ALL questions listed must be answered to earn credit for completing the text homework. Yes, even the Additional Exercises if they are present for this chapter.
Covalent bond lewis structure calculator November 4, 2020 by Odd-electron molecules have an odd number of valence electrons, and therefore have an unpaired electron. Thus by increasing the potential energy. However, some atoms will not give up or gain electrons easily. For example, consider the Lewis dot structure for carbon dioxide. This is a linear molecule, containing two polar carbon-oxygen double bonds. However, since the polar bonds are pointing exactly 180° away from each other, the bond polarities cancel out, and the molecule is nonpolar. A Lewis electron dot diagram (or electron dot diagram or a Lewis diagram or a Lewis structure) is a representation of the valence electrons of an atom that uses dots around the symbol of the element. Electrons exist outside of an atom‘s nucleus and are found in principal energy levels that contain only up to a specific number of electrons. Covalent bond lewis structure calculator. November 4, 2020; Posted in Uncategorized 0 Comments; each oxygen atom gets Neon's configuration. This is a qualitative explanation for covalent bond only.
(1) How do atoms form covalent bonds? What is the easiest way to distinguish a covalent bond from an ionic bond?
(2) For each of the following elements, draw their Lewis dot structures.
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(3) Study the given Lewis structure and provide the following information:
(4) Answer each question regarding the following structure:
(5) Draw the Lewis dot structures for each of the 7 diatomic elements in their diatomic states. Are these diatomic elements, when one atom is covalently bonded to another of the same element, considered molecules or compounds? Explain using the definition of whichever answer you choose.
(6) For each family or group number, describe the covalent bonding pattern found in organic compounds.
(7) Sketch the Lewis configurations for the following molecules. Include all lone pairs in the sketch and determine how many total electrons are in each molecule.
(8) What is an expanded octet? Which elements cannot form an expanded octet? Where on the periodic table are the elements that can form expanded octets located?
(9) Give the names of the following covalent compounds.
(10) Include the Lewis dot structure for each given molecule. Give both the electron geometry and molecular shape of the central atom(s).
(11) If a central atom has three bonding groups surrounding it, how can you differentiate between the possible molecular shapes it can take on? What electron geometry, molecular shape and bond angles would such a molecule have?
(12) For each of the following molecules, tell whether they are two-dimensional or three-dimensional based on their electron geometry.
(13) What are the approximate bond angles in the given molecules?
(14) In each of the following molecules, give the central atom’s molecular shape and the approximate bond angles.
a. O=C=O
b.
c. NH3
d.
e.
(15) Use your knowledge of what you’ve learned so far to provide the Lewis dot structures, electron geometry, molecular shape, bond angles, number of lone pair electrons, and the number of shared pair electrons for each molecule given.
(16) For each of the three carbons in this molecule, provide the requested information.
(17) Construction of acetic acid, CH3COOH
(18) Construction of acetonitrile, CH3CN
(19) Between the following pairs, which has the higher electronegativity?
(20) Describe the trend in electronegativity as you move left and right across the periodic table. Does electronegativity increase to the right or the left? Now do the same for moving up and down; does electronegativity increase as you go up or down?
(21) Sketch each of the following molecules to help you determine whether they are polar or non-polar. Draw dipole arrows to indicate polarity in polar molecules.
(22) Electronegativity is not the sole decider of polarity within a molecule. Keeping this in mind, determine if the following molecules are polar or not. If not, explain why.
(23) Are intermolecular forces considered to be bonds? Explain. Is an H-bond an exception?
(24) Which of the three intermolecular forces is the most common? List two other names that can be used to describe this interaction. What is its relative strength compared to the others?
(25) Explain why a dipole-dipole attraction is a stronger force than London Dispersion forces. What is the critical difference that makes this so?
(26) What is the dominant intermolecular forces in each of the following molecules?
(27) Water (H2O) is one of the most perfect H-bonding molecules we know of. Use your knowledge of H-bonding to explain why solid H2O (ice) floats in liquid H2O while in most other substances, the density of the solids is greater than their respective liquids.
(28) Intermolecular forces are significant for allowing molecules to do things that bonding alone will not allow for. Explain how something like DNA utilizes intermolecular forces to take on its helical shape without relying solely on covalent bonding.