Chem Exam 3

\- deltaH

endothermic

\+ deltaH

exothermic

lattice energy

energy required to separate a mole of an ionic solid into gaseous ions

Coulomb's law

energy of attraction = (charge 1 x charge 2)/distance

______ matters more than _______ for Coulomb's law

charge, distance

potential energy of covalent bonds (+ or -)

negative

bond order

# of bonds/# of locations

bond energy

energy required to overcome the electrostatic attraction of a bond and separate it

high bond order = ______ bond length = ______ bond energy

short, high

network covalent solids

a continuous network of covalent bonds

electronegativity

a value describing how well an atom can attract electrons in a molecule

electron affinity

amount of energy released when an electron is added to an atom

non-polar covalent bond

electrons shared equally

polar covalent bond

unequal sharing of electrons

polar covalent bonds have a ______ difference

electronegativity

metallic bonding has a _______ of ______ electrons

sea, delocalized

free radical

a molecule with an odd number of electrons

resonance structures

an average of all possible resonance structures

formal charge equation

valence electrons - 1/2(bonding electrons)-nonbonding electrons

formal charge rules for deciding structure

smaller better, more negative formal charge on more electronegative atom, charges add up to overall molecule charge

2 bonding groups (electron, molecular, & bond angle)

linear, linear, 180

3 bonding groups (electron, molecular, & bond angle)

trigonal planar, trigonal planar, 120

2 bonding groups, 1 lone pair (electron, molecular, & bond angle)

trigonal planar, bent,

4 bonding groups (electron, molecular, & bond angle)

tetrahedral, tetrahedral, 109.5

3 bonding groups, 1 lone pair (electron, molecular, & bond angle)

tetrahedral, trigonal pyramidal,

2 bonding groups, 2 lone pair (electron, molecular, & bond angle)

tetrahedral, bent,

5 bonding groups (electron, molecular, & bond angle)

trigonal bipyramidal, trigonal bipyramidal, 90 and 120

6 bonding groups (electron, molecular, & bond angle)

octahedral, octahedral, 90

levels of repulsion

lone pair > triple bond > double bond > single bond > free radical

isomers

same chemical formula, different shapes

cis isomers

molecules on same side of central atom

trans isomers

molecule on different sides of central atom

hybrid orbitals does not form _____ _______, just different ________

new orbitals, orientations

2 bonds

sp hybrid

3 bonds

sp2 hybrid

4 bonds

sp3 hybrid

5 bonds

sp3d hybrid

6 bonds

sp3d2 hybrid

sigma bonds

end-to-end overlap of single bonds

pi bonds

sideways overlap between double (1) and triple (2) bonds

alkanes

single bonds, saturated

alkenes

double bonds, unsaturated

alkynes

triple bonds, unsaturated

free rotation only in _____ bonds

sigma

1 carbon root

meth-

2 carbon root

eth-

3 carbon root

prop-

4 carbon root

but-

5 carbon root

pent-

6 carbon root

hex-

7 carbon root

hept-

8 carbon root

oct-

9 carbon root

non-

10 carbon root

dec-

alkane suffix

-ane

alkene suffix

-ene

alkyne suffix

-yne

aromatic hydrocarbons

6 carbon ring of delocalized electrons

alkene

alkyne

alcohol

haloalkane/halide

amine

aldehyde

ketone

carboxylic acid

ester

amide

nitrile

ether

primary alcohol

carbon bonded to 2H and 1 other C

secondary alcohol

carbon bonded to 1H and 2 other C

tertiary alcohol

carbon bonded to 3C

primary amine

1 bond between C&N

secondary amine

2 bonds between C&N

tertiary amine

3 bonds between C&N