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80% Quiz GCSE Chemistry > Topic 1 Structure of atom and periodic table > Flashcards

Topic 1 Structure of atom and periodic table Flashcards

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1
Q

What are the names of the 3 sub-atomic particles?

A

proton, neutron and electron

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2
Q

Where are protons and neutrons found?

A

in the nucleus

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3
Q

Where are electrons found?

A

in shells around the outside of the atom

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4
Q

What is the mass and charge of a proton?

A

mass = 1 charge = +1

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5
Q

What is the mass and charge of a neutron?

A

mass = 1 charge = 0

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6
Q

What is the mass and charge of an electron?

A

mass = almost 0 charge = -1

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7
Q

Where is all the mass of an atom found?

A

in the nucleus

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8
Q

What is the overall charge on an atom?

A

neutral

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9
Q

In a neutral atoms how is the number of electrons related to the number of protons?

A

Number of electrons = number of protons

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10
Q

How big is the nucleus compared to the size of the atom?

A

the nucleus is tiny compared to the size of the atom

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11
Q

What is the larger of the two numbers on the Periodic Table?

A

Relative atomic mass (mass number)

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12
Q

What is the smaller of the two numbers on the Periodic Table?

A

Atomic number

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13
Q

What does the atomic number of an atom tell you?

A

The number of protons

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14
Q

What does the mass number of an atom tell you?

A

The number of protons + number of neutrons

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15
Q

If the atomic number changes what happens to the atom?

A

The type of atom changes

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16
Q

Which atom has 7 protons?

A

Nitrogen

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17
Q

How can you calculate the number of electrons from the atomic number?

A

Number of electrons = number of protons = number of electrons

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18
Q

If an atom has an atomic number of 8, how many electrons does it have?

A

8

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19
Q

How can you calculate the number of neutrons from the mass number and the atomic number?

A

number of neutrons = mass number ? atomic number

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20
Q

How are atoms of different elements different from each other?

A

They have a different number of protons

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21
Q

What is the mass and charge of a neutron?

A

mass = 1 charge = neutral

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22
Q

How can an atom become heavier or lighter?

A

It can lose or gain a neutron

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23
Q

What is an isotope?

A

A heavier or lighter atom made by losing or gaining an neutron

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24
Q

Describe in terms of the sub atomic particles how isotopes of the same element are different from each other

A

They have the same number of protons and electrons but a different number of neutrons

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25
Q

What are the chemical properties of different isotopes like?

A

Isotopes have exactly the same chemical properties

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26
Q

Why are the chemical properties of different isotopes the same?

A

They are the same atom with the same number of protons and electrons and so react in the same way.

27
Q

If an element contains a small amount of a heavier isotope what would happen to the mass of the element?

A

It would increase slightly

28
Q

What does the Relative Atomic Mass take into account?

A

The different isotopes and their abundance (how much of them there are)

29
Q

Why is the Relative Atomic Mass sometimes not be a whole number?

A

Because it is an average mass taking into account all of the different isotopes and their abundances

30
Q

Higher ? What is the equation to calculate the Relative atomic mass of an atom given the mass and % abundance of the different isotopes?

A

(%/100 x mass of isotope1) + (%/100 x mass of isotope2) + (%/100 x mass of isotope3) etc.

31
Q

How did Mendeleev organise elements in his early Periodic Table?

A

According to increasing mass of the atoms

32
Q

Why did Mendeleev leave gaps in his Periodic Table ?

A

For elements that hadn?t yet been discovered

33
Q

What was similar about the elements in the same column in Mendeleev?s table?

A

They have similar chemical properties (he didn?t know about electrons!)

34
Q

Which elements did Mendeleev switch in his Periodic Table

A

Tellerium and Iodine

35
Q

Why did Mendeleev switch the position of some elements in his Periodic Table?

A

Because when they are ordered by mass the elements don?t have the same chemical reactions as other elements in their group

36
Q

What is a prediction?

A

An estimate based on the result fitting a pattern

37
Q

Why could Mendeleev predict the properties of elements that hadn?t been discovered?

A

Because how knew the properties of other elements in the same group and the properties fitted a pattern

38
Q

Describe one way that Mendeleev?s Periodic Table is different from the Modern Periodic Table

A

Mendeleev ordered his elements by increasing mass the modern Periodic Table is ordered according to increasing atomic number

39
Q

What is the atomic number of an element?

A

The number of protons

40
Q

How are elements arranged in the Modern Periodic Table?

A

In order of increasing atomic number

41
Q

What happens to the atomic number as you go along elements in the same period?

A

It increases by one each element

42
Q

Where are metals found in the Modern Periodic Table?

A

On the left hand side

43
Q

Where are non-metals found in the Modern Periodic Table?

A

On the right hand side

44
Q

What are the columns called in the Modern Periodic Table?

A

Groups

45
Q

Name 3 elements in group 1 of the Periodic Table

A

Lithium, Sodium, Potassium

46
Q

Name 3 elements in group 7 if the Periodic Table

A

Chlorine, Bromine, Fluorine

47
Q

What are the rows called in the Modern Periodic Table?

A

Periods

48
Q

Name the two elements in Period 1

A

Hydrogen and Helium

49
Q

How are Tellurium and Iodine arranged in the Modern Periodic Table?

A

Tellurium comes before Iodine as it has a lower atomic number

50
Q

Why is it correct to put Iodine in group 7 of the Modern Periodic Table?

A

It has similar chemical properties to the other elements in group 7

51
Q

How can ideas about isotopes explain why the mass of Tellurium is heavier than expected?

A

Tellurium has a number of heavier isotopes in high abundance which means it has a heavier mass than expected

52
Q

Where are electrons found in an atom?

A

In shells around the outside of the atom

53
Q

What does the atomic number tell you about the number of electrons in an atom?

A

The number of protons and therefore the number of electrons

54
Q

What is the rule for filling electrons in the first 3 shells?

A

2,8,8

55
Q

What is meant by the term ?electronic configuration??

A

The number of electrons written in the form 2,8,8

56
Q

Give the electronic configuration of the element with atomic number of 11

A

2,8,1

57
Q

What is similar about the electronic configuration of elements in the same group?

A

They all have the same number of electrons in the outer shell

58
Q

How does the electronic configuration of elements in the same period change as you move along the period?

A

One more electrons is added to the same shell

59
Q

Why are calcium and magnesium in the same group in the Periodic Table?

A

They both have two electrons in their outer shell

60
Q

Why are sodium and chlorine in the same period of the Periodic Table?

A

They both have their outer electrons in the same shell

61
Q

What can you say about the electronic configuration of metals in the Periodic Table?

A

They have 1, 2 or 3 extra electrons in their outer shell

62
Q

What can you say about the electronic configuration of non-metals in the Periodic Table?

A

They have 1, 2 or 3 gaps and need electrons to fill their outer shell

63
Q

What can you say about the electronic configuration of non-metals in the Periodic Table?

A

They have 1, 2 or 3 gaps and need electrons to fill their outer shell

80% Quiz GCSE Chemistry (3 decks)

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