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

21
Q

How many electrons can be held in a d sub shell

22
Q

How many orbitals are found in a F sub shell

23
Q

How many electrons can fill F sub shell

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
Why does 4s orbital fill before 3d orbital
4s orbital has a lower energy than 3d before its filled
26
Whats an ionic bond
Electrostatic attraction between positive and negative ions.
27
Why does giant ionic lattices conduct electricity when (l) but not when (s)
When (s) ions fixed in place - cannot move When (l) ions are mobile - freely carry charge
28
What’s a metallic bond
Electrostatic attraction between the positive metal ions and the sea of delocalised electrons
29
Why do giant metallic lattices have high MPs & BPs
Large amount of energy required to overcome strong metallic bonds
30
In what type of solvents do ionic lattices dissolve
Polar solvents E.g.water
31
Why are ionic compounds soluble in water
Water has polar bond Delta pos of H attracted and delta neg of O can attract ions
32
How many covalent bonds does a carbon form
4
33
How many covalent bonds does oxygen form
2
34
What’s a dative covalent bond
Bond where both of shared electrons are supplied by one atom
35
What does expansion of the octet mean
When a bonded atom has more than 8 electrons in the outer shell
36
What are the 2 types of covalent structure
Simple molecular lattice Giant covalent lattice
37
Why do simple molecular structures have low MPs & BPs
Small amount of energy is enough to overcome the intermolecular forces
38
Can simple molecular structures conduct electricity and why
No They’re non-conductors They have no free charged particles to move around
39
In that type of solvents do simple molecular structures dissolve in
Non-polar solvents
40
Examples of giant covalent structures
Diamond Graphite Silicon dioxide, SiO2
41
Properties of giant covalent structures
High MPs & BPs Non-conductors of electricity, except graphite Insoluble in polar & non-polar solvents
42
How does graphite conduct electricity
Delocalised electrons present between layers are able to move freely carrying charge
43
Why do giant covalent structures have high MPs & BPs
Strong CBs within molecules need to be broken which requires a lot of energy
44
Describe the structure of a diamond
3D tetrahedral structure of C atoms With each C atoms bonded to 4 others
45
By how many degrees does each lone pair reduce bond angle
2.5*
46
What does it mean when the bond is non-polar
Electrons in bond are evenly distributed
47
What’s the most electronegative element
Fluorine
48
What’s the strongest type of IMF
Hydrogen bonding