Structure S 1.3—Electron configurations - IE HL

What is the definition of first ionization energy (IE)?

• The energy released when an electron is added to a neutral atom.

• The energy needed to remove the first electron from a neutral atom.

• The energy required to remove all electrons from an atom.

• The energy needed to ionize a molecule rather than an atom.

How does the first ionization energy trend across a period in the periodic table?

• The first ionization energy increases across a period.

• The first ionization energy fluctuates randomly across a period.

• The first ionization energy decreases across a period.

• The first ionization energy remains constant across a period.

What is the trend in first ionization energy as you move down a group in the periodic table?

• The first ionization energy fluctuates unpredictably.

• The first ionization energy increases.

• The first ionization energy decreases.

• The first ionization energy remains constant.

Explain the concept of the limit of convergence in an emission spectrum.

• It describes the total number of electrons in an atom during emission.

• The limit of convergence refers to the minimum wavelength of light emitted.

• The limit of convergence in an emission spectrum is the maximum energy transition between electron states that results in photon emission.

• The limit of convergence is the point where all energy levels are equal.

How can you calculate the first ionization energy using spectral data?

• The first ionization energy is determined by the atomic mass of the element.

• Ionization energy can be calculated using the temperature of the gas phase.

• The first ionization energy can be calculated from the energy of the emitted photon during electronic transitions.

• The first ionization energy is equal to the sum of all electron affinities.

What is the relationship between frequency, wavelength, and energy in the context of ionization energy?

• Higher frequency and shorter wavelength correspond to higher energy, which is crucial for ionization energy.

• Energy is independent of frequency and wavelength in ionization.

• Lower frequency results in increased ionization energy.

• Higher wavelength leads to higher energy for ionization.

Why do metals generally have lower ionization energies compared to non-metals on the same period?

• Non-metals have lower ionization energies because they are larger in size.

• Metals have lower ionization energies due to their compact atomic structure.

• Metals easily gain electrons, which increases their ionization energy.

• Metals generally have lower ionization energies because their outer electrons are further from the nucleus and experience less effective nuclear charge.

What information can successive ionization energy data provide about an element's electron configuration?

• Successive ionization energies reveal the number of valence electrons and the electron configuration of an element.

• Successive ionization energies indicate the atomic mass of an element.

• Successive ionization energies show the element's reactivity with water.

• Ionization energy data can predict the melting point of an element.

How can you deduce the group of an element from its successive ionization energy data?

• The group can be determined by the atomic mass of the element.

• Ionization energy does not provide information about the group.

• The group of an element can be deduced by identifying large jumps in its successive ionization energies.

• The group is identified by the element's color in its natural state.

Why are log scales useful when discussing hydrogen ion concentration [H+] and ionization energies?

• Log scales help visualize large variations in hydrogen ion concentration and ionization energies.

• Log scales simplify the calculation of average ion concentrations.

• Log scales are primarily used for measuring electrical resistance.

• Log scales are only useful for temperature measurements.