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Chemical Bonding---AP CHEMISTRY

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Section 1

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Chemistry Science

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Date created

Mar 1, 2020

Cards (32)

Section 1

(32 cards)

Linear

Front

Results from an sp hybrid orbital; bond angle = 180 degrees; two electron domains

Back

Tetrahedral

Front

Results from an sp3 hybrid orbital; bond angle = 109.5 degrees; four electron domains

Back

Double/triple bond

Front

Sharing of two or three pairs of electrons, respectively; triple bond is the shortest and strongest bond

Back

Lattice energy

Front

Energy needed to separate an ionic lattice into a gaseous ions; increases with increasing ion charge or decreasing distance between the ions

Back

Nonpolar covalent bond

Front

Electrons are shared equally by two atoms in a bond

Back

Hybrid orbital

Front

Orbitals of two atoms that overlap/hybridize as the atoms bond

Back

Bond angle

Front

Angle between two bonds

Back

Bond order

Front

Bond order of 1 = single bond; bond order of 2 = double bond; bond order of 3 = triple bond

Back

Electron domain geometry

Front

Arrangement of electron domains around a central atom

Back

Bonding pair

Front

Electrons which are used in making bonds

Back

Polar covalent bond

Front

Electrons are shared unequally by two atoms in a bond

Back

Nonbonding pairs/Long pairs

Front

Electrons that do not participate in bonding

Back

Metallic bond

Front

Attraction of metallic nuclei with delocalized electrons

Back

Dipole

Front

The separation of charge

Back

Molecular geometry

Front

Arrangement of atoms

Back

Resonance structure

Front

A molecule that has more than one valid Lewis structure; true shape is a "blend" of all valid structures

Back

Valence-Shell Electron-Pair Repulsion Theory (VSEPR) Theory

Front

The shape of a molecule ultimately depends on the repulsions of electron domains; domains orient themselves to minimize repulsion

Back

Coulomb's Law

Front

Equation that describes the electrostatic force between two charges: F = (kQ1Q2)/(r^2)

Back

Ionic bond

Front

Attraction that results from the electrostatic forces that exist between ions of opposite charge

Back

Electronegativity

Front

Measure of the ability of an atom in a molecule to compete with other atoms for electrons

Back

Formal charge

Front

Charge that the atom would have if all atoms had the same electronegativity

Back

Polar molecule

Front

A molecule whose centers of positive and negative charge do not coincide; it thus has a positive end and a negative end

Back

Delocalized electrons

Front

Electrons that are not hindered to one atom; resonance structures with double/triple bonds have delocalized pi bonds---the pi bond is spread out over several atoms

Back

Electron domians

Front

Regions about a central atom in which electrons are likely found; can be bonding or nonbonding pairs

Back

Single bond

Front

Sharing of one pair of electrons; longest and weakest of bonds

Back

Molecular orbital

Front

Orbtial formed during bonding

Back

Pi bond

Front

Bonds in which p orbitals overlap sideways; double bond has one pi bond, triple bond has two pi bonds

Back

Lewis structure

Front

Diagram of electron distribution in a molecule

Back

Trigonal planar

Front

Results from an sp2 hybrid orbital; bond angle = 120 degrees; three electron domains

Back

Sigma bond

Front

Bond in which electrons lie directly between the two atoms; found in single bonds; one each in double or triple bonds

Back

Covalent bond

Front

Attraction between atoms that share electrons

Back

Octet rule

Front

The attempt by an atom to achieve a noble gas configuration

Back