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Chemistry > Electronic Structure and ionisation energy > Flashcards

Electronic Structure and ionisation energy Flashcards

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1
Q

How many orbitals in the a subshell ?

A

1

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2
Q

How many orbitals in the p subshell ?

A

3

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3
Q

How many orbitals in the d subshell ?

A

5

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4
Q

How many orbitals in the f subshell ?

A

7

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5
Q

Electrons fill up the what energy sublevels first

A

Lowest

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6
Q

What’s special about 3D and 4s ?

A

4s has lower energy level so it is filled up first

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7
Q

In orbitals describe the motion of the electrons

A

The electrons spin in opposite directions

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8
Q

How do electrons full orbitals ?

A

Singly before they start sharing

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9
Q

What is the electron configuration for chromium ?

A

3d^5, 4s^1

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10
Q

What is the electron configuration for copper ?

A

3d^10 4s^1

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11
Q

Why do copper and chromium donate one of their 4s electrons to the 3D sub shell ?

A

They’re happier with a more stable full or half full d sub shell

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12
Q

What else is special about transition metals ?

A

They loose their 4s electrons beige their 3D electrons even though the 4s electron she’ll is filled first

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13
Q

What is ionisation energy ?

A

The enthalpy change needed to remove 1 mole of electrons from 1 mole of gaseous atoms

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14
Q

What is the equation for the first ionisation energy ?

A

X(g) –> X+(g) +e-

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15
Q

What are the 3 factors affecting ionisation energy ?

A

Nuclear charge , distance from the nucleus and shielding

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16
Q

How does nuclear charge effect ionisation energy ?

A

The more protons there are in the nucleus the more positively charged the nucleus is and the stronger the attraction for the electrons.

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17
Q

How does distance from nucleus effect the ionisation energy ?

A

The closer the electron is to the nucleus the more strongly it will be attracted to the nucleus

18
Q

How does shielding effect ionisation energy ?

A

As the number of electrons between the outer electrons and the nucleus increases the outer electrons feel less attraction towards the nuclear charge. This lessens the pull of the nucleus

19
Q

What does successive ionisation energy involve ?

A

Removing additional electrons

20
Q

What is the definition of second ionisation energy ?

A

The enthalpy change required to removed 1 mole of electrons from 1 mole of gaseous ions to for 2+ ions

21
Q

Why within each she’ll do successive ionisation energies increase ?

A

As the electrons are being removed from and increasingly positive ion with less repulsion amongst the remaining electrons so they are held strongly by the nucleus

22
Q

Why are there big jumps when new shells are broken into ?

A

An electron is being removed from a shell that is closer to the nucleus

23
Q

What is the trend in first ionisation energy as you go down a group ?

A

The first ionisation energy decreases

24
Q

What is the trend in first ionisation energy as you go across a period ?

A

Increases

25
Q

What do graphs showing first ionisation energy energy down a group provide evidence for ?

A

That electron shells exist

26
Q

Why is it that ionisation energy decreases as you go down group 2 ?

A

Bea she there is shielding from the inner shells which shields the outer electrons from the attraction of the nucleus
Also the extra shells mean that the outer electrons are further away from the nucleus do the nucleus’ attraction will be greatly reduced.

27
Q

Why is it that as you go across the period the ionisation energy increases ?

A

This is due to change of the nucleus increasing as number of protons increases so there is a stronger nuclear attraction.
All the extra electrons are at roughly the same energy level ( similar shielding )

28
Q

Why is there a small drop from magnesium to aluminium in ionisation energy as you go across period 3 ?

A

Because aluminium a outer electron is in a 3p orbital rather than 3s. 3p orbital has a slightly higher energy than 3s orbital. So the electron is on avenger further from the nucleus
Also the 3p orbital has the additional shielding from the 3s^2 electrons

29
Q

In period 3 why is there a drop between group 5 and group 6 ( phosphorus and sulfur) ?

A

This is due to electron repulsion
Shielding is identical
Phosphorus soured electron is removed from a singly occupied orbital whereas in sulphur the electron is being removed from an orbital containing 2 electrons. More repulsion - easier to remove

30
Q

What is 1 mole ?

A

6.02 X 10^23

31
Q

What is the equation to find out mass , moles and mr?

A

Mass = mrx mole

32
Q

What is the equation for concentration ?

A

Concentration = moles/volume

33
Q

In the concentration calculation what is volume measures in ?

A

Dm ^3

34
Q

What is the units for concentration ?

A

Mol dm ^-3

35
Q

How do u convert cm^3 into dm^3 ?

A

Divide by 1000

36
Q

What is the ideal has equation ?

A

pV =nRT

37
Q

What is the unites for pressure ?

A

Pa

38
Q

What is the units for volume in the idea has equation ?

A

M^3

39
Q

What is the units for temperature in the ideal gas equation ?

A

K

40
Q

How do u convert degrees Celsius into k ?

A

+ 273

41
Q

What’s the maximum number of electrons can orbitals hold ?

A

2

Chemistry (7 decks)

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