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Chemistry > Chapter 5 Electrons and Bonding > Flashcards

Chapter 5 Electrons and Bonding Flashcards

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1
Q

What is a shell

A

A shell is an energy level, comprised of sub shells called s p d f. The shell number is called the principal quantum number ‘n’

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2
Q

What is an Atomic Orbital

A

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

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3
Q

What shape are s orbitals

A

The electron cloud is within the shape of a sphere

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4
Q

As the shell number ‘n’ increases, what happens to the radius of its s-orbital

A

It increases

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5
Q

What shape are p orbitals

A

Dumb-bell
There 3 orbitals at right angles to eachother

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6
Q

How many electrons can fit in s orbitals

A

2

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7
Q

How many electrons can fit in p orbitals

A

6

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8
Q

How many electrons can fit in d orbitals

A

10

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9
Q

How many electrons can fit in f orbitals

A

14

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10
Q

How many electrons can fit inside shell n=1

A

2

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11
Q

How many electrons can fit in shell n=2

A

8

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12
Q

How many electrons can fit in shell n=3

A

18

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13
Q

How many electrons can fit in shell n=4

A

32

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14
Q

What is the electron configuration

From 1s to 4f

A

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

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15
Q

What is the electron configuration

From 1s to 4f with the number of electrons in each sub-shell

A

1s²
2s²
2p⁶
3s²
3p⁶
4s²
3d¹⁰
4p⁶
4d¹⁰
4f¹⁴

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16
Q

How many s-orbitals are there in each shell from n = 1 onwards

A

1

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17
Q

How many p-orbitals are there in each shell from n = 2 onwards

A

3

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18
Q

When overlaped on to 1 diagram, why do the 3, p orbitals extend out further than the nucleus

A

They have a slightly higher energy

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19
Q

How many d-orbitals are there in each shell from n = 3 onwards

A

5

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20
Q

How many f-orbitals are there in each shell from n = 4 onwards

A

7

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21
Q

Which sub-shells are present in shell n = 1

A

1s

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22
Q

Which sub-shells are present in shell n = 2

A

2s + 2p

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23
Q

Which sub-shells are present in shell n = 3

A

3s + 3p + 3d

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24
Q

Which sub-shells are present in shell n = 4

A

4s + 4p + 4d + 4f

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25
Q

True or false:

4s fills before 3d

A

True

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26
Q

How would 2 electrons be represented in an orbital

Box diagram

A

|↑↓|

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27
Q

How are orbitals filled

A

Each orbital of the same energy is occupied before spin pairing occurs in the orbitals with 2 electrons paired together

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28
Q

Which of these has been drawn correctly

  1. |↑↓| |↑↓| | |
  2. |↑↓| |↑ | |↑ |
A

2 - |↑↓| |↑ | |↑ |

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29
Q

Write the electron configuration of Magnesium z=12

A

1s²2s²2p⁶3s²

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30
Q

How do you write the shorthand electron configuration

A

Find the previous noble gas and write the remaining electron configuration

31
Q

Write the electron configuration of Potassium Z=19

A

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹

32
Q

Write the electron configuration of Scandium Z=21

A

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹ 4s²

33
Q

Which sub-shell is filled first 4s or 3d

A

4s

34
Q

What two elements have an exemption to the rule of electron configuration

A

Chromium & Copper

35
Q

What is the electron configuration of Chromium

An exemption

A

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹

36
Q

What is the electron configuration of Copper

An exemption

A

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s¹

37
Q

If this is the electron configuration of an Mg atom, write the electron configuration of an Mg²⁺ ion

1s² 2s² 2p⁶ 3s²

A

1s² 2s² 2p⁶

38
Q

If this is the electron configuration of a Cl atom, write the electron configuration of a Cl⁻ ion

1s² 2s² 2p⁶ 3s² 3p⁵

A

1s² 2s² 2p⁶ 3s² 3p⁶

39
Q

Which sub-shell loses electrons first when forming electron configurations of Ions:
4s or 3d

A

4s

40
Q

If this is the electron configuration of an Fe ion, write the electron configuration of an Fe²⁺ ion

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s²

A

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶

41
Q

If this is the electron configuration of an Fe ion, write the electron configuration of an Fe³⁺ ion

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s²

A

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵

42
Q

What is Ionic bonding

A

The electrostatic attraction between positive ions (cations) and negative ions (anions)

43
Q

Give examples of common cations

A
  • Metal ions
    - K⁺
    - Ca²⁺
    - Mg²⁺
    - Al³⁺
  • Ammonium ion
    - NH₄⁺
44
Q

