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Chemistry > Module 2 - foundations of chemistry (year 1) > Flashcards

Module 2 - foundations of chemistry (year 1) Flashcards

Revise basic priciples of chemistry

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1
Q

What is the ideal gas constant?

A

8.31 J/mol K

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2
Q

Waht is Avogardo’s constent?

A

6.02x10^23

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3
Q

What is the bond angle and name of a molecule with:
2 Bone pairs
0 Lone pairs

A

Linear 180^o

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4
Q

What is the name and bond angle of a molecule with:
3 Bond pairs
0 Lone pairs

A

Trigonal planer 120^o

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5
Q

What is the name and bond angle of a molecule with:
4 bond pairs
0 lone pairs

A

Tetraheldral 109.5^o

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6
Q

What is the name and bond angle of a molecule with:
6 bone pairs
0 lone pairs

A

Octehedral 90^o

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7
Q

What is the name and bond angle of a molecule with:
3 bone pairs
1 lone pair

A

Triagonal Pyramidal 107^o

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8
Q

What is the name and bond angle of a molecule with:
2 bond pairs
2 lone pairs

A

Bent/ Non-linear 104.5^o

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9
Q

Define reletive isotopic mass

A

The mass of one isotope compared to 1/12 the mass of a carbon-12 atom

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10
Q

Define reletive atomic mass

A

The average mass of an atom compared to 1/12 the mass of a carbon-12 atom

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11
Q

Define reletive molecular mass

A

The average mass of a molecule compared to 1/12 the mass of a carbon-12 atom

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12
Q

What is the equation for reletive atomic mass

A

R.A.M = total(isotopic mass x % abundance)/100

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13
Q

Define a mole

A

The mass of a substance in grams, when there is the same number of atoms as the number of atoms in 12 grams of carbon-12

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14
Q

How do you calculate empirical formula?

A

1- divide each mass or mass percentage by their atomic mass
2- divide each number by the smallest number
3- (sometimes) multiply to make each number whole

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15
Q

How many electrons can a P orbital hold?

A

6 electrons

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16
Q

How many electrons can an S orbital hold?

A

2 electrons

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17
Q

How many electrons can a D orbital hold?

A

10 electrons

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18
Q

How many electrons can an F orbital hold?

A

14 electron

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19
Q

How many electrons can the second priciple energy level hold?

A

8 electrons

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20
Q

How many electrons can the third principle energy level hold?

A

18 electrons

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21
Q

How many electrons can the fourth principle energy level hold?

A

32 electrons

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22
Q

What are the limitations of the Octet rule?

A

It only applied to the first three periods

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23
Q

What is the Octet rule?

A

A theory that the shells of an atom can hold a maximum of 2,8,8 electrons respectively. This is actually the 1S orbital, 2S and 2P orbitals, then 3S and 3P orbitals.

24
Q

What is a spectator ion?

A

An ion which does not change state or oxidation number

25
Q

What does an ionic equation exclude?

A

Spectator ions

26
Q

What is the normal oxidation number of group 1 metals?

A

+1

27
Q

What is the normal oxidation number of a group 2 metal?

A

+2

28
Q

What is the normal oxidation state of Aluminium?

A

+3

29
Q

What is the normal oxidation number of Hydrogen?

What is the exception?

A

+1, unless in a metal hydride such as NaH

30
Q

What is the normal oxidation number of Fluorine?

What is the exception?

A

-1, flourine never has an exception

31
Q

What is the normal oxidation number of Bromine, Clorine and Iodine?
What is the exception?

A

-1, unless in a compound with Fluorine or Oxygen

32
Q

What is the normal oxidation number of Oxygen?

What is the exception?

A

-2, unless in a compound with Fluorine or in hydrogen peroxide (H2O2)

33
Q

How close do titre value have to be to be considered concordent results?

A

0.10cm^3

34
Q

How does too much indicator effect the titration?

A

The indicator contains a weak acid which slightly effects the ph of the solution. Only two to three drop should be used. Too much indicator would lead to slighlt lower titres (if the acid is in the burette).

35
Q

how does the jet effect the titration?

A

If the jet is not full then there will be a slightly higher titre than normal. The burette should be run with the acid or base to fill the jet.

36
Q

How do you wash the equitment before a titrtation?

A

Wash the conical flask with distilled water, the burette with the acid or base being used, and the other equipment with distilled water.

37
Q

How do you calculate %uncertainty?

A

%uncertainty = (uncertainty/average measurement) x100

38
Q

How do you calculate amount (mole)

A

mole(mol)= mass(g) / mr

39
Q

What is the name given to water in a crystal compound?

A

water of crystalisation

40
Q

How do you calculate concentration?

A

concentration (mol/dm^3) = amount (mol) / volume (dm^3)

41
Q

How do you calculate mass conentration?

A

mass concentration (g/dm^3) = mass (g) / volume (dm^3)

42
Q

What is the ideal gas equation?

A

PV=nRT

pressure (Pa) x volume (m^3) = amount (mol) x gas constent (JK^-1 mol^-1) x temperature (K)

43
Q

How do you convert celcius to kelvin?

A

+273

44
Q

How do you calculate atom econemy?

A

Atom econemy = (mass of usefull products / mass of reatents) x100

45
Q

Define an inoic bond?

A

The electrostatic attraction between tow oppersitely charged ions, formed by electron transfers.

46
Q

Define a covalent bond?

A

the electrostatic attraction between a shared pair of electrons and the nucli of the bonded atoms

47
Q

What is a dative bond?

A

A covalent bond, except all of the shared electrons come from one atom.

48
Q

What are the properties of a giant ionic lattice?

A

Good conductor of electricity but only when liquid
Good solubility in water
High boiling point
Usually crystal solids.

49
Q

What are the properties of simple covalent molecules?

A

poor eletrical conductivity
Poor solubility in water
Low boiling point
Usually a gas at room temperature

50
Q

What properties increase the atrractivity of a posetive ion?

A

Small atomic radius
Low sheilding
High nuclear charge

51
Q

What properties increase the attractivity of a negative ion?

A

Large atomic radius
High sheilding
Low atomic charge

52
Q

What increases the attractivity of a covalently bonded atom?

A

Low atomic radius
Low sheilding
High nuclear charge

53
Q

Define electonegativity

A

The relative tendancy of an atom in a covalent bond to attract electrons to itself.

54
Q

What factor effects induced dipole dipole forces (London forces)?

A

The more elctrons their are the stronger the dipoles become

55
Q

What does Van der waal’s forces reffer to?

A

Both induced and perminate dipole dipole forces

56
Q

What does a hydrogen bond form between?

A

A hydrogen atom and the lone pair of oxygen, fluorine or nitrogen.

Chemistry (2 decks)

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