General Chemistry

Question 1

In an exothermic reaction, increasing in temperature will result in a L shift or R shift?

Answer 1

Left shift

Question 2

If pressure is increased in a reaction, will products or reactants be favored?

Answer 2

Whichever side is less dense will increase

Question 3

If volume is increased in a reaction, will products or reactants be favored?

Answer 3

Whichever side is more dense will increase

Question 4

Bohr model equations for energy of quantum

Answer 4

E = hf

E = hc/wavelength = -13.6eV (1/n_i² - 1/n_f²)

Question 5

ground state -> excited state

Answer 5

electron can be excited to higher energy orbital if amont oof energy exactly equal to difference between 2 orbitals is transferred to electron

Question 6

Lyman series

Answer 6

n >= 2 –> n = 1

this has greatest E and therefore shortest wavelength

Question 7

Balmer series

Answer 7

n >= 3 –> n = 2

Question 8

Paschen series

Answer 8

n >= 4 –> n = 3

Question 9

mass #

Answer 9

protons + # neutrons = mass #

Question 10

atomic weight

Answer 10

weighted average of atomic / mass #’s

Question 11

atomic #

Answer 11

determined solely by # of protons

determines identity of element

Question 12

isotopes

Answer 12

elements with same atomic # (same # of protons) but varying # of neutrons

mass # of isotopes given by # after element (i.e. C-13)

Question 13

Heisenburg uncertainty principle

Answer 13

cannot simultaneously deterine perfectly both momentum and position of e-

Question 14

Pauli exclusion principle

Answer 14

no 2 electrons can have exact same set of 4 quantum #’s

Question 15

Hund’s rule

Answer 15

electrons prefer half or full-filled orbitals

Question 16

paramagnetic material

Answer 16

has unpaired e- and therefore will align with magnetic field

Question 17

diamagnetic material

Answer 17

all paired electrons

will be repelled by magnet

Question 18

max # electrons per shell

Answer 18

2n²

Question 19

max # electrons per subshell

Answer 19

4l + 2

Question 20

atomic radius increases

Answer 20

down group and down period

highest atomic radius = bottom L of periodic table

Question 21

electronegativity increases

Answer 21

up group and up period

most electronegative = top right of periodic table

Question 22

electron affinity becomes more exothermic

Answer 22

up group and up period

most exothermic = top right of periodic table

Question 23

ionization energy increases

Answer 23

up group and up period

highest ionization energy = top right of periodic table

*2nd ionization energy ALWAYS > 1st ionization energy

Question 24

acidity increases

Answer 24

down group and up period

highest acidity = bottom right of periodic table

Question 25

Fluorine periodic table trends

Answer 25

smallest atomic radius

highest ionization energy

most exothermic electron affinity

most electronegative

Question 26

formal charge rules

Answer 26

1) smallest formal charge preferred
2) less seperation between charges preferred
3) (-) charge on most electronegative atom

Question 27

formal charge equation

Answer 27

valence electrons - nonbonding - 1/2bonding

Question 28

gram equivalent weight formula

Answer 28

gram equivalent weight = (molar mass) / (# particles of interest)

Question 29

naming ions

Answer 29

fewest “O” –> hypo- ; -ite ; -ate ; per…ate <–most “O”

Question 30

Arrhenius equation and its significance

Answer 30

k = Ae^-Ea/RT

therefore, decreased activation energy and increased temperature –> increased k

Question 31

reaction rate increases when…

Answer 31

1) increased concentration
2) increased temperature therefore increased KE
3) added catalyst (this has no impact on k)

Question 32

zero-order reaction

Answer 32

rate = k[A]⁰[B]⁰ = k

only changes when temperature changes or catalyst added

Question 33

first-order reaction

Answer 33

rate = k[A] or k[B]

rate doubles when conc of reactants doubled; also changes via temp and catalyst

Question 34

second-order reaction

Answer 34

rate = k[A][B] or k[A]²

rate x 4 when reactants doubled

also changes via temp and catalyst

Question 35

law of mass action

Answer 35

k_eq = [C]^c[D]^d / [A]^a[B]^b

k_eq ONLY dependent on temperature

Question 36

determine whether reaction will continue in forward or reverse direction or if is at equilibrium

Answer 36

Q < K_eq –> forward rxn (♦G < 0)

Q = K_eq –> equilibrium

Q > K_eq –> reverse rxn (♦G > 0)

Question 37

given A(aq) + B(g) <–> C(g) + heat,

what will cause a R shift?

Answer 37

A or B added

C removed

pressure increase and volume decreased

temperature decreased

Question 38

given A(aq) + B(g) <–> C(g) + heat,

what constitutes a L shift?

Answer 38

C added

A or B removed

pressure decreased, volume increased

temperature increased