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HL Chemistry IB Revision
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Questions in this quiz (80)
1Check all reasons why the theoretical yield may not be accurate.
- ALoss of reactant/product
- BImpurities in reactants
- CToo much reactant added
- DIncomplete reaction
- EReaction is in equilibrium
2The Ideal Gas Laws
As pressure increases, volume [blank_start]decreases[blank_end] --> [blank_start]more[blank_end] collisions, less empty space
As temperature increases, volume [blank_start]increases[blank_end] --> [blank_start]more[blank_end] kinetic energy, particles move further
As temperature increases, pressure [blank_start]increases[blank_end] --> [blank_start]more[blank_end] kinetic energy, more collisions- Amore
- Bmore
- Cmore
- Ddecreases
- Eincreases
- Fincreases
3A real gas behaves most like an ideal gas at [blank_start]low[blank_end] pressure and [blank_start]high[blank_end] temperature because the particles are widely spaced, and are almost negligible volume.
A real gas behaves least like an ideal gas at [blank_start]high[blank_end] pressure and [blank_start]low[blank_end] temperature because the particles are close together and take up more volume - volume is [blank_start]greater[blank_end] than expected - and have stronger attractive forces - pressure is [blank_start]lower[blank_end] than expected.- Alow
- Bhigh
- Chigh
- Dlow
- Egreater
- Flower
4Relative atomic mass is the average mass of all the different isotopes of an atom
- ATrue
- BFalse
5Which color of visible light has the shortest wavelength and therefore the most energy?
- ARed
- BYellow
- CBlue
6Electromagnetic waves all travel at the same speed
- ATrue
- BFalse
7What is the speed of light?
[blank_start]3[blank_end].00 x 10^[blank_start]8[blank_end] m/s- A3
- B5
- C2
- D4
- E9
- F7
- G8
8When is an emission spectrum produced?
- AWhen an atom moves from a higher to a lower energy level
- BWhen an atom moves from a lower to a higher energy level
9What is the difference between a line spectrum and a continuous spectrum?
- ALine spectrum = discrete
Continuous spectrum = continuous energy levels - BLine spectrum = continuous
Continuous spectrum = discrete energy levels - CLine spectrum = shows energy changes
Continuous spectrum = does not show energy that atoms have absorbed
- ALine spectrum = discrete
10Which series is produced when electrons fall to the 2nd energy level, producing visible light?
- APaschen
- BLyman
- CBalmer
11Which series is produced when electrons fall from an excited state to the ground state, producing UV light?
- ALyman
- BBalmer
- CPaschen
12What is the transition that corresponds to ionization of an electron?
- A∞ --> 1
- B2--> ∞
- Coutermost level --> ∞
- D1 --> ∞
13What type of radiation is produced when the electron falls to the third energy level (n=3) in the Pachen series?
- AUV
- BInfrared
- CVisible light
14The energy in a photon of light emitted is equal to the energy change in an atom when an electron falls from an excited state.
- ATrue
- BFalse
15In an atomic orbital, what % chance is there of finding the electron?
- A85%
- B75%
- C100%
- D90%
16What is the correct order of electron orbitals/how many electrons does each contain?
[blank_start]s[blank_end] = 2
p = [blank_start]6[blank_end]
[blank_start]d[blank_end] = 10
f = 14- As
- Bp
- Cf
- D6
- E4
- F10
- G8
- Hd
- Ia
- Jb
17Which two elements below have 4s1 followed by a 3d orbital?
- AManganese and Sulfur
- BChromium and Copper
- CCopper and Sulfur
- DManganese and Chromium
18Effective nuclear charge is = number of [blank_start]protons[blank_end] - shielding [blank_start]electrons[blank_end]
- Aprotons
- Bneutrons
- Celectrons
- Dprotons
19Effective nuclear charge...
- Aincreases along a period, no change down a group
- Bincreases along a period, increases down a group
- Cdecreases along a period, no change down a group
- Ddecreases along a period, increases down a group
20Atomic radius...
- Adecreases across a period, increases along a group
- Bdecreases across a period, decreases along a group
- Cincreases across a period, decreases along a group
- Dincreases across a period, increases along a group
21For ionic radius...
- AIons in Groups 1-14 are smaller than their parent atoms, and ions in Groups 1-14 are larger than their parent atoms.
- BIons in Groups 1-14 are smaller than their parent atoms, and ions in Groups 1-14 are smaller than their parent atoms.
- CIons in Groups 1-14 are larger than their parent atoms, and ions in Groups 1-14 are larger than their parent atoms.
