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a level chemistry > module 2 section 2 - electrons, bonding and structure > Flashcards

module 2 section 2 - electrons, bonding and structure Flashcards

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1
Q

Do you think it 1s possible for electrons in the first shell to swap with elections in the second shell-explain your answer (3)

A
  • no
  • as each electron shell has a different energy level
  • amount of energy needed to transfer an electron from 1 electron shell to another is far too large
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2
Q

What are main energy levels called (l)

A

Principle energy levels

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3
Q

What is the number given to each energy level called (1)

A

Principle quantum number (n)

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4
Q

What is the lowest energy level

A

N=1

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5
Q

How many sublevels are in shell n= 1

A

1

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6
Q

What type af sub-shell is present in n=1

A

1s

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7
Q

How many electrons are found in the 1s subshell

A

2

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8
Q

What is the maximum number of electrons in n= 1

A

2

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9
Q

What sub-shells are present in n=2

A

-2s
- 2p

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10
Q

How many electrons can be in the 2s subshell

A

2

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11
Q

How many electrons can be held in the 2p subshell

A

6

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12
Q

What is the maximum number of electrons in shell n=2

A

8

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13
Q

What type af subshells are found in shell n= 3

A

. 3s
-3p
- 3d

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14
Q

How many electrons can be held in 3s

A

2

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15
Q

How many an electrons can be held in 3p

A

6

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16
Q

How many elections can de held in 3d

A

10

17
Q

How many electrons can the shell n=3 hold

A

18

18
Q

What sub levels are present in the shell n=4

A

•4s
• 4p
.4d
-4f

19
Q

How many electrons can 4s hold

A

2

20
Q

How many electrons can 3p hold

A

6

21
Q

How many electrons can 4d hold

A

10

22
Q

How many electrons can 4f hold

A

14

23
Q

How many electrons can be held in the shell n=4

A

32

24
Q

How many electrons can an atomic orbital hold?

A

2

25
Q

Describe the shape of the s-atomic orbital

A
  • Spherical shape
26
Q

Describe who the s-orbital increases un size

A

. When quantum number increases

27
Q

Describe the shape of the p-atomic orbital

A

Dumbbell shape

28
Q

Describe the trend of electronic configuration as you move along group 4 in the d-block (2)

A
  • Number of electrons in 3d increases by 1
    -Except chromium and copper are anomalous
29
Q

What is the electronic configuration of chromium

A

1s2. 2s2. 2p6. 3s2. 3p6. 4s1. 3d5.

30
Q

What is the electronic configuration of copper

A

1s2 2s2. 2p6. 3s2. 3p6. 4s1. 3d10

31
Q

Explain which orbitals d-block elements fill electrons., and remove electrons (2)

A

The 4s orbital

32
Q

Describe why electrons in an orbital must have opposite spins (2)

A
  • To counteract repulsion
  • between negatively charged electrons
33
Q

Explain why the 4s orbital is always filed before the 3d orbital (1)

A
  • because it has a lower energy level
34
Q

why do ionic compounds have giant ionic lattices (2)

A
  • oppositely charged ions interact with eachother
  • in all directions
35
Q

describe the solubility of ionic compounds (2)

A
  • soluble in polar solvents such as water
  • ions in ionic compounds can interact with polar water mlcl
36
Q

compare the solubility of an ionic compound containing Mg2+ and a different ionic compounds containing Na+ (3)

A
  • ionic compounds containing ions with higher charges (eg Mg2+) = less soluble
  • ionic compounds w ions w low charge (eg Na+) = more soluble
  • because electrostatic forces of attraction between ions = too strong for water to break down ionic lattic
37
Q

explain how sodium chloride dissolved in water (4)

A
  • before dissolving sodium and chloride ions held tightly together
  • due to string electrostatic forces of attraction
  • Na and all ions broken up by polar h20 mlcls
  • they interact with water mlcls
38
Q

describe the MP and BP of ionic compounds (3)

A
  • high MP + BP
  • strong electrostatic forces of attraction between opp charged ions
  • a lot energy needed to overcome
39
Q

describe and explain the electrical conductivity of ionic compounds (5)

A
  • poor as solid, good when dissolved in water or molten
  • poor as solid as ions fixed in position
  • so no mobile charge carriers
  • good when dissolved or melted and ionic lattice = broken
  • ions free to move as mobile charge carriers

a level chemistry (9 decks)

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