Inorganic memory module 3 Flashcards

1
Q

periodicity

A

The repeating trends in properties of the elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

First ionisation energy

A

The energy requires to remove one electron from ach atom of gaseous atoms of an elements to form one mole of gaseous 1+ ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What affects ionisation energy

A
  • atomic radius
  • electron sheildign
  • nuclear charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

metallic bonding

A

The strong electrostatic attraction between a metal cation and a sea of delocalised electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

disproportionation

A

a redox reaction in which the same element is both oxidised and reduced

e.g. Cl2(aq)+2NaOH(aq) –> NaClO(aq) + NaCl (aq) + H20(l)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Test for carbonates

A
  1. Add dilute nitric acid
  2. bubbles of C02 will be produced
  3. bubble through lime water to turn turn cloudy

CO3- + NO3- –> NO3- + C02 + H20

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Test for sulfate

A
  • add aqueous barium ions
  • formation of white precipitate of barium sulfate

Ba2+ + SO4^2- –> BaSO4 (s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Test for Halides

A
  1. Add aqueous silver nitrate to aqueous solution of halides
  2. form silver halide precipitations (white, cream and yellow)
  3. Add aqueous ammonia to test solubility

Ag+ + X- –> AgX (s)

chlorine - white, soluble in dilute NH3
Bromide - cream, soluble in concentrated NH3
Iodide - yellow, insoluble in concentrated NH3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Correct sequences of tests

A
  1. carbonate (no possibility of incorrect conclusions)
  2. sulfate (Carbonate with also produce what precipitate)
  3. halide (from silver carbonate and silver sulfate will not form precipitates)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Enthalpy

A

The measure of heat energy in a chemical system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

calculation for enthalpy change

A

^H = H (Products) - H(reactants)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Standard cons

A
  • 298 k
  • 100 kPa
  • 1.00 mol dm-3
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

The standard enthalpy change of reaction

A

^rH > the enthalpy change that accompanies a reaction in the molar quantities shown in the chemical equation under standard conditions, with all reactant and products in their standard conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

The standard enthalpy change of formations

A

The enthalpy changes that takes place when one mole of a compound is formed from is constituent elements, under standard conditions, with all reactant and products in their standard conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

The standard enthalpy change of combustion

A

The enthalpy change that accompanies the change that takes place when 1 mole of substance reacts completely with oxygen. Under standard conditions, with all reactant and products in their standard conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

The standard enthalpy change of neutralisation

A

The enthalpy changes the accompanies the reaction of an acid by a abase to form one mole of H20 (l). Under standard conditions, with all reactant and products in their standard conditions

17
Q

Specific heat capacity

A

energy required to raise the temperature of 1g of a substance by 1K

18
Q

calculate energy changes

A

q (joules)= mc^T
m = mass
c = water density

19
Q

Why is experimental ^cH values inaccurate

A
  • heat loss to the surroundings other then water
  • incomplete combustion
  • evaporation of alcohol from the wick
  • non-standard conditions
20
Q

Average bond enthalpies

A

The energy required to break one mole of a specific type of bond in a gaseous molecule (always endothermic)

enthalpy changes (^rH) = total bond enthalpy of reactants - total bond enthalpy of products

21
Q

limitation to bond enthalpy

A
  • only average used meaning the actual quantity would be variable
  • all species need to be gaseous molecules (so not standard enthalpy change calculated)
22
Q

Hess’ law

A

If a reaction can take place by two routes, and the starting and finishing conditions are the same the total enthalpy change in the same for each route

23
Q

Rate od a chemical reaction

A

measures how fast a reactant is being used or how fast a product is being formed.

rate = change in conc/time

24
Q

catalyst

A

a substance the increases the rate of a chemical reaction by providing an alternative reaction route with a lower activation energy, without a permeant change to itself
- homogenous (forms an immediate)
- heterogenous (provides a surface on which the reaction can take place)

25
Q

dynamic equilibrium

A
  • rate of froward and backward reaction equal
  • concentration of reactants and products do not change
26
Q

le chapeliers principale

A

when as system in equilibrium is subjected to an external change the system readjusts itself to minimise the effects of that change