Long Test 2 Flashcards
(129 cards)
1
Q
? is the arrangement of electrons in the orbitals of an atom
A
electron configuration
2
Q
a phenomenon wherein electrons that are closer to the nucleus slightly repel electrons that are farther out (offsetting the more dominant electron-nucleus attractions slightly)
A
shielding
3
Q
TRUE OR FALSE: electrons in orbitals that experience more shielding are more stabilized and thus higher in energy
A
false - it is less stabilized
4
Q
principle about building up the structures in the order of atomic numbers and their energies (lowest to highest)
A
aufbau principle
5
Q
What does Aufbau mean?
A
to build up
6
Q
pictorial representations of the electron configuration, showing the individual orbitals and the pairing arrangement of electrons
A
orbital diagrams
7
Q
what principle states that the lowest-energy configuration for an atom with electrons within a set of degenerate orbitals is having the maximum number of unpaired electrons
A
Hund’s rule
8
Q
TRUE OR FALSE: core electrons are the electrons located at the center of the atom
A
false - core electrons just occupy the inner shell orbitals
9
Q
electrons occupying the outermost shell orbitals (highest value of n)
A
valence electrons
10
Q
highest energy level orbitals of an atom
A
valence shell
11
Q
TRUE OR FALSE: main group elements consist of the s and p orbitals in the outermost shell
A
true
12
Q
how or when are ions formed?
A
they are formed when atoms gain or lose electrons
13
Q
what is a cation?
A
a positively charged ion that loses one or more electrons
14
Q
what is an anion
A
a negatively charged ion that gains one or more electrons
15
Q
how many periods are there in the periodic table?
A
6 periods
16
Q
how many groups are in the periodic table?
A
18 groups
17
Q
TRUE OR FALSE: cations have a shorter radius than their counterpart neutral atom
A
true
18
Q
TRUE OR FALSE: a longer radius means that it’s closer to the nucleus
A
false - it’s farther away
19
Q
as you go down from the periodic table, the number of electrons in the valence shell remains constant but the ? increases by one each time
A
principle quantum number
20
Q
one-half the distance between the nuclei of two identical atoms when they are joined by a covalent bond
A
covalent radius
21
Q
TRUE OR FALSE: increasing n = decreasing radius
A
false = radius increases
22
Q
the size of an ? also increases when the distance of the outermost electrons from the nucleus increases
A
atom
23
Q
left to right
a. smaller covalent radius
b. bigger covalent radius
c. same size
A
a.
24
Q
what is the effective nuclear charge? (Zeff)
A
the pull exerted on a specific electron by the nucleus, taking into account any electron-electron repulsions
25
what element has an equal nuclear charge (Z) and effective nuclear charge (Zeff)
hydrogen
26
TRUE OR FALSE: Zeff = Z - shielding
true
27
TRUE OR FALSE: effective nuclear charge is determined by the probability of another electron being between the electron of interest and the nucleus, as well as by the electron-electron repulsions the electron of interest encounters
false - shielding
28
? are adept at shielding
a. core electrons
b. valence electrons
a.
29
TRUE OR FALSE: electrons in different valence shells do not block the nuclear attraction experienced by each other as efficiently
false - electrons in the SAME valence shell
30
TRUE OR FALSE: Zeff increases as we move across a period
true
31
TRUE OR FALSE: the higher effective nuclear charge (stronger pull) experienced by electrons on the right side of the periodic table draws them closer to the nucleus, making the covalent radii smaller
true
32
the amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state
ionization energy
33
which is stronger? first ionization energy or second ionization energy?
second ionization energy
34
is ionization energy exothermic or endothermic?
endothermic
35
TRUE OR FALSE: ionization energy values are always negative
false - always positive
36
processes that involve the emission of light and that increase the energy of an atom
endothermic processes
37
processes that involve the emission of light but decrease the energy of an atom
exothermic processes
38
? is always required to remove electrons from atoms or ions
energy
39
as size (atomic radius) increases, the ionization energy ?
