A Comprehensive Guide to the ICP Periodic Table: Key Elements and Their Properties

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Overview The first stage of a trace analysis is planning the project. This chapter discusses the process of planning, which involves defining the problem and assessing the technical requirements needed to solve the problem. Without careful planning, achieving reliable results becomes a game of chance. Analytical projects fall into categories of non-routine, semi-routine, and routine: Non-routine - a project in which a validated method does not exist and little is known about the sample. Semi-routine - a project in which something significant can be stated about the sample and the method of analysis. Routine - a project in which the sample is chemically known and a validated method is available. This chapter assumes that the chemist will be analyzing samples that fall into one or more of the above categories. Before the planning process can begin, the analyst must examine the following: The need for sampling and sub-sampling Reagent quality Sample preparation Measurement QA/QC Reporting requirements Defining the Problem A discussion between the initiator and the analyst must occur, where questions are asked by both parties. The intent is to define the exact nature of the problem, why analytical work is needed, and how the results will be used following the completion of the project. Method validation requirements should also be addressed. These requirements can include either the availability of a certified reference material, or that of another validated technique -- one that is based largely on different principles. The problem's definition is further refined by asking other questions: What is it that you want to accomplish? What is the purpose? What is the current situation or state of affairs? What is taking place that you need to understand, prevent, or improve? What decisions will be made based upon the data? When the answers to these questions have been determined, the analyst is in a position to begin planning the analytical process. Detection Limits and Uncertainty The analyst should know the detection limits for all analytes at several possible wavelengths. Typically, these measurements are obtained during the establishment of the analytical instrument's capabilities. Modern axial view ICP-OES and ICP-MS instruments are likely to have detection limits under normal sample introduction modes that will meet or exceed the requirements. It is best to not rely upon the limits published by the manufacturer. In addition, the detection limits will be a function of the sample matrix, in both a physical and spectral sense. A key point involves the analytical blank. Due to numerous contamination issues, the analytical blank often determines the detection limit capabilities. It is best for the analyst to be conservative when noting the detection limits, making sure not to quote capabilities calculated from published data or determinations made under "ideal" conditions. For the less common elements, an estimate of the "real" detection limit would be a factor several times higher than the limit determined under ideal conditions. Thus, elements like Na, Mg, Ca, Fe, Cr, Cu, Zn, Si, Al, Cl, and S may have a detection limit that is significantly larger than expected, due to the analytical blank. The uncertainty of an analytical measurement is not limited to the measurement precision of the instrument. Rather, it is a statistical sum of the random and systematic errors that are encountered throughout the entire analytical process. The uncertainty is a combination of errors from sampling, storage, weight and volume manipulations, preparation, calibration, and measurement, during which contamination issues play a major role in trace determinations. The sampling error can be a major source of uncertainty. In many cases, an estimate of the sampling error can be impossible to judge. The initiator should be aware of this fact. In reality, the uncertainty of a trace measurement will not be known until the project is completed. The accuracy of this value will be only as good as the effort made to identify and measure all of the errors encountered during the entire analytical process. If measurements are being made between 3-5 times the detection limit for the less common elements, then an excellent uncertainty would be ± 30-70%. Constructing the Sampling Plan After the problem is defined, the planning process can begin. Analytical text books explain that you must consider the sample collection, sample storage, sample preparation, measurement, and reporting, along with any QA/QC requirements. With so many considerations, where should you start? A synthetic organic chemist will construct a plan by working backwards from the final product. A similar approach may work well for the trace analyst. Start by examining the following basic information: The analyte(s) of interest. The required detection limit(s). The uncertainty requirement(s). The chemical composition (matrix) of the sample. The quantity, availability, and history of the sample. Much of the above list can be determined based on information gathered while defining the problem. In most cases, analytical resources are available in-house to address the problem. For example: The basic information listed above is sufficient to determine whether publications or information is available in your reference library. Always start with a search of the literature. The identity and detection limit requirement of each analyte indicates the analyte measurement technique(s) required and the amount of sample required. The uncertainty requirement indicates the number of measurements, assuming there is sufficient sample available. The chemical composition of the sample, together with the identity of the analyte(s), indicates possible sample preparation routes. The identity of the analyte(s), together with the detection limit requirement(s), indicates the degree that contamination issues should be considered. This determines the need for analytical blanks and special apparatus or a clean area / room. The sample composition indicates potential interference issues. The sample composition or type indicates the uncertainty to be expected form the sample collection and/or the need to develop a sampling procedure and to determine sampling uncertainty. For example, the sample may be the only "world's supply", negating the need for a sampling procedure. The estimated sampling uncertainty can be used to define the analytical measurement precision (i.e. -- reducing the analytical error to less than one third of the sampling error serves no purpose). The basic information can provide the analyst with potential analytical measurement technique(s), suspected interferences, contamination issues, and the number of sample measurements required per determination (measurement refers to a complete analysis including sampling, preparation, instrumental analysis and reporting the final result and uncertainty). At this stage of the planning process, the analyst can determine if a certified reference material (CRM) should be obtained for method validation. In addition, the chemist can approximate the need for analytical reagents and apparatus and/or calibration standards. Lastly, estimate the time and cost of the project and base your initial approach on these estimates. Remember, there is always the possibility that more than one iteration may be required before an acceptable approach can be developed.


Inductively Coupled Plasma (ICP) analysis is a critical technique used in various industries to detect and measure trace metals. Understanding the behavior and characteristics of elements in this context is essential for accurate analysis. This guide will walk you through some key elements in the ICP Periodic Table, highlighting their properties, chemical behavior, and best practices for handling and storage.

