Chemical Bonding Notes
by Owen Borville
October 11-18, 2022
Chemistry
Terms for Chemical Bonds
Electrostatic Force=between electric charges of atoms’ nucleus and electrons
Polyatomic ion=filled valence electrons instead of sharing electrons
Formula unit=ratio of cations (+) to anions(-) needed to achieve neutrality and determine chemical formula
Crystal lattice=is an orderly 3-dimensional arrangement of atoms
Electron sea theory=is a sea of mobile electrons in metallic bond
Network covalent substance=is a covalent bond in continuous three dimensional network=e.g.=diamond
Chemical Bond= share or transfer of electrons among chemical elements and compounds. Chemical Bond=when atoms link or attach to each other to maximize stability =chemical bond=energy is usually released as a result
Atoms form chemical bonds in order to= become stable in the lowest energy state in their valence electron shells.
Octet Rule= atoms maximize stability when they have a full valence energy level, usually with 8 valence electrons in the outer energy level. Atoms will transfer, accept, or share electrons necessary to complete the outer valence shell of 8 electrons. Atoms can complete the octet rule by sharing or transferring electrons.
Covalent bonding=electrons are shared to produce the bond. Covalent bonding involves nonmetal ions tightly shared. Covalent compounds tend to be gasses, liquids, soft solids, and poor conductors of electricity. These are the properties of nonmetallic substances.
Ionic bonding=one atom loses an electron and another atom gains an electron by transferring; atoms in an ionic bond are held together by the opposite charges (+,-) Ionic bonding involves metallic and nonmetallic ions. Ionic compounds form solid crystalline substances and lattices. High melting points, good insulators.
Metallic bonding=is an electron sea of freely moving electrons shared by all metal atoms in the bond. An alloy is a metallic mixture. Delocalized electrons are free to move around and produce electricity and energy. The properties of metals are explained by metallic bonding, including the luster shine, malleability, and ductility. Alloy=is a mixture of metal atoms with another element with metal properties, eg, luster, malleability.
Double bond=sharing two pairs of electrons to complete the valence octet
Triple bond=sharing three pairs of electrons to complete the valence octet
Diatomic element=two atoms of the same element bonded together. The 7 diatomic elements are hydrogen (H), nitrogen (N), oxygen (O), fluorine (F), chlorine (Cl), bromine (Br), and iodine (I).
Polarity=is the unequal distribution of electrical charge=bond is shifted toward the more electronegative atom in a bond=polarity is the tendency of an object to form localized regions of opposite charge. Polarity=formation of two localized regions of opposite character
Electronegativity is the measure of the atom's ability to attract electrons to itself in a chemical bond
Lewis Structures=are two dimensional diagrams that show the bonds between two atoms using electron dot notation=Lewis structures represent only covalent bonds
Steps for Drawing Lewis Structures: Only Covalent Bonds
Oct. 17-18
1-Write the electron dot symbol for each element in the compound (use valence electrons according to group column number)
2-Determine how many valence electrons are available
3-Place the element with the most unpaired electrons in the center
4-Place remaining element symbols for the compound around the central atom
5-Create as many single bonds as possible by pairing up adjacent electrons
6-Create a second bond between the the atoms if needed to reach eight valence electrons
7-For ions, surround the Lewis Structure with brackets and place ion charge number on upper right
by Owen Borville
October 11-18, 2022
Chemistry
Terms for Chemical Bonds
Electrostatic Force=between electric charges of atoms’ nucleus and electrons
Polyatomic ion=filled valence electrons instead of sharing electrons
Formula unit=ratio of cations (+) to anions(-) needed to achieve neutrality and determine chemical formula
Crystal lattice=is an orderly 3-dimensional arrangement of atoms
Electron sea theory=is a sea of mobile electrons in metallic bond
Network covalent substance=is a covalent bond in continuous three dimensional network=e.g.=diamond
Chemical Bond= share or transfer of electrons among chemical elements and compounds. Chemical Bond=when atoms link or attach to each other to maximize stability =chemical bond=energy is usually released as a result
Atoms form chemical bonds in order to= become stable in the lowest energy state in their valence electron shells.
Octet Rule= atoms maximize stability when they have a full valence energy level, usually with 8 valence electrons in the outer energy level. Atoms will transfer, accept, or share electrons necessary to complete the outer valence shell of 8 electrons. Atoms can complete the octet rule by sharing or transferring electrons.
Covalent bonding=electrons are shared to produce the bond. Covalent bonding involves nonmetal ions tightly shared. Covalent compounds tend to be gasses, liquids, soft solids, and poor conductors of electricity. These are the properties of nonmetallic substances.
Ionic bonding=one atom loses an electron and another atom gains an electron by transferring; atoms in an ionic bond are held together by the opposite charges (+,-) Ionic bonding involves metallic and nonmetallic ions. Ionic compounds form solid crystalline substances and lattices. High melting points, good insulators.
Metallic bonding=is an electron sea of freely moving electrons shared by all metal atoms in the bond. An alloy is a metallic mixture. Delocalized electrons are free to move around and produce electricity and energy. The properties of metals are explained by metallic bonding, including the luster shine, malleability, and ductility. Alloy=is a mixture of metal atoms with another element with metal properties, eg, luster, malleability.
Double bond=sharing two pairs of electrons to complete the valence octet
Triple bond=sharing three pairs of electrons to complete the valence octet
Diatomic element=two atoms of the same element bonded together. The 7 diatomic elements are hydrogen (H), nitrogen (N), oxygen (O), fluorine (F), chlorine (Cl), bromine (Br), and iodine (I).
Polarity=is the unequal distribution of electrical charge=bond is shifted toward the more electronegative atom in a bond=polarity is the tendency of an object to form localized regions of opposite charge. Polarity=formation of two localized regions of opposite character
Electronegativity is the measure of the atom's ability to attract electrons to itself in a chemical bond
Lewis Structures=are two dimensional diagrams that show the bonds between two atoms using electron dot notation=Lewis structures represent only covalent bonds
Steps for Drawing Lewis Structures: Only Covalent Bonds
Oct. 17-18
1-Write the electron dot symbol for each element in the compound (use valence electrons according to group column number)
2-Determine how many valence electrons are available
3-Place the element with the most unpaired electrons in the center
4-Place remaining element symbols for the compound around the central atom
5-Create as many single bonds as possible by pairing up adjacent electrons
6-Create a second bond between the the atoms if needed to reach eight valence electrons
7-For ions, surround the Lewis Structure with brackets and place ion charge number on upper right