Chapter 4 Quarterly notes Flashcards

1
Q

Heisenbergs proposal answers question of where electrons are

A

Located if they are both par files and wave s

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2
Q

(Heisenberg) electrons are detected by their

A

Interaction with photons

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3
Q

(Heisenberg) because photons have about the same energy as electrons any attempt to locate a specific electron with a

A

Photon knocks the electron off its course

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4
Q

Erwin schrodingers used the hypothesis that electrons have a dual wave particle nature and

A

Developed an equation that treated electrons in atoms as waves

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5
Q

Quantization of electron energies was a

A

Natural outcome of schrodingers equation

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6
Q

Only waves of specific energies, and thus frequencies provide

A

Solutions to the equation

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7
Q

Quantum theory describes mathematically the

A

Wave properties of electrons and other very small particles

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8
Q

Electrons do not travel around the nucleus in

A

Neat orbits

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9
Q

Electrons exist in certain regions called

A

Orbitals

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10
Q

An orbital is a three dimensional

A

Region around the nucleus that indicated the probable location of an electron

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11
Q

Electrons in atoms orbitals also have

A

Quantized energies

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12
Q

An electrons energy level is not the only characteristic of an orbital that is indicated by

A

Solving the schrodinger equation.

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13
Q

Quantum numbers specify the properties of

A

Atomic orbitals and the properties of electrons in orbitals

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14
Q

Principal quantum number symbolized by

A

N

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15
Q

Principal quantum number indicates the

A

Main energy level occupied by the electron

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16
Q

Total number of orbitals in a given shel is equal to

A

n^2

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17
Q

Angular momentum quantum number symbolized by

18
Q

Angular momentum quantum number indicates the

A

Shape of the orbital

19
Q

For specific main energy level number of orbital shapes possible is equal to

20
Q

Values of n are

A

Positive integers only

21
Q

Values of l are zero and all

A

Positive integers less than or equal to n - 1

22
Q

When l equals 0 the shape is

23
Q

L = 1 shape is

24
Q

L = 2 shape is

25
L= 3 shape is
F
26
Magnetic quantum number symbolized by
M
27
Magnetic quantum number indicates the
Orientation of an orbital around the nucleus
28
Values of m are
Whole numbers including zero from -L to +L
29
Orientation of s corresponds to
M=0
30
3 p orbitals relate to m values of
-1 0 and +1
31
D orientations correspond to m values or
-2 -1 0 +1 +2
32
Number of electrons per main energy level
2n^2
33
Spin quantum number has only
Two possible values -1/2 or +1/2 | Which indicate the two fundamental soon states of an electron in an orbital
34
Electron configuration is the
Arrangement of electrons in an atom
35
Ground state configuration. Is the lowest
Energy arrangement of the electrons for each element
36
Aufbau principle l, an electron occupies
The lowest energy orbital that can receive it
37
Pauli exclusion principle, no two electrons in the same atom can
Have the same set of four quantum numbers
38
Hund's rule, orbitals of equal energy are each occupied by
One electron before any orbital is occupied by s second electron and all electrons in singly occupied orbitals must have the same spin state
39
Noble gases
The group 18 elements (helium neon argon krypton xenon and radon)
40
Noble gas notation
To simply writing an electron configuration symbol for the previous noble gas is enclosed in square brackets is used to represent part of the configuration
41
Heisenberg uncertainty principle states that it is
Impossible to determine simultaneously both the position and velocity of an electron or any other particle