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IB Chemistry > S1 Models of the particulate nature of matter > Flashcards

S1 Models of the particulate nature of matter Flashcards

(104 cards)

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1
Q

What does “Kelvin” mean?

A

Absolute temperature scale. Conversion from ºC by subtracting 273.15
from it

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2
Q

What does “Celsius” mean?

A

Unit of temperature. Conversion from K by adding 273.15 to it.

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3
Q

Features of Solids

A
  • Fixed volume
  • Fixed shape
  • Can vibrate in position but can’t change location
  • Closely packed
  • Strong inter-molecular forces
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4
Q

Features of Liquids

A
  • Fixed volume
  • Non-fixed shape
  • Particles can slide over each other and take their container’s shape
  • Slightly more spaced out particles than solids
  • Weaker inter-molecular forces than solids
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5
Q

Features of gases

A
  • Non-fixed volum​e
  • Non-fixed shape
  • Particles move freely in space
  • Fully spread out particles
  • Negligible inter-molecular forces
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6
Q

What is “Melting”?

A

Process in which particles in a solid substance gain enough kinetic energy to overcome its strong inter-molecular forces, allowing them to move freely and transition into a liquid state.

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7
Q

What is “Freezing”?

A

Process in which particles in a liquid lose enough kinetic energy to be held together by inter-molecular forces, making them slow down into a fixed location transitioning into a solid state.

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8
Q

What is “Vaporization”?

A

Process in which particles in a liquid gain enough kinetic energy to overcome any remaining inter-molecular forces, allowing them to move independently and transition to a gas.

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9
Q

What is “Evaporation”?

A

Vaporization that depends on vapor pressure, and happens in a liquid’s surface.

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10
Q

What is “Boiling”?

A

Vaporization that depends on temperature, and can happen anywhere.

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11
Q

What is “Condensation”?

A

Process in which particles in a gas lose enough kinetic energy to be held together by inter-molecular forces, making them slow down at a given location and transitioning into a liquid state.

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12
Q

What is “Sublimation”?

A

Sublimation is the direct transition of a solid into a gas when its vapor pressure exceeds the surrounding pressure before melting, typically occurring under low pressure or at temperatures below its melting point.

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13
Q

What is “Deposition”?​

A

Deposition is the direct transition of a gas into a solid when its vapor pressure drops below the surrounding pressure without passing through the liquid phase, typically occurring under low temperatures and high pressure. Also called “desublimation” as it frequently happens after sublimation.

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14
Q

What are “Elements”?

A

Elements are pure substances made up of atoms, each with the same number of protons. There are 118 known elements that are ordered in the periodic table. They can’t be broken down into simpler molecules by physical or chemical means.

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15
Q

What are “Compounds”?

A

Compounds are substances that are made out of two or more elements chemically bonded in the same way at a fixed ratio.

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16
Q

What is a “Boiling Point”?

A

The temperature at which a liquid boils into a gas.

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17
Q

What is a “Melting point”?

A

The temperature at which a solid melts into a liquid.

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18
Q

What are “Mixtures”?

A

Substances made out of two or more different types of elements or compounds.

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19
Q

What are “Homogeneous mixtures”?

A

Mixtures in which all of its components are in the same phase.

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20
Q

What are “Heterogeneous mixtures”?

A

Mixtures in which some of its components are in different phases.

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21
Q

What is the kinetic molecular theory?

A

The kinetic molecular theory is a model that explains the different states of matter, based on the idea that all molecules are constantly in motion, and that temperature is based on the speed at which such particles move.

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22
Q

What is a change of state?

A

Changes of state, according to the kinetic molecular theory, occur when particles’ kinetic energy changes to a point at which they can overcome their intermolecular attractive forces thanks to a supply of kinetic energy, or they lose kinetic energy until their intermolecular attractive forces overpower them.

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23
Q

Define endothermic

A

Reaction or change of state which absorbs energy in the form of heat.

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24
Q

Define exothermic

A

Reaction or change of state which releases energy in the form of heat.

