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chem u2 atomic structure and properties > Early Models of the Atom (2.1) > Flashcards

Early Models of the Atom (2.1) Flashcards

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1
Q

Which law did Antoine Lavoisier introduce?

A

Law of Conservation of Mass

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2
Q

Which law did Joseph Proust introduce?

A

Law of Definite Proportions

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3
Q

Which law did John Dalton introduce?

A

Law of Multiple Proportions

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4
Q

What were the 4 key points of Dalton’s atomic theory?

A
  1. Elements are made of atoms
  2. Atoms of a given element are identical; different elements have different atoms
  3. Compounds form when atoms join together; a given compound always has the same numbers and types of atoms
  4. Reactions involve the rearrangement of atoms (but don’t change the atoms themselves)
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5
Q

Who created the billiard ball model?

A

John Dalton

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6
Q

What is the charge-to-mass ratio of an electron?

A

charge on the electron (e) in coulombs (C) / mass in grams = -1.76 x 10⁸ C/g

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7
Q

Which model did J.J. Thompson create and how does it work?

A

Plum pudding model: entire atom is positively charged with negative electrons embedded in it

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8
Q

What did Ernest Rutherford conclude when he tested Thomson’s model?

A

The center of the atom must be positively charged and dense; used the term “protons” for the positively charged particles; most of the atom is empty space

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9
Q

Which model did Rutherford create and how does it work?

A

Nuclear atom model: an atom with a dense positive nucleus containing protons with electrons moving around the nucleus

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10
Q

Who suggested the existence of neutrons and why?

A

Rutherford; found that protons and electrons could only account for about half the mass of any atom

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11
Q

Who proved the existence of neutrons?

A

James Chadwick

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12
Q

Who first explained the idea of isotopes and what are they?

A

James Chadwick; atoms of the same element with different masses

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13
Q

Describe the nucleus

A

Very dense; contains nearly all of the atom’s mass

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14
Q

In standard atomic notation, what does each letter stand for?

A

A - the number of protons + neutrons (mass number)
Z - the number of protons (atomic number)
X - element symbol

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15
Q

What changes and what stays the same in isotopes?

A

The number of electrons and neutrons CAN change; the number of protons NEVER changes for any element

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16
Q

Describe how protons behave

A

Protons are tightly packed inside the nucleus - these particles repel each other

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17
Q

Describe how neutrons behave

A

Neutrons separate the protons reducing repulsion and stabilizing the nucleus

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18
Q

What force attracts protons and neutrons to each other?

A

Strong nuclear force

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19
Q

What is needed to make an atom stable?

A

The right balance of protons and neutrons

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20
Q

What happens when protons and neutrons are not properly balanced?

A

The nucleus becomes unstable and decays into a more stable nucleus

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21
Q

Define radioisotopes

A

Isotopes with unstable nuclei that decay into different (often more stable) isotopes

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22
Q

Define isotopic abundance

A

The percentage of a given isotope in a sample of an element

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23
Q

What is a mass spectrometer?

A

A measuring instrument used to determine the mass and abundance of isotopes

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24
Q

What do we call the data produced by mass spectrometers?

A

Mass spectrum

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25
Q

Define nuclear radiation

A

Energy or small particles emitted as an isotope decays

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26
Q

What are the 3 common types of nuclear radiation?

A
  1. Alpha particles
  2. Beta particles
  3. Gamma radiation
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27
Q

Define alpha particle

A

Same as He-4 atom (2 protons and 2 neutrons) with +2 charge; low energy - can be blocked by paper

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28
Q

Define beta particle

A

A negatively charged electron that can pass through paper but not metals

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29
Q

Define gamma radiation

A

High energy electromagnetic radiation; travels at speed of light and can penetrate most things except for lead

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30
Q

Define atomic mass unit

A

The mass of an element shown in the periodic table (atomic mass units, u); one atomic mass unit is equal to one twelfth the mass of a carbon-12 atom

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31
Q

How do you calculate average atomic mass?

