C1 - Particles Flashcards

1
Q

What constitutes as a particle?

A
  • Atoms
  • Ions
  • Molecules
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2
Q

What are the properties of a solid?

A
  • Regular lattice particle arrangement
  • Particles are very close
  • Particles vibrate about fixed positions
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3
Q

What are the properties of a liquid?

A
  • Random particle arrangement
  • Particles are close together with some gaps
  • Particles move around each other
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4
Q

What are the properties of a gas?

A
  • Random particle arrangement
  • Particles are far apart
  • Particles move quickly in all direction
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5
Q

In which state(s) can something not be compressed?

A

A substance in solid/liquid state cannot be compressed because there is no space for particles to move into.

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6
Q

Why can substances in the solid state not flow?

A

A solid substance cannot flow as it has a fixed shape. Particles vibrate about fixed positions and do not move.

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7
Q

Why do solids expand when heated?

A

When heated, particles in a solid gain kinetic energy and vibrate more. The space between the particles increase as a result, making the solid ‘expand’.

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8
Q

What is a Physical change?

A

A reversible change that doesn’t result in a new substance being formed.

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9
Q

What happens to the particles in a physical change?

A

During a physical change, the arrangement and movement of the particles change.

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10
Q

What is a Chemical change?

A

An irreversible change where new substances are formed.

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11
Q

What happens to the particles in a physical change?

A

During a chemical change, particles break their bonds and join in different ways, resulting in new substances to be formed.

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12
Q

What are the limitations of the particles model?

A

These three things are not taken into account:
- The forces between particles.
- The size of particles.
- The space between particles.

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13
Q

Define ‘molecule’.

A

Two or more atoms chemically joined together.

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14
Q

What are the relative atomic masses of:
Protons, Neutrons and Electrons.

A

Protons - 1
Neutrons - 1
Electrons - 0.0005 (1/2000)

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15
Q

What are the relative atomic charges of:
Protons, Neutrons and Electrons.

A

Protons: +1
Neutrons: 0
Electrons: -1

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16
Q

Define ‘isotope’.

A

A different atomic form of an element where atoms of an element have the same number of protons and electrons, but a different number of neutrons.

17
Q

Order Of Scientists - Developing the Atomic Model

A
  1. John Dalton - 1803
  2. JJ Thomson - 1897
  3. Ernest Rutherford - 1909
  4. Niels Bohr - 1913
18
Q

What did Dalton suggest?

A
  • All matter is made from atoms.
  • All atoms of an element are identical.
  • Different elements have different types of atoms.
  • Tiny solid balls.
19
Q

What did Thomson do?

A
  • Development of the ‘Plum Pudding Model’.
  • Shot beams of ‘cathode rays’ - their direction changed in electric/magnetic fields.
  • Concluded atoms are spheres of positive charge, scattered with elections.
  • Atoms are overall neutral.
20
Q

What did Rutherford do?

A
  • Gold foil experiment, fired beams of positively charged alpha particles at thin sheets of gold.
  • Contrary to what should’ve happened (particles go straight through), many were deflected.
  • A positively charged mass in the centre of the nucleus (called nucleus)
  • Electrons orbit the nucleus like planets do the sun.
21
Q

What did Bohr do?

A
  • He realised that orbiting electrons would be attracted to the oppositely charged nucleus, collapsing the atom.
  • Bohr suggested electrons occupied fixed energy levels (electron shells), around the nucleus.