1. Lithium (Li)

  • Location: Group 1, Period 2
  • Atomic Weight: 6.941
  • Coordination Number: 6 (assumed)
  • Chemical Form in Solution: Li⁺(aq)
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container, and do not return unused portions to the original container.
  • Chemical Compatibility: Soluble in HCl, HNO₃, H₂SO₄, and HF aqueous matrices. Stable with all metals and inorganic anions.
  • Stability: 2–100 ppb levels are stable for months in 1% HNO₃/LDPE container, while 1–10,000 ppm solutions are stable for years.
  • Sample Preparation: Dissolves rapidly in water; for ores, use sodium carbonate fusion in Pt⁰ followed by HCl dissolution.

2. Beryllium (Be)

  • Location: Group 2, Period 2
  • Atomic Weight: 9.01218
  • Coordination Number: 4
  • Chemical Form in Solution: Be⁺(H₂O)₄²⁺
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Soluble in HCl, HNO₃, H₂SO₄, and HF aqueous matrices. Stable with all metals and inorganic anions.
  • Stability: 2–100 ppb levels stable for months in 1% HNO₃/LDPE container; 1–10,000 ppm solutions are stable for years.
  • Sample Preparation: Metal dissolves best in diluted H₂SO₄; for BeO, use boiling acids or KHSO₄ fusion.

3. Boron (B)

  • Location: Group 13, Period 2
  • Atomic Weight: 10.811
  • Coordination Number: 4
  • Chemical Form in Solution: B(OH)₃ and B(OH)₄⁻
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Moderately soluble in HCl, HNO₃, H₂SO₄, and HF aqueous matrices, and very soluble in NH₄OH.
  • Stability: 2–100 ppb levels stable for months in 1% HNO₃/LDPE container; 1–1,000 ppm solutions stable for years.
  • Sample Preparation: Amorphous form is soluble in concentrated HNO₃ or H₂SO₄; for ores, avoid acid digestions and use caustic fusions in Pt⁰.

4. Carbon (C)

  • Location: Group 14, Period 2
  • Atomic Weight: 12.011
  • Coordination Number: 4
  • Chemical Form in Solution: Tartaric Acid (used to make Carbon standards)
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Moderately soluble in HCl, HNO₃, H₂SO₄, and HF aqueous matrices, and very soluble in NH₄OH.
  • Stability: 1000–10,000 ppm level stable for years in dilute acidic media in a glass container.
  • Sample Preparation: Use oxidative closed vessel fusion for elemental carbon, or Na₂O₂ fusion for organic compounds.

5. Sodium (Na)

  • Location: Group 1, Period 3
  • Atomic Weight: 22.98977
  • Coordination Number: 6 (assumed)
  • Chemical Form in Solution: Na⁺(aq)
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Soluble in HCl, HNO₃, H₂SO₄, and HF aqueous matrices. Stable with all metals and inorganic anions.
  • Stability: 2–100 ppb levels stable for months in 1% HNO₃/LDPE container; 1–10,000 ppm solutions stable for years.
  • Sample Preparation: Dissolves rapidly in water; for ores, use lithium carbonate fusion in a graphite crucible followed by HCl dissolution.

6. Magnesium (Mg)

  • Location: Group 2, Period 3
  • Atomic Weight: 24.305
  • Coordination Number: 6
  • Chemical Form in Solution: Mg(H₂O)₆²⁺
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Soluble in HCl, HNO₃, H₂SO₄. Avoid HF, H₃PO₄, and neutral to basic media.
  • Stability: 2–100 ppb levels stable for months in 1% HNO₃/LDPE container; 1–10,000 ppm solutions stable for years.
  • Sample Preparation: Best dissolved in diluted HNO₃; for oxides, use compatible aqueous acidic solutions.

7. Aluminum (Al)

  • Location: Group 13, Period 3
  • Atomic Weight: 26.98154
  • Coordination Number: 6
  • Chemical Form in Solution: Al(H₂O)₆³⁺
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Soluble in HCl, HNO₃, HF, and H₂SO₄. Avoid neutral media.
  • Stability: 2–100 ppb levels stable for months in 1% HNO₃/LDPE container; 1–10,000 ppm solutions stable for years.
  • Sample Preparation: Dissolves best in HCl/HNO₃; for oxides, use Na₂CO₃ fusion in Pt⁰.

8. Silicon (Si)

  • Location: Group 14, Period 3
  • Atomic Weight: 28.0855
  • Coordination Number: 6
  • Chemical Form in Solution: Si(OH)x(F)y²⁻
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Soluble in HCl, HF, H₃PO₄, H₂SO₄, and HNO₃. Avoid neutral to basic media.
  • Stability: 1–10,000 ppm single element solutions stable for years in 2–5% HNO₃/trace HF in an LDPE container.
  • Sample Preparation: Soluble in 1:1:1 H₂O/HF/HNO₃; for quartz, use Na₂CO₃ fusion in Pt⁰.

9. Phosphorus (P)

  • Location: Group 15, Period 3
  • Atomic Weight: 30.97376
  • Coordination Number: 6
  • Chemical Form in Solution: OP(OH)₂(O)¹⁻
  • Handling and Storage: Store tightly sealed at 20 ± 4°C. Avoid pipetting directly from the container.
  • Chemical Compatibility: Soluble in HCl, HNO₃, H₂SO₄, HF, water, and NH₄OH. Stable with all metals and inorganic anions under acidic conditions.
  • Stability: 1–10,000 ppm solutions stable for years in 0–1% HNO₃/LDPE container.
  • Sample Preparation: For oxides, use water; for ores, use Na₂CO₃ fusion in Pt⁰.

Each element in the ICP Periodic Table has unique properties that influence its behavior in analytical procedures. Proper handling, storage, and understanding of chemical compatibility are essential for accurate and reliable ICP analysis. This guide serves as a foundational reference for laboratory professionals and researchers who work with these critical elements.