Yinka F
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A level Chemistry (2.1 Atoms and Reactions) Quiz on Atoms and Reactions Quiz 1, created by Yinka F on 12/03/2018.

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Yinka F
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Atoms and Reactions Quiz 1

Question 1 of 13

1

Define isotope

Select one of the following:

  • A positively or negatively charged atom

  • Different forms of the same element with a different number of protons

  • Different forms of the same element with a different number of neutrons

  • A positively and negatively charged group of atoms

Explanation

Question 2 of 13

1

Isotopes have different physical properties

Select one of the following:

  • True
  • False

Explanation

Question 3 of 13

1

What did J. J. Thomson discover?

Select one or more of the following:

  • Protons

  • Electrons

  • Neutrons

  • Ions

  • Atoms weren't solid

  • Atoms are solid spheres

  • Shells

  • Plum pudding model

  • Tiny positively charged nucleus surrounded by a 'cloud' of negative electrons

Explanation

Question 4 of 13

1

What did Rutherford discover?

Select one or more of the following:

  • Protons

  • Electrons

  • Neutrons

  • Ions

  • Atoms aren't solid

  • Atoms are solid spheres

  • Shells

  • Plum pudding model

  • Tiny positively charged nucleus surrounded by a 'cloud' of negative electrons

Explanation

Question 5 of 13

1

Fill the blank spaces to complete the text.

The relative atomic mass is the mean mass of an atom of an element, compared to 1/12 of the mass of an atom of .

Explanation

Question 6 of 13

1

Define relative molecular mass

Select one of the following:

  • The average mass of a molecule compared to 1/12 of the mass of an atom of carbon-12

  • The weighted mean mass of an atom of an element, compared to 1/12 of the mass of an atom of carbon-12

  • The average mass of a formula unit, compared to 1/12 of the mass of an atom of carbon-12

  • The mass of an atom of an isotope of an element compared to 1/12 of the mass of an atom of carbon-12

Explanation

Question 7 of 13

1

What is the difference between relative formula mass and relative molecular mass?

Select one of the following:

  • Relative molecular mass is compared to 1/12 of the mass of an atom of carbon-12, whist formula is compared to the whole atom

  • Relative formula mass is used for charged molecules

  • Relative formula mass is used for compounds that are ionic or giant covalent

  • Relative formula mass is used for metallic compounds

Explanation

Question 8 of 13

1

How many particles are in one mole?

Select one of the following:

  • 6.02 x 10²⁴

  • 6.02 x 10²³

  • 6.02 x 10²⁶

  • 6.02 x 10²¹

Explanation

Question 9 of 13

1

What is the ideal gas equation?

Select one of the following:

  • pR = nVT

  • p = nRT

  • pT = nRV

  • pV = nRT

Explanation

Question 10 of 13

1

What is the equation that links concentration with moles and volume?

Select one of the following:

  • Moles = Concentration x Volume

  • Moles = Concentration / Volume

  • Moles = Volume/ Concentration

Explanation

Question 11 of 13

1

Fill the blank spaces to complete the text.

The empirical formula is the whole number of atoms of each element in a compound.

Explanation

Question 12 of 13

1

Fill the blank spaces to complete the text.

The molecular formula is the actual numbers of of each type of in a molecule.

Explanation

Question 13 of 13

1

When a hydrocarbon is burnt in excess oxygen, 8.8g of CO₂ and 3.6g of H₂O are made. What is the empirical formula of the hydrocarbon?

Select one of the following:

  • CH₄

  • C₂H₄

  • CH

  • CH₂

Explanation

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