Precision quiz - Periodic Trends in Chemistry

Electron Gain Enthalpy Trend Across a Period. Identify the incorrect statement among the following.

• Electron gain enthalpy becomes more negative across a period, indicating a greater tendency to gain electrons.

• Across a period, the change in energy when an electron is added becomes increasingly exothermic due to the atom's higher effective nuclear charge.

• The electron gain enthalpy becomes less negative as one moves across a period because atoms become less willing to accept additional electrons.

Ionization Enthalpy Across a Period. Identify the incorrect statement among the following.

• Ionization enthalpy increases from left to right across a period due to stronger nuclear attraction for the valence electrons.

• Across a period, the energy required to remove an electron rises because of the increased effective nuclear charge.

• The ionization enthalpy decreases across a period as the atomic number increases, making electrons easier to remove.

Ionic Radii of Cations and Anions. Identify the incorrect statement among the following.

• Cations are smaller than their parent atoms due to the loss of electrons reducing electron-electron repulsion.

• Anions increase in size compared to their neutral atoms because added electrons increase repulsion among electrons.

• The ionic radius of a cation is larger than its neutral atom due to the addition of an electron increasing attraction to nucleus.

Stability of Half-filled and Fully-filled Orbitals. Identify the incorrect statement among the following.

• Atoms with half-filled or fully-filled orbitals exhibit higher ionization energies due to their stable electronic configurations.

• The stability associated with half-filled and fully-filled subshells results in lower ionization enthalpies for these atoms.

• Half-filled and fully-filled orbital configurations contribute to increased stability and therefore increased ionization enthalpy.

Electron Gain Enthalpy Down a Group. Identify the incorrect statement among the following.

• Down a group, electron gain enthalpy becomes less negative, reflecting the increased atomic size and decreased nuclear attraction.

• The tendency to gain electrons and release energy decreases down a group due to the greater electron-nucleus distance.

• Electron gain enthalpy increases down a group, indicating a decreased ability to gain an electron due to higher nuclear charge.

Atomic Radius Trend Across a Period. Identify the incorrect statement among the following

• The atomic radius decreases across a period due to an increase in effective nuclear charge.

• Across a period, atomic size reduces as the nucleus pulls electrons closer with increasing proton count.

• Moving across a period, the atomic radius increases as electrons are added to the same energy level.

Atomic Radius Trend Down a Group. Identify the incorrect statement among the following.

• The atomic radius increases down a group as electron shells are added.

• Down a group, atomic size expands due to the addition of electron shells increasing the distance from the nucleus.

• As one moves down a group, the atomic radius decreases because of the increasing nuclear charge.

Electronegativity Down a Group. Identify the incorrect statement among the following.

• Electronegativity decreases down a group as atoms have a reduced ability to attract shared electrons due to increased atomic size.

• Down a group, the ability of an atom to attract bonding electrons diminishes because of the increased distance between the nucleus and the valence shell.

• As one moves down a group, electronegativity increases, reflecting the increased nuclear charge's effect on the atom's ability to attract electrons.

Electronegativity Across a Period. Identify the incorrect statement among the following.

• Electronegativity increases from left to right across a period due to the atoms' increased ability to attract electrons in a bond.

• As one progresses across a period, atoms more strongly attract bonding electrons due to the increased effective nuclear charge.

• Across a period, electronegativity decreases as the increased number of protons in the nucleus less effectively attracts shared electrons.

Ionization Enthalpy Down a Group. Identify the incorrect statement among the following.

• Down a group, ionization enthalpy decreases as outer electrons are further from the nucleus and more shielded.

• The energy needed to remove an electron decreases down a group because of the increased distance of valence electrons from the nucleus.

• Ionization enthalpy increases down a group as additional electron shells reduce the effective nuclear charge on valence electrons.