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Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is the Particle Theory of Matter?

A

The idea that all matter is made up of small particles

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2
Q

What is the arrangement of particles in a solid?

A

A regular pattern

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3
Q

What is the relative distance of particles in a solid?

A

Very close/tightly packed

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4
Q

What is the movement of particles in a solid?

A

Particles vibrate around a fixed point

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5
Q

What is the arrangement of particles in a liquid?

A

Random

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6
Q

What is the arrangement of particles in a gas?

A

Random

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7
Q

What is the relative distance of particles in a liquid?

A

Close

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8
Q

What is the relative distance of particles in a gas?

A

Far away from each other

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9
Q

Describe the movement of particles in a liquid

A

They move around each other

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10
Q

Describe the movement of particles in a gas

A

They move quickly in all directions

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11
Q

When particles are given more energy, how does their movement change?

A

They move quicker

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12
Q

What is the point that a solid changes into a liquid?

A

The melting point

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13
Q

What is the point in which liquid become a gas?

A

The boiling point

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14
Q

Describe the temperature when a substance changes state

A

Constant

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15
Q

Do bonds require energy to be broken?

A

Yes

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16
Q

Do bonds release energy when made?

A

Yes

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17
Q

Give 3 limitations of the particle model

A

It doesn’t take into account:

  • size of particles
  • forces of attraction
  • space between particles
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18
Q

Can a gas be compressed? (How much if so?)

A

Yes - a lot

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19
Q

Can a liquid be compressed? (How much if so?)

A

No

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20
Q

Can a solid be compressed? (How much if so?)

A

No

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21
Q

What happens to the forces of attraction when a solid becomes a liquid?

A

Some of them are overcome

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22
Q

What happens to the forces of attraction when a liquid becomes a gas?

A

All of them are overcome

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23
Q

Do bonds break when substances change state

A

NO, only the forces of attraction are overcome

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24
Q

What kind of temperatures are needed for bonds to break?

A

Very high

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25
Q

What is an atom?

A

The smallest part of an element that retains the properties of that element

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26
Q

What is the radius of an average atom?

A
  • 10

1 m

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27
Q

What is the mass of an average atom?

A

-23

10 g

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28
Q

Describe the structure of an atom

A

A central, positively charged nucleus surrounded by shells of negatively charged electrons

29
Q

Describe the radius of the nucleus in comparison to the whole atom

A

Much smaller

30
Q

What is the nucleus of an atom made up of?

A

Protons and neutrons

31
Q

Why does an atom have an overall neutral charge

A

Because there are the same numbers of protons and electrons

32
Q

What does the mass number of an element show?

A

The total number of protons and neutrons

33
Q

What does the atomic number of an element show?

A

The number of protons in an atom (therefore number of electrons too)

34
Q

What is an ion?

A

When an element loses or gains electrons

35
Q

What is the atomic mass unit of a proton?

A

1

36
Q

What is the Atomic mass unit (A.m.u) of a neutron?

A

1

37
Q

What is the A.m.u of an electron

A

1/2000

38
Q

What is the charge of a proton?

A

+1

39
Q

What is the charge of a neutron?

A

0

40
Q

What is the charge of an electron?

A

-1

41
Q

What is an isotope?

A

Atoms of the same element with the same atomic number but different mass number (due to a different number of neutrons)

42
Q

How many neutrons does a particle of Carbon-14 have? (Atomic number is 6)

A

8

43
Q

How many electrons does the first shell have?

A

2

44
Q

How many electrons do all other shells hold (for GCSE anyway)

A

8

45
Q

What kind of evidence lead to changes in the particle model?

A

Experimental evidence

46
Q

What year was Dalton’s model?

A

1803

47
Q

What was Dalton’s conclusions about the particle model

A

Atoms can’t be broken down into anything simpler
Atoms of a given element are identical to each other
Atoms of different elements are different from each other
During chemical reactions atoms rearrange to make different substances

48
Q

What did Dalton imagine atoms to be?

A

Tiny solid balls

49
Q

What did J.J Thomson discover?

A

The electron

50
Q

What model was developed by J.J Thomson?

A

The plum pudding model

51
Q

What conclusions did J.J Thomson conclude about the atom?

A

Atoms are overall neutral

Atoms are spheres of positive charge with electrons dotted around inside

52
Q

What year did J.J Thomson develop the plum pudding model?

A

1897

53
Q

The Geiger - Marsden Experiment took place in which years?

A

1909-1911

54
Q

How did Geiger and Marsden test the plum pudding model?

A

By firing positively charged particles at very thin gold foil

55
Q

What model did Ernest Rutherford discover?

A

Planetary model

56
Q

What year did Niels Bohr improve Rutherford’s model?

A

1913

57
Q

How did Niels Bohr improve Rutherford’s model?

A

Discovered that electrons occupy shells or energy levels around the nucleus

58
Q

What is a subatomic particle?

A

An object found in atoms (eg. Protons, neutrons and electrons

59
Q

What does RAM stand for? (Ar)

A

Relative atomic mass

60
Q

What does RMM stand for? (Mr)

A

Relative molecular mass

61
Q

What is the RAM?

A

The ratio of the average mass of one atom of an element to a twelfth of the mass of an atom of carbon-12

62
Q

What does RFM stand for? (Mr)

A

Relative formula mass

63
Q

What is the empirical formula of C6H12O6?

A

CH2O

64
Q

What is the empirical formula?

A

The simplest whole number ratio of each type of atom in a compound

65
Q

How can the empirical formula be calculated?

A

From the number of atoms present or by converting the mass of the element/compound

66
Q

What happens to the particles of a substance when it changes state?

A

The arrangement and movement of them change

67
Q

When substances change state, how does their mass change?

A

It’s stays the same (conservation of mass)

68
Q

How do you convert the mass of an element/compound to calculate the empirical formula?

A

Find the number of moles

Mass
RFM

Chemistry (8 decks)

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