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GCSE chemistry > C2 > Flashcards

C2 Flashcards

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1
Q

What area of the periodic table are the metals found in

A

Left

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2
Q

What area of the periodic table are the non metals found in

A

Right.

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3
Q

Rows are called…

A

Columbs

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4
Q

Vertical columns are called…

A

Groups

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5
Q

What does the group number tell you about the element

A

How many electrons the have in their outer shell

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6
Q

What type of ion do metals form when they react

A

Positivte ion

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7
Q

What do atoms generaLly react to form

A

A full outershell

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8
Q

What type of bond do metals have

A

Mettalic bond

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9
Q

What does a metallic bond cause metals to have

A

A similar basic physical propeties

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10
Q

What are metals great at

A

Conducting heat and electricity

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11
Q

What are group 1 elements know as

A

Alkali metals

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12
Q

What elements are in group 1

A

Lithium, sodium, pottasium, rubidium, caesium and francium

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13
Q

How many electrons do group 1 elements contain in their outershell and what does this mean

A

They all have 1 electron in their outershell meaning this makes them very reactive and have similar properties.

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14
Q

What are some properties of group 1 elements

A

Soft, low density

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15
Q

Trends in group 1

A
  • as you go down, increase in reactivity - as you go down, the electron gets further away from nucleus meaning the attraction between nucleas decreases
  • meaning lower melting points and boiling points as you go down
  • higher relative atomic mass as you go down
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16
Q

What ion do alkali metals form

A

+1 ion

17
Q

What happens when alkali metals react with water?

A

They react vigorously. More reactive as you go down. Lithium pottasium sodium float and move around whilst fizzing vigourously. They also produce hydrogen

18
Q

What is produced when reacted with chlorine

A

White salts called metal chlorides.

19
Q

What happens when alkali metals react with oxygen

A

They form metal oxide.
Lithium = lithium oxide
Sodium = sodium peroxide & sodium oxide
Pottassoum = pottassium peroxide & pottassium superoxide

20
Q

What are group 7 elements known as

A

Halogens

21
Q

Halogens and their appearence

A

Fluorine - very reactve, poisonous yellow gad
Chlorine - fairly reactive, poisenous dense green gas
Bromine - dense, poisonous red-brown volatile liquid
Iodine - dark grey crystalline solid or a purple vapour

22
Q

Trends of halogens

A

As you go down…
Less reactive - harder to gain an extra electron as further away from nucleus
Higher melting and boiling points
Higher relative atomic masses

23
Q

How many electrons are in halogens outer shell

A

7

24
Q

What can halogens form to get a full outershell?

A

Molecular compounds: share electrons via covalent bonding with other non metals. The compounds which form all have a simple-molecular structure

25
Q

What ion do halogens form

A

1- ion called halides when they react with metals. These all have ionc structures

26
Q

In halogens, how can a displacement reaction occur?

A

When a more reactive halogen reacts with a salt of the less reactive one

27
Q

What are group 0 elements called

A

Noble gases

28
Q

How many electrons do noble gases have in their outer shell and what does this mean

A

8 meaning they are extremely unreactive as they have a full outershell

29
Q

What are noble gases all?

A

Inert colourless gases.

30
Q

What do noble gases exist as

A

Monatomic gases

31
Q

What are the patterns in properties in noble gases!

A

Boiling points Increase as you go down.

32
Q

How do you find out the trend in reactivity in a group in the period table?

A

If the elements are trying to lose 1 or more electrons, the reactivity will increase because as the electrons get further away from the nucleus, it is easier to lose the electron. But if the elements are trying to gain, the reactivity decreases as it is harder to gain electrons as the electrons are further away from the nucleus

33
Q

What does electrostatic attraction depend on?

A

-the distance between the outermost electrons and the nucleus

-the number of occupied inner shells of electrons which have a shielding effect

-the size of the positive charge on the nucleus

34
Q

What to factor to decide how easy it is for atoms to lose or gain electrons from their outershell?

A

-the increased nuclear charge
-due to extra protons in the nucleus

35
Q

Problems with categorising elements in the 1800s:

A

-scientists had no idea of atomic structure or of protons
-only thing you could measure was atomic weight

36
Q

Why did mendaleev leave gaps?

A

To make sure thst elements with similar properties stayed in the same group. Some of these groups indicated the existence of undiscovered elements

37
Q

What did the discovery of isotopes confirm?

A

That mendaleev was correct not to place elements in a strict order of atomic weight but to also account for their properties

38
Q

Physical properties of metal?

A

-strong and can be bent or hammered
-great at conducting heat and electricity
-high melting and boiling points

39
Q

Non-metal physical properties?

A

-dull looking
-brittle
-low density
-dont conduct electricity

GCSE chemistry (10 decks)

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