Atoms and Elements Flashcards
(144 cards)
1
Q
What does the quantum mechanical model describe?
A
The behavior of electrons in atoms.
2
Q
True or False: In the quantum mechanical model, electrons are treated as particles with definite positions.
A
False
3
Q
What principle states that certain pairs of physical properties cannot be simultaneously known to arbitrary precision?
A
Heisenberg Uncertainty Principle
4
Q
Fill in the blank: The quantum mechanical model utilizes ______ to describe the probability of finding an electron in a specific location.
A
wave functions
5
Q
What is the primary equation used in the quantum mechanical model?
A
Schrödinger Equation
6
Q
Which scientist is most closely associated with the development of the quantum mechanical model?
A
Erwin Schrödinger
7
Q
True or False: The quantum mechanical model has replaced the Bohr model of the atom.
A
True
8
Q
What do we call the regions in an atom where there is a high probability of finding an electron?
A
orbitals
9
Q
Multiple Choice: Which of the following is NOT a type of orbital? A) s B) p C) d D) q
A
D) q
10
Q
What does the ‘n’ quantum number represent?
A
The principal energy level of an electron.
11
Q
Fill in the blank: The ______ quantum number describes the shape of an orbital.
A
angular momentum
12
Q
What is the maximum number of electrons that can occupy an s orbital?
A
2
13
Q
True or False: Electrons in the same orbital can have the same spin quantum number.
A
False
14
Q
What is the significance of the Pauli Exclusion Principle in the quantum mechanical model?
A
No two electrons can have identical sets of quantum numbers.
15
Q
Multiple Choice: Which quantum number describes the orientation of an orbital? A) principal B) angular momentum C) magnetic D) spin
A
C) magnetic
16
Q
What does the spin quantum number indicate?
A
The intrinsic angular momentum of an electron.
17
Q
Fill in the blank: The ______ principle explains the arrangement of electrons in an atom.
A
Aufbau
18
Q
What is the energy level of an electron in a hydrogen atom described by the quantum mechanical model?
A
Quantized
19
Q
True or False: The quantum mechanical model allows for the prediction of chemical behavior of atoms.
A
True
20
Q
What type of wave function is used to describe the probability distribution of an electron?
A
ψ (psi)
21
Q
Multiple Choice: Which of the following quantum numbers is not needed to describe an electron? A) principal B) angular momentum C) magnetic D) temperature
A
D) temperature
22
Q
What does the term ‘degenerate orbitals’ refer to?
A
Orbitals that have the same energy level.
23
Q
Fill in the blank: The quantum mechanical model incorporates the concept of ______, which is a fundamental aspect of particles at the quantum level.
A
wave-particle duality
24
Q
True or False: The quantum mechanical model can predict the exact path of an electron.
A
False
25
What is the role of the wave function in quantum mechanics?
It provides information about the probability of finding an electron in a region of space.
26
Multiple Choice: Which of the following is a characteristic of the quantum mechanical model? A) Electrons have fixed orbits B) Electrons are treated as waves C) Electrons have definite positions D) Electrons do not exist
B) Electrons are treated as waves
27
What is the significance of the quantum number 'l'?
It determines the shape of the orbital.
28
Fill in the blank: The quantum mechanical model predicts that electrons will fill orbitals in order of increasing ______.
energy
29
True or False: Quantum mechanics has applications beyond just atomic physics.
True
30
What does the term 'quantum state' refer to?
The set of quantum numbers that describe an electron's properties.
31
What is electron configuration?
The distribution of electrons of an atom or molecule in atomic or molecular orbitals.
32
True or False: The electron configuration of an atom determines its chemical properties.
True
33
Fill in the blank: The maximum number of electrons that can occupy a single orbital is ____.
2
34
What principle states that electrons fill orbitals starting from the lowest energy level?
Aufbau principle
35
Which rule states that no two electrons in an atom can have the same set of quantum numbers?
Pauli exclusion principle
36
What is the maximum number of electrons in the n=2 energy level?
8
37
What notation is used to represent the electron configuration of an element?
Spectroscopic notation
38
What is the electron configuration of oxygen?
1s² 2s² 2p⁴
39
Which element has the electron configuration of 1s² 2s² 2p⁶ 3s² 3p⁵?
Chlorine
40
True or False: Electrons occupy degenerate orbitals singly before pairing up.
True
41
What is the term for the arrangement of electrons in an atom?
Electron configuration
42
Fill in the blank: The electron configuration for helium is ____.
1s²
43
What is the electron configuration for sodium?
