CHEM 51A Chapter 1.3: Electrons, Bonds, and Lewis Structures

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30 Sep 2016

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Bonds are the glue that hold atoms together. 1: the force of repulsion between the two negatively charged electrons. 2: the force of repulsion between the two positively charged nuclei. 3: the forces of attraction between the positively charged nuclei and the negatively charged electrons: as hydrogen atoms get closer to each other, all of these forces get stronger. A drawing structure of molecules in which the electrons take central state. The electrons in the outermost she"ll of an atom. Skill builder: drawing the lewis dot structure of an atom. Draw the lewis dot structure of (a) a boron atom and (b) a nitrogen atom. Place one valence e- by itself on each side of the atom. If the atom has more than 4 valence e-s, the remaining e-s are paired with the e-s already drawn. 1. 5 draw a lewis don"t structure for each of the following atoms:

Related Questions

A covalent chemical bond is one in which:

A. Outer shell electrons are shared by two atoms so as to satisfactorily fill the outer electron shells of both.

B. Outer shell electrons of one atom are transferred to the inner electron shells of another atom.

C. Protons or neutrons are shared by two atoms so as to satisfy the requirements of both.

D. Electrons are removed from one atom and transferred to another atom so that the two atoms become oppositely charged

brownantelope470

Match the following terms with their definitions:

chemical bonds

[ Choose ] a stable attraction between two or more atoms the bonds in a ion a representation of an atom's valence electrons shared valence electrons between atoms bonds between chemicals full electron transfer leading to charge-charge attraction an elemental symbol with some dots around it the sharing of all electrons between two atoms

covalent bonds

ionic bonds

Lewis structure

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.

CHEM 51A Chapter 1.3: Electrons, Bonds, and Lewis Structures

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