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Chemistry > Unit 3: Atomic THeory > Flashcards

Unit 3: Atomic THeory Flashcards

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1
Q

which greek philosopher believed in atoms and which philosophers believed that matter is continuous?

A

Democritus

Aristotle and Plato

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2
Q

What four elements did the ancient greeks think matter was composed of?

A

Earth, Air, Water, Fire

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3
Q

John Dalton

A

An english chemist who in 1803 offered ideas about atoms in five statements, combined into Dalton’s Atomic Theory

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4
Q

By when was it accepted that two elements could combine to form a compound, and that pure samples would always have the same composition by mass?

A

1803

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5
Q

What is the first statement of Dalton’s Atomic Theory?

A

Matter is composed of extremely small particles called atoms.

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6
Q

Second statement of Dalton’s Atomic Theory?

A

Atoms of a given element are the same (identical), but different elements have different atoms.

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7
Q

Third statement of Dalton’s Atomic Theory?

A

Atoms cannot be subdivided, created or destroyed.

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8
Q

Fourth statement of Dalton’s Atomic Theory?

A

Atoms can combine to form compounds in simple whole number ratios.

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9
Q

Fifth statement of Dalton’s Atomic Theory?

A

In chemical reactions, atoms are combined, separated, or arranged.

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10
Q

Law of Multiple Proportions

A

Single whole number ratios that compounds are composed of.

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11
Q

why the 1800s they’d demonstrated that matter also had an…

A

electrical nature

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12
Q

what did benjamin franklin say about electricity?

A

that electricity is related to tiny, negatively charged particles

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13
Q

what were electrons named after?

A

greek word ‘elektron’ meaning amber

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14
Q

atoms are electrically

A

neutral

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15
Q

when did JJ Thomson experiment with cathode ray tubes?

A

1897

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16
Q

what was the first discovery of a subatomic particle

A

jj thomson’s experiments with cathode rays, which he concluded were a stream of negatively charged particles

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17
Q

what did jj thomson (confirmed by rober millikan) demonstrate with his experiments about the electron?

A

that an electron’s volume was very small in relation to it’s mass

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18
Q

the cathode rays were determined to behave like…

A

particles

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19
Q

what are the two conclusions made from the thomson cathode experiments?

A

1) If atoms are electrically neutral there must be a positively charged particle within the atom
2) if atoms have a mass there must be other particles within the atom which contain most of the mass.

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20
Q

what was thomson’s model of the atom called?

A

plum pudding model

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21
Q

when did rutherford do his gold foil experiment?

A

1911

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22
Q

explain the gold foil experiment

A

positive alpha particles were used to bombard a thin piece of gold foil with positively charged alpha particles

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23
Q

what did rutherford expect, if mass and charge were uniformly distributed throughout an atom?

A

that the alpha particles would pass through with a slight deflection.

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24
Q

conclusions of the gold foil experiment

A
  • most of the atom is empty space
  • the atom contains a small dense positive center (the nucleus)
  • electrons surrounding the nucleus orbit in a planetary fashion, proposing a planetary model.
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25
Q

results of the gold foil experiment

A
  • most particles passed through Au foil, since atoms are made up mostly of empty space
  • very few particles were deflected back towards the source of the alpha particles.
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26
Q

who discovered the neutron?

A

james chadwick

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27
Q

when and how did chadwick discover the neutron?

A

in 1932, when he bombarded Be atoms with alpha particles and they emitted an energetic stream of radiation.

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28
Q

why did it take so long for the neutron to be discovered?

A
  • it is neutral, so no charge

- difficult time, the great depression

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29
Q

describe Neils Bohr’s model of the atom

A
  • it placed each electron in a specific energy level
  • electrons moved in definite orbits around the nucleus like planets
  • these orbits/energy levels are located at certain distances from the nucleus
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30
Q

when did Neils Bohr create his model?

A

1913

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31
Q

bohr: lowest energy level is closest

A

to the nucleus

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32
Q

bohr: electrons can move between

A

energy levels

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33
Q

bohr. electrons will never be found

A

between levels

34
Q

what is the modern model of the atom?

A

the wave-mechanical model

35
Q

when did schrodinger propose his theories?

A

1926

36
Q

background of the wave-mechanical model

A

in 1926 schrodinger proposed that
- electrons have a dual wave-particle nature - electrons do no travel in orbits around the nucleus based on QUANTUM MECHANICS

37
Q

electrons exist in a…

A

three-dimensional region around the nucleus, with an orbital being the “probable” location of an electron.

38
Q

wave-mechanical model AKA

A

an electron cloud

39
Q

what is the probable location of an electron based on?

