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Atomic Structure Flashcards

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
What is an atom?
The smallest part of an element that retains the properties of that element
26
What is the radius of an average atom?
- 10 | 1 m
27
What is the mass of an average atom?
-23 | 10 g
28
Describe the structure of an atom
A central, positively charged nucleus surrounded by shells of negatively charged electrons
29
Describe the radius of the nucleus in comparison to the whole atom
Much smaller
30
What is the nucleus of an atom made up of?
Protons and neutrons
31
Why does an atom have an overall neutral charge
Because there are the same numbers of protons and electrons
32
What does the mass number of an element show?
The total number of protons and neutrons
33
What does the atomic number of an element show?
The number of protons in an atom (therefore number of electrons too)
34
What is an ion?
When an element loses or gains electrons
35
What is the atomic mass unit of a proton?
1
36
What is the Atomic mass unit (A.m.u) of a neutron?
1
37
What is the A.m.u of an electron
1/2000
38
What is the charge of a proton?
+1
39
What is the charge of a neutron?
0
40
What is the charge of an electron?
-1
41
What is an isotope?
Atoms of the same element with the same atomic number but different mass number (due to a different number of neutrons)
42
How many neutrons does a particle of Carbon-14 have? (Atomic number is 6)
8
43
How many electrons does the first shell have?
2
44
How many electrons do all other shells hold (for GCSE anyway)
8
45
What kind of evidence lead to changes in the particle model?
Experimental evidence
46
What year was Dalton’s model?
1803
47
What was Dalton’s conclusions about the particle model
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
What did Dalton imagine atoms to be?
Tiny solid balls
49
What did J.J Thomson discover?
The electron
50
What model was developed by J.J Thomson?
The plum pudding model
51
What conclusions did J.J Thomson conclude about the atom?
Atoms are overall neutral | Atoms are spheres of positive charge with electrons dotted around inside
52
What year did J.J Thomson develop the plum pudding model?
1897
53
The Geiger - Marsden Experiment took place in which years?
1909-1911
54
How did Geiger and Marsden test the plum pudding model?
By firing positively charged particles at very thin gold foil
55
What model did Ernest Rutherford discover?
Planetary model
56
What year did Niels Bohr improve Rutherford’s model?
1913
57
How did Niels Bohr improve Rutherford’s model?
Discovered that electrons occupy shells or energy levels around the nucleus
58
What is a subatomic particle?
An object found in atoms (eg. Protons, neutrons and electrons
59
What does RAM stand for? (Ar)
Relative atomic mass
60
What does RMM stand for? (Mr)
Relative molecular mass
61
What is the RAM?
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
What does RFM stand for? (Mr)
Relative formula mass
63
What is the empirical formula of C6H12O6?
CH2O
64
What is the empirical formula?
The simplest whole number ratio of each type of atom in a compound
65
How can the empirical formula be calculated?
From the number of atoms present or by converting the mass of the element/compound
66
What happens to the particles of a substance when it changes state?
The arrangement and movement of them change
67
When substances change state, how does their mass change?
It’s stays the same (conservation of mass)
68
How do you convert the mass of an element/compound to calculate the empirical formula?
Find the number of moles Mass RFM

Chemistry (8 decks)

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