Atomic Structure Flashcards

2- Structure and Bonding

1
Q

subatomic particles found in the dense nucleus of an atom

A

protons and neutrons

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

surrounds the dense nucleus

A

electrons

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

most of the mass is in the _________

A

nucleus

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

most of the volume is in the _____

A

electron cloud

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

indicates the total number of protons and the number of neutrons present in an atom

A

mass number

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

states the number of protons present in an atom

A

atomic number

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

atoms with the SAME number of protons but DIFFERENT numbers of neutrons

A

isotopes

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

almost 99% of the carbon found in nature

A

12C

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

the exact location of the electron
CANNOT be known; ONLY the electron density can be known

A

Quantum Mechanical Model

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

the probability that the electron will be in a certain region of space (orbital) at a given instant

A

electron density

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

Where do electrons move instead of circling around the nucleus in fixed orbits?

A

orbitals

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

each orbital has a characteristic _ and _.

A

shape, size (energy)

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

used to describe orbitals

A

Quantum Numbers

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

4 quantum numbers

A
  1. Principal
  2. Azimuthal/Angular Momentum
  3. Magnetic
  4. Electron Spin
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

symbol for Principal quantum number

A

n

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

symbol for Azimuthal/
Angular Momentum quantum number

A

l

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

symbol for Magnetic quantum number

A

m_l

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

symbol for Electron Spin quantum number

19
Q
  • indicates the main energy level or shell (size) of an electron in an atom
  • represents the average distance of the electron from the nucleus
20
Q

determines the shape (subshell) of the orbital

A

Azimuthal/
Angular Momentum

21
Q

specifies the orientation of the orbital in space

22
Q

describes the spin (direction) of an electron within an orbital

A

Electron Spin

23
Q

values can be any positive integer and indicates the energy level or shell where electrons are located

24
Q

ranges from 0 to (n-1) / s, p, d, f; corresponds to different sublevels within each principal energy level

A

Azimuthal/
Angular Momentum

25
ranges from **-l to +l** and defines the number of orbitals present within a sublevel
Magnetic
26
can have one of two possible values: **+1/2** (spin up) or **-1/2** (spin down).
Electron Spin
27
number of orbitals and electrons in s-subshell
one orbital, 2 electrons
28
number of orbitals and electrons in p-subshell
three orbitals, 6 electrons
29
number of orbitals and electrons in d-subshell
five orbitals, 10 electrons
30
number of orbitals and electrons in f-subshell
seven orbitals, 14 electrons
31
shape of s orbital
spherical
32
shape of p orbital
dumbbell
33
shape of four of the five d orbitals
cloverleaf
34
shape of the fifth d orbital
elongated dumbbell with a doughnut around its middle
35
describes where electrons are located around the nucleus of an atom
Electron Configuration
36
describes the orbitals occupied by the atom’s electrons when they are all in the available orbitals with the lowest energy
Ground-state electron configuration
37
* Electrons fill the lowest energy orbitals available before moving to higher energy orbitals. * This principle dictates the order in which electrons occupy atomic orbitals.
Aufbau Principle
38
* Electrons prefer to occupy degenerate orbitals (orbitals of the same energy) singly with parallel spins before pairing up. * This maximizes the total electron spin and stabilizes the atom. | This requires single occupancy before pairing.
Hund’s Rule
39
* No two electrons in a atom can have an identical set of four quantum numbers. * This means an orbital can hold a maximum of two electrons, and then the electrons must have opposite spins, +1/2 and -1/2.
Pauli Exclusion Principle
40
This principle states that it is impossible to simultaneously know the exact position and momentum (or velocity) of a particle, such as an electron.
Heisenberg's Uncertainty Principle
41
electrons below the outermost shell
Core Electrons
42
electrons in the outermost shell
Valence Electrons
43