1s² 2s² 2p⁶ 3s¹
44
Which block of the periodic table contains elements with the outermost electrons in s orbitals?
s-block
45
What is the electron configuration for carbon?
1s² 2s² 2p²
46
What does the notation '3d' represent in electron configuration?
A d orbital in the third energy level.
47
True or False: The d and f orbitals are filled after the s and p orbitals of the same principal energy level.
False
48
What is the electron configuration of neon?
1s² 2s² 2p⁶
49
Fill in the blank: The noble gas configuration for xenon is ____.
[Kr] 5s² 4d¹⁰ 5p⁶
50
What is the electron configuration for iron?
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶
51
Which principle explains the order in which orbitals are filled?
Aufbau principle
52
What element has the electron configuration of [Ne] 3s²?
Magnesium
53
Fill in the blank: The electron configuration for lithium is ____.
1s² 2s¹
54
What is the electron configuration for potassium?
1s² 2s² 2p⁶ 3s¹
55
True or False: The 4f orbitals are filled before the 5s orbital.
True
56
What does the term 'valence electrons' refer to?
Electrons in the outermost shell of an atom.
57
What is the electron configuration for silver?
[Kr] 5s¹ 4d¹⁰
58
Which element has the electron configuration [Ar] 4s² 3d¹⁰ 4p⁵?
Bromine
59
Fill in the blank: The electron configuration of an atom is determined by the ____ of the atom.
number of electrons
60
What is the electron configuration for sulfur?
1s² 2s² 2p⁶ 3s² 3p⁴
61
True or False: The electron configuration for an atom can change if it gains or loses electrons.
True
62
What is the electron configuration for argon?
1s² 2s² 2p⁶ 3s² 3p⁶
63
What is the significance of the quantum numbers in electron configuration?
They describe the properties of atomic orbitals and the electrons in them.
64
Fill in the blank: The first energy level can hold a maximum of ____ electrons.
2
65
What is the electron configuration for calcium?
1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
66
What is the electron configuration for the element with atomic number 11?
1s² 2s² 2p⁶ 3s¹ (Sodium)
67
Which electron configuration represents a noble gas?
1s² 2s² 2p⁶ (Neon)
68
True or False: Elements in the same group of the periodic table have similar electron configurations.
True
69
What is the electron configuration of the transition metal titanium?
[Ar] 4s² 3d²
70
Fill in the blank: The electron configuration for the element with atomic number 6 is ____.
1s² 2s² 2p² (Carbon)
71
What is the electron configuration for the halogen fluorine?
1s² 2s² 2p⁵
72
What element has the electron configuration [Kr] 5s² 4d⁹?
Silver
73
What are the three main types of elements in the periodic table?
Metals, nonmetals, and metalloids.
74
True or False: All metals are good conductors of electricity.
True.
75
Fill in the blank: Elements in Group 1 of the periodic table are known as __________ metals.
alkali
76
Which group contains the noble gases?
Group 18.
77
What is the primary characteristic of nonmetals?
They are poor conductors of heat and electricity.
78
Multiple choice: Which of the following is a characteristic of metalloids? A) Brittle B) Malleable C) Ductile D) All of the above
A) Brittle.
79
What type of bond do metals typically form?
Metallic bonds.
80
True or False: Halogens are found in Group 17.
True.
81
What is the common oxidation state of alkali metals?
+1.
82
Fill in the blank: The elements in group 2 are known as __________ metals.
alkaline earth
83
Which type of element is most likely to gain electrons?
Nonmetals.
84
Multiple choice: Which of the following is NOT a metalloid? A) Silicon B) Arsenic C) Sodium D) Boron
C) Sodium.
85
What property distinguishes noble gases from other elements?
They are inert and do not readily form compounds.
86
True or False: Transition metals are located in Groups 3 to 12.
True.
87
What is the general trend in reactivity for alkali metals as you move down the group?
Reactivity increases.
88
Fill in the blank: The ability of an element to lose electrons is known as __________.
metallic character.
89
What group contains the highly reactive alkali metals?
Group 1.
90
Multiple choice: Which of the following is a property of nonmetals? A) High melting points B) Dull appearance C) Good conductors D) Malleable
B) Dull appearance.
91
What is the typical oxidation state of alkaline earth metals?
+2.
92
True or False: All elements in Group 14 are nonmetals.
False.
93
What do you call the elements in Group 16?
Chalcogens.
94
Fill in the blank: The elements in Group 15 include __________.
nitrogen and phosphorus.
