Litio
•
0 likes•656 views
Lithium is a soft, silvery-white alkali metal with a melting point of 453.69 K and a boiling point of 1615 K. It is the lightest metal and least dense solid element. Lithium is highly reactive and flammable, so it is typically stored in mineral oil and corrodes quickly upon exposure to air. Due to its reactivity, lithium never occurs naturally in elemental form and is only found in ionic compounds.
Report
Share
Report
Share
Download to read offline
![3
Litio– Lithium
Mass: 6,941 u
[He]2s1
Melting point: 453,69 K
Boiling point: 1615 K
Density: 535 kg/m3
Discovery: Johan August (1817)
Under standard conditions it is the lightest metal and the least
dense solid element. Like all alkali metals, lithium is highly reactive and
flammable. For this reason, it is typically stored in mineral oil. When cut
open, lithium exhibits a metallicluster, but contact with moist
air corrodes the surface quickly to a dull silvery gray, then black tarnish.
Because of its high reactivity, lithium never occurs freely in nature, and
instead, only appears incompounds, which are usually ionic.](https://image.slidesharecdn.com/litio-130511140154-phpapp01/85/Litio-1-320.jpg)
Recommended
Oxidation Reduction Reactions
This document provides an overview of oxidation-reduction (redox) reactions including:
1. Defining oxidation as the loss of electrons and reduction as the gain of electrons.
2. Explaining that the reducing agent is oxidized and the oxidizing agent is reduced in redox reactions.
3. Detailing that the first step in understanding redox reactions is determining the oxidation number of each element in a compound.
1. group 0
The document discusses the properties and discovery of noble gases. It notes that:
- Noble gases (group 0) are very unreactive due to their full outer electron shells. This stability makes them similar across the group.
- Helium was first discovered on the sun in 1868. Argon was discovered in the 1890s after nitrogen from air was found to contain a small quantity of an inert element.
- Ramsay realized argon needed its own group and later discovered it contained traces of other noble gases - neon, krypton, and xenon. Radon was discovered in 1900.
chem Lab 5
Magnesium reacted immediately with hydrochloric acid, bubbling rapidly until fully dissolved. Zinc reacted more slowly with bubbling. Aluminum reacted slowly only with the stronger acid. Copper did not react at all. This is because magnesium, zinc and aluminum are more reactive than hydrogen in the acid, replacing it to form magnesium chloride, hydrogen gas and electrons in a single replacement reaction. Copper is less reactive than hydrogen and did not replace it.
Alkaline and alkaline earth metals
This document discusses the alkali and alkaline earth metals. It describes their location on the periodic table and their similar reactive properties. The alkali metals include lithium, sodium, potassium, rubidium, cesium, and francium. They are soft, reactive metals that are good conductors. The alkaline earth metals include beryllium, magnesium, calcium, strontium, barium, and radium. They have an oxidation state of +2 and are also very reactive. Both groups of metals are described in more detail with their discoveries, properties, and common uses. Melting and boiling points are also provided for each element.
Alkaline and Alkaline Earth Metals
This document discusses the alkali and alkaline earth metals. It provides information on their properties and classification in the periodic table. The alkali metals are soft, reactive, and have one outer electron. They include lithium, sodium, potassium, rubidium, cesium, and francium. The alkaline earth metals have a +2 oxidation state and include beryllium, magnesium, calcium, strontium, barium, and radium. Each metal is then described individually, noting their discovery, physical properties, and common uses. Melting and boiling points are also listed for comparison.
C3g Transition Elements
This document discusses properties and reactions of transition metals. It notes that transition metals are metals that conduct heat and electricity well and have high melting points. They often form colored compounds, like blue copper compounds and green iron(II) compounds. Transition metals also often act as catalysts in important reactions. The document then discusses how transition metal carbonates undergo thermal decomposition, releasing carbon dioxide. Specific reactions of iron, copper, manganese, and zinc carbonates decomposing this way are listed. Finally, the document explains how precipitation reactions with sodium hydroxide can be used to identify copper, iron(II), and iron(III) ions based on the color of precipitate formed.
4.3 (a) group 1
Alkali metals are elements found in Group 1 of the periodic table, including lithium, sodium, potassium, rubidium, cesium, and francium. They have low melting and boiling points, are soft, and become liquid or gas at room temperature as you move down the group. Their density increases as atomic mass increases more than atomic radius.
Transition Elements
The document summarizes key concepts about transition elements including:
1. Transition elements are defined as elements that can form at least one stable ion with a partially filled d subshell. Common errors in defining transition elements are also discussed.
2. The electronic configurations of transition elements and their ions are covered, noting exceptions like Cr and Cu.
3. Physical properties of transition elements discussed include atomic/ionic radii, ionization energy, melting points and how they vary within the period and group.
