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Chapter 12: Problem 55

Arrange the following metals in increasing order of expected melting point: Mo, Zr, Y, Nb. Explain this trend in melting points.

Short Answer

Expert verified
The order of metals in increasing expected melting point is: Yttrium (Y), Zirconium (Zr), Niobium (Nb), and Molybdenum (Mo). This trend is due to the decreasing atomic size and increasing metallic bonding strength as we move across the periodic table from group 3 to group 6.

Step by step solution

01

Identify the selected metals' atomic number and group

First, find the atomic number and group of each metal from the periodic table. The atomic number increases across a period (row) and down a group (column). The information for each metal is as follows: - Molybdenum (Mo): Atomic number 42, Group 6 - Zirconium (Zr): Atomic number 40, Group 4 - Yttrium (Y): Atomic number 39, Group 3 - Niobium (Nb): Atomic number 41, Group 5
02

Analyze the impact of atomic size on melting point

As we move across a period in the periodic table, the atomic size generally decreases due to the increasing number of protons in the nucleus, causing a stronger electrostatic attraction between protons and electrons. As a result, the metallic bonding strength increases, leading to higher melting points. The atomic size trend across a period (from group 3 to group 6) is: Y (largest) > Zr > Nb > Mo (smallest).
03

Analyze the impact of metallic bonding strength on melting points

Metallic bonding strength depends on the number of valence electrons available for delocalization, as these electrons form a "sea of electrons" that result in strong metallic bonds. A higher number of valence electrons leads to stronger metallic bonds and hence, higher melting points. The number of valence electrons for each metal are: - Yttrium (Y): 3 valence electrons - Zirconium (Zr): 4 valence electrons - Niobium (Nb): 5 valence electrons - Molybdenum (Mo): 6 valence electrons The trend in metallic bonding strength based on the number of valence electrons is: Y (weakest) < Zr < Nb < Mo (strongest).
04

Combine the factors and arrange the metals in increasing order of expected melting points

Based on the trends identified in steps 2 and 3: - Atomic size (with larger size leading to lower melting points): Y > Zr > Nb > Mo - Metallic bonding strength (with stronger bonding leading to higher melting points): Y < Zr < Nb < Mo Considering both factors and their impact on melting points: Y (largest atomic size, weakest metallic bonding) < Zr < Nb < Mo (smallest atomic size, strongest metallic bonding). Hence, the order of metals in increasing expected melting point is: Yttrium (Y), Zirconium (Zr), Niobium (Nb), and Molybdenum (Mo).

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