The early history of the isolation and work with fluorine and hydrogen fluoride is filled with accidents since both are extremely dangerous.
Eventually, electrolysis of a mixture of KF and HF carefully ensuring that the resulting hydrogen and fluorine would not come in contact in a platinum apparatus yielded the element. Fluorine was discovered in by Georgius Agricola. He originally found it in the compound Fluorspar, which was used to promote the fusion of metals.
It was under this application until , when Schwanhard discovered its usefulness in etching glass. Pure fluorine from the Latin fluere, for "flow" was was not isolated until by Henri Moissan, burning and even killing many scientists along the way. It has many uses today, a particular one being used in the Manhattan project to help create the first nuclear bomb.
Fluorine is the most electronegative element on the periodic table, which means that it is a very strong oxidizing agent and accepts other elements' electrons. Fluorine's atomic electron configuration is 1s 2 2s 2 2p 5. Fluorine is the most electronegative element because it has 5 electrons in it's 2P shell.
The optimal electron configuration of the 2P orbital contains 6 electrons, so since Fluorine is so close to ideal electron configuration, the electrons are held very tightly to the nucleus. The high electronegativity of fluorine explains its small radius because the positive protons have a very strong attraction to the negative electrons, holding them closer to the nucleus than the bigger and less electronegative elements. Because of its reactivity, elemental fluorine is never found in nature and no other chemical element can displace fluorine from its compounds.
Fluorine bonds with almost any element, both metals and nonmetals, because it is a very strong oxidizing agent. It is very unstable and reactive since it is so close to its ideal electron configuration. It forms covalent bonds with nonmetals, and since it is the most electronegative element, is always going to be the element that is reduced.
It will react explosively with many elements and compounds such as Hydrogen and water. This acid is very dangerous and when dissociated can cause severe damage to the body because while it may not be painful initially, it passes through tissues quickly and can cause deep burns that interfere with nerve function. There are also some organic compounds made of Fluorine, ranging from nontoxic to highly toxic.
Fluorine forms covalent bonds with Carbon, which sometimes form into stable aromatic rings. Bonds that fall in between the two extremes, having both ionic and covalent character, are classified as polar covalent bonds. Such bonds are thought of as consisting of partially charged positive and negative poles. Though ionic and covalent character represent points along a continuum, these designations are frequently useful in understanding and comparing the macroscopic properties of ionic and covalent compounds.
For example, ionic compounds typically have higher boiling and melting points, and they are also usually more soluble in water than covalent compounds.
Privacy Policy. Skip to main content. Basic Concepts of Chemical Bonding. Search for:. The Ionic Bond Ionic Bonding and Electron Transfer An ionic bond results from the transfer of an electron from a metal atom to a non-metal atom.
Learning Objectives Identify the key features of ionic bonds. Key Takeaways Key Points Ionic bonds are formed between cations and anions. A cation is formed when a metal ion loses a valence electron while an anion is formed when a non-metal gains a valence electron. They both achieve a more stable electronic configuration through this exchange. Ionic solids form crystalline lattices, or repeating patterns of atoms, with high melting points, and are typically soluble in water.
Key Terms electrolyte : An ionic compound which dissolves in H2O, making the resulting solution capable of conducting electricity. Lattice Energy Lattice energy is a measure of the bond strength in an ionic compound. Learning Objectives Describe lattice energy and the factors that affect it. Key Takeaways Key Points Lattice energy is defined as the energy required to separate a mole of an ionic solid into gaseous ions. Lattice energy cannot be measured empirically, but it can be calculated using electrostatics or estimated using the Born-Haber cycle.
Two main factors that contribute to the magnitude of the lattice energy are the charge and radius of the bonded ions. Key Terms exothermic reaction : A process which releases heat into its surroundings.
Formulas of Ionic Compounds Ionic formulas must satisfy the noble gas configurations for the constituent ions and the product compound must be electrically neutral. Learning Objectives Apply knowledge of ionic bonding to predict the formula of ionic compounds.
Key Takeaways Key Points The charge on the cations and anions in an ionic compound can be determined by the loss or gain of valence electrons necessary in order to achieve stable, noble gas electronic configurations.
The number of cations and anions that are combined in an ionic compound is the simplest ratio of whole integers that can be combined to reach electrical neutrality. The cation precedes the anion in both the written form and the formula. Key Terms noble gas : Any of the elements of group 18 of the periodic table, which are monatomic and, with very limited exceptions, inert, or non-reactive. Crystalline Lattice : Sodium chloride crystal lattice. Ionic vs Covalent Bond Character Ionic bonds can have some covalent character.
Learning Objectives Discuss the idea that, in nature, bonds exhibit characteristics of both ionic and covalent bonds. An ionic bond is based on attractive electrostatic forces between two ions of opposite charge. Ionic bonds involve a cation and an anion.
The bond is formed when an atom, typically a metal, loses an electron or electrons, and becomes a positive ion, or cation. Another atom, typically a non-metal, is able to acquire the electron s to become a negative ion, or anion.
One example of an ionic bond is the formation of sodium fluoride, NaF, from a sodium atom and a fluorine atom. In this reaction, the sodium atom loses its single valence electron to the fluorine atom, which has just enough space to accept it.
The ions produced are oppositely charged and are attracted to one another due to electrostatic forces. At the macroscopic scale, ionic compounds form lattices, are crystalline solids under normal conditions, and have high melting points. Most of these solids are soluble in H 2 O and conduct electricity when dissolved. The ability to conduct electricity in solution is why these substances are called electrolytes.
0コメント