Line spectrum of atomic hydrogen

For an electron to change from ground state to an excited stated it must...

• Absorb energy
• Release energy

Line emission spectrum shown below happens when

• Electron transition from lower to higher energy level.
• Electron transition from higher to lower energy level.
• Electron exist in fixed energy states
• Electron transition between different energy levels.

The parallel lines represents...

• energy levels of the atom
• energy levels of the electrons
• energy levels of the photons
• energy levels of the nucleus

If an electron moves from n=4 to n=2 it ____

• absorbs energy

• releases energy

A certain photon of light has a wavelength of 4.22x10^-7nm. What is the frequency? (v=c/λ)

• 7.11x10¹⁴ Hz
• 7.11Hz
• 1.41x10^-15
• -1.41x10¹⁵

What is a photon?

• When radiation burst through electric waves
• The emission of electrons from a metal caused by light striking the metal
• The rate at which a waves energy flows through a given unit of area.
• packets of electromagnetic energy

Certain blue lights have a frequencey of 6.91x10¹⁴Hz. What is the wavelength? (λ=c/v)

• 4.34x10²¹
• 4.34x10^-21
• 4.34x10^-7
• 2.07x10²³

How many lines are formed when electron undergoes transition from excited state n= 7 to ground state n= 1 in Lyman Series

• 4

• 5

• 6

• 7

Choose the correct line spectrum formed when electron falls down from n=5 to n =3

• 1

• 2

• 3

• 4

Lyman series is formed when electrons fall from higher energy levels to _______.

• n = 1
• n = 2
• n = 3
• n = 4