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GCSE Chemistry > Atom > Flashcards

Atom Flashcards

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1
Q

Define the term ‘atom’

A

An atom is the smallest part of an element that can still be recognised as that element

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2
Q

How do you know if a chemical equations is balanced

A

The number of atoms of each element on the reactants side will be equal to the number of atoms of each element on the products side

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3
Q

Define the term ‘electron’

A

An electron is a tiny particle with a negative charge. Electrons orbit the nucleus of atoms or ions in shells

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4
Q

Define the term ‘proton’

A

A proton is a tiny positive particle found inside the nucleus of an atom

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5
Q

Define the term ‘neutron’

A

A neutron is a dense particle found in the nucleus of an atom. It is electrically neutral, carrying no charge.

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6
Q

Define the term ‘shell’

A

A shell is an area in an atom, around its nucleus, where electrons are found.

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7
Q

Finish the sentence
All substances are made of tiny particles called ____________

A

All substances are made of tiny particles called atoms

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8
Q

Name the sub-atomic particles found in the atom

A

Protons, Neutrons and Electrons are sub-atomic particles are found in the atom

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9
Q

Name the sub atomic particles that make up the nucleus of an atom

A

Protons and Neutrons are found in the nucleus of an atoms

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10
Q

Where is the nucleus in an atom

A

The nucleus is in the middle of the atom

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11
Q

Where are the electrons found in

A

Electrons are found in electron shells, outside of the nucleus

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12
Q

What is an ion

A

An ion is a charged particle produced by the loss or gain of electrons

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13
Q

Define the term ‘element’

A

An element is a pure substance containing only one type of atom. An element cannot be broken down chemically into any simpler substance.

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14
Q

Define the term ‘compound’

A

A compound is a pure substance made when two or more different types of atoms are chemically bonded together.

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15
Q

Define the term ‘mixture’

A

A mixture is made up of two or more different substances that are not chemically bonded together

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16
Q

Why is a mixture easy to separate

A

A mixture is easy to separate as the substances that make up the mixture are not chemically bonded together.

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17
Q

Define the term ‘pure’

A

Pure - a material made up of one type of substance.

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18
Q

Define the term ‘molecule’

A

A particle made up of at least two atoms chemically bonded together by covalent bonds

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19
Q

State the relative mass of a proton

A

The relative mass of a proton is 1

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20
Q

State the relative mass of a neutron

A

The relative mass of a neutron is 1

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21
Q

State the relative mass of an electron

A

State the relative mass of a electron is 1/2000

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22
Q

Finish the sentence: Most of an atom is _________

A

Most of an atom is empty space

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23
Q

State the relative charge of the sub-atomic particles

A

Proton = +1
Neutron = 0
Electron = -1

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24
Q

Why does the nucleus have a positive charge

A

The nucleus is positively charged as the only charge in the nucleus are the protons which are positively charged. The neutrons have no charge.

25
Q

Draw the electronic structure (dot and cross diagram) of sodium
State it’s electron configuration

A

Sodium - 2, 8, 1

26
Q

Identify the mass number and the atomic number

https://d17hukvrbysd4e.cloudfront.net/blogImages/atomic-number-and-mass-number.jpg

A
27
Q

Define the term ‘mass number’

A

The mass number is the total number of protons and neutrons in the nucleus of a given atom.

28
Q

Define the term ‘atomic number’

A

The atomic number is the total number of protons in the nucleus of a given atom

29
Q

How would you find out how many neutrons an atom has.

A

Number of neutrons = mass number - atomic number

30
Q

What does the atomic number determine

A

The atomic number determines the type of atom. (For example, any atoms with 6 protons are carbon atoms)

31
Q

Explain why an atom is uncharged

A

An atom is uncharged as it has an equal number of positively charged protons and negatively charged electrons. These charges cancel out.

