Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Biomolecular Engineering > Atomic Structure and Bonding > Flashcards

Atomic Structure and Bonding Flashcards

1
Q

The general form of the time-independent Schrodinger equation is given by:

A

HΨ =EΨ

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

Equation that describes the discreet energy levels in the hydrogen case:

A

E_(n )= R_(H ) (1/n^2 )

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

What do this two symbols mean?
H
Ψ

A

H - mathematical operator used to describe both the potential and kinetic energy of an electron
Ψ - wave function that describes the wave nature of an electron

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

Ψ^2 is proportional to …

A

… the probability of finding an electron with a given set of quantum numbers
… probability density function

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

Quantum number n (meaning and characteristic)

A
  • principal quantum number

- describes the overall size

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

Quantum number l

A
  • orbital angular momentum quantum number
  • shape of the orbital
  • ranging from 0 to (n-1)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Quantum number ml

A
  • magnetic quantum number

- ranging from -l to l

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

Quantum number ms

A
  • electron spin quantum number

- -1/2 or +1/2

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

Every orbital in a sub-shell receives one electron before double occupation occurs

A

Hund’s Rule of maximum multiplicity

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

What is the ionization energy?

A

It’s how much energy it takes to strip an electron from an atom

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

What happens to the ionization energy when the size of the atom increases?

A

It decreases.

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

What happens to the ionization energy when the size of the atom decreases?

A

It increases.

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

There are three primary bonds:

A

Ionic, Metallic and Covalent

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

The ionic bonds occurs between:

A

An electropositive element and a electronegative element. Between a metal and a non-metal

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

In which bond there is transfer of electrons from one atom to another

A

Ionic Bond

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

The force of an ionic bond can be calculated by ….. Law:

A

Coulomb’s Law

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

The covalent bonds occurs between:

A

An electronegative element and a electronegative element (or with itself)

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

In which bond there is sharing of electrons

A

Covalent Bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Relative to the spin of the electrons, in covalent bonds they have to go through:

A

Spin Paring

20
Q

Relative to direction, covalent bonds are …

A

significant anisotropy which means, they are directionally dependent

21
Q

What’s the definition for electropositive:

A

Likely to give an electron

22
Q

What’s the definition for electronegative:

A

Likely to receive an electron

23
Q

Which bond leads to isotropic behaviour:

A

Ionic Bond

24
Q

Why are ionic bonds stable?

A

Because the charge-charge interaction leads to stable bonds which results in high melting temperatures and good chemical stability.

25
Q

Between hybrid orbitals there is a new bond formed called:

A

sigma bond

26
Q

What’s one characteristic of sigma bonds:

A

Rotational freedom

27
Q

What does hybridization means:

A

It’s the superposition of wave functions.

Concept of mixing atomic orbitals into new hybrid orbitals

28
Q

In a double bond, a … is formed:

A

π Bond

29
Q

How are sigma bonds formed?

A

They form between two covalently bonded atoms.

30
Q

Are π bonds stronger or weaker compared to sigma bonds? Why?

A

Weaker, because there is significantly less orbital overlap

31
Q

How are π bonds formed?

A

Between p orbitals that have the same direction.

32
Q

Do π bonds have rotational freedom?

A

No

33
Q

The metallic bond occurs between:

A

Electropositive elements

34
Q

What is the main characteristic of a metallic bond?

A

Simple lattice of protons and a “sea” of electrons

35
Q

Is there directionality in metallic bonds:

A

No

36
Q

Secondary Bond are also known as

A

Van der Waals forces

37
Q

Ideal Gas Law:

A

PV = N k_B T

38
Q

Describe polarizability

A

Ability to form instantaneous dipoles, determines the dynamical response of a bound system to external fields

39
Q

Keesom Forces form between …

A

… permanent dipoles

40
Q

Two permanent dipoles that interact with each other have the ability to …

A

… promote the local alignment of the molecule

41
Q

Debye Forces form between …

A

a molecule with a permanent dipole and a molecule with no dipole

42
Q

The type of secondary bond that is always present is

A

London Dispersion Forces

43
Q

Dispersion Forces form between …

A

Instantaneous Dipole (Spontaneous dipole) - Instantaneous Dipole (Induced Dipoles)

44
Q

In secondary bonds, pull of certain atoms can bias …

A

the spatial location of e- cloud

45
Q

Hydrogen Bonds form between:

A

H bonded to N, O or F and N, O or F

46
Q

Which is the strongest secondary bond?

A

Hydrogen Bond: 5-10 KT

VdW: ~ 1KT

Biomolecular Engineering (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions