Chapter 5, Problem 5.88EP

Successive substitution of F atoms for H atoms in the molecule NH₃ produces the molecules NH₂F, NHF₂, and NF₃.

1. a. Draw Lewis structures for each of the four molecules.
2. b. Using VSEPR theory, predict the geometry of each of the four molecules.
3. c. Specify the polarity (polar or nonpolar) for each of the four molecules.

Interpretation Introduction

Interpretation:

Lewis structures for the four molecules that are formed by successive substitution of $\text{F}$ atom instead of $\text{H}$ atom in ${\text{NH}}_{\text{3}}$ has to be drawn.

Concept Introduction:

Lewis structure clearly depicts the bonding and nonbonding electrons in the atom.  This is only partially useful for the molecule that contains one or more multiple bonds and when coordinate covalent bond is present in the molecule.  For drawing Lewis structure a systematic procedure is followed.  They are,

• The total number of valence electrons that is present in molecule is calculated by adding all the valence electrons of the atoms present in the molecule.
• The chemical symbols for the atoms that is present in the molecule is written in the order that they are bonded.  After this a single covalent bond is placed between each atoms as two electrons.
• The nonbonding electrons are added to each atom that is bonded to the central atom so that it contains octet of electrons.  For hydrogen alone the “octet” is only two electrons.
• The remaining electrons has to be placed on the central atom in the structure.
• If there is no octet of electrons present in the central atom, then use one or more pairs of nonbonding electrons that is bonded to the central atom to form double or triple bonds.
• The total number of electrons has to be counted and it has to be confirmed whether the count is same as that of the number of valence electrons that is available for bonding.

Explanation of Solution

Given molecules are ${\text{NH}}_{\text{3}}{\text{F, NHF}}_{\text{2}}{\text{, NF}}_{\text{3}}{\text{, and NH}}_{\text{3}}$.

For ${\text{NH}}_{\text{3}}$:

Given molecule is ${\text{NH}}_{\text{3}}$.  Nitrogen belongs to Group VA and it contains four valence electrons.  Hydrogen belongs to Group IA and it contains only one valence electron.  The total number of valence electrons present in ${\text{NH}}_{\text{3}}$ molecule is 8.  These atoms are written order they are bonded.  After the atomic symbol is written, two dots are placed between two atoms and this means a single covalent bond is present.  This can be given as,

The nonbonding electrons are added to the nitrogen atom.  This results in the structure as,

All the atoms present in the above structure contains octet of electrons.  The total number of electron dots present in the above structure is 8 and it is same as the valence electrons of ${\text{NH}}_{\text{3}}$ molecule.  The Lewis structure for ${\text{NH}}_{\text{3}}$ is drawn as,

For ${\text{NH}}_{\text{2}}\text{F}$:

Given molecule is ${\text{NH}}_{\text{2}}\text{F}$.  Nitrogen belongs to Group VA and it contains four valence electrons.  Hydrogen belongs to Group IA and it contains only one valence electron.  Fluorine belongs to Group VIIA and it contains seven valence electrons.  The total number of valence electrons present in ${\text{NH}}_{\text{2}}\text{F}$ molecule is 14.  These atoms are written order they are bonded.  After the atomic symbol is written, two dots are placed between two atoms and this means a single covalent bond is present.  This can be given as,

The nonbonding electrons are added to the fluorine atom and nitrogen atom.  This results in the structure as,

All the atoms present in the above structure contains octet of electrons.  The total number of electron dots present in the above structure is 14 and it is same as the valence electrons of ${\text{NH}}_{\text{2}}\text{F}$ molecule.  The Lewis structure for ${\text{NH}}_{\text{2}}\text{F}$ is drawn as,

For ${\text{NHF}}_{\text{2}}$:

