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AS - Level Chemistry Quiz on Chemistry f321 quiz, created by rosieoj2 on 26/02/2015.

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Chemistry f321 quiz

Question 1 of 34

1

What did John Dalton NOT predict about the atom?

Select one of the following:

  • Atoms are tiny particles that make up elements

  • Atoms cannot be divided

  • Atoms have negative electrons which move around in a 'sea' of electrons

  • All atoms of a given element are the same

Explanation

Question 2 of 34

1

What is J J Thomson most famous for?

Select one of the following:

  • Working out the number of atoms in a mole

  • Discovering that cathode rays are made up of a stream of particles called electrons

  • Finding a law allowing people to indirectly determine the enthalpy change of a reaction

  • Shooting JFK

Explanation

Question 3 of 34

1

Who carried out the gold leaf experiment, in which alpha particles were fired at a thin sheet of gold foil?

Select one of the following:

  • Dalton

  • Hess

  • Rutherford

  • Bohr

Explanation

Question 4 of 34

1

Which of these are Rutherford's main conclusions from his experiment into the structure of the atom?

Select one of the following:

  • The positive charge and most of the mass of the atom are concentrated at the centre, in the nucleus
    Negative electrons orbit the nucleus
    Electrons follow only certain paths
    Most of the atom is made up of empty space

  • The atom is made up of negative electrons in a 'sea' of positive charge

  • Atoms cannot be divided
    Atoms are tiny particles that make up elements

  • The overall charge of an atom is 0
    electrons orbit the nucleus
    Most of the atom is empty space
    The positive charge and most of the mass of an atom is centred in the middle, in the nucleus

Explanation

Question 5 of 34

1

what is the relative mass of an electron?

Select one of the following:

  • 1

  • 2000

  • 1/2000

  • 1/20 000

Explanation

Question 6 of 34

1

what is the definition of an isotope?

Select one of the following:

  • atoms of the same element with different numbers of neutrons

  • atoms of the same elements with different numbers of protons

  • atoms with different mass numbers

  • atoms with the same charges

Explanation

Question 7 of 34

1

How many atoms are in one mole?

Select one of the following:

  • 6.02 x 10 to the power of 24

  • 2.06 x 10 to the power of 13

  • 6.02 x 10 to the power of 23

  • 6.03 x 10 to the power of 24

Explanation

Question 8 of 34

1

what is the definition of relative isotopic mass?

Select one of the following:

  • the weighted mean mass of an atom compared to one-twelfth the mass of an atom of carbon-12

  • the weighted mean mass of an atom compared to twelve grams of carbon-12

  • the mass of an isotope of an element compared to twelve grams of carbon -12

  • the mass of an isotope of an element compare to one -twelfth the mass of one atom of carbon-12

Explanation

Question 9 of 34

1

what is the definition of relative atomic mass?

Select one of the following:

  • the weighted mean mass of an atom of an element compared to one-twelfth the mass of an atom of carbon-12

  • the weighted mean mass of an atom compared to 12 grams of carbon-12

  • the mass of an atom compared to one -twelfth the mass of an atom of carbon-12

  • the mass of an isotope of an element compared to one -twelfth the mass of one atom of carbon 12

Explanation

Question 10 of 34

1

what is the definition of a mole?

Select one of the following:

  • the amount of any substance containing as many particles as there are carbon atoms in exactly 12 grams of the crabon-12 isotope

  • the mass of 6.02 x 10 to the power of 23 atoms

  • a small mammal adapted to a subterranean lifestyle

  • the number of atoms per mole in a compound

Explanation

Question 11 of 34

1

how do you find the number of moles in a substance?

Select one of the following:

  • mr divided by the mass

  • mass divided by the mr

  • mass times the mr

  • mr squared minus the mass

Explanation

Question 12 of 34

1

what do you need to do to find the empirical formula?

Select one of the following:

  • list the elements, the mr, then divide by the smallest

  • list the elements, the experimental masses, number of moles, divide mass by moles, divide by smallest

  • list the elements, the experimental masses, mr, divide mass by mr, divide by smallest

  • list all the elements, experimental masses, mr, divide by smallest

Explanation

Question 13 of 34

1

what does Avogadro's hypothesis state?

Select one of the following:

  • there are 6.02 times 10 to the power of 23 molecules in a mole

  • the mr is calculated by adding the ar of all the elements present in the compound

  • the volume of gas stays the same regardless of RTP

  • equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

Explanation

Question 14 of 34

1

what is the formula for calculating the number of moles present in a gas at RTP?

