The image presents a diagram illustrating chemical bonding concepts, focusing on both ionic and covalent bonds.### Diagram Explanation:- **Na^+ Cl^-**: Represents an ionic bond. Sodium (Na) loses an electron to become positively charged (Na^+), and chlorine (Cl) gains an electron to become negatively charged (Cl^-). - **N≡N**: Depicts a triple covalent bond between two nitrogen atoms. The sharing of three pairs of electrons forms this strong covalent bond.### Multiple Choice Question:The question asks which parts of the model are best suited for predicting bond types based on the diagram.#### Options:1. **Part A and C**: It indicates charged particles from transferring electrons, suggesting an ionic bond.2. **Part B and D**: It describes a triple bond forming an ionic compound (Note: this is incorrect as triple bonds are covalent).3. **Part A and C**: Shows sharing of electrons creating an anion and cation (Note: slightly misleading, sharing characterizes covalent bonds, not ionic which involves electron transfer).4. **Part B and D**: Describes lone pairs leading to ionic bonding (Note: incorrect as lone pairs in the context of the nitrogen molecule relate to covalent bonding).Option 1 correctly describes ionic bonding characteristics. **Understanding the Lewis Model of Bonding**A student is using the Lewis model of bonding to determine ways to predict bond types from Lewis structures.**Diagram Explanation:**The diagram shows two parts:1. **Na⁺ Cl⁻ Structure:** - Sodium (Na) carries a positive charge. - Chlorine (Cl) carries a negative charge. - Dots around Cl represent electrons. - This illustrates an ionic bond, where electrons are transferred from Na to Cl.2. **N≡N Structure:** - Two nitrogen atoms are connected by a triple bond (three lines). - This shows a covalent bond, where electrons are shared.**Question:**Which of the following parts of the model are best suited for predicting bond types shown above?- **Options:** - ○ Part A and C, because it is showing charged particles from transferring electrons and therefore ionic. - ○ Part B and D, because it is describing a triple bond existing and therefore forming an ionic compound. - ○ Part A and C, because it is showing a sharing of the electrons by making an anion and cation.**Explanation:**- Part A and C are indicative of ionic bonding due to the transfer of electrons, resulting in charged particles (Na⁺ and Cl⁻).- Part B and D illustrate a covalent bond through the sharing of electrons in a triple bond (N≡N).This educational content helps students understand the distinction between ionic and covalent bonds using Lewis structures.

Which of the following parts of the model are best suited for predicting bond types shown above? Part A and C, because it is showing charged particles from transferring electrons and therefore ionic. O Part B and D, because it is describing a triple bond exist and therefore forming an ionic compound. Part A and C, because it is showing a sharing of the electrons by making an anion and cation. Part B and D, because it is describing the lone pairs of electrons on the atoms and therefore make the atoms bond ionically due to an unequal sharing of electrons.

Which of the following parts of the model are best suited for predicting bond types shown above? Part A and C, because it is showing charged particles from transferring electrons and therefore ionic. O Part B and D, because it is describing a triple bond exist and therefore forming an ionic compound. Part A and C, because it is showing a sharing of the electrons by making an anion and cation. Part B and D, because it is describing the lone pairs of electrons on the atoms and therefore make the atoms bond ionically due to an unequal sharing of electrons.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Formal Charges

Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.

Polarity Of Water

In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.

Valence Bond Theory Vbt

Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Question

100%

The image presents a diagram illustrating chemical bonding concepts, focusing on both ionic and covalent bonds.

### Diagram Explanation:

- **Na^+ Cl^-**: Represents an ionic bond. Sodium (Na) loses an electron to become positively charged (Na^+), and chlorine (Cl) gains an electron to become negatively charged (Cl^-).

- **N≡N**: Depicts a triple covalent bond between two nitrogen atoms. The sharing of three pairs of electrons forms this strong covalent bond.

### Multiple Choice Question:

The question asks which parts of the model are best suited for predicting bond types based on the diagram.

#### Options:

1. **Part A and C**: It indicates charged particles from transferring electrons, suggesting an ionic bond.
2. **Part B and D**: It describes a triple bond forming an ionic compound (Note: this is incorrect as triple bonds are covalent).
3. **Part A and C**: Shows sharing of electrons creating an anion and cation (Note: slightly misleading, sharing characterizes covalent bonds, not ionic which involves electron transfer).
4. **Part B and D**: Describes lone pairs leading to ionic bonding (Note: incorrect as lone pairs in the context of the nitrogen molecule relate to covalent bonding).

Option 1 correctly describes ionic bonding characteristics.

**Understanding the Lewis Model of Bonding**

A student is using the Lewis model of bonding to determine ways to predict bond types from Lewis structures.

**Diagram Explanation:**

The diagram shows two parts:
1. **Na⁺ Cl⁻ Structure:**
- Sodium (Na) carries a positive charge.
- Chlorine (Cl) carries a negative charge.
- Dots around Cl represent electrons.
- This illustrates an ionic bond, where electrons are transferred from Na to Cl.

2. **N≡N Structure:**
- Two nitrogen atoms are connected by a triple bond (three lines).
- This shows a covalent bond, where electrons are shared.

**Question:**

Which of the following parts of the model are best suited for predicting bond types shown above?

- **Options:**
- ○ Part A and C, because it is showing charged particles from transferring electrons and therefore ionic.
- ○ Part B and D, because it is describing a triple bond existing and therefore forming an ionic compound.
- ○ Part A and C, because it is showing a sharing of the electrons by making an anion and cation.

**Explanation:**

- Part A and C are indicative of ionic bonding due to the transfer of electrons, resulting in charged particles (Na⁺ and Cl⁻).
- Part B and D illustrate a covalent bond through the sharing of electrons in a triple bond (N≡N).

This educational content helps students understand the distinction between ionic and covalent bonds using Lewis structures.

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