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Chem Exam Qs > E/P Qs > Flashcards

E/P Qs Flashcards

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1
Q

What is an orbital

2

A

Region of space around nucleus that can hold up to 2 electrons with opposite spins.

Strictly this

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2
Q

Which block of periodic table would you find nickel or copper

A

D block

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3
Q

Structure and bond in SiO2

A

Giant covalent structure and single covalent bonds

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4
Q

What is the term given to the “ . x H2O” in a crystallised salt

A

Water of crystallisation

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5
Q

What is the relative mass of an electron

A

Negligible or 1/2000

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6
Q

What is meant by the term mole

A

Amount of substance that has same number of particles as there are atoms in 12g of carbon 12/
Avogadro’s number

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7
Q

Reaction of magnesium with water balanced equation

A

Ca + 2H2O arrow Ca(OH)2 + H2

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8
Q

Molecular formula meaning

A

Number and type of atoms making up a molecule or the number of atoms of each element

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9
Q

Why does magnesium have higher mp than chlorine

Structure and bonding explanation
6 marks

A

Mg has giant structure, metallic bonding, electrostatic attraction between cations and electrons. Cl has simple molecular with van der waals forces (london forces) between molecules which require less energy to overcome than metallic bonds.

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10
Q

Suggest why H2S has lower bp than H2O

A

No hydrogen bonding

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11
Q

What is electronegativity

A

Attraction of an atom for electrons in a covalent bond

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12
Q

Explain why the bp increases from sodium(group 1, 11 electron) to aluminium( grp 3, 13 electron)

A

Number of delocalised electrons increases, cation charge increases and attraction increases/metallic bonding gets stronger

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13
Q

Describe the structure of NaCl

A

Giant ionic lattice with alternating Na+ and Cl-

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14
Q

Shape and angle of SO2
S has 16 electrons
O has 8

A

Non linear 117.5

Or in range from 110-130

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15
Q

Predict the bond angle in SbH3 Sb is grp 5 element along with N

A

107 cos 3bp 1lp

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16
Q

At room temp X, is a liquid that doesn’t conduct electricity

Bonding and structure ofX?

A

Simple molecular (covalent bonding)

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17
Q

Predict with reason the bond angle of ammonia

4 marks

A

107
Electron pairs repel other electron pairs
Lone pair has more repulsion
Electron pairs get as far apart as possible

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18
Q

Suggest why PH3 has a lower bp than NH3

A

PH3 has weaker intermolecular forces

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19
Q

What is meant by term isotopes

A

Atom(s) of an element with different number of neutrons (and with different masses)

Strictly this

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20
Q

Why do isotopes have same chemical properties

A

Same number of electrons in outer shell
Or same electron config
Or same electron structure

Strictly this!

