Electronic structure of atoms - Concepts

Read the following statements:

I. Thermal energy
II. Electromagnetic radiation
III. High voltage sources

What energy sources can be used in order to obtain the emission line spectrum of an element?

• I and II

• II and III

• I and III

• I, II and III

Tags

NGSS.HS-PS4-3

What is the option that corresponds to the emission line spectrum in the image?

• A

• B

• C

• D

Tags

NGSS.HS-PS4-3

NGSS.HS-PS4-1

One of the uses of the emission line spectrum of a specific substance is to:

• Identify unknown substances

• Obtain the electromagnetic spectrum

• Know the energy level of the electrons

• Know the position of the electrons

Tags

NGSS.HS-PS4-3

Read the following statements:

I. The dense protonic nucleus is surrounded of electrons.

II. Electrons are revolving in concentric orbits

III. Energies of the electrons are quantized

• I and II

• II and III

• I and III

• I, II and III

How does the Rutherford-Bohr's atomic model explains the existence of the emission line spectrum and the colors of light?

• Electrons go from higher-energy orbits to lower-energy ones,

  emitting photons in the form of light.

• Electrons go from lower-energy orbits to higher-energy ones,

  emitting photons in the form of light.

• Electrons go from higher-energy orbits to lower-energy ones,

  absorbing photons in the form of light.

• Electrons go from lower-energy orbits to higher-energy ones,

  absorbing photons in the form of light.

Tags

NGSS.HS-PS4-3

What is the atom represented by the previous Bohr's atomic model?

• Si

• P

• S

• Cl

Tags

NGSS.HS-PS1-1

Read the following statements:

I. It explains the origin of the emission spectrum for Hydrogen only.

II. It is impossible to know both the position and the momentum of the electron

III. It does not specify the position of the electron in the atom.

What options correspond to deficiencies of the Bohr's atomic model?

• I and II

• I and III

• II and III

• I, II and III

In 1926, Erwin Schrödinger made the following contribution to the quantum mechanical model of the atom:

• Formulated a complicated equation that describes the

  behavior and energies of submicroscopic particles in general

• Indicated that the position and the momentum of the subatomic particles cannot be known both with certainty.

• Explained that the electron does not orbit the nucleus in a well-defined path, as Bohr thought

• Demonstrated the existence of a physical space called orbital, where the electrons are allocated in pairs

The probability of finding the electron in a certain space around the nucleus is known as:

• Schrödinger's equation

• Wavefunction

• Orbital

• Quantum numbers

What is the meaning of the azimutal quantum number?

• Orbital size and energy

• Orbital shape

• Orbital orientation

• Spin direction of the electron