- DIons in Groups 1-14 are larger than their parent atoms, and ions in Groups 1-14 are smaller than their parent atoms.
22Ionization energies...
- Aincrease across a period and decrease down a group
- Bdecrease across a period and decrease down a group
- Cincrease across a period and increase down a group
- Ddecrease across a period and increase down a group
23"A measure of the ability of an atom to attract electrons in a covalent bond." This is...
- Aelectron affinity
- Bionization energy
- Celectronegativity
- Datomic radius
24Electron affinity of an atom is...
- Athe energy change that occurs when one mole of electrons is added to one mole of gaseous atoms
- Bthe enthalpy change that occurs when one mole of electrons is added to one mole of gaseous atoms
- Cthe energy change that occurs when an electron is added an atom
25Al2O3 is basic
- ATrue
- BFalse
26Check the properties of an ionic compound.
- AHigh melting point
- BLow melting point
- CHigh boiling point
- DLow boiling point
- E(generally) soluble in polar solvents
- F(generally) soluble in non-polar solvents
- GLow volatility
- HDo not conduct in solid state but conduct when molten or in aqueous solution
- IBrittle
27Which molecules commonly have an incomplete octet?
- ABeCl2
- BBF3
- CAl2O3
- DC2H6
- ENaOH
28Species with 2 electron domains are...
- Abent/v-shaped
- Btetrahedral shape
- Clinear
29Species with three electron domains and no lone pairs are:
- Atrigonal pyramidal
- Bbent/v-shaped
- Ctriangular planar
30Species with three electron domains and one lone pair are:
- Atriangular planar
- Bbent/v-shaped
- Ctrigonal pyramidal
31Name the molecular geometry.
Species with 4 electron domains and no lone pairs: [blank_start]tetrahedral[blank_end]
Species with 4 electron domains and one lone pair: [blank_start]trigonal pyramidal[blank_end]
Species with 4 electron domains and two lone pairs: [blank_start]bent/v-shaped[blank_end]- Atetrahedral
- Btrigonal pyramidal
- Cbent, v-shaped, bent/v-shaped
32Which allotropes of carbon are sp2 hybridized?
- Afullerene C60
- Bdiamond
- Cgraphite
- Dgraphene
33In Silicon Dioxide (SiO2), each silicon is bonded to x oxygens, and each oxygen is bonded to y silicons.
- Ax = 4
y = 2 - Bx = 2
y = 1 - Cx = 2
y = 4
- Ax = 4
34Dipole-dipole attraction occurs between [blank_start]permanent[blank_end] dipoles.
- Apermanent
- Btemporary
- Cinstantaneous
- Dinduced
35Hydrogen bonds occur when a hydrogen is bonded to an atom of:
- AFluorine
- BOxygen
- CNitrogen
- DCarbon
- EChlorine
36In a polar solvent, solubility of polar covalent molecules increases as the polarity increases
- ATrue
- BFalse
37Key terms to include in a definition of metallic bonding?
- AA lattice of positive ions
- Bin a sea of delocalised electrons
- Cstrong forces of attraction
- Dionic bonds between metals
38What are alloys?
- Asolid solutions
- Bmixtures
- Ccompounds
39Which atoms will form expanded octets?
- APeriod 1
- BPeriod 2
- CPeriod 3 or below
40Species with five electron domains have triangular bipyramidal electron domain geometry with bond angles at 90°, 120° and 180°.
However, their molecular geometry is different when there are lone pairs. Which ones are correct?- AAll bonded: triangular pyramidal
- BAll bonded: triangular bipyramidal
- C4 bonded, 1 lone pair: see-saw
90°, 117°, 180° - D4 bonded, 1 lone pair: bent/v-shaped
117° - E3 bonded, 2 lone pairs: T-shaped
- F3 bonded, 2 lone pairs: bent/v-shaped
- G2 bonded, 3 lone pairs: linear
- H2 bonded, 3 lone pairs: bent/v-shaped
41What is the electron domain geometry shape of a species with 6 electron domains?
- Aoctahedral
- Btetrahedral
- Chexahedral
42Ozone absorbs damaging UV-B and UV-C in the ozone layer. The wavelengths of light it absorbs (for dissociation into free radicals) is below (nm)
- A330
in the range of 200 to 315nm - B242
- C400
- A330
43An sp2 hybridized atom has 3 sp2 hybrid orbitals and 1 unhybridized s orbital
- ATrue
- BFalse
44sp hybrid orbitals form when an atom is triple bonded.