decreases
40
(within a period) increasing Z = ? ionization energy
increasing
41
(down a group) increasing Z = ? ionization energy
decreasing
42
TRUE OR FALSE: the energy of the sub-shells increases as the angular momentum/secondary quantum number (l) increases
true
43
removing an electron from a cation is more difficult than removing an electron from a neutral atom because of the ?
electrostatic attraction to the cation
44
the attraction between the positively charged nucleus of an atom and the negatively charged electrons surrounding it
electrostatic attraction
45
energy charge for the process of adding an electron to a gaseous atom to form an anion
electron affinity
46
TRUE OR FALSE: the electron affinity process is endothermic
false - it can be endothermic or exothermic
47
(electron affinity) what is released when the gaseous atom accepts an electron?
energy
48
TRUE OR FALSE: (electron affinity) some elements require energy for the atom to be negatively charges and the value of their EA becomes positive
true
49
it becomes easier to add an electron across a series of atoms as the ? increases
effective nuclear charge of the atom
50
left to right across a period = EAs become more?
negative
51
element that has the highest ionization energy
helium
52
element that has highest value of electron affinity
chlorine
53
what does the periodic law state?
the properties of the elements are periodic functions of their atomic numbers
54
the periodic table is arranged by ?
the increasing order of their atomic numbers and groups atoms with similar properties in the same column
55
elements are arranged in how many periods or series?
seven
56
what are the main-group elements (or representative elements)?
groups 1,2, and 13-18
57
what are the transition metals?
groups 3-12
58
what do the inner transition metals consist of?
lanthanides (top row) and actinides (bottom row)
59
what are the group 1 elements called?
alkali metals
60
what are the group 2 elements called?
alkaline earth metals
61
what is group 15 called?
pnictogens
62
what is group 16 called?
chalcogens
63
what is group 17 called
hallogens
64
what is group 18 called?
noble gases or inert gases
65
what are monoatomic ions
ions formed from only one atom
66
ions that act as discrete units and are electrically charged molecules
polyatomic ions
67
polyatomic ions that contain one or more oxygen atoms
oxyanions
68
TRUE OR FALSE: Per- is a prefix meaning more oxygen atoms than -ite
false - more oxygen atoms than -ate
69
TRUE OR FALSE: Hypo- is a prefix meaning lesser oxygen atoms than -ite
true
70
what kind of bonds form when there is an equal sharing of electrons?
covalent bonds
71
what stabilizes ionic compounds?
electrostatic attractions between the ions of opposite charge present in the compound
72
a compounds that contains ions and is held together by ionic bonds
ionic compound
73
TRUE OR FALSE: ionic compounds are solids that melt at high temperatures and boil at even higher temperatures
TRUE
74
are ionic compounds good conductors of heat or not?
no, they are not (its ions are unable to flow except when molten)
75
TRUE OR FALSE: ionic compounds are negative in nature
false - they are electrically neutral
76
TRUE OR FALSE: molecular compounds usually exist as gases, low-boiling liquids, and low-melting solids
true
77
covalent compounds are a combination of?
nonmetals
78
TRUE OR FALSE: we use prefixes in naming ionic compounds
false - we only do so with covalent compounds
79
what does isoelectronic mean?
it refers to two atoms, ions, or molecules that have the same electronic structure and the same number of valence electrons
80
TRUE OR FALSE: covalent compounds are insoluble in water and are therefore poor conductors of heat in any state
true
81
H2 and Cl2 are considered what kind of covalent bonds?
pure covalent bonds
82
what is a polar covalent bond?
a covalent bond with unequal share or distribution of electrons
83
explain electron negativity
it is when an atom attracts the electrons toward themselves due to having higher electron density
84
what is the driving force behind covalent bonds?
the drive to completely fill the orbitals
85
The electrons in the H-Cl bond of a hydrogen chloride molecule spend more time near the chlorine atom than near the hydrogen atom. Which atom gets the partial negative charge and which one gets the positive partial charge?
