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chemistry > atomic structure + the periodic table > Flashcards

atomic structure + the periodic table Flashcards

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1
Q

Define malleable.

A

The ability of a metal to be formed into different shapes.

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2
Q

Define ductile.

A

The ability of a material to stretch and deform permanently.

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3
Q

Define brittle.

A

When a material fractures, breaks or snaps.

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4
Q

What 4 physical processes separate mixtures?

A

~Filtration
~Crystallisation
~Simple and fractional distillation
~Chromatography

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5
Q

What are mixtures?

A

2 or more elements or compounds that are not chemically combined.

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6
Q

What is the mass number?

A

Total number of protons and neutrons.

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7
Q

What is the atomic number?

A

The number of protons in an atom of an element.

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8
Q

What is the relative atomic mass an average of?

A

The abundance of isotopes of the element.

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9
Q

How do you calculate relative atomic mass?

A

(Isotope 1 mass x abundance) + (Isotope 2 mass x abundance) divided by 100

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10
Q

How is a compound formed or separated?

A

From elements and by chemical reactions.

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11
Q

What is the electronic structure?

A

When electrons occupy the lowest available energy levels/shells closest to the central nucleus.

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12
Q

John Newlands ordered his periodic table by…

A

Atomic weight (+the law of octaves)

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13
Q

What is law of octaves?

A

That similar properties occurred every 8th element.

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14
Q

When did the law of octaves stop working?

A

After calcium.

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15
Q

Dmitri Mendeleev ordered his periodic table by…

A

Atomic mass.

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16
Q

How is the current periodic table arranged?

A

Elements are in order of atomic number.

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17
Q

Elements with similar properties are…

A

In the same group.

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18
Q

Elements in the same group have the same amount of…

A

Electrons in their outer shell.

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19
Q

Metals react to form…

A

Positive ions.

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20
Q

Non metals do not…

A

Form positive ions.

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21
Q

When were electrons, protons and neutrons discovered?

A

In the early 20th century.

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22
Q

What disproved the order of atomic weight?

A

Knowledge of isotopes.

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23
Q

How many electrons do group 1/ alkali metals have in their outer shell?

A

1.

24
Q

What happens to reactivity as you go down group 1?

A

It increases.

25
Q

What do group 1/alkali metals react with water to form?

A

An alkaline solution and hydrogen.

26
Q

What do the group 1/alkali metals react with oxygen to form?

A

An oxide.

27
Q

What do the group 1/alkali metals react with chlorine to form?

A

A white precipitate.

28
Q

What happens when lithium reacts with oxygen?

A

A red flame and white solid is produced.

29
Q

What happens when lithium reacts with water?

A

It fizzes and gradually disappears.

30
Q

What happens when lithium reacts with chlorine?

A

A white powder is produced.

31
Q

What happens when sodium reacts with oxygen?

A

An orange flame and white solid is produced.

32
Q

What happens when sodium reacts with water?

A

It melts, fizzes and disappears quickly.

33
Q

What happens when sodium reacts with chlorine?

A

Yellow flame and clouds of white powder are produced.

34
Q

What happens when potassium reacts with oxygen?

A

A lilac flame is produced.

35
Q

What happens when potassium reacts with water?

A

Produces sparks and a lilac flame then disappears.

36
Q

What happens when potassium reacts with chlorine?

A

There is a more vigorous reaction than sodium.

37
Q

How many electrons do the group 0/ noble gases have in their outer shell?

A

8 (full).

38
Q

Which noble gas is an exception?

A

Helium as it only has 2 electrons in its full outer shell.

39
Q

What increases going down the group in group 0/ noble gases?

A

The boiling points and relative atomic mass.

40
Q

Why are the group 0 elements/ noble gases unreactive?

A

They have a stable electron arrangement meaning they don’t form molecules easily.

41
Q

What are transition elements like compared to group 1 elements.

A

~Much less reactive
~Are harder and stronger
~Higher melting points and density (except for mercury)

42
Q

What is manganese used as a catalyst for?

A

The decomposition of hydrogen peroxide.

43
Q

What is iron used as a catalyst for?

A

The haber process.

44
Q

What is nickel used as a catalyst for?

A

The manufacture of margarine.

45
Q

What are the typical properties of transition metals?

A

~Useful as catalysts
~Form coloured compounds
~Have ions with many different charges

46
Q

What are the properties of chromium?

A

Lustrous, brittle and hard metal.

47
Q

What are the properties of manganese?

A

Hard and very brittle, difficult to fuse, easy to oxidise.

48
Q

What are the properties of copper?

A

Highly ductile and conductive, malleable and soft.

49
Q

What are the properties of cobalt?

A

Brittle and hard with a high melting point.

50
Q

What are the properties of nickel?

A

Hard, malleable and ductile, decent conductor of heat and electricity.

51
Q

What are the properties of iron?

A

Good conductor, rusts easily in air and is strong,ductile and malleable.

52
Q

How many electrons does group 7/ the halogens have in their outer shell?

A

7.

53
Q

What forms when the group 7 elements/ the halogens react with metals?

A

Ionic compounds.

54
Q

What forms when the group 7 elements/ the halogens react with non metals?

A

Covalent compounds with a shared pair of electrons.

55
Q

What increases as you go down group 7/ the halogens?

A

~Relative molecular mass
~Melting and boiling point

56
Q

Why does reactivity decrease down group 7/ the halogens?

A

~As halogens react by gaining an electron
~Number of shells increase so less other electrons are attracted

57
Q

A decrease in reactivity in group 7 / the halogens means…

A

A more reactive halogen can displace a less reactive halogen in the aqueous solution of its salt.

chemistry (7 decks)

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