What is the chemical symbol for Mercury?
Mg
Hg
H
Mn
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Mercury
Dive into the enigmatic world of mercury, a liquid metal that fascinates with its unique properties and wide-ranging applications. From ancient alchemical practices to modern scientific and industrial uses, mercury’s versatility is unmatched. This guide explores mercury’s role in thermometers, dental amalgams, and even in the extraction of gold and silver. Discover the intriguing aspects of mercury, including its compounds, safety measures, and environmental impact, through practical examples and insightful analysis. Embrace the liquid marvel that is mercury, understanding its essence and significance in our world.
What is Mercury ?
Mercury is a unique, silvery liquid metal known for its remarkable properties and diverse range of applications, with the atomic number 80. It is distinguished by its ability to remain liquid at room temperature, making it exceptionally versatile in various scientific and industrial settings. mercury does not occur freely but is commonly found in the mineral cinnabar from which it is extracted through heating and condensing. Mercury’s applications span across multiple fields; it is used in the chemical industry as a catalyst in the production of chlorine and caustic soda via the chlor-alkali process, and in dentistry for amalgam fillings.
Mercury Formula
- Formula: Hg
- Composition: Consists of a single mercury atom.
- Bond Type: In its elemental form, mercury does not have bonds as it is a pure element. However, mercury can form covalent or ionic bonds when reacting with other elements.
- Molecular Structure: As a pure element, mercury does not form a molecular structure in the same sense as compounds like H₂. At room temperature, mercury is in a liquid state, unique among metals, without a fixed crystalline structure.
- Electron Sharing: In compounds, mercury typically shares electrons covalently or transfers electrons ionically, depending on the nature of the other element(s) it is bonding with.
- Significance: Mercury is known for its liquidity at room temperature and its ability to form amalgams with other metals, excluding iron. This makes it invaluable in various applications, including dental amalgams, thermometers, and barometers. Mercury’s compounds, especially its organomercury compounds, are used in catalysis and as antifungal agents in agriculture.
- Role in Chemistry: Mercury plays a critical role in electrochemistry and is pivotal in the production of chlorine and caustic soda via the chlor-alkali process. Its unique properties and reactions make it a significant element in both historical and modern chemical processes, contributing to various fields, including analytical chemistry and material science.
Atomic Structure of Mercury
Introduction to Mercury’s Atomic Properties
- Element Symbol: Hg (Hydrargyrum)
- Atomic Number: 80
- Atomic Mass: Approximately 200.59 u
Electron Configuration
- Shell Structure: 2, 8, 18, 32, 18, 2
- Electronic State: [Xe] 4f¹⁴ 5d¹⁰ 6s²
- Valence Electrons: 2 in the outermost shell
Physical Characteristics
- State at Room Temperature: Liquid
- Boiling Point: 356.73°C (674.11°F)
- Melting Point: -38.83°C (-37.89°F)
Chemical Properties
- Reactivity: Low, but forms amalgams with many metals
- Oxidation States: Most common are +1 and +2
- Electronegativity: Pauling scale – 2.00
Role in Compounds
- Common Compounds: Mercuric chloride (HgCl₂), Mercurous chloride (Hg₂Cl₂), Mercury fulminate (Hg(ONC)₂)
- Usage in Industry: Catalysts, electrical switches, and in the production of chlorine gas and caustic soda
Environmental Impact and Safety
- Toxicity: Highly toxic, exposure can damage the nervous, digestive, and immune systems
- Handling and Disposal: Requires special safety measures to avoid contamination and poisoning
Properties of Mercury
Physical Properties of Mercury
| Property | Value |
|---|---|
| Appearance | Silvery, liquid metal |
| Atomic Number | 80 |
| Atomic Mass | 200.592 u |
| Density at 20°C | 13.534 g/cm³ |
| Melting Point | -38.83°C (-37.89°F) |
| Boiling Point | 356.73°C (674.11°F) |
| State at 20°C | Liquid |
| Electrical Conductivity | 1.04 × 10^6 S/m |
| Thermal Conductivity | 8.30 W/(m·K) |
| Heat of Fusion | 2.29 kJ/mol |
| Heat of Vaporization | 59.11 kJ/mol |
| Specific Heat Capacity | 27.983 J/(mol·K) |
Chemical Properties of Mercury
Mercury, symbolized as Hg, stands out for being the only metal liquid at room temperature and exhibits unique chemical behaviors:
Oxidation States: Exhibits +1 (mercurous) and +2 (mercuric) oxidation states. Mercuric compounds, such as mercuric chloride (HgCl₂), are more stable and commonly encountered.
