Lecture 2

Question 1

human contribution to global warming

Answer 1

global warming by approximately 1 degree is caused by human made carbon dioxide

Question 2

lag in GHG emission

Answer 2

if GHG emissions were ceased, there would still be an increase in global warming bc there’s a lag between the GHG levels and the eventual temperature

Question 3

albedo effect

Answer 3

warming due to more dark soil, rocks, etc. exposed when ice is melting (there is less sunlight reflected)

Question 4

permafrost deposits of methane

Answer 4

warming due to the release of methane from clathrates when ice is melting (methane is trapped in ice lattices)

Question 5

carbon dioxide in oceans

Answer 5

warming due to the release of trapped GHG when oceans are warmed up

Question 6

inorganic chemistry’s affect on GHG

Answer 6

promote reactions that will use up carbon dioxide

Question 7

solar fuels

Answer 7

• produced when carbon dioxide is reacted with water, catalyzed by energy (sunlight)
• burning solar fuels does not add new carbon dioxide to the environment
• must be stored

Question 8

electron duality

Answer 8

behaves as both a particle and wave

Question 9

de Broglie wavelength

Answer 9

wavelength calculated by Planck’s constant over momentum

Question 10

photoelectron effect

Answer 10

• no electrons were emitted unless the threshold was reached

- intensity of light did not emit electrons below energy threshold, only when the light energy was above threshold level

Question 11

Heisenberg’s Uncertainty Principle

Answer 11

• the more precise a position is known, the less precise a momentum is known and vice versa
• uncertainty in position x uncertainty in momentum > Planck’s constant / 4*pi
• cannot know the precise position and momentum of a particle at the same time

Question 12

Schrodinger Equation

Answer 12

• described the energy of electrons as waves, denoted as wavefunction (psi)
• Hamiltonian operator (eigenfunction) x psi = energy of the electron x psi
• eigenfunction gives the energy of an electron in a H atom
• E is the energy
• psi can be treated mathematically to give shapes, phases, and nodes of an electron wave in an atom

Question 13

theories that formed the Schrodinger Equation

Answer 13

• took 3 months to formulate
• light was a solid beam; and
• light was a wave
• led to the equation

Question 14

integral of psi^2

Answer 14

• probability of finding the electron in a certain region of space defined by the integral limits
• integral of the overall space should equal 1

Question 15

shape of an orbital

Answer 15

• defined by the probability over space (integral of psi^2)

Question 16

orbital

Answer 16

• shape of region with highest probability of finding the elecron wave
• shape of stable wavefunction for an electron atom
• if an electron has a wavelength, the shape of the orbital represents a whole number of wavelengths, like a standing wave

Question 17

wavefunction

Answer 17

• a whole number of wavelengths
• a standing wave without destructive interference
• electrons of a given wavelength will have one stable shape

Question 18

Schrodinger Equation drawbacks

Answer 18

• only gives precise solutions for single electron systems

Question 19

polyelectron system

Answer 19

• polyelectron systems have electrons that are attracted to the nucleus, while also exhibiting repulsion against other electrons
• both electrons are moving, therefore there is no precise mathematical equation
• can be approximated because they behave like hydrogen atoms; approximations are good
• precise solution for helium DNE but it does for He+

Question 20

polar coordinates

Answer 20

• most convenient way to represent wavefunction
• r is the radius, the distance from the nucleus
• depends on the principal quantum number, n
• n = 0, 1, 2, 3…
• theta is the angle from perpendicular axis
• depends on the angular momentum quantum number, l
• l = n-1
• phi is the angle from one axis
• depends on the magnetic quantum number, ml
• ml = -l, …, 0, …, +l

Question 21

angular momentum quantum number of s orbitals

Answer 21

• n = 1

- l = 0

Question 22

angular momentum quantum number of p orbitals

Answer 22

• n = 2

- l = 1

Question 23

angular momentum quantum number of d orbitals

Answer 23

• n = 3

- l = 2