32
Q

Define the term isotope

A

Isotope - Atoms that have the same number of protons but a different number of neutrons

33
Q

Give an example of Isotopes

A

Carbon-12, Carbon-13, Carbon-14, Chlorine-35, Chlorine-37

34
Q

How are isotopes named

A

Isotopes are named by their mass number. For example Carbon-12 has a mas number of 12 (6 protons and 6 neutrons)

35
Q

Work out the number of protons, neutrons and electrons in:
Carbon-12
Carbon-13
Carbon-14

A

Carbon-12 : 6 protons, 6 electrons, 6 neutrons
Carbon-13 : 6 protons, 6 electrons, 7 neutrons
Carbon-14: 6 protons, 6 electrons, 8 neutrons

36
Q

When do you use relative atomic mass instead of mass number

A

The relative atomic mass is used when referring to the element as a whole

37
Q

Define the term ‘ relative atomic mass’ - A (subscript r)’

A

The relative atomic mass is the average mass of the atoms of an element, taking into account the different masses and abundances of all isotopes that make up the element.

38
Q

State the formula for relative atomic mass

A

relative atomic mass (A subscript r) = sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes

39
Q

Copper has two stable isotopes. Cu-63 has an abundance of 69.2% and Cu-65 has an abundance of 30.8%. Calculate the relative atomic mass of copper to 1 d.p.

A

relative atomic mass (A subscript r) = sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes

relative atomic mass = (69.2 x 63) + (30.8 x 65)/69.2+30.8
= 4359.6 + 2002/100
= 6361.6/100
= 63.616 = 63.6 (to 1.d.p)

40
Q

What term do you use (instead of mass number) when referring to the element as a whole

A

The relative atomic mass is used when referring to the element as a whole

41
Q

Complete the sentence
Isotopes exist in different _________ (some isotopes are more common than others)

A

Isotopes exist in different quantities (some isotopes are more common than others)

42
Q

What can energy levels also be called

A

Energy levels can be called ‘shells’

43
Q

How many electrons can each shell hold

A

1st shell - 2
2nd shell - 8
3rd shell - 8 etc.

44
Q

What does the period number tell you?

A

In the periodic table, the period number is equivalent to the number of electron shells an atom contains

45
Q

What does the group number tell you

A

In the periodic table, the group number shows the number electrons an atom has in it’s outer most shell.

46
Q

Which shell is the highest energy level
(1st, 2nd, 3rd shell)

A

The third shell is the highest energy level.

47
Q

Finish this sentence
As the distance from the nucleus increases, the _____ in the ______/_________ also increases

A

As the distance from the nucleus increases, the energy in the energy shell/electron also increases.

48
Q

What type of ions do metals form

A

Metals form positive ions

49
Q

What type of ions do non-metals form

A

Non-metals form negative ions

50
Q

What do metals need to do in order to form positive ions

A

A metal loses electrons to form positive ions

51
Q

What do NON METALS need to do in order to form NEGATIVE ions

A

A non-metal needs to lose electrons to form positive ions.

52
Q

Why do atoms react with other atoms

A

Atoms react with atoms, to gain, lose or share electrons from in order to achieve a full outer shell (noble gas configuration)

53
Q

Draw the electronic structure of a sodium ion
(state it’s electronic configuration)

A

https://www.gcsescience.com/sodium-ion.gif
[2,8]+

54
Q

Draw the electronic structure of an oxide ion

A

https://bam.files.bbci.co.uk/bam/live/content/z3tn4qt/small
[2,8]-

55
Q

What do group 4 elements do in terms of electrons

A

Group 4 atoms share electrons
Group 4 atoms don’t form ions but share electrons and form compounds.

56
Q

Why don’t noble gases need to form ions.

A

Noble gases do not need to form ions as they have a full outer shell (they all have 8 electrons in their outer shell, apart from helium which has 2). This means that they do not need to gain or lose (or share) electrons to achieve a full outer shell, to become stable.

57
Q

Why are Noble Gases so unreactive

A

Noble gases are unreactive because they have a full outer shell (they all have 8 electrons in their outer shell, apart from helium which has 2). This means that they do not need reactions to lose or gain or share electrons to achieve a full outer shell

58
Q

Where in the atom is majority of the mass.

A

Majority of the mass of an atom is in the nucleus

59
Q

When fluorine becomes an ion, what is it called

A

When fluorine becomes an ion, it is called a fluoride ion

GCSE Chemistry (43 decks)

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