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ADV CHEM UNIT 1 > KA 2: atomic orbitals, electronic configuration and the periodic table > Flashcards

KA 2: atomic orbitals, electronic configuration and the periodic table Flashcards

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1
Q

what are standing (stationary) waves?

A

waves that vibrate in time but do not move

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2
Q

what is an orbital?

A

different sizes and shapes of standing waves possible around the nucleus

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3
Q

What is the max. number of electrons that an orbital can hold

A

2

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4
Q

Name the four different shapes of orbitals

A

s,p,d,f

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5
Q

What is “quanta”?

A

the fixed amount of energy that electrons within an atom have

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6
Q

what can electrons be defined in terms of?

A

quantum number

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7
Q

For Principal Quantum Number:

-Name the symbol

-Say what values it can have

-What does it do

-What is it related to

A

-n

-can have values n=1,2,3,4…

-indicates main energy level for an electron

-is related to the size of the orbital

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8
Q

The higher the value of……

A

n, then the further the electrons are from the nucleus

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9
Q

For Angular Momentum Quantum Number:

-Name the symbol

-What does this determine

-What values can it have

A

-l

-can have values l=0,1,2,3 (up to n-1)

-it determines the shape of the subshell

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10
Q

For Magnetic Quantum Number:

-Name the symbol

-what values can it take

-what does it determine

A

-ml

-ml can take values of whole numbers (and zero) between -1 and +1

-determines the orientation of the orbital

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11
Q

How is the second shell organised?

A

one “s” orbital and three “p” orbitals

Three p orbitals are aligned along perpendicular axes.

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12
Q

For Spin Magnetic Quantum Number:

-what does it determine

-name the symbol

-what values can they take

A

-the direction of spin

-ms

-takes the values of -1/2 or +1/2

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13
Q

when an orbital contains two electrons they must…

A

be paired with spins opposed

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14
Q

In s orbitals:

-what is the value of l

-describe the trend

A

-l=0

-increasing size and energy as n increases

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15
Q

In p orbitals:

-what is the value of l

-what is it’s shape

-how many orbitals

-explain the trend

A

-l=1

-dumbbell shaped

-3 orbitals corresponding to ml= -1,0,1. These 3 orbitals have the same energy (degenerate)

-Energy and size increases with n(2p<3p<4p)

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16
Q

In d orbitals:

-what is the value of l

-what is it’s shape

-how many orbitals

-explain the trend

A

-l=2

-more complex dumbbell shapes

-5 orbitals (ml= -2,-1,0,1,2)(degenerate)

-energy and size increases with n (3d<4d)

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17
Q

describe the organisation of the third shell

A

max. 18 electrons

-2 in the s orbital

-6 in the 3 p orbitals

-10 remaining in the d orbitals (5 d orbitals)

18
Q

What does degenerate mean?

A

orbitals that have the same energy

19
Q

what is the periodic table subdivided into and what does that correspond to?

A

-s,p,d,f

-corresponds to the outer electronic configurations of these elements

20
Q

what does each box in box notation represent?

A

an atomic orbital

21
Q

what does box notation represent?

A

The relative energies corresponding to each orbital can be represented diagrammatically using orbital box notation for the first four shells of a multi-electron atom.

22
Q

What is the order of filling?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

23
Q

what does each thing correspond to in spectroscopic notation?

A

leading numbers=> the n numbers i.e. the shell

letters=> the sub-shell (l numbers)

subscript=> the total number of electrons within that sub-shell

24
Q

Name the three principles/rules

A

-The Aufbau Principle

-Hund’s rule

-The Pauli Exclusion Principle

25
Q

Explain the Aufbau principle

A

electrons fill orbitals in order of increasing energy

26
Q

Explain Hund’s rule

A

when degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts

27
Q

Explain the Pauli Exclusion Principle

A

No two electrons in one atom can have the same set of quantum numbers

as a consequence, no orbital can hold more than two electrons and these electrons have opposite spin

28
Q

what can the variation in first, second and subsequent ionisation energies with increasing atomic number for the first 36 elements can be explained by?

A

in terms of the relative stability of different subshell electronic configurations

29
Q

what does the variation give evidence for?

A

allows anomalies in the ionisation energies

30
Q

There is a special stability associated with half-filled and full subshells

Explain the trend

A

the more stable the electronic configuration, the higher the ionisation

31
Q

What can be used to predict the shapes of molecules and polyatomic ions?

A

VSEPR (valent shell electron pair repulsion)

32
Q

how do you find the total number of electron pairs surrounding a central atom?

A

-taking the total number of valence (outer) electrons on the central atom and adding one for each atom attached

-adding an electron for every negative charge

-removing an electron for every positive charge

-dividing the total number of electrons by two to give the number of electron pairs

33
Q

how can the shape of the molecule be determined?

A

by the atoms present based on the arrangement of electrons

34
Q

name the 5 different arrangements of electron pairs around a central atom

A

-linear for two electrons pairs

-trigonal planar for three

-tetrahedral for four

-trigonal bipyramidal for five

-octrahedral for six

35
Q

electrons pairs are…

A

negatively charged and repel each other

36
Q

whats one reason that electron pairs are organised the way they are?

A

to minimise repulsion/maximise separation

37
Q

what is the order of electron pair repulsions

A

non-bonding/non-bonding>non-bonding pair/bonding pair>bonding/bonding pair

38
Q

what does it mean if a molecule, or ion, has lone pairs on the central atom?

explain why this occurs

A

the shapes are slightly distorted away from the regular shapes

this is because of the extra repulsion caused by the lone pairs

39
Q

what is the lone-pair order?

A

bond pair-bond pair<lone pair-bond pair<lone pair-lone pair

40
Q

what do the different strengths of electron pair repulsion account for?

A

slight deviations from expected bond angles in molecules such as NH3 and H2O

ADV CHEM UNIT 1 (3 decks)

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