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AA IB Chemistry HL > Structure 1.1-1.3 > Flashcards

Structure 1.1-1.3 Flashcards

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1
Q

What is an atom?

A

the smallest particle of an element that retains the properties of it

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2
Q

What are the two broad categories in which we classify substances?

A

pure substances and mixtures

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3
Q

What do elements and compounds have in common?

A

they are pure substances

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4
Q

What are pure substances vs mixtures?

A

pure - made up of one type of substance with a fixed composition
mixtures - 2 or more substances combined, no fixed composition

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5
Q

What are elements?

A

building blocks of matter consisting of only one type of atom, cannot be broken down

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6
Q

What are ways in which elements can exist?

A

as individual atoms or atoms of the same element bonded together

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7
Q

What are allotropes?

A

different forms of an element in the same physical state

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8
Q

What are compounds?

A

pure substances composed of two or more different elements chemically combined in fixed ratios

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9
Q

Can compounds be separated using physical methods?

A

no because they are chemically bonded

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10
Q

What are physical methods of separation?

A

separation techniques based on the physical properties of the substance such as boiling point or solubility

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11
Q

What are mixtures?

A

combination of two or more elements or compounds
no fixed ratios
components retain individual properties

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12
Q

Can compounds be separated using physical methods?

A

yes, they contain pure substances which are not chemically bonded

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13
Q

What are 2 classifications of mixtures?

A

homogenous- has a uniform composition with no visible phases/boundaries
heterogenous- non-uniform composition with visible phases/boundaries

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14
Q

How is the distribution of components in hetero/homogenous mixtures?

A

homogenous - equally distributed and in the same state
heterogenous - unequally distributed

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15
Q

What is filtration?

A

separation of an insoluble solid from a liquid/solution
eg through a funnel

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16
Q

What is evaporation as a separation technique?

A

separating a mixture with a solute dissolved (usually in water)

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17
Q

What is solvation?

A

separation of a heterogeneous mixture of 2 solids based on differences in solubility

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18
Q

What is distillation?

A

separation of a liquid mixture based on difference in volatility/boiling points

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19
Q

What is chromatography?

A

used to separate components of a mixture
paper - separate mixture of solutes in a solvent

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20
Q

What is the stationary and mobile phases in chromatography?

A

mobile - solvent undergoing separation
stationary - paper used

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21
Q

How does chromatography work?

A

components of mixture move up paper at different rates due to different solubilities
components with a greater affinity for mobile phase move further up

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22
Q

What is recrystallisation?

A

a separation technique to remove impurities within a solid
uses varied solubilities of solids at different temperatures

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23
Q

Basic principles of recrystallisation?

A

impure mixture dissolved in hot solvent
any insoluble impurities filtered off
solution then cooled, solubility of solid decreases
desired product forms crystals leaving soluble impurities in the solution, then filtered

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24
Q

What is the nature of collisions between particles?

