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Advanced Higher Chemistry > Atomic Orbitals, Electron Configuration and The Periodic Table > Flashcards

Atomic Orbitals, Electron Configuration and The Periodic Table Flashcards

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1
Q

How are atomic spectra caused?

A

By electrons moving between different energy levelS.

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2
Q

What does the Quantum theory state?

A

That matter can only emit or absorb energy in small fixed amounts.

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3
Q

What is a quanta?

A

The certain fixed amount of energy an electron can possess.

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4
Q

What do quantum numbers define?

A

The energy of the electron.

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5
Q

What is the principle quantum number?

A

Electrons in atoms are arranged in a series of shell and each shell is described in a number. Represented by n

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6
Q

what is the relationship between n and the potential energy?

A

The higher the value of n, the higher the potential energy associated with the shell and the further from the nucleus the electron is likely to find.

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7
Q

What is the Pauli exclusion principle?

A

No two electrons in the same atom can have the same set of four quantum numbers.

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8
Q

What are the four quantum numbers?

A 
n = principle quantum numbers
l = angular momentum quantum numbers
ml = magnetic quantum number
ms = spin magnetic quantum number
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9
Q

What does the principle quantum number, n refer to?

A

Related to the size of the orbital, the numbers determine the size and energy of the shell.

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10
Q

What does the angular momentum quantum number refer to?

A

Determines the shape of the sub-shell and is labelled as s, p, d ,f. This can have a value from 0 to n-1

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11
Q

What orbital is present when l=0?

A

s orbital

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12
Q

What orbital is present when l=1

A

p orbital

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13
Q

What orbital is present when l=2

A

d orbital

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14
Q

What orbital is present when l=3

A

f orbital

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15
Q

How many electrons can an orbital hold?

A

Two electrons

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16
Q

How many s orbitals can be in each energy level?

A

One

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17
Q

How many p orbitals can be in each energy level?

A

Three

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18
Q

How many d orbitals can be present in each energy level?

A

Five

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19
Q

What is degenerate?

A

Orbitals that have the same energy/equal energy

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20
Q

What does Hund’s rule state?

A

Electrons fill degenerate orbitals singly with parallel spins before pairing up to fill the orbital.

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21
Q

What does aufbau principle state?

A

Electrons fill orbitals in order of increasing energy. Lowest energy subshells are filled first.

22
Q

What is magnetic quantum number?

A

Determines the orientation of non-spherical orbitals (p, d and f). This can have a value of -l to +l

23
Q

What is the range of values of magnetic quantum numbers in s orbitals?

A

ml will always equal 0

24
Q

What is the range of values of magnetic quantum numbers in p orbitals?

A

ml = -1,0,+1

25
Q

What is the range of values of magnetic quantum numbers in d orbitals?

A

ml = -2, -1, 0, 1, 2

26
Q

What is the spin magnetic number?

A

Indicaes the spin of an electron withn an orbital. Electrons will have opposite spins and can be either clockwise +1/2 or anticlockwise -1/2.

27
Q

What does ml stand for?

A

Magnetic quantum number

28
Q

What does ms stand for?

A

Spin magnetic quantum number

29
Q

What does l stand for?

A

Angular momentum number.

30
Q

what does n stand for?

A

principle quantum number

31
Q

What is the principle quantum number?

A

Related to the size of the orbital, the numbers determines the size and energy of the shell.

32
Q

What is the angular momentum quantum number?

A

Determines the shape of the sub-shell and is labelled as s, p, d, f. This can have a value from zero to n-1

33
Q

What does l = 0 signify?

A

Identify an s orbital (singular)

34
Q

What does l = 1 singify?

A

Identifies a p orbital (multiple)

35
Q

What does l = 2 signify?

A

Identifies a d orbital (multiple)

36
Q

What does l = 3 signify?

A

Identifies a f orbital (multiple)

37
Q

How many electrons maximum can an orbital hold?

A

2

38
Q

How many electrons can the first shell hold?

A

2

39
Q

How many electrons can the second shell hold and what types of orbitals would be present?

A

Can hold up to 8 electrons and would have 1s orbital and 3p orbitals.

40
Q

What does degenerate mean?

A

Orbitals that have the same energy are said to be degenerate.

41
Q

What does Hund’s rule state?

A

Hund’s rule states that when degenerate orbitals are available, electrons will fill each singly before pairing up.

42
Q

What does the aufbau principle state?

A

Electrons fill orbitals in order of increasing energy level.

43
Q

How many electrons could the third shell hold and what types of orbitals are present?

A

Can hold a maximum of 18 electrons with 1s, 3p and 5d.

44
Q

What is the magnetic quantum number (ml)?

A

Determines the orientation of non-spherical orbitals (p, d, f) and can have a value between -l and +l

45
Q

What the the ml values for different orbitals?

A

s: ml = 0
p: ml = -1, 0 or +1
d: ml = -2, -1, 0, +1

46
Q

What is the spin magnetic quantum number (ms)?

A

Indicates the spin of an electron within an orbital. Electrons pairs will have opposite spins and can be either clockwise +1/2 or anticlockwise -1/2

47
Q

What does the Pauli exclusion principle state?

A

No two electrons in the same atom can have the same set of four quantum numbers.

48
Q

Why does the 4s orbital fill before the 3d orbital?

A

The 4s orbital has lower energy than 3d therefore it will fill first.

49
Q

Why is an outer electron removed from 4s orbital instead of 3d orbital?

A

4s has lower energy than 3d therefore it is easier to remove an electron from 4s.

50
Q

what is ionisation energy?

A

The energy required to remove one mole of electrons from one mole of gaseous atoms.

51
Q

When will an element have higher ionisation energy?

A

When the orbital has two electrons making it stable or when there are half filled shells.

Advanced Higher Chemistry (14 decks)

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