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CHEMISTRY PAPER 1 GCSE FOUNDATION > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is an atom

A

An atom is the smallest piece of an element that can exist.

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2
Q

Atoms of different elements can be combined together to create what?

A

Atoms of different elements can be combined together to create compounds.

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3
Q

How many elements have been discovered

A

118 (or you can say around 100)

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4
Q

Na2O is the chemical _______ for sodium oxide.

A

Na2O is the chemical formula for sodium oxide.

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5
Q

Name four things that happen in a chemical reaction.

A
  1. At least one new substance must be formed.
  2. Detectable energy changes are common.
  3. No atoms are created or destroyed
  4. Compounds can be broken up or formed
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6
Q

Found on the right-hand side of chemical equations are the…

A

Products

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7
Q

Found on the left-hand side of chemical equations are the…

A

Reactants

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8
Q

Balance the symbol equation for the reaction of sodium with chlorine:
Na + Cl2 → 2NaCl.

A

2Na + Cl2 → 2NaCl.

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9
Q

What are the 2 types of chemical equations?

A
  1. word equations

2. symbol equations

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10
Q

What do you call a substance that is made up of 2 or more elements or compounds that haven’t been chemically combined together.

A

A mixture.

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11
Q

What is Chromatography used to separate?

A

Solutions with a different number of solvents (dissolved solids) in a solvent.

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12
Q

Give a 4 step description on the order of chromatography :

A
  1. A spot of the solution to be separated is placed at near the bottom of a chromatography paper.
  2. The paper is held up right. The bottom of the paper is dipped into a solvent.
  3. As the solvent soaks up the paper, it carries the solutes in the spot with it. The different solutes (solids) in the spot of solution, move at different speeds.
  4. This leaves a pattern of the separate solutes on the chromatography paper.
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13
Q

A) How many types of distillation are there?

B) What are the types of distillation called?

A

A) 2 types

B) Simple distillation, Fractional distillation.

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14
Q

Name 5 ways of separating mixtures.

A
  1. Simple distillation
  2. Fractional distillation
  3. Crystallisation
  4. Chromatography
  5. Filtration
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15
Q

A) What is crystallisation used for?

B) How is it done?

A

A) Crystallisation is used to separate the dissolved solid (solute) in a solution from the liquid (solvent).
B) It is done by heating the solution until the solvent evaporates. Left behind will be crystals of the solute.

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16
Q

Who thought up the plum pudding model of the atom?

A

J.J Thomson

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17
Q

Who discovered electrons?

A

J.J Thomson

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18
Q

What was the idea of the plum pudding model?

A

A ball of positive charge (dough), with negatively charged electrons (currants) mixed in with the ‘dough’.

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19
Q

When did J.J Thomson discover electrons?

A

1897

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20
Q

What did Ernest Rutherford’s discover?

A

Nuclear model : He had made an alpha scattering experiment where they fired alpha particles into gold foil and found that some alpha particles bounced back. This then led to his discovery of the nucleus that contained positively charged particles called protons.

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21
Q

In the alpha scattering experiment, why did the alpha particles bounce back?

A

This was because the alpha particles were positively charged. The alpha particles that came close to the nucleus would deflect or change direction. When the particles would bounce straight back, it meant that it had hit the positive protons in the nucleus.

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22
Q

Who was the developer of the modern model of the atom?

A

Niels Bohr

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23
Q

What was Niels Bohr’s discovery?

A

Niels Bohr discovered that electrons orbit (fly around) the nucleus at fixed distances.

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24
Q

A) What did James Chadwick discover?

B) When was James Chadwick’s discovery?

A

A) In 1932, James Chadwick discovered that some particles in the nucleus have no charge at all. He called them neutrons.
B) 1932

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25
Q

A) What is the relative charge of a proton?

B) Where are protons found in the atom?

A

A) Protons have a relative charge of +1

B) Protons are found in the nucleus

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26
Q

What does the atomic number of an element tell us?

A

Atomic number = number of protons the element has.

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27
Q

What is the average radius of atoms?

A

0.1 nanometres

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28
Q

How is the mass number (or relative mass) in an atom calculated?

A

The number of protons + the number of neutrons

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29
Q

What is the relative mass of an electron?

A

Approximately 0

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30
Q

How many times smaller is the nucleus of an atoms size compared to the atom ?

A

10,000

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31
Q

What is another name for the columns of the periodic table?

A

Groups

32
Q

Who was the first chemist to devise a periodic table?

A

John Newlands

33
Q

How was the first periodic table ordered?

A

By the weight of an element

34
Q

What did Dmitri Mendeleev realise and then do?

A

He realised that there might be undiscovered elements so he left gaps for them

35
Q

What did Dmitri Mendeleev predict?

A

He predicted the properties and masses of the undiscovered elements

36
Q

How did Dmitri Mendeleev order the periodic table?

A

By atomic number (number of protons)

37
Q

How is the modern periodic table slightly different to the previous periodic table by Dmitri Mendeleev?

A

It has the gaps that he left empty, now filled in with discovered elements.

38
Q

What discovery proved Mendeleev’s periodic table to be correct and Newlands’ to be wrong?

A

The discovery of protons and isotopes.

39
Q

Name 3 properties of metals.

A
  1. High melting and boiling points.
  2. Good conductors of heat and electricity
  3. All solids (except for mercury which is liquid at room temperature).
40
Q

Where are metals found on the periodic table and why?

