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A-LEVEL CHEMISTRY > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

What happened in 1661, in terms of history of the atom? (1)

A

Robert Boyle proposed that there were some substances that could not be made simpler (the chemical elements of today).

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2
Q

What happened in 1803, in terms of history of the atom? (2)

A

-John Dalton suggested that all the atoms of a particular element had the same mass and atoms of different elements had different masses.

-he also suggested that atoms could not be broken down.

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3
Q

What happened in 1896, in terms of history of the atom? (1)

A

-Henri Becquerel discovered radioactivity, meaning that atoms were not in disable like previously thought.

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4
Q

What happened in 1897, in terms of history of the atom? (3)

A

J.J. Thompson discovered the electron, the first subatomic particle to be discovered. He also showed that they had a negative charge and that they were the same in all elements.

He later suggested that electrons were located within the atom in circular arrangements, thus producing the plum pudding model.

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5
Q

What happened in 1911, in terms of history of the atom? (1)

A

Ernest Rutherford and his team found that most of the mass and all the positive charge of the atom was in a tiny central nucleus.

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6
Q

What are the three fundamental particles of the atom? (3)

A

-electron

-proton

-neutron

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7
Q

What is held within the nucleus? (2)

A

Protons and neutrons.

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8
Q

What is located outside of the nucleus? (1)

A

Electrons, arranged in shells or orbitals.

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9
Q

What is the relative charge and mass of a proton? (2)

A

Relative charge: +1

Relative mass: 1

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10
Q

What is he relative charge and mass of a neutron? (2)

A

Relative charge: 0

Relative mass: 1

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11
Q

What is the relative charge and mass of an electron? (2)

A

Relative charge: -1

Relative mass: 1/1840

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12
Q

How are the subatomic particles in the nucleus held together? (2)

A

They are held together by a force called the strong nuclear force. This is much stronger than the electrostatic forces of attraction.

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13
Q

What is the atomic number? (1)

A

The number of protons in an atom.

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14
Q

What is the symbol used in equations to represent the atomic number? (1)

A

Atomic number = Z

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15
Q

What is the mass number? (1)

A

The total number of protons and neutrons in the nucleus.

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16
Q

What is the symbol used in equations to represent the mass number? (1)

A

Mass number = A

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17
Q

What is the number of protons and neutrons in a nucleus often referred to as? (1)

A

The number of nucleons.

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18
Q

What is a isotope? (1)

A

Atoms with the same number of protons and a different number of neutrons.

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19
Q

What are some properties of isotopes? (2)

A

Different isotopes of the same element react chemically in exactly the same way as they have the same electron configuration.

Ted to vary in mass number because of the different number of neutrons in its nuclei.

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20
Q

What happened in 1913, in terms of the development of electron configuration? (3)

A

Niels Bohr suggested that the atom consisted of a tiny positive nucleus orbited by negatively-charged electrons to form an atom. Theorised that electrons moved from one shell to the next explained how atoms absorbed and gave out light, thus the beginning of the quantum theory.

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21
Q

What happened in 1928, in terms of the development of electron configuration? (2)

A

Erwin Schrödinger, created an equation that used the idea that electrons had some properties of waves . Led to a theory called quantum mechanics.

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22
Q

What happened in 1932, in terms of the development of electron configuration? (1)

A

James Chadwick discovered neutrons.

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23
Q

What did Gilbert Lewis do? (3)

A

-the inertness of the noble gases was related to their full outer shells.

-ions were formed by atoms losing or gaining electrons to get full outer shells.

-atoms could bond by sharing electrons to get full outer shells.

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24
Q

Why is Dalton’s model of the atom useful? (1)

A

Can be used to explain the geometries of crystals.

