Concept explainers
Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4.
- a. Draw Lewis structures for each of the five molecules.
- b. Using VSEPR theory, predict the geometry of each of the five molecules.
- c. Specify the polarity (polar or nonpolar) for each of the five molecules.
(a)
Interpretation:
Lewis structures for the five molecules that are formed by successive substitution of
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
For
Given molecule is
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
For
Given molecule is
Nonbonding electrons are added to the fluorine atom. The resulting structure is,
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
For
Given molecule is
Nonbonding electrons are added to the fluorine atom. The resulting structure is,
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
For
Given molecule is
Nonbonding electrons are added to the fluorine atom. The resulting structure is,
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
For
Given molecule is
Nonbonding electrons are added to the fluorine atom. The resulting structure is,
All the atoms present in the above structure contains octet of electrons. The total number of electron dots present in the above structure is 32 and it is same as the valence electrons of
(b)
Interpretation:
Molecule geometry has to be predicted for the five 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
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
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
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
The central atom in the above molecule is found to be carbon. This has four bonding electron groups and zero nonbonding electron groups. The arrangement around the central atom is tetrahedral arrangement. Looking for molecular geometry, the central atom that contains four bonding electron groups and zero nonbonding electron groups and it has tetrahedral geometry as per VSEPR theory.
Given molecule is
The central atom in the above molecule is found to be carbon. This has four bonding electron groups and zero nonbonding electron groups. The arrangement around the central atom is tetrahedral arrangement. Looking for molecular geometry, the central atom that contains four bonding electron groups and zero nonbonding electron groups and it has tetrahedral geometry as per VSEPR theory.
Given molecule is
The central atom in the above molecule is found to be carbon. This has four bonding electron groups and zero nonbonding electron groups. The arrangement around the central atom is tetrahedral arrangement. Looking for molecular geometry, the central atom that contains four bonding electron groups and zero nonbonding electron groups and it has tetrahedral geometry as per VSEPR theory.
Given molecule is
The central atom in the above molecule is found to be carbon. This has four bonding electron groups and zero nonbonding electron groups. The arrangement around the central atom is tetrahedral arrangement. Looking for molecular geometry, the central atom that contains four bonding electron groups and zero nonbonding electron groups and it has tetrahedral geometry as per VSEPR theory.
Given molecule is
The central atom in the above molecule is found to be carbon. This has four bonding electron groups and zero nonbonding electron groups. The arrangement around the central atom is tetrahedral arrangement. Looking for molecular geometry, the central atom that contains four bonding electron groups and zero nonbonding electron groups and it has tetrahedral geometry as per VSEPR theory.
(c)
Interpretation:
The five 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
Want to see more full solutions like this?
Chapter 5 Solutions
General, Organic, and Biological Chemistry
- hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?arrow_forwardTTT One or more positively-charged 1 negatively-charged atoms. A. Ionic bond B. Covalent bond atoms are electrostatically bound to one or more C. Metallic bond D. Hydrogen bond Hydrogen atoms are attached to a very electronegative atom. The hydrogen atom on 2 one molecule is attracted to the electronegative atom on another molecule. A. Ionic bond C. Metallic bond B. Covalent bond D. Hydrogen bond Electrons are not shared. Atoms have gained or lost valence electrons such that they 3 have a full octet of valence electrons. A. Ionic bond B. Covalent bond A. Ionic bond B. Covalent bond C. Metallic bond D. Hydrogen bond Atoms share two or more valence electrons with other atoms such that they have a 4 full octet of valence electrons. C. Metallic bond D. Hydrogen bond 5 The strongest type of chemical bond. A. Ionic bond B. Covalent bond C. Metallic bond D. Hydrogen bond Atoms are so tightly packed together that their valence electrons move freely from 6 atom to atom. A. Ionic bond B.…arrow_forward1. How many electrons will an iodine atom donate or accept, based on its number of valence electrons? A. Donate 7 electrons B. Donate 1 electron C. Accept 7 electrons D. Accept 1 electrons 2.What type of bond is formed between the two nitrogen atoms in diatomic nitrogen, N2? A. Triple Bond B. Double Covalent Bond C. Double Ionic Bond D. Single Bond 3.Which metal would form a stronger metallic bond? A. Lithium B. Sodium C. Strontium D. Tungsten 4. What holds the metal ions together in a lattice? A. Hydrogen Bonds B. Covalent Bonds C. Metallic Bonds D. Ionic Bondsarrow_forward
