3. On the basis of the number of covalent bonds possible for each atom, determine which...
V. (1.5 points) 1. For the following compound identify the polar covalent bonds and indicate the direction of dipole moment using 8+ and 8-. Of the polar bond you have selected, circle the mot polar bond. (0.75 point) H H 2. Indicate the atomic/hybrid orbitals that are involved in the formation of each o (sigma) and TT (pi) bond, in the following compound. The lone pairs of electrons of the nitrogen and oxygen atom are located in which orbitals? (0.75...
1 - 2. Identify which bonds in the following bonds are polar covalent bonds. C-Se, H-O, CI-CI. N--H, C-H. Determine which atom in the bonds you select has greater electronegativity.
Answer 1-4 (#3 and #4 are tables)
shell provides stability to the atom. Different chemical bonds are based on the way in which the atoms fill their valence shells. The major types of chemical bonds include: ionic bonds covalent bonds (both types, i.c. polar covalent and non-polar covalent bonds), and hydrogen bonds. Atoms can use two strategies to fill their valence shell: they can share electrons between their valence shells, or they can give or take electrons from other nearby...
The Lewis symbol for the nitrogen atom has _______ valence electrons. The number of covalent bonds which nitrogen usually forms in order to complete its valence shell and obey the octet rule is _______. 5, 2 3, 4 5, 3 5, 4 5, 1
1. Which of the following bonds is the most polar covalent but
not ionic?
2. Which of the following bonds is the least polar covalent
(but not non-polar covalent bond)?
3. For the following bonds assigned charges to each atom use +
and - for ionic compounds and S+ and S- for covalent bonds where
electrons are not equally shared. If a covalent bond has electrons
equally shared, leave it blank.
Would bonds in this compound be lonic or covalent (arcie sulfur atom? one)? Explain. e. Draw the Lewis structure. 18. a. What is the likely formula for a compound composed of sodium atoms and one sulfur atom? b. Would this compound be ionic or covalent (circle one)? Explain. c. Why would it be inappropriate to draw a Lewis structure (such as in Model 4) for this compound? 19. Without attempting to draw a Lewis structure, add up the total number...
6. For each of the following Lewis structures or skeletal structures, match it with the correct condensed structural formula. (10 points) Structures: Η Η Η Η i 1 H-C-C-C-C-H IT I 1 HH Η Η ОН H HC CH Η Η H3C H,c-c-BI H-C-C-OH Η Η H3C ОН OH Formulas: a. CH3CH2CH.CH b. (CH3)2CHCH.CH c. CH3CH2CHCHCH d. CH CH OH e. (CH3)3CBr f. CH:CH-COOH g. CH-COCH h. CHỊCH CHO i. C H OH j. CH, OH
Covalent Molecules and Lewis Structure Experiment 5 A. For each compound, show the calculation of the number of total valence electrons, the number of electrons used to form covalent bonds between the central atom and other atoms, and draw the Lewis structure. Remaining valence electrons Draw Lewis The Number of Calculation of Compound (Identify center atom) structure valence electrons used to form covalent the number of total valence electrons (I) (I-II bond (II) HS ( ) PH ( ) CH,CI...
Determine if each of the statements is true or false. 1) K2SO4 contains both polar covalent bonds and ionic bonds. [ Select ] 2) A covalent bond is formed through the transfer of electrons from one atom to another. True 3) When two atoms form a chemical bond, they lower the potential energy between the bonding atoms or ions. (Select]
Draw all possible resonance structures for SeO2, SeO32-, and SeO. Use the resonance structures to solve the problems below. (a) Arrange these species in order of increasing Se-O bond length (shortest bond first). SeO SeO2 (SeO3)2- Correct: Your answer is correct. (b) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an Se atom and an O atom bonded to this Se atom. (Hint: Average the number of bonds between Se and an...