A

Metals are found on the left of the periodic table because they have few electrons in their outer shell.

41
Q

What happens when metals react?

A

When metals react, they lose 1 or more of these negatively charged electrons to form positively charged ions.

42
Q

Where are non-metals found in the periodic table and why?

A

Non-metals are found on the right of the periodic table because they have many electrons in their outer shell.

43
Q

Name 3 properties of non-metals.

A
  1. Lower melting and boiling points.
  2. Often found as gases.
  3. Generally do not conduct heat or electricity.
44
Q

What are rows of the periodic table called?

A

Periods.

45
Q

What are isotopes?

A

Isotopes are atoms with the same number of protons but that have a different number of neutrons. ( we can also say that isotopes are elements with the same atomic number but different mass numbers).

46
Q

Define protium and its properties.

A
  1. Protium is a hydrogen atom with 1 proton and 0 neutrons.
  2. 99.98% of hydrogen atoms are protium.
  3. It is used in hydrogen fuel cells and the production of plastics.
47
Q

Define deutrium and its properties.

A

Deuterium is a hydrogen atom with 1 proton and 1 neutron.
Around 0.02% of hydrogen atoms are deuterium.
It is used in nuclear fusion.

48
Q

Define tritium and its properties.

A
  1. Tritium is a hydrogen atom with 1 proton and 2 neutrons.
  2. It is very rare.
  3. It is used in thermonuclear fusion weapons.
49
Q

How many protons do hydrogen atoms contain?

A

1

50
Q

What are the 3 isotopes of hydrogen?

A
  1. Protium
  2. Deutrium
  3. Tritium
51
Q

What is relative atomic mass (Ar)?

A

The relative atomic mass (Ar) is the average mass of all of the isotopes of an element. It takes into account how often each isotope is found (the isotope abundance)

52
Q

What is the formula for calculating relative atomic mass?

A

(isotope abundance% x isotope mass number)
__________________________________
isotope abundance%

53
Q

Calculate the relative atomic mass for chlorine

A

Cl may exist as 2 isotopes, 35Cl and 37Cl.
Isotope abundances:
75% 35Cl
25% 37Cl
so Ar = (0.75 x 35) + (0.25 x 37) = 35.5.

54
Q

What is the maximum capacity of electrons in the inner shell that is closest to the nucleus?

A

Maximum of 2 electrons.

55
Q

What is the maximum capacity of electrons in the next 2 shells (2nd and 3rd closest to the nucleus) after the inner shell.

A

Maximum of 8 electrons.

56
Q

An argon atom has 18 electrons, what is the electronic configuration for this argon atom?

A

2,8,8

57
Q

A calcium atom has 20 electrons, so the electron configuration is:
                   

A

2,8,8,2

58
Q

A phosphorous atom has 15 electrons, so the electron configuration is:
                   

A

2,8,5

59
Q

Tritium has _ neutrons. (fill in the blank)

A

2

60
Q

The most common isotope has _ neutrons.

A

0

61
Q

Which group is the noble gases?

A

Group 0

62
Q

Why are elements in group 0 unreactive?

A

They do not gain or lose electrons to fill up this shell as it is already full.

63
Q

Monatomic definition:

A

Consisting of only one atom.

64
Q

Diatomic definition:

A

Molecules composed of only two atoms. (They share electrons)

65
Q

What type of molecule do noble gases exist as?

A

Monatomic.

66
Q

1) What type of boiling points do the noble gases have?
2a) Do the boiling points of the gases increase or decrease moving down the periodic table?
2b) Give a reason why to contribute to your answer in question 2a.

A

1) Low boiling points.
2a) Their boiling points increase as you move down the periodic table.
2b) This is because the relative atomic mass increases lower down the periodic table.

67
Q

A) What type of density do the noble gases have?

B) Does the density increase or decrease as you move down the periodic table and why?

A

A) Low density

B) Their densities do increase as you move down the periodic table because of their increasing relative atomic mass

68
Q

Which group are the halogens?

A

Group 7

69
Q

Are halogens reactive or unreactive and why?

A

They have 7 electrons in their outer energy level/shell. They are very reactive because they easily accept an electron into this outer shell.

70
Q

How many electrons can a halogen gain and what type of ion does it form?

A

They can gain only 1 electron in chemical reactions and form a negative ion.

71
Q

What type of molecule do halogens exist in?

A

Diatomic molecules

72
Q

How are salts formed in a chemical reaction?

A

When a metal atom transfers its outer electron to a non-metal atom (like a group 7 atom), salts are formed.

73
Q

What is the result of a chemical reaction involving non-metals and metals.

A

A compound where both outer energy levels are full.

74
Q

Describe the reactivity of halogens. (Make 4 points)

A
  1. As you go down the group, the halogens become less reactive. This is because:
  2. The atoms gain more electron shells.
  3. The outer electron shell is further from the nucleus.
  4. The attraction between the nucleus and the electron (to be gained from another element) decreases
75
Q

What is the formula to calculate Rf?

A

distant travelled by substance
Rf= ____________________________
distance travelled by solvent

76
Q

Fill in the blank

Chlorine + ________=potassium chloride + bromine

A

Chlorine + potassium bromide = potassium chloride + bromine

CHEMISTRY PAPER 1 GCSE FOUNDATION (1 decks)

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