Question

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

Answer 1

you'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

Answer 2

rip

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

Answer 3

Whenever you get back ! =)

Answer 4

Si = 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

Answer 5

anyway, 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)

Answer 6

still there?

Answer 7

Yes i am

Answer 8

so fro bond polarity i would just say that they cancel out

Answer 9

\(\color{#0cbb34}{\text{Originally Posted by}}\) @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
\(\color{#0cbb34}{\text{End of Quote}}\)

Answer 10

electornegstivity for Si is 1.9

Answer 11

cl is -3

Answer 12

should be +3

Answer 13

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

Answer 14

nonpolar

Answer 15

=1.1

Answer 16

your book might be slightly different but an electronegativity difference of 1.1 should put it into the polar not nonpolar category

Answer 17

so the bond polarity = polar, while the overall molecule polarity = nonpolar

Answer 18

you'll repeat this process for SF4

Answer 19

sulfur (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

Answer 20

is it good otherwise

Answer 21

yes

Answer 22

then 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

Answer 23

so four bonds 0 lone pairs. geometry and shape are tethrahedral bond angle is 109.5

Answer 24

there's a lone pair on the central atom, so 1 lone pair not 0.

Answer 25

the geometry and shape are tetrahedral?

Answer 26

check the chart again

Answer 27

4 bonds 1 lone pair.

Answer 28

trigonal bipyramid and seesaw

Answer 29

good

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

Answer 30

then find the bond polarity based on the EN's of S and F

Answer 31

2.58 and 3.98

Answer 32

alright so what's the EN difference?

Answer 33

which one do you subtract from? The most electronegative?

Answer 34

higher value - lower value yes

Answer 35

3.98-2.58=1.4

Answer 36

good so what kind of bond would this be? polar, nonpolar, etc.?

Answer 37

polar covalent

Answer 38

good

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

Answer 39

IOnic?

Answer 40

is the whole molecular polar or nonpolar?

Answer 41

polar so nonpolar=?

Answer 42

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