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25
What is a reaction's Percentage Yield?
The percentage of product obtained in a reaction relative to the maximum theoretical yield it had: Percentage Yield = ((Actual Yield)/(Theoretical Yield))*100t
26
What is a proton?
Positively charged sub-atomic particle found in the nucleus of an atom.
27
What is a neutron?
Neutrally charged sub-atomic particle found in the nucleus of an atom.
28
What is an electron?
Negatively charged sub-atomic particle orbiting the nucleus of an atom.
29
Define Atomic Number (Z)
Refers to the amount of protons there are in an atom, used to differentiate different elements.
30
Define Mass Number (A)
Refers to the amount of Protons and Neutrons there are in a given atom
31
Define Isotope
An atom of a given element with a different mass number to that of another atom of the same element
32
Define Relative Atomic Mass (Ar)
The average mass of a naturally occurring atom relative to 1/12th of a carbon atom (i.e. using the carbon-12 scale).
33
Filtration
Process where a solid is separated from liquid through a membrane as a residue, while filtrate passes through.
34
Distillation
Process where solvents are separated from a solute when one has a lower boiling point than another. The solution is heated to the solvent's boiling point, which is collected as a gas and condensed.
35
Chromatography
Process where a mixture is passed through solution through a medium, where each component has a different refractive index (similar particles to medium have higher refractive indexes).
36
Crystallization
Process where a dissolved solid is extracted by boiling its solvent, making crystals.
37
Emission spectra
Light emitted by given atoms after their electrons become "excited" (constant energy supply is cut) as they drop from high energy levels back to their base ones.
38
Hydrogen emission spectrum proof
Proof that the electron in hydrogen can only exist in fixed energy levels, as the line spectra appear at distinct frequencies.
39
UV region of line spectrum
Electron drops to n=1
40
Visible light region of line spectrum
Electron drops to n=2
41
IR region of line spectrum
Electron drops to n≥3
42
Define mass defect
Difference between the mass of an isotope and the relative atomic mass of that element.
43
What causes radioactivity?
Unstable nuclei undergoing spontaneous decay.
44
What are the three main types of radioactive decay?
Alpha (α), beta (β), gamma (γ).
45
What is emitted during alpha decay?
A helium nucleus (i.e. 2 protons and 2 neutrons).
46
What is emitted during beta decay?
An electron/positron and a neutrino/anti-neutrino.
47
What is emitted during gamma decay?
High-energy electromagnetic radiation (gamma rays).
48
What is the role of neutrons in nuclear stability?
Prevent repulsion between protons from within the nucleus.
49
Define band of stability.
Ratio of neutrons to protons required for nuclear stability.
50
What is m/z?
Mass-to-charge ratio in a spectrometer.
51
What is Carbon-14 used for?
Carbon dating
52
What is an atomic orbital?
A region around the nucleus where an electron is likely to be found.
53
What types of orbitals are there?
s, p, d, f.
54
How many electrons can be held in an s orbital?
2
55
How many electrons can be held in an p orbital?
6
56
How many electrons can be held in a d orbital?
10
57
How many electrons can be held in an f orbital?
14
58
Shape of s orbital
Spherical
59
Shape of p orbital
dumbbell-shaped
60
What orbitals are present in the first energy level?
Only s.
61
What orbitals are present in the second energy level?
s & p.
62
What orbitals are present in the third energy level?
s, p, & d
63
What is an energy level?
A series of orbitals that share the same principal quantum number (n).
64
Order of orbital filling
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p
65
What does the Aufbau principle state?
Electrons fill the lowest energy orbitals first.
66
What does Hund's rule state?
Electrons fill orbitals singly before pairing.
67
What does Pauli's exclusion principle state?
No two electrons in the same shell can have the same spin (therefore there's max 2 electrons per orbital, opposite spins)
68
What causes emission spectra in atoms?
Photons are emitted when electrons fall from excited states to lower energy levels.
69
What type of spectrum is produced when atoms emit light?
Line emission spectrum.
70
What is the spin quantum number?
Describes the two possible spin states of an electron in an orbital: +½ or −½.
71
