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Unit 5 (Chem) - THE MAIN QUIZ (ADAPTIVE)

Total questions: 72

Worksheet time: 40mins

Name
Class
Date
1.
What is organic chemistry?
a)
chemistry relating to biological organisms
b)
chemistry involving carbon 
c)
chemistry involving micro-organisms
d)
chemistry involving oxygen
2.

Two types of hydrocarbons are ________

a)

saturated & unsaturated

b)

saturated & supersaturated

c)

polar & non-polar

d)

saturated & polysaturated

3.

What is the condensed formula of this structure?

a)

CH3CH2CH2OH

b)

CH3COCH3

c)

CH3CH2CHO

d)

CH3OCH2CH3

4.

How many hydrogens are missing from this extended structural formula?

a)

6

b)

7

c)

8

d)

9

5.

Name this compound

(a)  

6.

Name this compound

a)

propan-1-ol

b)

2-methlypropan-2-ol

c)

Propan-2-ol

7.

Fill in the blank for Free Radical Substitution:


Initiation >>> (a)   >>> Termination

8.

Free Radical: an uncharged molecule (typically highly reactive and short-lived) having an unpaired (a)  

9.

What does the "half-headed curly arrow" represent in chemistry?

a)

The movement of 2 electrons

b)

The movement of 1 electron

c)

The movement of a molecule

d)

The movement of a proton

10.
What is electrolysis?
a)
breaking down of a compound using a current
b)
making a compound using a current
11.
What is the name of the positive electrode?
a)
cathode
b)
anode
12.

Which is not a reason that cryolite is used in aluminum extraction?

a)

Cryolite dissolves aluminum oxide

b)

Cryolite reduces the melting point of aluminum oxide

c)

Cryolite decreases the cost of aluminum extraction

d)

Cryolite removes impurities from aluminum oxide

13.

What is the name of the ore that contains aluminum

a)

Bauxite

b)

Cryolite

c)

Aluminum oxide

d)

Heamatite

14.

The anode has to be replaced frequently in electrolysis of alumina because....

a)

The oxygen reacts with the carbon anode to form carbon dioxide

b)

Aluminum reacts with the carbon to form aluminum carbide

c)

The anode gets impurities that impact the extraction

d)

The anode is too hot and it will reduce their electrical conductivity

15.

Choose the half-equation that shows the discharge of aluminium ion.

a)

Al3+ - 3e- --> Al

b)

Al2+ + 3e- --> Al

c)

Al3+ + 3e- --> Al

d)

Al3+ --> Al + 3e-

16.
Describe oxidation in terms of electrons
a)
oxidation is gain of electrons
b)
oxidation is loss of electrons
17.

Which word matches this definition "a molecule or other species which can donate a proton (H+) or accept an electron pair in reactions"?

a)

Base

b)

Alkali

c)

Acid

d)

Amphoteric

18.

Which word matches this definition "a molecule or other species which can accept a proton or donate an electron pair in reactions"?

a)

Base

b)

Alkali

c)

Acid

d)

Amphoteric

19.

Which word matches this definition "a soluble substance which can accept a proton or donate an electron pair in reactions"?

a)

Base

b)

Alkali

c)

Acid

d)

Amphoteric

20.

Which word matches this definition "a molecule or other species which can accept a proton or donate a proton"?

a)

Base

b)

Alkali

c)

Acid

d)

Amphoteric

21.

Acids dissociate in water. Which equation below shows the correct dissociation for hydrochloric acid?

a)

HCl (aq) --> H (aq) + Cl (aq)

b)

HCl (aq) --> H+ (aq) + Cl+ (aq)

c)

HCl (l) --> H+ (aq) + Cl- (aq)

d)

HCl (aq) --> H+ (aq) + Cl- (aq)

22.

H+ (aq) + OH- (aq) --> H2O (l)


This ionic equation represents what process/reaction?

a)

Combustiion - Acid and an Alkali

b)

Neutralisation - Acid and an Alkali

c)

Neutralisation - Acid and a solid base

d)

Neutralisation - Base and an Alkali

23.

Which of the following is an amphoteric substance?

a)

HCl

b)

NaOH

c)

KOH

d)

Al2O3

24.

The oxide of a metal was found to react both with hydrochloric acid and with sodium hydroxide solution. Which one of the following is the best description of the oxide?

a)

acidic

b)

basic

c)

neutral

d)

amphoteric

25.

Some industrial companies use a specific chemical for effluent treatment - a process which neutralises acidic waste. What chemical is this?

a)

H2SO4

b)

HCl

c)

Ca(OH)2

d)

Al

26.