Recommended
Oxidation Reduction Reactions
This document provides an overview of oxidation-reduction (redox) reactions including:
1. Defining oxidation as the loss of electrons and reduction as the gain of electrons.
2. Explaining that the reducing agent is oxidized and the oxidizing agent is reduced in redox reactions.
3. Detailing that the first step in understanding redox reactions is determining the oxidation number of each element in a compound.
1. group 0
The document discusses the properties and discovery of noble gases. It notes that:
- Noble gases (group 0) are very unreactive due to their full outer electron shells. This stability makes them similar across the group.
- Helium was first discovered on the sun in 1868. Argon was discovered in the 1890s after nitrogen from air was found to contain a small quantity of an inert element.
- Ramsay realized argon needed its own group and later discovered it contained traces of other noble gases - neon, krypton, and xenon. Radon was discovered in 1900.
chem Lab 5
Magnesium reacted immediately with hydrochloric acid, bubbling rapidly until fully dissolved. Zinc reacted more slowly with bubbling. Aluminum reacted slowly only with the stronger acid. Copper did not react at all. This is because magnesium, zinc and aluminum are more reactive than hydrogen in the acid, replacing it to form magnesium chloride, hydrogen gas and electrons in a single replacement reaction. Copper is less reactive than hydrogen and did not replace it.
Alkaline and alkaline earth metals
This document discusses the alkali and alkaline earth metals. It describes their location on the periodic table and their similar reactive properties. The alkali metals include lithium, sodium, potassium, rubidium, cesium, and francium. They are soft, reactive metals that are good conductors. The alkaline earth metals include beryllium, magnesium, calcium, strontium, barium, and radium. They have an oxidation state of +2 and are also very reactive. Both groups of metals are described in more detail with their discoveries, properties, and common uses. Melting and boiling points are also provided for each element.
Alkaline and Alkaline Earth Metals
This document discusses the alkali and alkaline earth metals. It provides information on their properties and classification in the periodic table. The alkali metals are soft, reactive, and have one outer electron. They include lithium, sodium, potassium, rubidium, cesium, and francium. The alkaline earth metals have a +2 oxidation state and include beryllium, magnesium, calcium, strontium, barium, and radium. Each metal is then described individually, noting their discovery, physical properties, and common uses. Melting and boiling points are also listed for comparison.
C3g Transition Elements
This document discusses properties and reactions of transition metals. It notes that transition metals are metals that conduct heat and electricity well and have high melting points. They often form colored compounds, like blue copper compounds and green iron(II) compounds. Transition metals also often act as catalysts in important reactions. The document then discusses how transition metal carbonates undergo thermal decomposition, releasing carbon dioxide. Specific reactions of iron, copper, manganese, and zinc carbonates decomposing this way are listed. Finally, the document explains how precipitation reactions with sodium hydroxide can be used to identify copper, iron(II), and iron(III) ions based on the color of precipitate formed.
4.3 (a) group 1
Alkali metals are elements found in Group 1 of the periodic table, including lithium, sodium, potassium, rubidium, cesium, and francium. They have low melting and boiling points, are soft, and become liquid or gas at room temperature as you move down the group. Their density increases as atomic mass increases more than atomic radius.
Transition Elements
The document summarizes key concepts about transition elements including:
1. Transition elements are defined as elements that can form at least one stable ion with a partially filled d subshell. Common errors in defining transition elements are also discussed.
2. The electronic configurations of transition elements and their ions are covered, noting exceptions like Cr and Cu.
3. Physical properties of transition elements discussed include atomic/ionic radii, ionization energy, melting points and how they vary within the period and group.
Nomenclature handout
This document discusses the nomenclature (naming systems) for inorganic compounds, which differ depending on whether the compound is ionic or molecular. For ionic compounds, the cation is named first followed by the anion. Binary ionic compounds consisting of a metal and nonmetal are generally named by removing the ending from the nonmetal and adding -ide. For transition metals that form multiple ions, the modern system uses Roman numerals in parentheses after the metal to indicate charge. Molecular compounds are named by identifying the number of atoms of each element present using prefixes, and adding -ide to the second element. Several elements exist as diatomic molecules like H2, N2, O2, F2, Cl2, Br
Organometallic chemistry
This document provides an introduction to organometallic compounds. It defines organometallic compounds as those containing at least one metal-carbon bond. It discusses some of the main applications of organometallics in industries like pharmaceuticals and semiconductors. The document then covers various topics related to organometallics including their classification, nomenclature, preparation methods like metathesis and transmetallation reactions, and examples of important organometallic compounds like alkylaluminums.
