Inorganic Chemistry

Front 1

maximum number of electrons held by any shell

Back 1

2n^2

Front 2

what percent of a compound is left after 1 half life, 2, 3... to 6

Back 2

100, 50, 25, 12.5, 6.25, 3.125, 1.563

Front 3

what fraction of a compound is left after 1 half life, 2, 3... to 6

Back 3

1, 1/2, 1/4, 1/8, 1/16, 1/32, 1/64

1/(2^number of half lives)

Front 4

what is ionization energy?

Back 4

energy required to remove an electron

associated with oxidation

Front 5

what is the azimuthal number?

Back 5

l quantum number = type of subshell (s,p,d,f)

Front 6

what is electron affinity?

Back 6

energy change associated with gaining an electron (associated with reduction)

Front 7

trend for increasing atomic radius

Back 7

down and left (toward Francium)

Front 8

which radius is smaller, a neutral species or its cation?

Back 8

cation b/c it lost its valence e-

Front 9

which radius is larger, a neutral species or its anion?

Back 9

anion, gained e-

Front 10

compare Li+ and Na+

which is bigger?

Back 10

Na+ b/c it follows the atomic radius trend.

We can compare these two cations because they have the same charge.

Front 11

1st ionization energy trend

Back 11

right and up (toward He)

Front 12

Group 5A elements (N, P, As) have a higher 1st ionization energy than...

Back 12

group 6A elements (O, S, Se)

because group 5A has half full p orbitals which make it stable

Front 13

trend in electron affinity

Back 13

F

more negative ---------> Cl

Br

I

Front 14

trend in electronegativity

Back 14

up and right (toward F)

Front 15

When do you set up an ICE chart?

Back 15

dealing with solubility equilibria and common ion effect

asks about "molar solubility" AKA x

Front 16

7 strong acids

Back 16

HCl

HBr

HI

HNO3

HClO3

HClO4

H2SO4

Front 17

Strong Bases

Back 17

Group one metals: Li, Na, K, Rb, Cs

Group two metals: Ca, Sr, Ba

Front 18

arrhenius acid/base?

Back 18

acid: H+ donor in water

base: OH- donor in water

Front 19

Bronstead Lowry Acid/Base?

Back 19

Acid: H+ donor

Base: H+ acceptor

Front 20

Lewis Acid/Base?

Back 20

Acid: e- acceptor

Base: e- donor

(applies to EVERY reaction)

Front 21

Trend for binary acids

(H and some other atom)

Back 21

increases to right (EN) and down (size)

Front 22

Trend for Oxoacids

(H, O, and some other atom)

Back 22

1) more oxygen= more acidic

2) more EN heteroatom= more acidic

ex: HClO3 > HBrO3

Because Cl is more e- withdrawing causing molecule to be more stable after losing H+

Front 23

Formula for calculating pH

Back 23

pH=-log [H+]

Front 24

How do you solve for [H+] if given pH?

Back 24

10^-pH

Front 25

Shortcut for finding [H+] of weak acid

Back 25

[H+]= [Ka (HA)]^1/2

Front 26

Shortcut for finding [OH-] of weak base

Back 26

[OH-]= [Kb (A-)]^1/2

Front 27

if given Ka, how can you solve for Kb?

Back 27

Ka(Kb)=Kw

Kb= Kw/Ka

we know Kw=1x10^-14 @25 degrees C

Front 28

pKa + pKb = ?

Back 28

14

Front 29

cations are usually (acidic/basic)

while anions are usually __________

except for when the come from __________ then they are neutral/neglegible

Back 29

cations: acidic

anions: basic

a strong acid or base

Front 30

acidic anion that is an exception for pH of salts

Back 30

HSO4-

Front 31

Basic salts are more soluble in ______ solutions because...

Back 31

acidic, because H+ reacts with the anion and drives the reaction forward

Front 32

If there is 10X more acid than base in a buffer, what happens to the pH?

