AP CHEM TEST

intermolecular forces

forces of attraction between molecules

dipole-dipole forces

forces of attraction between polar molecules where the partial positive end of one molecule is attracted to the partial negative end of another molecule

Intramolecular

forces within a molecule

valence electrons - nonbonding electrons - bonds to the atom

formal charge equation

Polarizability

the ease with which the electron distribution in the atom or molecule can be distorted

Hydrogen bonding

the intermolecular force in which a hydrogen atom that is bonded to N, O, or F on one molecule is then bonded to an N, O, or F on another molecule

Increases

As temperatures rises, vapor pressure ______

Polar

Bonds of different elements

Nonpolar

Bonds of the same element

Low MP, non-conductor, weak IMF's

Characteristics of (covalent) molecular solid

3-D network, hard, high MP, Jon-conductor

Characteristics of covalent network solids

High MP and BP, brittle because repulsion of like charges when layers slide past each other

Characteristics of ionic solids

Good conductors, crystal lattice with "sea" of delocalized electrons, malleable, and ductile

Characteristics of metallic solids

Electronegative

Dipoles go towards the more ________ atom

Potential energy

Energy required to break a bond

Larger

Polarizability is more common in _______ electron clouds

Ionic bonding

Solid that does not conduct electricity in a solid state but becomes a conductor when melted or dissolved in water

Covalent network

Solid that doesn't conduct electricity in any phase and has a high melting point

Molecular (covalent)

Solid that doesn't conduct electricity in any phase and has a low melting point

Metallic bonding

Solid that is good electrical conductor

Longer bonds

The easiest bonds to break are

The stronger the attractive force

The greater the charger of ions

Lower the lattice energy

The larger the atomic radius the

The shortest bonds

The largest bond energies are in

Does not

The polar molecule ________ always have stronger IMF's

The stronger the attractive force

The smaller the ionic radius

The higher the lattice energy

The stronger the attractive force

Bond length

What decreases as bond order increases

Bond energy

What increases as bond order increases

Polar

When electron clouds are approximately the same size, the ______ molecule tends to have stronger IMF's

Interstitial because the smaller atoms fill in the spaces between larger atoms

Which alloys are strong and why?

sigma, pi

a double bond would be one _________ bond & one ________ bond

sigma

a single bond would be one ______________ bond

resonance structure

a structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion

sigma, pi

a triple bond would be one _______ bond & two ______ bonds

Ion-dipole forces

attractive forces between an ion and a polar molecule

The nonpolar molecule has a higher boiling point

Non polar molecules have stronger IMF's than polar molecules when

Potential energy is at a minimum

On a diagram of potential energy a stable bond occurs when

Too much repulsion

On a diagram of potential energy when potential energy is above zero there is

London dispersion

All molecules have ________ forces

Metallic solids

Alloys are

Stronger, lower

Higher boiling point means ______ IMF's and ______ vapor pressure

Stronger

Higher the boiling point the _______ the attractive forces

Up and across to the right

How do electronegativity and electron affinity increase on the periodic table

Across to the left & down

How does atomic and ionic radius increase on the periodic table

Up and across to the right

How does ionization energy increase on the periodic table

charge

If charged then the sam of formal charges will equal the

most electronegative atom

If it isn't possible for atoms to have a formal charge of zero, then favor the structure with the negative charge on the

More polar the bonds

In a polar covalent bond the greater the electronegativity difference the

Partial negative charge

In a polar covalent bond, the atom that has the most electronegativity will have a

London dispersion forces

Interactions between molecules or particles as a result of temporary or instantaneous dipoles

Weaker, higher

Lower boiling point means _______ IMF's and ________ vapor pressure