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DAT > Chemistry Atomic and Molecular Structure > Flashcards

Chemistry Atomic and Molecular Structure Flashcards

1
Q

The ___ is the basic building block of matter, representing the smallest unit of a chemical element

A

atom

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2
Q

The ___ and neutrons in an atom form the nucleus, the core of the atom

A

protons

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3
Q

The ___ exist outside the nucleus in characteristic regions of space called orbital

A

electrons

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4
Q

According to John Dalton, all ___ are composed of very small particles called atoms

A

elements

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5
Q

According to John Dalton, all ___ are composed of atoms of more than one element

A

compounds

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6
Q

According to John Dalton, for any given compound, the ___ of the numbers of atoms of any two of the elements present is either an integer or a simple fraction

A

ratio

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7
Q

According to John Dalton, a given chemical reaction involves only the ___, combination, or rearrangement of atoms; it does NOT result in the creation or destruction of atoms

A

separation

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8
Q

The ___ (Z) of an element is equal to the number of protons found in an atom of that element

A

atomic number

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9
Q

___ carry no charge and have a mass only slightly larger than that of protons, so they can still be considered to have a mass of approximately 1 u

A

neutrons

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10
Q

Different ___ of one element have different numbers of neutrons but the same number of protons

A

isotopes

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11
Q

The farther the ___ electrons are from the nucleus, the weaker the attractive force of the positively charged nucleus and the more likely the valence electrons are to be influenced by other atoms

A

valence

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12
Q

Therefore, the atomic number indicates the number of ___ in a neutral atom

A

electrons

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13
Q

A positive or negative ___ on an atom is due to a loss or gain of electrons; the result is called an ion

A

charge

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14
Q

Note that a (+) charge indicates a loss of negatively-charged electrons , whereas a (-) charges indicates a ___ of electrons

A

gain

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15
Q

The atomic ___ (A) of an atom is equal to the total number of nucleons (protons an neutrons)

A

mass number

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16
Q

mass number (A) = number of protons + ___

A

number of neutrons

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17
Q

On a larger scale, the ___ is the weight in grams per one mole (mol) of a given element (g/mol)

A

molecular weight

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18
Q

A ___ is a unit used to count particles and is represented by Avogadro’s number, 6.02 x 10^23 particles per mol

A

mole

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19
Q

___ are referred to either by the convention described above or, more commonly, by the name of the element followed by the mass number

A

isotopes

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20
Q

In 1900, Max Planck developed the first ___, proposing that energy emitted as electromagnetic radiation from matter comes in discrete bundles called quanta

A

quantum theory

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21
Q

The ___ of the electron is related to its orbital radius: the smaller the radius, the lower the energy state of the electron

A

energy

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22
Q

At the ___ level, the electron is in its lowest energy state

A

ground state

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23
Q

Because each element can have its electrons excited to different distinct energy levels, each element possesses a unique ___, which can be used as a fingerprint

A

atomic emission spectrum

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24
Q

When an electron is excited to a higher energy level, it must ___ energy

A

absorb

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25
Q

The ___ absorbed as an electron jumps from an orbital of low energy to one of higher energy is characteristic of that transition

A

energy

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26
Q

The excitation of electrons in a particular element results in energy absorptions at ___ wavelengths

A

specific

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27
Q

Thus, in addition to an ___, every element possesses a characteristic absorption spectrum

A

emission spectrum

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28
Q

Absorption spectra can thus be used in the identification of elements present in a gas ___ sample

A

phase

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29
Q

While the concepts put forth by Bohr offered a reasonable explanation for the structure of the hydrogen atom and ions containing only one ___ (such as He+ and Li2+), they did not explain the structures of atoms containing more than one electron

A

electron

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30
Q

Due to the flaws in the Bohr model, this is because Bohr’s ___ does not take into consideration the repulsion between multiple electrons surrounding one nucleus

A

model

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31
Q

An orbital is a ___ of the probability of finding an electron within a given region

A

orbital

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32
Q

In the current ___ description of electrons, pinpointing both the exact location and momentum of an electron at any given point in time impossible

A

quantum mechanical

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33
Q

The idea of an electron’s position not being quite known, this idea is best described by the ___ which states that it is impossible to simultaneously determine, with perfect accuracy, the momentum (defined as mass times velocity) and the position of an electron