chlorine gets the partial negative charge and hydrogen gets the partial positive charge
86
TRUE OR FALSE: electronegativity increases across a period
true
87
TRUE OR FALSE: electronegativity increases down a group
false - it decreases down a group
88
a collection of rules for naming things
nomenclature
88
compounds consisting of only two elements
binary compounds
88
ionic compounds that contain water molecules as integral components of their crystals
hydrates
89
what does the word anhydrous mean?
not hydrated
90
consists of an elemental symbol surrounded by one dot for each of its valence electrons
lewis structure
91
the tendency of main group atoms to form enough bonds to obtain eight valence electrons
octet rule
92
what do we call molecules that contain an odd number of electrons?
free radicals
93
how do we calculate for the formal charge?
#valence shell electrons of free atom - #lone pair electrons - 1/2#bonding electrons
94
TRUE OR FALSE: the concept of resonance states that if two or more lewis structures with the same arrangement of atoms can be written for a molecule or ion, the actual distribution of electrons is an average of that shown by the various lewis structures
true
95
what do we call the individual lewis structures (concept of resonance)
resonance forms
96
what do we call the actual electronic structure of the molecule or the average of the resonance forms?
resonance hybrid
97
the angle between any two bonds that include a common atom, usually measured in degrees
bond angle
98
distance between the nuclei of two bonded atoms along the straight line joining the nuclei
bond distance
99
What does VSEPR Theory stand for?
Valence shell electron-pair repulsion theory
100
this measures the extent of net charge separation in the molecule as a whole
dipole moment
101
compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound
binary acid
102
arrangement around a central atom of all regions of electron density (bonds, lone pairs, or unpaired electrons)
electron-pair geometry
103
molecule containing at least one main group element that has more than eight electrons in its valence shell
hypervalent molecule
104
compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the compound
oxyacid
105
quantity having magnitude and direction
vector
106
planck's constant (h) = ?
6.626 x 10^-34 J
107
TRUE OR FALSE: kinetic energy depended on the amplitude of the light
false - it depended on its frequency
108
Who won a Nobel prize for finding out that light striking the metal surface should not be viewed as a wave, but more as a stream of particles (photons) whose energy depended on their frequency?
Albert einstein
109
What is Planck's formula?
energy (E) = hv/hc over wavelength (v is the frequency and h is the constant)
110
higher frequency = ? wavelength
shorter
111
what is the rydberg's constant?
1.097 x 10^7m^-1
112
when the electron is in the lowest energy orbit it is in its ?
ground electronic state
113
what happens when the atom receives energy from an outside course?
the electron can move up to an orbit with a higher n value
114
what happens when the electron goes from an excited state to a less excited/ground state?
the difference in energy is released as a photon
115
what does the law of conservation of energy state?
we can neither create nor destroy energy
116
TRUE OR FALSE: electron's energy increases as n decreases
false - as n increases
117
electron's energy increases as the distance from the nucleus ?
increases
118
TRUE OR FALSE: De Broglie stated that the electron in a hydrogen atom could be better thought of as being a circular standing wave instead of a particle
true
119
Schrödinger described electrons as ?
three-dimensional stationary waves (wavefunctions)
120
quantum number that defines the location of the energy level
principle quantum number aka shell number
121
a general region in an atom within which an electron is most probable to reside
atomic orbital
122
quantum number that specifies the shape of the orbital
secondary quantum number (angular momentum)
123
region where the probability f finding an electron is zero (the value of the wavefunction ψ is zero)
radial node
124
quantum number that specifies the relative spatial orientation of a particular orbital
magnetic quantum number
125
degenerate orbitals have the same what?
n and energy
126
quantum number that describes an intrinsic electron "rotation" or "spinning"
spinning quantum number
127
what does the Pauli's exclusion principle state?
no two electrons in the same orbital can have the same exact set of four quantum numbers
