10. Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS2 A) CS2 = SC12 > CF4 B) SC12 > CF4 >CS2 C) CF4 > CS2 > SC12 D) CS2 > CF4 > SCl2 E) CF4 > CS2 > SCI2 Answer: D CF4 SCI2 15-c-51

= O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting the arrangement of electron groups around the centr... Answer the questions in the table below about the shape of the phosphorus trifluoride (PF3) How many electron groups are around the central phosphorus atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central phosphorus atom? (You may need to use the scrollbar to see all the choices.) (choose one) (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedral molecule.

Depending on the protein under study, the bond angle of a drug molecule can become critical to successfully deactivating a viral protein. For this reason, chemists are frequently concerned with the 3D shape of their molecules and their bond angles. The oxygen atom shown in the structure has a tetrahedral electronic geometry, meaning we would predict that it would have 109.5° bond angles. However, the actual structure, the bond angles are smaller than 109.5°. Explain why this compression occurs. Make sure to discuss what’s happening around/what groups are present around the oxygen atom.

Decide whether the Lewis structure proposed for each molecule is reasonable or not. Note: If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.

Some formulas can be drawn multiple ways; molecules that share the same formula but have different structure are called isomers. Draw three isomers with the formula C5H12O such that each atom makes the appropriate number of bonds, as indicated by their Lewis Dot Symbol. (There are many structures that work!)

Consider the molecule with skeletal structure C(1)-C(2)-N. The carbon atoms and the nitrogen atom are also bonded to hydrogen atoms to complete the octet and yield the formula C₂HyN. Which of the below is the best description of the bonding in this molecule? O sigma bond: C(2) sp³ to N sp² O pi bond: C(2) sp³ to N sp² O sigma bond: C(2) sp² to N sp³ O sigma bond: C(2) sp³ to N sp³

Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure :Z: I :Z: c=0 0 0 0 Is the proposed Lewis structure reasonable? O Yes. O No, it has the wrong number of valence electrons. The correct number is: O O No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* ■ Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* O Yes. O No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "0,0". X 3

Is the N¬N bond length in these molecules shorter or longer than the N¬N bond length in N2?

Effect of Differences in Electronegativity on Molecular Polarity For each molecule: Sketch each molecule as shown in the simulation. Include arrows to show the bond dipoles as well as a molecular dipole (if present). Circle polar or nonpolar to indicate the polarity of the molecule. Fill in the electronegativity values for each atom C. Oz vs HF O2 HF polar Electronegativity nonpolar polar nonpolar H=D F = Question 2a: Both of these molecules have the same molecular geometry; they are linear. How do differences in electronegativity affect the molecular polarity in linear molecules? Page 8 of 9 CHM CZ1 ONL Genmetru chrt p-ts voih 1032 Corvrinht e 2020-2021 B CSI A

Consider the bromate (BrO3) anion. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the bromine-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the bromine-oxygen bonds to be ... 口。 (choose one) X