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25
Why s Bohr’s model useful? (1)
Used for a simple model of ionic and covalent bonding.
26
What is the mass spectrometer? (1)
The most useful instrument for the accurate determination of relative atomic masses.
27
What is the relative atomic mass symbol? (1)
Ar
28
How is relative atomic mass defined? (1)
Are measured on a scale on which the mass of an atom of (12)C is defined as exactly 12.
29
What is the equation to calculate the relative atomic mass (Ar)? (1)
Average mass of 1 atom Relative atomic mass = ————————————— 1/12 mass of 1 atom of (12)C
30
What is the equation to calculate the relative molecular mass (Mr)? (1)
Average mass of molecule Relative molecular mass = ————————————— 1/12 mass of 1 atom of (12)C
31
What is an example of how mass spectrometers are used? (1)
They are used by forensic scientists to help identify substances such as illegal drugs.
32
What is the main function of a mass spectrometer? (1)
The principle of forming ions from the sample and then separating the ions according to the ratio of their charge to their mass.
33
What happens inside a time of flight mass spectrometer? (1)
The substance in the sample are converted to positive ions, accelerated to high speeds (which depends on their mass to ratio charge ratio), and arrive at a detector.
34
What happens at the vacuum stage, in terms of a time of flight mass spectrometer? (1)
The whole apparatus is kept under a high vacuum to prevent thee ions that are produced colliding with molecules from the air.
35
What are the two types of ionisation, in terms of time of flight mass spectrometry? (2)
-electrospray ionisation -electron impact
36
What is electrospray ionisation, in terms of time of flight mass spectrometry? (3)
-the sample is dissolved in volatile solvent and forced through a fine hole needle that is connected to the positive terminal of a high voltage supply. -this produces tiny positively charged droplets that have gained a proton from the solvent. -the solvent evaporates from the droplets into the vacuum and the droplets get smaller and smaller until they contain nothing but a single positively charged ion.
37
What s electron impact, in term of time of flight mass spectrometry? (1)
-the sample is vaporised and high energy electrons are fired at it from an electron gun, this usually knocks of one electron from one particles forming a 1+ ion.
38
What is a electron gun, in terms of electron impact? (1)
Is a hot wire filament with a current running through it that emits a beam of high energy electrons.
39
What is acceleration, in terms of time of flight mass spectrometry? (2)
Where the positive ions are attracted towards a negatively charged plate and accelerate towards it. (Lighter ions and more highly charged ions achieve a higher speed).
40
What is ion drift, in terms of time of flight mass spectrometry? (1)
The ions pass through a hole in the negatively charged plate, forming a beam and travel along a tube,called the flight tube, to a detector.
41
What is meant by detection, in terms of time of flight mass spectrometry? (2)
When ions with the same charge arrive at the detector, the light ones come first (have a higher velocity). The flight times are recorded. The positive ions pick up an electron from the detector, which causes a curent to flow.
42
What is meant by data analysis,in terms of time of flight mass spectrometry? (1)
The signal from the detector. Is passed to a computer hitch generates a mass spectrum.
43
What are the stags of time of flight mass spectrometry? (6)
-vacuum -ionisation -acceleration -ion drift -detection -data analysis
44
What is high resolution mass spectrometry? (1)
When mass spectrometers are used to measure relative atomic masses to five decimal places of an atomic mass unit.
45
What is low resolution mass spectrometry? (1)
When mass spectrometers are used to measure relative atomic masses to one decimal place of an atomic mass unit.
46
What is the relative atomic mass equation? (1)
(Isotope mass x relative abundance) + (isotope mass x relative abundance) Relative atomic mass = ——————————————————————————————————— 100
47
What is the symbol for a proton? (1)
P+
48
What is an atom? (1)
The smallest component of an element.
49
What are electron orbitals called? (2)
Energy levels or principal quantum levels
50
How are electron levels numbered? (1)
Are numbered 1, 2, 3 away from the nucleus.
51
What is the symbol for a neutron? (1)
N.
52
What did Millikan do? (1)
Measured the charge of an electron….
53
When was the Leiger Marston experiment? (1)
1909
54
What was the Leiger Marston experiment? (1)
