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Year 10 Chemistry > GCSE Atomic Structure > Flashcards

GCSE Atomic Structure Flashcards

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1
Q

History of structure of the atom:
Early 1800’s;
In his theory what did dalton state

A
  • All elements are made up of small invisible particles called atoms
  • Atoms can’t be created or destroyed
  • Atoms of different elements have different properties
  • When atoms combine they form molecules or compounds
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2
Q

History of structure of the atom:

1897 ‘Plum Pudding’ model of J.J Thomson: Who discovered the electron

A

J.J Thomson

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3
Q

History of structure of the atom:
1897 ‘Plum Pudding’ model of J.J Thomson: When J.J Thomson discovered the electron what happened to dalton’s atomic theory

A

It was modified

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4
Q

History of structure of the atom:
1897 ‘Plum Pudding’ model of J.J Thomson:
What did J.J Thomson propose

A

He proposed the ‘plum pudding’ model which stated that the negative electrons were embedded in a positive sphere (like the raisins in a plum pudding)

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5
Q

History of structure of the atom:

What happened in 1911

A

Ernest Rutherford revised J.J Thomson’s model to the model which has electrons orbiting a positive nucleus

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6
Q

History of structure of the atom:

What happened in 1932

A

James Chadwick discovered the neutron

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7
Q

Comprehension questions:

Who proposed the idea that matter is composed of small indivisible particles called atoms

A

Democritus and Leucippus

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8
Q

Comprehension questions:

What ideas did Aristotle propose

A

That matter was composed of 4 ‘elements’, air, earth, fire and water and he used these ideas to explain matter and its behaviour

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9
Q

Comprehension questions:

In 1908 John Dalton published his atomic theory, what did he state

A

That all elements are made up of small indivisible particles called atoms

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10
Q

Comprehension questions:

Name the scientist who discovered the electron

A

J.J Thomson

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11
Q

Comprehension questions:

What experiment was Thomson carrying out when he discovered the electron

A

The way gases conduct electricity

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12
Q

Comprehension questions:

In Thomson’s experiment how did he show the electrons had a negative charge

A

He passed high voltage across the terminals of a tube containing air and found out that the rays produced travelled in straight lines from the negative terminal and at these rays were deflected when they passed through charged plates

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13
Q

Comprehension questions:

What did Thomson’s model of the atom look like

A

A plum pudding

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14
Q

Comprehension questions:

How was it similar to a Christmas pudding

A

There are rings of negative electrons embedded in a sphere of positive charge, just like the currants embedded in a Christmas pudding

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15
Q

Comprehension questions:

Why did Thomson suggest that the atom was neutral

A

Because it contained equal numbers of positive and negative charges

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16
Q

Comprehension questions:

What did Rutherford discover about the atom

A

It consisted of electrons revolving around a positively charged nucleus

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17
Q

Comprehension questions:

Where is virtually all of an atoms mass contained

A

In the nucleus

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18
Q

Comprehension questions:

In what way was Rutherford’s model of the atom similar to planets revolving around the sun

A

The electrons revolving around the positively charged nucleus were like the planets revolving around the sun

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19
Q

Comprehension questions:

What part of the atom did James Chadwick discover in 1932

A

He showed that the nucleus of an atom contained 2 different types of particles, protons and new particles called neutrons

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20
Q

Comprehension questions:

How does the mass of a neutron compare with the mass of a proton

A

It is equal

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21
Q

Fill in the blanks:
Atom is composed of a small, dense, ………… charged nucleus composed of……….and……….with…………charged electrons in…….orbiting the……..