- ATrue
- BFalse
45Enthalpy (H) is a measure of the amount of [blank_start]heat[blank_end] energy in a substance, stored in teh [blank_start]bonds[blank_end] and [blank_start]intermolecular forces[blank_end]
- Aheat
- Bbonds, intermolecular forces
- Cintermolecular forces, bonds
46Standard Enthalpy Change of Combustion: enthalpy change for the [blank_start]complete[blank_end] combustion of [blank_start]one mole[blank_end] of a substance in [blank_start]excess oxygen[blank_end] under [blank_start]standard[blank_end] conditions
- Acomplete
- Bone mole
- Cexcess oxygen
- Dstandard
47The standard state of a substance is the [blank_start]pure[blank_end] form of the substance under [blank_start]standard[blank_end] conditions
- Apure
- Bstandard
48The unit of enthalpy is given in:
- AJ
- BkJ
- Ccal
- D°C
49When we do mc∆t, what do we assume?
- Ano heat loss from the system
- Ball heat goes from reaction to water
- Cthe solution is dilute
V(solvent) = V(water) - Dwater has a density of 1.00g cm-3
50Hess's law: the [blank_start]enthalpy[blank_end] change for any chemical reaction is [blank_start]independent[blank_end] of the route, provided the starting conditions and final conditions, and reactants and products, are the [blank_start]same[blank_end].
- Aenthalpy
- Bindependent
- Csame
51Standard enthalpy change of formation: the enthalpy change that occurs when [blank_start]one mole[blank_end] of a substance is formed from [blank_start]its elements[blank_end] in their [blank_start]standard[blank_end] states under [blank_start]standard[blank_end] conditions.
- Aone mole
- Bits elements
- Cstandard
- Dstandard
52bond enthalpy: energy needed to break [blank_start]one mole[blank_end] of bonds in [blank_start]gaseous[blank_end] molecules under [blank_start]standard[blank_end] conditions
- Aone mole
- Bstandard
- Cgaseous
53[blank_start]one mole[blank_end] of [blank_start]photons[blank_end] are needed to break one mole of bonds.
- Aphotons
- Bone mole
54first ionization energy corresponds to energy needed to form a [blank_start]positive[blank_end] ion
first electron affinity corresponds to energy needed to form a [blank_start]negative[blank_end] ion- Apositive
- Bnegatively charged
- Cpositively charged
- Dnegative
55lattice enthalpy is the enthalpy change that occurs when [blank_start]one mole[blank_end] of a [blank_start]solid[blank_end] ionic compound is separated into [blank_start]gaseous ions[blank_end] under [blank_start]standard[blank_end] conditions
- Asolid
- Bgaseous ions
- Cstandard
- Done mole
56The Born-Haber Cycle takes these steps
1. Enthalpy of [blank_start]atomization[blank_end] of reactants (normally just one as the other is gaseous already)
+ 2. Enthalpy of [blank_start]breaking[blank_end] bonds (of the other reactant which will probably be a diatomic molecule so x 0.5)
+ 3. Enthalpy of [blank_start]ionization[blank_end] of the cation (may need to go to 2nd)
+ 4. Enthalpy of [blank_start]affinity[blank_end] of the anion (may need to go to 2nd and normally -ve)
- 5. Enthalpy of formation of the products- Aatomization
- Blattice
- Cbreaking
- Dmaking
- Eionization
- Fseparation
- Gelectron affinity
- Hsublimation
57As ion radius increases, lattice enthalpy [blank_start]decreases[blank_end].
As ion charge increases, lattice enthalpy [blank_start]increases[blank_end].- Adecreases
- Bincreases
58Enthalpy change of solution: the enthalpy change when [blank_start]one mole[blank_end] of a [blank_start]solute[blank_end] is dissolved in a solvent to [blank_start]infinite[blank_end] dilution under [blank_start]standard[blank_end] conditions.
- Aone mole
- Binfinite
- Cstandard
- Dsolute
59Entropy is the distribution of available energy among the particles. An ordered state has a low entropy as there is low energy distribution. A disordered state has high entropy as there is a high degree of disorder.
What letter represents entropy?- AS
- BE
- CQ
- DM
60All states (except a perfect solid at 0°K) have positive entropy values.
- ATrue
- BFalse
61What is the correct order of the equation for ∆S(reaction)?
- AS(products) - S(reactants)
- BS(reactants) - S(products)
- CS(bonds formed) - S(bonds broken)
- DS(bonds broken) - S(bonds formed)
62What unit is ∆S (surroundings) in?
