Lecture 9

Question 1

Electro magnetic spectrum from low to high energy

Answer 1

Radio, microwave, infrared, visible, ultraviolet, x-ray, gamma

Question 2

Spectral lines

Answer 2

Lines caused by electronic process (electrons) and not nuclear process

Question 3

Rydberg equation

Answer 3

1/λ = R((1/nf^2) - (1/ni^2))

Question 4

Emission vs absorption of photon

Answer 4

Emission: nf<ni
Absorption: nf>ni

Question 5

Bohr model

Answer 5

Flat circles.
Uses Bohr orbits to describe physical motion and positions of electrons.
It fails to explain the various characteristics of atoms and atom behavior,including bonding and periodicity

Question 6

Atom changes to another stationary state

Answer 6

By absorbing or admitting a photon

Question 7

When the electron is in any orbit higher than n= 1…

Answer 7

The atom is in an excited state

Question 8

Bohr equation

Answer 8

ΔE = (-2.18X10^18) * ((1/nf^2) - (1/ni^2))

Question 9

1J =

Answer 9

= (kg * m^2) / s^2

Question 10

h =

Answer 10

= 6.626X10^-34

Question 11

Bohr constant

Answer 11

-2.18X10^-18

Question 12

Rhydberg constant

Answer 12

1.09677X10^7