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A Level - Chemistry > 1: Atomic Structure and the Periodic Table > Flashcards

1: Atomic Structure and the Periodic Table Flashcards

1
Q

What is the atomic number?

A

Number of protons

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2
Q

What is the mass number?

A

Number of protons and neutrons

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3
Q

What is the relative mass of each particle?

A

Proton - 1
Neutron - 1
Electron- 0.0005

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4
Q

What is an isotope?

A

Atoms of the same element with different numbers of neutrons

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5
Q

What are the properties of isotopes?

A

Same chemical properties (same electrons)

Slightly different physical properties (mass of atom)

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6
Q

What is the relative atomic mass (Ar)?

A

Weighted mean mass of an atom of an element, compared to 1/12 of the mass of an atom of Carbon-12
Average of the relative isotopic masses

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7
Q

What is the relative isotopic mass?

A

Mass of an atom of an isotope compared to 1/12 of the mass of an atom of Carbon-12
Usually a whole number

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8
Q

What is the relative molecular mass?

A

Average mass of molecule compared to 1/12 of the mass of an atom of the carbon-12

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9
Q

What is the calculation for the relative atomic mass?

A

Multiply each isotopic mass by % abundance, add them up

Then divide by 100

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10
Q

What are mass spectrometers?

A

Devices which find out what samples are made up of by measuring the masses of their components

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11
Q

What do mass spectrometers produce?

A

Mass spectra

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12
Q

What is on the y-axis of a mass spectra?

A

Abundance of ions (percentage)

Height of peak gives relative isotopic abundance

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13
Q

What is on the x-axis of a mass spectra?

A

m/z

Mass/charge ratio, most charges are +1 so usually just relative isotopic masses

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14
Q

How would you work out the relative atomic mass using a mass spectra?

A

Multiply relative isotopic mass by abundance and add up results
Divide by sum of the isotopic abundances

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15
Q

What are the 4 stages of mass spectroscopy?

A

Ionisation
Acceleration
Deflection
Detection

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16
Q

What happens in the ionisation stage of mass spectroscopy?

A

Sample bombarded with high energy electrons (causes one electron removed from each atom of sample)

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17
Q

What happens in the acceleration stage of mass spectroscopy?

A

All particles in sample accelerated to same kinetic energy

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18
Q

What happens in the deflection stage of mass spectroscopy?

A

Electromagnet creates magnetic field which deflects ions different amounts based on their m/z
Smaller the m/z, the larger the deflection

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19
Q

What happens in the detection stage of mass spectroscopy?

A

Ions hit detector which creates a current

The current is detected, amplified and recorded

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20
Q

What fields is mass spectroscopy used?

A

Radioactive dating
Space research
Sport to detect illegal drugs
Pharmaceutical industry

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21
Q

How would you calculate the isotopic mass from relative atomic mass and 2/3 isotopic masses?

A

Work out % abundance of unknown

Using Ar of element and the other two isotopes work out mass of isotope

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22
Q

What is the M peak?

A

Molecular ion peak - peak with highest m/z vlaue

Occurs due to formation of the molecular ion from the ionisation process

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23
Q

What are the first 4 energy subshells?

A

s
p
d
f

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24
Q

What is an orbital?

A

Bit of space that electrons move in

Electrons in the subshell have the same energy

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25
Q

What can be held in each orbital?

A

2 electrons

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26
Q

What happens to the 2 electrons in an orbital?

A

Spin-pairing

Electron spin in opposite directions

27
Q

How many orbitals are found in the s sub-level?

A

1 orbital - 2 electrons

28
Q

How many orbitals are found in the p sub-level?

A

3 orbitals - 6 electrons

29
Q

How many orbitals are found in the d sub-level?

A

5 orbitals - 10 electrons

30
Q

How many orbitals are found in the f sub-level?

A

7 orbitals - 14 electrons

31
Q

What is the first ionisation energy?

A

Energy required to remove 1 mole of electrons from 1 mole of atoms of a gaseous element to form gaseous ions

32
Q

What is the example equation for the first ionisation energy?

A

X (g) -> X+ (g) + electron

33
Q

What is the example equation for the second ionisation energy?

