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IT-RAD101 [PRELIMS] > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

This is the smallest part of an element.

A

Atoms

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2
Q

This has all the properties of an element.

A

Atoms

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3
Q

This is a million times smaller than a human hair.

A

Atoms

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4
Q

What is the diameter of an atom?

A

0.1 - 0.5 nanometers (OR 1x10^-10 to 5x10^-10 m)

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5
Q

Most atoms are empty space but has what?

A

Nucleus

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6
Q

What contains the nucleus?

A

Protons and neutrons, while the electrons only surround it.

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7
Q

Atoms are usually electrically neutral. (TRUE or FALSE)

A

True

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8
Q

This particle is negatively charged.

A

Electrons

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9
Q

Symbol for electron?

A

e-

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10
Q

This particle of an atom moves around the outside of nucleus

A

Electrons

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11
Q

TRUE or FALSE: The number of neutrons and protons are usually equal, which is why an atom as a whole is electrically neutral.

A

False, because it should be that the electrons and protons are equal, not neutrons and protons.

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12
Q

What is the mass of an electron particle?

A

9.110 x 10^-28 g

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13
Q

What is the amu (atomic mass unit) of an electron particle?

A

0.000549

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14
Q

Who discovered the electron particle?

A

Joseph John Thomson (1897)

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15
Q

This particle is larger and heavier than electrons.

A

Protons

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16
Q

This particle of an atom is positively-charged

A

Protons

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17
Q

TRUE or FALSE: Protons are located inside the nucleus of an atom.

A

True

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18
Q

This particle of an atom determines the element in the periodic table

A

Protons. In the periodic table, atomic number is the number of protons in an element, which helps in identifying the element itself as all elements have different atomic numbers.

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19
Q

What is the mass of a proton particle?

A

1.6727 x 10^-24 g

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20
Q

What is the amu (atomic mass unit) of a proton particle?

A

1.007316

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21
Q

This particle of an atom is slightly heavier than proton.

A

Neutron

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22
Q

Symbol for proton

A

p+

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23
Q

Symbol for neutron

A

n

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24
Q

This particle of an atom has no electric charge

A

Neutron

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25
Q

TRUE or FALSE: Neutrons are located inside the nucleus.

A

True

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26
Q

TRUE or FALSE: The num. of neutrons are always greater than the number of protons.

A

True. If the num. of protons become greater than the num. of neutrons, it might lead to an unstable (radioactive) atom.

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27
Q

The discovery of the proton particle is credited to whom?

A

Ernest Rutherford (1919)

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28
Q

What is the mass of a neutron particle?

A

1.6750 x 10^-24 g

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29
Q

What is the amu (atomic mass unit) of a neutron particle?

A

1.008701

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30
Q

Who discovered the neutron particle?

A

Sir James Chadwick (1932)

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31
Q

This is the center of an atom.

A

Nucleus

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32
Q

What is the term used to describe the combination of protons and neutrons?

A

Nucleons

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33
Q

TRUE or FALSE: Virtually, all mass of the atom is concentrated in the nucleus because the electrons’ mass is so little.

A

True

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34
Q

The nucleus is discovered by whom?

A

Ernest Rutherford (1911)

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35
Q

This is the push or pull upon an object from their interaction with each other.

A

Force

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36
Q

This is a theory wherein all four forces maybe related and in a relationship

A

Grand unified theory

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37
Q

This type of force holds the nucleons together.

A

Strong nuclear force

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38
Q

This is the strongest force but acts only at a short range (size of nucleus).

A

Strong nuclear force

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39
Q

This type of force uses pions and gluons.

A

Strong nuclear force

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40
Q

This type of force is found between charged particles.

A

Electromagnetic force

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41
Q

This type of force is wherein all electrical and magnetic forces are combined.

A

Electromagnetic force

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42
Q

Force responsible or holding the electrons in orbit

A

Electromagnetic force

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43
Q

This force holds the atoms together.

A

Electromagnetic force

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44
Q

TRUE or FALSE: Electromagnetic force is 0.7% as strong as the strong nuclear force, but this has infinite range.

A

True

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45
Q

This type of force uses photons.

A

Electromagnetic force

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46
Q

This is the force responsible for the decay of radioactive atoms

A

Weak nuclear force

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47
Q

This is the force responsible for the emission of particles from the nucleus.

A

Weak nuclear force

48
Q

This type of force causes the nuclear fusion in the sun and stars.

A

Weak nuclear force

49
Q

TRUE or FALSE: The weak nuclear force is one-millionth as strong as the strong nuclear force and has even shorter range (proton’s diameter)

50
Q

This type of force uses W and Z bosons.

A

Weak nuclear force

51
Q

This force is found in the pull between 2 object directly related to their masses and inversely related to the distance between them.

A

Gravitational force

52
Q

This is the most powerful force for massive and slow objects but has little effect at atomic level

A

Gravitational force

53
Q

Weakest of all forces but has infinite range

A

Gravitational force

54
Q

Gravitational force is thought to use a particle called what?

A

Gravitation, which is yet to be found

55
Q

This is a tabular display of the chemical elements.

A

Periodic Table

56
Q

Periodic table of elements are arranged by:

A
  1. Atomic number
  2. Electron configuration
  3. Chemical properties
57
Q

Who introduced the periodic table of elements?

A

Dmitri Mendeleev (1869)

58
Q

What is the initial count of elements introduced by Dmitri Mendeleev?

