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Chapter 10: Problem 36

Why would you expect elements zinc, cadmium, and mercury to be in the same chemical family?

Short Answer

Expert verified
Zinc, cadmium, and mercury are all in Group 12 with two valence electrons, resulting in similar chemical properties.

Step by step solution

01

Title - Look at the periodic table groups

Find zinc (Zn), cadmium (Cd), and mercury (Hg) on the periodic table. Notice that they are all in Group 12.
02

Title - Understand the group properties

Elements in the same group of the periodic table often have similar chemical properties. This is because they have the same number of electrons in their outermost shell (valence electrons).
03

Title - Count the valence electrons

Check the electron configuration or count the valence electrons for zinc, cadmium, and mercury. Each has two electrons in their outermost shell.
04

Title - Identify chemical behavior

Having the same number of valence electrons leads to similar chemical behaviors such as forming similar compounds and having similar reactivity.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

chemical families
Chemical families, also known as groups, are columns of elements on the periodic table. These elements share similar properties because they have the same number of valence electrons. This similarity makes their behaviors in chemical reactions quite alike. For example, elements in Group 12, such as zinc, cadmium, and mercury, display similarities in their chemical properties due to their shared family traits. Understanding chemical families can help predict how different elements will react and what compounds they may form.
valence electrons
Valence electrons are the electrons located in the outermost shell of an atom. These electrons play a crucial role in chemical reactions because they are the ones that interact with other atoms. Elements with the same number of valence electrons often exhibit similar chemical behaviors. For instance, zinc, cadmium, and mercury each have two valence electrons, which is why they are grouped together in Group 12. Knowing the number of valence electrons helps in understanding an element's reactivity and the types of bonds it can form.
element properties
Element properties refer to the characteristics and behaviors of different elements. These can include things like reactivity, electronegativity, and types of bonds they can form. Elements within the same group on the periodic table often share many of these properties due to having the same number of valence electrons. For example, zinc, cadmium, and mercury all share properties such as similar reactivity with other elements, and they tend to form similar types of compounds.
Group 12 elements
Group 12 elements on the periodic table include zinc (Zn), cadmium (Cd), and mercury (Hg). These elements are also known as the zinc group. They are metals and share several common properties due to their similar electron configuration, specifically having two valence electrons. Because of these valence electrons, they each exhibit similar chemical reactivity and tend to form +2 oxidation state in their compounds. Understanding Group 12 can help predict the behavior of these metals in various chemical reactions and their potential uses in industry.

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Most popular questions from this chapter

Identify the element and draw orbital diagrams for elements with these atomic numbers: (a) 22 (b) 18 (c) 33 (d) 35 (e) 25

Look for selenium in the periodic table. (a) Write the complete electron configuration for an atom of selenium. (b) Write the shorthand electron configuration for an atom of selenium. (c) How many valence electrons does selenium have? (d) Underline the valence electrons in the shorthand electron configuration.

How many orbitals exist in the fourth principal energy level? What are they, and in what periods can they be found?

Pick the electron structures that represent elements in the same chemical family: (a) \(1 s^{2} 2 s^{1}\) (b) \(1 s^{2} 2 s^{2} 2 p^{4}\) (c) \(1 s^{2} 2 s^{2} 2 p^{2}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\) (f) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}\) (g) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\) (h) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{1}\)

Which of the elements have these electron configurations? Give both the symbol and the name: (a) \(1 s^{2} 2 s^{2} 2 p^{1}\) (b) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}\) (c) \([\mathrm{Xe}] 6 s^{2} 4 f^{14} 5 d^{10} 6 p^{2}\) (d) \([\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{4}\)
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