The transition elements form a ________ of about 30 Metals in the________ of the Periodic Table.

a)

Block & catalysts

b)

Block & Middle

c)

Catalysts & Coloured

d)

High & Middle

27.

Which block on this periodic table represents the transition metals?

a)

s block

b)

d block

c)

p block

d)

f block

28.

Which of the following best explains the action of a transition element as homogeneous catalyst?

a)

It decreases the enthalpy of reaction

b)

It exhibits a variable oxidation states

c)

It supplies energy to increase the rate of effective collision

d)

It supplies electrons to facilitate adsorption through the formation of temporary bonds

29.

Choose the statement that defines transition elements correctly.

a)

A transition element is one that forms cations with a completely filled d-subshell of electrons

b)

A transition element is one that forms at least one compound with a partially filled d-subshell of electrons

c)

A transition element is one that can speed up then the rate of chemical reactions in industrial processes

d)

A transition element is one whose compounds dissolve in water to form aqueous solutions which are colored

30.
Transition elements show variableoxidation state due to
a)
small size
b)
unpaired electron
c)
incomplete d orbital
d)
none of these
31.

What is a ligand

a)

An atom, molecule or ion that forms a dative covalent bond to a central metal ion in a complex.

b)

An atom, molecule or ion that accepts a pair of electron from a central metal ion in a complex.

c)

A central metal ion with one or more covalent bonds to it

d)

A d-block element that has a partially filled d subshell

32.

Transition metals are added in small amounts to speed up the rate of some chemical reactions. They make them happen quicker but are not used up themselves. What are the transition metals being?

(a)  

33.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
34.

if less heat energy is released in making bonds in the products than is taken in when breaking bonds in the reactants

a)

Endothermic

b)

Exotermic

c)

Exothermic

d)

Entrothermic

35.

Endothermic:_________:__________

Exothermic:_________:__________

a)

positive:warm

negative:cold

b)

positive:warm

negative:warm

c)

positive:cold

negative:cold

d)

positive:cold

negative:warm

36.
Define 'Enthalpy'
a)
a) Energy stored in the movement of molecules in a substance
b)
b) The opposite of temperature
c)
c) The temperature of a molecule
d)
d) Energy stored in the chemical bonds in a substance
37.

Match the definition below to the correct term.

The enthalpy change that takes place when one mole of a compound is formed from its elements in their standard states under standard conditions.

a)

The enthalpy of neutralisation

b)

The enthalpy of combustion

c)

The enthalpy of formation

d)

The enthalpy of reaction

38.

What does the circle mean in ΔH°?

a)

Standard Conditions (T=298.15 K P=1 atm)

b)

Standard Temperature and Pressure (T=273.15 K P=1 atm)

c)

Degree K

d)

Degree C

39.

Define standard enthalpy of combustion.

a)

Heat released when one mole of substance is burnt completely in excess oxygen.

b)

Heat absorbed when one mole of substance is burnt completely in excess oxygen under standard state.

c)

Heat released when one mole of substance is burnt completely in excess oxygen under standard state.

d)

Heat change when one mole of substance is burnt partially in excess oxygen under standard state.

40.

Which of the equation below refers to the standard enthalpy of formation, ΔHfo?

a)

Na(g) ---> Na+(g) + e- ΔH = -364 kJmol-1

b)

C2H5OH(l) + 3O2(g) ---> 2CO2(g) + 3H2O (l) ΔH = - 1286 kJmol-1

c)

2C(s) + 2H2(g) ---> C2H4 (g) ΔH = - 52.3 kJmol-1

d)

Na+(g) ---> Na+(aq) ΔH = - 364 kJmol-1

41.

Using the equation q = mcΔT, calculate the energy change (J) for the following reaction. 100g of water. Butane is burned underneath. Start temp = 298K; End temp = 318K


Assume c = 4.18J/K/g. Also give your answer a postive or negative sign.

Decide whether your answer should

(a)  

42.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

43.

The minimum amount of energy needed for colliding particles to react is called the

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

44.

Which of the following transition elements is used as a catalyst in Haber’s process?

a)

Fe

b)

Ni

c)

Ti

d)

V

45.

Select all the correct terms linked to catalysts

a)

Speed up reaction

b)

Lower the activation energy required

c)

Provide an alternative reaction pathway

d)

They are re-usable

e)

They are always white in colour

46.

What is being represented in stage 1?

a)

Adsorption

b)

Reaction

c)

Desorption

47.

