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BIO1332 - Biochemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

Define chemistry:

A

Scientific discipline involved with elements and compounds composed of atoms, molecules and ions: their composition, structure, properties, behaviour and the changes they undergo during a reaction with other substances

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2
Q

Define element:

A

Simplest substances and are made up from simple particles

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3
Q

Define molecules:

A

More than one atom bonded together to either the same or different atoms

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4
Q

Define compound:

A
  • Combination of different types of atoms

- Pure substances which consists of two or more elements chemically combined

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5
Q

Define atom:

A

Smallest parts of an element that can exist chemically

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6
Q

Are atoms the smallest particles?

A

No

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7
Q

What is an atom composed of?

A
  • Neutrons
  • Protons
  • Electrons
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8
Q

When looking a periodic table what is above the chemical symbol?

A

Atomic number

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9
Q

When looking a periodic table what is bellow the chemical symbol?

A

Relative atomic mass

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10
Q

What is a nucleus of an atom made of?

A

Protons and neutrons

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11
Q

What is the symbol for a neutron?

A

n

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12
Q

What is the mass (kg) of a neutron?

A

1.675 x10^-27

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13
Q

What is the charge of a neutron?

A

0

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14
Q

What is the symbol for a proton?

A

p

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15
Q

What is the symbol for an electron?

A

e

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16
Q

What is the mass (kg) of a proton?

A

1.673 x 10^-27

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17
Q

What is the mass (kg) of a electron?

A

9.109 x 10^-31

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18
Q

What is the charge of a electron?

A

-1

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19
Q

What is the charge of a proton?

A

+1

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20
Q

Define atomic number:

A
  • Number of protons in nucleus

- Each element has its own atomic number

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21
Q

Define relative atomic mass:

A

-Sum of the number of protons and the neutrons in the nucleus of an atom

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22
Q

Define isotops:

A

Atoms of the same element with different numbers of neutrons

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23
Q

How can we see atoms?

A

Transmission Electron Microscopy (TEM)

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24
Q

How are atoms neutral?

A

Protons and electrons cancel out the charge

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25
Q

What is quantum?

A

Fixed or discrete amount of something

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26
Q

What does the absorption of an electron cause the electron to do?

A

Jump to an excited state

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27
Q

How do you remove the excited state of an electron?

A

Removing the radiation - it will drop back to to ground state and unit

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28
Q

What do emission spectrums show?

A

An electron absorbing a specific, fixed quantity of energy

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29
Q

What is Bohr’s model of the H atom?

A

-Bohr orbits are quantised = specific absorption of energy for each transmission
= r =kn^2

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30
Q

What is weird about electrons?

A

Demonstrate wave particle duality

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31
Q

What did Schrodinger propose?

A

That properties of waves could be used to explain the behaviour of electrons in atoms

32
Q

What is an electron in a particular orbit described as?

A

Wavefunction

33
Q

What is a wavefunction?

A

series of mathematical equations that model the distribution of electrons in an atom

34
Q

What doe the quantum model show about the nucleus?

A

It is surrounded by clouds of electrons

35
Q

What are regions of space referring to in the quantum model?

A

Electron or atomic orbitals

36
Q

What does cloud of electrons equal to?

A

Cloud of probability

37
Q

What is the atomic orbital theory?

A

Electrons in atoms are arranged in successive principle energy levels or shells

38
Q

How many electrons can be held in the first shell?

A

2 electrons

39
Q

How many electrons can be held in the second shell?

A

8 electrons

40
Q

How many electrons can be held in the third shell?

A

18 electrons

41
Q

What model did Dalton come up with?

A

Solid sphere model

42
Q

What were the positives about the solid sphere model?

A

Recognised atoms of a particular element differ form other elements

43
Q

What were the negative about the solid sphere model?

A

Atoms are indivisible - they are composed from subatomic particles

44
Q

What model did Thomson come up with?

A

Plum pudding model

45
Q

What are the positives about the plum pudding model?

A

Recognised electrons as components of atoms

46
Q

What are the negatives about the plum pudding model?

A

No nucleus; didn’t explain later experimental observations

47
Q

What model did Rutherford propose?

A

Nuclear model

48
Q

What are the positives of the nuclear model?

A

Realised positive charge was localised in the nucleus of the atom

49
Q

What are the negatives of the nuclear model?

A

Did not explain why electrons remain in orbit around the nucleus

50
Q

What model did Bohr propose?

A

Planetary model

51
Q

What are the positives of the planetary model?

A

Proposed stable electron orbits; explained the emission spectra of some elements

52
Q

What are the negatives of the planetary model?

A

Moving electrons should emit energy and collapse into the nucleus model did not work well for heavier atoms

53
Q

What model did Schrodinger propose?

A

Quantum model

54
Q

What are the positives of the quantum model?

A
  • Shows electrons don’t move around the nucleus in orbit, but clouds where they position is uncertain
  • Widely accepted as the most accurate model of the atom
55
Q

What is an atomic orbital?

A

Region around an atom where there is a high probability of finding an electron

56
Q

Finish the sentence:

Higher the principle quantum number…

A

the further the electron density spreads away from nucleus

57
Q

Describe the s-orbitals:

A
  • Spherical
  • Symmetrical about all three axis
  • Found at all principle quantum numbers
  • Hold max. of 2 electrons
58
Q

Describe the p-orbitals:

A
  • Three p orbitals
  • Identical in shape
  • Point in different directions, one along each axis
  • Found at principle quantum number n=2 and above
  • Each orbital holds a max. of 2 electrons
59
Q

Describe the d-orbitals:

A
  • Five d-orbitals
  • Complicated shape
  • Found at principle quantum number n=3 and above
  • Each orbital holds a max. of 2 electrons
60
Q

Describe the f-orbitals:

A
  • Seven f-orbitals
  • Very complicated shape
  • Found at principle quantum number n=4 and above
  • Each orbital holds a max. of 2 electrons
61
Q

How many electrons in n=1?

A

2

62
Q

What are the atomic orbitals in n=2?

A

1s

63
Q

How many electrons in n=2?

A

8

64
Q

What are the atomic orbitals in n=2?

A

2s 2px 2py 2pz

65
Q

How many electrons in n=3?

A

18

66
Q

What are the atomic orbitals in n=3?

A

3s 3px 3py 3pz

3dxy 3dxz 3dyz 3dx2-y2 3dz2

67
Q

How many electrons in n=4?

A

32

68
Q

What are the atomic orbitals in n=4?

A

4s 4px 4py 4pz
4dxy 4dxz 4dyz 4dx2-y2 4dz2
Seven 4f orbitals

69
Q

What are five 3d orbitals are?

A

Degenerate

70
Q

What is the electronic configuration?

A

Arrangement of electrons within an atom

71
Q

What is the Pauli exclusion principle?

A

Each individual orbital contains a max. of two electrons with opposite spins

72
Q

Why do two electrons in an orbital have opposite spins?

A

To mimosa repulsion between two electrons

73
Q

Finish the sentence:

Electrons occupy the …

A

lowest energy vacant orbitals

74
Q

What is the Hund’s rule of max. multiplicity?

A

Electrons fill a set of degenerate energy orbitals by keeping their spins parallel

75
Q

What is the Aufbau principle?

A

To populate orbitals for a given atom, start at the lowest energy orbital and work upwards

76
Q

What does an atom in the ground state?

A

A configuration with the greatest number of unpaired electrons

BIO1332 - Biochemistry (19 decks)

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