transitions between these states involve the absorption or emission of photons with energies precisely matching the energy difference between the levels.

The Interaction with Electromagnetic Radiation

The interaction of elements with electromagnetic radiation is highly specific and dependent on the energy of the radiation. When a photon of appropriate energy strikes an atom, an electron can be excited to a higher energy level. This absorption process results in a decrease in the intensity of the radiation at that particular wavelength.

Conversely, when an electron transitions from a higher energy level to a lower one, a photon is emitted. The wavelength of the emitted photon is directly related to the energy difference between the two levels. This emission process forms the basis of emission spectroscopy.

Analyzing Spectral Data for Elemental Composition

The interpretation of spectral data is a critical skill in elemental identification. Spectral data typically consists of a plot of intensity versus wavelength or frequency. The positions and intensities of peaks in the spectrum provide valuable information about the elemental composition of the sample.

Identifying Elements from Emission Spectra

Emission spectra are characterized by discrete lines at specific wavelengths, corresponding to the emission of photons by excited atoms. The wavelengths of these lines are unique to each element and serve as a definitive identifier. The intensity of each line is proportional to the concentration of the element in the sample.

Using Absorption Spectra for Elemental Analysis

Absorption spectra, on the other hand, show dips in intensity at specific wavelengths, corresponding to the absorption of photons by the sample. The wavelengths of these absorption dips are also unique to each element. Analyzing the absorption spectrum provides insights into the presence and concentration of specific elements.

Quantitative Analysis with Spectroscopic Data

Beyond qualitative identification, spectroscopic methods also facilitate quantitative analysis. By carefully calibrating the instrument and measuring the intensity of spectral lines or absorption bands, the concentration of an element can be determined with high accuracy. This is particularly useful in determining the composition of unknown samples or tracking the concentration of specific elements in a reaction.

Effective utilization of spectroscopy demands meticulous data analysis and a deep understanding of atomic structure and spectroscopic principles. With careful application, it provides a powerful method for identifying and quantifying elements.

So, there you have it! Hopefully, this guide has cleared up any confusion and you now know exactly what is the identity of element X from part B. Go forth and conquer those chemistry questions! Good luck!