A 
Positively
Neutrons
Protons
Negatively
Shells
Nucleus
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22
Q

Give the relative mass (atomic mass units), relative charge and position of the following particles:
Proton
Neutron
Electron

A

Proton:
Relative mass = 1
Relative charge = +1
Position = nucleus

Neutron:
Relative mass = 1
Relative charge = 0
Position = nucleus

Electron:
Relative mass = 1/1840
Relative charge = -1
Position = shells

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23
Q

Definition of atomic number

A

This is the number of protons in an atom

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24
Q

Definition of mass number

A

This is the total number of protons and neutrons in an atom

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25
Q

How do the atoms of one element differ from those of another

A

They always have different numbers of protons as this defines the element, however the number of neutrons and electrons vary to

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26
Q

In the periodic table there are two numbers beside each atomic symbol, what are they called

A

One is called the mass number and the other is called the atomic number

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27
Q

Fill in the blanks:
The number of protons in an atom is equal to its………..

As an atom is electrically neutral (i.e. No overall charge) then the number of……..must equal the number of………

The number of………in an atom is equal to its……………….. - …………….

A 
Atomic number
Electrons
Protons
Neutrons
Mass number
Atomic number
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28
Q

Calculate the number of sub atomic particles in each of the following:
Lithium (mass number of 7, atomic number of 3)

A 
P = 3
E = 3
N = 4
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29
Q

Calculate the number of sub atomic particles in each of the following:
Magnesium (with a mass number of 24 and an atomic number of 12)

A 
P = 12
E = 12
N = 12
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30
Q

Calculate the number of sub atomic particles in each of the following:
Oxygen (with a mass number of 16 and an atomic number of 8)

A 
P = 8
E = 8
N = 8
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31
Q

Calculate the number of sub atomic particles in each of the following:
Chlorine(with a mass number of 35 and an atomic number of 17)

A 
P = 17
E = 17
N = 18
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32
Q

Calculate the number of sub atomic particles in each of the following:
Nitrogen (with a mass number of 14 and an atomic number of 7)

A 
P = 7
E = 7
N = 7
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33
Q

Calculate the number of sub atomic particles in each of the following:
Helium (with a mass number of 4 and an atomic number of 2)

A 
P = 2
E = 2
N = 2
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34
Q

Calculate the number of sub atomic particles in each of the following:
Potassium (with a mass number of 39 and an atomic number of 19)

A 
P = 19
E = 19
N = 20
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35
Q

Calculate the number of sub atomic particles in each of the following:
Fluorine (with a mass number of 19 and an atomic number of 9)

A 
P = 9
E = 9
N = 10
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36
Q

Calculate the number of sub atomic particles in each of the following:
Aluminium (with a mass number of 27 and an atomic number of 13)

A 
P = 13
E = 13
N = 14
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37
Q

Calculate the number of sub atomic particles in each of the following:
Boron (with a mass number of 11 and an atomic number of 5)

A 
P = 5
E = 5
N = 6
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38
Q

Calculate the number of sub atomic particles in each of the following:
Beryllium (with a mass number of 9 and an atomic number of 4)

A 
P = 4
E = 4
N = 5
39
Q

Calculate the number of sub atomic particles in each of the following:
Neon (with a mass number of 20 and an atomic number of 10)

A 
P = 10
E = 10
N = 10
40
Q

Electronic structure:

Where are electrons arranged and where

A

In shells around the nucleus

41
Q

Electronic structure:

What shell do electrons enter first

A

The shell closest to the nucleus

42
Q

Electronic structure:

What must happen to each shell before starting to fill the next

A

Each shell must be filled with its full quota before starting to fill the next shell

43
Q

Electronic structure:

Shell number 1 (closest to the nucleus) can take how many electrons

A

A maximum of 2

44
Q

Electronic structure:

All the other shells bar the first have a maximum of how many electrons

A

8

45
Q

Electronic structure:

What is the rule for positioning electrons

A

In second and subsequent shells, the electrons are placed at 12 o’clock, 3 o’clock, 6 o’clock and 9 o’clock, before being paired in the same order

46
Q

What is the electronic configuration for lithium (atomic number 3)

A

2,1

47
Q

What is the electronic configuration for magnesium (atomic number 12)

A

2,8,2

48
Q

What is the electronic configuration for oxygen (atomic number 8)

A

2,6

49
Q

What is the electronic configuration for chlorine (atomic number 17)

A

2,8,7

50
Q

What is the electronic configuration for nitrogen (atomic number 7)

