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Chemistry > Unit 1 > Flashcards

Unit 1 Flashcards

1
Q

How many States and Substates of matter exist?

A

There are Three States of Matter; Solid, Liquid and Gas.
There are 12 Substates of Matter; Plasma, Super Atom, Liquid Crystalline, etc

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2
Q

How are Intermolecular Forces, Potential Energy and Kinetic Energy of Matter related to each other?

A

Intermolecular Forces are directly proportional to Potential Energy

Intermolecular Forces are inversely proportional to Kinetic Energy

Potential Energy is inversely proportional to Kinetic Energy

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3
Q

What were the Two Basic Philosophies our earliest ancestors had regarding the Nature of Matter?

A
  1. Continuous Nature:- Matter is not made of Particles
  2. Discontinuous Nature:- Matter is made of Particles
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4
Q

Which ancient philosophers believed that matter was not made of particles (Continuous Nature)?

A

Empedocles
Plato
Aristotle

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5
Q

The Ancient Philosopher Democritus believed what regarding the nature of Matter?

A

He believed that Matter was comprised of Particles (Discontinuous Nature)
He named these minuscule invisible particles as ‘atomos’ meaning uncuttable and indivisible.

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6
Q

Dalton’s Atomic Theory is a combination of;

A

The Law of Conservation of Mass
&
The Law of Definite Proportions

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7
Q

What did the Law of Conservation of Mass state?

A

The Law of Conservation of Mass states that the Total Magnitude of Mass of a Closed System remains constant during Reactions

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8
Q

Why was the Law of Conservation of Mass rejected?

A

The Law of Conservation of Mass was rejected after the acceptance of Einstein’s Theory of Relativity.
This is because this theory stated that a change in energy is directly correlated to a change in mass so all reactions which are endothermic or exothermic involve an Energy change and thereby involve a Mass change.

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9
Q

What does the Law of Definite Proportions state?

A

The Law of Definite Proportions states that the Ratio of Mass of Any compound is constant regardless of where the composite elements are from.
In other words it states that atoms if the same element are identical regardless of their source.

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10
Q

Why was the Law of Definite Proportions rejected?

A

It was rejected after after the Discovery of Isotopes.

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11
Q

Who discovered Isotopes?

A

William Aston

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12
Q

Who proposed the Law of Conservation of Mass?

A

Antoine Lavoisier

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13
Q

The Law of Definite Proportions was proposed by;

A

Joseph Proust

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14
Q

What was an assumption made by Dalton’s Atomic Theory that was later proved to be false?

A

Dalton’s Atomic Theory stated that Elements could only form Compounds in simple ratios which was discovered to be untrue.

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15
Q

Electric Nature is common among all Matter and therefore there must be a Common phenomena in all matter being

A

A common charged particle. An Atom of Electricity. An Electron.

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16
Q

Who named the Electron?

A

Johnstone Stoney

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17
Q

What is some evidence towards the existence of the Electric Nature of Matter?

A

Electrostatic Forces
Electrochemical Cells
Electrolysis

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18
Q

When does Matter demonstrate its Electric Nature?

A

When Electrons move from one place to another

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19
Q

Who discovered the Charge of One Mol of Electrons?

A

Michael Faraday discovered that the Charge of One Mole of Electrons is 96485 C = 1 F ~=~96500 C.
From this the Charge of One Electron = F/L = 1.602 x 10^-19 C

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20
Q

F is the unit given for the Charge of 1 mol of Electrons but is also equal to

A

=Charge of 1 mol of Protons
=Charge of 1 mol of Monopositive Cations
=Charge of 1 mol of Mononegative Anions
~=~96500 C
Etcetera:
=1/3 x Charge of 1 mol of Tripositive Cations

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21
Q

F/L is the equation by which one can obtain the Charge of 1 Electron but it is also equal to

A

=Charge of 1 Proton
=Charge of 1 Monopositive Cation
=Charge of 1 Mononegative Anion
=1.602 x 10^-19 C
Etcetera:
=1/4 x Charge of 1 Tetranegative Anion

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22
Q

Who were the first scientists to isolate the Electron?

