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What are valence electrons? For main group elements, the number of valence electrons of an element is equal to its group number. Show that this is true for the following elements: \(\mathrm{Al}, \mathrm{Sr}, \mathrm{K}, \mathrm{Br}, \mathrm{P}, \mathrm{S}, \mathrm{C}\)

Short Answer

Expert verified
For main group elements, the number of valence electrons is equal to their group number, which matches for Al, Sr, K, Br, P, S, and C as per their group placement.

Step by step solution

01

Understand Valence Electrons

Valence electrons are the electrons in the outermost electron shell of an atom. For main group elements, these are the electrons that are involved in chemical bonding. The number of valence electrons determines the chemical properties of an element.
02

Identify Group Numbers

Locate each element in the periodic table to identify its group number. Main group elements have their valence electrons equal to the group number in the periodic table.
03

Check Valence Electrons for Each Element

- **Aluminum (Al):** Group 13, so it has 3 valence electrons. - **Strontium (Sr):** Group 2, so it has 2 valence electrons. - **Potassium (K):** Group 1, so it has 1 valence electron. - **Bromine (Br):** Group 17, so it has 7 valence electrons. - **Phosphorus (P):** Group 15, so it has 5 valence electrons. - **Sulfur (S):** Group 16, so it has 6 valence electrons. - **Carbon (C):** Group 14, so it has 4 valence electrons.

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Key Concepts

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

Main Group Elements
The term 'main group elements' refers to the s- and p-block elements on the periodic table. These elements are crucial as they include all nonmetals, alkali metals, and alkaline earth metals, among others. They range from groups 1 and 2 on the left to groups 13 through 18 on the right.
These elements play a huge role in chemical biology and industrial processes due to their varied chemical properties and readiness to form various compounds. Their valence electrons are especially easy to understand—these electrons determine how they will bond chemically, bringing us to the next topic.
Periodic Table
The periodic table is like a high school seating chart of elements, offering a wealth of information at a glance. Each column is called a group, and each row is called a period. The elements are arranged in increasing atomic number, which is the number of protons in their nucleus.
Groups in the periodic table for main group elements are labeled from 1 to 18. This arrangement helps us easily determine properties like the number of valence electrons. By simply knowing an element's position, you can gather a simple yet thorough understanding of its chemical characteristics.
Chemical Bonding
Chemical bonding is the interaction that holds atoms together for the formation of compounds. The main types of chemical bonds are ionic, covalent, and metallic bonds. Valence electrons play an essential role in the process.
In covalent bonds, atoms share valence electrons, leading to molecule formation. In ionic bonds, atoms tend to give or take electrons to achieve a full valence shell, sometimes called an 'octet'. Understanding bonding helps in predicting how and why molecules are formed, and how they interact with each other.
Group Number
Group numbers are essentially labels for the columns of the periodic table. For main group elements, the group number is equal to the number of valence electrons in a neutral atom of that element. This holds true across several groups:
  • For Group 1 elements, they have 1 valence electron.
  • For Group 14 elements like Carbon, they have 4 valence electrons.
  • For Group 17 like Bromine, they have 7 valence electrons.
This predictable pattern allows chemists to understand and predict the element's chemical properties based merely on its position on the table.
Chemical Properties
The chemical properties of an element refer to its propensity to undergo chemical changes or react with other elements. These properties are primarily determined by the number of valence electrons, which explain an element's tendency to gain, lose, or share electrons.
Knowing these properties, we can predict possible chemical reactions and understand the logical grouping of elements in the periodic table. For example, elements in Group 1 are highly reactive metals, while elements in Group 18 are noble gases, known for their lack of reactivity due to full valence shells.

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Most popular questions from this chapter

Although it is possible to determine the second, third, and higher ionization energies of an element, the same cannot usually be done with the electron affinities of an element. Explain.

The atomic radius of \(\mathrm{K}\) is \(227 \mathrm{pm}\) and that of \(\mathrm{K}^{+}\) is \(138 \mathrm{pm} .\) Calculate the percent decrease in volume that occurs when \(\mathrm{K}(g)\) is converted to \(\mathrm{K}^{+}(g) .\) (The volume of a sphere is \(\frac{4}{3} \pi r^{3}\), where \(r\) is the radius of the sphere.)

A student is given samples of three elements, \(X, Y,\) and \(\mathrm{Z}\), which could be an alkali metal, a member of Group 4A, or a member of Group 5A. She makes the following observations: Element \(\mathrm{X}\) has a metallic luster and conducts electricity. It reacts slowly with hydrochloric acid to produce hydrogen gas. Element \(Y\) is a light yellow solid that does not conduct electricity. Element \(Z\) has a metallic luster and conducts electricity. When exposed to air, it slowly forms a white powder. A solution of the white powder in water is basic. What can you conclude about the elements from these observations?

$$ \begin{aligned} &\text { Explain which of the following cations is larger, and }\\\ &\text { why: } \mathrm{Cu}^{+} \text {or } \mathrm{Cu}^{2+} \end{aligned} $$

As discussed in the chapter, the atomic mass of argon is greater than that of potassium. This observation created a problem in the early development of the periodic table because it meant that argon should be placed after potassium. (a) How was this difficulty resolved? (b) From the following data, calculate the average atomic masses of argon and potassium: Ar-36 (35.9675 amu, 0.337 percent), \(\mathrm{Ar}-38(37.9627 \mathrm{amu}, 0.063\) percent \()\) Ar- \(40(39.9624\) amu, 99.60 percent), \(\mathrm{K}-39(38.9637\) amu, 93.258 percent \(), \mathrm{K}-40(39.9640 \mathrm{amu}, 0.0117\) percent \()\) K-41 \((40.9618\) amu, 6.730 percent).

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