Electron structure Flashcards

1
Q

How many electrons can occupy the first shell?

A

2

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

How many electrons can occupy the second shell?

A

8

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

How many electrons can occupy the third shell?

A

18

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

How many electrons can occupy the fourth shell?

A

32

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

True of false?

Electron shells make up a model that helps us to visualise something that cannot be seen

A

True

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

What happen to the energy as the shell number increases?

A

The energy increases as the shell number increases

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

What is another name for the shell number or energy level number?

A

The principle quantum number n

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

What is meant by the term atomic orbital?

A

An atomic orbital is a region around the nucleus that can hold up to two electrons with opposite spins

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

What is the maximum number of electrons that can be found in an orbital?

A

Two

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

What are the four different types of orbitals that you can get?

A

s-, p-, d-, and f- orbitals

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

True or flase? Each type of orbital has a diffreent shape.

A

True

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

What type of orbital is shown in the diagram?

A

S- orbital

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

How many s-orbitals can each shell contain?

A

Each shell contains one s-orbital

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

Describe the trend between shell number and radius of the s-orbital.

A

The greater the shell number, the greater the radius of the s-orbital.

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

What type of orbital is shown in the diagram below

A

p-orbital

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

What shape can we liken a p-orbital to?

A

A dumb-bell

17
Q

What is the maximum amount of electrons each p-orbital can contain?

A

Two

18
Q

How many p-orbitals can each shell contain?

A

Each shell can contain three p-orbitals

19
Q

Is there a way to distinguish between the three p-orbitals per shell or not?

A

Yes; px, py and pz

20
Q

Describe the trend between shell number and distance from the nucleus of the p-orbital.

A

The greater the shell number, the further the p-orbital is from the nucleus

21
Q

Each shell from n = 3 contains how many d-orbitals?

A

Five

22
Q

Each shell from n = 4 contains how many f-orbitls?

A

Seven

23
Q

True or false? Each new shell gains a new type of orbital in addition to the ones in the previous shell.

A

True

24
Q

What is the order for filling the electron shells?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 4d, 4f

25
Q

Explain why sub shell 4s fills before subshell 3d in terms of energy levels.

A

The highest energy level in the third shell overlaps with the lowest energy level in the fourth shell. Sub shells fill in order of incresing energy levels. 3d is at a higher ennergy level than 4s and so 4s fills first.

26
Q

Why must electrons be shown by opposite spins (as either an arrow pointing up or down)?

A

Because the opposite spins help to counteract the repulsion between the negative charges of the two electrons.

27
Q

Describe how electrons fill up sub shells within an orbital.

A

One electron occupies each orbital before pairing starts. This prevents any repulsion from occuring between paired electrons until there is no further orbital available at the same energy level.

28
Q

What is meant by the term shorthand electron configuration?

A

Electron configurations that are expressed much more simply in terms of the previous noble gas plus the outer electron sub-shells

29
Q

Pactice quetsion:

What is the full and shorthand configurations of electrons for Li?

A

1s2 2s1 [He]2s1

30
Q

Pactice quetsion:

What is the full and shorthand configurations of electrons for Na?

A

1s2 2s2 2p6 3s1

[Ne]3s1

31
Q

What is the name given to the species that form when an atom loses an electron?

A

Cation

32
Q

What is the name given to the species that forms when an atom gains an electron?

A

Anions

33
Q

Which area of the periodic table is given the name of s-block? p-block? d-block?

A
34
Q

True or false? Despite the fact that 4s fills before 3d, 4s loses electrons first

A

True

35
Q

Why does copper not fill 4s before 3d?

A

Because it is more stable for it to end in d5 or d10 due to minimum repulsion between electrons