Chemical Bonding in the Physical Sciences
by Owen Borville
October 14, 2022
Physical Science
Chemical Bond=share or transfer of electrons among chemical elements and compounds
Atoms form chemical bonds form in order to become stable in the lowest energy state in their valence electron shells.
Octet Rule=atoms are stable 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;
atoms in an ionic bond are held together by the opposite charges (+,-) Ionic bonding involves metallic and nonmetallic ions. Ionic compounds form crystalline substances.
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.
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=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.
Electronegativity is the measure of the atom's ability to attract electrons to itself in a chemical bond
Lewis Structures=two dimensional diagrams that show the bonds between two atoms using electron dot notation=Lewis structures represent covalent bonds
by Owen Borville
October 14, 2022
Physical Science
Chemical Bond=share or transfer of electrons among chemical elements and compounds
Atoms form chemical bonds form in order to become stable in the lowest energy state in their valence electron shells.
Octet Rule=atoms are stable 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;
atoms in an ionic bond are held together by the opposite charges (+,-) Ionic bonding involves metallic and nonmetallic ions. Ionic compounds form crystalline substances.
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.
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=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.
Electronegativity is the measure of the atom's ability to attract electrons to itself in a chemical bond
Lewis Structures=two dimensional diagrams that show the bonds between two atoms using electron dot notation=Lewis structures represent covalent bonds