#2 SCH3U Lesson

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o=c=0 ö-s=ö 10. Lewis electron dot diagrams for CO2 and SO2 are given above. Which of the following is true regarding the molecular geometry and the polarity for both substances? A. they are both linear because they only have two non-central atoms B. they are both polar molecules due to the polar bonds between the central atom and oxygen C. the lone pair of electrons on the S atom in SO, make it a polar bent molecule D. they are both nonpolar because the formal charge on each atom is zero 150 to 140 130

F od When can a covalent bond be polar? O when the value of electronegativity between the bonded atoms is equal when the molecular shape is a tridimensional network F2 when there is a distinct difference in the value of electronegativity between the bonded atoms when two atoms are dissimilar in electron valence (@ F3 # F4 $ F5 % F6 A F7 F8 & F9 * F10 28 F11 @ F12 Ô Prt Sc Insert ^ M Del

ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting deviations from ideal bond angles Consider the chlorite (C102) a 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 chlorine-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the chlorine-oxygen bonds to be... 0 0 (choose one) X 3 1/5

Consider the perbromate (BrO4) 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 ... 0 口。 (choose one) X 3

Predicting deviations from ideal bond angles Consider the nitrogen trifluoride (NF3) molecule. 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 nitrogen-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the nitrogen-fluorine bonds to be ... 0 口。 (choose one) (choose one) about the same bigger smaller

Answer the questions in the table below about the shape of the sulfur hexachloride (SCI) molecule. What word or two-word phrase best describes the shape of the SCI molecule? 6 What is the angle between the sulfur-chlorine bonds? (If there is more than one angle, pick the smallest.) 0 口。 X Start over Ś

Which statements are true and which are false? SeF4 has a tetrahedral structure.Bond angles for IF6+ are 60 °. Selenium tetrafluoride (SeF4) is a non-polar molecule. NO3- has only two resonance Lewis structures. Carbon tetrachloride (CCl4) is a non-polar molecule.  KrF4 is a polar molecule.

For each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. compound hydrogen-bonding force Between molecules of the compound? Between molecules of the compound and molecules of water? formula or Lewis name structure O yes O yes formaldehyde CH,O O no O no H. O yes O yes methanol н -с —ӧ—н O no O no H. N- C: O yes O no O yes O no N-chloromethylamine Н-С H.

for number 10 Shape                                                   Type of Molecule tetrahedral                                             nonpolar prymidal                                                 polar bent                                                        ionic trihonal planar linear diatomic monoatomic ion

Answer the questions in the table below about the shape of the tribromide (Br3) anion. What word or two-word phrase best describes the shape of the Br3 anion? What is the angle between the bromine-bromine bonds? (If there is more than one angle, pick the smallest.) 0 口。 X Ś

Complete the following table. Only consider the 'central' atom when filling in the steric # , # of bonding electron groups and # of lone pairs. Report Table MGP.6: Geometry and Polarity of Group 2 Compounds Determining polarity for group 2 compounds Steric # Electron Geometry # of bonding electron groups # of lone pairs Molecular Geometry How many bonds have a dipole? If present, do the dipoles cancel each other? Is this molecule polar? N₂ N/A N/A N/A N/A N/A Choose... Choose... - Choose... Choose... ▼ ✓ Choose... linear m bent HCN trigonal planar square planar tetrahedral trigonal pyramidal square pyramidal trigonal bipyramidal seesaw t-shaped octahedral Choose... Choose... Choose... Choose... Choose... Choose... Choose... Choose... H3O+ Choose... Choose... - Choose... Choose... - N/A N/A 1₂ N/A N/A N/A Choose.. Choose... - Choose... Choose... - Choose... Choose... Choose... Choose... NH4* Choose... Choose... - Choose... Choose... ▾ C C Cho Cho

For each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. name compound N,N- dichloromethylamine hydrogen iodide hypobromous acid formula or Lewis structure H :CI: T н – с – -N-CI: H HI HBrO Between molecules of the compound? yes Ono 0000 yes no yes hydrogen-bonding force no Between molecules of the compound and molecules of water? oooo yes no yes no yes no X hid do Ar

Which of the following molecules contains polar covalent bonds ONLY?   I. CH4 II.  KNO3 III.  H2O     II AND III ONLY     I ONLY     I, II, and III     II ONLY     I AND III ONLY     III ONLY

For the molecule CHCl3, draw its Lewis Structure and then answer the following questions based on that structure. (The central atom in each case is the atom with the lowest electronegativity). How many valence electrons are in the molecule? (Remember to add an electron for each negative charge or to subtract one for each positive charge). How many lone pairs of electrons are in the central atom of the molecule? What is the electron pair geometry of the molecule?  Tetrahedral Octahedral Triangular planar Trigonal Pyramidal Which of these structures could represent the three dimensional molecular shape of the molecule CHCl3? (Rotate the structures to perceive 3D shape. Pay attention to the angles!)   What is (are) the bond angle(s) at the central atom of the molecule CHCl3?     104.5°    109.5°    90°    180° Would the molecule's structure be polar, nonpolar, or ionic?  polar nonpolar ionic

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