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Physical chemistry > Atomic structure > Flashcards

Atomic structure Flashcards

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1
Q

What is the relative mass of a proton?

A

1

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2
Q

What is the relative mass of a neutron?

A

1

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3
Q

What is the relative mass of an electron?

A

1/2000

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4
Q

What is the relative charge of a proton?

A

+1

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5
Q

What is the relative charge of a neutron?

A

0

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6
Q

What is the relative charge of an electron?

A

-1

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7
Q

What is the top number on the periodic table?

A

Mass number

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8
Q

What is the bottom number on the periodic table?

A

Atomic number

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9
Q

What is the mass number?

A

Total number of protons and neutrons.

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10
Q

What is the atomic number?

A

Number of protons (and therefore electrons).

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11
Q

Do negative ions have more protons or electrons?

A

More electrons

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12
Q

What is an isotope?

A

An atom with the same number of protons but different number of neutrons.

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13
Q

Do isotopes have the same chemical properties?

A

Yes

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14
Q

What affects chemical properties?

A

Configuration of electrons.

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15
Q

What affects physical properties?

A

Mass

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16
Q

Do isotopes have the same physical properties?

A

No

17
Q

What did John Dalton discover about the atom?

A

*atoms are spheres
*each element is made from different spheres

18
Q

What did J.J.Thompson discover about the atom?

A

*discovered electrons
*came up with the plum pudding model
*the atom isn’t solid

19
Q

What is the plum pudding model?

A

The atom is made up of a positive ‘pudding’ and negative ‘plum’ electrons.

20
Q

What did Ernest Rutherford discover about the atom?

A

*discovered small and positively charged nucleus
*atom is mainly empty space
*negative electron cloud

21
Q

Explain Rutherford’s gold leaf experiment.

A

*positive alpha particles fired at thin gold leaf
*most went through (mainly empty space)
*small amount were deflected back (hit small positive nucleus)

22
Q

What did Neils Bohr discover about the atom?

A

*electrons were in fixed shells

23
Q

What did Neils Bohr think was the problem with Rutherford’s atomic model?

A

The negative electron cloud would collapse into the positive nucleus.

24
Q

Describe Neils Bohr’s experiement.

A

*EM radiation was absorbed by electrons causing them to move between shells
*electrons emit this radiation when they move to lower energy levels

25
Q

What was the order of discoveries about the atom?

A

*John Dalton - 1803
*J.J.Thompson - 1897
*Ernest Rutherford - 1909
*Neils Bohr - 1913

26
Q

What is different now about the atomic structure to Bohr’s model?

A

Not all electrons in the same shell have the same energy, therefore there are sub-shells.

27
Q

What are the four steps involved in time of flight mass spectrometry?

A
  1. ionisation
  2. acceleration
  3. ion drift
  4. detection
28
Q

What are the 2 ways of ionising a sample?

A

*electrospray ionisation
*electron impact ionsiation

29
Q

Describe electrospray ionisation.

A

*sample is dissolved and pushed through nozzel at high pressure - turns into gas
*high voltage is applied to sample - each particle gains a H+ ion

30
Q

Describe electron impact ionisation.

A

*sample is vaporised
*electron gun fires high energy electrons at it
*one electron is knocked off each particle - forming 1+ ions

31
Q

Describe acceleration in mass spectrometry.

A

Ions are accelerated by an electric field to give them all the same kinetic energy.

32
Q

Describe ion drift in mass spectrometry.

A

*ions enter a region with no electric field
*lighter ions drift faster than heavy ones

33
Q

Describe detection in mass spectrometry.

A

*lighter ions reach the detector first
*when charged particles hit the detector they produce an electrical current
*mass spectrum is produced

34
Q

Define relative atomic mass.

A

The average mass of an atom of an element when measured on a scale on which the mass of C12 is exactly 12.

35
Q

What is the symbol for atomic mass?

A

Ar

36
Q

Define relative molecular mass.

A

The average mass of a molecule when measured on a scale on which the mass of C12 is exactly 12.

37
Q

Define relative isotopic mass.

A

The mass of an atom of an isotope of an element when measured on a scale on which the mass of C12 is exactly 12.

Physical chemistry (10 decks)

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