A

Sum the known isotopes for an element multiplied by their percentage abundance

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32
Q

Define electromagnetic radiation

A

One of the many ways energy travels; travels at the speed of light through a vacuum

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33
Q

Define wavelength

A

The distance between peaks or troughs in a wave

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34
Q

What is frequency?

A

The number of waves (cycles) per second that pass a given point per second

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35
Q

Which wavelength radiation has the highest frequency?

A

Short-wavelength radiation

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36
Q

What’s the speed of light formula?

A

(wavelength in m)(frequency in Hz) = C (speed of light)

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37
Q

What did Max Planck discover about matter?

A

Matter could not absorb or emit any quantity of energy

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38
Q

What did Planck mean by “energy is quantized”?

A

It could only be absorbed or emitted in whole number multiples of hv

39
Q

What do the letters in hv stand for?

A 
v = frequency
h = Planck's constant 6.626x10^-34 J-s
40
Q

What is the formula for the change in energy for a system?

A 
Delta E (Change in energy) = nhv
(n = an integer, h = Planck's constant, v = frequency)
41
Q

Define continuous spectrum

A

The spectrum observed when light is passed through a prism (a rainbow)

42
Q

Which light contains all wavelenghts?

A

White light

43
Q

Define line spectrum

A

The spectrum observed when the emission spectrum of an element is passed through a prism (only a few discrete lines are seen)

44
Q

What is the quantum model and who created it?

A

Niels Bohr proposed that the electron in hydrogen moves around the nucleus on fixed orbits (shells)

45
Q

What did Bohr conclude about the movement of electrons?

A

They could only orbit in fixed paths or shells around the nucleus

46
Q

What is Coulomb’s Law?

A

The force between two charged particles is proportional to the magnitude of the charges and inversely proportional to the square of the distance between them

47
Q

What is the Heisenberg Uncertainty Principle?

A

There is a limit to precisely knowing the position and momentum of a particle

48
Q

What did De Broglie reason about the electron?

A

The electron, long considered to be a particle, showed wave properties too

49
Q

In Schrodinger’s equation, what does the H, w and E stand for?

A

H: the operator
W: wave function
E: total energy of atom

50
Q

The more accurately we know a particle’s position…

A

The less accurately we know momentum

51
Q

What are probability distributions?

A

The probability of finding an electron in a given space

52
Q

Where does one have the greatest probability of finding an electron and why?

A

Closest to the nucleus, because the further away the electron is, the more space it can occupy

53
Q

What shape are s orbitals? How many electrons can they hold?

A

Spherical; can hold a maximum of 2 electrons

54
Q

What shape are p orbitals and how many electrons can they hold in total?

A

Dumbbells/figure 8s; have 3 lobes (x, y, z) each holding 2 electrons for a total of 6 electrons

55
Q

What shape are d orbitals and how many electrons can they hold in total?

A

Dumbbells/figure 8s; have 5 lobes each holding 2 electrons for a total of 10 electrons

56
Q

What shape are f orbitals and how many electrons can they hold in total?

A

Dumbbells/figure 8s; have 7 lobes each holding 2 electrons for a total of 14 electrons

57
Q

What is the aufbau principle?

A

In the ground state of an atom or ion, electrons fill orbitals of the lowest energy levels before occupying higher levels

58
Q

Give the first twelve in the filling order of orbitals

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s

59
Q

What is the electron correlation problem?

A

Since the exact pathways of electrons cannot be calculated, their exact repulsions cannot be calculated either

60
Q

What is the shielding effect?

A

Inner shell electrons shield outer shell electrons from the pull of the nucleus

61
Q

What is the order of the energies of orbitals (lowest to highest)

A

s < p < d < f

62
Q

What is the Pauli Exclusion Principle?

A

Only 2 electrons with opposite spin can occupy an orbital

63
Q

What is Hund’s Rule?

