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Alia - Chemistry > Lecture 5/6-The Electronic Configuration Of The Atom > Flashcards

Lecture 5/6-The Electronic Configuration Of The Atom Flashcards

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1
Q

Where are e- in an atom?

A

In stable energy levels

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2
Q

What does the absorbtion of a photon of light do?

A

Allow the e- to jump to a higher level

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3
Q

What does the jumping down of an e- to a lower level do?

A

Emits a photon of light

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4
Q

If you measure the energy of the photon that has jumped up + down, what will you find?

A

The energy difference between levels (they are not evenly spaced)

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5
Q

What is 1st ionisation energies?

A

The energy required to remove 1 mole of e- from 1 mole of gaseous atoms to form one mole of positive ions

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6
Q

Why are ionization energies positive?

A

Energy must be put into the system to pull the negative e- away from the positive protons

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7
Q

Why does higher nuclear charge have a higher ionization energy?

A

Because there is a greater pull of the nucleus on the e-

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8
Q

What is e- affinity?

A

The energy required to add 1 mole of e- to 1 mole of gaseous atoms to form 1 mole of gaseous negative ions

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9
Q

Cl-(g) + e- —> Cl-(g)

A

E- affintiy

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10
Q

The more negative the e- affinity the ……

A

more STABLE the negative ion

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11
Q

Why is the 2nd e- affinity positive?

A

Because energy needs to be put in to add e- to a negative ion

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12
Q

Atomic size trends

A

Increases down a group

Decreases across a period

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13
Q

1st Ionization energy trends

A

Decrease down the group

Increase across a period

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14
Q

1st E- affinity trends

A

Less negative down a group

More negative across a period

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15
Q

What are orbitals?

A

Regions in space where there’s a 95% probability finding a particular e-

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16
Q

What does the quantum number n indicate

A
  • The distance of an e- from the nucleus
  • The energy of an e-
  • Number of e- a shell can hold
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17
Q

The higher the quantum number n the?

A

The further away from the nucleus the e- is

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18
Q

Higher energy e- are less tightly held and so….

A

more easily removed (higher n)

19
Q

n can have how many electrons?

A

2n^2

20
Q 
How many e- can:
K shell
L shell
M shell
N shell
have?
A

K shell n=1 ,so e- = 2
L shell n=2 ,so e-=8
M shell n=3 ,so e-=18
N sheel n=4 ,so e-=32

21
Q

What is a subshell?

A

A group of orbitals with the same energy

22
Q

The value of l depends on what quantum number?

A

n

23
Q

What values can l have?

A

From 0 to n-1

24
Q

What are spin quantum numbers?

A

The clock-wise + anticlockwise spinning of e- produces opposite magnetic fields

25
Q

Why is Gd3+ used for medical imaging?

A

The 7 unpaired electrons have the same spin (½) but a much smaller size than protons so it can be magnetized @RT

26
Q

What other ions/elements can be used for medical imaging?

A

Iron , nickel , cobalt

27
Q

What does the Azimuthal quantum number indicate?

A

The subshell an e- is in

28
Q 
If the value of l is:
-0
-1
-2
-3
what subshell is it in?
A

0=s
1=p
2=d
3=f

29
Q

Does the energy of the subshell increase with increasing of l?

A

YES

30
Q

What is the maximum number of e- a given subshell can hold?

A

2(2l+1)

31
Q 
If l is
0=s
1=p
2=d
3 =f
then how many e- can it hold
A

s=2
p=6
d=10
f=14

32
Q 
What is the shape of the:
s orbital
p orbital
d orbital
f orbital
A 
s = spherical
p = dumbbell
d = more complex
f = still more complex
33
Q

What do magnetic quantum numbers represent ? (m/m1)

A

The orbitals in a given subshell

34
Q

What do magnetic quantum numbers indicate?

A

The direction of a particular orbital relative to the magnetic field/axes

35
Q

Does magnetic quantum numbers indicate energy?

A

NO

36
Q

m can have an integral value of what?

A

-1 through 0 to +1

37
Q

For a given value of l, total number of m value is what?

A

(2l+1)

38
Q

Heisenberg’s uncertainty principle

A

You cannot determine the position + momentum of an e- at the same time

39
Q

Aufbau principle

A

E- enter the lowest available energy level 1st

40
Q

Hund’s rule of max multiplicity

A

When in orbitals of equal energy , e- will try to remain unpaired (minimises repulsion between like charges , so the system is more stable)

41
Q

Pauli exclusion principle

A

No 2 e- can have the same 4 quantum numbers

-Only 2 e- can go in each orbital , if they’re of opposite spin

42
Q

What are the special cases / exceptions?

A 
Chromium = 4s1 3d5
Copper = 4s1 3d10
43
Q

A large jump between successive ionisation energy indicates what?

A

A change in energy level from which the e- has been removed

Alia - Chemistry (12 decks)

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