Reaction with Oxygen: Forms mercuric oxide (HgO) when heated with oxygen: 2 Hg+O₂→2 HgO₂
Amalgamation: Readily forms amalgams with many metals except iron, useful in metal extraction processes.
Acid Reactions: Inert to dilute acids but dissolves in nitric acid and hot concentrated sulfuric acid, forming mercuric nitrate and sulfate.
Organomercury Compounds: Forms toxic organomercury compounds, such as methylmercury (CH₃Hg⁺), highlighting environmental and health risks.
Volatility: Mercury vapor is highly toxic, requiring careful handling and ventilation.
Thermodynamic Properties of Mercury
| Property | Value |
|---|---|
| Melting Point | -38.83°C (-37.89°F) |
| Boiling Point | 356.73°C (674.11°F) |
| Heat of Fusion | 2.29 kJ/mol |
| Heat of Vaporization | 59.11 kJ/mol |
| Specific Heat Capacity | 27.983 J/(mol·K) |
| Thermal Conductivity | 8.34 W/(m·K) |
Material Properties of Mercury
| Property | Value |
|---|---|
| State at Room Temperature | Liquid |
| Density | 13.534 g/cm³ at 20°C |
| Molar Volume | 14.09 cm³/mol |
| Young’s Modulus | N/A (Liquid State) |
| Shear Modulus | N/A (Liquid State) |
| Bulk Modulus | 25 GPa |
Electromagnetic Properties of Mercury
| Property | Value |
|---|---|
| Electrical Conductivity | 1.04×10^6 S/m |
| Electrical Resistivity | 96 nΩ·m (at 0°C) |
| Magnetic Susceptibility | -28.0·10^-6 cm^3/mol |
| Superconducting Point | 4.15 K |
Nuclear Properties of Mercury
| Property | Value |
|---|---|
| Natural Isotopes | ^196Hg, ^198Hg, ^199Hg, ^200Hg, ^201Hg, ^202Hg, ^204Hg |
| Most Stable Isotope | ^202Hg (Half-life: >1.4×10^21 years) |
| Neutron Cross Section | 374.8 barns (for ^196Hg) |
| Neutron Mass Absorption | 0.056 (for ^196Hg) |
Preparation of Mercury
The preparation of mercury, a unique metal that is liquid at room temperature, primarily involves the extraction and refinement from its most common ore, cinnabar (mercury sulfide, HgS). Here’s a concise overview of the process:
Extraction from Cinnabar
- Ore Processing: Cinnabar ore is crushed and heated in a furnace.
- Thermal Decomposition: The heating process triggers a reaction where cinnabar decomposes, releasing mercury vapor and leaving behind sulfur dioxide.HgS+O₂→Hg+SO₂
Mercury Vapor Collection
- Cooling: The mercury vapor is then cooled in a series of condensers.
- Liquid Mercury: This cooling process condenses the vapor back into liquid mercury, which is collected at the bottom.
Purification
- Distillation: To remove impurities, the liquid mercury undergoes distillation, a process that takes advantage of mercury’s low boiling point compared to other contaminants.
- Triple Distillation: For high-purity applications, mercury may be distilled multiple times
Chemical Compounds of Mercury
- Mercury(II) Chloride (HgCl₂)
- A potent antiseptic historically used, also known as corrosive sublimate.
- Equation:
- Mercury(I) Chloride (Hg2Cl₂)
- Known as calomel, used in electrochemistry and as a medicinal purgative.
- Equation:
- Mercury(II) Oxide (HgO)
- Decomposes upon heating, producing mercury and oxygen, used in mercury batteries.
- Equation:
- Mercury(II) Sulfide (HgS)
- Occurs naturally as cinnabar, used as a pigment and in mercury extraction.
- Equation:
- Mercury(I) Nitrate (Hg2(NO₃)₂)
- Utilized in antiseptic formulations and the preparation of other mercury compounds.
- Equation:
- Mercury(II) Fulminate (Hg(CNO)₂)
- A primary explosive used in detonators, highly sensitive to friction and impact.
