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

Unit 1 - chemical changes and structure Flashcards

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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

A

No

25
Q

What type of bonding stairs electrons

A

Covalent bond

26
Q

What type of bonding transfers electrons

A

Ionic bond

27
Q

If the electronegativity difference is zero what kind of bonding occurs

A

Pure covalent bonding or non-polar bonding

28
Q

What difference of electronegativity what cause polar covalent bonding

A

> 0<=2

29
Q

If a compound has an electronegativity greater than 2 what type of bond would be present

A

Iconic bonding

30
Q

Does the element with the higher or lower electronegativity pull the electron closer

A

Higher electronegativity

31
Q

What type of bonds are C-H always

A

Non-polar covalent

32
Q

What type of molecules are deflected by a charged rod

A

Polar molecules

33
Q

If all the bonds in a molecule are non-polar what type of molecule is it

A

Non-polar molecule

34
Q

What type of molecule is formed when there are polar bonds present and the molecule is symmetrical

A

Non-polar molecule

35
Q

What type of molecule is formed when there are polar bonds present and the molecule is non-symmetrical

A

Polar molecule

36
Q

Do polar molecules have high or low melting/boiling points

A

High

37
Q

What type of intermolecular forces are present in polar molecules

A

Permanent dipole to permanent dipole interactions

38
Q

Do non-polar molecules have high pr low melting/boiling points

A

Low

39
Q

What type of intermolecular forces do non-polar molecules have

A

London dispersion forces

40
Q

How do Vander Waal forces occur

A

When electrons in atoms move randomly around forming slight temporary dipoles

41
Q

When noble gases are in gas form is there an attraction between atoms

A

No, Van der Waal forces only from when gas is turned into a liquid

42
Q

Why does the boiling point increase as you go down the noble gas group

A
  • mass increases (atom gets bigger)
  • boiling point increases
  • due to stronger Van der Waal forces
43
Q

Intermolecular forces are the attraction between what

A

Attraction between molecules

44
Q

What are intramolecular forces

A

Holds atom together

Eg - polar covalent bonds

45
Q

What are the 3 types of intermolecular forces

A
  • london dispersion forces (LDF)
  • permanent dipole to permanent dipole interactions
  • hydrogen bonding
46
Q

What type of intermolecular force has the strongest strength

A

Hydrogen bonding

47
Q

What type of intermolecular force is the attraction between temporary dipoles

A

London dispersion forces

48
Q

What elements does hydrogen bond to for hydrogen bonding

A

N, O or F (Nandos On Friday)

49
Q

What causes more LDFs to be present

A
  • bigger molecule
  • more electrons
  • higher melting/boiling points
  • more LDF present
50
Q

What effect does hydrogen bonding have on a molecule

A
  • increased b.p/m.p
  • increased viscosity
  • increased solubility
51
Q

Why is ice less dense than water

A
  • hydrogen bonding

- causes ice to have an open/ expanded structure

52
Q

What forces are broken when a covalent molecule melts

A

Van der Waal forces

53
Q

What are ionic or polar molecules soluble in

A

Polar solvents (water)

54
Q

What are non-polar or covalent molecular molecules soluble in

A

Non-polar solvents (pentane)

55
Q

Are metals an covalent networks soluble or insoluble

A

Insoluble

Higher Chemistry (3 decks)

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