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Chemistry Alevel > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is an atom?

A

The smallest unit of an element that retains it’s chemical properties, consisting of protons, neutrons and electrons

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2
Q

What is a proton?

A

À positively charged subatomic particle found in the nucleus of an atom

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3
Q

What is a neutron?

A

À subatomic particle with no charge, found in the nucleus of an atom

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4
Q

What is an electron?

A

À negatively charged subatomic particle that orbits the nucleus of an atom

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5
Q

What is an atomic number?

A

The number of protons in the nucleus of an atom, which determines the nucleus identity

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6
Q

What is a mass number?

A

The total number of protons and neutrons in an atoms nucleus

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7
Q

What is an isotope?

A

An atom of the same element with the same number of protons but a diferent number of neutrons, resulting in a positive or negative charge

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8
Q

What is an ion?

A

An atom or molecule that has gained or lost one or more electrons resulting in a positive or negative charge

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9
Q

What is relative atomic mass?

A

The weighted average mass of an atom of an element compared to 1/12th of the mass of a carbon-12 atom

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10
Q

What is electron configuration?

A

The arrangement of atoms in an atoms energy levels, sub levels and orbital

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11
Q

What are energy levels?

A

Discrete regions around the nucleus where electrons are likely to be found, also known as shells

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12
Q

What are orbitals?

A

Regions within an energy level where there is a high probability of finding an electron; can hold up to 2 electrons with oposite spins

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13
Q

What is ionisation energy?

A

The energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions

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14
Q

What is first ionisation energy?

A

The energy required to remove one electron from each atom to one mole of gaseous atoms to form one mole of gaseous 1+ ions

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15
Q

What is Successive ionisation energy?

A

The energy required to remove electrons from an atom one by one, after the first electron has been removed

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16
Q

What is atomic radius?

A

The distance from the nucleus to the outer electrons of an atom

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17
Q

What was democritus theory on atoms?

A

He first came up with the idea that everything was made up of atoms and that these are small fundamental balls

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18
Q

What was daltons theory on atoms?

A

In 1803, Dalton realised things were made up of diferent atoms that can be joined together and that there is a diferent atom for each element

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19
Q

What was Thompson discovery?

A

In 1897, Thompson discovered the electron using cathode rays. He came up with the plum pudding model - a theory that suggests atoms are balls of positive charge with negative electrons embedded in it

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20
Q

What was Rutherfords discovery?

A

In 1912, he ddi the alpha scattering experiment. He fired alpha particles at a gold sheet. He discovered that atoms have a small dense positively charged nucleus and empty space and electrons

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21
Q

What did Neil’s bohr discover?

A

. In 1913, he discovered that electrons occupy in orbitals
. Each shell has a fixed energy
. When electrons move between shells, electromagnetic radiation is emitted or absorbed
. Because the energy of shells is fixed, radiation will have a fixed frequency

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22
Q

What did chadwick discover?

A

Neutrons in the nucleus in 1932

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23
Q

What is a sublevel/sub shell?

A

Diferent shaped orbitals called s, p, d and f

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24
Q

How do you calculate the maximum number of electrons a shell can hold?