Lanthanide and actinide chemistry
Lanthanide and Actinide Chemistry by Dr. Susovan Bhowmik,
Assistant Prof. Bankura Sammilani College, West Bengal
Chemical Families Notes
The document discusses various chemical groups and families, including their properties and common uses. It covers the alkali metals, alkaline earth metals, transition metals, inner transition metals (lanthanides and actinides), and other nonmetal groups such as carbon, nitrogen, oxygen, halogens, noble gases, and hydrogen. For each group, it highlights some of the most abundant elements, their physical and chemical characteristics, and important commercial applications.
Chapter 8 redox reactions ppt for class 11 CBSE
This document discusses oxidation-reduction (redox) reactions and oxidation states. It defines oxidation as the loss of electrons and reduction as the gain of electrons. Redox reactions involve the transfer of electrons from one atom to another. Oxidation numbers are used to track electron transfers and determine if a substance is being oxidized or reduced in a reaction. Common oxidation states of elements are discussed. Rules are provided for determining oxidation numbers based on electronegativity differences in molecules and ions.
Periodic table of elements
Argon is the third most common gas in the atmosphere. It is a colorless, odorless noble gas with the chemical symbol Ar. Argon has 18 protons, 18 electrons, and is found in Group 18 of the periodic table. It is non-reactive due to its full outer electron shell, but can form some compounds. Argon has several industrial uses including in lighting and welding.
Transition Metal Carbonyl Compounds
Transition metal carbonyls form when carbon monoxide bonds to a transition metal through both sigma and pi bonding. This synergistic metal-ligand bonding strengthens the metal-carbon bond. Metal carbonyls can be classified based on the ligands present and the number/structure of metal atoms. They exhibit a variety of reactions including substitution, reactions with halogens, and disproportionation. Metal carbonyls display properties related to their toxicity, magnetic behavior, thermal stability, and thermodynamic instability.
Oxidation reduction reaction
The document discusses various types of chemical reactions including oxidation-reduction, thermal dissociation, corrosion, and rancidity. It provides examples of oxidation-reduction reactions and explains that they involve the loss or gain of oxygen or hydrogen. Thermal dissociation reactions are described as reactions where compounds split into simpler substances when heated. Corrosion and rancidity are discussed as oxidation processes that damage iron structures and cause fats and oils to smell foul, respectively.
Dinitrogen complexes
Dinitrogen complexes are coordination compounds containing the N2 molecule as a ligand. There are several possible modes of bonding between dinitrogen and metals, including terminal ("end-on") bonding, lateral ("side-on") bonding, and bridge bonding via one or both nitrogen atoms. Only terminal, terminal bridge, and structures with two metal atoms on each nitrogen atom have been conclusively demonstrated. The first dinitrogen complex was discovered in 1965 and contained a stable [(NH3)5RuN2] structure.
coordination compounds
The document discusses coordination compounds and their classification. It begins by introducing coordination compounds and providing examples like chlorophyll and hemoglobin. It then summarizes Werner's theory of coordination compounds from 1898, which proposed that metals form primary ionic bonds and secondary non-ionic bonds of fixed coordination number with ligands in coordination spheres. The document defines key terms like ligands, coordination number, and isomers. It also describes common coordination polyhedra and provides rules for naming coordination compounds.
C6b Redox Reactions
Rusting is an example of a redox reaction where:
1. Iron loses electrons and is oxidized.
2. Oxygen gains electrons and is reduced.
3. For rusting to occur, iron needs to be in contact with both oxygen and water, and acids or salts can catalyze the reaction.
solids, liquids and gases
The document provides information about the states of matter - solids, liquids, and gases. It explains that all substances are made up of particles and the key difference between the three states is how strongly the particles are attracted to each other and how much they move. Solids have particles that are strongly attracted and do not move around much. Liquids have particles that are less strongly attracted and can move past each other. Gases have particles that move freely and are rarely touching. The document also discusses diffusion, which is the spreading out of particles, and provides examples of how smells diffuse through the air or liquids.
Oxidation reduction reactions
The document discusses oxidation-reduction (redox) reactions. It defines oxidation as the loss of electrons and reduction as the gain of electrons. Redox reactions always involve both an oxidation and a reduction process. The substance undergoing oxidation is the reducing agent as it loses electrons, while the substance undergoing reduction is the oxidizing agent as it gains electrons. Assigning oxidation numbers to atoms allows identification of which substances are oxidized and reduced in a reaction.
Names and formulas of ionic compounds
This document discusses writing formulas for ionic compounds and naming ionic compounds and oxyanions. It provides rules for determining the formula unit of ionic compounds based on the ratio of ions present. Cation symbols are always written first, followed by anion symbols. Subscripts indicate the number of each ion. Polyatomic ions act as individual units in formulas. Oxyanions contain nonmetals bonded to oxygen. Five rules are provided for naming ionic compounds based on cation and anion names and oxidation states.