A

Crook, Hitoph and Plucker

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23
Q

What is a Crook’s Tube?

A

A Crook’s Tube otherwise known as a Cathode Ray Tube or a Discharge Tube is the name given for the special setup by which Electrons/Cathode Ray Particles can be separated from Gaseous Matter

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24
Q

Who discovered the Specific Charge of Electrons?

A

The Charge of Electrons per Unit Mass was discovered by J.J.Thomson and was found to be =1.76 x 10^8 C.g^-1

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25
Q

The Oil Drop Test was performed by whom and for what discovery?

A

Robert Millikan performed the Oil Drop Test to discover the Charge of an Electron and found it to be =1.602 x 10^-19 C

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26
Q

We can use the Specific Charge of Electrons and the Charge of 1 Electron to obtain the Mass of 1 Electron=

A

=Charge of 1 Electron / Specific Charge of Electrons
=1.602 x 10^-19 C / 1.76 x 10^8 C.g^-1
=9.1 x 10^-28 g

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27
Q

What are the Experimental Evidences for Electrons to show both Particle and Wave Nature?

A

Particle Nature:- The ability of Electrons to perform Work like moving a Very Light Paddle necessitates them having a Mass

Wave Nature:- The Diffraction Pattern of Electrons implies their Wave Nature

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28
Q

How can one obtain Mathematical/Physical Evidence of the Dual Nature of Electrons?

A

By applying Einsteins Equation, Plancks Equation and the Wave Equation we can obtain De Brougly’s Equation which is: lambda=h/mc where
-lambda-Wavelength
-h-Planck’s Constant
-m-Mass
-c-Speed of Light
implying that Electrons must have values gor Wavelength and mass at the same time

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29
Q

Through what experiment were Positive Rays/Anode Rays/Canal Rays discovered?

A

A modified version of of the Cathode Ray Tube Experiment where the Crook’s Tube was swapped with a Perforated Cathode Ray Tube

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30
Q

Who discovered Anode Rays/Canal Rays/Positive Rays?

A

Eugen Goldstein

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31
Q

Who introduced the Plum Pudding Model regarding the Atomic Structure?

A

J.J.Thomson

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32
Q

What was the Plum Pudding Model?

A

The Plum Pudding Model was a Theory regarding Atomic Structure that stated that Electrons were embedded in a Positively Charged Sphere (Proton)

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33
Q

What are X Rays?

A

X Rays are a type of Electromagnetic Radiation that are placed in between Ultraviolet Light and Gamma Rays on the Electromagnetic Spectrum

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34
Q

Who discovered X Rays?

A

Wilhelm Roentgen

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35
Q

How are X Rays formed?

A

X Rays are formed when Accelerated Cathode Rays strike upon a Metal or Metal Anode.
The Cathode Rays interact with the Metal or Metal Anode and emit X Rays.

36
Q

What is Radioactivity?

A

The Spontaneous Emission of Radiation from Unstable Nuclei to become Stable Nuclei is known as Radioactivity

37
Q

Some Examples of Radioactive Elements are;

A

Francium, Radium, Polonium and other such elements with heavy nuclei or vary large mass numbers

38
Q

Is the Emission of Radiation an Endothermic or Exothermic Process?

A

It is an Exothermic Process because it is a Stabilisation Process

39
Q

How many types of Radiation are there? What are they?

A

There are 3 Types of Radiation; Alpha Rays, Beta Rays, Gamma Rays.

40
Q

Who discovered that Radiation was of three types?

A

Ernest Rutherford

41
Q

By what experiment were they three types of Radiation discovered?

A

The Gold Foil Experiment.
A Radioactive substance was covered by a Thick Lead block except in the direction of a ZnS Screen placed a some distance away. An Electric Field was set up in the area between the substance and the screen. Glow spots would form on the ZnS Screen where the Radiation reached it.

