Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Chapter 5 - Structure and Bonding > Flashcards

Chapter 5 - Structure and Bonding Flashcards

1
Q

What can an electron be thought of as ?

A

A negatively charged cloud with the shape of an orbital, called an electron cloud

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

Shells are regarded as what ?

A

Energy levels

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

What happens to energy as the shell number increases ?

A

Energy increases

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

What is the shell number referred to as ?

A

Principal quantum number (n)

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

What are shells made up of ?

A

Atomic orbitals

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

What is an orbital ?

A
  • An orbital is an area around the nucleus where electrons with opposite spin are likely to be found
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are the different orbitals ?

A
  • S orbitals
  • P orbitals
  • D orbitals
  • F orbitals
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How many electrons can be held in an orbital ?

A

One or two, no more

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

How many orbitals does each type contain ?

A
  • S - one
  • P - three
  • D - five
  • F - seven
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How many electrons can be held in each type of orbital ?

A
  • S - two
  • P - six
  • D - ten
  • F - fourteen
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the shape of an s orbital ?

A

Spherical

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

What is the shape of a p orbital ?

A
  • Dumbbell

- Theres three types, one in each plane (x,y and z)

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

What are the rules of orbital fillings ?

A
  • Orbitals fill in order of increasing energy
  • Electrons pair with opposite spins
  • Orbitals with the same energy are occupied singly first
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Explain the rule of orbitals filling in order of increasing energy

A
  • 1s is filled first
  • Then 2s and 2p
  • Then 3s, 3p, 4s and then 3d
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Where does this rule cause confusion ?

A
  • The 3d sub-shell has higher energy than the 4s.

- So the 4s fills before the 3d

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

State the orbital filling until the 4th shell

A
  • 1s
  • 2s, 2p
  • 3s, 3p, 4s, 3d
  • 4p, 4d, 4f
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Explain the rule of electrons pair with opposite spins

A
  • Electrons are negatively charged and repel one another
  • Electrons can have spin up or spin down
  • If electrons have opposite spin, the charge repulsion is counteracted enough for both to be in the orbital, they cancel out
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Explain the rule of orbital filling when the same energy subshells are occupied singly first

A
  • Within a sub shell, the orbitals have the same energy
  • One electron occupies each orbital before pairing begins.
  • This prevents repulsion until no unoccupied orbitals remain
19
Q

How can electron configuration be shortened ?

A
  • 1s2 can be expressed as [He]
  • 1s2 2s2 2p6 can be expressed as [Ne]
  • 1s2 2s2 2p6 3s2 3p6 can be expressed as [Ar]
20
Q

What is this format called ?

A

Shorthand notation

21
Q

What happens in terms of energy sub-shells when forming ions ?

A

The highest energy sub shells lose or gain electrons

22
Q

What is ionic bonding ?

A

The electrostatic attraction between oppositely charged ions

23
Q

In what directions are ions attracted to other ions ?

A

In all directions

24
Q

What is the result of ions attracting oppositely charged ions in all directions ?

A

Giant ionic lattice

25
Q

How are the melting and boiling points of ionic compounds explained ?

A

High temperatures are required to provide the energy to overcome the strong electrostatic attraction between the ions

26
Q

What happens to the melting points for giant ionic lattices, when ionic charge increases ?

A

Melting point increases as there is a stronger attraction between ions

27
Q

When are ionic compounds soluble ?

A

They dissolve in polar solvents such as water

28
Q

What does solubility require ?

A
  • The ionic lattice must be broken down

- Water molecules must attract and surround the ions

29
Q

What does solubility (of ionic compounds) depend on ?

A

The strength of the attraction within the giant ionic lattice and the attractions between ions and water molecules

30
Q

When can ionic compounds conduct electricity ?

A
  • When molten or dissolved in water
31
Q

Why can’t ionic compounds conduct electricity when solid ?

A
  • The ions are in a fixed position

- This means that they can not carry charge

32
Q

Why can ionic compounds conduct electricity when molten or dissolved in water ?

A
  • The solid ionic lattice breaks down

- The ions are now free to move and carry charge

33
Q

Summarise the properties of most ionic compounds

A
  • High melting and boiling points
  • Tend to dissolve in polar solvents such as water
  • Conduct electricity only in the liquid state or in aqueous solution
34
Q

What is covalent bonding ?

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

35
Q

What actually is a covalent bond ?

A

The overlap of two atomic orbitals, each containing one electron, to give a shared pair of electrons.

36
Q

How does covalent bonding differ to ionic bonding ?

A
  • The attraction in covalent bonding is localised

- This means it only acts on the shared pair of electrons and the nuclei of the two bonded atoms

37
Q

How can covalent bonding be displayed ?

A

With dot and cross diagrams

38
Q

What is a multiple covalent bond ?

A

Two atoms share more than one pair of electrons

39
Q

What is a double bond ?

A

A double bond occurs when the electrostatic attraction is between two shared pairs of electrons, and the nuclei of the bonding atoms

40
Q

What is a triple bond ?

A

A triple bond occurs when the electrostatic attraction is between three shared pairs of electrons, and the nuclei of the bonding atoms

41
Q

What is a dative covalent bond ?

A
  • A dative covalent bond occurs when the shared pair of electrons has been supplied by one of the bonding atoms only
  • Originally a lone pair
42
Q

Give an example of a dative covalent bond

A
  • An ammonia molecule donates its lone pair of electrons to an H+ ion.
  • Forming an ammonium ion
43
Q

What is average bond enthalpy ?

A
  • A measure of covalent bond strength.

- Larger value = stronger bond

Chemistry (29 decks)

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