CM-UY 1004 Lecture Notes - Lecture 14: Covalent Bond, Valence Electron, Chemical Bond

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OC2021796

1 Nov 2017

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Document Summary

Chemical bond: attractive forces holding 2+ atoms together. Covalent bond: results from sharing electrons between nonmetals. Valence electrons: outermost electrons participating in chemical bonding. 2 similar atoms bond, none of them want to lose or gain an electron to form an. Covalency: number of bonds they tend to form. Decreases as more bonds are formed/more repulsive forces and maximize the attractive force electrons are shared. Electronegativity: ability of one atoms in a molecule to attract electrons to itself. Higher electronegativity you"re negative and the one with the lower electronegativity becomes positive. Polar covalent bond or polar bond: covalent bond with greater electron density around one of the 2 atoms. Bond polarity is based on highest electronegativity. Subtract the electronegativities from each other classify the bond. Writing lewis structures: electronegative element goes in center for each positive charge. Draw skeletal structure of compound with what atoms are bonded together. least.

Related Questions

1. True or False. a. A positively charged ion is called an anion. b. If an atom gives up an electron, it creates negatively charged ion. c. Valence electrons are the electrons that are available for bonding and located in the shells closest to the nucleus. d. An ionic bond is the result of electron sharing. e. When atoms gain, lose, or share electrons they do so in order to have an electron configuration of a noble gas. f. As you go across the periodic table left to right, electronegativity will increase. g. The number of valence electrons an atom has is equal to the atomic number. h. Fluorine cannot be the central atom due to the fact that is can only accept 2 electrons. i. When a covalent bond occurs, the atoms overlap one another to create a new orbital. The more overlapping, the stronger the bond. j. A triple bond is considered to be a weak bond.