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F321 Chemistry > Electronic Structure > Flashcards

Electronic Structure Flashcards

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1
Q

What is the name given to the shell and its distance from the nucleus?

A

Principal quantum number.

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2
Q

What is the principle quantum number of the first shell?

A

1

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3
Q

What is the principle quantum number of the second shell?

A

2

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4
Q

What is the principle quantum number of the third shell?

A

3

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5
Q

What gives a shell a larger principal quantum number?

A

The further the shell is from the nucleus.

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6
Q

What sub shell does the 1st shell contain?

A

1s

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7
Q

What sub shells does the 2nd shell contain?

A

2s and 2p

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8
Q

What sub shells does the 3rd shell contain?

A

3s, 3p and 3d.

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9
Q

What sub shell does the 4th shell contain?

A

4s, 4p, 4d and 4f.

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10
Q

What is the number or orbitals and maximum electrons for the s sub-shell?

A

Number of orbitals- 1

Maximum electrons- 2

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11
Q

What is the number or orbitals and maximum electrons for the p sub-shell?

A

Number of orbitals- 3

Maximum electrons- 6

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12
Q

What is the number or orbitals and maximum electrons for the d sub-shell?

A

Number of orbitals- 5

Maximum electrons- 10

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13
Q

What is the number or orbitals and maximum electrons for the f sub-shell?

A

Number of orbitals- 7

Maximum electrons- 14

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14
Q

What is the s orbital shape?

A

Spherical

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15
Q

What is the p orbital shape?

A

Dumbell-shaped.

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16
Q

What 3 ways can you show electron configuration?

A

Sub shell notation
Arrows in boxes
Energy level diagrams

17
Q

Which electron shells are filled up first?

A

Electrons fill orbitals singly before they start sharing, so the two electrons in the 2p sub-shells should be in separate orbitals.

18
Q

Which one of the first, second or third ionisations of thallium produces an ion with the electron configuration [Xe] 5d10 6s1?

A

Second

19
Q

State the general trend in first ionisation energies from carbon to neon.
Deduce the element that deviates from this trend and explain why this element deviates from the trend.

A

Increase
Oxygen / O
Paired electrons in a (2)p orbital

20
Q

Write an equation, including state symbols, for the reaction that occurs when the first ionisation energy of carbon is measured.

A

C(g) → C+(g) + e(-)

21
Q

Explain why the second ionisation energy of carbon is higher than the first ionisation energy of carbon.

A

(More energy to) remove an electron from a (more) positive ion.

22
Q

Deduce the element in Period 2, from lithium to neon, that has the highest second ionisation energy.

A

Lithium

23
Q

Explain the trend of increase across Period 2 of ionisation energy.

A
  • Number of protons increases.
  • Outermost electrons are in the same shell
  • Greater nuclear attraction (on outermost electrons)
24
Q

The first ionisation energy of oxygen is less than the first ionisation energy of fluorine.

A
  • O has one less proton and so a smaller nuclear charge.
  • Atomic radius of O is larger.
  • Outer electrons are attracted less strongly (to the nucleus) in O.
25
Q

When oxygen reacts with metals it forms oxide ions.
Write the electron configurations, in terms of sub-shells, of an oxygen atom and an oxide ion.
Hence, explain why this reaction of oxygen is typical of a non-metal.

A

1s2 2s2 2p4 and 1s2 2s2 2p6

In the reaction oxygen has formed a negative ion (by gaining two electrons.

26
Q

Complete the electron configuration of a magnesium atom.

A

1s2 2s2 2p6 3s2

27
Q

Write an equation to represent the second ionisation energy of magnesium. Include state symbols.

A

Mg+(g) -> Mg2+(g) + e–

28
Q

Explain why there is an increase in first ionisation energy between F and Ne.

A

Ne has one more proton
Outermost electrons are in the same shell
Greater nuclear attraction on outermost electrons

29
Q

Explain why there is a decrease in first ionisation energy between Ne and Na.

A

Na has one more shell
Outermost electron experiences greater shielding
Less nuclear attraction on outermost electrons

30
Q

Why is the first ionisation energy of strontium larger than the first ionisation energy of rubidium?

A

Sr has one more proton and therefore greater nuclear charge.
Atomic radius of Sr is smaller.
Sr has greater nuclear attraction on outer electrons / outer shell.

31
Q

Why is the second ionisation energy of rubidium larger than the second ionisation energy of strontium?

A

2nd IE of Rb involves removing electron from shell.

Stronger nuclear attraction on outermost electron of Rb.

32
Q

Explain why xenon has a lower first ionisation energy than neon.

A

Xe has a bigger atomic radius and more shielding.

33
Q

What is meant by an orbital?

A

A region (within an atom) that can hold up to two electrons with opposite spin.

34
Q

State the total number of electrons occupying the p orbitals in one chlorine atom.

A

11

35
Q

How many electrons are there in one ion of Ca2+?

A

18

36
Q

Write the equation that represents the third ionisation energy of Al.

A

Al2+(g) -> Al3+(g) + e–

37
Q

Define successive ionisation energy

A

A measure of the energy required to remove each electron in turn.

F321 Chemistry (25 decks)

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