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Chemistry - S1 > Periodic Table > Flashcards

Periodic Table Flashcards

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1
Q

Differences between Mendeleev’s table and Modern Periodic Table

A

Elements arranged in order of atomic weight - elements arranged in order of atomic number

No noble gases present (not discovered) - noble gases present

Gaps are left for undiscovered elements

No block of transition metals presents - a block of transition metals is present

No actinides or lanthanides present - actinides and lanthanides are present (block of elements at the bottom of the table.)

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2
Q

Differences between metal and non-metal

A

Melting point - High - Low ( except graphite and diamond)

Malleability - malleable - not malleable

Ductility - ductile - not ductile

Sonority - sonorous - not sonorous

Conduction of heat/electricity - Good - Poor

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3
Q

What are common factors of ionic equations

A

2 species
No spectator ions present

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4
Q

What is a displacement reaction? And ionic version of a displacement reaction

A

A more reactive element can displace a less reactive element in a compound

Magnesium + Copper Sulfate —> Magnesium sulfate + Copper

Mg + CuSO4 —> MgSO4 + Cu

Ionic equation removes spectator ions

Mg(s) + Cu(aq) —> Mg(aq) + Cu(s). (Add in charges)

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5
Q

What is an neutralisation reaction? And the ionic version?

A

When an alkaline and acidic substance neutralise each other and create a salt + water

E.g Sodium Hydroxide + Hydrochloric acid —> sodium chloride + water
NaOH + HCl —> NaCl + H2O

Ionic equation removes spectator ions

OH(aq) + H(aq) —> H2O(l). (Add in charges)

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6
Q

What is a precipitation reaction? And the ionic version?

A

Precipitation reactions occur when cations and anions in aqueous solution combine to form an insoluble ionic solid called a precipitate.

Barium chloride + sodium sulfate —> Barium sulfate + sodium chloride

BaCl2 + Na2SO4 —> BaSO4 + 2NaCl

Ionic

Ba(aq). + SO4(aq) —> BaSO4(s) (Add in charges)

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7
Q

oxidation reaction

A

Alkali metal + oxygen —> alkali metal oxide

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8
Q

Alkaline hydroxide reaction

A

Alkali metal + water —> alkali metal hydroxide + hydrogen

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9
Q

Why and how are group 1 metals stored?

A

They are stored in oil to stop them reacting with the oxygen

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10
Q

Properties of group 1 metals

A

Are metals with low density

Lithium, Sodium and Potassium are less dense than water and float on its surface.

Have low melting and boiling points

They are stored in oil as they tarnish rapidly in air

Are soft enough to be cut by a knife

Shiny when freshly cut but rapidly tarnish in air

React rapidly with water and form an alkaline solution alkaline and Hydrogen gas.

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11
Q

What are the observations for lithium’s reaction with water

A

> Moves on the water surface
bubbles
heat released
Li disappears at the end of the reaction
colourless solution produced

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12
Q

What are the observations for Sodium’s reaction with water

A

> Moves on the water surface
Na melts into a tiny ball
bubbles
heat released
Na disappears at the end of the reaction
colourless solution produced

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13
Q

What are the observations for Potassium’s reaction with water

A

> Moves on the water surface
K melts into a tiny ball
produces a lilac flame
bubbles
heat released
Na disappears at the end of the reaction
colourless solution produced
crackles at the end of the reaction

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14
Q

Word and symbol equation for lithium + water

A

Lithium + Water —> Lithium Hydroxide + Hydrogen
2Li(s) + 2H2O(l) —> 2LiOH(aq) + H2(g)

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15
Q

Word and symbol equation for Sodium + water

A

Sodium + Water —> Sodium Hydroxide + Hydrogen
2Na(s) + 2H2O(l) —> 2NaOH(aq) + H2(g)

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16
Q

Word and symbol equation for Potassium + water

A

Potassium + Water —> Potassium Hydroxide + Hydrogen
2K(s) + 2H2O(l) —> 2KOH(aq) + H2(g)

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17
Q

Symbol equation for half equations for group 1 ions

A

X —> x+ + e-
Na —> Na+ + e-

18
Q

Why does reactivity increase going down group 1

A

As you go down group 1 the outer shell’s electrons are further from the nuclear charge.

They are less strongly attracted to the positive nucleus and easier to lose.

19
Q

What colour is the halogen fluorine and what state is it at room temperature

A

Pale yellow - gas

20
Q

What colour is the halogen Chloride and what state is it at room temperature

A

Green-yellow. - gas

21
Q

What colour is the halogen bromine and what state is it at room temperature

A

Red-brown - liquid

22
Q

What colour is the halogen iodine and what state is it at room temperature

A

Grey-black - solid

23
Q

What happens to iodine when heated

A

Sublimes and produces a purple vapour

24
Q

Half equations for group 7 ions

A

X2 + 2e- —> 2X-
I2 + 2e- —> 2I-

25
Q

Why does reactivity decrease going down group 7

A

As the number of shells increases the outer shells is further from the attraction of the positive nucleus so its more difficult to attract the incoming electron.

26
Q

Displacement of halogens

A

A more reactive halogen will always displace a less reactive halide from its compounds in solution.

27
Q

Colour of halogen chlorine in solution

A

Pale green solution

28
Q

Colour of halogen Bromine in solution

A

Orange solution

29
Q

Colour of halogen iodine in solution

A

Brown solution

30
Q

How does toxicity effect halogens?

A

All halogens are toxic and it decreases going down the group

31
Q

Properties of elements in group 0

A

Colourless gases at room temp

unreactive/inert

32
Q

What happens to the boiling points of elements in group 0 as you go down the group?

A

They increase as the strength of the van deer Waals forces increases.

32
Q

Why are elements in group 0 unreactive?

A

As they are already stable, have a full outer shell of electrons and don’t need to gain or lose electrons.

33
Q

What are the physical properties of transition metals?

A
  • High Melting Point
  • High Density
  • Low Reactivity with water
  • Reacts to form ions with different charges
  • Form coloured compounds
34
Q

What colour is copper (ll) oxide

A

Black

35
Q

What colour is copper (ll) carbonate

A

Green

36
Q

What colour is hydrated copper (ll) sulphate

A

Blue

37
Q

What colour are copper (ll) salts usually in solution

A

Blue

37
Q

What are the physical properties or group 1 metals?

A

Low melting point
Low density
Very reactive with cold water
react to form 1+ ions e.g. K+
Forms white compounds

38
Q

What can you do when risk assessing for the reaction of alkali metals and water?

A

Use tweezers to lift the metals to prevent handling the metal directly as it could react with water in the skin

Use a safety screen as this prevents corrosive hydroxide solution from splashing out and causing damage to the skin

39
Q

How do you prepare alkali metals for reaction with water?

A
  1. Cut a small piece of metal
  2. Remove the oil layer with filter paper
  3. Use tweezers to drop the metal into a large trough of water behind a safety screen and wearing safety glasses

Chemistry - S1 (8 decks)

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