A

heisenberg uncertainty principal

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34
Q

Concerning the Heisenberg uncertainty principal, this means that if the ___ of the electron is being measured accurately, its position will not be certain, and vice versa

A

momentum

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35
Q

___ states that any electron in an atom can be completely described by four ___: n, l,m sub l, and m sub s

A

modern atomic theory

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36
Q

Furthermore, according to the pauli exclusion principle, no two ___ in a given atom can possess the same set of four quantum numbers

A

electrons

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37
Q

The ___ and energy of an electron described by its quantum numbers is known as its energy state

A

position

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38
Q

The ___ of n limits the values of l, which in ___ limit the values of m sub l

A

value

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39
Q

The values of three of the ___ qualitatively give information about the orbitals: n about the size, l about the shape, and m sub l about the orientation of the orbital

A

quantum numbers

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40
Q

Think of the ___ as becoming more specific as one goes from n to l to m sub l to m sub s

A

quantum numbers

41
Q

The first quantum number is commonly known as the ___ and is denoted by the letter n

A

principal quantum number

42
Q

The first quantum number, this is the quantum number used in Bohr’s model that can theoretically take on any positive integer value and represents the ___ where an electron is present in an atom

A

shell

43
Q

The maximum n that can be used to describe the ___ of an element at its ground state corresponds with that element’s period (row) in the periodic table

A

electrons

44
Q

Nitrogen is in period 2, so neutral Nitrogen in its ground state has ___ with n values of 1 and 2

A

electrons

45
Q

The larger the integer value of n, the ___ the energy level and radius of the electron’s orbit

A

higher

46
Q

The ___ number of electrons in an electron shell n is 2n^2

A

maximum

47
Q

The difference in energy between ___ shells decreases as the distance from the nucleus increases

A

adjacent

48
Q

The ___ difference between the third and fourth shells (n=3 and n=4) is less than that between the second and third shells (n=2 and n=3)

A

energy

49
Q

The second quantum number is called the ___ and is designated by the letter l

A

azimuthal (angular momentum) quantum number

50
Q

The second quantum number, this tells us the shape of the ___ and refers to the subshells or sublevels that occur within each principal energy level

A

orbitals

51
Q

For any given n, the ___ of l can be any integer in the range of 0 to n-1

A

value

52
Q

The four ___ corresponding to l=0,1,2,and 3 are known as the sharp, principal, diffuse, and fundamental subshells, or s,p,d, and f subshells respectively

A

subshells

53
Q

The greater the value of l, the ___ the value of the subshell

A

greater

54
Q

However, the ___ of subshells from different principal energy levels may overlap

A

energies

55
Q

For example, the 4s subshell will have a lower energy than the 3d subshell because its average distance from the ___ is smaller

A

nucleus

56
Q

The first two columns (of the periodic table) show the atoms that have their ___ electrons in the s subshell

A

valence

57
Q

The right “block” of the ___ table represents atoms that are filling the six spaces in the p subshell

A

periodic

58
Q

Columns 3-12 represent the d block, and the Lanthanide and ___ series are the f block

A

Actinide

59
Q

The third quantum number is the ___ and is designated m sub l

A

magnetic quantum number

60
Q

As far as the third quantum number is concerned, this number describes the orientation of the ___ in space

A

orbital

61
Q

An orbital is a specific ___ within a subshell that may contain no more than two electrons

A

region

62
Q

The ___ specifies the particular orbital within a subshell where an electron is highly likely to be found at a given point in time

A

magnetic quantum number

63
Q

The possible ___ of m sub l are all integers from l to -l including 0

A

values

64
Q

Therefore, the s subshell (l=0), has only one possible ___ of m sub l (0) and will contain one orbital; in contrast, the p subshell (l=1) has three possible m sub l values (-1, 0, +1) and three orbitals

A

value

65
Q

The d subshell (l =2) has five possible m sub l values (-2,-1,0,+1,+2) and five orbitals; the f subshell (l=3) has seven possible m sub l values (-3,-2,-1,0,+1,+2,+3) and contains ___ orbitals

A

seven

66
Q

The ___ and energy of each orbital are dependent upon the subshell in which the orbital is found

A

shape

67
Q

A p subshell with its three possible m sub l values (-1,0+1) has three dumbbell-shaped orbitals that are ___ in space around the nucleus along the x, y, and z axes

A

oriented

68
Q

Each p subshell has these three ___, they are often referred to as p sub x, p sub y, and p sub z

