the Periodic table Flashcards

1
Q

What are group 0 elements known as?

A

noble gases

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2
Q

noble gases have full outer shells which means ….

A

they have a very stable electron configuration making them unreactive and do not easily form molecules

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3
Q

boiling points of noble gases increases….

and why

A

with relative atomic mass (going down the group)

this is because the atoms get larger so the intermolecular forces between forces become stronger = more energy needed to overcome these forces

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4
Q

What are group 1 elements known as?

A

alkali metals

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5
Q

how many electrons does group 1 have in the outer shell?

A

1

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6
Q

Group 1 boiling and melting point _______ as you go down the group

A

decreases

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7
Q

Why does Group 1 become more reactive as you go down the group?

A

because the outer electron gets further away from the influence of the nucleus, so it can be lost more easily

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8
Q

Why are alkali metals stored under oil?

A

because they react vigourously with oxygen and water, inclucding moisture in the air

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9
Q

alkali metal + water =

A

metal hydroxide + hydrogen gas

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10
Q

Group 1 metals have _________ density

A

low

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11
Q

which group 1 metals float because they are less dense than water?

A

sodium, lithium and potassium

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12
Q

metal hyrdoxide dissolved in water =

A

alkaline solution

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13
Q

alkali metals + non-metals =

A

ionic compounds

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14
Q

What are group 7 (which are non-metals) known as?

A

halogens

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15
Q

why do group 7 elements have similar reactions

A

because they all have 7 electrons in their outer shell

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16
Q

reactivity in group 7 elements ________ as you go down the group

17
Q

why does reactivity in group 7 elements decrease as you go down the group

A

because the outer shell gets further away from the nucleus, so it is less easy to gain an electron

18
Q

The further down Group 7 the element is ________ its relative molecular mass, melting point and boiling point

A

the higher

19
Q

Halogens + metals =

A

ionic salts

20
Q

what happens when halogens and metals react?

A

a halide ion with a negative charge (-1) is formed

21
Q

what happens when alkali metals react with non-metals?

ions

A

a metal ion with a positive charge (+1) is formed

22
Q

A more reactive halogen will __________ a less reactive halogen from an _____________ of its salt

A

displace

aqueous solution

23
Q

where are transtion metals?

A

in the centre of the periodic table, between groups 2 and 3

24
Q

what are the features of transition metals?

A
  • form coloured compounds

- they have ions with different charges

25
what are the properties of transition metals?
``` good conductors of heat and electricity can be easily bent or hammered into shape dense strong shiny ```
26
what can transition metals be used for?
catalysts to speed up chemical reactions
27
how did Newlands arrange the elements in the periodic table?
in order of atomic weight
28
Why was ordering elements in order of atomic weight a bad thing?
because some of the elements were in the wrong place
29
what did medeleev realised and what did he do
that some elements had yet to be discovered and left gaps to allow for their discovery used the periodic table to predict the existence and properties of new elements he also reordered some elements
30
How did Mendeleev reorder the elements?
each element was placed in a group with elements that had similar properties
31
what did scientists realise when subatomic particles were later discovered
that Mendeleev had organised the elemnts in order of increasing atomic number
32
transition metals are ______ reactive than alkali metals
less