Back 32

pH goes down by 1

Front 33

If there is 10X more base than acid in a buffer, what happens to the pH?

Back 33

pH goes up by 1

Front 34

when is a buffer at its maximum capacity?

Back 34

when ratio of acid to conjugate base is 1:1

which is also when pH = pKa

BECUASE

pH=pKa+ log [A-]/[HA]

this part turns into 0

Front 35

What are three ways to make a buffer?

Back 35

i) ~1 eq weak acid / 1 eq of conjugate base

ex: HF and F-

ii) ~1 eq weak acid / 1/2 eq of strong base

ex: HF and NaOH

iii)~1 eq weak base / 1/2 eq of strong acid

ex: NaF and HCl

Front 36

what is the pH at equivalence point for

1) SA/SB

2) WA/SB

3) SA/WB

Back 36

1) 7

2) >7

3) <7

Whichever one is "strong" wins

Front 37

What does the equivalence point of a titration tell you?

Back 37

mol acid = mol base

also tells you what pKa your indicator needs to be

Front 38

Why does a strong acid weak base titration have a pH <7 @ equiv. ?

Back 38

conjugate acid undergoes hydrolysis and dissociates (releasing H+)

Front 39

Why does a weak acid strong base titration have a pH > 7 @ equiv. ?

Back 39

conjugate base undergoes hydrolysis and forms hydroxide.

Front 40

What does the half equivalence point of a titration tell you?

Back 40

pOH=pKb

[HA]=[A-]

pH=pKa

Front 41

Will it take more NaOH to titrate 10 mols of HCl or 10 mols of acetic acid?

Back 41

Wether you have a strong acid or weak acid, if you have an equal number of mols of s. acid and w. acid it will take the same number of mols of NaOH to titrate it.

Front 42

equation to use when solving for how much titrant to add to analyte of a given volume and concentration

Back 42

nA MA VA = nB MB VB

n= how many H+ or OH- dissociate

M= molarity

V= volume (does not need to be in L b/c it will cancel out)

Front 43

What is the standard enthalpy of formation of any element or diatomic molecule in its most stable form?

Back 43

zero

ex: Cl2(s) would not be zero since Cl2 is a gas in its most stable state, not a solid

Front 44

when looking at which ion has the largest radius you should first look at...

Back 44

which ion has the most - charges b/c gain of e- increases atomic size greatly

Front 45

what happens if you mix a transition metal with NH3

Back 45

transition metals have a tendency to form complex ions which makes their salts more soluble

Front 46

Nucleotides with atomic numbers greater than _____ are radioactive and unstable

Back 46

83

Front 47

do all molecules of an ideal gas have the same kinetic energy at constant temperature?

Back 47

no, Boltzmann distribution curve says that at nay given temperature molecules of a gas move at different speeds.

Front 48

Formula for calculating E0 cell

Back 48

E0= E0red + E0ox

If given table of red. potentials keep the more positive (reduction) one and flip the symbol of the more negative one (oxidation).

These values should not be multiplied by stoichiometric values

Front 49

Galvanic Voltaic Cells

Back 49

spontaneous, Ecell>0

negative delta G

produce electricity

e- flow from anode to cathode

Front 50

Electrolytic Voltaic Cells

Back 50

non spontaneous, Ecell<0

consume electricity

e- flow from anode to cathode

Front 51

Formula for calculating non standard cell potential

Back 51

E=E0 - (0.0592/n) log Q

n= e- transferred

Q= [prod]/[react]

Front 52

How do you increase Ecell?

Decrease?

Back 52

increase= shift to right

decrease= shift to left

Front 53

What are allotropes?

Back 53

different forms of the same element.

ex: O2 and O3

diamond and graphite

Front 54

Strong acids such as HClO4 and HCl give off the most particles which will _________ the freezing point and ________ the boiling point to the greatest extent.

Back 54

lower

raise

Front 55

Formula when given specific heat of metal

Back 55

deltaH= m c deltaT