4.1.2🫧 Flashcards

1
Q

What are the elements of the periodic table arranged in?

A

In order of atomic number.

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2
Q

What do groups show?

A

Elements with similar properties, that are in columns.

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3
Q

What do elements in he same group have?

A

The same amount of electrons on the outer shells.

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4
Q

How did john newland the periodic table?

A

He ordered his table in order of atomic weight.
He realised properties occurred every 8th element. 9octaves)

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5
Q

How did Mendeleev arrange the periodic table?

A

He ordered the periodic table by order of atomic mass, but not always - in some places he changed the order based on atomic weights.

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6
Q

What did Mendeleev do that no one else had done before?

A

He left gaps for elements that he thought had not been discovered before.
He also predicted the properties of future elements such as aluminium.

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7
Q

What did the knowledge of isotopes explain?

A

It made it possible to explain why the order based on atomic weights was not always correct.

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8
Q

What happened with the discoveries of the subatomic particles and the periodic table?

A

It allowed the periodic table to be ordered in atomic number, when this was done all elements were placed in the correct groups.

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9
Q

What do metals react to form?

A

Positive ions (lose electrons)

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10
Q

How many elements are metals?

A

Majority

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11
Q

Where are the metals found on the periodic table?

A

Found too the left and towards the bottom of the periodic table.

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12
Q

What do non metals form when they react?

A

They form negative ions.

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13
Q

Where are non metals found on the periodic table?

A

Towards the right and top of the periodic table.

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14
Q

What are the names of the group 1 metals?

A

Alkali metals

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15
Q

What are the properties / characteristics of group 1?

A

Low density, soft, very reactive with oxygen and water.

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16
Q

What is the trend in reactivity as you go down the group?

A

It increases

17
Q

What happens to melting and boiling point as you go down the group 1

A

Decreases

18
Q

Group 1 metal + water =

A

Metal hydroxide + hydrogen

19
Q

Group 1 metal + chlorine =

A

Metal chloride salt

20
Q

Group 1 metal + oxygen =

A

Metal oxide

21
Q

What are group 0 called?

A

Noble gases

22
Q

What are the properties of group 0 gases?

A

Unreactive as they are inert (stable arrangement, full outer shells), colourless gases, non flammable.

23
Q

What happens to boiling point as you go down group 0

A

It increases

24
Q

What are group 7 called?

A

Halogens

25
Q

What are the properties of group 7 elements

A

They are diatomic / exist in pairs.
7 electrons on the pouter shells.

26
Q

What happens to reactivity as you go down group 7?

A

It decreases

27
Q

What happens to melting and boiling points as you go down group 7?

A

They increase.

28
Q

What type of reactivity occurs in group 7?

A

Covalent bonds with non metals, ionic bonds with metals. More reactive elements displace less reactive elements, from an aqueous solution of its salt.

29
Q

What are the properties of the transition metals. (Compare to group 1)

A

Are harder and stronger, higher melting points and densities, much less reactive and don’t react as vigorously with oxygen and water.

30
Q

What are the typical properties of transition metals?

A

They form ions with different charges. Form brightly coloured compounds. Are useful as catalysts.