A

Ensure each orbital has a single electron before doubly filling

64
Q

How is our modern periodic table arranged?

A

According to atomic number

65
Q

What are three characteristics of metals?

A
  1. Conduct heat and electricity
  2. Are malleable
  3. Are ductile
66
Q

Do metals lose or gain electrons? What ions do they form?

A

Metals tend to lose electrons to form positive ions (cations)

67
Q

Do nonmetals lose or gain electrons? What ions do they form?

A

Nonmetals tend to gain electrons forming negative ions (anions)

68
Q

State the periodic law

A

When the elements are arranged by atomic number, their chemical and physical properties recur periodically

69
Q

What is a period and how does it work?

A

A row in the periodic table; as you go across a period, electrons are being added to the same shell until it is full at the noble gases

70
Q

What is a group and how does it work?

A

A column in the periodic table; all elements within the same group have similar properties; electrons in the same group have the same valence electron configuration

71
Q

What are alkali metals?

A

Soft, shiny metals; good conductors of heat and electricity; malleable and ductile; form 1+ cations when reacting with nonmetals; very reactive

72
Q

What are alkaline earth metals?

A

Shiny metals; good conductors of heat and electricity; malleable and ductile; form 2+ cations; reactive, but less than alkali

73
Q

What are transition metals?

A

Groups 3-11; very hard metals with high melting points; can form a variety of compounds with other elements due to their complex electron arrangement; often used as catalysts

74
Q

What are metalloids?

A

The “staircase elements”; have properties of both metals and nonmetals; are shiny, but poor conductors of electricity

75
Q

What are nonmetals?

A

All gases that are not noble gases or halogens; not as reactive as halogens, more reactive than noble gases

76
Q

What are halogens?

A

Very reactive (dangerous) nonmetals; form 1- anions; poisonous; solids, liquids or gases, tend to form salts; not shiny and do not conduct electricity

77
Q

What are noble gases?

A

Extremely non reactive; have a full outer shell

78
Q

What is condensed electron configuration?

A

Place the atomic symbol for the last noble gas in square brackets, then add the valence electrons for the element

79
Q

What are isoelectronic elements/ions?

A

Elements/ions that have the same electron configuration

80
Q

What are inner electrons called?

A

Core electrons

81
Q

Give an example of how (n+1)s orbitals fill before the nd orbitals

A

4s orbitals fill before 3d orbitals since 4s electrons can get closer to the nucleus providing more stability to the atom

82
Q

What is true of groups 1-8 of the periodic table, when it comes to electron configurations?

A

Elements have the same number of valence electrons as their group number; they also have the same valence electron configurations

83
Q

What is the atomic radius and what units is it measured in?

A

The distance from the centre of an atom to the boundary within which the electrons spend most of their time; measured in picometers

84
Q

What trend is visible with atomic radius?

A

Atomic radius increases down a group and decreases across a period

85
Q

What is effective nuclear charge? Provide a formula

A

The nuclear charge experienced by the outermost electrons of an atom, as a result of the shielding by the inner shell electrons; ENC = # protons - # inner electrons

86
Q

What is the ionic radius?

A

The size of an ion as measured from the center of an ion to its outermost electrons

87
Q

What is ionization energy?

A

The amount of energy (kJ/mol) required to remove the outermost electron from an atom or ion in the gaseous state

88
Q

What trend is observed with ionization energy?

A

Ionization energy increases across a period, and decreases down a group

89
Q

What is electron affinity?

A

The energy change that occurs when an electron is added to a neutral atom

90
Q

What unit is electron affinity measured in?

A

kJ/mol

91
Q

What trend is found with electron affinity?

A

Electron affinity increases across a period and decreases down a group

92
Q

What is electronegativity?

A

The relative ability of an atom to attract shared electrons

93
Q

What trend is found with electronegativity?

A

Electronegativity increases across a period and decreases down a group

chem u2 atomic structure and properties (4 decks)

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