Chemistry of Alkali Metals MANIK
Chemistry of alkali and alkaline earth metals and halogen compounds including their
Pharmaceutical applications.
oxidising and reducing agent
this is about the topic of chemistry the oxidising and reducing agent it tell about the defination of the oxidation as wellas oxidising agent.
rules in naming organic compound
This document provides rules for naming inorganic compounds, including binary molecular compounds, ionic compounds, oxyanions, and acids. It explains that Greek prefixes are used to indicate the number of elements in binary compounds, with the more electronegative element written last with an -ide ending. For ionic compounds, the cation name comes first followed by the anion name with -ide ending. Oxyanion names follow patterns with -ate, -ite, per-, and hypo- prefixes indicating oxygen content. Acid names are derived from the related anion name by changing endings to -ic or -ous according to specific rules outlined in the document.
C04 elements and compounds
The document is a chapter about elements and compounds from a chemistry textbook. It contains the following key points in 3 sentences:
The chapter defines elements as substances that cannot be broken down further, while compounds are substances made of two or more elements chemically bonded together. It explains that elements are represented by chemical symbols and compounds by chemical formulas showing the ratios of atoms present. The chapter also discusses writing and balancing chemical equations to represent chemical reactions in terms of reactants and products.
Reactions & Formulas
This is an example of a combustion reaction. Propane (C3H8) is burning in oxygen gas (O2), producing carbon dioxide (CO2) and water vapor (H2O) as products. The balanced chemical equation is:
C3H8 + 5O2 → 3CO2 + 4H2O
Holmio.carlos ruiz rubio 3 b
Holmium is a silvery-white metal that is too reactive to be found uncombined in nature. It has a melting point of 1734 K and a boiling point of 2993 K. Holmium was discovered in 1878 by Delafontaine and Soret.
Bario jose angel guillen romero 3ºb
Barium is a soft, silvery-white metal that was discovered in 1772. It has a medium density and good electrical conductivity. While ultrapure barium is difficult to prepare, barium and barium alloys are commonly used to remove unwanted gases from vacuum tubes.
Aluminio
Aluminum is a metal with a low density and ability to resist corrosion through passivation. It is vital to the aerospace industry due to its use in lightweight structural components made from aluminum and its alloys. The most widely used aluminum compounds are oxides and sulfates.
More Related Content
What's hot
Nomenclature handout
This document discusses the nomenclature (naming systems) for inorganic compounds, which differ depending on whether the compound is ionic or molecular. For ionic compounds, the cation is named first followed by the anion. Binary ionic compounds consisting of a metal and nonmetal are generally named by removing the ending from the nonmetal and adding -ide. For transition metals that form multiple ions, the modern system uses Roman numerals in parentheses after the metal to indicate charge. Molecular compounds are named by identifying the number of atoms of each element present using prefixes, and adding -ide to the second element. Several elements exist as diatomic molecules like H2, N2, O2, F2, Cl2, Br
Organometallic chemistry
This document provides an introduction to organometallic compounds. It defines organometallic compounds as those containing at least one metal-carbon bond. It discusses some of the main applications of organometallics in industries like pharmaceuticals and semiconductors. The document then covers various topics related to organometallics including their classification, nomenclature, preparation methods like metathesis and transmetallation reactions, and examples of important organometallic compounds like alkylaluminums.
Lanthanide and actinide chemistry
Lanthanide and Actinide Chemistry by Dr. Susovan Bhowmik,
Assistant Prof. Bankura Sammilani College, West Bengal
Chemical Families Notes
The document discusses various chemical groups and families, including their properties and common uses. It covers the alkali metals, alkaline earth metals, transition metals, inner transition metals (lanthanides and actinides), and other nonmetal groups such as carbon, nitrogen, oxygen, halogens, noble gases, and hydrogen. For each group, it highlights some of the most abundant elements, their physical and chemical characteristics, and important commercial applications.
Chapter 8 redox reactions ppt for class 11 CBSE
This document discusses oxidation-reduction (redox) reactions and oxidation states. It defines oxidation as the loss of electrons and reduction as the gain of electrons. Redox reactions involve the transfer of electrons from one atom to another. Oxidation numbers are used to track electron transfers and determine if a substance is being oxidized or reduced in a reaction. Common oxidation states of elements are discussed. Rules are provided for determining oxidation numbers based on electronegativity differences in molecules and ions.
Periodic table of elements
Argon is the third most common gas in the atmosphere. It is a colorless, odorless noble gas with the chemical symbol Ar. Argon has 18 protons, 18 electrons, and is found in Group 18 of the periodic table. It is non-reactive due to its full outer electron shell, but can form some compounds. Argon has several industrial uses including in lighting and welding.