What is being represented in stage 2?

a)

Adsorption

b)

Reaction

c)

Desorption

48.

What is being represented in stage 3?

a)

Adsorption

b)

Reaction

c)

Desorption

49.

Convert

 0oC0^oC  to Kelvin

a)

 −273 K-273\ K  

b)

 273 K273\ K  

c)

 32 K32\ K  

d)

 −32 K-32\ K  

50.

Convert

 0 K0\ K  to Celsius

a)

 273oC273^oC  

b)

 −273oC-273^oC  

c)

 32oC32^oC  

d)

 −32oC-32^oC  

51.

Convert

 0 K0\ K  to Celsius

a)

 273oC273^oC  

b)

 −273oC-273^oC  

c)

 32oC32^oC  

d)

 −32oC-32^oC  

52.

What is the boiling point of water on the Kelvin scale?

a)

 0K0^{ }K 

b)

 373K373^{ }K 

c)

 100K100^{ }K 

d)

 212K212^{ }K 

53.

The enthalpy change when 1 mole of a compound is completely burned in excess oxygen forming combustion products in their standard states. This is the enthalpy of ....

a)

Combustion

b)

Formation

c)

Ionisation

d)

Atomisation

54.

C (g)+ O2 (g)--> CO2 (g)

a)

Ionisation

b)

Combustion

c)

hydration

d)

solution

55.

Why is the enthalpy change of combustion, ΔHC, always negative?

a)

This is because the reaction is exothermic - more energy is given out creating new bonds in products than is taken in breaking the old bonds in the reactants

b)

This is because the reaction is exothermic - less energy is given out creating new bonds in products than is taken in breaking the old bonds in the reactants

c)

This is because the reaction is endothermic - more energy is given out creating new bonds in products than is taken in breaking the old bonds in the reactants

d)

This is because the reaction is endothermic - less energy is given out creating new bonds in products than is taken in breaking the old bonds in the reactants

56.

The enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions. This is the enthalpy of.....

a)

Combustion

b)

Formation

c)

Lattice breaking

d)

Ionisation

57.

½ H2 (g) + ½ Cl2 (g) --> HCl (g)

a)

Formation

b)

Combustion

c)

Atomisation

d)

Ionisation

58.

The enthalpy change when 1 mole of aqueous ions is formed from gaseous ions

a)

Formation

b)

Combustion

c)

Hydration

d)

Lattice breaking

59.

Na+ (g) + Cl- (g) --> Na+ (aq) + Cl- (aq)

a)

Formation

b)

Solution

c)

Combustion

d)

Hydration

60.

Why is the enthalpy change of hydration, ΔHC, always negative?

a)

This is because the reaction is exothermic - lots of energy is released when the polar water molecules form attractions/bonds to the positive and negative ions on the substance

b)

This is because the reaction is endothermic - not much energy is released when the polar water molecules form attractions/bonds to the positive and negative ions on the substance

61.

Hess's Law states that...

a)

all reactions are reversible

b)

the enthalpy change of a reaction is independent of the route taken (I.e. Route 1 = Route 2)

c)

the direct route results in a greater enthalpy change

d)

the indirect route results in a lower enthalpy change as energy is lost in the second step

62.

Hess' Law makes use of which principle to calculate the enthalpy change of a reaction?

a)

The law of conservation of energy

b)

The law of conservation of matter

c)

The law that you will always find a lost item in the last place you look for it

d)

Murphy's law

63.

Elements in their standard state always have standard enthalpies of ________.

a)

-396 kJ/mol

b)

33.2 kJ/mol

c)

0.0 kJ/mol

d)

396 kJ/mol

64.

Calculate ΔH


(don't include units - they are assume to be kJ/mol)

(a)  

65.
Bond angle for trigonal planar
a)
120o
b)
109.5o
c)
104.5o
d)
107o
66.
Bond angle for tetrahedral
a)
120o
b)
109.5o
c)
104.5o
d)
107o
67.
Bond angle for linear
a)
120o
b)
109.5o
c)
180o
d)
107o
68.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

69.

What is the hybridization of this molecule shown.

a)

sp

b)

sp2

c)

sp3

d)

sp4

70.

What is the hybridization of the Carbon atom indicated by the arrow?

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

dsp3 hybridization

71.

Which of the following images represents a Trigonal Planar molecular geometry?

a)
b)
c)
d)
72.

What is the bond angle for the CH4 molecule?

a)

120°

b)

107°

c)

109.5°

d)

90°

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