A

2,5

51
Q

What is the electronic configuration for helium (atomic number 2)

A

2

52
Q

What is the electronic configuration for potassium (atomic number 19)

A

2,8,8,1

53
Q

What is the electronic configuration for fluorine (atomic number 9)

A

2,7

54
Q

What is the electronic configuration for aluminium (atomic number 13)

A

2,8,3

55
Q

What is the electronic configuration for boron (atomic number 5)

A

2,3

56
Q

What is the electronic configuration for beryllium (atomic number 4)

A

2,2

57
Q

What is the electronic configuration for neon (atomic number 10)

A

2,8

58
Q

How many electrons do each of the following elements have and what is there electronic configuration:
Element A - mass number 9 and has 5 neutrons
Element D - mass number 12 and has 6 neutrons
Element E - mass number 40 and has 22 neutrons
Element G - mass number 39 and has 20 neutrons
Element H - mass number 31 and has 15 neutrons

A

Element A - has 4 electrons and an electronic configuration of 2,2

Element D - has 6 electrons and an electronic configuration of 2,4

Element E - has 18 electrons and an electronic configuration of 2,8,8

Element G - has 19 electrons and an electronic configuration of 2,8,8,1

Element H - has 16 electrons and an electronic configuration of 2,8,6

59
Q

If I have an electronic configuration of 2,8,3 and my mass number is 27 what element am I and what is my atomic number

A

Aluminium and 13

60
Q

If my mass number is 24 and my atomic number is 12 what element am I and what is my electronic configuration

A

Magnesium and 2,8,2

61
Q

If I’m the element fluorine my atomic number is 9, what’s my electronic configuration and mass number

A

19 and 2,7

62
Q

If I have an electronic configuration of 2,6 and my mass number is 16 what element am I and what is my atomic number

A

Oxygen and 8

63
Q

What’s the definition of an isotope

A

Isotopes are atoms of an element with the same atomic number but a different mass number indicating a different number of neutrons

64
Q

What are two common isotopes

A

Chlorine 35 and chlorine 37

Chlorine 35 has 17 protons, 17 electrons and 18 neutrons

Chlorine 37 has 17 protons, 17 electrons and 20 neutrons

65
Q

Calculating the relative atomic mass of chlorine from the mass numbers and abundances of isotopes:
Naturally occurring sample,
75% of the atoms will have a mass number of 35
25% of the atoms will have a mass number of 37
Work out the average mass number

A 
Average mass number =
 (75x35) + (25x37)
--------------------
              100
= 35.5
66
Q

Mass spectrum of isotopes:

Imagine a mass spectrum for an example of chlorine, what is the label on the y axis

A

Relative abundance

67
Q

Mass spectrum of isotopes:

Imagine a mass spectrum for an example of chlorine, what does the peak height show you

A

The relative abundance of each isotope of chlorine

68
Q

Mass spectrum of isotopes:
Imagine a mass spectrum for an example of chlorine, when the charged is +1 the axis always indicates the mass of the substance. What are the two mass number for the two isotopes of chlorine

A

35 and 37

69
Q

Mass spectrum of isotopes:
Imagine a mass spectrum for an example of chlorine, the ration for the peak heights for the sample of chlorine is 3:1 for chlorine 35 and chlorine 37 respectively. Calculate the average RAM for chlorine

A 
         4 = 35.5
70
Q

Use the info below to identify which two are isotopes:
Substance A has 8 protons, 8 neutrons and 8 electrons
Substance B has 10 protons, 10 neutrons and 10 electrons
Substance C has 8 protons, 10 neutrons and 8 electrons
Substance D has 8 protons, 8 neutrons and 10 electrons

A

A and C

71
Q

Complete the following to show the number of protons men neutrons and electrons in the three isotopes of carbon:
An isotope of carbon has a mass number of 12 and an atomic number of 6
An isotope of carbon has a mass number of 13 and an atomic number of 6
An isotope of carbon has a mass number of 14 and an atomic number of 6

