Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chem 20 > unit A-topic two > Flashcards

unit A-topic two Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

VESPER stands for

A

valance electron pair repulsion theory

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

VESPER is

A

a simple molecule geometry around central atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

central atom

A

atom in the middle of the geometry formation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what do the bonds require in VESPER?

A

to be as far away as possible

think of balloon example

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

trigonal pyramidal

A

one electron clouds forces down, three other bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

bent or angular

A

a v shape, has two lone pairs and two bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

linear

A

straight line, up to one or two bonds

no lone pairs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

double bonds

A

rigid, forces into linear shape with two bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

tetrahedral

A

classic pyramid, with four bonds and no electron clouds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

trigonal planar

A

three bonds no electron cloud

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

when you don’t know central atom

A

-who has the most bonding atoms

  • count only bonds DIRECTLY to central atoms
  • similar atoms beside each other
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

nonpolar covalent bond

A

close to sharing electrons equally

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

polar covalent bonds

A

unequal sharing of electrons (a slight charge)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

polar in other words means…

A

difference in charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

covalent in other words means..

A

sharing of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

ionic compounds behave similarly to the covalent bond BUT

A

need a polar covalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

dipole

A

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

18
Q

dipoles point in opposite directions

A

non polar

19
Q

dipoles point the same way

A

polar

has a charge that is consistent

20
Q

polar substances dissolve in

A

polar solvents

21
Q

nonpolar substances dissolve in

A

nonpolar solvents

22
Q

intra molecular force

A

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

23
Q

inter molecular force

A

between the molecules as a whole

24
Q

do polar and nonpolar dissolve together?

A

polar and nonpolar won’t dissolve between the two

25
Q

van der waals

A

sum of attractive or repulsive forces between molecules

basically how electrons react

26
Q

types of van der waals

A
  • force between two permanent dipoles (polar)

- force between two instantaneously induced dipoles

27
Q

London dispersion force

A

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

28
Q

explain how the LDF works

A

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

29
Q

dipole dipole force

A
  • slightly stronger interforce containing a permanent dipole
  • much weaker than intra bonds (ionic and covalent)
  • molecules must be touching or nearly touching
30
Q

hydrogen bonding

A

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

31
Q

boiling points are determined by

A

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

32
Q

boiling point in polar molecules

A

means additional attraction so a higher BP

33
Q

boiling point in hydrogen bonds

A

even higher boiling point

34
Q

only having an LDF bond means

A

that the molecule is weaker

also means that it is going to have a lower BP

35
Q

in C4H9OH what does the OH mean

A

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

36
Q

metallic bonding

A

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)
37
Q

metal alloid

A

mixture of metals that can still experience metallic bonding

38
Q

since electrons in metals can be moved

A

that allows metals to be shaped - malleable

39
Q

network covalent bonding

A

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

40
Q

examples of network cov bonding

A

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

chem 20 (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions