Chapter 12: Problem 53
Which would you expect to be the more ductile element, (a) \(\mathrm{Ag}\) or \(\mathrm{Cr}\) (b) Zn or Ge? In each case explain your reasoning.
Short Answer
Expert verified
(a) Silver (Ag) is expected to be more ductile than Chromium (Cr) due to its higher metallic character and lower electronegativity.
(b) Zinc (Zn) is expected to be more ductile than Germanium (Ge) because of its higher metallic character and lower electronegativity.
Step by step solution
01
Understand ductility
Ductility is a property of a material that indicates its ability to be stretched into a wire without breaking. Ductile materials are usually metals, as they have a crystalline atomic structure that allows the atoms to slide past one another easily. Generally, elements with higher metallic character and lower electronegativity are more ductile.
02
Compare Ag (Silver) and Cr (Chromium)
Ag and Cr are present in the periodic table as follows:
\( \mathrm{Ag} \): Period 5, Group 11 (transition metal)
\( \mathrm{Cr} \): Period 4, Group 6 (transition metal)
Ag is one period below Cr in the periodic table, and elements in the higher periods generally have more metallic character than elements in the lower periods due to the shielding effect of inner electrons. Metals with higher metallic character are generally more ductile. Also, Ag has relatively lower electronegativity than Cr.
From these observations, we can conclude that \( \mathrm{Ag} \) (Silver) is expected to be more ductile than \( \mathrm{Cr} \) (Chromium).
03
Compare Zn (Zinc) and Ge (Germanium)
Zn and Ge are present in the periodic table as follows:
\( \mathrm{Zn} \): Period 4, Group 12 (transition metal)
\( \mathrm{Ge} \): Period 4, Group 14 (metalloid)
Zn is a transition metal, whereas Ge is a metalloid. Transition metals generally have higher metallic character than metalloids, which makes them more ductile. Additionally, Zn has lower electronegativity compared to Ge.
From these observations, we can conclude that \( \mathrm{Zn} \) (Zinc) is expected to be more ductile than \( \mathrm{Ge} \) (Germanium).
To summarize:
(a) Ag is expected to be more ductile than Cr because it has higher metallic character and lower electronegativity.
(b) Zn is expected to be more ductile than Ge because it has higher metallic character and lower electronegativity.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Metallic Character
Metals are often associated with certain properties, and one of these is their metallic character. This term refers to how easily an element can lose electrons, a property that enhances its ability as a conductor of electricity and heat. Metallic character is important because it influences other properties like ductility, which is the ability of a metal to be stretched into thin wires.
In the periodic table, elements on the left side usually exhibit strong metallic character. These are your typical metals, like sodium and magnesium. As you move across a period to the right, elements generally become less metallic. This is because their atoms have stronger nuclei, making it harder for them to lose electrons. The metallic character also increases as you move down a group in the periodic table. This is due to electron shielding, which reduces the effective nuclear charge felt by the outermost electrons, allowing them to be more easily lost.
In the periodic table, elements on the left side usually exhibit strong metallic character. These are your typical metals, like sodium and magnesium. As you move across a period to the right, elements generally become less metallic. This is because their atoms have stronger nuclei, making it harder for them to lose electrons. The metallic character also increases as you move down a group in the periodic table. This is due to electron shielding, which reduces the effective nuclear charge felt by the outermost electrons, allowing them to be more easily lost.
- More metallic character implies better ability to conduct heat and electricity.
- Higher metallic character often correlates with higher ductility.
Electronegativity
Electronegativity is a concept that describes the tendency of an atom to attract electrons in a chemical bond. This property influences an element's chemical behavior, including its reactivity and bonding characteristics. In simple terms, elements with high electronegativity, like fluorine, strongly attract electrons, while those with low electronegativity, like cesium, do not.
Low electronegativity in metals often correlates with high metallic character. This is because metals, particularly those with low electronegativity, tend to lose electrons to form positive ions. The "lower the electronegativity, the more metallic the character" idea helps explain why elements with lower electronegativity, like zinc (Zn) and silver (Ag), are more ductile as they can form metals more easily.
Low electronegativity in metals often correlates with high metallic character. This is because metals, particularly those with low electronegativity, tend to lose electrons to form positive ions. The "lower the electronegativity, the more metallic the character" idea helps explain why elements with lower electronegativity, like zinc (Zn) and silver (Ag), are more ductile as they can form metals more easily.
- High electronegativity means strong pull on shared electron pairs.
- Low electronegativity in metals correlates with higher ductility.
Transition Metals
Transition metals are a group of elements found in the middle of the periodic table, specifically in groups 3 to 12. They are known for their distinctive properties, which include the ability to form colored compounds, a variety of oxidation states, and high conductivity of electricity. What makes them stand out is their partially filled d-subshell, which contributes significantly to their unique chemical and physical properties.
One key feature of transition metals is their general ability to be ductile. This is because the metallic bonding in these elements allows for a significant degree of freedom for the atoms, enabling the metal to be shaped or drawn into wires without breaking. For example, zinc (Zn), a transition metal, is more ductile than germanium (Ge), a metalloid.
One key feature of transition metals is their general ability to be ductile. This is because the metallic bonding in these elements allows for a significant degree of freedom for the atoms, enabling the metal to be shaped or drawn into wires without breaking. For example, zinc (Zn), a transition metal, is more ductile than germanium (Ge), a metalloid.
- Transition metals have partially filled d-subshells.
- They are known for various oxidation states.
- Generally exhibit high ductility due to metallic bonding.