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Chemistry Semester 2 > Unit 7- Electrons > Flashcards

Unit 7- Electrons Flashcards

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1
Q

Hund’s rule

A

Electrons fill one per orbital in the same sublevel before pairing up
-If they have the option, they will pick another orbital rather than join an orbital where they have to share with another electron

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2
Q

Thompson model

A
  • 1870

- Plum pudding with the one positive charge and multiple negative charges

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3
Q

Electrons are place in orbitals of lowest energy was first stated by

A

Aufbau

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4
Q

What aspects of Bohr’s model did we change

A
  • Electrons do not move around in predictable paths

- Shapes of orbitals are not all circular

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5
Q

Color speed relationship

A

All are the same

3.00x 10^8 m/s

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6
Q

How do you tell how big an electron jump is

A

The bigger the electron jump, the bigger the energy

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7
Q

What color has the longest wavelength

A

Red

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8
Q

Pauli Exclusion principal

A

Maximum 2 electrons per orbital with opposite spins

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9
Q

How do energy and wavelength relate

A

They are opposites

-With high energy, there is low wavelength

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10
Q

JJ Thompson discovery

A
  • Energy is moved by a magnet-> energy beam has a negative charge
  • “something” has mass
  • Particle
  • Subparticle inside an atom (metal)
  • Plum pudding model (pudding is positive and plums are negative)
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11
Q

Most stable orbitals

A
  1. Completely filled up P orbitals
  2. Completely filled other orbitals (D,S,F)
  3. Exactly half filled orbitals
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12
Q

Problems with Bohr

A
  • Heisenberg Uncertainty principle: 1920’s
  • It is impossible to know both the location and velocity of electrons
  • We are no longer looking for exact locations-> now we’re looking for where they are likely located “areas of probability” (90% of the time)
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13
Q

How do frequency and wavelength relate

A

As wavelength decreases, frequency increases as long as speed is maintained

  • Wavelength times frequency equals speed of wave (3.00 times 10^8 meters per sec
  • W times F = C
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14
Q

Wavelength

A

The distance between consecutive waves (represented by w or an upside down y)

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15
Q

Orbital notation rule

A

Electrons spread out before they pair up and pair up before they move up.

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16
Q

What orbital is shaped like a 4 leaf clover

A

D orbitals

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17
Q

F orbital

  • Shape
  • Number of orbitals
  • First energy level
  • Number of electrons
A

Shape- complicated
# of orbitals- 7
1st energy level- 4
# of electrons- 14

18
Q

Schrodinger’s Wave mechanical modle

A

Calculated “regions of probability” (orbitals) for electrons

about 90% of the time or for 90% of electrons

19
Q

What aspects of Bohr’s model did we keep

A
  • Energy levels established by Bohr have remained the same

- Electrons moving outside the nucleus have remained the same

20
Q

Orbital notation

A

Shows whether elections are are paired or unpaired and whether the orbitals are empty or full
-This effects stability

21
Q

How do the +/- work with electrons

A

+ # electrons is losing electrons

- # electrons is gaining electrons

22
Q

p orbital

  • Shape
  • Number of orbitals
  • First energy level
  • Number of electrons
A

Shape: Infinity sign
# of orbitals: 3
1st energy level: 2
# of electrons- 6

23
Q

Orbital conclusion

A

Electrons will spread out before they pair up and pair up before they move up in energy

24
Q

D orbital

  • Shape
  • Number of orbitals
  • First energy level
  • Number of electrons
A 
Shape- four leaf clover or infinity sign through a donut
# of orbitals- 5
1st energy level- 3
# of electrons- 10
25
Q

Why do noble gases not react

A

They are the most stable, they have completely filled P orbitals, everything else will try to get higher on the list and if they can’t get higher, they tend to be relatively stable. (If it is difficult to move up, they are stable bc they don’t want to move down)

26
Q

Building to a new model- Debroglie

A

-1923
-Theory that matter has wavelike properties
w= h divided by mass time velocity
-We don’t see wave movement because the wavelength is so incredibly small.H= 6.626 times 10 neg 34

27
Q

Energy

A

Energy of a wave is directly related to frequency (represented by e)

28
Q

Frequency

A

The number of waves that pass in a second (represented by f)

29
Q

Unstable wave pattern

A

-When energy is added, it collapses and doesn’t create color that we can see because it emits color too quickly for us to see it before it collapses

30
Q

What color would correspond to the largest electron jump out of:
Blue, Red, yellow, and orange

A

Blue, bigger energy means bigger jump

31
Q

Aufbau principle

A

Electrons fill the lowest available energy orbitals first

32
Q

S orbital

  • Shape
  • Number of orbitals
  • First energy level
  • Number of electrons
A

Shape- Circle or sphere
# of orbitals: 1
1st energy level: 1
# of electrons: 2

33
Q

What scientist is credited with the idea that particles have wavelike properties

A

DeBroglie

34
Q

Color highest to lowest energy

A 
Violet (smallest wavelength)
Blues
Greens
Yellows
Oranges
Reds (highest wavelength)
35
Q

If a sample of EM radiation has a long wavelength,it has a relatively_____ energy

A

Low

36
Q

Bohr’s model of the atom was the

A

Solar system model

37
Q

Stable wave pattern

A
  • Traces same path

- When energy is added it makes color that we can see because it emits color for a long enough time that we can see it

38
Q

Least stable orbitals

A

-Partially filled orbitals

39
Q

Building to a new model- -Planck and Einstein

A
  • Working with light

- Light has dual nature (wave properties and particle properties)

40
Q

Dalton model

A

-1807

Just a circle

41
Q

Rutherford/Bohr model

A
  • 1910/1930

- Orbital system. One center and multiple rings around the center

Chemistry Semester 2 (5 decks)

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