Transition Metal Carbonyl Compounds
Transition metal carbonyls form when carbon monoxide bonds to a transition metal through both sigma and pi bonding. This synergistic metal-ligand bonding strengthens the metal-carbon bond. Metal carbonyls can be classified based on the ligands present and the number/structure of metal atoms. They exhibit a variety of reactions including substitution, reactions with halogens, and disproportionation. Metal carbonyls display properties related to their toxicity, magnetic behavior, thermal stability, and thermodynamic instability.
Oxidation reduction reaction
The document discusses various types of chemical reactions including oxidation-reduction, thermal dissociation, corrosion, and rancidity. It provides examples of oxidation-reduction reactions and explains that they involve the loss or gain of oxygen or hydrogen. Thermal dissociation reactions are described as reactions where compounds split into simpler substances when heated. Corrosion and rancidity are discussed as oxidation processes that damage iron structures and cause fats and oils to smell foul, respectively.
Dinitrogen complexes
Dinitrogen complexes are coordination compounds containing the N2 molecule as a ligand. There are several possible modes of bonding between dinitrogen and metals, including terminal ("end-on") bonding, lateral ("side-on") bonding, and bridge bonding via one or both nitrogen atoms. Only terminal, terminal bridge, and structures with two metal atoms on each nitrogen atom have been conclusively demonstrated. The first dinitrogen complex was discovered in 1965 and contained a stable [(NH3)5RuN2] structure.
coordination compounds
The document discusses coordination compounds and their classification. It begins by introducing coordination compounds and providing examples like chlorophyll and hemoglobin. It then summarizes Werner's theory of coordination compounds from 1898, which proposed that metals form primary ionic bonds and secondary non-ionic bonds of fixed coordination number with ligands in coordination spheres. The document defines key terms like ligands, coordination number, and isomers. It also describes common coordination polyhedra and provides rules for naming coordination compounds.
C6b Redox Reactions
Rusting is an example of a redox reaction where:
1. Iron loses electrons and is oxidized.
2. Oxygen gains electrons and is reduced.
3. For rusting to occur, iron needs to be in contact with both oxygen and water, and acids or salts can catalyze the reaction.
solids, liquids and gases
The document provides information about the states of matter - solids, liquids, and gases. It explains that all substances are made up of particles and the key difference between the three states is how strongly the particles are attracted to each other and how much they move. Solids have particles that are strongly attracted and do not move around much. Liquids have particles that are less strongly attracted and can move past each other. Gases have particles that move freely and are rarely touching. The document also discusses diffusion, which is the spreading out of particles, and provides examples of how smells diffuse through the air or liquids.
Oxidation reduction reactions
The document discusses oxidation-reduction (redox) reactions. It defines oxidation as the loss of electrons and reduction as the gain of electrons. Redox reactions always involve both an oxidation and a reduction process. The substance undergoing oxidation is the reducing agent as it loses electrons, while the substance undergoing reduction is the oxidizing agent as it gains electrons. Assigning oxidation numbers to atoms allows identification of which substances are oxidized and reduced in a reaction.
Names and formulas of ionic compounds
This document discusses writing formulas for ionic compounds and naming ionic compounds and oxyanions. It provides rules for determining the formula unit of ionic compounds based on the ratio of ions present. Cation symbols are always written first, followed by anion symbols. Subscripts indicate the number of each ion. Polyatomic ions act as individual units in formulas. Oxyanions contain nonmetals bonded to oxygen. Five rules are provided for naming ionic compounds based on cation and anion names and oxidation states.
Chemistry of Alkali Metals MANIK
Chemistry of alkali and alkaline earth metals and halogen compounds including their
Pharmaceutical applications.
oxidising and reducing agent
this is about the topic of chemistry the oxidising and reducing agent it tell about the defination of the oxidation as wellas oxidising agent.
rules in naming organic compound
This document provides rules for naming inorganic compounds, including binary molecular compounds, ionic compounds, oxyanions, and acids. It explains that Greek prefixes are used to indicate the number of elements in binary compounds, with the more electronegative element written last with an -ide ending. For ionic compounds, the cation name comes first followed by the anion name with -ide ending. Oxyanion names follow patterns with -ate, -ite, per-, and hypo- prefixes indicating oxygen content. Acid names are derived from the related anion name by changing endings to -ic or -ous according to specific rules outlined in the document.
