PEEK

Miki Hori1, Kazuo Ohkuma2, Tatsushi Kawai1

  • 1Department of Dental Materials Science, Aichi Gakuin University School of Dentistry, Japan.

まとめ

新しい2部構成の粘着剤は,非共性π-π相互作用を利用して,ポリエーテルケトン (PEEK) と効果的に結合します. この新しいアプローチは,攻撃的な化学処理なしで,強固で信頼性の高い粘着性を提供し,歯科のアプリケーションを前進させます.

関連する概念動画

Types of Chemical Bonds02:37

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert N. Lewis. He developed a model called the Lewis model to explain the type and formation of different bonds. Chemical bonding is central to chemistry; it explains how atoms or ions bond together to form molecules. It explains why some bonds are strong and others are weak, or why one carbon bonds with two oxygens and not three; why water is H2O and not H4O. 
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Types of Chemical Bonds02:36

Types of Chemical Bonds

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Chemical Bonds02:40

Chemical Bonds


Atoms participate in a chemical bond formation to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest to it in atomic number. Ionic, covalent, and metallic bonds are some of the important types of chemical bonds. Bond energy and bond length determine the strength of a chemical bond.
Types of Chemical Bonds
An ionic bond is formed due to electrostatic attraction between cations and anions. Often, the ions are formed by the transfer of electrons...
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Introduction to Chemical Bonds01:01

Introduction to Chemical Bonds

Chemical Bonds
The electrons of the outermost energy level determine the energetic stability of the atom and its tendency to form chemical bonds with other atoms. The innermost electron shell has a maximum capacity of two electrons, but the next two electron shells can each have a maximum of eight electrons. This is known as the octet rule, which states that, with the exception of the innermost shell, atoms are most stable energetically when they have eight electrons in their valence shell, the...
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Bond Energies and Bond Lengths02:49

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, that is, the energy necessary to separate the bonded atoms. Separating any pair of bonded atoms requires energy — the stronger a bond, the greater the energy required to break it.
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Valence Bond Theory02:45

Valence Bond Theory

Overview of Valence Bond Theory
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