- Equation:
Isotopes of Mercury
Below is a table highlighting some of the notable isotopes of mercury, including both stable and radioactive varieties:
| Isotope | Half-Life | Notes |
|---|---|---|
| ¹⁹⁶Hg | Stable | One of the most common stable isotopes, used in research. |
| ¹⁹⁸Hg | Stable | Also stable, present in the environment. |
| ¹⁹⁹Hg | Stable | Frequently used in NMR spectroscopy due to its nuclear spin. |
| ²⁰⁰Hg | Stable | Another stable isotope, contributing to mercury’s natural abundance. |
| ²⁰¹Hg | Stable | Used in atomic clocks and for studying brain function via tracing techniques. |
| ²⁰²Hg | Stable | The most abundant mercury isotope found in nature. |
| ²⁰⁴Hg | Stable | The least abundant stable mercury isotope. |
| ¹⁹⁴Hg | 444 years | A beta-emitter, used in research. |
| ²⁰³Hg | 46.612 days | Emits beta and gamma radiation, used in industrial and medical applications. |
Uses of Mercury
Mercury’s unique properties make it invaluable across various industries and applications:
Thermometers and Barometers: Due to its liquid state at room temperature and high coefficient of expansion, mercury is used in precise thermometers, barometers, and manometers.
Dental Amalgams: Mercury’s ability to form amalgams with other metals makes it an essential component in dental fillings, providing durability and ease of application.
Electrical Switches: Mercury’s conductivity and liquid state are exploited in silent, non-sparking electrical switches, relays, and other devices where a stable, durable conductor is needed.
Chlor-alkali Process: Used in the production of chlorine and sodium hydroxide (caustic soda) through the electrolysis of brine, mercury acts as a catalyst, making the process more efficient.
Gold and Silver Mining: Mercury’s property of forming amalgams with gold and silver allows for the efficient extraction of these metals from their ores.
Preservatives and Lamps: Mercury compounds serve as preservatives in some paints and cosmetics. Mercury vapor lamps, including fluorescent lamps, use mercury to produce light, offering energy efficiency and long life.
Scientific Research: Due to its nuclear properties, mercury isotopes are used in scientific research, including nuclear physics experiments and as tracers in environmental and biological studies.
Production of Mercury
Primary Sources
- Cinnabar Ore: The most common mercury ore, mined and then heated in a furnace to vaporize the mercury.
- By-Product: Mercury is also obtained as a by-product of mining for other metals, such as zinc and gold.
Extraction Process
- Mining: Cinnabar ore is extracted from mercury mines.
- Roasting: The ore is heated in air to release mercury vapor.
- Condensation: Mercury vapor is cooled and condensed into liquid mercury.
- Purification: The liquid mercury is purified through distillation or filtration processes.
Global Production
- Leading Producers: China, Kyrgyzstan, and Chile are among the top producers of mercury.
- Regulations: The production and trade of mercury are regulated globally due to its toxicity and environmental impact.
Applications of Mercury
In Industry
- Chlor-alkali Process: Used in the production of chlorine and caustic soda.
- Electrical and Electronics: In switches, thermostats, and fluorescent lighting.
- Gold Mining: Amalgamation process to extract gold from ore.
Scientific Applications
- Barometers and Thermometers: Utilizing mercury’s high density and thermal expansion properties.
- Spectrometry: Mercury-vapor lamps are used in spectroscopy for ultraviolet light sources.
Medical Uses
- Dental Amalgams: Mercury is used in amalgam materials for dental fillings.
- Preservatives and Medicinal Compounds: Thiomersal, a mercury-containing compound, is used as a preservative in vaccines.
Environmental and Health Concerns
- Toxicity: Mercury and its compounds are highly toxic, leading to restrictions on its use in many applications.
- Alternatives: Efforts are underway to find safer alternatives for many of mercury’s applications to reduce environmental and health risks.
Mercury’s unique physical and chemical properties make it a fascinating element with a range of applications, from industrial to scientific. Despite its versatility, the toxic nature of mercury and its compounds calls for cautious handling and responsible environmental management. Understanding mercury’s properties and preparation underscores its significance while highlighting the need for safety and sustainability in its use
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Practice Test
What is the atomic number of Mercury?
79
80
81
82
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At room temperature, Mercury is in which state of matter?
Solid
Liquid
Gas
Plasma
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What is the most common ore of Mercury?
Galena
Cinnabar
Sphalerite
Hematite
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Mercury forms amalgams with which type of elements?
Nonmetals
Metalloids
Metals
Noble gases
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Which of the following is a health concern associated with Mercury exposure?
Bone fracture
Muscle hypertrophy
Neurotoxicity
Hair loss
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Which of the following is a use of Mercury in the industrial sector?
Fertilizer production
Chlor-alkali process
Textile manufacturing
Cement production
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Which of the following compounds is used as a preservative in vaccines and contains Mercury?
Thimerosal
Formaldehyde
Ethanol
Benzalkonium chloride
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What is the boiling point of Mercury?
356.7°C
500°C
250°C
100°C
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Which type of Mercury is the most toxic to humans?
Elemental Mercury
Methylmercury
Mercurous chloride
Mercuric oxide
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