Ch.8 - Basic Concepts of Chemical Bonding

Problem 11a

Chapter 8, Problem 11a

(a) True or false: An element's number of valence electrons is the same as its atomic number.

Verified step by step guidance

Step 1: Understand the definition of atomic number. The atomic number of an element is the number of protons in the nucleus of an atom of that element.

Step 2: Understand the concept of valence electrons. Valence electrons are the electrons in the outermost shell of an atom that are involved in chemical bonding.

Step 3: Recognize that for main group elements, the number of valence electrons is often related to the group number in the periodic table, not the atomic number.

Step 4: Consider examples to illustrate the difference. For instance, carbon has an atomic number of 6, but it has 4 valence electrons.

Step 5: Conclude that the statement is false because the number of valence electrons is not the same as the atomic number.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Valence Electrons

Valence electrons are the electrons located in the outermost shell of an atom. They play a crucial role in chemical bonding and reactions, as they are the electrons that can be gained, lost, or shared when atoms interact. The number of valence electrons varies among elements and is determined by the group number in the periodic table.

Atomic Number

The atomic number of an element is the number of protons found in the nucleus of its atoms. It uniquely identifies an element and determines its position in the periodic table. While the atomic number also indicates the number of electrons in a neutral atom, it does not directly correspond to the number of valence electrons, which can differ based on the element's group.

Periodic Table Groups

Elements in the periodic table are organized into groups based on similar chemical properties and the number of valence electrons. For example, elements in Group 1 have one valence electron, while those in Group 2 have two. Understanding these groupings helps predict how elements will react chemically, but it is important to note that the atomic number does not equal the number of valence electrons for most elements.

Recommended video:

Guided course

05:33

Periodic Table: Group Names

Related Practice

Open Question

Fill in the blank with the appropriate numbers for both electrons and bonds (considering that single bonds are counted as one, double bonds as two, and triple bonds as three). (a) Fluorine has _ valence electrons and makes _ bond(s) in compounds. (b) Oxygen has _ valence electrons and makes _ bond(s) in compounds. (c) Nitrogen has _ valence electrons and makes _ bond(s) in compounds. (d) Carbon has _ valence electrons and makes _ bond(s) in compounds.

Textbook Question

The molecule shown here is styrene, C8H8, a benzene derivative that is used to make a number of polymers, including polystyrene. The shorthand notation for the benzene ring (described in Section 8.6) is used. Three of the carbon–carbon bonds are numbered in the structure.

a. Which of the three bonds is the strongest?

b. Which of the three bonds is the longest?

c. Which of the three bonds is best described as halfway between a single and a double bond? [Sections 8.6 and 8.8]

Textbook Question

Consider the Lewis structure for the polyatomic oxyanion shown here, where X is an element from the third period (Na - Ar). By changing the overall charge, n, from 1- to 2- to 3- we get three different polyatomic ions. For each of these ions (b) determine the formal charge of the central atom, X;

887

views

Textbook Question

(b) How many valence electrons does a nitrogen atom possess?

(a) True or false: The hydrogen atom is most stable when it has a full octet of electrons.

737

views