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CHEM A LEVEL > Electron Configuration > Flashcards

Electron Configuration Flashcards

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1
Q

What are main energy levels/ shells split into?

A
  • Sub-shells (orbitals.)
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2
Q

What are the 4 types of orbitals?

A
  • s,p,d,f.
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3
Q

How many sub-orbitals does an s orbital contain?

A
  • One sub- orbital.
    MAXIMUM NUMBER OF ELECTRONS IN SUB SHELL = 2
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4
Q

How many electrons does 1 sub- orbital hold?

A
  • 2 electrons.
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5
Q

How many sub -orbitals does a p orbital cotain?

A
  • Three sub- orbitals
    MAXIMUM NUMBER OF ELECTRONS IN SUB-SHELL = 6
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6
Q

How many sub- orbitals does a d orbital contain?

A
  • Five sub- orbitals
    MAXIMUM NUMBER OF ELECTRONS IN SUB-SHELL = 10
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7
Q

What sub-shell does the first energy level have?

A
  • An s sub-shell.(orbital)
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8
Q

What sub-shells does the second energy level have?

A
  • An s sub-shell. (orbital)
  • A p sub shell. (orbital)
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9
Q

What sub-shells does the third energy level have?

A
  • An s sub-shell (orbital)
  • A p sub-shell (orbital)
  • A d sub-shell (orbital.)
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10
Q

What sub-shells does the fourth energy level have?

A
  • An s sub shell (orbital)
  • A p sub shell (orbital)
  • A d sub shell (orbital)
  • (A f sub-shell.)
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11
Q

What order are the sub-shells filled with electrons in?

(Draw out diagram/ do cross down technique.)

A

1s, 2s, 2p,3s,3p,4s,3d,4p,5s, 4d, 5p, 6s

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12
Q

Finish sentence

Groups 1 and 2 are ….. ……. elements.

A

s block

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13
Q

FIllin gaps

Groups 3 to 12 are ….. ……. elements.

A

d block

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14
Q

Fill the gaps

Groups 3 to 0 are ….. ….. elements

A

p block.

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15
Q

Explain what each aspect of this configuration: (1s¹) means

A
  • 1 = first MAIN ENERGY LEVEL.
  • s: type of orbital.
  • 1 = number of electrons in the orbital.
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16
Q

What is an orbital?

A
  • Orbital: a region of space where there is a high probability of finding an electron.
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17
Q

What equation will allow you to calculate the total number of electrons found in n main energy level?

A

2n²

18
Q

What shape does the s sub-shell have?

A
  • A spherical shape.
19
Q

What is the shape of the p orbital?

A
  • Each sub-orbital in p orbital in shape of dumbell.
  • All together = shape of flower

Refer to Gautum notes if needed.

20
Q

Give two reasons why the 1s orbital is the most stable.

A
  • Closest orbital to nucleus.
  • Posesses least amount of energy.
21
Q

Finish the sentence

As the energy of the orbitals increase, the stability of the orbitals …….

A
  • Decreases.
22
Q

How many sub-orbitals is f orbital made up of?

A
  • 7 sub -orbitals
    MAXIMUM OF 14 ELECTRONS OVERALL
23
Q

What are the two elements that are the exceptions to filling orbitals in order and then moving onto the next (ie. they have a half-filled orbital?)

A
  • Chromium
  • Copper.
24
Q

What would you EXPECT the electron configuration of chromium to be?
What actually is the configuration?

A
  • EXPECT: 1s²2s²2p⁶3s²3p⁶4s²3d⁴
  • ACTUAL:
  • 1s²2s²2p⁶3s²3p⁶4s¹3d⁵
    (Only PARTIALLY FILLED s orbital.)
25
Q

What would you expect the electron configuration of copper to be? What actually is the configuration?

A

EXPECT:
- 1s²2s²2p⁶3s²3p⁶4s²3d⁹
ACTUAL:
- 1s²2s²2p⁶3s²3p⁶3d¹⁰4s¹

26
Q

Why is the s orbital only partially filled in chromium and copper (ie. only one electron filled in s orbital and the electrons start filling in d orbital straight awa?)

A
  • The arrangements are of lower energy so are more stable.
27
Q

What property do electrons have (beginning with s?)

A
  • Spin.
28
Q

What is the spin of two electrons in the same orbital like?

A
  • ## They have opposite spins.
29
Q

What are electrons represented by in the spin diagrams? What does the direction of the arrows show?

A
  • Electrons are represented by arrows.
  • Direction of the arrows show the different directions of spin.
30
Q

When doing box diagrams (ie. bus seating) how are the electrons filled in the sub-orbitals?

A
  • You fill each sub-orbital individually before you start to pair the electrons up.
  • Ie. if you had a p orbital –> 3 sub-orbitals and there were 3 electrons, the 3 electrons would go in the 3 separate sub orbitals (no two electrons would be paired together.)
31
Q

Why do electrons fill individually in sub-orbitals before being paired up?

A
  • Because if two electrons are in the same sub-orbital they will repel each other even more (requires even more energy to put the electrons in the same sub-orbital.)
32
Q

What does the opposite direction of spin of electrons in each sub-orbital reduce?

A
  • The opposite direction of each of electrons in each sub-orbital reduces the mutal repulsion between the paired electrons.
33
Q

What is the short-hand way of writing the electron configuration of Titanium (22 electrons?) How do you do the short-hand electron configuration?

A
  • (Ar) 4s²3d²
  • Locate noble gas above the element.
  • Go horizontally across until you reach your element (as you enter s block fill the s orbital and move onto the d block - fill the d orbital until you reach titanium: in this example.)
34
Q

Short-hand configuration of chromium.

A

(Ar) 4s¹ 3d⁵

35
Q

Where are electrons removed from when we ionise transition metals?

A
  • Electrons are lost from the 4s orbital FIRST and then from the 3d, 3p, 3s etc (going down.)
36
Q

What is the short- hand electronic structure of Chromium? What does spin diagram look like?

A

(Ar)4s¹3d⁵
All filled up to 3p. 4s only partially filled, one extra in 3d.
the s orbital is partially-filled even in the short-hand configuration

37
Q

KLP

Short-hand notation of V³⁺

A

(Ar) 3d²
NORMAL SHORT- HAND STRUCTURE? - (Ar)4s² 3d³.
- Take away 3 electrons - take two from 4s FIRST and then from the 3d!!

38
Q

KLP

If you want to write the electron configuration of a transition ion, what should you do?

3 STEPS!!

A

1.) Write electron configuration of the atom.
2.) Then, take out electrons from the 4s first AND then the 3d.
3. ) There, you will have the full electron configuration of the ion.

39
Q

Write the full electron configuration of S2- and the short-hand structure.

A
  • S²⁻: 1s²2s²2p⁶3s²3p⁶
  • (Ar) 3s²3p⁶
40
Q

In general, how do we fill electrons in spin diagrams? Why do we do this?

A
  • Put each electron in separate sub-orbital before starting to pair them up.
  • This requires less energy to do than if you started pairing electrons up to start off with (repulison force.)

CHEM A LEVEL (16 decks)

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