Why does oxygen have a lower first ionization energy than nitrogen?
Because oxygen has electron pairing in one of its p orbitals, which causes electron-electron repulsion, making it easier to remove an electron.
72
What can be used to observe line spectra?
Gas discharge tubes along with diffraction gratings or prisms.
73
What does a continuous spectrum show?
All wavelengths of visible light in a seamless range, like a rainbow.
74
How does a line spectrum differ from a continuous spectrum?
A line spectrum consists of discrete lines at specific wavelengths, unlike a continuous range of colors.
75
Why do emission spectra provide evidence for unique elements?
Each element has a distinct set of energy levels, producing a unique pattern of spectral lines.
76
How does an element’s highest main energy level relate to its period?
The principal quantum number (n) of the highest occupied energy level corresponds to the element's period on the periodic table.
77
What does the block of an element on the periodic table indicate?
It shows the type of orbital (s, p, d, f) being filled with electrons for that element.
78
What sublevel is being filled in the p-block?
The p orbital sublevel.
79
Which block contains the transition metals?
The d-block.
80
Which model of the atom explains line spectra?
The Bohr model.
81
What led to the development of quantum mechanics?
The inability of classical models to explain atomic spectra and fine structure.
82
What did Thomson's cathode ray experiments contribute to atomic theory?
They led to the discovery of the electron and introduced the concept of subatomic particles.
83
Why did the Bohr model need refinement?
It couldn't account for the spectra of multi-electron atoms or explain fine structures in spectral lines.
84
Define "emission spectrum."
A series of spectral lines emitted by atoms when electrons fall from higher to lower energy levels.
85
What is the Heisenberg uncertainty principle?
It states that it's impossible to simultaneously know both the exact position and momentum of an electron.
86
What is a mole?
A mole is a specific amount of substance, 6.02x10²³.
87
What is molar mass?
The mass of one mole of any given substance, measured in g mol⁻¹.
88
What is molecular formula?
The number of atoms of each element in a single particlo of a substance.
89
What is empirical formula?
The simplest whole number ratio of atoms of each element in the particle of a substance (e.g. ethane's molecular formula is C₂H₆, but its empirical formula is CH₃).
90
Define solute
The substance that is dissolved.
91
Define solvent
The substance that dissolves a solute.
92
Define solution
The resultant mixture after a solute is dissolved in a solvent.
93
What are half-equations?
Equations that show the movement of electrons when there's changes in oxidation states, they look only at specific atoms.
94
What are spectator ions?
Ions that become dissociated in an environment during a reaction and take no part in it.
95
What are excess or limiting reagents?
The limiting reagent runs out first, stopping the reaction, while the excess reagent is left over.
96
What is percentage yield?
The percentage of product that a reaction yields in practice (during experiments) in relation to what it should theoretically yield.
97
What is atom economy?
The amount of mass of products that are useful after a reaction. 100% means all of the products find a practical use.
98
What are standard solutions?
Solutions with a precisely known concentration of a solute.
99
What is a titration?
Method through which the acidity of a substance is calculated by mixing it with a substance of known, opposite pH under and indicator.
100
What is Avogadro's law?
At the same temperature and pressure, equal volumes of different gases contain the same amount of molecules.
101
What is the ideal gas equation and each unit in it?
- P Pressure (Pa) - V Volume (m³) - n Amount of Substance (mol) - R Universal Gas Constant (8.314 J/(mol·K)) - T Temperature (K)
102
How much volume does a gas occupy at STP?
22.4L (0,0224m³)
103
How is the value for absolute zero temperature found?
By extrapolating the curve in the Volume-Temperature graph to find a value for absolute zero (-273.15ºC i.e. 0K)
104
What are the differences between real and ideal gases?
- Real gas particles occupy volume, not negligible as in the ideal gas model - There are significant (Van der Waals) forces of attraction between gases in many cases

IB Chemistry (2 decks)

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