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Chemistry 101 > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

Specific heat capacity

A

amount of (thermal) energy required to change temperature of 1 degree Celsius of 1.0 g material

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2
Q

Exothermic

A

Delta T < 0

-q

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3
Q

Endothermic

A

Delta T > 0

+q

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4
Q

calorimetry

A

the study of heat flow accompanies a chemical process

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5
Q

When does Delta H=q

A 
As long as q is measured with masses equivalent to make ratios in balanced rxn
ie Ch4(16g/mol)+2O2 etc eqn
question: 16gCh4 in excess O2
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6
Q

-qrxn =

A

+qsoln

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7
Q

+qsoln=

A

(mcDeltaT)soln

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8
Q

light admitted at specific energy values in the spectrum, light source produced light of

A

only specific (or certain) wavelengths

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9
Q

Bohr’s model of the H atom

A

Neils Bohr
-The presence of 4 distinct bands of light in the visible region of the atomic emission spectrum for hydrogen is based on the way energy reacts with certain electorons

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10
Q

how long do electrons stay in an excited state

A

short time

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11
Q

+E to system

A

e- jumps up

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12
Q

from system

A

e- jumps down

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13
Q

Neils bohr’s model to explain the lines spectrum of hydrogen

A

based on classical physics explaining macro scale phenomenon: 4 points

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14
Q

four points of Neil boars model

A
  1. only specific orbits allowed e- resides on orbits
  2. e- in orbit has specific E
    -e- won’t radiate E
    -e- won’t spiral into nucleus
  3. e- jump low –> high must absorb E
    e- jumps high –>low must emit E
  4. use precipitate number (n) to identify orbits
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15
Q

e- wants to be

A

in lowest E

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16
Q

Quantized E

A

specific amount needed for a specific transition Exact! no more no less

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17
Q

e- from high states to low

A

can make stops

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18
Q

e- from low states to high

A

can’t make stops

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19
Q

Delta energy and wavelength

A

as E goes up wave length goes down

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20
Q

frequency and wavelength

A

as wavelength goes up frequency goes down

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21
Q

frequency and delta energy

A

as E goes up frequency goes up

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22
Q

Spectrum

A

400 0

V I B G Y O R

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23
Q

boars model of H atom was good because

A

explained absorption and emissions

-H atom only has 1 e-

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24
Q

boars model of H bad because

A
  • only explains few (one electron) systems
  • violates classical physics
  • violates uncertainty principle:
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25
Q

what was the uncertainty principle

A

can’t know both E and position at the same time

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26
Q

treating electrons as waives in an atom

A
  • particle/wave duality of light

- particle/wave duality of e-

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27
Q

how does light behave

A

like a particle

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28
Q

how fast does the wave travel through space at

A

speed of light

frequency)(wave length

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29
Q

photon

A

light particle, smallest packet of energy

E=h(frequency)

30
Q

how does matter emit and absorb energy

A

in units of hu’s

31
Q

plancles constant

A

h

32
Q

wave calc

A

c=(length)(frequency)

33
Q

particle calc

A

e=h(frequency)

34
Q

what is light

A

the one type of electromagnetic radiation (emr). Oscilating orthogonal wave traveling through space at c (constant speed)

35
Q

waves interacting with atoms

A

Dif waves react Dif w atoms

36
Q

Quantum mechanics

A

treats e- behavior as a wave

-Describe e- wave functions equation

37
Q

Regions in space with high probability of electron density

A

orbitals

38
Q

how many electrons does each orbital hold

A

2

39
Q

S orbital

A

probability density is spherical

-only one allowed

40
Q

P orbital

A

prob. density is peanut shaped

- only 3 allowed

41
Q

D orbital

A

Prob density is doubled up or doughnut

-only 5 allowed

42
Q

F orbital

A

prob density is fancy

-only 7 allowed

43
Q

Energy related to orbitals

A 
1 S
2 S P
3 S P D
4 S P D F
5 S P D F
6 S P D F
7 S P D F
44
Q

n

A

principle quantum number

-Energy level

45
Q

l

A

angular momentum shape

46
Q

Ml

A

magnetic orientation

47
Q

Letter related to l number

A 
S 0
P 1
D 2
F 3
Have a value of n, l is allowed from 0 up to n-1
48
Q

L number related to Ml number

A

0 0
1 -1,0,1
2 -2,-1,0,1,2
3 -3.-2,-1,0,1,2,3

49
Q

Pauli exclusion principle

A

no two e- can have the same set of quantum numbers

50
Q

how to name a quantum

A

(n,l,Ml,Ms)

51
Q

Ms

A

electron

52
Q

Hunds rule

A

maximize parallels spins before spin pair

53
Q

Degenerate

A

same enegy

54
Q

AUFBAV principle

A

fill orbitals from low E–>high E

55
Q

Noble gasses

A

Stable because of electron conferrence are composed of full and closed shells

56
Q

Valence electron

A

Do all the work: gained, lost, involved in reactions, and bonding

57
Q

Transition metals

A

Don’t follow an 8 valence electron rule; follow an 18 valence electronic rule

58
Q

What are the exceptions to transition metals following the 18 valence e rule

A

Cr
Mg
Cu
Ag

59
Q

Spin pairing energy

A

When energy change costs energy

-delta E between orbits

60
Q

Energy to promote v energy to pair

A

Less energy to promote than to pair

61
Q

Atom to cation

A

Size decreases because it

Loses electrons and more protons pull electrons harder

62
Q

Atom to anion

A

Size increases bc gains electrons and less protons so weaker pull

63
Q

Period left to right in terms of atom size

A

Size decreases because pull towards nucleus increases

64
Q

Size of atoms group top to bottom

A

Size increases because N is related to size

65
Q

Effective nuclear charger (Zeff) period left to right

A

Increases (#P-#core electrons)

66
Q

Effective nuclear charge (Zeff) group too to bottom

A

Stays the same

67
Q

Number of core electrons

A

Atomic number of noble gas before element

68
Q

Zeff

A

Never negative

Always less than Z

69
Q

Trends on periodic table

A 
Effective nuclear charge (Zeff)
Size of atoms/ions
Ionization energy (Ez)
70
Q

Valence electron attraction

A

Only attracted to a portion of the total net nuclear charge

71
Q

Isoelectronic Set

A

Cations, anions, neutral all with same electron configuration

72
Q

What is shield build from between inside protons and outside valence electron

A

Build from core electrons block full nuclear charge from pulling on valence electrons

Chemistry 101 (4 decks)

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