electrostatic attraction holding two atoms together; two nuclei attracted to the electrons between

releases energy

requires energy

complete transfer of electrons; metal and non metal; salt

electrons are shared between atoms; nonmetals

ability for an atom to steal an electron from another when bonding; large number indicates strength

covalent

ionic

product of two molecules divided by their distance

ordered 3D array of particles; high energy determined by higher charge, then smaller size

equal sharing of electrons

unequal sharing of electrons

separation of electrical charge created when atoms with different electronegativities form a covalent bond

quantifies extent of charge separation; measured by applied electric field, increases as dipole increases

molecule with net dipole; asymmetric charge distribution - dipoles don't cancel

infrared inactive

infrared active

infrared active

communal sharing of electrons known as a "sea of electrons" - allows for malleability and the absorption of excess energy

first nonmetal: #prefix+element name second nonmetal: #prefix+element name+-ide suffix

cation charge implied - name of element; anion name is element + -ide

roman numeral indicates charge of cation

covalent bonds with charge; named cation + anion

A salt that contains water of crystallization; name ionic salt and add [prefix] hydrate

absorb water from air; forms desiccants, filters, etc

the salt crystals without water molecules in the compound

hydro(root)ic acid

-ate turns to -ic -ite turns to -ous

prediction of valence electrons divided between bonding electrons and lone pairs

atoms tend to lose, gain or share electrons in order to acquire a full set of eight valence electrons

covalent bond in which two pairs of electrons are shared between two atoms

covalent bond in which two atoms share three pairs of electrons

the number of shared electron pairs between two atoms

the average distance between the nuclei of two bonded atoms; shorter = stronger, higher order bond; longer = longer, lower order bond

multiple arrangements of electrons; reality is an "average" of all structures

rearranged electrons not atoms, same net charge; no more structures than bonding sites

spreading of electrons over more than one bond - greater spread (low kinetic) closer to the nucleus (low potential) reduces energy

of valence electrons - ( # dots + # lines)

atoms in third row or below can accommodate more than eight electrons

best arrangement of atoms is one that minimizes repulsion - keeps electrons as far away from each other as possible

number of atoms bonded to central atom + number of lone pairs on central atom

the geometrical arrangement of the electron groups

the arrangement of bonded atoms, differs from electron geometry when lone pairs are present

sn=2, 180

sn=3, 120

sn=4, 109.5

sn=5, 90/120

sn=6, 90

angle between nuclei

sn=3, 117, 2 bonds, 1 lone pair

sn=4, 107, 3 bonds, 1 lone pair

sn=4, 104.5, 2 bonds, 2 lone pairs

sn=5, <90/<120, 4 bonds, 1 lone pair

sn=5, <90, 3 bonds, 2 lone pairs

sn=6, 90, 5 bonds, 1 lone

sn=6, <90, 4 bonds, 2 lone

subunit imparts characteristic behavior

single bond between carbons

double bond between carbons

triple bond between carbons

bond in front of plane

bond behind the plane

parallel to plane

max number of hydrogens per carbon in chain

less than max number of hydrogens per carbon in the chain

same chemical formula, different structure

same molecular formula, different connectivity

same covalent arrangements but differ in spatial arrangements

two like groups on same side of c=c

two like groups on opposite sides of c=c

different rotations about C-C bonds

isomers that are mirror images of each other

an atom at which the interchange of two groups produces a stereoisomer; carbon attached to 4 nonequivalent atoms/groups

amine; carboxylic acid with R group in middle - chiral if R is not hydrogen (glycine)

all bonds from from overlap of two half filled valence orbitals, bond = increased density

applicable, explains shapes

valence electrons belong to atom; doesn't explain magnetism, absorption/emission, or bond energy values

head-head overlap producing a single bond with electron density along internuclear axis, stronger bond that lowers energy

side-side overlap of p orbitals with electron density above/below axis; planar node through bond axis; allows for multiple bonds to be formed

wave functions of all electrons change when atoms approach each other, electrons do not belong to any one atom, orbitals extend over entire molecule

a molecular orbital that can be occupied by two electrons of a covalent bond

a molecular orbital that is higher in energy than any of the atomic orbitals from which it was formed

one node parallel to atomic bond

two nodes perpendicular to atomic bond

amino acid structure is primary structure

carboxylic acid reacts with amine end - hydrolysis creates water

carbonyl O with H-N on amino acid four structures away

ring of six carbons with six molecular orbitals from combining PZ atomic orbitals

many energy levels closely spaced together

behaves as giant molecule, #MO as #atoms-bands

partially filled/filled band

molecular orbitals higher in energy and distinctly separated from occupied valence band

valence and conduction bands overlap, allowing electrons to easily delocalize

valence band full with small gap to conduction band; as group number increases, band gap increases

chemically altering band gap by replacing atoms to increase conductivity

electron rich, populating conduction band

electron poor, less electrons in valence create "holes" that allow for movement of electrons

assumes gas molecules have insignificant volumes compared to their container volume, moves randomly and constantly, collide elastically, no intermolecular forces and that average kinetic energy is proportional to temperature

average energy of motion

gas escapes through a tiny opening, heavier gases diffuse more slowly