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Advanced higher chemistry > Unit 1 Inorganic Chemistry: Key Area 2 - Atomic orbitals, electronic configurations and the periodic table > Flashcards

Unit 1 Inorganic Chemistry: Key Area 2 - Atomic orbitals, electronic configurations and the periodic table Flashcards

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1
Q

How can the discrete lines in an atomic spectra be explained?

A

The discrete lines observed in atomic spectra can be explained if electrons, like photons, also display the properties of both particles and waves.

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2
Q

What are orbitals defined as?

A

An area where there is a 90% probability of finding an electron

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3
Q

What are the 4 quantum numbers?

A
  • Principle Quantum Number (n)
  • Angular Momentum Quantum Number (l)
  • Magnetic Quantum Number (m)
  • Spin Magnetic Quantum Number (ms)
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4
Q

What is the meaning of the Principle Quantum Number?

A

Energy level

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5
Q

What is the meaning of the Angular Momentum Quantum number?

A

shape of the orbital

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6
Q

What is the meaning of the Quantum number?

A

orientation

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7
Q

What is the meaning of the Spin magnetic Quantum number?

A

Electron spin

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8
Q

What is the fixed amount of energy of electrons within atoms called?

A

quanta

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9
Q

What does the principle quantum number tell you about an atom?

A

The average relative distance of the electron from the nucleus. Is measure in n= 1,2,3,4…

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10
Q

What does a higher value of n in the principle quantum number indicate?

A

The higher the value of n, the higher the potential energy associated with the shell and electrons are easier to remove from an atom

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11
Q

If the value of n is 1, what is the value of l and the subsequent sub-shell?

A

l=0 and 1s

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12
Q

If the value of n is , what is the value of l and the subsequent sub-shell?

A

l = 0/1 and 2s/2p

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13
Q

If the value od n is 3, what is the value of l and the subsequent sub-shell?

A

l = 0/1, and 3s/3p, 3d

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14
Q

If the value od n is 4, what is the value of l and the subsequent sub-shell?

A

l = 0/1, 2/3 and 4s/4p, 4d/4f

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15
Q

How many atomic orbitals are there within a s sub shell?

A

1

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16
Q

How many atomic orbitals are there within a p sub shell?

A

3

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17
Q

What are the key features of the s orbital?

A
  • spherical

- the s orbital in the first shell is smaller than the s orbital in the second shell

18
Q

What are the key features of the p orbital?

A
  • each p orbital has two lobes
  • three p orbitals have DEGENERATE (have the same energy as the other).
  • they are aligned along perpendicular axes
19
Q

What are different about d orbitals?

A

the five d orbitals are DEGENERATE with each other but have higher energies than the s and p orbitals in the same shell

20
Q

What MUST be known about orbitals?

A
  • The shapes of s and p orbitals
  • Max number of electrons in any orbital
  • Recognise d orbitals from diagrams
  • Know that d has a different shape
21
Q

If the value of l is 0/1, what is the value of m and the type of atomic orbital?

A

m -1,0,+1 and 2s/2p

22
Q

If the value of l is 2, what is the value of m and the type of atomic orbital?

A

m = -2,-1,0,+1,+2 and 3s,3p,3d

23
Q

What value of s in the spin quantum number represents clockwise rotation?

A

S = +1/2

24
Q

What value of s in the spin quantum represents an anti- clockwise rotation?

A

S = -1/2

25
Q

What is the maximum amount of electrons an orbital can hold?

A

2

26
Q

In any orbital containing 2 electrons what must happen?

A

The electrons must be paired with the spins opposed represented as a box with a arrow pointing up and other pointing down, where the box represents an orbital

27
Q

What is the Pauli Exclusion Principle?

A

The Pauli Exclusion Principle states that - No two electrons in the same atom can have the same set of four quantum numbers. (no orbital can hold more than 2 electrons and the two electrons must have opposite spins)

28
Q

What are the three rules used to determine in which orbital, electrons of an element are located?

A
  • The Aufbau Principle
  • Hund’s Rule
  • The Pauli Exclusion Principle
29
Q

What does the Aufbau principle state?

A

That electrons fill the orbitals of increasing energy, meaning that the electrons will fill the orbitals starting with the orbital of lowest energy).

30
Q

What does Hund’s rule state?

A

For degenerate orbitals, electrons will fill each orbital singly and with parallel spins, before pairing up to fill the orbitals.

31
Q

What happens to the sub-shell as the principle number increases?

A

The sub-shell will increase in energy.

32
Q

What is different about the 3d shell?

A

The 3d shell has greater energy than the 4s sub-shell.

33
Q

What is the ionisation energy?

A

The energy required to remove one mole of electrons from one mole of atoms in the gaseous state.

34
Q

Why between Be and B as well as Mg and Al is there a decrease in ionisation energy?

A

A full sub shell is a stable arrangement. For an element begins a new sub shell there is a decrease in stability.

35
Q

Why between N and O as well as P and S is there a decrease in ionisation energy?

A

A half full sub shell is also a relatively stable arrangement.

36
Q

How do molecules cope with excess electrons?

A

Extra orbitals are needed which come from empty d orbitals

37
Q

In order to predict molecular shape, what must be considered?

A

That all outer shell electrons (valence electrons) of the central atom repel each other. Must also consider bonding and non-bonding electron pairs.

38
Q

What is the process of predicting molecular shape called?

A

The Valence Shell Electron Pair Repulsion theory (VSEPR)

39
Q

In a neutral atom, what is the equation for electron pairs?

A

EP = no. of outer electrons + no. of bonding electrons / 2

40
Q

What is the equation for electron pairs with ions?

A

EP = no. of outer electrons + no. of bonded electrons (+ an electron for each negative charge and - an electron for each positive charge) / 2

41
Q

What is descending order of repulsion effect?

A
  • non bonding / non bonding
  • non bonding / bonding
  • bonding / bonding

Advanced higher chemistry (5 decks)

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