What is the electron pair structure (electron geometry), shape (molecular shape), bond angle, bond polarity, and or molecular polarity for the following ions, compounds, or molecules? SiCL4 SF4

5 months agoyou'd start w/ the lewis structure and then make the electron pair structure + and molecular shape based on the number of bonds and lone pairs

5 months ago|dw:1540103900836:dw|

5 months agorip well whenever you get back, for SiCl4 I got 4 bonds + 0 lone pairs, so what would that be

5 months ago|dw:1540161547971:dw|

5 months agoWhenever you get back ! =)

5 months agoSi = 4 valence electrons Cl = 7 valence electrons so 4 + 4(7) = 32 electrons = 16 pairs so you need to fill up all lone pairs on chlorines. there shouldn't be any leftover electrons on silicon

5 months ago|dw:1540164298779:dw|

5 months agoanyway, so that's 4 bonds and 0 lone pairs on the central atom (only consider lone pairs on the central atom for this) so the electron geometry and shape are both tetrahedral, bond angle is 109.5 degrees bond polarity, well, idk if they're looking for a quantitative or qualitative response, you would have to check your textbook for the electronegativity values of S and Cl and subtract them, then classify the bond between S and Cl based on that the overall molecule is nonpolar since the bond polarities cancel out (4 equal bonds)

5 months agostill there?

5 months agoYes i am

5 months agoso fro bond polarity i would just say that they cancel out

5 months ago\(\color{#0cbb34}{\text{Originally Posted by}}\) @Vocaloid bond polarity: you would have to check your textbook for the electronegativity values of Si and Cl and subtract them, then classify the bond between Si and Cl based on that \(\color{#0cbb34}{\text{End of Quote}}\)

5 months agoelectornegstivity for Si is 1.9

5 months agocl is -3

5 months agoshould be +3

5 months agothen you'd subtract 3 - 1.9 and check your book to see how your book classifies it (polar, nonpolar, covalent, etc.)

5 months agononpolar

5 months ago=1.1

5 months ago|dw:1540167638922:dw| your book might be slightly different but an electronegativity difference of 1.1 should put it into the polar not nonpolar category

5 months agoso the bond polarity = polar, while the overall molecule polarity = nonpolar

5 months agoyou'll repeat this process for SF4

5 months ago|dw:1540171221123:dw|

5 months agosulfur (6 valence) fluorine (7 valence) so 6 + 4(7) = 34, or 17 pairs of electrons, so there should only be 1 electron pair on the central atom

5 months agois it good otherwise

5 months agoyes

5 months agothen check the chart for the number of lone pairs and bonds to see what the electron and molecular geometries are https://s-media-cache-ak0.pinimg.com/736x/62/14/b5/6214b5e947f25877e06d9ac7654ee088.jpg

5 months agoso four bonds 0 lone pairs. geometry and shape are tethrahedral bond angle is 109.5

5 months agothere's a lone pair on the central atom, so 1 lone pair not 0.

5 months agothe geometry and shape are tetrahedral?

5 months agocheck the chart again

5 months ago4 bonds 1 lone pair.

5 months agotrigonal bipyramid and seesaw

5 months agogood bond angles for this one are complex but it's about ~90 deg, 180 deg, 120 degrees

5 months agothen find the bond polarity based on the EN's of S and F

5 months ago2.58 and 3.98

5 months agoalright so what's the EN difference?

5 months agowhich one do you subtract from? The most electronegative?

5 months agohigher value - lower value yes

5 months ago3.98-2.58=1.4

5 months agogood so what kind of bond would this be? polar, nonpolar, etc.?

5 months agopolar covalent

5 months agogood any ideas about the whole molecule's polarity? as a hint consider the lone electron pair on the central atom

5 months agoIOnic?

5 months agois the whole molecular polar or nonpolar?

5 months agopolar so nonpolar=?

5 months agothe whole molecule is polar, (due to the lone e' pair) so that's it

5 months ago