A

elastic - no loss in k.e

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25
What are the properties of solids/liquids/gases?
solids: - cant be compressed - strong forces of attraction - fixed shape and volume - do not flow liquids: - can flow - weaker forces of attraction - no fixed shape, but a fixed volume - cant be compressed gases: - no fixed shape nor volume - weakest forces of attraction - can be compressed due to distance - most k.e
26
Solid --> gas
sublimation
27
Sublimation
solid --> gas
28
Deposition
gas --> solid
29
Gas --> solid
deposition
30
What does vaporisation encompass?
evaporation and boiling
31
When do changes of state occur?
when a substance loses or gains energy
32
The temperature in K...
is directly proportional to the average k.e of particles in the substance
33
Describe a heating curve.
heat is added, temp increases once melting point is reached, temperature is constant as heat is used to overcome intermolecular forces heat is added, temp increases once b.p is reached, temp is constant
34
What is an atom composed of?
mostly empty space occupied by the - electrons surround a very dense + nucleus
35
Composition of an atomic nucleus?
contains protons and neutrons (nucleons) extremely dense, contains all the atomic mass positively charged
36
Are atoms charged?
no - electrically neutral because they contain the same number of p+ and e-
37
What are isotopes?
atoms of the same element with different numbers of neutrons
38
What is Z?
atomic number - protons
39
What is A?
mass number - number of p+n
40
How are positive and negative ions formed?
positive - lose electrons, become x+ negative - gain electrons, become x-
41
What is the relative atomic mass? How is it calculated?
average mass of an atom multiply mass number of each isotope by % abundance
42
How are the abundances of isotopes determined?
using a mass spectrometer uses a measurement of the mass to charge ratio of ions
43
What are emission spectra?
range of frequencies/wavelengths of electromagnetic radiation emitted during an electron transition from a higher to a lower energy level
44
What is the wavelength?
distance between two crests in a wave
45
What is the frequency?
number of waves that pass a point in one second
46
A wave with high energy has...
high frequency and short wavelengths
47
A wave with low energy has...
low frequency and long wavelengths
48
Of the regions in the electromagnetic spectrum, which have the least and most energy?
radio - lowest energy, lowest frequency, longest wavelength gamma - highest energy, highest frequency, shortest wavelength
49
regions of the e.m spectrum from least to most energy
radio microwave infrared visible ultraviolet x-rays gamma rays
50
What is a continuous spectrum?
a spectrum showing all the wavelengths/frequencies of visible light
51
What does an emission line spectrum show?
only specific wavelength and frequencies coloured lines on a black background
52
What is the ground state?
energy level n=1, closest to the nucleus
53
How can electrons transition between energy levels?
by absorbing or emitting energy
54
In what form do electrons absorb energy or emit?
in the form of photons, small packets of energy
55
What happens when an electron absorbs energy?
it transitions from a lower energy level to a higher energy level, now being in an excited state which is less stable than the ground state the unstable electron emits the same amount of energy that it absorbed as it transitions back down amount of energy emitted by the electron corresponds to the wavelength of visible light
56
What determines the amount of energy emitted by an electron?
depends on the size of the transition more energy emitted with bigger transitions
57
For a hydrogen emission spectrum, which transitions form each colour?
n = 6 to 2 -> violet n = 5 to 2 -> indigo n = 4 to 2 -> blue n = 3 to 2 -> red
58
Describe the transitions of electrons in a hydrogen model.
higher energy to levels to n=1: UV radiation higher energy levels to n=2: visible higher energy levels to n=3: infrared
59
How are energy levels spaced?
unevenly - converge at higher energies
60
What is the energy level n=infinity?
the point when the electron has been completely removed from the attraction of the nucleus, ionising the atom
61
What is the Heisenberg uncertainty principle?
it is not possible to know both the location and velocity of electrons
62
How can we use models to overcome the uncertainty principle?
instead of knowing exactly where an electron is, we assign regions of space (atomic orbitals) where electrons are located
63
How are the main energy levels divided?
into sublevels based on the shape of the atomic orbitals
64
Define an atomic orbital.
Regions of space where there is a high probability of finding an electron
65
How many electrons can occupy an atomic orbital?
2 electrons per atomic orbital with specific orientations
66
Shapes and compositions of the s and p orbitals:
s - spherical, only one s atomic orbital per sublevel, max 2 electrons p - dumbbell shaped, three per sublevel, max 6 electrons total
67
What is the d sublevel?
sublevel containing 5 atomic orbitals (10 electrons max)
68
What is the Aufbau principle?
when adding electrons to an atom, the lower energy orbitals must be filled first
69
What is the Pauli exclusion principle?
an atomic orbital can only hold 2 electrons and they must have opposite spins
70
What is Hund's rule?
when filling orbitals of the same energy, each orbital is singly filled before being doubly filled
71
Which have most/least energy out of s,p,d orbitals?
lowest energy - s middle - p highest energy - d
72
What are degenerate orbitals?
atomic orbitals within the same sublevel
73
What are and how are the exceptions to the Aufbau principle?
Copper and chromium - only 1 electron in the 4s
74
What is a nuclear force?
the force that attracts subatomic particles together
75
What is the ionisation energy?
energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous 1+ ions
76
What does ionisation refer to?
the process of removing electrons from an atom in its ground state from n=1 to n=infinity
77
78
What is the convergence limit?
the point at which energy levels in an atom converge, when the electron has been removed
79
What can we use the convergence limit to calculate?
wavelength/frequency of convergence limit can be used to calculate the ionisation energy through the equation E=hf and c=wavelength*f
80
What are successive ionisation energies?
energies required to remove more and more electrons from an ion that is becoming increasingly positive
81
What is the process of successive ionisation?
removing successive e- from an atom or cation
82
In which order are electrons successively removed?
1st - higher energy sublevels Last - lower energy sublevels
83
What is the trend for successive ionisation energies and why?
they increase because the electrons become increasingly positive, leading to a stronger attraction between the nucleus and the e- large increases between different energy levels
84
What is the trend in energy levels for successive ionisation energies?
large increase in energy between energy levels, indicating that the next electron is an energy level closer to the nucleus

AA IB Chemistry HL (12 decks)

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