A

Use the equation 2n², n being the number of the energy level

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25
What must 2 electrons in the same orbital have?
Oposite spins. Electrons either have up spins or down spins
26
Equation of first ionisation energy
Element --> +ion + e-
27
What the electrons in an atom attracted to?
The positive charge of protons in the nucleus
28
What happens to the ionisation energy when there is a greater force of attraction between the outer electrons and the nucleus?
The greater the force of attraction is between the outer electrons and the nuclues, the greater the ionisation energy is
29
What are the 3 factors that effects ionisation energy?
. Atomic radius . Charge on the nucleus . Shielding
30
How does atomic radius affect ionisation energy?
As the atomic radius increases, the force of attraction between the elouter electrons and nucleus decreases, therefore resulting in a decrease in ionisation energy
31
How does nucleus charge affect ionisation energy?
The more protons there are in the nucleus, the bigger the force of attraction is between the outer electrons and the nucleus, therefore resulting in a higher ionisation energy
32
How does shielding effect ionisation energy?
Electrons in the outer shell are repelled by electrons in inner shells. This sheilding effect reduces forces of attraction between outer electrons and nuclues, causing a decrease in ionisation energy
33
Why does ionisation energy increase when electrons are removed from an atom?
Because each time an electron is removed, the remaining electrons in the outer shell are pulled slightly closer to the nucleus, causing a greater force of attraction between outer electrons and nucleus
34
Why does ionisation energy decrease as you move down a group?
Because as you move down a group, the number of shells in the atom increases, which means there is an icnrease in sheilding as you move down the group. And increase in sheilding means the outer electrons are further away from the nucleus so forces of attraction aren't that strong, causing ionisation energy to fall
35
Why does ionisation energy increase as you move across a period?
Because the nuclear charge increases as the number of protons increases, increasing the force of attraction between the outer electrons and the nucleus. Because of this, the atomic radius decreases across a period. Both of these factors means the outer electrons are more attracted to the nucleus, causing ionisation to increase across a period
36
Why do all isotope of an atom react in the same way?
Because they all have the same electronic configuration
37
What is abundance?
Tell us how common each isotope is
38
What is the mass specrometer used for?
To determine the mass number and abundance of isotopes
39
How does the time of flight mass specrometer work?
. Take sample of the element we are interested in and place it into the sample chamber. The sample contains all the diferent isotopes of that element . The atoms then go through ionisation, turning them into +ions. The ions are attracted to a negatively charged plate. An electric field causes the ions to accelerate, increasing the kinetic energy of the ions. All the ions with the same charge will have the same kinetic energy. After passing the plate, the ions then travel to the detector where they gain electrons and become neutral atoms.
40
What does the transfer of electrons at the detector in a mass specrometer cause?
Causes a current to flow
41
How does the mass specrometer determine the mass of isotopes?
The time taken for the isotope to move down the drift chamber
42
How does the mass specrometer determine the abundance of the isotopes?
By measuring the size of the current produced when the isotope hits the detector
43
Why is the inside of a mass specrometer a vacuum?
To prevent ions from colliding with molecules in the air
44
What takes up most of the volume of an atom
The electrons moving around the nucleus in orbitals
45
What does the number of protons in an atom identify
It identifies the element
46
What determines the chemical properties of an element?
The number and arrangment of electrons
47
Why do isotopes of the same element have the same chemical properties
Because they have the same electronic configuration
48
Why do isotopes of the same element have different physical properties
Because they have different masses and physical properties depend on the mass of the atom
49
What is relative isotopic mass
The mass of an atom of an isotope of an element relative to the mass of 1/12th if a carbon 12 atom
50
How do you calculate relative atomic mass
(Isotopic mass x percentage + isotopic mass + percentage) ÷ 100
51
What is relative molecular mass
The average mass of a molecule relative to the 1/12th of the mass of a carbon 12 atom
52
What is relative formula mass
The average mass of all the elements in a compound
53
How are atoms ionised
Done in 2 ways: . Electrospray ionisation - sample is dissolved in solvent and pushed through a small nozzle at a high pressure. A high voltage is applied to it, causing each particle to gain an H+ ion. The solvent is then removed,leaving a gass of +ions . Electron impact ionisation - sample is vapourised, and electrons gun is used to fire electrons at it. This knocks an electron off of each particle, leaving a +ion
54
Whatcis a mass spectrum
A type of graph produced by a mass spectrometer. It shows information on the sample passed through the mass spectrometer
55
What does each line on the graph represent if the sample is an element
Each line will represent a different isotopes of the element
56
What does the x axis and y axis represent in a mass spectrometer
X axis represents the mass/charge of the ions and the y axis represents the abundance of the ions as a percentage
57
What is a way elements can be identified?
Mass spectrometry. Elements with different isotopes produce more than one line in a mass spectrum because the isotopes have different masses. This produces characteristic patterns that can be used as fingerprints to identify certain elements
58
What is a way elements can be identified?
Mass spectrometry. Elements with different isotopes produce more than one line in a mass spectrum because the isotopes have different masses. This produces characteristic patterns that can be used as fingerprints to identify certain elements
59
Whycare second ionisation energies greater than first ionisation energies
Because the electron is being removed from a positive ion and not an atom, which will require more energy. The electron configuration will also contribute to how much larger the second ionisation energy is compared to the first
60
What is the ionisation trend in group 2
. First ionisation energy decreases as you move down group 2
61
What does theyrenf in ionisation energy in group 2 prove
That electrons shells really exsist as the increasing of electrons shells down group 2 increases shielding and reduces nucleus attraction as nucleus and outer electrons are further away. These factors decrease ionisation energy

Chemistry Alevel (8 decks)

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