C04 elements and compounds
The document is a chapter about elements and compounds from a chemistry textbook. It contains the following key points in 3 sentences:
The chapter defines elements as substances that cannot be broken down further, while compounds are substances made of two or more elements chemically bonded together. It explains that elements are represented by chemical symbols and compounds by chemical formulas showing the ratios of atoms present. The chapter also discusses writing and balancing chemical equations to represent chemical reactions in terms of reactants and products.
Reactions & Formulas
This is an example of a combustion reaction. Propane (C3H8) is burning in oxygen gas (O2), producing carbon dioxide (CO2) and water vapor (H2O) as products. The balanced chemical equation is:
C3H8 + 5O2 → 3CO2 + 4H2O
What's hot (19)
Viewers also liked
Holmio.carlos ruiz rubio 3 b
Holmium is a silvery-white metal that is too reactive to be found uncombined in nature. It has a melting point of 1734 K and a boiling point of 2993 K. Holmium was discovered in 1878 by Delafontaine and Soret.
Bario jose angel guillen romero 3ºb
Barium is a soft, silvery-white metal that was discovered in 1772. It has a medium density and good electrical conductivity. While ultrapure barium is difficult to prepare, barium and barium alloys are commonly used to remove unwanted gases from vacuum tubes.
Aluminio
Aluminum is a metal with a low density and ability to resist corrosion through passivation. It is vital to the aerospace industry due to its use in lightweight structural components made from aluminum and its alloys. The most widely used aluminum compounds are oxides and sulfates.
Plutonio javier rodriguez moscatel
Plutonium is a radioactive transuranic element with an atomic number of 94. It is an actinide metal that has a silver-gray appearance which darkens when exposed to air. Plutonium exhibits six allotropic states and four oxidation states, and reacts with carbon, halogens, nitrogen and silicon.
Mercurio
Mercury is a heavy, silvery metal that is liquid at room temperature. It has a high density and is a good conductor of electricity, though not a strong conductor of heat. Mercury easily forms alloys with other metals like gold and silver but not iron. While insoluble in water, it is soluble in nitric acid. Exposure through inhalation, ingestion, or contact can be harmful as mercury irritates skin, eyes, and respiratory tract.
Neón javier rodriguez moscatel
Neon is a noble gas with an atomic mass of 20.18. It was discovered in 1898 by William Ramsay and Morris Travers. Neon has a melting point of -248.6°C and a boiling point of -246°C. It has a density of 0.89994 kg/m3 and is lighter than helium with a cooling power per unit volume 40 times higher than liquid helium and 3 times greater than liquid hydrogen, making it cheaper than helium for most applications using liquid gases.
Neodimio
Neodymium is a rare earth metal with a melting point of 1297 K and boiling point of 3347 K. It has a density of 7.01 g/cm3 and is found in significant quantities in the minerals monazite and bastnasite, though not naturally in metallic form. Neodymium compounds are often a reddish-purple color due to the Nd3+ ion.
Ununoctio javier rodriguez moscatel
Ununoctium (Uuo) is a synthetic element with atomic number 118, atomic mass of 244.06, and chemical symbol Uuo. It is predicted to be a solid with a boiling point of 320°C and density of 13.65 kg/m3. Robert Smola czukń is credited with discovering the element through experiments conducted at the Joint Institute for Nuclear Research.
Samario
Samarium is a silvery metal that readily oxidizes in air. It is a lanthanide element with an atomic mass of 150.36 u that typically assumes an oxidation state of +3. Samarium has no significant biological role, is only slightly toxic, and its compounds are commonly used as reducing agents in chemical synthesis.
Curio.carlos ruiz rubio 3 b
Curium is a radioactive chemical element with the symbol Cm and atomic number 96. It is produced by bombarding uranium or plutonium with neutrons in nuclear reactors, with one tonne of spent nuclear fuel containing about 20 grams of curium. Curium is a hard, dense, silvery metal that has a relatively high melting point and boiling point for an actinide element.
Francio
Francium is a highly radioactive alkali metal that was discovered in 1939 and is the second least abundant element in nature. It has only one electron in its valence shell like other alkali metals and decays into astatine, radium, and radon. Francium has a melting point of 300K and boiling point of 950K with a density of 1870 kg/m3, but there are no commercial applications due to its scarcity and instability, being only used for research in biology and atomic structure.
Osmio
Osmium is a hard, bluish-white transition metal that is the densest naturally occurring element with a density of 22.59 g/cm3. It melts at 3306 K and boils at 5285 K. Osmium is typically found in nature as an alloy in platinum ores and its alloys with other platinum group metals are used for applications requiring extreme hardness and durability like fountain pen tips and electrical contacts.
Magnesio
Magnesium is the fourth most common element in the Earth, making up 13% of the planet's mass and a large fraction of the mantle. It has an atomic mass of 24.3247u, a melting point of 923K, and a boiling point of 1363K. Magnesium has a common oxidation state of +2, is an alkaline earth metal, and the third most abundant dissolved element in seawater due to its high solubility.
