Atomic Structure Flashcards
1
Q
This is the smallest part of an element.
A
Atoms
2
Q
This has all the properties of an element.
A
Atoms
3
Q
This is a million times smaller than a human hair.
A
Atoms
4
Q
What is the diameter of an atom?
A
0.1 - 0.5 nanometers (OR 1x10^-10 to 5x10^-10 m)
5
Q
Most atoms are empty space but has what?
A
Nucleus
6
Q
What contains the nucleus?
A
Protons and neutrons, while the electrons only surround it.
7
Q
Atoms are usually electrically neutral. (TRUE or FALSE)
A
True
8
Q
This particle is negatively charged.
A
Electrons
9
Q
Symbol for electron?
A
e-
10
Q
This particle of an atom moves around the outside of nucleus
A
Electrons
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.
12
Q
What is the mass of an electron particle?
A
9.110 x 10^-28 g
13
Q
What is the amu (atomic mass unit) of an electron particle?
A
0.000549
14
Q
Who discovered the electron particle?
A
Joseph John Thomson (1897)
15
Q
This particle is larger and heavier than electrons.
A
Protons
16
Q
This particle of an atom is positively-charged
A
Protons
17
Q
TRUE or FALSE: Protons are located inside the nucleus of an atom.
A
True
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.
19
Q
What is the mass of a proton particle?
A
1.6727 x 10^-24 g
20
Q
What is the amu (atomic mass unit) of a proton particle?
A
1.007316
21
Q
This particle of an atom is slightly heavier than proton.
A
Neutron
22
Q
Symbol for proton
A
p+
23
Q
Symbol for neutron
A
n
24
Q
This particle of an atom has no electric charge
A
Neutron
25
TRUE or FALSE: Neutrons are located inside the nucleus.
True
26
TRUE or FALSE: The num. of neutrons are always greater than the number of protons.
True. If the num. of protons become greater than the num. of neutrons, it might lead to an unstable (radioactive) atom.
27
The discovery of the proton particle is credited to whom?
Ernest Rutherford (1919)
28
What is the mass of a neutron particle?
1.6750 x 10^-24 g
29
What is the amu (atomic mass unit) of a neutron particle?
1.008701
30
Who discovered the neutron particle?
Sir James Chadwick (1932)
31
This is the center of an atom.
Nucleus
32
What is the term used to describe the combination of protons and neutrons?
Nucleons
33
TRUE or FALSE: Virtually, all mass of the atom is concentrated in the nucleus because the electrons' mass is so little.
True
34
The nucleus is discovered by whom?
Ernest Rutherford (1911)
35
This is the push or pull upon an object from their interaction with each other.
Force
36
This is a theory wherein all four forces maybe related and in a relationship
Grand unified theory
37
This type of force holds the nucleons together.
Strong nuclear force
38
This is the strongest force but acts only at a short range (size of nucleus).
Strong nuclear force
39
This type of force uses pions and gluons.
Strong nuclear force
40
This type of force is found between charged particles.
Electromagnetic force
41
This type of force is wherein all electrical and magnetic forces are combined.
Electromagnetic force
42
Force responsible or holding the electrons in orbit
Electromagnetic force
43
This force holds the atoms together.
Electromagnetic force
44
TRUE or FALSE: Electromagnetic force is 0.7% as strong as the strong nuclear force, but this has infinite range.
True
45
This type of force uses photons.
Electromagnetic force
46
This is the force responsible for the decay of radioactive atoms
Weak nuclear force
47
This is the force responsible for the emission of particles from the nucleus.
Weak nuclear force
48
This type of force causes the nuclear fusion in the sun and stars.
Weak nuclear force
49
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)
True
50
This type of force uses W and Z bosons.
Weak nuclear force
51
This force is found in the pull between 2 object directly related to their masses and inversely related to the distance between them.
Gravitational force
52
This is the most powerful force for massive and slow objects but has little effect at atomic level
Gravitational force
53
Weakest of all forces but has infinite range
Gravitational force
54
Gravitational force is thought to use a particle called what?
Gravitation, which is yet to be found
55
This is a tabular display of the chemical elements.
Periodic Table
56
Periodic table of elements are arranged by:
1. Atomic number
2. Electron configuration
3. Chemical properties
57
Who introduced the periodic table of elements?
Dmitri Mendeleev (1869)
58
What is the initial count of elements introduced by Dmitri Mendeleev?
65 elements
59
As of 2019, how many elements are known?