42
Q

Alpha Rays are also referred to as

A

Helium Nucleus

43
Q

Of the 3 types of Radiation released by Radioactive Elements which is an Electromagnetic Radiation?

A

Gamma Ray

44
Q

Electrons, Cathode Rays and Beta Rays are identical in every aspect except

A

Where they originate from.
If they originate from a Very High Voltage and Very Low Pressure Environment they are Cathode Rays.
If they originate from Energy Levels they are Electrons.
If they originate from Unstable Nuclei they are Beta Rays.

45
Q

Alpha Rays can Gain Electrons to

A

Become Helium Atoms

46
Q

How many types of Reactions are there? What are they?

A

There are Three types of Reactions;
Chemical Reactions
Physical Reactions
Nuclear Reactions

47
Q

What are Chemical Reactions?

A

Chemical Reactions are Reactions which occur by the gaining or liberating of Electrons. They are Reactions in which Electrons participate.

48
Q

Are Chemical Reactions reversible or irreversible?

A

Some Chemical Reactions are Reversible and the Others are not.

49
Q

What are Physical Reactions?

A

Physical Reactions are Reactions in which the distance in between particles change therefore they occur due to the change in Intermolecular Forces in between Particles.

50
Q

Are Physical Reactions reversible or irreversible?

A

All Physical Reactions are reversible.

51
Q

What are Nuclear Reactions?

A

Nuclear Reactions are Reactions which occur in the Nuclei of Atoms and are reactions in which the type of element of the reactants changes.

52
Q

Are Nuclear Reactions reversible or irreversible?

A

All Nuclear Reactions are irreversible.

53
Q

What must be considered when balancing Number Reactions?

A

The only thing that must be considered when balancing Nuclear Reactions is that the Sum of the Atomic Numbers and the Sum of the Mass Numbers of the Reactants and Product sides are equal.

54
Q

Why was Thomson’s Plum Pudding Model rejected?

A

Because it could not explain
Spectrums
Flame Test
& Ionisation Energy

55
Q

The scientists Rutherford, Geiger and Marsden famously performed which experiment?

A

The Gold Foil Test/The Alpha-Particle Scattering Test

56
Q

The Gold Foil Test/Alpha-Particle Scattering Test resulted in the discovery of

A

The Nucleus (As Tiny Points where the Mass and Positive Charge of Atoms were stored)
The Typical Radius of Atoms=10^-8 cm Type
The Typical Radius of Nucleus=10^-12,10^-13 Type

57
Q

What is a Nucleon?

A

A Nucleon is a Particle of an Atomic Nucleus and can therefore refer to either a Proton or a Neutron.

58
Q

By which experiment were Isotopes discovered?

A

Mass Spectrometric Analysis

59
Q

A Mass Spectrometric Analysis of an Element can be used to obtain

A

Number of Isotopes
Abundance of Each Isotope
Accurate Relative Atomic Mass of the Element

60
Q

how does one calculate the Accurate Relative Atomic Mass of an Element with Isotopes?

A

The Relative Atomic Mass of each Isotope is multiplied by the Percentage of the Isotope that exists in a sample of the Element. The Sum of this will give you the Accurate Relative Atomic Mass of the Isotope.

61
Q

Why is it that some elements like Oxygen and Hydrogen are considered to have Relative Atomic Masses of 16 and 1 respectively when isotopes pf those elements exist?

A

This is because in both of these cases the percentage of their isotopes that exist in a sample of the element is negligible.

62
Q

The Heaviest Isotope of Elements are generally

A

Unstable and Radioactive

63
Q

Isotopes of an Element are different in their

A

Physical properties

64
Q

Isotopes of an Element are Identical in their

A

Chemical properties

65
Q

Who introduced the Planetary Model of the Atom? What was it?

A

Ernest Rutherford
The Planetary Model of the Atom states that the Protons and Neutrons of an Atom were contained in a tiny Nucleus and that the Electrons of an Atom move around the Nucleus at different Energy Levels depending on their Energies.

66
Q

Who introduced the Meson Theory and Why?

