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Chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

What are the two components of the structure of a metal?

A

A lattice of positive metal ions and a sea of delocalised electrons

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2
Q

What is metallic bonding?

A

The electrostatic attraction between the positive metal ions and the negative delocalised electrons

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3
Q

is metallic bonding a strong or weak attraction?

A

Strong

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4
Q

3 metal properties

A

high melting points, able to conduct electricity and are malleable

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5
Q

Why do metals have high melting points?

A

The metallic bond bonding is usually very strong so lots of energy is needed to break it

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6
Q

Why can metals conduct electricity?

A

Because the delocalised electrons are free to move through the lattice

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7
Q

Why are metals malleable?

A

The layers of metal ions can slide over each other

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8
Q

What is thermal decomposition?

A

A thermal decomposition reaction is when heat energy is used to break down a substance

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9
Q

Equation for the thermal decomposition of metal carbonates?

A

metal carbonate –> metal oxide + carbon dioxide

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10
Q

thermal decomposition of copper carbonate with colours?

A

copper carbonate (green solid) –> copper oxide (black solid) + carbon dioxide (colourless gas)

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11
Q

What is downward delivery?

A

Carbon dioxide is denser then air so it sinks to the bottom of a test tube and stays there until you want to use it.

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12
Q

3 most reactive metals?

A

Potassium (K), Sodium (Na), Lithium (Li)

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13
Q

Metal + water equation?

A

metal + water –> metal hydroxide + hydrogen

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14
Q

Magnesium + water observations?

A

Effervescence - due to the hydrogen gas produced
Solid disappears - due to being used up in this reaction

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15
Q

What are group 1 metals also called?

A

alkalimetals

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16
Q

Observations for Li, Na or K with water?

A

Solid floats - less dense than water
Effervescence - hydrogen gas is produced
Solid moves - the effervescence propels it around the surface of the water
Solid disappears - it is used up in the reactions

17
Q

What colour does the universal indicator turn after a group 1 metal and water react?

A

dark blue

18
Q

Why are metal hydroxides alkalis?

A

the donation OH-

19
Q

Colour of potassium flame?

A

lilac

20
Q

Why do the group 1 metals get more reactive as you go down the group?

A

The atoms get bigger and have move shells
The outer electron is further from the nucleus
The attraction between the nucleus and the outer electron is weaker
So less energy is needed to break the attraction

21
Q

Metal + steam reaction equation?

A

metal + steam –> metal oxide + hydrogen

22
Q

Conducting a magnesium and steam reaction

A

Conducted in a horizontal tube
Some wet wool is heated to generate steam for the Mg to react with
The hydrogen gas produced is ignited to safely destroy it

23
Q

Why do metals react with cold water and hot steam to produce different products?

A

Steam has more energy, so both bonds in the molecule can break - O, H, H
Cold water has less energy, so only one bond can break - H, OH

24
Q

Why is hydrogen ignited?

A

To safely destroy it

25
Q

Acid + metal reaction equation?

A

acid + metal –> salt + hydrogen

26
Q

What metal salt does hydrochloric acid (HCl) make?

A

metal chloride

27
Q

What metal salt does sulphuric acid (H2SO4) make?

A

metal sulphate

28
Q

What metal salt does nitric acid (HNO3) make?

A

metal nitrate

29
Q

What metal salt does phosphoric acid (H3PO4) make?

A

metal phosphate

30
Q

2 observations in an acid + metal reaction

A

The metal disappears - it is used up in the reaction
There is fizzing - because hydrogen is produced

31
Q

Displacement reactions

A

More reactive metals can displace less reactive metals from their compounds

32
Q

displacement reaction - magnesium + copper sulphate (with colours)

A

magnesium (grey solid) + copper sulphate (blue solution) –> copper (pink-orange solid) + magnesium sulphate (colourless solution)

33
Q

2 common displacement observations

A

Solid colour change
Solution colour change

Chemistry (6 decks)

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