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elements of life > electronic configuration > Flashcards

electronic configuration Flashcards

1
Q

what are electrons shells labelled with

A

a principle quantum number (n)

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2
Q

the higher the value of n….

A

… further away it is from the nucleus

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3
Q

the further the shell is from the nucleus…

A

….the higher the energy associated with the shell

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4
Q

what does each shell have a limit for

A

the number of electrons it can hold

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5
Q

how many electrons can the n=1 shell hold

A

2

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6
Q

how many electrons can the n=2 shell hold

A

8

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7
Q

how many electrons can the n=3 shell hold

A

18

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8
Q

how many electrons can the n=4 shell hold

A

32

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9
Q

what is a filled shell

A

a shell which contains its maximum number of electrons

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10
Q

how are electrons arranged

A

so the lower energy shells are filled first

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11
Q

what is ionisation energy

A

the energy required to remove one electron from each atom in one mole of free gasesous atoms of the element

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12
Q

elements with high ionisation enthalpies…

A

…are difficult to ionise and very unreactive

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13
Q

elements with low ionisation enthalpies…

A

are easy to ionise and very reactive

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14
Q

what are shells split into

A

subshells

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15
Q

what are the subshells

A

s, p, d, f

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16
Q

what is the maximum number of electrons that each subshell can hold

A

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

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17
Q

which subshell is in the first energy level and how many electrons does it hold altogether

A

s subshell (holding only two electrons)

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18
Q

which subshell is in the 2nd energy level and how many electrons does it hold altogether

A

s subshell (two e-)
p subshell (6 e-)
so altogether 8 electrons

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19
Q

which subshell is in the 3rd energy level and how many electrons does it hold altogether

A

s subshell (2 e-)
p subshell (6e-)
d subshell (10e-)
so altogether 18 electrons

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20
Q

which subshell is in the 4th energy level and how many electrons does it hold altogether

A

s subshell (2e-)
p subshell (6e-)
d subshell (10e-)
f subshell (14e-)
so altogether 32 electrons

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21
Q

what do subshells within a shell have

A

different energies

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22
Q

are the energies within a subshell fixed

A

no they can decrease as the charge on the nucleus increases from one element to the next in the periodic table

23
Q

what are the subshells divided into

A

atomic orbitals

24
Q

where can electron in a given orbital be found

A

in a particular region of space around the nucleus

25
Q

how many atomic orbitals in an s subshell

A

1 atomic orbital

26
Q

how many atomic orbitals in a p subshell

A

3

27
Q

how many atomic orbitals in a d subshell

A

5

28
Q

how many atomic orbitals in a f subshell

A

7

29
Q

when do orbitals in the same subshell have the same energy

A

in an isolated atom

30
Q

why is the probability of finding an electron inside an atom unknown

A

the position of an electron can’t be exactly mapped for an electron in a given orbital

31
Q

how many electrons can be in one atomic orbital

A

2

32
Q

what do electrons in atoms have

A

every electron spins at the same rate

33
Q

when do electrons occupy the same orbital

A

if they have opposite or paired spins

34
Q

what do the box and the two arrow represent

A

the box is the atomic orbital and the arrows represent electrons

35
Q

what do you need to describe any electron in an atom

A

the electron shell its in
the orbital within the subshell
the subshell
its spin

36
Q

what kind of shape do atomic orbitals have

A

a 3d shape

37
Q

what does the 3d shape of an atomic orbital represent

A

the volume of space where there is a high probability of finding up to 2 electrons

38
Q

what is the electronic configuration

A

the arrangement of electrons in shells and orbitals

39
Q

how are orbitals filled

A

in a definite order to produce the lowest energy arrangement as possible

40
Q

in which order are orbitals filled

A

in order of increasing energy

41
Q

what happens when there is more than one orbital with the same energy

A

these orbitals are first occupied singly by electrons. this keeps electrons in an atom as far away from each other as possible.

42
Q

when can electrons pair up

A

when every orbital is singly occupied

43
Q

what kind of spin do electrons in singly occupied orbitals have

A

a parallel spin to ensure the lowest energy arrangement

44
Q

what does these all represent
1s₂

A

big 1 = principal quantum number (shell)
s = subshell
little 2 = no. of electrons

45
Q

why is 4s filled before 3d

A

it has a lower energy level

46
Q

what is the electronic configuration of vanadium

A

1) 23e-
2) electrons go into lowest energy shells and subshells
1s2 2s2 2p6 3s2 3p6
3) energy of 4s subshell is lower than the 3d subshell so is filled first
4) remaining e- go into the 3d subshell
1s2 2s2 2p6 3s2 3p6 4s3 3d3

47
Q

electronic configuration of S2-

A

sulfur - 1s2 2s2 2p6 3s2 3p4
-2 ion so need to add 2 electrons
1s2 2s2 2p6 3s2 3p6

48
Q

electronic configuration of Na+

A

Na - 1s2 2s2 2p6 3s1
+1 ion so need to take away one e-
1s2 2s2 2p6

49
Q

order of shells and subshells filled

A

1s
2s
2p
3s
3p
4s
3d
4p
4s is filled before 3d but its written 3d then 4s

50
Q

how can you tell an elements electron configuration from the periodic table

A

look at the period
look at the block
count along the block
Bromine
period 4, p-block, 5 spaces along the block
4p5

51
Q

what is the electronic configuration of chromium

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1

52
Q

what is the electronic configuration of copper

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1

53
Q

why dont copper and chromium fill in order

A

The reason Copper and Chromium have a slighly odd electron configuration is because of stability. By only having 1 electron in the 4s oribtal, Chromium is able to have 1 electron in each of it’s 3d orbitals, this configuration is more stable than by having 4s2 3d4

elements of life (15 decks)

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