Cromo javier rodriguez moscatel
Chromium is a chemical element with an atomic number of 24 that was discovered by Johann Gottlob Lehmann. It is a transition metal that is hard, brittle, and gray in color. Chromium has a high resistance to corrosion.
Darmstadtium
Darmstadtium is a synthetic element with an atomic mass of 281. It is predicted to behave as the heavier homologue to platinum based on its position in the periodic table as a member of group 10, although no chemical experiments have confirmed this. Darmstadtium was first synthesized in 1994 at the Gesellschaft fur Schwerionenforschung and is calculated to have similar properties to nickel, palladium, and platinum due to its position in the d-block.
Teluro
Tellurium is a brittle, silver-white metalloid that was discovered in 1782 in Transylvania. It is chemically related to selenium and sulfur. Tellurium has a density of 6.24 g/cm3, melts at 722.66 K and boils at 1261 K. The primary use of tellurium is in alloys to improve machinability, especially in steel and copper alloys.
Erbio
Erbium is a rare earth metal that was discovered in 1842 by Carl Gustaf Mosander. It has a melting point of 1802 K and a boiling point of 3141 K. Erbium is malleable and soft yet stable in air, though it does not oxidize as quickly as some other rare earth metals. Its salts are rose-colored and it has characteristic absorption spectra bands in visible light, ultraviolet, and near infrared.
Niquel
Nickel is a silvery-white lustrous metal that belongs to the transition metals. It has a melting point of 1728 K and a boiling point of 3186 K. Nickel is hard and ductile but develops a protective oxide surface that slows its reaction with air, though it can be powdered to increase chemical activity through higher exposed surface area.
Viewers also liked (20)
More from jvprofe
Isaac newton
Isaac Newton was an English scientist born in 1643 who made fundamental contributions to physics, mathematics, and optics. He developed the laws of motion and universal gravitation, which dominated the scientific view of the physical universe for the next three centuries. Newton also invented calculus and made advances in optics, compiling a set of principles of reflection, refraction, and color. Newton served as a member of Parliament and published his seminal work Philosophiae Naturalis Principia Mathematica, establishing classical mechanics.
Satélites Geoestacionario
Los satélites geoestacionarios orbitan la Tierra a una altura de aproximadamente 35,930 km, lo que les permite dar una vuelta completa cada 24 horas y permanecer fijos sobre un punto de la superficie terrestre. El documento calcula esta altura aplicando la segunda ley de Newton y la fórmula para la velocidad orbital, sustituyendo los valores conocidos de la masa de la Tierra, su radio y el periodo orbital de 24 horas.
La luz segundo eso
La luz es energía que se propaga en forma de ondas electromagnéticas y puede viajar a través del vacío. Se propaga en línea recta a una velocidad de 300,000 km/s. Las fuentes de luz incluyen cuerpos calientes, reacciones químicas y estrellas. La luz blanca está compuesta por la mezcla de colores del arco iris y los objetos reflejan o absorben diferentes colores, determinando su apariencia.
Chemical reaction activities
This document contains a series of chemistry activities and problems for students involving chemical reactions and stoichiometry. The activities explore the differences between physical and chemical changes, conservation of mass, moles, molecules, atoms and balanced chemical equations. Students are tasked with identifying reaction types, balancing equations, calculating moles, masses and volumes of substances involved in various chemical reactions. Key concepts covered include the mole concept, the law of conservation of mass, the law of definite proportions, and stoichiometric calculations.
Lista segundo bac
O documento lista as notas finais de vários alunos no exame final de Física 2o Bachillerato. A maioria dos alunos teve notas entre 3 e 9, com alguns reprovados ou que precisam fazer todo o exame novamente. Dois alunos se saíram particularmente bem com notas acima de 8.
Examen fisica moderna soluciones
Este documento presenta las soluciones a varios problemas de física relacionados con la física nuclear y la relatividad. En la primera sección se calcula el trabajo de extracción y la longitud de onda umbral para la emisión de electrones de potasio iluminado con luz amarilla de sodio. La segunda sección calcula la constante de desintegración, el número de núcleos y la actividad de una muestra radioactiva inicial y después de un año. La tercera sección calcula el tiempo dilatado y la distancia recorrida por una nave
Estaño javier rodriguez moscatel
Tin is a chemical element with symbol Sn and atomic number 50. It has two possible oxidation states of +2 and the more stable +4. Tin is the 49th most abundant element and has 10 stable isotopes, more than any other element on the periodic table. It was discovered in 1854 by Julius Pelegrin and has a melting point of 231.9°C and a boiling point of 2,603°C.
