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A - Level Chemistry > C5 Electrons And Bonding > Flashcards

C5 Electrons And Bonding Flashcards

1
Q

What are shells regarded as

A

Energy levels

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2
Q

What is the principle quantum number n

A

Shell number or energy level number

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3
Q

What is the formula for the maximum number of electrons in a shell n

A

2n^2

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4
Q

What are shells made up of

A

Atomic orbitals

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5
Q

What is an atomic orbital

A

A regional around the nucleus that can hold up to 2 electrons, with opposite spins

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6
Q

How many electrons can an orbital hold

A

1 or 2 electrons but no more

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7
Q

What are the different types of orbitals

A

S-

P-

D-

F-

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8
Q

Do the orbitals have the same shapes

A

No

They each have different shapes

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9
Q

What is a shell

A

A group of orbitals with the same principle quantum number

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10
Q

How many electrons can the 1st shell hold

A

2

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11
Q

How many electrons can the 2nd shell hold

A

8

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12
Q

How many electrons can the 3rd shell hold

A

18

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13
Q

How many electrons can the 4th shell hold

A

32

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14
Q

What’s the shape of an s-orbital

A

Spherical

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15
Q

What’s the shape of a p-orbital

A

Dumb-bell shape

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16
Q

How many orbitals are found in a s-sub shell

A

1

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17
Q

How many electrons can be held in a s-subshell

A

2

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18
Q

How many orbitals does p-sub shell have

A

3

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19
Q

How many electrons can be held in a p-subshell

A

6

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20
Q

How many orbitals are present in a D sub shell

A

5

21
Q

How many electrons can be held in a d sub shell

A

10

22
Q

How many orbitals are found in a F sub shell

A

7

23
Q

How many electrons can fill F sub shell

A

14

24
Q

What are the rules by which electrons are arranged in the shell

A

Electrons are added 1 at a time

Lowest available energy level is filled first

Each energy level must be filled before the next one can fill

Each orbital is filled singly before pairing

4s is filled before 3d

25
Q

Why does 4s orbital fill before 3d orbital

A

4s orbital has a lower energy than 3d before its filled

26
Q

Whats an ionic bond

A

Electrostatic attraction between positive and negative ions.

27
Q

Why does giant ionic lattices conduct electricity when (l) but not when (s)

A

When (s) ions fixed in place - cannot move

When (l) ions are mobile - freely carry charge

28
Q

What’s a metallic bond

A

Electrostatic attraction between the positive metal ions and the sea of delocalised electrons

29
Q

Why do giant metallic lattices have high MPs & BPs

A

Large amount of energy required to overcome strong metallic bonds

30
Q

In what type of solvents do ionic lattices dissolve

A

Polar solvents

E.g.water

31
Q

Why are ionic compounds soluble in water

A

Water has polar bond

Delta pos of H attracted and delta neg of O can attract ions

32
Q

How many covalent bonds does a carbon form

A

4

33
Q

How many covalent bonds does oxygen form

A

2

34
Q

What’s a dative covalent bond

A

Bond where both of shared electrons are supplied by one atom

35
Q

What does expansion of the octet mean

A

When a bonded atom has more than 8 electrons in the outer shell

36
Q

What are the 2 types of covalent structure

A

Simple molecular lattice

Giant covalent lattice

37
Q

Why do simple molecular structures have low MPs & BPs

A

Small amount of energy is enough to overcome the intermolecular forces

38
Q

Can simple molecular structures conduct electricity and why

A

No

They’re non-conductors

They have no free charged particles to move around

39
Q

In that type of solvents do simple molecular structures dissolve in

A

Non-polar solvents

40
Q

Examples of giant covalent structures

A

Diamond

Graphite

Silicon dioxide, SiO2

41
Q

Properties of giant covalent structures

A

High MPs & BPs

Non-conductors of electricity, except graphite

Insoluble in polar & non-polar solvents

42
Q

How does graphite conduct electricity

A

Delocalised electrons present between layers are able to move freely carrying charge

43
Q

Why do giant covalent structures have high MPs & BPs

A

Strong CBs within molecules need to be broken which requires a lot of energy

44
Q

Describe the structure of a diamond

A

3D tetrahedral structure of C atoms

With each C atoms bonded to 4 others

45
Q

By how many degrees does each lone pair reduce bond angle

A

2.5*

46
Q

What does it mean when the bond is non-polar

A

Electrons in bond are evenly distributed

47
Q

What’s the most electronegative element

A

Fluorine

48
Q

What’s the strongest type of IMF

A

Hydrogen bonding

A - Level Chemistry (31 decks)

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