- AJ K-1 mol -1
- BJK mol -1
- CK mol J-1
- DJ-1 K-1 mol-1
63Well well well, its Gibbs Free Energy. I still don't know what that thing is, something to do with how much of the energy is able to do "useful" work. What is useful? What isn't?
All I know is that Gibbs Free Energy is useful because it can tell us whether or not a reaction is spontaneous, and whether or not it is possible. The definition of Gibbs is ∆G = ∆H - T∆S.
For a reaction to be spontaneous, Gibbs must be:- Anegative
- Bpositive
64What are some ways we can measure rate of reaction?
- AChange in volume of gas produced against time
- BChange in mass against time
- CChange in transmission of light: colorimetry
- DTitration, using quenching
- EConductivity changes (if ions change)
- FEndpoint reactions: timing until a certain point is reached
65Activation energy is the [blank_start]minimum[blank_end] value of [blank_start]kinetic energy[blank_end] which [blank_start]particles[blank_end] must have before they are able to react.
- Akinetic energy
- Bparticles
- Cminimum
66A catalyst modifies the collision geometry of the particles so they are more likely to react.
- ATrue
- BFalse
67Label the graph below showing the graphs for different orders of reaction.
- Arate vs time graph
- Bconcentration vs time graph
- Crate
- Dtemperature
- E1st order
- F2nd order
- G2 order
- H1 order
- Izero-order
- Jorder 0
- Kconcentration vs time
- Lrate vs time
- M0 order
- Nconcentration of reactant A
- Omass of reactant A
- Pfirst-order
- Qthird-order
- Rsecond-order
- S3rd order
68The rate determining step is the fastest step in the reaction.
- ATrue
- BFalse
69With a 10°C increase in temperature, there is always a doubling of rate of reaction.
- ATrue
- BFalse
70The value of A, the Arrhenius constant, indicates:
- Athe frequency of collisions and the probability they have proper orientations
- Bthe frequency of collisions
- Cthe probability the collisions have proper orientations
- Dthe activation energy of a reactant
71In a state of equilibrium, there is no [blank_start]net[blank_end] change in [blank_start]concentration[blank_end] of products and reactants in a closed system of dynamic [blank_start]forward[blank_end] and [blank_start]backward[blank_end] reactions
- Aconcentration
- Bnet
- Cforward
- Dbackward
72Which change in the system affects the Kc of the equilibrium?
- AChange in concentration of any reactant/product
- BChange in pressure/volume
- CChange in temperature
- DAddition of catalyst
73Le Chatelier's Principle: A system at equilibrium when subjected to a [blank_start]change[blank_end] will respond in such a way as to [blank_start]minimise[blank_end] the [blank_start]effect[blank_end] of the [blank_start]change[blank_end].
- Achange
- Bminimise
- Cchange
- Deffect
74Oh no, its Gibbs again. I knew he'd come back. This time he has made his way into equilibrium. Let's see... Gibbs says, a system has the highest possible value of entropy when free energy is at a minimum. THis is equilbrium.
Gibbs, I have no idea what that means, but all I have to know is the following true things:- AIf ∆G is large negative, there are more products at equilibrium
- BIf ∆G is large positive, there are more reactants at equilibrium
- CIf ∆G = zero, the concentrations are exactly the same.
- DIf ∆G is large negative, there are more reactants at equilibrium
- EIf ∆G is large positive, there are more products at equilibrium
75The equilibrium constant is the ratio of the rate constants of the forwards and backwards reactions.
- ATrue
- BFalse
76A Bronsted-Lowry acid is a proton (H+) acceptor
- ATrue
- BFalse
77Al2O3 (Aluminium Oxide) is amphiprotic.
- ATrue
- BFalse
78Salt: the [blank_start]ionic[blank_end] compound formed when the [blank_start]hydrogen[blank_end] of an acid is replaced by a [blank_start]metal[blank_end] or other [blank_start]positive[blank_end] ion
- Aionic
- Bhydrogen
- Cmetal
- Dpositive
79Enthalpy of neutralisation: enthalpy change that occurs when an [blank_start]acid[blank_end] and a [blank_start]base[blank_end] react to form [blank_start]1 mole[blank_end] of water. it is always [blank_start]exo[blank_end]thermic.
- Aacid
- Bbase
- C1 mole, one mole
- Dexo
80pH + pOH = 14.00 at 298K
- ATrue
- BFalse
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- Year 12 Chemistry Quiz on HL Chemistry IB Revision, created by Hazel S on 24/04/2017.
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- Hazel S
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