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Chapter 5: Problem 55

Write the valence electron configuration for each of the following: a. alkali metals b. Group 4A (14) c. Group \(7 \mathrm{~A}(17)\) d. Group \(5 \mathrm{~A}(15)\)

Short Answer

Expert verified
Alkali metals: 1 valence electron; Group 4A: 4 valence electrons; Group 7A: 7 valence electrons; Group 5A: 5 valence electrons.

Step by step solution

01

Understand the Periodic Table Groups

Familiarize yourself with the periodic table groups. Alkali metals are in Group 1, Group 4A (14) consists of elements starting with Carbon, Group 7A (17) contains halogens, and Group 5A (15) has elements starting with Nitrogen.
02

Identify Valence Electrons for Alkali Metals (Group 1)

Alkali metals have one valence electron. For example, the configuration for Sodium (Na) is [Ne]3s鹿.
03

Identify Valence Electrons for Group 4A (14)

Elements in Group 4A have four valence electrons. For instance, Carbon (C) has the configuration 2s虏2p虏, and Silicon (Si) has the configuration [Ne]3s虏3p虏.
04

Identify Valence Electrons for Group 7A (17)

Group 7A elements have seven valence electrons. For example, Chlorine (Cl) has the configuration [Ne]3s虏3p鈦�.
05

Identify Valence Electrons for Group 5A (15)

Group 5A elements have five valence electrons. Nitrogen (N), for instance, has the configuration 2s虏2p鲁, and Phosphorus (P) has the configuration [Ne]3s虏3p鲁.

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Key Concepts

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

alkali metals
Alkali metals are a group of elements in Group 1 of the periodic table. They include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). These elements are characterized by having a single valence electron in their outermost electron shell.

For example:
  • Lithium (Li): 1s虏2s鹿
  • Sodium (Na): [Ne]3s鹿
  • Potassium (K): [Ar]4s鹿
The presence of one valence electron makes alkali metals highly reactive, especially with water. This also gives them their characteristic properties, such as being soft and having low melting points.
Group 4A elements
Group 4A elements, also known as Group 14 elements, include carbon (C), silicon (Si), germanium (Ge), tin (Sn), and lead (Pb). These elements have four valence electrons.

For example:
  • Carbon (C): 2s虏2p虏
  • Silicon (Si): [Ne]3s虏3p虏
  • Germanium (Ge): [Ar]3d鹿鈦�4s虏4p虏
The four valence electrons make these elements versatile in forming covalent bonds, and they play a crucial role in organic chemistry and semiconductor technology.
Group 7A elements
Group 7A elements, also known as Group 17 elements or halogens, include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). These elements have seven valence electrons.

For example:
  • Fluorine (F): 2s虏2p鈦�
  • Chlorine (Cl): [Ne]3s虏3p鈦�
  • Bromine (Br): [Ar]3d鹿鈦�4s虏4p鈦�
With seven valence electrons, halogens are extremely reactive and readily form compounds by gaining one electron to achieve a stable octet configuration.
Group 5A elements
Group 5A elements, also known as Group 15 elements, include nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). These elements have five valence electrons.

For example:
  • Nitrogen (N): 2s虏2p鲁
  • Phosphorus (P): [Ne]3s虏3p鲁
  • Arsenic (As): [Ar]3d鹿鈦�4s虏4p鲁
The five valence electrons allow these elements to form three covalent bonds with other atoms, making them essential in various biological processes and industrial applications.
periodic table groups
The periodic table groups are vertical columns in the periodic table of elements. Each group contains elements with similar chemical properties due to their similar valence electron configurations.

Some key groups include:
  • Group 1: Alkali metals
  • Group 2: Alkaline earth metals
  • Group 14: Group 4A elements
  • Group 17: Group 7A elements
  • Group 15: Group 5A elements
Understanding the groups helps predict the chemical behavior and reactivity of the elements.
valence electrons
Valence electrons are the outermost electrons in an atom and are primarily responsible for an element's chemical properties. These electrons participate in forming chemical bonds.

Key points about valence electrons:
  • They determine the reactivity of an element.
  • Elements in the same group have the same number of valence electrons.
  • The number of valence electrons can often be deduced from an element's group number.
For example, alkali metals (Group 1) have 1 valence electron, while the elements in Group 7A have 7 valence electrons.
electron configuration examples
Electron configuration is a way to represent the arrangement of electrons in an atom. It describes the orbitals in which electrons reside.

Here are some examples:
  • Lithium (Li): 1s虏2s鹿
  • Sodium (Na): [Ne]3s鹿
  • Carbon (C): 2s虏2p虏
  • Chlorine (Cl): [Ne]3s虏3p鈦�
  • Nitrogen (N): 2s虏2p鲁
These configurations help understand the chemical behavior and reactivity of elements, especially their valence electrons which are crucial for forming chemical bonds.

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Most popular questions from this chapter

Place the following types of electromagnetic radiation in order of increasing wavelengths: the blue color in a rainbow, X-rays, and microwaves from an oven.

a. How many \(3 d\) electrons are in Fe? (5.4) b. How many \(5 p\) electrons are in Ba? c. How many \(4 d\) electrons are in I? d. How many \(7 s\) electrons are in Ra?

Match the following with \(s\) or \(p\) orbitals: \((5.3)\) a. two lobes b. spherical shape c. found in \(n=1\) d. found in \(n=3\)

Write the complete electron configuration for each of the following: a. nitrogen b. chlorine c. strontium d. neon

Write the group number using both \(\mathrm{A} / \mathrm{B}\) and 1 to 18 notations for elements that have the following outer electron configuration: a. \(2 s^{2}\) b. \(3 s^{2} 3 p^{3}\) c. \(4 s^{2} 3 d^{5}\) d. \(5 s^{2} 4 d^{10} 5 p^{4}\)
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