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A Level Chemistry > Chapter 5 - Electrons and bonding (MODULE 2) > Flashcards

Chapter 5 - Electrons and bonding (MODULE 2) Flashcards

(49 cards)

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1
Q

How many electrons can fit in the
- n=1
- n=2
- n=3
- n=4

shells

A
  • 2
  • 8
  • 18
  • 32
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2
Q

what are shell numbers called

A

principle quantum numbers ‘n’

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3
Q

What is an orbital

A

a region in space around the nucleus where there is a high probability of finding an electron

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4
Q

how many electrons can an orbital hold

A

2

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5
Q

What are the four types of orbital

A

s, p, d, f

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6
Q

What shape is an s orbital
- what is the relation between shell number and radius of s orbitals

A

sphere
- the greater the value of n, the greater the radius of the s orbital

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7
Q

What is the shape of a p orbital
- How many p orbitals are there per energy level
- What are they known as
- What is the correlation between shell number and distance from the nucleus for p orbitals

A
  • dumbell e.g. (8) or infinity symbol
  • 3
  • Px, Py, Pz
  • greater the value of n, the further from the nucleus
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8
Q

Fill the blanks

Each shell from n= __, contains ___ d- orbitals

A

3, 5

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9
Q

Fill the blanks

Each shell from n= __, contains ___ f- orbitals

A

4, 7

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10
Q

How many
- s orbitals
- p orbitals
- d orbitals
- f orbitals
- total electrons

are present in the n=1 shell

A
  • 1
  • 0
  • 0
  • 0
  • 2
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11
Q

How many
- s orbitals
- p orbitals
- d orbitals
- f orbitals
- total electrons

are present in the n=2 shell

A
  • 1
  • 3
  • 0
  • 0
  • 8
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12
Q

How many
- s orbitals
- p orbitals
- d orbitals
- f orbitals
- total electrons

are present in the n=3 shell

A
  • 1
  • 3
  • 5
  • 0
  • 18
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13
Q

How many
- s orbitals
- p orbitals
- d orbitals
- f orbitals
- total electrons

are present in the n=4 shell

A
  • 1
  • 3
  • 5
  • 7
  • 32
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14
Q

How do orbitals fill up (2)

A

in order of increasing energy
- within a subshell, one electron occupies each orbital before pairing starts

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15
Q

How do energy levels vary across subshells and shells

A

in a shell, s has least energy, then p, then d, then f
However 3d has higher energy than 4s, so 4s fills up first

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16
Q

Why are electrons drawn with arrows facing different directions

A

because they have opposite spins,

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17
Q

why do electrons in an orbital have opposite spins

A

to counteract the repulsion between their negative charges

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18
Q

Which columns are part of the
- ‘s’ block
- ‘p’ block
- ‘d’ block
- ‘f’ block

A
  • group 1 and 2
  • group 3-8
  • transition
  • transition
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19
Q

What are positive ions called
- how are they formed

A
  • cations
  • when atoms lose electrons
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20
Q

What are negative ions called
- how are they formed

Study These Flashcards
A
  • anions
  • when atoms gain electrons
21
Q

Which subshell do s-block atoms lose electrons from when becoming ions

22
Q

Which subshell do p-block atoms gain electrons to when becoming ions

23
Q

Which subshell do d-block atoms lose electrons from when becoming ions

24
Q

What is an ionic bond

Study These Flashcards
A

the electrostatic attraction between positive and negative ions

25
What happens during ionic bonding
electrons are donated from metals/ammonium to non-metals/polyatomic ions. Forming positive and negative ions
26
What structure is formed through ionic bonding
giant ionic lattice
27
What state are most ionic compounds at room temperature - why
solid - at room temp, there is insufficient energy to overcome strong electrostatic forces of attraction between oppositely charged ions
28
Why do ionic compounds have high melting and boiling points
lots of energy required to overcome strong electrostatic forces of attraction between ions
29
What type of substances do lots of ionic compounds dissolve in
polar solvents
30
Why are ionic compounds made of ions with large charges not very soluble
because electrostatic forces are stronger and may be too strong for the solvent to break down the lattice structure.
31
What factor does solubility of ionic compounds depend on
strengths of attractions within the lattice
32
What is the electrical conductivity of ionic compounds and why
solid: doesn't conduct - ions in fixed positions liquid and dissolved: conducts electricity - charged particles (ions) free to move and carry charge
33
What is a covalent bond
a strong electrostatic force of attraction between a shared pair of electrons and the nuclei of the bonded atoms
34
What type of substances do covalent bonds occur in
non metal - non metal compounds - polyatomic ions
35
What are the three types of structure for covalent bonds - give an example of each
small molecule, giant covalent structure, charged polyatomic ions - H2, SiO2, NH4+
36
What does localised mean in terms of covalent bonds
the bond acts solely between the shared pair and the nuclei of the two bonded atoms
37
what is a molecule
the smallest part of a covalent compound that can exist whilst retaining the chemical properties of the compound
38
what happens to electrons in ionic and covalent bonding
ionic - transferred covalent - shared
39
What does a displayed formula show
the relative positioning of atoms and the bonds between them as lines
40
What are paired atoms that aren't shared known as
lone pairs
41
Why can elements in the n=3 shell bond to have more than 8 electrons in the outer shell e.g. ClF5
because n=3 shell can have up to 18 electrons
42
In the reaction of sulfur and fluorine, what determines how many fluorines bind to each sulfur
the amount of outer shell sulfur electrons that are paired e.g. if 2 unpaired then 2 fluorines, all 6 unpaired then 6 fluorides
43
WHat is a double covalent bond
the attraction between two shared pairs of electrons and the nuclei of the bonded atoms
44
What is a triple covalent bond
the attraction between three shared pairs of electrons and the nuclei of the bonded atoms
45
WHat is a dative covalent bond - what is another name for this
when both of the shared pair come from a single atom, originally was a lone pair - coordinate bond
46
Where is the dative covalent bond in NH4+
when NH3 reacts with H+, and NH3 donates a lone pair to form the dative covalent bond
47
how is a dative covalent bond written in displayed formula
as a line with an arrow from donor pair to other pair
48
What is avergae bond enthalpy used as a measure of
a measure of covalent bond strength
49
What is the correlation between average bind enthalpy and bond strength
the greater the average bond enthalpy, the more energy needed to break it and therefore the stronger the bond

A Level Chemistry (16 decks)

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