Chapter 9 Flashcards
(25 cards)
A drawing that represents chemical bonds between atoms as shared or transferred electrons; the valence electrons of atoms are represented as dots
Lewis electron-dot structures (Lewis structures)
A chemical bond formed between two oppositely charged ions, generally a metallic cation and a nonmetallic anion, that are attracted to one another by electrostatic forces
Ionic bond
A chemical bond in which two atoms share electrons that interact with the nuclei of both atoms, lowering the potential energy of each through electrostatic interactions
Covalent bond
The type of bonding that occurs in metal crystals, in which metal atoms donate their electrons to an electron sea, delocalized of the entire crystal lattice
Metallic bonding
Represent the valence electrons of main-group elements as dots surrounding the abbreviation for the element
Lewis symbol
A Lewis structure with eight dots, signifying a filled outer electron shell for s and p block elements
Octet
A Lewis structure with two dots, signifying a filled outer electron shell for the elements H and He
Duet
The sharing or transfer of electrons to attain stable electron configurations for the bonding atoms
Chemical bond
The tendency for most bonded atoms to possess or star eight electrons in their outer shell to obtain stable electron configurations and lower their potential energy
Octet rule
The engird associated with forming a crystalline lattice from gaseous ions
Lattice energy
A hypothetical series of steps based on Hess’ law that represents the formation of an ionic compound from its constituent elements
Born- Haber cycle
A pair of electrons shared between two atoms
Bonding pair
A pair of electrons associated with only one atom
Lone pair (nonbonding electrons)
The bond that forms when two electrons are shared between two atoms
Double bond
The bond that forms when three electron pairs are shared between two atoms
Triple bond
A covalent bond between two atoms with significantly different electronegativities, resulting in an uneven distribution of electron density
Polar covalent bond
The ability of an atom to attract electrons to itself in a covalent bond
Electronegativity
A measure of the separation of positive and negative charge in a molecule
Dipole moment
The ratio of a bond’s actual dipole moment it would have it the electron were transferred completely from one atoms to the other, multiplied by 100%
Percent ionic character
Two or more valid Lewis structures that are shown with double-headed arrows between them to indicate that the actual structure of the molecule is intermediate between them
Resonance structures
The actual structure of a molecule that is intermediate between two or more resonance structures
Resonance hybrid
The charge that an atom in a Lewis structure would have if all the bonding electrons were shared equally between the bonded atoms
Formal charge
A molecule or ion with an odd number of electrons in its Lewis structure
Free radical
The energy required to break 1 mol of the bond in the gas phase
Bond energy