Given molecule is ${\text{NHF}}_{\text{2}}$.  Nitrogen belongs to Group VA and it contains four valence electrons.  Hydrogen belongs to Group IA and it contains only one valence electron.  Fluorine belongs to Group VIIA and it contains seven valence electrons.  The total number of valence electrons present in ${\text{NHF}}_{\text{2}}$ molecule is 20.  These atoms are written order they are bonded.  After the atomic symbol is written, two dots are placed between two atoms and this means a single covalent bond is present.  This can be given as,

The nonbonding electrons are added to the fluorine atom and nitrogen atom.  This results in the structure as,

All the atoms present in the above structure contains octet of electrons.  The total number of electron dots present in the above structure is 20 and it is same as the valence electrons of ${\text{NHF}}_{\text{2}}$ molecule.  The Lewis structure for ${\text{NHF}}_{\text{2}}$ is drawn as,

For ${\text{NF}}_{\text{3}}$:

Given molecule is ${\text{NF}}_{\text{3}}$.  Nitrogen belongs to Group VA and it contains four valence electrons.  Fluorine belongs to Group VIIA and it contains seven valence electrons.  The total number of valence electrons present in ${\text{NF}}_{\text{3}}$ molecule is 26.  These atoms are written order they are bonded.  After the atomic symbol is written, two dots are placed between two atoms and this means a single covalent bond is present.  This can be given as,

The nonbonding electrons are added to the nitrogen atom and fluorine atoms.  This results in the structure as,

All the atoms present in the above structure contains octet of electrons.  The total number of electron dots present in the above structure is 26 and it is same as the valence electrons of ${\text{NF}}_{\text{3}}$ molecule.  The Lewis structure for ${\text{NF}}_{\text{3}}$ is drawn as,

Interpretation Introduction

Interpretation:

Molecule geometry has to be predicted for the four molecules using VSEPR theory.

Concept Introduction:

Information about the number of bonds and types of bonds can be obtained from Lewis structure but the molecular geometry cannot be obtained.  Three dimensional arrangement of atoms in a molecule can be given by molecular geometry.  Physical and chemical properties are determined by the molecular geometry of the molecule.

Using VSEPR theory and Lewis structure, the molecular geometry of the molecule that contain less number of atoms can be predicted.  VSEPR theory uses the information from Lewis structure of the molecule to predict the molecular geometry of the molecule.  Main concept of VSEPR theory is that electron pairs that are present in the valence shell adopt arrangement in a way that minimize the repulsion between like charges.

If the central atom contains two electron pairs, then it has to be far apart means, it has to be on opposite side of the nucleus.  This means the angle has to be $180°$ between them.  This type of arrangement for electron pair result in linear.

If the central atom contains three electron pairs, then it has to be far apart means, it has to be on corner of a triangle.  This means the angle has to be $120°$ between them.  This type of arrangement for electron pair result in trigonal planar.

If the central atom contains four electron pairs, then it has to be far apart means, it has to be in a tetrahedral arrangement.  This means the angle has to be $109°$ between them.  This type of arrangement for electron pair result in tetrahedral.

The collection of valence electron that is present in localized region about central atom in a molecule is known as VSEPR electron group.  This may contain two electrons, four electrons, or six electrons.  The electron group that contain four and six electrons repel each other.

Tetrahedral VSEPR electron group:

The four electron pairs can be of three VSEPR electron groups.  They are 4 bonding electron groups, 3 bonding and 1 nonbonding electron groups, and 2 bonding and 2 nonbonding electron groups.  The molecular geometry that is associated with 4 bonding electron groups is tetrahedral.  The molecular geometry that is associated with 3 bonding and 1 nonbonding electron groups is trigonal pyramidal.  The molecular geometry that is associated with 2 bonding and 2 nonbonding electron groups is angular.

Trigonal planar VSEPR electron group:

The three electron pairs can be of two VSEPR electron groups.  They are 3 bonding electron groups, and 2 bonding and 1 nonbonding electron groups.  The molecular geometry that is associated with 3 bonding electron groups is trigonal planar.  The molecular geometry that is associated with 2 bonding and 1 nonbonding electron groups is angular.

