Brainscape's Knowledge GenomeTM

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


See full index

Gen chem > exam 3 > Flashcards

exam 3 Flashcards

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

ionization energy….

A

increases as the column increases and decreases as you go down a group

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

after a full shell, after a half shell

A

ionization energy drops

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

the 5th electron taken out creates a huge jump in energy, what group is this element in?

A

group 14, (C, Si, Ge,….)

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

Electron affinity

A

energy change from stealing an electron
(ex flourine EA= -349) only negative for the first electron stolen

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

electron affinity trend

A

to the right and up (same full shell half shell trend)

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

electrostatic potential energy equation

A

Eel is proportional to (Q1 x Q2)/d
Q= attraction d = distance

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

delocalized

A

an electron able to travel 3 or more atoms over from the one it came from

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

covalent bonds

A

both elements share electrons evenly due to high ionization energy

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

lewis symbol

A

basically lewis struct but just one element

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

cations = anions = (type of energy)

A

ionization energy. Electron affinity

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

larger charges = larger _______

A

lattice energies

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

larger distance = ______ lattice energy

A

smaller

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

Born-Haber cycle

A

graph to figure out the lattice energy
think deltaH = deltaH1 +deltaH2 +or -…… -lattice energy. in KJ/Mol

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

Born-Haber cycle rules

A

must get to a form that is 1 mole to 1 mol in gaseous state

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

lattice energy equation

A

( Q1 x Q2 ) / distance

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

octet rule exemptions

A

B, P, S, Se, Br, Te, I

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

lewis structure rules (6)

A
  1. count the number of valence
  2. adjust for electron charge
  3. Draw skeleton (central atom with single bonds) (central atom is most electro-positive (Fr is king) and or first)
  4. distribute leftover electrons to other atoms to fill out octet (most electronegative first)
  5. place any remaining on the central atom
  6. if center doesn’t have octet, make double bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

check for lewis structure

A
  1. Complete octets?
  2. formal charges match?
    3.multiple lewis structures?
  3. valence structures?
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

ionic, polar, nonpolar charge difference

A

> 1.9, POLAR, <0.4 in electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

dipole moment

A

Q (charge) x r (distance). greater difference = greater dipole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

dipole unit

A

Debyes (D) or (wierd u)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

1 debye =

A

3.33564 x 10^−30 C·m

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Angstroms

A

unit of length, 10^-10 meters

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

electron charge

A

1.60 x 10^-19 C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

formal charge

A

extra electrons that added to the normal valence

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

formal charges for H2O

A

H= 0 O=0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

charge of _ is perfect, _ is preferable, _ is not correct

A

0,1,2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

if to fill a middle octect with 8 fluorine must become positive _______

A

this CANNOT happen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

when you have multiple lewis structure with same charges possible, choose _______

A

the more EN element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

hypervalence

A

when in period 3 or lower, to reduce formal charge mid atom can expand the valence

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

resonance structures

A

LOOK FOR OXYGENS, equavalent lewis structures that describe a molecule, give ya decimal bond orders

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

bond order

A

resonance bonds over amount of bonds (double and single are still one) Plus 1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

how to fill out octets

A

start at the outer and then go inner

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Take a moment to memorize vseper models and draw them

A

oky doky

35
Q

BOISTERIOUS Boron rules

A

boron can only have 6 electrons to complete the octet

36
Q

radical

A

unpaired electron

37
Q

S and F compounds

A

SF2, SF4, SF6

38
Q

Xe and F compounds

A

XeF4

39
Q

higher bond order = ______ angstrums

A

smaller angstrums, the atoms are closer together

40
Q

bond enthalpy units and sign

A

KJ/mol, + (its the energy needed to break the bond)

41
Q

2 bonds, 0 lone pairs, angle?

A

linear, 180

42
Q

3 bonds, 0 lone pairs, angle?

A

Trigonal Planar, 120

43
Q

4 bonds, 0 lone pairs, angle?

A

Tetrahedral, 109.5

44
Q

5 bonds, 0 lone pairs, angle?

A

trigonal bipyramidal, 120 and 90

45
Q

6 bonds, 0 lone pairs, angle?

A

Octahedral, 90

46
Q

electron domains

A

bonds or lone pairs in a compound. (double bonds count as one)

47
Q

2 bonds, 1 lone pair, angle?

A

bent or angular, <120

48
Q

3 bonds, 1 lone pair, angle?

A

trigonal pyramidal, <109.5

49
Q

2 bonds, 2 lone pairs, angle?

A

bent (2) or angular, «109.5

50
Q

Vsepr acronym

A

Valence Shell Electron Pairs Repulsion

51
Q

4 bonds, 1 lone pair, angle?

A

Seesaw, <120 and <90

52
Q

3 bonds, 2 lone pairs, angle?

A

T-shape, <90

53
Q

2 bonds, 3 lone pairs, angle?

A

linear, 180

54
Q

5 bonds, 1 lone pair, angle?

A

square pyramid, <90

55
Q

4 bonds, 2 lone pairs, angle?

A

square planar, 90

56
Q

3 bonds, 3 lone pairs, angle?

A

T-shape, <90

57
Q

2 bonds 4 lone pairs, angle?

A

linear, 180

58
Q

practice drawing vsepr models

A

oky doky

59
Q

trigonal bipyramidal where 120 and 90?

A

the equatorial (three atom ring) = 120, axis position (like the poles of a planet) = 90

60
Q

which take up more space? lone pair or bond

A

lone pair

61
Q

(fill in chapter 9 part that you missed)

A

oki

62
Q

sigma bond

A

first bond, on axis bond, head to head overlap,

63
Q

Pi bond

A

off axis bond, side to side overlap, like two faces melting together.

64
Q

Pi bonds live in ____

A

P orbitals

65
Q

sigma bonds live in ____

A

hybridized orbitals

66
Q

double bond = ___

A

Pi bond

67
Q

single bond = _____

A

sigma bond

68
Q

triple bond = ____

A

sigma AND pi bond

69
Q

Pi bonds prevents _____

A

ROTATION of a single side of a molecule

70
Q

bonding orbital

A

the orbital that goes to a lower energy level and is constructively interferring (-energy)

71
Q

antibonding orbital

A

the orbital goes up and destructively interferes with the bond (+ energy denoted with star *)

72
Q

node

A

area where you’ll never find an electron. only antibonding orbital has node

73
Q

bond order calculation

A

1/2 bonding electrons - antibonding electrons = bond order

74
Q

hybridization

A

blending S and P orbitalts

75
Q

study MOS PI bond structures

A

oki

76
Q

diamagnetic (die)

A

spins of electrons being paired that kill magnetism

77
Q

paramagnetic

A

has unpaired electrons that can be lined up to become magnetic

78
Q

born haber process

A

the steps to find the lattice energy

79
Q

a planar molecule

A

has all of its atoms in the same plane (can ya twist the fucker)

80
Q

0 unpaired electrons = >0 unparied electrons =

A

diamagnetic paramagnetic

81
Q

Angstrom = ?

A

1x 10^-10 m

82
Q

delocalized pi bonds have 2 e- per ______ while localized just have _____

A

p orbital, 2

83
Q

electron domain vs molecular domain

A

electron does NOT care about nonbonding pairs. molecular DOES care

84
Q
A

Gen chem (6 decks)

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