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21
Q

Define relative atomic mass

A

The weighted ‘mean mass of an atom compared with 1/12 mass of a carbon 12’ atom

Strictly this

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22
Q

SbCl3 is polar
Why
2 marks

A

Difference in electronegativity or have a dipole

Molecule is not symmetrical so dipoles don’t cancel out

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23
Q

Why do all grp 7 elements react similarly to each other

A

Have same number of electrons in outer shell

Strictly this

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24
Q

Why does sodium oxide not conduct electricity when solid state

A

Ions are fixed in position in a lattice

Strictly this

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25
Why does first ionisation energy decrease from mg to al? Same period (2)
Mg electron removed from 3s and Al electron removed from 3p sub shell 3p has higher energy than 3s
26
How can GC-MS identify compound
GC separates the components and allows RF to be calculated and compared to data-books/ values and identify compound. Mass spectra allows fragment ions analysed
27
Why is TMS used in NMR
It is a standard which sample is compared to/reference
28
Why is deuterated solvents used in proton NMR
It has no H which would show up in H NMR as a peak
29
How use GC to predict compounds and relative proportion
From retention times and from their peak areas
30
Why would there be uncertainty about using GC alone to predict number of esters in mixture
Some have very similar retention times
31
Use of nmr in medicine Region of electromagnetic spectrum used in proton NMR
MRI scans Radio waves
32
Describe test to confirm carbonyl group and product identify carbonyl compound
2,4DNP and form orange precipitate Crystal melting point and compare to database and known values
33
What do curly arrows represent
Movement of an electron pair
34
Heterolytic fission?
Breaking of covalent bond And when one species takes both electrons
35
Number of stereoisomers the Ni (en)2 Cl2 can form
3 as 2 cis trans and one of cis is an optical isomer Be careful not to count optical and cis isomer twice
36
Tru/Fals? Abt transition element Element has atoms with partially filled d sub shell Multiple oxidation state in compounds Form coloured ions
F as it is not atom, it is its ions T T
37
Explain which block is sodium in
S block and highest energy electron in s sub shell
38
Why is lattice enthalpy of K2O less exothermic than Na2O K number is 19, Na atomic number is 11 (2)
Na has smaller atomic radius so nuclear attraction increases
39
Oxidation equation of alcohol to carboxylic acid
Alcohol + 2[O] —> carboxylic acid +H2O
40
How to recrystallise to obtain pure sample from impure (2)
Dissolve in MINIMUM quantity of HOT solvent Let it cool, filter and dry
41
Test for phenol
Add bromine and white precipitate or pH paper turns red but no reaction with carbonate
42
SF6 bond angle and shape
Octahedral 90
43
Which element react reacts with water to form an acidic solution
Cl As disproportionation as HCl and HClO formed
44
Why can in some cases kc calculated using number of moles rather than cOnc
Same volume cancels out or same number of moles in each side of equation
45
What technique to determine equilibrium amount of a weak acid
Titration
46
2 disadv and adv of fuel cells than fossil fuels (4)
Adv: only H2O formed so non polluting Greater efficiency Disadv: H2 difficult to store H2 difficult to manufacture/ limited life cycle of H2 absorber
47
Standard electrode potential? (3)
Potential difference of electrochemical cell comprising of a half cell combined with a standard hydrogen electrode 100kPa, 1M, 298K
48
Diagram on how to measure electrode potential of Cu half cell
Cu half cell with Cu ions and copper rod Attach to hydrogen half cell which is platinum electrode, H2 gas input, H+ solution 1M Salt bridge and voltmeter
49
Why is a polymer with C=O bond more likely to be degradeable (2)
C=O absorb radiation and breaks and ester link hydrolysed.
50
Explain process of addition polymerisation
Monomers with C=C High pressure and temp Pi bond breaks and many molecules join to form a long chain
51
Explain how en act as bidentate ligand (2)
Donates 2 lone pairs to metal ion Lone pair on N
52
Aq Cu2+ and NH3 Complex ion and colour
Blue [Cu (NH3)4(H2O)2]2+
53
What is an a (alpha) amino acid general formula
RCH(NH2)COOH The C is a chiral centre
54
Nitrobenzene to phenylamine Equation and conditions
Nitrobenzene + 6[H] —> phenylamine +2H2O Sn and conc HCl and excess NaOH Heat reflux
55
Entropy definition
Measure of dispersal of energy Or degree of disorder
56
Why is first ionisation energy of He and Be higher than Li He - 2 Li-3 Be-4 (4)
Electrons are in lower energy in He so greater nuclear attraction on outer shell electron Nuclear charge increase for Be so decrease in atomic radius
57
Explain why buffer solution formed
Acid is partially neutralised and A- ions produced
58
Why are operational conditions different in industry
High pressure expensive and dangerous but can increase yield Increase temp for faster rate of reaction but lower yield Catalyst reduce fuel expense and increase rate
59
2 observation that shows ca more reactive than mg when add water
Ca fizzes faster Ca dissolves quicker
60
Why does increasing temp increase rate of reaction (2)
Faster rate and more frequent collisions More particles have energy above Ea Strictly this
61
Average bond enthalpy
Enthalpy change/ energy required to break 1 mole of a specific covalent bond in gas phase
62
Describe and explain factors affecting value of Lattice enthalpy (3)
Decrease in ionic size and increase in charge so more negative LE and more attraction Attraction between ions
63
Explain why reaction happen spontaneously even if negative entropy change and negative enthalpy change (1)
Negative value of H more significant than negative value of tS
64
Explain difference in LE between NaF, NaCl and MgF2 (3)
Cl ion larger than F so smaller charge density mg2+ is smaller than Na+ and has greater charge F- greater attraction for cation Mg2+ greater attraction for anion
65
Explain in terms of kc why equilibrium yield of ammonia (product) increase as pressure increase (3)
Kc is same Increased pressure increases conc terms on bottom of kc expression more than top Top of kc expression increase and bottom decrease until kc reached
66
A solid organic compound purified by recrystallisation True/false Organic compound more soluble in hot solvent Hot solution cooled before pure organic compound collected MP of purified compound is lower than impure
True True False as mp of impure is lower and wider range
67
Iodine-sodium thiosulfate titration what indicator and colour change in end point
Starch Black to colourless
68
Test for ammonium ion
Add NaOH and then heat Gas produced and put near damp red litmus paper blue
69
How to store hydrogen in hydrogen fuel cell
Liquified under pressure
70
Two reasons why uncertain whether reaction predicted from E values may not take place (2)
Slow rate Conditions not standard
71
Standard solution preparation
Weigh out mass of solid Dissolve in small amount of distill water in beaker less than 250cm3 Transfer to 250cm3 volumetric flask and rinse beaker and add washings to volumetric flask Make up to the mark line and meniscus base is on line Mix by inverting the volumetric flask after putting stopper
72
Equation for lattice enthalpy of magnesium bromide
Mg2+ (g) + 2Br1(g) arrow MgBr2 (s)
73
Which type of reaction has highest atom economy Substitution Hydrolysis Elimination Addition
Addition
74
Which compound in water is most acidic Carboxylic acid or acyl chloride
Acyl chloride as cl can disproportionation with water and form HClO and HCl It is more reactive and acidic
75
Explain why reactive increases down grp 2 metals (3)
Atomic radius increase More shielding Nuclear attraction decreases Ionisation energy decreases
76
Enthalpy change of hydration (2)
1 mole of gaseous ions dissolve in water and form hydrated ions
77
Predict and explain enthalpy of hydration of F- and Cl- (2)
F- is more negative as F ion smaller size F ion has greater attraction to water
78
Average bond enthalpy (2)
Breaking of 1 mole of bond in gaseous molecule
79
Explain why difficult to predict whether enthalpy change of solution become more or less exothermic down group for magnesium halide (4)
Halide ion larger down grp LE less exothermic down grp Hydration enthalpy is less exothermic down grp Difficult to predict whether LE or hydration enthalpy has bigger effect
80
Bidentate ligand? (2)
Donates two lone pairs of electron and form 2 coordinate bonds to metal ion
81
1 important feature of fuel cell thats different from conventional storage cell (1)
Fuel react with oxygen to give electrical energy

Chem Exam Qs (1 decks)

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