Inorganic exam

hexagonal close packing pattern

ABABAB

hexagonal close packing coordination number

12

cubic close packing pattern

ABCABCABC

cubic close packing coordination number

12

ABCC violates close packing because ____ adjacent layers are in register

2

2 types of interstitial holes

tetrahedral and octahedral

tetrahedral hole formed between ___ spheres

4

2N tetrahedral holes per __ spheres

N

octahedral holes are formed between ___ spheres

3

__ octahedral holes for every N spheres

N

primitive cubic arrangement of anions with cations in every hole

CsCl

coordination number for CsCl arrangement

8

NaCl structure has ______ type holes and ___ coordination

octahedral, 6:6

substitutional solid solutions have solute atoms ______ host atoms in the original lattice

replace

substitutional solid solutions require _____ radii

similar

interstitial solid solutions involve _____, non-metal atoms that occupy interstitial _____ in the metal lattice without disrupting the crystal structure

small, voids

interstitial atoms must be much ______ than host atoms

smaller

value for corner atom

1/8

value for face atom

1/2

value for edge atom

1/4

value for center atom

1

radii ______ as positive charge increases

decreases

radii ______ for more positively charged atoms because of the stronger Zeff

decreases

radii _______ as coordination number increases

increases

radii _____ with coordination number because packing more neighbors around a central atom ______ electrostatic repulsion and forces neighboring ions out

increase, increase

higher lattice enthalpies correspond to ____ charge and _____ radii

higher, smaller

higher lattice enthalpy = ______ crystal stability

greater

high lattice energy ______ dissolution because crystal is more stable than dissolving

resists

_______ energy needs to overcome lattice energy if something will dissolve

hydration

NaCl has ___ lattice energy, so it is likely to dissolve

ions of smaller size = large lattice energies, tend to be ________ (like LiF, MgO)

insoluble

ions with large size ______ = lower lattice energy, more soluble (like NaCl, RbCl)

mismatch

Bronsted Lowry acid is a proton ______

donor

Bronsted Lowry base is a proton ________

acceptor

Lewis acid is an electron ________

acceptor

Lewis base is an electron ______

donor

solvent auto_______: 2AB —>A+ + AB2-

ionization

for hexaaqua metal ions, acidity ________ with higher charge density/polarizing power

increases

Pauling’s Rule

8-5p

Pauling’s Rule is for ____

pKa

p in pauling’s rules is equal to number of oxo oxygens (non ________)

hydroxyl

hard species: _____ ionic radius, high ox. state/charge, low polarizability

small

soft species: _____ ionic radius, low ox. states, highly polarizable

large

hard acids prefer ____ bases, soft acids prefer ______ base

hard, soft

H+, Li+, Na+, Al3+, Fe3+

hard acids

F-, OH-, O2-, H2O, NH3

hard bases

Ag+, Au+, Hg2+, Cd2+

soft acids

I-, S2-, CN-, R3P

soft bases

Fe2+, Cu2+, Zn2+

borderline acids

why are borderline acids likely to be essential to life but toxic in excess

they can bind to hard N in proteins and soft S in amino acids

most hard ____ metal ions are neither essential nor toxic

acids

all _____ acid metal ions are toxic when concentration is in tens of mg/kg

soft

most common hard _____ are not toxic

bases

hypothetical charge an atom would have if all its bonds to other atoms were ionic

oxidation state

Spontaneous reaction when delta G is less than ___, E is greater than ___, and Keq is greater than ___

0, 0, 1

[products]^x / [reactants]^y = __

Q

pH dependent potentials involve a _______ half reaction with ___ ions involved

reduction, H+

if a reaction consumes protons, increasing the pH causes a _______ in reduction potential (now less spontaneous)

decrease

single oxidation state is simultaneously oxidized and reduced

disproportionation

2Cu+ —>Cu2+ + Cu is an example of _________

disproportionation

2 different oxidation states reaction to form a single intermediate state is ________

comproportionation

Ag2+ + Ag —> 2Ag+ is an example of __________

comproportionation

oxidizing agent is the species that gets ______

reduced

reducing agent is the species that gets _________

oxidized

the _______ point on a Frost diagram is the most stable oxidation state

lowest

if species lies below straight line on frost diagram, is is unstable towards _________

comproportionation

if species lies above straight line on frost diagram, species is unstable towards ________

disproportionation

steep _______ slope on frost diagram is a strong oxidizing agent

positive

steep _____ slope on frost diagram is a strong reducing agent

negative

horizontal lines on pourbaix diagram is pure ______ transitions, so pH independent

redox

slanted lines on pourbaix diagram is coupled _____ and proton transfer transitions

redox

vertical lines on pourbaix diagram is pure acid-base/_______ transitions

precipitation

________ diagrams show the temperature dependence of stability of compounds

Ellingham

elements on Ellingham diagram can be ______ by those that lie below it’s line

reduced

lower line on ellingham diagram = more negative ___ = more stable and harder to reduce

delta G