- TIT Electrons are not shared. Atoms have gained or lost valence electrons such that they 3 have a full octet of valence electrons. A. Ionic bond B. Covalent bond C. Metallic bond D. Hydrogen bond Atoms share two or more valence electrons with other atoms such that they have a 4 full octet of valence electrons. A. Ionic bond B. Covalent bond C. Metallic bond D. Hydrogen bond 5 The strongest type of chemical bond. A. Ionic bond B. Covalent bond C. Metallic bond D. Hydrogen bond Atoms are so tightly packed together that their valence electrons move freely from 6 atom to atom. A. Ionic bond B. Covalent bond A. Ionic bond B. Covalent bond C. M allic bond D. Hydrogen bond 7 Chemical bond that forms between a nonmetal atom and a metal atom. A. Ionic bond C. Metallic bond B. Covalent bond D. Hydrogen bond 8 Chemical bond that forms between many metal atoms. A. Ionic bond C. Metallic bond B. Covalent bond D. Hydrogen bond 9 Chemical bond that forms between nonmetal atom and another nonmetal…arrow_forward1. Which is an example of a non-polar molecule that contains polar covalent bonds? A. H2O B. NH3 C. N2 D. CBr4 2. Which of the following molecules dissolves in water? A. C6H6 B. CBr4 C. CH3OH D. CCl4 3. SO3 molecules are ____. A. nonpolar B. either C. polar D. None of them 4. A polar molecule is one in which there is a separation of charge caused by ___. A. an uneven number of electron pairs B. an average distribution of electrons C. a non-uniform electron distribution D. a complete loss of electrons 5. Which of the following molecule is not polar? A. HF B. water (H2O) C. ammonia (NH3) D. H2arrow_forwardConsider the Lewis structure shown below. The A-B bonds are polar. Is this molecule polar or nonpolar? Why? B A B 1. This molecule is nonpolar. 2. This molecule is polar. Because 3. The bond dipoles point in opposite directions and cancel each other out. 4. The molecule contains polar bonds. 5. The bond dipoles add together, leaving an overall molecular dipole.arrow_forward
- TTTTTTTTTTT Atoms of oxygen can form many different types of covalent chemical bonds. Which 19 covalent bond can atoms of oxygen form? A. Single bonds only B. Single bonds & Double bonds C. Single bonds, Double bonds, & Triple bonds D. None of the options listed. Which element's atoms can only form one single bond and no others in a covalent 20 compound? A. Hydrogen B. Helium C. Lithium D. Beryllium Which element's atoms can only form one single bond and no others in a covalent 21 compound? A. Selenium B. Arsenic C. Aluminum D. Bromine Consider the covalent compound H₂O. 22 How many total valence electrons are in one molecule? A. 2 C. 8 B. 6 D. 10 Consider the covalent compound H₂O. 23 How many unshared pairs of electrons are in one molecule? C. 3 pairs A. 1 pair B. 2 pairs D. 4 pairs Consider the covalent compound NF3. 24 How many total valence electrons are in one molecule? A. 22 B. 26 C. 28 D. 32 Consider the covalent compound NF3. 25 How many unshared pairs of electrons are in one…arrow_forwarda. Predict the formula of thecompound formed from aluminum and fluorine.b. Calculate the electronegativity difference between aluminum and fluorine.c. Is the AlF bond ionic, polar covalent, or nonpolar covalent?d. Write the name of the compound formed from aluminum and fluorine..e. Is this compound ionic, polar covalent, or nonpolar covalent?f. Is this compound water soluble? ( give the all answer with stepwise and type the answer.)arrow_forwardConsider the compound NO3. Is NO, a polar or nonpolar molecule? A. Polar molecule B. Nonpolar molecule C. Not enough information has been providedarrow_forward
- Which type of bond results from the sharing of electron(s) between two atoms? A. Ionic B. Covalent C. Hydrogen D. Electrovalentarrow_forward4. It is important to know the geometry of a molecule because the geometry A. affects the physical and chemical properties of the substance B. will give the Lewis structure of the molecule C. will determine whether the molecule is ionic or covalent D. B and C 5. If there are four L4) electron pairs around tbe central atom of a molecule thesearrow_forward1. What kind of elements will form an ionic compound? Will form between non-metal elements and metal elements. 2. In an ionic compound the charge on-metal ion is Dosin and nonmetal ion is 3. What kind of ions are likely to form from following elements and how. a. Calcium b. Bromine c. Aluminum d. Potassium e. Охуgen 4. Label as ionic or covalent and name them. a. NaBr b. FezN2 c. PCI3 d. NaNO3 e. CBr4 7arrow_forward
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningLiving By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHERChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co