Give examples of common anions

A
  • Non-metal ions
    • Cl⁻
    • O²⁻
    • S²⁻
  • Polyatomic ions
    • SO₄²⁻
    • CO₃²⁻
    • NO₃⁻
45
Q

What is the structure of ionic compounds

A
  • Oppositely charged ions attract each other strongly
  • Each ion attracts oppositely charged ions in all directions
  • In the solid state, the ions build up into a giant ionic lattice
  • Ions are closely packed in a regular lattice arrangement
46
Q

Describe the arrangement of ions in the ionic lattice of Sodium Chloride

A
  • Regular cubic arrangement of Na⁺ and Cl⁻ ions
  • Each Na⁺ ion is surrounded by 6 Cl⁻ ions
  • Each Cl⁻ ion is surrounded by 6 Na⁺ ions
47
Q

What are the properties of ionic compounds

A
  • Solid at room temperature
  • High melting and boiling points
  • Tend to dissolve in polar solvents such as water
  • Conduct electricity only when molten or in aqueous solution (not when solid
48
Q

Why are ionic compounds solid at room temperature

A

At room temperature there isn’t energy to overcome electrostatic attractive forces between cations and anions in the giant ionic lattice

49
Q

Why do ionic compounds have high melting and boiling points

A
  • Large electrostatic attractive forces between cations and anions in the giant ionic lattice
  • High temperatures are needed to provide the energy required to overcome these forces
  • Therefore most ionic compounds have high melting and boiling points
50
Q

What 2 factors affect melting and boiling point of ions

A
  • Ionic charges
  • Size of ions
51
Q

How does the ionic charge affect the strength of the bond

A

The strength of the ionic bond increases when the charge on the ions increases

52
Q

How does the sixe of the ions affect the strength of the bond

A

The strength of the ionic bond increases when the size of the ions decreases

53
Q

Do ionic compounds tend to dissolve in polar solvents such as water

A

Yes

54
Q

Can ionic compounds conduct electricity in solid state

A

No

55
Q

Why can’t ionic compounds conduct electricity in solid state

A
  • Ions held in fixed positions in giant ionic lattice
  • No mobile charge carriers
  • No electrical conductivity
56
Q

Why can ionic compounds conduct electricity in liquid or aqueous state

A
  • Ions are free to move
  • Ions are mobile charge carriers
  • Electricity is conducted
57
Q

What is an element

A

A substance made up of only one type of atom

58
Q

What is a compound

A

A substance consisting of two or more elements chemically bonded together

59
Q

What is a molecule

A

A group of atoms covalently bonded together

60
Q

What is covalent bonding

A

Covalent bonding is the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

61
Q

Where can covalent bonding occur

A
  • Non metalic elements
  • Compounds of non-metalic elements
  • Polyatomic ions
62
Q

What is a covalent bond

A

the overlap of atomic orbitals, each containing one electron, to give a shared pair of electrons

63
Q

Show the displayed formula of a hydrogen molecule

A

H — H

64
Q

Is a covalent bond localised

A

Yes

65
Q

Where is a covalent bond localised

A

The electrostatic attraction is localised and is solely between the shared pair of electrons in the covalent bond and the nuclei of the bonding atoms

66
Q

True or False:

An ion attracts oppositely charged ions in all directions resulting in a giant ionic lattice

A

True

67
Q

What is a shared pair of electrons called

A

A shared pair of electrons is called a bonded pair of electron

68
Q

What is a pair of non-bonding electrons called

A

A pair of non-bonding electrons is called a lone pair of electrons

69
Q

How many covalent bonds can an atom of each element form:

Hydrogen
Oxygen
Nitrogen
Carbon

HONC

A

Hydrogen - 1
Oxygen - 2
Nitrogen - 3
Carbon - 4

70
Q

When can an expansion of the octet occur

A

From n=3 when a d-sub-shell becomes available

71
Q

What is a double covalent bond

A

The electrostatic attraction is between two shared pairs of electrons and the nuclei of the bonding atoms

72
Q

What is a triple covalent bond

A

The electrostatic attraction is between three shared pairs of electrons and the nuclei of the bonding atoms

73
Q

What is a dative covalent bond

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only. Shown as an arrow, with the arrow pointing away from the atom that contributes both electrons

74
Q

Give an example of an ion containing dative covalent bonds

A

NH₄⁺

Chemistry (16 decks)

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