95
Multiple choice: Which group contains the least reactive elements? A) Alkali metals B) Alkaline earth metals C) Noble gases D) Halogens
C) Noble gases.
96
What is the primary characteristic of alkaline earth metals?
They are reactive but less so than alkali metals.
97
True or False: Metals tend to form anions.
False.
98
Which element is the most electronegative?
Fluorine.
99
Fill in the blank: The elements in Group 3 to 12 are known as __________ metals.
transition
100
What does the term 'periodicity' refer to in the context of the periodic table?
The repeating pattern of chemical and physical properties.
101
Multiple choice: Which of the following elements is a metalloid? A) Aluminum B) Germanium C) Chlorine D) Calcium
B) Germanium.
102
What is the common characteristic of halogens?
They are highly reactive nonmetals.
103
What is the periodic law?
The periodic law states that the properties of elements are a periodic function of their atomic numbers.
104
True or False: Atomic radius generally increases down a group.
True
105
Fill in the blank: Elements in the same group have similar __________.
chemical properties
106
Which element has the highest electronegativity?
Fluorine
107
What trend does ionization energy follow across a period?
Ionization energy generally increases across a period.
108
What is the atomic radius trend as you move from left to right across a period?
The atomic radius decreases.
109
True or False: Metals tend to have higher electronegativities than nonmetals.
False
110
Which group of elements is known as the noble gases?
Group 18
111
What is the primary reason for the increase in ionization energy as you move across a period?
Increased nuclear charge.
112
Short answer: What is electronegativity?
Electronegativity is the tendency of an atom to attract electrons in a bond.
113
Which group contains the alkali metals?
Group 1
114
True or False: Nonmetals generally have higher ionization energies than metals.
True
115
What happens to the electronegativity of elements as you move down a group?
Electronegativity decreases.
116
Fill in the blank: The __________ effect explains the decrease in ionization energy down a group.
shielding
117
What is the trend in metallic character as you move down a group?
Metallic character increases.
118
Which element has the smallest atomic radius in the second period?
Neon
119
True or False: The transition metals are found in groups 3-12.
True
120
What is the trend in reactivity for alkali metals as you move down the group?
Reactivity increases.
121
Short answer: What is the significance of the octet rule?
The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons.
122
Which element is the most reactive nonmetal?
Fluorine
123
What is the trend in electron affinity as you move across a period?
Electron affinity generally increases.
124
True or False: The lanthanides and actinides are considered inner transition metals.
True
125
Fill in the blank: The elements in group 17 are known as __________.
halogens
126
What is the trend in boiling points for noble gases as you move down the group?
Boiling points increase.
127
Which ion has a larger radius: Na+ or Ne?
Na+
128
True or False: Anions are larger than their parent atoms.
True
129
What is the primary factor influencing the periodic trends in atomic size?
The effective nuclear charge.
130
Short answer: What is a metalloids?
Metalloids are elements that have properties of both metals and nonmetals.
131
What is the trend in density for alkali metals as you move down the group?
Density generally increases.
132
Which element is known for having the highest ionization energy?
Helium
133
Fill in the blank: The __________ principle states that no two electrons can have the same set of quantum numbers.
Pauli exclusion
134
What is ionization energy?
The energy required to remove an electron from an atom or ion in the gas phase.
135
True or False: Ionization energy generally increases across a period from left to right.
True
136
Fill in the blank: The effective nuclear charge experienced by an electron is usually ______ than the actual nuclear charge due to electron shielding.
less
137
What trend is observed in ionization energy as you move down a group in the periodic table?
Ionization energy generally decreases.
138
Which element has the highest first ionization energy: Lithium (Li), Sodium (Na), or Neon (Ne)?
Neon (Ne)
139
What is electron affinity?
The energy change that occurs when an electron is added to a neutral atom in the gas phase.
140
True or False: Electron affinity typically becomes more negative across a period.
True
141
Short Answer: How does effective nuclear charge affect ionization energy?
Higher effective nuclear charge increases ionization energy because electrons are held more tightly by the nucleus.
142
Multiple Choice: Which factor does NOT affect ionization energy? A) Atomic radius B) Electron configuration C) Atomic mass D) Effective nuclear charge
C) Atomic mass
143
What is the relationship between electron affinity and reactivity in nonmetals?
Nonmetals with high electron affinity are generally more reactive.
144
what is the difference b/w ionization energy and electron affinity?
ionization energy requires energy to be removed from 1 electron of an atom, while electron affinity requires energy to be added to 1 electron of an atom