Linear VSEPR electron group:

The two electron pairs can be of only one VSEPR electron groups.  It is only 2 bonding electron groups and the geometry associated with it is linear geometry.

Explanation of Solution

Given molecule is ${\text{NH}}_{\text{3}}$.  Lewis structure of ${\text{NH}}_{\text{3}}$ can be given as,

The central atom in the above molecule is found to be nitrogen.  This has three bonding electron groups and one nonbonding electron groups.  The arrangement around the central atom is trigonal pyramidal.  Looking for molecular geometry, the central atom that contains three bonding electron groups and one nonbonding electron groups and it has trigonal pyramidal geometry as per VSEPR theory.

Given molecule is ${\text{NH}}_{\text{2}}\text{F}$.  Lewis structure of ${\text{NH}}_{\text{2}}\text{F}$ can be given as,

The central atom in the above molecule is found to be nitrogen.  This has three bonding electron groups and one nonbonding electron groups.  The arrangement around the central atom is trigonal pyramidal.  Looking for molecular geometry, the central atom that contains three bonding electron groups and one nonbonding electron groups and it has trigonal pyramidal geometry as per VSEPR theory.

Given molecule is ${\text{NHF}}_{\text{2}}$.  Lewis structure of ${\text{NHF}}_{\text{2}}$ can be given as,

The central atom in the above molecule is found to be nitrogen.  This has three bonding electron groups and one nonbonding electron groups.  The arrangement around the central atom is trigonal pyramidal.  Looking for molecular geometry, the central atom that contains three bonding electron groups and one nonbonding electron groups and it has trigonal pyramidal geometry as per VSEPR theory.

Given molecule is ${\text{NF}}_{\text{3}}$.  Lewis structure of ${\text{NF}}_{\text{3}}$ can be given as,

The central atom in the above molecule is found to be nitrogen.  This has three bonding electron groups and one nonbonding electron groups.  The arrangement around the central atom is trigonal pyramidal.  Looking for molecular geometry, the central atom that contains three bonding electron groups and one nonbonding electron groups and it has trigonal pyramidal geometry as per VSEPR theory.

Interpretation Introduction

Interpretation:

The four molecules that are given has to be classified as polar and nonpolar.

Concept Introduction:

Measure of the degree of inequality in attraction of the bonding electrons to the various locations present within a molecule is known as molecular polarity.  This can also be said in terms of electron attraction and that is in a molecule one part is favored than the other parts of the molecule.

If in a molecule there is an uneven distribution of electronic charges means it is known as polar molecule.  If there is a symmetrical distribution of electron charge over the molecule means it is known as nonpolar molecule.  Two factors that decide molecular polarity is bond polarity and geometry of molecule.  If a molecule is symmetrical means then there won’t be any molecular polarity because the effect given by the polar bonds may cancel out each other.

The polarity of the bonds, arrangement of the bonds determines the degree of molecular polarity.  If the electronegativity difference is more, then the molecule will be more polar.

Explanation of Solution

Given molecules are ${\text{NH}}_{\text{3}}{\text{F, NHF}}_{\text{2}}{\text{, NF}}_{\text{3}}{\text{, and NH}}_{\text{3}}$.  Molecular geometry of ${\text{NH}}_{\text{3}}{\text{F, NHF}}_{\text{2}}{\text{, NF}}_{\text{3}}{\text{, and NH}}_{\text{3}}$ are trigonal pyramidal.  All the molecules have nonbonding electrons on the nitrogen atom.  Due to this the bond polarities do not cancel out each other.  Hence, ${\text{NH}}_{\text{3}}{\text{F, NHF}}_{\text{2}}{\text{, NF}}_{\text{3}}{\text{, and NH}}_{\text{3}}$ molecules will be polar in nature.