equations

Question 1

energy of a quantum

Answer 1

E = hf 
h = plancks constant

Question 2

energy of an electron

Answer 2

E = -Rh/ n^2 
Rh = Rydberg constant
n= quantum #

Question 3

energy of an e- is _______ proportional to the principle quantum # (n)

Answer 3

directly proportional, bc of the negative sign in the equation, as n increases, gets closer to 0 (thus increasing)

Question 4

the energy of an e- _________ the further out from the nucleus that is is located

Answer 4

increases

Question 5

electromagnetic energy

Answer 5

of photons emitted by e- that return to ground state

E=hc/lambda

h= planck's constant
c = speed of light = 3*10^8
lambda = wavelength

Question 6

the energy difference between two shells _________ as the distance from the nucleus increases

Answer 6

decreases

so the energy diff. between n=3 and n=4 is less than the energy diff. between n=1 and n=2

Question 7

range of possible values for l (azimuthal quantum #)

Answer 7

0 - (n-1)

Question 8

for any value of n, there will be a max of ______ electrons

Answer 8

2n^2

2 per orbital

Question 9

draw out e- subshell flow diagram

Answer 9

do it

Question 10

E = hc/lambda = ?

Answer 10

-Rh*(1/ni^2-1/nf^2)

Question 11

planck’s constant

Answer 11

6.62610^-34 Js

Question 12

diatomic elements (7)

Answer 12

H2
N2
O2
F2
Cl2
Br2
I2

Question 13

dipole moment equation

Answer 13

u= qr

q = charge magnitude
r = distance between 2 partial charges

Question 14

in lewis structure, which atom is the central atom?

Answer 14

the least electronegative

Question 15

difference between electronic geometry and molecular geometry?

Answer 15

electronic includes bonding and lone pairs around central atom

molecular geometry describes spatial arrangement of only the bonding pairs

Question 16

gram equivalent weight

Answer 16

molar mass/n

equiv. weight of a compound is the mass that provides one mole of charge

ex. need 49g of H2SO4 (molar mass=98g/mol) to produce one mole of H+ ions
bc it can donate 2 H’s, n=2

Question 17

equivalents

Answer 17

mass of compound / gram equivalent weight

Question 18

normality

Answer 18

equivalents/liter

Question 19

molarity

Answer 19

normality/ n

Question 20

% composition

Answer 20

(mass of X in formula/ formula weight of compound) * 100%

Question 21

percent yield

Answer 21

(actual yield/theoretical yield) * 100%

Question 22

what is the only factor that can change the rate of a zero-order rxn?

Answer 22

temperature

Question 23

1st law of thermodynamics

Answer 23

deltaU = Q-W

total internal energy = heat(Q) - work (W)

Question 24

specific heat equation

Answer 24

specific heat (q) = mass (m)* specific heat of substance (c) * delta T (change in temp)

Question 25

specific heat of H20 (l)

Answer 25

1 cal/ g*celsius

Question 26

celsius to F equation

Answer 26

F = (9/5)*C + 32

Question 27

when do gases deviate from ideal behavior?

Answer 27

high pressure, low temp

Question 28

KE =? (in terms of gas molecules)

Answer 28

KE = .5mv^2 = (3/2)kT k = boltzmann constant

Question 29

graham's law equation

Answer 29

r1/r2 = sqrt(M2/M1) r1 and r2 = rates of diffusion/effusion

Question 30

osmotic pressure equation

Answer 30

osmotic pressure = iMRT i= van't hoff factor (ex. NaCl, i=2) M=molarity R= ideal gas constant T = temp (K)

Question 31

freezing/boiling pt depression equation

Answer 31

deltaT = iKm i= van't hoff factor K= proportionality constant m=molality

Question 32

all ________ and _______ salts are completelhy soluble

Answer 32

all sodium and all nitrate salts are completely soluble

Question 33

strong acids (7)

Answer 33

``` HCl HBr HI H2SO4 HNO3 HClO3 HClO4 ```

Question 34

weak acids (6)

Answer 34

``` HF HCN acetic acid H2O HSO4- NH4+ ```

Question 35

strong bases (6)

Answer 35

``` NaOH KOH CaOH2 CaO NaO NH2- ```

Question 36

weak bases (6)

Answer 36

``` acetate - CH3COO- H2O SO4^2- CN- F- NH3 ```