unit A-topic two

Question 1

VESPER stands for

Answer 1

valance electron pair repulsion theory

Question 2

VESPER is

Answer 2

a simple molecule geometry around central atoms

Question 3

central atom

Answer 3

atom in the middle of the geometry formation

Question 4

what do the bonds require in VESPER?

Answer 4

to be as far away as possible

think of balloon example

Question 5

trigonal pyramidal

Answer 5

one electron clouds forces down, three other bonds

Question 6

bent or angular

Answer 6

a v shape, has two lone pairs and two bonds

Question 7

linear

Answer 7

straight line, up to one or two bonds

no lone pairs

Question 8

double bonds

Answer 8

rigid, forces into linear shape with two bonds

Question 9

tetrahedral

Answer 9

classic pyramid, with four bonds and no electron clouds

Question 10

trigonal planar

Answer 10

three bonds no electron cloud

Question 11

when you don’t know central atom

Answer 11

-who has the most bonding atoms

• count only bonds DIRECTLY to central atoms
• similar atoms beside each other

Question 12

nonpolar covalent bond

Answer 12

close to sharing electrons equally

Question 13

polar covalent bonds

Answer 13

unequal sharing of electrons (a slight charge)

Question 14

polar in other words means…

Answer 14

difference in charge

Question 15

covalent in other words means..

Answer 15

sharing of electrons

Question 16

ionic compounds behave similarly to the covalent bond BUT

Answer 16

need a polar covalent bond

Question 17

dipole

Answer 17

arrow that helps point charge flow, one end positive one end negative
points to higher electronegativity

Question 18

dipoles point in opposite directions

Answer 18

non polar

Question 19

dipoles point the same way

Answer 19

polar

has a charge that is consistent

Question 20

polar substances dissolve in

Answer 20

polar solvents

Question 21

nonpolar substances dissolve in

Answer 21

nonpolar solvents

Question 22

intra molecular force

Answer 22

within a molecule itself (the bonds between atoms/elements)

Question 23

inter molecular force

Answer 23

between the molecules as a whole

Question 24

do polar and nonpolar dissolve together?

Answer 24

polar and nonpolar won’t dissolve between the two

Question 25

van der waals

Answer 25

sum of attractive or repulsive forces between molecules | basically how electrons react

Question 26

types of van der waals

Answer 26

- force between two permanent dipoles (polar) | - force between two instantaneously induced dipoles

Question 27

London dispersion force

Answer 27

weakest inter-force, greater the electrons (or larger the molecule) greater the attraction

Question 28

explain how the LDF works

Answer 28

insanely fast speed of reaction, makes it push away there are continuous interactions instantaneously induced dipoles

Question 29

dipole dipole force

Answer 29

- slightly stronger interforce containing a permanent dipole - much weaker than intra bonds (ionic and covalent) - molecules must be touching or nearly touching

Question 30

hydrogen bonding

Answer 30

the strongest, special case of dipole bonding using just F,O,N that bond with a H

Question 31

boiling points are determined by

Answer 31

the amount of electrons (more you have, higher the BP) and the size of an electron

Question 32

boiling point in polar molecules

Answer 32

means additional attraction so a higher BP

Question 33

boiling point in hydrogen bonds

Answer 33

even higher boiling point

Question 34

only having an LDF bond means

Answer 34

that the molecule is weaker | also means that it is going to have a lower BP

Question 35

in C4H9OH what does the OH mean

Answer 35

it just shows an easy way to see where the bonding is taking place

Question 36

metallic bonding

Answer 36

metals have a very tight crystal lattice structure (and high BP) this allows electrons to pass/share easily and keep sharing - loosing electrons - very conductive of electricity (low electronegativity)

Question 37

metal alloid

Answer 37

mixture of metals that can still experience metallic bonding

Question 38

since electrons in metals can be moved

Answer 38

that allows metals to be shaped - malleable

Question 39

network covalent bonding

Answer 39

forms a lattice rigid network covalent bonding that is extremely strong consistent covalency and repeated patterns give it the strength

Question 40

examples of network cov bonding

Answer 40

diamond- tetrahedral connections, that are repeated and extremely strong graphite- has layers of bonds, planar