All elements either emit or absorb certain frequencies of light. Evidence from atomic line spectra supports the Bohr model of the atom using photon frequency calculations.
A line emission spectrum has lines of individual frequencies - what is their significance?
Different elements can have different colours depending on the number of electrons in the atom
Different frequencies of light do travel at the same speed but this has no relevance to line spectra or relativity
There are individual energy levels around the atom which electrons can occupy
What is the relationship between the line spectrum frequency and the energy level?
E = hf where E is the highest energy level
E2 – E1= hf Where E2 – E1 is the energy change between upper and lower energy levels
E = hf where E is the lowest energy level
Which diagram shows the correct labeling of energy levels within an atom?
Sunlight has certain frequencies missing from the full continuous spectrum shown by white light - what is the reason for these missing frequencies?
The sun does not contain elements responsible for the emission of these frequencies
The sun’s atmosphere has elements that absorb the frequencies
The frequencies are missing due to redshift of radiation of the sun
If the absorption spectrum for an element is compared to the emission spectrum which of the statements is correct?
There are lines in the emission spectrum which match to other elements
The gaps in the absorption spectrum match to lines in the emission spectrum
The emission and absorption spectra are identical
How is an absorption spectrum formed?
Photons from a continuous spectrum causing electrons to be promoted to upper energy levels
Electrons from upper energy levels taking the energy from photons
Photons from a continuous spectrum changing their frequency to other photons
What is the number of lines in an emission spectrum due to electron transitions between three excited energy levels and a ground state?