A

The Meson Theory was introduced by Yukawa to explain how a Nucleus containing only Protons and Neutrons as defined by the Planetary Model of the Atom remained Stable despite the Repulsive Forces that would be acting.

67
Q

What is the Meson Theory?

A

The Meson Theory states that within a Nucleus whenever Two Protons are about to repel each other a Neutron emits a Negative Meson to Neutralise one of the Protons.

68
Q

What is the Descending Order of the Nucleus Stability as dependent on the Ratio of
The Number of Neutrons (nn) : The Number of Protons (np)

A

nn/np=1
nn/np=multiple of 4
nn/np=multiple of 2
nn/np=multiple of 3

69
Q

What happens if there is an Unnecessarily Larger number of Neutrons than Protons within a Nucleus?

A

This means that when Protons are about to meet an Excessive number of Mesons will form which destabilises the Nucleus. As such the Nucleus is likely to release some of the Neutrons as Beta Rays or other Radiation.

70
Q

Is the conversion of a Neutron to a negatively charged Meson and a Proton a Exothermic or a Endothermic Reaction?

A

By analysing the masses of Neutrons, Protons and Mesons we can identify that a Mass loss takes place during the above conversion. This means a Energy loss / Energy release also took place.
As the conversion is an Exothermic Process we can infer that it is a Stabilisation Process as well.

71
Q

Rutherford’s Planetary Model of the Atom failed to explain;

A

Stability of the Nucleus as stated in the model
Spectra
Flame Test
Ionisation Energies

72
Q

What is a Wave?

A

A mode of Energy Transmission

73
Q

What is a Wave Cycle?

A

A Wave Cycle consists of One Peak/Crest and One Trough.

74
Q

What is the Frequency(f) of a Wave?

A

The Number of Wave Cycles that occur per second.

75
Q

What is the Wavelength(lambda) of a Wave?

A

The Distance between two consecutive peaks or troughs.

76
Q

What is the Amplitude of a Wave?

A

The Distance between the Midline of a Wave and a peak or trough.

77
Q

How is the Energy of a Wave related to it’s Wavelength?

A

The Energy of a Wave is inversely proportional to it’s Wavelength

78
Q

How is the Stability of a Wave related to it’s Frequency?

A

The Stability of a Wave is inversely proportional to it’s Frequency

79
Q

How is the Stability of a Wave related to it’s Wavelength?

A

The Stability of a Wave is directly proportional to it’s Wavelength

80
Q

What is the Wavelength Range of Visible Light?

A

Red ~> Violet = 700nm ~> 400 nm

81
Q

What is a Line Spectrum?

A

A Line Spectrum is otherwise known as a Discontinuous Spectrum and is obtained when Discontinuous Radiation is sent through a Spectrometer. Discontinuous Radiation is Radiation which does not contain all the possible Wavelengths and Frequencies.

82
Q

Where is the Infinite Energy Level in an Atom?

A

It is at the closest point to the atom where the Nuclear Attraction is Zero.

83
Q

How can Atoms have an Infinite Number of Energy Levels?

A

This is because referring to their number as infinite is a way to demonstrate that Electrons of any Energy may be accommodated by the atom.

84
Q

What is the Energy at the Infinite Energy Level of an Atom?
What does this imply?

A

We consider it to be Zero.
This implies that all the other Energy Levels have Negative Energies.

85
Q

What is the variation of the Energy Difference between consecutive Energy Levels of an Atom?

A

The Energy Difference between adjacent Energy Levels is continuously halved among consecutive Energy Level Pairs.

86
Q

How can one obtain a Discontinuous Spectrum using Solids?

A

The Reaction of a Flame with an Inert Metal, their Chlorides or Graphite releases Radiation that forms a Discontinuous Spectrum once passed through a Spectrometer.

87
Q

How can one obtain a Line Spectrum using a Gas or Vapour?

A

Simply passing an electric current through a Gas or Vapour releases Radiation that forms a Discontinuous Spectrum upon contacting a Spectrometer.

Chemistry (2 decks)

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