Select one of the following:

  • volume (dm cubed) divided by 24.0

  • volume (cm cubed) divided by 24.0

  • Volume (dm cubed) divided by 23.0

  • volume times mr divided by 24.0

Explanation

Question 15 of 34

1

what is the formula for calculating the number of moles in a liquid?

Select one of the following:

  • volume (cm cubed) times concentration

  • volume (dm cubed) divided by concentration

  • volume (dm cubed) times concentration

  • volume (dm cubed) times mr

Explanation

Question 16 of 34

1

What is the definition of an acid?

Select one of the following:

  • A substance with a pH of less than 7

  • A substance the neutralises an alkali

  • A proton donator

  • A dehydrated salt

Explanation

Question 17 of 34

1

What is the definition of an alkali?

Select one of the following:

  • A soluble base

  • A base that dissolves in water to release OH minus ions

  • A substance that is above pH 7

  • The opposite to an acid

Explanation

Question 18 of 34

1

What is the definition of a base?

Select one of the following:

  • A proton acceptor

  • A soluble alkali

  • A substance that is pH7

  • A substance that is above pH 7

Explanation

Question 19 of 34

1

What is the formula of nitric acid?

Select one of the following:

  • NH2

  • HN03

  • H2NO3

  • NaCl

Explanation

Question 20 of 34

1

What is the definition of a salt?

Select one of the following:

  • Formed when an acid and an alkali neutralise each other

  • Formed when the H+ ion in an acid is replaced by a metal ion or other positive ion

  • A popular seasoning

  • A mildly acidic substance (pH5-6) that is formed in the presence of an acid catalyst

Explanation

Question 21 of 34

1

Acid + carbonate --> ??

Select one of the following:

  • Salt + hydrogen + water

  • Salt + hydrogen + carbon dioxide

  • Salt + hydrogen

  • Salt + carbon dioxide + water

Explanation

Question 22 of 34

1

Acid + base --> ??

Select one of the following:

  • Salt + hydrogen

  • Salt + water

  • Salt + oxygen + water

  • Salt + carbon dioxide + water

Explanation

Question 23 of 34

1

Acid + alkali --> ??

Select one of the following:

  • Salt + water

  • Salt + hydrogen + metal oxide

  • Metal oxide + hydrogen

  • Salt + oxygen + water

Explanation

Question 24 of 34

1

What is the definition of... a) hydrated and b) anhydrous

Select one of the following:

  • a) a crystalline compound containing water molecules, b) and crystalline compound containing no water molecules

  • a) an aqueous solution, b) a liquid solution

  • a) a crystalline compound containing water molecules, b) a substance that contains no water molecules

  • a) a crystalline structure, b) a simple covalent structure

Explanation

Question 25 of 34

1

What does water of crystallisation refer to?

Select one of the following:

  • the water molecules that form an essential part of the crystalline structure of a substance

  • the water needed in order to hydrate a substance

  • water molecules that are able to form a crystalline structure under extreme conditions

  • the crystalline structure of non-metals

Explanation

Question 26 of 34

1

What is the oxidation number of an uncombined event?

Select one of the following:

  • 1

  • 0

  • -1

  • +2

Explanation

Question 27 of 34

1

What is the oxidation number of combined fluorine?

Select one of the following:

  • +1

  • 0

  • -1

  • +3

Explanation

Question 28 of 34

1

What is the oxidation number of combined oxygen?

Select one of the following:

  • -2

  • +2

  • +3

  • -1

Explanation

Question 29 of 34

1

What is the oxidation number of combined hydrogen?

Select one of the following:

  • -1

  • 0

  • -2

  • +1

Explanation

Question 30 of 34

1

What is it called when electrons are lost from an element in a reaction?

Select one of the following:

  • Reduction

  • Reductation

  • Oxidation

  • Minimisim

Explanation

Question 31 of 34

1

What is it called when electrons are gained by an atom in a reaction?

Select one of the following:

  • Oxidation

  • Reduction

  • Inheritance

  • Maximism

Explanation

Question 32 of 34

1

What is a reducing agent?

Select one of the following:

  • a reagent that oxidises another species

  • a reagent that is reduced in a reaction

  • a reagent that reduces another species

  • an atom that has been reduced

Explanation

Question 33 of 34

1

What is a redox reaction?

Select one of the following:

  • A reaction where the same element is both reduced and oxidised

  • A reaction which is both endo- and exothermic

  • A reaction that has a total enthalpy change of 0

  • A reaction in which both reduction and oxidation take place

Explanation

Question 34 of 34

1

What is an oxidising agent?

Select one of the following:

  • a reagent that oxidises another species

  • a species that has been oxidised

  • a reagent that accelerates the rate of reduction

  • a reagent that release energy when exposed to oxygen

Explanation

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