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

A

L

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

A

N

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

A

S

23
Q

L = 1 shape is

A

P

24
Q

L = 2 shape is

A

D

25
Q

L= 3 shape is

A

F

26
Q

Magnetic quantum number symbolized by

A

M

27
Q

Magnetic quantum number indicates the

A

Orientation of an orbital around the nucleus

28
Q

Values of m are

A

Whole numbers including zero from -L to +L

29
Q

Orientation of s corresponds to

A

M=0

30
Q

3 p orbitals relate to m values of

A

-1 0 and +1

31
Q

D orientations correspond to m values or

A

-2 -1 0 +1 +2

32
Q

Number of electrons per main energy level

A

2n^2

33
Q

Spin quantum number has only

A

Two possible values -1/2 or +1/2

Which indicate the two fundamental soon states of an electron in an orbital

34
Q

Electron configuration is the

A

Arrangement of electrons in an atom

35
Q

Ground state configuration. Is the lowest

A

Energy arrangement of the electrons for each element

36
Q

Aufbau principle l, an electron occupies

A

The lowest energy orbital that can receive it

37
Q

Pauli exclusion principle, no two electrons in the same atom can

A

Have the same set of four quantum numbers

38
Q

Hund’s rule, orbitals of equal energy are each occupied by

A

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
Q

Noble gases

A

The group 18 elements (helium neon argon krypton xenon and radon)

40
Q

Noble gas notation

A

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
Q

Heisenberg uncertainty principle states that it is

A

Impossible to determine simultaneously both the position and velocity of an electron or any other particle