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Chemistry > C4 - Chemical Patterns > Flashcards

C4 - Chemical Patterns Flashcards

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1
Q

What two properties are elements groups based on?

A

Relative atomic mass and properties

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2
Q

What did Johann Döbereiner do?

A

He noticed triads that linked patterns of the relative atomic masses of three elements

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3
Q

What did John Newlands do?

A

Noticed octaves where every eight element had similar properties

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4
Q

Why did scientists reject Döbereiner and Newlands’ ideas and accept Mendeleev’s?

A

The triads and octaves patterns didn’t work for all elements

New elements that were discovered fitted Mendeleev’s predictions

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5
Q

How was helium discovered?

A

Scientists looked at the light from the sun, split it using a prism and examined it’s line spectra noticing helium amongst it

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6
Q

What is the charge and mass for all three parts of an atom?

A

Proton, +1 charge, mass of 1
Neutron, 0 charge, mass of 1
Electron, -1 charge, mass of nearly 0

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7
Q

How can you work out the relative atomic mass of an element?

A

Proton number + neutron number = relative atomic mass

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8
Q

Give an example of how electron arrangements are used using Oxygen (8 electrons):

A

With dots e.g. 2.6

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9
Q

Number of electrons in an atom is _________ the proton number

A

Equal to

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10
Q

How many electrons are allowed in the first 4 shells and how can this information be found in the periodic table? (5)

A

In Shell 1=2, 2=8, 3=8, 4=18

Number of elements in a period = number of electrons allowed in that shell

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11
Q

The _____ an electron shell is to the nucleus, the _____ the energy level

A

Closer, lower

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12
Q

Period

A

A row in the periodic table

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13
Q

The _____ the proton number, the _____ the melting point and the _____ the boiling point

A

Higher, lower, higher

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14
Q

Describe the main properties of Elements in group 0 (2)

A

They have full outer shells and are Unreactive or inert gases

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15
Q

Link the number of outer shell electrons to an element’s likelihood to be metal or non metal:

A

Elements with up to 3 electrons in their outer shell are metals

Elements with 5 or more electrons in their outer shell are non metals

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16
Q

Group

A

A vertical column in the periodic table

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17
Q

Describe group 1 elements (3)

A
  • Alkali metals
  • Can be cut with a knife to reveal a shiny surface
  • they tarnish quickly in moist air
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18
Q

How are group 1 elements stored? And why?

A

In oil, to prevent them from reacting with air or water

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19
Q

The _______ the group one element in the periodic table, the ______ reactive

A

Lower down = more reactive

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20
Q

What are the chemical hazards of group one metals and their products? (3)

A

They are flammable and their hydroxides are harmful and corrosive

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21
Q

What is the equation for the reaction of a group one element and water?

A

Metal + water -> metal hydroxide + hydrogen

22
Q

The general balanced with state symbols equation for the reaction of group one elements is? (Using M to represent them)

A

2 M(s) + 2 H2O(l) -> H2(g) + 2 MOH (aq)

23
Q

Where are the transition metals in the periodic table?

A

In the middle

24
Q

Thermal disposition

A

Thermal disposition: when a substance breaks down into two or more substances

25
Q

What are the general properties of metals? (5)

A

Good conductors, high melting + boiling points, shiny, dense, strong

26
Q

What is the name of the group 7 elements?

A

The halogens

27
Q

What is the appearance of chlorine at room temperature and what is the colour of its gas?

A

Pale green gas at room temperature

28
Q

What is the appearance of bromine at room temperature and what is the colour of its gas?

A

Red-brown liquid at room temperature and reddish brown gas

29
Q

What is the appearance of iodine at room temperature and what is the colour of its gas?

A

Dark grey solid at room temperature and purple gas

30
Q

Diatomic molecules

A

Molecules of elements that always feature two atoms joined together

31
Q

As you go down the halogen group the melting and boiling points ______

A

Increase

32
Q

What are the chemical hazards of he halogens and how must they be used?

A

They are corrosive and toxic and must be used in a fume cupboard

33
Q

What do group 7 elements react with metals to form?

A

Metal halides

34
Q

Further down the halogen group, they become _____ reactive

A

Less reactive down the group

35
Q

Displacement reactions

A

When a more reactive halogen takes the place of a less reactive halogen in a compound

36
Q

What are the uses of chlorine and iodine?

A

They are used for sterilising wounds and water

37
Q

Ionic compounds

A

Compounds made of ions of different elements

38
Q

Crystal lattice

A

The regular pattern that ionic compounds are arranged in

39
Q

What state do ionic compounds need to be in to conduct electricity and why?

A

They need to be dissolved or melted so that the ions are fee to move to the electrodes to complete the circuit

40
Q

What are the main properties of ionic compounds? (3)

A
  • Solid
  • High melting points
  • Soluble
41
Q

Electrolysis

A

The process by which electricity is passed through ionic compounds to break them down into other substances

42
Q

In electrolysis what is the charge of the anode?

A

Positive

43
Q

In electrolysis what is the charge of the cathode?

A

Negative

44
Q

In electrolysis what is the charge of the anions and what are they?

A

Negatively charged ions that are attracted to the anode

45
Q

In electrolysis what is the charge of the cathions and what are they?

A

Positively charged ions that are attracted to the cathode

46
Q

Covalent bonding

A

When two elements are bonded by sharing electrons

47
Q

What are the properties of covalently bonded elements? (3)

A

Gases/ liquids with low melting and boiling points that don’t conduct electricity

48
Q

Ionic bonding

A

When elements gain electrons from or lose electrons to other elements and become charged

49
Q

What charge are elements of group 1 and elements of group 7 when ionised?

A

Group 1 = 1+ charge

Group 7 = 1- charge

50
Q

Isotopes

A

Atoms of an element with a different number of neutrons

51
Q

What does the state symbols: s, l, g and aq mean?

A 
s = solid
l = liquid
g = gas
aq = aqueous
52
Q

Who arranged the periodic table?

A

Russian Chemist Dmitri Mendeleev

Chemistry (6 decks)

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