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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

1
Q

How can the discrete lines in 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

How do electrons behave in an atom?

A

Electrons behave as standing (stationary) waves in an atom. These are waves that vibrate in time but do not move in space. There are different sizes and shapes of standing wave possible around the nucleus, known as orbitals. Orbitals can hold a maximum of two electrons.

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3
Q

What are orbitals defined as?

A

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

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4
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 (s)
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5
Q

What is the meaning of the Principal Quantum Number?

A

Energy Level

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6
Q

What is the meaning of the Angular Momentum Quantum Number?

A

Shape of the Orbital

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7
Q

What is the meaning of the Quantum Number?

A

Orientation

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8
Q

What is the meaning of the Quantum Number?

A

Electron Spin

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9
Q

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

A

Quanta

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10
Q

What does the Principal Quantum Number tell you about an atom?

A

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

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11
Q

What does a higher value of n in the Principal 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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12
Q

What does the angular momentum quantum number describe?

A

The shape of the orbital.

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13
Q

What are the possible values of l in the angular momentum number but what is used instead?

A

Any integer value from 0 to n-1. L = 0,1,2 and 3 but letters s,p,d and f are used instead.

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14
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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15
Q

If the value of n is 2, what is the value of l and the subsequent sub-shell?

A

l = 0/1 and 2s/2p

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16
Q

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

A

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

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17
Q

If the value of 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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18
Q

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

A

1

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19
Q

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

A

3

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20
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.

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21
Q

What are the key features of the p orbital?

A
  • Each p orbital has two lobes.
  • Three p orbitals are DEGENERATE (have the same energy as each other).
  • They are aligned along perpendicular axes.
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22
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.

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23
Q

What MUST be known about orbitals?

A
  • The shapes of s and p orbitals and be able to draw them. • Max number of 2 electrons in any orbital
  • Recognise d orbitals from diagrams
  • Know that d 2 has a different shape
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24
Q

What does the magnetic quantum number do?

A

• Distinguishes orbitals in same shell and subshell by
giving them a different orientation in space;
• Only non-spherical molecules.
• Values = -l to +l

25
Q

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

A

m = 0 and 1s

26
Q

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

A

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

27
Q

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

A

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

28
Q

What does the value of s in the spin quantum number represent?

A

The rotation around the axis of the electron.

29
Q

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

A

S = +1/2

30
Q

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

A

S = -1/2

31
Q

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

A

2

32
Q

How does each electron in an orbital behave?

A

Each electron in an orbital has a spin which causes it to behave like a tiny magnet. It can spin clockwise, or anti-clockwise.

33
Q

What symbol represents a clockwise rotation?

A

An arrow pointing up.

34
Q

What symbol represents an anti-clockwise rotation?

A

An arrow pointing down.

35
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.

36
Q

What is the Pauli Exclusion Principle?

A

No two electrons in one atom can have the same set of four quantum numbers, therefore, no orbital can hold more than two electrons and these two electrons must have opposite spins.

37
Q

What are the 3 rules used to determine in which orbital electrons of an element are located?

A
  • The Aufbau Principle
  • Hund’s Rule
  • The Pauli Exclusion Principle
38
Q

What does the Aufbau principle state?

A

That electrons will fill orbitals starting with the orbital of lowest energy.

39
Q

What does Hund’s Rule state?

A

For degenerate orbitals, electrons will fill each orbital singly before any orbital gets a second electron and spin pairing starts.

40
Q

What happens to sub-shells as the principle quantum number increases?

A

They increase in energy.

41
Q

What is different about the 3d shell?

A

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

42
Q

Efvrvfrtv

A

Rgvrtv

43
Q

5th5yb

A

6hb5yb5yh

44
Q

Thbyn

A

Hyhyhy

45
Q

What is the ionisation energy?

A

The energy require to remove one mole of electrons from one mole of gaseous atoms.

46
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.

47
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.

48
Q

What are types of unusual bonding?

A

Mo;eco;es which do not achieve a stable octet and molecules that have in excess of a stable octet.

49
Q

How are molecules that do not achieve a stable octet affected?

A

The are very reactive/unstable.

50
Q

How do molecules cope with excess electrons?

A

Extra orbitals are needed which come from the empty d-orbitals.

51
Q

What are Dative Covalent Bonds?

A

Covalent bonds formed when both electrons come from the same atom and are also known as co-ordinate covalent bonds.

52
Q

How are Dative Covalent bonds drawn?

A

An arrow head points from the donor atom to the receptor atom.

53
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.

54
Q

What is the process of predicting molecular shape called?

A

The Valence Shell Electron Pair Repulsion theory (VSEPR).

55
Q

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

A

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

56
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 every positive charge) / 2

57
Q

What is descending order of repulsive effect?

A
  • non-bonding/non-bonding
  • non-bonding/bonding
  • bonding/bonding
58
Q

Why are bond angles smaller for NH3 and H2O than tetrahedral?

A

Due to lone pair electron repulsion.

Advanced Higher Chemistry (6 decks)

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