4. classification of elements quiz II

K⁺, Ar, Cl⁻, and S²⁻ are

Classifying species with 18 electrons

Isotopes

Isoelectronic

Isomers

Isobars

Why is the ionic radius of a sulfide ion larger than the ionic radius of a potassium ion?

Comparing ionic radii of isoelectronic ions

The ionic radius always decreases with increasing atomic number

Positive ions always have smaller radii than negative ions

The potassium ion has more protons in its nucleus than the sulfide ion

The sulfide ion is doubly charged; the potassium ion is singly charged

Which among the following is NOT an isoelectronic species with the group N³⁻, O²⁻, F⁻, Ne⁺, Mg²⁺, Al³⁺, Cl⁷⁺?

Identifying non-isoelectronic species

Cl⁷⁺

Mg²⁺

O²⁻

Ne⁺

Which among the following is true for isoelectronic ions?

Definition of isoelectronic species

Have same number of protons

Have same number of electrons

Have same number of neutrons

All of them

Slater's rules are used to calculate

Application of Slater's rules

Atomic radius

Effective nuclear charge

Electronegativity

Electron affinity

Which of the following oxides of nitrogen is isoelectronic with CO₂?

Isoelectronic molecules with CO₂

NO₂

N₂O

NO

N₂O₂

Which one of the following sets of ions represents a collection of isoelectronic species?

Identifying isoelectronic sets

N³⁻, O²⁻, F⁻, S²⁻

K⁺, Cl⁻, Ca²⁺, Sc³⁺

Li⁺, Na⁺, Mg²⁺, Ca²⁺

Ba²⁺, Sr²⁺, K⁺, Ca²⁺

Which of the following best describes the correct order of oxygen, fluorine, and nitrogen's atomic radii?

Comparing atomic radii of N, O, F

O < F < N

N < F < O

F < O < N

O < N < F