Atomic + Molecular Structure Flashcards

1
Q

What did Dalton’s Atomic Theory state?

A
  • All elements are composed of atoms
  • Atoms of 1 element differ from atoms of other elements
  • All compounds of composed of different atoms
  • No destruction/construction of atoms
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2
Q

Protons weigh about

A

1 amu

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3
Q

The atomic # (or Z) equals to the

A

Number of protons

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4
Q

The further the valence electron is from the nucleus the

A

Weaker the attraction is between the electron and the nucleus

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5
Q

Rutherford stated that the atom has a

A

Densely-charged nucleus which accounts for a small portion of the volume

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6
Q

Planck developed the first quantum theory, proposing that

A

Energy is emitted as electromagnetic radiation in quanta

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7
Q

What is the energy of a quantum?

A

E = h • f

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8
Q

What is the angular momentum (L) according to the Bohr model?

A

L = nh / 2π

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9
Q

The energy of the electron is given by

A

E = -Rh / n^2

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10
Q

The energy of an electron is related to the

A

Orbital radius

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11
Q

The smaller the radius means the

A

Lower the energy

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12
Q

What is the electromagnetic energy of protonss?

A

E = h•c / wavelength

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13
Q

Each element maintains its own

A

Atomic emission spectrum

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14
Q

The Lyman series describes emission to

A

n = 1 (UV)

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15
Q

The Balmer series describes emission to

A

n = 2 (UV + Vis)

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16
Q

The Pascher series describes emission to

A

n = 3 (Inf)

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17
Q

What is the equation to find energy level transitions?

A

E = -Rh (1/ni^2 - 1/nf^2)

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18
Q

The pauli exclusion principle states that

A

No 2 electrons in a given atom have the same 4 quantum numbers

19
Q

The max number of n correlates to the

A

Number of the period

20
Q

The larger the n the

A

Higher the energy level + radius

21
Q

The max number of electrons in a SHELL is denoted by

22
Q

As the distance from the nucleus increases, the

A

Difference in energy between adjacent shells decreases

23
Q

The azimuthal quantum number (l) ranges from

24
Q

When l = 0, the orbital is

25
When l = 1, the orbital is
P
26
When l = 2, the orbital is
D
27
When l = 3, the orbital is
F
28
The maximum number of electrons found in a subshell can be found by
4l + 2
29
The greater the value of l, the greater the
Energy
30
The magnetic quantum number (ml) ranges from
l to -l
31
Two electrons in the same orbital must have
Opposite spins
32
Electrons in different orbitals with the same ms values have
Parallel spins
33
Electrons in the same orbitals with different ms values have
Paired spins
34
The Aufbau principle states that
Subshells are filled from the lowest to highest energy
35
Which equation allows for one to determine subshell energy?
(n + 1)
36
The lower the sum of (n+1) the
Lower the energy
37
Hund's Rule states that
Orbitals are filled first before pairing
38
When a molecule is paramagnetic it means that it contains
Unpaired electrons
39
How does the magnetic field act when an atom is paramagnetic?
It aligns the spin of the electrons and attracts them
40
Diamagnetic atoms lack
Unpaired electrons
41
Diamagnetic atoms are repelled by the
Magnetic field
42
Which atoms are stable?
Ones with half-filled or fully-filled subshells
43
Half-filled subshells are found in columns
6 and 12