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Higher Chemistry > Unit 1 - chemical changes and structure > Flashcards

Unit 1 - chemical changes and structure Flashcards

1
Q

How does particle size affect the rate of reaction

A
  • smaller particle size
  • larger surface area
  • increased successful collisions
  • faster rate
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2
Q

How does concentration affect reaction rate

A
  • higher concentration
  • more particles present in given volume
  • more successful collisions
  • faster rate
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3
Q

What causes particles to have an kinetic energy greater than or equal to the activation energy

A

Increase in temperature

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4
Q

How can a reaction be made more economical

A

Lower temperature and add a catalyst

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5
Q

Will adding a catalyst raise or lower the activation energy

A

Lower activation energy

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6
Q

How is the activation energy found from a potential energy diagram

A

From the reactant (R) to the peak of the graph

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7
Q

When calculating the potential energy of a reaction from a potential energy diagram how can you tell if reaction is exothermic or endothermic

A

Exothermic - negative value for H, R higher than P

Endothermic - positive value for H, P higher than R

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8
Q

How could the reverse reaction be found

A

By switching R and P around

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9
Q

What is the covalent radius

A

Measure of the size of an atom

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10
Q

What is ionisation energy

A

Energy required to remove one mole of electrons from one mole of gaseous atoms

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11
Q

What is electronegativity

A

The attraction an atom of an element has for bonding electrons

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12
Q

As you go across the periodic table why does covalent radius decrease

A
  • increased nuclear charge

- pulls electrons closer

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13
Q

Why does first ionisation energy increase as you go across the periodic table

A
  • increased nuclear charge
  • smaller radius
  • outer electrons more tightly held
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14
Q

Why does electronegativity increase as you go across the periodic table

A
  • increased nuclear charge
  • smaller radius
  • outer electrons more tightly held
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15
Q

As you go down the periodic table why does covalent radius increase

A

Increased number of electron shells

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16
Q

Why does first ionisation energy decrease as you go down the periodic table

A
  • increased number of shells
  • atom bigger
  • electrons further from nucleus
  • increased shielding effect by inner electrons
  • outer electrons less strongly held
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17
Q

Why does electronegativity decrease as you go down the periodic table

A
  • increased number of shells
  • atom bigger
  • electrons further from nucleus
  • increased shielding effect by inner electrons
  • outer electrons less strongly held
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18
Q

What is ionic bonding between

A

Metal + non-metal

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19
Q

Will ionic compounds conduct

A

Yes when in liquid or molten

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20
Q

What elements form a covalent network

A

Si, B, C

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21
Q

What type of bonding and structure forms between two non-metals

A

Covalent molecular

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22
Q

What are the boiling points of a metallic lattice like

A

Fairly high

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23
Q

What are the elements that form a monatomic structure

A

He, Ne, Ar

24
Q

Will monatomic compounds conduct

25
What type of bonding stairs electrons
Covalent bond
26
What type of bonding transfers electrons
Ionic bond
27
If the electronegativity difference is zero what kind of bonding occurs
Pure covalent bonding or non-polar bonding
28
What difference of electronegativity what cause polar covalent bonding
>0<=2
29
If a compound has an electronegativity greater than 2 what type of bond would be present
Iconic bonding
30
Does the element with the higher or lower electronegativity pull the electron closer
Higher electronegativity
31
What type of bonds are C-H always
Non-polar covalent
32
What type of molecules are deflected by a charged rod
Polar molecules
33
If all the bonds in a molecule are non-polar what type of molecule is it
Non-polar molecule
34
What type of molecule is formed when there are polar bonds present and the molecule is symmetrical
Non-polar molecule
35
What type of molecule is formed when there are polar bonds present and the molecule is non-symmetrical
Polar molecule
36
Do polar molecules have high or low melting/boiling points
High
37
What type of intermolecular forces are present in polar molecules
Permanent dipole to permanent dipole interactions
38
Do non-polar molecules have high pr low melting/boiling points
Low
39
What type of intermolecular forces do non-polar molecules have
London dispersion forces
40
How do Vander Waal forces occur
When electrons in atoms move randomly around forming slight temporary dipoles
41
When noble gases are in gas form is there an attraction between atoms
No, Van der Waal forces only from when gas is turned into a liquid
42
Why does the boiling point increase as you go down the noble gas group
- mass increases (atom gets bigger) - boiling point increases - due to stronger Van der Waal forces
43
Intermolecular forces are the attraction between what
Attraction between molecules
44
What are intramolecular forces
Holds atom together | Eg - polar covalent bonds
45
What are the 3 types of intermolecular forces
- london dispersion forces (LDF) - permanent dipole to permanent dipole interactions - hydrogen bonding
46
What type of intermolecular force has the strongest strength
Hydrogen bonding
47
What type of intermolecular force is the attraction between temporary dipoles
London dispersion forces
48
What elements does hydrogen bond to for hydrogen bonding
N, O or F (Nandos On Friday)
49
What causes more LDFs to be present
- bigger molecule - more electrons - higher melting/boiling points - more LDF present
50
What effect does hydrogen bonding have on a molecule
- increased b.p/m.p - increased viscosity - increased solubility
51
Why is ice less dense than water
- hydrogen bonding | - causes ice to have an open/ expanded structure
52
What forces are broken when a covalent molecule melts
Van der Waal forces
53
What are ionic or polar molecules soluble in
Polar solvents (water)
54
What are non-polar or covalent molecular molecules soluble in
Non-polar solvents (pentane)
55
Are metals an covalent networks soluble or insoluble
Insoluble

Higher Chemistry (3 decks)

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