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A Level Chemistry > Chapter 5 - Electrons and bonding > Flashcards

Chapter 5 - Electrons and bonding Flashcards

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1
Q

Where are shells with the highest energy levels located?

A

Further from the nucleus

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2
Q

What are the four types of sub-shells?

A

S-orbital
P-orbital
D-orbital
F-orbital

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3
Q

How many orbitals are there in an S sub-shell?

A

1

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4
Q

How many electrons can fit in the S sub-shell?

A

2

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5
Q

How many orbitals are there in the P sub-shell?

A

3

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6
Q

How many electrons are can fit in the P sub-shell?

A

6

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7
Q

How many orbitals are there in the D sub-shell?

A

5

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8
Q

How many electrons can fit in the D sub-shell?

A

10

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9
Q

How many orbitals are there in the F sub-shell?

A

7

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10
Q

How many electrons can fit in the F sub-shell?

A

14

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11
Q

What is an orbital?

A

An area of space that an electron moves in

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12
Q

What is spin-pairing?

A

When there are two electrons in an orbital, they must spin in opposite directions

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13
Q

What is the shape of S orbitals?

A

Spherical

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14
Q

What is the shape of P orbitals?

A

Dumbbell

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15
Q

How many P orbitals are there?

A

3

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16
Q

What is sub shell notation?

A

You write the energy shell, then sub-shell, then the number of electrons, e.g. 1s2 2s2 2p6

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17
Q

How to show electron configuration using the electrons in boxes method?

A

Each box represents one orbital and each arrow represents one electron
One arrow must go up and the other down

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18
Q

What is important to remember about the 4s sub-shell?

A

It is at a lower energy level than the 3d sub-shell, so will fill first but also empties first
We also write the 3d sub-shell first

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19
Q

In what manner will electrons fill orbitals with the same energy level?

A

Singly

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20
Q

What is an ionic bond?

A

An eletrostatic attraction between two oppositely charged ions

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21
Q

How can you work out the formula of an ionic compound?

A

Work out the charges on the ions and ensure it is balanced so the total charge is zero

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22
Q

What is n electronic orbital?

A

A region around the nucleus that can hold up to two electrons

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23
Q

What is a sub-shell?

A

Orbitals of the same type are grouped together

24
Q

What is important to remember about two electrons in the same orbital?

A

They must have opposite spins

25
Q

Why does the 4s shell fill before the 3d sub-shell?

A

It is at a lower energy level

26
Q

What is shorthand notation for electronic structure?

A

You write the symbol of the previous noble gas plus the outer electron sub-shells

27
Q

What are the three blocks of the periodic table?

A

S-block
P-block
D-block

28
Q

Where is the S-block?

A

The first two groups of the periodic table

29
Q

Where is the P-block?

A

The 6 groups on the right

30
Q

Where is the D-block?

A

The central 10 groups

31
Q

What does the block an element is in represent?

A

The highest energy electrons will be in that sub-shell

32
Q

What do dot and cross diagrams show?

A

The arrangement of electrons in an atom

33
Q

How to draw a dot and cross diagram?

A

Draw the outer shell of electrons inside a square bracket, using dots and crosses to show where the electrons came from. The charge should be indicated outside the bracket

34
Q

Example of a giant ionic lattice

A

Sodium chloride

35
Q

Why does sodium chloride have a high melting point?

A

It has very strong ionic bonds

36
Q

3 characteristics of ionic compounds

A

They can conduct electricity when molten but not solid
High melting and boiling points
Tend to dissolve in water

37
Q

Why can ionic compounds only conduct electricity when molten or dissolved?

A

In a solid, the ions are fixed in position by the ionic bonds, but when molten are mobile and can carry a charge

38
Q

Why do ionic compounds have high melting and boiling points?

A

A lot of energy is needed to overcome the strong electrostatic forces

39
Q

When will the melting point of an ionic lattice be higher?

A

For ions with greater charges, e.g. Ca 2+

40
Q

Why do ionic compounds tend to dissolve in water?

A

Water is a polar solvent, so the charged ends of the water molecule are attracted to the charged ions and pull the ions from the lattice, causing it to dissolve

41
Q

What does the solubility of an ionic compound depend upon?

A

The attractions within the lattice and the attraction between the ions and water molecules

42
Q

What is a covalent bond?

A

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

43
Q

What happens when two atoms bond covalently?

A

Orbital overlap occurs

44
Q

How to represent covalent bonds

A

Dot and cross diagrams with their outer orbitals overlapping

45
Q

What is the displayed formula?

A

It shows how the relative positioning of atoms and the bonds between them

46
Q

Give to exceptions to the octet rule

A

Boron trifluoride

Sulfur hexafluoride

47
Q

Why is boron trifluoride an exception?

A

Boron only has 6 outer electrons, not 8

48
Q

Why is sulfur hexafluoride an exception?

A

Sulfur has 12 electrons in its outer shell

49
Q

What are multiple covalent bonds?

A

When two atoms share more than one pair of electrons

50
Q

The best example of a double covalent bond

A

Oxygen, O2

51
Q

What is a double covalent bond?

A

When two atoms share two pairs of electrons

52
Q

The best example of a triple bond

A

Nitrogen, N2

53
Q

What is a triple bond?

A

The electrostatic attraction between three shared pairs of atoms and the nuclei of the bonded atoms

54
Q

What is special about CO2?

A

It has two double bonds

55
Q

What are dative covalent bonds?

A

Where both electrons come from one atom

56
Q

The best example of a dative covalent bond

A

NH3 and H+

57
Q

How do you know when to use a dative bond?

A

Draw the dot and cross diagram of the two components

Where there are two spare electrons on one atom, this becomes the dative bond

A Level Chemistry (29 decks)

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