A

Isotope 1: 6 electrons, 6 protons and 6 neutrons

Isotope 2: 6 electrons, 6 protons and 7 neutrons

Isotopes 3: 6 electrons, 6 protons and 8 neutrons

72
Q

Chlorine exists naturally as 2 isotopes chlorine 35 and chlorine 37 in the ratio 3:1 respectively.
Show why the relative atomic mass of chlorine is 35.5

A 
         4 = 35.5
73
Q

Calculate the relative atomic mass of boron given that it contains 20% boron 10 and 80% boron 11

A 
RAM =
(20x10) + (80x11)
------------------
             100
= 10.8
74
Q

Which one of the following is not found in the nucleus of an atom;
Proton, neutron, electron

A

Electron

75
Q

Uranium has two common isotopes, uranium 235 and uranium 238, (both have an atomic number of 92)
What is the atomic number of uranium

A

92

76
Q

Uranium has two common isotopes, uranium 235 and uranium 238, (both have an atomic number of 92)
Why does uranium 238 have a greater atomic number than the uranium 235 isotope

A

Because it has 3 extra neutrons

77
Q

Uranium has two common isotopes, uranium 235 and uranium 238, (both have an atomic number of 92)
Give one way in which atoms of the two uranium isotopes are similar

A

They have the same number of protons and electrons (same atomic number)

78
Q

Chlorine exists as 2 isotopes, chlorine 35 and chlorine 37:

Give one way in which these isotopes are similar

A

They are the same element due to the atomic number

79
Q

Chlorine exists as 2 isotopes, chlorine 35 and chlorine 37:

Give one way in which these two isotopes are different

A

They have different mass numbers

80
Q

A sample of silicon contains 92.18% silicon 28, 4.70% silicon 29 and 3.12% silicon 30. Calculate the RAM of silicon

A 
RAM = 
(92.18x28) + (4.70x29) + (3.12x30)
-------------------------------------
                             100
= 28.11
81
Q

Atoms into ions:

Atoms with electric charges are called….

A

Ions

82
Q

Atoms into ions:

Those with positive charges are called……

A

Cations

83
Q

Atoms into ions:

Those with negative charges are called……

A

Anions

84
Q 
Formation of cations (positive ions):
Sodium atom -----> sodium ion
P = 11
E = 11       2,8,1     ------->            
N = 12
A

Loses Na+
——-> P = 11 2,8
1 electron E = 10
N = 12

85
Q 
Formation of cations (positive ions):
Calcium atom -----> calcium ion
P = 20
E = 20       2,8,8,2     ------->            
N = 20
A

Loses Ca2+
——-> P = 20 2,8,8
2 electrons E = 18
N = 20

86
Q 
Formation of cations (positive ions):
Aluminium atom -----> aluminium ion
P = 13
E = 13       2,8,3     ------->            
N = 14
A

Loses Al3+
——-> P = 13 2,8
3 electrons E = 10
N = 14

87
Q 
Formation of anions (negative ions):
Chlorine atoms -----> chloride ion
P = 17
E = 17       2,8,7     ------->            
N = 18
A

Gains Cl-
——-> P = 17 2,8,8
1 electron E = 18
N = 18

88
Q 
Formation of anions (negative ions):
Oxygen atom -----> oxygen ion
P = 8
E = 8       2,6     ------->            
N = 8
A

Gains O2-
——-> P = 8 2,8
2 electrons E = 10
N = 8

89
Q 
Formation of anions (negative ions):
Nitrogen atom -----> nitrogen ion
P = 7
E = 7       2,5     ------->            
N = 7
A

Gains N3-
——-> P = 7 2,8
3 electrons E = 10
N = 7

90
Q

GENERAL RULE

A

Metals form positive ions

Non metals form negative ions

91
Q

What do u find in every science lab

A

A periodic table

92
Q

How is the periodic table arranged

A

By atomic number

93
Q

The atomic number tells us the number of protons in an element, what else does it tell us

A

The number of electrons orbiting the nucleu

Year 10 Chemistry (4 decks)

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