A

65 elements

59
Q

As of 2019, how many elements are known?

A

118 elements

60
Q

What is the element 118

A

Organesson (synthesiszed in 2002)

61
Q

In the periodic table, this is the number of protons in the nucleus of an atom

A

Atomic number (Z)

62
Q

This is expressed in atomic mass units (AMU), and is equivalent to the number of protons and neutrons (num. of nucleons) in the atom

A

Atomic mass (A)

63
Q

TRUE or FALSE: Atomic mass allows for the relative abundances of different isotopes.

64
Q

These are metals in Group 1 except Hydrogen

A

Alkali Metals (g1)

65
Q

These metals are extremely reactive and highly flammable / explosive in water

A

Alkali Metals (G1)

66
Q

These metals are highly reactive but its reactions occur more slowly than alkali

A

Alkaline-Earth Metals (G2)

67
Q

These metals are rarely found alone in nature ; has 2 valence electrons

A

Alkaline-Earth Metals (G2)

68
Q

These are silvery-white metals

A

Lanthanides (G3)

69
Q

These tarnish easily in contact with air

A

Lanthanides (G3)

70
Q

These are all radioactive wherein only Thorium (H) and Uranium (U) occur naturally on Earth

A

Actinides (G3: bottom of table)

71
Q

Lanthanides and Actinides are also called what?

A

Inner-transition metals

72
Q

These are hard, shiny, but malleable metals

A

Transition Metals (G3-G12)

73
Q

These metals are considered to be good conductors

A

Transition Metals (G3-G12)

74
Q

These are almost the same with transition metals, but these are softer and conduct more poorly

A

Post-transition Metals (G13-G17)

75
Q

These represent transition from metals to non-metals

A

Metalloids (G13-G17)

76
Q

These are used as semi-conductors

A

Metalloids (G13-G17)

77
Q

This is also called as semi-metals or poor metals

A

Metalloids (G13-G17)

78
Q

These are mostly gases including Hydrogen

A

Non-metal Groups (G14-G16)

79
Q

These are highly reactive, and combines with alkaline to form salts

A

Halogen (G17)

80
Q

These are colorless, odorless, and non-reactive

A

Noble gases (G18)

81
Q

How many periods are there in the periodic table?

82
Q

How many groups are there in the periodic table?

83
Q

These tell the energy level of the element’s valence electron/s

84
Q

This is the determination of the volume of space in which electrons orbiting the nucleus are most likely to be found

A

Electron Configuration

85
Q

TRUE or FALSE: a closer electron to the nucleus means it is lower in energy

86
Q

The maximum number of electrons per shell can be denoted as:

A

2n^2, n is the shell number

87
Q

Shell number n is called the what?

A

Principal quantum number

88
Q

Each electron shell is divided into what?

A

Sub-shells or sub-energy levels

89
Q

What are the sub-shells?

A

s, p, d, f

90
Q

These are complex-shaped high probability regions of space around the nucleus which is occupied by electron shells

91
Q

This is a principle wherein 2 electrons must spin in opposite directions in a single orbital

A

Pauli exclusion principle

92
Q

TRUE or FALSE: Orbitals can contain 2 or more electrons

A

False, orbitals can only contain up to 2 electrons (Pauli exclusion principle)

93
Q

This depends on the number of electrons in the outermost shell

A

Valence of an atom

94
Q

TRUE or FALSE: no outer shell can contain more than 8 electrons

95
Q

TRUE or FALSE: the orbital of the lowest energy shell will be filled in first, followed by the next higher orbital, and so on

96
Q

These are the electrons found in the outermost shell of an atom

A

Valence electron

97
Q

They determine the combining capacity of an atom

A

Valence electron

98
Q

TRUE or FALSE: if outer shell is filled (8), they are least reactive.

99
Q

This is the strength of an attachment of an electron to the nucleus of an atom

A

Electron binding energy

100
Q

TRUE or FALSE: Closer electron to the nucleus means tighter Eb (Electron binding energy)

101
Q

Symbol of electron binding energy:

102
Q

Unit of electron binding energy:

103
Q

TRUE or FALSE: Electrons with many protons are more tightly bound to nucleus and requires more energy to ionize an atom

104
Q

This is the ejection of an electron from an atom creating an ion pair

A

Ionization

105
Q

What are the ion pairs:

A
  1. Cation (+)
  2. Anion (-)
106
Q

This word is proposed by Truman P. Kohman in 1947

107
Q

Who proposed the word nuclide?

A

Truman P. Kohman

108
Q

These are from nucleus, an atomic species wherein it has a definite num. of protons and neutrons arrange in a definite order in the nucleus

109
Q

These are nuclides that are unstable and thus decay by emission of particles or EM radiations or by spontaneous fission

A

Radionuclides

110
Q

These are nuclides of the same element with same atomic numbers BUT different mass numbers

111
Q

These are nuclides of different elements with same mass number BUT different atomic numbers

112
Q

These are nuclides that have the same number of neutron number BUT different number of proton

A

Isotones (TIP: just subtract mass number and atomic number per element and see if the answer would be the same for all elements. Thus, their neutron numbers are the same, indicating that they are isotones.)

113
Q

These are nuclides with the same element, same atomic number BUT has different energy states

114
Q

These are nuclides in a metastable state

115
Q

This is usually restricted to refer to isomers with half-lives of 10^-9 seconds or longer

A

Metastable state

IT-RAD101 [PRELIMS] (5 decks)

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