5.8 The Bohr Atomic Model

Select all that apply. The electronvolt

• measures large amounts of energy

• measures small amounts of energy

• is equivalent to 1.6 * 10^-19 J

• is equivalent to 1.6 * 10^-19 C

• is the amount of energy gained by an electron moving through 1 V of potential difference

If a particle has 1.344 * 10^-17 J of energy, it is the same thing as saying that it has

• 13 eV of energy

• 27 eV of energy

• 63 eV of energy

• 84 eV of energy

If a particle has 54 eV of energy, it's the same thing as saying that it has

• 8.64 * 10^-16 J of energy

• 8.64 * 10^-18 J of energy

• 3.64 * 10^-19 J of energy

• 7.13 * 10^-19 J of energy

How much energy does a ground state electron have in a hydrogen molecule?

• - 13.6 eV

• - 3.4 eV

• - 1.51 eV

• - 0.85 eV

What does it mean when an electron has a positive amount of energy?

• the electron is moving in a positive electric field

• the particle is actually a proton

• the electron is ionized and therefore bound to the atom

• the electron is ionized and therefore unbound to the atom

Calculate the energy of the n = 7 state for hydrogen.

• - 13.6 eV

• - 0.85 eV

• - 0.54 eV

• - 0.28 eV

If an electron in a hydrogen atom moves from the n = 7 to the n = 4 state, what is the wavelength of the emitted photon?

• 4.4 * 10^-6 m

• 1.5 * 10^-6 m

• 2.2 * 10^-6 m

• 8.9 * 10^-6 m

What did Rutherford's atomic model fail to explain?

• why atoms explode

• why atoms implode

• atomic structure

• why atoms are stable

How did Bohr's atomic model improve our understanding of atomic structure?

• he said that electrons orbit the nucleus in random patterns

• he said that electrons orbit the nucleus with fixed orbitals at varying energies

• he said that electrons orbit the nucleus with varying orbitals at varying energies

• he said that electrons orbit the nucleus with fixed orbitals at fixed energies

When moving in a stationary orbit, electrons

• absorb energy

• radiate energy

• do not absorb energy

• do not radiate energy