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Chemisty GCSE > Topic One-particles > Flashcards

Topic One-particles Flashcards

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1
Q

What are the relative masses of a

proton, neutron and electron?

A

Proton: 1
Neutron: 1
Electron: 1/1836

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2
Q

What are the relative charges of a

proton, neutron and electron?

A

Proton: +1
Neutron: 0
Electron: -1

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3
Q

What is an ion?

A

an atom or molecule with a positive or

Negative charge.

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4
Q

How is an ion formed?

A

When an atom or molecule gains or loses electron(s), Positive ions are formed when an electron is lost.

Negative ions are formed when an electron is gained.

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5
Q

What does the atomic number tell you

about an element?

A

The atomic number is unique to each
element and tells you the number of
protons an element has.

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6
Q

What is the mass number?

A

The combined total of the number of

protons and neutrons in the nucleus of an atom of an element.

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7
Q

What are isotopes?

A

Atoms of the same element with the

same number of protons but a different number of neutrons.

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8
Q

How does the atomic number and mass

number differ between isotopes of the same element?

A

Atomic number is the same as an element always has the same number of protons.

Mass number is different as there are
different numbers of neutrons.

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9
Q

Why do atoms contain equal numbers of protons and electrons?

A

Atoms have a stable overall charge of O.
Protons are positively charged and electrons are
negatively charged so they must be present in
equal numbers for charges to balance.

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10
Q

How can you calculate the number of
neutrons, given the mass number and
atomic number of an element?

A

Number of neutrons =

mass number - atomic number

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11
Q

Boron has the atomic number 5 and
mass number 11. How many protons,
electrons and neutrons does boron
have?

A

5 protons
5 electrons
6 neutrons

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12
Q

Sodium has the atomic number 11 and mass number 23. How many protons, electrons and neutrons does the Na+ion have?

A

11 protons
10 electrons (one has been to form the positive ion)
12 neutrons

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13
Q

Compare the typical size of atoms and

small molecules

A

Atoms and small molecules are both incredibly small.
Small molecules are larger than atoms because they are
made of atoms.
The typical atomic radii and bond length are in the order
of 10-10m.

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14
Q

What change did Niels Bohr propose to the nuclear model of an atom?

A

Electron shells around the nucleus.

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15
Q

Describe the structure of an atom

A 
A small central nucleus made up of
protons and neutrons (positively
charged).
Electrons orbit (move around) the
nucleus in shells (negatively charged)
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16
Q

Where is the mass of the atom

concentrated?

A

In the nucleus

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17
Q

Compare the sizes of the nuclear radius and the atomic radius

A

The nuclear radius is much smaller than the atomic radius.

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18
Q

Who designed and carried out the gold foil experiment?

A

Ernest Rutherford designed the
experiment.
Geiger and Marsden carried out the
experiment.

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19
Q

What did Rutherford discover from his

gold foil experiment?

A

He shot a beam of positively charged particles into a sheet of
gold foil.
Most particles passed straight through indicating that atoms
were mostly empty space.
A few particles were deflected and a few bounced directly
back showing that there must be a positively charged
nucleus.

20
Q

Describe Rutherford’s model of the atom

A 
Mass is concentrated in the central
nucleus.
Mostly empty space.
Electrons travel in random paths
around the nucleus.
21
Q

Describe the atomic model proposed by JJ Thomson

A

The plum pudding model:

Negative electrons scattered through a positively charged material.

22
Q

What are the three subatomic particles in an atom?

A

Protons
Neutrons
Electrons

23
Q

Who described atoms as ‘solid spheres’?

A

John Dalton

24
Q

What was dalton’s theory?

A

Atoms cannot be created, divided or destroyed.
Atoms of the same element are exactly the same an
atoms of different elements are different.
Atoms join with other atoms to make new substance

25
Q

What discovery caused the Dalton model of an atom to change?

A

The discovery of subatomic particles

26
Q

How did JJ Thomson discover the

electron?

A 
Thomson conducted an experiment
using a cathode ray tube. The beam
moved towards the positively charged
plate so he knew the particles must have
a negative charge.
27
Q

What is an advantage of the current

particle model?

A

It provides a simple understandable
model to explain the three states of
matter.

28
Q

‘Particles in the particle model are
represented by________ _________
Fill in the gaps
(Higher only)

A

Inelastic spheres

29
Q

What are the limitations of the particle
model?
(Higher only)

A

Doesn’t take into account forces of attraction between
particles. The amount of energy required to cause a
change of state depends on these forces.
Doesn’t take into account the size of particles and
space between them. The nature of particles depends
on the structure and bonding of a substance.

30
Q

Liquid A has a higher boiling point than liquid B. What does this tell you about the forces between the particles in liquid A?
(Higher only)

A

Liquid A has greater forces of attraction between the particles.

31
Q

What is meant by the terms element and compound?

A

Elements are substances made up of
only one type of atom.
Compounds are made up of atoms of
different elements.

32
Q

Why do solids, liquids and gases expand when heated?

A

When a substance is heated the molecules vibrate faster. This causes the space
between the atoms to increase.

33
Q

Substance A melts at -200°C and boils at -183°C. What state is A at -174°C?

A

Liquid

34
Q

Substance B melts at -5°C and boils at

23°C. What state is A at -7°C?

A

Solid

35
Q

Describe what happens, in terms of
particles, when a liquid is heated and
evaporates into a gas

A

When heated, the particles in a liquid expand.
Some particles on the surface gain sufficient energy to overcome the intermolecular forces
and evaporate. At the boiling point, all of the liquid particles gain enough energy to evaporate.

36
Q

Describe what happens, in terms of
particles, when a solid is heated and
melts into a liquid

A

When heated, particles absorb thermal energy
and convert it into kinetic energy. The particles in
the solid vibrate more, causing the solid to
expand until the structure breaks and the solid
turns into a liquid.

37
Q

True or false?
‘Physical changes are relatively easy to
reverse’

A

TRUE
Relatively easy to reverse since no new
product is formed during the changes of
state.

38
Q

How does a physical change differ from a chemical change?

A

A physical change involves changes in the forces
between particles. The particles themselves remain the
same and the chemical properties remain the same.
A chemical change is different as it affects the chemical
properties of the substance.

39
Q

What are the names for the state
changes from solid to liquid and vice
versa?

A

Solid—› liquid: Melting

Liquid—› solid: Freezing

40
Q

What are the names for the state
changes from liquid to gas and vice
versa?

A

Liquid—› gas: Evaporation

Gas—› liquid: Condensation

41
Q

Describe the forces between particles in solids, liquids and gases

A

Solids: Strong forces of attraction between particles which
keep them in fixed positions

Liquids: Weaker attractive forces than in solids.

Gases: Weakest intermolecular forces so particles move
randomly.

42
Q

How do the relative energies of particles

in a solid, liquid and gas compare?

A

Particles in a solid have the least amount
of energy.
Particles in a gas have the most energy.

43
Q

Describe the arrangement and

movement of particles in gases

A

The particles are well separated with no regular arrangement.
The particles vibrate and move freely at high speeds.

44
Q

Describe the arrangement and

movement of particles in liquids

A

The particles are close together but able to move past each other.
The particles vibrate and move around each other.

45
Q

Describe the arrangement and

movement of particles in solids

A

The particles are packed closely together in a regular arrangement.
The particles vibrate in fixed positions.

46
Q

What are the three states of matter?

A

Solid
Liquid
Gas

Chemisty GCSE (4 decks)

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