Seaborgio
Element 106, seaborgium, has an electron configuration of [Rn] 5f14 6d4 7s2 and a predicted density of 35 g·cm−3. It was first synthesized in 1974 by bombarding a target of californium-249 with oxygen-18 ions, producing seaborgium-263 which decays by alpha emission with a half-life of 0.9 seconds, with its discovery reported by scientists at the Joint Institute for Nuclear Research in Dubna, USSR and the Lawrence Berkeley Laboratory.
Gadolinio
Gadolinium is a silvery-white, malleable and ductile rare-earth metal with a melting point of 1585 K and boiling point of 3546 K. It has an electron configuration of [Xe] 4f7 5d1 6s2 and density of 7.90 g·cm−3. Gadolinium was first detected spectroscopically in 1880 by de Marignac and was isolated in 1886, making it one of the last rare-earth elements to be discovered.
Titatnium
Titanium is a transition metal with the symbol Ti that has a low density and silver color. It has a melting point of 1941 K and boiling point of 3560 K. Titanium is found in many minerals deposits like rutile and ilmenite that are widely distributed in the Earth's crust and lithosphere, and it is also found in living things, rocks, water, and soil.
Disprosio
Dysprosium is a rare earth element with a metallic, bright silver luster. It is soft enough to be cut with a knife and can be machined without sparking if overheating is avoided. Dysprosium's physical characteristics can be greatly affected even by small amounts of impurities.
Bromo
Bromine is a red-brown, corrosive and toxic liquid that was isolated in 1825-1826 by two chemists. It has properties between chlorine and iodine and is part of the halogen group with an atomic number of 35. While rare in the Earth's crust, bromine accumulates in oceans and is commercially extracted from brine pools, with over 556,000 tonnes produced globally in 2007.
Fermio
Fermium is an artificial radioactive element discovered in 1952 through nuclear transmutation of lighter elements. It has no stable isotopes and the longest lived isotope, fermium-257, has a half-life of around 100 days. Fermium-258 has an extremely short half-life of 0.38 milliseconds, suggesting an instability in elements around this mass number in the periodic table.
Cerio
Cerium is a silvery-white metallic element with an atomic mass of 140.116 u that is part of the lanthanide series of elements following lanthanum in the periodic table. It was discovered in 1803 and has a melting point of 1071 K and boiling point of 3699K, with a density of 6689 kg/m3. Some derivatives of cerium are used in fireworks, as a ceramic material in iron alloys for firestones, and cerium oxide is used for polishing lenses and in permanent magnet alloys, though cerium has a moderate level of toxicity and will ignite spontaneously when exposed to air between 65-80 degrees C.
Azufre
Sulfur is a chemical element with the symbol S and atomic number 16. It has a melting point of 388.36K and boiling point of 717.87K. Sulfur is found in native form in volcanic regions and forms sulfides and sulfates, and is necessary for protein synthesis in living organisms. It is mainly used as a fertilizer but also in the manufacture of gunpowder, laxatives, matches, and insecticides.
Astato
Astatine is a radioactive chemical element that occurs on Earth only through the radioactive decay of heavier elements. It has no stable isotopes, with astatine-210 being the most stable isotope. Observed properties of astatine are consistent with it being a heavier analog of the element iodine.
Transferencia de electrones quimica
El documento trata sobre reacciones redox y procesos electroquímicos. Explica la corrosión del hierro y técnicas para paliarla como el pasivado y recubrimientos. También describe tipos de pilas como la leclanché, de botón y recargables, mencionando sus componentes. Por último, detalla procesos metalúrgicos e industriales como la electrolisis del NaCl y Al2O3 para obtener cloro y aluminio.
Transferencia de electrones quimica
El documento describe diferentes procesos redox de importancia industrial y tecnológica, incluyendo la corrosión del hierro, técnicas para prevenirla como el pasivado y recubrimientos, pilas como la leclanché y alcalinas, procesos electrolíticos para obtener metales como el aluminio y sodio, y recubrimientos por electrodeposición como la galvanostegia y galvanoplastia.
More from jvprofe (18)
Litio
- 1. 3 Litio– Lithium Mass: 6,941 u [He]2s1 Melting point: 453,69 K Boiling point: 1615 K Density: 535 kg/m3 Discovery: Johan August (1817) Under standard conditions it is the lightest metal and the least dense solid element. Like all alkali metals, lithium is highly reactive and flammable. For this reason, it is typically stored in mineral oil. When cut open, lithium exhibits a metallicluster, but contact with moist air corrodes the surface quickly to a dull silvery gray, then black tarnish. Because of its high reactivity, lithium never occurs freely in nature, and instead, only appears incompounds, which are usually ionic.