6+7 Flashcards

1
Q

C=

A

Wavelength * frequency

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2
Q

H * frequency =

A

Energy

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3
Q

E =

A

C* H / wavelength

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4
Q

What is h

A

6.626x10^-34

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5
Q

What is c

A

2.998x10^8

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6
Q

10 Å =

A

1 nm

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7
Q

I m =

A

10^10 Å

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8
Q

/\ E =

A

-RvH(1/nf^2-1/ni^2)

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9
Q

n=

A

Principle QN

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10
Q

l=

A

Angular momentum QN

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11
Q

ml =

A

Magnetic QN

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12
Q

ms=

A

Magnetic spin

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13
Q

How do you get the max # of e-

A

2(n)^2

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14
Q

What is l

A

Spdf

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15
Q

How do you figure out ml

A

-l to +l

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16
Q

What does the s orbital look like

A

A circle

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17
Q

What does the P orbital look like

A

An 8

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18
Q

What does the d orbital look like

A

8’s crossing X

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19
Q

Ms= ^ = v=

A
^ = +1/2 
V = -1/2
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20
Q

Hund’s rule

A

For degenerate orbitals the lowest energy is attained when the # of e- with the same spin is maximized

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21
Q

Irregularities

A

Occur when e- want to half fill s + d orbitals

22
Q

4s2 3d4 will turn into what if irregular

23
Q

Electron configuration

A

1s2 2s2 2p6 …

24
Q

Orbital diagram

A

^v ^v ^v^v^v

25
Dmitri Mendeleev
Came to the conclusion that elements should be grouped
26
Henry Moseley
Came up with the concept of atomic #
27
What do you add as you grow across a period
E-
28
What do you add as you go down a group
Energy levels
29
List the order of increasing size for cations anions and parents
Cations parents anions
30
Isoelectronics
Have the same # of e- | Same electron configuration
31
Ionizations energy
Minimum amount of energy it takes to remove an e-
32
What happens to ionization energy as it goes across a period
Increase
33
What happens to ionizations energy as it does down a group
Decrease
34
Electron affinity
When you add an e- | Exothermic
35
Electronegativity
Ability of an e- to attract e-s to itself
36
What happens to electronegative as it goes down a group
Decreases
37
What happens to Electronegativity as you go across a period
Increase
38
What happens to atomic radius as you go down a group
Increase
39
What happens to atomic radius as you go across a period
Decrease
40
What happens to s and P groups when they are with transition metals
Colored because metal ions can have a +1 oxidation #
41
What color flame does Li have
Red pink
42
What color flame does Na have
Orange
43
What color flame does K have
Purple
44
How do you get absorbable into %
``` Y = absorbance X = molarity X*L of solution = moles Moles / mass from periodic table Mass / total mass * 100 ```
45
What color is close to 400
Purple
46
What color is close to 700
Red
47
Rh =
2.18x10^-18
48
Avagadros #
6.022x10^23
49
Units for frequency
1/s
50
Units for wavelength
m
51
Units for E
J/ photon
52
Home many visible lines are there on the light spectrum for H
4