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Chemistry - S1 > Periodic Table > Flashcards

Periodic Table Flashcards

1
Q

Metal + Oxygen

A

Metal Oxide

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2
Q

Metal + Cold Water

A

Metal Hydroxide + Hydrogen

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3
Q

Metal + Steam

A

Metal Oxide + Hydrogen

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4
Q

Metal oxide + acid

A

Salt + Water

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5
Q

Acid + Base

A

Salt + Water

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6
Q

Metal Carbonate + Acid

A

Salt + Water + Carbon Dioxide

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7
Q

Difference between Mendeleev’s table and the modern periodic tabele

A

Mendeleev:
Arranged the elements in order of atomic weight
No noble gases present
Gaps were left for undiscovered elements
no block of transition metals
Actinides and lanthanides not present

Modern:
Arranged the elements in order of atomic number
noble gases present
block of transition metals
Actinides and lanthanides present

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8
Q

Differences between the properties of metals and non-metals:

A

Metals:
High Melting and boiling point
malleable
ductile
sonorous
good conductors of heat/electricity

Non-Metals:
low Melting and boiling point ( except graphite and diamond)
not malleable
not ductile
not sonorous
poor conductors of heat/electricity

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9
Q

What is a Displacement reaction and its ionic equation?

A

Ionic equation: The two metals that get displaced eg
Mg(s) + Cu2+ (aq) —> Mg2+(aq) + Cu

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10
Q

What is a Neutralisation reaction and its ionic equation?

A

An Acid and A base react to create a salt with a neutral pH of & and water

Ionic equation:
0H- (aq) + H+(aq) —-> H2O (I)

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11
Q

What is a Precipitation reaction and its ionic equation example?

A

When two aqueous solution react to form an insoluble solid

Ionic equation: Ba2+ (aq) + SO4 2- (aq) —> BaSO4 (S)

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12
Q

what is this reaction called and what does it equal?

alkali metal + oxygen = ?

A

Alkali Metal Oxide

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13
Q

What are the 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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14
Q

Alkali metal + Water

A

alkali metal hydroxide + Hydrogen

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15
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 tot the skin

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16
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
17
Q

Observations for Lithium reacting with water

A

bubbles
heat released
moves on the surface
colourless solution produced
Li disappeared at the end of the reaction

18
Q

Observations for Sodium reacting with water

A

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

19
Q

Observations for Potassium reacting with water

A

Lilac flame
bubbles
heat released
K melts into a tiny ball
moves on the surface
crackles at the end
colourless solution produced
K disappears quickly

20
Q

Balanced equation that applies to lithium, sodium and potassium reacting with water -

A

2 Li (s) + 2 H2O (I) —-> 2LiOH (aq) + H2 (g)

20
Q

What are the half equations for group 1 ions?

A

X –> X+ + e-

e.g K –> K+ + e-

20
Q

Why does reactivity increase going down group 1?

A

Group I elements have 1 electron in their outer shell. When they react they lose their outer electron to obtain a full outer shell. They become more reactive as you go down the group as the outer electron becomes further away from the positive nucleus.

21
Q

What colour and state is fluorine

A

Pale yellow - gas

21
Q

What colour and state is chlorine

A

green-yellow - gas

22
Q

What colour and state is bromine

A

red-brown - liquid

23
Q

What colour and state is iodine

A

grey-black - solid

24
Q

What does iodine do?

A

Sublimes and produces a purple vapour

24
Q

What is the half equation for group 7 ions?

A

Halogen –> Halide Ion + e-

e.g I2 + 2e- –> 2I-

25
Q

Wy does reactivity decrease going down group 7?

A

As thee outer shell is further away from the positive attraction of the nucleus so it is more difficult to attract an incoming electron.

25
Q

What colour is Chlorine in solution?

A

Pale green solution

26
Q

What colour is Bromine in solution?

A

Orange solution

27
Q

What colour is Iodine in solution?

A

Brown solution

28
Q

What are thee properties of Halogens?

A
  • Are non-metals
  • Are poisonous
  • Are smelly
  • React readily with metals to form compounds & Diatomic
29
Q

Properties of the noble gases?

A

Colourless gases at room temp
stable/inert

30
Q

Why are noble gases unreactive?

A

As they are already stable and have a full outer shell of electrons

31
Q

Why does the boiling point of noble increase as you go down the group?

A

As the strength of Van Deer Waals forces increases

32
Q

Properties of transition metals?

A
  • High melting point
  • High density
  • Low reactivity with water
  • React to form ions with different charges
  • Form coloured compounds
33
Q

What colour is:
copper(II) oxide
copper (II) carbonate
hydrated copper(II) sulfate
copper(II) salts

A

copper(II) oxide is black;
copper (II) carbonate is green;
hydrated copper(II) sulfate is blue; and
copper(II) salts are usually blue in solution

34
Q

Properties of group one metals?

A

Low melting and boiling point
Low density
Vey reactive with cold water
react to form 1+ ions
form white compounds

Chemistry - S1 (6 decks)

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