
(a)
Interpretation:
The explanation for the order of atomic radii in the order
Concept introduction:
Atomic radius: Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.
The atomic radius follows general trend in periodic table that it gets decreases as we move from left to right and increases from top to bottom of the table.
Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus. Effective nuclear charge increases across a period because increasing nuclear charge with no accompanying increase in shielding effect.
(b)
Interpretation:
The explanation for the increase in order of density
Concept introduction:
Density and atomic radii:
The relationship between density and atomic radii of elements is given by,

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Chapter 20 Solutions
General Chemistry: Atoms First
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- Potassium (K) blends with germanium (Ge) to form a Zintl phase with a chemical formula of K4Ge4. Which of the following elements would you expect potassium to blend with to form an alloy? Electronegativities: As (2.0), Cl (3.0), Ge (1.8), K (0.8), S (2.5), Ti (1.5) Group of answer choices Arsenic (As) Sulfur (S) Chlorine (Cl) Titanium (Ti)arrow_forwardConsider two elements, X and Z. Both have cubic-based unit cells with the same edge lengths. X has a bcc unit cell while Z has a fcc unit cell. Which of the following statements is TRUE? Group of answer choices Z has a larger density than X X has more particles in its unit cell than Z does X has a larger density than Z Z has a larger unit cell volume than Xarrow_forwardHow many particles does a face-centered cubic (fcc) unit cell contain? Group of answer choices 2 14 8 4arrow_forward
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