A strong attractive force that exists between atoms in a molecule
Chemical bond
Electrostatic forces that exist between ions of opposite charge
Ionic bond
The sharing of electrons between two atoms
Covalent bonds
Bonding, usually in solid metals, in which the bonding electrons are relatively free to move throughout the three-dimension structure
Metallic bonds
Involved in chemical bonding
Valence electrons
The chemical symbol for an element, with a dot for each valence electron
Lewis symbol
Atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons
Octet rule
Formation of ions usually very (blank)
Exothermic
The energy required to completely separate a mole of a solid ionic compound into its gaseous ions
Lattice energy
Electrostatic energy equation thing
Eel=?Q?Q?/d (Qs are charges of particles; d is the distance between their centers)
?
8.99*10? J-m/C�
Lattice energy (blank) as the charges on the ions increase and as their radii decrease
Increases
Which shell do transition metals lose from first?
S
A thermodynamic cycle based on Hess's law that relates the lattice energy of an ionic substance to its enthalpy of formation and to other measurable quantities
Born-Haber Cycle
Random equation about lattice energy...
?H=-?Hlattice
A representation of covalent bonding in a molecule that is drawn using Lewis symbols
Lewis structure
A covalent bond involving one electron pair
Single bond
A covalent bond involving two electron pairs
Double bond
A covalent bond involving three electron pairs
Triple bond
The distance between the nuclei of the atoms involved in a bond
Bond length
Distance between bonded atoms (blank) as the number of shared electron pairs increases
Decreases
Queen
Fluorine
Pattern of electronegativity across a period; why?
Increases; Zeff increases and electrons are therefore closer to the nucleus
Pattern of electronegativity down a group; why?
Decreases; because of shielding
Ionic
2-4
Polar covalent
2-1
Moderately polar covalent
1-.4
Nonpolar
<.4
Greater difference in electronegativity=
More polar bond
Pattern of bond length down a group
Increases
A measure of the degree to which the electrons are shared unequally between two atoms in a chemical bond
Bond polarity
A covalent bond in which the electrons are shared equally
Nonpolar covalent bond
A covalent bond in which the electrons are not shared equally
Polar covalent bond
The ability of an atom in a molecule to attract electrons to itself
Electronegativity
Greater electronegativity=
Greater ability to attract electrons=more negative electron affinity=higher ionization energy
A molecule in which the centers of a positive and negative charge do not coincide
Polar molecule
A molecule with one end having a partial negative charge and the other end having a partial positive charge
Dipole
A measure of the separation and magnitude of the positive and negative charges in polar molecules
Dipole moment
Magnitude of dipole moment
�
�=
Qr
e=
1.60*10?�? C
1 D=
3.34*10?�? C-m
As electronegativity difference decreases, bond length (blank) and dipole moment (blank)
Increases; decreases
The charge the atom would have it all the atoms in the molecule had the same electronegativity
Formal charge
Multiple ways to connect the atoms to each other
Resonance
ROY has (blank) energy than BIV
lower
Resonance structures:
COOH?, O?, C?H?, NO??, SO?
Exceptions to the Octet Rule:
Molecules and polyatomic ions containing an odd number of electrons; molecules and polyatomic ions in which an atom has fewer than an octet of valence electrons; molecules and polyatomic ions in which an atom has more than an octet of valence electrons
More than octet of valence electrons occurs when...
The central atom is bonded to smaller and more electronegative atoms (F, Cl, O, etc.)
The enthalpy change for the breaking of a particular bond in one mole of a gaseous substance
Bond enthalpy
Bond enthalpy
D(bond type)
The bond enthalpy is always a (blank) quantity
Positive
The greater the bond enthalpy, the (blank the bond)
Stronger
?Hrxn=
?(bond enthalpies of bonds broken)-?(bond enthalpies of bonds formed)
As the number of bonds between two atoms increases, the bond grows (blank) and (blank)
Shorter and stronger