A level Chemistry OCR A- Module 2 Flashcards

1
Q

Define isotope

A

Atoms of the same element with different number of neutrons and the same number of protons.

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2
Q

Why do isotopes have the same chemical properties?

A

They have the same configuration of electrons.

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3
Q

Why do isotopes have different physical properties?

A

Physical properties depend on the mass of the atom. They have the different masses.

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4
Q

What is the relative mass of an electron?

A

1/2000

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5
Q

What is the relative mass of a neutron?

A

1

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6
Q

What is the relative mass of a proton?

A

1

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7
Q

What is the mass number?

A

The total number of protons and neutrons in the nucleus of an atom.

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8
Q

What is the atomic number?

A

The number of protons in the nucleus of an atom.

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9
Q

What does Thomson’s model explain.

A

Atoms are not solid and indivisible, an atom contains even smaller, negatively charged particles- electrons

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10
Q

What was JJ Thomson’s model called?

A

The plum pudding model- a positively charged sphere with negative electrons embedded in it.

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11
Q

What does Rutherford’s model explain?

A

That the plum pudding model isn’t right; there’s a tiny positively charged nucleus at the centre of the atom surrounded by a ‘cloud’ of negative electrons.

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12
Q

How did Ernest Rutherford prove his theory?

A

He conducted the famous gold foil experiment; they fired alpha particles (positively charged) at an extremely thin sheet of gold. Most of the alpha particles passed straight through the gold atoms and a small number were deflected backwards through more than 90*.

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13
Q

Name the scientists who conducted the gold foil experiment?

A

Ernest Rutherford, Hans Geiger and Ernest Marsden.

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14
Q

What modifications were made to Rutherford’s model?

A

jgv

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15
Q

Describe the main features of Bohr’s model?

A
  • Electrons only exist in fixed shells, nowhere in between
  • Each shell has a fixed energy
  • When an electron moves between shells electromagnetic radiation is emitted or absorbed
  • Because the energy of shells is fixed, the radiation will have a fixed frequency
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16
Q

What does Bohr’s model explain?

A

Some elements are inert- noble gases.

Shells of an atom can only hold fixed numbers of electrons, and that an element’s reactivity is due to its electrons.

17
Q

How is evidence used to accept or reject particular models?

A

tf

18
Q

Define the relative atomic mass

A

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

19
Q

Define the relative isotopic mass

A

The weighted mean mass of an isotope compared to 1/12 the mass of an atom of carbon-12

20
Q

How do you calculate the relative isotopic mass of an element?

A
  1. Multiply each relative isotopic mass by its % relative isotopic abundance and add up the results
  2. Divide by 100
21
Q

How do you calculate the relative atomic mass from mass spectra?

A
  1. Multiply each relative isotopic mass by its relative abundance and add up the results
  2. Divide by the sum of the relative abundances
22
Q

Define relative molecular mass

A

The