A

orbitals

69
Q

The fourth quantum number is also called the ___ and is denoted by m sub s

A

spin quantum number

70
Q

The ___ of a particle is its intrinsic angular momentum and is a characteristic of a particle

A

spin

71
Q

The two spin orientations are ___ +1/2 and -1/2

A

orientations

72
Q

Whenever two electrons are in the same orbital, they must have opposite spins due to the ___ exclusion principle

A

pauli

73
Q

Electrons in different ___ (different m sub l values) with the same m sub s values are said to have parallel spins

A

orbitals

74
Q

Electrons with opposite spins (different m sub s values) in the same orbital (same m sub l value) are often ___ to as paired

A

referred

75
Q

For a given atom or ion, the pattern by which ___ are filled and the number of electrons within each principal level and subshell are designated by an electron configuration

A

subshells

76
Q

In ___ notation, the first number denotes the principal energy level, the letter designates the subshell, and the superscript gives the number of electrons in that subshell

A

electron configuration

77
Q

According to the ___ principle, subshells are filled from lowest to highest energy, and each subshell will fill completely before electrons begin to enter the next one

A

aufbau

78
Q

The (n+l) rule is used to ___ subshells by increasing energy

A

rank

79
Q

Pertaining to the (n+l) rule, this rule states that the lower the sum of the first and second ___, the lower the energy of the subshell

A

quantum numbers

80
Q

If two ___ possess the same (n+l) value, the subshell with the lower n value has a lower energy and will fill first

A

subshells

81
Q

Similar to a greyhound bus filling up, ___ will go to empty orbitals before pairing up

A

electrons

82
Q

In the case of uncharged atoms, the number of ___ equals the atomic number

A

electrons

83
Q

If the atom is ___, the number of electrons is equal to the atomic number plus the extra electrons if the atom is negative or the atomic number minus the missing electrons if the atom is positive

A

charged

84
Q

In ___ that contain more than one orbital, such as the 2p subshell with its three orbitals, the orbitals will fill according to Hund’s rule

A

subshells

85
Q

Hund’s rule states that, within a given ___, orbitals are filled such that there are a maximum number of half-filled orbitals with parallel spins

A

subshell

86
Q

Electrons “prefer” empty orbitals to half-filled ones because a pairing ___ must be overcome for two electrons carrying repulsive negative charges to exist in the same orbital

A

energy

87
Q

The presence of paired or unpaired electrons affects the chemical and ___ properties of an atom or molecule

A

magnetic

88
Q

If the material has unpaired electrons, a magnetic field will ___ the spins of these electrons and weakly attract the atom to the field

A

align

89
Q

___ which have aligned magnetic fields and that have electrons which weakly attract the atom to the field are paramagnetic

A

materials

90
Q

Materials that have no unpaired ___ and are slightly repelled by a magnetic field are said to be diamagnetic

A

electrons

91
Q

The valence electrons of an atom are those electrons that exist in its outer ___ shell or that are available for chemical bonding

A

energy

92
Q

For elements in Groups IA and IIA, only the ___ s electrons are valence electrons

A

outermost

93
Q

For elements in Groups IIIA through VIIIA, the outermost s and p electrons in the highest energy ___ are valence electrons

A

shell

94
Q

For transition elements, the valence electrons are those in the outermost s subshell and in the d subshell of the ___ energy shell

A

next-to-outermost

95
Q

For the inner transition elements (the lanthanide and actinide series), the valence electrons are those in the s subshell of the outermost energy shell, the d subshell of the next-to-outermost energy shell, and the f ___ of the energy shell two levels below the outermost shell

A

subshell

96
Q

Atoms with half-filled and ___subshells are extremely stable

A

fully-filled

97
Q

Atoms with half filled and fully filled ___ are stable, so much so that some molecules will move electrons from a lower energy subshell into higher one to half fill the subshell

A

subshells

98
Q

For ___: it would be expected to have a valence shell configuration of 4s2 3d4. However, if it moves one s electron into the d subshell, then both subshells will be half filled. So, in reality, Cr exists as 4s1 3d5. The same thing is true for all other elements in column 6

A

chromium

99
Q

All atoms in column 11 will move one electron to complete the d subshell and, as a result, have a half-filled s ___Copper (Cu) will exist as 4s1 3d10

A

subshell

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