Atomic and Nuclear Structure Flashcards

1
Q

A = Atomic …

A

Atomic Mass Number

Total number of protons + neutrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Z = Atomic …

A

Atomic Number. Total number of protons.

Determines the number of electrons, and therefore the chemical properties of the atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

A - Z = …

A

A - Z = atomic mass number - number of protons = number of neutrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Isotopes have …

A

Same number of protons, different number of neutrons.

Same chemical behavior, different mass, and different nuclear decay properties.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Energy-mass relation?

Energy–momentum relation?

A

E = mc^2

E^2 = (pc)^2 + (m_0c^2)^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Electron mass?

How many times the proton mass?

A

0.511 MeV

roughly 1/1800 of proton or neutron mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Proton mass?

More or less than neutron mass?

How many times the electron mass?

A

938.3 MeV

A bit less than neutron mass.
roughly 1836 times electron mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Neutron mass?

More or less than proton mass?

A

939.6 MeV

A bit more than proton mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Electron Orbits - Principle quantum

Letters, and number of electrons.

A

Letters: K, L, M, N, O, …
Principle Quantum number: 1, 2, 3, 4, 5, …

Number of electrons 2n^2
n = quantum number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Electron binding energy vs. proximity to nucleus?

A

Electron binding energy increases with proximity to the nucleus by radius squared (r^2).

Closer to nucleus means lower energy level (more favorable).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Change in electron orbit results in / is caused by?

A

Release and absorption of energy.

Absorbed energy pushes electron in higher orbit (excitation) or frees it from atom if the absorbed energy is larger than its binding energy (ionization).

Falling down from higher to lower orbits releases energy equal to the energy difference of the two shells.
Energy is either transferred to higher shell electrons, which will be ejected from the atom as an Auger electron.
or
emitted in the form of a characteristic x-ray (photon)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What defines the chemical properties of an atom?

A

Number of protons (Z).

Same number of protons but different number of neutrons are the isotopes of an atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

The four fundamental forces in nature?

A

Strong Nuclear Force - “glues” the nucleus together - 1

Electromagnetic (Coulombic) Force - attraction and repulsion of charged particles - 1/37

Weak Nuclear Force - inside particles - 10^-6

Gravity - 10^-39

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Which fundamental forces are infinite, which are short ranged?

A

Infinite: Gravity and EM (1/r^2 dependence)

Short ranged (few femtometers): Strong and weak forces.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Size of hydrogen nucleus and electron cloud.

A

Nucleus: 1.70 fm (Femtometer = 1 × 10^-15 m)

Electron cloud: ~ 0.1 nm = 1 × 10^-10 m = 1 Å

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Excitation of an atom means …

A

A electron is moved from a given shell to a higher n shell that is either empty or does not contain a full complement of electrons.

17
Q

Ionization of an atom means …

A

A electron is removed from the atom (i.e. the electron is supplied with enough energy to overcome its binding energy in a shell).

18
Q

Auger electron

A

Electron which is ejected from atom because it received energy from an other electron falling into a lower orbit.