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General Flashcards

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1
Q

What is the test for 3° alcohols to isolate them from 1 and 2

A

Add K2Cr2O7 (stays orange for 3°, 1° and 2° react so colour changes to green

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2
Q

Equation for enthalpy change of formation

A

(Sign) mass of Liquid x 4.18 x change in temp/1000 x lim moles

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3
Q

Define enthalpy change of formation

A

Enthalpy change when 1 mole of a substance is formed from its elements under standard conditions

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4
Q

Define Enthalpy change of combustion

A

Enthalpy change when one mole of a substance is completely combusted under standard conditions

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5
Q

Equation for enthalpy change of combustion

A

(Negative) (mass of H2O x 4.18 x change in temp)/(1000 x mol fuel)

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6
Q

Effect of ozone in stratosphere

A

Absorbs high energy UV

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7
Q

Effect of ozone in troposphere

A

Photochemical smog, respiratory problems

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8
Q

Physical properties of haloalkanes

A

Covalent bonding, simple molecular structure, usually liquid at RTP, don’t mix well with water

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9
Q

Group 2 physical properties

A

High mpt/bpt, density greater than group 1 elements

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10
Q

Group 2 reaction with water observations

A

Silver solid reacts with effervescence to produce cloudy solution (alkaline)

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11
Q

Group 2 oxides reaction with H2O?

A

Produces hydroxides

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12
Q

Acid + Base -> ?

A

Salt + Water

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13
Q

Group 2 trends down group

A

Solubility of Carbonates decreases, everything else increases (reactivity, thermal stability etc.)

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14
Q

How are emission spectra formed

A

Atom heated to high temperature, electrons excited to higher energy level, energy given out as em rad when electrons drop back down, rad passed through prism coloured lines seen

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15
Q

How are absorption spectra formed

A

White light passes through cooled sample of gas, energy absorbed to raise electrons to higher energy levels, rad passed through prism, black lines show missing frequencies

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16
Q

What shape are s and p orbitals

A

S - spherical, P - dumbbell shaped

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17
Q

What are subshells

A

Groups of orbitals of the same type

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18
Q

Define covalent bonding

A

Electrostatic attraction between shared pairs of electrons and two positive nuclei

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19
Q

Exceptions to covalent bonding rule

A

H forms 1 bond, Be forms 2 cov bonds, Al forms 3 cov bonds, S can form 2 or 6, P can form 3 or 5

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20
Q

Define metallic bonding

A

Electrostatic attraction between a lattice of positive ions and a sea of delocalised electrons

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21
Q

Define ionic bonding

A

Electrostatic attraction between ions of opposite charges

22
Q

What structure do ionic compounds have

A

Giant 3D lattice

23
Q

How do ionic compounds dissolve in water

A

Water molecules cluster around the ions, positive ions are attracted to O and negative ions attracted to H, water molecules overcome bonds in the compound and pull the ions apart

24
Q

Define stereoisomerism

A

Compounds with the same structural formula but with a different arrangement

25
Q

What are E/Z isomers

A

When there is no free rotation about the C=C bond, with two different groups attached to each C atom including one H on each carbon

26
Q

Conditions for cracking

A

500°c, Al2O3 catalyst, no O2

27
Q

How do homogenous catalysts work

A

Reactant gas absorbs on the catalysts surface
Bonds in reactant molecules are weakened and break
New product bonds form
The product molecules desorb from the surface

28
Q

Physical properties of alkanes

A

Low mpt/bpt
Insoluble in water
Soluble in organic solvents
Less dense than water

29
Q

Chemical properties of alkanes

A

Generally unreactive
Non polar
Strong C-C and C-H bonds

30
Q

How to balance half equations

A

Balance atoms other than O and H
Add H2O to balance O
Add H+ to balance H
Add e- to balance charge

31
Q

How do IdId bonds form

A

Electrons constantly moving
Causes uneven distribution of charge
Causes instantaneous dipole in 1
Induces other dipoles in neighbouring molecules

32
Q

What are PdPd bonds

A

Attraction between molecules with permanent dipoles
Only in polar molecules

33
Q

Which solvents do polar/nonpolar molecules dissolve in

A

Polar dissolves in polar
Nonpolar dissolves in nonpolar

34
Q

How do PdId bonds form

A

A permanent dipole can induce a temporary one in a species that is normally non polar such as HCl and Cl2

35
Q

What is Hydrogen Bonding

A

A type of strong PdPd bond
Electrostatic attraction between a very delta+ H atom and a LP of e- on a N O or F atom
Very high mpt bpt
Strength depends on electronegativity and number of H bonds

36
Q

What radiation does the sun emit

A

Mainly UV with some visible

37
Q

What is a nucleophile

A

A negative or partially negative species that forms a dative bond by donating a pair of electrons

38
Q

Define electronegativity

A

A measure of the ability of an atom to attract the bonding pair of electrons in a covalent bond to itself

39
Q

Solubility of Nitrates and Ethanoates

A

All are soluble

40
Q

Solubility of Sulphates

A

All soluble except
BaSO4, PbSO4, CaSO4

41
Q

Solubility of Halides

A

All soluble except
AgX and PbX

42
Q

Solubility of Carbonates

A

All insoluble except
Na, K, NH4

43
Q

Solubility of Hydroxides

A

All insoluble except
Li, Na, K, Ca

44
Q

Solubility of Oxides

A

All insoluble
Group 1 and 2 oxides react with water to form hydroxides

45
Q

Carbonate test

A

Add an acid, effervescence
Bubble gas through lime water
Goes from colourless to cloudy white

46
Q

Sulphate test

A

Nitric acid and Barium nitrate
White precipitate

47
Q

Halide ion test

A

Nitric Acid, Silver Nitrate
Cl- White Precipitate
Br- Cream precipitate
I- Yellow precipitate

48
Q

Physical properties of alcohols

A

Polar
Higher mpt/bpt than alkanes
Small alcohols are water soluble

49
Q

Define ionisation energy

A

Energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms

50
Q

What order should anion tests be carried out (Sulphate, Carbonate, Halide)

A

Carbonate
Sulphate
Halide

Chem (4 decks)

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