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Chemistry GCSE! > Periodic Table > Flashcards

Periodic Table Flashcards

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1
Q

Does reactivity increase or decrease down group 1? Why?

A

Increase

The atoms get larger, so the electrostatic attraction between the outer electron and the positive nucleus is weaker so the electron is more easily lost

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2
Q

Does reactivity increase or decrease down group 7? Why?

A

Decrease

The atoms get larger, which means the electrostatic attraction between the positive nucleus, and the electron being gained is weaker, which makes it harder to gain the electron

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3
Q

Do transition metals have a high or low melting point?

A

High

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4
Q

Does mp/bp increase or decrease down group 1?

A

Decreases

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5
Q

Does mp/bp increase or decrease down group 7?

A

Increases

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6
Q

Are transition metals reactive?

A

Not really

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7
Q

Are transition metals good conductors?

A

Good thermal conductors

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8
Q

Are group 1 metals good thermal conductors?

A

👍

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9
Q

Colour of the compounds group one metals make

A

White

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10
Q

What colour are the compounds that transition metals make?

A

Various colours

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11
Q

Do both group 1 metals and transition metals form ionic compounds with non metals?

A

👍

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12
Q

Are group one metals ALL diatomic??

A

NO
none are
Group seven is made up of all diatomic molecules

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13
Q

What is the name given to group 7

A

Halogens

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14
Q

What’s the name given to group 0/8??

A

Noble gases

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15
Q

What’s special about the electron structure of the noble gases?

A

Full outer shells

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16
Q

Are noble gases reactive?

A

No because they have full outer shells and do not need to share or transfer electrons

17
Q

Some food packets contain argon gas - why??

A

It’s unreactive so the food will not go stale and will stay fresh
Argon is the most abundant noble gas

18
Q

Intermolecular forces _________ down the group

(Noble gases)

A

Increase

19
Q

Give two differences between the physical properties of elements in group 1 and those in the transition elements

A

Group one has low density

Group 1 has relatively low mps

20
Q

Relative Melting points across table

A

⬇️ ⬆️ ⬇️ ⬇️

Groups:
1. Tm. 7. 0.

21
Q

Reactivity across table

A

Down group reactivity

⬆️. ❌. ⬇️. ❌.

22
Q

Describe Newlands table

A

He arranged them in order of increasing atomic mass
He found that every eight elements had similar properties, so arrange them in eight groups
He called it, the law of octaves

23
Q

What problems were found with Newlands table, and why wasn’t it accepted?

A

There were no gaps left for undiscovered elements, so there were many more dissimilar elements in a column and no room for new elements

24
Q

Mandeleev organise the elements in order of…

A

Atomic weight
Also known as relative atomic mass

25
Q

Mandeleev organise the elements in order of atomic weight. This meant that some elements were…

A

In the wrong order, and sometimes place in groups with elements that were similar
This led to pair reversals
E.g. iodine and Tellurium
Iodine has low atomic weight, however, similar chemical properties to chlorine and bromine so they were switched

26
Q

Two special features of Mandeleev periodic table were…

A

It had gaps
It showed elements with similar chemical properties lined up in groups

27
Q

The gaps in Mandeleev’s periodic table were important, because

A

It was easier to make predictions about undiscovered elements and their properties

28
Q

How is the periodic table organised now?

A

Elements
- organised in order of creasing atomic number
- groups of elements with similar properties

29
Q

What does the period number tell us?

A

The number of occupied electron shells

30
Q

What does the group number tell us?

A

The number of electrons in the outer shell of an element

31
Q

What does the term periodic mean in terms of the periodic table?

A

Repeating properties

32
Q

How were the pair reversals resolved?

A

Isotopes
Because tellurium is 128, 130 was so abundant

Chemistry GCSE! (11 decks)

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