A

X+ (g) -> X2+ (g) + electron

34
Q

What factors affect ionisation energy?

A

Distance from nucleus
Nuclear charge (no. of protons)
Shielding

35
Q

Why does 1st ionisation energy decrease as you go down groups?

A

Effective nuclear charge doesn’t change
Distance from nucleus increases
Shielding increases

36
Q

Why does 1st ionisation energy increase as you go across periods?

A

Effective nuclear charge doesn’t change
Distance from nucleus decreases a very small amount
Shielding

37
Q

Why does ionisation energy drop from phosphorus to sulphur?

A

Phosphorus - 3 electrons in the outer sub-level fill up each orbitals
Sulphur - 4 electrons mean that two electrons are in one orbital, they repel each other and therefore less energy required

38
Q

What is the exception with subshell notation?

A

4s subshell has a lower energy level than the 3d subshell

4s fills up first

39
Q

What is the electronic configuration of chromium?

A

1s2 2s2 2p6 3s2 3p6 3d5 4s1

40
Q

What is the electronic configuration of copper?

A

1s2 2s2 2p6 3s2 3p6 3d10 4s1

41
Q

What is the electromagnetic spectrum?

A

Energy that is transmitted as waves with a spectrum of frequencies

42
Q

What are electron shells also known as?

A

Quantum cells

Energy levels

43
Q

What is excitation?

A

Electrons take in the energy from their surroundings and move to a higher energy level

44
Q

What happens in de-excitation?

A

Electrons release specific amounts of energy and drop to a lower energy level
Produces a specific frequency of light

45
Q

How can the emission spectra be displayed?

A

Line spectra of discrete coloured lines

Each spectrum for each element is different

46
Q

What are the four basic principles of quantum shells?

A

Only exists in fixed orbits
Fixes energy
When electrons move between orbits EM radiation is emitted or absorbed
Radiation will have a fixed frequency

47
Q

Why is the 1st ionisation energy of O less than N?

A 
The extra electron of oxygen will cause it to go into an orbital with another electron (2p4) 
Nitrogen is (2p3), therefore only one electron in each orbital
48
Q

What is constant with elements in the same period?

A

Same number of electron shells

49
Q

What is constant with elements in the same group?

A

Same number of electrons in their outer shell (similar chemical properties)

50
Q

What is periodicity?

A

Repeating pattern in physical (and other) properties across period 2 & 3

51
Q

How does atomic radius change across a period?

A

Decreases - as protons increases so the positive charge increases and electrons are pulled closer

52
Q

What is the s-block?

A

Group 1 and 2, outer electron always in s-orbital

Easily loses electron

53
Q

What is the d-block?

A

Most transition metals in the central block, outer electron in d-orbital

54
Q

What is the p-block?

A

Groups 3-0, outer electron in p-orbital

55
Q

How does boiling point change across period 2 and 3?

A

Generally increases to group 4 then decreases to 8

56
Q

What elements in group 2 has the highest and lowest boiling temperature?

A

Highest - Carbon (Group 4)

Lowest - Neon (Group 8 )

57
Q

Explain the trend of melting/boiling points across a period

A

Group 1-3 have metallic bonding, increasing in strength due to increased charge density
Group 4 has giant covalent lattice and strong covalent bonds
Groups 6-7 simple molecular structures
Group 8 noble gases

58
Q

Why do noble gases have low boiling points?

A

Exist as individual atoms and therefore have very weak London forces

59
Q

Why does Sulphur have an unusually high boiling/melting point?

A

Naturally occurs as S8

Larger London forces as more electrons

60
Q

What block of the periodic table is chromium found?

A

d

1s2 2s2 2p6 3p6 4s2 3d4

61
Q

What will have the highest to lowest ionisation of the following species:
S S+ S-

A

Highest: S+
S
Lowest: S-

62
Q

What would be the groups of the elements (with consecutive atomic numbers) with the following ionisation energies:
1680, 2080, 496, 738

A

7, 8, 1, 2

63
Q

Why do increasing numbers of protons not have a large effect if there are also more electrons?

A

Extra shells and electrons meaning the force is spread more and therefore effectively the same

A Level - Chemistry (26 decks)

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