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CfE Higher Chemistry - Unit 1 Revision
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The anomalous density of ice (less than liquid water) is best described due to ...
 
Hydrogen bonding between molecules
 
Permanent dipole-permanent dipole attractions
 
The low polarity of the molecules
 
London dispersion forces
The melting point of group 0 elements increases down the group. This is because...
 
Temporary dipoles increase in strength
 
The atoms weigh more
 
The atoms become less reactive
 
Hydrogen bond increases
Which of these forces are weakest?
 
London dispersion
 
ionic bond
 
hydrogen bond
 
Permanent dipole - permanent dipole
Which of the following is least likely to dissolve in petrol (C8H16)?
 
NaCl
 
CO<sub>2</sub>
 
I<sub>2</sub>
 
C<sub>5</sub>H<sub>12</sub>
Which of the following compounds is likely to be most ionic?
 
Caesium fluoride
 
Lithium fluoride
 
Sodium fluoride
 
Potassium fluoride
Which of the following molecules are polar?
 
NH<sub>3</sub>
 
CO<sub>2</sub>
 
CH<sub>4</sub>
 
CF<sub>4</sub>
Which of the following does not contain pure covalent bonding?
 
hydrogen chloride
 
hydrogen
 
chlorine
 
nitrogen chloride
Elements with the lowest electronegativity are found ...
 
At the botttom left of the Periodic Table
 
At the top right of the Periodic Table
 
At the top left of the Periodic Table
 
At the bottom right of the Periodic Table
Which of the following does not increase across a period?
 
atomic size
 
nuclear charge
 
strength of London dispersion force
 
ionisation energy
The bonding and structure in the compound silicon dioxide is ....
 
covalent network
 
covalent molecular
 
metallic
 
monatomic
The bonding and structure in the element carbon (as graphite) is ....
 
covalent network
 
covalent molecular
 
metallic
 
monatomic
The bonding and structure in the element helium is ....
 
monatomic
 
covalent molecular
 
covalent network
 
metallic
The bonding and structure in the element tin is ....
 
metallic
 
covalent molecular
 
covalent network
 
monatomic
The bonding and structure in the element sulphur is ....
 
covalent molecular
 
covalent network
 
metallic
 
monatomic
An increase in temperature ....
 
increases the average kinetic energy of the reactants
 
increases the activation energy
 
increases the energy released in a reaction
 
lowers the activation energy
Which of the following is incorrect about the activation energy
 
it can sometimes be negative
 
it is the energy required to form the activated complex
 
it is lowered by the addition of a catalyst
 
it is the minimum kinetic energy needed to start a reaction
Exothermic reactions ...
 
always have a - enthalpy change
 
always have a + enthalpy change
 
are always reversible
 
are not reversible
The enthalpy change for a reaction is calculated from.....
 
the difference between the reactant and product energy
 
the difference between the reactant and highest peak energy
 
the difference between the product and highest peak energy
 
the energy of the highest peak
The activation energy for a reverse reaction is calculated from.....
 
the difference between the product and highest peak energy
 
the difference between the reactant and product energy
 
the difference between the reactant and highest peak energy
 
the energy of the highest peak
When reactants lose energy to form products, which of the following must be true?
 
the reaction is exothermic
 
the activation energy is high
 
the activation energy is very low
 
the reaction is endothermic
A chemical reaction had a relative rate of 0.25 min-1. How long did the reaction take to end?
 
4 mins
 
25 mins
 
0.25 mins
 
40 mins
An increase in which of the following will have the largest impact on reaction rate?
 
temperature
 
concentration
 
pressure
 
surface area
A chemical reaction took 10 seconds to end. The rate of this reaction is ...
 
0.1 s<sup>-1</sup>
 
10 s
 
0.1 s
 
10 s<sup>-1</sup>
Which of the following is required for a successful collision?
 
the correct geometry
 
a high concentration
 
energy lower than the activation energy
 
a large surface area
Which of following is not likely to have a significant effect on the rate of a reaction?
 
volume/mass of reactants
 
concentration of reactants
 
surface area of reactants
 
temperature of reactants
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