(c) electron configuration and atomic orbitals Flashcards

1
Q

What does a quantum number describe?

A

An electrons location in space.

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2
Q

How many numbers make up a quantum number?

A

4

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3
Q

What does the first quantum number represent?

A

An electrons energy level.

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4
Q

What does the second quantum number represent?

A

An electrons sub-shell/ orbital.

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5
Q

What does the third quantum number represent?

A

The orientation of the orbital.

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6
Q

What does the fourth quantum number represent?

A

The spin of the electron.

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7
Q

What is important regarding quantum numbers within electrons?

A

That no two electrons can have the same quantum number.

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8
Q

What is the first quantum number also known as?

A

The principle quantum number.

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9
Q

How is the first quantum number denoted?

A

The letter ‘n’.

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10
Q

What is an orbital?

A

An area of space where you could find an electron.

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11
Q

What is the likelihood of finding an electron in an orbital?

A

90%

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12
Q

What makes electrons similar to photons?

A

They both have wave/ particle duality.

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13
Q

How are orbitals/ sub-shells denoted?

A

The letter ‘L’.

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14
Q

What is the range of L?

A

L=0-> n-1

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15
Q

If n=3 what does L equal?

A

L=0,1,2

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16
Q

What does the different values of L relate to?

A

The different shaped orbitals.

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17
Q

If L=0 what is the type and shape of the orbital?

A

S orbital and a sphere.

18
Q

If L=1 what is the type and shape of the orbital?

A

P orbital and dumbbell.

19
Q

If L=2 what is the type and shape of the orbital?

A

d orbital and double dumbbell.

20
Q

If L=3 what is the type of orbital?

A

f.

21
Q

What is the third quantum number represented by?

A

M L.

22
Q

What is the range of ML?

A

ML= -L->+L

23
Q

For L=0 what does ML equal?

A

0

24
Q

If ML equals 0 how many numbers are there and by association how many orientations are there?

A

1 number so 1 orientation.

25
Q

How many orientations does the S orbital have?

A

1

26
Q

For L=1 what does ML equal?

A

-1, 0, +1

27
Q

If ML=-1, 0, +1 how many numbers are there and therefore how many orientations are there?

A

3 numbers so 3 orientations.

28
Q

How does the dum bell change its orientation to fit 3 orientations on a cartesian diagram?

A

The dumbbell lies on each different axis.

29
Q

How many orientations does the P orbital have?

A

3

30
Q

For L=2 what does ML equal?

A

ML= -2,-1,0,1,2

31
Q

If ML=2 how many numbers are there and therefore how many orientations are there?

A

5 numbers so 5 orientations.

32
Q

What does dz^2 look like?

A

A dumbbell along the z axis with a circle around the middle at the origin.

33
Q

How many orientations does the d orbital have?

A

5

34
Q

If L=3 what does ML equal?

A

ML=-3,-2,-1,0,1,2,3

35
Q

if ML=3 how many numbers are there and therefore how many orientations are there?

A

7 numbers so 7 orientations.

36
Q

What is the fourth quantum number represented by?

A

Ms

37
Q

If a single headed arrow is pointing up what is its number?

A

+1/2

38
Q

If a single headed arrow is pointing down what is its number?

A

-1/2

39
Q

What does Aufbaus’ Principle state?

A

Electrons must fill the lowest energy orbitals first.

40
Q

What does the Pauli exclusion principle state?

A

Orbitals can hold a maximum of 2 electrons and these electrons must have opposite spins.

41
Q

What is Hunds’ rule?

A

If there are degenerate (same energy) orbitals, electrons will fill unoccupied orbitals before ‘doubling up’.

42
Q

What is the correct order for increasing energy levels in orbitals for box notation?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 4d, 4f.