Alpha particles were fired at a thin gold foil, most passed through unaffected, few passed through but deflected, very few reflected backwards towards the source.
55
What did the Leiger Marston experiment suggest? (2)
Suggested that the mass (protons + neutrons) and positive charge (protons) of atom are concentrated in a very small part of an atom, (nucleus).
56
What is the overall charge of the atom? (1)
Overall atom has no charge.
57
What are the isotopes of bromine? (2)
-(79) Br = 50% abundance -(81) Br = 50% abundance
58
What are the isotopes of chlorine? (2)
-(35) Cl = 75% abundance -(37) Cl = 25% abundance
59
What is the formula of bromomethane? (1)
CH(3)Br
60
What is the formula of chloromethane? (1)
CH(3)Cl
61
What is the standard atom known as? (2)
The Standard atom is an atom of carbon with a mass of 12. -we compare the masses of all molecules on this atom.
62
What is the Mr value? (1)
Sum of Ar values of each atom in said formula.
63
What are the sub-levels named in any given principal level? (4)
-‘s’ -‘p’ -‘d’ -‘f’
64
What are the sub-levels in the first quantum? (1)
1s
65
What are the sub-levels in the second quantum? (2)
2s and 2p.
66
What are the sub-levels in the third quantum? (3)
3s, 3p and 3d.
67
What are the sub-levels in the fourth quantum? (4)
4s, 4p, 4d and 4f.
68
What are the sub-levels in the fifth quantum? (5)
5s, 5p, 5d, 5f and 5g.
69
How much can each sub-level hold? (1)
Each sub-level type can hold up to a fixed maximum number of e-.
70
How many e- can sub-level ‘s’ hold? (1)
2 e.g. 1s(2)
71
How many e- can sub-level ‘p’ hold? (1)
6 e.g. 2p(6)
72
How many e- can sub-level ‘d’ hold? (1)
10 e.g. 3d(10)
73
What is the Aubaw principle? (1)
States that ‘electrons fill the sub-levels in order of increasing energy’.
74
What determines how strong electron orbitals are? (1)
Th closer the orbitals get to the nucleus the stronger hold they have.
75
What does isoelectric mean? (1)
Have the same electron configuration e.g sodium and neon.
76
What is an orbital? (1)
An orbital is a region of space where there is a high probability of finding an electron.
77
How many orbitals are in sub-level ‘s’? (1)
1 orbital.
78
How many orbitals are in sub-level ‘p’? (1)
3 orbitals.
79
How many orbitals are in sub-level ‘d’? (1)
5 orbitals.
80
What are ‘s’ orbitals? (1)
Are all spherical, positioned inside each other with increasing radius.
81
What are ‘p’ orbitals? (1)
Are three ‘dumbbell’ shapes at right angles to each other.
82
What is meant by electron spins? (1)
Electrons spin in opposite directions.
83
How many electrons can each quantum level hold? (1)
The maximum number of electrons in each orbital is 2 with opposite spin.
84
How do we represent electron orbitals? (1)
Boxes are used to represent orbitals.
85
What is the symbol for an electron? (1)
E-
86
What is ionisation energy, in terms of electron configuration? (1)
When electrons are removed from atoms and the energy it takes to remove them can be measured, therefore making the atom a positive ion.
87
What is ionisation energy measured in,in terms of electron configuration? (1)
Measured in kJ mol (-1)
88
How is ionisation energy abbreviated, in terms of electron configuration? (1)
IE.
89
What is the first IE, in terms of electron configuration? (1)
When the first electron needs the least energy to remove it because it is being removed from a neutral atom.
90
What is the second IE, in terms of electron configuration? (1)
The second electron needs more energy than the first because it is being removed from a +1 ion.
91
what are the trends in ionisation energies in periods ,in terms of electron configuration? (1)
-generally increase across a period because the nuclear charge is increasing and this makes it more difficult to remove an electron.
92
What are the trends in ionisation energies in groups, in terms of electron configuration? (1)
There is a general decrease in first ionisation energy going down group 2 and the same pattern is seen in other groups, this is because the outer electron is in a main level that gets further from the nucleus in each case.
93
When will ionisation energy increase, in terms of electron configuration? (3)
-when protons increase -when shielding decreases -when the radius decreases
94
When will ionisation energy decrease, in terms of electron configuration? (3)
-when protons decrease -when shielding increases -when the radius increases
95
What does the group number mean,in terms of electron configuration? (1)
Is the number of electrons in the outer energy level.
96
What is the period number, in terms of electron configuration? (1)
Is the number of energy levels.

A-LEVEL CHEMISTRY (58 decks)

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