A

how much energy the electron has

40
Q

the most dense area in the wave model…

A

is where the most probability of finding an electron lies

41
Q

timeline of atomic theory: 6 dates

A
  • greek model in 400 BC
  • dalton model in 1803
  • thomson model in 1897
  • rutherford model in 1911
  • bohr model in 1913
  • wave model (modern) in 1926
  • james chadwick neutron 1932
42
Q

list the masses of a proton, neutron, and electron

A

1 amu, 1 amu, and 1/1836 amu (0 in notation)

43
Q

describe symbol for subatomic particles

A

(before letter) superscript mass, subscript charge, letter (p, n, or e-)

44
Q

what does amu stand for and who defined it?

A

atomic mass unit, john dalton

45
Q

1 amu = ____ mass of carbon-12 atom

A

1/12 of the mass

46
Q

1 C-12 atom =

A

12 amu

47
Q

ions

A

charged particles created by the gaining or losing of electrons

48
Q

all metals ___ electrons, therefore…

A

lose, therefore they always become positive ions

49
Q

nucleons

A

protons and neutrons, found in the nucleus

50
Q

sum of the nucleons =

A

the mass of the nucleus

51
Q

Isotope

A

Atoms of the same element that have different mass numbers,

52
Q

What are the three isotopes of Hydrogen

A

Protium, deuterium, and tritium

53
Q

What is another name for heavy water?

A

Deuterium

54
Q

Nuclide

A

Term for any isotope

55
Q

Name the number of protons and neutrons for protium, deuterium, and tritium.

A

Protium: 1, 0
Deuterium: 1, 1
Tritium: 1, 2

56
Q

What isotope of hydrogen makes up 99.985% of the hydrogen on earth? 0.015%? Trace amounts?

A

Protium, deuterium, tritium

57
Q

Average atomic mass

A

The atomic mass is the average mass of all naturally occurring isotopes.

58
Q

How do you calculate the atomic mass/average atomic mass?

A

Take the percent abundance (as a decimal), multiply that by the mass number of the isotope, and divide this by 100.
Do this for all isotopes
Add up the products.

59
Q

Mass spectrometer

A

Used to detect isotopes by shooting an ion beam through a magnet that separates the lighter atoms from the heavier ones, which then are shot toward ion detectors.

60
Q

Neils Bohr model: electrons are attracted to a positive nucleus but…

A

remain in orbit which revolve around a center nucleus.

61
Q

Orbits(shells) are also called

A

Principal Energy Levels (PELs)

62
Q

According to Bohr’s model, what are the only regions in which electrons can be found ?

A

PELs

63
Q

What are the five points of Bohr’s atomic theory?

A
  1. Electrons are located in energy levels outside the nucleus.
  2. No change in energy when electron is in an energy level.
  3. Ground state is when the electron is it the lowest possible energy state that it is stable in.
  4. Change in energy occurs when the electron changes energy levels.
  5. E- absorb energy to move to a higher energy level as release energy to move to a lower one.
64
Q

Ionization energy

A

Lowest amount of energy needed to remove an electron from an atom.

65
Q

Name the max # of electrons for the first 4 PELs

A

2, 8, (for first 20 elements)8 (21 and up) 18, 32

66
Q

One orbital can hold up to _____ electrons and must be going in _____ directions

A

2 electrons, opposite

67
Q

what did bohr not know?

A

He didn’t know why only certain energies were allowed, and called these allowed energies Energy Levels.

68
Q

an electron will only absorb

A

as much energy as needed to move to a certain level

69
Q

what are the four quantum numbers

A

n, l, m sub l , m sub s

70
Q

what do each of the four quantum numbers stand for

A

in order: energy level, shape, orientation, and spin direction

71
Q

what range is accepted in ‘shape’ to represent different sublevels?

A

0(s), 1 (p), 2(d), 3(f)

72
Q

quantum mechanical model: (4 points)

A
  • in each energy level e- occupy sublevels/atomic orbitals
  • principal quantum number = number of energy sublevels
  • sublevels are s, p, d, f
  • they have different shapes, s = spherical, p = dumbbell, d and f are very complex.
73
Q

Principal QN is related to

A

the size and energy of the orbital

74
Q

Angular momentum QN

A

relates to the shape of the orbital (0,1,2,3) (l)

75
Q

Magnetic QN

A

relates to the orientation of the orbital in space relative to other orbitals

76
Q

Electron spin QN

A

relates to the spin states of the electrons. The spinning creates a magnetic field.

77
Q

what block is the s block on the periodic table?

A

the first two groups

78
Q

what block is the p group

A

last 6 groups

79
Q

what block is the d group

A

transition metals

80
Q

what is the f block?

A

lanthanides and actinides

Chemistry (17 decks)

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