Chemical Bonding Notes
Chapter 6: Chemical Bonds
Section 6.1: Ionic Bonding
Chemical bond: the force that holds atoms of elements and ions together to become a stable, new substance called a compound.
-the number of valence electrons determines if an atom will form a chemical bond. -metals tend to give up electrons to other atoms. -nonmetals tend to take electrons from other atoms.
-noble gases will not form a chemical bond because these atoms already have a full outer shell of energy.
Ionization: the process of gaining or losing electrons to become an ion. -ion: atom that has a net positive or negative charge. -anion (negative ion): an ion with a negative charge. -cation (positive ion): an ion with a positive charge.
Oxidation number: number of electrons an atom gains, loses, or shares when it forms a chemical bond. -remember this pattern: +1, +2, +3, +/-4, -3, -2, -1, 0 -example: -sodium (Na): -valence electrons = 1 -oxidation number = +1 -resulting ion = Na+1
Rule of oxidation numbers: the sum of all the oxidation numbers of all atoms in a molecule must equal zero, indications that the molecule is neutral.
SHORTCUT: flip the oxidation numbers to get the final compound.
Ionic bond: chemical bond that involves the transfer of electron(s) from one atom (metal) to another atom (nonmetal).
-meaning the metal atom becomes a positive ion and the nonmetal atom becomes a negative ion. -resulting net charge is zero.
Chemical formula: notation showing what elements a compound contains and the ratio of those atoms in a compound. -Li (+1) + F (-1) = LiF -Ca (+2) + F (-1) = CaF2
Properties of Ionic Bonds: -energy for formation of ionic bonds:
-ionization energy: the amount of energy required to remove an electron from an atom.
-as the number of valence electrons increases, the ionization energy increases.
-electron affinity (love): how strongly atoms of an element attract electrons. -as the ionization
Section 6.1: Ionic Bonding
Chemical bond: the force that holds atoms of elements and ions together to become a stable, new substance called a compound.
-the number of valence electrons determines if an atom will form a chemical bond. -metals tend to give up electrons to other atoms. -nonmetals tend to take electrons from other atoms.
-noble gases will not form a chemical bond because these atoms already have a full outer shell of energy.
Ionization: the process of gaining or losing electrons to become an ion. -ion: atom that has a net positive or negative charge. -anion (negative ion): an ion with a negative charge. -cation (positive ion): an ion with a positive charge.
Oxidation number: number of electrons an atom gains, loses, or shares when it forms a chemical bond. -remember this pattern: +1, +2, +3, +/-4, -3, -2, -1, 0 -example: -sodium (Na): -valence electrons = 1 -oxidation number = +1 -resulting ion = Na+1
Rule of oxidation numbers: the sum of all the oxidation numbers of all atoms in a molecule must equal zero, indications that the molecule is neutral.
SHORTCUT: flip the oxidation numbers to get the final compound.
Ionic bond: chemical bond that involves the transfer of electron(s) from one atom (metal) to another atom (nonmetal).
-meaning the metal atom becomes a positive ion and the nonmetal atom becomes a negative ion. -resulting net charge is zero.
Chemical formula: notation showing what elements a compound contains and the ratio of those atoms in a compound. -Li (+1) + F (-1) = LiF -Ca (+2) + F (-1) = CaF2
Properties of Ionic Bonds: -energy for formation of ionic bonds:
-ionization energy: the amount of energy required to remove an electron from an atom.
-as the number of valence electrons increases, the ionization energy increases.
-electron affinity (love): how strongly atoms of an element attract electrons. -as the ionization