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Lower Sixth Chemistry > Topic 1 Atomic Structure > Flashcards

Topic 1 Atomic Structure Flashcards

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1
Q

What is an atom

A

An atom is the smallest uncharged part of an element.

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2
Q

The relative mass of a proton

A

1

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3
Q

The relative mass of a neutron

A

1

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4
Q

The relative mass of an electron

A

1/1840 = 0.000543

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5
Q

What is the atomic number

A

The atomic number is the number of protons in an atom

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6
Q

What is the mass number

A

The total number of particles in the nucleus
(No. of protons + neutrons)

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7
Q

What is the no. of neutrons

A

Mass number - Atomic number

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8
Q

What are isotopes

A

Isotopes are the same type of atoms (same no. of protons/atomic number) but a different no. of neutrons

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9
Q

What is the relative atomic mass

A

Relative atomic mass (Ar) is the weighted mean of the atoms of a normal sample relative to 1/12 the mass of the C-12 isotope

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10
Q

What is the relative isotopic mass

A

Relative isotopic mass is the mass of an isotope of the element relative to 1/12 the mass of the C-12 isotope

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11
Q

What is relative molecular mass

A

Relative molecular mass (Mr) is the mass of a molecule relative to 1/12 the mass of the C-12 isotope

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12
Q

What is the relative formula mass

A

Relative formula mass is the sum of all the atomic masses of all the atoms in a particular formula

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13
Q

alternative name to hydrogen-1

A

protium

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14
Q

alternative name to hydrogen-2

A

deuterium

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15
Q

alternative name to hydrogen-3

A

tritium

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16
Q

What are the processes in a mass spectrometer

A
  1. sample is vapourised
  2. sample is ionised by an electron gun shooting electrons to knock off the existing electrons
  3. the ions are accelerated by an electric field
    4.the accelerated ions pass through a magnetic field and are deflected
  4. the ions are detected and recorded
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17
Q

Why must the tube in a mass spectrometer be under vacuum

A

so the ions won’t collide with air molecules that could affect the path the ions are taking

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18
Q

What m/z mean

A

mass/charge

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19
Q

What is the molecular/parent ion

A

the peak with the highest mass caused by the ion formed from the whole molecule

20
Q

Where to find the molecular ion

A

the largest peak at the end of the m/z graph

21
Q

Where could we use mass spectrometers in real life

A

-in sport to detect the use of anabolic steroids
-by pharmaceutical industries to identify synthesized compounds as possible potential drugs

22
Q

Why do certain substances produce different colours when placed in flames

A

-the heat energy from the flame causes electrons to move to a higher energy level shell.
-the electrons drop back down again and give out energy
-this energy is given out in the form of light
-this energy drop is always same for a particular type of atom, so the flame exhibits a particular colour

23
Q

Which metals atom emit coloured flames

A

lithium
sodium
potassium
calcium
strontium
barium

24
Q

Why do some metals don’t display colours

A

the energy given back out is not in the visible light spectrum

25
Q

what is ionisation energy

A

the energy required to remove an electron from an atom

26
Q

Definition of first ionisation energy

A

the energy required to remove one electron from each atom in one mole of gaseous atoms producing one mole of gaseous ions with one positive charge

27
Q

example of first ionisation

A

Cl (g) => Cl+ (g) + e-

28
Q

What does the magnitude of the first ionisation energy tell us

A

the magnitude tells us about the force of attraction between the nucleus and the outer electrons

29
Q

what factors influence the attraction between an electron to the nucleus depends on

A

-charge in the nucleus - number of protons (positive charge) in the nucleus, higher the charge, greater the attraction

-distance from the nucleus, smaller the distance, greater the attraction

-shielding from inner electrons/shells, less inner electrons/shells, greater the attraction

30
Q

trends for first ionisation energies across a period

A

TREND 1: general increase
TREND 2: little drop from group 2 to 3
TREND 3: little drop from group 5 to 6
TREND 4: big drop from group 0 to 1/ one period to another

31
Q

Reasons for TREND 1

A

-increase in nuclear charge
-similar shielding and distance
-attraction between outer e- and nucleus

32
Q

Reasons for TREND 2

A

-distance and shielding increase from s to p orbital
-attraction between outer e- and nucleus decrease
-(despite higher nuclear charge)

33
Q

Reasons for TREND 3

A

-outer electron is group 6 is sharing a p orbital
-repulsion between the electrons in the p orbital
-attraction between outer e- and nucleus decrease

34
Q

Reasons for TREND 4

A

-large increase in distance and shielding, into a new electron shell
-attraction between outer e- and nucleus decrease
-(despite higher nuclear charge)

35
Q

Which group has the highest ionisation energy

A

noble gases

36
Q

which group has the smallest ionisation energy

A

group 1

37
Q

what is the relative charge of a proton

A

1+

38
Q

what is the relative charge of an electron

A

1-

39
Q

what is the relative charge of a neutron

A

0

40
Q

when to use RFM

A

could for everything

41
Q

when to use RMM

A

non ion compounds, involving molecules,

42
Q

what is a mass spectrometer used for

A

to determine the relative atomic and molecular mass

43
Q

what does the peak on the graph for a mass spectrometer tell

A

number of each type of ions present, isotopes

44
Q

why do peaks occur at other numbers lower, e.g. 35 and 37 for chlorine

A

molecules break up in the mass spectrometer

45
Q

how is the RMM calculated using the graph

A

the mass value of the molecular/parent ion

46
Q

patterns in graphs for the same compounds

A

molecules in the compound will always break up the same way and in the same proportion
therefore will produce the same pattern in the mass spectrograph

47
Q

how to answer an ionisation energy question

A

PSDS
P-protons (no. of)/nuclear charge
S-shielding(no. of)
D-distance from nucleus
S-strength of attraction

Lower Sixth Chemistry (14 decks)

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