118 elements
60
What is the element 118
Organesson (synthesiszed in 2002)
61
In the periodic table, this is the number of protons in the nucleus of an atom
Atomic number (Z)
62
This is expressed in atomic mass units (AMU), and is equivalent to the number of protons and neutrons (num. of nucleons) in the atom
Atomic mass (A)
63
TRUE or FALSE: Atomic mass allows for the relative abundances of different isotopes.
True
64
These are metals in Group 1 except Hydrogen
Alkali Metals (g1)
65
These metals are extremely reactive and highly flammable / explosive in water
Alkali Metals (G1)
66
These metals are highly reactive but its reactions occur more slowly than alkali
Alkaline-Earth Metals (G2)
67
These metals are rarely found alone in nature ; has 2 valence electrons
Alkaline-Earth Metals (G2)
68
These are silvery-white metals
Lanthanides (G3)
69
These tarnish easily in contact with air
Lanthanides (G3)
70
These are all radioactive wherein only Thorium (H) and Uranium (U) occur naturally on Earth
Actinides (G3: bottom of table)
71
Lanthanides and Actinides are also called what?
Inner-transition metals
72
These are hard, shiny, but malleable metals
Transition Metals (G3-G12)
73
These metals are considered to be good conductors
Transition Metals (G3-G12)
74
These are almost the same with transition metals, but these are softer and conduct more poorly
Post-transition Metals (G13-G17)
75
These represent transition from metals to non-metals
Metalloids (G13-G17)
76
These are used as semi-conductors
Metalloids (G13-G17)
77
This is also called as semi-metals or poor metals
Metalloids (G13-G17)
78
These are mostly gases including Hydrogen
Non-metal Groups (G14-G16)
79
These are highly reactive, and combines with alkaline to form salts
Halogen (G17)
80
These are colorless, odorless, and non-reactive
Noble gases (G18)
81
How many periods are there in the periodic table?
7
82
How many groups are there in the periodic table?
18
83
These tell the energy level of the element's valence electron/s
Periods
84
This is the determination of the volume of space in which electrons orbiting the nucleus are most likely to be found
Electron Configuration
85
TRUE or FALSE: a closer electron to the nucleus means it is lower in energy
True
86
The maximum number of electrons per shell can be denoted as:
2n^2, n is the shell number
87
Shell number n is called the what?
Principal quantum number
88
Each electron shell is divided into what?
Sub-shells or sub-energy levels
89
What are the sub-shells?
s, p, d, f
90
These are complex-shaped high probability regions of space around the nucleus which is occupied by electron shells
Orbitals
91
This is a principle wherein 2 electrons must spin in opposite directions in a single orbital
Pauli exclusion principle
92
TRUE or FALSE: Orbitals can contain 2 or more electrons
False, orbitals can only contain up to 2 electrons (Pauli exclusion principle)
93
This depends on the number of electrons in the outermost shell
Valence of an atom
94
TRUE or FALSE: no outer shell can contain more than 8 electrons
True
95
TRUE or FALSE: the orbital of the lowest energy shell will be filled in first, followed by the next higher orbital, and so on
True
96
These are the electrons found in the outermost shell of an atom
Valence electron
97
They determine the combining capacity of an atom
Valence electron
98
TRUE or FALSE: if outer shell is filled (8), they are least reactive.
True
99
This is the strength of an attachment of an electron to the nucleus of an atom
Electron binding energy
100
TRUE or FALSE: Closer electron to the nucleus means tighter Eb (Electron binding energy)
True
101
Symbol of electron binding energy:
Eb
102
Unit of electron binding energy:
Volt (eV)
103
TRUE or FALSE: Electrons with many protons are more tightly bound to nucleus and requires more energy to ionize an atom
True
104
This is the ejection of an electron from an atom creating an ion pair
Ionization
105
What are the ion pairs:
1. Cation (+)
2. Anion (-)
106
This word is proposed by Truman P. Kohman in 1947
Nuclide
107
Who proposed the word nuclide?
Truman P. Kohman
108
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
Nuclide
109
These are nuclides that are unstable and thus decay by emission of particles or EM radiations or by spontaneous fission
Radionuclides
110
These are nuclides of the same element with same atomic numbers BUT different mass numbers
Isotopes
111
These are nuclides of different elements with same mass number BUT different atomic numbers
Isobars
112
These are nuclides that have the same number of neutron number BUT different number of proton
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
These are nuclides with the same element, same atomic number BUT has different energy states
Isomers
114
These are nuclides in a metastable state
Isomers
115
This is usually restricted to refer to isomers with half-lives of 10^-9 seconds or longer
Metastable state
