Answer the following questions based on the given electron...

Answer the following questions based on the given electron configurations and identify the elements. a. Arrange these atoms in order of increasing size: $[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{6} ;[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{1} ;[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{3}$ b. Arrange these atoms in order of decreasing first ionization energy: [Ne] $3 s^{2} 3 p^{5} ;[\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{3} ;[\operatorname{Ar}] 4 s^{2} 3 d^{10} 4 p^{5}$.

Answer the following questions based on the given electron configurations and identify the elements.
a. Arrange these atoms in order of increasing size:
$[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{6} ;[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{1} ;[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{3}$
b. Arrange these atoms in order of decreasing first ionization energy: [Ne] $3 s^{2} 3 p^{5} ;[\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{3} ;[\operatorname{Ar}] 4 s^{2} 3 d^{10} 4 p^{5}$.

Key Concepts

Electron Configuration

Electron configuration describes the arrangement of electrons in an atom's orbitals. It provides the basis for understanding how electrons fill available energy levels and subshells, which is crucial when predicting chemical properties and periodic behavior.

Periodic Trends

Periodic trends are recurring patterns in the properties of elements across the periodic table. Trends such as atomic size and ionization energy emerge from the systematic changes in electron configurations and nuclear charge as one moves across periods or down groups.

Atomic Size (Atomic Radius)

Atomic size refers to the distance from the nucleus to the outermost electron shell and is influenced by factors such as effective nuclear charge and electron-electron repulsion. As electrons are added and orbitals are filled, variations in atomic radius can be analyzed using these factors.

First Ionization Energy

First ionization energy is the energy required to remove the most loosely held electron from a gaseous atom. It is affected by the effective nuclear charge, atomic radius, and electron shielding, and it generally increases across a period and decreases down a group.

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom, after accounting for the shielding effect of inner electrons. It is a key factor in determining both the size of an atom and the energy required to remove an electron.

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