Electronic structure Flashcards

(44 cards)

1
Q

what is the uncertainty principle

A

you can never know both the exact location and velocity of a subatomic particle at the same time

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2
Q

what are ionization energies

A

ionization energies are measures of the amount of energy needed to remove electrons from atoms (or ions)

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3
Q

what is the definition for first ionization energy

A

the energy required to remove one mole of electrons from one mole of gaseous atoms to for one mole of gaseous psositive ions

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4
Q

why are ionization energies always positive

A

because electrons and protons attract one another so energy must be added to the system to pull the electron away

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5
Q

why does an atom with a high nuclear charge have a high ionization energy

A

the greater the pull of the nucleus the harder it will be to pull an electron away (more energy required) so higher ionization energy

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6
Q

what do ionization trends give evidence for

A

electrons being in shells and subshells

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7
Q

what is electron affinity

A

the amount of energy needed to add electrons to atoms/ions

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8
Q

what is the definition of the first electron affinity

A

the energy required to add one mole of electrons to one mole of a gaseous atom to form one mole of gaseous negative ions

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9
Q

why is first electron affinities negative

A

indicates energy is released on the addition of the electron
the more negative the electron affinity, the more stable the negative ion that is formed

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10
Q

what is the trend of atomic size

A

increases down a group, decreases across a period

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11
Q

what is the trend of first ionization energy

A

decreases down a group and increases across a period

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12
Q

what is the trend of first electron affinity

A

becomes less negative down a group and become more negative across a period

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13
Q

what is an orbital

A

a region in space where there is a given (usually 95%) probability of finding a particular electron
cannot specify the definite or exact position of an electron in an atom

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14
Q

what do quantum numbers do

A

identify the various energy levels available with the atom in which the electrons can reside
they are identification numbers “address” for each electron in an atom
- they specify the position (or location) of an electron in an atom
- predict the direction of spin or rotation of the electron
- determine the energy and angular momentum of an electron

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15
Q

name the four quantum numbers that are required to specify the character of an electron

A
  • principal quantum numbers (n)
  • azimuthal or subsidaiart quantum numbers (l)
  • magnetic quantum numbers (m)
  • spin quantum numbers (s)
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16
Q

in poly-electron atoms what are principal energy levels called and referred to by

A

they are called shells and referred to by letter - K, L, M….

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17
Q

what principle quantum number do principal energy levels correspond to

A

the principal quantum number ‘n’

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18
Q

what does the K equal

19
Q

what does the L shell equal

20
Q

which shell doesn’t contain multiple orbitals

21
Q

what does ‘n’ indicate

A

DISTANCE OF ELECTRONS FROM NUCLEUS
higher the ‘n’ the further away the electron from the nucleus
ENERGY OF ELECTRONS
higher the ‘n’ higher energy electrons - less tightly held so easier to remove

22
Q

what is the rule for the maximum number of electrons a shell can hold
give examples

A
2(n^2)
K - n = 1 so max = 2 
L - n = 2 so max = 8
M - n = 3 so max = 18
N - n = 4 so max = 32
23
Q

what is a subshell

A

a group of orbitals with the same energy

24
Q

what quantum number describes a subshell

A

azimuthal or subsidiary quantum number ‘l’

25
how does the value of 'l' depend on the value of 'n'
'l' equals all values from 0 to (n-1) | e.g. if n = 2 l = 0, 1
26
what subshells do the values of l 0, 1, 2, 3 correspond to
``` 0 = s 1 = p 2 = d 3 = f ```
27
what is the maximum number of electrons a given subshell can hold
``` 2(2l+1) e.g l = 0 so no. of electrons = 2 l = 1 so no. of electrons = 6 l = 2 so no. of electrons = 10 l = 3 so no. of electrons = 14 ```
28
what shape does l = 0 s-orbital represent
spherical
29
what shape does l = 1 p-orbital represent
dumbbell
30
what shape does l = 2 d-orbital represent
more complex
31
what shape does 1 = 3 f-orbital represent
still more complex
32
magnetic quantum numbers
- represents the orbitals in a given subshell - indicates the direction of a particular orbital relative to the magnetic field/axes - does not indicate energy - tells us the number of orbitals present in the subshell
33
what does the value of m equal
m = -l to +l | e.g. l = 2 so m = -2, -1, 0, 1, 2
34
if m = 0 how many orbitals are in each level
one
35
if m = 1 how many orbitals are in each level
three - Px, Py, Pz
36
if m = 2 how many orbitals are in each level
five d-orbitals
37
if m = 3 how many orbitals are in each level
7 f-orbitals
38
how to know what ml =
ml is where the final electron lands | e.g 3p^5 has 5 electrons and the 5th electron lands on 0 orbital so ml = 0
39
how to know what ms equals
ms equals either -1/2 or +1/2 this depends on whether the final electron is pointing up or down if the arrow is pointing down ms = -1/2 if the arrow is pointing up ms = +1/2
40
``` if n = 3 l = 2 ml = 1 ms = -1/2 identify the electron ```
``` n = 3 means energy level 3 l =2 means d-orbital d-orbital has 5 orbitals ml = 1 so the electron is in 1 orbital and facing down as ms = -1/2 so 3d9 ```
41
if an ion is negative are electrons added or taken away
added
42
if an ion is positive are electrons added or taken away
taken away
43
define diamagnetic
no unpaired electrons
44
define paramagnetic
at least 1 unpaired electron