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A-Level OCR Chemistry > 5. Electrons and bonding > Flashcards

5. Electrons and bonding Flashcards

1
Q

What are shells?

A

A group of atomic orbitals with the same principal quantum number N.

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2
Q

What are atomic orbitals?

A

A region around the nucleus that can hold up to two electrons, with opposite spins.

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3
Q

What are the 4 types of orbitals?

A
  1. s
  2. p
  3. d
  4. f
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4
Q

What is the shape of s-orbital?

A

Spherical

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5
Q

What is the shape of p-orbital?

A

Dumb-bell shape

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6
Q

How many orbitals make up a s-subshell?

A

1

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7
Q

How many orbitals make up a p-subshell?

A

3

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8
Q

How many orbitals make up a d-subshell?

A

5

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9
Q

How many orbitals make up a f-subshell?

A

7

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10
Q

How many orbitals are there in the 1st shell?

A

1

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11
Q

How many orbitals are there in the 2nd shell?

A

4

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12
Q

How many orbitals are there in the 3rd shell?

A

9

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13
Q

How many orbitals are there in the 4th shell?

A

16

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14
Q

How many electrons can fill a s-orbital?

A

2

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15
Q

How many electrons can fill a p-orbital?

A

6

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16
Q

How many electrons can fill a d-orbital?

A

10

17
Q

How many electrons can fill a f-orbital?

A

14

18
Q

How many electrons can fill the 1st shell?

A

2

19
Q

How many electrons can fill the 2nd shell?

A

8

20
Q

How many electrons can fill the 3rd shell?

A

18

21
Q

How many electrons can fill the 4th shell?

A

32

22
Q

What orbital is in the 1st shell?

A

s-orbital

23
Q

What orbitals are in the 2nd shell?

A

s- and p-orbital

24
Q

What orbitals are in the 3rd shell?

A

s-, p- and d- orbital

25
Q

What orbitals are in the 4th shell?

A

s-, p-, d- and f-orbital

26
Q

Rearrange the orbitals in terms of energy level.

A

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

27
Q

What is ionic bonding?

A

Electrostatic attraction between positive and negative ions.

28
Q

What are giant ionic lattices?

A

A three-dimensional structure of oppositely charged ions that are strongly attracted in all directions, bonded together by strong ionic bonds.

29
Q

How are ionic compounds’ melting point and boiling point? Why?

A

Ionic compounds have high melting point and boiling point, because they have strong electrostatic attractions between ions, which requires a lot of energy to overcome.

30
Q

How are ionic compounds’ solubility?

A

Ionic compounds dissolve in polar solvents, eg. water. Polar molecules break down the lattice and surround each ion in solution.

31
Q

How are ionic compounds’ electrical conductivity in solid state? Why?

A

Ionic compounds can’t conduct electricity in solid state, because ions are fixed and can’t move to carry electric charge.

32
Q

How are ionic compounds’ electrical conductivity in liquid state? Why?

A

Ionic compounds can conduct electricity in liquid state, because ions can move freely and carry electric charge.

33
Q

How are ionic compounds’ electrical conductivity in aqueous state? Why?

A

Ionic compounds can conduct electricity in aqueous state, because ions can move freely and carry electric charge.

34
Q

What is covalent bonding?

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

35
Q

What is dative covalent bonding?

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atom only.

36
Q

What is average bond enthalpy? What does it mean?

A

A measurement of covalent bond strength. The larger the value of the average bond enthalpy, the stronger the covalent bond.

37
Q

How are covalent compounds’ electrical conductivity? Why?

A

Covalent compounds can’t conduct electricity in any state, because they don’t have mobile electrons.

38
Q

How are covalent compounds’ melting point and boiling point? Why?

A

Covalent compounds have low melting and boiling point, because they have weak London forces, which are easy to overcome and separate the molecule.

A-Level OCR Chemistry (10 decks)

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